The formal charges of atoms (1),(2) and (3) i | vedclass

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

Vedclass · Accepted Answer

$0, +1, 0$

Vedclass · Answer

(B) The formula for formal charge is: $	ext{Formal charge} = 	ext{Valence electrons} - 	ext{Non-bonding electrons} - \frac{1}{2} 	imes 	ext{Bonding electrons}$.In the ion $[\underset{(1)}{\ddot{O}}=\underset{(2)}{N}=\underset{(3)}{\ddot{O}}]^{+}$,the nitrogen atom is bonded to two oxygen atoms with double bonds.For oxygen $(1)$: $	ext{Valence electrons} = 6$,$	ext{Non-bonding electrons} = 4$,$	ext{Bonding electrons} = 4$. $	ext{Formal charge} = 6 - 4 - \frac{4}{2} = 0$.For nitrogen $(2)$: $	ext{Valence electrons} = 5$,$	ext{Non-bonding electrons} = 0$,$	ext{Bonding electrons} = 8$. $	ext{Formal charge} = 5 - 0 - \frac{8}{2} = +1$.For oxygen $(3)$: $	ext{Valence electrons} = 6$,$	ext{Non-bonding electrons} = 4$,$	ext{Bonding electrons} = 4$. $	ext{Formal charge} = 6 - 4 - \frac{4}{2} = 0$.Thus,the formal charges are $0, +1, 0$.

The formal charges of atoms $(1)$,$(2)$ and $(3)$ in the ion $[\underset{(1)}{O}=\underset{(2)}{N}=\underset{(3)}{O}]^{+}$ are:

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