Preferred IUPAC name
Other names
110-82-7 YesY
3D model (Jmol) Interactive image
ChEBI CHEBI:29005 YesY
ChemSpider 7787 YesY
DrugBank DB03561 YesY
ECHA InfoCard 100.003.461
KEGG C11249 YesY
PubChem 8078
Molar mass 84.16 g·mol−1
Appearance Colorless liquid
Odor Sweet, gasoline-like
Density 0.7781 g/mL, liquid
Melting point 6.47 °C (43.65 °F; 279.62 K)
Boiling point 80.74 °C (177.33 °F; 353.89 K)
Solubility Soluble in ether, alcohol, acetone
Miscible with olive oil
Vapor pressure 78 mmHg (20 °C)[2]
Viscosity 1.02 cP at 17 °C
-156 kJ/mol
-3920 kJ/mol
Safety data sheet See: data page
F Xn N
R-phrases R11, R38, R65, R67, R50/53
S-phrases (S2), S9, S16, S25, S33, S60, S61, S62
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 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine 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
Flash point −20 °C (−4 °F; 253 K)
245 °C (473 °F; 518 K)
Explosive limits 1.3%-8%[2]
Lethal dose or concentration (LD, LC):
12705 mg/kg (rat, oral)
813 mg/kg (mouse, oral)[3]
17,142 ppm (mouse, 2 hr)
26,600 ppm (rabbit, 1 hr)[3]
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 300 ppm (1050 mg/m3)[2]
REL (Recommended)
TWA 300 ppm (1050 mg/m3)[2]
IDLH (Immediate danger)
1300 ppm[2]
Related compounds
Related cycloalkanes
Related compounds
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).
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Infobox references

Cyclohexane is a cycloalkane with the molecular formula C6H12 (abbreviated to Cy).[4] Cyclohexane is mainly used for the industrial production of adipic acid and caprolactam, which are precursors to nylon. Cyclohexane is a colourless, flammable liquid with a distinctive detergent-like odor, reminiscent of cleaning products (in which it is sometimes used).[5]


Modern production

On an industrial scale, cyclohexane is produced by hydrogenation of benzene.[6] Producers of cyclohexane accounts for approximately 11.4% of global demand for benzene.[7] The reaction is highly exothermic, with ΔH(500 K) = 216.37 kJ/mol). Dehydrogenation commenced noticeably above 300 °C, reflecting the favorable entropy for dehydrogenation.[8]

Historical methods

Unlike benzene, cyclohexane is not easily obtained from natural resources such as coal. For this reason, early investigators synthesized their cyclohexane samples.[9]

Early failures

Surprisingly their cyclohexanes boiled higher by 10°C than either hexahydrobenzene or hexanaphtene but this riddle was solved in 1895 by Markovnikov, N.M. Kishner, and Nikolay Zelinsky when they reassigned "hexahydrobenzene" and "hexanaphtene" as methylcyclopentane, the result of an unexpected rearrangement reaction.


In 1894 Baeyer synthesized cyclohexane starting with a Dieckmann condensation of pimelic acid followed by multiple reductions:

In the same year E. Haworth and W.H. Perkin Jr. (1860–1929) prepared it via a Wurtz reaction of 1,6-dibromohexane.


Cyclohexane is rather unreactive, being a non-polar, hydrophobic hydrocarbon. It reacts with superacids, such as HF + SbF5, which will lead to cracking. Substituted cyclohexanes, however, may be reactive under a variety of conditions, many of which are important in organic chemistry.


Commercially most of cyclohexane produced is converted into cyclohexanonecyclohexanol mixture (or "KA oil") by catalytic oxidation. KA oil is then used as a raw material for adipic acid and caprolactam.[8] It is used as a solvent in some brands of correction fluid.

Laboratory uses

Cyclohexane is sometimes used as an organic solvent.

Cyclohexane is also used for calibration of differential scanning calorimetry (DSC) instruments, because of a convenient crystal-crystal transition at −87.1 °C.[12]

Cyclohexane vapour is used in vacuum carburizing furnaces, in heat treating equipment manufacture.


The 6-vertex edge ring does not conform to the shape of a perfect hexagon. The conformation of a flat 2D planar hexagon has considerable angle strain because its bonds are not 109.5 degrees; the torsional strain would also be considerable because all of the bonds would be eclipsed bonds. Therefore, to reduce torsional strain, cyclohexane adopts a three-dimensional structure known as the chair conformation. There are also two other intermediate conformers; half chair, which is the most unstable conformer, and twist boat, which is more stable than the boat conformer. This was first proposed as early as 1890 by Hermann Sachse, but only gained widespread acceptance much later. The new conformation puts the carbons at an angle of 109.5°. Half of the hydrogens are in the plane of the ring (equatorial) while the other half are perpendicular to the plane (axial). This conformation allows for the most stable structure of cyclohexane. Another conformation of cyclohexane exists, known as boat conformation, but it interconverts to the slightly more stable chair formation. If cyclohexane is mono-substituted with a large substituent, then the substituent will most likely be found attached in an equatorial position, as this is the slightly more stable conformation.

Cyclohexane has the lowest angle and torsional strain of all the cycloalkanes, as a result cyclohexane has been deemed a 0 in total ring strain.

Solid phases

Cyclohexane has two crystalline phases. The high-temperature phase I, stable between 186 K and the melting point 280 K, is a plastic crystal, which means the molecules retain some rotational degree of freedom. The low-temperature (below 186 K) phase II is ordered. Two other low-temperature (metastable) phases III and IV have been obtained by application of moderate pressures above 30 MPa, where phase IV appears exclusively in deuterated cyclohexane (note that application of pressure increases the values of all transition temperatures).[13]

Cyclohexane phases[13]
NoSymmetry Space group a (Å) b (Å) c (Å) Z T (K) P (MPa)
I Cubic Fm3m 8.61 4 195 0.1
II Monoclinic C2/c 11.23 6.44 8.20 4 115 0.1
III Orthorhombic Pmnn 6.54 7.95 5.29 2 235 30
IV Monoclinic P12(1)/n1 6.50 7.64 5.51 4 160 37

Here Z is the number structure units per unit cell; the unit cell constants a, b and c were measured at the given temperature T and pressure P.

See also


  1. Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. pp. 4, 137. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4.
  2. 1 2 3 4 5 "NIOSH Pocket Guide to Chemical Hazards #0163". National Institute for Occupational Safety and Health (NIOSH).
  3. 1 2 "Cyclohexane". Immediately Dangerous to Life and Health. National Institute for Occupational Safety and Health (NIOSH).
  5. Campbell, M. Larry (2011). "Cyclohexane". doi:10.1002/14356007.a08_209.pub2.
  6. Fred Fan Zhang, Thomas van Rijnman, Ji Soo Kim, Allen Cheng "On Present Methods of Hydrogenation of Aromatic Compounds, 1945 to Present Day" Lunds Tekniska Högskola 2008
  7. Market Study Benzene, Ceresana, July 2011
  8. 1 2 Michael Tuttle Musser "Cyclohexanol and Cyclohexanone" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005.
  9. Warnhoff, E. W. (1996). "The Curiously Intertwined Histories of Benzene and Cyclohexane". J. Chem. Ed. 73 (6): 494. doi:10.1021/ed073p494.
  10. See:
    • Bertholet (1867) "Nouvelles applications des méthodes de réduction en chimie organique" (New applications of reduction methods in organic chemistry), Bulletin de la Société chimique de Paris, series 2, 7 : 53-65.
    • Bertholet (1868) "Méthode universelle pour réduire et saturer d'hydrog'ene les composés organiques" (Universelle method for reducing and saturating with hydrogen organic compounds), Bulletin de la Société chimique de Paris, series 2, 9 : 8-31. From page 17: "En effet, la benzine, chauffée à 280° pendant 24 heures avec 80 fois son poids d'une solution aqueuse saturée à froid d'acide iodhydrique, se change à peu près entièrement en hydrure d'hexylène, C12H14, en fixant 4 fois son volume d'hydrog'ene: C12H6 + 4H2 = C12H14 … Le neuveau carbure formé par la bezine est un corps unique et défini: il bout à 69°, et offre toutes les propriétés et la composition de l'hydrure d'hexylène extrait des pétroles." (In effect, benzene, heated to 280° for 24 hours with 80 times its weight of an aqueous solution of cold saturated hydroiodic acid, is changed almost entirely into hydride of hexylene, C12H14, [Note: this formula for hexane (C6H14) is wrong because chemists at that time used the incorrect atomic mass for carbon.] by fixing [i.e., combining with] 4 times its volume of hydrogen: C12H6 + 4H2 = C12H14 … The new carbon compound formed by benzene is a unique and well-defined substance: it boils at 69° and presents all the properties and the composition of hydride of hexylene extracted from oil.)
  11. Adolf Baeyer (1870) "Ueber die Reduction aromatischer Kohlenwasserstoffe durch Jodphosphonium" (On the reduction of aromatic compound by phosphonium iodide [H4IP]), Annalen der Chemie und Pharmacie, 155 : 266-281. From page 279: "Bei der Reduction mit Natriumamalgam oder Jodphosphonium addiren sich im höchsten Falle sechs Atome Wasserstoff, und es entstehen Abkömmlinge, die sich von einem Kohlenwasserstoff C6H12 ableiten. Dieser Kohlenwasserstoff ist aller Wahrscheinlichkeit nach ein geschlossener Ring, da seine Derivate, das Hexahydromesitylen und Hexahydromellithsäure, mit Leichtigkeit wieder in Benzolabkömmlinge übergeführt werden können." (During the reduction [of benzene] with sodium amalgam or phosphonium iodide, six atoms of hydrogen are added in the extreme case, and there arise derivatives, which derive from a hydrocarbon C6H12. This hydrocarbon is in all probability a closed ring, since its derivatives — hexahydromesitylene [1,3,5 - trimethyl cyclohexane] and hexahydromellithic acid [cyclohexane-1,2,3,4,5,6-hexacarboxylic acid] — can be converted with ease again into benzene derivatives.)
  12. Price, D. M. (1995). "Temperature Calibration of Differential Scanning Calorimeters". Journal of Thermal Analysis. 45 (6): 1285–1296. doi:10.1007/BF02547423.
  13. 1 2 Mayer, J.; Urban, S.; Habrylo, S.; Holderna, K.; Natkaniec, I.; Würflinger, A.; Zajac, W. (1991). "Neutron Scattering Studies of C6H12 and C6D12 Cyclohexane under High Pressure". Physica status solidi (b). 166 (2): 381. doi:10.1002/pssb.2221660207.

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