methyl radical

Its first ionization potential (yielding the methenium ion, {{chem|CH|3|+}}) is {{val|9.837|0.005|ul=eV}}. {{cite journal | last1 = Golob | first1 = L. | last2 = Jonathan | first2 = N. | last3 = Morris | first3 = A. | last4 = Okuda | first4 = M. | last5 = Ross | first5 = K.J. | year = 1972 | title = The first ionization potential of the methyl radical as determined by photoelectron spectroscopy | journal = Journal of Electron Spectroscopy and Related Phenomena | volume = 1 | issue = 5| pages = 506–508 | doi = 10.1016/0368-2048(72)80022-7 | bibcode = 1972JESRP...1..506G }}

The carbon centre in methyl can bond with electron-donating molecules by reacting:

:{{Chem|CH|3|•}} + R^• → {{Chem|RCH|3}}

Because of the capture of the nucleophile (R^•), methyl has oxidising character. Methyl is a strong oxidant with organic chemicals. However, it is equally a strong reductant with chemicals such as water. It does not form aqueous solutions, as it reduces water to produce methanol and elemental hydrogen:

:2 {{Chem|CH|3|•}} + 2 {{Chem|H|2|O}} → 2 {{Chem|CH|3|OH}} + {{Chem|H|2}}

The molecular geometry of the methyl radical is trigonal planar (bond angles are 120°), although the energy cost of distortion to a pyramidal geometry is small. All other electron-neutral, non-conjugated alkyl radicals are pyramidalized to some extent, though with very small inversion barriers. For instance, the t-butyl radical has a bond angle of 118° with a {{cvt|0.7|kcal/mol|kJ/mol}} barrier to pyramidal inversion. On the other hand, substitution of hydrogen atoms by more electronegative substituents leads to radicals with a strongly pyramidal geometry (112°), such as the trifluoromethyl radical, {{chem|CF|3|•}}, with a much more substantial inversion barrier of around {{cvt|25|kcal/mol|kJ/mol}}.Anslyn E.V. and Dougherty D.A., Modern Physical Organic Chemistry (University Science Books, 2006), p.57

Methyl undergoes the typical chemical reactions of a radical. Below approximately {{Convert|1100|C|K|-2}}, it rapidly dimerises to form ethane. Upon treatment with an alcohol, it converts to methane and either an alkoxy or hydroxyalkyl. Reduction of methyl gives methane. When heated above, at most, {{Convert|1400|C|K|-2}}, methyl decomposes to produce methylidyne and elemental hydrogen, or to produce methylene and atomic hydrogen:

:{{Chem|CH|3|•}} → CH^• + {{Chem|H|2}}

:{{Chem|CH|3|•}} → {{Chem|CH|2|•}} + H^•

Methyl is very corrosive to metals, forming methylated metal compounds:

:M + n {{Chem|CH|3|•}} → M(CH₃)_n

Some radical SAM enzymes generate methyl radicals by reduction of S-adenosylmethionine.{{cite journal|author1=Ribbe, M. W. |author2=Hu, Y. |author3=Hodgson, K. O. |author4=Hedman, B. |title=Biosynthesis of Nitrogenase Metalloclusters|journal=Chemical Reviews|year=2014|volume=114|issue=8|pages=4063–4080|doi=10.1021/cr400463x|pmc=3999185|pmid=24328215}}

It can be produced by the ultraviolet photodissociation of acetone vapour at 193 nm:{{cite journal|last1=Hall|first1=G. E.|last2=Vanden Bout|first2=D.|last3=Sears|first3=Trevor J.|title=Photodissociation of acetone at 193 nm: Rotational- and vibrational-state distributions of methyl fragments by diode laser absorption/gain spectroscopy|journal=The Journal of Chemical Physics|date=1991|volume=94|issue=6|page=4182|doi=10.1063/1.460741|publisher=AIP Publishing|bibcode = 1991JChPh..94.4182H |url=https://zenodo.org/record/1232934}}

:{{Chem|C|3|H|6|O}} → CO + 2 {{Chem|CH|3|•}}

It is also produced by the ultraviolet dissociation of halomethanes:

:{{Chem|CH|3|X}} → X^• + {{Chem|CH|3|•}}

{{Details|Atmospheric methane#Removal processes}}

It can also be produced by the reaction of methane with the hydroxyl radical:

:OH^• + CH₄ → {{Chem|CH|3|•}} + H₂O

This process begins the major removal mechanism of methane from the atmosphere. The reaction occurs in the troposphere or stratosphere. In addition to being the largest known sink for atmospheric methane, this reaction is one of the most important sources of water vapor in the upper atmosphere.

This reaction in the troposphere gives a methane lifetime of 9.6 years. Two more minor sinks are soil sinks (160 year lifetime) and stratospheric loss by reaction with ^•OH, ^•Cl and ^•O¹D in the stratosphere (120 year lifetime), giving a net lifetime of 8.4 years.{{cite web

| url=http://www.grida.no/climate/ipcc_tar/wg1/134.htm#4211

| title=Trace Gases: Current Observations, Trends, and Budgets

| work=Climate Change 2001, IPCC Third Assessment Report

| publisher=IPCC/United Nations Environment Programme}}

Methyl radicals can also be obtained by pyrolysis of azomethane, CH₃N=NCH₃, in a low-pressure system.

Methyl was discovered in interstellar medium in 2000 by a team led by Helmut Feuchtgruber who detected it using the Infrared Space Observatory. It was first detected in molecular clouds toward the centre of the Milky Way.{{cite web|title=ISO detects a new molecule in interstellar space|url=http://sci.esa.int/science-e/www/object/index.cfm?fobjectid=21831|work=Science & Technology|publisher=European Space Agency|access-date=17 June 2013}}

{{Reflist}}

{{Molecules detected in outer space}}

{{Hydrides by group}}

Category:Astrochemistry

Category:Free radicals

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