The bond angle in NF_{3} (102.3^{circ}) is sm | vedclass

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(C) In $NH_{3}$, the electronegativity of $N$ $(3.04)$ is higher than that of $H$ $(2.20)$, so the bonding electron pairs are shifted towards $N$. Thi

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opposite polarity of $N$ in the two molecules

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(C) In $NH_{3}$, the electronegativity of $N$ $(3.04)$ is higher than that of $H$ $(2.20)$, so the bonding electron pairs are shifted towards $N$. This increases the repulsion between the bonding pairs, leading to a larger bond angle $(107.2^{\circ})$.In $NF_{3}$, the electronegativity of $F$ $(3.98)$ is higher than that of $N$ $(3.04)$, so the bonding electron pairs are shifted away from $N$ towards $F$. This reduces the repulsion between the bonding pairs, resulting in a smaller bond angle $(102.3^{\circ})$.Therefore, the difference in the polarity of the $N-X$ bond (where $X = H$ or $F$) causes the difference in bond angles.

$A$. $SnCl_2$	$I$. Trigonal planar
$B$. $NH_3$	$II$. Linear
$C$. $I_3^{-}$	$III$. Angular
$D$. $SO_3$	$IV$. Trigonal pyramidal

The bond angle in $NF_{3}$ $(102.3^{\circ})$ is smaller than $NH_{3}$ $(107.2^{\circ})$. This is because of

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