In organic chemistry, a radical anion is a free radical species that carries a negative charge. Radical anions are encountered in organic chemistry as reduced derivatives of polycyclic aromatic compounds, e.g. sodium naphthenide. An example of a non-carbon radical anion is the superoxide anion, formed by transfer of one electron to an oxygen molecule. Radical anions are typically indicated by
M\bullet
Many aromatic compounds can undergo one-electron reduction by alkali metals. The electron is transferred from the alkali metal ion to an unoccupied antibonding p-p п* orbital of the aromatic molecule. This transfer is usually only energetically favorable if the aprotic solvent efficiently solvates the alkali metal ion. Effective solvents are those that bind to the alkali metal cation: diethyl ether < THF < 1,2-dimethoxyethane < HMPA. In principle any unsaturated molecule can form a radical anion, but the antibonding orbitals are only energetically accessible in more extensive conjugated systems. Ease of formation is in the order benzene < naphthalene < anthracene < pyrene, etc. Salts of the radical anions are often not isolated as solids but used in situ. They are usually deeply colored.
Cyclooctatetraene is reduced by elemental potassium to the dianion. The resulting dianion is a 10-pi electron system, which conforms to the Huckel rule for aromaticity. Quinone is reduced to a semiquinone radical anion. Semidiones are derived from the reduction of dicarbonyl compounds.
The pi-radical anions are used as reducing agents in specialized syntheses. Being soluble in at least some solvents, these salts act faster than the alkali metals themselves. The disadvantages are that the polycyclic hydrocarbon must be removed. The reduction potential of alkali metal naphthalene salts is about 3.1 V (vs Fc+/0). The reduction potentials of the larger systems are lower, for example acenaphthalene is 2.45 V.[5] Many radical anions are susceptible to further reduction to dianions.
| naphthalene | Li+ | -3.09 V | can be reduced to dianion |
| naphthalene | Na+ | -3.09 V | |
| biphenyl | Li+ | -3.18 V | |
| anthracene | Na+ | -2.53 V | |
| perylene | Na+ | -2.19 V | includes dme solvate |
Addition of a proton source (even water) to a radical anion results in protonation, i.e. the sequence of reduction followed by protonation is equivalent to hydrogenation. For instance, the anthracene radical anion forms mainly (but not exclusively) 9,10-dihydroanthracene. Radical anions and their protonation are central to the Birch reduction.
Radical anions of polycyclic aromatic compounds function as ligands in organometallic chemistry.[7]
Cationic radical species are much less common than the anions. Denoted
M+\bullet
Some compounds containing the dioxygenyl cation can be prepared in bulk.[9]
Radical cations figure prominently in the chemistry and properties of conducting polymers. Such polymers are formed by the oxidation of heterocycles to give radical cations, which condense with the parent heterocycle. For example, polypyrrole is prepared by oxidation of pyrrole using ferric chloride in methanol:
n C4H4NH + 2 FeCl3 → (C4H2NH)n + 2 FeCl2 + 2 HClOnce formed, these polymers become conductive upon oxidation.[10] Polarons and bipolarons are radical cations encountered in doped conducting polymers.