Cyanide

A cyanide is a chemical compound that contains the group C≡N. 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 anion CN. For the salts such as sodium cyanide and potassium cyanide, these compounds 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 CN group is linked by a covalent bond to carbon. For example, in acetonitrile, the cyanide group is bonded to methyl (CH3). Because they do not release cyanide ions, nitriles are generally far less toxic than cyanide salts. Some nitriles, which occur naturally as cyanohydrins, release hydrogen cyanide.

Cyanide anion
Ball-and-stick model of the cyanide anion
Names
Systematic IUPAC name
Cyanide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
UNII
Properties
CN
Molar mass 26.018 g·mol−1
Conjugate acid Hydrogen cyanide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Nomenclature and etymology

Cyanide-montage
The cyanide ion, CN.
From the top:
1. Valence-bond structure
2. Space-filling model
3. Electrostatic potential surface
4. "Carbon lone pair"

In IUPAC nomenclature, organic compounds that have a –C≡N functional group are called nitriles. Thus, nitriles are organic compounds.[3][4] An example of a nitrile is CH3CN, acetonitrile, also known as methyl cyanide. Nitriles usually do not release cyanide ions. A functional group with a hydroxyl and cyanide bonded to the same carbon is called cyanohydrin. Unlike nitriles, cyanohydridins do release hydrogen cyanide. In inorganic chemistry, salts containing the C≡N ion are referred to as cyanides.

The word is derived from the Greek kyanos, meaning dark blue, as a result of its being first obtained by the heating of the pigment known as Prussian blue.

Bonding

The cyanide ion is isoelectronic with carbon monoxide and with molecular nitrogen.[5][6]

Occurrence and reactions

In nature

Removal of cyanide poison from cassava
Removal of cyanide from cassava in Nigeria.

Cyanides are produced by certain bacteria, fungi, and algae and are found 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.[7] 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.[8][9]

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.

Interstellar medium

The cyanide radical ·CN has been identified in interstellar space.[10] The cyanide radical (called cyanogen) is used to measure the temperature of interstellar gas clouds.[11]

Pyrolysis and combustion product

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.[12]

Coordination chemistry

The cyanide anion is a ligand for many transition metals.[13] The high affinities of metals for this anion can be attributed to its negative charge, compactness, and ability to engage in π-bonding. Well-known complexes include:

  • hexacyanides [M(CN)6]3− (M = Ti, V, Cr, Mn, Fe, Co), which are octahedral in shape.
  • the tetracyanides, [M(CN)4]2− (M = Ni, Pd, Pt), which are square planar in their geometry;
  • the dicyanides [M(CN)2] (M = Cu, Ag, Au), which are linear in geometry.

Among the most important cyanide coordination compounds are the octahedrally coordinated compounds 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.[14] 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.

The enzymes called hydrogenases 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.[15]

Organic derivatives

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. Thus, CH3CN can be called methyl cyanide but more commonly is referred to as acetonitrile. 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.

RX + CN → RCN + X (nucleophilic substitution) followed by
  1. RCN + 2 H2O → RCOOH + NH3 (hydrolysis under reflux with mineral acid catalyst), or
  2. 2 RCN + LiAlH4 + (second step) 4 H2O → 2 RCH2NH2 + LiAl(OH)4 (under reflux in dry ether, followed by addition of H2O)

Manufacture

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.[16][17]

2 CH4 + 2 NH3 + 3 O2 → 2 HCN + 6 H2O

Gaseous hydrogen cyanide may be dissolved in aqueous sodium hydroxide solution to produce sodium cyanide.

Toxicity

Many cyanides are highly toxic. The cyanide anion is an inhibitor of the enzyme cytochrome c oxidase (also known as aa3) in the fourth complex of the electron transport chain (found in the 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.[18] 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.[19]

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.[12] 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 as little as 200 mg, or exposure to airborne cyanide of 270 ppm, is sufficient to cause death within minutes.[19]

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.

Antidote

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.[20]

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.[21]

Sensitivity

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.[22]

Applications

Mining

Cyanide is mainly produced for the mining of gold and silver: It helps dissolve these metals and their ores. In the cyanide process, finely ground high-grade ore is mixed with the cyanide (concentration of about two kilogram NaCN per tonne); low-grade ores are stacked into heaps and sprayed with a cyanide solution (concentration of about one kilogram NaCN per ton). The precious metals are complexed by the cyanide anions to form soluble derivatives, e.g., [Au(CN)2] and [Ag(CN)2].[23]

4 Au + 8 NaCN + O2 + 2 H2O → 4 Na[Au(CN)2] + 4 NaOH

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:

Ag2S + 4 NaCN + H2O → 2 Na[Ag(CN)2] + NaSH + NaOH

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 resulting in numerous cases of human and aquatic species mortality.

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.

Cyanide is also used in electroplating, where it stabilizes metal ions in the electrolyte solution prior to their deposition.

Industrial organic chemistry

Some nitriles are produced on a large scale, e.g., adiponitrile is a precursor to nylon. Such compounds are often generated by combining hydrogen cyanide and alkenes, i.e., hydrocyanation: RCH=CH2 + HCN → RCH(CN)CH3. Metal catalysts are required for such reactions.

Medical uses

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.[24]

Illegal fishing and poaching

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.[25]

Poachers in Africa have been known to use cyanide to poison waterholes, to kill elephants for their ivory.[26]

Pest control

M44 cyanide devices are used in the United States to kill coyotes and other canids.[27] 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.[28] Cyanide is also effective for controlling the dama wallaby, another introduced marsupial pest in New Zealand.[29] A licence is required to store, handle and use cyanide in New Zealand.

Niche uses

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.

Cyanides are used as insecticides for fumigating ships.[30] Cyanide salts are used for killing ants,[31] and have in some places been used as rat poison[32] (the less toxic poison arsenic is more common).[33]

Although usually thought to be toxic, cyanide and cyanohydrins have been demonstrated to increase germination in various plant species.[34][35]

Human poisoning

Deliberate cyanide poisoning of humans has occurred many times throughout history.[36] For notable cyanide deaths, see Cyanide poisoning: History.

Most significantly, hydrogen cyanide released from pellets of Zyklon-B was used extensively in the systematic mass murders of the Holocaust, especially in extermination camps. Poisoning by hydrogen cyanide gas within a gas chamber (as a salt of hydrocyanic acid is dropped into a strong acid, usually sulfuric acid) is one method of executing a condemned prisoner as the condemned prisoner eventually breathes the lethal fumes.

Food additive

Due to the high stability of their complexation with iron, ferrocyanides (Sodium ferrocyanide E535, Potassium ferrocyanide E536, and Calcium ferrocyanide E538[37]) 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.[38]

Chemical tests for cyanide

Prussian blue

Iron(II) sulfate is added to a solution suspected of containing cyanide, such as the filtrate from the sodium fusion test. The resulting mixture is acidified with mineral acid. The formation of Prussian blue is a positive result for cyanide.

para-Benzoquinone in DMSO

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.[39]

Copper and an aromatic amine

As used by fumigators to detect hydrogen cyanide, copper(II) salt and an aromatic amine such as benzidine is added to the sample; as an alternative to benzidine an alternative amine di-(4,4-bis-dimethylaminophenyl) methane can be used. A positive test gives a blue color. Copper(I) cyanide is poorly soluble. By sequestering the copper(I) the copper(II) is rendered a stronger oxidant. The copper, in a cyanide facilitated oxidation, converts the amine into a colored compound. The Nernst equation explains this process. Another good example of such chemistry is the way in which the saturated calomel reference electrode (SCE) works. The copper, in a cyanide-facilitated oxidation, converts the amine into a colored compound.

Pyridine-barbituric acid colorimetry

A sample containing inorganic cyanide is purged with air from a boiling acid solution into a basic absorber solution. The cyanide salt absorbed in the basic solution is buffered at pH 4.5 and then reacted with chlorine to form cyanogen chloride. The cyanogen chloride formed couples pyridine with barbituric acid to form a strongly colored red dye that is proportional to the cyanide concentration. This colorimetric method following distillation is the basis for most regulatory methods (for instance EPA 335.4) used to analyze cyanide in water, wastewater, and contaminated soils. Distillation followed by colorimetric methods, however, have been found to be prone to interferences from thiocyanate, nitrate, thiosulfate, sulfite, and sulfide that can result in both positive and negative bias. It has been recommended by the USEPA (MUR March 12, 2007) that samples containing these compounds be analyzed by Gas-Diffusion Flow Injection Analysis—Amperometry.

Corrinoids colorimetry

A solution of aquacyano-corrinoids, such as cobalamin or cobinamide, reacts with free cyanide in an aqueous sample. The binding of cyanide to the corrinoid cobalt center leads to a color change from orange to violet,[40] allowing for semi-quantification by naked-eye. Precise quantification of the cyanide content is feasible by UV-vis spectroscopy.[41][42] Absorption of the corrinoid on a solid phase,[43] allows detection of cyanide even in colored samples, rendering this method appropriate for the analysis of cyanide in water, wastewater, blood, and food.[44][45] Furthermore, this technology is non-toxic and considerably less prone to interference than the pyridine-barbituric acid colorimetry method.

Gas diffusion flow injection analysis—amperometry

Instead of distilling, the sample is injected into an acidic stream where the HCN formed is passed under a hydrophobic gas diffusion membrane that selectively allows only HCN to pass through. The HCN that passes through the membrane is absorbed into a basic carrier solution that transports the CN to an amperometric detector that accurately measures cyanide concentration with high sensitivity. Sample pretreatment determined by acid reagents, ligands, or preliminary UV irradiation allow cyanide speciation of free cyanide, available cyanide, and total cyanide respectively. The relative simplicity of these flow injection analysis methods limit the interference experienced by the high heat of distillation and also prove to be cost effective since time consuming distillations are not required.

References

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  3. ^ IUPAC Gold Book nitriles
  4. ^ NCBI-MeSH Nitriles
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  15. ^ 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". Science. 299 (5609): 1067–70. Bibcode:2003Sci...299.1067R. doi:10.1126/science.1080972. PMID 12586941.
  16. ^ 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): 2005–18. doi:10.1002/cber.19270600857.
  17. ^ 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): 593–5. doi:10.1002/ange.19350483702.
  18. ^ 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.
  19. ^ a b Biller, José (2007). Interface of neurology and internal medicine (illustrated ed.). Lippincott Williams & Wilkins. p. 939. ISBN 978-0-7817-7906-7., Chapter 163, page 939
  20. ^ Cyanide Toxicity~treatment at eMedicine
  21. ^ Chaudhary, M.; Gupta, R. "Cyanide Detoxifying Enzyme: Rhodanese" Current Biotechnology, 2012, vol. 1, pp. 327-335. doi:10.2174/2211550111201040327
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  23. ^ Rubo, Andreas; Kellens, Raf; Reddy, Jay; Steier, Norbert; Hasenpusch, Wolfgang (2006). "Alkali metal cyanides". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.i01_i01. ISBN 978-3527306732.
  24. ^ 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.
  25. ^ 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".
  26. ^ Poachers kill 80 elephants with cyanide in Zimbabwe ABC News, 25 September 2013. Retrieved 30 October 2015.
  27. ^ Shivik, John A.; Mastro, Lauren; Young, Julie K. (2014). "Animal attendance at M-44 sodium cyanide ejector sites for coyotes". Wildlife Society Bulletin. 38: 217–220. doi:10.1002/wsb.361.
  28. ^ Green, Wren (July 2004). "The use of 1080 for pest control" (PDF). New Zealand Department of Conservation. Retrieved 8 June 2011.
  29. ^ 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).
  30. ^ "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.
  31. ^ "Reregistration Eligibility Decision (RED) Sodium Cyanide" (PDF). EPA.gov. 1 September 1994. p. 7. 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.
  32. ^ "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.
  33. ^ "Deadliest Poisons Used by Man". PlanetDeadly.com. 18 November 2013. Archived from the original on 11 May 2016. Retrieved 2 September 2016.
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  36. ^ Bernan (2008). Medical Management of Chemical Casualties Handbook (4 ed.). Government Printing Off. p. 41. ISBN 978-0-16-081320-7., Extract p. 41
  37. ^ Bender, David A.; Bender, Arnold Eric (1997). Benders' dictionary of nutrition and food technology (7 ed.). Woodhead Publishing. p. 459. ISBN 978-1-85573-475-3. Extract of page 459
  38. ^ Schulz, Horst D.; Hadeler, Astrid; Deutsche Forschungsgemeinschaft (2003). Geochemical processes in soil and groundwater: measurement—modelling—upscaling. Wiley-VCH. p. 67. ISBN 978-3-527-27766-7. Extract of page 67
  39. ^ 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): 103–7. doi:10.1016/0041-008X(80)90225-2. PMID 7423496.
  40. ^ Pratt, J.M. (1972). Inorganic Chemistry of Vitamin B12. Academic Press. p. 44.
  41. ^ Zelder, F.H. (2008). "Specific Colorimetric Detection of Cyanide Triggered by a Conformational Switch in Vitamin B12". Inorganic Chemistry. 47 (4): 1264–1266. doi:10.1021/ic702368b. PMID 18205304.
  42. ^ Mannel-Croise, Zelder (2009). "Side chains of cobalt corrinoids control the sensitivity and selectivity in the colorimetric detection of cyanide". Inorganic Chemistry. 48 (4): 1272–1274. doi:10.1021/ic900053h. PMID 19161297.
  43. ^ Mannel-Croise, Zelder (2012). "Complex samples cyanide detection with immobilized corrinoids". ACS Applied Materials & Interfaces. 4 (2): 725–729. doi:10.1021/am201357u. PMID 22211318.
  44. ^ Tivana, Da Cruz Francisco, Zelder, Bergenståhl, Dejmek (2014). "Straightforward rapid spectrophotometric quantification of total cyanogenic glycosides in fresh and processed cassava products" (PDF). Food Chemistry. 158: 20–27. doi:10.1016/j.foodchem.2014.02.066. PMID 24731309.CS1 maint: Multiple names: authors list (link)
  45. ^ Mannel-Croise, Zelder (2012). "Rapid visual detection of blood cyanide" (PDF). Analytical Methods. 4 (9): 2632–2634. doi:10.1039/c2ay25595b.

External links

Safety data (French):

Acetonitrile

Acetonitrile is the chemical compound with the formula CH3CN. This colourless liquid is the simplest organic nitrile (hydrogen cyanide is a simpler nitrile, but the cyanide anion is not classed as organic). It is produced mainly as a byproduct of acrylonitrile manufacture. It is used as a polar aprotic solvent in organic synthesis and in the purification of butadiene.In the laboratory, it is used as a medium-polarity solvent that is miscible with water and a range of organic solvents, but not saturated hydrocarbons. It has a convenient liquid range and a high dielectric constant of 38.8. With a dipole moment of 3.92 D, acetonitrile dissolves a wide range of ionic and nonpolar compounds and is useful as a mobile phase in HPLC and LC–MS. The N≡C−C skeleton is linear with a short C≡N distance of 1.16 Å.Acetonitrile was first prepared in 1847 by the French chemist Jean-Baptiste Dumas.

Amygdalin

Amygdalin (from Ancient Greek: ἀμυγδαλή amygdálē "almond") is a naturally occurring chemical compound, famous for falsely being promoted as a cancer cure. It is found in many plants, but most notably in the seeds (kernels) of apricot, bitter almonds, apple, peach, and plum.

Amygdalin is classified as a cyanogenic glycoside because each amygdalin molecule includes a nitrile group, which can be released as the toxic cyanide anion by the action of a beta-glucosidase: eating amygdalin will cause it to release cyanide in the human body, and may lead to cyanide poisoning.Since the early 1950s, both amygdalin and a modified form named laetrile have been promoted as alternative cancer treatments, often using the misnomer vitamin B17. But studies have found them to be clinically ineffective in the treatment of cancer, as well as potentially toxic or lethal when taken by mouth, due to cyanide poisoning. The promotion of laetrile to treat cancer has been described in the medical literature as a canonical example of quackery, and as "the slickest, most sophisticated, and certainly the most remunerative cancer quack promotion in medical history". Neither amygdalin nor laetrile is a vitamin.

Cassava

Manihot esculenta, commonly called cassava (), manioc, yuca, macaxeira, mandioca, aipim and Brazilian arrowroot, is a woody shrub native to South America of the spurge family, Euphorbiaceae. It is extensively cultivated as an annual crop in tropical and subtropical regions for its edible starchy tuberous root, a major source of carbohydrates. Though it is often called yuca in Spanish and in the United States, it is not related to yucca, a shrub in the family Asparagaceae. Cassava, when dried to a powdery (or pearly) extract, is called tapioca; its fried, granular form is named garri.

Cassava is the third-largest source of food carbohydrates in the tropics, after rice and maize. Cassava is a major staple food in the developing world, providing a basic diet for over half a billion people. It is one of the most drought-tolerant crops, capable of growing on marginal soils. Nigeria is the world's largest producer of cassava, while Thailand is the largest exporter of dried cassava.

Cassava is classified as either sweet or bitter. Like other roots and tubers, both bitter and sweet varieties of cassava contain antinutritional factors and toxins, with the bitter varieties containing much larger amounts. It must be properly prepared before consumption, as improper preparation of cassava can leave enough residual cyanide to cause acute cyanide intoxication, goiters, and even ataxia, partial paralysis, or death. The more toxic varieties of cassava are a fall-back resource (a "food security crop") in times of famine or food insecurity in some places. Farmers often prefer the bitter varieties because they deter pests, animals, and thieves.

Cyanide

A cyanide is a chemical compound that contains the group C≡N. This group, known as the cyano group, consists of a carbon atom triple-bonded to a nitrogen atom.In inorganic cyanides, the cyanide group is present as the anion CN−. For the salts such as sodium cyanide and potassium cyanide, these compounds are highly toxic. 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 CN group is linked by a covalent bond to carbon. For example, in acetonitrile, the cyanide group is bonded to methyl (CH3). Because they do not release cyanide ions, nitriles are generally far less toxic than cyanide salts. Some nitriles, which occur naturally as cyanohydrins, release hydrogen cyanide.

Cyanide poisoning

Cyanide poisoning is poisoning that results from exposure to a number of forms of cyanide. Early symptoms include headache, dizziness, fast heart rate, shortness of breath, and vomiting. This may then be followed by seizures, slow heart rate, low blood pressure, loss of consciousness, and cardiac arrest. Onset of symptoms is usually within a few minutes. If a person survives, there may be long-term neurological problems.Toxic cyanide-containing compounds include hydrogen cyanide gas and a number of cyanide salts. Poisoning is relatively common following breathing in smoke from a house fire. Other potential routes of exposure include workplaces involved in metal polishing, certain insecticides, the medication nitroprusside, and certain seeds such as those of apples and apricots. Liquid forms of cyanide can be absorbed through the skin. Cyanide ions interfere with cellular respiration, resulting in the body's tissues being unable to use oxygen.Diagnosis is often difficult. It may be suspected in a person following a house fire who has a decreased level of consciousness, low blood pressure, or high blood lactate. Blood levels of cyanide can be measured but take time. Levels of 0.5–1 mg/L are mild, 1–2 mg/L are moderate, 2–3 mg/L are severe, and greater than 3 mg/L generally result in death.If exposure is suspected, the person should be removed from the source of exposure and decontaminated. Treatment involves supportive care and giving the person 100% oxygen. Hydroxocobalamin (vitamin B12a) appears to be useful as an antidote and is generally first-line. Sodium thiosulphate may also be given. Historically cyanide has been used for mass suicide and by the Nazis for genocide.

Cyanogen

Cyanogen is the chemical compound with the formula (CN)2. It is a colorless, toxic gas with a pungent odor. The molecule is a pseudohalogen. Cyanogen molecules consist of two CN groups – analogous to diatomic halogen molecules, such as Cl2, but far less oxidizing. The two cyano groups are bonded together at their carbon atoms: N≡C−C≡N, although other isomers have been detected. The name is also used for the CN radical, and hence is used for compounds such as cyanogen bromide (NCBr).Cyanogen is the anhydride of oxamide:

H2NC(O)C(O)NH2 → NCCN + 2 H2Oalthough oxamide is manufactured from cyanogen by hydrolysis:

NCCN + 2 H2O → H2NC(O)C(O)NH2

Gas chamber

A gas chamber is an apparatus for killing humans or other animals with gas, consisting of a sealed chamber into which a poisonous or asphyxiant gas is introduced. The most commonly used poisonous agent is hydrogen cyanide; carbon dioxide and carbon monoxide have also been used. Gas chambers were used as a method of execution for condemned prisoners in the United States beginning in the 1920s and continue to be a legal execution method in three states. During the Holocaust, large-scale gas chambers designed for mass killing were used by Nazi Germany as part of their genocide program. The use of gas chambers in North Korea has also been reported.

Hydrogen cyanide

Hydrogen cyanide (HCN), sometimes called prussic acid, is a chemical compound with the chemical formula HCN. It is a colorless, extremely poisonous and flammable liquid that boils slightly above room temperature, at 25.6 °C (78.1 °F). HCN is produced on an industrial scale and is a highly valuable precursor to many chemical compounds ranging from polymers to pharmaceuticals.

Nitrile

A nitrile is any organic compound that has a −C≡N functional group. The prefix cyano- is used interchangeably with the term nitrile in industrial literature. Nitriles are found in many useful compounds, including methyl cyanoacrylate, used in super glue, and nitrile rubber, a nitrile-containing polymer used in latex-free laboratory and medical gloves. Nitrile rubber is also widely used as automotive and other seals since it is resistant to fuels and oils. Organic compounds containing multiple nitrile groups are known as cyanocarbons.

Inorganic compounds containing the −C≡N group are not called nitriles, but cyanides instead. Though both nitriles and cyanides can be derived from cyanide salts, most nitriles are not nearly as toxic.

Potassium cyanide

Potassium cyanide is a compound with the formula KCN. This colorless crystalline salt, similar in appearance to sugar, is highly soluble in water. Most KCN is used in gold mining, organic synthesis, and electroplating. Smaller applications include jewelry for chemical gilding and buffing.Potassium cyanide is highly toxic. The moist solid emits small amounts of hydrogen cyanide due to hydrolysis, which smells like bitter almonds. Not everyone, however, can smell this; the ability to do so is a genetic trait.The taste of potassium cyanide has been described as acrid with a burning sensation.

Sodium cyanide

Sodium cyanide is an inorganic compound with the formula NaCN. It is a white, water-soluble solid. Cyanide has a high affinity for metals, which leads to the high toxicity of this salt. Its main application, in gold mining, also exploits its high reactivity toward metals. It is a strong base. When treated with acid, it forms the toxic gas hydrogen cyanide:

NaCN + H2SO4 → HCN + NaHSO4

Zyklon B

Zyklon B (German: [tsyˈkloːn ˈbeː] (listen); translated Cyclone B) was the trade name of a cyanide-based pesticide invented in Germany in the early 1920s. It consisted of hydrogen cyanide (prussic acid), as well as a cautionary eye irritant and one of several adsorbents such as diatomaceous earth. The product is infamous for its use by Nazi Germany during the Holocaust to murder approximately one million people in gas chambers installed at Auschwitz-Birkenau, Majdanek, and other extermination camps.

Hydrogen cyanide, a poisonous gas that interferes with cellular respiration, was first used as a pesticide in California in the 1880s. Research at Degesch of Germany led to the development of Zyklon (later known as Zyklon A), a pesticide which released hydrogen cyanide upon exposure to water and heat. It was banned after a similar product was used by Germany as a chemical weapon in World War I. In 1922, Degesch was purchased by Degussa, where a team of chemists that included Walter Heerdt and Bruno Tesch developed a method of packaging hydrogen cyanide in sealed canisters along with a cautionary eye irritant and one of several adsorbents such as diatomaceous earth. The new product was also named Zyklon, but it became known as Zyklon B to distinguish it from the earlier version. Uses included delousing clothing and fumigating ships, warehouses, and trains.

In early 1942, Zyklon B emerged as the preferred killing tool of Nazi Germany for use in extermination camps during the Holocaust. Around a million people were killed using this method, mostly at Auschwitz. Tesch was executed in 1946 for knowingly selling the product to the SS for use on humans. Hydrogen cyanide is now rarely used as a pesticide, but still has industrial applications. Firms in several countries continue to produce Zyklon B under alternative brand names, including Detia-Degesch, the successor to Degesch, who renamed the product Cyanosil in 1974.

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