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+The Project Gutenberg EBook of The Elements of Blowpipe Analysis, by 
+Frederick Hutton Getman
+
+This eBook is for the use of anyone anywhere at no cost and with
+almost no restrictions whatsoever.  You may copy it, give it away or
+re-use it under the terms of the Project Gutenberg License included
+with this eBook or online at www.gutenberg.org
+
+
+Title: The Elements of Blowpipe Analysis
+
+Author: Frederick Hutton Getman
+
+Release Date: June 25, 2010 [EBook #32974]
+
+Language: English
+
+Character set encoding: ISO-8859-1
+
+*** START OF THIS PROJECT GUTENBERG EBOOK THE ELEMENTS OF BLOWPIPE ANALYSIS ***
+
+
+
+
+Produced by The Online Distributed Proofreading Team at
+https://www.pgdp.net. (This file was produced from images
+generously made available by The Internet Archive/American
+Libraries.)
+
+
+
+
+
+
+
+THE ELEMENTS OF BLOWPIPE ANALYSIS
+
+[Illustration]
+
+
+
+
+THE
+
+ELEMENTS OF BLOWPIPE
+
+ANALYSIS
+
+BY
+
+FREDERICK HUTTON GETMAN, F.C.S.
+
+INSTRUCTOR IN CHEMISTRY IN THE STAMFORD HIGH SCHOOL
+
+New York
+THE MACMILLAN COMPANY
+LONDON: MACMILLAN & CO., LTD.
+1899
+
+_All rights reserved_
+
+
+COPYRIGHT, 1899,
+
+BY THE MACMILLAN COMPANY.
+
+Norwood Press
+J. S. Cushing & Co.--Berwick & Smith
+Norwood Mass. U.S.A.
+
+Transcriber's note: A word surrounded by underscores like _this_
+signifies the word is italics in the text. A word surrounded by cedillas
+like ~this~, signifies the word is bolded in the text. For numbers and
+equations, underscores before bracketed numbers in equations denote a
+subscript.
+
+
+PREFACE
+
+
+These few pages are intended to serve a twofold purpose,--to give the
+student a general outline of Blowpipe Analysis, and to introduce him to
+the methods of Determinative Mineralogy.
+
+Every effort has been made to simplify details so that the book may be
+used in both High Schools and Colleges.
+
+Tables for "systematic" examination have been intentionally omitted, for
+in the author's estimation these tend to dull the student's power of
+observation, and to make him place little value upon minute details.
+
+The alphabetic arrangement has been followed for the sake of convenience
+when referring to the book.
+
+The last chapter is not intended to serve as a key to determining the
+minerals therein described, but rather it is added to give the student
+exercise in Blowpipe Analysis, and at the same time to point out the
+_methods_ of Determinative Mineralogy.
+
+Finally, the author would acknowledge his indebtedness to the following
+works: "Manual of Qualitative Analysis," Fresenius; "Qualitative
+Chemical Analysis," Venable; Roscoe and Schorlemmer's "Treatise on
+Chemistry"; Foye's "Hand-Book of Mineralogy"; Dana's "Mineralogy";
+Kobell's "Tafeln zur Bestimmung der Mineralien"; etc.
+
+FREDERICK HUTTON GETMAN.
+
+STAMFORD, CONN.,
+
+Feb. 22, 1899.
+
+
+
+
+TABLE OF CONTENTS
+
+
+CHAPTER I
+                                                             PAGE
+Apparatus and Reagents                                        1-7
+
+
+CHAPTER II
+
+General Outline of Blowpipe Analysis                            8
+
+Definitions                                                     9
+
+Examination on Charcoal Alone                                  10
+
+Examination on Charcoal with Sodium Carbonate                  13
+
+Examination in Tube with Sodium Carbonate and Charcoal         15
+
+Examination on Platinum Wire                                   16
+
+Examination in Borax Bead                                      17
+
+Examination with Cobalt Nitrate                                20
+
+
+CHAPTER III
+
+General Reactions for the Detection of the Metallic
+Elements in Simple Compounds                                   22
+
+Aluminum                                                       23
+
+Antimony                                                       24
+
+Arsenic                                                        25
+
+Bismuth                                                        25
+
+Cadmium                                                        26
+
+Chromium                                                       26
+
+Cobalt                                                         27
+
+Copper                                                         28
+
+Iron                                                           28
+
+Lead                                                           29
+
+Manganese                                                      30
+
+Mercury                                                        30
+
+Nickel                                                         31
+
+Silver                                                         32
+
+Tin                                                            32
+
+Zinc                                                           33
+
+The Alkali Metals                                              34
+
+Ammonium                                                       34
+
+Potassium                                                      35
+
+Sodium                                                         35
+
+Lithium                                                        36
+
+The Alkaline Earths                                            36
+
+Barium                                                         36
+
+Calcium                                                        37
+
+Strontium                                                      37
+
+The Acid Elements                                              37
+
+Borates                                                        37
+
+Bromides                                                       38
+
+Chlorides                                                      38
+
+Fluorides                                                      38
+
+Iodides                                                        39
+
+Nitrates                                                       39
+
+Phosphates                                                     40
+
+Silicates                                                      40
+
+Sulphides                                                      41
+
+
+CHAPTER IV
+
+Behavior of Some of the Principal Ores before the Blowpipe     43
+
+Ores of Antimony                                               46
+
+Ores of Arsenic                                                47
+
+Ores of Bismuth                                                48
+
+Ores of Chromium                                               49
+
+Ores of Cobalt                                                 50
+
+Ores of Copper                                                 52
+
+Ores of Iron                                                   57
+
+Ores of Lead                                                   60
+
+Ores of Manganese                                              63
+
+Ores of Mercury                                                64
+
+Ores of Nickel                                                 65
+
+Ores of Silver                                                 66
+
+Ores of Tin                                                    69
+
+Ores of Zinc                                                   70
+
+
+COMPARATIVE TABLES
+
+I. Colors of Coatings on Charcoal                              73
+
+II. Flame Colorations                                          73
+
+III. Colors of Borax Beads in oxidizing Flame                  74
+
+IV. Colors of Borax Beads in reducing Flame                    75
+
+V. Colors of Microcosmic Salt Beads in oxidizing Flame         76
+
+VI. Colors of Microcosmic Salt Beads in reducing Flame         77
+
+
+[Illustration: THE BLOWPIPE Fig. 1]
+
+[Illustration: BUNSEN BURNER Fig. 2]
+
+[Illustration: CHARCOAL BORERS Fig. 3]
+
+[Illustration: AGATE MORTAR & PESTLE Fig. 4]
+
+[Illustration: FORCEPS Fig. 5]
+
+[Illustration: HAMMER Fig. 6]
+
+[Illustration: 3-CORNERED FILES Fig. 7]
+
+
+
+
+BLOWPIPE ANALYSIS
+
+
+
+
+CHAPTER I
+
+
+The blowpipe was first applied to mineral analysis in 1733 by Anton
+Swab, and its applications have since been improved and extended by
+various chemists, among whom may be mentioned Bergmann, Cronstedt, Gahn,
+Berzelius, and Plattner.
+
+
+~Blowpipe.~--The common blowpipe of the jeweller is not particularly well
+suited to the operations of blowpipe analysis, since the flame has often
+to be kept playing upon the assay for some time, and the condensed
+moisture of the breath would seriously interfere with the passage of
+the air through the jet. One of the best and least expensive forms of
+blowpipe is shown in Fig. 1. This consists, as is seen from the
+illustration, of a conical-shaped tube of tin closed at the wide end and
+formed into a mouthpiece at the small end; soldered into the tube at the
+large end, and at right angles to its axis, is a small brass tube which
+terminates in a conical tip pierced with a very fine hole. With this
+pipe it is possible to perform all of the operations of mineral
+analysis.
+
+Some little practice is necessary to keep the flame steady and to take
+the breath at the same time.
+
+No rule can well be given to the beginner, but his experience becomes
+his best guide.
+
+
+~Bunsen Flame.~--Any kind of flame can be used for the blowpipe, provided
+it be not too small; but since almost every laboratory to-day is
+furnished with gas and the Bunsen burner (Fig. 2), it will only be
+necessary to describe the use of the flame from this source. Upon
+examining the Bunsen flame with care, it will be seen that the flame
+consists of three distinct parts.
+
+A dark inner cone which consists of gas not yet raised to the ignition
+point. Beyond this there is a luminous cone, where combustion is
+incomplete owing to lack of oxygen, and outside of this we find the
+non-luminous cone where the gas is completely burned.
+
+This outer envelope is the hottest portion of the flame, and is known as
+the "oxidizing" flame because there is an excess of oxygen which is
+imparted to substances placed therein.
+
+The luminous cone is known as the "reducing" flame, for in it metallic
+oxides are reduced, the oxygen being taken up by the small incandescent
+particles of carbon.
+
+If the air-holes at the base of the Bunsen burner be opened, the two
+inner cones become elongated, and the flame appears almost colorless.
+
+The blowpipe enables us to get an oxidizing and a reducing flame of
+better form and greater power. To do this we cut off the air supply at
+the base of the burner and turn off the gas until the flame is about 1
+cm. high; then upon introducing the blowpipe, and blowing a strong
+continuous jet of air across the Bunsen flame, we produce an oxidizing
+flame about 4-5 cm. in length. If the tip of the blowpipe be held
+outside of the Bunsen flame, and the pressure of the stream of air be
+diminished, we obtain a reducing flame.
+
+
+~Supports.~--For supports, charcoal, platinum, and glass are chiefly used.
+The charcoal should be made from some light wood, such as alder. It
+should be well burnt, and should not scintillate or smoke.
+
+The platinum supports are generally in the form of wire and foil.
+Platinum-tipped forceps are frequently employed in blowpipe analysis.
+
+Glass is used in the form of tubing.
+
+Hard glass tubing, 3 mm. bore, is drawn off into ignition tubes 7-8 cm.
+in length. Several dozen of these tubes should be made before commencing
+the tests of the next chapter.
+
+
+~Apparatus.~--A small agate mortar, 4-5 cm. in diameter, should be
+provided in which to grind the samples to be examined.
+
+The pestle, which should also be of agate, must be adapted to the
+mortar in shape and size.
+
+Two pairs of forceps will also be needed.
+
+One pair should be of steel, and the other pair of brass, with fine
+points.
+
+Of other apparatus, the most necessary is:--
+
+    A small hammer and anvil.
+
+    Two three-cornered files.
+
+    Small piece of cobalt glass, about 5 × 10 cm.
+
+    Pocket magnifying lens.
+
+    Several small watch glasses--for metallic beads, etc.
+
+
+~Chemicals.~--A list of the principal chemicals is here given:--
+
+    Sodium carbonate, Na_{2}CO_{3}.
+
+    Borax, Na_{2}B_{4}O_{7} + 10 H_{2}O.
+
+    Microcosmic salt, (HNaNH_{4}), PO_{4} + 8 H_{2}O.
+
+    Cobalt nitrate, Co(NO_{3})_{2} + 5 H_{2}O.
+
+    Potassium cyanide, KCN.
+
+    Hydrochloric acid, (dilute), HCl + nH_{2}O.
+
+    Litmus paper, red and blue.
+
+    Brazil-wood paper.
+
+Any other special reagents which may be needed will be mentioned as
+required.
+
+
+
+
+CHAPTER II
+
+GENERAL OUTLINE OF BLOWPIPE ANALYSIS
+
+
+     [ABBREVIATIONS: O. F. for oxidizing flame, R. F. for
+     reducing flame, Ch. for charcoal, Ct. for coating, Bp. for
+     blowpipe.]
+
+In order to examine a substance before the blowpipe to determine the
+presence or absence of certain elements, it becomes necessary to arrange
+a systematic method. As with all branches of chemical work, one's
+success is largely dependent upon neatness of manipulation and
+carefulness of observation.
+
+The following order of observation is essentially that given by
+Berzelius:--
+
+     1. Examination on charcoal by itself.
+
+     2. Examination on charcoal with Na_{2}CO_{3}.
+
+     3. Examination in ignition tube with Na_{2}CO_{3} and
+     charcoal.
+
+     4. Examination on platinum wire.
+
+     5. Examination in borax bead.
+
+     6. Examination with Co(NO_{3})_{2}.
+
+After having examined a body in these six different ways, we shall be
+able to say what are its principal constituents.
+
+Before describing the method of carrying out these six different
+operations, it will be necessary to give a few definitions of terms
+which we shall have frequent occasion to employ.
+
+
+~Definitions.~--_Ignition_ is the heating of a substance to a high
+temperature.
+
+_Fusion_ is the heating of a substance to the melting-point.
+
+_Intumescence_ is the swelling of the substance upon heating.
+
+_Decrepitation_ is the crackling of a substance due to the sudden
+expansion of combined water upon heating.
+
+_Deflagration_ is the burning of a substance with explosive violence,
+generally due to excess of oxygen.
+
+_Incandescence_ is the white light emitted by a substance that is
+infusible when subjected to a high temperature.
+
+
+~Examination on Charcoal alone.~--The size of the assay should be about
+that of a mustard seed. This is sufficiently large to show all of the
+reactions clearly, and though a larger piece would exhibit the
+characteristic phenomena, yet much more effort is required. A very
+small, shallow hole should be cut in the Ch. to receive the assay. The
+Bp. flame should be directed at an angle of about 30° with the surface
+of the Ch. Considerable care must be taken lest the hole in the Ch. is
+burned too deep and the assay lost in the coal.
+
+The force of the air from the jet must also be borne in mind for a
+strong blast, or sudden puffs may blow the substance away.
+
+The following changes are to be looked for:--
+
+_a._ Whether the substance is volatile or non-volatile.
+
+_Illustrations._ Examine before the Bp. on Ch. some arsenious oxide,
+As_{2}O_{3}, also some alumina, Al_{2}O_{3}.
+
+_b._ Whether the substance is fusible or infusible.
+
+_Illustrations._ Examine before the Bp. on Ch. some silver oxide, AgO,
+also some zinc oxide, ZnO.
+
+_c._ Whether the substance is alkaline or non-alkaline when placed upon
+moistened red litmus.
+
+_Illustrations._ Ignite some calcium carbonate, CaCO_{3}, before the Bp.
+on Ch., and place residue on moistened red litmus. In like manner,
+examine some magnesium carbonate, MgCO_{3}.
+
+_d._ Color of coating on Ch. caused by combination of metal and oxygen
+due to heat of Bp. flame.
+
+_Illustrations._ Examine some oxide of lead, PbO, before the Bp. on Ch.,
+also some oxide of cadmium, CdO.
+
+_e._ Decrepitation.
+
+_Illustration._ Examine some sodium chloride, NaCl, before the Bp. on
+Ch.
+
+_f._ Deflagration.
+
+_Illustrations._ Examine some potassium nitrate, KNO_{3}, before the Bp.
+on Ch., also some ammonium nitrate, NH_{4}NO_{3}.
+
+_g._ Intumescence.
+
+_Illustration._ Examine some alum,
+
+    K_{2}Al_{2}(SO_{4})_{4},
+
+before the Bp. on Ch.
+
+_h._ Incandescence.
+
+_Illustration._ Examine some oxide of barium, BaO, before the Bp. on Ch.
+
+_i._ Formation of a metallic bead--color and malleability.
+
+_Illustration._ Examine some silver oxide, AgO, before the Bp. on Ch.
+
+
+~Examination on Charcoal with Na_{2}CO_{3}.~--Metallic compounds are often
+difficult to reduce with the blowpipe flame alone, and hence no bead is
+obtained. In order to facilitate reduction and the obtaining of a
+metallic bead, the substance in a finely powdered condition is mixed
+with four parts of sodium carbonate, Na_{2}CO_{3}, and ignited before
+the Bp. on Ch. The metallic compound is decomposed, the metal being
+transformed into the carbonate, which in turn, through the agency of the
+Ch. and the heat of the flame, is reduced to the free metal. Sometimes
+the reduction is made easier by adding to the substance about its own
+bulk of potassium cyanide, KCN, which takes up oxygen from the compound
+and is converted into potassium cyanate, KCNO.
+
+The reactions in reducing copper sulphate, CuSO_{4}, with Na_{2}CO_{3}
+and with KCN before the blowpipe, are here given:--
+
+    CuSO_{4} + Na_{2}CO_{3} = CuCO_{3} + Na_{2}SO_{4} }  (1)
+              2CuCO_{3} + C = 3CO_{2} + 2Cu           }
+
+    CuSO_{4} + Na_{2}CO_{3} = CuCO_{3} + Na_{2}SO_{4} }
+                   CuCO_{3} = CuO + CO_{2}            }  (2)
+                  CuO + KCN = Cu + KCNO               }
+
+After obtaining beads, it is well to obtain their coatings, for
+oftentimes it is only in this way that we can distinguish between the
+metals.
+
+
+~Examination in Tube with Na_{2}CO_{3} and Charcoal.~--If the substance in
+a finely pulverized condition be mixed with twelve parts, Na_{2}CO_{3},
+and six parts of charcoal powder and the mixture be placed in an
+ignition tube and subjected to heat, the acid of the substance combines
+with the soda and the metal is set free.
+
+If this metal is volatile, a sublimate is formed in the upper end of the
+tube.
+
+Mercury deposits in minute globules, which may be seen with the
+magnifying glass. Arsenic forms a ring, which, when examined with the
+magnifying glass, is seen to be made up of minute crystals. Ammonia is
+recognized by its characteristic odor, and also by its turning a slip
+of moistened red litmus (held over the mouth of the tube) blue.
+
+
+~Examination on Platinum Wire.~--Many substances possess the property of
+imparting to the colorless flame of the Bunsen burner characteristic
+colors.
+
+The chlorides of these substances exhibit these flame reactions best,
+and hence before applying the flame tests we dip the wire which serves
+as a support into hydrochloric acid and then into the substance. When
+the substance has been taken up on the wire, it is placed in the edge of
+the long colorless flame of the Bunsen burner near the apex, when
+instantly the flame becomes tinged with the characteristic color of the
+substance.
+
+_Illustrations._ Sodium compounds color the flame yellow, and a crystal
+of potassium dichromate appears colorless in the sodium light.
+
+This sodium reaction is extremely delicate, it being possible to detect
+with ease a quantity of a sodium salt less than 1/3000000 of a milligram
+in weight.
+
+Potassium colors the flame purplish-violet.
+
+Barium colors the flame apple-green.
+
+Strontium colors the flame crimson.
+
+Calcium colors the flame orange-red, distinguished from strontium, by
+appearing gray when seen through blue glass.
+
+Boracic acid colors the flame green when the substance has been
+moistened with glycerine.
+
+
+~Examination in Borax Bead.~--Borax, Na_{2}B_{4}O_{7}, and microcosmic
+salt,
+
+    NaNH_{4}H . PO_{4},
+
+possess the property of dissolving many of the metallic oxides at the
+temperature of the Bunsen flame.
+
+For example, with oxide of cobalt, the following reactions take place
+with the two fluxes:--
+
+    CoO + Na_{2}B_{4}O_{7} = Co(BO_{2})_{2} + 2 NaBO_{2}.
+
+On heating, NaNH_{4}H. PO_{4}, it is decomposed into the metaphosphate
+of sodium, NaPO_{3},
+
+    CoO + NaPO_{3} = CoNaPO_{4}.
+
+Now in such cases of solution the metallic oxides impart a
+characteristic color to the flux.
+
+The platinum wire is the best support,--it is heated to incandescence in
+the Bunsen flame, and then is quickly dipped into the borax, when a
+small globule will adhere,--this is removed to the flame again when the
+borax melts to a clear glassy bead. While the bead is still melted,
+touch it to the finely pulverized substance and replace in the flame.
+In a few seconds the small particles of the substance will have
+dissolved, and the bead will be seen to have assumed the color
+characteristic of the substance. Note the color when hot and then when
+cold; often there is a wide difference. Then, too, the test should be
+made in both O. F. and R. F.
+
+Some analysts prefer to make a small loop in the end of the wire before
+taking up the borax to make the bead. Care should be taken to see that
+the bead is colorless before bringing it in contact with the substance.
+
+As the depth of color produced is largely dependent upon the amount of
+substance taken, some little caution should be exercised to insure
+taking up about the same quantity each time.
+
+_Illustrations._ Make several beads, and note the colors characteristic
+of the following oxides: cobalt, nickel, iron, manganese, chromium, and
+copper.
+
+The microcosmic salt bead dissolves almost every oxide except silica,
+SiO_{2}, and this is seen to float about in the melted mass. This is
+used as a test for silica.
+
+
+~Examination with Co(NO_{3})_{2}.~--If after examination on the Ch. _per
+se_, a white infusible residue remains, it is moistened with a drop of
+cobalt nitrate Co(NO_{3})_{2} and re-ignited before the Bp., when a
+change of color will be observed. This change in color is owing to the
+fact that the heat of the Bp. flame decomposes the cobalt nitrate,
+nitric acid being driven off, and the remaining CoO forming with the
+oxide of the residue a colored mass.
+
+_Illustrations._ Ignite before the Bp. on Ch. the following
+oxides,--allow to cool, add a drop of Co(NO_{3})_{2}, re-ignite, and
+note color,--aluminum, magnesium, zinc, and calcium.
+
+Care should be taken to thoroughly ignite before adding the cobalt
+nitrate solution.
+
+With the six methods of examination just given almost every simple
+substance can be detected, but should any doubt remain, a few simple
+tests in the "liquid way" will be sufficient to substantiate the
+blowpipe examination.
+
+
+
+
+CHAPTER III
+
+GENERAL REACTIONS FOR THE DETECTION OF THE METALLIC ELEMENTS IN SIMPLE
+COMPOUNDS
+
+
+For the sake of convenience, rather than for scientific reasons, the
+following compounds have been arranged in alphabetic order. Also the
+oxides of the elements have been taken, since they exhibit the reactions
+to best advantage.
+
+The student should work through carefully each one of the tests and
+satisfy himself as to the characteristic reactions of the various
+elements, for only in this way can he expect to recognize the substances
+when presented to him as "unknowns." It is advisable to provide a
+note-book and rule it as follows:--
+
+-----------------------------------------------------------------------------
+                         BEHAVIOR OF SUBSTANCE                              |
+----------------------------------------------------------------------------|
+Before Bp.| Before Bp.  | In ignition | In flame| In flame  | After first   |
+on Ch.    | on Ch. with | tube with   |   on    | with borax| ignition      |
+alone     | Na_{2}CO_{3}| Na_{2}CO_{3}| platinum| bead      | with          |
+          |             | and Ch.     |  wire   |           | Co(NO_{3})_{2}|
+----------------------------------------------------------------------------|
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+----------------------------------------------------------------------------|
+_Remarks_ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _             |
+                                                                            |
+_Substance_ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _             |
+----------------------------------------------------------------------------
+
+
+1. ~Aluminum, Al_{2}O_{3}.~--Before the Bp. on Ch. Infusible. No change.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Forms an infusible compound
+with slight intumescence.
+
+In ignition tube with Na_{2}CO_{3} and Ch. No change. Moisture driven
+off.
+
+In flame on platinum wire. No change. Becomes incandescent.
+
+In flame with borax bead. In O. F. dissolves slowly, forming a
+colorless glass which remains so on cooling.
+
+With Co(NO_{3})_{2}. Mass becomes blue upon re-ignition.
+
+
+2. ~Antimony, Sb_{2}O_{3}.~--Before the Bp. on Ch. In O. F. volatilizes
+without change. In R. F. is reduced and volatilized. White coating of
+antimonious oxide deposited on Ch. Blue tinge imparted to flame.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Readily reduced. White brittle
+bead. Very volatile, giving characteristic white coating.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Volatilized.
+
+In flame on platinum wire. Volatilized. Colors flame greenish blue.
+
+With borax bead on platinum wire. In O. F. dissolves to a colorless
+glass.
+
+With Co(NO_{3})_{2}.____
+
+
+3. ~Arsenic, As_{2}O_{3}.~--Before the Bp. on Ch. Very volatile. Strong
+garlic odor to fumes.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced with emission of
+arsenical fumes.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Volatilizes, forming a
+mirror-like deposit of metallic As in the cooler part of tube.
+
+In flame on platinum wire____
+
+With borax bead on platinum wire____
+
+With Co(NO_{3})_{2}.____
+
+
+4. ~Bismuth, Bi_{2}O_{3}.~--Before the Bp. on Ch. Yields a
+coating--orange-yellow when hot, lemon-yellow when cold. The yellow
+coating usually has a white outline.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Easily reduced to metallic
+bismuth. Yellow bead brittle, but less so than antimony.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. small quantity dissolves to a
+clear yellow glass, which becomes colorless when cold.
+
+With Co(NO_{3})_{2}____
+
+
+5. ~Cadmium, CdO.~--Before the Bp. on Ch. Gives a coating on the coal.
+Reddish-brown when cold. Very volatile.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Readily reduced. The metal
+volatilizes easily, giving the characteristic coating.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead. In O. F. dissolves to a clear yellowish bead, colorless
+when cold.
+
+With Co(NO_{3})_{2}____
+
+
+6. ~Chromium, Cr_{2}O_{3}.~--Before the Bp. on Ch. No change.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Cannot be reduced. Soda sinks
+in Ch. and a green colored mass remains.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+
+~With borax bead.~ Dissolves slowly but colors intensely. Yellow while
+hot, green when cold.
+
+With microcosmic salt bead. Colors red when hot, green when cold.
+
+With Co(NO_{3})_{2}____
+
+
+7. ~Cobalt, CoO.~--Before the Bp. on Ch. In O. F. unchanged. In R. F. is
+reduced to the metal and is magnetic.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced to a gray magnetic
+mass.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. colors very intensely blue,
+both hot and cold.
+
+With Co(NO_{3})_{2}____
+
+
+8. ~Copper, CuO.~--Before the Bp. on Ch. Fuses to a black globule, which
+can be reduced with some difficulty.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Readily reduced to metallic
+bead, which is red in color, hard, malleable.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire. Colors flame emerald-green.
+
+With borax bead on platinum wire. In O. F. green when hot, blue when
+cold.
+
+With Co(NO_{3})_{2}____
+
+
+9. ~Iron, Fe_{2}O_{3}.~--Before the Bp. on Ch. In O. F. unchanged. In R.
+F. becomes black and magnetic.
+
+Before the Bp. on Ch. with Na_{2}CO_{3} Reduced to a metallic powder,
+magnetic.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. red while hot, yellow when
+cold.
+
+With Co(NO_{3})_{2}____
+
+
+10. ~Lead, PbO.~--Before the Bp. on Ch. Easily reduced to the metal, bead
+very malleable. Coating yellow, surrounded by white ring.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Instantly reduced. Coats the
+Ch. upon further blowing.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Reduced to the metal.
+
+In flame on platinum wire. Tinges flame blue.
+
+With borax bead on platinum wire. In O. F. dissolves easily, forming a
+limpid glass.
+
+With Co(NO_{3})_{2}____
+
+
+11. ~Manganese, Mn_{2}O_{3}.~--Before the Bp. on Ch. At high temperature
+turns red.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Is not reduced.
+
+Before the Bp. in O. F. on platinum foil with Na_{2}CO_{3}. Transparent
+green mass when hot. Opaque, bluish-green when cold.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Not reduced.
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. violet-red while hot,
+amethyst-red when cold.
+
+With Co(NO_{3})_{2}____
+
+
+12. ~Mercury, HgO.~--Before the Bp. on Ch. Instantly reduced. Very
+volatile.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced and volatilized.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Sublimes condensing in the
+upper part of the tube as a metallic ring which is seen with the lens to
+consist of minute globules of mercury.
+
+In flame on platinum wire____
+
+With borax bead on platinum wire____
+
+With Co(NO_{3})_{2}____
+
+
+13. ~Nickel, NiO.~--Before the Bp. on Ch. In O. F. unchanged. In R. F.
+reduced to metal, slightly magnetic.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Easily reduced to the metal.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. violet while hot,
+reddish-brown when cold.
+
+With Co(NO_{3})_{2}____
+
+
+14. ~Silver, AgO.~--Before the Bp. on Ch. Easily reduced to the metal.
+White, malleable, hard bead. Coats the coal dark red near assay.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Instantly reduced to metallic
+globule.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Reduced to the metal.
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. partially dissolved. Bead
+becomes milk-white.
+
+With Co(NO_{3})_{2}____
+
+
+15. ~Tin, SnO_{2}.~--Before the Bp. on Ch. Coats the coal yellow while
+hot, dirty white when cool. Not reduced.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced to metallic tin. White,
+hard, malleable bead. Coating white and close to assay.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. small quantity dissolves to
+limpid glass.
+
+With Co(NO_{3})_{2}. Greenish-blue color.
+
+
+16. ~Zinc, ZnO.~--Before the Bp. on Ch. Upon ignition becomes yellow. Is
+not reduced.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced to metal. Rapidly
+volatilized, coating the coal white.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. yellow while hot, limpid
+glass when cold.
+
+With Co(NO_{3})_{2}. Green mass.
+
+Having now given the principal reactions for the most important metals,
+we will proceed to the examination of the alkali metals, the alkaline
+earths, and some of the acid elements.
+
+
+THE ALKALI METALS
+
+17. ~Ammonium, NH_{4}.~--This hypothetical compound is commonly classed
+among the alkali metals from its close resemblance to the members of
+this group.
+
+To detect the presence of this hypothetical metal, mix the assay with
+about four parts of Na_{2}CO_{3}, place in an ignition tube, and apply
+heat. The odor of the evolved gas will be recognized, and if a piece of
+red litmus paper be moistened and held at the mouth of the tube, it will
+be turned blue by the escaping ammonia gas.
+
+We are not authorized to infer the pre-existence of ammonium, however,
+from the appearance of this reaction, for the presence of nitrogenous
+organic matter in the substance, which would be decomposed by this
+treatment, would give rise to such a reaction.
+
+
+18. ~Potassium.~--Potassium is recognized by the color which its salts
+impart to the Bunsen flame. If a portion of a salt of potassium be held
+on a platinum wire in the flame, it imparts a blue-violet tint which
+rapidly disappears.
+
+
+19. ~Sodium.~--Like potassium, this alkali metal is detected by the color
+which its salts give to the flame.
+
+If a sodium salt be held on the platinum wire in the flame, it imparts
+an intense yellow color.
+
+The extreme delicacy of this reaction has been mentioned elsewhere. The
+value of this test is really lessened by its great delicacy, for it is
+possible to detect minute quantities of sodium in almost all substances,
+although it may not be in chemical combination. As an example, draw the
+platinum wire between the fingers, and then place in flame, and note
+presence of sodium.
+
+
+20. ~Lithium, Li_{2}O.~--In the Bunsen flame on the platinum wire it
+imparts a carmine-red tinge.
+
+Hydrochloric acid on the sample augments the coloration.
+
+
+THE ALKALINE EARTHS
+
+21. ~Barium, BaO.~--In the Bunsen flame on the platinum wire it imparts an
+apple-green coloration. This reaction is intensified by moistening the
+sample with hydrochloric acid.
+
+
+22. ~Calcium, CaO.~--In the Bunsen flame on the platinum wire it imparts
+an orange-red color, which appears gray when seen through blue glass.
+
+Hydrochloric acid on the sample makes the color more intense.
+
+
+23. ~Strontium, SrO.~--In the Bunsen flame on the platinum wire it imparts
+an intensely red color, which is increased by converting the substance
+into the chloride.
+
+
+THE ACID ELEMENTS
+
+24. ~Borates.~--If the substance be finely powdered, moistened with
+glycerine, and then placed on a platinum wire in the Bunsen flame, it
+imparts a brilliant green color.
+
+If turmeric paper be dipped into a solution of a borate, and then be
+dried at 100° C., it is turned to a peculiar red color. These two
+reactions are extremely delicate.
+
+
+25. ~Bromides.~--Bromides treated with microcosmic salt and oxide of
+copper on platinum wire impart to the flame a greenish-blue color, the
+edges being decidedly green.
+
+
+26. ~Chlorides.~--Chlorides are treated in the same way as bromides. The
+color imparted to the flame is azure-blue.
+
+To discriminate between bromides and chlorides more clearly, the
+substance is mixed with anhydrous potassium bisulphate and fused in an
+ignition tube.
+
+Bromine and sulphur dioxide are evolved (if the substance be a bromide),
+the tube being filled with a yellow gas possessing the characteristic
+odor of bromine.
+
+
+27. ~Fluorides.~--A small portion of the substance in a finely powdered
+condition is placed in one of the ignition tubes, a strip of moist
+Brazil-wood paper is introduced into the open end, and heat is applied.
+Hydrofluoric acid is evolved, and the red color of the paper is changed
+into a straw-yellow.
+
+Mica, containing only 0.75% of fluorine, shows the reaction clearly.
+
+
+28. ~Iodides.~--Iodides are treated, as the bromides and chlorides, in a
+bead of microcosmic salt with oxide of copper. The flame is colored
+green.
+
+Fused with potassium bisulphate in an ignition tube the violet vapors of
+iodine are evolved, and thus iodides may be distinguished from chlorides
+and bromides.
+
+
+29. ~Nitrates.~--If a nitrate be heated upon charcoal before the Bp.,
+violent deflagration occurs. If the substance containing the nitric
+acid be mixed with a _very small_ quantity of finely powdered potassium
+cyanide, the deflagration is accompanied with ignition and detonation.
+
+If the substance be mixed in a dry condition with dry potassium
+bisulphate, and is then heated in an ignition tube, red-brown nitrous
+fumes are evolved. This reaction takes place if there is but a small
+quantity of nitrate present.
+
+
+30. ~Phosphates.~--Phosphates impart to the flame a bluish green color.
+The color is made more intense by moistening the substance with
+sulphuric acid, and then taking the paste so formed on the platinum wire
+and placing it in the Bunsen flame.
+
+
+31. ~Silicates.~--Silicates, when treated with microcosmic salt on a
+platinum wire, suffer decomposition; the bases unite with the
+phosphoric acid to form a transparent glass in which the silica may be
+seen floating as a cloudy mass.
+
+The bead must only be examined for silica while hot, since on cooling it
+becomes opaque.
+
+
+32. ~Sulphides.~--Many sulphides, when heated in an ignition tube,
+volatilize and give a sublimate of sulphur in combination with the
+metallic portion of the substance.
+
+A very delicate test for sulphur in whatever combination it may be found
+in a substance, and which may be performed with great ease, is to mix
+the finely powdered assay with four parts, Na_{2}CO_{3}, and fuse in an
+ignition tube. When thoroughly fused the tube is broken, and the fused
+mass is placed on a bright silver coin, and a drop of water is added.
+If the substance contains sulphur, a black spot will be observed on the
+coin where the fused mass was placed.
+
+Before going on to the next chapter, the student should assure himself
+of his familiarity with the reactions just given, and he should practise
+with various substances, the nature of which is unknown to him.
+
+
+
+
+CHAPTER IV
+
+BEHAVIOR OF SOME OF THE PRINCIPAL ORES BEFORE THE BLOWPIPE
+
+
+For the sake of practice, and as a fitting introduction to
+"Determinative Mineralogy," this chapter is appended. It is not intended
+to give a detailed account of the minerals, but rather to set before the
+student the most marked characters, such as hardness, specific gravity,
+color, lustre, etc.
+
+To determine the hardness of a mineral, we try to scratch it with the
+minerals forming an arbitrary "scale of hardness," proceeding
+successively from the softest to the hardest. When we say that a certain
+mineral has hardness = 4, we mean that the mineral is scratched by 4 on
+the scale, and that 4 on the scale is scratched by the mineral. The
+scale of hardness chiefly in use is the Mohs-Breithaupt scale, which is
+as follows:--
+
+    1. Talc, common laminated light green variety.
+
+    2. Gypsum, crystallized.
+
+    3. Calcareous spar, transparent variety.
+
+    4. Fluor spar, crystalline.
+
+    5. Apatite, transparent.
+
+    6. Orthoclase, white cleavable variety.
+
+    7. Quartz, transparent.
+
+    8. Topaz, transparent.
+
+    9. Sapphire, cleavable variety.
+
+    10. Diamond.
+
+It seldom happens in determining the hardness of a mineral that its
+hardness exactly conforms to that of some one member of the scale. In
+such cases we generally estimate the hardness. For example, suppose a
+mineral was harder than 4, but softer than 5, and that it was nearer 5
+than 4, then we would call its hardness 4-3/4.
+
+In order to preserve the scale some operators use a three-cornered file,
+first cutting the mineral and then the scale until a number is found,
+which is abraded to about the same depth as the mineral under
+examination.
+
+Since a set of minerals forming a scale of hardness is not always at
+hand, the following scale given by Chapman is appended:--
+
+     1. Yields easily to the nail.
+
+     2. Yields with difficulty to the nail or just receives an
+     impression from it. Does not scratch a copper coin.
+
+     3. Scratches a copper coin but is also scratched by it,
+     being of about the same degree of hardness.
+
+     4. Not scratched by a copper coin. Does not scratch glass.
+
+     5. Scratches glass with difficulty, leaving its powder on
+     it. Yields readily to the knife.
+
+     6. Scratches glass easily. Yields with difficulty to the
+     knife.
+
+     7. Does not yield to the knife. Yields to the edge of a
+     file, though with difficulty.
+
+     8, 9, 10. Harder than flint.
+
+Specific gravity cannot well be determined without the aid of a balance,
+and hence its value here is not great.
+
+As in the preceding chapter, alphabetic arrangement will be employed.
+
+
+ORES OF ANTIMONY
+
+~Stibnite~, Sb_{2}S_{3}, Sb . 71, S . 29.--[A]H = 2, G = 4.52-4.62. Of
+lead-gray color and metallic lustre. Consists of a large number of
+needle-shaped crystals. Brittle. Fuses in candle flame. In an ignition
+tube yields a sublimate of sulphur. On Ch. before the Bp. it is
+volatilized, giving antimony coating and tinges the flame pale blue.
+
+[Footnote A: H = Hardness, G = Specific Gravity.]
+
+
+ORES OF ARSENIC
+
+~Native Arsenic, As.~--This contains traces of Sb, Ag, Fe, Co, and Ni.
+
+H = 3.5, G = 5.7-5.8. Dark gray in color. Fracture tin-white, tarnishing
+rapidly. Volatilizes before the Bp. on Ch. without melting, giving white
+coating of arsenious acid and characteristic garlic odor. In ignition
+tube it sublimes, giving arsenical ring.
+
+
+~Realgar~, AsS, As . 70, S . 30.--H = 1.5-2, G = 3.56. Bright red to
+orange-red color and resinous lustre. In an ignition tube it fuses and
+finally sublimes. The sublimate when cool is red and transparent. Fuses
+readily before the Bp. on Ch. and burns with pale yellowish flame,
+emitting gray-white fumes having garlic odor.
+
+
+~Orpiment~, As_{2}S_{3}, As . 61, S . 39.--
+
+    H = 1.5-2.0, G = 3.4-3.5.
+
+Lemon-yellow in color and resinous or pearly lustre. Sectile. Before the
+Bp. on Ch. behaves like realgar, but in an ignition tube it gives a dark
+yellow sublimate which is transparent.
+
+
+ORES OF BISMUTH
+
+~Native Bismuth, Bi.~--This contains traces of As, Te, and S.
+
+H = 2.0-2.5, G = 9.7-9.83. Color, silver-white, slightly tinged with
+red. Metallic lustre. Brittle when cold, but may be laminated when hot.
+Before the Bp. on Ch. behaves like pure Bi.
+
+
+~Bismuthite~, Bi_{2}O_{3} . 90, CO_{2} . 7, H_{2}O . 3,--
+
+    H = 4.0-4.5, G = 6.9-7.8.
+
+Usually of a white or light greenish color and vitreous lustre, in
+acicular crystallizations. In an ignition tube decrepitates, yielding
+water and turning gray. Before the Bp. on Ch. it fuses easily and is
+reduced to metallic globule, coating the Ch. with Bi_{2}O_{3}. With
+Na_{2}CO_{3} it occasionally gives the sulphur reaction.
+
+
+ORES OF CHROMIUM
+
+~Chromic Iron Ore~, FeO . 32, Cr_{2}O_{3} . 68.--Al_{2}O_{3}, Fe_{2}O_{3},
+MnO, and MgO are commonly present. H = 5.5, G = 4.32-4.57. Occurs
+usually massive. Color, iron-black to brownish black. In many varieties
+strongly magnetic. Lustre, shining and somewhat metallic. Heated in an
+ignition tube, remains unchanged. Infusible before the Bp. on Ch.
+Before the Bp. on Ch. with Na_{2}CO_{3} and KCN yields metallic iron. In
+borax bead it slowly dissolves to a clear transparent glass, which is a
+beautiful green when cool.
+
+
+ORES OF COBALT
+
+~Smaltite~, Co(Fe, Ni) As_{2}, Co . 28, As . 72.--H = 5.5, G = 6.37-7.30.
+Color, tin-white or steel-gray. Lustre, metallic. When heated to redness
+in an ignition tube it yields a sublimate of metallic arsenic. Before
+the Bp. on Ch. it fuses readily, with emission of arsenical fumes, to a
+grayish black magnetic globule. This globule may be examined for iron,
+cobalt, and nickel with the borax bead.
+
+
+~Cobaltite~, CoS_{2} + CoAs_{2}, Co . 36, As . 45, S . 19.--H = 5.5, G =
+6.0-6.3. Color, silver-white tinged with red. Metallic lustre. Before
+the Bp. on Ch. fuses easily, with emission of copious arsenical fumes,
+to a gray magnetic globule. Remains unchanged in the ignition tube.
+
+
+~Linnaeite~, (Co, Ni)_{3}S_{4}, (Co, Ni)58, S . 42.--H = 5.5, G = 4.8-5.0.
+Color, bright steel-gray, sometimes reddish. Lustre, metallic.
+Crystallizes in the regular octahedron. Before the Bp. on Ch. fuses to a
+metallic globule which is attracted by the magnet. With borax bead gives
+reaction for cobalt.
+
+
+~Erythrite~, Co_{3}O_{8}As_{2} + 8 H_{2}O, As_{2}S_{5} . 38.4, CoO . 37.6,
+H_{2}O . 24.0.--
+
+    H = 1.5-2.0, G = 2.95.
+
+Color, crimson to peach-red. When crystallized, of pearly lustre, but
+frequently dull and earthy. Heated in ignition tube gives off water, and
+color changes to blue or green. Before the Bp. on Ch. in R. F. it emits
+arsenical fumes and melts to a dark gray globule which with the borax
+bead reacts for cobalt.
+
+
+ORES OF COPPER
+
+~Native Copper, Cu.~--
+
+    H = 2.5-3, G = 8.5-8.9.
+
+Color, copper-red. Lustre, metallic. Occurs usually massive and very
+arborescent. Before the Bp. on Ch. it fuses, and if the heat is
+sufficiently high it assumes a bright bluish-green surface; on cooling
+it is covered with a coat of black oxide. In the borax bead it reacts
+for copper.
+
+
+~Chalcopyrite~, CuFeS_{2}, Cu . 35, Fe . 30, S . 35.--H = 3.5-4, G =
+4.1-4.3. Color, brass-yellow, often golden-yellow. Lustre, metallic.
+Occurs crystallized, but is generally found massive. Is easily
+scratched with a knife. Heated in an ignition tube decrepitates, and
+occasionally yields a faint sublimate of sulphur. Before the Bp. on Ch.
+it blackens, but becomes red again on cooling. Before the Bp. on Ch.
+with Na_{2}CO_{3} and KCN it is reduced, and the metals are obtained in
+separate masses. It reacts with the borax bead for copper and iron.
+
+
+~Copper Glance~, Cu_{2}S, Cu . 80, S . 20.--H = 2.5-3.0, G = 5.5-5.8.
+Color, dark blue to steel-gray. Occurs in compact masses, often very
+shining. Before the Bp. on Ch. fuses to a globule which boils and emits
+glowing drops. Sulphur dioxide escapes abundantly, and the outer flame
+is colored blue. Before the Bp. on Ch. with Na_{2}CO_{3} yielding a
+metallic globule.
+
+
+~Tetrahedrite~, 4 CuS + Sb_{2}S_{3}.--Frequently contains silver, iron,
+mercury, and zinc. H = 3.0-4.0, G = 4.5-5. Color, steel-gray to
+iron-black. Heated in an ignition tube fuses and gives a sublimate of
+antimonious oxide. When mercury is present this condenses in the upper
+part of the tube, forming the characteristic mirror. Before the Bp. on
+Ch. it fuses readily to a metallic globule, emitting dense white fumes;
+zinc and antimony coatings are deposited on the Ch. After long ignition
+before the Bp., if the mineral is finely powdered and mixed with
+Na_{2}CO_{3} and KCN, the ore is reduced to the metal.
+
+
+~Cuprite~, Cu_{2}O, Cu . 89, O . 11.--
+
+    H = 3.5-4.0, G = 5.5-6.15.
+
+Color, intense crimson-red. Before the Bp. on Ch. blackens and fuses
+quietly, and finally yields a metallic globule of copper. Before the Bp.
+on Ch. with Na_{2}CO_{3} and KCN it is easily reduced.
+
+
+~Malachite~, 2 CuO + CO_{2} + H_{2}O, CuO . 72, CO_{2} . 20, H_{2}O . 8.--
+
+    H = 3.5-4.0, G = 3.90-4.03.
+
+Color, bright green. Occurs generally in mammillated concretions.
+Lustre, shining and fracture, silky. Heated in an ignition tube yields
+water and blackens. Before the Bp. on Ch. it fuses to a metallic
+globule. Before the Bp. on Ch. with Na_{2}CO_{3} and KCN it is easily
+reduced. With borax bead gives characteristic coloration.
+
+
+~Azurite~, 3 CuO + 2 CO_{2} + H_{2}O, CuO . 69, CO_{2} . 26, H_{2}O . 5.--
+
+    H = 3.5-4.0, G = 3.77-3.83.
+
+Color, azure-blue. Occurs usually in crystallized or globular masses.
+Lustre, earthy or vitreous. Before the Bp. and with other reagents
+behaves like malachite.
+
+
+~Chrysocolla~, CuO + SiO_{2} + 2 H_{2}O, SiO_{2} . 34.2, CuO . 45.3,
+H_{2}O . 20.5.--H = 2.0-3.0, G = 2. Color, bluish-green, closely
+resembling malachite. Occurs usually as an incrustation, its surface
+being very smooth, like enamel. In an ignition tube it blackens and
+yields water. Before the Bp. on Ch. in O. F. it blackens, coloring the
+flame bright green; in the R. F. it turns red. Before the Bp. on Ch.
+with Na_{2}CO_{3} yields metallic copper. In borax bead it reacts for
+copper.
+
+
+~Atacamite~, CuCl_{2} + 3 CuO_{2}H_{2}--Cl . 16.6, O . 20.3, Cu . 50.1,
+H_{2}O . 13.0.--
+
+    H = 3.0-3.5, G = 3.75-3.77.
+
+Color, green to blackish green. Lustre, adamantine to vitreous. In an
+ignition tube yields water. Before the Bp. on Ch. colors flame blue.
+Before the Bp. on Ch. with Na_{2}CO_{3} and KCN is reduced to the metal.
+In borax bead it reacts for copper.
+
+
+ORES OF IRON
+
+~Limonite~, 2 Fe_{2}O_{3} + 3 H_{2}O, Fe_{2}O_{3} . 86, H_{2}O . 14.--H =
+5.0-5.5, G = 3.6-4.0. Color, brown to ochre-yellow. Earthy or
+semi-metallic in appearance. In an ignition tube yields water. Before
+the Bp. on Ch. infusible. In borax bead reacts for iron.
+
+
+~Hematite~, Fe_{2}O_{3}, Fe . 70, O . 30.--
+
+    H = 5.5-6.5, G = 4.9-5.3.
+
+Color, dark steel-gray to iron-black. Lustre, metallic. When pulverized
+yields a red powder. Before the Bp. on Ch. infusible. After long
+roasting becomes magnetic. In borax bead gives usual indications of
+iron.
+
+
+~Magnetite~, Fe_{3}O_{4}, FeO . 31, Fe_{2}O_{3} . 69.--
+
+    H = 5.5-6.5, G = 5.17-5.18.
+
+Color, iron-black. Lustre, shining and metallic. Pulverized, its powder
+is black. It is strongly magnetic. Fuses with difficulty before the Bp.
+on Ch. In borax bead reacts for iron.
+
+
+~Pyrites~, FeS_{2}, Fe . 47, S . 53.--
+
+    H = 6.0-6.5, G = 4.95-5.20.
+
+Color, brass-yellow. Lustre, metallic. Occurs commonly in cubes. It
+often contains small quantities of Au, Ag, Cu, As, Co, and Mn. Heated in
+an ignition tube gives a sublimate of sulphur, the residue becoming
+magnetic. Before the Bp. on Ch. in O. F. sulphur is burned off and the
+red oxide remains. This residue may then be examined for iron, etc.
+
+
+~Marcasite~ (White Iron Pyrites).--Having the same general composition as
+pyrite, but much lighter in color. Crystals, prismatic. Before the Bp.
+on Ch. behaves like pyrite.
+
+
+~Pyrrhotite~, Fe_{7}S_{8}, Fe . 60.5, S . 39.5.--
+
+    H = 3.5-4.5, G = 4.58-4.64.
+
+Color, bronze-yellow. Closely resembles pyrite, but may be distinguished
+from it by being feebly magnetic. Heated in an ignition tube yields no
+sublimate. Before the Bp. on Ch. fuses to a magnetic globule, which
+exhibits a yellowish crystalline structure when fractured.
+
+
+~Mispickel~, FeAsS, Fe . 34, As . 46, S . 20.--H = 5.5-6.0, G = 6.0-6.2.
+Color, silver-white. Lustre, metallic; very brittle. Often associated
+with it we find small quantities of Co, Ag, and Au. Heated in an
+ignition tube it first yields a red sublimate of sulphide of arsenic,
+and then afterward a crystalline sublimate of metallic arsenic. Before
+the Bp. on Ch. emits dense fumes of arsenic and deposits a coating on
+the coal; it then fuses to a globule which behaves like pyrrhotite.
+
+
+~Siderite~, FeCO_{3}, FeO . 62, CO_{2} . 38.--H = 3.5-4.5, G = 3.7-3.9.
+Color, grayish yellow to reddish brown. Lustre, pearly. Crystallizes in
+rhombohedrons with curved faces; these crystals are distinctly cleavable
+and massive. Heated in an ignition tube it decrepitates with evolution
+of carbon dioxide. Before the Bp. on Ch. infusible. Before the Bp. on
+Ch. with Na_{2}CO_{3} it fuses to a magnetic mass. With borax bead it
+reacts for iron and sometimes for manganese.
+
+
+ORES OF LEAD
+
+~Galena~, PbS, Pb . 87, S . 13.--
+
+    H = 2.5, G = 7.4-7.6.
+
+Color, bluish gray, slowly tarnishing. Lustre, metallic. Crystals in the
+form of cubes. Heated in an ignition tube it sometimes decrepitates and
+yields a sublimate of sulphur. Before the Bp. on Ch. easily reduced to
+the metallic state, the Ch. becoming coated with sulphate and oxide of
+lead. The metallic globule usually contains a little silver. To separate
+this, the process known as "cupellation" is employed. A hole is bored
+into the Ch. about 1 cm. in diameter and about 6 mm. deep. Into this
+hole is placed a stiff paste made by mixing finely pulverized bone-ash
+with a little soda and water. This paste is pressed in hard, and then
+the surface is smoothed off, and the centre is slightly depressed with
+the rounded end of a glass rod. The charcoal so prepared is set in a
+warm place to allow the paste to dry. When the paste is quite dry the
+small globule of lead is placed in the depression in the centre of the
+bone-ash "cupel," and is there exposed to the O. F. from the Bp. The
+lead is oxidized and is absorbed by the bone-ash, while any silver
+present will remain in the central depression as a bright shining bead.
+
+
+~Cerusite~, PbCO_{3}, PbO . 84, CO_{2} . 16.--H = 3.0-3.5, G = 6.46-6.57.
+Color, white, gray, or yellow. Lustre, adamantine. Crystallizes in
+prismatic needles. When heated in an ignition tube carbon dioxide is
+evolved and the residue turns yellow. Before the Bp. on Ch. readily
+reduced to metallic lead.
+
+
+~Anglesite~, PbSO_{4}, PbO . 74, SO_{3} . 26.--H = 2.0-3.0, G = 6.12-6.39.
+Color, yellow, gray, and brown. Lustre, adamantine, resinous. Heated in
+an ignition tube decrepitates, and sometimes yields a little water.
+Before the Bp. on Ch. fuses to a clear bead, which on cooling becomes
+opaque. Before the Bp. on Ch. with Na_{2}CO_{3} is reduced to the metal
+giving a yellow coating. The Na_{2}CO_{3} absorbed by the coal reacts
+for S.
+
+
+ORES OF MANGANESE
+
+~Pyrolusite~, MnO_{2}, Mn . 63.2, O . 36.8.--H = 2.0-2.5, G = 4.82. Color,
+iron-black to steel-gray. Lustre, non-metallic. Heated in an ignition
+tube yields generally a little water, and if the temperature be high
+enough, oxygen is evolved. Before the Bp. on Ch. infusible. In borax
+bead gives characteristic color.
+
+
+~Psilomelane~, Mn_{2}O_{3} + H_{2}O.--
+
+    H = 5.5-6.0, G = 3.7-4.7.
+
+Color, iron-black to steel-gray. Generally resembles pyrolusite, but is
+distinguished from it by its superior hardness. It frequently contains
+BaO and Li_{2}O. It behaves before the Bp. like pyrolusite.
+
+
+~Wad~ (Bog Manganese).--This mineral is essentially MnO_{2}, MnO, and
+H_{2}O, with small quantities of Fe_{2}O_{3}, Al_{2}O_{3}, BaO, SiO_{2},
+etc., associated with it.
+
+H = 0.5-6.0, G = 3.0-4.2. Color, dull black. Heated in an ignition tube
+yields water in abundance, otherwise it behaves like pyrolusite.
+
+
+ORES OF MERCURY
+
+~Native Mercury, Hg.~--G = 13.5-13.6. Color, silver-white. Is liquid at
+all ordinary temperatures. Heated in an ignition tube is volatilized,
+the vapors condensing in the upper end of tube to small metallic
+globules of Hg. Before the Bp. on Ch. it is volatilized. Frequently
+contains Ag.
+
+
+~Cinnabar~, HgS_{2}, Hg . 86, S . 14.--
+
+    H = 2.0-2.5, G = 8.0-8.2.
+
+Color, scarlet-red to brick-red. Lustre, non-metallic. When pulverized
+yields a powder of vermilion-red color. Heated in an ignition tube it
+volatilizes, yielding a black sublimate, which by friction becomes red.
+Before the Bp. on Ch. it is wholly volatilized. Heated in an ignition
+tube with Na_{2}CO_{3} metallic mercury sublimes, condensing in the
+upper portion of the tube in minute globules.
+
+
+ORES OF NICKEL
+
+~Millerite~, NiS, Ni . 64.4, S . 35.6.--
+
+    H = 3.0-3.5, G = 5.2-5.6.
+
+Color, brass-yellow. Brittle. Before the Bp. on Ch. it fuses to a
+magnetic, metallic globule. The roasted mineral gives in the borax bead
+the color reaction characteristic of nickel, and sometimes that of
+cobalt, which is often associated with it.
+
+
+~Niccolite~, NiAs, Ni . 44, As . 56.--
+
+    H = 5.0-5.5, G = 7.35-7.67.
+
+Color, pale copper-red. Lustre, metallic. Very brittle. Heated in an
+ignition tube yields a copious sublimate of arsenious oxide, the residue
+falling to a greenish powder. Before the Bp. on Ch. fuses to a white
+brittle globule emitting arsenical fumes. In borax bead gives color
+characteristic of nickel. Frequently in this mineral a portion of the
+arsenic is replaced by antimony.
+
+
+ORES OF SILVER
+
+~Native Silver, Ag.~--
+
+    H = 2.5-3.0, G = 10.1-11.0.
+
+Color, silver-white. Lustre, metallic. Ductile and malleable. Usually
+occurs associated with Au, As, Sb, Cu, Fe, etc. Before the Bp. on Ch.
+easily fuses to a globule which is surrounded with a dark red coating on
+the coal.
+
+
+~Argentite~, Ag_{2}S, Ag . 87.1, S . 12.9.--
+
+    H = 2.0-2.5, G = 7.20-7.36.
+
+Color, blackish lead-gray. Lustre, metallic. Very sectile. Before the
+Bp. on Ch. in O. F. intumesces with evolution of sulphur dioxide,
+finally yielding a metallic globule of Ag.
+
+
+~Pyrargyrite~, Ag_{3}SbS_{3}, Ag . 59.8, Sb . 22.5, S . 17.7.--H = 2.5, G
+= 5.77-5.86. Color, black to dark cochineal-red. Lustre, metallic,
+adamantine. In an ignition tube it yields on continued heating a
+sublimate of antimony sulphide. Before the Bp. on Ch. it gives a coating
+of antimony trioxide. Before the Bp. on Ch. with Na_{2}CO_{3} is
+reduced to metallic silver.
+
+
+~Proustite~, Ag_{3}S_{3}As, Ag . 65.5, As . 15.1, S . 19.4.--H = 2.0-2.5,
+G = 5.57-5.64. Color, light red. Lustre, splendent, adamantine. Before
+the Bp. on Ch. it behaves like pyrargyrite, save that it gives off
+arsenical fumes instead of antimonious oxide.
+
+
+~Stephanite~, Ag_{5}S_{4}Sb, Ag . 68.5, Sb . 15.3, S . 16.2.--H = 2.0-2.5,
+G = 6.2-6.3. Color, iron-black to blackish gray. Lustre, metallic. Very
+brittle and fragile. In an ignition tube it decrepitates, fuses, and
+finally yields a slight sublimate of antimony trisulphide. Before the
+Bp. on Ch. gives a coating of antimonious oxide. Before the Bp. on Ch.
+with Na_{2}CO_{3} a globule of metallic silver is obtained. The mineral
+frequently contains copper and iron.
+
+
+~Kerargyrite~, AgCl, Ag . 75.3, Cl . 24.7.--H = 1.0-1.5, G = 5.52. Color,
+white, gray, yellowish, greenish to blue. Lustre, resinous, adamantine.
+Soft like wax. Fuses easily in a candle-flame. Before the Bp. on Ch. it
+is readily reduced to metallic silver.
+
+
+ORES OF TIN
+
+~Cassiterite~, SnO_{2}, Sn . 79, O . 21.--
+
+    H = 6.0-7.0, G = 6.8-7.0.
+
+Color, brown, black. Lustre, adamantine, brilliant. Occurs crystallized
+in square prisms. Reëntrant angles characteristic. Before the Bp. on Ch.
+with Na_{2}CO_{3} and KCN reduced to a metallic globule of tin. In the
+borax bead gives characteristic reaction.
+
+
+~Stannite~, 2 Cu_{2}S . SnS_{2} + 2 (FeS . ZnS) Sn . S_{2}.--H = 4.0, G =
+4.3-4.5. Color, steel-gray to iron-black. Lustre, metallic. Occurs
+usually massive and disseminated. Heated in an ignition tube it yields
+sulphur dioxide. Before the Bp. on Ch. it emits sulphur dioxide and
+becomes covered with oxide of tin. Before the Bp. on Ch. with
+Na_{2}CO_{3} and KCN it gives an impure globule of copper. A very
+difficult mineral to determine.
+
+
+ORES OF ZINC
+
+~Calamine~, H_{2}Zn_{2}O_{5}Si, SiO_{2} . 25.0, ZnO . 67.5, H_{2}O .
+7.5.--H = 4.5-5.0, G = 3.4-3.5. Color, white, gray, bluish, or brown.
+Lustre, vitreous. Brittle. In an ignition tube yields water when heated
+and becomes milky white. Before the Bp. on Ch. practically infusible.
+With Co(NO_{3})_{2} it assumes a green color which passes into a fine
+blue when the heat is increased.
+
+
+~Smithsonite~,
+
+    Zn . CO_{3}, ZnO . 64.8, CO_{2} . 35.2.--
+
+H = 5, G = 4.30-4.45. Color, gray, yellow, brown, and green. Lustre,
+vitreous, pearly. Heated in an ignition tube CO_{2} is evolved, residue
+appearing white. It often contains impurities of Cd, Pb, Fe, Mn, Ca, and
+Mg. When these are present the residue in the ignition tube becomes dark
+on cooling. Before the Bp. on Ch. with Na_{2}CO_{3} and exposed to the
+R. F. it is decomposed. It gives the characteristic reaction for zinc
+with Co(NO_{3})_{2}.
+
+
+~Zincite~, ZnO, Zn . 80.3, O . 19.7--
+
+    H = 4.0-4.5, G = 5.43-5.70.
+
+Color, blood-red. Lustre, brilliant, subadamantine. Before the Bp. on
+Ch. infusible. Before the Bp. on Ch. with Na_{2}CO_{3} gives coating of
+zinc oxide. Gives characteristic reaction with Co(NO_{3})_{2}. It
+frequently contains a small quantity of Mn_{2}O_{3}, which may be
+detected in the borax bead.
+
+
+~Sphalerite~, ZnS, Zn . 67, S . 33.--
+
+    H = 3.5-4.0, G = 3.9-4.1.
+
+Color, yellow to black. Lustre, resinous, brilliant, and sometimes
+submetallic. Heated in an ignition tube sometimes decrepitates. Before
+the Bp. on Ch. infusible. Before the Bp. on Ch. with Na_{2}CO_{3} easily
+reduced. With Co(NO_{3})_{2} gives the characteristic reaction. It
+frequently contains small quantities of Cd, Hg, Sn, Pb, Au, Ag, etc.
+
+
+I
+
+TABLE OF COLORS OF COATINGS ON CHARCOAL
+
+--------------------------------------------------
+ Element |    Color Hot           | Color Cold    |
+---------|------------------------|---------------|
+Antimony | (Rather volatile)      | White         |
+         |                        |               |
+Arsenic  | (Very volatile)        | White         |
+         |                        |               |
+Bismuth  | Orange-Yellow          | Lemon-Yellow  |
+         |                        |               |
+Cadmium  | Brownish Yellow        | Reddish Brown |
+         |                        |               |
+Lead     | Lemon-Yellow (volatile)| Lemon-Yellow  |
+         |                        |               |
+Silver   | Dark Red               | Dark Red      |
+         |                        |               |
+Tin      | Faint Yellow           | White         |
+         |                        |               |
+Zinc     | Yellow                 | White         |
+--------------------------------------------------
+
+
+II
+
+TABLE OF FLAME COLORATIONS
+
+------------------------------------
+  Red        |  Yellow  |  Green    |
+-------------|----------|-----------|
+Calcium      |  Sodium  |  Barium   |
+             |          |           |
+Lithium      |          |  Boron    |
+             |          |           |
+Strontium    |          |  Iodine   |
+-------------|----------|-----------|
+Bluish Green | Blue     |   Violet  |
+-------------|----------|-----------|
+Bromine      | Chlorine | Potassium |
+             |          |           |
+Copper       |          |           |
+             |          |           |
+Phosphorus   |          |           |
+------------------------------------
+
+
+III
+
+TABLE OF COLORS OF BORAX BEADS IN OXIDIZING FLAME
+
+---------------------------------------------------------
+ Element |    Color Hot           |    Color Cold       |
+---------|------------------------|---------------------|
+Aluminum |  Colorless to Cloudy   | Colorless to Cloudy |
+         |                        |                     |
+Antimony |  Yellowish             | Colorless           |
+         |                        |                     |
+Barium   | Colorless to Opaque    | Colorless to Opaque |
+         |                        |                     |
+Bismuth  | Yellow                 | Colorless           |
+         |                        |                     |
+Cadmium  | Yellow                 | Colorless to White  |
+         |                        |                     |
+Calcium  | Colorless              | Colorless           |
+         |                        |                     |
+Chromium | Reddish Yellow         | Yellowish Green     |
+         |                        |                     |
+Cobalt   | Blue                   | Blue                |
+         |                        |                     |
+Copper   | Green                  | Greenish Blue       |
+         |                        |                     |
+Iron     | Orange                 | Yellow              |
+         |                        |                     |
+Lead     | Yellow                 | Colorless           |
+         |                        |                     |
+Magnesium| Colorless              | Colorless           |
+         |                        |                     |
+Manganese| Violet                 | Reddish Violet      |
+         |                        |                     |
+Nickel   | Violet                 | Reddish Brown       |
+         |                        |                     |
+Silver   | Colorless              | Milk-White          |
+         |                        |                     |
+Strontium| Colorless to Opaque    | Colorless to Opaque |
+         |                        |                     |
+Tin      | Colorless              | Colorless           |
+         |                        |                     |
+Zinc     | Yellowish              | Colorless           |
+---------------------------------------------------------
+
+
+IV
+
+TABLE OF COLORS OF BORAX BEADS IN REDUCING FLAME
+
+------------------------------------------------
+Element    | Color Hot       | Color Cold      |
+------------------------------------------------
+Aluminum   | Colorless       | Colorless       |
+           |                 |                 |
+Antimony   | Colorless       | Cloudy          |
+           |                 |                 |
+Barium     | Colorless       | Colorless       |
+           |                 |                 |
+Bismuth    | Colorless       | Gray--Cloudy    |
+           |                 |                 |
+Cadmium    | Colorless       | Gray--Cloudy    |
+           |                 |                 |
+Calcium    | Colorless       | Colorless       |
+           |                 |                 |
+Chromium   | Green           | Green           |
+           |                 |                 |
+Cobalt     | Blue            | Blue            |
+           |                 |                 |
+Copper     | Colorless       | Red             |
+           |                 |                 |
+Iron       | Yellowish Green | Yellowish Green |
+           |                 |                 |
+Lead       | Colorless       | Gray            |
+           |                 |                 |
+Magnesium  | Colorless       | Colorless       |
+           |                 |                 |
+Manganese  | Colorless       | Pink            |
+           |                 |                 |
+Nickel     | Colorless       | Gray--Cloudy    |
+           |                 |                 |
+Silver     | Colorless       | Gray            |
+           |                 |                 |
+Strontium  | Colorless       | Colorless       |
+           |                 |                 |
+Tin        | Colorless       | Colorless       |
+           |                 |                 |
+Zinc       | Colorless       | Gray            |
+------------------------------------------------
+
+
+V
+
+TABLE OF COLORS OF MICROCOSMIC SALT BEADS IN OXIDIZING FLAME
+
+---------------------------------------------------
+ Element  |  Color Hot        | Color Cold         |
+---------------------------------------------------|
+Aluminum  | Colorless         | Colorless          |
+          |                   |                    |
+Antimony  | Yellowish         | Colorless          |
+          |                   |                    |
+Barium    |Colorless to Opaque| Colorless to Opaque|
+          |                   |                    |
+Bismuth   | Yellow            | Colorless          |
+          |                   |                    |
+Cadmium   | Yellowish         | Colorless          |
+          |                   |                    |
+Calcium   | Colorless         | Colorless to Opaque|
+          |                   |                    |
+Chromium  | Reddish           | Green              |
+          |                   |                    |
+Cobalt    | Blue              | Blue               |
+          |                   |                    |
+Copper    | Green             | Greenish Blue      |
+          |                   |                    |
+Iron      | Red               | Brownish Red       |
+          |                   |                    |
+Lead      | Yellowish         | Colorless          |
+          |                   |                    |
+Magnesium | Colorless         | Colorless          |
+          |                   |                    |
+Manganese | Brownish Violet   | Reddish Violet     |
+          |                   |                    |
+Nickel    | Reddish           | Yellow             |
+          |                   |                    |
+Silver    | Yellowish         | Yellowish          |
+          |                   |                    |
+Strontium | Colorless         | Colorless          |
+          |                   |                    |
+Tin       | Colorless         | Colorless          |
+          |                   |                    |
+Zinc      | Yellowish         | Colorless          |
+---------------------------------------------------
+
+
+VI
+
+TABLE OF COLORS OF MICROCOSMIC SALT BEADS IN REDUCING FLAME
+
++-----------+-------------+--------------+
+|  Element  |  Color Hot  |  Color Cold  |
+|-----------+-------------+--------------+
+| Aluminum  | Colorless   | Colorless    |
+|           |             |              |
+| Antimony  | Colorless   | Gray--Cloudy |
+|           |             |              |
+| Barium    | Colorless   | Colorless    |
+|           |             |              |
+| Bismuth   | Colorless   | Gray--Cloudy |
+|           |             |              |
+| Cadmium   | Colorless   | Gray--Cloudy |
+|           |             |              |
+| Calcium   | Colorless   | Colorless    |
+|           |             |              |
+| Chromium  | Reddish     | Green        |
+|           |             |              |
+| Cobalt    | Blue        | Blue         |
+|           |             |              |
+| Copper    | Dark Green  | Brownish Red |
+|           |             |              |
+| Iron      | Red         | Reddish      |
+|           |             |              |
+| Lead      | Colorless   | Gray--Opaque |
+|           |             |              |
+| Magnesium | Colorless   | Colorless    |
+|           |             |              |
+| Manganese | Colorless   | Colorless    |
+|           |             |              |
+| Nickel    | Colorless   | Gray         |
+|           |             |              |
+| Silver    | Colorless   | Gray         |
+|           |             |              |
+| Strontium | Colorless   | Colorless    |
+|           |             |              |
+| Tin       | Colorless   | Colorless    |
+|           |             |              |
+| Zinc      | Colorless   | Gray--Cloudy |
+------------+-------------+--------------+
+
+
+THE PRACTICAL METHODS
+
+OF
+
+ORGANIC CHEMISTRY
+
+AUTHORIZED TRANSLATION
+
+12mo. Cloth. Price, $1.60, _net_
+
+    BY                                            TRANSLATED BY
+    LUDWIG GATTERMANN, Ph.D.,                 WILLIAM SHAFER, Ph.D.,
+    _Professor in University_   _Instructor in Organic Chemistry_
+    _of Heidelberg._                       _in Lehigh University._
+
+       *       *       *       *       *
+
+THE GUARDIAN.
+
+     "The selection and judgment throughout is excellent. The
+     book is a most useful, practical adjunct to any good
+     text-book on organic chemistry."
+
+PHARMACEUTICAL REVIEW.
+
+     "This is a book that should be in the library of every
+     teacher of organic chemistry, and one which will no doubt be
+     of great value to students in their second year of organic
+     chemistry. Its chief peculiarity and merit is in the great
+     stress laid on practical laboratory work.... It is
+     permanently a worker's guide."
+
+NATURE.
+
+     "Since the advance of organic chemistry in this country
+     must, in a measure, depend on the nature of the available
+     text-books, both the author and the translator deserve our
+     thanks for providing us with a work such as the present
+     one."
+
+       *       *       *       *       *
+
+PUBLISHED BY
+THE MACMILLAN COMPANY
+66 FIFTH AVENUE, NEW YORK
+
+
+OUTLINES
+
+OF
+
+INDUSTRIAL CHEMISTRY
+
+A TEXT-BOOK FOR STUDENTS
+
+By FRANK HALL THORP, Ph.D.,
+
+_Instructor in Industrial Chemistry in the Massachusetts Institute of
+Technology._
+
+Cloth. 8vo. Price, $3.50 _net_
+
+       *       *       *       *       *
+
+JAMES LEWIS HOWE,
+
+_Department of Chemistry, Washington and Lee University._
+
+     "The book is brought thoroughly up to date, and in some
+     cases the lines of probable development are nicely
+     foreshadowed. The descriptions are particularly lucid and
+     the illustrations well selected.
+
+     The general arrangement and make-up of the book is
+     excellent, and ... altogether the book fills well a need
+     long felt by teachers of Industrial Chemistry.
+
+     I shall adopt the book for my class and shall take pleasure
+     in recommending it."
+
+CHARLES E. COATES, Jr., Ph.D.,
+
+_Professor of Chemistry, Louisiana State University._
+
+     "I have examined it carefully and think it a most excellent
+     book, meeting a want I have long felt in my higher classes.
+     I have introduced it in this year's classes."
+
+W. A. NOYES, in _Science_.
+
+     "The descriptions of processes, while necessarily concise,
+     are clear and interesting. The author has evidently made a
+     careful study of recent methods of manufacture as well as of
+     older, standard processes. The frequent reference to
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+  <head>
+    <meta http-equiv="Content-Type" content="text/html;charset=iso-8859-1" />
+    <title>
+      The Project Gutenberg eBook of The Elements Of Blowpipe Analysis, by Frederick Hutton Getman, F.C.S..
+    </title>
+    <style type="text/css">
+
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+<pre>
+
+The Project Gutenberg EBook of The Elements of Blowpipe Analysis, by 
+Frederick Hutton Getman
+
+This eBook is for the use of anyone anywhere at no cost and with
+almost no restrictions whatsoever.  You may copy it, give it away or
+re-use it under the terms of the Project Gutenberg License included
+with this eBook or online at www.gutenberg.org
+
+
+Title: The Elements of Blowpipe Analysis
+
+Author: Frederick Hutton Getman
+
+Release Date: June 25, 2010 [EBook #32974]
+
+Language: English
+
+Character set encoding: ISO-8859-1
+
+*** START OF THIS PROJECT GUTENBERG EBOOK THE ELEMENTS OF BLOWPIPE ANALYSIS ***
+
+
+
+
+Produced by The Online Distributed Proofreading Team at
+https://www.pgdp.net. (This file was produced from images
+generously made available by The Internet Archive/American
+Libraries.)
+
+
+
+
+
+
+</pre>
+
+
+
+
+<h1>THE ELEMENTS OF BLOWPIPE ANALYSIS</h1>
+
+
+<hr style="width: 65%;" />
+<h4>THE</h4>
+
+<h2>ELEMENTS OF BLOWPIPE</h2>
+
+<h2>ANALYSIS</h2>
+
+<h4>BY</h4>
+
+<h2>FREDERICK HUTTON GETMAN, F.C.S.</h2>
+
+<h3>INSTRUCTOR IN CHEMISTRY IN THE STAMFORD HIGH SCHOOL</h3>
+
+<p class="center">
+New York<br />
+THE MACMILLAN COMPANY<br />
+LONDON: MACMILLAN &amp; CO., LTD.<br />
+1899<br />
+<br />
+<i>All rights reserved</i><br />
+<br />
+<br />
+<span class="smcap">Copyright, 1899</span>,<br />
+<br />
+<span class="smcap">By</span> THE MACMILLAN COMPANY.<br />
+<br />
+Norwood Press<br />
+J. S. Cushing &amp; Co.&mdash;Berwick &amp; Smith<br />
+Norwood Mass. U.S.A.<br />
+</p>
+
+
+
+<hr style="width: 65%;" /><p><span class='pagenum'><a name="Page_v" id="Page_v">[Pg v]</a></span></p>
+<h2>PREFACE</h2>
+
+
+<p>These few pages are intended to serve a twofold purpose,&mdash;to give the
+student a general outline of Blowpipe Analysis, and to introduce him to
+the methods of Determinative Mineralogy.</p>
+
+<p>Every effort has been made to simplify details so that the book may be
+used in both High Schools and Colleges.</p>
+
+<p>Tables for "systematic" examination have been intentionally omitted, for
+in the author's estimation these tend to dull the student's power of
+observation, and to make him place little value upon minute details.</p>
+
+<p>The alphabetic arrangement has been followed for the sake of convenience
+when referring to the book.<span class='pagenum'><a name="Page_vi" id="Page_vi">[Pg vi]</a></span></p>
+
+<p>The last chapter is not intended to serve as a key to determining the
+minerals therein described, but rather it is added to give the student
+exercise in Blowpipe Analysis, and at the same time to point out the
+<i>methods</i> of Determinative Mineralogy.</p>
+
+<p>Finally, the author would acknowledge his indebtedness to the following
+works: "Manual of Qualitative Analysis," Fresenius; "Qualitative
+Chemical Analysis," Venable; Roscoe and Schorlemmer's "Treatise on
+Chemistry"; Foye's "Hand-Book of Mineralogy"; Dana's "Mineralogy";
+Kobell's "Tafeln zur Bestimmung der Mineralien"; etc.</p>
+
+<p class="right">
+<span class="smcap">Frederick Hutton Getman.</span><br />
+<br />
+<span class="smcap">Stamford, Conn.</span>,<br />
+<br />
+Feb. 22, 1899.<br />
+</p>
+
+
+
+<hr style="width: 65%;" /><p><span class='pagenum'><a name="Page_vii" id="Page_vii">[Pg vii]</a></span></p>
+<h2>TABLE OF CONTENTS</h2>
+
+
+<p>
+CHAPTER I<br />
+<span class="tocnum">PAGE</span><br />
+Apparatus and Reagents                                       <span class="tocnum"><a href='#Page_1'>1</a>-7</span><br />
+<br />
+<br />
+CHAPTER II<br />
+<br />
+General Outline of Blowpipe Analysis                           <span class="tocnum"><a href='#Page_8'>8</a></span><br />
+<br />
+Definitions                                                    <span class="tocnum"><a href='#Page_9'>9</a></span><br />
+<br />
+Examination on Charcoal Alone                                 <span class="tocnum"><a href='#Page_10'>10</a></span><br />
+<br />
+Examination on Charcoal with Sodium Carbonate                 <span class="tocnum"><a href='#Page_13'>13</a></span><br />
+<br />
+Examination in Tube with Sodium Carbonate and Charcoal        <span class="tocnum"><a href='#Page_15'>15</a></span><br />
+<br />
+Examination on Platinum Wire                                  <span class="tocnum"><a href='#Page_16'>16</a></span><br />
+<br />
+Examination in Borax Bead                                     <span class="tocnum"><a href='#Page_17'>17</a></span><br />
+<br />
+Examination with Cobalt Nitrate                               <span class="tocnum"><a href='#Page_20'>20</a></span><br />
+<br />
+<br />
+CHAPTER III<br />
+<br />
+General Reactions for the Detection of the Metallic
+Elements in Simple Compounds                                  <span class="tocnum"><a href='#Page_22'>22</a></span><br />
+<br />
+Aluminum                                                      <span class="tocnum"><a href='#Page_23'>23</a></span><br />
+<br />
+Antimony                                                      <span class="tocnum"><a href='#Page_24'>24</a></span><br />
+<br />
+Arsenic                                                       <span class="tocnum"><a href='#Page_25'>25</a></span><br />
+<br />
+Bismuth                                                       <span class="tocnum"><a href='#Page_25'>25</a></span><br />
+<br />
+Cadmium                                                       <span class="tocnum"><a href='#Page_26'>26</a></span><br />
+<br />
+Chromium                                                      <span class="tocnum"><a href='#Page_26'>26</a></span><br />
+<br />
+<span class='pagenum'><a name="Page_viii" id="Page_viii">[Pg viii]</a></span>Cobalt                                                        <span class="tocnum"><a href='#Page_27'>27</a></span><br />
+<br />
+Copper                                                        <span class="tocnum"><a href='#Page_28'>28</a></span><br />
+<br />
+Iron                                                          <span class="tocnum"><a href='#Page_28'>28</a></span><br />
+<br />
+Lead                                                          <span class="tocnum"><a href='#Page_29'>29</a></span><br />
+<br />
+Manganese                                                     <span class="tocnum"><a href='#Page_30'>30</a></span><br />
+<br />
+Mercury                                                       <span class="tocnum"><a href='#Page_30'>30</a></span><br />
+<br />
+Nickel                                                        <span class="tocnum"><a href='#Page_31'>31</a></span><br />
+<br />
+Silver                                                        <span class="tocnum"><a href='#Page_32'>32</a></span><br />
+<br />
+Tin                                                           <span class="tocnum"><a href='#Page_32'>32</a></span><br />
+<br />
+Zinc                                                          <span class="tocnum"><a href='#Page_33'>33</a></span><br />
+<br />
+The Alkali Metals                                             <span class="tocnum"><a href='#Page_34'>34</a></span><br />
+<br />
+Ammonium                                                      <span class="tocnum"><a href='#Page_34'>34</a></span><br />
+<br />
+Potassium                                                     <span class="tocnum"><a href='#Page_35'>35</a></span><br />
+<br />
+Sodium                                                        <span class="tocnum"><a href='#Page_35'>35</a></span><br />
+<br />
+Lithium                                                       <span class="tocnum"><a href='#Page_36'>36</a></span><br />
+<br />
+The Alkaline Earths                                           <span class="tocnum"><a href='#Page_36'>36</a></span><br />
+<br />
+Barium                                                        <span class="tocnum"><a href='#Page_36'>36</a></span><br />
+<br />
+Calcium                                                       <span class="tocnum"><a href='#Page_37'>37</a></span><br />
+<br />
+Strontium                                                     <span class="tocnum"><a href='#Page_37'>37</a></span><br />
+<br />
+The Acid Elements                                             <span class="tocnum"><a href='#Page_37'>37</a></span><br />
+<br />
+Borates                                                       <span class="tocnum"><a href='#Page_37'>37</a></span><br />
+<br />
+Bromides                                                      <span class="tocnum"><a href='#Page_38'>38</a></span><br />
+<br />
+Chlorides                                                     <span class="tocnum"><a href='#Page_38'>38</a></span><br />
+<br />
+Fluorides                                                     <span class="tocnum"><a href='#Page_38'>38</a></span><br />
+<br />
+Iodides                                                       <span class="tocnum"><a href='#Page_39'>39</a></span><br />
+<br />
+Nitrates                                                      <span class="tocnum"><a href='#Page_39'>39</a></span><br />
+<br />
+Phosphates                                                    <span class="tocnum"><a href='#Page_40'>40</a></span><br />
+<br />
+Silicates                                                     <span class="tocnum"><a href='#Page_40'>40</a></span><br />
+<br />
+<span class='pagenum'><a name="Page_ix" id="Page_ix">[Pg ix]</a></span>Sulphides                                                     <span class="tocnum"><a href='#Page_41'>41</a></span><br />
+<br />
+<br />
+CHAPTER IV<br />
+<br />
+Behavior of Some of the Principal Ores before the Blowpipe    <span class="tocnum"><a href='#Page_43'>43</a></span><br />
+<br />
+Ores of Antimony                                              <span class="tocnum"><a href='#Page_46'>46</a></span><br />
+<br />
+Ores of Arsenic                                               <span class="tocnum"><a href='#Page_47'>47</a></span><br />
+<br />
+Ores of Bismuth                                               <span class="tocnum"><a href='#Page_48'>48</a></span><br />
+<br />
+Ores of Chromium                                              <span class="tocnum"><a href='#Page_49'>49</a></span><br />
+<br />
+Ores of Cobalt                                                <span class="tocnum"><a href='#Page_50'>50</a></span><br />
+<br />
+Ores of Copper                                                <span class="tocnum"><a href='#Page_52'>52</a></span><br />
+<br />
+Ores of Iron                                                  <span class="tocnum"><a href='#Page_57'>57</a></span><br />
+<br />
+Ores of Lead                                                  <span class="tocnum"><a href='#Page_60'>60</a></span><br />
+<br />
+Ores of Manganese                                             <span class="tocnum"><a href='#Page_63'>63</a></span><br />
+<br />
+Ores of Mercury                                               <span class="tocnum"><a href='#Page_64'>64</a></span><br />
+<br />
+Ores of Nickel                                                <span class="tocnum"><a href='#Page_65'>65</a></span><br />
+<br />
+Ores of Silver                                                <span class="tocnum"><a href='#Page_66'>66</a></span><br />
+<br />
+Ores of Tin                                                   <span class="tocnum"><a href='#Page_69'>69</a></span><br />
+<br />
+Ores of Zinc                                                  <span class="tocnum"><a href='#Page_70'>70</a></span><br />
+<br />
+<br />
+COMPARATIVE TABLES<br />
+<br />
+I. Colors of Coatings on Charcoal                             <span class="tocnum"><a href='#Page_73'>73</a></span><br />
+<br />
+II. Flame Colorations                                         <span class="tocnum"><a href='#Page_73'>73</a></span><br />
+<br />
+III. Colors of Borax Beads in oxidizing Flame                 <span class="tocnum"><a href='#Page_74'>74</a></span><br />
+<br />
+IV. Colors of Borax Beads in reducing Flame                   <span class="tocnum"><a href='#Page_75'>75</a></span><br />
+<br />
+V. Colors of Microcosmic Salt Beads in oxidizing Flame        <span class="tocnum"><a href='#Page_76'>76</a></span><br />
+<br />
+VI. Colors of Microcosmic Salt Beads in reducing Flame        <span class="tocnum"><a href='#Page_77'>77</a></span><br />
+</p>
+
+
+
+<hr style="width: 65%;" /><p><span class='pagenum'><a name="Page_x" id="Page_x">[Pg x]</a></span></p>
+<div class="figcenter" style="width: 650px;">
+<img src="images/fig1.jpg" width="650" height="950" alt="" title="" />
+</div>
+
+
+
+<hr style="width: 65%;" /><p><span class='pagenum'><a name="Page_1" id="Page_1">[Pg 1]</a></span></p>
+<h2>BLOWPIPE ANALYSIS</h2>
+
+
+
+<hr style="width: 65%;" />
+<h2>CHAPTER I</h2>
+
+
+<p>The blowpipe was first applied to mineral analysis in 1733 by Anton
+Swab, and its applications have since been improved and extended by
+various chemists, among whom may be mentioned Bergmann, Cronstedt, Gahn,
+Berzelius, and Plattner.</p>
+
+
+<p><b>Blowpipe.</b>&mdash;The common blowpipe of the jeweller is not particularly well
+suited to the operations of blowpipe analysis, since the flame has often
+to be kept playing upon the assay for some time, and the condensed
+moisture of the breath would seriously interfere with the passage of
+the<span class='pagenum'><a name="Page_2" id="Page_2">[Pg 2]</a></span> air through the jet. One of the best and least expensive forms of
+blowpipe is shown in Fig. 1. This consists, as is seen from the
+illustration, of a conical-shaped tube of tin closed at the wide end and
+formed into a mouthpiece at the small end; soldered into the tube at the
+large end, and at right angles to its axis, is a small brass tube which
+terminates in a conical tip pierced with a very fine hole. With this
+pipe it is possible to perform all of the operations of mineral
+analysis.</p>
+
+<p>Some little practice is necessary to keep the flame steady and to take
+the breath at the same time.</p>
+
+<p>No rule can well be given to the beginner, but his experience becomes
+his best guide.</p>
+
+
+<p><b>Bunsen Flame.</b>&mdash;Any kind of flame can be used for the blowpipe, provided
+it be<span class='pagenum'><a name="Page_3" id="Page_3">[Pg 3]</a></span> not too small; but since almost every laboratory to-day is
+furnished with gas and the Bunsen burner (Fig. 2), it will only be
+necessary to describe the use of the flame from this source. Upon
+examining the Bunsen flame with care, it will be seen that the flame
+consists of three distinct parts.</p>
+
+<p>A dark inner cone which consists of gas not yet raised to the ignition
+point. Beyond this there is a luminous cone, where combustion is
+incomplete owing to lack of oxygen, and outside of this we find the
+non-luminous cone where the gas is completely burned.</p>
+
+<p>This outer envelope is the hottest portion of the flame, and is known as
+the "oxidizing" flame because there is an excess of oxygen which is
+imparted to substances placed therein.</p>
+
+<p>The luminous cone is known as the "reducing" flame, for in it metallic
+oxides<span class='pagenum'><a name="Page_4" id="Page_4">[Pg 4]</a></span> are reduced, the oxygen being taken up by the small incandescent
+particles of carbon.</p>
+
+<p>If the air-holes at the base of the Bunsen burner be opened, the two
+inner cones become elongated, and the flame appears almost colorless.</p>
+
+<p>The blowpipe enables us to get an oxidizing and a reducing flame of
+better form and greater power. To do this we cut off the air supply at
+the base of the burner and turn off the gas until the flame is about 1
+cm. high; then upon introducing the blowpipe, and blowing a strong
+continuous jet of air across the Bunsen flame, we produce an oxidizing
+flame about 4-5 cm. in length. If the tip of the blowpipe be held
+outside of the Bunsen flame, and the pressure of the stream of air be
+diminished, we obtain a reducing flame.<span class='pagenum'><a name="Page_5" id="Page_5">[Pg 5]</a></span></p>
+
+
+<p><b>Supports.</b>&mdash;For supports, charcoal, platinum, and glass are chiefly used.
+The charcoal should be made from some light wood, such as alder. It
+should be well burnt, and should not scintillate or smoke.</p>
+
+<p>The platinum supports are generally in the form of wire and foil.
+Platinum-tipped forceps are frequently employed in blowpipe analysis.</p>
+
+<p>Glass is used in the form of tubing.</p>
+
+<p>Hard glass tubing, 3 mm. bore, is drawn off into ignition tubes 7-8 cm.
+in length. Several dozen of these tubes should be made before commencing
+the tests of the next chapter.</p>
+
+
+<p><b>Apparatus.</b>&mdash;A small agate mortar, 4-5 cm. in diameter, should be
+provided in which to grind the samples to be examined.</p>
+
+<p>The pestle, which should also be of agate,<span class='pagenum'><a name="Page_6" id="Page_6">[Pg 6]</a></span> must be adapted to the
+mortar in shape and size.</p>
+
+<p>Two pairs of forceps will also be needed.</p>
+
+<p>One pair should be of steel, and the other pair of brass, with fine
+points.</p>
+
+<p>Of other apparatus, the most necessary is:&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">A small hammer and anvil.<br /></span>
+</div><div class="stanza">
+<span class="i0">Two three-cornered files.<br /></span>
+</div><div class="stanza">
+<span class="i0">Small piece of cobalt glass, about 5 &times; 10 cm.<br /></span>
+</div><div class="stanza">
+<span class="i0">Pocket magnifying lens.<br /></span>
+</div><div class="stanza">
+<span class="i0">Several small watch glasses&mdash;for metallic beads, etc.<br /></span>
+</div></div>
+
+
+<p><b>Chemicals.</b>&mdash;A list of the principal chemicals is here given:&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">Sodium carbonate, Na<sub>2</sub>CO<sub>3</sub>.<br /></span>
+</div><div class="stanza">
+<span class="i0">Borax, Na<sub>2</sub>B<sub>4</sub>O<sub>7</sub> + 10 H<sub>2</sub>O.<br /></span>
+</div><div class="stanza">
+<span class='pagenum'><a name="Page_7" id="Page_7">[Pg 7]</a></span><span class="i0">Microcosmic salt, (HNaNH<sub>4</sub>), PO<sub>4</sub> + 8 H<sub>2</sub>O.<br /></span>
+</div><div class="stanza">
+<span class="i0">Cobalt nitrate, Co(NO<sub>3</sub>)<sub>2</sub> + 5 H<sub>2</sub>O.<br /></span>
+</div><div class="stanza">
+<span class="i0">Potassium cyanide, KCN.<br /></span>
+</div><div class="stanza">
+<span class="i0">Hydrochloric acid, (dilute), HCl + nH<sub>2</sub>O.<br /></span>
+</div><div class="stanza">
+<span class="i0">Litmus paper, red and blue.<br /></span>
+</div><div class="stanza">
+<span class="i0">Brazil-wood paper.<br /></span>
+</div></div>
+
+<p>Any other special reagents which may be needed will be mentioned as
+required.</p>
+
+
+
+<hr style="width: 65%;" /><p><span class='pagenum'><a name="Page_8" id="Page_8">[Pg 8]</a></span></p>
+<h2>CHAPTER II</h2>
+
+<h3>GENERAL OUTLINE OF BLOWPIPE ANALYSIS</h3>
+
+
+<div class="blockquot"><p>[<span class="smcap">ABBREVIATIONS</span>: O. F. for oxidizing flame, R. F. for
+reducing flame, Ch. for charcoal, Ct. for coating, Bp. for
+blowpipe.]</p></div>
+
+<p>In order to examine a substance before the blowpipe to determine the
+presence or absence of certain elements, it becomes necessary to arrange
+a systematic method. As with all branches of chemical work, one's
+success is largely dependent upon neatness of manipulation and
+carefulness of observation.</p>
+
+<p>The following order of observation is essentially that given by
+Berzelius:&mdash;</p>
+
+<div class="blockquot"><p>1. Examination on charcoal by itself.</p>
+
+<p><span class='pagenum'><a name="Page_9" id="Page_9">[Pg 9]</a></span>2. Examination on charcoal with Na<sub>2</sub>CO<sub>3</sub>.</p>
+
+<p>3. Examination in ignition tube with Na<sub>2</sub>CO<sub>3</sub> and
+charcoal.</p>
+
+<p>4. Examination on platinum wire.</p>
+
+<p>5. Examination in borax bead.</p>
+
+<p>6. Examination with Co(NO<sub>3</sub>)<sub>2</sub>.</p></div>
+
+<p>After having examined a body in these six different ways, we shall be
+able to say what are its principal constituents.</p>
+
+<p>Before describing the method of carrying out these six different
+operations, it will be necessary to give a few definitions of terms
+which we shall have frequent occasion to employ.</p>
+
+
+<p><b>Definitions.</b>&mdash;<i>Ignition</i> is the heating of a substance to a high
+temperature.</p>
+
+<p><i>Fusion</i> is the heating of a substance to the melting-point.</p>
+
+<p><i>Intumescence</i> is the swelling of the substance upon heating.<span class='pagenum'><a name="Page_10" id="Page_10">[Pg 10]</a></span></p>
+
+<p><i>Decrepitation</i> is the crackling of a substance due to the sudden
+expansion of combined water upon heating.</p>
+
+<p><i>Deflagration</i> is the burning of a substance with explosive violence,
+generally due to excess of oxygen.</p>
+
+<p><i>Incandescence</i> is the white light emitted by a substance that is
+infusible when subjected to a high temperature.</p>
+
+
+<p><b>Examination on Charcoal alone.</b>&mdash;The size of the assay should be about
+that of a mustard seed. This is sufficiently large to show all of the
+reactions clearly, and though a larger piece would exhibit the
+characteristic phenomena, yet much more effort is required. A very
+small, shallow hole should be cut in the Ch. to receive the assay. The
+Bp. flame should be directed at an angle of about 30&deg; with the surface
+of the Ch. Considerable care must be taken lest the hole in<span class='pagenum'><a name="Page_11" id="Page_11">[Pg 11]</a></span> the Ch. is
+burned too deep and the assay lost in the coal.</p>
+
+<p>The force of the air from the jet must also be borne in mind for a
+strong blast, or sudden puffs may blow the substance away.</p>
+
+<p>The following changes are to be looked for:&mdash;</p>
+
+<p><i>a.</i> Whether the substance is volatile or non-volatile.</p>
+
+<p><i>Illustrations.</i> Examine before the Bp. on Ch. some arsenious oxide,
+As<sub>2</sub>O<sub>3</sub>, also some alumina, Al<sub>2</sub>O<sub>3</sub>.</p>
+
+<p><i>b.</i> Whether the substance is fusible or infusible.</p>
+
+<p><i>Illustrations.</i> Examine before the Bp. on Ch. some silver oxide, AgO,
+also some zinc oxide, ZnO.</p>
+
+<p><i>c.</i> Whether the substance is alkaline or non-alkaline when placed upon
+moistened red litmus.<span class='pagenum'><a name="Page_12" id="Page_12">[Pg 12]</a></span></p>
+
+<p><i>Illustrations.</i> Ignite some calcium carbonate, CaCO<sub>3</sub>, before the Bp.
+on Ch., and place residue on moistened red litmus. In like manner,
+examine some magnesium carbonate, MgCO<sub>3</sub>.</p>
+
+<p><i>d.</i> Color of coating on Ch. caused by combination of metal and oxygen
+due to heat of Bp. flame.</p>
+
+<p><i>Illustrations.</i> Examine some oxide of lead, PbO, before the Bp. on Ch.,
+also some oxide of cadmium, CdO.</p>
+
+<p><i>e.</i> Decrepitation.</p>
+
+<p><i>Illustration.</i> Examine some sodium chloride, NaCl, before the Bp. on
+Ch.</p>
+
+<p><i>f.</i> Deflagration.</p>
+
+<p><i>Illustrations.</i> Examine some potassium nitrate, KNO<sub>3</sub>, before the Bp.
+<span class='pagenum'><a name="Page_13" id="Page_13">[Pg 13]</a></span>on Ch., also some ammonium nitrate, NH<sub>4</sub>NO<sub>3</sub>.</p>
+
+<p><i>g.</i> Intumescence.</p>
+
+<p><i>Illustration.</i> Examine some alum,</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">K<sub>2</sub>Al<sub>2</sub>(SO<sub>4</sub>)<sub>4</sub>,<br /></span>
+</div></div>
+
+<p>before the Bp. on Ch.</p>
+
+<p><i>h.</i> Incandescence.</p>
+
+<p><i>Illustration.</i> Examine some oxide of barium, BaO, before the Bp. on Ch.</p>
+
+<p><i>i.</i> Formation of a metallic bead&mdash;color and malleability.</p>
+
+<p><i>Illustration.</i> Examine some silver oxide, AgO, before the Bp. on Ch.</p>
+
+
+<p><b>Examination on Charcoal with Na<sub>2</sub>CO<sub>3</sub>.</b>&mdash;Metallic compounds are often
+difficult to reduce with the blowpipe flame alone, and hence no bead is
+obtained. In order to facilitate reduction and the obtaining of a
+metallic bead, the substance in a finely powdered condition is mixed
+<span class='pagenum'><a name="Page_14" id="Page_14">[Pg 14]</a></span>with four parts of sodium carbonate, Na<sub>2</sub>CO<sub>3</sub>, and ignited before
+the Bp. on Ch. The metallic compound is decomposed, the metal being
+transformed into the carbonate, which in turn, through the agency of the
+Ch. and the heat of the flame, is reduced to the free metal. Sometimes
+the reduction is made easier by adding to the substance about its own
+bulk of potassium cyanide, KCN, which takes up oxygen from the compound
+and is converted into potassium cyanate, KCNO.</p>
+
+<p>The reactions in reducing copper sulphate, CuSO<sub>4</sub>, with Na<sub>2</sub>CO<sub>3</sub>
+and with KCN before the blowpipe, are here given:&mdash;</p>
+
+
+
+<div class='center'>
+<table border="0" cellpadding="4" cellspacing="0" summary="">
+<tr><td align='left'>CuSO<sub>4</sub></td><td align='left'>+</td><td align='left'>Na<sub>2</sub>CO<sub>3</sub></td><td align='left'>=</td><td align='left'>CuCO<sub>3</sub></td><td align='left'>+</td><td align='left'>Na<sub>2</sub>SO<sub>4</sub></td><td align='left'>}</td><td align='left'>(1)</td></tr>
+<tr><td align='left'>2CuCO<sub>3</sub></td><td align='left'>+</td><td align='left'>C</td><td align='left'>=</td><td align='left'>3CO<sub>2</sub></td><td align='left'>+</td><td align='left'>2Cu</td><td align='left'>}</td></tr>
+<tr><td align='left'>&nbsp;</td></tr>
+<tr><td align='left'>CuSO<sub>4</sub></td><td align='left'>+</td><td align='left'>Na<sub>2</sub>CO<sub>3</sub></td><td align='left'>=</td><td align='left'>CuCO<sub>3</sub></td><td align='left'>+</td><td align='left'>Na<sub>2</sub>SO<sub>4</sub></td><td align='left'>}</td></tr>
+<tr><td align='left'>CuCO<sub>3</sub></td><td align='left'>&nbsp;</td><td align='left'>&nbsp;</td><td align='left'>=</td><td align='left'>CuO</td><td align='left'>+</td><td align='left'>CO<sub>2</sub></td><td align='left'>}</td><td align='left'>(2)</td></tr>
+<tr><td align='left'>CuO</td><td align='left'>+</td><td align='left'>KCN</td><td align='left'>=</td><td align='left'>Cu</td><td align='left'>+</td><td align='left'>KCNO</td><td align='left'>}</td></tr>
+</table></div>
+
+<p><span class='pagenum'><a name="Page_15" id="Page_15">[Pg 15]</a></span></p>
+
+<p>After obtaining beads, it is well to obtain their coatings, for
+oftentimes it is only in this way that we can distinguish between the
+metals.</p>
+
+
+<p><b>Examination in Tube with Na<sub>2</sub>CO<sub>3</sub> and Charcoal.</b>&mdash;If the substance in
+a finely pulverized condition be mixed with twelve parts, Na<sub>2</sub>CO<sub>3</sub>,
+and six parts of charcoal powder and the mixture be placed in an
+ignition tube and subjected to heat, the acid of the substance combines
+with the soda and the metal is set free.</p>
+
+<p>If this metal is volatile, a sublimate is formed in the upper end of the
+tube.</p>
+
+<p>Mercury deposits in minute globules, which may be seen with the
+magnifying glass. Arsenic forms a ring, which, when examined with the
+magnifying glass, is seen to be made up of minute crystals. Ammonia is
+recognized by its characteristic<span class='pagenum'><a name="Page_16" id="Page_16">[Pg 16]</a></span> odor, and also by its turning a slip
+of moistened red litmus (held over the mouth of the tube) blue.</p>
+
+
+<p><b>Examination on Platinum Wire.</b>&mdash;Many substances possess the property of
+imparting to the colorless flame of the Bunsen burner characteristic
+colors.</p>
+
+<p>The chlorides of these substances exhibit these flame reactions best,
+and hence before applying the flame tests we dip the wire which serves
+as a support into hydrochloric acid and then into the substance. When
+the substance has been taken up on the wire, it is placed in the edge of
+the long colorless flame of the Bunsen burner near the apex, when
+instantly the flame becomes tinged with the characteristic color of the
+substance.</p>
+
+<p><i>Illustrations.</i> Sodium compounds color the flame yellow, and a crystal
+of potassium<span class='pagenum'><a name="Page_17" id="Page_17">[Pg 17]</a></span> dichromate appears colorless in the sodium light.</p>
+
+<p>This sodium reaction is extremely delicate, it being possible to detect
+with ease a quantity of a sodium salt less than 1/3000000 of a milligram
+in weight.</p>
+
+<p>Potassium colors the flame purplish-violet.</p>
+
+<p>Barium colors the flame apple-green.</p>
+
+<p>Strontium colors the flame crimson.</p>
+
+<p>Calcium colors the flame orange-red, distinguished from strontium, by
+appearing gray when seen through blue glass.</p>
+
+<p>Boracic acid colors the flame green when the substance has been
+moistened with glycerine.</p>
+
+
+<p><b>Examination in Borax Bead.</b>&mdash;Borax, Na<sub>2</sub>B<sub>4</sub>O<sub>7</sub>, and microcosmic
+salt,</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">NaNH<sub>4</sub>H . PO<sub>4</sub>,<br /></span>
+</div></div>
+
+<p>possess the property of dissolving many of<span class='pagenum'><a name="Page_18" id="Page_18">[Pg 18]</a></span> the metallic oxides at the
+temperature of the Bunsen flame.</p>
+
+<p>For example, with oxide of cobalt, the following reactions take place
+with the two fluxes:&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">CoO + Na<sub>2</sub>B<sub>4</sub>O<sub>7</sub> = Co(BO<sub>2</sub>)<sub>2</sub> + 2 NaBO<sub>2</sub>.<br /></span>
+</div></div>
+
+<p>On heating, NaNH<sub>4</sub>H. PO<sub>4</sub>, it is decomposed into the metaphosphate
+of sodium, NaPO<sub>3</sub>,</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">CoO + NaPO<sub>3</sub> = CoNaPO<sub>4</sub>.<br /></span>
+</div></div>
+
+<p>Now in such cases of solution the metallic oxides impart a
+characteristic color to the flux.</p>
+
+<p>The platinum wire is the best support,&mdash;it is heated to incandescence in
+the Bunsen flame, and then is quickly dipped into the borax, when a
+small globule will adhere,&mdash;this is removed to the flame again when the
+borax melts to a clear glassy bead. While the bead is still melted,
+touch it to<span class='pagenum'><a name="Page_19" id="Page_19">[Pg 19]</a></span> the finely pulverized substance and replace in the flame.
+In a few seconds the small particles of the substance will have
+dissolved, and the bead will be seen to have assumed the color
+characteristic of the substance. Note the color when hot and then when
+cold; often there is a wide difference. Then, too, the test should be
+made in both O. F. and R. F.</p>
+
+<p>Some analysts prefer to make a small loop in the end of the wire before
+taking up the borax to make the bead. Care should be taken to see that
+the bead is colorless before bringing it in contact with the substance.</p>
+
+<p>As the depth of color produced is largely dependent upon the amount of
+substance taken, some little caution should be exercised to insure
+taking up about the same quantity each time.</p>
+
+<p><i>Illustrations.</i> Make several beads, and<span class='pagenum'><a name="Page_20" id="Page_20">[Pg 20]</a></span> note the colors characteristic
+of the following oxides: cobalt, nickel, iron, manganese, chromium, and
+copper.</p>
+
+<p>The microcosmic salt bead dissolves almost every oxide except silica,
+SiO<sub>2</sub>, and this is seen to float about in the melted mass. This is
+used as a test for silica.</p>
+
+
+<p><b>Examination with Co(NO<sub>3</sub>)<sub>2</sub>.</b>&mdash;If after examination on the Ch. <i>per
+se</i>, a white infusible residue remains, it is moistened with a drop of
+cobalt nitrate Co(NO<sub>3</sub>)<sub>2</sub> and re-ignited before the Bp., when a
+change of color will be observed. This change in color is owing to the
+fact that the heat of the Bp. flame decomposes the cobalt nitrate,
+nitric acid being driven off, and the remaining CoO forming with the
+oxide of the residue a colored mass.</p>
+
+<p><i>Illustrations.</i> Ignite before the Bp. on Ch. the following
+<span class='pagenum'><a name="Page_21" id="Page_21">[Pg 21]</a></span>oxides,&mdash;allow to cool, add a drop of Co(NO<sub>3</sub>)<sub>2</sub>, re-ignite, and
+note color,&mdash;aluminum, magnesium, zinc, and calcium.</p>
+
+<p>Care should be taken to thoroughly ignite before adding the cobalt
+nitrate solution.</p>
+
+<p>With the six methods of examination just given almost every simple
+substance can be detected, but should any doubt remain, a few simple
+tests in the "liquid way" will be sufficient to substantiate the
+blowpipe examination.</p>
+
+
+
+<hr style="width: 65%;" /><p><span class='pagenum'><a name="Page_22" id="Page_22">[Pg 22]</a></span></p>
+<h2>CHAPTER III</h2>
+
+<h3>GENERAL REACTIONS FOR THE DETECTION OF THE METALLIC ELEMENTS IN SIMPLE
+COMPOUNDS</h3>
+
+
+<p>For the sake of convenience, rather than for scientific reasons, the
+following compounds have been arranged in alphabetic order. Also the
+oxides of the elements have been taken, since they exhibit the reactions
+to best advantage.</p>
+
+<p>The student should work through carefully each one of the tests and
+satisfy himself as to the characteristic reactions of the various
+elements, for only in this way can he expect to recognize the substances
+when presented to him as "unknowns." It is advisable to provide a
+note-book and rule it as follows:<span class='pagenum'><a name="Page_23" id="Page_23">[Pg 23]</a></span>&mdash;</p>
+
+<pre>
+-----------------------------------------------------------------------------
+                         <span class="smcap">Behavior of Substance</span>                                  |
+----------------------------------------------------------------------------|
+Before Bp.| Before Bp.  | In ignition | In flame| In flame  | After first   |
+on Ch.    | on Ch. with | tube with   |   on    | with borax| ignition      |
+alone     | Na<sub>2</sub>CO<sub>3</sub>       | Na<sub>2</sub>CO<sub>3</sub>      | platinum| bead      | with           |
+          |             | and Ch.     |  wire   |           | Co(NO<sub>3</sub>)<sub>2</sub>       |
+----------------------------------------------------------------------------|
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+----------------------------------------------------------------------------|
+<i>Remarks</i> _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _               |
+                                                                            |
+<i>Substance</i> _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _               |
+----------------------------------------------------------------------------
+</pre>
+
+<p>1. <b>Aluminum, Al<sub>2</sub>O<sub>3</sub>.</b>&mdash;Before the Bp. on Ch. Infusible. No change.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Forms an infusible compound
+with slight intumescence.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch. No change. Moisture driven
+off.</p>
+
+<p>In flame on platinum wire. No change. Becomes incandescent.</p>
+
+<p>In flame with borax bead. In O. F.<span class='pagenum'><a name="Page_24" id="Page_24">[Pg 24]</a></span> dissolves slowly, forming a
+colorless glass which remains so on cooling.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>. Mass becomes blue upon re-ignition.</p>
+
+
+<p>2. <b>Antimony, Sb<sub>2</sub>O<sub>3</sub>.</b>&mdash;Before the Bp. on Ch. In O. F. volatilizes
+without change. In R. F. is reduced and volatilized. White coating of
+antimonious oxide deposited on Ch. Blue tinge imparted to flame.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Readily reduced. White brittle
+bead. Very volatile, giving characteristic white coating.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch. Volatilized.</p>
+
+<p>In flame on platinum wire. Volatilized. Colors flame greenish blue.</p>
+
+<p>With borax bead on platinum wire. In O. F. dissolves to a colorless
+glass.</p>
+
+<p><span class='pagenum'><a name="Page_25" id="Page_25">[Pg 25]</a></span></p><p>With Co(NO<sub>3</sub>)<sub>2</sub>.____</p>
+
+
+<p>3. <b>Arsenic, As<sub>2</sub>O<sub>3</sub>.</b>&mdash;Before the Bp. on Ch. Very volatile. Strong
+garlic odor to fumes.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Reduced with emission of
+arsenical fumes.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch. Volatilizes, forming a
+mirror-like deposit of metallic As in the cooler part of tube.</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead on platinum wire____</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>.____</p>
+
+
+<p>4. <b>Bismuth, Bi<sub>2</sub>O<sub>3</sub>.</b>&mdash;Before the Bp. on Ch. Yields a
+coating&mdash;orange-yellow when hot, lemon-yellow when cold. The yellow
+coating usually has a white outline.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Easily reduced to metallic
+bismuth. Yellow bead brittle, but less so than antimony.</p>
+
+<p><span class='pagenum'><a name="Page_26" id="Page_26">[Pg 26]</a></span></p><p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch.____</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead on platinum wire. In O. F. small quantity dissolves to a
+clear yellow glass, which becomes colorless when cold.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>5. <b>Cadmium, CdO.</b>&mdash;Before the Bp. on Ch. Gives a coating on the coal.
+Reddish-brown when cold. Very volatile.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Readily reduced. The metal
+volatilizes easily, giving the characteristic coating.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch.____</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead. In O. F. dissolves to a clear yellowish bead, colorless
+when cold.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p><span class='pagenum'><a name="Page_27" id="Page_27">[Pg 27]</a></span></p><p>6. <b>Chromium, Cr<sub>2</sub>O<sub>3</sub>.</b>&mdash;Before the Bp. on Ch. No change.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Cannot be reduced. Soda sinks
+in Ch. and a green colored mass remains.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch.____</p>
+
+<p>In flame on platinum wire____</p>
+
+
+<p><b>With borax bead.</b> Dissolves slowly but colors intensely. Yellow while
+hot, green when cold.</p>
+
+<p>With microcosmic salt bead. Colors red when hot, green when cold.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>7. <b>Cobalt, CoO.</b>&mdash;Before the Bp. on Ch. In O. F. unchanged. In R. F. is
+reduced to the metal and is magnetic.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Reduced to a gray magnetic
+mass.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch.____</p>
+
+<p>In flame on platinum wire____<span class='pagenum'><a name="Page_28" id="Page_28">[Pg 28]</a></span></p>
+
+<p>With borax bead on platinum wire. In O. F. colors very intensely blue,
+both hot and cold.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>8. <b>Copper, CuO.</b>&mdash;Before the Bp. on Ch. Fuses to a black globule, which
+can be reduced with some difficulty.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Readily reduced to metallic
+bead, which is red in color, hard, malleable.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch.____</p>
+
+<p>In flame on platinum wire. Colors flame emerald-green.</p>
+
+<p>With borax bead on platinum wire. In O. F. green when hot, blue when
+cold.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>9. <b>Iron, Fe<sub>2</sub>O<sub>3</sub>.</b>&mdash;Before the Bp. on Ch. In O. F. unchanged. In R.
+F. becomes black and magnetic.<span class='pagenum'><a name="Page_29" id="Page_29">[Pg 29]</a></span></p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> Reduced to a metallic powder,
+magnetic.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch.____</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead on platinum wire. In O. F. red while hot, yellow when
+cold.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>10. <b>Lead, PbO.</b>&mdash;Before the Bp. on Ch. Easily reduced to the metal, bead
+very malleable. Coating yellow, surrounded by white ring.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Instantly reduced. Coats the
+Ch. upon further blowing.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch. Reduced to the metal.</p>
+
+<p>In flame on platinum wire. Tinges flame blue.</p>
+
+<p>With borax bead on platinum wire.<span class='pagenum'><a name="Page_30" id="Page_30">[Pg 30]</a></span> In O. F. dissolves easily, forming a
+limpid glass.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>11. <b>Manganese, Mn<sub>2</sub>O<sub>3</sub>.</b>&mdash;Before the Bp. on Ch. At high temperature
+turns red.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Is not reduced.</p>
+
+<p>Before the Bp. in O. F. on platinum foil with Na<sub>2</sub>CO<sub>3</sub>. Transparent
+green mass when hot. Opaque, bluish-green when cold.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch. Not reduced.</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead on platinum wire. In O. F. violet-red while hot,
+amethyst-red when cold.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>12. <b>Mercury, HgO.</b>&mdash;Before the Bp. on Ch. Instantly reduced. Very
+volatile.</p>
+
+<p><span class='pagenum'><a name="Page_31" id="Page_31">[Pg 31]</a></span></p><p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Reduced and volatilized.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch. Sublimes condensing in the
+upper part of the tube as a metallic ring which is seen with the lens to
+consist of minute globules of mercury.</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead on platinum wire____</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>13. <b>Nickel, NiO.</b>&mdash;Before the Bp. on Ch. In O. F. unchanged. In R. F.
+reduced to metal, slightly magnetic.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Easily reduced to the metal.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch.____</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead on platinum wire. In O. F. violet while hot,
+reddish-brown when cold.</p>
+
+<p><span class='pagenum'><a name="Page_32" id="Page_32">[Pg 32]</a></span></p><p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>14. <b>Silver, AgO.</b>&mdash;Before the Bp. on Ch. Easily reduced to the metal.
+White, malleable, hard bead. Coats the coal dark red near assay.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Instantly reduced to metallic
+globule.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch. Reduced to the metal.</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead on platinum wire. In O. F. partially dissolved. Bead
+becomes milk-white.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>____</p>
+
+
+<p>15. <b>Tin, SnO<sub>2</sub>.</b>&mdash;Before the Bp. on Ch. Coats the coal yellow while
+hot, dirty white when cool. Not reduced.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Reduced to metallic tin. White,
+hard, malleable bead. Coating white and close to assay.<span class='pagenum'><a name="Page_33" id="Page_33">[Pg 33]</a></span></p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch.____</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead on platinum wire. In O. F. small quantity dissolves to
+limpid glass.</p>
+
+<p>With Co(NO<sub>3</sub>)<sub>2</sub>. Greenish-blue color.</p>
+
+
+<p>16. <b>Zinc, ZnO.</b>&mdash;Before the Bp. on Ch. Upon ignition becomes yellow. Is
+not reduced.</p>
+
+<p>Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub>. Reduced to metal. Rapidly
+volatilized, coating the coal white.</p>
+
+<p>In ignition tube with Na<sub>2</sub>CO<sub>3</sub> and Ch.____</p>
+
+<p>In flame on platinum wire____</p>
+
+<p>With borax bead on platinum wire. In O. F. yellow while hot, limpid
+glass when cold.</p>
+
+<p><span class='pagenum'><a name="Page_34" id="Page_34">[Pg 34]</a></span></p><p>With Co(NO<sub>3</sub>)<sub>2</sub>. Green mass.</p>
+
+<p>Having now given the principal reactions for the most important metals,
+we will proceed to the examination of the alkali metals, the alkaline
+earths, and some of the acid elements.</p>
+
+
+<h3><span class="smcap">The Alkali Metals</span></h3>
+
+<p>17. <b>Ammonium, NH<sub>4</sub>.</b>&mdash;This hypothetical compound is commonly classed
+among the alkali metals from its close resemblance to the members of
+this group.</p>
+
+<p>To detect the presence of this hypothetical metal, mix the assay with
+about four parts of Na<sub>2</sub>CO<sub>3</sub>, place in an ignition tube, and apply
+heat. The odor of the evolved gas will be recognized, and if a piece of
+red litmus paper be moistened and held at the mouth of the tube, it will
+be turned blue by the escaping ammonia gas.</p>
+
+<p>We are not authorized to infer the pre-existence of ammonium, however,
+from the<span class='pagenum'><a name="Page_35" id="Page_35">[Pg 35]</a></span> appearance of this reaction, for the presence of nitrogenous
+organic matter in the substance, which would be decomposed by this
+treatment, would give rise to such a reaction.</p>
+
+
+<p>18. <b>Potassium.</b>&mdash;Potassium is recognized by the color which its salts
+impart to the Bunsen flame. If a portion of a salt of potassium be held
+on a platinum wire in the flame, it imparts a blue-violet tint which
+rapidly disappears.</p>
+
+
+<p>19. <b>Sodium.</b>&mdash;Like potassium, this alkali metal is detected by the color
+which its salts give to the flame.</p>
+
+<p>If a sodium salt be held on the platinum wire in the flame, it imparts
+an intense yellow color.</p>
+
+<p>The extreme delicacy of this reaction has been mentioned elsewhere. The
+value<span class='pagenum'><a name="Page_36" id="Page_36">[Pg 36]</a></span> of this test is really lessened by its great delicacy, for it is
+possible to detect minute quantities of sodium in almost all substances,
+although it may not be in chemical combination. As an example, draw the
+platinum wire between the fingers, and then place in flame, and note
+presence of sodium.</p>
+
+
+<p>20. <b>Lithium, Li<sub>2</sub>O.</b>&mdash;In the Bunsen flame on the platinum wire it
+imparts a carmine-red tinge.</p>
+
+<p>Hydrochloric acid on the sample augments the coloration.</p>
+
+
+<h3><span class="smcap">The Alkaline Earths</span></h3>
+
+<p>21. <b>Barium, BaO.</b>&mdash;In the Bunsen flame on the platinum wire it imparts an
+apple-green coloration. This reaction is intensified by moistening the
+sample with hydrochloric acid.<span class='pagenum'><a name="Page_37" id="Page_37">[Pg 37]</a></span></p>
+
+
+<p>22. <b>Calcium, CaO.</b>&mdash;In the Bunsen flame on the platinum wire it imparts
+an orange-red color, which appears gray when seen through blue glass.</p>
+
+<p>Hydrochloric acid on the sample makes the color more intense.</p>
+
+
+<p>23. <b>Strontium, SrO.</b>&mdash;In the Bunsen flame on the platinum wire it imparts
+an intensely red color, which is increased by converting the substance
+into the chloride.</p>
+
+
+<h3><span class="smcap">The Acid Elements</span></h3>
+
+<p>24. <b>Borates.</b>&mdash;If the substance be finely powdered, moistened with
+glycerine, and then placed on a platinum wire in the Bunsen flame, it
+imparts a brilliant green color.</p>
+
+<p>If turmeric paper be dipped into a solution of a borate, and then be
+dried at 100&deg; C., it is turned to a peculiar red<span class='pagenum'><a name="Page_38" id="Page_38">[Pg 38]</a></span> color. These two
+reactions are extremely delicate.</p>
+
+
+<p>25. <b>Bromides.</b>&mdash;Bromides treated with microcosmic salt and oxide of
+copper on platinum wire impart to the flame a greenish-blue color, the
+edges being decidedly green.</p>
+
+
+<p>26. <b>Chlorides.</b>&mdash;Chlorides are treated in the same way as bromides. The
+color imparted to the flame is azure-blue.</p>
+
+<p>To discriminate between bromides and chlorides more clearly, the
+substance is mixed with anhydrous potassium bisulphate and fused in an
+ignition tube.</p>
+
+<p>Bromine and sulphur dioxide are evolved (if the substance be a bromide),
+the tube being filled with a yellow gas possessing the characteristic
+odor of bromine.</p>
+
+
+<p>27. <b>Fluorides.</b>&mdash;A small portion of the substance in a finely powdered
+condition is<span class='pagenum'><a name="Page_39" id="Page_39">[Pg 39]</a></span> placed in one of the ignition tubes, a strip of moist
+Brazil-wood paper is introduced into the open end, and heat is applied.
+Hydrofluoric acid is evolved, and the red color of the paper is changed
+into a straw-yellow.</p>
+
+<p>Mica, containing only 0.75% of fluorine, shows the reaction clearly.</p>
+
+
+<p>28. <b>Iodides.</b>&mdash;Iodides are treated, as the bromides and chlorides, in a
+bead of microcosmic salt with oxide of copper. The flame is colored
+green.</p>
+
+<p>Fused with potassium bisulphate in an ignition tube the violet vapors of
+iodine are evolved, and thus iodides may be distinguished from chlorides
+and bromides.</p>
+
+
+<p>29. <b>Nitrates.</b>&mdash;If a nitrate be heated upon charcoal before the Bp.,
+violent deflagration occurs. If the substance containing<span class='pagenum'><a name="Page_40" id="Page_40">[Pg 40]</a></span> the nitric
+acid be mixed with a <i>very small</i> quantity of finely powdered potassium
+cyanide, the deflagration is accompanied with ignition and detonation.</p>
+
+<p>If the substance be mixed in a dry condition with dry potassium
+bisulphate, and is then heated in an ignition tube, red-brown nitrous
+fumes are evolved. This reaction takes place if there is but a small
+quantity of nitrate present.</p>
+
+
+<p>30. <b>Phosphates.</b>&mdash;Phosphates impart to the flame a bluish green color.
+The color is made more intense by moistening the substance with
+sulphuric acid, and then taking the paste so formed on the platinum wire
+and placing it in the Bunsen flame.</p>
+
+
+<p>31. <b>Silicates.</b>&mdash;Silicates, when treated with microcosmic salt on a
+platinum wire,<span class='pagenum'><a name="Page_41" id="Page_41">[Pg 41]</a></span> suffer decomposition; the bases unite with the
+phosphoric acid to form a transparent glass in which the silica may be
+seen floating as a cloudy mass.</p>
+
+<p>The bead must only be examined for silica while hot, since on cooling it
+becomes opaque.</p>
+
+
+<p>32. <b>Sulphides.</b>&mdash;Many sulphides, when heated in an ignition tube,
+volatilize and give a sublimate of sulphur in combination with the
+metallic portion of the substance.</p>
+
+<p>A very delicate test for sulphur in whatever combination it may be found
+in a substance, and which may be performed with great ease, is to mix
+the finely powdered assay with four parts, Na<sub>2</sub>CO<sub>3</sub>, and fuse in an
+ignition tube. When thoroughly fused the tube is broken, and the fused
+mass is placed on a bright silver coin, and a drop<span class='pagenum'><a name="Page_42" id="Page_42">[Pg 42]</a></span> of water is added.
+If the substance contains sulphur, a black spot will be observed on the
+coin where the fused mass was placed.</p>
+
+<p>Before going on to the next chapter, the student should assure himself
+of his familiarity with the reactions just given, and he should practise
+with various substances, the nature of which is unknown to him.</p>
+
+
+
+<hr style="width: 65%;" /><p><span class='pagenum'><a name="Page_43" id="Page_43">[Pg 43]</a></span></p>
+<h2>CHAPTER IV</h2>
+
+<h3>BEHAVIOR OF SOME OF THE PRINCIPAL ORES BEFORE THE BLOWPIPE</h3>
+
+
+<p>For the sake of practice, and as a fitting introduction to
+"Determinative Mineralogy," this chapter is appended. It is not intended
+to give a detailed account of the minerals, but rather to set before the
+student the most marked characters, such as hardness, specific gravity,
+color, lustre, etc.</p>
+
+<p>To determine the hardness of a mineral, we try to scratch it with the
+minerals forming an arbitrary "scale of hardness," proceeding
+successively from the softest to the hardest. When we say that a certain
+mineral has hardness = 4, we mean that the mineral is scratched by 4 on
+the scale, and<span class='pagenum'><a name="Page_44" id="Page_44">[Pg 44]</a></span> that 4 on the scale is scratched by the mineral. The
+scale of hardness chiefly in use is the Mohs-Breithaupt scale, which is
+as follows:&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">1. Talc, common laminated light green variety.<br /></span>
+</div><div class="stanza">
+<span class="i0">2. Gypsum, crystallized.<br /></span>
+</div><div class="stanza">
+<span class="i0">3. Calcareous spar, transparent variety.<br /></span>
+</div><div class="stanza">
+<span class="i0">4. Fluor spar, crystalline.<br /></span>
+</div><div class="stanza">
+<span class="i0">5. Apatite, transparent.<br /></span>
+</div><div class="stanza">
+<span class="i0">6. Orthoclase, white cleavable variety.<br /></span>
+</div><div class="stanza">
+<span class="i0">7. Quartz, transparent.<br /></span>
+</div><div class="stanza">
+<span class="i0">8. Topaz, transparent.<br /></span>
+</div><div class="stanza">
+<span class="i0">9. Sapphire, cleavable variety.<br /></span>
+</div><div class="stanza">
+<span class="i0">10. Diamond.<br /></span>
+</div></div>
+
+<p>It seldom happens in determining the hardness of a mineral that its
+hardness exactly conforms to that of some one member of the scale. In
+such cases we generally estimate the hardness. For example, suppose<span class='pagenum'><a name="Page_45" id="Page_45">[Pg 45]</a></span> a
+mineral was harder than 4, but softer than 5, and that it was nearer 5
+than 4, then we would call its hardness 4-3/4.</p>
+
+<p>In order to preserve the scale some operators use a three-cornered file,
+first cutting the mineral and then the scale until a number is found,
+which is abraded to about the same depth as the mineral under
+examination.</p>
+
+<p>Since a set of minerals forming a scale of hardness is not always at
+hand, the following scale given by Chapman is appended:&mdash;</p>
+
+<div class="blockquot"><p>1. Yields easily to the nail.</p>
+
+<p>2. Yields with difficulty to the nail or just receives an
+impression from it. Does not scratch a copper coin.</p>
+
+<p>3. Scratches a copper coin but is also scratched by it,
+being of about the same degree of hardness.<span class='pagenum'><a name="Page_46" id="Page_46">[Pg 46]</a></span></p>
+
+<p>4. Not scratched by a copper coin. Does not scratch glass.</p>
+
+<p>5. Scratches glass with difficulty, leaving its powder on
+it. Yields readily to the knife.</p>
+
+<p>6. Scratches glass easily. Yields with difficulty to the
+knife.</p>
+
+<p>7. Does not yield to the knife. Yields to the edge of a
+file, though with difficulty.</p>
+
+<p>8, 9, 10. Harder than flint.</p></div>
+
+<p>Specific gravity cannot well be determined without the aid of a balance,
+and hence its value here is not great.</p>
+
+<p>As in the preceding chapter, alphabetic arrangement will be employed.</p>
+
+
+<h3><span class="smcap">Ores of Antimony</span></h3>
+
+<p><b>Stibnite</b>, Sb<sub>2</sub>S<sub>3</sub>, Sb . 71, S . 29.&mdash;<a name="FNanchor_A_1" id="FNanchor_A_1"></a><a href="#Footnote_A_1" class="fnanchor">[A]</a>H = 2, G = 4.52-4.62. Of
+lead-gray color and metallic lustre. Consists of a large number<span class='pagenum'><a name="Page_47" id="Page_47">[Pg 47]</a></span> of
+needle-shaped crystals. Brittle. Fuses in candle flame. In an ignition
+tube yields a sublimate of sulphur. On Ch. before the Bp. it is
+volatilized, giving antimony coating and tinges the flame pale blue.</p>
+
+<div class="footnote"><p><a name="Footnote_A_1" id="Footnote_A_1"></a><a href="#FNanchor_A_1"><span class="label">[A]</span></a> H = Hardness, G = Specific Gravity.</p></div>
+
+
+<h3><span class="smcap">Ores of Arsenic</span></h3>
+
+<p><b>Native Arsenic, As.</b>&mdash;This contains traces of Sb, Ag, Fe, Co, and Ni.</p>
+
+<p>H = 3.5, G = 5.7-5.8. Dark gray in color. Fracture tin-white, tarnishing
+rapidly. Volatilizes before the Bp. on Ch. without melting, giving white
+coating of arsenious acid and characteristic garlic odor. In ignition
+tube it sublimes, giving arsenical ring.</p>
+
+
+<p><b>Realgar</b>, AsS, As . 70, S . 30.&mdash;H = 1.5-2, G = 3.56. Bright red to
+orange-red color and resinous lustre. In an ignition tube it fuses and
+finally sublimes. The sublimate<span class='pagenum'><a name="Page_48" id="Page_48">[Pg 48]</a></span> when cool is red and transparent. Fuses
+readily before the Bp. on Ch. and burns with pale yellowish flame,
+emitting gray-white fumes having garlic odor.</p>
+
+
+<p><b>Orpiment</b>, As<sub>2</sub>S<sub>3</sub>, As . 61, S . 39.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 1.5-2.0, G = 3.4-3.5.<br /></span>
+</div></div>
+
+<p>Lemon-yellow in color and resinous or pearly lustre. Sectile. Before the
+Bp. on Ch. behaves like realgar, but in an ignition tube it gives a dark
+yellow sublimate which is transparent.</p>
+
+
+<h3><span class="smcap">Ores OF Bismuth</span></h3>
+
+<p><b>Native Bismuth, Bi.</b>&mdash;This contains traces of As, Te, and S.</p>
+
+<p>H = 2.0-2.5, G = 9.7-9.83. Color, silver-white, slightly tinged with
+red. Metallic lustre. Brittle when cold, but may be laminated when hot.
+Before the Bp. on Ch. behaves like pure Bi.<span class='pagenum'><a name="Page_49" id="Page_49">[Pg 49]</a></span></p>
+
+
+<p><b>Bismuthite</b>, Bi<sub>2</sub>O<sub>3</sub> . 90, CO<sub>2</sub> . 7, H<sub>2</sub>O . 3,&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 4.0-4.5, G = 6.9-7.8.<br /></span>
+</div></div>
+
+<p>Usually of a white or light greenish color and vitreous lustre, in
+acicular crystallizations. In an ignition tube decrepitates, yielding
+water and turning gray. Before the Bp. on Ch. it fuses easily and is
+reduced to metallic globule, coating the Ch. with Bi<sub>2</sub>O<sub>3</sub>. With
+Na<sub>2</sub>CO<sub>3</sub> it occasionally gives the sulphur reaction.</p>
+
+
+<h3><span class="smcap">Ores OF Chromium</span></h3>
+
+<p><b>Chromic Iron Ore</b>, FeO . 32, Cr<sub>2</sub>O<sub>3</sub> . 68.&mdash;Al<sub>2</sub>O<sub>3</sub>, Fe<sub>2</sub>O<sub>3</sub>,
+MnO, and MgO are commonly present. H = 5.5, G = 4.32-4.57. Occurs
+usually massive. Color, iron-black to brownish black. In many varieties
+strongly magnetic. Lustre, shining and somewhat metallic. Heated in an
+ignition tube, remains unchanged. Infusible before the Bp. on Ch.<span class='pagenum'><a name="Page_50" id="Page_50">[Pg 50]</a></span>
+Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> and KCN yields metallic iron. In
+borax bead it slowly dissolves to a clear transparent glass, which is a
+beautiful green when cool.</p>
+
+
+<h3><span class="smcap">Ores of Cobalt</span></h3>
+
+<p><b>Smaltite</b>, Co(Fe, Ni) As<sub>2</sub>, Co . 28, As . 72.&mdash;H = 5.5, G = 6.37-7.30.
+Color, tin-white or steel-gray. Lustre, metallic. When heated to redness
+in an ignition tube it yields a sublimate of metallic arsenic. Before
+the Bp. on Ch. it fuses readily, with emission of arsenical fumes, to a
+grayish black magnetic globule. This globule may be examined for iron,
+cobalt, and nickel with the borax bead.</p>
+
+
+<p><b>Cobaltite</b>, CoS<sub>2</sub> + CoAs<sub>2</sub>, Co . 36, As . 45, S . 19.&mdash;H = 5.5, G =
+6.0-6.3. Color, silver-white tinged with red. Metallic lustre. Before
+the Bp. on Ch. fuses easily, with<span class='pagenum'><a name="Page_51" id="Page_51">[Pg 51]</a></span> emission of copious arsenical fumes,
+to a gray magnetic globule. Remains unchanged in the ignition tube.</p>
+
+
+<p><b>Linnaeite</b>, (Co, Ni)<sub>3</sub>S<sub>4</sub>, (Co, Ni)58, S . 42.&mdash;H = 5.5, G = 4.8-5.0.
+Color, bright steel-gray, sometimes reddish. Lustre, metallic.
+Crystallizes in the regular octahedron. Before the Bp. on Ch. fuses to a
+metallic globule which is attracted by the magnet. With borax bead gives
+reaction for cobalt.</p>
+
+
+<p><b>Erythrite</b>, Co<sub>3</sub>O<sub>8</sub>As<sub>2</sub> + 8 H<sub>2</sub>O, As<sub>2</sub>S<sub>5</sub> . 38.4, CoO . 37.6,
+H<sub>2</sub>O . 24.0.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 1.5-2.0, G = 2.95.<br /></span>
+</div></div>
+
+<p>Color, crimson to peach-red. When crystallized, of pearly lustre, but
+frequently dull and earthy. Heated in ignition tube gives off water, and
+color changes to blue or green. Before the Bp. on Ch. in R. F. it<span class='pagenum'><a name="Page_52" id="Page_52">[Pg 52]</a></span> emits
+arsenical fumes and melts to a dark gray globule which with the borax
+bead reacts for cobalt.</p>
+
+
+<h3><span class="smcap">Ores of Copper</span></h3>
+
+<p><b>Native Copper, Cu.</b>&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 2.5-3, G = 8.5-8.9.<br /></span>
+</div></div>
+
+<p>Color, copper-red. Lustre, metallic. Occurs usually massive and very
+arborescent. Before the Bp. on Ch. it fuses, and if the heat is
+sufficiently high it assumes a bright bluish-green surface; on cooling
+it is covered with a coat of black oxide. In the borax bead it reacts
+for copper.</p>
+
+
+<p><b>Chalcopyrite</b>, CuFeS<sub>2</sub>, Cu . 35, Fe . 30, S . 35.&mdash;H = 3.5-4, G =
+4.1-4.3. Color, brass-yellow, often golden-yellow. Lustre, metallic.
+Occurs crystallized, but is generally found massive. Is easily
+scratched<span class='pagenum'><a name="Page_53" id="Page_53">[Pg 53]</a></span> with a knife. Heated in an ignition tube decrepitates, and
+occasionally yields a faint sublimate of sulphur. Before the Bp. on Ch.
+it blackens, but becomes red again on cooling. Before the Bp. on Ch.
+with Na<sub>2</sub>CO<sub>3</sub> and KCN it is reduced, and the metals are obtained in
+separate masses. It reacts with the borax bead for copper and iron.</p>
+
+
+<p><b>Copper Glance</b>, Cu<sub>2</sub>S, Cu . 80, S . 20.&mdash;H = 2.5-3.0, G = 5.5-5.8.
+Color, dark blue to steel-gray. Occurs in compact masses, often very
+shining. Before the Bp. on Ch. fuses to a globule which boils and emits
+glowing drops. Sulphur dioxide escapes abundantly, and the outer flame
+is colored blue. Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> yielding a
+metallic globule.</p>
+
+
+<p><b>Tetrahedrite</b>, 4 CuS + Sb<sub>2</sub>S<sub>3</sub>.&mdash;Frequently contains silver, iron,
+mercury, and zinc.<span class='pagenum'><a name="Page_54" id="Page_54">[Pg 54]</a></span> H = 3.0-4.0, G = 4.5-5. Color, steel-gray to
+iron-black. Heated in an ignition tube fuses and gives a sublimate of
+antimonious oxide. When mercury is present this condenses in the upper
+part of the tube, forming the characteristic mirror. Before the Bp. on
+Ch. it fuses readily to a metallic globule, emitting dense white fumes;
+zinc and antimony coatings are deposited on the Ch. After long ignition
+before the Bp., if the mineral is finely powdered and mixed with
+Na<sub>2</sub>CO<sub>3</sub> and KCN, the ore is reduced to the metal.</p>
+
+
+<p><b>Cuprite</b>, Cu<sub>2</sub>O, Cu . 89, O . 11.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 3.5-4.0, G = 5.5-6.15.<br /></span>
+</div></div>
+
+<p>Color, intense crimson-red. Before the Bp. on Ch. blackens and fuses
+quietly, and finally yields a metallic globule of copper. Before the Bp.
+<span class='pagenum'><a name="Page_55" id="Page_55">[Pg 55]</a></span>on Ch. with Na<sub>2</sub>CO<sub>3</sub> and KCN it is easily reduced.</p>
+
+
+<p><b>Malachite</b>, 2 CuO + CO<sub>2</sub> + H<sub>2</sub>O, CuO . 72, CO<sub>2</sub> . 20, H<sub>2</sub>O . 8.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 3.5-4.0, G = 3.90-4.03.<br /></span>
+</div></div>
+
+<p>Color, bright green. Occurs generally in mammillated concretions.
+Lustre, shining and fracture, silky. Heated in an ignition tube yields
+water and blackens. Before the Bp. on Ch. it fuses to a metallic
+globule. Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> and KCN it is easily
+reduced. With borax bead gives characteristic coloration.</p>
+
+
+<p><b>Azurite</b>, 3 CuO + 2 CO<sub>2</sub> + H<sub>2</sub>O, CuO . 69, CO<sub>2</sub> . 26, H<sub>2</sub>O . 5.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 3.5-4.0, G = 3.77-3.83.<br /></span>
+</div></div>
+
+<p>Color, azure-blue. Occurs usually in crystallized or globular masses.
+Lustre, earthy or vitreous. Before the Bp. and with other reagents
+behaves like malachite.<span class='pagenum'><a name="Page_56" id="Page_56">[Pg 56]</a></span></p>
+
+
+<p><b>Chrysocolla</b>, CuO + SiO<sub>2</sub> + 2 H<sub>2</sub>O, SiO<sub>2</sub> . 34.2, CuO . 45.3,
+H<sub>2</sub>O . 20.5.&mdash;H = 2.0-3.0, G = 2. Color, bluish-green, closely
+resembling malachite. Occurs usually as an incrustation, its surface
+being very smooth, like enamel. In an ignition tube it blackens and
+yields water. Before the Bp. on Ch. in O. F. it blackens, coloring the
+flame bright green; in the R. F. it turns red. Before the Bp. on Ch.
+with Na<sub>2</sub>CO<sub>3</sub> yields metallic copper. In borax bead it reacts for
+copper.</p>
+
+
+<p><b>Atacamite</b>, CuCl<sub>2</sub> + 3 CuO<sub>2</sub>H<sub>2</sub>&mdash;Cl . 16.6, O . 20.3, Cu . 50.1,
+H<sub>2</sub>O . 13.0.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 3.0-3.5, G = 3.75-3.77.<br /></span>
+</div></div>
+
+<p>Color, green to blackish green. Lustre, adamantine to vitreous. In an
+ignition tube yields water. Before the Bp. on Ch. colors flame blue.
+Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> and KCN is reduced to the metal.
+In borax bead it reacts for copper.<span class='pagenum'><a name="Page_57" id="Page_57">[Pg 57]</a></span></p>
+
+
+<h3><span class="smcap">Ores of Iron</span></h3>
+
+<p><b>Limonite</b>, 2 Fe<sub>2</sub>O<sub>3</sub> + 3 H<sub>2</sub>O, Fe<sub>2</sub>O<sub>3</sub> . 86, H<sub>2</sub>O . 14.&mdash;H =
+5.0-5.5, G = 3.6-4.0. Color, brown to ochre-yellow. Earthy or
+semi-metallic in appearance. In an ignition tube yields water. Before
+the Bp. on Ch. infusible. In borax bead reacts for iron.</p>
+
+
+<p><b>Hematite</b>, Fe<sub>2</sub>O<sub>3</sub>, Fe . 70, O . 30.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 5.5-6.5, G = 4.9-5.3.<br /></span>
+</div></div>
+
+<p>Color, dark steel-gray to iron-black. Lustre, metallic. When pulverized
+yields a red powder. Before the Bp. on Ch. infusible. After long
+roasting becomes magnetic. In borax bead gives usual indications of
+iron.</p>
+
+
+<p><b>Magnetite</b>, Fe<sub>3</sub>O<sub>4</sub>, FeO . 31, Fe<sub>2</sub>O<sub>3</sub> . 69.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 5.5-6.5, G = 5.17-5.18.<br /></span>
+<span class='pagenum'><a name="Page_58" id="Page_58">[Pg 58]</a></span></div></div>
+
+<p>Color, iron-black. Lustre, shining and metallic. Pulverized, its powder
+is black. It is strongly magnetic. Fuses with difficulty before the Bp.
+on Ch. In borax bead reacts for iron.</p>
+
+
+<p><b>Pyrites</b>, FeS<sub>2</sub>, Fe . 47, S . 53.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 6.0-6.5, G = 4.95-5.20.<br /></span>
+</div></div>
+
+<p>Color, brass-yellow. Lustre, metallic. Occurs commonly in cubes. It
+often contains small quantities of Au, Ag, Cu, As, Co, and Mn. Heated in
+an ignition tube gives a sublimate of sulphur, the residue becoming
+magnetic. Before the Bp. on Ch. in O. F. sulphur is burned off and the
+red oxide remains. This residue may then be examined for iron, etc.</p>
+
+
+<p><b>Marcasite</b> (White Iron Pyrites).&mdash;Having the same general composition as
+pyrite, but much lighter in color. Crystals, prismatic. Before the Bp.
+on Ch. behaves like pyrite.<span class='pagenum'><a name="Page_59" id="Page_59">[Pg 59]</a></span></p>
+
+
+<p><b>Pyrrhotite</b>, Fe<sub>7</sub>S<sub>8</sub>, Fe . 60.5, S . 39.5.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 3.5-4.5, G = 4.58-4.64.<br /></span>
+</div></div>
+
+<p>Color, bronze-yellow. Closely resembles pyrite, but may be distinguished
+from it by being feebly magnetic. Heated in an ignition tube yields no
+sublimate. Before the Bp. on Ch. fuses to a magnetic globule, which
+exhibits a yellowish crystalline structure when fractured.</p>
+
+
+<p><b>Mispickel</b>, FeAsS, Fe . 34, As . 46, S . 20.&mdash;H = 5.5-6.0, G = 6.0-6.2.
+Color, silver-white. Lustre, metallic; very brittle. Often associated
+with it we find small quantities of Co, Ag, and Au. Heated in an
+ignition tube it first yields a red sublimate of sulphide of arsenic,
+and then afterward a crystalline sublimate of metallic arsenic. Before
+the Bp. on Ch. emits dense fumes of arsenic and deposits a coating on
+the<span class='pagenum'><a name="Page_60" id="Page_60">[Pg 60]</a></span> coal; it then fuses to a globule which behaves like pyrrhotite.</p>
+
+
+<p><b>Siderite</b>, FeCO<sub>3</sub>, FeO . 62, CO<sub>2</sub> . 38.&mdash;H = 3.5-4.5, G = 3.7-3.9.
+Color, grayish yellow to reddish brown. Lustre, pearly. Crystallizes in
+rhombohedrons with curved faces; these crystals are distinctly cleavable
+and massive. Heated in an ignition tube it decrepitates with evolution
+of carbon dioxide. Before the Bp. on Ch. infusible. Before the Bp. on
+Ch. with Na<sub>2</sub>CO<sub>3</sub> it fuses to a magnetic mass. With borax bead it
+reacts for iron and sometimes for manganese.</p>
+
+
+<h3><span class="smcap">Ores of Lead</span></h3>
+
+<p><b>Galena</b>, PbS, Pb . 87, S . 13.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 2.5, G = 7.4-7.6.<br /></span>
+</div></div>
+
+<p>Color, bluish gray, slowly tarnishing. Lustre, metallic. Crystals in the
+form of cubes.<span class='pagenum'><a name="Page_61" id="Page_61">[Pg 61]</a></span> Heated in an ignition tube it sometimes decrepitates and
+yields a sublimate of sulphur. Before the Bp. on Ch. easily reduced to
+the metallic state, the Ch. becoming coated with sulphate and oxide of
+lead. The metallic globule usually contains a little silver. To separate
+this, the process known as "cupellation" is employed. A hole is bored
+into the Ch. about 1 cm. in diameter and about 6 mm. deep. Into this
+hole is placed a stiff paste made by mixing finely pulverized bone-ash
+with a little soda and water. This paste is pressed in hard, and then
+the surface is smoothed off, and the centre is slightly depressed with
+the rounded end of a glass rod. The charcoal so prepared is set in a
+warm place to allow the paste to dry. When the paste is quite dry the
+small globule of lead is placed in the depression in the centre of the
+bone-ash "cupel," and is there exposed to the<span class='pagenum'><a name="Page_62" id="Page_62">[Pg 62]</a></span> O. F. from the Bp. The
+lead is oxidized and is absorbed by the bone-ash, while any silver
+present will remain in the central depression as a bright shining bead.</p>
+
+
+<p><b>Cerusite</b>, PbCO<sub>3</sub>, PbO . 84, CO<sub>2</sub> . 16.&mdash;H = 3.0-3.5, G = 6.46-6.57.
+Color, white, gray, or yellow. Lustre, adamantine. Crystallizes in
+prismatic needles. When heated in an ignition tube carbon dioxide is
+evolved and the residue turns yellow. Before the Bp. on Ch. readily
+reduced to metallic lead.</p>
+
+
+<p><b>Anglesite</b>, PbSO<sub>4</sub>, PbO . 74, SO<sub>3</sub> . 26.&mdash;H = 2.0-3.0, G = 6.12-6.39.
+Color, yellow, gray, and brown. Lustre, adamantine, resinous. Heated in
+an ignition tube decrepitates, and sometimes yields a little water.
+Before the Bp. on Ch. fuses to a clear bead, which on cooling becomes<span class='pagenum'><a name="Page_63" id="Page_63">[Pg 63]</a></span>
+opaque. Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> is reduced to the metal
+giving a yellow coating. The Na<sub>2</sub>CO<sub>3</sub> absorbed by the coal reacts
+for S.</p>
+
+
+<h3><span class="smcap">Ores of Manganese</span></h3>
+
+<p><b>Pyrolusite</b>, MnO<sub>2</sub>, Mn . 63.2, O . 36.8.&mdash;H = 2.0-2.5, G = 4.82. Color,
+iron-black to steel-gray. Lustre, non-metallic. Heated in an ignition
+tube yields generally a little water, and if the temperature be high
+enough, oxygen is evolved. Before the Bp. on Ch. infusible. In borax
+bead gives characteristic color.</p>
+
+
+<p><b>Psilomelane</b>, Mn<sub>2</sub>O<sub>3</sub> + H<sub>2</sub>O.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 5.5-6.0, G = 3.7-4.7.<br /></span>
+</div></div>
+
+<p>Color, iron-black to steel-gray. Generally resembles pyrolusite, but is
+distinguished from it by its superior hardness. It frequently<span class='pagenum'><a name="Page_64" id="Page_64">[Pg 64]</a></span> contains
+BaO and Li<sub>2</sub>O. It behaves before the Bp. like pyrolusite.</p>
+
+
+<p><b>Wad</b> (Bog Manganese).&mdash;This mineral is essentially MnO<sub>2</sub>, MnO, and
+H<sub>2</sub>O, with small quantities of Fe<sub>2</sub>O<sub>3</sub>, Al<sub>2</sub>O<sub>3</sub>, BaO, SiO<sub>2</sub>,
+etc., associated with it.</p>
+
+<p>H = 0.5-6.0, G = 3.0-4.2. Color, dull black. Heated in an ignition tube
+yields water in abundance, otherwise it behaves like pyrolusite.</p>
+
+
+<h3><span class="smcap">Ores of Mercury</span></h3>
+
+<p><b>Native Mercury, Hg.</b>&mdash;G = 13.5-13.6. Color, silver-white. Is liquid at
+all ordinary temperatures. Heated in an ignition tube is volatilized,
+the vapors condensing in the upper end of tube to small metallic
+globules of Hg. Before the Bp. on Ch. it is volatilized. Frequently
+contains Ag.<span class='pagenum'><a name="Page_65" id="Page_65">[Pg 65]</a></span></p>
+
+
+<p><b>Cinnabar</b>, HgS<sub>2</sub>, Hg . 86, S . 14.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 2.0-2.5, G = 8.0-8.2.<br /></span>
+</div></div>
+
+<p>Color, scarlet-red to brick-red. Lustre, non-metallic. When pulverized
+yields a powder of vermilion-red color. Heated in an ignition tube it
+volatilizes, yielding a black sublimate, which by friction becomes red.
+Before the Bp. on Ch. it is wholly volatilized. Heated in an ignition
+tube with Na<sub>2</sub>CO<sub>3</sub> metallic mercury sublimes, condensing in the
+upper portion of the tube in minute globules.</p>
+
+
+<h3><span class="smcap">Ores of Nickel</span></h3>
+
+<p><b>Millerite</b>, NiS, Ni . 64.4, S . 35.6.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 3.0-3.5, G = 5.2-5.6.<br /></span>
+</div></div>
+
+<p>Color, brass-yellow. Brittle. Before the Bp. on Ch. it fuses to a
+magnetic, metallic globule. The roasted mineral gives in the borax bead
+the color reaction characteristic<span class='pagenum'><a name="Page_66" id="Page_66">[Pg 66]</a></span> of nickel, and sometimes that of
+cobalt, which is often associated with it.</p>
+
+
+<p><b>Niccolite</b>, NiAs, Ni . 44, As . 56.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 5.0-5.5, G = 7.35-7.67.<br /></span>
+</div></div>
+
+<p>Color, pale copper-red. Lustre, metallic. Very brittle. Heated in an
+ignition tube yields a copious sublimate of arsenious oxide, the residue
+falling to a greenish powder. Before the Bp. on Ch. fuses to a white
+brittle globule emitting arsenical fumes. In borax bead gives color
+characteristic of nickel. Frequently in this mineral a portion of the
+arsenic is replaced by antimony.</p>
+
+
+<h3><span class="smcap">Ores of Silver</span></h3>
+
+<p><b>Native Silver, Ag.</b>&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 2.5-3.0, G = 10.1-11.0.<br /></span>
+</div></div>
+
+<p>Color, silver-white. Lustre, metallic. Ductile and malleable. Usually
+occurs associated<span class='pagenum'><a name="Page_67" id="Page_67">[Pg 67]</a></span> with Au, As, Sb, Cu, Fe, etc. Before the Bp. on Ch.
+easily fuses to a globule which is surrounded with a dark red coating on
+the coal.</p>
+
+
+<p><b>Argentite</b>, Ag<sub>2</sub>S, Ag . 87.1, S . 12.9.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 2.0-2.5, G = 7.20-7.36.<br /></span>
+</div></div>
+
+<p>Color, blackish lead-gray. Lustre, metallic. Very sectile. Before the
+Bp. on Ch. in O. F. intumesces with evolution of sulphur dioxide,
+finally yielding a metallic globule of Ag.</p>
+
+
+<p><b>Pyrargyrite</b>, Ag<sub>3</sub>SbS<sub>3</sub>, Ag . 59.8, Sb . 22.5, S . 17.7.&mdash;H = 2.5, G
+= 5.77-5.86. Color, black to dark cochineal-red. Lustre, metallic,
+adamantine. In an ignition tube it yields on continued heating a
+sublimate of antimony sulphide. Before the Bp. on Ch. it gives a coating
+<span class='pagenum'><a name="Page_68" id="Page_68">[Pg 68]</a></span>of antimony trioxide. Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> is
+reduced to metallic silver.</p>
+
+
+<p><b>Proustite</b>, Ag<sub>3</sub>S<sub>3</sub>As, Ag . 65.5, As . 15.1, S . 19.4.&mdash;H = 2.0-2.5,
+G = 5.57-5.64. Color, light red. Lustre, splendent, adamantine. Before
+the Bp. on Ch. it behaves like pyrargyrite, save that it gives off
+arsenical fumes instead of antimonious oxide.</p>
+
+
+<p><b>Stephanite</b>, Ag<sub>5</sub>S<sub>4</sub>Sb, Ag . 68.5, Sb . 15.3, S . 16.2.&mdash;H = 2.0-2.5,
+G = 6.2-6.3. Color, iron-black to blackish gray. Lustre, metallic. Very
+brittle and fragile. In an ignition tube it decrepitates, fuses, and
+finally yields a slight sublimate of antimony trisulphide. Before the
+Bp. on Ch. gives a coating of antimonious oxide. Before the Bp. on Ch.
+with Na<sub>2</sub>CO<sub>3</sub> a globule of metallic silver is obtained. The mineral
+frequently contains copper and iron.<span class='pagenum'><a name="Page_69" id="Page_69">[Pg 69]</a></span></p>
+
+
+<p><b>Kerargyrite</b>, AgCl, Ag . 75.3, Cl . 24.7.&mdash;H = 1.0-1.5, G = 5.52. Color,
+white, gray, yellowish, greenish to blue. Lustre, resinous, adamantine.
+Soft like wax. Fuses easily in a candle-flame. Before the Bp. on Ch. it
+is readily reduced to metallic silver.</p>
+
+
+<h3><span class="smcap">Ores of Tin</span></h3>
+
+<p><b>Cassiterite</b>, SnO<sub>2</sub>, Sn . 79, O . 21.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 6.0-7.0, G = 6.8-7.0.<br /></span>
+</div></div>
+
+<p>Color, brown, black. Lustre, adamantine, brilliant. Occurs crystallized
+in square prisms. Re&euml;ntrant angles characteristic. Before the Bp. on Ch.
+with Na<sub>2</sub>CO<sub>3</sub> and KCN reduced to a metallic globule of tin. In the
+borax bead gives characteristic reaction.</p>
+
+
+<p><b>Stannite</b>, 2 Cu<sub>2</sub>S . SnS<sub>2</sub> + 2 (FeS . ZnS) Sn . S<sub>2</sub>.&mdash;H = 4.0, G =
+4.3-4.5. Color,<span class='pagenum'><a name="Page_70" id="Page_70">[Pg 70]</a></span> steel-gray to iron-black. Lustre, metallic. Occurs
+usually massive and disseminated. Heated in an ignition tube it yields
+sulphur dioxide. Before the Bp. on Ch. it emits sulphur dioxide and
+becomes covered with oxide of tin. Before the Bp. on Ch. with
+Na<sub>2</sub>CO<sub>3</sub> and KCN it gives an impure globule of copper. A very
+difficult mineral to determine.</p>
+
+
+<h3><span class="smcap">Ores of Zinc</span></h3>
+
+<p><b>Calamine</b>, H<sub>2</sub>Zn<sub>2</sub>O<sub>5</sub>Si, SiO<sub>2</sub> . 25.0, ZnO . 67.5, H<sub>2</sub>O .
+7.5.&mdash;H = 4.5-5.0, G = 3.4-3.5. Color, white, gray, bluish, or brown.
+Lustre, vitreous. Brittle. In an ignition tube yields water when heated
+and becomes milky white. Before the Bp. on Ch. practically infusible.
+With Co(NO<sub>3</sub>)<sub>2</sub> it assumes a green color which passes into a fine
+blue when the heat is increased.<span class='pagenum'><a name="Page_71" id="Page_71">[Pg 71]</a></span></p>
+
+
+<p><b>Smithsonite</b>,</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">Zn . CO<sub>3</sub>, ZnO . 64.8, CO<sub>2</sub> . 35.2.&mdash;<br /></span>
+</div></div>
+
+<p>H = 5, G = 4.30-4.45. Color, gray, yellow, brown, and green. Lustre,
+vitreous, pearly. Heated in an ignition tube CO<sub>2</sub> is evolved, residue
+appearing white. It often contains impurities of Cd, Pb, Fe, Mn, Ca, and
+Mg. When these are present the residue in the ignition tube becomes dark
+on cooling. Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> and exposed to the
+R. F. it is decomposed. It gives the characteristic reaction for zinc
+with Co(NO<sub>3</sub>)<sub>2</sub>.</p>
+
+
+<p><b>Zincite</b>, ZnO, Zn . 80.3, O . 19.7&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 4.0-4.5, G = 5.43-5.70.<br /></span>
+</div></div>
+
+<p>Color, blood-red. Lustre, brilliant, subadamantine. Before the Bp. on
+Ch. infusible. Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> gives coating of
+<span class='pagenum'><a name="Page_72" id="Page_72">[Pg 72]</a></span>zinc oxide. Gives characteristic reaction with Co(NO<sub>3</sub>)<sub>2</sub>. It
+frequently contains a small quantity of Mn<sub>2</sub>O<sub>3</sub>, which may be
+detected in the borax bead.</p>
+
+
+<p><b>Sphalerite</b>, ZnS, Zn . 67, S . 33.&mdash;</p>
+
+<div class="poem"><div class="stanza">
+<span class="i0">H = 3.5-4.0, G = 3.9-4.1.<br /></span>
+</div></div>
+
+<p>Color, yellow to black. Lustre, resinous, brilliant, and sometimes
+submetallic. Heated in an ignition tube sometimes decrepitates. Before
+the Bp. on Ch. infusible. Before the Bp. on Ch. with Na<sub>2</sub>CO<sub>3</sub> easily
+reduced. With Co(NO<sub>3</sub>)<sub>2</sub> gives the characteristic reaction. It
+frequently contains small quantities of Cd, Hg, Sn, Pb, Au, Ag, etc.<span class='pagenum'><a name="Page_73" id="Page_73">[Pg 73]</a></span></p>
+
+<hr style="width: 65%;" />
+
+<h3>I</h3>
+
+<h4><span class="smcap">Table of Colors of Coatings on Charcoal</span></h4>
+
+
+<div class='center'>
+<table border="1" cellpadding="4" cellspacing="0" summary="">
+<tr><td align='left'>Element</td><td align='left'> Color Hot</td><td align='left'> Color Cold</td></tr>
+<tr><td align='left'>Antimony</td><td align='left'> (Rather volatile)</td><td align='left'> White</td></tr>
+<tr><td align='left'>Arsenic</td><td align='left'> (Very volatile)</td><td align='left'> White</td></tr>
+<tr><td align='left'>Bismuth</td><td align='left'> Orange-Yellow</td><td align='left'> Lemon-Yellow</td></tr>
+<tr><td align='left'>Cadmium</td><td align='left'> Brownish Yellow</td><td align='left'> Reddish Brown</td></tr>
+<tr><td align='left'>Lead</td><td align='left'> Lemon-Yellow (volatile)</td><td align='left'> Lemon-Yellow</td></tr>
+<tr><td align='left'>Silver</td><td align='left'> Dark Red</td><td align='left'> Dark Red</td></tr>
+<tr><td align='left'>Tin</td><td align='left'> Faint Yellow</td><td align='left'> White</td></tr>
+<tr><td align='left'>Zinc</td><td align='left'> Yellow</td><td align='left'> White</td></tr>
+</table></div>
+
+
+<h3>II</h3>
+
+<h4><span class="smcap">Table of Flame Colorations</span></h4>
+
+
+<div class='center'>
+<table border="1" cellpadding="4" cellspacing="0" summary="">
+<tr><td align='left'>Red</td><td align='left'> Yellow</td><td align='left'> Green</td><td align='left'>Bluish Green</td><td align='left'> Blue</td><td align='left'> Violet</td></tr>
+<tr><td align='left'>Calcium</td><td align='left'> Sodium</td><td align='left'> Barium</td><td align='left'>Bromine</td><td align='left'> Chlorine</td><td align='left'> Potassium</td></tr>
+<tr><td align='left'>Lithium</td><td align='left'></td><td align='left'> Boron</td><td align='left'>Copper</td><td align='left'></td><td align='left'></td></tr>
+<tr><td align='left'>Strontium</td><td align='left'></td><td align='left'> Iodine</td><td align='left'>Phosphorus</td><td align='left'></td><td align='left'></td></tr>
+</table></div>
+
+<p><span class='pagenum'><a name="Page_74" id="Page_74">[Pg 74]</a></span></p>
+
+
+<h3>III</h3>
+
+<h4><span class="smcap">Table of Colors of Borax Beads in Oxidizing Flame</span></h4>
+
+
+<div class='center'>
+<table border="1" cellpadding="4" cellspacing="0" summary="">
+<tr><td align='left'>Element</td><td align='left'> Color Hot</td><td align='left'> Color Cold</td></tr>
+<tr><td align='left'>Aluminum</td><td align='left'> Colorless to Cloudy</td><td align='left'> Colorless to Cloudy</td></tr>
+<tr><td align='left'>Antimony</td><td align='left'> Yellowish</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Barium</td><td align='left'> Colorless to Opaque</td><td align='left'> Colorless to Opaque</td></tr>
+<tr><td align='left'>Bismuth</td><td align='left'> Yellow</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Cadmium</td><td align='left'> Yellow</td><td align='left'> Colorless to White</td></tr>
+<tr><td align='left'>Calcium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Chromium</td><td align='left'> Reddish Yellow</td><td align='left'> Yellowish Green</td></tr>
+<tr><td align='left'>Cobalt</td><td align='left'> Blue</td><td align='left'> Blue</td></tr>
+<tr><td align='left'>Copper</td><td align='left'> Green</td><td align='left'> Greenish Blue</td></tr>
+<tr><td align='left'>Iron</td><td align='left'> Orange</td><td align='left'> Yellow</td></tr>
+<tr><td align='left'>Lead</td><td align='left'> Yellow</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Magnesium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Manganese</td><td align='left'> Violet</td><td align='left'> Reddish Violet</td></tr>
+<tr><td align='left'>Nickel</td><td align='left'> Violet</td><td align='left'> Reddish Brown</td></tr>
+<tr><td align='left'>Silver</td><td align='left'> Colorless</td><td align='left'> Milk-White</td></tr>
+<tr><td align='left'>Strontium</td><td align='left'> Colorless to Opaque</td><td align='left'> Colorless to Opaque</td></tr>
+<tr><td align='left'>Tin</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Zinc</td><td align='left'> Yellowish</td><td align='left'> Colorless</td></tr>
+</table></div>
+
+<p><span class='pagenum'><a name="Page_75" id="Page_75">[Pg 75]</a></span></p>
+
+
+<h3>IV</h3>
+
+<h4><span class="smcap">Table of Colors of Borax Beads in Reducing Flame</span></h4>
+
+
+
+<div class='center'>
+<table border="1" cellpadding="4" cellspacing="0" summary="">
+<tr><td align='left'>Element</td><td align='left'> Color Hot</td><td align='left'> Color Cold</td></tr>
+<tr><td align='left'>Aluminum</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Antimony</td><td align='left'> Colorless</td><td align='left'> Cloudy</td></tr>
+<tr><td align='left'>Barium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Bismuth</td><td align='left'> Colorless</td><td align='left'> Gray&mdash;Cloudy</td></tr>
+<tr><td align='left'>Cadmium</td><td align='left'> Colorless</td><td align='left'> Gray&mdash;Cloudy</td></tr>
+<tr><td align='left'>Calcium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Chromium</td><td align='left'> Green</td><td align='left'> Green</td></tr>
+<tr><td align='left'>Cobalt</td><td align='left'> Blue</td><td align='left'> Blue</td></tr>
+<tr><td align='left'>Copper</td><td align='left'> Colorless</td><td align='left'> Red</td></tr>
+<tr><td align='left'>Iron</td><td align='left'> Yellowish Green</td><td align='left'> Yellowish Green</td></tr>
+<tr><td align='left'>Lead</td><td align='left'> Colorless</td><td align='left'> Gray</td></tr>
+<tr><td align='left'>Magnesium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Manganese</td><td align='left'> Colorless</td><td align='left'> Pink</td></tr>
+<tr><td align='left'>Nickel</td><td align='left'> Colorless</td><td align='left'> Gray&mdash;Cloudy</td></tr>
+<tr><td align='left'>Silver</td><td align='left'> Colorless</td><td align='left'> Gray</td></tr>
+<tr><td align='left'>Strontium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Tin</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Zinc</td><td align='left'> Colorless</td><td align='left'> Gray</td></tr>
+</table></div>
+
+<p><span class='pagenum'><a name="Page_76" id="Page_76">[Pg 76]</a></span></p>
+
+
+<h3>V</h3>
+
+<h4><span class="smcap">Table of Colors of Microcosmic Salt Beads in Oxidizing Flame</span></h4>
+
+
+
+<div class='center'>
+<table border="1" cellpadding="4" cellspacing="0" summary="">
+<tr><td align='left'>Element</td><td align='left'> Color Hot</td><td align='left'> Color Cold</td></tr>
+<tr><td align='left'>Aluminum</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Antimony</td><td align='left'> Yellowish</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Barium</td><td align='left'>Colorless to Opaque</td><td align='left'> Colorless to Opaque</td></tr>
+<tr><td align='left'>Bismuth</td><td align='left'> Yellow</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Cadmium</td><td align='left'> Yellowish</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Calcium</td><td align='left'> Colorless</td><td align='left'> Colorless to Opaque</td></tr>
+<tr><td align='left'>Chromium</td><td align='left'> Reddish</td><td align='left'> Green</td></tr>
+<tr><td align='left'>Cobalt</td><td align='left'> Blue</td><td align='left'> Blue</td></tr>
+<tr><td align='left'>Copper</td><td align='left'> Green</td><td align='left'> Greenish Blue</td></tr>
+<tr><td align='left'>Iron</td><td align='left'> Red</td><td align='left'> Brownish Red</td></tr>
+<tr><td align='left'>Lead</td><td align='left'> Yellowish</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Magnesium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Manganese</td><td align='left'> Brownish Violet</td><td align='left'> Reddish Violet</td></tr>
+<tr><td align='left'>Nickel</td><td align='left'> Reddish</td><td align='left'> Yellow</td></tr>
+<tr><td align='left'>Silver</td><td align='left'> Yellowish</td><td align='left'> Yellowish</td></tr>
+<tr><td align='left'>Strontium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Tin</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Zinc</td><td align='left'> Yellowish</td><td align='left'> Colorless</td></tr>
+</table></div>
+
+<p><span class='pagenum'><a name="Page_77" id="Page_77">[Pg 77]</a></span></p>
+
+
+<h3>VI</h3>
+
+<h4><span class="smcap">Table of Colors of Microcosmic Salt Beads in Reducing Flame</span></h4>
+
+
+<div class='center'>
+<table border="1" cellpadding="4" cellspacing="0" summary="">
+<tr><td align='left'>Element</td><td align='left'> Color Hot</td><td align='left'> Color Cold</td></tr>
+<tr><td align='left'>Aluminum</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Antimony</td><td align='left'> Colorless</td><td align='left'> Gray&mdash;Cloudy</td></tr>
+<tr><td align='left'>Barium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Bismuth</td><td align='left'> Colorless</td><td align='left'> Gray&mdash;Cloudy</td></tr>
+<tr><td align='left'>Cadmium</td><td align='left'> Colorless</td><td align='left'> Gray&mdash;Cloudy</td></tr>
+<tr><td align='left'>Calcium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Chromium</td><td align='left'> Reddish</td><td align='left'> Green</td></tr>
+<tr><td align='left'>Cobalt</td><td align='left'> Blue</td><td align='left'> Blue</td></tr>
+<tr><td align='left'>Copper</td><td align='left'> Dark Green</td><td align='left'> Brownish Red</td></tr>
+<tr><td align='left'>Iron</td><td align='left'> Red</td><td align='left'> Reddish</td></tr>
+<tr><td align='left'>Lead</td><td align='left'> Colorless</td><td align='left'> Gray&mdash;Opaque</td></tr>
+<tr><td align='left'>Magnesium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Manganese</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Nickel</td><td align='left'> Colorless</td><td align='left'> Gray</td></tr>
+<tr><td align='left'>Silver</td><td align='left'> Colorless</td><td align='left'> Gray</td></tr>
+<tr><td align='left'>Strontium</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Tin</td><td align='left'> Colorless</td><td align='left'> Colorless</td></tr>
+<tr><td align='left'>Zinc</td><td align='left'> Colorless</td><td align='left'> Gray&mdash;Cloudy</td></tr>
+</table></div>
+
+
+<hr style="width: 65%;" />
+
+
+<h2>THE PRACTICAL METHODS</h2>
+
+<h4>OF</h4>
+
+<h2>ORGANIC CHEMISTRY</h2>
+
+<h4>AUTHORIZED TRANSLATION</h4>
+
+<h4>12mo. Cloth. Price, $1.60, <i>net</i></h4>
+
+
+<div class='center'>
+<table border="0" cellpadding="4" cellspacing="3" summary="">
+<tr><td align='center'></td><td align='center'>BY</td><td align='center'>TRANSLATED BY</td></tr>
+<tr><td align='center'></td><td align='center'>LUDWIG GATTERMANN, Ph.D.,</td><td align='center'>WILLIAM SHAFER, Ph.D.,</td></tr>
+<tr><td align='center'></td><td align='center'><i>Professor in University</i></td><td align='center'><i>Instructor in Organic Chemistry</i></td></tr>
+<tr><td align='center'></td><td align='center'><i>of Heidelberg.</i></td><td align='center'><i>in Lehigh University.</i></td></tr>
+</table></div>
+
+
+<hr style='width: 45%;' />
+
+<h3>THE GUARDIAN.</h3>
+
+<div class="blockquot"><p>"The selection and judgment throughout is excellent. The
+book is a most useful, practical adjunct to any good
+text-book on organic chemistry."</p></div>
+
+<h3>PHARMACEUTICAL REVIEW.</h3>
+
+<div class="blockquot"><p>"This is a book that should be in the library of every
+teacher of organic chemistry, and one which will no doubt be
+of great value to students in their second year of organic
+chemistry. Its chief peculiarity and merit is in the great
+stress laid on practical laboratory work.... It is
+permanently a worker's guide."</p></div>
+
+<h3>NATURE.</h3>
+
+<div class="blockquot"><p>"Since the advance of organic chemistry in this country
+must, in a measure, depend on the nature of the available
+text-books, both the author and the translator deserve our
+thanks for providing us with a work such as the present
+one."</p></div>
+
+<hr style='width: 45%;' />
+
+<p class="center">
+PUBLISHED BY<br />
+THE MACMILLAN COMPANY<br />
+66 FIFTH AVENUE, NEW YORK<br />
+</p>
+
+<hr style='width: 45%;' />
+
+<h3>OUTLINES</h3>
+
+<h4>OF</h4>
+
+<h2>INDUSTRIAL CHEMISTRY</h2>
+
+<h3>A TEXT-BOOK FOR STUDENTS</h3>
+
+<h3>By FRANK HALL THORP, Ph.D.,</h3>
+
+<h4><i>Instructor in Industrial Chemistry in the Massachusetts Institute of
+Technology.</i></h4>
+
+<h4>Cloth. 8vo. Price, $3.50 <i>net</i></h4>
+
+<hr style='width: 45%;' />
+
+<h3>JAMES LEWIS HOWE,</h3>
+
+<h4><i>Department of Chemistry, Washington and Lee University.</i></h4>
+
+<div class="blockquot"><p>"The book is brought thoroughly up to date, and in some
+cases the lines of probable development are nicely
+foreshadowed. The descriptions are particularly lucid and
+the illustrations well selected.</p>
+
+<p>The general arrangement and make-up of the book is
+excellent, and ... altogether the book fills well a need
+long felt by teachers of Industrial Chemistry.</p>
+
+<p>I shall adopt the book for my class and shall take pleasure
+in recommending it."</p></div>
+
+<h3>CHARLES E. COATES, Jr., Ph.D.,</h3>
+
+<h4><i>Professor of Chemistry, Louisiana State University.</i></h4>
+
+<div class="blockquot"><p>"I have examined it carefully and think it a most excellent
+book, meeting a want I have long felt in my higher classes.
+I have introduced it in this year's classes."</p></div>
+
+<h3>W. A. NOYES, in <i>Science</i>.</h3>
+
+<div class="blockquot"><p>"The descriptions of processes, while necessarily concise,
+are clear and interesting. The author has evidently made a
+careful study of recent methods of manufacture as well as of
+older, standard processes. The frequent reference to
+American practice is an important feature which
+distinguishes the book from other works on chemical
+technology. A select bibliography follows each subject, and
+will be found very useful."</p></div>
+
+<hr style='width: 45%;' />
+
+<p class="center">
+PUBLISHED BY<br />
+THE MACMILLAN COMPANY<br />
+66 FIFTH AVENUE, NEW YORK<br />
+</p>
+
+
+
+
+
+
+
+
+<pre>
+
+
+
+
+
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+The Project Gutenberg EBook of The Elements of Blowpipe Analysis, by
+Frederick Hutton Getman
+
+This eBook is for the use of anyone anywhere at no cost and with
+almost no restrictions whatsoever.  You may copy it, give it away or
+re-use it under the terms of the Project Gutenberg License included
+with this eBook or online at www.gutenberg.org
+
+
+Title: The Elements of Blowpipe Analysis
+
+Author: Frederick Hutton Getman
+
+Release Date: June 25, 2010 [EBook #32974]
+
+Language: English
+
+Character set encoding: ASCII
+
+*** START OF THIS PROJECT GUTENBERG EBOOK THE ELEMENTS OF BLOWPIPE ANALYSIS ***
+
+
+
+
+Produced by The Online Distributed Proofreading Team at
+https://www.pgdp.net. (This file was produced from images
+generously made available by The Internet Archive/American
+Libraries.)
+
+
+
+
+
+
+
+THE ELEMENTS OF BLOWPIPE ANALYSIS
+
+[Illustration]
+
+
+
+
+THE
+
+ELEMENTS OF BLOWPIPE
+
+ANALYSIS
+
+BY
+
+FREDERICK HUTTON GETMAN, F.C.S.
+
+INSTRUCTOR IN CHEMISTRY IN THE STAMFORD HIGH SCHOOL
+
+New York
+THE MACMILLAN COMPANY
+LONDON: MACMILLAN & CO., LTD.
+1899
+
+_All rights reserved_
+
+
+COPYRIGHT, 1899,
+
+BY THE MACMILLAN COMPANY.
+
+Norwood Press
+J. S. Cushing & Co.--Berwick & Smith
+Norwood Mass. U.S.A.
+
+Transcriber's note: A word surrounded by underscores like _this_
+signifies the word is italics in the text. A word surrounded by cedillas
+like ~this~, signifies the word is bolded in the text. For numbers and
+equations, underscores before bracketed numbers in equations denote a
+subscript.
+
+
+PREFACE
+
+
+These few pages are intended to serve a twofold purpose,--to give the
+student a general outline of Blowpipe Analysis, and to introduce him to
+the methods of Determinative Mineralogy.
+
+Every effort has been made to simplify details so that the book may be
+used in both High Schools and Colleges.
+
+Tables for "systematic" examination have been intentionally omitted, for
+in the author's estimation these tend to dull the student's power of
+observation, and to make him place little value upon minute details.
+
+The alphabetic arrangement has been followed for the sake of convenience
+when referring to the book.
+
+The last chapter is not intended to serve as a key to determining the
+minerals therein described, but rather it is added to give the student
+exercise in Blowpipe Analysis, and at the same time to point out the
+_methods_ of Determinative Mineralogy.
+
+Finally, the author would acknowledge his indebtedness to the following
+works: "Manual of Qualitative Analysis," Fresenius; "Qualitative
+Chemical Analysis," Venable; Roscoe and Schorlemmer's "Treatise on
+Chemistry"; Foye's "Hand-Book of Mineralogy"; Dana's "Mineralogy";
+Kobell's "Tafeln zur Bestimmung der Mineralien"; etc.
+
+FREDERICK HUTTON GETMAN.
+
+STAMFORD, CONN.,
+
+Feb. 22, 1899.
+
+
+
+
+TABLE OF CONTENTS
+
+
+CHAPTER I
+                                                             PAGE
+Apparatus and Reagents                                        1-7
+
+
+CHAPTER II
+
+General Outline of Blowpipe Analysis                            8
+
+Definitions                                                     9
+
+Examination on Charcoal Alone                                  10
+
+Examination on Charcoal with Sodium Carbonate                  13
+
+Examination in Tube with Sodium Carbonate and Charcoal         15
+
+Examination on Platinum Wire                                   16
+
+Examination in Borax Bead                                      17
+
+Examination with Cobalt Nitrate                                20
+
+
+CHAPTER III
+
+General Reactions for the Detection of the Metallic
+Elements in Simple Compounds                                   22
+
+Aluminum                                                       23
+
+Antimony                                                       24
+
+Arsenic                                                        25
+
+Bismuth                                                        25
+
+Cadmium                                                        26
+
+Chromium                                                       26
+
+Cobalt                                                         27
+
+Copper                                                         28
+
+Iron                                                           28
+
+Lead                                                           29
+
+Manganese                                                      30
+
+Mercury                                                        30
+
+Nickel                                                         31
+
+Silver                                                         32
+
+Tin                                                            32
+
+Zinc                                                           33
+
+The Alkali Metals                                              34
+
+Ammonium                                                       34
+
+Potassium                                                      35
+
+Sodium                                                         35
+
+Lithium                                                        36
+
+The Alkaline Earths                                            36
+
+Barium                                                         36
+
+Calcium                                                        37
+
+Strontium                                                      37
+
+The Acid Elements                                              37
+
+Borates                                                        37
+
+Bromides                                                       38
+
+Chlorides                                                      38
+
+Fluorides                                                      38
+
+Iodides                                                        39
+
+Nitrates                                                       39
+
+Phosphates                                                     40
+
+Silicates                                                      40
+
+Sulphides                                                      41
+
+
+CHAPTER IV
+
+Behavior of Some of the Principal Ores before the Blowpipe     43
+
+Ores of Antimony                                               46
+
+Ores of Arsenic                                                47
+
+Ores of Bismuth                                                48
+
+Ores of Chromium                                               49
+
+Ores of Cobalt                                                 50
+
+Ores of Copper                                                 52
+
+Ores of Iron                                                   57
+
+Ores of Lead                                                   60
+
+Ores of Manganese                                              63
+
+Ores of Mercury                                                64
+
+Ores of Nickel                                                 65
+
+Ores of Silver                                                 66
+
+Ores of Tin                                                    69
+
+Ores of Zinc                                                   70
+
+
+COMPARATIVE TABLES
+
+I. Colors of Coatings on Charcoal                              73
+
+II. Flame Colorations                                          73
+
+III. Colors of Borax Beads in oxidizing Flame                  74
+
+IV. Colors of Borax Beads in reducing Flame                    75
+
+V. Colors of Microcosmic Salt Beads in oxidizing Flame         76
+
+VI. Colors of Microcosmic Salt Beads in reducing Flame         77
+
+
+[Illustration: THE BLOWPIPE Fig. 1]
+
+[Illustration: BUNSEN BURNER Fig. 2]
+
+[Illustration: CHARCOAL BORERS Fig. 3]
+
+[Illustration: AGATE MORTAR & PESTLE Fig. 4]
+
+[Illustration: FORCEPS Fig. 5]
+
+[Illustration: HAMMER Fig. 6]
+
+[Illustration: 3-CORNERED FILES Fig. 7]
+
+
+
+
+BLOWPIPE ANALYSIS
+
+
+
+
+CHAPTER I
+
+
+The blowpipe was first applied to mineral analysis in 1733 by Anton
+Swab, and its applications have since been improved and extended by
+various chemists, among whom may be mentioned Bergmann, Cronstedt, Gahn,
+Berzelius, and Plattner.
+
+
+~Blowpipe.~--The common blowpipe of the jeweller is not particularly well
+suited to the operations of blowpipe analysis, since the flame has often
+to be kept playing upon the assay for some time, and the condensed
+moisture of the breath would seriously interfere with the passage of
+the air through the jet. One of the best and least expensive forms of
+blowpipe is shown in Fig. 1. This consists, as is seen from the
+illustration, of a conical-shaped tube of tin closed at the wide end and
+formed into a mouthpiece at the small end; soldered into the tube at the
+large end, and at right angles to its axis, is a small brass tube which
+terminates in a conical tip pierced with a very fine hole. With this
+pipe it is possible to perform all of the operations of mineral
+analysis.
+
+Some little practice is necessary to keep the flame steady and to take
+the breath at the same time.
+
+No rule can well be given to the beginner, but his experience becomes
+his best guide.
+
+
+~Bunsen Flame.~--Any kind of flame can be used for the blowpipe, provided
+it be not too small; but since almost every laboratory to-day is
+furnished with gas and the Bunsen burner (Fig. 2), it will only be
+necessary to describe the use of the flame from this source. Upon
+examining the Bunsen flame with care, it will be seen that the flame
+consists of three distinct parts.
+
+A dark inner cone which consists of gas not yet raised to the ignition
+point. Beyond this there is a luminous cone, where combustion is
+incomplete owing to lack of oxygen, and outside of this we find the
+non-luminous cone where the gas is completely burned.
+
+This outer envelope is the hottest portion of the flame, and is known as
+the "oxidizing" flame because there is an excess of oxygen which is
+imparted to substances placed therein.
+
+The luminous cone is known as the "reducing" flame, for in it metallic
+oxides are reduced, the oxygen being taken up by the small incandescent
+particles of carbon.
+
+If the air-holes at the base of the Bunsen burner be opened, the two
+inner cones become elongated, and the flame appears almost colorless.
+
+The blowpipe enables us to get an oxidizing and a reducing flame of
+better form and greater power. To do this we cut off the air supply at
+the base of the burner and turn off the gas until the flame is about 1
+cm. high; then upon introducing the blowpipe, and blowing a strong
+continuous jet of air across the Bunsen flame, we produce an oxidizing
+flame about 4-5 cm. in length. If the tip of the blowpipe be held
+outside of the Bunsen flame, and the pressure of the stream of air be
+diminished, we obtain a reducing flame.
+
+
+~Supports.~--For supports, charcoal, platinum, and glass are chiefly used.
+The charcoal should be made from some light wood, such as alder. It
+should be well burnt, and should not scintillate or smoke.
+
+The platinum supports are generally in the form of wire and foil.
+Platinum-tipped forceps are frequently employed in blowpipe analysis.
+
+Glass is used in the form of tubing.
+
+Hard glass tubing, 3 mm. bore, is drawn off into ignition tubes 7-8 cm.
+in length. Several dozen of these tubes should be made before commencing
+the tests of the next chapter.
+
+
+~Apparatus.~--A small agate mortar, 4-5 cm. in diameter, should be
+provided in which to grind the samples to be examined.
+
+The pestle, which should also be of agate, must be adapted to the
+mortar in shape and size.
+
+Two pairs of forceps will also be needed.
+
+One pair should be of steel, and the other pair of brass, with fine
+points.
+
+Of other apparatus, the most necessary is:--
+
+    A small hammer and anvil.
+
+    Two three-cornered files.
+
+    Small piece of cobalt glass, about 5 x 10 cm.
+
+    Pocket magnifying lens.
+
+    Several small watch glasses--for metallic beads, etc.
+
+
+~Chemicals.~--A list of the principal chemicals is here given:--
+
+    Sodium carbonate, Na_{2}CO_{3}.
+
+    Borax, Na_{2}B_{4}O_{7} + 10 H_{2}O.
+
+    Microcosmic salt, (HNaNH_{4}), PO_{4} + 8 H_{2}O.
+
+    Cobalt nitrate, Co(NO_{3})_{2} + 5 H_{2}O.
+
+    Potassium cyanide, KCN.
+
+    Hydrochloric acid, (dilute), HCl + nH_{2}O.
+
+    Litmus paper, red and blue.
+
+    Brazil-wood paper.
+
+Any other special reagents which may be needed will be mentioned as
+required.
+
+
+
+
+CHAPTER II
+
+GENERAL OUTLINE OF BLOWPIPE ANALYSIS
+
+
+     [ABBREVIATIONS: O. F. for oxidizing flame, R. F. for
+     reducing flame, Ch. for charcoal, Ct. for coating, Bp. for
+     blowpipe.]
+
+In order to examine a substance before the blowpipe to determine the
+presence or absence of certain elements, it becomes necessary to arrange
+a systematic method. As with all branches of chemical work, one's
+success is largely dependent upon neatness of manipulation and
+carefulness of observation.
+
+The following order of observation is essentially that given by
+Berzelius:--
+
+     1. Examination on charcoal by itself.
+
+     2. Examination on charcoal with Na_{2}CO_{3}.
+
+     3. Examination in ignition tube with Na_{2}CO_{3} and
+     charcoal.
+
+     4. Examination on platinum wire.
+
+     5. Examination in borax bead.
+
+     6. Examination with Co(NO_{3})_{2}.
+
+After having examined a body in these six different ways, we shall be
+able to say what are its principal constituents.
+
+Before describing the method of carrying out these six different
+operations, it will be necessary to give a few definitions of terms
+which we shall have frequent occasion to employ.
+
+
+~Definitions.~--_Ignition_ is the heating of a substance to a high
+temperature.
+
+_Fusion_ is the heating of a substance to the melting-point.
+
+_Intumescence_ is the swelling of the substance upon heating.
+
+_Decrepitation_ is the crackling of a substance due to the sudden
+expansion of combined water upon heating.
+
+_Deflagration_ is the burning of a substance with explosive violence,
+generally due to excess of oxygen.
+
+_Incandescence_ is the white light emitted by a substance that is
+infusible when subjected to a high temperature.
+
+
+~Examination on Charcoal alone.~--The size of the assay should be about
+that of a mustard seed. This is sufficiently large to show all of the
+reactions clearly, and though a larger piece would exhibit the
+characteristic phenomena, yet much more effort is required. A very
+small, shallow hole should be cut in the Ch. to receive the assay. The
+Bp. flame should be directed at an angle of about 30 deg. with the
+surface of the Ch. Considerable care must be taken lest the hole in the
+Ch. is burned too deep and the assay lost in the coal.
+
+The force of the air from the jet must also be borne in mind for a
+strong blast, or sudden puffs may blow the substance away.
+
+The following changes are to be looked for:--
+
+_a._ Whether the substance is volatile or non-volatile.
+
+_Illustrations._ Examine before the Bp. on Ch. some arsenious oxide,
+As_{2}O_{3}, also some alumina, Al_{2}O_{3}.
+
+_b._ Whether the substance is fusible or infusible.
+
+_Illustrations._ Examine before the Bp. on Ch. some silver oxide, AgO,
+also some zinc oxide, ZnO.
+
+_c._ Whether the substance is alkaline or non-alkaline when placed upon
+moistened red litmus.
+
+_Illustrations._ Ignite some calcium carbonate, CaCO_{3}, before the Bp.
+on Ch., and place residue on moistened red litmus. In like manner,
+examine some magnesium carbonate, MgCO_{3}.
+
+_d._ Color of coating on Ch. caused by combination of metal and oxygen
+due to heat of Bp. flame.
+
+_Illustrations._ Examine some oxide of lead, PbO, before the Bp. on Ch.,
+also some oxide of cadmium, CdO.
+
+_e._ Decrepitation.
+
+_Illustration._ Examine some sodium chloride, NaCl, before the Bp. on
+Ch.
+
+_f._ Deflagration.
+
+_Illustrations._ Examine some potassium nitrate, KNO_{3}, before the Bp.
+on Ch., also some ammonium nitrate, NH_{4}NO_{3}.
+
+_g._ Intumescence.
+
+_Illustration._ Examine some alum,
+
+    K_{2}Al_{2}(SO_{4})_{4},
+
+before the Bp. on Ch.
+
+_h._ Incandescence.
+
+_Illustration._ Examine some oxide of barium, BaO, before the Bp. on Ch.
+
+_i._ Formation of a metallic bead--color and malleability.
+
+_Illustration._ Examine some silver oxide, AgO, before the Bp. on Ch.
+
+
+~Examination on Charcoal with Na_{2}CO_{3}.~--Metallic compounds are often
+difficult to reduce with the blowpipe flame alone, and hence no bead is
+obtained. In order to facilitate reduction and the obtaining of a
+metallic bead, the substance in a finely powdered condition is mixed
+with four parts of sodium carbonate, Na_{2}CO_{3}, and ignited before
+the Bp. on Ch. The metallic compound is decomposed, the metal being
+transformed into the carbonate, which in turn, through the agency of the
+Ch. and the heat of the flame, is reduced to the free metal. Sometimes
+the reduction is made easier by adding to the substance about its own
+bulk of potassium cyanide, KCN, which takes up oxygen from the compound
+and is converted into potassium cyanate, KCNO.
+
+The reactions in reducing copper sulphate, CuSO_{4}, with Na_{2}CO_{3}
+and with KCN before the blowpipe, are here given:--
+
+    CuSO_{4} + Na_{2}CO_{3} = CuCO_{3} + Na_{2}SO_{4} }  (1)
+              2CuCO_{3} + C = 3CO_{2} + 2Cu           }
+
+    CuSO_{4} + Na_{2}CO_{3} = CuCO_{3} + Na_{2}SO_{4} }
+                   CuCO_{3} = CuO + CO_{2}            }  (2)
+                  CuO + KCN = Cu + KCNO               }
+
+After obtaining beads, it is well to obtain their coatings, for
+oftentimes it is only in this way that we can distinguish between the
+metals.
+
+
+~Examination in Tube with Na_{2}CO_{3} and Charcoal.~--If the substance in
+a finely pulverized condition be mixed with twelve parts, Na_{2}CO_{3},
+and six parts of charcoal powder and the mixture be placed in an
+ignition tube and subjected to heat, the acid of the substance combines
+with the soda and the metal is set free.
+
+If this metal is volatile, a sublimate is formed in the upper end of the
+tube.
+
+Mercury deposits in minute globules, which may be seen with the
+magnifying glass. Arsenic forms a ring, which, when examined with the
+magnifying glass, is seen to be made up of minute crystals. Ammonia is
+recognized by its characteristic odor, and also by its turning a slip
+of moistened red litmus (held over the mouth of the tube) blue.
+
+
+~Examination on Platinum Wire.~--Many substances possess the property of
+imparting to the colorless flame of the Bunsen burner characteristic
+colors.
+
+The chlorides of these substances exhibit these flame reactions best,
+and hence before applying the flame tests we dip the wire which serves
+as a support into hydrochloric acid and then into the substance. When
+the substance has been taken up on the wire, it is placed in the edge of
+the long colorless flame of the Bunsen burner near the apex, when
+instantly the flame becomes tinged with the characteristic color of the
+substance.
+
+_Illustrations._ Sodium compounds color the flame yellow, and a crystal
+of potassium dichromate appears colorless in the sodium light.
+
+This sodium reaction is extremely delicate, it being possible to detect
+with ease a quantity of a sodium salt less than 1/3000000 of a milligram
+in weight.
+
+Potassium colors the flame purplish-violet.
+
+Barium colors the flame apple-green.
+
+Strontium colors the flame crimson.
+
+Calcium colors the flame orange-red, distinguished from strontium, by
+appearing gray when seen through blue glass.
+
+Boracic acid colors the flame green when the substance has been
+moistened with glycerine.
+
+
+~Examination in Borax Bead.~--Borax, Na_{2}B_{4}O_{7}, and microcosmic
+salt,
+
+    NaNH_{4}H . PO_{4},
+
+possess the property of dissolving many of the metallic oxides at the
+temperature of the Bunsen flame.
+
+For example, with oxide of cobalt, the following reactions take place
+with the two fluxes:--
+
+    CoO + Na_{2}B_{4}O_{7} = Co(BO_{2})_{2} + 2 NaBO_{2}.
+
+On heating, NaNH_{4}H. PO_{4}, it is decomposed into the metaphosphate
+of sodium, NaPO_{3},
+
+    CoO + NaPO_{3} = CoNaPO_{4}.
+
+Now in such cases of solution the metallic oxides impart a
+characteristic color to the flux.
+
+The platinum wire is the best support,--it is heated to incandescence in
+the Bunsen flame, and then is quickly dipped into the borax, when a
+small globule will adhere,--this is removed to the flame again when the
+borax melts to a clear glassy bead. While the bead is still melted,
+touch it to the finely pulverized substance and replace in the flame.
+In a few seconds the small particles of the substance will have
+dissolved, and the bead will be seen to have assumed the color
+characteristic of the substance. Note the color when hot and then when
+cold; often there is a wide difference. Then, too, the test should be
+made in both O. F. and R. F.
+
+Some analysts prefer to make a small loop in the end of the wire before
+taking up the borax to make the bead. Care should be taken to see that
+the bead is colorless before bringing it in contact with the substance.
+
+As the depth of color produced is largely dependent upon the amount of
+substance taken, some little caution should be exercised to insure
+taking up about the same quantity each time.
+
+_Illustrations._ Make several beads, and note the colors characteristic
+of the following oxides: cobalt, nickel, iron, manganese, chromium, and
+copper.
+
+The microcosmic salt bead dissolves almost every oxide except silica,
+SiO_{2}, and this is seen to float about in the melted mass. This is
+used as a test for silica.
+
+
+~Examination with Co(NO_{3})_{2}.~--If after examination on the Ch. _per
+se_, a white infusible residue remains, it is moistened with a drop of
+cobalt nitrate Co(NO_{3})_{2} and re-ignited before the Bp., when a
+change of color will be observed. This change in color is owing to the
+fact that the heat of the Bp. flame decomposes the cobalt nitrate,
+nitric acid being driven off, and the remaining CoO forming with the
+oxide of the residue a colored mass.
+
+_Illustrations._ Ignite before the Bp. on Ch. the following
+oxides,--allow to cool, add a drop of Co(NO_{3})_{2}, re-ignite, and
+note color,--aluminum, magnesium, zinc, and calcium.
+
+Care should be taken to thoroughly ignite before adding the cobalt
+nitrate solution.
+
+With the six methods of examination just given almost every simple
+substance can be detected, but should any doubt remain, a few simple
+tests in the "liquid way" will be sufficient to substantiate the
+blowpipe examination.
+
+
+
+
+CHAPTER III
+
+GENERAL REACTIONS FOR THE DETECTION OF THE METALLIC ELEMENTS IN SIMPLE
+COMPOUNDS
+
+
+For the sake of convenience, rather than for scientific reasons, the
+following compounds have been arranged in alphabetic order. Also the
+oxides of the elements have been taken, since they exhibit the reactions
+to best advantage.
+
+The student should work through carefully each one of the tests and
+satisfy himself as to the characteristic reactions of the various
+elements, for only in this way can he expect to recognize the substances
+when presented to him as "unknowns." It is advisable to provide a
+note-book and rule it as follows:--
+
+-----------------------------------------------------------------------------
+                         BEHAVIOR OF SUBSTANCE                              |
+----------------------------------------------------------------------------|
+Before Bp.| Before Bp.  | In ignition | In flame| In flame  | After first   |
+on Ch.    | on Ch. with | tube with   |   on    | with borax| ignition      |
+alone     | Na_{2}CO_{3}| Na_{2}CO_{3}| platinum| bead      | with          |
+          |             | and Ch.     |  wire   |           | Co(NO_{3})_{2}|
+----------------------------------------------------------------------------|
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+          |             |             |         |           |               |
+----------------------------------------------------------------------------|
+_Remarks_ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _             |
+                                                                            |
+_Substance_ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _             |
+----------------------------------------------------------------------------
+
+
+1. ~Aluminum, Al_{2}O_{3}.~--Before the Bp. on Ch. Infusible. No change.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Forms an infusible compound
+with slight intumescence.
+
+In ignition tube with Na_{2}CO_{3} and Ch. No change. Moisture driven
+off.
+
+In flame on platinum wire. No change. Becomes incandescent.
+
+In flame with borax bead. In O. F. dissolves slowly, forming a
+colorless glass which remains so on cooling.
+
+With Co(NO_{3})_{2}. Mass becomes blue upon re-ignition.
+
+
+2. ~Antimony, Sb_{2}O_{3}.~--Before the Bp. on Ch. In O. F. volatilizes
+without change. In R. F. is reduced and volatilized. White coating of
+antimonious oxide deposited on Ch. Blue tinge imparted to flame.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Readily reduced. White brittle
+bead. Very volatile, giving characteristic white coating.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Volatilized.
+
+In flame on platinum wire. Volatilized. Colors flame greenish blue.
+
+With borax bead on platinum wire. In O. F. dissolves to a colorless
+glass.
+
+With Co(NO_{3})_{2}.____
+
+
+3. ~Arsenic, As_{2}O_{3}.~--Before the Bp. on Ch. Very volatile. Strong
+garlic odor to fumes.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced with emission of
+arsenical fumes.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Volatilizes, forming a
+mirror-like deposit of metallic As in the cooler part of tube.
+
+In flame on platinum wire____
+
+With borax bead on platinum wire____
+
+With Co(NO_{3})_{2}.____
+
+
+4. ~Bismuth, Bi_{2}O_{3}.~--Before the Bp. on Ch. Yields a
+coating--orange-yellow when hot, lemon-yellow when cold. The yellow
+coating usually has a white outline.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Easily reduced to metallic
+bismuth. Yellow bead brittle, but less so than antimony.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. small quantity dissolves to a
+clear yellow glass, which becomes colorless when cold.
+
+With Co(NO_{3})_{2}____
+
+
+5. ~Cadmium, CdO.~--Before the Bp. on Ch. Gives a coating on the coal.
+Reddish-brown when cold. Very volatile.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Readily reduced. The metal
+volatilizes easily, giving the characteristic coating.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead. In O. F. dissolves to a clear yellowish bead, colorless
+when cold.
+
+With Co(NO_{3})_{2}____
+
+
+6. ~Chromium, Cr_{2}O_{3}.~--Before the Bp. on Ch. No change.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Cannot be reduced. Soda sinks
+in Ch. and a green colored mass remains.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+
+~With borax bead.~ Dissolves slowly but colors intensely. Yellow while
+hot, green when cold.
+
+With microcosmic salt bead. Colors red when hot, green when cold.
+
+With Co(NO_{3})_{2}____
+
+
+7. ~Cobalt, CoO.~--Before the Bp. on Ch. In O. F. unchanged. In R. F. is
+reduced to the metal and is magnetic.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced to a gray magnetic
+mass.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. colors very intensely blue,
+both hot and cold.
+
+With Co(NO_{3})_{2}____
+
+
+8. ~Copper, CuO.~--Before the Bp. on Ch. Fuses to a black globule, which
+can be reduced with some difficulty.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Readily reduced to metallic
+bead, which is red in color, hard, malleable.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire. Colors flame emerald-green.
+
+With borax bead on platinum wire. In O. F. green when hot, blue when
+cold.
+
+With Co(NO_{3})_{2}____
+
+
+9. ~Iron, Fe_{2}O_{3}.~--Before the Bp. on Ch. In O. F. unchanged. In R.
+F. becomes black and magnetic.
+
+Before the Bp. on Ch. with Na_{2}CO_{3} Reduced to a metallic powder,
+magnetic.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. red while hot, yellow when
+cold.
+
+With Co(NO_{3})_{2}____
+
+
+10. ~Lead, PbO.~--Before the Bp. on Ch. Easily reduced to the metal, bead
+very malleable. Coating yellow, surrounded by white ring.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Instantly reduced. Coats the
+Ch. upon further blowing.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Reduced to the metal.
+
+In flame on platinum wire. Tinges flame blue.
+
+With borax bead on platinum wire. In O. F. dissolves easily, forming a
+limpid glass.
+
+With Co(NO_{3})_{2}____
+
+
+11. ~Manganese, Mn_{2}O_{3}.~--Before the Bp. on Ch. At high temperature
+turns red.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Is not reduced.
+
+Before the Bp. in O. F. on platinum foil with Na_{2}CO_{3}. Transparent
+green mass when hot. Opaque, bluish-green when cold.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Not reduced.
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. violet-red while hot,
+amethyst-red when cold.
+
+With Co(NO_{3})_{2}____
+
+
+12. ~Mercury, HgO.~--Before the Bp. on Ch. Instantly reduced. Very
+volatile.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced and volatilized.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Sublimes condensing in the
+upper part of the tube as a metallic ring which is seen with the lens to
+consist of minute globules of mercury.
+
+In flame on platinum wire____
+
+With borax bead on platinum wire____
+
+With Co(NO_{3})_{2}____
+
+
+13. ~Nickel, NiO.~--Before the Bp. on Ch. In O. F. unchanged. In R. F.
+reduced to metal, slightly magnetic.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Easily reduced to the metal.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. violet while hot,
+reddish-brown when cold.
+
+With Co(NO_{3})_{2}____
+
+
+14. ~Silver, AgO.~--Before the Bp. on Ch. Easily reduced to the metal.
+White, malleable, hard bead. Coats the coal dark red near assay.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Instantly reduced to metallic
+globule.
+
+In ignition tube with Na_{2}CO_{3} and Ch. Reduced to the metal.
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. partially dissolved. Bead
+becomes milk-white.
+
+With Co(NO_{3})_{2}____
+
+
+15. ~Tin, SnO_{2}.~--Before the Bp. on Ch. Coats the coal yellow while
+hot, dirty white when cool. Not reduced.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced to metallic tin. White,
+hard, malleable bead. Coating white and close to assay.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. small quantity dissolves to
+limpid glass.
+
+With Co(NO_{3})_{2}. Greenish-blue color.
+
+
+16. ~Zinc, ZnO.~--Before the Bp. on Ch. Upon ignition becomes yellow. Is
+not reduced.
+
+Before the Bp. on Ch. with Na_{2}CO_{3}. Reduced to metal. Rapidly
+volatilized, coating the coal white.
+
+In ignition tube with Na_{2}CO_{3} and Ch.____
+
+In flame on platinum wire____
+
+With borax bead on platinum wire. In O. F. yellow while hot, limpid
+glass when cold.
+
+With Co(NO_{3})_{2}. Green mass.
+
+Having now given the principal reactions for the most important metals,
+we will proceed to the examination of the alkali metals, the alkaline
+earths, and some of the acid elements.
+
+
+THE ALKALI METALS
+
+17. ~Ammonium, NH_{4}.~--This hypothetical compound is commonly classed
+among the alkali metals from its close resemblance to the members of
+this group.
+
+To detect the presence of this hypothetical metal, mix the assay with
+about four parts of Na_{2}CO_{3}, place in an ignition tube, and apply
+heat. The odor of the evolved gas will be recognized, and if a piece of
+red litmus paper be moistened and held at the mouth of the tube, it will
+be turned blue by the escaping ammonia gas.
+
+We are not authorized to infer the pre-existence of ammonium, however,
+from the appearance of this reaction, for the presence of nitrogenous
+organic matter in the substance, which would be decomposed by this
+treatment, would give rise to such a reaction.
+
+
+18. ~Potassium.~--Potassium is recognized by the color which its salts
+impart to the Bunsen flame. If a portion of a salt of potassium be held
+on a platinum wire in the flame, it imparts a blue-violet tint which
+rapidly disappears.
+
+
+19. ~Sodium.~--Like potassium, this alkali metal is detected by the color
+which its salts give to the flame.
+
+If a sodium salt be held on the platinum wire in the flame, it imparts
+an intense yellow color.
+
+The extreme delicacy of this reaction has been mentioned elsewhere. The
+value of this test is really lessened by its great delicacy, for it is
+possible to detect minute quantities of sodium in almost all substances,
+although it may not be in chemical combination. As an example, draw the
+platinum wire between the fingers, and then place in flame, and note
+presence of sodium.
+
+
+20. ~Lithium, Li_{2}O.~--In the Bunsen flame on the platinum wire it
+imparts a carmine-red tinge.
+
+Hydrochloric acid on the sample augments the coloration.
+
+
+THE ALKALINE EARTHS
+
+21. ~Barium, BaO.~--In the Bunsen flame on the platinum wire it imparts an
+apple-green coloration. This reaction is intensified by moistening the
+sample with hydrochloric acid.
+
+
+22. ~Calcium, CaO.~--In the Bunsen flame on the platinum wire it imparts
+an orange-red color, which appears gray when seen through blue glass.
+
+Hydrochloric acid on the sample makes the color more intense.
+
+
+23. ~Strontium, SrO.~--In the Bunsen flame on the platinum wire it imparts
+an intensely red color, which is increased by converting the substance
+into the chloride.
+
+
+THE ACID ELEMENTS
+
+24. ~Borates.~--If the substance be finely powdered, moistened with
+glycerine, and then placed on a platinum wire in the Bunsen flame, it
+imparts a brilliant green color.
+
+If turmeric paper be dipped into a solution of a borate, and then be
+dried at 100 deg. C., it is turned to a peculiar red color. These two
+reactions are extremely delicate.
+
+
+25. ~Bromides.~--Bromides treated with microcosmic salt and oxide of
+copper on platinum wire impart to the flame a greenish-blue color, the
+edges being decidedly green.
+
+
+26. ~Chlorides.~--Chlorides are treated in the same way as bromides. The
+color imparted to the flame is azure-blue.
+
+To discriminate between bromides and chlorides more clearly, the
+substance is mixed with anhydrous potassium bisulphate and fused in an
+ignition tube.
+
+Bromine and sulphur dioxide are evolved (if the substance be a bromide),
+the tube being filled with a yellow gas possessing the characteristic
+odor of bromine.
+
+
+27. ~Fluorides.~--A small portion of the substance in a finely powdered
+condition is placed in one of the ignition tubes, a strip of moist
+Brazil-wood paper is introduced into the open end, and heat is applied.
+Hydrofluoric acid is evolved, and the red color of the paper is changed
+into a straw-yellow.
+
+Mica, containing only 0.75% of fluorine, shows the reaction clearly.
+
+
+28. ~Iodides.~--Iodides are treated, as the bromides and chlorides, in a
+bead of microcosmic salt with oxide of copper. The flame is colored
+green.
+
+Fused with potassium bisulphate in an ignition tube the violet vapors of
+iodine are evolved, and thus iodides may be distinguished from chlorides
+and bromides.
+
+
+29. ~Nitrates.~--If a nitrate be heated upon charcoal before the Bp.,
+violent deflagration occurs. If the substance containing the nitric
+acid be mixed with a _very small_ quantity of finely powdered potassium
+cyanide, the deflagration is accompanied with ignition and detonation.
+
+If the substance be mixed in a dry condition with dry potassium
+bisulphate, and is then heated in an ignition tube, red-brown nitrous
+fumes are evolved. This reaction takes place if there is but a small
+quantity of nitrate present.
+
+
+30. ~Phosphates.~--Phosphates impart to the flame a bluish green color.
+The color is made more intense by moistening the substance with
+sulphuric acid, and then taking the paste so formed on the platinum wire
+and placing it in the Bunsen flame.
+
+
+31. ~Silicates.~--Silicates, when treated with microcosmic salt on a
+platinum wire, suffer decomposition; the bases unite with the
+phosphoric acid to form a transparent glass in which the silica may be
+seen floating as a cloudy mass.
+
+The bead must only be examined for silica while hot, since on cooling it
+becomes opaque.
+
+
+32. ~Sulphides.~--Many sulphides, when heated in an ignition tube,
+volatilize and give a sublimate of sulphur in combination with the
+metallic portion of the substance.
+
+A very delicate test for sulphur in whatever combination it may be found
+in a substance, and which may be performed with great ease, is to mix
+the finely powdered assay with four parts, Na_{2}CO_{3}, and fuse in an
+ignition tube. When thoroughly fused the tube is broken, and the fused
+mass is placed on a bright silver coin, and a drop of water is added.
+If the substance contains sulphur, a black spot will be observed on the
+coin where the fused mass was placed.
+
+Before going on to the next chapter, the student should assure himself
+of his familiarity with the reactions just given, and he should practise
+with various substances, the nature of which is unknown to him.
+
+
+
+
+CHAPTER IV
+
+BEHAVIOR OF SOME OF THE PRINCIPAL ORES BEFORE THE BLOWPIPE
+
+
+For the sake of practice, and as a fitting introduction to
+"Determinative Mineralogy," this chapter is appended. It is not intended
+to give a detailed account of the minerals, but rather to set before the
+student the most marked characters, such as hardness, specific gravity,
+color, lustre, etc.
+
+To determine the hardness of a mineral, we try to scratch it with the
+minerals forming an arbitrary "scale of hardness," proceeding
+successively from the softest to the hardest. When we say that a certain
+mineral has hardness = 4, we mean that the mineral is scratched by 4 on
+the scale, and that 4 on the scale is scratched by the mineral. The
+scale of hardness chiefly in use is the Mohs-Breithaupt scale, which is
+as follows:--
+
+    1. Talc, common laminated light green variety.
+
+    2. Gypsum, crystallized.
+
+    3. Calcareous spar, transparent variety.
+
+    4. Fluor spar, crystalline.
+
+    5. Apatite, transparent.
+
+    6. Orthoclase, white cleavable variety.
+
+    7. Quartz, transparent.
+
+    8. Topaz, transparent.
+
+    9. Sapphire, cleavable variety.
+
+    10. Diamond.
+
+It seldom happens in determining the hardness of a mineral that its
+hardness exactly conforms to that of some one member of the scale. In
+such cases we generally estimate the hardness. For example, suppose a
+mineral was harder than 4, but softer than 5, and that it was nearer 5
+than 4, then we would call its hardness 4-3/4.
+
+In order to preserve the scale some operators use a three-cornered file,
+first cutting the mineral and then the scale until a number is found,
+which is abraded to about the same depth as the mineral under
+examination.
+
+Since a set of minerals forming a scale of hardness is not always at
+hand, the following scale given by Chapman is appended:--
+
+     1. Yields easily to the nail.
+
+     2. Yields with difficulty to the nail or just receives an
+     impression from it. Does not scratch a copper coin.
+
+     3. Scratches a copper coin but is also scratched by it,
+     being of about the same degree of hardness.
+
+     4. Not scratched by a copper coin. Does not scratch glass.
+
+     5. Scratches glass with difficulty, leaving its powder on
+     it. Yields readily to the knife.
+
+     6. Scratches glass easily. Yields with difficulty to the
+     knife.
+
+     7. Does not yield to the knife. Yields to the edge of a
+     file, though with difficulty.
+
+     8, 9, 10. Harder than flint.
+
+Specific gravity cannot well be determined without the aid of a balance,
+and hence its value here is not great.
+
+As in the preceding chapter, alphabetic arrangement will be employed.
+
+
+ORES OF ANTIMONY
+
+~Stibnite~, Sb_{2}S_{3}, Sb . 71, S . 29.--[A]H = 2, G = 4.52-4.62. Of
+lead-gray color and metallic lustre. Consists of a large number of
+needle-shaped crystals. Brittle. Fuses in candle flame. In an ignition
+tube yields a sublimate of sulphur. On Ch. before the Bp. it is
+volatilized, giving antimony coating and tinges the flame pale blue.
+
+[Footnote A: H = Hardness, G = Specific Gravity.]
+
+
+ORES OF ARSENIC
+
+~Native Arsenic, As.~--This contains traces of Sb, Ag, Fe, Co, and Ni.
+
+H = 3.5, G = 5.7-5.8. Dark gray in color. Fracture tin-white, tarnishing
+rapidly. Volatilizes before the Bp. on Ch. without melting, giving white
+coating of arsenious acid and characteristic garlic odor. In ignition
+tube it sublimes, giving arsenical ring.
+
+
+~Realgar~, AsS, As . 70, S . 30.--H = 1.5-2, G = 3.56. Bright red to
+orange-red color and resinous lustre. In an ignition tube it fuses and
+finally sublimes. The sublimate when cool is red and transparent. Fuses
+readily before the Bp. on Ch. and burns with pale yellowish flame,
+emitting gray-white fumes having garlic odor.
+
+
+~Orpiment~, As_{2}S_{3}, As . 61, S . 39.--
+
+    H = 1.5-2.0, G = 3.4-3.5.
+
+Lemon-yellow in color and resinous or pearly lustre. Sectile. Before the
+Bp. on Ch. behaves like realgar, but in an ignition tube it gives a dark
+yellow sublimate which is transparent.
+
+
+ORES OF BISMUTH
+
+~Native Bismuth, Bi.~--This contains traces of As, Te, and S.
+
+H = 2.0-2.5, G = 9.7-9.83. Color, silver-white, slightly tinged with
+red. Metallic lustre. Brittle when cold, but may be laminated when hot.
+Before the Bp. on Ch. behaves like pure Bi.
+
+
+~Bismuthite~, Bi_{2}O_{3} . 90, CO_{2} . 7, H_{2}O . 3,--
+
+    H = 4.0-4.5, G = 6.9-7.8.
+
+Usually of a white or light greenish color and vitreous lustre, in
+acicular crystallizations. In an ignition tube decrepitates, yielding
+water and turning gray. Before the Bp. on Ch. it fuses easily and is
+reduced to metallic globule, coating the Ch. with Bi_{2}O_{3}. With
+Na_{2}CO_{3} it occasionally gives the sulphur reaction.
+
+
+ORES OF CHROMIUM
+
+~Chromic Iron Ore~, FeO . 32, Cr_{2}O_{3} . 68.--Al_{2}O_{3}, Fe_{2}O_{3},
+MnO, and MgO are commonly present. H = 5.5, G = 4.32-4.57. Occurs
+usually massive. Color, iron-black to brownish black. In many varieties
+strongly magnetic. Lustre, shining and somewhat metallic. Heated in an
+ignition tube, remains unchanged. Infusible before the Bp. on Ch.
+Before the Bp. on Ch. with Na_{2}CO_{3} and KCN yields metallic iron. In
+borax bead it slowly dissolves to a clear transparent glass, which is a
+beautiful green when cool.
+
+
+ORES OF COBALT
+
+~Smaltite~, Co(Fe, Ni) As_{2}, Co . 28, As . 72.--H = 5.5, G = 6.37-7.30.
+Color, tin-white or steel-gray. Lustre, metallic. When heated to redness
+in an ignition tube it yields a sublimate of metallic arsenic. Before
+the Bp. on Ch. it fuses readily, with emission of arsenical fumes, to a
+grayish black magnetic globule. This globule may be examined for iron,
+cobalt, and nickel with the borax bead.
+
+
+~Cobaltite~, CoS_{2} + CoAs_{2}, Co . 36, As . 45, S . 19.--H = 5.5, G =
+6.0-6.3. Color, silver-white tinged with red. Metallic lustre. Before
+the Bp. on Ch. fuses easily, with emission of copious arsenical fumes,
+to a gray magnetic globule. Remains unchanged in the ignition tube.
+
+
+~Linnaeite~, (Co, Ni)_{3}S_{4}, (Co, Ni)58, S . 42.--H = 5.5, G = 4.8-5.0.
+Color, bright steel-gray, sometimes reddish. Lustre, metallic.
+Crystallizes in the regular octahedron. Before the Bp. on Ch. fuses to a
+metallic globule which is attracted by the magnet. With borax bead gives
+reaction for cobalt.
+
+
+~Erythrite~, Co_{3}O_{8}As_{2} + 8 H_{2}O, As_{2}S_{5} . 38.4, CoO . 37.6,
+H_{2}O . 24.0.--
+
+    H = 1.5-2.0, G = 2.95.
+
+Color, crimson to peach-red. When crystallized, of pearly lustre, but
+frequently dull and earthy. Heated in ignition tube gives off water, and
+color changes to blue or green. Before the Bp. on Ch. in R. F. it emits
+arsenical fumes and melts to a dark gray globule which with the borax
+bead reacts for cobalt.
+
+
+ORES OF COPPER
+
+~Native Copper, Cu.~--
+
+    H = 2.5-3, G = 8.5-8.9.
+
+Color, copper-red. Lustre, metallic. Occurs usually massive and very
+arborescent. Before the Bp. on Ch. it fuses, and if the heat is
+sufficiently high it assumes a bright bluish-green surface; on cooling
+it is covered with a coat of black oxide. In the borax bead it reacts
+for copper.
+
+
+~Chalcopyrite~, CuFeS_{2}, Cu . 35, Fe . 30, S . 35.--H = 3.5-4, G =
+4.1-4.3. Color, brass-yellow, often golden-yellow. Lustre, metallic.
+Occurs crystallized, but is generally found massive. Is easily
+scratched with a knife. Heated in an ignition tube decrepitates, and
+occasionally yields a faint sublimate of sulphur. Before the Bp. on Ch.
+it blackens, but becomes red again on cooling. Before the Bp. on Ch.
+with Na_{2}CO_{3} and KCN it is reduced, and the metals are obtained in
+separate masses. It reacts with the borax bead for copper and iron.
+
+
+~Copper Glance~, Cu_{2}S, Cu . 80, S . 20.--H = 2.5-3.0, G = 5.5-5.8.
+Color, dark blue to steel-gray. Occurs in compact masses, often very
+shining. Before the Bp. on Ch. fuses to a globule which boils and emits
+glowing drops. Sulphur dioxide escapes abundantly, and the outer flame
+is colored blue. Before the Bp. on Ch. with Na_{2}CO_{3} yielding a
+metallic globule.
+
+
+~Tetrahedrite~, 4 CuS + Sb_{2}S_{3}.--Frequently contains silver, iron,
+mercury, and zinc. H = 3.0-4.0, G = 4.5-5. Color, steel-gray to
+iron-black. Heated in an ignition tube fuses and gives a sublimate of
+antimonious oxide. When mercury is present this condenses in the upper
+part of the tube, forming the characteristic mirror. Before the Bp. on
+Ch. it fuses readily to a metallic globule, emitting dense white fumes;
+zinc and antimony coatings are deposited on the Ch. After long ignition
+before the Bp., if the mineral is finely powdered and mixed with
+Na_{2}CO_{3} and KCN, the ore is reduced to the metal.
+
+
+~Cuprite~, Cu_{2}O, Cu . 89, O . 11.--
+
+    H = 3.5-4.0, G = 5.5-6.15.
+
+Color, intense crimson-red. Before the Bp. on Ch. blackens and fuses
+quietly, and finally yields a metallic globule of copper. Before the Bp.
+on Ch. with Na_{2}CO_{3} and KCN it is easily reduced.
+
+
+~Malachite~, 2 CuO + CO_{2} + H_{2}O, CuO . 72, CO_{2} . 20, H_{2}O . 8.--
+
+    H = 3.5-4.0, G = 3.90-4.03.
+
+Color, bright green. Occurs generally in mammillated concretions.
+Lustre, shining and fracture, silky. Heated in an ignition tube yields
+water and blackens. Before the Bp. on Ch. it fuses to a metallic
+globule. Before the Bp. on Ch. with Na_{2}CO_{3} and KCN it is easily
+reduced. With borax bead gives characteristic coloration.
+
+
+~Azurite~, 3 CuO + 2 CO_{2} + H_{2}O, CuO . 69, CO_{2} . 26, H_{2}O . 5.--
+
+    H = 3.5-4.0, G = 3.77-3.83.
+
+Color, azure-blue. Occurs usually in crystallized or globular masses.
+Lustre, earthy or vitreous. Before the Bp. and with other reagents
+behaves like malachite.
+
+
+~Chrysocolla~, CuO + SiO_{2} + 2 H_{2}O, SiO_{2} . 34.2, CuO . 45.3,
+H_{2}O . 20.5.--H = 2.0-3.0, G = 2. Color, bluish-green, closely
+resembling malachite. Occurs usually as an incrustation, its surface
+being very smooth, like enamel. In an ignition tube it blackens and
+yields water. Before the Bp. on Ch. in O. F. it blackens, coloring the
+flame bright green; in the R. F. it turns red. Before the Bp. on Ch.
+with Na_{2}CO_{3} yields metallic copper. In borax bead it reacts for
+copper.
+
+
+~Atacamite~, CuCl_{2} + 3 CuO_{2}H_{2}--Cl . 16.6, O . 20.3, Cu . 50.1,
+H_{2}O . 13.0.--
+
+    H = 3.0-3.5, G = 3.75-3.77.
+
+Color, green to blackish green. Lustre, adamantine to vitreous. In an
+ignition tube yields water. Before the Bp. on Ch. colors flame blue.
+Before the Bp. on Ch. with Na_{2}CO_{3} and KCN is reduced to the metal.
+In borax bead it reacts for copper.
+
+
+ORES OF IRON
+
+~Limonite~, 2 Fe_{2}O_{3} + 3 H_{2}O, Fe_{2}O_{3} . 86, H_{2}O . 14.--H =
+5.0-5.5, G = 3.6-4.0. Color, brown to ochre-yellow. Earthy or
+semi-metallic in appearance. In an ignition tube yields water. Before
+the Bp. on Ch. infusible. In borax bead reacts for iron.
+
+
+~Hematite~, Fe_{2}O_{3}, Fe . 70, O . 30.--
+
+    H = 5.5-6.5, G = 4.9-5.3.
+
+Color, dark steel-gray to iron-black. Lustre, metallic. When pulverized
+yields a red powder. Before the Bp. on Ch. infusible. After long
+roasting becomes magnetic. In borax bead gives usual indications of
+iron.
+
+
+~Magnetite~, Fe_{3}O_{4}, FeO . 31, Fe_{2}O_{3} . 69.--
+
+    H = 5.5-6.5, G = 5.17-5.18.
+
+Color, iron-black. Lustre, shining and metallic. Pulverized, its powder
+is black. It is strongly magnetic. Fuses with difficulty before the Bp.
+on Ch. In borax bead reacts for iron.
+
+
+~Pyrites~, FeS_{2}, Fe . 47, S . 53.--
+
+    H = 6.0-6.5, G = 4.95-5.20.
+
+Color, brass-yellow. Lustre, metallic. Occurs commonly in cubes. It
+often contains small quantities of Au, Ag, Cu, As, Co, and Mn. Heated in
+an ignition tube gives a sublimate of sulphur, the residue becoming
+magnetic. Before the Bp. on Ch. in O. F. sulphur is burned off and the
+red oxide remains. This residue may then be examined for iron, etc.
+
+
+~Marcasite~ (White Iron Pyrites).--Having the same general composition as
+pyrite, but much lighter in color. Crystals, prismatic. Before the Bp.
+on Ch. behaves like pyrite.
+
+
+~Pyrrhotite~, Fe_{7}S_{8}, Fe . 60.5, S . 39.5.--
+
+    H = 3.5-4.5, G = 4.58-4.64.
+
+Color, bronze-yellow. Closely resembles pyrite, but may be distinguished
+from it by being feebly magnetic. Heated in an ignition tube yields no
+sublimate. Before the Bp. on Ch. fuses to a magnetic globule, which
+exhibits a yellowish crystalline structure when fractured.
+
+
+~Mispickel~, FeAsS, Fe . 34, As . 46, S . 20.--H = 5.5-6.0, G = 6.0-6.2.
+Color, silver-white. Lustre, metallic; very brittle. Often associated
+with it we find small quantities of Co, Ag, and Au. Heated in an
+ignition tube it first yields a red sublimate of sulphide of arsenic,
+and then afterward a crystalline sublimate of metallic arsenic. Before
+the Bp. on Ch. emits dense fumes of arsenic and deposits a coating on
+the coal; it then fuses to a globule which behaves like pyrrhotite.
+
+
+~Siderite~, FeCO_{3}, FeO . 62, CO_{2} . 38.--H = 3.5-4.5, G = 3.7-3.9.
+Color, grayish yellow to reddish brown. Lustre, pearly. Crystallizes in
+rhombohedrons with curved faces; these crystals are distinctly cleavable
+and massive. Heated in an ignition tube it decrepitates with evolution
+of carbon dioxide. Before the Bp. on Ch. infusible. Before the Bp. on
+Ch. with Na_{2}CO_{3} it fuses to a magnetic mass. With borax bead it
+reacts for iron and sometimes for manganese.
+
+
+ORES OF LEAD
+
+~Galena~, PbS, Pb . 87, S . 13.--
+
+    H = 2.5, G = 7.4-7.6.
+
+Color, bluish gray, slowly tarnishing. Lustre, metallic. Crystals in the
+form of cubes. Heated in an ignition tube it sometimes decrepitates and
+yields a sublimate of sulphur. Before the Bp. on Ch. easily reduced to
+the metallic state, the Ch. becoming coated with sulphate and oxide of
+lead. The metallic globule usually contains a little silver. To separate
+this, the process known as "cupellation" is employed. A hole is bored
+into the Ch. about 1 cm. in diameter and about 6 mm. deep. Into this
+hole is placed a stiff paste made by mixing finely pulverized bone-ash
+with a little soda and water. This paste is pressed in hard, and then
+the surface is smoothed off, and the centre is slightly depressed with
+the rounded end of a glass rod. The charcoal so prepared is set in a
+warm place to allow the paste to dry. When the paste is quite dry the
+small globule of lead is placed in the depression in the centre of the
+bone-ash "cupel," and is there exposed to the O. F. from the Bp. The
+lead is oxidized and is absorbed by the bone-ash, while any silver
+present will remain in the central depression as a bright shining bead.
+
+
+~Cerusite~, PbCO_{3}, PbO . 84, CO_{2} . 16.--H = 3.0-3.5, G = 6.46-6.57.
+Color, white, gray, or yellow. Lustre, adamantine. Crystallizes in
+prismatic needles. When heated in an ignition tube carbon dioxide is
+evolved and the residue turns yellow. Before the Bp. on Ch. readily
+reduced to metallic lead.
+
+
+~Anglesite~, PbSO_{4}, PbO . 74, SO_{3} . 26.--H = 2.0-3.0, G = 6.12-6.39.
+Color, yellow, gray, and brown. Lustre, adamantine, resinous. Heated in
+an ignition tube decrepitates, and sometimes yields a little water.
+Before the Bp. on Ch. fuses to a clear bead, which on cooling becomes
+opaque. Before the Bp. on Ch. with Na_{2}CO_{3} is reduced to the metal
+giving a yellow coating. The Na_{2}CO_{3} absorbed by the coal reacts
+for S.
+
+
+ORES OF MANGANESE
+
+~Pyrolusite~, MnO_{2}, Mn . 63.2, O . 36.8.--H = 2.0-2.5, G = 4.82. Color,
+iron-black to steel-gray. Lustre, non-metallic. Heated in an ignition
+tube yields generally a little water, and if the temperature be high
+enough, oxygen is evolved. Before the Bp. on Ch. infusible. In borax
+bead gives characteristic color.
+
+
+~Psilomelane~, Mn_{2}O_{3} + H_{2}O.--
+
+    H = 5.5-6.0, G = 3.7-4.7.
+
+Color, iron-black to steel-gray. Generally resembles pyrolusite, but is
+distinguished from it by its superior hardness. It frequently contains
+BaO and Li_{2}O. It behaves before the Bp. like pyrolusite.
+
+
+~Wad~ (Bog Manganese).--This mineral is essentially MnO_{2}, MnO, and
+H_{2}O, with small quantities of Fe_{2}O_{3}, Al_{2}O_{3}, BaO, SiO_{2},
+etc., associated with it.
+
+H = 0.5-6.0, G = 3.0-4.2. Color, dull black. Heated in an ignition tube
+yields water in abundance, otherwise it behaves like pyrolusite.
+
+
+ORES OF MERCURY
+
+~Native Mercury, Hg.~--G = 13.5-13.6. Color, silver-white. Is liquid at
+all ordinary temperatures. Heated in an ignition tube is volatilized,
+the vapors condensing in the upper end of tube to small metallic
+globules of Hg. Before the Bp. on Ch. it is volatilized. Frequently
+contains Ag.
+
+
+~Cinnabar~, HgS_{2}, Hg . 86, S . 14.--
+
+    H = 2.0-2.5, G = 8.0-8.2.
+
+Color, scarlet-red to brick-red. Lustre, non-metallic. When pulverized
+yields a powder of vermilion-red color. Heated in an ignition tube it
+volatilizes, yielding a black sublimate, which by friction becomes red.
+Before the Bp. on Ch. it is wholly volatilized. Heated in an ignition
+tube with Na_{2}CO_{3} metallic mercury sublimes, condensing in the
+upper portion of the tube in minute globules.
+
+
+ORES OF NICKEL
+
+~Millerite~, NiS, Ni . 64.4, S . 35.6.--
+
+    H = 3.0-3.5, G = 5.2-5.6.
+
+Color, brass-yellow. Brittle. Before the Bp. on Ch. it fuses to a
+magnetic, metallic globule. The roasted mineral gives in the borax bead
+the color reaction characteristic of nickel, and sometimes that of
+cobalt, which is often associated with it.
+
+
+~Niccolite~, NiAs, Ni . 44, As . 56.--
+
+    H = 5.0-5.5, G = 7.35-7.67.
+
+Color, pale copper-red. Lustre, metallic. Very brittle. Heated in an
+ignition tube yields a copious sublimate of arsenious oxide, the residue
+falling to a greenish powder. Before the Bp. on Ch. fuses to a white
+brittle globule emitting arsenical fumes. In borax bead gives color
+characteristic of nickel. Frequently in this mineral a portion of the
+arsenic is replaced by antimony.
+
+
+ORES OF SILVER
+
+~Native Silver, Ag.~--
+
+    H = 2.5-3.0, G = 10.1-11.0.
+
+Color, silver-white. Lustre, metallic. Ductile and malleable. Usually
+occurs associated with Au, As, Sb, Cu, Fe, etc. Before the Bp. on Ch.
+easily fuses to a globule which is surrounded with a dark red coating on
+the coal.
+
+
+~Argentite~, Ag_{2}S, Ag . 87.1, S . 12.9.--
+
+    H = 2.0-2.5, G = 7.20-7.36.
+
+Color, blackish lead-gray. Lustre, metallic. Very sectile. Before the
+Bp. on Ch. in O. F. intumesces with evolution of sulphur dioxide,
+finally yielding a metallic globule of Ag.
+
+
+~Pyrargyrite~, Ag_{3}SbS_{3}, Ag . 59.8, Sb . 22.5, S . 17.7.--H = 2.5, G
+= 5.77-5.86. Color, black to dark cochineal-red. Lustre, metallic,
+adamantine. In an ignition tube it yields on continued heating a
+sublimate of antimony sulphide. Before the Bp. on Ch. it gives a coating
+of antimony trioxide. Before the Bp. on Ch. with Na_{2}CO_{3} is
+reduced to metallic silver.
+
+
+~Proustite~, Ag_{3}S_{3}As, Ag . 65.5, As . 15.1, S . 19.4.--H = 2.0-2.5,
+G = 5.57-5.64. Color, light red. Lustre, splendent, adamantine. Before
+the Bp. on Ch. it behaves like pyrargyrite, save that it gives off
+arsenical fumes instead of antimonious oxide.
+
+
+~Stephanite~, Ag_{5}S_{4}Sb, Ag . 68.5, Sb . 15.3, S . 16.2.--H = 2.0-2.5,
+G = 6.2-6.3. Color, iron-black to blackish gray. Lustre, metallic. Very
+brittle and fragile. In an ignition tube it decrepitates, fuses, and
+finally yields a slight sublimate of antimony trisulphide. Before the
+Bp. on Ch. gives a coating of antimonious oxide. Before the Bp. on Ch.
+with Na_{2}CO_{3} a globule of metallic silver is obtained. The mineral
+frequently contains copper and iron.
+
+
+~Kerargyrite~, AgCl, Ag . 75.3, Cl . 24.7.--H = 1.0-1.5, G = 5.52. Color,
+white, gray, yellowish, greenish to blue. Lustre, resinous, adamantine.
+Soft like wax. Fuses easily in a candle-flame. Before the Bp. on Ch. it
+is readily reduced to metallic silver.
+
+
+ORES OF TIN
+
+~Cassiterite~, SnO_{2}, Sn . 79, O . 21.--
+
+    H = 6.0-7.0, G = 6.8-7.0.
+
+Color, brown, black. Lustre, adamantine, brilliant. Occurs crystallized
+in square prisms. Reentrant angles characteristic. Before the Bp. on Ch.
+with Na_{2}CO_{3} and KCN reduced to a metallic globule of tin. In the
+borax bead gives characteristic reaction.
+
+
+~Stannite~, 2 Cu_{2}S . SnS_{2} + 2 (FeS . ZnS) Sn . S_{2}.--H = 4.0, G =
+4.3-4.5. Color, steel-gray to iron-black. Lustre, metallic. Occurs
+usually massive and disseminated. Heated in an ignition tube it yields
+sulphur dioxide. Before the Bp. on Ch. it emits sulphur dioxide and
+becomes covered with oxide of tin. Before the Bp. on Ch. with
+Na_{2}CO_{3} and KCN it gives an impure globule of copper. A very
+difficult mineral to determine.
+
+
+ORES OF ZINC
+
+~Calamine~, H_{2}Zn_{2}O_{5}Si, SiO_{2} . 25.0, ZnO . 67.5, H_{2}O .
+7.5.--H = 4.5-5.0, G = 3.4-3.5. Color, white, gray, bluish, or brown.
+Lustre, vitreous. Brittle. In an ignition tube yields water when heated
+and becomes milky white. Before the Bp. on Ch. practically infusible.
+With Co(NO_{3})_{2} it assumes a green color which passes into a fine
+blue when the heat is increased.
+
+
+~Smithsonite~,
+
+    Zn . CO_{3}, ZnO . 64.8, CO_{2} . 35.2.--
+
+H = 5, G = 4.30-4.45. Color, gray, yellow, brown, and green. Lustre,
+vitreous, pearly. Heated in an ignition tube CO_{2} is evolved, residue
+appearing white. It often contains impurities of Cd, Pb, Fe, Mn, Ca, and
+Mg. When these are present the residue in the ignition tube becomes dark
+on cooling. Before the Bp. on Ch. with Na_{2}CO_{3} and exposed to the
+R. F. it is decomposed. It gives the characteristic reaction for zinc
+with Co(NO_{3})_{2}.
+
+
+~Zincite~, ZnO, Zn . 80.3, O . 19.7--
+
+    H = 4.0-4.5, G = 5.43-5.70.
+
+Color, blood-red. Lustre, brilliant, subadamantine. Before the Bp. on
+Ch. infusible. Before the Bp. on Ch. with Na_{2}CO_{3} gives coating of
+zinc oxide. Gives characteristic reaction with Co(NO_{3})_{2}. It
+frequently contains a small quantity of Mn_{2}O_{3}, which may be
+detected in the borax bead.
+
+
+~Sphalerite~, ZnS, Zn . 67, S . 33.--
+
+    H = 3.5-4.0, G = 3.9-4.1.
+
+Color, yellow to black. Lustre, resinous, brilliant, and sometimes
+submetallic. Heated in an ignition tube sometimes decrepitates. Before
+the Bp. on Ch. infusible. Before the Bp. on Ch. with Na_{2}CO_{3} easily
+reduced. With Co(NO_{3})_{2} gives the characteristic reaction. It
+frequently contains small quantities of Cd, Hg, Sn, Pb, Au, Ag, etc.
+
+
+I
+
+TABLE OF COLORS OF COATINGS ON CHARCOAL
+
+--------------------------------------------------
+ Element |    Color Hot           | Color Cold    |
+---------|------------------------|---------------|
+Antimony | (Rather volatile)      | White         |
+         |                        |               |
+Arsenic  | (Very volatile)        | White         |
+         |                        |               |
+Bismuth  | Orange-Yellow          | Lemon-Yellow  |
+         |                        |               |
+Cadmium  | Brownish Yellow        | Reddish Brown |
+         |                        |               |
+Lead     | Lemon-Yellow (volatile)| Lemon-Yellow  |
+         |                        |               |
+Silver   | Dark Red               | Dark Red      |
+         |                        |               |
+Tin      | Faint Yellow           | White         |
+         |                        |               |
+Zinc     | Yellow                 | White         |
+--------------------------------------------------
+
+
+II
+
+TABLE OF FLAME COLORATIONS
+
+------------------------------------
+  Red        |  Yellow  |  Green    |
+-------------|----------|-----------|
+Calcium      |  Sodium  |  Barium   |
+             |          |           |
+Lithium      |          |  Boron    |
+             |          |           |
+Strontium    |          |  Iodine   |
+-------------|----------|-----------|
+Bluish Green | Blue     |   Violet  |
+-------------|----------|-----------|
+Bromine      | Chlorine | Potassium |
+             |          |           |
+Copper       |          |           |
+             |          |           |
+Phosphorus   |          |           |
+------------------------------------
+
+
+III
+
+TABLE OF COLORS OF BORAX BEADS IN OXIDIZING FLAME
+
+---------------------------------------------------------
+ Element |    Color Hot           |    Color Cold       |
+---------|------------------------|---------------------|
+Aluminum |  Colorless to Cloudy   | Colorless to Cloudy |
+         |                        |                     |
+Antimony |  Yellowish             | Colorless           |
+         |                        |                     |
+Barium   | Colorless to Opaque    | Colorless to Opaque |
+         |                        |                     |
+Bismuth  | Yellow                 | Colorless           |
+         |                        |                     |
+Cadmium  | Yellow                 | Colorless to White  |
+         |                        |                     |
+Calcium  | Colorless              | Colorless           |
+         |                        |                     |
+Chromium | Reddish Yellow         | Yellowish Green     |
+         |                        |                     |
+Cobalt   | Blue                   | Blue                |
+         |                        |                     |
+Copper   | Green                  | Greenish Blue       |
+         |                        |                     |
+Iron     | Orange                 | Yellow              |
+         |                        |                     |
+Lead     | Yellow                 | Colorless           |
+         |                        |                     |
+Magnesium| Colorless              | Colorless           |
+         |                        |                     |
+Manganese| Violet                 | Reddish Violet      |
+         |                        |                     |
+Nickel   | Violet                 | Reddish Brown       |
+         |                        |                     |
+Silver   | Colorless              | Milk-White          |
+         |                        |                     |
+Strontium| Colorless to Opaque    | Colorless to Opaque |
+         |                        |                     |
+Tin      | Colorless              | Colorless           |
+         |                        |                     |
+Zinc     | Yellowish              | Colorless           |
+---------------------------------------------------------
+
+
+IV
+
+TABLE OF COLORS OF BORAX BEADS IN REDUCING FLAME
+
+------------------------------------------------
+Element    | Color Hot       | Color Cold      |
+------------------------------------------------
+Aluminum   | Colorless       | Colorless       |
+           |                 |                 |
+Antimony   | Colorless       | Cloudy          |
+           |                 |                 |
+Barium     | Colorless       | Colorless       |
+           |                 |                 |
+Bismuth    | Colorless       | Gray--Cloudy    |
+           |                 |                 |
+Cadmium    | Colorless       | Gray--Cloudy    |
+           |                 |                 |
+Calcium    | Colorless       | Colorless       |
+           |                 |                 |
+Chromium   | Green           | Green           |
+           |                 |                 |
+Cobalt     | Blue            | Blue            |
+           |                 |                 |
+Copper     | Colorless       | Red             |
+           |                 |                 |
+Iron       | Yellowish Green | Yellowish Green |
+           |                 |                 |
+Lead       | Colorless       | Gray            |
+           |                 |                 |
+Magnesium  | Colorless       | Colorless       |
+           |                 |                 |
+Manganese  | Colorless       | Pink            |
+           |                 |                 |
+Nickel     | Colorless       | Gray--Cloudy    |
+           |                 |                 |
+Silver     | Colorless       | Gray            |
+           |                 |                 |
+Strontium  | Colorless       | Colorless       |
+           |                 |                 |
+Tin        | Colorless       | Colorless       |
+           |                 |                 |
+Zinc       | Colorless       | Gray            |
+------------------------------------------------
+
+
+V
+
+TABLE OF COLORS OF MICROCOSMIC SALT BEADS IN OXIDIZING FLAME
+
+---------------------------------------------------
+ Element  |  Color Hot        | Color Cold         |
+---------------------------------------------------|
+Aluminum  | Colorless         | Colorless          |
+          |                   |                    |
+Antimony  | Yellowish         | Colorless          |
+          |                   |                    |
+Barium    |Colorless to Opaque| Colorless to Opaque|
+          |                   |                    |
+Bismuth   | Yellow            | Colorless          |
+          |                   |                    |
+Cadmium   | Yellowish         | Colorless          |
+          |                   |                    |
+Calcium   | Colorless         | Colorless to Opaque|
+          |                   |                    |
+Chromium  | Reddish           | Green              |
+          |                   |                    |
+Cobalt    | Blue              | Blue               |
+          |                   |                    |
+Copper    | Green             | Greenish Blue      |
+          |                   |                    |
+Iron      | Red               | Brownish Red       |
+          |                   |                    |
+Lead      | Yellowish         | Colorless          |
+          |                   |                    |
+Magnesium | Colorless         | Colorless          |
+          |                   |                    |
+Manganese | Brownish Violet   | Reddish Violet     |
+          |                   |                    |
+Nickel    | Reddish           | Yellow             |
+          |                   |                    |
+Silver    | Yellowish         | Yellowish          |
+          |                   |                    |
+Strontium | Colorless         | Colorless          |
+          |                   |                    |
+Tin       | Colorless         | Colorless          |
+          |                   |                    |
+Zinc      | Yellowish         | Colorless          |
+---------------------------------------------------
+
+
+VI
+
+TABLE OF COLORS OF MICROCOSMIC SALT BEADS IN REDUCING FLAME
+
++-----------+-------------+--------------+
+|  Element  |  Color Hot  |  Color Cold  |
+|-----------+-------------+--------------+
+| Aluminum  | Colorless   | Colorless    |
+|           |             |              |
+| Antimony  | Colorless   | Gray--Cloudy |
+|           |             |              |
+| Barium    | Colorless   | Colorless    |
+|           |             |              |
+| Bismuth   | Colorless   | Gray--Cloudy |
+|           |             |              |
+| Cadmium   | Colorless   | Gray--Cloudy |
+|           |             |              |
+| Calcium   | Colorless   | Colorless    |
+|           |             |              |
+| Chromium  | Reddish     | Green        |
+|           |             |              |
+| Cobalt    | Blue        | Blue         |
+|           |             |              |
+| Copper    | Dark Green  | Brownish Red |
+|           |             |              |
+| Iron      | Red         | Reddish      |
+|           |             |              |
+| Lead      | Colorless   | Gray--Opaque |
+|           |             |              |
+| Magnesium | Colorless   | Colorless    |
+|           |             |              |
+| Manganese | Colorless   | Colorless    |
+|           |             |              |
+| Nickel    | Colorless   | Gray         |
+|           |             |              |
+| Silver    | Colorless   | Gray         |
+|           |             |              |
+| Strontium | Colorless   | Colorless    |
+|           |             |              |
+| Tin       | Colorless   | Colorless    |
+|           |             |              |
+| Zinc      | Colorless   | Gray--Cloudy |
+------------+-------------+--------------+
+
+
+THE PRACTICAL METHODS
+
+OF
+
+ORGANIC CHEMISTRY
+
+AUTHORIZED TRANSLATION
+
+12mo. Cloth. Price, $1.60, _net_
+
+    BY                                            TRANSLATED BY
+    LUDWIG GATTERMANN, Ph.D.,                 WILLIAM SHAFER, Ph.D.,
+    _Professor in University_   _Instructor in Organic Chemistry_
+    _of Heidelberg._                       _in Lehigh University._
+
+       *       *       *       *       *
+
+THE GUARDIAN.
+
+     "The selection and judgment throughout is excellent. The
+     book is a most useful, practical adjunct to any good
+     text-book on organic chemistry."
+
+PHARMACEUTICAL REVIEW.
+
+     "This is a book that should be in the library of every
+     teacher of organic chemistry, and one which will no doubt be
+     of great value to students in their second year of organic
+     chemistry. Its chief peculiarity and merit is in the great
+     stress laid on practical laboratory work.... It is
+     permanently a worker's guide."
+
+NATURE.
+
+     "Since the advance of organic chemistry in this country
+     must, in a measure, depend on the nature of the available
+     text-books, both the author and the translator deserve our
+     thanks for providing us with a work such as the present
+     one."
+
+       *       *       *       *       *
+
+PUBLISHED BY
+THE MACMILLAN COMPANY
+66 FIFTH AVENUE, NEW YORK
+
+
+OUTLINES
+
+OF
+
+INDUSTRIAL CHEMISTRY
+
+A TEXT-BOOK FOR STUDENTS
+
+By FRANK HALL THORP, Ph.D.,
+
+_Instructor in Industrial Chemistry in the Massachusetts Institute of
+Technology._
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+Cloth. 8vo. Price, $3.50 _net_
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+       *       *       *       *       *
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+     The general arrangement and make-up of the book is
+     excellent, and ... altogether the book fills well a need
+     long felt by teachers of Industrial Chemistry.
+
+     I shall adopt the book for my class and shall take pleasure
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+CHARLES E. COATES, Jr., Ph.D.,
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+_Professor of Chemistry, Louisiana State University._
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+     "I have examined it carefully and think it a most excellent
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+     I have introduced it in this year's classes."
+
+W. A. NOYES, in _Science_.
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+     "The descriptions of processes, while necessarily concise,
+     are clear and interesting. The author has evidently made a
+     careful study of recent methods of manufacture as well as of
+     older, standard processes. The frequent reference to
+     American practice is an important feature which
+     distinguishes the book from other works on chemical
+     technology. A select bibliography follows each subject, and
+     will be found very useful."
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