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Galvanization is a process in which a protective layer of zinc is applied to iron or steel to prevent it from rusting or corroding. This is typically done by dipping the metal into molten zinc, which forms a protective coating on the surface. The process may also involve electroplating, where a thin layer of zinc is deposited onto the metal through an electric current.

When iron or steel is dipped into the molten zinc, a chemical reaction occurs between the zinc and the iron. This reaction forms a layer of zinc-iron alloy, which bonds strongly with the iron substrate. On the outermost surface, a layer of pure zinc adheres to the zinc-iron alloy, creating a multi-layered coating that is resistant to corrosion.

Galvanizing iron protects it from corrosion in the following ways: 1. **Physical Barrier:** The layer of zinc coating acts as a physical barrier, separating the iron from the surrounding environment. This prevents moisture, air, and other potentially corrosive substances from coming into contact with the iron and initiating the rusting process. 2. **Sacrificial Anode:** Zinc is more reactive than iron, which means it will corrode before the iron. As a result, if there are any breaks or imperfections in the zinc coating, the zinc will act as a "sacrificial anode." This means that the zinc will corrode first, protecting the iron beneath by diverting the corrosion process away from the underlying metal. To sum up, galvanization is a process that applies a protective zinc coating to iron or steel to prevent corrosion. It protects the metal by creating a physical barrier and acting as a sacrificial anode. This prolongs the life of the iron or steel by preventing rust and corrosion.