Electrolysis is a chemical process that uses electrical energy to drive a non-spontaneous chemical reaction, typically by breaking chemical bonds in a compound. It occurs in an electrolytic cell, where two electrodes are placed in an electrolyte solution, and an external voltage is applied.

During electrolysis:

• Positive ions (cations) move to the cathode (negative electrode) and gain electrons (reduction).
• Negative ions (anions) move to the anode (positive electrode) and lose electrons (oxidation).

A classic example is the electrolysis of water, which splits water molecules (H₂O) into hydrogen gas (H₂) at the cathode and oxygen gas (O₂) at the anode.

Electrolysis is widely used in:

• Metal extraction (e.g., aluminum from bauxite)
• Electroplating metals
• Producing chemicals like chlorine and hydrogen

It is also a key technology in developing clean hydrogen fuel, contributing to future sustainable energy systems.