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Pi bonds in benzene would be delocalized. When you draw the Lewis structure, it alternates between single and double bonds. In reality, there are no alternating bonds, which is why benzene is usually drawn with a circle inside a hexagon. The p-orbitals overlap side-to-side and electrons are delocalized.
Pi bonds are delocalized when there is conjugation in a molecule, which is when there are multiple pi bonds separated by single bonds. For example, 1,3-butadiene has conjugation because it has multiple double bonds separated by only one sigma bond. If there is more than one sigma bond, then the bonds are not conjugated. This is why benzene has delocalized pi bonds, as it has extensive conjugation around the ring.
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