In ionic compounds, what happens to the ions in their solid state?

In ionic compounds, the ions are held in place within a rigid lattice structure when in their solid state. This is due to the strong electrostatic forces of attraction between the positively charged cations and the negatively charged anions. These forces create a stable arrangement where each ion is surrounded by oppositely charged ions, effectively locking them into fixed positions.

The rigidity of this lattice structure is what gives ionic solids their characteristic properties, such as high melting and boiling points, as well as their inability to conduct electricity in solid form. While the ions are not free to move, they can become mobile when the solid is dissolved in water or melted, leading to electrical conductivity in those states. This stability in the solid phase contrasts with the behavior of atoms or molecules that might move more freely in other types of materials.