Peroksiides

Peroksiides are chemical compounds characterized by the presence of a peroxide functional group, which consists of an oxygen–oxygen single bond (–O–O–). This structure distinguishes them from other oxygen-containing compounds such as oxides or alcohols. Peroxide bonds are relatively unstable compared to other covalent bonds, making peroksiides reactive and often useful in various industrial and laboratory applications.

Peroksiides can be classified into organic and inorganic types. Organic peroksiides include compounds like hydrogen peroxide (H₂O₂), which is a simple yet important peroksiide used as a disinfectant, bleaching agent, and oxidizing agent. Other examples include organic hydroperoxides (R–OOH) and diacyl peroksiides (R–CO–O–O–CR), which are commonly used in polymerization reactions, such as the curing of epoxy resins.

Inorganic peroksiides, such as sodium perokside (Na₂O₂) and barium perokside (BaO₂), are ionic compounds that decompose into metal oxides and oxygen gas when heated. These compounds are often employed in oxygen generation systems, such as those used in spacecraft or underwater breathing apparatus.

Peroksiides are highly reactive due to the weak O–O bond, which can lead to spontaneous decomposition, especially in the presence of catalysts, heat, or organic materials. This reactivity makes them potentially hazardous, requiring careful handling and storage to prevent explosions or fires. Proper storage conditions, such as refrigeration and exclusion from organic contaminants, are essential for maintaining stability.

Applications of peroksiides extend beyond industrial uses. In environmental remediation, peroksiides are utilized in advanced oxidation processes to break down pollutants. They also play a role in organic synthesis, where controlled oxidation reactions are necessary for producing pharmaceuticals and specialty chemicals. Despite their utility, their oxidative nature necessitates strict safety protocols to mitigate risks associated with their use.