Select correct statement(s) : — Chemical Bonding Chemistry Question

💡 Solution & Explanation

Step 1: Check the dipole moments: CH3Cl (~1.87 D) is larger than CH3F (~1.85 D) because the significantly larger C-Cl bond distance outweighs the higher electronegativity of Fluorine. Step 2: Check the bond angles: in CH3F, the highly electronegative Fluorine atom draws s-character toward itself (increasing p-character in the C-F bond). According to Bent's rule, this leaves more s-character in the C-H bonds, opening up the H-C-H bond angle. Step 3: Consequently, CH3Cl has a larger dipole moment than CH3F, but its H-C-H bond angle is smaller. This makes statement (c) correct.