Cadmium cyanide
| Names | |
|---|---|
| IUPAC name
Cadmium(II) cyanide | |
| Identifiers | |
542-83-6  | |
| ChemSpider | 61630 |
| |
| Jmol-3D images | Image |
| PubChem | 68335 |
| |
| Properties | |
| Cd(CN)2 | |
| Molar mass | 164.45 g/mol |
| Appearance | white cubic crystals |
| Density | 2.226 g/cm3 |
| 1.71 g/100 mL (15 °C) 2.2 g/100 mL (20 °C) | |
| Solubility | slightly soluble in alcohol dissolves in alkali, metal cyanides and hydroxides |
| Related compounds | |
| Other anions |
Cadmium chloride, Cadmium iodide |
| Other cations |
Zinc cyanide, Calcium cyanide, Magnesium cyanide |
| Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
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| Infobox references | |
Cadmium cyanide is an inorganic compound with the formula Cd(CN)2. This white crystalline compound is used in electroplating.[1] It is very toxic, along with other cadmium and cyanide compounds.
Usage
It is used as an electrolyte for electrodeposition of thin metallic cadmium coatings on metal to protect against corrosion.
Preparation and structure
Cadmium cyanide is prepared by treating cadmium hydroxide with hydrogen cyanide:[2]
- Cd(OH)2 + 2 HCN → Cd(CN)2 + 2 H2O
It adopts a diamondoid structure, like Zn(CN)2.
Reactions
Like zinc cyanide, cadmium cyanide is fairly soluble in water, which is unusual for metal cyanides. The solubility increases with the additional cyanide, this reaction proceeding via "[Cd(CN)3]−" and [Cd(CN)4]2−. With acids, its solutions evolve hydrogen cyanide.
References
- ↑ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- ↑ 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.
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