Question

Explain electroplating with chemical equations.

Answer 1

Electroplating is the application of electrolytic cells in which a thin layer of metal is deposited onto an electrically conductive surface.

A cell consists of two electrodes (conductors), usually made of metal, which are held apart from one another. The electrodes are immersed in an electrolyte (a solution).

When an electric current is turned on, positive ions in the electrolyte move to the negatively charged electrode (called the cathode). Positive ions are atoms with one electron too few. When they reach the cathode, they combine with electrons and lose their positive charge.
At the same time, negatively charged ions move to the positive electrode (called the anode). Negatively charged ions are atoms with one electron too many). When they reach the positive anode they transfer their electrons to it and lose their negative charge.

In one form of electroplating, the metal to be plated is located at the anode of the circuit, with the item to be plated located at the cathode. Both the anode and the cathode are immersed in a solution which contains a dissolved metal salt (e.g., an ion of the metal being plated) and other ions which act to permit the flow of electricity through the circuit.
Direct current is supplied to the anode, oxidizing its metal atoms and dissolving them in the electrolyte solution. The dissolved metal ions are reduced at the cathode, plating the metal onto the item. The current through the circuit is such that the rate at which the anode is dissolved is equal to the rate at which the cathode is plated. Electroplating Example

A simple example of the electroplating process is the electroplating of copper in which the metal to be plated (copper) is used as the anode and the electrolyte solution contains the ion of the metal to be plated (Cu²⁺ in this example). Copper goes into solution at the anode as it is plated at the cathode. A constant concentration of Cu²⁺ is maintained in the electrolyte solution surrounding the electrodes:

anode: Cu(s) → Cu²⁺(aq) + 2 e^-

cathode: Cu²⁺(aq) + 2 e^- → Cu(s)