In molecules of the type AX_2L_n (where L rep | vedclass

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(C) According to the $VSEPR$ theory,the bond angle depends on the number of lone pairs $(n)$ and the geometry of the molecule. For $n=0$ ($AX_2$,linea

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Will be maximum for $n=3$

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(C) According to the $VSEPR$ theory,the bond angle depends on the number of lone pairs $(n)$ and the geometry of the molecule. For $n=0$ ($AX_2$,linear),the angle is $180^{\circ}$. For $n=1$ ($AX_2L$,bent),the angle is $For $n=2$ ($AX_2L_2$,bent),the angle is $For $n=3$ ($AX_2L_3$,linear),the lone pairs occupy the equatorial positions of a trigonal bipyramidal geometry,resulting in an $X-A-X$ bond angle of $180^{\circ}$. Thus,the bond angle is maximum for $n=3$ in this specific series.

List-$I$ (Compound)	List-$II$ (Structure)
$A$. $ClF_3$	$1$. Square planar
$B$. $PCl_5$	$2$. Tetrahedral
$C$. $IF_5$	$3$. Trigonal bipyramidal
$D$. $CCl_4$	$4$. Square pyramidal
$E$. $XeF_4$	$5$. $T$-shaped

In molecules of the type $AX_2L_n$ (where $L$ represents lone pairs and $n$ is its number),there exists a bond between element $A$ and $X$. The $\angle XAX$ bond angle:

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