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| ImageNameR1 = Spacefill model of hydrogen cyanide
| ImageNameR1 = Spacefill model of hydrogen cyanide
| IUPACName = {{Unbulleted list|Formonitrile<ref>{{Cite web|title=Hydrogen Cyanide - Compound Summary|url=http://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=768|work=PubChem Compound|publisher=National Center for Biotechnology Information|accessdate=4 June 2012|location=USA|date=16 September 2004|at=Identification}}</ref> ''(substitutive)''|Hydridonitridocarbon<ref>{{Cite web|title=hydrogen cyanide (CHEBI:18407)|url=https://www.ebi.ac.uk/chebi/searchId.do?chebiId=18407|work=Chemical Entities of Biological Interest|Publisher=European Bioinformatics Institute|accessdate=4 June 2012|location=UK|date=18 October 2009|at=Main}}</ref> ''(additive)''}}
| IUPACName = {{Unbulleted list|Formonitrile<ref>{{Cite web|title=Hydrogen Cyanide - Compound Summary|url=http://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=768|work=PubChem Compound|publisher=National Center for Biotechnology Information|accessdate=4 June 2012|location=USA|date=16 September 2004|at=Identification}}</ref> ''(substitutive)''|Hydridonitridocarbon<ref>{{Cite web|title=hydrogen cyanide (CHEBI:18407)|url=https://www.ebi.ac.uk/chebi/searchId.do?chebiId=18407|work=Chemical Entities of Biological Interest|Publisher=European Bioinformatics Institute|accessdate=4 June 2012|location=UK|date=18 October 2009|at=Main}}</ref> ''(additive)''}}
| OtherNames = {{Unbulleted list|Formic anammonide|Hydrocyanic acid|Prussic acid|Zyklon B
| OtherNames = {{Unbulleted list|Formic anammonide{{Citation needed|date=June 2012}}|Hydrocyanic acid{{Citation needed|date=June 2012}}|Methanenitrile{{Citation needed|date=June 2012}}|Prussic acid{{Citation needed|date=June 2012}}|Zyklon B{{Citation needed|date=June 2012}}
}}
}}
| Section1 = {{Chembox Identifiers
| Section1 = {{Chembox Identifiers

Revision as of 09:29, 16 July 2012

Hydrogen cyanide
Skeletal formula of hydrogen cyanide with the explicit hydrogen added
Ball and stick model of hydrogen cyanide
Ball and stick model of hydrogen cyanide
Spacefill model of hydrogen cyanide
Spacefill model of hydrogen cyanide
Names
IUPAC name
  • Formonitrile[1] (substitutive)
  • Hydridonitridocarbon[2] (additive)
Other names
Identifiers
3D model (JSmol)
3DMet
ChEBI
ChemSpider
ECHA InfoCard 100.000.747 Edit this at Wikidata
EC Number
  • 200-821-6
KEGG
MeSH Hydrogen+Cyanide
RTECS number
  • MW6825000
UNII
UN number 1051
  • InChI=1S/CHN/c1-2/h1H checkY
    Key: LELOWRISYMNNSU-UHFFFAOYSA-N checkY
  • C#N
Properties
CHN
Molar mass 27.026 g·mol−1
Appearance Very pale, blue, transparent liquid
Odor Oil of bitter almond
Density 687 mg mL−1
Miscible
Solubility in ethanol Miscible
75 μmol Pa−1 kg−1
Acidity (pKa) 9.21[3]
Basicity (pKb) 4.79
1.2675 [4]
Viscosity 201 μPa s
Structure
Linear
2.98 D
Thermochemistry
71.00 kJ K−1 mol−1 (at 27 °C)
113.01 J K−1 mol−1
-4.999 MJ kg−1
642 kJ mol−1[5]
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
4
4
1
Flash point −17.8 °C
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Hydrogen cyanide (with the historical common name of Prussic acid) is an inorganic compound[6] with chemical formula HCN. It is a colorless, extremely poisonous liquid that boils slightly above room temperature at 26 °C (79 °F). Hydrogen cyanide is a linear molecule, with a triple bond between carbon and nitrogen. A minor tautomer of HCN is HNC, hydrogen isocyanide.

Hydrogen cyanide is weakly acidic with a pKa of 9.2. It partly ionizes in water solution to give the cyanide anion, CN–. A solution of hydrogen cyanide in water is called hydrocyanic acid. The salts of hydrogen cyanide are known as cyanides.

HCN has a faint, bitter, almond-like odor that only some people are able to detect owing to a genetic trait.[7] The volatile compound has been used as inhalation rodenticide and human poison. Cyanide ions interfere with iron-containing respiratory enzymes.

HCN is produced on an industrial scale and is a highly valuable precursor to many chemical compounds ranging from polymers to pharmaceuticals.

History of discovery

The red colored ferricyanide ion, one component of Prussian blue

Hydrogen cyanide was first isolated from a blue dye (Prussian blue) which had been known from 1704 but whose structure was unknown. It is now known to be a coordination polymer with a complex structure and an empirical formula of hydrated ferric ferrocyanide. In 1752, the French chemist Pierre Macquer made the important step of showing that Prussian blue could be converted to iron oxide plus a volatile component and that these could be used to reconstitute the dye. The new component was what we now know as hydrogen cyanide. Following Macquer's lead, it was first isolated from Prussian blue in pure form and characterized about 1783 by the Swedish chemist Carl Wilhelm Scheele, and was eventually given the German name Blausäure (lit. "Blue sour") because of its acidic nature in water and its derivation from Prussian blue. In English it became known popularly as Prussic acid.

In 1787 the French chemist Claude Louis Berthollet showed that Prussic acid did not contain oxygen, an important contribution to acid theory, which had hitherto postulated that acids must contain oxygen[8] (hence the name of oxygen itself, which is derived from Greek elements that mean "acid-former" and are likewise calqued into German as Sauerstoff). In 1815 Joseph Louis Gay-Lussac deduced Prussic acid's chemical formula. The radical cyanide in hydrogen cyanide was given its name from the Greek word for blue, again owing to its derivation from Prussian blue.

Production and synthesis

Hydrogen cyanide forms in at least limited amounts from many combinations of hydrogen, carbon, and ammonia. Hydrogen cyanide is currently produced in great quantities by several processes, as well as being a recovered waste product from the manufacture of acrylonitrile.[6] In the year 2000, 732,552 tons were produced in the US.[9][dead link]

The most important process is the Andrussow oxidation invented by Leonid Andrussow at IG Farben in which methane and ammonia react in the presence of oxygen at about 1200 °C over a platinum catalyst:[10]

2 CH4 + 2 NH3 + 3 O2 → 2 HCN + 6 H2O

The energy needed for the reaction is provided by the partial oxidation of methane and ammonia.

Of lesser importance is the Degussa process (BMA process) in which no oxygen is added and the energy must be transferred indirectly through the reactor wall:[11]

CH4 + NH3 → HCN + 3H2

This reaction is akin to steam reforming, the reaction of methane and water to give carbon monoxide and hydrogen.

In the Shawinigan Process, hydrocarbons, e.g. propane, are reacted with ammonia:

C3H8 + 3 NH3 → 3 HCN + 7 H2

When heated strongly, formamide decomposes to hydrogen cyanide and water vapor:

CH(O)NH2 → HCN + H2O

In the laboratory, small amounts of HCN are produced by the addition of acids to cyanide salts of alkali metals:

H+ + NaCN → HCN + Na+

This reaction is sometimes the basis of accidental poisonings because the acid converts a nonvolatile cyanide salt into the gaseous HCN.

Historical methods of production

The demand for cyanides for mining operations in the 1890s was met by George Thomas Beilby, who patented a method to produce hydrogen cyanide by passing ammonia over glowing coal in 1892. This method was used until Hamilton Castner in 1894 developed a synthesis starting from coal, ammonia, and sodium yielding sodium cyanide, which reacts with acid to form gaseous HCN.

Applications

HCN is the precursor to sodium cyanide and potassium cyanide, which are used mainly in gold and silver mining and for the electroplating of those metals. Via the intermediacy of cyanohydrins, a variety of useful organic compounds are prepared from HCN including the monomer methyl methacrylate, from acetone, the amino acid methionine, via the Strecker synthesis, and the chelating agents EDTA and NTA. Via the hydrocyanation process, HCN is added to butadiene to give adiponitrile, a precursor to Nylon 66.[6]

Occurrence

HCN is obtainable from fruits that have a pit, such as cherries, apricots, apples, and bitter almonds, from which almond oil and flavoring are made. Many of these pits contain small amounts of cyanohydrins such as mandelonitrile and amygdalin, which slowly release hydrogen cyanide.[12][13] One hundred grams of crushed apple seeds can yield about 10 mg of HCN.[citation needed] Some millipedes release hydrogen cyanide as a defense mechanism,[14] as do certain insects, such as some burnet moths. Hydrogen cyanide is contained in the exhaust of vehicles, in tobacco and wood smoke, and in smoke from burning nitrogen-containing plastics. So-called "bitter" roots of the cassava plant may contain up to 1 gram of HCN per kilogram.[15][16]

HCN and the origin of life

Hydrogen cyanide has been discussed as a precursor to amino acids and nucleic acids. For example, HCN is proposed to have played a part in the origin of life.[17] Although the relationship of these chemical reactions to the origin of life theory remains speculative, studies in this area have led to discoveries of new pathways to organic compounds derived from the condensation of HCN.[18]

HCN in space

See also: Astrochemistry

HCN has been detected in the interstellar medium.[19] Since then, extensive studies have probed formation and destruction pathways of HCN in various environments and examined its use as a tracer for a variety of astronomical species and processes. HCN can be observed from ground-based telescopes through a number of atmospheric windows.[20] The J=1→0, J=3→2, J= 4→3, and J=10→9 pure rotational transitions have all been observed.[19][21][22]

HCN is formed in interstellar clouds through one of two major pathways:[23] via a neutral-neutral reaction (CH2 + N → HCN + H) and via dissociative recombination (HCNH+ + e- → HCN + H). The dissociative recombination pathway is dominant by 30%; however, the HCNH+ must be in its linear form. Dissociative recombination with its structural isomer, H2NC+ produces hydrogen isocyanide (HNC), exclusively.

HCN is destroyed in interstellar clouds through a number of mechanisms depending on the location in the cloud.[23] In photon-dominated regions (PDRs), photodissociation dominates, producing CN (HCN + ν → CN + H). At further depths, photodissociation by cosmic rays dominate, producing CN (HCN + cr → CN + H). In the dark core, two competing mechanisms destroy it, forming HCN+ and HCNH+ (HCN + H+ → HCN+ + H; HCN + HCO+ → HCNH+ + CO). The reaction with HCO+ dominates by a factor of ~3.5. HCN has been used to analyze a variety of species and processes in the interstellar medium. It has been suggested as a tracer for dense molecular gas[24][25] and as a tracer of stellar inflow in high-mass star-forming regions.[26] Further, the HNC/HCN ratio has been shown to be an excellent method for distinguishing between PDRs and X-ray-dominated regions (XDRs).[27]

Hydrogen cyanide as a poison and chemical weapon

Main article: Cyanide poisoning

A hydrogen cyanide concentration of 300 mg/m3 in air will kill a human within about 10 minutes.[28] A hydrogen cyanide concentration of 3500 ppm (about 3200 mg/m3) will kill a human in about 1 minute.[28] The toxicity is caused by the cyanide ion, which halts cellular respiration by inhibiting an enzyme in mitochondria called cytochrome c oxidase.

Hydrogen cyanide absorbed into a carrier for use as a pesticide (under IG Farben's brand name Cyclone B, or in German Zyklon B, with the B standing for Blausäure)[29] was employed by Nazi Germany in the mid-20th century in extermination camps. The same product is currently made in the Czech Republic under the trademark "Uragan D2." Hydrogen cyanide is also the agent used in gas chambers employed in judicial execution in some U.S. states, where it is produced during the execution by the action of sulfuric acid on an egg-sized mass of potassium cyanide.

Hydrogen cyanide is commonly listed amongst chemical warfare agents known as blood agents.[30] As a substance listed under Schedule 3 of the Chemical Weapons Convention as a potential weapon which has large-scale industrial uses, manufacturing plants in signatory countries which produce more than 30 tonnes per year must be declared to, and can be inspected by, the Organisation for the Prohibition of Chemical Weapons.

Under the name prussic acid, HCN has been used as a killing agent in whaling harpoons.[31]

Hydrogen cyanide gas in air is explosive at concentrations over 5.6%.[32] This is far above its toxicity level.

References

  1. ^ "Hydrogen Cyanide - Compound Summary". PubChem Compound. USA: National Center for Biotechnology Information. 16 September 2004. Identification. Retrieved 4 June 2012.
  2. ^ "hydrogen cyanide (CHEBI:18407)". Chemical Entities of Biological Interest. UK. 18 October 2009. Main. Retrieved 4 June 2012. {{cite web}}: Unknown parameter |Publisher= ignored (|publisher= suggested) (help)
  3. ^ Perrin, D.D., Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution; 2nd Ed., Pergamon Press; Oxford, 1982.
  4. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  5. ^ Gary R. Maxwell (19 May 2004). Synthetic Nitrogen Products: A Practical Guide to the Products and Processes. Springer. p. 348. ISBN 978-0-306-48225-0. Retrieved 3 June 2012.
  6. ^ a b c Ernst Gail, Stephen Gos, Rupprecht Kulzer, Jürgen Lorösch, Andreas Rubo, Manfred Sauer (2004). "Cyano Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Verlag, Weinheim: Wiley-VCH. doi:10.1002/14356007.a08+159.pub2.{{cite encyclopedia}}: CS1 maint: multiple names: authors list (link)
  7. ^ "Cyanide, inability to smell". Online Mendelian Inheritance in Man. Retrieved 2010-03-31.
  8. ^ Brian T Newbold (1999-11-01). "Claude Louis Berthollet: A Great Chemist in +he french Tradition". Canadian Chemical News. Retrieved 2010-03-31.
  9. ^ The Innovation Group. The Innovation Group. Retrieved on 2012-06-02.
  10. ^ L. Andrussow (1935). "The catalytic oxydation of ammonia-methane-mixtures to hydrogen cyanide". Angewandte Chemie. 48 (37): 593–595. doi:10.1002/ange.19350483702.
  11. ^ F. Endter (1958). "Die technische Synthese von Cyanwasserstoff aus Methan und Ammoniak ohne Zusatz von Sauerstoff". Chemie Ingenieur Technik. 30 (5): 281–376. doi:10.1002/cite.330300506.
  12. ^ J. Vetter (2000). "Plant cyanogenic glycosides". Toxicon. 38 (1): 11–36. doi:10.1016/S0041-0101(99)00128-2. PMID 10669009.
  13. ^ D. A. Jones (1998). "Why are so many food plants cyanogenic?". Phytochemistry. 47 (2): 155–162. doi:10.1016/S0031-9422(97)00425-1. PMID 9431670.
  14. ^ M. S. Blum, J. P. Woodring (1962). "Secretion of Benzaldehyde and Hydrogen Cyanide by the Millipede Pachydesmus crassicutis (Wood)". Science. 138 (3539): 512–513. Bibcode:1962Sci...138..512B. doi:10.1126/science.138.3539.512. PMID 17753947.
  15. ^ Aregheore E. M, Agunbiade O. O. (1991). "The toxic effects of cassava (manihot esculenta grantz) diets on humans: a review". Vet. Hum. Toxicol. 33 (3): 274–275. PMID 1650055.
  16. ^ White W. L. B., Arias-Garzon D. I., McMahon J. M., Sayre R. T. (1998). "Cyanogenesis in Cassava, The Role of Hydroxynitrile Lyase in Root Cyanide Production". Plant Physiology. 116 (4): 1219–1225. doi:10.1104/pp.116.4.1219. PMC 35028. PMID 9536038.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  17. ^ Matthews, C. N. "The HCN World: Establishing Protein-Nucleic Augucid Life via Hydrogen Cyanide Polymers" in Cellular Origin and Life in Extreme Habitats and Astrobiology (2004), 6 (Origins : Genesis, Evoluation and Diversity of Life), pp. 121–135.
  18. ^ Al-Azmi, A.; Elassar, A.-Z. A.; Booth, B. L. (2003). "The Chemistry of Diaminomaleonitrile and its Utility in Heterocyclic Synthesis". Tetrahedron. 59 (16): 2749. doi:10.1016/S0040-4020(03)00153-4.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  19. ^ a b Snyder, Lewis E.; Buhl, David (1971). "Observations of Radio Emission from Interstellar Hydrogen Cyanide". Astrophysical Journal. 163: L47. Bibcode:1971ApJ...163L..47S. doi:10.1086/180664.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  20. ^ Treffers, R; Larson, Harold P.; Fink, Uwe; Gautier, Thomas N. (1978). "Upper limits to trace constituents in Jupiter's atmosphere from an analysis of its 5-μm spectrum". Icarus. 34 (2): 331. Bibcode:1978Icar...34..331T. doi:10.1016/0019-1035(78)90171-9.
  21. ^ Bieging, J. H.; Shaked, S.; Gensheimer, P. D. (2000). "Submillimeter‐ and Millimeter‐Wavelength Observations of SiO and HCN in Circumstellar Envelopes of AGB Stars". Astrophysical Journal. 543 (2): 897. Bibcode:2000ApJ...543..897B. doi:10.1086/317129.
  22. ^ Schilke, P. and Menten, K. M. (2003). "Detection of a Second, Strong Sub-millimeter HCN Laser Line toward Carbon Stars". Astrophysical Journal. 583: 446. Bibcode:2003ApJ...583..446S. doi:10.1086/345099.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  23. ^ a b Boger, G. I. and Sternberg, A. (2005). "CN and HCN in Dense Interstellar Clouds". Astrophysical Journal. 632: 302. arXiv:astro-ph/0506535. Bibcode:2005ApJ...632..302B. doi:10.1086/432864.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  24. ^ Gao, Y. and Solomon, P. M. (2004). "The Star Formation Rate and Dense Molecular Gas in Galaxies". Astrophysical Journal. 606: 271. arXiv:astro-ph/0310339. Bibcode:2004ApJ...606..271G. doi:10.1086/382999.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  25. ^ Gao, Y. and Solomon, P. M. (2004). "HCN Survey of Normal Spiral, Infrared‐luminous, and Ultraluminous Galaxies". Astrophysical Journal Supplements. 152: 63. arXiv:astro-ph/0310341. Bibcode:2004ApJS..152...63G. doi:10.1086/383003.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  26. ^ Wu, J. and Evans, N. J. (2003). "Indications of Inflow Motions in Regions Forming Massive Stars". Astrophysical Journal. 592 (2): L79. arXiv:astro-ph/0306543. Bibcode:2003ApJ...592L..79W. doi:10.1086/377679.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  27. ^ Loenen; A. F.; et al. (2007). Proceedings IAU Symposium. 202. {{cite journal}}: Missing or empty |title= (help); Unknown parameter |author-separator= ignored (help)
  28. ^ a b Environmental and Health Effects. Cyanidecode.org. Retrieved on 2012-06-02.
  29. ^ Dwork, Deborah (1996). Auschwitz, 1270 to the present. Norton. p. 443. ISBN 0-393-03933-1. {{cite book}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  30. ^ "Hydrogen Cyanide". Organisation for the Prohibition of Chemical Weapons. Retrieved 2009-01-14.
  31. ^ Poison Hand Darted Harpoons and Lances.
  32. ^ Documentation for Immediately Dangerous to Life or Health Concentrations (IDLHs) – 74908.
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