In the ozone (O_3) molecule,the formal charge | vedclass

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

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$1$

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(D) The structure of the ozone $(O_3)$ molecule consists of a central oxygen atom double-bonded to one terminal oxygen atom and single-bonded to another terminal oxygen atom. The central oxygen atom has $6$ valence electrons. In the resonance structure,the central oxygen atom forms $3$ bonds (total $6$ bonding electrons) and has $1$ lone pair ($2$ electrons). Using the formula: $	ext{Formal charge} = 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: $V = 6$,$L = 2$,$B = 6$. $	ext{Formal charge} = 6 - 2 - \frac{1}{2}(6) = 6 - 2 - 3 = +1$.

In the ozone $(O_3)$ molecule,the formal charge on the central oxygen atom is:

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