Which of the following contains the maximum n | vedclass

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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.

$A$. $SnCl_2$	$I$. Trigonal planar
$B$. $NH_3$	$II$. Linear
$C$. $I_3^{-}$	$III$. Angular
$D$. $SO_3$	$IV$. Trigonal pyramidal

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

Similar Questions

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

How many of the following molecules have two lone pairs of electrons on the central atom?
$SF_6$,$BF_3$,$ClF_3$,$PCl_5$,$BrF_5$,$XeF_4$,$H_2O$,$SF_4$

Identify the wrongly matched pair.
Molecule $\quad$ $\quad$ Shape or geometry of molecule

Match the following:
$A$. $SnCl_2$ $I$. Trigonal planar
$B$. $NH_3$ $II$. Linear
$C$. $I_3^{-}$ $III$. Angular
$D$. $SO_3$ $IV$. Trigonal pyramidal

The correct answer is:

Which set of species is arranged in order of increasing $O-N-O$ bond angle?

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