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They are essentially the same. Resonance refers to the movement of electrons within a molecule, delocalization refers to electrons being able to spread out. Delocalization can be thought of as a result or characteristic of resonance, but delocalization may also refer to electrons movements within solid state metals, which is not quite resonance.
A molecule with resonance refers to the fact that it has multiple bonds that can be placed in different locations within the molecule, without moving the individual atoms in the molecule. When a molecule has resonance, the electrons aren't localized at one particular atom, but rather they are delocalized throughout the whole molecule.
A resonance refers to one structure of many different but equivalent lewis structures of a molecule. The term "delocalization" refers to an electron that doesn't belong to just one single bond. A delocalized electron is spread out over the molecule. Professor Lavelle mentioned that a true representation of a molecule is one which combines all resonance structures, as shown by experimental data that all bonds are of equal lengths. The equivalent bond lengths is due to this delocalization of electrons.
Delocalization refers to electron moves around the atom to different bonds, which leads to resonance structure. This is why when you average out the bond length, they are all the same instead of a double bond being shorter than a single bond
Delocalization just represents a compound's typical behavior of dispersing charges to exterior elementsNatalie Benitez 1C wrote:So in terms of delocalization can we say this occurs when atoms form bonds with each other because in a way they are spreading out their electrons through sharing them?
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