Chemistry Regents Practice Test 2026 – Complete Prep Resource

The process in which an element loses electrons is known as oxidation. When an element loses electrons, its oxidation state increases, reflecting a loss of negative charge. Oxidation commonly occurs in chemical reactions, especially in redox (reduction-oxidation) reactions, where one substance is oxidized and another is reduced.

In the context of oxidation, it’s essential to understand that this process often involves a transfer of electrons between substances. For instance, in a reaction between a metal and a non-metal, the metal tends to lose electrons and become positively charged, while the non-metal gains those electrons, leading to a reduction in its oxidation state.

The other terms related to different chemical processes help delineate why oxidation is specifically defined as the loss of electrons. Reduction refers to the gain of electrons, neutralization involves the reaction between acids and bases resulting in the formation of water and a salt, and combustion pertains to a chemical reaction involving a substance's reaction with oxygen, often producing heat and light. Therefore, these other processes do not encompass the specific action of losing electrons as clearly as oxidation does.