The compound(s) with 2 lone pairs of electron | vedclass

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(B) To determine the number of lone pairs on the central atom,we use the formula: $	ext{Lone pairs} = \frac{1}{2} 	imes (V - N - C)$,where $V$ is th

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$B, C$

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(B) To determine the number of lone pairs on the central atom,we use the formula: $	ext{Lone pairs} = \frac{1}{2} 	imes (V - N - C)$,where $V$ is the number of valence electrons of the central atom,$N$ is the number of monovalent atoms bonded to it,and $C$ is the charge on the species.$1$. For $BrF_5$: Central atom $Br$ has $7$ valence electrons. It is bonded to $5$ $F$ atoms. $	ext{Lone pairs} = \frac{1}{2} 	imes (7 - 5) = 1$.$2$. For $ClF_3$: Central atom $Cl$ has $7$ valence electrons. It is bonded to $3$ $F$ atoms. $	ext{Lone pairs} = \frac{1}{2} 	imes (7 - 3) = 2$.$3$. For $XeF_4$: Central atom $Xe$ has $8$ valence electrons. It is bonded to $4$ $F$ atoms. $	ext{Lone pairs} = \frac{1}{2} 	imes (8 - 4) = 2$.$4$. For $SF_4$: Central atom $S$ has $6$ valence electrons. It is bonded to $4$ $F$ atoms. $	ext{Lone pairs} = \frac{1}{2} 	imes (6 - 4) = 1$.Thus,$ClF_3$ and $XeF_4$ have $2$ lone pairs on their central atoms. The correct option is $B$.

List-$I$	List-$II$
$A$. $XeO_{3}$	$I$. $BrF_{5}$
$B$. $XeF_{2}$	$II$. $NH_{3}$
$C$. $XeO_{2}F_{2}$	$III$. $[I_{3}]^{-}$
$D$. $XeOF_{4}$	$IV$. $SF_{4}$

The compound$(s)$ with $2$ lone pairs of electrons on the central atom is(are):
$(A)$ $BrF_5$
$(B)$ $ClF_3$
$(C)$ $XeF_4$
$(D)$ $SF_4$

Similar Questions

Match List-$I$ with List-$II$ according to shape.

List-$I$ List-$II$

$A$. $XeO_{3}$ $I$. $BrF_{5}$

$B$. $XeF_{2}$ $II$. $NH_{3}$

$C$. $XeO_{2}F_{2}$ $III$. $[I_{3}]^{-}$

$D$. $XeOF_{4}$ $IV$. $SF_{4}$

Choose the correct answer from the options given below :

Which of the following compounds has a central atom with one lone pair of electrons and three bond pairs of electrons?

Which of the following represents the correct Lewis structure for the cyanate ion $(OCN^-)$?

The correct statement about $ICl_5$ and $ICl_4^-$ is

According to the Valence Shell Electron Pair Repulsion $(VSEPR)$ theory,what is the shape of $ClO_3^-$?

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The compound$(s)$ with $2$ lone pairs of electrons on the central atom is(are):$(A)$ $BrF_5$$(B)$ $ClF_3$$(C)$ $XeF_4$$(D)$ $SF_4$