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 Oxidation is a chemical reaction where a metal or nonmetal electron yields, and therefore increases its oxidation state. The opposite chemical reaction known as oxidationreduction, is when a chemical species accept electrons. These two reactions always occur together, is when a substance is oxidized, it is always the action of another isreduced

 An electron transfers and the other accepts. For this reason, we prefer the general term of redox reactions
 The more oxidizing substance that exists is the cationKrF because the Kr easily forms with F

 The most common oxidizing agents are potassium permanganate (KMnO4), potassium dichromate (K2Cr2O7), hydrogen peroxide (H2O2),nitric acid (HNO3), the hipohalitos and HALATES (eg sodium hypochlorite (NaClO) very oxidant in alkaline medium, the potassium bromate (KBrO3)). Ozone (O3) is a strong oxidantOxidation rates
Slow oxidation
Which almost always occurs in metals by water or air, causing erosion and loss of brightness and other properties characteristic of metals,releasing negligible amounts of heat, to melt a metal oxidation is accelerated, but the heat comes mainly from source that melted the metal and non-chemical process (anexception would be the welding aluminum.)

 Rapid oxidation
 Which occurs during what would already be burning, releasing significant amounts of heat, in the form of fire, andoccurs primarily in substances containing carbon and hydrogen (hydrocarbons)
 Combinations

When oxygen is combined with metal oxides can be either basic or peroxides, theseoxides are characterized by basic type.

If oxygen is combined with a nonmetal oxides form acids also called characterized as anhydrides and acid type (acting as an acid).
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