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Skeletal formula of hexane
Skeletal formula of hexane with all implicit carbons shown, and all explicit hydrogens added
Ball and stick model of hexane
Spacefill model of hexane
IUPAC name
Other names
3D model (JSmol)
ECHA InfoCard 100.003.435
EC Number 203-777-6
MeSH n-hexane
RTECS number MN9275000
UN number 1208
Molar mass 86.178 g·mol−1
Appearance Colorless liquid
Odor Petrolic
Density 0.6606 g mL−1[3]
Melting point −96 to −94 °C; −141 to −137 °F; 177 to 179 K
Boiling point 68.5 to 69.1 °C; 155.2 to 156.3 °F; 341.6 to 342.2 K
9.5 mg L−1
log P 3.764
Vapor pressure 17.60 kPa (at 20.0 °C)
7.6 nmol Pa−1 kg−1
UV-vismax) 200 nm
−74.6·10−6 cm3/mol
Viscosity 0.3 mPa·s
265.2 J K−1 mol−1
296.06 J K−1 mol−1
−199.4–−198.0 kJ mol−1
−4180–−4140 kJ mol−1
Main hazards Reproductive toxicity – After aspiration, pulmonary oedema, pneumonitis, and death [4]
Safety data sheet See: data page
GHS pictograms GHS02: Flammable GHS07: Harmful GHS08: Health hazard GHS09: Environmental hazard
GHS signal word DANGER
H225, H304, H315, H336, H361fd, H373, H401, H411
P201, P202, P210, P233, P240, P241, P242, P243, P260, P264, P271, P273, P280, P281, P301+330+331, P310, P302+352, P303+361+353, P304+340, P312, P308+313, P314, P332+313, P363, P370+378
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., gasolineHealth code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentineReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
Flash point −26.0 °C (−14.8 °F; 247.2 K)
234.0 °C (453.2 °F; 507.1 K)
Explosive limits 1.2–7.7%
Lethal dose or concentration (LD, LC):
25 g kg−1 (oral, rat)
28710 mg/kg (rat, oral)[6]
56137 mg/kg (rat, oral)[6]
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 500 ppm (1800 mg/m3)[5]
REL (Recommended)
TWA 50 ppm (180 mg/m3)[5]
IDLH (Immediate danger)
1100 ppm[5]
Related compounds
Related alkanes
Supplementary data page
Refractive index (n),
Dielectric constantr), etc.
Phase behaviour
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references

Hexane /ˈhɛksn/ is an alkane of six carbon atoms, with the chemical formula C6H14.

The term may refer to any of the five structural isomers with that formula, or to a mixture of them.[7] In IUPAC nomenclature, however, hexane is the unbranched isomer (n-hexane); the other four isomers are named as methylated derivatives of pentane and butane. IUPAC also uses the term as the root of many compounds with a linear six-carbon backbone, such as 2-methylhexane.

Hexanes are significant constituents of gasoline. They are all colorless liquids, odorless when pure, with boiling points between 50 and 70 °C (122 and 158 °F). They are widely used as cheap, relatively safe, largely unreactive, and easily evaporated non-polar solvents.


Common name IUPAC name Text formula Skeletal formula
normal hexane
hexane CH3(CH2)4CH3 Hexane-2D-Skeletal.svg
isohexane 2-methylpentane (CH3)2CH(CH2)2CH3 2-metilpentāns.svg
3-methylpentane CH3CH2CH(CH3)CH2CH3 3-metilpentāns.svg
2,3-dimethylbutane (CH3)2CHCH(CH3)2 2,3-dimetilbutāns.svg
neohexane 2,2-dimethylbutane (CH3)3CCH2CH3 2,2-dimetilbutāns.svg


In industry, hexanes are used in the formulation of glues for shoes, leather products, and roofing. They are also used to extract cooking oils (such as canola oil or soy oil) from seeds, for cleansing and degreasing a variety of items, and in textile manufacturing. They are commonly used in food based soybean oil extraction in the United States, and are potentially present as contaminants in all soy food products in which the technique is used; the lack of regulation by the FDA of this contaminant is a matter of some controversy.[8][9]

A typical laboratory use of hexanes is to extract oil and grease contaminants from water and soil for analysis.[10] Since hexane cannot be easily deprotonated, it is used in the laboratory for reactions that involve very strong bases, such as the preparation of organolithiums. For example, butyllithiums are typically supplied as a hexane solution.[citation needed]

Hexanes are commonly used in chromatography as a non-polar solvent. Higher alkanes present as impurities in hexanes have similar retention times as the solvent, meaning that fractions containing hexane will also contain these impurities. In preparative chromatography, concentration of a large volume of hexanes can result in a sample that is appreciably contaminated by alkanes. This may result in a solid compound being obtained as an oil and the alkanes may interfere with analysis.[citation needed]


Hexanes are chiefly obtained by refining crude oil. The exact composition of the fraction depends largely on the source of the oil (crude or reformed) and the constraints of the refining. The industrial product (usually around 50% by weight of the straight-chain isomer) is the fraction boiling at 65–70 °C (149–158 °F).

Physical properties[edit]

All alkanes are colorless.[11][12] The boiling points of the various hexanes are somewhat similar and, as for other alkanes, are generally lower for the more branched forms. The melting points are quite different and the trend is not apparent.[13]

Isomer M.P. (°C) M.P. (°F) B.P. (°C) B.P. (°F)
n-hexane −95.3 −139.5 68.7 155.7
3-methylpentane −118.0 −180.4 63.3 145.9
2-methylpentane (isohexane) −153.7 −244.7 60.3 140.5
2,3-dimethylbutane −128.6 −199.5 58.0 136.4
2,2-dimethylbutane (neohexane) −99.8 −147.6 49.7 121.5

Hexane has considerable vapor pressure at room temperature:

Temperature (°C) Temperature (°F) Vapor pressure (mmHg) Vapor pressure (kPa)
−40 −40 3.36 0.448
−30 −22 7.12 0.949
−20 −4 14.01 1.868
−10 14 25.91 3.454
0 32 45.37 6.049
10 50 75.74 10.098
20 68 121.26 16.167
25 77 151.28 20.169
30 86 187.11 24.946
40 104 279.42 37.253
50 122 405.31 54.037
60 140 572.76 76.362


Like most alkanes, hexane characteristically exhibits low reactivity and are suitable solvents for reactive compounds. Commercial samples of n-hexane however often contains methylcyclopentane, which features tertiary C-H bonds, which are incompatible with some radical reactions.[14]


The acute toxicity of n-hexane is rather low, requiring grams per kilogram. Inhalation of n-hexane at 5000 ppm for 10 minutes produces marked vertigo; 2500-1000 ppm for 12 hours produces drowsiness, fatigue, loss of appetite, and paresthesia in the distal extremities; 2500–5000 ppm produces muscle weakness, cold pulsation in the extremities, blurred vision, headache and anorexia.[15] The National Institute for Occupational Safety and Health (NIOSH) has set a recommended exposure limit (REL) for hexane isomers (not n-hexane) of 100 ppm (350 mg/m3 (0.15 gr/cu ft)) over an 8-hour workday.[16]

Hexane and other volatile hydrocarbons (petroleum ether) present an aspiration risk.[17] n-Hexane is sometimes used as a denaturant for alcohol, and as a cleaning agent in the textile, furniture, and leather industries. It is slowly being replaced with other solvents.[18]

Like gasoline, hexane is highly volatile and is an explosion risk.


Occupational hexane poisoning has occurred with Japanese sandal workers, Italian shoe workers,[19] Taiwan press proofing workers, and others.[20] Analysis of Taiwanese workers has shown occupational exposure to substances including n-hexane.[21] In 2010–2011, Chinese workers manufacturing iPhones were reported to have suffered hexane poisoning.[22][23]

Hexane was identified as being the cause of the Louisville sewer explosions on February 13, 1981, that destroyed more than 13 miles (21 km) of sewer lines and streets in the center of Louisville in Kentucky, United States


n-Hexane is biotransformed to 2-hexanol and further to 2,5-hexanediol in the body. The conversion is catalyzed by the enzyme cytochrome P450 utilizing oxygen from air. The pathway is called omega oxidation. 2,5-Hexanediol may be further oxidized to 2,5-hexanedione, which is neurotoxic and produces a polyneuropathy.[18] In view of this behavior, replacement of n-hexane as a solvent has been discussed. n-Heptane is a possible alternative.[24]

See also[edit]


  1. ^ Hofmann, August Wilhelm Von (1 January 1867). "I. On the action of trichloride of phosphorus on the salts of the aromatic monamines". Proceedings of the Royal Society of London. 15: 54–62. doi:10.1098/rspl.1866.0018. Archived from the original on 28 April 2018. Retrieved 28 April 2018 – via rspl.royalsocietypublishing.org.
  2. ^ "n-hexane – Compound Summary". PubChem Compound. USA: National Center for Biotechnology Information. 16 September 2004. Identification and Related Records. Archived from the original on 8 March 2012. Retrieved 31 December 2011.
  3. ^ William M. Haynes (2016). CRC Handbook of Chemistry and Physics (97th ed.). Boca Raton: CRC Press. p. 3–298. ISBN 978-1-4987-5429-3.
  4. ^ GHS Classification on [PubChem]
  5. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0322". National Institute for Occupational Safety and Health (NIOSH).
  6. ^ a b "n-Hexane". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  7. ^ "C5 and C6 alkanes". A and B Scott Organic Chemistry. Archived from the original on 13 October 2007. Retrieved 30 October 2007.
  8. ^ "The Tofurky Company : Our Ingredients". Tofurky.com. Archived from the original on 17 March 2015. Retrieved 17 March 2015.
  9. ^ Palmer, Brian (26 April 2010). "A study found hexane in soy protein. Should you stop eating veggie burgers?". Slate.com. Archived from the original on 9 March 2015. Retrieved 17 March 2015.
  10. ^ Use of ozone depleting substances in laboratories. The Nordic Council (2003). ISBN 92-893-0884-2
  11. ^ "Organic Chemistry-I" (PDF). Nsdl.niscair.res.in. Archived (PDF) from the original on 29 October 2013. Retrieved 17 February 2014.
  12. ^ "13. Hydrocarbons | Textbooks". Textbook.s-anand.net. Archived from the original on 6 October 2014. Retrieved 17 February 2014.
  13. ^ William D. McCain (1990). The properties of petroleum fluids. PennWell. ISBN 978-0-87814-335-1.
  14. ^ Koch, H.; Haaf, W. (1973). "1-Adamantanecarboxylic Acid". Organic Syntheses.; Collective Volume, 5, p. 20
  15. ^ "N-HEXANE". Toxicology data network Hazardous Substances Data Bank. National Library of Medicine. Archived from the original on 4 September 2015.
  16. ^ "CDC – NIOSH Pocket Guide to Chemical Hazards – Hexane isomers (excluding n-Hexane)". www.cdc.gov. Archived from the original on 31 October 2015. Retrieved 3 November 2015.
  17. ^ Gad, Shayne C (2005), "Petroleum Hydrocarbons", Encyclopedia of Toxicology, 3 (2nd ed.), Elsevier, pp. 377–379
  18. ^ a b Clough, Stephen R; Mulholland, Leyna (2005). "Hexane". Encyclopedia of Toxicology. 2 (2nd ed.). Elsevier. pp. 522–525.
  19. ^ Rizzuto, N; De Grandis, D; Di Trapani, G; Pasinato, E (1980). "N-hexane polyneuropathy. An occupational disease of shoemakers". European Neurology. 19 (5): 308–15. doi:10.1159/000115166. PMID 6249607.
  20. ^ n-Hexane, Environmental Health Criteria (122), World Health Organization, 1991, archived from the original on 19 March 2014
  21. ^ Liu, C. H.; Huang, C. Y.; Huang, C. C. (2012). "Occupational Neurotoxic Diseases in Taiwan". Safety and Health at Work. 3 (4): 257–67. doi:10.5491/SHAW.2012.3.4.257. PMC 3521924. PMID 23251841.
  22. ^ "Workers poisoned while making iPhones – ABC News (Australian Broadcasting Corporation)". Abc.net.au. 26 October 2010. Archived from the original on 8 April 2011. Retrieved 17 March 2015.
  23. ^ David Barboza (22 February 2011). "Workers Sickened at Apple Supplier in China". The New York Times. Archived from the original on 7 April 2015. Retrieved 17 March 2015.
  24. ^ Filser JG, Csanády GA, Dietz W, Kessler W, Kreuzer PE, Richter M, Störmer A (1996). "Comparative estimation of the neurotoxic risks of n-hexane and n-heptane in rats and humans based on the formation of the metabolites 2,5-hexanedione and 2,5-heptanedione". Adv Exp Med Biol. Advances in Experimental Medicine and Biology. 387: 411–427. doi:10.1007/978-1-4757-9480-9_50. ISBN 978-1-4757-9482-3. PMID 8794236.

External links[edit]