How many of the following molecules have two | vedclass

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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} 	imes (V - N)$,where $V$ is the nu

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$3$

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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} 	imes (V - N)$,where $V$ is the number of valence electrons of the central atom and $N$ is the number of bonding electrons (shared with surrounding atoms).$1$. $SF_6$: $S$ has $6$ valence electrons,$6$ bonds. Lone pairs = $\frac{1}{2} 	imes (6 - 6) = 0$.$2$. $BF_3$: $B$ has $3$ valence electrons,$3$ bonds. Lone pairs = $\frac{1}{2} 	imes (3 - 3) = 0$.$3$. $ClF_3$: $Cl$ has $7$ valence electrons,$3$ bonds. Lone pairs = $\frac{1}{2} 	imes (7 - 3) = 2$.$4$. $PCl_5$: $P$ has $5$ valence electrons,$5$ bonds. Lone pairs = $\frac{1}{2} 	imes (5 - 5) = 0$.$5$. $BrF_5$: $Br$ has $7$ valence electrons,$5$ bonds. Lone pairs = $\frac{1}{2} 	imes (7 - 5) = 1$.$6$. $XeF_4$: $Xe$ has $8$ valence electrons,$4$ bonds. Lone pairs = $\frac{1}{2} 	imes (8 - 4) = 2$.$7$. $H_2O$: $O$ has $6$ valence electrons,$2$ bonds. Lone pairs = $\frac{1}{2} 	imes (6 - 2) = 2$.$8$. $SF_4$: $S$ has $6$ valence electrons,$4$ bonds. Lone pairs = $\frac{1}{2} 	imes (6 - 4) = 1$.The molecules with two lone pairs are $ClF_3$,$XeF_4$,and $H_2O$. Total count is $3$.

How many of the following molecules have two lone pairs of electrons on the central atom?
$SF_6$,$BF_3$,$ClF_3$,$PCl_5$,$BrF_5$,$XeF_4$,$H_2O$,$SF_4$

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How many of the following molecules have two lone pairs of electrons on the central atom?$SF_6$,$BF_3$,$ClF_3$,$PCl_5$,$BrF_5$,$XeF_4$,$H_2O$,$SF_4$