Final answer:
Solid ionic compounds are non-conductive due to the immobility of ions in their crystalline structure, while ionic solutions are conductive because the dissolution or melting frees the ions, allowing them to move and carry an electric current.
Step-by-step explanation:
Conductivity of Ionic Compounds in Different States
The ionic bonding model illustrates why solid ionic compounds are typically non-conductive, whereas ionic solutions conduct electricity. In a solid state, ionic compounds form a rigid crystalline structure where ions are held together by strong ionic bonds, which prevent the ions from moving. In this state, the immobility of ions means that solid ionic compounds cannot conduct electricity. However, when ionic compounds are dissolved in water or melted, the crystalline structure breaks down, allowing ions to move freely. This mobility of ions in aqueous solutions or molten state makes them good conductors of electricity.
If an ionic compound is in a liquid (molten) state, one would expect it to be conductive. This is because the strong ionic bonds are disrupted, giving cations and anions the freedom to move. This mobility of ions in the liquid state enables the transfer of electric current.