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-$I$ (Shape)	List-$II$ (Molecules)
$A$. $T$-shaped	$I$. $XeF_4$
$B$. Trigonal planar	$II$. $SF_4$
$C$. Square planar	$III$. $ClF_3$
$D$. See-saw	$IV$. $BF_3$

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

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