Which of the following pairs contains 2 lone | vedclass

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

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$I_{3}^{+}, H_{2}O$

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(C) To determine the number of lone pairs on the central atom,we use the formula: $	ext{Lone pairs} = \frac{1}{2} (V - B)$,where $V$ is the number of valence electrons of the central atom and $B$ is the number of bonding electrons (or atoms bonded to it).$1$. $I_{3}^{+}$: The central $I$ atom has $7$ valence electrons. It forms $2$ bonds with other $I$ atoms and has a positive charge,so $V = 7 - 1 = 6$. Bonding electrons $B = 2$. Lone pairs = $\frac{1}{2} (6 - 2) = 2$.$2$. $H_{2}O$: The central $O$ atom has $6$ valence electrons. It forms $2$ bonds with $H$ atoms. Lone pairs = $\frac{1}{2} (6 - 2) = 2$.Both $I_{3}^{+}$ and $H_{2}O$ have $2$ lone pairs on their central atoms. Therefore,option $C$ is correct.

List-$I$	List-$II$
$A. ICl$	$i. \text{Linear}$

$B. ICl_3$	$ii. \text{T-Shape}$
$C. ClF_5$	$iii. \text{Square pyramidal}$
$D. IF_7$	$iv. \text{Pentagonal bipyramidal}$

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

Similar Questions

Match List-$I$ with List-$II$.
List-$I$ List-$II$
$A. ICl$ $i. \text{Linear}$
$B. ICl_3$ $ii. \text{T-Shape}$
$C. ClF_5$ $iii. \text{Square pyramidal}$
$D. IF_7$ $iv. \text{Pentagonal bipyramidal}$

Choose the correct answer from the options given below:

The number of lone pairs of electrons on the central atom of $BrF_5, XeO_3, SO_2$ respectively are

Amongst the following,the linear species is:

The shapes of nitrite $(NO_2^-)$ and nitrile $(NO_2^-)$ respectively are

The shape of the molecule $ClF_3$ is

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