The formal charges on the atoms marked as (1) | vedclass

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(C) The formula for formal charge is: $	ext{Formal charge} = 	ext{Valence electrons} - 	ext{Non-bonding electrons} - \frac{1}{2}(	ext{Bonding elec

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$0, +1, 0, -1$

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(C) The formula for formal charge is: $	ext{Formal charge} = 	ext{Valence electrons} - 	ext{Non-bonding electrons} - \frac{1}{2}(	ext{Bonding electrons})$.For atom $(1)$ (Oxygen): Valence $e^- = 6$, Non-bonding $e^- = 4$, Bonding $e^- = 4$. $	ext{FC} = 6 - 4 - \frac{4}{2} = 0$.For atom $(2)$ (Nitrogen): Valence $e^- = 5$, Non-bonding $e^- = 0$, Bonding $e^- = 8$. $	ext{FC} = 5 - 0 - \frac{8}{2} = +1$.For atom $(3)$ (Oxygen): Valence $e^- = 6$, Non-bonding $e^- = 4$, Bonding $e^- = 4$. $	ext{FC} = 6 - 4 - \frac{4}{2} = 0$.For atom $(4)$ (Oxygen): Valence $e^- = 6$, Non-bonding $e^- = 6$, Bonding $e^- = 2$. $	ext{FC} = 6 - 6 - \frac{2}{2} = -1$.Thus, the formal charges are $0, +1, 0, -1$.

The formal charges on the atoms marked as $(1)$ to $(4)$ in the Lewis representation of $HNO_3$ molecule respectively are

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