oksidation

Oksidation is a chemical process in which the oxidation state of atoms increases as electrons are lost, usually to an oxidizing agent. In classical terms, oxidation was defined as a reaction with oxygen, but the modern definition is based on electron transfer and redox chemistry. An oxidation reaction may involve oxygen, but it can also occur with other oxidants such as hydrogen peroxide, permanganate, or halogens, and it can occur without oxygen in many biological and organic reactions.

Mechanistically, oxidation involves the loss of electrons by one species and concurrent gain by another (the oxidant). The donor is called the reducing agent, and the acceptor is the oxidizing agent. The oxidation state is a formal accounting method used to track electron transfer. Oxidation can occur with the formation of bonds to oxygen or with the removal of hydrogen (dehydrogenation). In organic chemistry, common oxidation sequences include alcohols becoming aldehydes and then carboxylic acids, while metals can rise to higher positive oxidation states.

Examples range from everyday and industrial processes to biology. The rusting of iron involves iron moving from 0 to higher oxidation states in oxides. Combustion, such as methane reacting with oxygen to form carbon dioxide and water, is a rapid oxidation. In biology, glucose oxidation in cellular respiration releases energy as electrons are transferred to carrier molecules.

Applications and implications of oxidation span energy production, metal corrosion, organic synthesis, and environmental chemistry. Oxidation states and redox potentials are measured to predict reactivity. Control of oxidation is important in preventing damage, while targeted oxidation is a key step in many industrial processes and biosynthetic pathways.