| 词条 | Acetyl cyanide |
| 释义 |
| Watchedfields = changed | verifiedrevid = 443418328 | Name = Acetyl cyanide | ImageFile = Acetyl cyanide.png | ImageSize = 120px | ImageName = Acetyl cyanide | PIN = Acetyl cyanide[1] | SystematicName = Ethanoyl cyanide | OtherNames = 2-Oxopropanenitrile[1] Pyruvonitrile Propanenitrile 2-oxo- α-Oxopropionitrile Oxopropionitrile Oxypropionitrile Pyruvic acid nitrile 2-Oxopropionitrile 2-Oxopropiononitrile |Section1={{Chembox Identifiers | SMILES = CC(=O)C#N | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/C3H3NO/c1-3(5)2-4/h1H3 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = QLDHWVVRQCGZLE-UHFFFAOYSA-N | CASNo = 631-57-2 | CASNo_Ref = {{cascite|correct|CAS}} | EC_number = 211-159-2 | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 62638 | PubChem = 69430 | Beilstein = 1737633 | UNII = ULO441649V |Section2={{Chembox Properties | C=3 | H=3 | N=1 | O=1 | Appearance = Clear, yellow liquid | Density = 0.9745 g/cm3 | BoilingPtC = 92.3 | Solvent = eth, ace, CH3CN | VaporPressure = 51.9300003051758 mmHg | RefractIndex = 1.3764 | SpecificSurfaceArea = 40.86 Å2 |Section4={{Chembox Thermochemistry }} |Section7={{Chembox Hazards | FlashPtC = 14.44 | ExternalSDS = External MSDS | MainHazards = | NFPA-H = 2 | NFPA-F = 3 | NFPA-R = 0 | NFPA-S = | FlashPt = | AutoignitionPt = | ExploLimits = | LD50 = | SkinHazard = May be harmful if absorbed through skin. Causes skin irritation. | EyeHazard = Causes eye irritation. | InhalationHazard = Toxic if inhaled. Causes respiratory tract irritation. | IngestionHazard = Toxic if swallowed. | GHSPictograms = {{GHS flame}} {{GHS skull and crossbones}} | GHSSignalWord = Danger | HPhrases = {{H-phrases|225}} {{H-phrases|301}} {{H-phrases|315}} {{H-phrases|331}} {{H-phrases|335}} {{H-phrases|401}} {{H-phrases|412}} | PPhrases = {{P-phrases|210}} {{P-phrases|261}} {{P-phrases|273}} {{P-phrases|301+310}} {{P-phrases|311}} | TLV = | TLV-TWA = | TLV-STEL = | PEL = }} Acetyl cyanide is a chemical compound that contains both a nitrile and a carbonyl functional group. Therefore, the molecule falls into the cyanide group as well due to the presence of the carbon nitrogen triple bond. This molecule is part of the acyl cyanide family. This compound is also known as pyruvonitrile or 2-oxopropionitrile. PropertiesAcetyl cyanide typically exists as a clear, colorless liquid. The structure of acetyl cyanide was determined through the joint use of electron diffraction intensities and rotational constants. These values helped to determine that the average thermal bond distances are 1.116±0.011 Å, 1.167±0.010 Å, 1.208±0.009 Å, 1.477±0.008 Å and 1.518±0.009 Å. Additionally, the bond angles in the structure 124.6±0.7°, 114.2±0.9°, 179.2±2.2° and 109.2±0.7°. This places the single C-C bond at a larger bond distance than the bonds within the vinylacetylene, acrylonitrile and propynal molecules.[2] HazardsAcetyl cyanide is a highly flammable compound. Therefore, this compound should be kept away from sources of heat, flames, and sparks. Acetyl cyanide's toxicological properties have not been thoroughly investigated. However, it is known that the molecule is toxic if inhaled and would cause a respiratory tract irritation. Also the chemical may cause skin irritation if absorbed through the skin. The compound's toxic affects would target the peripheral nervous system, central nervous system, and the blood stream. While this chemical has not been confirmed to be a carcinogen, exposure to this chemical causes irritation to the respiratory system and skin. Additionally, acetyl cyanide is toxic by both inhalation and ingestion. Furthermore, this compound may be toxic to aquatic organisms, possibly causing long-term adverse effects in the aquatic environment.[3] ReactionsDue to the flammable properties of this molecule, hazardous decomposition could occur within the molecule under extreme heat, forming chemicals such as carbon oxides and nitrogen oxide. Therefore heat, flame, and sparks should all be kept away from this molecule in order to prevent this decomposition from occurring. Additionally, this molecule should not interact with strong acids and strong bases to ensure that hazardous reactions are prevented.[4] Two main types of reactions can occur with acetyl cyanide as a reactant; aldol condensation and enolate substitution. Aldol condensation can occur when acetyl cyanide reacts with (Z)-but-2-enal to form (2E,4E)-hexa-2,4-dienoyl cyanide: Enolate substitution can occur when acetyl cyanide reacts with bromomethane to form propanoyl cyanide.[5] Relatively little data has been collected about the possible thermal and photochemical decompositions and kinetic rearrangements. Acetyl cyanide is one of the few carbonyl compound prototypes for which photochemical and thermal dissociations involving ground and excited state surfaces are extensively studied. Their thermal and photofragmenation dynamics are considered to be different from the frequently studied carbonyl compounds with substituents from the first-row substituents. For example, formyl cyanide does not undergo unimolecular decomposition to HCN and CO spontaneously. However, acetyl cyanide, also a member of this family, breaks down through this unimolecular decomposition at 470 °C. This reaction occurs through decarbonylation. This division of the molecule to a ketone and hydrogen cyanide were noted to be under competitive circumstances. This caused a study of the thermal unimolecular reactions that acetyl cyanide undergoes. The unimolecular decompositions that acetyl cyanide undergo have been confirmed to be less energetically favorable than the molecule undergoing isomerization to acetyl isocyanide. However, through other photolysis experiments have resulted in the formation of a CN radical through acetyl cyanide decomposing into CH3CO + CN or CH3COCN.[6] SynthesisAcetyl cyanide is a member of the acyl cyanide family. This molecule is catalytically synthesized at 350 °C from ketene and hydrogen cyanide. This is the most thermodynamically stable method of producing this molecule synthetically.[7] Additionally, this compound can by produced through the hydration of an alkyne through mercuric sulfate catalysis. The reaction shown below displays this occurring from the reagent prop-2-ynenitrile. Alkyne hydration with this same molecule can occur through hydroboration as well without the presence of a catalyst.[8] References1. ^1 {{cite book | title = Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book) | publisher = The Royal Society of Chemistry | date = 2014 | location = Cambridge | pages = 796–797, 903 | doi = 10.1039/9781849733069-FP001 | isbn = 978-0-85404-182-4}} 2. ^{{cite journal | doi=10.1016/0022-2860(74)85121-5 | volume=20 | issue=3 | title=Molecular structure of acetyl cyanide as studied by gas electron diffraction | journal=Journal of Molecular Structure | pages=437–448| year=1974 | last1=Sugié | first1=Masaaki | last2=Kuchitsu | first2=Kozo | bibcode=1974JMoSt..20..437S }} 3. ^http://www.sigmaaldrich.com/catalog/product/fluka/16000?lang=en®ion=US{{dead link|date=October 2016 |bot=InternetArchiveBot |fix-attempted=yes }} 4. ^http://www.sigmaaldrich.com/catalog/product/fluka/16000?lang=en®ion=US{{dead link|date=October 2016 |bot=InternetArchiveBot |fix-attempted=yes }} 5. ^http://www.chemsink.com/compound/69430/{{full|date=September 2018}} 6. ^http://www.quantchem.kuleuven.ac.be/minh/Articles/JPCA/jp9724582.pdf{{dead link|date=October 2016 |bot=InternetArchiveBot |fix-attempted=yes }} 7. ^http://www.quantchem.kuleuven.ac.be/minh/Articles/JPCA/jp9724582.pdf{{dead link|date=October 2016 |bot=InternetArchiveBot |fix-attempted=yes }} 8. ^http://www.chemsink.com/compound/69430/{{full|date=September 2018}} Further reading
1 : Nitriles |
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