Question

Ionic compounds are good conductors of electricity under specific conditions . Name 2 conditions and give reasons

Answer 1

Ionic compounds are not good at conducting electricity in the solid state, but they do conduct electricity when dissolved in water or when they are in the molten state (liquid by melting).
The reason why ionic compounds do not pass electrons well is because of the bond of electrons that were passed over and the attraction made by the balance of ion charge.
If you were to make a solution of ions, in that case it would conduct electricity well, but in that case, the ions freely move which is the opposite case to the ionic compound structure. The ions are also able to move freely when the ionic compound has been heated enough to melt the substance

Answer 2

Answer:

Ionic compounds consist of ions which are charged particles.

Ionic compounds in the solid state do not conduct electricity because the movement of ions in the solid is not  possible due to their rigid structure.

An aqueous solution of ionic compounds  consists of mobile ions which allow them to move towards oppositely charged electrodes and thus the  conduction of electricity is possible.

In molten state the electrostatic forces of attraction between the oppositely charged ions are overcome due to  heat. Thus, the ions move freely and conduct electricity.