In a solution of an ionic compound in water, ions are present, allowing for the conduction of electricity as charged particles move to the opposite electrodes. Ionic compounds in the solid state do not conduct electricity due to their rigid structure, but in the molten state, the electrostatic forces are overcome, enabling ions to move freely and conduct electricity.
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In ionic compounds, such as salts, ions are held together by strong electrostatic forces in a crystalline lattice. In the solid state, these ions are fixed in their positions and unable to move, leading to poor electrical conductivity. However, in the molten state or when dissolved in a solution, the crystal lattice breaks down, and the ions become free to move. This movement of ions allows the compound to conduct electricity. In solution or molten states, cations and anions migrate towards the respective electrodes, facilitating the flow of electric current through the ionic compound.