Peroksid

Peroksid refers to a family of chemical compounds that contain the peroxide group, characterized by an O–O single bond. They are divided into inorganic peroxides, such as metal peroxides, and organic peroxides in which the peroxide functionality is bound to carbon. The simplest and most widely encountered example is hydrogen peroxide (H2O2).

Inorganic peroxides include substances such as sodium peroxide (Na2O2), calcium peroxide (CaO2) and barium peroxide (BaO2). These compounds commonly act as sources of oxygen and as oxidizing agents. They can react with water or acids to produce hydrogen peroxide, oxygen, or hydroxide species, and their stability varies with temperature and moisture.

Organic peroxides feature carbon–oxygen–oxygen linkage (R–O–O–R′ or ROOR′) and are frequently used as radical initiators in polymerization or curing reactions. They are generally more unstable and can be sensitive to heat, friction, or shock, making handling and storage more hazardous than many inorganic peroxides. Some organic peroxides are also used as initiators in synthetic chemistry or as components in explosives.

Production and use vary by type. Hydrogen peroxide is industrially produced mainly by the anthraquinone process and is employed for bleaching, disinfection, and as an oxidizer in chemical synthesis. Inorganic peroxides are usually prepared by direct oxidation of oxides or elements with oxygen and serve roles in oxygen supply, bleaching, or oxidation. Organic peroxides are formed by reactions of hydroperoxides or autoxidation of organics and are valued for initiating polymerization, though they require stringent safety controls.

Safety and handling are critical for peroksider, as they are strong oxidizers with potential explosive or shock sensitivity in certain forms. Proper storage, segregation from organic materials, and temperature control are essential.