The formal charges of N_{(1)},N_{(2)},and O a | vedclass

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(B) The formal charge $(FC)$ is calculated as: $FC = (	ext{Total valence electrons}) - (	ext{Non-bonding electrons}) - \frac{1}{2}(	ext{Bonding ele

Vedclass · Accepted Answer

$-1, +1, 0$

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(B) The formal charge $(FC)$ is calculated as: $FC = (	ext{Total valence electrons}) - (	ext{Non-bonding electrons}) - \frac{1}{2}(	ext{Bonding electrons})$.For $N_{(1)}$ (terminal nitrogen with $4$ non-bonding electrons and $2$ bonding electrons from a double bond): $FC = 5 - 4 - \frac{1}{2}(4) = -1$.For $N_{(2)}$ (central nitrogen with $0$ non-bonding electrons and $8$ bonding electrons from two double bonds): $FC = 5 - 0 - \frac{1}{2}(8) = +1$.For $O$ (oxygen with $4$ non-bonding electrons and $4$ bonding electrons from a double bond): $FC = 6 - 4 - \frac{1}{2}(4) = 0$.Thus,the formal charges are $-1, +1, 0$.

The formal charges of $N_{(1)}$,$N_{(2)}$,and $O$ atoms in the structure $N_{(1)} = N_{(2)} = O$ are respectively:

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