Observe the following structure. The formal c | vedclass

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(B) The formal charge can be calculated by the formula: $	ext{Formal charge} = [	ext{Total number of valence electrons in the free state}] - [	ext{

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$0, 0, -1$

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(B) The formal charge can be calculated by the formula: $	ext{Formal charge} = [	ext{Total number of valence electrons in the free state}] - [	ext{Total number of non-bonding (lone pair) electrons}] - \frac{1}{2} [	ext{Total number of bonding (shared) electrons}]$.For atom $1$ (Oxygen): Valence electrons = $6$,non-bonding electrons = $4$,bonding electrons = $4$.$	ext{Formal charge} = 6 - 4 - \frac{1}{2}(4) = 6 - 4 - 2 = 0$.For atom $2$ (Nitrogen): Valence electrons = $5$,non-bonding electrons = $2$,bonding electrons = $6$.$	ext{Formal charge} = 5 - 2 - \frac{1}{2}(6) = 5 - 2 - 3 = 0$.For atom $3$ (Oxygen): Valence electrons = $6$,non-bonding electrons = $6$,bonding electrons = $2$.$	ext{Formal charge} = 6 - 6 - \frac{1}{2}(2) = 6 - 6 - 1 = -1$.Thus,the formal charges are $0, 0, -1$.

Observe the following structure. The formal charges on the atoms $1, 2, 3$ respectively are:

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