Which of the following pairs contains 2 lone | 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} (V - B)$,where $V$ is the number of

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$I_{3}^{+}, H_{2}O$

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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 - B)$,where $V$ is the number of valence electrons of the central atom and $B$ is the number of bonding electrons (or atoms bonded to it).$1$. $I_{3}^{+}$: The central $I$ atom has $7$ valence electrons. It forms $2$ bonds with other $I$ atoms and has a positive charge,so $V = 7 - 1 = 6$. Bonding electrons $B = 2$. Lone pairs = $\frac{1}{2} (6 - 2) = 2$.$2$. $H_{2}O$: The central $O$ atom has $6$ valence electrons. It forms $2$ bonds with $H$ atoms. Lone pairs = $\frac{1}{2} (6 - 2) = 2$.Both $I_{3}^{+}$ and $H_{2}O$ have $2$ lone pairs on their central atoms. Therefore,option $C$ is correct.

List-$I$ (Species)	List-$II$ (Number of lone pairs of electrons on the central atom)
$(a)$ $XeF_{2}$	$(i)$ $0$
$(b)$ $XeO_{2}F_{2}$	$(ii)$ $1$
$(c)$ $XeO_{3}F_{2}$	$(iii)$ $2$
$(d)$ $XeF_{4}$	$(iv)$ $3$

List-$I$ (Molecule)	List-$II$ (Shape)
$A$. $XeF_4$	$I$. Square pyramidal
$B$. $ClF_3$	$II$. Pentagonal bipyramidal
$C$. $BrF_5$	$III$. Square planar
$D$. $IF_7$	$IV$. Bent $T$-shape

Which of the following pairs contains $2$ lone pairs of electrons on the central atom?

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Match the following:

List-$I$ (Molecule) List-$II$ (Shape)

$A$. $XeF_4$ $I$. Square pyramidal

$B$. $ClF_3$ $II$. Pentagonal bipyramidal

$C$. $BrF_5$ $III$. Square planar

$D$. $IF_7$ $IV$. Bent $T$-shape

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