In which of the following molecules,the maxim | vedclass

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(D) To determine the number of lone pairs on the central atom,we use the formula: $	ext{Lone pairs} = \frac{1}{2} 	imes (V - N)$,where $V$ is the nu

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$XeF_2$

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(D) To determine the number of lone pairs on the central atom,we use the formula: $	ext{Lone pairs} = \frac{1}{2} 	imes (V - N)$,where $V$ is the number of valence electrons of the central atom and $N$ is the number of electrons involved in bonding (monovalent atoms).$1$. For $NH_3$: Central atom $N$ has $5$ valence electrons. It forms $3$ bonds. $	ext{Lone pairs} = \frac{1}{2} 	imes (5 - 3) = 1$.$2$. For $H_2O$: Central atom $O$ has $6$ valence electrons. It forms $2$ bonds. $	ext{Lone pairs} = \frac{1}{2} 	imes (6 - 2) = 2$.$3$. For $ClF_3$: Central atom $Cl$ has $7$ valence electrons. It forms $3$ bonds. $	ext{Lone pairs} = \frac{1}{2} 	imes (7 - 3) = 2$.$4$. For $XeF_2$: Central atom $Xe$ has $8$ valence electrons. It forms $2$ bonds. $	ext{Lone pairs} = \frac{1}{2} 	imes (8 - 2) = 3$.Thus,$XeF_2$ has the maximum number of lone pairs $(3)$ on the central atom.

List-$I$	List-$II$
$A. ICl$	$i. \text{Linear}$

$B. ICl_3$	$ii. \text{T-Shape}$
$C. ClF_5$	$iii. \text{Square pyramidal}$
$D. IF_7$	$iv. \text{Pentagonal bipyramidal}$

In which of the following molecules,the maximum number of lone pairs is present on the central atom?

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Match List-$I$ with List-$II$.
List-$I$ List-$II$
$A. ICl$ $i. \text{Linear}$
$B. ICl_3$ $ii. \text{T-Shape}$
$C. ClF_5$ $iii. \text{Square pyramidal}$
$D. IF_7$ $iv. \text{Pentagonal bipyramidal}$

Choose the correct answer from the options given below:

Statement $I$ : $SO_2$ and $H_2O$ both possess $V$-shaped structure.
Statement $II$ : The bond angle of $SO_2$ is less than that of $H_2O$.
In the light of the above statements,choose the most appropriate answer from the options given below:

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