Lithium cyanide
Identifiers | |
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3D model (JSmol) |
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ChemSpider | |
ECHA InfoCard | 100.017.554 |
PubChem CID |
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UN number | 1935 |
| |
Properties | |
LiCN | |
Molar mass | 32.959 g/mol |
Appearance | White Powder |
Density | 1.073 g/cm3 (18 °C) |
Melting point | 160 °C (320 °F; 433 K) Dark colored |
Boiling point | N/A |
Soluble | |
Henry's law constant (kH) |
N/A |
Structure | |
- | |
Fourfold | |
Hazards | |
Safety data sheet | 742899 |
EU classification (DSD) (outdated) |
T+, Very Toxic N, Dangerous for the environment |
R-phrases (outdated) | 26/27/28-32-50/53 |
S-phrases (outdated) | 7-28-29-45-60-61 |
NFPA 704 | |
Flash point | 57 °C (135 °F; 330 K) |
N/A | |
Related compounds | |
Related compounds |
Sodium cyanide, Potassium cyanide, Hydrogen cyanide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
Infobox references | |
Lithium cyanide is an inorganic compound with the chemical formula LiCN. It is a white, hygroscopic, water-soluble powder that finds only niche uses.
Preparation
LiCN arises from the interaction of lithium hydroxide andhydrogen cyanide. A laboratory-scale preparation uses acetone cyanohydrin as a surrogate for HCN: [4]
- (CH3)2C(OH)CN + LiH → (CH3)2CO + LiCN + H2
Reactions
The compound decomposes to cyanamide and carbon when heated to a temperature close to but below 600°C. Acids react to give hydrogen cyanide.[5]
Lithium cyanide can be used as a reagent for cyanation.[6]
- RX + LiCN → RCN
References
- ↑ J. A. Lely,, J. M. Bijvoet (1942), "The Crystal Structure of Lithium Cyanide", Recueil des Travaux Chimiques des Pays-Bas, 61, London: WILEY-VCH Verlag
- ↑ Haynes, W.M (2013), "Bernard Lewis", in Bruno, Thomas., Handbook of Chemistry and Physics (93 ed.), Boca Raton, Florida: Fitzroy Dearborn
- ↑ Material Safety Data Sheet: Lithium Cyanide, 0.5M Solution in N,N-Dimethylformamide, Fisher Scientific, 16 June 1999
- ↑ Tom Livinghouse (1981). "Trimethylsilyl Cyanide: Cyanosilylation of p-Benzoquinone". Org. Synth. 60: 126. doi:10.15227/orgsyn.060.0126.
- ↑ L. Pesce (2010). "Cyanides". Kirk‐Othmer Encyclopedia of Chemical Technology. Wiley-VCH. doi:10.1002/0471238961.0325011416051903.a01.pub2.
- ↑ "Non-aqueous cyanation of halides using lithium cyanide". Elsevier. Retrieved 2012-10-17.
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