In terms of electron transfer, what defines oxidation and reduction?

Oxidation and reduction are fundamental concepts in chemistry that describe the transfer of electrons between species.

In the context of electron transfer, oxidation is defined specifically as the loss of electrons. When a substance undergoes oxidation, it has a higher oxidation state after the reaction because it has lost negative charge (electrons). This loss of electrons makes the oxidized species more positively charged or less negatively charged.

Reduction, on the other hand, is defined as the gain of electrons. When a substance is reduced, it has a lower oxidation state due to the addition of electrons. Gaining electrons impart more negative charge, making the reduced species more negatively charged or less positively charged.

Therefore, the correct definition stating that oxidation is the loss of electrons and reduction is the gain of electrons aligns perfectly with the accepted definitions in redox chemistry, which is essential for understanding various chemical reactions, such as combustion, corrosion, and biological processes like cellular respiration.