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Acetone peroxide (/ æ s ə ˈ t ə ʊ n p ɛr ˈ ɒ k s aɪ d / ⓘ also called APEX and mother of Satan [3] [4]) is an organic peroxide and a primary explosive. It is produced by the reaction of acetone and hydrogen peroxide to yield a mixture of linear monomer and cyclic dimer, trimer, and tetramer forms. The monomer is dimethyldioxirane.
The Baeyer–Villiger oxidation is an organic reaction that forms an ester from a ketone or a lactone from a cyclic ketone, using peroxyacids or peroxides as the oxidant. [1] The reaction is named after Adolf von Baeyer and Victor Villiger who first reported the reaction in 1899.
Others have only peroxide ligands: molybdate reacts in alkaline media with peroxide to form red peroxomolybdate Mo(O 2) 2− 4. [6] The reaction of hydrogen peroxide with aqueous titanium(IV) gives a brightly orange-red colored peroxy complex that is a useful test for titanium as well as hydrogen peroxide. [5]
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.
The solution may be mixed before application or directly applied to the material, applying the sulfuric acid first, followed by the peroxide. Due to the self-decomposition of hydrogen peroxide, piranha solution should always be used freshly prepared (extemporaneous preparation).
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]
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 ...
Especially when in concentrated form, organic peroxides can decompose by self-oxidation, since organic peroxides contain both an oxidizer (the O-O bond) and fuel (C-H and C-C bonds). A "self-accelerating decomposition" occurs when the rate of peroxide decomposition generates heat at a faster rate than it can be dissipated to the environment ...