* Ionic Bonding: Sodium chloride (NaCl) is held together by ionic bonds. This means that the sodium ions (Na+) and chloride ions (Cl-) are strongly attracted to each other due to electrostatic forces.
* Fixed Positions: These ions are locked in a rigid, crystalline lattice structure. They are not free to move around.
* No Free Charge Carriers: In order to conduct electricity, charged particles need to be able to move freely. Since the ions in a sodium chloride crystal are fixed, they cannot carry an electrical current.
However, sodium chloride does conduct electricity when dissolved in water or melted.
* Dissolving: When sodium chloride dissolves in water, the ionic bonds are broken, and the ions become free to move around in the solution.
* Melting: When sodium chloride melts, the ions are no longer fixed in the lattice structure and can move freely.
In both cases, the free movement of charged ions allows for the conduction of electricity.
