||It has been suggested that this article be merged with Ethyl group, Propyl and Butyl to Alkyl. (Discuss) Proposed since January 2013.|
A methyl group is an alkyl derived from methane, containing one carbon atom bonded to three hydrogen atoms — CH3. The group is often abbreviated Me. Such hydrocarbon groups occur in many organic compounds. While the methyl group is usually part of a larger molecule, it can be found on its own in either of three forms: anion, cation or radical. The anion has eight valence electrons, the radical seven and the cation six. All three forms are highly reactive and rarely observed.
Methyl cation, anion, and radical 
Methyl cation 
The methylium cation (CH3+) exists in the gas phase, but is otherwise not encountered. Some compounds are considered to be sources of "CH3+", and this simplification is used pervasively in organic chemistry. For example, protonation of methanol gives a strongly electrophilic methylating reagent:
- CH3OH + H+ → CH3+ + H2O
Methyl anion 
The methanide anion (CH3−) similarly exists only in rarefied gas phase or under exotic conditions. It can be produced by electrical discharge in ketene at low pressure (less than one torr) and its enthalpy of reaction was determined as about 252.2±3.3 kJ/mol.
In discussing mechanisms of organic reactions, it is often a useful simplification to consider methyl lithium and related Grignard reagents as salts of "CH3−", although this view is fiction. Such reagents are generally prepared from the methyl halides:
- M + CH3X → MCH3
where M is an alkali metal.
Methyl radical 
The methyl radical has the formula CH3. It exists in dilute gases, but in more concentrated form it readily dimerizes to ethane. It can be produced by thermal decomposition of only certain compounds, especially those with an -N=N- linkage.
The reactivity of a methyl group depends on the adjacent substituents. Methyl groups can be quite unreactive. For example, in organic compounds, the methyl group resists attack by even the strongest acids.
The oxidation of a methyl group occurs widely in nature and industry. The oxidation products derived from methyl are CH2OH, CHO, and CO2H. For example, permanganate often converts a methyl group to a carboxyl (-COOH) group, e.g. the conversion of toluene to benzoic acid. Ultimately oxidation of methyl groups gives protons and carbon dioxide, as seen in combustion.
Demethylation (the transfer of the methyl group to another compound) is a common process, and reagents that undergo this reaction are called methylating agents. Common methylating agents are dimethylsulfate, methyl iodide, and methyl triflate. Methanogenesis, the source of natural gas, arises via a demethylation reaction.
Certain methyl groups can be deprotonated. For example, the acidity of the methyl groups in acetone ((CH3)2CO) is about 1020 more acidic than methane. The resulting carbanions are key intermediates in many reactions in organic synthesis and biosynthesis. Fatty acids arise in this way.
Free radical reactions 
When placed in benzylic or allylic positions, the C-H bond strength is decreased, and the reactivity of the methyl group increases. One manifestation of this enhanced reactivity is the photochemical chlorination of the methyl group in toluene to give benzyl chloride.
French chemists Jean-Baptiste Dumas and Eugene Peligot, after determining methanol's chemical structure, introduced "methylene" from the Greek methy = "wine" + hȳlē = "wood" (patch of trees) with the intention of highlighting its origins, "alcohol made from wood (substance)", but with Greek language errors: the Greek for "wood (substance)" is xylo-. The term "methyl" was derived in about 1840 by back-formation from "methylene", and was then applied to describe "methyl alcohol".
See also 
- March, Jerry (1992). Advanced organic chemistry: reactions, mechanisms, and structure. John Wiley & Sons. ISBN 0-471-60180-2.
- G. Barney Ellison , P. C. Engelking , W. C. Lineberger (1978), "An experimental determination of the geometry and electron affinity of methyl radical CH3" Journal of the American Chemical Society, volume 100, issue 8, pages 2556–2558. doi:10.1021/ja00476a054
- Thauer, R. K., "Biochemistry of Methanogenesis: a Tribute to Marjory Stephenson", Microbiology, 1998, volume 144, pages 2377–2406.
- M. Rossberg et al. “Chlorinated Hydrocarbons” in Ullmann’s Encyclopedia of Industrial Chemistry 2006, Wiley-VCH, Weinheim. doi:10.1002/14356007.a06_233.pub2
- Annales de chimie et de physique. 1835. p. 9.