How is oxidation related to the loss of electrons?

Oxidation is defined as a chemical process in which an atom, ion, or molecule loses electrons as it interacts with another chemical species. This loss of electrons is a fundamental criterion for identifying oxidation within [oxidation-reduction (redox) reactions].123

The relationship between oxidation and electron loss is characterized by the following principles:

• Electron Transfer: In a redox reaction, the species being oxidized donates electrons to an oxidizing agent. This transfer results in an increase in the oxidized substance's [oxidation number].12
• Reciprocity: Oxidation and reduction are coupled processes; the loss of electrons by one species (oxidation) is always accompanied by the gain of electrons by another (reduction).34
• Generalized Theory: While the term "oxidation" originally referred specifically to the reaction of substances with oxygen, modern chemical theory recognizes electron loss as a universal definition that encompasses oxygen-atom transfer, hydrogen-atom loss, and direct electron transfer.21

By losing electrons, the substance undergoes a change in its composition and energy state, which dictates its subsequent chemical behavior and stability.1