In a redox reaction, what happens to the reducing agent?

In a redox reaction, the reducing agent is the species that donates electrons to another substance, leading to the reduction of that substance. In this process, the reducing agent itself undergoes oxidation, which means it loses electrons. Since oxidation is defined as the loss of electrons, the reducing agent will undergo a change in its oxidation state, typically increasing.

This concept is central to understanding redox reactions. For instance, in a reaction where zinc metal is combined with copper(II) sulfate, zinc serves as the reducing agent. It donates electrons to copper ions, reducing them to metallic copper, while zinc itself becomes oxidized to zinc ions. The transformation of the reducing agent into a higher oxidation state is what makes it identifiable as the reducing agent in the first place, as it plays a crucial role in facilitating the overall electron transfer process.

In contrast, other options do not accurately describe the behavior of the reducing agent. For instance, stating that it remains unchanged misrepresents the essential role of the agent in the redox process, as it must necessarily undergo change. Describing it as disappearing may imply it is consumed without noting the change in its oxidation state, which is a key aspect of redox chemistry. Saying that it gets reduced is