The formal charge on the central oxygen atom | vedclass

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(D) The formal charge on an atom in a Lewis structure is calculated using the formula:Formal Charge = (Total number of valence electrons on the free a

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$+1$

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(D) The formal charge on an atom in a Lewis structure is calculated using the formula:Formal Charge = (Total number of valence electrons on the free atom) - ($\frac{1}{2}$ $	imes$ Total number of shared electrons) - (Total number of unshared valence electrons).For the central oxygen atom in the ozone $(O_3)$ molecule:$1$. The central oxygen atom has $6$ valence electrons in its free state.$2$. It forms one double bond with one oxygen atom and one single bond with another oxygen atom,sharing a total of $6$ electrons ($3$ bonds $	imes$ $2$ electrons per bond).$3$. It has $2$ unshared electrons (one lone pair).Formal Charge = $6 - \frac{1}{2}(6) - 2 = 6 - 3 - 2 = +1$.

List-$I$ (Molecule Species)	List-$II$ (Property/Shape)
$A$. $SO_2Cl_2$	$I$. Paramagnetic
$B$. $NO$	$II$. Diamagnetic
$C$. $NO_2^-$	$III$. Tetrahedral
$D$. $I_3^-$	$IV$. Linear

The formal charge on the central oxygen atom in ozone $(O_3)$ is:

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Match List-$I$ with List-$II$ :

List-$I$ (Molecule Species) List-$II$ (Property/Shape)

$A$. $SO_2Cl_2$ $I$. Paramagnetic

$B$. $NO$ $II$. Diamagnetic

$C$. $NO_2^-$ $III$. Tetrahedral

$D$. $I_3^-$ $IV$. Linear

Choose the correct answer from the options given below :

The compound in which the number of $d\pi - p\pi$ bonds are equal to those present in $ClO_4^{-}$ is:

Select the $CORRECT$ statement.

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