Which property is NOT associated with ionic compounds?

Ionic compounds are known for their distinct characteristics due to the strong electrostatic forces between the oppositely charged ions. One of their most notable properties is that they have high melting and boiling points, which occur because a substantial amount of energy is required to break the ionic bonds that hold the ions together in a lattice structure.

When we consider the electrical conductivity of ionic compounds, they typically conduct electricity when they are dissolved in water or molten, allowing the ions to move freely. However, in their solid state, the ions are held firmly in place within the lattice structure and cannot move freely, which is why ionic compounds do not conduct electricity in this form.

Regarding solubility, ionic compounds tend to be soluble in polar solvents, such as water, because the polar molecules can stabilize the individual ions once they are separated from the lattice.

Therefore, the characteristic of poor electrical conductivity in the solid state aligns with what is generally accepted for ionic compounds, confirming that the first three properties mentioned are indeed associated with them. It is this understanding of ionic compounds' behavior in different states that solidifies the choice linked to good conductivity in solid form as the one that does not apply.