Chemistry - CHEMICAL BONDING Question with Solution | TestHub

The correct options are B, C, and D.

Option A is incorrect because the bond angle in $IC{l}_2^{-}$ is $180^{\circ }$ (linear), while in $I(CN{)}_2^{-}$ it is also $180^{\circ }$ (linear). Both are $s{p}^{3}d$ hybridized with three lone pairs and two bonding pairs.

Option B is correct. $C{H}_{3}Cl$ has a larger dipole moment than $C{H}_{3}F$. Although F is more electronegative, the C-Cl bond length is greater, leading to a larger dipole moment.

Option C is correct. $Sb{H}_3$ has a higher boiling point than $N{H}_3$. While $N{H}_3$ has hydrogen bonding, $Sb{H}_3$ has stronger London dispersion forces due to its larger size and higher molecular weight, which dominate over hydrogen bonding in this comparison.

Option D is correct. The electronegativity of carbon increases with increasing s-character. In $C_2{H}_2$ (sp hybridized), carbon has 50% s-character, while in $C_2{H}_4$ (sp² hybridized), carbon has 33.3% s-character. Therefore, carbon in $C_2{H}_2$ is more electronegative than carbon in $C_2{H}_4$.