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From what I understood in class, I believe this means that the electrons in that structure are not bound to one specific covalent bond between two atoms but are instead shared amongst many of the atoms in that molecule. Hope this helps.
Because the actually resonance structure is a blend of all possible Lewis structures. So, the electrons in double bonds are not bound to one specific bond between two atoms but rather located among the bonds between the atoms throughout the molecule.
Since the actual structure of the molecule is an average of its possible resonance structures, this means that the electrons are not involved in just one bond, but shared among multiple bonds throughout the same molecule.
From what i understood and wrote in my notes, for an electron to be delocalized means it can be shared in different positions of the molecule. For example with benzene, an electron can be bonded between different carbon atoms, not some set three.
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