Molecular autoionization

In chemistry, molecular autoionization is a chemical reaction between molecules of the same substance to produce ions. If a pure liquid partially dissociates into ions, it is said to be self-ionizing. In most cases the oxidation number on all atoms in such a reaction remains unchanged. Such autoionization can be protic, or non-protic.

Examples

Protic solvents

s often undergo some autoionization :

2 H2O <=> H3O+ + OH-
*The self-ionization of water is particularly well studied, due to its implications for acid-base chemistry of aqueous solutions.
2 NH3 <=> NH4+ + NH2-
2 H2SO4 <=> H3SO4+ + HSO4-
3 HF <=> H2F+ + HF2-
*Here proton transfer between two HF combines with homoassociation of and a third HF to form
Non-protic solvents
2 PF5 <=> PF6- + PF4+
N2O4 <=> NO+ + NO3-
* Here the nitrogen oxidation numbers change from to.
2 BrF3 <=> BrF2+ + BrF4-

These solvents all possess atoms with odd atomic numbers, either nitrogen or a halogen. Such atoms enable the formation of singly charged, nonradical ions, which are the most favorable autoionization products. Protic solvents, mentioned previously, use hydrogen for this role. Autoionization would be much less favorable in solvents such as sulfur dioxide or carbon dioxide, which have only even-atomic-number atoms.

Coordination chemistry

Autoionization is not restricted to neat liquids or solids. Solutions of metal complexes exhibit this property. For example, compounds of the type are unstable with respect to autoionization forming.

Molecular autoionization

Examples

Protic solvents

Non-protic solvents

Coordination chemistry