What is the number of lone pairs of electrons | vedclass

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(B) The number of lone pairs on the central $Xe$ atom can be calculated using the formula: $	ext{Lone pairs} = \frac{1}{2} (V - M)$,where $V$ is the

Vedclass · Accepted Answer

$3, 2, 1$

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(B) The number of lone pairs on the central $Xe$ atom can be calculated using the formula: $	ext{Lone pairs} = \frac{1}{2} (V - M)$,where $V$ is the number of valence electrons of the central atom and $M$ is the number of monovalent atoms attached.For $XeF_2$: $V = 8$,$M = 2$. $	ext{Lone pairs} = \frac{1}{2} (8 - 2) = 3$.For $XeF_4$: $V = 8$,$M = 4$. $	ext{Lone pairs} = \frac{1}{2} (8 - 4) = 2$.For $XeF_6$: $V = 8$,$M = 6$. $	ext{Lone pairs} = \frac{1}{2} (8 - 6) = 1$.Thus,the number of lone pairs is $3, 2, 1$.

List-$I$	List-$II$
$A$. $XeF_4$	$1$. Pyramidal
$B$. $XeF_6$	$2$. $T$-shape
$C$. $XeO_3$	$3$. Distorted octahedral
$D$. $XeOF_2$	$4$. Square planar

What is the number of lone pairs of electrons on the $Xe$ atom in the molecules $XeF_2$,$XeF_4$,and $XeF_6$ respectively?

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At $143 \ K$,the reaction of $XeF_4$ with $O_2F_2$ produces a xenon compound $Y$. The total number of lone pair$(s)$ of electrons present on the whole molecule of $Y$ is . . . . .

Select the correct matching.

List-$I$ List-$II$

$A$. $XeF_4$ $1$. Pyramidal

$B$. $XeF_6$ $2$. $T$-shape

$C$. $XeO_3$ $3$. Distorted octahedral

$D$. $XeOF_2$ $4$. Square planar

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