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A delocalized pi bond is present in a molecule that has double bonds and also has resonance. For example, CO3 2- would have delocalized pi bonds because the multiple bond character is spread over three oxygen atoms.
You will find delocalized pi bonds in molecules that have resonance. This is because, in resonance, the electrons are delocalized over a pair of atoms, so the pi bond would be a delocalized pi bond.
Delocalized pi bonds exist when a molecule has resonance, in which say double or triple bonds can be placed in different locations in the Lewis structure. If there is no resonance, there will be no delocalized pi bonds!
You get delocalized pi bonds when there is resonance in a structure. This means that the double or triple bonds can be in different positions so the electrons (pi bond) are delocalized around the molecule.
Localized electrons exhibit normal behavior, a localized lone pair remains close to one atom, and a localized bond pair travels between two atoms. Resonance hybrids necessarily contain some "abnormal" electrons. In a delocalized pi bond, instead of sticking near one atom, it visits two atoms.
Delocalized pi bonds occur in molecules that have resonance structures in which the double or triple bonds can be drawn in different locations between atoms. The electrons are free to move over more than two nuclei.
Delocalized pi bond is formed when 2 or more pi bonds are too close together so that they overlap. As a result, the electrons are free to move in the overlapped region. An example would be benzene where 3 pi bonds overlap, causing the formation of 6 delocalized electrons.
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