Fe→Fe2++2e−cap F e right arrow cap F e raised to the 2 plus power plus 2 e raised to the negative power
One of the most fascinating intersections of these sciences is . Some metals, like aluminum and stainless steel, are technically very reactive. However, they corrode so quickly at first that they form a dense, ultra-thin oxide layer on their surface. This layer is non-porous and electrically insulating, effectively "unplugging" the electrochemical cell and stopping further decay. If this film is scratched, electrochemistry immediately kicks in to repair it—unless the environment (like chloride ions in salt) is aggressive enough to prevent healing. Controlling the Reaction Electrochemistry and Corrosion Science
This is where the actual damage happens. At the anode, metal atoms lose electrons and turn into ions that dissolve into the surrounding environment. For iron, this looks like: Fe→Fe2++2e−cap F e right arrow cap F e