* Solid State: In the solid state, ionic compounds exist as a rigid lattice structure. The ions are held tightly in fixed positions by strong electrostatic forces. This means there are no free-moving charge carriers (ions) to carry an electric current.
* Dissolved or Molten State: When dissolved in water or melted, the ionic lattice breaks down. The ions become free to move around.
* Dissolving: Water molecules surround the ions and pull them apart, disrupting the crystal lattice. The ions are now free to move independently in the solution.
* Melting: The heat energy overcomes the electrostatic forces holding the ions together in the lattice, allowing them to move freely.
* Conduction: When an electric potential is applied across the solution or molten ionic compound, the free ions move towards the oppositely charged electrode. This movement of charged particles constitutes an electric current.
In summary: Electrovalent compounds conduct electricity because they contain free ions that can carry the electrical current. These free ions are only available when the compound is dissolved in water or melted, allowing the ions to move freely.
