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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-$I$ Molecule/ion	List-$II$ Bond pair : lone pair (on the central atom)
$A. ICl_2^-$	$I. 4 : 2$
$B. H_2O$	$II. 4 : 1$
$C. SO_2$	$III. 2 : 3$
$D. XeF_4$	$IV. 2 : 2$

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

The correct order of bond angles in the following compounds/species is:

In $SOCl_{2}$, the $Cl-S-Cl$ and $Cl-S-O$ bond angles are

The number of molecules/ions that show linear geometry among the following is $.........$
$SO_2, BeCl_2, CO_2, N_3^{-}, NO_2, F_2O, XeF_2, NO_2^{+}, I_3^{-}, O_3$

Match the List-$I$ with List-$II$.

List-$I$ Molecule/ion List-$II$ Bond pair : lone pair (on the central atom)

$A. ICl_2^-$ $I. 4 : 2$

$B. H_2O$ $II. 4 : 1$

$C. SO_2$ $III. 2 : 3$

$D. XeF_4$ $IV. 2 : 2$

Choose the correct answer from the options given below:

If the dipole moments of $H_2S$,$NH_3$,$NF_3$,and $BF_3$ are $0.95 \ D$,$1.47 \ D$,$0.23 \ D$,and $0.0 \ D$ respectively,the molecule that has a trigonal planar structure is:

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