How does rusting demonstrate electron transfer in a redox reaction?

Rusting is a classic example of an oxidation-reduction (redox) reaction, a process defined by the transfer of electrons between chemical species.12

In the context of rusting, the reaction demonstrates electron transfer through the following steps:

• Oxidation of Iron: When iron is exposed to oxygen and moisture, atoms on the metal's surface lose electrons. This loss of electrons is the oxidation half of the reaction, transforming the iron into iron ions.34
• Reduction of Oxygen: These released electrons are accepted by oxygen molecules present in the environment. This gain of electrons constitutes the reduction half of the reaction.24
• Formation of Rust: The moisture acts as a medium that facilitates this essential electron transfer. The resulting iron ions combine with oxygen and water to form hydrated iron oxides, which we recognize as the reddish-brown substance known as rust.34

Essentially, the iron acts as a reducing agent by giving up electrons, while oxygen acts as an oxidizing agent by accepting them. This continuous exchange of electrons is the fundamental mechanism that drives the corrosion of the metal.24