Jump to content

Cyanide

From Wikipedia, the free encyclopedia
(Redirected from Cyano group)
This article is about the class of chemical compounds. For other uses, see Cyanide (disambiguation).
Not to be confused with Nitrile.
Cyanide
Space-filling model of the cyanide anion: carbon bound to smaller nitrogen atom
Names
Systematic IUPAC name
Nitridocarbonate(II)
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
UNII
  • InChI=1S/CN/c1-2/q-1
    Key: XFXPMWWXUTWYJX-UHFFFAOYSA-N
  • [C-]#N
Properties
CN−
Molar mass 26.018 g·mol−1
Conjugate acid Hydrogen cyanide
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 The cyanide ion CN− is one of the most poisonous chemicals. It may cause death in minutes.
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

In chemistry, cyanide (from Greek kyanos 'dark blue') is a chemical compound that contains a C≡N functional group. This group, known as the cyano group, consists of a carbon atom triple-bonded to a nitrogen atom.[1]

In inorganic cyanides, the cyanide group is present as the cyanide anion −C≡N. This anion is extremely poisonous. Soluble salts such as sodium cyanide (NaCN) and potassium cyanide (KCN) are highly toxic.[2] Hydrocyanic acid, also known as hydrogen cyanide, or HCN, is a highly volatile liquid that is produced on a large scale industrially. It is obtained by acidification of cyanide salts.

Organic cyanides are usually called nitriles. In nitriles, the −C≡N group is linked by a single covalent bond to carbon. For example, in acetonitrile (CH3−C≡N), the cyanide group is bonded to methyl (−CH3). Although nitriles generally do not release cyanide ions, the cyanohydrins do and are thus toxic.

Bonding

[edit]

The cyanide ion −C≡N is isoelectronic with carbon monoxide −C≡O+ and with molecular nitrogen N≡N. A triple bond exists between C and N. The negative charge is concentrated on carbon C.[3][4]

Occurrence

[edit]

In nature

[edit]
Removal of cyanide from cassava in Nigeria.

Cyanides are produced by certain bacteria, fungi, and algae. It is an antifeedant in a number of plants. Cyanides are found in substantial amounts in certain seeds and fruit stones, e.g., those of bitter almonds, apricots, apples, and peaches.[5] Chemical compounds that can release cyanide are known as cyanogenic compounds. In plants, cyanides are usually bound to sugar molecules in the form of cyanogenic glycosides and defend the plant against herbivores. Cassava roots (also called manioc), an important potato-like food grown in tropical countries (and the base from which tapioca is made), also contain cyanogenic glycosides.[6][7]

The Madagascar bamboo Cathariostachys madagascariensis produces cyanide as a deterrent to grazing. In response, the golden bamboo lemur, which eats the bamboo, has developed a high tolerance to cyanide.

The hydrogenase enzymes contain cyanide ligands attached to iron in their active sites. The biosynthesis of cyanide in the NiFe hydrogenases proceeds from carbamoyl phosphate, which converts to cysteinyl thiocyanate, the CN− donor.[8]

Interstellar medium

[edit]

The cyanide radical •CN has been identified in interstellar space.[9] Cyanogen, (CN)2, is used to measure the temperature of interstellar gas clouds.[10]

Pyrolysis and combustion product

[edit]

Hydrogen cyanide is produced by the combustion or pyrolysis of certain materials under oxygen-deficient conditions. For example, it can be detected in the exhaust of internal combustion engines and tobacco smoke. Certain plastics, especially those derived from acrylonitrile, release hydrogen cyanide when heated or burnt.[11]

Organic derivatives

[edit]
Main article: Nitriles
See also: Isocyanide

In IUPAC nomenclature, organic compounds that have a −C≡N functional group are called nitriles.[12][13] An example of a nitrile is acetonitrile, CH3−C≡N. Nitriles usually do not release cyanide ions. A functional group with a hydroxyl −OH and cyanide −CN bonded to the same carbon atom is called cyanohydrin (R2C(OH)CN). Unlike nitriles, cyanohydrins do release poisonous hydrogen cyanide.

Reactions

[edit]

Protonation

[edit]

Cyanide is basic. The pKa of hydrogen cyanide is 9.21. Thus, addition of acids stronger than hydrogen cyanide to solutions of cyanide salts releases hydrogen cyanide.

Hydrolysis

[edit]

Cyanide is unstable in water, but the reaction is slow until about 170 °C. It undergoes hydrolysis to give ammonia and formate, which are far less toxic than cyanide:[14]

CN− + 2 H2O → HCO−2 + NH3

Cyanide hydrolase is an enzyme that catalyzes this reaction.

Alkylation

[edit]

Because of the cyanide anion's high nucleophilicity, cyano groups are readily introduced into organic molecules by displacement of a halide group (e.g., the chloride on methyl chloride). In general, organic cyanides are called nitriles. In organic synthesis, cyanide is a C-1 synthon; i.e., it can be used to lengthen a carbon chain by one, while retaining the ability to be functionalized.[15]

RX + CN− → RCN + X−

Redox

[edit]

The cyanide ion is a reductant and is oxidized by strong oxidizing agents such as molecular chlorine (Cl2), hypochlorite (ClO−), and hydrogen peroxide (H2O2). These oxidizers are used to destroy cyanides in effluents from gold mining.[16][17][18]

Metal complexation

[edit]

The cyanide anion reacts with transition metals to form M-CN bonds. This reaction is the basis of cyanide's toxicity.[19] The high affinities of metals for this anion can be attributed to its negative charge, compactness, and ability to engage in π-bonding.

Among the most important cyanide coordination compounds are the potassium ferrocyanide and the pigment Prussian blue, which are both essentially nontoxic due to the tight binding of the cyanides to a central iron atom.[20] Prussian blue was first accidentally made around 1706, by heating substances containing iron and carbon and nitrogen, and other cyanides made subsequently (and named after it). Among its many uses, Prussian blue gives the blue color to blueprints, bluing, and cyanotypes.

Manufacture

[edit]
Main article: Hydrogen cyanide § Production and synthesis

The principal process used to manufacture cyanides is the Andrussow process in which gaseous hydrogen cyanide is produced from methane and ammonia in the presence of oxygen and a platinum catalyst.[21][22]

2 CH4 + 2 NH3 + 3 O2 → 2 HCN + 6 H2O

Sodium cyanide, the precursor to most cyanides, is produced by treating hydrogen cyanide with sodium hydroxide:[14]

HCN + NaOH → NaCN + H2O

Toxicity

[edit]
Main article: Cyanide poisoning

Among the most toxic cyanides are hydrogen cyanide (HCN), sodium cyanide (NaCN), potassium cyanide (KCN), and calcium cyanide (Ca(CN)₂). These compounds are extremely poisonous and require careful handling to avoid severe health risks. The cyanide anion is an inhibitor of the enzyme cytochrome c oxidase (also known as aa3), the fourth complex of the electron transport chain found in the inner membrane of the mitochondria of eukaryotic cells. It attaches to the iron within this protein. The binding of cyanide to this enzyme prevents transport of electrons from cytochrome c to oxygen. As a result, the electron transport chain is disrupted, meaning that the cell can no longer aerobically produce ATP for energy.[23] Tissues that depend highly on aerobic respiration, such as the central nervous system and the heart, are particularly affected. This is an example of histotoxic hypoxia.[24]

The most hazardous compound is hydrogen cyanide, which is a gas and kills by inhalation. For this reason, an air respirator supplied by an external oxygen source must be worn when working with hydrogen cyanide.[11] Hydrogen cyanide is produced by adding acid to a solution containing a cyanide salt. Alkaline solutions of cyanide are safer to use because they do not evolve hydrogen cyanide gas. Hydrogen cyanide may be produced in the combustion of polyurethanes; for this reason, polyurethanes are not recommended for use in domestic and aircraft furniture. Oral ingestion of a small quantity of solid cyanide or a cyanide solution of as little as 200 mg, or exposure to airborne cyanide of 270 ppm, is sufficient to cause death within minutes.[24]

Organic nitriles do not readily release cyanide ions, and so have low toxicities. By contrast, compounds such as trimethylsilyl cyanide (CH3)3SiCN readily release HCN or the cyanide ion upon contact with water.[25]

Antidote

[edit]

Hydroxocobalamin reacts with cyanide to form cyanocobalamin, which can be safely eliminated by the kidneys. This method has the advantage of avoiding the formation of methemoglobin (see below). This antidote kit is sold under the brand name Cyanokit and was approved by the U.S. FDA in 2006.[26]

An older cyanide antidote kit included administration of three substances: amyl nitrite pearls (administered by inhalation), sodium nitrite, and sodium thiosulfate. The goal of the antidote was to generate a large pool of ferric iron (Fe3+) to compete for cyanide with cytochrome a3 (so that cyanide will bind to the antidote rather than the enzyme). The nitrites oxidize hemoglobin to methemoglobin, which competes with cytochrome oxidase for the cyanide ion. Cyanmethemoglobin is formed and the cytochrome oxidase enzyme is restored. The major mechanism to remove the cyanide from the body is by enzymatic conversion to thiocyanate by the mitochondrial enzyme rhodanese. Thiocyanate is a relatively non-toxic molecule and is excreted by the kidneys. To accelerate this detoxification, sodium thiosulfate is administered to provide a sulfur donor for rhodanese, needed in order to produce thiocyanate.[27]

Sensitivity

[edit]

Minimum risk levels (MRLs) may not protect for delayed health effects or health effects acquired following repeated sublethal exposure, such as hypersensitivity, asthma, or bronchitis. MRLs may be revised after sufficient data accumulates.[28]

Applications

[edit]

Mining

[edit]
Main article: Gold cyanidation

Cyanide is mainly produced for the mining of silver and gold: It helps dissolve these metals allowing separation from the other solids. In the cyanide process, finely ground high-grade ore is mixed with the cyanide (at a ratio of about 1:500 parts NaCN to ore); low-grade ores are stacked into heaps and sprayed with a cyanide solution (at a ratio of about 1:1000 parts NaCN to ore). The precious metals are complexed by the cyanide anions to form soluble derivatives, e.g., [Ag(CN)2]− (dicyanoargentate(I)) and [Au(CN)2]− (dicyanoaurate(I)).[14] Silver is less "noble" than gold and often occurs as the sulfide, in which case redox is not invoked (no O2 is required). Instead, a displacement reaction occurs:

The "pregnant liquor" containing these ions is separated from the solids, which are discarded to a tailing pond or spent heap, the recoverable gold having been removed. The metal is recovered from the "pregnant solution" by reduction with zinc dust or by adsorption onto activated carbon. This process can result in environmental and health problems. A number of environmental disasters have followed the overflow of tailing ponds at gold mines. Cyanide contamination of waterways has resulted in numerous cases of human and aquatic species mortality.[29]

Aqueous cyanide is hydrolyzed rapidly, especially in sunlight. It can mobilize some heavy metals such as mercury if present. Gold can also be associated with arsenopyrite (FeAsS), which is similar to iron pyrite (fool's gold), wherein half of the sulfur atoms are replaced by arsenic. Gold-containing arsenopyrite ores are similarly reactive toward inorganic cyanide.[30][31]

Industrial organic chemistry

[edit]

The second major application of alkali metal cyanides (after mining) is in the production of CN-containing compounds, usually nitriles. Acyl cyanides are produced from acyl chlorides and cyanide. Cyanogen, cyanogen chloride, and the trimer cyanuric chloride are derived from alkali metal cyanides.

Medical uses

[edit]

The cyanide compound sodium nitroprusside is used mainly in clinical chemistry to measure urine ketone bodies mainly as a follow-up to diabetic patients. On occasion, it is used in emergency medical situations to produce a rapid decrease in blood pressure in humans; it is also used as a vasodilator in vascular research. The cobalt in artificial vitamin B12 contains a cyanide ligand as an artifact of the purification process; this must be removed by the body before the vitamin molecule can be activated for biochemical use. During World War I, a copper cyanide compound was briefly used by Japanese physicians for the treatment of tuberculosis and leprosy.[32]

Illegal fishing and poaching

[edit]
Main article: Cyanide fishing

Cyanides are illegally used to capture live fish near coral reefs for the aquarium and seafood markets. The practice is controversial, dangerous, and damaging but is driven by the lucrative exotic fish market.[33]

Poachers in Africa have been known to use cyanide to poison waterholes, to kill elephants for their ivory.[34]

Pest control

[edit]

M44 cyanide devices are used in the United States to kill coyotes and other canids.[35] Cyanide is also used for pest control in New Zealand, particularly for possums, an introduced marsupial that threatens the conservation of native species and spreads tuberculosis amongst cattle. Possums can become bait shy but the use of pellets containing the cyanide reduces bait shyness. Cyanide has been known to kill native birds, including the endangered kiwi.[36] Cyanide is also effective for controlling the dama wallaby, another introduced marsupial pest in New Zealand.[37] A licence is required to store, handle and use cyanide in New Zealand.

Cyanides are used as insecticides for fumigating ships.[38] Cyanide salts are used for killing ants,[39] and have in some places been used as rat poison[40] (the less toxic poison arsenic is more common).[41]

Niche uses

[edit]

Potassium ferrocyanide is used to achieve a blue color on cast bronze sculptures during the final finishing stage of the sculpture. On its own, it will produce a very dark shade of blue and is often mixed with other chemicals to achieve the desired tint and hue. It is applied using a torch and paint brush while wearing the standard safety equipment used for any patina application: rubber gloves, safety glasses, and a respirator. The actual amount of cyanide in the mixture varies according to the recipes used by each foundry.

Cyanide is also used in jewelry-making and certain kinds of photography such as sepia toning.

Although usually thought to be toxic, cyanide and cyanohydrins increase germination in various plant species.[42][43]

Human poisoning

[edit]
Main article: Cyanide poisoning

Deliberate cyanide poisoning of humans has occurred many times throughout history.[44] Common salts such as sodium cyanide are involatile but water-soluble, so are poisonous by ingestion. Hydrogen cyanide is a gas, making it more indiscriminately dangerous, however it is lighter than air and rapidly disperses up into the atmosphere, which makes it ineffective as a chemical weapon.

Food additive

[edit]

Because of the high stability of their complexation with iron, ferrocyanides (Sodium ferrocyanide E535, Potassium ferrocyanide E536, and Calcium ferrocyanide E538[45]) do not decompose to lethal levels in the human body and are used in the food industry as, e.g., an anticaking agent in table salt.[46]

Chemical tests for cyanide

[edit]

Cyanide is quantified by potentiometric titration, a method widely used in gold mining. It can also be determined by titration with silver ion. Some analyses begin with an air-purge of an acidified boiling solution, sweeping the vapors into a basic absorber solution. The cyanide salt absorbed in the basic solution is then analyzed.[47]

Qualitative tests

[edit]

Because of the notorious toxicity of cyanide, many methods have been investigated. Benzidine gives a blue coloration in the presence of ferricyanide.[48] Iron(II) sulfate added to a solution of cyanide, such as the filtrate from the sodium fusion test, gives prussian blue. A solution of para-benzoquinone in DMSO reacts with inorganic cyanide to form a cyanophenol, which is fluorescent. Illumination with a UV light gives a green/blue glow if the test is positive.[49]

References

[edit]
  1. ^ "cyanides". IUPAC Gold Book. 2014. doi:10.1351/goldbook.C01486.
  2. ^ "Environmental and Health Effects of Cyanide". International Cyanide Management Institute. 2006. Archived from the original on 30 November 2012. Retrieved 4 August 2009.
  3. ^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.[page needed]
  4. ^ G. L. Miessler and D. A. Tarr "Inorganic Chemistry" 3rd Ed, Pearson/Prentice Hall publisher, ISBN 0-13-035471-6.[page needed]
  5. ^ "ToxFAQs for Cyanide". Agency for Toxic Substances and Disease Registry. July 2006. Retrieved 2008-06-28.
  6. ^ Vetter, J. (2000). "Plant cyanogenic glycosides". Toxicon. 38 (1): 11–36. doi:10.1016/S0041-0101(99)00128-2. PMID 10669009.
  7. ^ Jones, D. A. (1998). "Why are so many food plants cyanogenic?". Phytochemistry. 47 (2): 155–162. Bibcode:1998PChem..47..155J. doi:10.1016/S0031-9422(97)00425-1. PMID 9431670.
  8. ^ Reissmann, Stefanie; Hochleitner, Elisabeth; Wang, Haofan; Paschos, Athanasios; Lottspeich, Friedrich; Glass, Richard S.; Böck, August (2003). "Taming of a Poison: Biosynthesis of the NiFe-Hydrogenase Cyanide Ligands" (PDF). Science. 299 (5609): 1067–1070. Bibcode:2003Sci...299.1067R. doi:10.1126/science.1080972. PMID 12586941. S2CID 20488694. Archived (PDF) from the original on 2020-11-23.
  9. ^ Pieniazek, Piotr A.; Bradforth, Stephen E.; Krylov, Anna I. (2005-12-07). "Spectroscopy of the Cyano Radical in an Aqueous Environment" (PDF). The Journal of Physical Chemistry A. 110 (14): 4854–4865. Bibcode:2006JPCA..110.4854P. doi:10.1021/jp0545952. PMID 16599455. Archived from the original (PDF) on 2008-09-11. Retrieved 2008-08-23.
  10. ^ Roth, K. C.; Meyer, D. M.; Hawkins, I. (1993). "Interstellar Cyanogen and the Temperature of the Cosmic Microwave Background Radiation" (PDF). The Astrophysical Journal. 413 (2): L67–L71. Bibcode:1993ApJ...413L..67R. doi:10.1086/186961.
  11. ^ a b Anon (June 27, 2013). "Facts about cyanide:Where cyanide is found and how it is used". CDC Emergency preparedness and response. Centers for Disease Control and Prevention. Retrieved 10 December 2016.
  12. ^ IUPAC Gold Book nitriles
  13. ^ NCBI-MeSH Nitriles
  14. ^ a b c Rubo, Andreas; Kellens, Raf; Reddy, Jay; Steier, Norbert; Hasenpusch, Wolfgang (2006). "Alkali Metal Cyanides". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.i01_i01. ISBN 978-3527306732.
  15. ^ Pollak, Peter; Romeder, Gérard; Hagedorn, Ferdinand; Gelbke, Heinz-Peter (2000). "Nitriles". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_363. ISBN 3-527-30673-0.
  16. ^ Young, C. A., & Jordan, T. S. (1995, May). Cyanide remediation: current and past technologies. In: Proceedings of the 10th Annual Conference on Hazardous Waste Research (pp. 104–129). Kansas State University: Manhattan, KS. https://engg.ksu.edu/HSRC/95Proceed/young.pdf
  17. ^ Dmitry Yermakov. "Cyanide Destruction | SRK Consulting". srk.com. Retrieved 2 March 2021.
  18. ^ Botz Michael M. Overview of cyanide treatment methods. Elbow Creek Engineering, Inc. http://www.botz.com/MEMCyanideTreatment.pdf
  19. ^ Sharpe, A. G. The Chemistry of Cyano Complexes of the Transition Metals; Academic Press: London, 1976[page needed]
  20. ^ Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 978-0-12-352651-9.
  21. ^ Andrussow, Leonid (1927). "Über die schnell verlaufenden katalytischen Prozesse in strömenden Gasen und die Ammoniak-Oxydation (V)" [About the quicka catalytic processes in flowing gases and the ammonia oxidation (V)]. Berichte der Deutschen Chemischen Gesellschaft (in German). 60 (8): 2005–2018. doi:10.1002/cber.19270600857.
  22. ^ Andrussow, L. (1935). "Über die katalytische Oxydation von Ammoniak-Methan-Gemischen zu Blausäure" [About the catalytic oxidation of ammonia-methane mixtures to cyanide]. Angewandte Chemie (in German). 48 (37): 593–595. Bibcode:1935AngCh..48..593A. doi:10.1002/ange.19350483702.
  23. ^ Nelson, David L.; Cox, Michael M. (2000). Lehniger Principles of Biochemistry (3rd ed.). New York: Worth Publishers. pp. 668, 670–71, 676. ISBN 978-1-57259-153-0.
  24. ^ a b Biller, José (2007). "163". Interface of neurology and internal medicine (illustrated ed.). Lippincott Williams & Wilkins. p. 939. ISBN 978-0-7817-7906-7.
  25. ^ "MSDS of trimethylsilyl cyanide" (PDF). Gelest Inc. 2008. Archived (PDF) from the original on 2022-10-10. Retrieved 2022-08-16.
  26. ^ Cyanide Toxicity~treatment at eMedicine
  27. ^ Chaudhary, M.; Gupta, R. (2012). "Cyanide Detoxifying Enzyme: Rhodanese". Current Biotechnology. 1 (4): 327–335. doi:10.2174/2211550111201040327.
  28. ^ Toxicological Profile for Cyanide (PDF) (Report). U.S. Department of Health and Human Services. 2006. pp. 18–19. Archived (PDF) from the original on 2004-03-31.
  29. ^ Kumar, Rahul; Saha, Shouvik; Sarita, Dhaka; Mayur B., Kurade; Kang, Chan Ung; Baek, Seung Han; Jeong, Byong-Hun (2016). "Remediation of cyanide-contaminated environments through microbes and plants: a review of current knowledge and future perspectives". Geosystem Engineering. 70 (1): 28–40. doi:10.1080/12269328.2016.1218303. S2CID 132571397. Retrieved 24 April 2022.
  30. ^ Konyratbekova, Saltanat Sabitovna; Baikonurova, Aliya; Akcil, Ata (2015-05-04). "Non-cyanide Leaching Processes in Gold Hydrometallurgy and Iodine-Iodide Applications: A Review". Mineral Processing and Extractive Metallurgy Review. 36 (3): 198–212. doi:10.1080/08827508.2014.942813. ISSN 0882-7508.
  31. ^ Zhang, Yan; Cui, Mingyao; Wang, Jianguo; Liu, Xiaoliang; Lyu, Xianjun (2022). "A review of gold extraction using alternatives to cyanide: Focus on current status and future prospects of the novel eco-friendly synthetic gold lixiviants". Minerals Engineering. 176: 107336. doi:10.1016/j.mineng.2021.107336.
  32. ^ Takano, R. (August 1916). "The treatment of leprosy with cyanocuprol". The Journal of Experimental Medicine. 24 (2): 207–211. doi:10.1084/jem.24.2.207. PMC 2125457. PMID 19868035. Retrieved 2008-06-28.
  33. ^ Dzombak, David A; Ghosh, Rajat S; Wong-Chong, George M. Cyanide in Water and Soil. CRC Press, 2006, Chapter 11.2: "Use of Cyanide for Capturing Live Reef Fish".
  34. ^ Poachers kill 80 elephants with cyanide in Zimbabwe ABC News, 25 September 2013. Retrieved 30 October 2015.
  35. ^ Shivik, John A.; Mastro, Lauren; Young, Julie K. (2014). "Animal attendance at M-44 sodium cyanide ejector sites for coyotes". Wildlife Society Bulletin. 38 (1): 217–220. Bibcode:2014WSBu...38..217S. doi:10.1002/wsb.361.
  36. ^ Green, Wren (July 2004). "The use of 1080 for pest control" (PDF). New Zealand Department of Conservation. Retrieved 8 June 2011.
  37. ^ Shapiro, Lee; et al. (21 March 2011). "Effectiveness of cyanide pellets for control of dama wallabies (Macropus eugenii)" (PDF). New Zealand Journal of Ecology. 35 (3). Archived (PDF) from the original on 2015-02-03.
  38. ^ "Sodium Cyanide". PubChem. National Center for Biotechnology Information. 2016. Retrieved 2 September 2016. Cyanide and hydrogen cyanide are used in electroplating, metallurgy, organic chemicals production, photographic developing, manufacture of plastics, fumigation of ships, and some mining processes.
  39. ^ "Reregistration Eligibility Decision (RED) Sodium Cyanide" (PDF). EPA.gov. 1 September 1994. p. 7. Archived (PDF) from the original on 2022-10-10. Retrieved 2 September 2016. Sodium cyanide was initially registered as a pesticide on December 23, 1947, to control ants on uncultivated agricultural and non-agricultural areas.
  40. ^ "Tariff Information, 1921: Hearings on General Tariff Revision Before the Committee on Ways and Means, House of Representatives". AbeBooks.com. US Congress, House Committee on Ways and Means, US Government Printing Office. 1921. p. 3987. Retrieved 2 September 2016. Another field in which cyanide is used in growing quantity is the eradication of rats and other vermin – especially in the fight against typhus.
  41. ^ "Deadliest Poisons Used by Man". PlanetDeadly.com. 18 November 2013. Archived from the original on 11 May 2016. Retrieved 2 September 2016.
  42. ^ Taylorson, R.; Hendricks, SB (1973). "Promotion of Seed Germination by Cyanide". Plant Physiol. 52 (1): 23–27. doi:10.1104/pp.52.1.23. PMC 366431. PMID 16658492.
  43. ^ Mullick, P.; Chatterji, U. N. (1967). "Effect of sodium cyanide on germination of two leguminous seeds". Plant Systematics and Evolution. 114: 88–91. doi:10.1007/BF01373937. S2CID 2533762.
  44. ^ Bernan (2008). Medical Management of Chemical Casualties Handbook (4th ed.). Government Printing Off. p. 41. ISBN 978-0-16-081320-7., Extract p. 41
  45. ^ Bender, David A.; Bender, Arnold Eric (1997). Benders' dictionary of nutrition and food technology (7th ed.). Woodhead Publishing. p. 459. ISBN 978-1-85573-475-3. Extract of page 459
  46. ^ Schulz, Horst D.; Hadeler, Astrid; Deutsche Forschungsgemeinschaft (2003). Geochemical processes in soil and groundwater: measurement – modelling – upscaling. Wiley-VCH. p. 67. doi:10.1002/9783527609703. ISBN 978-3-527-27766-7.
  47. ^ Gail, Ernst; Gos, Stephen; Kulzer, Rupprecht; Lorösch, Jürgen; Rubo, Andreas; Sauer, Manfred (2004). "Cyano Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a08_159.pub2. ISBN 978-3527306732.
  48. ^ Schwenecke, H.; Mayer, D. (2005). "Benzidine and Benzidine Derivatives". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_539. ISBN 978-3527306732.
  49. ^ Ganjeloo, A; Isom, GE; Morgan, RL; Way, JL (1980). "Fluorometric determination of cyanide in biological fluids with p-benzoquinone*1". Toxicology and Applied Pharmacology. 55 (1): 103–107. doi:10.1016/0041-008X(80)90225-2. PMID 7423496.
[edit]
Wikisource has the text of the 1911 Encyclopædia Britannica article "Cyanide".
Wikimedia Commons has media related to Cyanides.
Safety data (French)
Retrieved from "https://en.wikipedia.org/w/index.php?title=Cyanide&oldid=1236512508"