Methylene (compound)

"Methanediyl" and "Methylidene" redirect here. For the moieties, see Methylene bridge and Methylene group.
Methylene (compound)
Names
IUPAC name
Dihydridocarbon(2•)[1]
Other names
Identifiers
1696832
2465-56-7
ChEBI CHEBI:29357 Yes
ChemSpider 109779 Yes
56
Jmol-3D images Image
MeSH carbene
PubChem 123164
Properties
CH
22•
Molar mass 14.0266 g mol−1
Appearance Colourless gas
Reacts
Thermochemistry
193.93 J K−1 mol−1
Std enthalpy of
formation (ΔfHo298)
 386.39 kJ mol−1
Related compounds
Related compounds
 Methyl (CH3)
Methylidyne (CH)
Carbide (C)
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references

Methylene (systematically named methylidene, and dihydridocarbon), also called carbene is an organic compound with the chemical formula CH
2 (also written [CH
2]). It is a colourless gas that fluoresces in the mid-infrared range, and only persists in dilution, or as an adduct.

Methylene is the simplest carbene.[2]:p.7[3] It is usually detected only at very low pressures, very low temperatures, or as a short-lived intermediate in chemical reactions.[4]

Nomenclature

The trivial name carbene is the preferred IUPAC name. The systematic names methylidene and dihydridocarbon, valid IUPAC names, are constructed according to the substitutive and additive nomenclatures, respectively.

Methylidene is viewed as methane with two hydrogen atoms removed. By default, this name pays no regard to the radicality of the methylene. Although in a context where the radicality is considered, it can also name the non-radical excited state, whereas the radical ground state with two unpaired electrons is named methanediyl.

Methylene is also used as the trivial name for the substituent groups methanediyl (>CH
2), and methylidene (=CH
2). Methylene has an electron affinity of 0.65 eV [5]

Discovery and preparation

The compound was first detected and studied around 1960, by infrared spectroscopy in frozen gas matrix isolation experiments.[6][7] The first suggested use of methylene was by D. Duck in 1944.[8][9]

Methylene can be prepared, under suitable conditions, by decomposition of compounds with a methylidene or methanediyl group, such as ketene (ethenone) (CH
2=CO), diazomethane (linear CH
2=N
2), diazirine (cyclic [-CH
2-N=N-]) and diiodomethane (I-CH
2-I). The decomposition can be effected by photolysis, photosensistized reagents (such as benzophenone), or thermal decomposition.[4][10]

Chemical properties

Radicality

Many of methylene's electronic states lie relatively close to each other, giving rise to varying degrees of radical chemistry. The ground state is a triplet radical with two unpaired electrons (X̃3B1),[10] and the first excited state is a singlet non-radical (ã1A1). With the singlet non-radical only 38 kJ above the ground state,[10] a sample of methylene exists as a mixture of electronic states even at room temperature, giving rise to complex reactions. For example, reactions of the triplet radical with non-radical species generally involves abstraction, whereas reactions of the singlet non-radical not only involves abstraction, but also insertion or addition.

[CH
2]2•(X̃3B1) + H
2O → [CH
3]• + [HO]•
[CH
2](ã1A1) + H
2O → H
2CO + H
2 or H
3COH

The singlet state is also more sterospecific than the triplet.[10]

Structure

Unsolvated methylene will spontaneously autopolymerise to form various excited oligomers, the simplest of which, is the excited form of the alkene ethylene. The excited oligomers, decompose rather than decay to a ground state. For example, the excited form of ethylene decomposes to acetylene and atomic hydrogen.[10]

2 CH
2 → H
2CCH*
2 → HCCH + 2 H

Unsolvated, excited methylene will form stable ground state oligomers.

2 CH*
2 → H
2CCH
2

The ground state of methylene has an ionisation energy of 10.396 eV. It has a bent configuration, with H-C-H angle of 133.84 °,[10] and is thus paramagnetic. (The correct prediction of this angle was an early success of ab initio quantum chemistry.[10]) However conversion to a linear configuration requires only 5.5 kcal/mol.[10]

This state has a slightly higher energy (by about 9 kcal/mol) than the triplet state,[10] and its H-C-H angle is smaller, about 102°. In dilute mixtures with an inert gas, the two states will convert to each other until reaching an equilibrium.[10]

Chemical reactions

Organic chemistry

Neutral methylene complexes undergo different chemical reactions depending on the pi character of the coordinate bond to the carbon centre. A weak contribution, such as in diazomethane, yields mainly substitution reactions, whereas a strong contribution, such as in ethenone, yields mainly addition reactions. Upon treatment with a standard base, complexes with a weak contribution convert to a metal methoxide. With strong acids (e.g., fluorosulfuric acid), they can be protonated to give CH
3L+
. Oxidation of these complexes yields formaldehyde, and reduction yields methane.

Free methylene undergoes the typical chemical reactions of a carbene. Addition reactions are very fast and exothermic.[11]

When the methylene molecule is in its state of lowest energy, the unpaired valence electrons are in separate atomic orbitals with independent spins, a configuration known as triplet state.

Methylene may gain an electron yielding a monovalent anion methanidyl (CH•−
2), which can be obtained as the trimethylammonium (CH
3)4N+
 salt by the reaction of phenyl sodium C
6H
5Na with trimethylammonium bromide.[4] The ion is bent too, with a H-C-H angle of about 103°.[10]

Reactions with inorganic compounds

Methylene is also a common ligand in coordination compounds, such as copper methylene CuCH
2.[12]

Methylene can bond as a terminal ligand, which is called methylidene, or as a bridging ligand, which is called methanediyl.

See also

References

  1. ↑ 1.0 1.1 "methanediyl (CHEBI:29357)". Chemical Entities of Biological Interest. UK: European Bioinformatics Institute. 14 January 2009. IUPAC Names. Retrieved 2 January 2012.
  2. ↑ Roald Hoffman (2005), Molecular Orbitals of Transition Metal Complexes. Oxford. ISBN 0-19-853093-5
  3. ↑ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version:  (2006–) "carbenes".
  4. ↑ 4.0 4.1 4.2 W. B. DeMore and S. W. Benson (1964), Preparation, properties, and reactivity of methylene. In Advances in Photochemistry, John Wiley & Sons, 453 pages. ISBN 0470133597
  5. ↑ http://webbook.nist.gov/cgi/cbook.cgi?ID=C2465567&Units=SI&Mask=20#Ion-Energetics
  6. ↑ William B. DeMore, H. O. Pritchard, and Norman Davidson (1959), Photochemical experiments in rigid media at low temperatures. II. The reactions of methylene, cyclopentadienylene and diphenylmethylene. Journal of the American Chemical Society, volume 81, issue 22, pages 5874–5879. doi:10.1021/ja01531a008
  7. ↑ Marilyn E. Jacox and Dolphus E. Milligan (1963), 'Infrared study of the reactions of CH2 and NH with C2H2 and C2H4 in solid argon.Journal of the American Chemical Society, volume 85, issue 3, pages 278–282. doi:10.1021/ja00886a006
  8. ↑ "The Spin States of Carbenes. (No. 3036)", P.P. Gaspar and G.S. Hammond, Chapter 12 in "Carbene Chemistry", Vol. 1. W. Kirmse, Editor, Academic Press, New York, pp 235-274 (1964)
  9. ↑ "If I mix CH2 with NH4 and boil the atoms in osmotic fog, I should get speckled nitrogen." Walt Disney's Comics and Stories, issue 44, 1944
  10. ↑ 10.0 10.1 10.2 10.3 10.4 10.5 10.6 10.7 10.8 10.9 10.10 Isaiah Shavitt (1985), Geometry and singlet-triplet energy gap in methylene: A critical review of experimental and theoretical determinations. Tetrahedron, volume 41, issue 8, page 1531 doi:10.1016/S0040-4020(01)96393-8
  11. ↑ Milan Lazár (1989), Free radicals in chemistry and biology. CRC Press. ISBN 0-8493-5387-4
  12. ↑ Sou-Chan Chang, Zakya H. Kafafi, Robert H. Hauge, W. Edward Billups, and John L. Margrave (1987), Isolation and characterization of copper methylene (CuCH2) via FTIR matrix isolation spectroscopy. Journal of the American Chemical Society, volume 109 pages 4508-4513. doi:10.1021/ja00249a013.