NEET 2026 (Phase 1) · ChemistryResonancePrevious Year Question
For the ozone (\ce{O3}) Lewis structure shown in the figure — a central O atom (1) doubly bonded to one terminal O atom (2) and singly bonded to the other terminal O atom (3) — the correct formal charges on the oxygen atoms numbered 2, 1 and 3 respectively are:
- A.$-1$, $0$, $+1$
- B.$0$, $+1$, $-1$✓
- C.$0$, $0$, $0$
- D.$+1$, $0$, $-1$
Correct Answer
(B) $0$, $+1$, $-1$
Solution & Explanation
\textbf{Answer:} (B) $0$, $+1$, $-1$ \textbf{Solution:} Formal charge $= V - L - \tfrac{1}{2}S$. Terminal O (2, double-bonded, 4 lone-pair electrons): $6 - 4 - \tfrac{1}{2}(4) = 0$; central O (1, one double + one single bond, 2 lone-pair electrons): $6 - 2 - \tfrac{1}{2}(6) = +1$; terminal O (3, single-bonded, 6 lone-pair electrons): $6 - 6 - \tfrac{1}{2}(2) = -1$.
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