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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} (V - B)$,where $V$ is the number of

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$1$,$0$,and $2$ lone pairs of central atom respectively

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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} (V - B)$,where $V$ is the number of valence electrons of the central atom and $B$ is the number of bonding electrons (assuming single bonds).$1$. For $SF_4$: Sulfur $(S)$ has $6$ valence electrons. It forms $4$ bonds with $F$ atoms. $	ext{Lone pairs} = \frac{1}{2} (6 - 4) = 1$.$2$. For $CF_4$: Carbon $(C)$ has $4$ valence electrons. It forms $4$ bonds with $F$ atoms. $	ext{Lone pairs} = \frac{1}{2} (4 - 4) = 0$.$3$. For $XeF_4$: Xenon $(Xe)$ has $8$ valence electrons. It forms $4$ bonds with $F$ atoms. $	ext{Lone pairs} = \frac{1}{2} (8 - 4) = 2$.Thus,the number of lone pairs are $1$,$0$,and $2$ respectively. The correct option is $D$.

List-$I$	List-$II$
$A. XeF_4$	$I. See-saw$
$B. SF_4$	$II. Square planar$
$C. NH_4^{+}$	$III. Bent T-shaped$
$D. BrF_3$	$IV. Tetrahedral$

The correct statement regarding the number of lone pairs on the central atoms of the molecules $SF_4$,$CF_4$,and $XeF_4$ is:

Similar Questions

Which among the following species does not have an angular shape?
$I.$ $ICl_2^+$
$II.$ $NH_2^-$
$III.$ $CS_2$
$IV.$ $H_2Se$

The $H_3O^{+}$ ion has the following shape:

The shape of the methane molecule is:

Match List-$I$ with List-$II$:
List-$I$ List-$II$
$A. XeF_4$ $I. See-saw$
$B. SF_4$ $II. Square planar$
$C. NH_4^{+}$ $III. Bent T-shaped$
$D. BrF_3$ $IV. Tetrahedral$

Choose the correct answer from the options given below:

In which of the following species is the central atom not surrounded by exactly $8$ valence electrons?

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