Resonance structures are not real bonding depictions.
The actual molecule is a resonance hybrid, an average
of the resonance forms.
For O3, two of the electron pairs (one bonding, one non-
bonding) are delocalized (i.e., their density is spread over
the entire molecule). This effect yields two identical O-O
bonds, each consisting of a single bond (localized electron
pair) and a partial double bond (from one of the delocalized
electron pairs). Resonance effects lead to fractional bond
orders.
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