Oxidant

an electron reaction in a redox reaction called an oxidant. Oxidants oxidize other substances and are reduced by themselves. When it gets electrons, its own chemical value (or oxidation) decreases. Oxidants are usually lively non-metallic monotones (e.g.
O 2,
cl


2
2




Br2 ), metal ions (e.g.
Fe


3


,
Sn
4


), High price Oxygenated compounds
elements
such as KMnO 4 br, br K2




2


O

7

,
KClO3


,
HNO


3

,
H


2


SO 4

br (thick), PbO br br 2 br and peroxides (e.g. H br). 2


O

2


、
Na


2


O

2


、
BaO


2


）。 Whether a substance is an oxidant or a reducing agent cannot be absolutely. Because the same substance (sulfur dioxide in the following example) is used as an oxidant in one reaction and a reducing agent in another reaction. The size of oxidant oxidation capacity can be judged according to the size of
, the standard electrode potential E (volt) made up of its oxidation and reduction states. The higher (or more positive) the value of E,D, the stronger the oxidation capacity of the oxidant, or the stronger the oxidation state of the substance.