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

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$XeF_2$

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(C) To determine the number of lone pairs on the central atom,we use the formula: $	ext{Lone pairs} = \frac{1}{2} (V - N)$,where $V$ is the number of valence electrons of the central atom and $N$ is the number of bonding electrons (or atoms attached).$1$. In $SiF_4$: $Si$ has $4$ valence electrons and forms $4$ bonds. Lone pairs = $\frac{1}{2} (4 - 4) = 0$.$2$. In $BrF_3$: $Br$ has $7$ valence electrons and forms $3$ bonds. Lone pairs = $\frac{1}{2} (7 - 3) = 2$.$3$. In $XeF_2$: $Xe$ has $8$ valence electrons and forms $2$ bonds. Lone pairs = $\frac{1}{2} (8 - 2) = 3$.$4$. In $SF_4$: $S$ has $6$ valence electrons and forms $4$ bonds. Lone pairs = $\frac{1}{2} (6 - 4) = 1$.Comparing these,$XeF_2$ has the maximum number of lone pairs $(3)$.

Which of the following molecules has the maximum number of lone pairs on the central atom?

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