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Cyanogen is the chemical compound with the formula (CN)2. It is a colorless, toxic gas with a pungent odor. The molecule is a pseudohalogen. Cyanogen molecules consist of two CN groups — analogous to diatomic halogen molecules, such as Cl2, but far less oxidizing. The two cyano groups are bonded together at their carbon atoms: N≡C−C≡N, although other isomers have been detected.[1] Certain derivatives of cyanogen are also called “cyanogen” even though they contain only one CN group. For example cyanogen bromide has the formula NCBr.[2] Cyanogen is the anhydride of oxamide:
[edit] PreparationCyanogen is typically generated from cyanide compounds. One laboratory method entails thermal decomposition of mercuric cyanide:
Alternatively, one can combine solutions of copper(II) salts (such as copper(II) sulfate) with cyanides, an unstable copper(II) cyanide is formed which rapidly decomposes into copper(I) cyanide and cyanogen.[3]
Industrially, it is created by the oxidation of hydrogen cyanide, usually using chlorine over an activated silicon dioxide catalyst or nitrogen dioxide over a copper salt. It is also formed when nitrogen and acetylene are reacted by an electrical spark or discharge.[4] [edit] ParacyanogenParacyanogen is produced by polymerization of cyanogen through pyrolysis of heavy metal cyanides. [5] [edit] HistoryCyanogen has a long history and was most likely generated first by Carl Scheele around 1782 while he was studying hydrogen cyanide.[6][7] The first confirmed synthesis was reported 1802, when it was used to make what is now known as cyanogen chloride. It attained importance with the growth of the fertilizer industry in the late nineteenth century and is still an important intermediate in the production of many fertilizers. It is also used as a stabilizer in the production of nitrocellulose. [edit] SafetyLike other inorganic cyanides, cyanogen is very toxic, as it undergoes reduction to cyanide, which binds more strongly than oxygen to the cytochrome c oxidase complex, thus interrupting the mitochondrial electron transfer chain. Cyanogen gas is an irritant to the eyes and respiratory system. Inhalation can lead to headache, dizziness, rapid pulse, nausea, vomiting, loss of consciousness, convulsions, and death, depending on exposure.[8] Cyanogen produces the second hottest known natural flame (after carbon subnitride) with a temperature of over 4525°C (8180°F) when it burns in oxygen.[9] [edit] See also[edit] References
[edit] External links
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