Acetyl cyanide

Acetyl cyanide

Names
IUPAC name 2-Oxopropanenitrile
Other names Pyruvonitrile; Propanenitrile, 2-oxo-; α-Oxopropionitrile; Oxopropionitrile; Oxypropionitrile; Pyruvic acid nitrile; 2-Oxopropionitrile; CH3C(O)CN; 2-Oxopropiononitrile
Identifiers
CAS Number	631-57-2 Y
3D model (JSmol)	Interactive image
Beilstein Reference	1737633
ChemSpider	62638 Y
ECHA InfoCard	100.010.146
EC Number	211-159-2
CompTox Dashboard (EPA)	DTXSID10212430
InChI InChI=1S/C3H3NO/c1-3(5)2-4/h1H3 Y Key: QLDHWVVRQCGZLE-UHFFFAOYSA-N Y
SMILES CC(=O)C#N
Properties
Chemical formula	C3H3NO
Molar mass	69.063 g·mol−1
Appearance	Clear, yellow liquid
Density	0.9745 g/cm3
Boiling point	92.3 °C (198.1 °F; 365.4 K)
Vapor pressure	51.9300003051758 mmHg
Refractive index (nD)	1.3764
Specific Surface Area	40.86 Å2
Hazards
Occupational safety and health (OHS/OSH):
Ingestion hazards	Toxic if swallowed.
Inhalation hazards	Toxic if inhaled. Causes respiratory tract irritation.
Eye hazards	Causes eye irritation.
Skin hazards	May be harmful if absorbed through skin. Causes skin irritation.
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H225 H301 H315 H331 H335 H401 H412
Precautionary statements	P210 P261 P273 P301+P310 P311
NFPA 704 (fire diamond)	2 3 0
Flash point	14.44 °C (57.99 °F; 287.59 K)
Safety data sheet (SDS)	External MSDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is YN ?) Infobox references

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.

Properties

Acetyl cyanide typically exists as a clear, yellow 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.

Hazards

Acetyl 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.

Reactions

Due 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.

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.

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.

Synthesis

Acetyl 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.

Additionally, this compound can by produced through the hydration of an alkyne through mecuric 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.

References

• http://www.sciencedirect.com/science/article/pii/0022286074851215
• Lide, David R., W. M. Haynes, and Thomas J. Bruno, eds. CRC Handbook of Chemistry and Physics. 93rd ed. Boca Raton, FL: CRC, 2012. Web. 17 Oct. 2012.
• http://ull.chemistry.uakron.edu/erd/Chemicals/24000/23535.html
• http://www.chemspider.com/Chemical-Structure.62638.html