peroxidy

Peroxides are chemical compounds characterized by a peroxide group, an O−O single bond, within their structure. The best-known example is hydrogen peroxide (H2O2). Peroxides are typically divided into inorganic peroxides, organic peroxides, and hydroperoxides (the latter containing the O−O bond adjacent to a hydrogen, −OOH). Inorganic peroxides include alkali and alkaline earth peroxides such as sodium peroxide (Na2O2) and barium peroxide (BaO2); many metal peroxides derive from the reaction of a metal oxide with oxygen. Organic peroxides feature the O−O bond linking two hydrocarbon fragments, exemplified by benzoyl peroxide and tert‑butyl peroxide; these compounds are important as radical initiators in polymerization and curing processes. Hydrogen peroxide, while also a peroxide, is often discussed separately due to its wide use and unique properties.

The O−O bond in peroxides is comparatively weak relative to most covalent bonds, so peroxides are typically reactive oxidants that decompose to generate radicals and oxygen. H2O2 can decompose thermally or catalytically (often with transition metals or enzymes). Industrially, hydrogen peroxide is produced by the anthraquinone process and used as an oxidant or bleaching agent. Inorganic peroxides are prepared by direct oxidation of oxides with oxygen, or by reaction of hydroxides with oxygen; some are formed by the combination of alkali metals with O2.

Applications include bleaching and disinfection (H2O2), polymer manufacturing and resin curing (organic peroxides), and niche roles in propellants and chemistry that require controlled oxygen release. Safety considerations are important: peroxides can be shock- or heat-sensitive, may form explosive mixtures with organic materials, and require careful storage and handling.