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Delocalized pi bonds are pi bonds where the e- are free to move over more than two nuclei, like the example of Benzene that Prof. Lavelle gave. Delocalized pi bonds can also be thought of as where there are pie bonds with resonance structures, since the lewis structures we draw are not entirely accurate; in reality, the bond lengths are combinations of the resonance structures, and therefore if there are any pi bonds involved in the changing resonance structures then those pibonds are delocalized. When it is just between two atoms and it does not have any free space for the e- to move between other atoms as well, it is localized.
Delocalized pi bonds are when electrons are free to move around in the molecule. Thus, delocalized pi bonds occur when the Lewis structure has resonance and has double or triple bonds. The delocalized electrons in the double or triple bonds result in a delocalized pi bond.
A delocalized pi bond is similar to the concept of delocalized electrons that occur within resonance structures. When a molecule has different resonant structures, the pi bond can be blended to different areas.
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