Cadmium hydroxide is an inorganic compound with the formula Cd(OH)2. It is a white crystalline ionic compound that is a key component of nickel–cadmium battery.[5]

Structure

Cadmium hydroxide adopts the same structure as Mg(OH)2, consisting of slabs of metal centers, each bonded by six hydroxide ligands.[6] The Cd(OH)2 structure is a recurring motif in inorganic chemistry. For example it is adopted by vanadium ditelluride.[7]

Preparation, and reactions

Cadmium hydroxide is produced by treating an aqueous solution containing Cd2+ (say cadmium nitrate) with sodium hydroxide:[8][5]

Cd(NO3)2 + 2 NaOH → Cd(OH)2 + 2 NaNO3

Cd(OH)2 and cadmium oxide exhibit similar reactions. Cadmium hydroxide is more basic than zinc hydroxide. It forms the anionic complex [Cd(OH)4]2− when treated with concentrated base. It forms complexes with cyanide, thiocyanate, and ammonia.

Cadmium hydroxide loses water on heating, producing cadmium oxide. Decomposition commences at 130 °C and is complete at 300 °C. Reactions with mineral acids (HX) gives the corresponding cadmium salts (CdX2). With hydrochloric acid, sulfuric acid, and nitric acid, the products are cadmium chloride, cadmium sulfate, and cadmium nitrate, respectively.[8][5]

Uses

It is generated in storage battery anodes, in nickel-cadmium and silver-cadmium storage batteries in its discharge:

2 NiO(OH) + 2 H2O + Cd → Cd(OH)2 + 2 Ni(OH)2

References

  1. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
  2. ^ Perrin, D. D., ed. (1982) [1969]. Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution. IUPAC Chemical Data (2nd ed.). Oxford: Pergamon (published 1984). Entry 22. ISBN 0-08-029214-3. LCCN 82-16524.
  3. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
  4. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH).
  5. ^ a b c Karl-Heinz Schulte-Schrepping, Magnus Piscator "Cadmium and Cadmium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2007 Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_499.
  6. ^ Hemmingsen, L.; Bauer, R.; Bjerrum, M. J.; Schwarz, K.; Blaha, P.; Andersen, P., "Structure, Chemical Bonding, and Nuclear Quadrupole Interactions of β-Cd(OH)2:  Experiment and First Principles Calculations", Inorganic Chemistry 1999, volume 38, 2860-2867. doi:10.1021/ic990018e
  7. ^ Bronsema, K.D.; Bus, G.W.; Wiegers, G.A. (1984). "The Crystal Structure of Vanadium Ditelluride, V1+xTe2". Journal of Solid State Chemistry. 53 (3): 415–421. doi:10.1016/0022-4596(84)90120-8.
  8. ^ a b F. Wagenknecht; R. Juza (1963). "Cadmium hydroxide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1096.
Allikas: http://en.wikipedia.org/wiki/Cadmium_hydroxide
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