In which of the following,the formal charge i | vedclass

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(B) The formal charge $(FC)$ is calculated using the formula: $FC = V - L - \frac{1}{2}B$,where $V$ is the number of valence electrons,$L$ is the numb

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$ClO_4^-$

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(B) The formal charge $(FC)$ is calculated using the formula: $FC = V - L - \frac{1}{2}B$,where $V$ is the number of valence electrons,$L$ is the number of lone pair electrons,and $B$ is the number of bonding electrons.$1.$ In $ClO_4^-$,the most stable structure involves the central $Cl$ atom forming three double bonds and one single bond with oxygen atoms. The $FC$ on $Cl = 7 - 0 - \frac{1}{2}(14) = 0$. The $-1$ formal charge is located on the single-bonded oxygen atom.$2.$ In $ICl_2^-$,the $FC$ on the central $I$ atom is $7 - 6 - \frac{1}{2}(4) = -1$.$3.$ In $Br_3^-$,the $FC$ on the central $Br$ atom is $7 - 6 - \frac{1}{2}(4) = -1$.$4.$ In $H_3O^{+}$,the $FC$ on the central $O$ atom is $6 - 2 - \frac{1}{2}(6) = +1$.Therefore,in $ClO_4^-$,the formal charge is not on the central atom.

In which of the following,the formal charge is $NOT$ on the central atom in the most stable canonical form?

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