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In addition to hydrogen peroxide, some other major classes of peroxides are: Peroxy acids, the peroxy derivatives of many familiar acids, examples being peroxymonosulfuric acid and peracetic acid, and their salts, one example of which is potassium peroxydisulfate. Main group peroxides, compounds with the linkage E−O−O−E (E = main group ...
Hydrogen peroxide is a chemical compound with the formula H 2 O 2.In its pure form, it is a very pale blue [5] liquid that is slightly more viscous than water.It is used as an oxidizer, bleaching agent, and antiseptic, usually as a dilute solution (3%–6% by weight) in water for consumer use and in higher concentrations for industrial use.
In chemistry, main group peroxides are peroxide derivatives of the main group elements. Many compounds of the main group elements form peroxides (R−O−O−R'), and a few are of commercial significance. [1]
The general structure of an organic peroxide. In organic chemistry, organic peroxides are organic compounds containing the peroxide functional group (R−O−O−R′).If the R′ is hydrogen, the compounds are called hydroperoxides, which are discussed in that article.
The use of peroxide compounds in detergents is often reflected in their trade names; for example, Persil is a combination of the words perborate and silicate. Some peroxide salts release oxygen upon reaction with carbon dioxide. This reaction is used in generation of oxygen from exhaled carbon dioxide on submarines and spaceships.
Barium peroxide arises by the reversible reaction of O 2 with barium oxide. The peroxide forms around 500 °C and oxygen is released above 820 °C. [1] 2 BaO + O 2 ⇌ 2 BaO 2. This reaction is the basis for the now-obsolete Brin process for separating oxygen from the atmosphere. Other oxides, e.g. Na 2 O and SrO, behave similarly. [4]
Sodium peroxide is an inorganic compound with the formula Na 2 O 2.This yellowish solid is the product of sodium ignited in excess oxygen. [3] It is a strong base. This metal peroxide exists in several hydrates and peroxyhydrates including Na 2 O 2 ·2H 2 O 2 ·4H 2 O, Na 2 O 2 ·2H 2 O, Na 2 O 2 ·2H 2 O 2, and Na 2 O 2 ·8H 2 O. [4] The octahydrate, which is simple to prepare, is white, in ...
Many industrial peroxides are produced using hydrogen peroxide. Reactions with aldehydes and ketones yield a series of compounds depending on conditions. Specific reactions include addition of hydrogen peroxide across the C=O double bond: R 2 C=O + H 2 O 2 → R 2 C(OH)OOH. In some cases, these hydroperoxides convert to give cyclic diperoxides: