Oxidatiestaat

Oxidatiestaat, also known as the oxidation state or oxidation number, is a theoretical charge assigned to an atom in a chemical compound. It is a bookkeeping device used to keep track of electron transfer in redox reactions. The oxidation state refers to the number of electrons an atom would either lose or gain if all bonding electrons were transferred to the more electronegative element. By convention, oxygen is normally assigned an oxidation state of –2, hydrogen +1, and fluorine –1.

In an uncharged compound, the sum of the oxidation states of all atoms must equal zero. In charged ions, the sum equals the ion’s charge. For example, in the sulfate ion SO₄²⁻, sulfur typically has a +6 oxidation state, each oxygen –2, and the total is –2 as required. The oxidation state is not an observable property; it is a formalism that aids in elemental analysis, chemical formula construction, and the deduction of possible reaction mechanisms.

The assignment of oxidation states follows a set of rules standardized by the International Union of Pure and Applied Chemistry. These rules account for electronegativity differences, special cases such as metal–ligand bonding in coordination compounds, and common oxidation numbers for transition metals. While the oxidation state concept simplifies complex electronic structures, it remains a fundamental tool in teaching and practicing inorganic chemistry, allowing chemists to predict reactivity, understand electron flow, and balance redox equations.