Oxidanten

Oxidanten (Dutch for oxidants) are substances that accept electrons from other species during redox reactions. By taking electrons, they oxidize the donor and become reduced themselves. In chemistry, the term oxidant is used interchangeably with oxidizing agent, and the strength of an oxidant is often described by its standard reduction potential.

Common oxidants span inorganic and organic types. Inorganic oxidants include molecular oxygen (O2), ozone (O3), hydrogen peroxide (H2O2), hypochlorite (ClO−), permanganate (MnO4−), and various nitrates or nitrites that can act as electron acceptors under certain conditions. Organic oxidants encompass a range of compounds such as organic peroxides and nitro-containing species, which can participate in oxidation reactions similarly to their inorganic counterparts.

Oxidants play key roles in nature and industry. In biology, they serve as terminal electron acceptors in cellular respiration (oxygen is the primary oxidant in aerobic organisms; other oxidants can prevail in anaerobic environments, such as nitrate, nitrite, or sulfate). In industry, oxidants are used for disinfection and sterilization (for example, chlorine and ozone-based systems), bleaching, and as initiators or facilitators in polymerization and chemical synthesis.

Measurement and safety considerations are important. Redox potential (E°) and oxidation-reduction potential (ORP) quantify the oxidizing strength of a system. Because oxidants can be highly reactive and corrosive, they require careful handling, appropriate storage away from reductants and organic materials, and adherence to safety protocols.