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Redox (Oxidization States (Oxidation–reduction reactions are reactions in…
Redox
Oxidization States
Oxidation–reduction reactions are reactions in which electrons are transferred from one reactant to another.
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Redox reactions can be balanced using the half-reaction method, in which the oxidation and reduction reactions are balanced separately and then added. This method differs slightly for redox reactions in acidic and in basic solutions.
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The transfer of electrons does not need to be a complete transfer for the reaction to qualify as a redox reaction, such as the formation of a polar covalent bond.
The oxidation state or oxidation number is a positive or negative whole number that represents the 'charge' an atom in a compound would have if all shared electrons were assigned to the atom with a greater attraction for those electrons.
An oxidizing agent is a substance that causes the oxidation of another substance. An oxidizing agent gains electrons and is reduced.
A reducing agent is a substance that causes the reduction of another substance. A reducing agent loses electrons and is oxidized.
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A redox reaction is any reaction in which there is a change in the oxidation states of atoms in going from reactants to products.