Cyclohexane Properties Cyclohexane Hazards Cyclohexane MSDS Freezing Point of Cyclohexane Hexane Toluene Naphthalene Methylene Chloride
| Cyclohexane | Cyclohexane_conformation | Cyclohexane-1,2-diol | Cyclohexane-1,2-dione_hydrolase | Cyclohexane_(data_page) | 1,2-Cyclohexane_dicarboxylic_acid_diisononyl_ester | Cyclohexane-1,2-diol_dehydrogenase | Cyclohexane-1,3-dione_hydrolase | Methylene_cyclohexane | Cyclohexane_dimethanol | Benzene | Inositol | Cyclohexane-1,3_diene | Dimethyl-cyclohexane-ethanamine | Cyclopentane | Cycloalkane | Hexachlorocyclohexane | Dithiane | Spirodecane | Cyclohexanecarboxylic_acid |
|Jmol-3D images||Image 1|
|Molar mass||84.16 g/mol|
|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 in water||Immiscible|
|Solubility||soluble in ether, alcohol, acetone
miscible with olive oil
|Refractive index (nD)||1.42662|
|Viscosity||1.02 cP at 17 °C|
|Std enthalpy of
|Std enthalpy of
|EU classification||Flammable ('F)
the environment (N)
Severe eye irritant, may cause corneal clouding
|R-phrases||R11, R38, R65, R67, R50/53|
|S-phrases||(S2), S9, S16, S25, S33, S60, S61, S62|
|Flash point||−20 °C; −4 °F; 253 K|
|Autoignition temperature||245 °C; 473 °F; 518 K|
|Supplementary data page|
|n, εr, etc.|
Solid, liquid, gas
|Spectral data||UV, IR, NMR, MS|
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Cyclohexane is a cycloalkane with the molecular formula C6H12. Cyclohexane is used as a nonpolar solvent for the chemical industry, and also as a raw material for the industrial production of adipic acid and caprolactam, both of which being intermediates used in the production of nylon. On an industrial scale, cyclohexane is produced by reacting benzene with hydrogen. Producers of cyclohexane account for approximately 11.4% of global demand for benzene. Because of its unique chemical and conformational properties, cyclohexane is also used in labs in analysis and as a standard. Cyclohexane has a distinctive detergent-like odor, reminiscent of cleaning products (in which it is sometimes used).
The 6-vertexed ring does not conform to the shape of a perfect 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, a combination of angle and torsional strain. This also makes cyclohexane the most stable of the cycloalkanes and therefore will produce the least amount of heat (per CH2 unit) when burned compared to the other cycloalkanes.
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).
|No||Symmetry||Space group||a (Å)||b (Å)||c (Å)||Z||T (K)||P (MPa)|
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.
Pure cyclohexane in itself is rather unreactive, being a non-polar, hydrophobic hydrocarbon. It can react with very strong acids such as the superacid system HF + SbF5, which will cause forced protonation and "hydrocarbon cracking". Substituted cyclohexanes, however, may be reactive under a variety of conditions, many of which being important to organic chemistry. Cyclohexane is highly flammable.
The specific arrangement of functional groups in cyclohexane derivatives, and indeed in most cycloalkane molecules, is extremely important in chemical reactions, especially reactions involving nucleophiles. Substituents on the ring must be in the axial formation to react with other molecules. For example, the reaction of bromocyclohexane and a common nucleophile, a hydroxide anion (OH−), would result in cyclohexene:
This reaction, commonly known as an elimination reaction or dehalogenation (specifically E2), requires that the bromine substituent be in the axial formation, opposing another axial H atom to react. Assuming that the bromocyclohexane was in the appropriate formation to react, the E2 reaction would commence as such:
Note: All three steps happen simultaneously, characteristic of all E2 reactions.
The reaction above will generate mostly E2 reactions and as a result the product will be mostly (~70%) cyclohexene. However, the percentage varies with conditions, and generally, two different reactions (E2 and SN2) compete. In the above reaction, an SN2 reaction would substitute the bromine for a hydroxyl (OH−) group instead, but once again, the Br must be in axial to react. Once the SN2 substitution is complete, the newly substituted OH group would flip back to the more stable equatorial position quickly (~1 millisecond).
Commercially most of cyclohexane produced is converted into cyclohexanone–cyclohexanol mixture (or "KA oil") by catalytic oxidation. KA oil is then used as a raw material for adipic acid and caprolactam. Practically, if the cyclohexanol content of KA oil is higher than cyclohexanone, it is more likely (economical) to be converted into adipic acid, and the reverse case, caprolactam production is more likely. Such ratio in KA oil can be controlled by selecting suitable oxidation catalyst. Cyclohexane is sometimes used as a nonpolar organic solvent.
Although much is already known about this cyclic hydrocarbon, research is still being done on cyclohexane and benzene mixtures and solid phase cyclohexane to determine hydrogen yields of the mix when irradiated at −195 °C.
Heat treating equipment manufacturer Surface Combustion uses cyclohexane as a carbon carrying gas in their high purity vacuum carburizing furnaces.
Unlike compounds like benzene, cyclohexane cannot easily be obtained from natural resources such as coal. Toward the end of the nineteenth century early chemical investigators had to depend on organic synthesis. It took them 30 years to flesh out the details. In 1867 Marcellin Berthelot reduced benzene with hydroiodic acid at elevated temperatures. He incorrectly identified the reaction product as n-hexane not only because of the convenient match in boiling point (69 °C) but also because he did not believe benzene was a cyclic molecule (like his contemporary August Kekulé) but rather some sort of association of acetylene. In 1870 one of his sceptics Adolf von Baeyer repeated the reaction and pronounced the same reaction product hexahydrobenzene and in 1890 Vladimir Markovnikov believed he was able to distill the same compound from Caucasus petroleum calling his concoction hexanaphtene.
and in the same year E. Haworth and W.H. Perkin Jr. (1860–1929) did the same in a Wurtz reaction of 1,6-dibromohexane.
Surprisingly their cyclohexanes boiled higher by 10°C than either hexahydrobenzene or hexanaphtene but this riddle was solved in 1895 by Markovnikov, rearrangement reaction.
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