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diff --git a/.gitattributes b/.gitattributes new file mode 100644 index 0000000..6833f05 --- /dev/null +++ b/.gitattributes @@ -0,0 +1,3 @@ +* text=auto +*.txt text +*.md text diff --git a/32974-8.txt b/32974-8.txt new file mode 100644 index 0000000..6ab1d75 --- /dev/null +++ b/32974-8.txt @@ -0,0 +1,2415 @@ +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.... 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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 & 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 & Co.—Berwick & 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,—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>—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>—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>—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>—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:—</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 × 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—for metallic beads, etc.<br /></span> +</div></div> + + +<p><b>Chemicals.</b>—A list of the principal chemicals is here given:—</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:—</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>—<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>—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<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:—</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—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>—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:—</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'> </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'> </td><td align='left'> </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>—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>—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>—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:—</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,—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<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>—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,—allow to cool, add a drop of Co(NO<sub>3</sub>)<sub>2</sub>, re-ignite, and +note color,—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>—</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>—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>—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>—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>—Before the Bp. on Ch. Yields a +coating—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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>—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° 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>—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>—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>—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>—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>—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>—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>—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>—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:—</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:—</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.—<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>—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.—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.—</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>—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,—</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.—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.—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.—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.—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.—</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>—</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.—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.—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>.—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.—</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.—</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.—</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.—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>—Cl . 16.6, O . 20.3, Cu . 50.1, +H<sub>2</sub>O . 13.0.—</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.—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.—</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.—</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.—</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).—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.—</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.—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.—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.—</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.—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.—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.—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.—</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).—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>—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.—</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.—</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.—</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>—</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.—</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.—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.—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.—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.—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.—</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. Reëntrant 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>.—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.—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.—<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—</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.—</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—Cloudy</td></tr> +<tr><td align='left'>Cadmium</td><td align='left'> Colorless</td><td align='left'> Gray—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—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—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—Cloudy</td></tr> +<tr><td align='left'>Cadmium</td><td align='left'> Colorless</td><td align='left'> Gray—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—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—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. 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Thus, we do not necessarily +keep eBooks in compliance with any particular paper edition. + + +Most people start at our Web site which has the main PG search facility: + + https://www.gutenberg.org + +This Web site includes information about Project Gutenberg-tm, +including how to make donations to the Project Gutenberg Literary +Archive Foundation, how to help produce our new eBooks, and how to +subscribe to our email newsletter to hear about new eBooks. + + +</pre> + +</body> +</html> diff --git a/32974-h/images/fig1.jpg b/32974-h/images/fig1.jpg Binary files differnew file mode 100644 index 0000000..d313d67 --- /dev/null +++ b/32974-h/images/fig1.jpg diff --git a/32974.txt b/32974.txt new file mode 100644 index 0000000..b3316db --- /dev/null +++ b/32974.txt @@ -0,0 +1,2415 @@ +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.... 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