In the context of electrochemical cells, what happens during oxidation?

During oxidation in the context of electrochemical cells, a substance loses electrons. This process is fundamental to understanding redox reactions, where oxidation and reduction occur simultaneously.

When a substance is oxidized, its oxidation state increases because the loss of electrons results in a higher positive charge. For example, when iron (Fe) is oxidized to iron(III) ions (Fe³⁺), it loses three electrons. This phenomenon is crucial in electrochemical cells as it enables the flow of electrons from the anode to the cathode, generating electric current.

In redox reactions, the counterpart to oxidation is reduction, which involves the gaining of electrons. This interplay allows for energy transfer in electrochemical processes. The notion of charge stabilization relates to the overall system's dynamics but does not define the oxidation process itself. Therefore, recognizing that oxidation specifically refers to the loss of electrons is vital for understanding electrochemical reactions.