How do ionic compounds behave in their solid state regarding electrical conductivity?

Ionic compounds, when in their solid state, do not conduct electricity. This is primarily due to the fixed position of the ions within the rigid lattice structure of the solid. The ions are held together by strong electrostatic forces between the positively charged cations and negatively charged anions, which restricts their movement. Since electrical conductivity depends on the flow of charged particles, and in solid ionic compounds, the ions are not free to move, there is no electrical conductivity.

However, if ionic compounds are melted or dissolved in a solvent, the rigid structure breaks down, and the ions become free to move. This mobility allows them to conduct electricity in these states. Thus, while the solid state of ionic compounds does not enable conductivity, their behavior changes with temperature or phase, leading to conductivity when they are either molten or dissolved in solution.