Cobalt(II) cyanide
| Names | |
|---|---|
| IUPAC name
Cobalt(II) cyanide | |
| Other names
cobaltous cyanide | |
| Identifiers | |
542-84-7  20427-11-6 (dihydrate)  26292-31-9 (trihydrate) | |
| 3D model (Jmol) | Interactive image |
| ChemSpider | 61631 |
| ECHA InfoCard | 100.008.028 |
| PubChem | 68336 |
| |
| |
| Properties | |
| Co(CN)2 | |
| Molar mass | 110.968 g/mol (anhydrous) 147.00 g/mol (dihydrate) 165.02 g/mol (trihydrate) |
| Appearance | deep-blue powder hygroscopic (anhydrous) reddish-brown powder (dihydrate) |
| Density | 1.872 g/cm3 (anhydrous) |
| Melting point | 280 °C (536 °F; 553 K) (anhydrous) |
| insoluble[1] | |
| Solubility | dihydrate degraded with dissolution by NaCN, KCN, NH4OH, HCl |
| Related compounds | |
| Other anions |
Cadmium chloride, Cadmium iodide |
| Other cations |
Zinc cyanide, Calcium cyanide, Magnesium cyanide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| verify (what is ?) | |
| Infobox references | |
Cobalt(II) cyanide is the inorganic compound with the formula Co(CN)2. It is coordination polymer that has attracted intermittent attention over many years in the area of inorganic synthesis and homogeneous catalysis.
Uses
Cobalt(II) cyanide has been used as a precursor to cobalt carbonyl.[2]
Preparation
The trihydrate salt is obtained as a reddish-brown precipitate by adding potassium cyanide to a cobalt salt solution.:[3]
- CoCl2(H2O)6 + 2 KCN → Co(CN)2 + 2 KCl + 6 H2O
Hydrated Co(CN)2 dissolves in the presence of excess potassium cyanide, forming a red solution of K4Co(CN)6. This material further oxidizes to yellow K3Co(CN)6.
References
- ↑ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- ↑ Heinz W. Sternberg, Irving Wender, Milton Orchin Cobalt Tetracarbonyl Hydride: (Cobalt Hydrocarbonyl) Inorganic Syntheses, 1957, vol. V, p. 192. doi:10.1002/9780470132364.ch55
- ↑ John H. Bigelow, "Potassium Hexacyanocobaltate(III)" Inorganic Syntheses, 1946, Volume I1, p. 225.
| Salts and covalent derivatives of the cyanide ion | |||||||||||||||||||
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| HCN | He | ||||||||||||||||||
| LiCN | Be(CN)2 | B | C | NH4CN | OCN−, -NCO |
FCN | Ne | ||||||||||||
| NaCN | Mg(CN)2 | Al(CN)3 | SiCN | P(CN)3 | SCN−, -NCS, (SCN)2, S(CN)2 |
ClCN | Ar | ||||||||||||
| KCN | Ca(CN)2 | Sc(CN)3 | Ti(CN)4 | VO(CN)3 | Cr(CN)3 | Mn(CN)2 | Fe(CN)3, Fe(CN)64+, Fe(CN)63+ |
Co(CN)2, Co(CN)3 |
Ni(CN)2 Ni(CN)42− |
CuCN | Zn(CN)2 | Ga(CN)3 | Ge | As(CN)3 | SeCN− (SeCN)2 Se(CN)2 |
BrCN | Kr | ||
| RbCN | Sr(CN)2 | Y(CN)3 | Zr(CN)4 | Nb | Mo | Tc | Ru | Rh | Pd(CN)2 | AgCN | Cd(CN)2 | In(CN)3 | Sn | Sb | Te(CN)2, Te(CN)4 |
ICN | XeCN | ||
| CsCN | Ba(CN)2 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg2(CN)2, Hg(CN)2 |
TlCN | Pb(CN)2 | Bi(CN)3 | Po | At | Rn | |||
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| ↓ | |||||||||||||||||||
| La | Ce(CN)3, Ce(CN)4 |
Pr | Nd | Pm | Sm | Eu | Gd(CN)3 | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||||
| Ac | Th | Pa | UO2(CN)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
This article is issued from Wikipedia - version of the 11/24/2016. The text is available under the Creative Commons Attribution/Share Alike but additional terms may apply for the media files.