|Molar mass||58.09 g/mol|
|Density and phase||0.79 g/cm³, liquid|
|Solubility in water||miscible|
|Melting point||−94.9 °C (178.2 K)|
|Boiling point||56.3 °C (329.4 K)|
|Viscosity||0.32 cP at 20 °C|
|Molecular shape||trigonal planar at C=O|
|Dipole moment||2.91 D|
|EU classification||Flammable (F)
|R-phrases||, , ,|
|S-phrases||, , ,|
|Flash point||−20 °C|
in air (by volume)
|2.55% - 12.80%|
|Autoignition temperature||465 °C|
|Supplementary data page|
|Structure & properties||n, εr, etc.|
|Thermodynamic data||Phase behaviour
Solid, liquid, gas
|Spectral data||UV, IR, NMR, MS|
|Except where noted otherwise, data are given for
materials in their standard state (at 25 °C, 100 kPa)
Acetone (also known as propanone, dimethyl ketone, 2-propanone, propan-2-one and β-ketopropane) is the simplest representative of the group of chemical compounds known as ketones. It is a colorless, volatile, flammable liquid. In addition to being manufactured as a chemical, acetone is also found naturally in the environment, including in small amounts in the human body.
Small amounts of acetone are metabolically produced in the body, mainly from fat. Fasting significantly increases its endogenous production (see ketosis). Acetone can be elevated in cases of diabetes.
Most of the worldwide industrial production of acetone (and phenol) is currently based on a method called the cumene process. This process converts two relatively cheap starting materials, benzene and propylene, into acetone and phenol. Another reactant is oxygen (from the air). The reaction is named after cumene (isopropyl benzene), the intermediate material formed during the process.
The overall reaction may be written as follows:
Before the invention of the cumene process, acetone was produced by the dry distillation of acetates, such as calcium acetate.
Acetone has a melting point of −95.4 °C and boiling point of 56.53 °C. It has a relative density of 0.819 (at 0 °C). It acts as a solvent and is readily miscible with other solvents, including water, ethanol, and diethyl ether.
At relatively low concentrations, acetone is not very toxic. It can, however, irritate and damage skin and the mucosal lining of the mouth. Its fumes should be avoided, as inhalation may lead to liver damage. In addition, one should always wear goggles when handling the substance, as it can cause permanent eye damage (corneal clouding).
Contamination of water, food (such as milk), or air (by acetone vapors) can lead to chronic exposure to acetone. A number of acute poisoning cases have been described. Accidental intake of large amounts of acetone may lead to unconsciousness and death.
Animal studies have shown that long-term exposure to acetone can damage the kidneys, liver, and nerves, increase birth defects, and lower the reproductive capacity of males (only). It is not known if the same effects would occur in humans. Pregnant women should avoid contact with acetone and its fumes, to avoid the possibility of birth defects, including brain damage.
Interestingly, acetone has been shown to have anticonvulsant effects in animal models of epilepsy, in the absence of toxicity, when administered at low (millimolar) concentrations. It has been hypothesized that the high-fat, low-carbohydrate, ketogenic diet used clinically to control drug-resistant epilepsy in children works by elevating acetone in the brain.
All links retrieved August 17, 2012.
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