The correct answer is Option C: If assertion is correct but reason is incorrect.

Explanation:

• Assertion: LiCl (Lithium Chloride) is indeed predominantly a covalent compound. This is due to the high polarizing power of the small lithium ion (Li⁺), which distorts the electron cloud of the larger chloride ion (Cl⁻), resulting in a significant degree of electron sharing and hence covalency.


• Reason: The reason provided is incorrect. The electronegativity difference between lithium (Li) and chlorine (Cl) is substantial. It is this difference in electronegativity that creates the polarity in the Li-Cl bond, making it an ionic bond with some covalent character.

Key Point: The high polarizing power of the Li⁺ ion, due to its small size and high charge density, is the main reason for the covalent character of LiCl, not the small electronegativity difference.