Peroxide

Peroxide is a compound containing an oxygen-oxygen single bond or the peroxide anion, O₂²⁻. The O-O group in a peroxide is called the peroxide group or peroxo group. In contrast to oxide ions, the oxygen atoms in the peroxide ion have an oxidation state of −1.

The simplest stable peroxide is hydrogen peroxide. Superoxides, dioxygenyls, ozones and ozonides are considered separately. Peroxide compounds can be roughly divided into organic and inorganic. Whereas the inorganic peroxides have an ionic, salt-like character, the organic peroxides are dominated by the covalent bonds. The oxygen-oxygen chemical bond of peroxide is unstable and easily split into reactive radicals via homolytic cleavage.

Types of Peroxides

Inorganic Peroxides

Inorganic peroxides are compounds with an oxygen-oxygen bond and a metal. The most common peroxides are sodium peroxide, barium peroxide, and hydrogen peroxide.

Organic Peroxides

Organic peroxides are organic compounds containing the peroxide functional group (ROOR’). If the R’ is hydrogen, the compounds are called organic hydroperoxides. The O-O bond easily breaks, and free radicals of the form RO. are formed.

Uses of Peroxides

Peroxides have a variety of applications in the world today. They are used in detergents, bleaching agents, disinfectants, and as polymerization initiators. Hydrogen peroxide is commonly used as a mild disinfectant for cuts and scrapes.

Safety and Health Effects

Peroxides are harmful to the skin and eyes, and inhalation or ingestion can cause respiratory and digestive problems. They can also be explosive when mixed with organic materials.

See Also

• Oxide
• Hydrogen peroxide
• Sodium peroxide
• Barium peroxide

Peroxide Resources
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