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.

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

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