Cyanogen iodide: Difference between revisions
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==Applications== |
==Applications== |
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Cyanogen iodide has been used in taxidermy as a preservative |
Cyanogen iodide has been used in taxidermy as a preservative<ref>{{ cite encyclopedia | title = Cyanogen halide | encyclopedia = Encyclopædia Britannica (online) | year = 2012 | publisher = Encyclopædia Britannica Inc. | url = http://www.britannica.com/EBchecked/topic/147758/cyanogen-halide | accessdate = 2012-04-12 }}</ref><ref name=Poh/>, becuase of its toxivity.<ref name=Poh>{{ cite book | author = Pohanish, R. P. | title = Sittig’s Handbook of Toxic and Hazardous Chemicals and Carcinogens | edition = 6th | chapter = Cyanogen iodide | year = 2011 | page = 808 | publisher = Elsevier | isbn = 978-1-4377-7869-4 | url = https://books.google.com/books?id=RYt0Wzb60b4C&pg=PA808 }}</ref> |
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==History== |
==History== |
Revision as of 13:18, 4 March 2019
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Names | |||
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IUPAC name
Carbononitridic iodide[2]
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Systematic IUPAC name
Iodoformonitrile[citation needed] | |||
Other names
Iodine cyanide[1]
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Identifiers | |||
3D model (JSmol)
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ChemSpider | |||
ECHA InfoCard | 100.007.322 | ||
EC Number |
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PubChem CID
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RTECS number |
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CompTox Dashboard (EPA)
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Properties[3] | |||
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 | |||
Thermochemistry | |||
Std enthalpy of
formation (ΔfH⦵298) |
160.5–169.1 kJ mol−1 | ||
Hazards | |||
NFPA 704 (fire diamond) | |||
Related compounds | |||
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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Cyanogen iodide or iodine cyanide (ICN) is a pseudohalogen composed of iodine and the cyanide group. It is a relatively volatile and highly toxic inorganic compound. It occurs as white crystals that react slowly with water to form hydrogen cyanide.[4][5][6]
Synthesis
Cyanogen iodide is prepared by combining I2 and a cyanide, most commonly sodium cyanide in ice-cold water. The product is extracted with ether.[4][5][6]
- I2 + NaCN → NaI + ICN
Applications
Cyanogen iodide has been used in taxidermy as a preservative[7][8], becuase of its toxivity.[8]
History
Cyanogen iodide was first synthesized in 1824 by the French chemist Georges-Simon Serullas (1774–1832).[9]
Cyanogen iodide was considered one of the impurities in commercially sold iodine before the 1930s.[citation needed]
Hazards
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.[8][10][11][12]
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.[13]
Solutions in pyridine
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.[14]
External links
- "IODINE CYANIDE ICSC: 0662". INCHEM.
References
- ^ The Merck Index (10th ed.). Rahway, NJ: Merck & Co. 1983. p. 385.
- ^ "Iodine cyanide - Compound Summary". PubChem Compound. USA: National Center for Biotechnology Information. 27 March 2005. Identification. Retrieved 4 June 2012.
- ^ 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
{{cite journal}}
: CS1 maint: multiple names: authors list (link); 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. Retrieved October 29, 2011.
{{cite journal}}
: Cite journal requires|journal=
(help)CS1 maint: postscript (link) - ^ 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.