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A resonance hybrid is a blending of the Lewis structures for a molecule. For example, with the nitrate ion, you have 3 possible Lewis structures where the double bonds are in different positions. However, instead of only having one structure represent the nitrate ion (NO3-), it's better to have a resonance hybrid of them, a blend of them together. This resonance is depicted with double headed arrows between each structure to show that all of them are valid.
A resonance hybrid represents electron delocalization. Though the Lewis structures may indicate a different between the single and double bonds, suggesting a difference in bond length, if a molecule or compound is a resonance hybrid then the electrons delocalize and there is no difference in bond length—rather, all bonds of the same type will have the same bond length.
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