What is the role of electrons in redox reactions?

In redox reactions, electrons play the role of being transferred from one atom to another.

In more detail, redox reactions, also known as oxidation-reduction reactions, are a type of chemical reaction that involve a transfer of electrons between two species. The term 'redox' comes from two concepts: reduction and oxidation. Oxidation refers to the loss of electrons, while reduction refers to the gain of electrons.

In a redox reaction, there is always an element that loses electrons (gets oxidised) and another that gains electrons (gets reduced). The atom that loses electrons becomes more positive (since electrons are negatively charged), and is known as the reducing agent. On the other hand, the atom that gains electrons becomes more negative and is known as the oxidising agent.

For example, in the reaction between sodium and chlorine to form sodium chloride, sodium loses an electron (is oxidised) and chlorine gains that electron (is reduced). Sodium is the reducing agent because it provides the electron that chlorine needs to become reduced.

Electrons play a crucial role in these reactions as their transfer leads to the formation of new compounds with different properties. Understanding the movement of electrons in redox reactions is fundamental to understanding many processes in chemistry, including how batteries work, how certain types of bacteria produce energy, and how our bodies utilise oxygen in cellular respiration.

In summary, electrons are the key players in redox reactions. They are the ones being transferred, causing atoms to be oxidised or reduced, and leading to the formation of new substances.