سيانوجين
سيانوجين Cyanogen هو مركب كيميائي صيغته (CN)2. أبسط نتريد الكربون، وهو غاز عديم اللون وشديد السمية برائحة حريفة/حرّاقة. الجزيء هو 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.[6] The name is also used for the CN radical,[7] and hence is used for compounds such as cyanogen bromide (NCBr)[8] (but see also Cyano radical.)
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| الأسماء | |||
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| اسم أيوپاك المفضل
Oxalonitrile[4] | |||
| اسم أيوپاك النظامي
Ethanedinitrile[4] | |||
| أسماء أخرى | |||
| Identifiers | |||
| رقم CAS | |||
3D model (JSmol)
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| مرجع بايلستاين | 1732464 | ||
| ChEBI | |||
| ChemSpider | |||
| ECHA InfoCard | 100.006.643 
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| رقم EC |
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| مرجع Gmelin | 1090 | ||
| عناوين مواضيع طبية MeSH | |||
PubChem CID
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| رقم RTECS |
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| UNII | |||
| UN number | 1026 | ||
CompTox Dashboard (EPA)
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| InChI | InChI={{{value}}} | ||
| SMILES | |||
| الخصائص | |||
| الصيغة الجزيئية | C2N2 | ||
| كتلة مولية | 52.03 g mol-1 | ||
| المظهر | Colourless gas | ||
| الرائحة | pungent, almond-like | ||
| الكثافة | 950 mg mL−1 (at −21 °C) | ||
| نقطة الانصهار | |||
| نقطة الغليان | |||
| قابلية الذوبان في الماء | 45 g/100 mL (at 20 °C) | ||
| قابلية الذوبان | soluble in ethanol, ethyl ether | ||
| ضغط البخار | 5.1 atm (21 °C)[5] | ||
| kH | 1.9 μmol Pa−1 kg−1 | ||
| القابلية المغناطيسية | -21.6·10−6 cm3/mol | ||
| معامل الانكسار (nD) | 1.327 (18 °C) | ||
| الكيمياء الحرارية | |||
| الإنتالپية المعيارية للتشكل ΔfH |
309.07 kJ mol−1 | ||
| الانتالبية المعيارية للاحتراق ΔcH |
−1.0978–−1.0942 MJ mol−1 | ||
| Standard molar entropy S |
241.57 J K−1 mol−1 | ||
| المخاطر | |||
| خطر رئيسي | forms cyanide in the body; flammable[5] | ||
| صفحة بيانات السلامة | inchem.org | ||
| ن.م.ع. مخطط تصويري |   
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| ن.م.ع. كلمة الاشارة | Danger | ||
| H220, H331, H410 | |||
| P210, P261, P271, P273, P304+P340, P311, P321, P377, P381, P391, P403, P403+P233, P405, P501 | |||
| NFPA 704 (معيـَّن النار) | |||
| حدود الانفجار | 6.6–32%[5] | ||
| حدود التعرض الصحية بالولايات المتحدة (NIOSH): | |||
PEL (المسموح)
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none[5] | ||
REL (الموصى به)
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TWA 10 ppm (20 mg/m3)[5] | ||
IDLH (خطر عاجل)
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N.D.[5] | ||
| مركبات ذا علاقة | |||
alkanenitriles ذات العلاقة
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مركـّبات ذات علاقة
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DBNPA | ||
ما لم يُذكر غير ذلك، البيانات المعطاة للمواد في حالاتهم العيارية (عند 25 °س [77 °ف]، 100 kPa). | |||
 verify (what is   ?)
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| مراجع الجدول | |||
Cyanogen is the anhydride of oxamide:
- H2NC(O)C(O)NH2 → NCCN + 2 H2O
although oxamide is manufactured from cyanogen by hydrolysis:[9]
- NCCN + 2 H2O → H2NC(O)C(O)NH2
. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
التحضير
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.[10]
- 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.[11]
المتزامرات
السيانوجين هو NCCN. وهناك متزامرات أقل استقراراً يختلف فيها ترتيب الذرات. Isocyanogen (أو cyanoisocyanogen) هو NCNC, diisocyanogen هو CNNC، و diazodicarbon[بحاجة لمصدر] هو CCNN.
Paracyanogen
Paracyanogen is a polymer of cyanogen. It can be best prepared by heating mercuric cyanide. It can also be prepared by heating silver cyanide, silver cyanate, cyanogen iodide or cyanuric iodide.[12] It can also be prepared by the polymerization of cyanogen at 300 to 500 °C (572 to 932 °F) in the presence of trace impurities. Paracyanogen can also be converted back to cyanogen by heating to 800 °C (1,470 °F).[9] Based on experimental evidence, the structure of this polymeric material is thought to be rather irregular, with most of the carbon atoms being of sp2 type and localized domains of π conjugation.[13]
التاريخ
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 κυανός (kyanos, blue) and γεννάω (gennao, I create), because cyanide was first isolated by the Swedish chemist Carl Wilhelm Scheele from the pigment "Prussian blue".[14] By the 1850s, cyanogen soap was used by photographers to remove silver stains from their hands.[15] It attained importance with the growth of the fertilizer industry in the late 19th century and remains an important intermediate in the production of many fertilizers. It is also used as a stabilizer in the production of nitrocellulose.
Cyanogen is commonly found in comets.[16] In 1910 a spectroscopic analysis of Halley's Comet found cyanogen in the comet's tail, which led to public fear that the Earth would be poisoned as it passed through the tail. People in New York wore gas masks, and merchants sold quack-treatment "comet pills" claimed to neutralise poisoning.[16] Because of the extremely diffuse nature of the tail, there was no effect when the planet passed through it.[17][18]
السلامة
Like other 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.[19] Lethal dose through inhalation typically ranges from 100 to 150 milligrams (1.5 to 2.3 grains).
Cyanogen produces the second-hottest-known natural flame (after carbon subnitride) with a temperature of over 4,525 °C (8,177 °F) when it burns in oxygen.[20][21]
في الثقافة الشعبية
In the Doctor Who serial "The Brain of Morbius" (the 5th serial of season 13), the Doctor synthesizes cyanogen using hydrogen cyanide as a starting material and vents it through a pipe to stop Solon from performing surgery on the brain of Morbius's body, however he completes it but shortly after dies of cyanogen poisoning.
In Dragnet (1987) Friday (Dan Aykroyd) and Streebek (Tom Hanks) are tracking down the villain who stole "the pseudohalogenic compound cyanogen".[22]
انظر أيضاً
المراجع
- ^ "oxalonitrile (CHEBI:29308)". Chemical Entities of Biological Interest. UK: European Bioinformatics Institute. 27 October 2006. Main. Retrieved 6 June 2012.
- ^ أ ب NIOSH Pocket Guide to Chemical Hazards. Department of Health and Human Services, Centers for Disease Control, National Institute for Occupational Safety & Health. September 2007. p. 82.
- ^ أ ب The Merck Index (10th ed.). Rahway, NJ: Merck & Co. 1983. p. 385. ISBN 9780911910278.
- ^ أ ب "Front Matter". Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 902. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4.
- ^ أ ب ت ث ج ح NIOSH Pocket Guide to Chemical Hazards 0161
- ^ 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. Bibcode:2008IJQC..108.1137R. doi:10.1002/qua.21586.
- ^ Irvine, William M. (2011). "Cyanogen Radical". Encyclopedia of Astrobiology. p. 402. doi:10.1007/978-3-642-11274-4_1806. ISBN 978-3-642-11271-3.
- ^ قالب:OrgSynth
- ^ أ ب Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 320–321. ISBN 978-0-08-037941-8.
- ^ 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. (January 1889). "The Fixation of Atmospheric Nitrogen". Journal of the American Chemical Society. 11 (1): 2–27. doi:10.1021/ja02126a001.
- ^ Bircumshaw, L. L.; F. M. Tayler; D. H. Whiffen (1954). "Paracyanogen: its formation and properties. Part I". J. Chem. Soc.: 931–935. doi:10.1039/JR9540000931.
- ^ Maya, Leon (1993). "Paracyanogen Reexamined". Journal of Polymer Science Part A (Submitted manuscript). 31 (10): 2595–2600. Bibcode:1993JPoSA..31.2595M. doi:10.1002/pola.1993.080311020.
- ^ Gay-Lussac, J. L. (1815). "Recherches sur l'acide prussique". Annales de Chimie. 95: 136–231. Gay-Lussac names cyanogen on p. 163.
- ^ Crookes, William, ed. (1859). "Photographic News: A Weekly Record of the Process of the Photography": 11.
{{cite journal}}: Cite journal requires|journal=(help) - ^ أ ب Cometary Poison Gas Geyser Heralds Surprises NASA, 2010-11-02.
- ^ Comet's Poisonous Tail.
- ^ Halley's Comet 100 years ago.
- ^ 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.
- ^ J. B. Conway; R. H. Wilson Jr.; A. V. Grosse (1953). "The Temperature of the Cyanogen-Oxygen Flame". Journal of the American Chemical Society. 75 (2): 499. doi:10.1021/ja01098a517.
- ^ "The trichlornitromethane and the pseudo-halogenic compound cyanogen". Retrieved August 18, 2021.
وصلات خارجية
