perosides

Peroxides are a class of chemical compounds that contain a covalent bond between two oxygen atoms, specifically an oxygen-oxygen single bond (O-O). This O-O bond is relatively weak, making peroxides reactive and often unstable. The general formula for peroxides is R-O-O-R', where R and R' can be hydrogen, alkyl groups, or other organic or inorganic substituents. Hydrogen peroxide (H2O2) is the most well-known example, and it is a common antiseptic and bleaching agent.

The presence of the weak O-O bond is responsible for the characteristic properties of peroxides. They are often strong oxidizing agents, meaning they readily accept electrons from other substances, causing those substances to be oxidized. This oxidizing power makes them useful in various applications, including disinfection, bleaching, and as initiators in polymerization reactions. However, their reactivity also means they can be hazardous. Many peroxides are sensitive to heat, shock, or friction and can decompose exothermically, sometimes explosively.

Organic peroxides, where R and R' are organic groups, are particularly important in industrial chemistry. They are widely used as free radical initiators in the production of polymers like polyethylene and polyvinyl chloride. Inorganic peroxides, such as sodium peroxide (Na2O2) and barium peroxide (BaO2), are also strong oxidizers and find use in applications like bleaching and in the production of oxygen. Due to their inherent instability, the handling, storage, and transportation of peroxides require strict safety precautions to prevent accidents.