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A galvanic cell uses spontaneous redox reactions to generate electrical energy, while an electrolytic cell applies electrical energy to drive nonspontaneous reactions. In a galvanic cell, chemical energy converts to electrical energy. In an electrolytic cell, an external power source supplies the energy needed to force the electrochemical reaction to occur.

The cathode is where reduction occurs, and the anode is where oxidation occurs. You can remember this with the mnemonic 'Red Cat'—reduction at cathode. The electrode with the higher standard reduction potential acts as the cathode and is reduced, while the electrode with lower reduction potential acts as the anode and is oxidized.

The electrolyte solution contains ions and dissolved salts that enable electron flow and ion movement between electrodes. When external voltage is applied, ions in the electrolyte are attracted to electrodes with opposite charges, facilitating the half-reactions. The electrolyte's concentration and conductivity directly affect the cell's resistance and current flow.

Electroplating deposits one metal onto another metal's surface using an electrolytic cell. The metal to be plated comprises the anode and is oxidized to form cations. These cations are then reduced at the cathode, forming a thin metal layer on the surface. The amount of metal plated depends on the applied current and the concentration of metal cations available.

Faraday's constant relates electrical current to moles of electrons transferred. Electrical charge equals current in amperes multiplied by time in seconds. Dividing this charge by Faraday's constant (96,485 coulombs per mole) yields the moles of electrons transferred. This determines how much metal cation is reduced and deposited during electroplating.

A redox reaction involves electron transfer between chemical species. Oxidation occurs when a species loses electrons, while reduction occurs when a species gains electrons. In electrolytic cells, applied electrical energy drives these redox reactions to occur. The oxidation half-reaction happens at the anode, and the reduction half-reaction occurs at the cathode.

The standard reduction potential of electrode materials determines which metal is oxidized or reduced first. Metals with higher reduction potentials are reduced preferentially. Higher electrolyte concentration increases solution conductivity, lowering resistance and increasing current flow, which allows more metal ions to be reduced and deposited onto the cathode surface.