The incomplete Lewis representation of CO_3^{ | vedclass

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Question

(A) The formal charge $(F.C.)$ on an atom in a Lewis structure is calculated using the formula: $F.C. = 	ext{Valence } e^- - 	ext{Lone pair } e^- -

Vedclass · Accepted Answer

$a : 0, b : 0, c : -1$

Vedclass · Answer

(A) The formal charge $(F.C.)$ on an atom in a Lewis structure is calculated using the formula: $F.C. = 	ext{Valence } e^- - 	ext{Lone pair } e^- - \frac{1}{2} 	ext{Shared } e^-$. For the given structure of $CO_3^{2-}$: $1$. For Carbon atom $(a)$: It has $4$ valence electrons,$0$ lone pair electrons,and $8$ shared electrons (forming $4$ bonds). $F.C. 	ext{ on } C_{(a)} = 4 - 0 - \frac{1}{2}(8) = 4 - 4 = 0$. $2$. For Oxygen atom $(b)$: It is double-bonded to Carbon. It has $6$ valence electrons,$4$ lone pair electrons,and $4$ shared electrons. $F.C. 	ext{ on } O_{(b)} = 6 - 4 - \frac{1}{2}(4) = 6 - 4 - 2 = 0$. $3$. For Oxygen atom $(c)$: It is single-bonded to Carbon. It has $6$ valence electrons,$6$ lone pair electrons,and $2$ shared electrons. $F.C. 	ext{ on } O_{(c)} = 6 - 6 - \frac{1}{2}(2) = 6 - 6 - 1 = -1$. Thus,the formal charges are $a=0, b=0, c=-1$.

The incomplete Lewis representation of $CO_3^{2-}$ is given below. The formal charges on atoms marked as $a$,$b$,and $c$,respectively,are

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