Among LiCl, BeCl2, BCl3 and CCl4 the covalent bond character follows the order:

Explanation

The correct order of covalent character among these compounds is LiCl < BeCl2 < BCl3 < CCl4. This is determined by Fajans' rules, which state that covalent character increases with greater positive charge on the cation and ability to polarize the anion. LiCl is primarily ionic due to lithium's small size and the high electronegativity of chlorine, giving it a significantly ionic character. BeCl2, BCl3, and CCl4 exhibit increasing covalent character due to their molecular nature and the higher charge density associated with their cations. - Option A is incorrect because it suggests LiCl has the highest covalent character, which contradicts its ionic nature. - Option C misrepresents the ranking by placing CCl4 above BCl3, which is incorrect as BCl3 is more covalent. - Option D incorrectly ranks BeCl3 without considering its lower covalent character relative to BCl3. Thus, the correct answer is the one that correctly represents the increasing covalent character.