the total number of electrons (electron) that an atom either gains or loses in order to form a chemical bond (chemical bonding) with another atom.

Each atom that participates in an oxidation-reduction reaction (q.v.) is assigned an oxidation number that reflects its ability to acquire, donate, or share electrons. The iron ion Fe³⁺, for example, has an oxidation number of +3 because it can acquire three electrons to form a chemical bond, while the oxygen ion O²⁻ has an oxidation number of −2 because it can donate two electrons. In an electronically neutral substance, the sum of the oxidation numbers is zero; for example, in hematite (Fe₂O₃) the oxidation number of the two iron atoms (+6 in total) balances the oxidation number of the three oxygen atoms (−6).

Certain elements assume the same oxidation number in different compounds; fluorine, for example, has the oxidation number −1 in all its compounds. Others, notably the nonmetals and the transition elements, can assume a variety of oxidation numbers; for example, nitrogen can have any oxidation number between −3 (as in ammonia, NH₃) and +5 (as in nitric acid, HNO₃).

In the nomenclature of inorganic chemistry, the oxidation number of an element that may exist in more than one oxidation state is indicated by a roman numeral in parentheses after the name of the element—e.g., iron(II) chloride (FeCl₂) and iron(III) chloride (FeCl₃).