# Hexamethylbenzene

Hexamethylbenzene, also known as mellitene, is a hydrocarbon with the molecular formula C$_{12}$H$_{18}$ and the condensed structural formula C$_6$(CH$_3$)$_6$. It is an aromatic compound and a derivative of benzene, where benzene's six hydrogen atoms have each been replaced by a methyl group. In 1929, Kathleen Lonsdale reported the crystal structure of hexamethylbenzene, demonstrating that the central ring is hexagonal and flat and thereby ending an ongoing debate about the physical parameters of the benzene system. This was a historically significant result, both for the field of X-ray crystallography and for understanding aromaticity.
Hexamethylbenzene can be oxidised to mellitic acid, which is found in nature as its aluminium salt in the rare mineral mellite. Hexamethylbenzene can be used as a ligand in organometallic compounds. An example from organoruthenium chemistry shows structural change in the ligand associated with changes in the oxidation state of the metal centre, though the same change is not observed in the analogous organoiron system.
In 2016 the crystal structure of the hexamethylbenzene dication C $_6$(CH $_3$)$^{2+}$ $_6$ was reported in Angewandte Chemie International Edition, showing a pyramidal structure in which a single carbon atom has a bonding interaction with six other carbon atoms. This structure was "unprecedented", as the usual maximum valence of carbon is four, and it attracted attention from New Scientist, Chemical & Engineering News, and Science News. The structure does not violate the octet rule since the carbon–carbon bonds formed are not two-electron bonds, and is pedagogically valuable for illustrating that a carbon atom "can [directly bond] with more than four atoms". Steven Bachrach has demonstrated that the compound is hypercoordinated but not hypervalent, and also explained its aromaticity. The idea of describing the chemical bonding in compounds and chemical species in this way through the lens of organometallic chemistry was proposed in 1975, soon after the dication C $_6$(CH $_3$)$^{2+}$ $_6$ was first observed.

## Nomenclature and properties

The complete IUPAC name for this compound is 1,2,3,4,5,6-hexamethylbenzene. The locants (the numbers in front of the name) are superfluous, however, as the name hexamethylbenzene uniquely identifies a single substance and thus is the formal IUPAC name for the compound. It is an aromatic compound, with six π electrons (satisfying Hückel's rule) delocalised over a cyclic planar system; each of the six ring carbon atoms is sp$^2$ hybridised and displays trigonal planar geometry, while each methyl carbon is tetrahedral with sp$^3$ hybridisation, consistent with the empirical description of its structure. Solid hexamethylbenzene occurs as colourless to white crystalline orthorhombic prisms or needles with a melting point of 165–166 °C, a boiling point of 268 °C, and a density of 1.0630 g cm$^{−3}$. It is insoluble in water, but soluble in organic solvents including benzene and ethanol.
Hexamethylbenzene is sometimes called mellitene, a name derived from mellite, a rare honey-coloured mineral (μέλι meli (GEN μέλιτος melitos) is the Greek word for honey.) Mellite is composed of a hydrated aluminium salt of benzenehexacarboxylic acid (mellitic acid), with formula Al $_2$[C $_6$(CO $_2$) $_6$]•16H $_2$O. Mellitic acid itself can be derived from the mineral, and subsequent reduction yields mellitene. Conversely, mellitene can be oxidised to form mellitic acid:
Treatment of hexamethylbenzene with a superelectrophilic mixture of methyl chloride and aluminum trichloride (a source of Me$^{δ⊕}$Cl---$^{δ⊖}$AlCl$_3$) gives heptamethylbenzenium cation, one of the first carbocations to be directly observed.

### Structure

In 1927 Kathleen Lonsdale determined the solid structure of hexamethylbenzene from crystals provided by Christopher Kelk Ingold. Her X-ray diffraction analysis was published in Nature and was subsequently described as "remarkable ... for that early date". Lonsdale described the work in her book Crystals and X-Rays, explaining that she recognised that, though the unit cell was triclinic, the diffraction pattern had pseudo-hexagonal symmetry that allowed the structural possibilities to be restricted sufficiently for a trial-and-error approach to produce a model. This work definitively showed that hexamethylbenzene is flat and that the carbon-to-carbon distances within the ring are the same, providing crucial evidence in understanding the nature of aromaticity.

## Preparation

The compound can be prepared by reacting phenol with methanol at elevated temperatures over a suitable solid catalyst such as alumina. The mechanism of the process has been studied extensively, with several intermediates having been identified. Alkyne trimerisation of dimethylacetylene also yields hexamethylbenzene in the presence of a suitable catalyst.
In 1880, Joseph Achille Le Bel and William H. Greene reported what has been described as an "extraordinary" zinc chloride-catalysed one-pot synthesis of hexamethylbenzene from methanol. At the catalyst's melting point (283 °C), the reaction has a Gibbs free energy (ΔG) of −1090 kJ mol$^{−1}$ and can be idealised as:
    15 CH $_3$OH → C $_6$(CH $_3$) $_6$ + 3 CH $_4$ + 15 H $_2$O
Le Bel and Greene rationalised the process as involving aromatisation by condensation of methylene units, formed by dehydration of methanol molecules, followed by complete Friedel–Crafts methylation of the resulting benzene ring with chloromethane generated in situ. The major products were a mixture of saturated hydrocarbons, with hexamethylbenzene as a minor product. Hexamethylbenzene is also produced as a minor product in the Friedel–Crafts alkylation synthesis of durene from p-xylene, and can be produced by alkylation in good yield from durene or pentamethylbenzene.
Hexamethylbenzene is typically prepared in the gas phase at elevated temperatures over solid catalysts. An early approach to preparing hexamethylbenzene involved reacting a mixture of acetone and methanol vapours over an alumina catalyst at 400 °C. Combining phenols with methanol over alumina in a dry carbon dioxide atmosphere at 410–440 °C also produces hexamethylbenzene, though as part of a complex mixture of anisole (methoxybenzene), cresols (methylphenols), and other methylated phenols. An Organic Syntheses preparation, using methanol and phenol with an alumina catalyst at 530 °C, gives approximately a 66% yield, though synthesis under different conditions has also been reported.
The mechanisms of such surface-mediated reactions have been investigated, with an eye to achieving greater control over the outcome of the reaction, especially in search of selective and controlled ortho-methylation. Both anisole and pentamethylbenzene have been reported as intermediates in the process. Valentin Koptyug and co-workers found that both hexamethylcyclohexadienone isomers (2,3,4,4,5,6- and 2,3,4,5,6,6-) are intermediates in the process, undergoing methyl migration to form the 1,2,3,4,5,6-hexamethylbenzene carbon skeleton.
Trimerisation of three 2-butyne (dimethylacetylene) molecules yields hexamethylbenzene. The reaction is catalyzed by triphenylchromium tri-tetrahydrofuranate or by a complex of triisobutylaluminium and titanium tetrachloride.

## Uses
### Synthetic uses

Hexamethylbenzene can be used as a ligand in organometallic compounds.

### Other uses

Hexamethylbenzene has no commercial or widespread uses. It is exclusively of interest for chemical research.

## Reactions

It forms orange-yellow 1:1 adduct with picryl chloride, probably due to π-stacking of the aromatic systems.
Oxidation with trifluoroperacetic acid or hydrogen peroxide gives 2,3,4,5,6,6-hexamethyl-2,4-cyclohexadienone:)
It has also been used as a solvent for $^3$He-NMR spectroscopy.
Just as with benzene itself, the electron-rich aromatic system in hexamethylbenzene allows it to act as a ligand in organometallic chemistry. The electron-donating nature of the methyl groups—both that there are six of them individually and that there are six meta pairs among them—enhance the basicity of the central ring by six to seven orders of magnitude relative to benzene. Examples of such complexes have been reported for a variety of metal centres, including cobalt, chromium, iron, rhenium, rhodium, ruthenium, and titanium. Known cations of sandwich complexes of cobalt and rhodium with hexamethylbenzene take the form [M(C $_6$(CH $_3$) $_6$) $_2$]$^{n+}$ (M = Co, Fe, Rh, Ru; n = 1, 2), where the metal centre is bound by the π electrons of the two arene moieties, and can easily be synthesised from appropriate metal salts by ligand exchange, for example:
    CoBr $_2$ + 2 AlBr $_3$ → [Co(C $_6$(CH $_3$) $_6$) $_2$]$^{2+}$ + 2 AlBr$^−$ $_4$
The complexes can undergo redox reactions. The rhodium and cobalt dications undergo a one-electron reduction with a suitable active metal (aluminium for the cobalt system, zinc for the rhodium), and the equations describing the reactions in the cobalt system are as follows:
    3 [Co(C $_6$(CH $_3$) $_6$) $_2$]$^{2+}$ + Al → 3 [Co(C $_6$(CH $_3$) $_6$) $_2$]$^+$ + Al$^{3+}$
In the field of organoruthenium chemistry, the redox interconversion of the analogous two-electron reduction of the dication and its neutral product occurs at −1.02 V in acetonitrile and is accompanied by a structural change. The hapticity of one of the hexamethylbenzene ligands changes with the oxidation state of the ruthenium centre, the dication [Ru(η$^6$-C$_6$(CH$_3$)$_6$)$_2$]$^{2+}$ being reduced to [Ru(η$^4$-C$_6$(CH$_3$)$_6$)(η$^6$-C$_6$(CH$_3$)$_6$)], with the structural change allowing each complex to comply with the 18-electron rule and maximise stability.
The equivalent iron(II) complex undergoes a reversible one-electron reduction (at −0.48 V in aqueous ethanol), but the two-electron reduction (at −1.46 V) is irreversible, suggesting a change in structure different from that found in the ruthenium system.

### Dication

The isolation of an ion with composition C $_6$(CH $_3$) $_6$H$^+$ was first reported from investigations of hexamethyl Dewar benzene in the 1960s; a pyramidal structure was suggested based on NMR evidence and subsequently supported by disordered crystal structure data. In the early 1970s theoretical work led by Hepke Hogeveen predicted the existence of a pyramidal dication C $_6$(CH $_3$)$^{2+}$ $_6$, and the suggestion was soon supported by experimental evidence. Spectroscopic investigation of the two-electron oxidation of benzene at very low temperatures (below 4 K) shows that a hexagonal dication forms and then rapidly rearranges into a pyramidal structure:
Two-electron oxidation of hexamethylbenzene would be expected to result in a near-identical rearrangement to a pyramidal carbocation, but attempts to synthesise it in bulk by this method have been unsuccessful. However, a modification of the Hogeveen approach was reported in 2016, along with a high-quality crystal structure determination of [C $_6$(CH $_3$) $_6$][SbF $_6$] $_2$•HSO $_3$F. The pyramidal core is about 1.18 ångströms high, and each of the methyl groups on the ring is located slightly above that base plane to give a somewhat inverted tetrahedral geometry for the carbons of the base of the pyramid. The preparation method involved treating the epoxide of hexamethyl Dewar benzene with magic acid, which formally abstracts an oxide anion (O$^{2−}$ ) to form the dication:
Though indirect spectroscopic evidence and theoretical calculations previously pointed to their existence, the isolation and structural determination of a species with a hexacoordinate carbon bound only to other carbon atoms is unprecedented, and has attracted comment in Chemical & Engineering News, New Scientist, Science News, and ZME Science. The carbon atom at the top of the pyramid is bonding with six other atoms, an unusual arrangement as the usual maximum valence for this element is four. The molecule is aromatic and avoids exceeding the octet on carbon by having only a total of six electrons in the five bonds between the base of the pyramid and its apex. That is, each of the vertical edges of the pyramid is only a partial bond rather than a normal covalent bond that would have two electrons shared between two atoms. Although the top carbon does bond to six others, it does so using a total of no more than eight electrons.
The dication, noting the weak bonds forming the upright edges of the pyramid, shown as dashed lines in the structure, have a Wiberg bond order of about 0.54; it follows that the total bond order is 5 × 0.54 + 1 = 3.7 < 4, and thus the species is not hypervalent, though it is hypercoordinate. The differences in bonding in the dication—the ring having aromatic character and the vertical edges being weak partial bonds—are reflected in variations of the carbon–carbon bond lengths: the ring bonds are 1.439–1.445 Å,, the bonds to the methyl groups are 1.479–1.489 Å,, and the vertical edges are 1.694–1.715 Å. Bachrach rationalised the three-dimensional aromaticity of the dication by considering it as comprising the ring C $_5$(CH $_3$)$^+$ $_5$ as a four-electron donor and topped by the CCH$^+$ $_3$ fragment, which provides two electrons, for a total of six electrons in the aromatic cage, in line with Hückel's rule for n = 1. From the perspective of organometallic chemistry, the species can be viewed as [(η$^5$ –C $_5$(CH $_3$) $_5$)C(CH $_3$)] . This satisfies the octet rule by binding a carbon(IV) centre (C$^{4+}$ ) to an aromatic η$^5$–pentamethylcyclopentadienyl anion (six-electron donor) and methyl anion (two-electron donor), analogous to the way the gas-phase organozinc monomer [(η$^5$ –C $_5$(CH $_3$) $_5$)Zn(CH $_3$)], having the same ligands bound to a zinc(II) centre (Zn$^{2+}$ ) satisfies the 18 electron rule on the metal.
It has been commented that "[i]t's super important that people realize that, although we're taught carbon can only have four friends, carbon can be associated with more than four atoms" and added that the "carbon isn't making six bonds in the sense that we usually think of a carbon-carbon bond as a two-electron bond." "It is all about the challenge and the possibility to astonish chemists about what can be possible."