What are the formal charges on the terminal o | vedclass

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(D) The structure of ozone $(O_3)$ consists of a central oxygen atom double-bonded to one terminal oxygen atom and single-bonded to another terminal o

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$0, -1$

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(D) The structure of ozone $(O_3)$ consists of a central oxygen atom double-bonded to one terminal oxygen atom and single-bonded to another terminal oxygen atom.Using the formal charge formula: $FC = V - L - \frac{1}{2}B$,where $V$ is the number of valence electrons,$L$ is the number of lone pair electrons,and $B$ is the number of bonding electrons.For the central oxygen atom: $FC = 6 - 2 - \frac{1}{2}(6) = +1$.For the terminal oxygen atom with a double bond: $FC = 6 - 4 - \frac{1}{2}(4) = 0$.For the terminal oxygen atom with a single bond: $FC = 6 - 6 - \frac{1}{2}(2) = -1$.Thus,the formal charges on the terminal oxygen atoms are $0$ and $-1$.

List-$I$ (molecule/ion)	List-$II$ (Number of lone pairs of electrons on the central atom)
$(A)$ $XeF_2$	$(I)$ $2$
$(B)$ $XeO_3$	$(II)$ $0$
$(C)$ $XeF_4$	$(III)$ $3$
$(D)$ $PF_6^-$	$(IV)$ $1$

What are the formal charges on the terminal oxygen atoms of the ozone $(O_3)$ molecule?

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