| Cyanogen | |
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Ethanedinitrile |
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Other names
Cyanogen |
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| Identifiers | |
| CAS number | 460-19-5  |
| PubChem | 9999 |
| ChemSpider | 9605 |
| EC number | 207-306-5 |
| UN number | 1026 |
| ChEBI | CHEBI:29308 |
| RTECS number | GT1925000 |
| Jmol-3D images | Image 1 |
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| Properties | |
| Molecular formula | C2N2 |
| Molar mass | 52.03 g mol−1 |
| Density | 0.95 g/cm3 (liquid, −21 °C) |
| Melting point |
-28 °C, 245 K, -18 °F |
| Boiling point |
-21 °C, 252 K, -6 °F |
| Solubility in water | 450 mL/100 mL (20 °C) |
| Hazards | |
| MSDS | ICSC 1390 |
| EU Index | 608-011-00-8 |
| EU classification | Flammable (F) Very Toxic (T+) Dangerous for the environment (N) |
| R-phrases | R11, R23, R50/53 |
| S-phrases | (S1/2), S23, S45, S60, S61 |
| NFPA 704 |
 4
4
2
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| Flash point | Flammable gas |
| Explosive limits | 6.6–42.6% |
| Related compounds | |
| Related compounds | Cyanogen fluoride Cyanogen chloride Cyanogen bromide Cyanogen iodide |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
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.[1] Certain derivatives of cyanogen are also called "cyanogen" even though they contain only one CN group. For example cyanogen bromide has the formula NCBr.[2]
Cyanogen is the anhydride of oxamide:
- H2NC(O)C(O)NH2 → NCCN + 2 H2O
Contents |
Preparation [link]
Cyanogen is typically generated from cyanide compounds. One laboratory method entails thermal decomposition of mercuric cyanide:
- 2 Hg(CN)2 → (CN)2 + Hg2(CN)2
Alternatively, one can combine solutions of copper(II) salts (such as copper(II) sulfate) with cyanides, an unstable copper(II) cyanide is formed which rapidly decomposes into copper(I) cyanide and cyanogen.[3]
- 2 CuSO4 + 4 KCN → (CN)2 + 2 CuCN + 2 K2SO4
Industrially, it is created by the oxidation of hydrogen cyanide, usually using chlorine over an activated silicon dioxide catalyst or nitrogen dioxide over a copper salt. It is also formed when nitrogen and acetylene are reacted by an electrical spark or discharge.[4]
Paracyanogen [link]
Paracyanogen is produced by polymerization of cyanogen through pyrolysis of heavy metal cyanides.[5]
History [link]
Cyanogen was first synthesized in 1815 by Joseph Louis Gay-Lussac, who determined its empirical formula and named it. Gay-Lussac coined the word "cyanogène" from the Greek words κύανος (kyanos, blue) and γεννάω (gennao, I create), because cyanide was first isolated by the Swedish chemist Carl Wilhelm Scheele from the pigment "Prussian blue".[6] It attained importance with the growth of the fertilizer industry in the late nineteenth century and is still an important intermediate in the production of many fertilizers. It is also used as a stabilizer in the production of nitrocellulose.
Safety [link]
Like other inorganic cyanides, cyanogen is very toxic, as it readily undergoes reduction to cyanide, which poisons the cytochrome c oxidase complex, thus interrupting the mitochondrial electron transfer chain. Cyanogen gas is an irritant to the eyes and respiratory system. Inhalation can lead to headache, dizziness, rapid pulse, nausea, vomiting, loss of consciousness, convulsions, and death, depending on exposure.[7]
Cyanogen produces the second hottest known natural flame (after carbon subnitride) with a temperature of over 4525 °C when it burns in oxygen.[8]
See also [link]
References [link]
- ^ Ringer, A. L.; Sherrill, C. D.; King, R. A.; Crawford, T. D. (2008). "Low-lying singlet excited states of isocyanogen". International Journal of Quantum Chemistry 106 (6): 1137–1140. DOI:10.1002/qua.21586.
- ^ Hartman, W. W.; Dreger, E. E. (1943). "Cyanogen Bromide" (pdf). Organic Syntheses, Collected Volume 2: 150. https://www.orgsyn.org/orgsyn/pdfs/CV2P0150.pdf.
- ^ Brotherton, T. K.; Lynn, J. W. (1959). "The Synthesis And Chemistry Of Cyanogen". Chemical Reviews 59 (5): 841–883. DOI:10.1021/cr50029a003.
- ^ Breneman, A. A. (1889). Showing the Progress and Development of Processes for the manufacture of Cyanogen and its Derivates. "The Fixation of Atmospheric Nitrogen". Journal of the American Chemical Society 11 (1): 2–27. DOI:10.1021/ja02126a001.
- ^ "Paracyanogen". https://www.thefreedictionary.com/Paracyanogen.
- ^ Gay-Lussac, J. L. (1815). "Recherches sur l'acide prussique". Annales de Chimie 95: 136–231. https://books.google.com/books?id=m9s3AAAAMAAJ&pg=PA136.
- ^ Muir, G. D., ed. (1971). Hazards in the Chemical Laboratory. London: The Royal Institute of Chemistry.
- ^ Thomas, N.; Gaydon, A. G.; Brewer, L. (1952). "Cyanogen Flames and the Dissociation Energy of N2". The Journal of Chemical Physics 20 (3): 369–374. Bibcode 1952JChPh..20..369T. DOI:10.1063/1.1700426.
External links [link]
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Wikimedia Commons has media related to: cyanogen |
https://wn.com/Cyanogen
Cyanogen (disambiguation)
Cyanogen is a chemical compound.
Cyanogen may also refer to:
Podcasts:
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by Cinjun
Blue Flashing Light
by: CinjunSaturday evening
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Thinking how you can settle the score
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Blue flashing light last Saturday night
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Are we all just afraid of the heat
But it's Saturday night and I'm lying alone
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