Acetone
From Freepedia
| Acetone | |
|---|---|
| Image:Acetone.png | |
| General | |
| Systematic name | 2-Propanone |
| Other names | β-ketopropane dimethyl ketone |
| Molecular formula | C3H6O |
| SMILES | CC(=O)C |
| Molar mass | 58.09 g/mol |
| Appearance | clear colourless liquid |
| CAS number | [67-64-1] |
| Properties | |
| 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 |
| Structure | |
| Molecular shape | trigonal planar at C=O |
| Dipole moment | 2.91 D |
| Hazards | |
| MSDS | External MSDS |
| NFPA 704 | Image:Nfpa h1.pngImage:Nfpa f3.pngImage:Nfpa r0.png |
| Main hazards | flammable |
| Flash point | < -20 °C |
| R/S statement | R: 11, 36/37/38, 66/67, S: 9, 16, 23, 26, 33 |
| RTECS number | AL31500000 |
| Supplementary data page | |
| Structure & properties | n, εr, etc. |
| Thermodynamic data | Phase behaviour Solid, liquid, gas |
| Spectral data | UV, IR, NMR, MS |
| Related compounds | |
| Related aldehydes | formaldehyde acetaldehyde |
| Related ketones | 2-butanone |
| Related compounds | water alcohol toluene |
| Except where noted otherwise, data are given for materials in their standard state (at 25°C, 100 kPa) Infobox disclaimer and references | |
- For an alternate use of "acetone", see Acetone (music).
In chemistry, acetone (also known as propanone, dimethyl ketone, 2-propanone, propan-2-one and beta-ketopropane) is the simplest representative of the ketones.
Acetone is a colorless mobile flammable liquid with melting point at -95.4 °C and boiling point at 56.53 °C. It has a relative density of 0.819 (at 0 °C). It is readily soluble in water, ethanol, ether, etc., and itself serves as an important solvent. The most familiar household use of acetone is as the active ingredient in nail polish remover. Acetone is also used to make plastic, fibers, drugs, and other chemicals. Acetone is listed as a Table II precursor under the United Nations Convention Against Illicit Traffic in Narcotic Drugs and Psychotropic Substances[1].
Contents |
Biological aspects
As a member of the ketone bodies it is present in very small quantity in normal urine and in the blood. Larger quantities can be found after starvation and in diabetic patients with severe insulin deficiency (that is untreated or inadequately treated persons); a fruity smell of the breath caused by acetone is one symptom of diabetic ketoacidosis. See ketone bodies for more information.
Acetone occurs naturally in plants, trees, volcanic gases, forest fires, and as a product of the breakdown of body fat. It is present in vehicle exhaust, tobacco smoke, and landfill sites. Industrial processes contribute more acetone to the environment than natural processes. It is found among the products formed in destructive distillation of wood, sugar, cellulose, etc., and for this reason it is always present in crude wood spirit, from which the greater portion of it may be recovered by fractional distillation.
Chemistry
It forms a hydrazone with phenyl hydrazine and an oxime with hydroxylamine. Reduction by sodium amalgam converts it into isopropyl alcohol; oxidation by chromic acid gives carbon dioxide and acetic acid. It reacts with ammonia to form di- and triacetoneamines. It also unites directly with hydrocyanic acid to form the nitrile of α-hydroxyisobutyric acid.
By the action of various reagents, such as lime, caustic potash, hydrochloric acid, etc., acetone is converted into aldol condensation products, mesityl oxide C6H10O, phorone C9H14O, etc. On distillation with sulfuric acid (H2SO4), it is converted into mesitylene C9H12 (symmetrical trimethylbenzene). Acetone has also been used in the artificial production of indigo. In the presence of iodine and an alkali it gives iodoform.
Uses
An important industrial use for acetone its reaction with phenol, used for the manufacture of bisphenol A. Bisphenol A is an important component of many polymers such as polycarbonates, polyurethanes and epoxy resins. Acetone is also used extensively for the safe transporting and storing of acetylene. Vessels containing a porous material are filled with acetone then acetylene, which dissolves into the acetone. One liter of acetone can dissolve around 250 liters of acetylene.
Acetone is often the primary (or only) component in nail polish remover. Acetone can be used as a fuel additive to increase fuel economy and engine performance.
Health effects
Acetone can result in unconsciousness and damage to the skin in the mouth. Skin contact can result in irritation and damage to the skin.
The smell and respiratory data are known mostly from animal studies. Kidney, liver, and nerve damage, increased birth defects, and lowered reproduction ability of males (only) occurred in animals exposed long-term. It is not known if these same effects would be exhibited in humans.
Interestingly, acetone has been shown to have anticonvulsant effects in animal models of epilepsy, in the absence of toxicity, when administered in millimolar concentrations (see: Likhodii et al, 2003).
