Potassium_gold_cyanide

Potassium dicyanoaurate

Potassium dicyanoaurate

Chemical compound

Potassium dicyanoaurate (or potassium gold cyanide) is an inorganic compound with formula K[Au(CN)2]. It is a colorless to white solid that is soluble in water and slightly soluble in alcohol. The salt itself is often not isolated, but solutions of the dicyanoaurate ion ([Au(CN)2]−) are generated on a large scale in the extraction of gold from its ores.[3]

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Production

In mining of gold from dilute sources, gold is selectively extracted by dissolution in aqueous solutions of cyanide, provided by dissolving sodium cyanide, potassium cyanide and/or calcium cyanide. The reaction for the dissolution of gold, the "Elsner Equation", is:

4 Au + 8 KCN + O2 + 2 H2O → 4 K[Au(CN)2] + 4 KOH

In this process, oxygen is the oxidant.[4]

It can also be produced by reaction of gold(I) salts with excess potassium cyanide.

AuCl + 2 KCN → K[Au(CN)2] + KCl

Structure

dicyanoaurate is a rod-shaped anion.

Potassium dicyanoaurate is a salt. The dicyanoaurate anion is linear according to X-ray crystallography.[3] On the basis of infrared spectroscopy, the dicyanoaurate anion adopts a very similar structure in sodium dicyanoaurate (NaAu(CN)2).[5]

Uses

Dicyanoaurate is the soluble species that is the focus of gold cyanidation, the hydrometallurgical process for winning gold from dilute ores. In fact, sodium cyanide, not the potassium salt, is more widely used in commercial processes.[6]

Aside from its major use as an intermediate in the extraction of gold, potassium dicyanoaurate is often used in gold plating applications.

The compound containing gold(III) cyanide is also known: potassium tetracyanoaurate(III), K[Au(CN)4]. Its use is less common.

The potassium ion can be replaced with quaternary ammonium cations as in tetrabutylammonium dicyanoaurate.[7]

Safety

The ingestion of gram quantities of potassium dicyanoaurate has led to death.[8]

References

  1. [1]
    Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.82. ISBN 978-1439855119.
  2. ↑
    Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
  3. [3]
    Rosenzweig, A.; Cromer, D. T. (1959). "The Crystal Structure of KAu(CN)2". Acta Crystallographica. 12 (10): 709–712. doi:10.1107/S0365110X59002109.
  4. [4]
    Treatment of Ores Containing Reactive Iron Sulphides. Multi Mix Systems
  5. [5]
    Chadwick, B.M.; Frankiss, S.G. (1976). "Vibrational Spectra and Structures of Some Dicyanoaurate(I) Complexes". Journal of Molecular Structure. 31 (1): 1–9. Bibcode:1976JMoSt..31....1C. doi:10.1016/0022-2860(76)80113-5.
  6. [6]
    Rubo, Andreas; Kellens, Raf; Reddy, Jay; Steier, Norbert; Hasenpusch, Wolfgang (2006). "Alkali Metal Cyanides". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.i01_i01. ISBN 978-3527306732.
  7. [7]
    Stender, Matthias; Olmstead, Marilyn M.; Balch, Alan L.; Rios, Daniel; Attar, Saeed (2003). "Cation and Hydrogen Bonding Effects on the Self-Association and Luminescence of the Dicyanoaurate Ion, Au(CN)2−". Dalton Transactions (22): 4282. doi:10.1039/b310085e.
  8. [8]
    Wright, I. H.; Vesey, C. J. (September 1986). "Acute poisoning with gold cyanide". Anaesthesia. 41 (9): 936–939. doi:10.1111/j.1365-2044.1986.tb12920.x. PMID 3022615.
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