For the ozone ($\mathrm{O}{}_3$) 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:

Solution & Explanation

\textbf{Answer:} (B) $0$, $+1$, $-1$ \textbf{Solution:} Formal charge $=V-L-\frac{1}{2}S$. Terminal O (2, double-bonded, 4 lone-pair electrons): $6-4-\frac{1}{2}(4)=0$; central O (1, one double + one single bond, 2 lone-pair electrons): $6-2-\frac{1}{2}(6)=+1$; terminal O (3, single-bonded, 6 lone-pair electrons): $6-6-\frac{1}{2}(2)=-1$.