The maximum number of lone pairs of electrons | vedclass

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(A) To find the number of lone pairs on the central atom,we determine the hybridization and geometry for each species:$1$. For $ClO_3^-$: The central

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$3$

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(A) To find the number of lone pairs on the central atom,we determine the hybridization and geometry for each species:$1$. For $ClO_3^-$: The central atom $Cl$ has $7$ valence electrons. It forms $3$ double bonds with $O$ atoms and has $1$ negative charge. The number of lone pairs = $(7 + 1 - 6)/2 = 1$ lone pair.$2$. For $XeF_4$: The central atom $Xe$ has $8$ valence electrons. It forms $4$ single bonds with $F$ atoms. The number of lone pairs = $(8 - 4)/2 = 2$ lone pairs.$3$. For $SF_4$: The central atom $S$ has $6$ valence electrons. It forms $4$ single bonds with $F$ atoms. The number of lone pairs = $(6 - 4)/2 = 1$ lone pair.$4$. For $I_3^-$: The central atom $I$ has $7$ valence electrons. It forms $2$ single bonds with $I$ atoms and has $1$ negative charge. The number of lone pairs = $(7 + 1 - 2)/2 = 3$ lone pairs.Comparing the number of lone pairs: $ClO_3^-$ $(1)$,$XeF_4$ $(2)$,$SF_4$ $(1)$,$I_3^-$ $(3)$.The maximum number of lone pairs is $3$.

List-$I$	List-$II$
$A. BrF_5$	$I. AB_4E$,see-saw
$B. SF_4$	$II. AB_4E_2$,square planar
$C. XeF_4$	$III. AB_5E$,square pyramidal
$D. ClF_3$	$IV. AB_3E_2$,$T$-shape

The maximum number of lone pairs of electrons on the central atom from the following species is $........$. $ClO_3^-$,$XeF_4$,$SF_4$ and $I_3^-$

Similar Questions

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Provide the different spatial arrangements of $SF_4$ including its electron pairs.

Atoms in a $P_4$ molecule of white phosphorus are arranged regularly in the following way:

Which of the following molecules has the lowest bond angle?

Match the following:

List-$I$ List-$II$

$A. BrF_5$ $I. AB_4E$,see-saw

$B. SF_4$ $II. AB_4E_2$,square planar

$C. XeF_4$ $III. AB_5E$,square pyramidal

$D. ClF_3$ $IV. AB_3E_2$,$T$-shape

The correct answer is:

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