Rusting

Rusting is a corrosion process primarily affecting iron and its alloys, leading to the formation of an orange-brown flaky coating that is commonly known as rust.
Rust is actually a mixture of various hydrated iron(III) oxides and hydroxides such as Fe2O3.xH2O and Fe(OH)3.
The process of rusting accelerates in the presence of electrical conductors like saltwater, acid or base, and slows in a dry and oxygen-free environment.

The process of rusting involves two half-cell reactions: an anode reaction that takes place at a region of the metal surface and results in the oxidation of iron to iron(II) ions, and a cathode reaction that occurs at a separate region of the metal surface and reduces oxygen in the presence of water.
The iron metal acts as the anode and corrodes, losing electrons to become iron(II) ions: Fe → Fe2+ + 2e-
The dissolved oxygen in water, with assistance from hydrogen ions, takes up these electrons at the cathode, forming water: O2 + 4H+ + 4e- → 2H2O
Under damp conditions, the iron(II) ions are further oxidized to iron(III) ions which react with oxygen and water to produce rust: 4Fe2+ + O2 + 4H2O → 4Fe(OH)3

Rusting can lead to significant economic losses due to damage to metal structures and degradation of their mechanical properties.
In addition to increased fragility and loss of mechanical strength, the presence of rust can also cause aesthetic deterioration and potentially health risks due to contamination of drinking water or food contact surfaces.

One common way to prevent rusting is by galvanising, which involves coating the iron or steel surface with a protective layer of zinc.
Another method, known as cathodic protection, involves attaching a more reactive metal (e.g., magnesium) to the iron surface to act as a sacrificial anode.
Rusting can also be prevented or delayed by physical and chemical barriers such as paint, oil or oxidation-resistant alloys.

Understanding the redox reactions involved in the rusting process helps in designing strategies to prevent or mitigate rusting.
Rusting presents an interesting case of corrosion as a naturally occurring, spontaneous redox process that can be slowed down or prevented using electrochemical principles and techniques.