The correct formal charges on oxygen atoms nu | vedclass

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

Vedclass · Accepted Answer

$0, +1, -1$

Vedclass · Answer

(D) The formula for formal charge is: $	ext{Formal charge} = (	ext{Valence electrons}) - (	ext{Non-bonding electrons}) - \frac{1}{2}(	ext{Bonding electrons})$.For oxygen atom $2$ (terminal oxygen with double bond): Valence electrons = $6$, Non-bonding electrons = $4$, Bonding electrons = $4$. Formal charge = $6 - 4 - \frac{1}{2}(4) = 6 - 4 - 2 = 0$.For oxygen atom $1$ (central oxygen): Valence electrons = $6$, Non-bonding electrons = $2$, Bonding electrons = $6$. Formal charge = $6 - 2 - \frac{1}{2}(6) = 6 - 2 - 3 = +1$.For oxygen atom $3$ (terminal oxygen with single bond): Valence electrons = $6$, Non-bonding electrons = $6$, Bonding electrons = $2$. Formal charge = $6 - 6 - \frac{1}{2}(2) = 6 - 6 - 1 = -1$.Thus, the formal charges on oxygen atoms $2, 1$ and $3$ are $0, +1$ and $-1$ 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 correct formal charges on oxygen atoms numbered $2$, $1$ and $3$ respectively are:

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