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FRANCOIS XAVIER STREET MONTREAL, CANADA. » LlCOLE DC r/rCLCINE CT DE Cllinur^GIE IE r,?«';TREAL, /iCULTE BE MtDECINE DE L'UNiVERSiTE LAVAL, A M©NTR£AL iWt^V ^ Enteral accordinjj to Act of I'.arli.imeiit of Canada, in the year one thousand eight hundred and seventy-five, by A. H. KoLLMYBR, A. M., M. D., in the Office of the Minister of Agricuhure, at Ottawa. O ii 'hcm PREFACE. The present work on Modern Chemistry has been written and published in the hope that it will prove useful to all who, from business occupation or from any other circumstance, may not have sufficient time at their disposal to consult those more voluminous works which have already contributed so much towards the advancement and improvement of this branch of Science. The main object of the author has been to compress into as small a space as possible everything is actually required to CORRIGENDA. P,«ge 6, line Ut, lor non-raetallic comitoumli and thiir more important compoiimls, read non-metallic elementii, Ac. Page 16, I'm- 16, NH, (Ammonia) ought to have been digcribed at page 10 lus one of the compounds of Nitrogen. Page 62, line 7,./i>r Didynium, read Didymium. Piige 70, line 1,/or tallic, redd metallic. of style to simplicity of es, independent of its modern system ; us easily refresh their xxxxu oiiuui\^ tiiiu*.- u,iivA y^A^\jk\\jLXKj\j ^t^jw\j uiKLu lu ucis iicij^cu tu uuiUL uuu tiitj luuuiuurKy which guide the student on his journey through tliis intricate but interesting study, or that it has served to stimulate him to a more thorough investigation of tliis noble science, then it will have fully accomplished the desire of THE AUTHOR. Montreal, November, '875. .hCU), ^tcouDrr:rDrc;.crTDrc:n...c,r,c.^,Tn,,, ^"'^IVERolTE LAVAL, A iifONTf?tAL, Enteral ace V t h c n h oi in V PREFACE. The present work on Modern Chemistry has been written and published m the hope that it will prove useful to all who, from business occupation or from any otlier circumstance, may not have sufficient time at their disposal to consult those more voluminous works which liave alreadv ( ontributed so much towards the advancement and improvement of this branch of Science. The main olyect of the r.at^^.or has been to compress into as small a space as possible everything connected with the study that deserves attction, and to give no more explanatory matter than is actually required to render each subject perfectly intelligible. In order to effect this end, he has sacrificed elegance of style to simplicity of language, and has on some occasions even thrown himself open to the charge of tautology. The tabular form liere adopted is with few exceptions original and affords many advantages, independent of i^^ being more easily remembered and more readily understood. It will be found to be especially adapted to the wants of 1. Students intending to present themselves for examinations ; 2. Persons who have learned the old notation and wish to become acquainted with tlie modern system ; 3. Those who desire to keep t' "'jlves posted on this subject, and who can thuf. '.asily refresh their memories without doing so at the expense of their other engagements ; And should time and experience prove that it has helped to point out the landmarks which guide the s.,adent on his journey through this intricate but interesting study, or tliat it has served to stimidate him to a more thorough investigation of this noble science, then it will have fully accomplished the desire of THE AUTHOR. Montreal, November, 1875. cor poi one Hj, lasl ID • O/3 not it is ther thu£ only figui whic CHEMIA COARTATA; OR, THE KEY TO MODERN CHEMISTRY. Ghemistby ia that branch of the natural sciencca vrhich investigates tho nature ami prnpartloit of nil bodies entering into the composition of the universe. It investigates the action between the integrant molecules or utoitm of bodloH, and studies the force or power by virtue of which every combination is eScoted. All bodies are divided in Chemistry into Compound and Simple : — A Compound hodij oiin bo Hopnrntcd into two or more simple ones; a Simple body cannot. The simple bodies are called Elements, and arc 6' 'n number. Somo of tlioso are Gaieouf, viz. Oxygen, Hydrogen, Nitrogen, CMilorine, and perhaps Fluorine ; two only are liquid, viz. Brom'no and Mercury ; and tho remaining 58 arc solid ; the last (solids) are generally divided into Non-Metallic and Metallic. All the elements are dogoriboil under tlio name of Inorganic Chemistry, in contradistinction to a large number of complicated compounds, many of which oxlRt nnturally In plants and in animals, called Organic. The elementary bodies are represented in chemical /ormuZit; and equationt, by certain «lmrii(!terH termed Si/mhoh. Tho symbol not only Vepresents the substance specified, but also a certain amount of that element, that In, Itx eouibinlii^ <|Unntity or atomic tvright ns it is more properly called ; thus, stands, not only simply for Oxygen, but also denotes that thoro aro 10 piirts of it in the compound, or if there be more, the fact is made evident by the addition of a small figure (called the co-ejjlcienl) plnodd Inimodintely under the symbol, thus, 0„ O3, meaning twice or thrice 16, f'rt is, 32 and 48 parts, for it is an ettahlished law \n oli«nil«try that all tuhitances unite in only one proportion, or in multiples 0/ t,ia^ proportion. Take for instance Oxygen, which unlton only In (|UniititicB as represented by the figures 16, 32, 48, 64, &c., (multiples of 16) and never in smaller quantities ; and Nitrogen, uh 14, 28, 42, 50, &o., all multiples of 14, which is its atomic weight. The following table represents the sixty-four elementary bodies, with their appropriate symbols and atomic weights : — No. Namr. Syvbul. Atumio Weight. No. 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 61 62 63 64 Naux. SniBOL. ATomo Weiobt. 1 Aluiuinum.. Al Sb As Ba Be Bi B Br Cd Cs Ca C Ce CI Cr Co Cu U E F Au II In I Ir Fe La Pb Li Mg Mn 27.4 122 75 137 9.4 210 11 80 112 133 40 12 92 35.5 52.2 58.8 63.4 95 112.6 19 107 1 74 127 198 56 93.6 207 7 24 35 200 Molybdenum Nickel Mo Ni Nb N Os Pd P Pt K Rh Rb Ru Se Si Ag Na Sr S Ta To Tb r ' T. Sn Ti W U V Y Zn Zr 96 2 Antiinonv rStibiuni^ 58.8 3 Arccnio Niobium 94 4 Barium Nitrogen 14 5 Uervllitiiii Osmium • 199.2 n Bismuth Boron Oxvcon 16 7 Palladium 106.0 8 Bromine Phosphorus Platinum 31 fl Ciidmium 197.4 10 CflBsium Potassium fKalium') 39.1 11 Ciilciura Rhodium 104.4 1? Carbon llubidium 85.4 13 Cerium Chlorine Chromium KutheniuiU 104.4 14 Selenium 79.4 15 Silicium ..• 28 16 Cobal Silver (Argentum) 108 17 Copper (Cuprum) Didyuium Sodium rNatriumt.. 23 IS Strontium 8.76 10 Krbiuni Sulphur • 32 "0 Fluorine Tantalum 182 ?1 Gold (Aurum) Tellurium 128 ?? Hvdrcen Terbium? ?3 Indium Thallium 204 94 Iodine Thorinum 15.7 ?5 Iridium, Tin (Stannum) • 118 20 Iron (Ferrum^ • Titanium 50 07 Lanthanium Tungsten (Wolfram) 184 "8 Lead (Plumbum) Lithium Uranium 120 99 Vanadium Yttrium Zinc 51.2 30 Magnesium 61.7 SI Manganese 65.2 32 Mercury (Hydrarfryrum) Zirconium 89.6 Tho SDiallcBt quantity to which a body can bo reduced is called an atom ; it must thcrcforo bo regarded us a definite quantity ; moreover, the atoms of all bodies are of the same size, yet they are found to differ greatly in weight; and, if the atom of Hydrogen bo taken as the standard of comparison, and is counted to weigh one, then the atom of Oxygen will bo found to weigh 16, that of Nitrogen 14, and that of Sulphur 32, &c.; hence, these numbers ore called tho atomic weights. An atom is tho smaiiost quantity that can enter into combination with another element. But an atom cannot exist alone as such, it must he united with another atom, and the two (or more as is often tho cose) th':n constitute a molecule; thus, 0, H, & N are atoms, and can combine with other bodies, but, if free, then they combine with one of their own atoms, and really exist, as 0^, H, and Nj, that is, as molecules. An atom combining with inother, forms a molecule, whether the element be the same or not ; thus, H and H form one molecule of Hydrogen ; H and CI form one molecule of Hydrochloric acid ; and H, C and N form ono molecule of Hydrocyanic acid. In otiier words, ono atom cannot exist alone, it must bo combined with something else, and if no other presents itself, for which it ha i a strongc* attraction, it will unite with another atom of itself and form a molecule. A molecule on tho other hand, may consist of 2, 3, 4, or more atoms, as seen in a molecule of water H^ 0, (here are 3 atoms), of Ammonia NH, (4 atoms) &o. Yet, though atoms combine .. ..a. .in definite proportions, it has been ascertained that their powers of replacing ono another in compound bodies vary greatly ; thus, one atom of Oxygen will replace iwo atoms of Hydrogen in any compound; while ono atom of Nitrogen will take the place of three of Hydrogen ; and an atom of Carbon displaces /o«r of Hydrogen or two of Oxygen. This has led to their being arranged into groups that will show their power of replacing each other in chemical compounds ; — this is called their Qmnti- valence. Thus, the elementary atoms are divided into Moniealent or Monads ; Diualents or Dyads ; Trivalents or Triads ; Tetravalents or Tetrads, &e. ; and tho elements are said to be Monatomic, Diatomic, Triaic Tretratomic, &c., according to the number of Hydrogen atoms which ono atom of each can replace, for the atom H is taken as the standard for comparison and is tho typical monad. The quantivalenoe of an element is usually expressed by Roman numerals placed after the symbol, thus, H' (monad;, 0" (dyad) N'" (triad), C'^ (tetrad), &c., and it is of the utmost importance that the quantivalenoe of each atom should bo constantly kept in mind, in studying the numerous chemical decompositions as they present themselves, in order that the changes that take place ghould ba thoroughly understood, as the numerals are generally omitted. Roman numerals are used for this purpose, so that they should not be confounded with the ordinary co-efiBcients which are placed either under or before the atom ; thus, Oj, N3, or '20 and 3N, — 4- The laws regulating chemical combinations are the following : — 1st. The law of Constant proportion. — The same substance always contains the same elements united in the same proportion. 2nd, The law of Multiple proportion. — When one body combines with another in severi'l proportions, the higher proportions are always multiples of the first or lowest. 3rd. The hvf of Reciprocal proi>ortion, — If two bodies unite with a third, the proportions in which they combine with that third body are measures or multiples of the proportion in which they combine with each other. The combining quantity of a compound body is the sum of the combining proportions of its constituent.-^ ; tl'.jj, take wiiter (IIjO) we get 2 for Hydrogen and 16 for Oxygen, =: (equals) 18, which is the combining quantity of that fluid ; and ilNO, Nitric Acid would bo 1 for the Hydrogen, 14 for Nitrogen, 3 times 16 of Ox gen = (equals) 18, would prove 03 as its combining proportion, which is correct. Nomenclature. — When one atom of an element unites with the atom of another, in sevenil proportions, distinctive names are given to the compounds so formed ; thus, we might have with a metal and oxygen M^O, MO, M^Oa, MOj, MO3, MO4, &3., and these are distin^'uished as suboxide, monoiiile, sesquiojcitlc, dioxide, trioxide and tctroxide respectively ; the compound resulting being always called '.u ide. If Chlorine, Iodine, Sulphur, or, in fact, any non-metallic clement were subtitutcd for the Oxygen, then Clilorides, Iodides, and Sulphides would be formed, which might be either sub-, mono-, scdqui-, di-, tri-, or tctrasulphides, according to the number of atoms of each united with one of the metal. If two acidd are formed with one element, then the name of the higher terminates in tc, and the lower in ous ; as Sulphuric, Sulphurous, Nitric, Nitrous, &o. There are two methods of ascertaining the composition of any substance ; these are : — 1st. By Si/nthesis, or forming the substance by bringing the elements of which it is composed together by appropriate m-ians* 2nd. Bi/ Analysis, or decomposing the body and separating it into its simple elements. The latter may be of two kinds :— (a) Qualitative Analysis, which merely finds out the ingredients, and, (6) Quantitative Analysis, which ascertains the amount of each ingredient present. A Chemical Formula represents a molec-jle either of an element or of a compound. It has four functions : — 1st. It indicates at a glance the names of the elements in a molecule. 2nd. Its symbol or symbols, togetber with a small figure attached to the foot of any symbol, show the number of atoms in a molecule. 3rd. It stands for a constant weight of a compound, the molecular weight, that is, the sum of the weights of the atoms iu a molecule. 4th. It represents two volumes of the substance In a state of gas or vapor. In the case of bodies that cannot be volatilized, *.liis statement is only probably correct. A volume means a measure. The combining volumes of all elementary gases are equal, excepting those of Phosphorus and Arsenic wMch are only half those ofthe other elements iu the gaseous state, and those of Mercury and Cadmium which arc double those of the other elements. A Chemical Equation or a Cliemical Diagram is a collection of formula) and symbols, so placed on paper as to form a picture or illustration of the state of things hr/ore and after that attack of molecules on each other, which results in the formation of new substances. A Chemiail Coinpound is one in which definite weights of constituents liave combined, and during combination have undergone an entire change of properties. A " compound," in pharmacy, is an intimate mixtu'c; of substances, but still only a mixture ; it is not a chemical compound, the ingredients have not entered into chemical union or combination. A Solid is a substance, the molecules of which are more or loss iininobilc, though probably not in absolute contact. A Liquid is a substance whose molecules move so freely about each other that it readily assumes and retains the form of any vessel in which it is placed. A Gas is a substance, the molecules of which are so far apart that they seem to have lost all attraction for each other, and indeed to have acquired the property of repulsion to such an extent that they are only prevented from receding to a still greater extent by the pr>-ssure of surrounding matter. Gravity means simply weight; but specific jravity means relative weight, or weight compared to a standard. Air is taken as the standard of comparison for gases, and water for lijuids and solids ; but only because they are more convenient and always at baud ; any- thing else would servo the purpose as well, but might net be so easily procured. Lately, Hydrogen, being the lightest of all known substances, has been proposed as the standard, and much can bo said in favor of its adoption. Density means the comparative mass, and is often used synonomously with specific g...;ltj, i,^ they bear such a close relationship, (for weight depends on the amount of the mass) though their meaning is in reality altogether different, I^ote, — An acute accent is often used in this work to represent the word acid ; thus, Sulphuric', Nitric', Phosphoric', &o, 6 NON-METALLIC COMPOUNDS. AND SunSTANCB. Synonyms. HiSTOBY. Obtainkd From. DRCOUI'OglTIONI. Oxygen. Empyreal air. Dephlogisticated air. Disc, in 1774 by Scheele and Priestley. Forms l-5th of air, " 8-9th8 of water. « 2-3rd8 of earth. (1) Mercuric Oxide. (2) Manganese dioxide. (3) Potassium Chlorate. (1) HgO heated =Hg+0 (2) 3MnOJ)etttod^MiiA+0, (3) KCIO, heated =KUl+0, Ozone. Is allotropic Oxygen. Sohonbein 1840. (1) Phosphorus and Oxvgen. (2) Electricity &Oxygen (1) Let Phosphorus BtanJ in nio'iNt Oxygen. (2) Pass Electricity through dry Osygon. Hydrogen. Inflammable air. Forms l-9th of water by weight. Disc, by Cavendish 1766. (1) Zinc and Sulphuric' (2) Zinc and Hydro- chloric' (3) Water and Sodium. (4) Steam, and Iron filings heated. (1) Zn+n,SO^=ZnSO,+n, (2) Zn+2nCl=ZnCIa+ir, (3) 2H,0+NH,=2Nan04-n, (4) 3Fe-f 411,0= FoA+^lIi H,0 Water. Hydrogen Monoxide Exists as vnpor, liquid, and solid (Ice). Our Globe is r imposed of 27 parts ot water, to 10 of earthy matter. Mix 2 volumes of Hy- drogen with 1 of Oxygen. Union can bo effeoted by tho aid of an electric spark. THEIR MORE IMPORTANT COMPOUNDS. Propektikb. Tests. Symbol 0. Combining weight 16. Sp. gravity 1.1057. 1 litre weighs 1.43028 grm. 100 0. i. weighs 34 grs. A gas, without color, odor, or taste, unliquifiable, sup- ports life and combustion, but, if inhaled in excess, will cause death from over-stimulation. It is a Dyad. 1. It will relight a freshly blown-out candle as long as there is a red glow on the wick. 2. It forms red fumes with Nitro2;en Dioxide. 3. It turns the white Ferrocyanide of Iron blue. 4. Combustible bodies burn in it wit h great brilliancy ' It has a strong oppressive odor, oxidizes metals, frees Iodine, Chlorine, &c., corrodes India rubber, bleaches Litmus, heat converts it into ordinary Oxygen. It consists of 3 volumes of Oxygen, condensed into 2 of Ozone, and, when it oxidizes a metal, it does so without any diminution in bulk. Saturate paper withaSolutionof Starch and of Potas- sium Iodide; on exposure to air, if Ozone be present, it turns blue, from freeing the Iodine and forming the blue Iodide of Amiden. It is supposed to be disinfectant. Symbol H Comb, weight 1 Sp. gr. 0.0692 1 litre weighs 0.08961 grm. 100 o.i. weigh 2.14 grs. A gas, without color, odor, or taste, unliquifiable, does not support life or combustion, but is not poisonous ; when respired it renders the voice puerile ; is the lightest of all gases — 14^ times lighter than air. 1. It is inflammable, burns with a pale blue flame, evolving little light, but great heat. 2. Mixed with half its volume of Oxygen, it will explode, forming vapor of water. 3. It gives no red fumes with Nitrogen Dioxide. Sp. gravity ot vapor 0.6220 of liquid 1.000 of ice 0.940 A bluish liquid, freezes at 0°C, (32° F.), boils at 100" C. (212° F.), it reaches its greatest density at4°5C. (40° F.), is 815 times heavier than air ; is the great- est solvent ktiown ; hot dissolves more than cold, ex- cept of Sodium Chloride, Lime and Magnesia. 1. When pure, no residue is left on evaporation. 2. It should form a clear solution with Lead Acetate. It unites with bodies and forms Hydrates ; and it may exist in salts as water of crystallizatioH ; the latter can be expelled by heat. -8- Sdbbtanoe. BruONTMS. HisTour. Obtained From. Decoupositioni, H,0, Hydrogen Dioxide. Thenard, 1818. Barium Dioxide, Water and Carbon Dioxide. BaO,+H,0-fCO.=BaCO,+IIA ca led also somctiiuoH OxyguniiUiiI Wfltot , Nitrogen Azote. Rutherford, 1772 Forms 4-5thB of air. (1) Liquor Ammonia and Chlorine gas. (2) Potassium Nitrite and Ammonium Chloride. (3)Phosphorusand Air. (1) NH,+3CI=3HC1+N (2) KNO.+NII«CI=KOI+2ir,04^N, (3) Bum the Phosphorus in a bull j«p coo' taining air, the Oxygon is burnt off mid N is left. The atmosphere. Is 45 miles deep, and weighs 151bs. on every square inch of the earth's surfoce. Thp -'ases composing it are nly in a state of mixl. ; iodide of AniiJen. If the Iodine bo in ooiub''iatiou as in KI, then CI or an acid must be addea before the Starcli test can bo applied. -18- SciisTANCK. Synonyms. UlSTOBY. OiiTAiNEt) From. DECOUrOSITIONS. HI Hydrogen Iodide. Hydriodic Acid. (1) Phosphorus, Iodine Water. (2) Indinc,Sulphuretted Hydroficn k Water. (1) P,4I,+6H,0=2n3PO,+6FII. (2) Ij suspended in HjO+HjS=:S deposited and 2ni remains in solution. NI. Nitrogen Iodide. Iodine and Liquor Ammonia. 61+4NU.=3NHJ+NI, Bromine Balard. 1820 It exists in sea water as Magnesium Bromide. Sea water. Chlorine, Ether, Solution of Potash, Manpincec diuxido, Sulphuric'. Evaporate sea water and remove the leas soluble salts, pass 01 tlirough to free the Br. from the Mngnesium; add Ether which brings the Br. to the surface, separate the Ethereal solution by a pipette ; add the KHO and evapor.-ito to dryness; then add tlio MnO, and IIjSOi (V MgBr.4-Cl,=Mf:Ci,+Br, (.b) ')KHO+3Br,=3H,0+KBrO,+5KBr (0) 2KBr+MnO,+2H,SO,= K,S0«-fMnS0.+2H,0+Br, Fluorine Exists as Fluor-spar. Has never been isolated. HP Hydropren Fluoride. Hydrofluoric Acid. Scheele. Fluor Spar and Sulphuric'. CaF,+n,S04=CaS0,+2HF H.SiF, Hydrofluosilicic Acid. Hydrogen Fluosilicate. Fluor Spar, Sulphuric', QlasB, and Water. (a) CaF,+n,S0.=CaS0,+2nF (b) 4HF+SiO,r^2H,0+SiF, (c) 3SiF.4-4H,0=SiH.O«+^H>SiF, iM- 19- Propeeties. Tests. An acid gas, fumes, soluble in water. The solution spoils in a very short time, the Iodine being set free. Two oxides of Iodine exist but are unimportant, they are IjOj and IjO,. Compounds are also formed with Nitrogen and Chlorine. A dark powder, explodes, often spontaneously. The slightest touch will cause it to explode even under water. Symb. Br. Comb, weight 80 Sp. gr. ' 2.97G " " vapor ' 5.41 1 litre weighs G.99 grms. A brownish rod liquid, suffocating odor, produces symptoms of Influenza or Catarrh for several days after it has been inhaled. It is poisonous, bleaches, is disinfectant, soluble in 15.3 parts of water, but freely in Alcohol, Kther, and Chloroform ; freezes at— 7°C (19°F.) boils at 63°C (143'F.) 1. Silver Nitrate gives a light ,yrf/oio precipitate but sparingly soluble in Ammonia. 2. Solution of Starch gives an orange Bromide of Amiden. Hydrobromio' may be prepared like Hydriodic'. Bromic'&Hypobromous'are prepared by the same means adopted for getting tlie cor- responding Chlorine compounds. Ether will (Separate Bromine from any of its watery solutions and rises to the surface of theliquid with it, acquir- ing a yellow or red color from it ; Chloroform does the same but sinks to the bottom of the fluid. Symb. F. Weight 19 Supposed to be a gas. It attacks and destroys all vessels used to obtain it. Sp. gr. 1.0G09 A corrosive fluid, fumes very irritating, used in the ■ arts to etch on glass. Its etching on glass is a delicate test for its presence. No compound of Fluorine and Oxygen is kuowu. The solution is separated by filtration and is kept to precipitate the Salts of Potash. Any salt of Potash is thrown down by this ucid as uu insoluble UydroftmsiUcate. 20 DIATOMIC NON-METALLIC SunSTANCE. Stnoxyms. History. Odtaixkd FnoM. DKOOUIumiTIIINNi Sulphur Native in Sicily, Cali- fornia, &c., occurs also as metallic Sulphides and Sulphates. The native Sulphur. Distill it in clay vohhiiIh ii:t(i rccciviTM ; nicU, pour into wnnden imouMm, whi-n it con- i^tHuU'i^ lirlnutoiif ; wiiim tliis Ih Hiil)liincd into largo chainborn it rorms Fldwrrn of Sulphur : ami thin again wanlicd well with water is Sulphur Latum, SO, Sulphur dioxide. Sulphurous oxide. Sulphurous Anhy- dride. Copper and Sulpliuric'. Cu-f2lI,S().=CuSO,-f2ll,<)H-S(t,,MiUHtbo collected over mercury, uh wiitor takes up 30 times its own voluiuo of Iho gas. H,S03 Sulphurous Acid. Hydrogen Sulphite. Stoht. Sulphur dioxide and Water. so,+H,()=n,so. SO, Sulphur Trioxido. Sulphuric Anhydride. Sulphuric oxide Anhydrous Sulphuric'. Nordhausen Sulphuric Distill the acid and colliiot in n cooloJ reoeivor. Acid. i H.SO. Sulphuric Acid. Hydrogen Sulphate. Valentine, 15th century (a) Commercial. (b) Nordhausen. • ( Nitric Acid vnpor J. Sulphurous Anhydride (_ Steam, and Air. (a) iHNO.+jjso.+aH.Or^ N,(),4-:nT,so, the NjOj alworbs 0, Croni llui air and becomes N,{\ thou N,(),-f L'S(),-}-2H,0 = NA agttin-{-2llaHU, ami thJN change from NjOj to N,(), coiilinuoit liii all tho SOj is converted by iilil oi tlio iteain present into H,HU4. Heating Ferrous Sul- phate. (b) 2FeSO,-Fo,0,-fSO,-f-H(). which unites with tlio baitio water in the Halt, thus, 2S0.-fn,0=-H,S,(), it HeemH to bomadoupof U,H04-f-!S0,. ELEMENTS (TYPE O") 21 Pbopkrties. Tests. Symb. _ S Comb, weight 32 Sp. gr. 1.98—2.04 " " vapor 2.22 1 litre weighs 2.8G7 grras. A yellow solid, crystalline or amorphous, insoluble in Water and Alcohol, but dissolves in Turpentine, Oils and Carbon Bisulphide; it melts at 1U°C. (232^F.), gets thick at 249'C. (488=F.) ; at 400°C (792^F.) it gets thin again and boils. (1) Its color ; (2) It burns forming SO, gas; (3) Small quantities may be detected by boiling it with Sulutio7i, of Potash and Lead Acetate when it becomes browtiish Mack. There are severJ allotropic (i. e. modified) forms of Sulphur : (a) Prismatic; (b) Octahedral; (o) Brimstone; (d) Plastic; (e) Black; (f) Blue. Sp. pr. 2.21 1 litre weighs 2.8G05 100 cubic inches 08 grs. A colorless, suifocnting poisonous gas, does not support combustion, liquifies at — 17='.8C. (0°F.) ; at — 6'C. (17°F.), with water vapor it crystallizes. (1) It bleaches Litmus &o. ; (2) Its odour; (3) It is acid ; (4) It frees Iodine and if Starch be present, it produces the blue Iodide of Amidea (or sometimes called Iodide of Starch.) A colorless liquid, witk the characteristic smell of burning sulphur. 1. Apply the sane tests as for SOj gas. 2. It reduces G Id Chloride and precipitates metallic Gold. Sp. gr. 2.77 White silky crystals resembling asbestos. (a) A heavy oily corrosive liquid, which blackens and chars the skin, wood, &c., it boils at 327''C (020° F) and freezes at— 20''C (^— 15°F.) Deliquescent; hisses like hot iron if put into water. Sp. gr. 1.842 1. With metallic copper, sulphurous anhydride is given off ; known by its odor, &o. 2. Mixed with an equal quantity of icater, heat is evolved. 3. Baryta water gives a white precipitate of Barium Sulphate, insoluble in Alkalies, and in all Acids except boiling Sulphuric'. Sp. gr. 1.900 (b) A heavy dark fuming liquid, used only in the arts, chiefly as a solvent for Indigo. ¥ \ — 22 — % i t ^ BUBSTINCE. Stnonysis. Bistort. OnTAINEU Ffom. DKOnUPOSITIONS, H.S,0, Hyposulphurous Acid. Thiosulphuric Acid. Known in 1 CI 8. Digest Sulphur with Potassium Sulphite. K,S03+S=K,S,03 H,S,0. rithionic Acid. HyposulphurlcAcid. Trit'iionio Acid. Manganese dioxide, Wnt«r, Sulphurous Anhydride, Barium Hydrate&Sulphuric'. Potas.sium Ilyposul- pliit«,and Sulphurous Anhydride. MnO,+2H,0+2SO,= MnS,0.-f 811,0, tlio Barium is then added wliinh (iirniH H« S,0, and is dcconipou'd by n,HO,,= I>ttS 0.+H,SA ESX). 2K,S,0,+-'5SO,=2K,R,,(\-fH tlin aoi.l nmy be freed by HydroihioHJlicio noid. H;S,0, Tetrathionic Acid. Fordos & Jelis. Iodine and Barium j 2BaS„0,+lj=naI,-fHaS,04 I'ruo It, witli Hyposulphite. HjSO, H^S^O^ Pentathionic Acid. Wnckenrodcr. Hydrogen Sulphide and 5H,SOa+5HaS=5S+i)H,0-flI,H,{), Sulphurous'. H.S Hydrocon .Sulphide. Sulph-hydric Acid. HydrosulphuricAcid. Sulphuretted Hydro- Sclicclo. 1777 (a) Ferrous Sulphide (1) FeS+n,SO,=FeSO.+H,H and Sulphuric'. (b) Antimonious Sul- (2) Sb,S34-GHCl=2SbCi,+:UI,H phidc and Hydro- chloric'. HaSj Hydrogen Disulphido Sulphur, Slaked Lime, Water & Sulphuric'. (a) .3Ca04-S«=2CnS,-|-raSA (b) CaS,+H,S0,=CaSO,-f H,S, 2S,4-C,= 2C8, cs, Carbon Disulphide. Lanipadius. 1796 Charcoitl and Sulphur. n-' -23- PROl'F.nilKS. Tests. i The acid cannot however be freed from the Potassium. 1 It dissolves Silver Chloride, and is thoroforo UNfld in Photography. Sp.gr. 1.34.7 Colorless, odorless, sour, liquid. It reddens vegetable blues. The salts do not depo"it Sulphur on the odditlon of an acid. It may be er,r.'ientratcd, but is Boon decomposed into S+II.SO,+ILSO, It gives no precipitate with Baryta or Lood HuUm. BaS,Oe+II,SO,=BaSO,+lI,S,Oa t^itrio acid throws down Sulphur with it, Colorless, odorless, but with an acid and bitter taste. Sp. ftr. 1.175 1 Utrc weighs 1.52 grm. 100 cubic inches 35 grs. A colorless, inflammable, foetid gas, liquifies by 17 atmospheres, is a narcotic poison, its solution acts as an acid and reddens Litmus. Salts ' iiid Cadmium give yellow preoU pii ;r, Lead, Bismuth, Mercury, itiiJ Sil • .own or black; Tin brown ox yMiw ; Antimony orange; Gold and Platinum, llntls precipitates. Its odor is also a good tOf*t, Sp. gr. 1.769 A yellow viscid liquid, with an odor like rotten eggs. Slowly decomposes into S and H,S. Metallic oxides decompose it immediately. Sp. gr. 1.272 ♦' " vapor 2.69 A transparent colorless liquid, of great refractive and dispersive powers, foetid odor, inflammable. It dissolves Sulphur, Iodine, Bromine, PliOHpljorun, Camphor, Caoutchouc, Gutta Perchu, Bilumun and Oils. 24- SCBSTANCEg. Stkontus. Bistort. Obtainkd Fbom. DRCouposmoNS. Selenium Berzelius 1817 Found as Lead Selenide Selenium Dioxide, Water & Sulphurous Anhydride. H,SeO,+2SO.+H,0 =2II,S0.+Se SeO, Selenious Anhydride. Burn Selenium in air or in pure Oxygen gas. H.SeO, Selenious Acid. The foregoing and water. SeO,+H,0=H,SeO, SeO. Selenic Anhydride. Not yet obtained. HvSeO^ Selenic Acid. Hydrogen Selenate. Hydrogen Sclcnide. Lead Selenate and Sul- phuretted Hydrogen. PbSeO..+H,S=PbS+H,SeO« H,Se St'lenuretted Hydrogen Iron Selenide and Sulphuric'. FeSe+ H,SC\= FcSO,+H,So Tellurium Found as Gold, Silver, & Bismuth Tclluridos. Bismuth Sulpho- The process for its preparation is very com- Telluride and plicated and unimportant. Sodium Carbonate. It forma 2 oxides and acids, and with i Hydrogen a compound like H,S As certain French weights and measures have been mentioned, it will not be out of place to give a slight sketch of the Metrical System. A metre is a standard measure kept in Paris, with which all other weights and measures are to be compared, (it is about 39i inches long and is sup^.osed to represent the l-10,000,000th part of the distance from the e(iuator to the pole). This metro is graduated in lOths (or t?ecime/res) ; lOOtlis (or centimetres) / and lOOOths (^or millimetres). By this means length is computed; using, however, Greek numerals whenever the quantity is greater than a metre ; thus 10 metres is a Decametre; 100 a Hectometre; and 1000 a Kilo- metre ; while Latiii numerals are exclusively employed to designate quantities less than u metre. -23- Symb. Comb, weight Sp. gr. PROPKBTlEa. Tests. Se 79.5 4.3 A brownish-red semi-transparent solid with a metallic | If heated, it smells of decaying horse-radish, lustre, it melts at 100°C (212°F.), is volatile, - It burns, but not as steadily as Sulphur, tinges flame blue. A crystalline solid. A powerful acid, resembling Sulphuric. ! ( It decomposes Carbonates, Nitrates and Chlorides. ■; It precipitates Lead .^.nd Silver salts. (^ It is decomposed by Hydrogen Sulphide. Sp. gr. 2.624 Sp. gr. 2.795 Syiiib. Comb. Sp. gr. weight Te 129 6.2G Resembles Sulphurio'jdecomposes by heat into Selenious' and Oxygen. It dissolves Gold but not Platinum. A colorless gas, soluble in water, inflammable. A silvery brittle substance, metallic in appearance, a bad conductor of heat and electricity. It excites catarrh and destroys the sense of smell. It burns. The compounds are not important, but resemble those of Sulphur and Selenium. For measuring Liquids. — A cubic decimetre is employed and is called a Litre ; it is about IJ pints Imperial measure, (i. e. 20 cz. to the pint). It is also divided into lOths, lOOths, and lOOOths parts, named also Deci-, Cenli-, and Miliditres : 10 litres constitute a Decalitre; 100 a Hectolitre; and 1000 a Kilolitre, For weighing Solids. — A cubic centimetre of water represents a gramme and is equal to about 15^ grains. The gramme is also subdivided into lOths, lOOths, and lOOOths or Deci-, Centi-, ani Milligrammes ; while 10 grammes make a Decagramme; 100 a Hectogramme; and 1000 a Kilogramme. 26 TRIATOMIC NON-METALLIC Substance. SrNllNVMS. UlSTOKT. OllTilNKl) FbOM. Decoupositio.ns. Phosphorus Brnndt 1069 Exists in bono, urine, find .'ilbtiniuii. Plants absorb it from the soil, these are eaten by animals and con- verted into Phos- phates. Bono ashes, Charcoal, Water, Sulphuric'. (a) Ca, (PO0,-f 2n,SO,=2f aS0,4-Can, (PO,), (b) Call, (P0,),=2ll,0-f Ca (PC),), (.c) 3C» (,PO,),4-5C,= Ca,(PO,)»+10 CO +P4 Amorphous I'lios- pliorus. Schriittcr. Heat Phosphorus in Nitrogen, for several days, at a temperature of 24.0° C (4G4.°F) PH, Phosphoretted Hy- drogen, V A gas. Caustic Potash, Phos- phorus, Slaked Lime, and Water. P,+3CaH,0,-f 6H,0=:3CaH,P,04 +2PH, PH, A liquid. Calcium Phosphite and Water. Convey the gas through a tube cooled by a freezing mixture. P.H A solid. Light decomposes PHj into ordinary PH, and solid PjH which is often seen on the inside of jars when by exposure to light PHj has lost the power of spontaneous inflammability. HJO. Ilydrofjen Ilypo- phosphito. Ilypophospliorous'. Barium Hypophosphito and Sulphuric'. Ba (H,PO,),+H,SO«=BaS04+2n.H,PO, ELEMENTS; (TYPE N"") 27 Pudl'KllTIKS. Tksis. Symbol P Comb, weigbt .^1 Sp. gr. 1.77 " " vapor 4.32 1 litre weiglis 5.542 grms. A yellow, soft, waxy solid, must bo kept uiuler water, iis it takes fire in air, foriiiiiig iMiospborie', eilial- ing an odor like garlic, is soluble in Alcobol, Ktbor, Oils, Bisulphide of Carbon, and Napbtba, is phos- phorescent, melts at 44°C. (11 TF), boils at 280°C. (53G°F.) To detect Phosphorus, dry the substance, and heat a thin layer on a metal plate in the dark, when it becomes luminous: — or after drying, digest it with Carbon Disulphide, filter, put in a watch glass, floating on hot water, when it should be come pliosphorescent. Kcd, opaque, insoluble in CSj, not luminous. At 2i)0"(.' (fjOO-Fj becomes common phosphorus, used for hicifer matches. Sp. gr. 1.24 A gas, with fa>tid garlic-like odor, burns with u bril- liant white flame forming water and PA);, If pure is not spontaneously combustible, but usually is so from containing the next substance PII, A very volatile colorless li(juid of high refractive power. Spontaneously inflammable ; renders the former gas the same when its vapor is present even in the smallest proportion. It is very unstable. Phospiioretted Hydrogen does not affect the salts of lioad, but those of Silver and Gold deposit their metals by its action. A strong acid syrupy fluid, a powerful deoxydizcr. It precipitates Gold and Silver from their solutions. 28- SUB3TA.NCE. SySOXYMS. Distort. OuTAiNKD From. Dgcoupositions. PvO. Phosphorous Anhy- dride. Burn Phosphorus in a little air. HPO, ITydro<;en Phosphite. Phosphorous Acid. (a) The preceding and Water. (b) Phosphorus Tri- chloride and Watcv. (a) PA+3H,0=2n,POa (b) PCi,+3H,0=3HCl+n3P03 P.O. Pliosphoric Anhy- dride. Burn Phosphorus in Oxygen gas. Phosphoric Acid. ( V Hydro;;en Metaphos- phate PA+n,0=2HP0, Hydrogen Pyrophos- phate p,o.+2ii,o=ir,p,o, Hydrogen Orthophos- phate PA+3II.,0=2Il3P0« Silver Metaphosphate and Suipliuretted Hydrogen. 2AgPOa-fH,S=Ag,S+2nPO. Silver Pyrophosphate and Sulphuretted Hydrogen. Ag,PA+2H,S=2Ag3S+n,P,0, Silver Orthophosphate and Sulphuretted Hydrogen. 2Ag3PO,-f3U,S=3Ag,S+2H3PO, Boron Boric Anhydride. Hydrogen Borate. Boric Acid. Boracio Acid. Davy. Boric Oxide and Sodium BA+6Na=3Na,04-B, BO, Or Boric Oxide. Exists naturally in Tus- cany, and as Sodium Borate in Thibet and California. Heat Boracio Acid. 2n,B0,=3H,0+BA H,B03 Borax and Sulphuric'. 2NaH B,0.+-2n ,SO,-f 4H,0r. SXaHSO.+iHjBO, -29- PROI'KUTIFS. Tkrtb. A soft white readily volatile powder. It liiniWR diiwiif I'runt Ihtiir m It hlnMiK wligii th In deliquescent crystals ; decompose readily. old, Silver, Mercury and Platiuum utions. In soft, snow white, volatile, deliquescent flukes. rown into water. A transparent glassy mass, called Glacial Phosphoric acid. It is monobasic. (l)Hllvi-p NItmto (2) MMgiiimhlllt Hiil|.hiili'A Nir, (:)) AiMiiiiiiiliiiii MolyliiliiiK (4) Alliiimi'it itiiil Auulig' UUTA- PVBO- onriiopnosHUATE. It is tetrabusic. Wlilto pr. White pr. Noil), White pr. 1 None, 1 None. Wlilt.1 pr,' None. Yellow precip. White. A pleasant sour liquid. It is tribasic , ydlow. None. B 11 2.C8 A dull grey powder, may be in crystals however. iriiuiitfld it buriw in uir, forming Boric oxide (BjO,) Crystallizes in pearly plates from the solution as it cools, sour, scarcely affects Litmus ; is tribasic. (1) Tt linKtm (lnmo urcun. (i!j It nivuM a, tvd color to Turmeric. 80 TETRATOMIC NON-METALLIC SunSTANCR. Synonyms. History. Obtained Fhom. DtxouposmoNs, Silicon Borzelins 1R24. Exists in Sand & Quartz Potassium Silico-Fluo- ride and Potassium. K,SiFe+K,=CKF+Si. SiO. Silicic Anhydride. Quartz, Sand, Flint and Agate. Heat Silicic' H,SiO.^H,0+SiO, HSiOa Hydrojien Silicate. Silicic Acid. Potassium Silicate and Hydrochloric'. K,SiO,4-2Iiri = -2Kri4-H,Sit)n must 1m< prepared by I)ialysis.-t= In the fbrc<;ning decompositions it will be observed that a certain element and often a whole frroiip of elements will lunve one compound, and attach itself to another, forming a new substance whose characters and ])ropertios are porliaps altogether dillereiit fnini tlinso from which it was produced. How do wo account (or this preference that one chemical body apjiears to show towards anntlirr 'I The only answer that can bo given to this question is that it is duo to a pecnlbir force, called Chemlr'tl Affhiili/ or Chiini'r'i/ Attrnvlioii. To this power we are indebted for the value of our tests ; for Barium in solutions will always attach itself to Sulphuric Acid if it ho present, Calcium to Oxalic', a Silver Salt to Chlorine, &c. : — for every element appears to possess likes, dislikes or an iiidilferenco towards its fellow elements, even in a more marked degree than these propensities exist between human beings. :i: This is a process employed in ehcmioal manipnlations for separating liodies ; it depends upon tlic fntt tlint nil crystalliznlile sntistnnies (rnllcd cr;isUilloi(ls) cun pass in solution thronph a parchnicnt ]mptr ; whilst all t;nni-likc nmor|)lioiis siilistnncos (m/loi'h ) sik li iis (iiiutincnis Silioic', A-c, cannot pass. Tin- Diulyzer used for this purpose is a tlat drum or sieve made out of parchment paper into which the siibstauces are thrown, and the drum is then floated on a large surface of water. ELEMENTS; (TYPE C'^) 81 I'llOPKBTlKg. TitSTS. Svnil). Si 22 Jifiisity 2.49 A brown powJer, but niny be crystalline also, it may bo Amorphous, Griiphitoidal and Crystalline. The crystalline will cut p;las3 liko a diamond. It burns on hcatin<=;, forming Silicif'. Density. 2.C4 A snow white insoluble gritty powder, almost infusible. Potassium Hydrate (boiling) dissolves it, forming Potassium Silicate. It is the chief nfjent of petrifaction, a clear limpid fluid, but apt to beconio jully'like. Frequent mention has been made of temperature, and it bccoires necessary to understand the differences between the two thormometers most commonly used, Centogrado and Fahrenheits, and the conversion of the degrees of the one into those of the other. To convert + degrees (t, e, above zero) of F. into C. — Subtract 32, multiply by a, and divide by 9 ; thus : — 212°F— 32=180 X 5=900-5.'J=100°C. • To convert + degrees (i. e. above zero) of C. into F. — Multiply by 9, divide by 5, and add 32 ; thus : — 100°C X 9=900^5=180+32=212°F. To convert — degrees (t. e. below zero) of F. into C. — Add 32, multiply by 5, and divide by 9 ; thus : — — 40°F+32 = 72 X 5 = 3G0^9=— 40°C. To convert — degrees (i. e. below zero) of C. into F. — Multiply by 9, divide by 5, and subtract 32; thus ; — lU^C X 9=300^5=72— 32=— 40°F. I m ^Bsmmmmsm CHEMISTRY OF THE METALS. p, Forty-nine metuls are known — these arc characterized by bcinp; good conductors of heat and electricity, the y arc susceptible of beinf!j polislicd and of reflecting lii;ht ; they arc usually dense and heavy ; malleable, ductile, and tenacious. If a solution of a niet'iUio salt be subjected to electrolytic decomposition, the metal will always be found at the negative pole, showing metals to bo electro-positive. These metals unite with the non-metallic elements and form salts. A salt may be dcQned to be the union of an electro-positivo with an electro-negative. Salts may be Deliquescent; these absorb moisture from the atmosphere and liquify: Ej)loretcent \\\\\c\\ \itai with their water of crystallization and fall to powder : and Permanent when they suffer no change on exposure. The same nomenclature is adopted for salts as has already been mentioned with regaridynium. Aluminum ; Cerium ; Thallium ; Auruni. Tfti 1- ] M'l''*'"""i ; I'alladium ; Uhodiuin ; Iridium; Ruthenium; Osmium; Stannum ; Titanium; Nickel; Cobalt; Iron; ' '■ '*' I i Manganesinm ; Uranium ; Indium. Pentads i Antimony ; Arsenic ; Hismuth ; Vanadium ; Tantalum ; Niobium. I IIk.\ads I Chro;nium ; Wolfram or Tunust(?n ; Molvbdonum. r -^ 04 MONAD Najiks. Potassium Formula, Ac. K. Weight 39 Sp. gr. 0.865 KCl KI KBr K,0 K^Oj KHOT KCIO3 K,CO, Kn.co, History, Ac. PuErARKD FhOM. DKCOm'OIITKINB. Kalium. Davy. Chloride. Iodide. Bromide. Monoxide. Dioxide. Tetroxidc. Hydroxide. Chlorite. Carlionato Bicarboiiute. I'otassium Carbonate KJCO,4-2C = .^CO^-KJ diHtlU mid collect 1S07 i and Charcoal. i under Naphthii, Left after heating the KC103=30+KC1 Chlorate. Iron Iodide and Potash reIa+K,C0,= Fc"C0.-f2Kl Carbonate. ; Lilfo the Iodide using FeBr,+K3COa=I''oCO;,-|-l,'Kllr Bromine. 1 "i'i^ssiuiu Hydroxide 2X110+ K,=r 1 1,-|-2 K,,( ► and Potassium. ' Produced when K^O^ is Has never been obtained puro. made. I Burn Potassium in dry Kj-|-04=KoO, Oxygen. I Potassium Carbonate j KjC0,+CaU,0,= CuC0,4-L'K IIO and Lime Hydrate. Solution of Potash and j aK.G+CI.^^.'iKCl-f KCK), Chlorine wis. Wood ashes and Water, j Lixiviate, filter, deeolorizo iumI ovnjKirato. I Pass Carbon Dioxide ! K,C0a+n.0+C0,=2KllC0, through K,C0,&\Vater.! METALS. 35 PROI'KKTIKS. Tests. A blue, white, soft, lustrous metal, oxydizcs in air, thrown on water it unites with tlic Oxygen and ii^nitcs tiic lIy(lroj;cn. In salt bitterish cubea like common salt. 1. Tartaric' gives a w'ute precipitate of Cream of Tartar. In milk-white, opaque, cubes, anhydrous, fusible. 2. Perchloric' also gives a white precipitate. Somewhat similar to the Iodide. 3. Hydrofluosilicio' gives a white precipitate. Whito, deliiiuesccnt, caustio, melts, and volatilizes. 4. Platmic Lhloriue with a httle Hydrochloric acid and a little Alcohol gives a yellow precipitate of the double Chloride (KPtClO 5. Potash salts tinge the flame of a blow-pipe vioht. 6. On spectrum analysis a bright lino is seen at the red and another at the limit of the violet band. 7. The salts are Alkaline : i, e. they restore the color to Litmus Chrome yellow, cakes at 280'. Whito, deliquescent, soluble, alkaline, rods or masses. Flat, tabular, anhydrous crystals, taste of Nitre. In whito crystals, soluble in water, deliquescent. In largo rhombic prisms, anhydrous, soluble in -t of water. that has been reddened with an acid. -se- tt '' Naues. Formula, Ao. IIisTonr, Ac. Prkpared From. DliCOSU'OHITinNM, K,S04 Sulphate. From residue loft after inakinj^ HNO3. Add Potassium Carbonnto till fiirei'VdHddiieo ceases. KHSO^ Bibulphatc. KjSOj with more Sul- phuric'. Evaporate, dry, redissolvo and rufryHlulli/o. KiSOj.SOj j Anb.jtli-osulphatc. Sulphate, Sulphuric' and Water. KNO. Nitrate. Occurs nalive iu lllast ; But may be made (ird/icuilh/, Indies. K^S Monosulpliidc. r Solution of I'otnHh and , KlIS+KUO= ll.O+K.S 1 KulphiirottcdIIydrogcn, | j then add an much more t Solution of I'otnsh. K,S, Disulpliido. Expouo n Solution of KII 8 till turbid, then eva- porate in vacuo. 2KUS+0 = llaO-|-K,8, K,S, Trisulphide. f I'liss vnjiorof Oiirbon iJi- •1 sulpliidc ovor ignited ( Potassium Carbonate. 2K,(JO,4-L',CS,=C0»+4t'O-f:iK,H, KA TctraHuIphidc. Reduce K,SO^ with CS,. K,S0,+2CS,=.-QC0-fS0,-f-K.H, K,S. Pentasulpliidc. Melt Sulphur with dry ; 3K,C03+S„=30O,+K,SuO,-f-liK,S, Carbonate. | KH8 Hydrosulphatc. PaR8lI,Sthrouj:hCaus. 2II,S+2KllU=21I.04-aKU8 tic I'otashin solution. — 37 — Propkrtieb. Tests. Bitter, neutral, rhombic prisms, atihyilious, soluble in 20 of water. » Sour, flattened, rhombic prisms, soluble in water. Is in delicate needles, is decomposed by a large ijuantity of water. G >.Hed rhombic prisms, soluble in 7 of water. It is doubtful if it has ever been procured pure. Orange colored, easily fusible. Forms with the Sulphate, Liver of Sulphur, The latter is soluble in alcohol and is so separated. ■n — 38 I' 'li- lt !:: Names. FlIHSIUL.E, Ac. lIlSTOKV, Ac. Natrium. Davy. 1803. Phrpauei) From. Decosh'ositioss. Sodium Na. 2,'] Sp. gr. 0.972 Obtained like Potassium. Na.,0; NaA; NallO; Nail CO,; NallSO,; NaS .are all prepared like the Potassium salts. NaCl Na,CO„10ILO Chloride. Common salt. Evaporate water ot brine-springs. Sodium Chloride, Sul- phuric', Coal, Chalk. Neutral Carbonate, (a)2NaCl+lI,.S0,=NaCl+NaHS0,+HCl (b) NaC14-NanS04=Na.,SO^+IICl (c).Na,SO,+2C,=Na,S4-4CO (d) Na,S+CaCO,= CaS+Na,C0, Na,SO„10II,O Sulphate. Sodium Chloride and Sulphuric' 2NaCl+ILSO,=Na,S04+2HCl Na.SjOa Hyposulphite. NaNO, i Nitrate. Sodium Sulphide & S. Occurs native in Peru. Na.,S(V,4-S = Na.,SA Called also Cubic or Chili Nitro. NaBOj Mctaboratc. Borax and Sodium Carbonate. 2BO2NaB,,O„10n,O Bil.nratc or Borax. ! Native •nTIiibet& Persia NaJIP04,12n,0 Na,PO„ 1211,0 Disodic Orthopho.sphato. Acid Calcium Phos- j phatc, and Sodium Carbonate. CaH,2P0,+Na,C0,=CaHP04+C0,+IIa 0+Na,HP04 Tri-iodicOrthopho.vphate Disodic Phosphate and Caustic Soda. Na JI PO^+NaHO = H.O+Na.POj NaHaPOjjHjO ' Mnno.sodic Orthnphos- Disndic Piiosphate and ! pliate. 1 Phosphoric'. im -S9- Pnoi'KnTiKS. They all resemble the corresponding Potassium preparations very clofcly. Not deliquescent, as soluble in cold as in hot water, inanuCaeturcd in England, Spain and Canada. Oblique rhombic prisms, cfHoresccnt; undergoes aqueous and igneous fusion — soluble in 2 of water. Oblique rhombic prisms, soluble, look as if wet with water. Largo rcsrular soluble crystals. Deliquescent rhombohedrons. In large crystals, containing SiljO. Six sided efflorescent crystals. Efflorescent oblique rhombic prisms. Sis sided slender prisms. Prismatic acid crystals. Tksts. 1. Soda Salts arc alkaline. 2. They give no precipitates with the Potash tests. 3. Neither Quicklime nor Potash will evolve Ammonia with Sola Salts. 4. Motantimonate of Potash throws down a white precipitate. f). They tinge the blow-pipe flame yellow. 0. On spectrum analysis a bright line is seen in the yellow band. 40- Nami-:?*. F0UMUI,.K, &C, UlSTOHY, Ac. I'llKPAKKn PllOU. DkC0M1"0S1T[0X3. Na,NII„TIP0„4II,0 Microcosiiiic Salt. Disoilio riiospliatc ami SaI;inniioiii;ic in solu- tions, tiUerctevaporatc. Na,ni'0,+Nri,Cl=NaCl+Na,NII„IIP04 Nal'O, N!i,r,O„10ILO 5Iotii])lioHpliatc. l\vropliosi)liatc. lluat Mierocosuiic salt. Heat Disodic Ortlio- phospliatc. Na (Nil,) lI,P0,= H,04-NII,+NalU 2Na,II,P0,=II,0+Na,PA Ammonium NII^ 18 Cliloridc. _ Salaiiiinoniac. Salamiiioniac it Mercury. Place these between Platinum plates and pass electricity tlirou;j;li. NH4CI 7Nii;),sor Liipiid of pis works and irydrochlorio'. NlIJIO+lICl^II.O+NlljCl 2NII,IIO+II,SO,=2IT,0+(NII.),SO, (Nn,),II^((i(\Vf-HIN0,=3CO,+3II,0' +4NII,N0, Siiliiliato, Liil\iid of jxas works and Siilpiiuric'. NlI^NOa Nitrate, Carbonate and Nitric'. iNHJI.CO, (NII,)JI,(CO,0, IJicarbonate. Sc?(iuicarbonatc. Solution of Ammonia and CO, f.'as. Salaninioniae & Chalk. NII,1I0+C0,=NH,IIC03 NIIJIS Sulph-IiyJratc. Liquor Ammonia and 2NII,IIO+2H,S=2II,0+2NIl4lIS Sulpli-liydric'. ' | NIIJIO Ilyilroxidc. Solution of Ainiiinnia. Salaninioniae and Quick-; 2NII,C14-CaO = CaCl,4-H,0+2NH, with limo. I water, this is supposed to form Nil, HO 41 — PUOI'EIITIKS. Tests. White prismatic crystals. Transparent, glassy, fusible, deliquescent. Brilliant peruiaueut crystals, alkaline, soluble. An amalgam is formed, but they cannot be separated. An amalgam is a solution of a metal in Mercury, which has the power of dissolving many metals, as Gold, Silver, &c. White tough fibrous masses, difficult to powder. 1. The odor; moreover the salts are all volatilized by heat. Long flat sis sided prisms, soluble in 2 of water. 2. Tartaric' gives a white precipitate. 3. Platinum Chloride gives a yellow precipitate. 4. Silver Nitrate with Ammonia gives a yellow precipitate. 6. Nessler's test for Ammonia and its salts. — Add a solution of 6 sided prisms, soluble in 2 parts of water. In large crystals soluble in 8 parts of water. In large crysf-tlline musses. Mercuric Chloride to one of x'otassium Iodide and a little caustic Potash, a brown precipitate or coloration is immediately produced, consisting of Dimercur-ammonium Iodide — it is a A fcetid solution used for testing. A pungent alkaline liquid, Sp. gr. 0.891. most delicate test, 2(2KI.HgT,)4-NH,+3KHO=NHg"J. H,0+7KI4-2II,0. — 42 — Naues. F0RMIL.B, lie. IIisTonY, ie. Pefpaiikd From. Decompositions. (NH,),CO, (NHO.CO Carbamate of Ammonia. Dry Ammonia and Carbon Dioxide gases mixed and cooled. Carbamic acid has never been isolated. Carbamide. Dry Ammonia and Pliopgcne gases. 2NII,-fCOCI,=2HCl+(Nn,),CO Caesium Cs. 12.3 Bunscn. 1860 Waters of Durkheim and Nauhcim. Decompose the Chloride with Mercury and electricity. Rubidium Rb. 85 Bunsen. 18G0 In Durkheim and Nau- Leim waters. Prepared like Cajsium. Lithium Argentum Li. 7 Ag. 108 Arfwedson. 1817 Sp. gr. 10.5 Occurs in minerals. Exists as Sulphides and Argentiferous galena, al most every specimen of native Lead Sul- phide contains also i^ilver Sulphide. Prepared like Ctcsium. Density, 0.59. The ore is ground, mixed with common salt, and roasted, which converts the Silver into Chloride, then Iron scraps arc added. 6AgCl+2Fc=2FeCl,+3Ag, AqCl. Chloride. Nitrate and Sodium Chloride. AgNO,+NaCl-NaNO,+AgCl -*-[ri- Iodide. Nitrate and Potassium Iodide. AgNO.+KI=KNO.+AgI. Ag.O Monoxide. Nitrate and solution of Potash. 2AgN0.+KII0=KN0,+IIN0.+Ag,0 A ■!*1 — 46- NlUKS. FORUUL.V, Sit. HiSTOBT, ic. Preparkd Fkoii. DKCOUrOSITIONS. strontium Sr. 87 Hope. 1792 Native as Carbonate and Sulphate. Like Lithium. Density 2.5 Calcium Ca. 40 Davy. 1808 Native as Carbonate and Sulphnte. Like the i'ormer. CaO Oxide (Quicklime). Heat the Carbonate. CaCO,=CO,-fCaO CaHA Hydroxide. Quicklime and Water. Slaked lime & Chlorine gas. Fdund associated with Zinc. CaO+H,0=CaHA (Slaked lime.) CaCl„CaClA Chlorinated Lime . l>CaO+Cl.= CaCl„CaClA Cadmium Cd. 112 Stromeyer. 1817 Prepared with Zinc, it comes over first by distillation. Zinc Zn. 65 Density 6.8 Found as Carbonate ((^alaininc). lluast and mix with Charcoal and distill. ZnCl, Chloride. Zinoand Hydrochloric'. Zn+2HCl = H,+ZnL'l, ZnO Oxide. Heat the Carbomitc. ZnCOn=CO,+ZnO (Philosophers' wool). ZnS0,7H,0 Sulphate. Zine and Sulphuric'. 1 Zn+H,SO<=nj+ZnSO, (white vitriol). ZnCO. Carbonate. Native or from Sulphate and Sodium Carbonate Found pure and as pyrites. ZnSO,+Na,CO,= Na,SO«+ZnCO, Copper Cu (Cuprum) 03.5 Density 8.6 Prepared by a very complicated process (un important ) CuO Cuprio Oxide. Heat (Nipper in iiir. Or heat t'.ie Nitrate. _47- Pbopkrties. Tkbts. A heavy wliite metal, oxydizcs in air. Tingc3 flame carmino-rcd. Bright bands in the blue and yellow of spectrum. A light yellow ozydizablc metal. 1. Alkalies and Carbonates give a white precipitate. 11 grs. dissolve in 1 pint of water at 16°C ; at 100° only 7 grains. 2. Sulphuric' and Oxalic' give white precipitates. (3) Ammonium A white powder called Milk of Lime. Oxalate detects 1-50,000 pt. of a grain. (4) Green and oranga bands are seen in the spectrum. (5) The Chloride gives an orange tint to flame. A disiufeetant and bleacher. Like Tin but harder, it burns, density 8.7 1. Alkalies and Carbonates give white precipitates. (2) Ilydro- sulptiuric' a yellow precipitate. (3) Sulphide of Ammonium gives a yellow precipitate. Blue-white and crystalline. 1. Alkalies and Carbonates white precipitates. 2. Hydrosulphurio' whito precipitate in neutral solutions ; none if acid. White, fusible, deliquescent. A white flocculent powder. .3. Potassium Cyanide a white precipitate. Soluble, right rhonibie prisms. 4. Ammonium Sulphide a white precipitate. Pink when native ; white when precipitated. 5. Charcoal, Sodium Carbonate and the blow-pipe give yellow (ZnO) becomes white on cooling. A red metal. 1. Alkalies give a pale blue precipitate (CuITjOj) Black, dense, soluble in ucids. 2. Ammonia intense blue color. (3) Ammonia Carbonate deep blue. -48- ■;: ? u Kaxes. FoBMVL^, iiO. Distort, &o. PBEfABED FbOM. OROOMPaglTIONI. Cn,0 Cuprous Oxide. Black Oxide & Copper filiD^S. Iloat together ; or from Sulphate, QluooRo, and Fotassium Ilydroxidu. CuS0.,5H,0 Sulphate. Copper and Sulphuric'. Cu+2H,SO,=80,+2H,04-Ctt804 (bluo vitriol ) Hydrargyrum Hg. 200 Density 13.59 Hg"CI, Jlercury. Quicltsilver. Native pure, and as Cinnabar, &c. Roast tho Cinnabar ond oolloot the Mercury as it BublimoH, Mercuric Chloride. Mercuric Sulphate and Sodium Chloride. HgSO,+2NaCl = Na,80.+ng"CI, (Corro- sive Sublimate,) Hg.CI. Mcrcurous Chloride. Mercuric Sulphate.Mcr- cury,Sodium Chloride. HgS0,+Hi,'+2NuCl=Nn,S0,+Ug,CJ, (Calomel,) Hg"I Mercuric Iodide. Mercuric Chloride and rotassiuu) Iodide. Mercury, Iodine, Spirits of Wine. Hg"Cl,+2KI = 2KC14-llg"r, Hg,I. Mercurous Iodide. 2Hg4-I.= Hg,I, HgO Mercuric Oxide. Heat Mercuric Nitrate. 2Hg4-4HNO.=4NO,+21I,0+2nKO (rod precipitate). ) Hg.O Mercurous Oxide. Mcrcurous Nitrate and Solution of Potash, 2HgNO.+2KHO=2KN0.+n,04-H«.O Hg"(NO.). Mercuric Nitrate. Mercuric Oxide and Nitric'. UgO+2liNO,=n,0-fllK"(NO.), Hfr.(NO.).,2H,0 Mercurous Nitrate. Mercury & cold Nitric'. 2Hg-f4nNO.=^2NO,-f2lI,0+nn.(NO,), -49- PllOPKRTlKa. Tksts. Transparent, ruby-red crystals, makes glass red. 4. Carbonates pale blue. (5) Potassium Ferrocyanide a reddish brown. Blue soluble crystals. 6. Sulphhydric' and Annnonium Sulphide give black precipitates. A white, viilatilc, liijuid metal, I'rceZes at — 40^ and boils at iJ.iO^C. 1. All the salts sublime and may be decomposed by heat. 2. Charcoal and dried Sodium Carbonate yield metallic Mercury, (this is the reduction test.) Semitransparcnt masses or prisms, very poisonous. A white powder, insoluble, amorphous, deuKiiy 7.14. 3. Slips of Copper placed in an acidulated solution become covered with Ilg. 4. Stannous Chloride when in excess precipitates the metal. A beautiful scarlet powder, sometimes in crystals. An olive green powder. 1. Sulphhydric acid precipitates.... MBUCDROLS. MKKCl'UIC SALTS. In ked crystals : yellow when finely powdered. Black. Black. Black. Bliick. White then black Olive Green. White. Black. Blick. A dark grey insoluble powder ; seen also in black wash. 3. Alkalies _. 4. Ammonia and its Carbonate.... 5. Alkaline Carbonates Yellow. White. A syrupy liiiuid but may be crystallized. llcd-lirown. 6. Potassium Iodide Red. 7. Hydrochloric Acid or) None. Large colorless soluble crystals. soluble Chlorides j mi "S^ — BO- V. ■ 11 Namks. Plumbum Beryllium FoiiMui,.!;, ike. IIiaToiiV, Ac. I'liKi'AiiEn Fhom. Dkciimi'iihitiii.vk, Us 'SO, Ili-vS I'b Pbr. I'bO Pb,0, I'bO,, I'b.O rbco. Bo I iMcrcuric Sulpliiitc. ! Mercury & Sulpburic'. IIo;4-2ri,SO,=:S(),-t-'ill,()-f ll«S(>, Mercuric SulpbiJe. Native, .iml frmn Rlcr- I'rcpiircMl by it!riil.) rediio H. ri pat Oxide lor a long 3PbO+0=l'b,; t, ( I'iplunibii' 'I'llriDiide.) time. I Iii-vst red lead in Pb,0,+4IINO„-.T21I,0-f 'Jl'b ( N'( i,j,«f Nitiie'. I'bOj Heat tbe .Monoxider t 21'b0=:0+lM).j0 liCail Acetate and Cur- j bon Dioxide mis. 9.4 Occurs ns t^iiicale. j Ciiloride aiid f«odiuni. I'ass tiie v;ipor ol' the (liijoridu iivur .Siidiiiiii, I'BDl'KliTIKS. A wliite crystalline powder. lied, crystalline or anuirphous, used as a paint. A black precipitate. Bluc-wliite, soft, malleable, volatile at a white heat. — Bl — Tests. 1 Yellow powder or in yellow iridescent sspangles. In Ptraw-colnrcd plates. A red, insoluble powder, used as a piint. A deep brown powder called puce hivini. A trrey powder. A wliite insoluble powder called U'/uVc Lcul. A wliite nict.d, often called rilueinuin, density 2 i. 1. Alkalies cause a white precip. 2. Caibnnatos ii wliilo preeI|iitiito. 3. Ammonia a white precipitate. 4. .Sulphniio' a wliito " ! . I . • '5. Sulph-hydric' a black " 0. Amnioiiiiiiii Siil|ihidii ii liliiek, I , I 7. Potassium Iodide, 3'ellow " S. I'Dtiissium tJlironiiilc, yellow, 0. >?odiuni Chloride, white " ,10, Pot.■ls^illlll l''c'rroeyiini(l(', while, : 11. Charcoal, Sodium Carbonate and the bluw-pipo (livii the inrtiil. Its salts are colorless anil sweet; siives no blue beinl will) Coh.ilt. Nitrate and the blow-pipe. — 82 — If '• Naufs. F0HMU1..E &o. Distort, Ac. Phkpabed From. Decompositions. Thorium Th 115.75 Found as Silicates. Clilnride and Sodium. Like Beryllium. Yttrium Y Eb" G1.7 Found as Silicates Chloride and Sodium. Like Beryllium. Erbium 1112.G In yturbite. By a very complicated process of no import- ance. Lanthanum La 92.8 Cerite, Allnnito. Chloride and Sodium. Like Beryllium. Didynium Di 9C (■ryplolito, &c. Chloride and Sodium. Like Beryllium. An nUoy is a mixture of metals, which may b; cither ii'tturnl or arliCiclnl, the latter being produced by simply fusing the metals together. The alloy formed between Pt, Pd, Rh, Ir and Fe is an illustration of the first variety or native, and the following will gcrv as examples of those artificially prepared : — Gun metal Cu !)0 Sn 10 parts. Bronze Cu 91. Sn fi, Pb 1. Brass Cu .'8, Zn 34. Bell metal Cu 78, Sn 'J2. Speculum metal Cu 75, Sn 25. German .-ilver Cu 100, Zn GO, Ni 40 Biitannia metal Sn 9, Sb 1, and soinctiines also small quantities of Cu, Zn and Bi Pewter I'lumbcrs' Solder Fine Solder Type mctiil Standard Silver Standard Gold Zn 12, Sb l,Cu (a little). Pb 2. Sn I, Pb 1, Sn 2. Pb 7:?, Sb 17, Sn 10. Ag222, Cu 18. An 22, Cu (or Ag) 2, When Ilg is one of the component metals, the alloy is called an amalgnm; thus, wo have the amalgams of Au, Ag, Sn, NII4, &0' — S3~ I'Rdl'KRTIKS. Tests. A prey jinwilcr, acquirinf; a iiietallic lusrre by pressure. A blttckish j^rey powder. Alkalies precipitate white Hydrates. Never isolated ; the salts are rosc-colorcd. Erbia is rose-colored. Characteristic bands arc seen in the spectrum. Grey powder, detoiuposcs water, salts colorleHs. Alkalies throw down white Hydrates. Grey piiwdi^r, docoiiipo-es water, salts ro-e-cnlnrcd. Alkalies cause rose-colored precipitates. Dislilldtion is an operation in which a volatile substance is converted by heat into a vapor, which is afterwards condensed in a 6uit;ible appiratus where it assumes a liipiid form. But when the product condonres as a solid then the process is termed SiiUimalion, When dry organic matter is distilled until all volatile products are expelled, the operation is called Dry or Destructive Distillntion, When several volatile substances, having dilTerent boiling points, .re in a state of mixture, they may be separated by Fractional Distillntion ; i. e, by collecting the products as they arc driven off at dilTerent degrees of heat, and condensing them separately. Pruipitiiiion is produced when a body passes to the solid state so rapidly as to previ nt the particles from arranging themselves into any regular form, and therefore the substance falls as a more or less fine powder. (.■ii/stnlliz'ition. — When bodies in passing from the liquid or gaseous states assume regular geometrical forms, the process is termed crystallization, and the solid bodies cri/stnls. 54 TRIAD >'l u Namks. F(inMn,.K, ito. IIJSTOBY, Ac. PliKl'AnEl) FllO\f. Di:i"OMi>osrri(i\s. Aluminum Al 27.4- ' Density 2.0 Cliloriilc niid Fodiu-n. Alumina, Oil. Lamp- blat'ii and Chlorine. Like IJeryllium. Al.Cle CliloriJo. Alp .;-r,+('l,=:3C0+AUCl„ j:ot by dis- tillation. Al,Oa Oxiilc (AluiiiiiKi). isolation of Alum ami Ammonia. AIJI.O,, fills down ; this must be ignited Al;(), remains. A1,'"(S0.). Sulpliatc. Aluminum Hydrate and ^ulpliuric'. This Siiliihate eomliiiies with other Sulphates as Silver, Huhidiuni and Amnioniuiu (ormiiiii .\'nms Al'"NFI,(SO,).,4-12 Common Alum. H,0 Isniaili' Irom Aluminous ]t is roisod. i'X'«)scil to air. lixiviatccl with Clay. watiT. Sa -.. nioiiiae is addod to remove lion, tins IS ('rystaliizcd. Cerium Co 92 Kiaprofli. 1803 Fi'iim the Ciiloride and Soilinm. Found in Iron and Cop- per jiyrites. Like IJeryllium. Thallium Tl 20-1 Crookcs. IbGl Subject ii solution of the Sulphates to elec- ti'olysis. Aurum (Gold) Au l'JG.7 Density 11).5 Found puro.orin alloys: 2Au('l:,4-(;FeS04=2Fc;"(SO,)a+2Fc"'Cl3 j;iit hy ilissolvinj; it in -j-AUj Nilrornuri itic' and jincipitalin;; with Ferrous Sulphate. AuCl 1 Aureus CMoridn. AuCl, ' Anrio Clilori.Ic. Heat Auric Chloiide. AuCr-Cl,+AuCl (joM & Nitromuriatic'. i METALS. Q8 Pbopertiks. Silvcr-liko, unaffectcil by nir, Snlpliurcttcd llydrnircn, &c. Tksts. A transparent, waxy, culork'ss sub.-tance, with a urystullino .■•tructuro. A white, tasteless, coherent mass. Thin pearly phitcH, sweet astrini^ent t:i;-te ami acid reaction. Many so called Alums cont.iin no alum, it is replaced by Iron, Malitraiiese, &c. Common Ammonia Alum is in lar^o crystals. 1. Alkalies give white precipitate-i, soluble in excess. \i. Ammonia iina a white precipitate insoluble in esccss. ?>. Carbonates liivc white precipitates insoluble in excess. 4. Amnmnium Sul[)hide ;;ives a white precipitate of Hydrate. 5. Any salt of Aluminum with Cobalt Nitrate, gives a very A grey powder, decompo-es water, the salts are colorless. characteristic blue bead with the blow-pipe. ^iolid Potassium Sulphate gives a white precipitate with a Cerous salt. A soft lead-like metal, streaks pnper like I'lnmbngo. A soil vellow metal, soluble in Selenie Aeil and in Nitrnmuri.itie, is the most m:illeil)le oi' metals, it may bo beaten into leaves 1 2U0,0U0 of an inch thick. A yellowish white mass. A red ervstalline miss, verv ile!ii|iie-e iit. (lives iin intiMisi' ureoii line in tlu! s|icctruiti, INimimuiiotiU?.- !i k'reon colnr tu tiiiiiio. Cburcuali Smlumi Carbunalo iiiij iIib 1)1"W-impo reduce it. I TilALLIIUS. THAI.I.IC. 4. Alkiilics, Ammonia and Ciirh'-njite.-* yivo A. riilniidcs iind liroiiiidcs-- (1. (Ix;ilic' Arid 7. I'hiifphcirii) Acid 8. Ari»enio II. I'otatisiuin Ferrooynnido. ■ 10. !'i)(iissiiiin Fi'rncyiinido,. 11. I'liliissium Chniiimto !'_'. IMalinic Chlurides If. Iiididos 1 1. /,ii c :iTid trim ttirnw d"wn iTV-liil^ i.t Tliolli'im f""" all iis pnlts. Notliing. Brown precip Wliiiu. None. Mono. AVIiiii' pieeip. White. White. Vellow. Yellow. (ireen. Yelluw. Yellow. Pale yet low. Yellow. Ti Sirs Foi; Oiil.i). 1. Ferrous Sulpliaieaivr-i a brown prt'uipit itc. ■J. The blow pipe };ivca :i metallic li",id. ;'.^tannou,.!Cllloride^'iv•P3 Ihe l^nriilr nf CVoofirv, l.(j.\alie Acid slowly rediiee;' Hold. 5. Siilph-hydrie' civcs a blai'k priM'ipilaio su- hiblo in Anaip.inia Ml 66 TETRAD ■^ .'■'; Names. Ft). MUl.E &o. History, Ac. Paifi'ABED From. Decompo!»ition». Platinum Pt 10.74 Density 21.5 Kxists usnnlly as an alloy of Si Ivor, &c. Prrpari'd like Aureus (.'lijnriilc. Tlie preparation is very complicated. Ft"Clj Piatlnous Cliloridc. Platliiio Chloride. Pt'^CI, J'latinum and >"itro- muriatic'. Palladium I'd lOli.D Density 11.8 Associated with I'iati- num. Unimportant. Rhodium llh 104 Density 10.6 Assneiated witli I'lati- DUin also. Unimportant. Iridium Ir 198 Density 21.15 Associated with the former. Ruthenium Ku 104 Density 8.G Assnciatcd with the Ibrnier. Osmium 03 199 Density 10 Associated with the forcgointt. METALS. 87 PnOPERTlES. Tksth. Forms 2 sotj of salts, one set dyad, the other tetrad. 1. Sulph-liydrio' iiml AtiiiMoniuin Sulphide give a brown precipitate. Insoluble j^rcenish-gfey powder. 2. Tho^ChloriJo tliniWH down n yellow precipitate with Potash and with Aniinniiin, but not with Soda, and is used in analysis to separate K from Ntt. A red or brown deliquescent mass. Resembles Platinum and also forms 2 sets of salts. r 1. MtTomy Cyiinldii kIvcn n yi'ltnw prprlpltiiU-. \ 2, i'otiiHsiimt Imllilii kIvi'M It lilitc'k prucip., will iletect 1 in 500,(100 parts. Wiiite, coherent, spongy, biittle; salts are piuk. t 1. Siilpli-liyilrlii' mill Aliiinnnliim MiilpliMi! nivc n bro-vr. prcoipitiite. J 2. SnlplmtdH 11 ViOlmv (pule), (;i) Ainiiioniii .,:. 1 CarbonatiM n yollow. J 4. AlUiillnii i;|ilmli|i'N mill ^fl'rnlry Cyaniilc givu no prucipitates. ( 5 Zinc pruL'ipltuti'N iii.tulllf llliiiilliim. A white, brittle metal ; forms Iridious and Iridic Salts. Ammonium or PotimHluin CJiilorldo gives a dark brown-red precipitate. Porous masses ; also forms 2 sets of salts. 'I. Fused witli riidiUBliiMi NItfiitn It formi* nn ornnpre-red solution. ' 2. FotnfiHluni Hiilpliii-(!yitiiatu kIvoa n rL'd,chauKing to violut on licating. 3. Lead Actat" kIvi'K u purplifrod prufipitate. A black metal : it forms Osmious and Osmic Salts. ■ 1. Pungont, dlmiKriMiiilild odof wIkui licati'd, irritatino: and noisr.uoiis. 2. Sulpli-hydijij' U AiiUMnnlitln Hiilplilduulvoaycllow-biown precipitate. 3. Silvur Njtrati', ollvi'-Ki M. (4) Stannous Cliloride a brown. 5. Tannin no pi'Ki'lpllati'i blitaliluo color. (G) Potassium solutions a dark brown, 7. Potassium I'Viriniyrtiildo gfocn and then blue. ^8) Potassium Iodide purplii-rml, D. Zinc and Hodinni l'*ofm«to thniw down metallic Osmium. -B8- Namks. FonMui..G, &e. UlSTOBY, ite. Prki'arkd Fiiosi. Okcuufositions. Ferrum (Iron) Fo 5G Density 7.8 Found pure and as Sulphide. Iron and Hydrochloric'. Proceed as for getting .^l anganesc. Fed, Ferrous Chloride. Ferric Chloride. Fe+2nCl = II,+FeUl, Fo.CI. Ferrous Chloride, Ily- drnchlorio' and Nitric'. CFeCl,+6IICl+2lINO,-2NO+4IJ,0+ 3Fe,,Cl, FcO Ferrous Oxide. Solution ot a Ferrous Salt and Ammonia. Solution of a Ferric Salt and Ammonia. Dry the white precipitate in an atmosphero of Ilydroiren. Fe,0. Ferric Oxide Dry the precipitate. Fe,0, Fcrroso-ferrio Oxide. From a solution of the mixed Sulphates and Sodium Hydroxide. Occurs native also as Loadstone. ( (a) FcSO,+2NaIIO = Xa,SO.+Fe2HO ) (b) Fc.,(SO,),+CXaI10=3Na,S0.4- 1 ' Fe,t;II() ( (c) Fc2UO+FcXjnO = 4II.,0+re304 K.FoO, Potassium Ferrate. Ferrous Sulphate. Ferric Oxide and Nitre heated. FeOj and IIjFeOj have never been isolated. Fc"S04 From Iron pyrites (Fc SO. FeS,+Fe4-40,=2FeSO« Fe'",(S0.)3 Ferric Sulphate. Ferrous Sulphate, Sul- CFeSO.+3II,SO,+2IINO,=4lIjO+2NO phuric', and Nitric'. [ +3Fe,(S04), Titonium Ti 50 Density 50 Titanium Potassio-Flu- oridc and Potassium. Red h' •89- Pbopkbtirs. Tests. White, soft, tough. 1. 2. 3. 4. 5. «. 7. Alkalies, Ammonia and Car- bonates give PKimoiH. riRnic. Wliite becoming green tlieu brown. No cliange. Black. Wbite turns blue. None niuo None Grcon, deliquescent crystals, oxydizo rnpidly in air. Fo.xy red. Red liydrated crystals, soluble in water and in alcohol. Sulph-hydric' Wliito (Sulpliur.) White, becomes dark green and then red on cxjiosuro. Ammonium Sulpliide Potassium Ferrocyanide .... Potassium Sulphocyanide... Potassium Ferrioyanidu.... '''incture of Galls liliitk. KcdJish brown ; occurs native as Hicmatite. Blue. l!loo(!-re;I. In powder or in octahedral crystals, magnetic. Green, lilue black. With ice cold water it forms a deep amethystine colored solution of K,I'cO,. Green, soluble crystals, called Copperas or green vitriol. A buff colored amorphou.s mass. llesemblcs Tin, forms 2 sets of salts also. 1. Tincture of Galls gives an orange precipitate. 2. Potassium Firrocviinide gives a dark browu. 3. liorax and Titanic O.vide form a glass which is yellow while hot, but becomes violet in cooling 60 Namrs. F0BMUI,.B, io. HiSTOIlY, i-0. Prki-arkd Fiiom. Decompositions. Manganesium Mil 55 Density 7.115 Manganous Oxide. Calcined Carlionate, Borax, Ciinrcoal, Packed in a crucible and fused by a red heat. MnO Carbonate and Hydro- gen gas. Pass the gas over the heated Carbonate. MD3O4 M nnsranoso-manganic Oxido. Native as ilausuiannitc. Or heat MnOa to whiteness in the air. Mn.O, Manganic Oxide. Native. Expose hydrated monoxide to the air. MnO, Binoxidc. The moti. commoa na- tural form. A natural mineral. Biclihirido and an Al- kaline Carbonate. Called Pyrolusite. Mn,0, Varvicito. MnCO, Carbo;iato. Manganatc of Potash. Mix the solutions and it falls as a precipitate. K.MnO, Fuse Binoxidc with Potash. Manganic Acid has never been isolated. KjMiijO, Permanganate of Potasli. Manganafc and water. :)K,MnO,-(-2II,0 = MnO,,-f-4KIIO+ K,MnA Stannum Sn (Tin) 11 G Density 7.3 Found chiefly ns Tin Oxide. The ore is crushed and heated with coal ; the Tin fuses out. Il.SnO, Stannic Acid. Alkaline Stannntcs and un acid. — Gl- Pr.i.. ..a..f:o. Tksts. A reddish, brittle, lustrous metal, decomposes water. I. 2. 4. 5. G. A green powder ; a strong base. Alkalies, Ammonia and Carbonates give white precipitates, becoming brown. A neutral oxide. Sulph-hydric', no change. Brown or black ; a leuble base. Ammonium Sulphide, a flesh colored Sulphide. Black ; 5 neutral oxide. Potassium Ferrocyanide, a white precipitate. Kesoinbles .MnU..., but is liarder and more brilliant. An insoluble bulT-colorea or white powder; when heated it COj and absorbs 0. ioses With Borax and a blow-pipe, forms an amethystine-red bead in the outer flame, and none in the inner flame. Heated on Platinum foil with Sodium Carbonate it yields a green mass of Sodium iManganate. A {^reen salino mass, may be in crystals. Dark purple crystals. Condy's fluid is a solution of this salt. White; when htited it oxydizes toriuiw^ putti/ powdtr. 1. 2. 3. Alk'ilit's, Ammonia find Carbonatefl BTANNOCa. Wliito. Darli brown, Purple. STANNIC. There is also a Metastannio Acid (lI,„Sn40,s). Wliito. Sulpli-liyilriu' am' Ammonium Sulpliiile.... Auric Chloride Yellow, None. 11 i — 62 't: Nauks. FoRMUL.E, Jto. UlSTORT, &a. rnKPAHKi) From. DKfdMi'imrriiiNH. Uranium U 120 Density 18.4 Uranous Oxide. Deeompase the Chlo- riilc witli Potassiuin. Fdiinil ill Uruiiito and I'itehblendo. These salt.s nro used in Plidtogrniihy and in enamel painting;. UO UjOj and Hydrogen. Ilcat tiie former in a Htrnani ol' the latter gaH. u.o, u.o. Uranoso-uranic Oxide, Uraiiic Oxide Ignite the metal in air. Heat the Nitrate. Metal and Chlorine gas. UCl,^ Uranous Chloride. Ilcat the metal in tlio pm, Uraiiic 0::ycliloride. Uranous OxiJo and Chlorine ga.s. Kxist.s in Zinc blende. Found as au Arsenide. Indium In 74 Ni ■ 58.8 It wa,'* discovered by hpcoiniui an»!y^'iH. Nickel Density 8.8 Heat the Oxalate to it white liuat. Cobalt Co 58.8 Density 8.5 Found associated with Nickel. And obtained like that metal. Cn(NO,). CoCl. Cobaitous Nitrate. Cobaltous Cliloridc. Metal and Nitric'. Oxide & Hydrochloric'. 63- Proi'kiities. A black powdor, or in fused white ni;llcab1e globules, it forms llran- ous and Uranic Insults. A brown powder, sometimes crystalline, dissolves in acids and forms {jrecn salts. A dark green soft powder. A yellowish powder— it unites with luctuls and forms salts called Ifmnntes. In dark-screen regular octahedron crystals, forininjj; an emerald- green solution witli water. A yoUow crystalline mass, soluble in water. Soft, lead-grey, blackens paper like lead. White and malleable ; the salts arc unimportant. AVhite, brilliant, tenacious : forms two sets of salts. Used in the laboratory in blow- pipe tests, llose-colorcd crystals. Tksts. UnANIC. 1. Water forms solutions that arc Green Yellow. 2. Caustie Alkalies give a Ileil-lirowu Yelliiw. 3. Alkaline Carbonates give Uieen Yellow. 4. Ammonium Sulphide liliiek Kdue. 5. Potassium Feirocyanide Ueil-lirowni 6. Borax and a Plioaphorous ealt with any salt of Uranium, will form u green glass. Indium gives 2 indigo-colored linos in the spectrum. ' 1. AlknlieB, Ammonia .lue).'r(nviiif; red, 2. Ammonia '■ lied grows brown. 3. Sodium & Ammonium Carbonate.! I'iuk. 4. PotflShium Kerroeyanide I Gr.yi,-li green. 5. I'otjisfiium Cyanide jYellowisli brown. tj. rulph-hydric' No ( liiiiige. 7, Ammonium Sulphide, I'laek. conALTia. Dark brown. Brownish red. tirueii, Blaek. 64 .1 ill PENTAD Names. FonMUL.s, lie. HiSTOBT, iL-0, Prepaeed FnoM. Decompobitionb. Stibium Sb 122 SbCl, Density 6.8 Found as Sulphide. Antimonious Sulpliidc and Hydrochloric'. The nictul, hcut and Chlorine gas. Zinc, Sulphuric', Anti- monious Oxide. Antimonious Sulphide, Water and Soda Car- bonate. Freed by fusion, &o., called Antimony. Antimonious CliloriJc. Sb,Sa+GHCl=3H,S-f2ShCI. SbCl. Antinionic Chloride. Antlnioniurcttod lly- droffon. Stibine. Sb4-5Cl=SbCl. Sbll, Sb,0. Autinionioua Oxide. 2SbCl,-f3Na,CO,=6NttCl-f:iCO,4.Hb,0, sbA Tctroxido. Antiinou'o Oxide. Native us Corvantite. Or heat the metal in the air for doniu tlnio. Sb,0. H8bO., Antimonic Anhydride. Heat Antinionic Hydrate. Antimonic Acid. Mctttntimonic Acid. Antimony and Nitric'. H.Sb,0, Antinionic Chloride and Water. 2SbCl,+7H.O=10HC4-H,Kb,O, K,H,Sb,0, Potassium Hydrogen Metniitinionatc. Antinionato of Potash. l'otas.'*ium Antimonate & I'otassium Hydrate. Fuse together. KSbO, Antimony and Nitre. Fuse together. SbA Antimonious Sulphide. Native. (}nlled Black Antimony, Sb,S. Autimonio Huiphido. Tcrsulphide, Sodium Carbonate, Sulphur, and Lime Hydrate. Boil in water and ndd diluloil HiilphiirlK A(ii(i and SbjOj falls down ((julden .Siiijiliiiriil.), METALS. PllOPERTIES. Tksts. Bluisli-wliite, lustrous, brittle, crystalline. A wliiite crystalline mass, its solution is Butter of Antimony. A colorless volatile liquid. 1. Ammonium Sulphide gives an orange precipitate, 2. Alkalies and Carbonates give white precipifntes. A gas, burns with a greenish flame. A white powder, acts as an acid and forms Antimonites, which arc liowevcr very unstable. 3. Zinc and Iron reduce the salts to the metal, ns a blnek powJor. 4. SbHs burns and deposits 2 rings on a plate hold in tlie (liiino soluble in Ammonium Sulphide, but not in a snlutinn of V,h\rf rinated Lime, nor in Nitric', which distinguirthoN it from ArKoiil- urctted Hydrogen (.^sH,). 5. i'used with Charcoal and Sodium Carbonate, a britlla Kl"lMlle of Antimonium appears, and the Charcoal is covered Ibr snnio distance with the O.xide (SbjO,). A grcy-whito powder, infusible. A straw-colored acid powder, insoluble in water. A white powder, soluble, aciil, monobasie. It is dibasic and forms 2 series of salts, normal and acid Metanti- monates. Its solution is used as a test lor Sodium, with which it gives a white granular precipitate, the only known insoluble .^alt of Soda. The.«e 2 acids resemble iMetaphosphorie' (lIl'Oj) and Pyrophos- phoric' (II.P.O,). Lcid iirey, brittle, crystalline. A golden-yellow, flocculent powder. -ee- NaUE!). FoimnL^, ielyl ._74. OxiDESi !lETH'^u^. (CJI.).O (CJI,).A) (cjr„).o (C.H,3),() (C,II„)...0 (CnIL3).0 (C„n,„),o (CJl3,).0 IIydhoxiuks (Ik Alcoholb. cn3Ho CHJIO CJI,1I0 CJI.IIO cyi„iio C.IIJIO C,II,.1I0 ChII„IIO C,II„IIO c,oii„iio C„1I„1U) C„II,.HO C„II,,IIO C,.H,,IIO c„ii.3iio c,,Ti„no C,„II.,IIO AldEIIYI)E3. CH,0 C,H,0 CJI,0 C,II,„0 C,JI„0 C,I1„0 C,oII,oO C„II„0 ACIDB. CHO, C,H„0, C.H„0, c.ii„o, CioHjoOi C|,n„o, c„ii„u, LjjIijjUj I Formic'. Acetic', Propianio'. Butylio'. Valerianic'. Caproic'. (Enanthylic' Capric'. Peiarf^onic'. ^Uutic'. Laurie'. Cj,n„0, Myristic'. Palmitic'. 3Iar:j;ario'. Stearic'. Araehic'. liehenic'. Ccrotic'. Melissic'. Wherever vacancies occur in this tabic it indicates that such compounds have not yet been isolated. It will be observed that the saturated compounds nrc rejjarded as Jfi/druks of the fomjmiuil nulioils, the ojulet are known as Ethers, tlie lii/dio.n'des as Alcohols, their compounds with Acetic' and other acida are called Ethercul iSalls, each furnishes an AhUh^Ju and ouo or more acids. — 73 — Sulurated Ilydio-Carhons may however be t prived of one or more molecules of IT, and give rise to new Jiomologous series ; thus, Methane CHj may become CHj, Ethane CJIe is cor .crtcd into CjHj, Propane CjHg forms C^Hs, &c., &c., these arc therefore molecules of unsaturated hydro-carhons, having two bonds frco and unconibined, and on this account they act as Dyads, And again CjHj, C3H,., and C4II, may each by appropriate means lose anotlior molecule of H, and other new series arise^ viz. : — CjHj, CjHj, CJTs, each being a quadrivalent or tetrad radical. The following table will better illustrate these series, it includes however only the first 6, together with the names that have been proposed for each by Dr. Hofman ; — let Sories PakaKI'INS. 2nd Sories. Olkfinks. 3rd Series. 4th Series. 5tli Series. 6th Series. 7th Series. CII, Methane. Methene. c.ii. Ethane. CJI, Ethenu. CJT, Etliinc. Propane. C3II, Propcuc. CJT. Propine. Propone. C.H,o Quartane. Quartcnc. cji, Quartino. c,ii. Quartone. CJT, Quartuno. QuiTitano. Quintcno. Quiutinc. Quintono. Sextone. Quintuno. Sextune. cjr, C,;H,. Sextuiio. C,H|, Scstene. C.TI,o Sextinc. CeH, C.H, m II - 76 — If the preceding table be read from left to ri^bt, each line will pre in t an isologous series, each molcoulo dilToring from tbo one preceding it by H, less, but if read from above downwards then it affords an example of a homologous scries, nboro ouoh (lilforM from its immediate neighbours in CH,. It has been shewn already that saturated hydro-carbons may give up one or more of their II atoms in oxchnn>;o fur iinothcr element; thus, from Methane CII4 we may get CH3CI, CllaClj, CIICI3, and CClj, and these suhstilntion compnumh may ho ronnrdod as being formed of CI with radicals CH,', CHj", CH'", and C'^', which arc monad, dyad, triad and tetrad rcspoctivoly ; llir ijumilivnknce Jppendinj altogether upon the numher of 11 atoms wilhdraKnfrom the original saturated molecule. Tiioso of even (|UiuilivaU'nuo, dyads and tetrads, contain even numbers of II atoms, but tho'.o of uneven quantivalence, monads, triads and pentads, oontiiin odd numbers of II atoms, and are supposed to exist as double molecules, as seen in Methyl (CHj),, Ethyl (CjIIj),, &o. These lultur am diHtinguished by names ending in yl. The annexed table will illustrate these peculiarities regarding the quantivalence, as well uh tliii manner in which these compounds are named. CH. Methaue. (CII,)' Methyl. Methene. (CIl)'" Mothcnyl. (CJI,)'" Ethenyl. (CJIO'" Propenyl. Clle Ethane. (C,II,)- Ethyl. CCJi)" Etheuo. Ethine. (CJI)^ Ethinyl. (C.II.)^ Propinyl. CJI, Propane. (C.II,)' Propyl (CJI.O" Propcnc. (CJI,)'^- Propine. Propuno, (C.rir" Proponyl, All the Oi'.OANic Compounds may be arranged into the following 20 groups ; Class 1. Ilydro-carbnns with even number of Hydrogen atoms. Class 6. Mercaptans or Sulphur Alonhols. Class 2. Alcohols. Class G. Selenium Alcohols Class 3. Haloid Ethers. Class 7. Sulphur and Selenium Ethers. Class 4. Oxygen Ethers. Class 8 Compound Ethers. Class 9. Aldehydes. Class 10. Organic Acids. Class II. Acid Halldes, Class 12. Acid Oxides. Class 13. Ketones. — 77 — Class 16. Phosphorus, Arsenic and Antimony coiT.pounds, resem- bling those of Classes 14 and 15. Class 17. Organo-metallio compounds not analagous to Ammonia or Ammonium salts. Class 18. Amides. Class 19. Amic acids. Class 20. Substances not included in any of the preceding groups. Class 14. Amines. Class 15. Alcoholic Ammonium compounds. Each of these classes we will now proceed to describe : 1st Cl'iss. — Hydro-carbons witu even no.mhers of HyrnoQEN atoms; yet it must not be forgotten that these aic often regarded as Hydrides of organic radicals containing uneven numbers of H ato'iip ; thus, CHj may be considered to be CHjH. Now let us turn again to Dr. Hofmau"s table of the Hydro-ei.rbons at page 75, and eiiamine separately the various series which it presents to us : — Id Series. — C,|Ha-|-j* or Paraffins (pariim offiuis) wliich are all saturated hydro-carbons, and owe their name to the fact that from being saturated they show no tendency to unite with other substances. No less than 10 of the paraffins have been prepared, con. taining from I to 16 atoms of Caibon in each molecule; many of them exist naturally in both American and other mineral oils; they are: — (1) Methane CH, {2) Ethane CJI, (3) Propane Cllg (4) Quartanc CJI,„ (5) Quintano C,H„ (6) Scxtane C,IIu (7) Soptane C,H,j (8) Ootane CJI,, (9) Nonano C9H30 (10) Decane CiJI,, (11) Undecanc C„H.„ (12) Duodecane Ci,Hj, (13) Tridecane C„H., (14) QuatuordecancCuHji, (15)Quindecano CuHj, (16)Sexdooane C„H34 The first four of these arc fas«e. us. the rest arc liquids, whoso boiling points and specific gravities rise as the molecular weight incrca.ses ; though natural productions yet they can be prepared artificially ; 1st. By the action of Zinc on Alcoholic Iodides ; 2nd. Ry the dry distillation of Boghead and Cannel coal, &c. 4( In a formula like this C„ U j -\-i tbu n stands for any number of Carbon atoms. — 78 — 2nd Series. — C„Il3„ or Olcfines ; these arc all exact multiples of CHj ; they arc 13 in number :— Methcnc CHj Ethene CjH4 Propeno CjHj Quarteno CJIj Quir.tene CjHk, Sextenc CjH „ Scptcne 0,11,4 Octcnc Cgil,,, Nonene CJIu Decene C,(|IT~o Sexdcceno C,eII„ Septivigintcne CjJIj, The higher compounds of this scries are solid, the lower encs are gaseous, and the intermediate are liquid, and tluilr builiii^ |ii)iulN rise also with the increase of the Carbon atom in their constitution. Tlicy may be prepared by decomposing nascent I'liniHliiH l)y tliu action of Zinc or Sodium on Alcoholic Iodides, or by decomposing at a red heat Butyrates, Acetates, &c. 3rd Series. — C„IIj — ,. Five only of those have been procured ; they arc : — Ethine C,H, Propino C3II4 Quartine C^IIe Quintinc CjIIs Hextino t'jil,, The first two are gases, the others arc liquids. They may be prepared by heating Sodium Ethylato with Hrnniidpn of tho Olefine derivatives. 4lh Series. — C„I1,„ — j. Quintono CjTIj is the only known compound of this series; and certain voliililo oils Cimiiil rfiiidy formed in some particular plants, called Terpcncs, C,JI,iii arc also included under this head. <^, !ntonc is a liquid and may be prepared from Alcoholic Potiish with Quintinc Dibromidc ; it is both sexvalent and (ilriivniitnt. Terpev.es are found more Ofpecially in Coniferous and Aurantiaecous plants ; they include Oils of Turpentiiu), Uer^'uiiint, Lumon, Orange, Caraway, Cloves, Juniper, Thyme and many others. ^th Series. — C„Hj„ — or Aromatic Ilydro-carbons. Six only have been prepared, they arc ; — Benzene CaHg Toluene C,II, Xylene C(II„ Cumnno C,Hi, Cymeno C,oII,4 Ainyliylone CJiJIi, Except the last they may all bo procured by fractional distillation from tho lighter oil obtained during tho degtruotlvn di«lill(itlon of coal ; they arc nil liquids, 8th &TKS.— C„IL„— 12. dth Serks.—CJl^—U. lOth Series.— C„U,,—\6. Uth ScnVs.— C„IIj„— 18. V2lh »SVriM.— C„IL„— 24. -79- 6tJi Series. — C,,!!,,, — 8. Two only of these have been prepared, viz.: I'hcnylcne CoH, and Cinnamcno CJIbj liltio In known concerning the first, but the latter is an oil and exists in Storax. ItJi Series. — C„IL„ — 10. Only two of these arc supposed to have been separated and they are not yet named. Naphthalene C,„II, only has been proeurcd ; it is unimportant. Diphenyl C|.,II|o and Dibenzyl CuIIn are alone known of this series, both are solids. Stilbcne CuIIu only is prepared ; it is in mother-of-pearl-iike plates. Anthracene C,|II,o is prepared by the dry distillation of coal, it is in small micaceous platoH, Chryseno CiJIu, heat Diphenyl in a tube with II gas, it is in yellow crystall'iic plates. Class IF. — AlcoiIolc ; these arc organic compounds composed of hydro-carbon radicals (hence called Alcohol radieiil.t) ooinblliccl with (HO) Ilydroxyl. The tcriii Alcohol was at one time applied exclusively to Spirits of Wine, but is now used to (U!'ij,'niilo a numerous class of organic compounds, which differ greatly from each other both in appearance and in properties, but yet thi'y ri'Hcinblo one another however, in being all saturated hydrocarbons in which one or more of the II atoms have been replaced by (FlO) Ifyiiroxyl ; and IS these radicals differ from each other iu their quantivalence, so wc may have monatomic, diiitomic; (riatomio anil imli/nliimiii Alcohols, according to the number of (HO) Ilydroxyl molecules tb.ey contain ; thus, from Propane CJIs three Alcohols may bn |ii'n(Mirt'it i (CjH,)' (110) or Propyl Alcohol, which is monatomic ; (CJIo)" (HO)i Propene Alcnhol, which is diatomic; and (CaU,,)'" ( ilO), or Propenyl Alcohol, which is triatomic. Alcohols may also bo divided into ;»rimf(n/, srco»(fan/ or fcr(i'(ry according as the atom of Carbon that is combinel wllli llir Ilydroxyl is also directly united with 1, 2 or 3 other carbon atoms ; thus : c-5 \l % (no CILCH, CIL o 8 «3 ci OH, CHj 1 CHa % { HO H 80 MONATOMIC ALCOHOLS AND SOME SUBSTANCKS. FORUUI,^, Synonyms. Prepared From. Process and Decompositions. Methyl Alcohol CH,(HO) Methyl Alcohol. Wood Spirit. Hydroxymethane. Carbinol. (1) Oil of Wintcrgrcen and solution of Potash. (2) Destructive distil- lation of wood. (1) C,HA,nCH,+KHO=KHC,HA +CH,(HO) (2) It conies over first on distillinp; wood ; add Lime, which forms Pyroiignite, and distill. UH,0, Formic Acid. Methyl Chloride. Wood Spirit and Air. CH,HO-f 0,= H,0-f CH jO, CH,C1 Wood Spirit, Sulpiiuric' and Sodium Chloride. 00 CH,II0+H,S0.= H,0+CIl3,H.S0, (t) CH„HS0,-f NaCl = NaHSO,-f CH,C1 CHJ Methyl Iodide. Woad Spirit,Phosphorus a id Iodine. Prepared by distillation. (CH.),0 Methyl Oxide or Ether. Wood Spirit and Sul- phuric'. ('ll, it burns, the vapor causes coughing and diffieidty in breathing. It becomes oxydized in the air, or with Platinum black ; thus, CVir„lI0+0;,= II,,0-|-('3n,0 or Valcnunic Acid. The same is elTocted by Fousel Oil, Sulphuric' and I'otassium Bichromate. — 84 - SCBSTANCKS. Formula, &o. Synonyms. Pbkfabkd Fnou, PB00E83 AND DECOMPOSITION. Hexyl Alcohol c.n„(iio) American Petroleum, &c. Process complicated. Heptyl Alcohol C,II,,(IIO) Hydrogen and (Enan- thylic Aldehyde. C,IImO+II,=C,II.,(HOj Octyl Alcohol C.H„(HO) Castor Oil and Potash. C,JI„034-2KnO = KjC,.lI,oO,+ II,+ 1 CJI„(IIO) Nonyl Alcohol C,H„(HO) 1 American Petroleum. SexdecylAlcoh'l C,6n33(HO) Cctyl Alcohol. Spcrmacetti and Potash. C„II„0„C,„H„+KII0 = KC,„1I,.0,+ C,oII«(iIO) Oeryl Alcohol C„H„(HO) Chinese Wax and Potash. C,,II„0=,0„H,,,+KHO=KC„H,A+ c„H,,,(HO) Myricyl Alcohol C3on|j|(HO) Bees Wax and Potash, The decomposition is like the precodinsj;. Besides these nionatomic Alcohols wc havo others constituted as follows : — Vinyl Alcohol 02113(110) ; Allyl Alcohol Callj(IIO) ; Camphol C,.n„(HO) ; Styryl Alcohol CjrXlIO) ; Cholesterine C,|,H,,(HO). POLYATOMIC ALCOHOLS AND SOME Diatomic Alco- hols. (C.,1U"(H0), They are called Glycols. Four only of these Al- I cohols are known. They are Ethone Alcohol CJI^(IIO),; Propene Alcohol CalleCHO), ; - 88 — Phopertirs, Ac. TKIItl AMI) Rkuarkb. Tlicro arc 10 cf these Isomeric Alcoho.?, viz. : 3 primary, 4 second- ary, and 3 tertiary, Unlmportont. A colorless oily aromatic liquid, insolubl •■ in water. Sp. gr. 0.819. A limpid oily aromatic liquid, sp. gr. 0.823. A liquid, boils at lOCC. (305°F.) sp. gr. 0.899. Is in white crystals. It is soluble ill water, CiiNtor Oil contains Ricinolcio Acid. Spermacetti Is compoiiod of Pttliiiitato of Cctyl. A waxy substance. This wax is tlio Corotftt« of Coryl. A crystalline substance with a silky lustre. I Wax contains Myrlclri wJiloh \» tho Palmitate of Myricyl. Primary Aromatir Alcohols .—Benzyl Alcohol C,II,(I10) ; Xylyl Alcohol (\II,/II()) ; Cymyl Alcohol Ci„IIi3(tI0) ; Sycoceryl Alcohol CgllsjClIO). Secondary/ Aromatic Alcohols .■—'Phoml (or Carbolio Acid) C,lI,(HO) and Crcsol C,H,(IIO). OF THEIR PRINCIPAL DERIVATIVES. Butyleno Alcohol (!.II,(nO)j; Octcne Alcohol CJI„(HO),. In these Alcohol)* II, U rtipliiood by (IIO), *n^ ":^a> IMAGE EVALUATION TEST TARGET (MT-3) 1.0 I.I 1.25 ■f 1^ IIM ir 1^ mil 2.0 1.4 V ^ Va ^^^k^^ ^v% Hiotographic Sciences Corporation 23 WEST MAIN STREET WEBSTER, N.Y. 14580 (716)S72-4S03 %^ % f '6^ — 86- SUBSTANCKS. FoBUCLiS. Synonyms. Pbepabed Fhom. Process and Decompositions. Triatomic Alco- hols, (C!„H,„)'"(H0)3 Only 3 are described. Ethyl Alcohol and Chlorinated Lime. Propenyl Alcohol CJTj(HO),; Quintenyl Alcohol U,H8(HO)3 ; CHCl, Methenyl Chloride, Chloroform. 2C,H5(HO)+5CaClA=2CaC03+2CaCl, +CaH,0,+4H,0-f2CHCl, CHBr, Bromoform. Bromine, Potash, Al- cohol, CHI, C,H,(H0)3 Iodoform. Iodine, Potash, Alcohol. Suet and Potash. Propenyl Alcohol or Glycerin. C,H.(C„H,,A)a+3KH0 = aKUJi^A+CJI.CHO), CsH.CNOs), Nitro- glycerin. Glycerin, JJitric', Sul- phuric'. C,nj(HO),+3nNO3=3IJ,O+C3ll5(NO0. Tetratomio Al- cohol. (C,He)"(HO), Erythrite. Is the only one known. Exists in *hc proto-coccus vulgaris. Pentatomic Al- cohols. (C,H,)^(HO), Finite, ! Found in the sap of the Californian pine. (CeHO^(HO). Querjite. M ay be obtained from acorns. Eexatoroic Al- cohols. (CeH,)^'(HO). Mantiite. Exists in Manna. Also in some sea-weeds and Mushrooms. (C.H,)^'(HO), Dulcite. i Exists in Mdampjirnm neinoromm. — 87- 33+2CaCl, C,H,(iN03). iian pine. brooms. Propebties, &0. Tests and Reuabes. Methcnyl Alcohol CII(H0)3 ; the latter has not yet been isolated, but its ethers are important, being Chloroform, &c. In these Alcohols (HO), replace Hj. A colorless liquid, sp. gr. 1.48, of vapor 4.116, boils at 6rC. (141°F.), bums with a green flame ; is anocsthctic. To detect it in fluids. — Put the fluid in a test tube, heat and as CI and HCl pass off, test for them with Silver Nitrate, or with Potassium Iodide and Starch. A heavy volatile liquid. Sp. gr. 2.9. A yellow crystalline solid. A colorles'. vieoid liquid, sweet, sp. gr. 1.27, not fermentable, mixes with water. Suet is composed of the Stearate of Glycerin. Heated Glycerin gives off an irritating vapor called Acrolein C,H«0 A heavy oily explosive liquid, used for blasting. Extremely dangerous to handle as it is so explosive. A saccharine substance in large transparent crystals. Sweet, soluble in water and not fermentable. Is in hard sweet nodules. Not fermentable. Two Pontatomio Alcohols only are known ; this and the next one to be described. Is in hard gritty soluble crystals. Thin 4-sided prisms, sweet, soluble in water. Not fermentable except under unusual conditions. Is in sweet crystalline prisms. Most vegetable sugars are included in this class of Alcohols. I 1 ;•!- -88- Class III. Haloid Ethers. — These are compounds of hydro-carbon radicals with the Halogens CI, Br and I, such as (CH,)'C1, or Methyl Chloride ; (CjH4)"Brj, Ethyl Bromide; (CjHs)'"!,, or Propeiyl Iodide, which have been already described at page 80. Class IV. Oxygen Ethers — which are compounds of hydro-carbon radicals with ; examples, (CjH5)jO or Ethyl Oxide ; (C,H4)„0 Ethene Oxide, &c., they are also called Alcoholic Oxides and are described at page 82. Class V. Merca^tans — so called from their readiness to unite with Mercury (corpora mcrcurio apta) or Sulphur Alcohols, are compounds analagous to the Alcohols, but the of the HO is replaced by S as in Methyl Mercaptan (CH3)HS which however has been fully described at page 80, as well as Ethyl Mercaptan C^H^FB at page 82. Class VI. Se JENIUM AicoHOT.s are analagous to the Mercaptans but Se is substituted for the 9 in these compounds. Class VII. Sulphur and Selcnium Ethers are similar compounds to the Oxygen Lthers, but S and Se are substituted for the Oxygen in these preparations. Class VIII. Compound Ethers are produced by the substitution of an alcohol-radical for an atom of H of an acid, in precisely the same manner as an ordinary metallic salt is formed ; (CjHi)H,S04 Monethylic Sulphate; (CjH,)jS04 Diethylio Sulphate. These preparations are also commonly regar cd as Ethereal Salts. Numerous examples have been already given in the preceding tables. Certain vegetable principles called Glycosides arc regarded as Compound Ethers of the Alcohols, these oc ebuUiticn with a dilute acid yield glucose, hence the name ; they are : — 14. 15. 16. 17. 1. ^Esculin C,iH„Ois from Horse-chestnuts. 2. Amygdalin C,oHj,NO,„3HjO from Almonds. 3. Cathartic Acid C,8oH,„N8p.4S Amyl i-82 Analysis, definition of. . 4 Antimony and Salts 64 Anhydride Sulphuric .... 20 Anhydride Sulphurous . . 20 Aqua Fortis 10 " Uegia 14 Argentumand salts 42 Aromatic Alcohols 36 At senio and Salts 66 Arslnes.... 93 Atmonphero 8 Atomic theory 3 " woighU 1,2,3 Attraction, Chemical .... 30 Aurum, (Qold) 54 Azote 8 Barium and salts 44 Bell metal 62 Beryllium 60 Biamuth and salts 66 Bisulphide of Carbon.... 22 Black fiux 67 Borax 38 Boron ft its compounds., 28 Brass 52 Britannia metal 63 British gum 90 Bromine and compounds. 18 Bromoform 86 Bronze 52 Butter of Antimony 64 Butyl 74 Cicsinm 42 Cadmium 46 Calamine 46 Calcium and salts 4(> Calomel 48 Cnrbamic Acid 43 Carbamide 43 Carbinol 80 Carbon & compounds. 10-12 << disuiphido 22 Cassius, Purple of 55 Cerium 64 Coryi Alcohol 84 Cetyl Alcohol 84 Chemical Compounds, deflnition of 5 Chemical Aflinity 30 " Attraction... 30 Chemistry, definition of. 1 " classification of bodies in, 1 '■ combining laws of 4 Chlorine and comp's . .14-16 Chloroform 8S Choke damp 12 Chromium and comp's.. 6 Cinnabar 60 -98- H I [< -; ClaBBific'n of non-motaln . 1 3 " mctiilH.s.T " organic bodiuH.TG rohnlt 02 Colloidf. :!o Cofflicicnts 1 Coliimbimn cNioLiiini).. .CO Combinutiou 1))' volnnii!. . B " liy wi'iKlit..l-,'l Compound Aiiimdiiijis. . . .ni " KlluTK HH " Kiidicnlrt 73 Copper and its hiiIIh. .46, .18 Copperas fiO CorroBive Siiblimnte 48 CrystJilIoidH 30 Cyanogen <(: compounds. .04 Cyanic Acid i).t Cyanurie Acid ■ !I4 Dehydrating agents 72 Deoxydiziug " 72 DiftlyHis 30 Diamond 10 Diagram, deflnition of. . . . 6 Diastase 00 Diatomic Alcoliolg 84 Didymium 62 Density 5 Dextrine 00 Distillation ,^3 " dry or destructive 63 " fractional r,3 Dolomite 44 Dutch Liquid 13 Dyads, non-metallic 13 " metiillie 33 Elementary l)odic8,tahleof 2 Kiiuations 1, 5 Krl]iura 52 Kthane 75, 77 Kthen 12, 78 Kther 74,82 Kfhereal Salts 88 Ktlu-rs Haloid 88 " Oxygen 88 " Selenium 88 " Sulphur 88 Kthyl Alcohol k compd'3.82 Ktli\lene 12 Kthylenic dichloride.... 13 Kuehlorino 17 Ferricyanogcn salts 04 Kerrocyanogen salts .... 04 Ferrum and salts 58 Fire damp 12 Fixed air 12 Fluorine 18 Flux, black G7 Formuhe 1,4 " Empirical ?2 " Kational 72 Fonsel or Fusel Oil 82 French weights and measures 24 Oalena 50 Gas, definition of a 5 Herman Silver ., .53 Olui inum (Beryllium)... 50 (lliuo. MaiiKuiieNit and tnUs,...60 Kfaiirilln 86 MannltiiNii 81) MarHJi UHH 12 Marnh'ri lent 07 MiixhIi'iiI ,. ., .50 MllllOKM ,, 80 Mereaptai 82, H8 " Melhyl 80 Men iiry niid naltN.. .48, 50 Mi'ri iii'je ('vaiildo 91 MelaU, deiliilllon of .. ..32 " iliiKuJlliatkin or-SS MetailieiUlU 06 Melliane 12, 7B, '.1 Melh.-iii. 75, 78 Melhyl 7t " Aleohid k coiMps.PO Melll.l-vl 70 Metric i tiy«leiii, Kr'.!ticli,24 Mleriironiiilinalt 40 Mole. I|I"H 3 MidyhdellUlM 08 MouimIn, Moii-tnetallic, .13 " nielflllle 33 Monutoml" Aleoli'tllllic.,.l3 II 33 olioU. .80-82 14 il 84 MnIlN 38 02 30 Nitre Cubic 38 " Sweet spirits of.... 83 Nitric Acid 10 Nitriles ,...92 Nitrous Acid 10 Nitro-liydrochloric Acid. . 14 Nitroglycerin 80 Nitrogen and compounds. 8 Nomenclature 4 Nouane , 77 Nonene 78 Non-metallic elements. . .13 Nonyl Alcohol 84 Nordliauscn Sulph'c Acid. 20 Notation, Chemical 1-2 Octane 77 Octeno 78 Jctyl Alcohol 84