The electrical conductivity of ionic compounds is generally quite low when they are in a solid state. This is because the ions in a solid are tightly bound to their lattice positions and are unable to move freely. However, when an ionic compound is dissolved in water or another polar solvent, the ions become separated from each other and are free to move, allowing the compound to conduct electricity. The electrical conductivity of an ionic solution increases with the concentration of the compound, as there are more ions present to carry the electrical current.

The electrical conductivity of ionic compounds can also be affected by the temperature. As the temperature increases, the ions in a compound become more mobile, allowing the compound to conduct electricity more efficiently. This is why some ionic compounds, such as sodium chloride, become more conductive when they are heated.

In summary, the electrical conductivity of ionic compounds is generally low in a solid state but increases when the compound is dissolved in a solvent or when the temperature is increased.