Lithium cyanide explained

Lithium cyanide is an inorganic compound with the chemical formula LiCN. It is a toxic, white coloured, hygroscopic, water-soluble salt that finds only niche uses.

Preparation

LiCN is produced from the reaction of lithium hydroxide and hydrogen cyanide. A laboratory-scale preparation uses acetone cyanohydrin as a surrogate for HCN:[1]

(CH3)2C(OH)CN + LiH → (CH3)2CO + LiCN + H2

Uses

The compound decomposes to cyanamide and carbon when heated to a temperature close to but below 600 °C. Acids react to give hydrogen cyanide.[2]

Lithium cyanide can be used as a reagent for organic compound cyanation.[3]

RX + LiCN → RCN + LiX

Notes and References

  1. Trimethylsilyl Cyanide: Cyanosilylation of p-Benzoquinone. Tom. Livinghouse. Org. Synth.. 1981. 60. 126. 10.15227/orgsyn.060.0126.
  2. Encyclopedia: 10.1002/0471238961.0325011416051903.a01.pub2. Cyanides . Wiley-VCH. Kirk‐Othmer Encyclopedia of Chemical Technology. 2010. L. Pesce. Kirk-Othmer Encyclopedia of Chemical Technology . 978-0471238966 .
  3. Non-aqueous cyanation of halides using lithium cyanide . Tetrahedron Letters . 28 . 36 . 4189–4190 . Elsevier. 10.1016/S0040-4039(00)95575-8 . 1987 . Harusawa . Shinya . Yoneda . Ryuji . Omori . Yukie . Kurihara . Takushi .

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