How is oxidation defined in chemistry?

In chemistry, oxidation is defined as the loss of electrons. This definition is rooted in the concept of redox reactions, where oxidation and reduction occur simultaneously. When a substance undergoes oxidation, it experiences an increase in oxidation state due to the removal of electrons. This process is crucial in various chemical reactions, including those involving metals and non-metals.

For instance, in the reaction between zinc and copper sulfate, zinc loses electrons to become zinc ions, thereby oxidizing. This loss of electrons enables it to react with another chemical species (the copper ions, in this case) that gains those electrons and undergoes reduction. The movement of electrons is fundamental to the understanding of how substances interact in redox chemistry.

This understanding contrasts with other definitions, such as the gain of protons or neutrons, which do not relate to the concept of oxidation. Protons and neutrons are subatomic particles that contribute to the nucleus of an atom, while oxidation specifically pertains to the electron transfer process. Additionally, the gain of electrons is defined as reduction, not oxidation, thereby clarifying the distinct roles these terms play in redox reactions.