Oxidation-Reduction (Redox) Reaction
The combination of the processes involved in the flow of electrons from a reducing agent (reducer) to an oxidizing agent (oxidant). The total number of electrons lost by one substance is the same as the total number of electrons gained by another substance. Oxidation and reduction always occur together simultaneously and are really opposite sides of the same reaction, which is often called the redox reaction. In earlier years, oxidation referred to the combining of a substance with, or addition of, oxygen; and reduction meant the loss or reduction of oxygen. As chemistry became more advanced, it was seen that the real key to what was happening was the gain or loss of electrons. The following definitions now apply. Oxidation is the loss of electrons from the reducing agent (which is said to have "been oxidized" in the process). Since electrons carry negative charges, oxidation results in an increase of positive valence. Reduction is the acquiring of electrons (the ones lost in the oxidation process) by the oxidizing agent (which is said to have "been reduced" in the process). Because electrons (carrying negative charges) have been acquired, reduction results in a lowering (a reduction) of positive valence. It may be helpful to remember that the word "agent" refers to an active substance that produces or brings about some effect. Therefore the oxidizing agent is the substance that brings about the oxidation; the reducing agent is the substance that brings about the reduction.

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