Cyanogen chloride
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| Names | |
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| IUPAC name
Cyanic chloride
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| Other names
Chloroformonitrile, Chlorine cyanide, Carbononitridic chloride, CK
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.007.321 |
| EC Number |
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PubChem CID
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| RTECS number |
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| UN number | 1589 |
CompTox Dashboard (EPA)
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| Properties | |
| CNCl | |
| Molar mass | 61.46 g/mol |
| Appearance | colorless gas |
| Density | 1.186 g/cm3 (liquid) |
| Melting point | −6 °C |
| Boiling point | 13 °C[1] |
| Soluble | |
| Vapor pressure | 1987 kPa (21.1 °C) |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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Highly toxic[2] |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Cyanogen chloride is an inorganic compound with the formula NCCl. This linear, triatomic pseudohalogen is an easily condensed colorless gas. More commonly encountered in the laboratory is the related compound cyanogen bromide, a room-temperature solid that is widely used in biochemical analysis and preparation.
Synthesis, basic properties, structure
Although the formula is written CNCl, cyanogen chloride is a molecule with the connectivity ClCN. Carbon and chlorine are linked by a single bond, and carbon and nitrogen by a triple bond. It is a linear molecule, as are the related cyanogen halides (NCF, NCBr, NCI). Cyanogen chloride is produced by the oxidation of sodium cyanide with chlorine. This reaction proceeds via the intermediate cyanogen ((CN)2).[3]
- NaCN + Cl2 → ClCN + NaCl
The compound trimerizes in the presence of acid to the heterocycle called cyanuric chloride.
Cyanogen chloride is slowly hydrolyzed by water to release hydrogen cyanide
- ClCN + H2O → HCN + HOCl
Applications in synthesis
Cyanogen chloride is a precursor to the sulfonyl cyanides[4] and chlorosulfonyl isocyanate, a useful reagent in organic synthesis.[5]
Safety
Also known as CK, cyanogen chloride is a highly toxic blood agent, and was once proposed for use in chemical warfare. It causes immediate injury upon contact with the eyes or respiratory organs. Symptoms of exposure may include drowsiness, rhinorrhea (runny nose), sore throat, coughing, confusion, nausea, vomiting, edema, loss of consciousness, convulsions, paralysis, and death.[2] It is especially dangerous because it is capable of penetrating the filters in gas masks, according to U.S. analysts. CK is unstable due to polymerization, sometimes with explosive violence.[6]
Cyanogen chloride is listed in schedule 3 of the Chemical Weapons Convention: all production must be reported to the OPCW.
References
- ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- ^ a b "CYANOGEN CHLORIDE (CK)". The Emergency Response Safety and Health Database. NIOSH.
- ^ Coleman, G. H.; Leeper, R. W.; Schulze, C. C. (1946). "Cyanogen Chloride". Inorganic Syntheses. 2: 90–94. doi:10.1002/9780470132333.ch25.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ Vrijland, M. S. A. (1988). "Sulfonyl Cyanides: Methanesulfonyl Cyanide" (PDF). Organic Syntheses; Collected Volumes, vol. 6, p. 727.
- ^ Graf, R. (1973). "Chlorosulfonyl Isocyanate" (PDF). Organic Syntheses; Collected Volumes, vol. 5, p. 226.
- ^ FM 3-8 Chemical Reference Handbook. US Army. 1967.
External links
- Murphy-Lavoie, H. "Cyanogen Chloride Poisoning". eMedicine. MedScape.
- "National Pollutant Inventory – Cyanide compounds fact sheet". Australian Government.