When two metals are immersed in an electrolyte connected by a wire, where do electrons flow?

In an electrochemical cell, when two metals are immersed in an electrolyte and connected by a wire, the flow of electrons occurs from the anode to the cathode. This flow happens because the anode is the site of oxidation, where metal atoms lose electrons and enter the electrolyte as positive ions. Electricity is the movement of electrons, so when oxidation takes place at the anode, the liberated electrons move through the wire toward the cathode.

At the cathode, reduction takes place, where the incoming electrons are accepted by ions in the electrolyte or by the metal itself. This process converts the positive ions back into neutral metal or contributes to the discharge of ions in the electrolyte, which completes the circuit. Understanding this electron flow is essential in the study of corrosion processes, as it helps in identifying how different metals behave in electrolyte solutions, ultimately affecting their susceptibility to corrosion.