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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 - M - C + A)$, where $V$ is the

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$I_3^{-}$

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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 - M - C + A)$, where $V$ is the number of valence electrons of the central atom, $M$ is the number of monovalent atoms, $C$ is the cationic charge, and $A$ is the anionic charge.$A) \ ClO_3^{-}$: Central atom $Cl$ $(V=7)$. $3$ oxygen atoms are divalent. Lone pairs $= \frac{1}{2} (7 - 0 - 0 + 1) = 4$ electrons, which corresponds to $1$ lone pair.$B) \ XeF_4$: Central atom $Xe$ $(V=8)$. $4$ fluorine atoms are monovalent. Lone pairs $= \frac{1}{2} (8 - 4) = 2$ lone pairs.$C) \ SF_4$: Central atom $S$ $(V=6)$. $4$ fluorine atoms are monovalent. Lone pairs $= \frac{1}{2} (6 - 4) = 1$ lone pair.$D) \ I_3^{-}$: Central atom $I$ $(V=7)$. $2$ iodine atoms are monovalent. Lone pairs $= \frac{1}{2} (7 - 2 + 1) = 3$ lone pairs.Thus, $I_3^{-}$ has the maximum number of lone pairs $(3)$ on the central atom.

$S_8$	$A$
$P_4$	$B$
$S_6$	$C$
$O_3$	$D$

Which of the following contains the maximum number of lone pairs on the central atom?

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