In the following electron-dot structure, calc | vedclass

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(A) The formula for formal charge is: $	ext{Formal charge} = 	ext{Valence electrons} - (\frac{1}{2} 	imes 	ext{Bonding electrons} + 	ext{Non-bond

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$-1, +1, -1$

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(A) The formula for formal charge is: $	ext{Formal charge} = 	ext{Valence electrons} - (\frac{1}{2} 	imes 	ext{Bonding electrons} + 	ext{Non-bonding electrons})$.For the structure $: \ddot{N}_1 = N_2 = \ddot{N}_3 :$For $N_1$ (left nitrogen): $	ext{Valence electrons} = 5$, $	ext{Bonding electrons} = 4$, $	ext{Non-bonding electrons} = 4$.$	ext{Formal charge} = 5 - (\frac{1}{2} 	imes 4 + 4) = 5 - (2 + 4) = -1$.For $N_2$ (middle nitrogen): $	ext{Valence electrons} = 5$, $	ext{Bonding electrons} = 8$, $	ext{Non-bonding electrons} = 0$.$	ext{Formal charge} = 5 - (\frac{1}{2} 	imes 8 + 0) = 5 - 4 = +1$.For $N_3$ (right nitrogen): $	ext{Valence electrons} = 5$, $	ext{Bonding electrons} = 4$, $	ext{Non-bonding electrons} = 4$.$	ext{Formal charge} = 5 - (\frac{1}{2} 	imes 4 + 4) = 5 - (2 + 4) = -1$.Thus, the formal charges are $-1, +1, -1$.

In the following electron-dot structure, calculate the formal charge from left to right for the nitrogen atoms: $: \ddot{N} = N = \ddot{N} :$

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