Organic peroxides is an organic compound containing peroxide functional group (ROOR '). If R 'is hydrogen, these compounds are called hydroperoxides, which are discussed in this article. Peresters are peroxy analogs of esters and have a general structure RC (O) OOR. The O-O bond of peroxides is easily broken, producing free radicals in the form of RO • (dots represent unpaired electrons). Therefore, Organic peroxides can be used as an initiator for some types of polymerization, such as epoxy resin used in glass reinforced plastics. MEKP and Benzoyl peroxide are commonly used for this purpose. However, the same properties also mean that Organic peroxides can intentionally or unintentionally initiate explosive polymerization in materials with unsaturated Chemical bond, a process that has been used in explosives. Organic peroxides,
The O-O bond length in peroxides is about 1.45 Å, and the R-O-O angle (R=H, C) is about 110 ° (water like). Typically, C − O − O − R (R=H, C) Dihedral angle is about 120 °. The O-O bond is relatively weak, with a bond dissociation energy of 45-50 kcal/mol (190-210 kJ/mol), which is less than half of the strength of the C-C, C-H, and C-O bonds.
Peroxides play an important role in biology. Many aspects of biodegradation or aging are attributed to the formation and decay of peroxides formed by oxygen in the air. A range of biological and artificial antioxidants are used to combat these effects. There are hundreds of known peroxides and hydroperoxides derived from fatty acids, steroids, and terpenes. Fatty acids form many 1,2-dioxenes. The biosynthesis of prostaglandins is carried out through endoperoxides (a class of bicyclic peroxides). In fireflies, Luciferase catalyzes the oxidation of Luciferin to produce peroxy compound 1,2-di Oxetane. Dineneneba oxheterocyclobutane is unstable and will spontaneously decay into carbon dioxide and excited ketones, which release excess energy through luminescence (Bioluminescence).