The correct response should focus on the interactions between the ionic compound and the polar solvent that result in the dissociation of the ionic compound. Here's a more detailed and accurate description:
When an ionic compound dissolves in a polar solvent, such as water, the positive and negative ions of the ionic compound are surrounded by the polar solvent molecules. The polar molecules have positive and negative ends (dipoles) that interact with the oppositely charged ions of the ionic compound. The positive end of the polar solvent molecules is attracted to the negatively charged ions (anions) of the ionic compound, while the negative end of the polar solvent molecules is attracted to the positively charged ions (cations).
These interactions lead to the ionic compound dissociating into its individual ions, as the solvent molecules pull the ions away from the solid structure. Ultimately, the ions become solvated (surrounded by solvent molecules), allowing the ionic compound to dissolve in the polar solvent effectively. This process is driven by the energy released during the solvation of the ions, which overcomes the lattice energy holding the ionic compound together.
This explanation encompasses the concepts of attraction between opposite charges, the role of solvent molecules, and the energy considerations involved in the dissolution process.