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Orbitals aren't actual physical "places" for electrons to stay in, they just describe the probability of finding an electron in a specific region. So if an electron isn't "in" an orbital, that orbital doesn't exist, because the probability of finding an electron there is zero.
In terms of resonance Lewis Structure, electrons can be delocalized if they are free to move throughout the plane. This means that a double bond between Oxygen and Nitrogen, for example in the structure NO3, can be moved between any of the Oxygens while the remaining two form a single bond with Nitrogen.
In the terms of this class, it's an electron that isn't associated with a bond or single atom, so it's free to move about in the atom's space. It isn't "localized" or held to a specific region, like it would most likely be if it were in a bond.
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