In the Lewis dot structure of carbonate ion s | vedclass

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(B) The formal charge $(FC)$ is calculated using the formula: $FC = 	ext{Valence electrons} - 	ext{Non-bonding electrons} - \frac{1}{2} 	imes 	ext

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$-1, 0, -1$

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(B) The formal charge $(FC)$ is calculated using the formula: $FC = 	ext{Valence electrons} - 	ext{Non-bonding electrons} - \frac{1}{2} 	imes 	ext{Bonding electrons}$.For oxygen atom $1$ (single bond,$6$ lone pair electrons): $FC = 6 - 6 - \frac{1}{2} 	imes 2 = -1$.For oxygen atom $2$ (double bond,$4$ lone pair electrons): $FC = 6 - 4 - \frac{1}{2} 	imes 4 = 0$.For oxygen atom $3$ (single bond,$6$ lone pair electrons): $FC = 6 - 6 - \frac{1}{2} 	imes 2 = -1$.Thus,the formal charges on oxygen atoms $1, 2,$ and $3$ are $-1, 0,$ and $-1$ respectively.

In the Lewis dot structure of carbonate ion shown,the formal charges on the oxygen atoms $1, 2,$ and $3$ are respectively:

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