What is electrolytic reduction? Explain with the help of an example.

Electrolytic reduction is a process in which electricity is used to extract a metal from its compound by reducing its ions to pure metal. In this process, an electric current is passed through a molten or dissolved ore, causing the metal ions to gain electrons and get converted into metal atoms.

Explanation:
Many metals, especially reactive metals like aluminium, magnesium, and sodium, are found in nature as compounds (like oxides or chlorides). These compounds cannot be reduced by simple heating or chemical methods. Instead, we use electrolysis, where an electric current breaks the bond between the metal and oxygen (or another element).

During electrolysis:

• The metal ions move towards the cathode (negative electrode) where they gain electrons (reduction) and get deposited as pure metal.

• Non-metal ions move to the anode (positive electrode) and are oxidized.

Example:
Aluminium is obtained from its ore bauxite (Al₂O₃) by electrolytic reduction.

• The bauxite is first purified and converted to molten aluminium oxide.

• During electrolysis, aluminium ions (Al³⁺) move towards the cathode and get reduced to aluminium metal by gaining electrons.

• The oxygen ions (O²⁻) go to the anode and are released as oxygen gas.

Chemical reaction:
At cathode: Al³⁺ + 3e⁻ → Al
At anode: O²⁻ → ½O₂ + 2e⁻

Conclusion:
Electrolytic reduction is important to extract metals like aluminium from their compounds, where electricity helps in separating metal from other elements.