What leads to galvanic corrosion?

Galvanic corrosion occurs when two different metals are in electrical contact with each other while being immersed in an electrolyte, such as water. The fundamental principle behind this process is that the more noble metal (with a higher electrode potential) will resist corrosion, while the less noble metal (with a lower electrode potential) will corrode preferentially. This creates a galvanic cell, where the environment facilitates the flow of electrons, leading to the deterioration of the less noble metal.

The presence of dissimilar metals is crucial because when they come into contact, they establish an electrochemical reaction. This reaction results in the transfer of electrons from the less noble metal to the more noble one, leading to corrosion at the site of the less noble metal. This phenomenon is common in marine environments where metals such as aluminum and steel may be used together, often necessitating protective measures like coatings or the use of sacrificial anodes to mitigate the effects.

While exposure to moisture can promote corrosion processes, it is the contact between dissimilar metals that specifically defines galvanic corrosion. High temperatures may accelerate corrosion processes in general but do not directly cause galvanic corrosion. The application of paint generally serves as a protective barrier to prevent corrosion rather than being a contributing factor. Thus, the