Difference between revisions of "Acetone" - New World Encyclopedia
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− | + | '''Acetone''' (also known as '''propanone''', '''dimethyl ketone''', '''2-propanone''', '''propan-2-one''' and '''β-ketopropane''') is the simplest representative of the group of [[chemical compound]]s known as ''[[ketone]]s''. 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. | |
− | + | Acetone is a highly effective [[solvent]] for many organic compounds and is the active ingredient in [[nail polish]] remover. It is also used to make various [[plastic]]s, [[fiber]]s, [[drug]]s, and other chemicals. | |
− | + | == Occurrence 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]]. | |
== Characteristics == | == Characteristics == | ||
+ | |||
+ | During [[World War I]], a new process of producing acetone through [[bacterium|bacterial]] [[Fermentation (biochemistry)|fermentation]] was developed by [[Chaim Weizmann]], (who later became the first president of [[Israel]]), to help the British war effort. | ||
+ | |||
+ | Before the invention of the [[cumene process]] acetone was produced by the dry [[distillation]] of [[acetate]]s, for example [[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 (molecule)|water]], [[ethanol]], and [[diethyl ether|ether]]. | 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 (molecule)|water]], [[ethanol]], and [[diethyl ether|ether]]. | ||
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== Uses == | == Uses == | ||
− | An important industrial use for acetone involves its reaction with [[phenol]] | + | * An important industrial use for acetone involves its reaction with [[phenol]] to produce [[bisphenol A]], which is a valuable component of many polymers, such as [[polycarbonate]]s, [[polyurethane]]s, and [[epoxy resin]]s. |
− | + | * Another industrial application involves its use as a general purpose cleaner in paint and ink manufacturing operations. | |
− | + | * Acetone is also used extensively for the safe transport and storage of [[acetylene]]. Vessels containing a porous material are first filled with acetone followed by acetylene, which dissolves into the acetone. One liter of acetone can dissolve around 250 liters of acetylene. | |
− | + | * It is often the primary (or only) component in [[nail polish]] remover.<ref>[[Acetonitrile]], another organic solvent, is sometimes used as well.</ref> It is also used as a [[superglue]] remover. It can be used for thinning and cleaning [[fiberglass]] [[resin]]s and [[epoxy|epoxies]], and it is highly effective in removing stains by permanent markers. | |
− | + | * It can be used as an agent in art work. When rubbed on the back of any laser print or laser photocopy, it produces a rough ready effect. | |
− | + | * It has been used in the manufacture of [[cordite]]. | |
− | + | * It is a strong solvent for most [[plastic]]s (including those used in consumer-targeted water bottles) and synthetic fibers. | |
+ | |||
+ | * It is used as a [[desiccant|drying agent]], as it is readily miscible with water and is volatile. | ||
+ | |||
+ | * In the laboratory, acetone is used as a [[chemical polarity|polar]] [[aprotic solvent]] (solvent that does not release hydrogen ions) in a variety of [[organic reaction]]s. | ||
==Health effects== | ==Health effects== | ||
− | + | At relatively low concentrations, acetone is not very toxic. It can, however, irritate and damage [[skin]] and the [[mucosa]]l 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 [[kidney]]s, [[liver]], and [[nerve]]s, increase [[birth defect]]s, 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.<ref name="Likhodii">Likhodii et al., ''Ann Neurol.'', 54(2) (2003): 219–226.</ref> 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.<ref name="Likhodii"/> | |
− | + | == Chemical safety measures == | |
− | + | Due to chemical incompatibilities, it is recommended that acetone should be kept away from [[bromine]], [[chlorine]], [[nitric acid]], [[sulfuric acid]] and [[trichloromethane]]. | |
− | Due to incompatibilities, it is recommended | ||
== See also == | == See also == | ||
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==References== | ==References== | ||
− | * McMurry, John. 2004. ''Organic Chemistry'', 6th ed. Belmont, C.A.: Brooks/Cole. ISBN 0534420052 | + | * McMurry, John. 2004. ''Organic Chemistry'', 6th ed. Belmont, C.A.: Brooks/Cole. ISBN 0534420052. |
− | * Morrison, Robert T., and Robert N. Boyd. 1992. ''Organic Chemistry'', 6th ed. Englewood Cliffs, N.J.: Prentice Hall. ISBN 0136436692 | + | * Morrison, Robert T., and Robert N. Boyd. 1992. ''Organic Chemistry'', 6th ed. Englewood Cliffs, N.J.: Prentice Hall. ISBN 0136436692. |
− | * Solomons, T. W. Graham and Craig B. Fryhle. 2004. ''Organic Chemistry'', 8th ed. Hoboken, N.J.: John Wiley. ISBN 0471417998 | + | * Solomons, T. W. Graham, and Craig B. Fryhle. 2004. ''Organic Chemistry'', 8th ed. Hoboken, N.J.: John Wiley. ISBN 0471417998. |
==External links== | ==External links== | ||
− | |||
− | * [http://www.cem.msu.edu/~reusch/VirtualText/intro1.htm#info Virtual Textbook of Organic Chemistry] | + | * [http://www.cem.msu.edu/~reusch/VirtualText/intro1.htm#info Virtual Textbook of Organic Chemistry.] Retrieved June 29, 2007. |
− | * [http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc00/icsc0087.htm Acetone] | + | * [http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc00/icsc0087.htm Acetone.] ''International Occupational Safety and Health Information Centre''. Retrieved June 29, 2007. |
− | * [http://www.npi.gov.au/database/substance-info/profiles/3.html Acetone Fact Sheet] | + | * [http://www.npi.gov.au/database/substance-info/profiles/3.html Acetone Fact Sheet] ''National Pollutant Inventory, Australian Government Department of the Environment and Water Resources''. Retrieved June 29, 2007. |
− | * [http://www.cdc.gov/niosh/npg/npgd0004.html Acetone] | + | * [http://www.cdc.gov/niosh/npg/npgd0004.html Acetone.] ''NIOSH Pocket Guide to Chemical Hazards''. Retrieved June 29, 2007. |
− | * [http://webbook.nist.gov/chemistry/ NIST Chemistry WebBook] | + | * [http://webbook.nist.gov/chemistry/ NIST Chemistry WebBook.] ''National Institute of Standards and Technology''. Retrieved June 29, 2007. |
[[Category:Physical sciences]] | [[Category:Physical sciences]] |
Revision as of 01:09, 8 July 2007
Acetone[1] | |
---|---|
General | |
Systematic name | Propanone |
Other names | β-ketopropane Dimethyl ketone, |
Molecular formula | CH3COCH3 |
SMILES | CC(=O)C |
Molar mass | 58.09 g/mol |
Appearance | Colorless 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 |
EU classification | Flammable (F) Irritant (Xi) |
NFPA 704 | |
R-phrases | R11, R36, R66, R67 |
S-phrases | S2, S9, S16, S26 |
Flash point | −20 °C |
Flammable limits in air (by volume) |
2.55% - 12.80% |
Autoignition temperature | 465 °C |
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 ketones | Butanone |
Related solvents | Water Ethanol Isopropanol Toluene |
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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.
Acetone is a highly effective solvent for many organic compounds and is the active ingredient in nail polish remover. It is also used to make various plastics, fibers, drugs, and other chemicals.
Occurrence 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.
Characteristics
During World War I, a new process of producing acetone through bacterial fermentation was developed by Chaim Weizmann, (who later became the first president of Israel), to help the British war effort.
Before the invention of the cumene process acetone was produced by the dry distillation of acetates, for example 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 ether.
Uses
- An important industrial use for acetone involves its reaction with phenol to produce bisphenol A, which is a valuable component of many polymers, such as polycarbonates, polyurethanes, and epoxy resins.
- Another industrial application involves its use as a general purpose cleaner in paint and ink manufacturing operations.
- Acetone is also used extensively for the safe transport and storage of acetylene. Vessels containing a porous material are first filled with acetone followed by acetylene, which dissolves into the acetone. One liter of acetone can dissolve around 250 liters of acetylene.
- It is often the primary (or only) component in nail polish remover.[2] It is also used as a superglue remover. It can be used for thinning and cleaning fiberglass resins and epoxies, and it is highly effective in removing stains by permanent markers.
- It can be used as an agent in art work. When rubbed on the back of any laser print or laser photocopy, it produces a rough ready effect.
- It has been used in the manufacture of cordite.
- It is a strong solvent for most plastics (including those used in consumer-targeted water bottles) and synthetic fibers.
- It is used as a drying agent, as it is readily miscible with water and is volatile.
- In the laboratory, acetone is used as a polar aprotic solvent (solvent that does not release hydrogen ions) in a variety of organic reactions.
Health effects
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.[3] 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.[3]
Chemical safety measures
Due to chemical incompatibilities, it is recommended that acetone should be kept away from bromine, chlorine, nitric acid, sulfuric acid and trichloromethane.
See also
Notes
ReferencesISBN links support NWE through referral fees
- McMurry, John. 2004. Organic Chemistry, 6th ed. Belmont, C.A.: Brooks/Cole. ISBN 0534420052.
- Morrison, Robert T., and Robert N. Boyd. 1992. Organic Chemistry, 6th ed. Englewood Cliffs, N.J.: Prentice Hall. ISBN 0136436692.
- Solomons, T. W. Graham, and Craig B. Fryhle. 2004. Organic Chemistry, 8th ed. Hoboken, N.J.: John Wiley. ISBN 0471417998.
External links
- Virtual Textbook of Organic Chemistry. Retrieved June 29, 2007.
- Acetone. International Occupational Safety and Health Information Centre. Retrieved June 29, 2007.
- Acetone Fact Sheet National Pollutant Inventory, Australian Government Department of the Environment and Water Resources. Retrieved June 29, 2007.
- Acetone. NIOSH Pocket Guide to Chemical Hazards. Retrieved June 29, 2007.
- NIST Chemistry WebBook. National Institute of Standards and Technology. Retrieved June 29, 2007.
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