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The problem is that we 'know' the shapes of atomic orbitals from solutions of the Schroedinger equation, but do not know the shapes of molecular orbitals.
These are concepts that are used to explain why molecules have the shape that they do. Resonance and delocalisation are really both the same. Resonance suggests that there is rapid interchange between one electronic form and another whereas delocalisation suggests that the 'average' of the resonance forms is actually a better description.
Delocalisation can occur when orbitals overlap that have the same energy.
These are concepts that are used to explain why molecules have the shape that they do. Resonance and delocalisation are really both the same. Resonance suggests that there is rapid interchange between one electronic form and another whereas delocalisation suggests that the 'average' of the resonance forms is actually a better description.
Delocalisation can occur when orbitals overlap that have the same energy.
Alternate double and single bonds are conjugation. Yes, this also gives rise to resonance (delocalisation) because the p orbitals are all orientated in the same plane and can overlap.
Resonance forms can be seen by movement of pairs of electrons. If the electronic structure can be rearranged by movement of electron pairs then resonance is possible.
Learn some of the classic resonances such as the sulphate ion, the carbonate ion and the carboxylate ion and it will start to make sense.
Resonance forms can be seen by movement of pairs of electrons. If the electronic structure can be rearranged by movement of electron pairs then resonance is possible.
Learn some of the classic resonances such as the sulphate ion, the carbonate ion and the carboxylate ion and it will start to make sense.
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