Oksidanten

Oksidanten, or the oxidant, is a substance that accepts electrons from another species in a redox (oxidation-reduction) reaction, becoming reduced in the process. In such reactions, oxidants act as electron acceptors and increase the oxidation state of the species being oxidized. The strength of an oxidant is related to its standard reduction potential (E°); substances with higher E° values are stronger oxidants.

In aqueous and many other solutions, the reactivity of oxidants depends on conditions such as pH and solvent, but in general, strong oxidants readily react with many reducing agents and can drive rapid chemical change. Common oxidants include molecular oxygen (O2), hydrogen peroxide (H2O2), ozone (O3), chlorine (Cl2) and hypochlorite (ClO−), permanganate (MnO4−), and dichromate (Cr2O7^2−). Nitrates (NO3−) and perchlorates (ClO4−) also serve as oxidants under appropriate conditions.

Applications of oxidants span disinfection, bleaching, and chemical synthesis. Oxygen serves as the terminal oxidant in aerobic respiration, enabling energy production in many organisms. Hydrogen peroxide and chlorine-based species are widely used for sterilization and water treatment, while permanganate and dichromate act as oxidants in organic synthesis and analytical chemistry.

Safety and handling: oxidants can be highly reactive and may ignite or explode when in contact with fuels or reducing agents. They can be corrosive or toxic and require careful storage, separation from incompatible materials, and proper protective equipment in handling.

See also: redox reaction, reducing agent, standard reduction potential, oxidation state.