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If a molecule's dipole moments cancel out, does this mean that structures with resonance have no net dipole movement? I think that was the case for neutral sulfite (SO3); it has resonance but the real molecule in reality has the bond length equal to the average of the bond lengths of the resonance structures, and the dipole moments cancel each other.
If a molecule does have dipole moments I'm not sure resonance would necessarily cancel out the dipole moments. This is because a molecule's dipole moments are due to the electrons being closer to one atom than the other in one specific bond of the molecule. Resonance distributes the electron density throughout the entire molecule, but that does not mean that electrons are shared equally between two atoms that have a high difference in electronegativity. So resonance would distribute the electron density evenly between let's say all the O-H bonds in a molecule, but within the O-H bonds, electrons are more closely gathered to oxygen which still creates a dipole moment (if the symmetry of the molecule does not cancel out the polarities).
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