Cobalt(II) cyanide
| Names | |
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| IUPAC name
Cobalt(II) cyanide
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| Other names
cobaltous cyanide
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.008.028 |
PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| 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 |
| +3825·10−6 cm3/mol | |
| Related compounds | |
Other anions
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Cadmium chloride, Cadmium iodide |
Other cations
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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).
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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
[edit]Cobalt(II) cyanide has been used as a precursor to dicobalt octacarbonyl.[2]
Preparation and structure
[edit]The trihydrate salt is obtained as a reddish-brown precipitate by adding two equivalents of potassium cyanide to a cobalt salt solution:[3]
- CoCl2(H2O)6 + 2 KCN → Co(CN)2 + 2 KCl + 6 H2O
With excess cyanide, the red brown dicyanide dissolves to give pentacyanocobaltate.[4]
Solid cobalt(II) cyanide is a coordination polymer consisting of cobalt ions linked by cyanide units in a cubic arrangement, each such cobalt atom having octahedral geometry, and an additional cobalt atom in half of the cubic cavities.[5] That is, the structure is actually Co[Co(CN)3]2 in a zeolite-like structure. It forms hydrates and other inclusion complexes by having substances diffuse into the cavities that do not contain the cobalt atoms.[5]
References
[edit]- ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, Florida: CRC Press. ISBN 0-8493-0487-3.
- ^ Sternberg, Heinz W.; Wender, Irving; Orchin, Milton; Lynch Jr., M. A.; Sesny, W. J. (1957). "Cobalt Tetracarbonyl Hydride". Inorganic Syntheses. Inorganic Syntheses. Vol. 5. pp. 192–195. doi:10.1002/9780470132364.ch55. ISBN 9780470132364.
- ^ Bigelow, John H.; Bailar Jr., John C. (1946). "Potassium Hexacyanocobaltate(III)". Inorganic Syntheses. Inorganic Syntheses. Vol. 2. pp. 225–227. doi:10.1002/9780470132333.ch72. ISBN 9780470132333.
- ^ Kwiatek, Jack (1968). "Reactions Catalyzed by Pentacyanocobaltate(II)". Catalysis Reviews. 1: 37–72. doi:10.1080/01614946808064700.
- ^ a b Weiss, Armin; Rothenstein, W. (1963). "Cobalt(II) Cyanide, its Three-Demensional Frame-work Structure and Zeolitic Compounds". Angewandte Chemie International Edition. 2 (7): 396. doi:10.1002/anie.196303962.
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