The Lewis structure for O_3 molecule is given | vedclass

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Question

(A) The formal charge is calculated using the formula: $	ext{Formal charge} = 	ext{Total valence electrons} - 	ext{Total non-bonding electrons} - \

Vedclass · Accepted Answer

$-1, 0, +1$

Vedclass · Answer

(A) The formal charge is calculated using the formula: $	ext{Formal charge} = 	ext{Total valence electrons} - 	ext{Total non-bonding electrons} - \frac{1}{2} 	imes 	ext{Total bonding electrons}$.For oxygen atom $1$ (single bonded,$6$ lone pair electrons): $	ext{F.C.} = 6 - 6 - \frac{1}{2}(2) = -1$.For oxygen atom $2$ (double bonded,$4$ lone pair electrons): $	ext{F.C.} = 6 - 4 - \frac{1}{2}(4) = 0$.For oxygen atom $3$ (central atom,$2$ lone pair electrons,$6$ bonding electrons): $	ext{F.C.} = 6 - 2 - \frac{1}{2}(6) = +1$.Thus,the formal charges on oxygen atoms $1, 2, 3$ are $-1, 0, +1$ respectively.

Column $I$ (Molecules)	Column $II$ (Number of lone pairs on central atom)
$A. \ NH_3$	$1. \ \text{Two}$
$B. \ H_2O$	$2. \ \text{Three}$
$C. \ XeF_2$	$3. \ \text{Zero}$
$D. \ CH_4$	$4. \ \text{Four}$
	$5. \ \text{One}$

The Lewis structure for $O_3$ molecule is given below. The correct formal charges on oxygen atoms labelled $1$,$2$,$3$ are respectively.

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