Summary
Cyanogen iodide or iodine cyanide (ICN) is a pseudohalogen composed of iodine and the cyanide group. It is a highly toxic inorganic compound. It occurs as white crystals that react slowly with water to form hydrogen cyanide.[5][6][7]
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| Names | |||
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| Preferred IUPAC name
Carbononitridic iodide[2] | |||
| Other names
Iodine cyanide[1]
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| ECHA InfoCard | 100.007.322 | ||
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CompTox Dashboard (EPA)
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| Properties[4] | |||
| ICN | |||
| Molar mass | 152.9219 g mol−1 | ||
| Appearance | White crystals | ||
| Density | 1.84 g mL−1 | ||
| Melting point | 146.7 °C (296.1 °F; 419.8 K) | ||
| Reacts | |||
| Vapor pressure | 0.001 bar (298.4K)[3] | ||
| Thermochemistry | |||
Std enthalpy of
formation (ΔfH⦵298) |
160.5–169.1 kJ mol−1 | ||
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| NFPA 704 (fire diamond) | |||
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Related alkanenitriles
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references
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Synthesis edit
Cyanogen iodide is prepared by combining I2 and a cyanide, most commonly sodium cyanide in ice-cold water. The product is extracted with diethyl ether.[5][6][7]
- I2 + NaCN → NaI + ICN
Applications edit
Cyanogen iodide has been used in taxidermy as a preservative[8][9] because of its toxicity.[9]
History edit
Cyanogen iodide was first synthesized in 1824 by the French chemist Georges-Simon Serullas (1774–1832).[10]
Cyanogen iodide was considered one of the impurities in commercially sold iodine before the 1930s.[citation needed]
Hazards edit
Cyanogen iodide is toxic if inhaled or ingested and may be fatal if swallowed or absorbed through the skin. Cyanogen iodide may cause convulsions, paralysis and death from respiratory failure. It is a strong irritant and may cause burns to the eyes and skin if contacted. If cyanogen iodide is heated enough to undergo complete decomposition, it may releases toxic fumes of nitrogen oxides, cyanide and iodide. A fire may cause the release of poisonous gas. Cyanogen iodide decomposes when contacted with acids, bases, ammonia, alcohols, and with heating. ICN slowly reacts with water or carbon dioxide to produce hydrogen cyanide.[9][11][12][13]
It is classified as an extremely hazardous substance in the United States as defined in Section 302 of the U.S. Emergency Planning and Community Right-to-Know Act (42 U.S.C. 11002), and is subject to strict reporting requirements by facilities which produce, store, or use it in significant quantities.[14]
Solutions in pyridine edit
Cyanogen iodide solutions in pyridine conduct electric current. Dilute solutions of ICN in pyridine are colorless at first, but upon standing become successively yellow, orange, red-brown and deep red-brown. This effect is due to a change in conductivity, which in turn is due to the formation of an electrolyte. When electrical conductivity of ICN is compared with that of iodine-pyridine solutions, the formation of the electrolyte in ICN proceeds much more slowly. Results confirm that cyanides are much weaker salts in pyridine than are iodides, although cyanogen iodide solutions are able to be dissolved in pyridine giving solutions with electrical conductivity that increases over time and results in maximum values.[15]
External links edit
- "IODINE CYANIDE ICSC: 0662". INCHEM.
References edit
- ^ The Merck Index (10th ed.). Rahway, NJ: Merck & Co. 1983. p. 385. ISBN 9780911910278.
- ^ International Union of Pure and Applied Chemistry (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013. The Royal Society of Chemistry. p. 799. doi:10.1039/9781849733069. ISBN 978-0-85404-182-4.
- ^ Cyanogen Iodide in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD) (retrieved 2022-09-16)
- ^ 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 Bak, B.; Hillebert, A. (1952). "CYANOGEN IODIDE". Organic Syntheses. 32: 29; Collected Volumes, vol. 4, p. 207.
- ^ a b Langlois, M. (1860). "CYANOGÈNE Action de l'iode sur une solution concentrée de cyanure de potassium". Comptes Rendus. 51: 29.
- ^ a b Langlois, M. (1860). "Ueber die Einwirkung des Jods auf concentrirte Cyankaliumlösung". Annalen der Chemie und Pharmacie. 116 (3): 288. doi:10.1002/jlac.18601160303.
- ^ "Cyanogen halide". Encyclopædia Britannica (online). Encyclopædia Britannica Inc. 2012. Retrieved 2012-04-12.
- ^ a b c Pohanish, R. P. (2011). "Cyanogen iodide". Sittig's Handbook of Toxic and Hazardous Chemicals and Carcinogens (6th ed.). Elsevier. p. 808. ISBN 978-1-4377-7869-4.
- ^ Serullas (1824). "Nouveau composé d'iode, d'azote et de charbon ou cyanure d'iode" [New compound of iodine, nitrogen, and carbon, or cyanide of iodine]. Annales de Chimie et de Physique. 2nd series (in French). 27: 184–195.
- ^ "Iodine cyanide - Compound Summary (CID 10478)". PubChem. NIH.
- ^ "Iodine Cyanide; International Chemical Safety Card No. 0662 (U.S. National Version)". National Institute for Occupational Safety and Health, Centers for Disease Control and Prevention. 2005. Retrieved 2012-04-12.
- ^ "Cyanogen Iodide". ChemicalBook.
- ^ "40 C.F.R.: Appendix A to Part 355—The List of Extremely Hazardous Substances and Their Threshold Planning Quantities" (PDF) (July 1, 2008 ed.). Government Printing Office. Archived from the original (PDF) on February 25, 2012. Retrieved October 29, 2011.
{{cite journal}}: Cite journal requires|journal=(help) - ^ Audrieth, L. F.; Birr, E. J. (1933). "Anomalous Electrolytes. I. The Electrical Conductivity of Solutions of Iodine and Cyanogen Iodide in Pyridine". Journal of the American Chemical Society. 55 (2): 668–673. doi:10.1021/ja01329a030.