Methylene (compound)

Methylene (IUPAC name: Methylidene, also called carbene or methene) is an organic compound with the chemical formula (also written ). 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. It is usually detected only at very low temperatures, or as a short-lived intermediate in chemical reactions.

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, and methylidene.

Methylidene group


A methylidene group is any part of a molecule that consists of a CH2= group. The group may be represented as \dCH2, where the '=' denotes the double bond.

In contrast, methylene is connected to the rest of the molecule by two single bonds. The distinction is often important, because the double bond is chemically different from two single bonds.



The same name (methylidene) was used for the distinct molecule CH2, also known as carbene. Formerly the methylene name was used for all three isomers (methylene, methylidene, and carbene).

Many organic compounds are named and classified as if they were the result of substituting a methylidene group for two adjacent hydrogen atoms of some parent molecule (even if they are not actually obtained that way). Thus, for example, methylenecyclopropene is named after cyclopropene.

Discovery and preparation
Methylene can be prepared by decomposition of compounds with a methylidene or methanediyl group, such as ketene (ethenone) (=CO), diazomethane (linear =), diazirine (cyclic [--N=N-]) and diiodomethane (I--I). The decomposition can be effected by photolysis, photosensitized reagents (such as benzophenone), or thermal decomposition. Methylene can be produced by photolysis of diazomethane. In its ultraviolet spectrum, gaseous methylene absorbs at around 141.5 nm. It was shown to have a bond angle of about 140°.

The reactions of methylene were also studied around 1960 by infrared spectroscopy using matrix isolation experiments.

Radical character
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), and the first excited state is a singlet non-radical (ã1A1). With the singlet non-radical only 38 kJ above the ground state, 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.
 * 2•(X̃3B1) + → • + [HO]•
 * (ã1A1) + →  +  or

The singlet state is also more stereospecific than the triplet.

Methylene spontaneously autopolymerises 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.
 * 2 →  → HCCH + 2 H

Unsolvated, excited methylene will form stable ground state oligomers.
 * 2 →

Structure
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°, and is thus paramagnetic. (The correct prediction of this angle was an early success of ab initio quantum chemistry. ) However conversion to a linear configuration requires only 5.5 kcal/mol.

The singlet state has a slightly higher energy (by about 9 kcal/mol) than the triplet state, 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.

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. 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.

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, which can be obtained as the trimethylammonium (4) salt by the reaction of phenyl sodium with trimethylammonium bromide (4). The ion has bent geometry, with a H-C-H angle of about 103°.

Reactions with inorganic compounds
Methylene is also a common ligand in coordination compounds, such as copper methylene.

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

In popular culture
The formula of the methylene molecule (CH2) was mentioned as part of a Disney comic by the Donald Duck character in a comic in 1944 in a humorous vein. In the same spirit, the comic was eventually cited in the scientific literature by Peter Gaspar and George S. Hammond. The comic has been cited in other sources since, including a widely adopted textbook in organic chemistry by Robert Morrison and Robert Boyd.