JEE Main 2026 — Chemical Bonding and Molecular Structure Question with Solution

The formal charge (F.C.) of an atom in a Lewis structure is calculated using the formula:
F.C. = [Total valence electrons] - [Total non-bonding (lone pair) electrons] - $\frac{1}{2}$[Total bonding (shared) electrons]
For atom (1) Oxygen: Valence $e^{-}=6$, Lone pair $e^{-}=4$, Bonding $e^{-}=4$.
$F.C.=6-4-\frac{1}{2}(4)=0$
For atom (2) Nitrogen: Valence $e^{-}=5$, Lone pair $e^{-}=0$, Bonding $e^{-}=8$.
$F.C.=5-0-\frac{1}{2}(8)=+1$
For atom (3) Oxygen: Valence $e^{-}=6$, Lone pair $e^{-}=4$, Bonding $e^{-}=4$.
$F.C.=6-4-\frac{1}{2}(4)=0$
For atom (4) Oxygen: Valence $e^{-}=6$, Lone pair $e^{-}=6$, Bonding $e^{-}=2$.
$F.C.=6-6-\frac{1}{2}(2)=-1$
The formal charges are $0,+1,0,-1$ respectively.