Which of the following pairs of compounds con | vedclass

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

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$BrF_5$ and $XeF_6$

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(A) To determine the number of lone pairs on the central atom,we use the formula: $	ext{Lone pairs} = \frac{1}{2} (V - N)$,where $V$ is the number of valence electrons of the central atom and $N$ is the number of bonding electrons (monovalent atoms attached).$A$: $BrF_5$ ($Br$ has $7$ valence $e^-$,$5$ bonded $F$ atoms): $	ext{Lone pairs} = \frac{1}{2} (7 - 5) = 1$. $XeF_6$ ($Xe$ has $8$ valence $e^-$,$6$ bonded $F$ atoms): $	ext{Lone pairs} = \frac{1}{2} (8 - 6) = 1$.$B$: $ICl$ ($I$ has $7$ valence $e^-$,$1$ bonded $Cl$ atom): $	ext{Lone pairs} = \frac{1}{2} (7 - 1) = 3$. $H_2S$ ($S$ has $6$ valence $e^-$,$2$ bonded $H$ atoms): $	ext{Lone pairs} = \frac{1}{2} (6 - 2) = 2$.$C$: $ClF_3$ ($Cl$ has $7$ valence $e^-$,$3$ bonded $F$ atoms): $	ext{Lone pairs} = \frac{1}{2} (7 - 3) = 2$. $XeF_2$ ($Xe$ has $8$ valence $e^-$,$2$ bonded $F$ atoms): $	ext{Lone pairs} = \frac{1}{2} (8 - 2) = 3$.$D$: $IF_7$ ($I$ has $7$ valence $e^-$,$7$ bonded $F$ atoms): $	ext{Lone pairs} = \frac{1}{2} (7 - 7) = 0$. $XeF_4$ ($Xe$ has $8$ valence $e^-$,$4$ bonded $F$ atoms): $	ext{Lone pairs} = \frac{1}{2} (8 - 4) = 2$.Thus,$BrF_5$ and $XeF_6$ both have $1$ lone pair on their central atoms.

List-$I$ Molecule/ion	List-$II$ Bond pair : lone pair (on the central atom)
$A. ICl_2^-$	$I. 4 : 2$
$B. H_2O$	$II. 4 : 1$
$C. SO_2$	$III. 2 : 3$
$D. XeF_4$	$IV. 2 : 2$

Which of the following pairs of compounds consists of an equal number of lone pairs of electrons in the valence shell of the central atom?

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Which of the following represents pairs of isostructural species?

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

Match the List-$I$ with List-$II$.

List-$I$ Molecule/ion List-$II$ Bond pair : lone pair (on the central atom)

$A. ICl_2^-$ $I. 4 : 2$

$B. H_2O$ $II. 4 : 1$

$C. SO_2$ $III. 2 : 3$

$D. XeF_4$ $IV. 2 : 2$

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