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
631-57-2 YesY
1737633
ChemSpider 62638 YesY
EC Number 211-159-2
Jmol interactive 3D Image
Properties
C3H3NO
Molar mass 69.06 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
1.3764
40.86 Å2
Hazards
Safety data sheet External MSDS
GHS pictograms
GHS signal word Danger
H225 H301 H315 H331 H335 H401 H412
P210 P261 P273 P301+310 P311
  • Flammable (F)
  • Toxic (T)
  • Dangerous for the environment (N)
R-phrases R11, R23/25, R51/53, R37/38
S-phrases S45, S61, S36/37
Ingestion hazard Toxic if swallowed.
Inhalation hazard Toxic if inhaled. Causes respiratory tract irritation.
Eye hazard Causes eye irritation.
Skin hazard May be harmful if absorbed through skin. Causes skin irritation.
NFPA 704
Flammability code 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g., gasoline) Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
3
2
0
Flash point 14.44 °C (57.99 °F; 287.59 K)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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. [1]

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.[2]

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.[3]

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.[4]

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.[5]

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. [6]

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.[7]

References

  1. ↑ http://www.sciencedirect.com/science/article/pii/0022286074851215
  2. ↑ http://www.sigmaaldrich.com/catalog/product/fluka/16000?lang=en&region=US
  3. ↑ http://www.sigmaaldrich.com/catalog/product/fluka/16000?lang=en&region=US
  4. ↑ http://www.chemsink.com/compound/69430/
  5. ↑ http://www.quantchem.kuleuven.ac.be/minh/Articles/JPCA/jp9724582.pdf
  6. ↑ http://www.quantchem.kuleuven.ac.be/minh/Articles/JPCA/jp9724582.pdf
  7. ↑ http://www.chemsink.com/compound/69430/
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