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Originally appearing in Volume V19, Page 660 of the 1911 Encyclopedia Britannica.
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CALEDONIA 1900. 1901. 1902. 1903. 1904. 1905. 1906. 1907. 1908. Metric tons . 100,319 133,676 129,653 77,360 98,665 125,289 130,688 101,708 120,028 (See See also:Rothwell's See also:Mineral See also:Industry (1908), PP. 666, 67o).

The See also:

metal may also be obtained on the small See also:scale by the reduction of the See also:oxide by See also:hydrogen or by See also:carbon, by ignition of the oxalate or of See also:nickel ammonium oxalate (J. J. See also:Berzelius), by reduction of the chloride in a current of hydrogen (E. Peligot), by See also:electrolysis of nickel ammonium sulphate (Winkler, Zeit. anorg. Chem. 1894, 8, p. I), and by reduction of the chloride with See also:calcium See also:carbide. It is a greyish See also:white metal, and is very malleable and ductile. Its specific gravity varies according to the method employed for its preparation, the extreme values being 8.279 and 9.25. It melts between 1400-1600° C. Its specific See also:heat increases with rise of temperature, the mean value from 15° to See also:loo C. being o• 1084 (A. Naccari, Gaze., 1888, 18, p.

13). It is magnetic, but loses its See also:

magnetism when heated, the loss being See also:complete at about 340-3500 C. On the See also:physical constants see H. Copaux, Comptes rend us, 1905, 140, p. 651. Nickel occludes hydrogen readily, is attacked by the halogen elements, and oxidizes easily when heated in See also:air. In the massive See also:state it is unacted upon by dry air, but if moistened with acidified See also:water, oxidation takes See also:place slowly. When obtained by reduction processes at as See also:low a temperature as possible the finely divided metal so formed is pyrophoric, and according to P. See also:Schutzenberger (Comptes rendus, 1891, 113, p. 177) dry hydrochloric See also:acid See also:gas converts this See also:form into nickel chloride and a volatile See also:compound of See also:composition NiHC1. It decomposes water at a red heat. According to E.

St Edme (Comptes rend us, 1886, ro6, p. 1079) See also:

sheet nickel is passive to nitric acid, and the metal remains passive even when heated to redness in a current of hydrogen. On the reduction of organic compounds by hydrogen in the presence of metallic nickel see P. See also:Sabatier and J. B. Senderens, See also:Ann. Chico. Phys., 1905 [8], 4, pp. 319, 433. It rapidly oxidizes when fused with See also:caustic soda, but is scarcely acted upon by caustic potash (W. Dittmar, Jour. See also:Soc.

Chem. Ind., 1884, 3, p. 103). Hydrochloric and sulphuric acids are almost without See also:

action on the metal, but it dissolves readily in dilute nitric acid. Nickel salts are antiseptic; they See also:arrest See also:fermentation and stop the growth of See also:plants. Nickel carbonyl, however, is extremely poisonous. On the toxic properties of (See also:Liebig). M. Ilinski and G. v. Knorre (Ber., 1885, 18, p. 169) See also:separate the metals by adding nitroso-,8-naphthol in the presence of 50 % acetic acid, a precipitate of cobalti nitroso-$-naphthol, [CioH6O(NO)]aCo, insoluble in hydrochloric acid, being formed, whilst the corresponding nickel compound dissolves in hydrochloric acid. E.

Pinerua separates the metals by taking See also:

advantage of the fact that See also:cobalt chloride is soluble in See also:ether which has been saturated with hydrochloric acid gas at low temperature. For an examination of the above and other methods see E. Hintz, Zeit. anal. Chem., 1891, 30, p. 227. Nickel fluoride, NiF2, obtained by the action of hydrofluoric acid on nickel chloride, crystallizes in yellowish See also:green prisms which volatilise above loon° C. It is difficultly soluble in water, and combines with the alkaline fluorides to form See also:double salts. Nickel chloride, NiC12, is obtained in the anhydrous See also:condition by See also:heating the hydrated See also:salt to 14o° C., or by gently heating the finely divided metal in a current of See also:chlorine. It readily sublimes when heated in a current of chlorine, forming See also:golden yellow scales. It is easily reduced when heated in hydrogen. It forms crystalline compounds with See also:ammonia and the organic bases. It is soluble in See also:alcohol and in water.

Three hydrated forms are known, viz. a mono-, di-, and hexa-See also:

hydrate; the latter being the form usually obtained by the See also:solution of the oxide or carbonate in hydrochloric acid. Nickel chloride ammonia, NiC12.6NHa, is obtained as a white See also:powder when anhydrous nickel chloride is exposed to the action of ammonia gas (H. See also:Rose, Pogg. Ann., 1830, 96, p. 155), or in the form of See also:blue octahedra by evaporating a solution of nickel chloride in aqueous ammonia. When heated to loo° C. it loses four molecules of ammonia. Two hydrated forms have been described, one containing three molecules of water and the other See also:half a See also:molecule. Numerous double chlorides of nickel and other metals are known. The bromide and iodide of nickel resemble the chloride and are prepared in a similar See also:fashion. Several sulphides of the See also:element have been obtained. A sub-sulphide, Ni2S(?), results when the sulphate is heated with See also:sulphur or when the precipitated monosulphide is heated in a current of hydrogen. It forms a See also:light yellow amorphous See also:mass which is almost insoluble in acids.

The monosulphide, NiS, is obtained by heating nickel with sulphur, by heating the monoxide with sulphuretted hydrogen to a red heat, and by heating See also:

potassium sulphide with nickel chloride to 16o-18o° C. When prepared by dry methods it is an exceedingly See also:stable, yellowish, somewhat crystalline mass. When prepared by the precipitation of nickel salts with alkaline sulphide in neutral solution it is a greyish See also:black amorphous compound which readily oxidizes in moist air, forming a basic nickel sulphate. The freshly precipitated sulphide is soluble in sulphurous acid and some-what soluble in hydrochloric acid and yellow ammonium sulphide (see H. Baubigny, Comptes rendus, 1882, 94, pp. 961, 1183; 95, p. 34). Nickel sulphate, NiSO4, is obtained anhydrous as a yellow powder when any of its hydrates are heated. When heated with carbon it is reduced to the metal. It forms hydrates containing one, two, five, six and seven molecules of water. The heptahydrate is obtained by dissolving the metal or its oxide, hydroxide or carbonate in dilute sulphuric acid (preferably in the presence of a small quantity of nitric acid), and allowing the solution to crystallize between 15° and 2o° C. It crystallizes in See also:emerald-green rhombic prisms and is moderately soluble in water.

It effloresces gradually on exposure to air and passes into the hexahydrate. It loses four molecules of water of See also:

crystallization when heated to too° C. and becomes anhydrous at about 300° C. The hexahydrate is dimorphous, a tetragonal form being obtained by crystallization of a solution of the heptahydrate between 20° and 3o° C., and a See also:monoclinic form between 500 and 7o° C. Nickel sulphate combines with many metallic sulphates to form double salts, and also forms addition compounds with ammonia See also:aniline and See also:hydroxylamine. The nitrate, Ni(NOa)2.6H20, is obtained by dissolving the metal in dilute nitric acid and concentrating the solution between 40° and 5o° C. It crystallizes in green prisms which deliquesce rapidly on exposure to moist air. Nickel carbonyl, Ni(CO)4, is obtained as a colourless See also:mobile liquid by passing carbon monoxide over reduced nickel at a temperature of about 6o° C. (L. See also:Mond, See also:Lanier and Quincke, Jour. Chem. Soc., 1890, 57, p. 749).

It boils at 43 C. (751 mm.), and sets at -25° C. to a mass of crystalline needles. It is readily soluble in See also:

hydrocarbon solvents, in See also:chloroform and in alcohol. Its See also:critical pressure is 30 atmospheres and its critical temperature is in the neighbourhood of 195° C. (J. See also:Dewar, Proc. See also:Roy. Soc., 1903, 71, p. 427). It decomposes with explosive violence when heated rapidly. Dewar and See also:Jones (Journ. Chem.

Soc., 1904, p. 203) have made an exhaustive study of its reactions, and find that it is decomposed by the See also:

halogens (dissolved in carbon tetrachloride) with liberation of carbon monoxide and formation of a nickel halide. See also:Cyanogen iodide and See also:iodine mono- and tri-chloride effect similar decompositions with simultaneous liberation of iodine; sulphuric acid reacts slowly, forming nickel sulphate and liberating hydrogen and carbon monoxide. Hydrochloric and hydrobromic acids are without action; hvdriodic acid only reacts slowly. With aromatic See also:hydrocarbons in the presence of anhydrous See also:aluminium chloride, in the See also:cold, there is a large See also:evolution of hydrochloric acid gas, and an aldehyde is formed ; at loo C., on the other See also:hand, See also:anthracene derivatives are produced. Thus by using See also:benzene, See also:benzaldehyde and anthracene are obtained. Dewar and Jones suggest that in the latter reaction it is themetallic nickel which is probably the reducing See also:agent effecting the See also:change, since it is only dissolved in any quantity when the anthracene hydrocarbon is produced. When mesitylene is used, the reaction does not proceed beyond the aldehyde See also:stage since hydrocarbon formation is prevented by the presence of a methyl See also:group in the ortho-position to the -CHO group. Acids and alkalis are in See also:general without action on nickel carbonyl. The vapour of nickel carbonyl See also:burns with a luminous See also:flame, a cold See also:surface depressed in the flame being covered with a black See also:deposit of nickel. It is an extremely powerful See also:poison. Mond and his assistants have discovered several other carbonyls.

For example cobalt gives Co(CO)4, as See also:

orange crystals which melt at 51°, decomposing at a higher temperature, giving Co(CO)3 and CO at 6o°; Co(CO)3 forms See also:jet black crystals. For See also:iron carbonyls see IRON; also L. Mond, H. Hirtz and M. D. Cowap, Jour. Chem. Soc., 1910, 97, p. 798. Nickel carbonate, NiCOa, is obtained in the anhydrous state by heating nickel chloride with calcium carbonate in a sealed See also:tube to 15o° C. (H. de See also:Senarmont, Ann. Chim.

Phys., 185o [31, 30, 138). It crystallizes in microscopic rhombohedra insoluble in cold acids. By precipitation of nickel salts with solutions of the alkaline See also:

carbonates, basic carbonates of variable composition are obtained. Numerous determinations of the atomic See also:weight of nickel have been published, the values obtained varying from 58.o to approximately 59.5• The more See also:recent See also:work of T. W. See also:Richards and See also:Cushman (Chem. See also:News, 1899, 79, 163, 1i4, 185) gives for the atomic weight of the metal the values 58.69 and 58.70.

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