1. The Nature of Ionic Compounds

* Ionic compounds are formed by the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions). These ions are held together in a rigid, crystalline lattice structure.

2. The Solid State: No Conductivity

* In the solid state, the ions are locked in place within the crystal lattice. While they have charges, they are unable to move freely. This lack of mobile charge carriers is why solid ionic compounds are poor conductors of electricity.

3. The Liquid State: Free Ions and Conductivity

* When an ionic compound is melted, the strong electrostatic forces holding the ions together are weakened. The ions gain the freedom to move around within the liquid.

* This mobility of ions is crucial for conductivity. When a voltage is applied across the molten ionic compound, the positively charged ions (cations) migrate towards the negative electrode (cathode), and the negatively charged ions (anions) migrate towards the positive electrode (anode).

* This movement of charged particles constitutes an electric current.

In Summary:

The ability of molten ionic compounds to conduct electricity stems from the release of ions from the rigid lattice structure, allowing them to move freely and carry an electrical current.