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explain oxidation and reduction?
Oxidation and reduction are two types of chemical reactions that often work together. Oxidation and reduction reactions involve an exchange of electrons between reactants. For many students, the confusion occurs when attempting to identify which reactant was oxidized and which reactant was reduced.

Oxidation occurs when a reactant loses electrons during the reaction. Reduction occurs when a reactant gains electrons during the reaction. This often occurs when metals are reacted with acid. Consider the reaction between zinc metal and hydrochloric acid.

Zn(s) + 2 HCl(aq) ? ZnCl2(aq) + H2(g)

If this reaction where broken down to the ion level:

Zn(s) + 2 H+(aq) + 2 Cl-(aq) ? Zn2+(aq) + 2 Cl-(aq) + 2 H2(g)

First, look at what happens to the zinc atoms. Initially, we have a neutral zinc atom. As the reaction progresses, the zinc atom loses two electrons to become a Zn2+ ion.

Zn(s) ? Zn2+(aq) + 2 e-.


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