The statement, “Corrosion of metal is due to electrical currents of electrochemical origin, stop current stop corrosion” is true.

• Electrochemical corrosion of metals occurs when electrons from atoms at the surface of the metal are transferred to a suitable electron acceptor or depolarizer. Water must be present to serve as a medium for the transport of ions.
• The most common depolarizers are oxygen, acids, and the cations of less active metals.
• Because the electrons flow through the metallic object itself, the anodic and cathodic regions (the two halves of the electrochemical cell) can be at widely separated locations.
• Anodic regions tend to develop at locations where the metal is stressed or is protected from oxygen.
• Contact with a different kind of metal, either direct or indirect, can lead to corrosion of the more active one.
• Corrosion of steel can be inhibited by galvanizing, that is, by coating it with zinc, a more active metal whose dissolution leaves a negative charge on the metal which inhibits the further dissolution of Fe²⁺.
• Cathodic protection using an external voltage source is widely used to protect underground structures such as tanks, pipelines, and piers. The source can be a sacrificial anode of zinc or aluminum or a line-operated or photovoltaic power supply.

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