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Interpretation: The delocalized molecular orbital differ from localized molecular orbital such that in
Concept Introduction: Molecular orbitals are formed by the combination of the atomic orbitals of the atoms in the molecule. The properties of the newly formed molecular orbital will be different from their individual atomic orbitals. In molecular orbital theory, electrons shared by atoms in a molecule reside in the molecular orbitals.
In localized molecular orbital, molecular orbitals are considered to be localized between the individual bonds.
Delocalized molecular orbitals are extended over two or more atoms, these are not confined to adjacent bonding atoms. Therefore, the electrons are free to move around the entire molecule.
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Chemistry: Atoms First
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- Consider acetyl salicylic acid, better known as aspirin. Its structure is (a) How many sigma and pi bonds are there in aspirin? (b) What are the approximate values of the angles marked (in blue) A, B, and C? (c) What is the hybridization of each atom marked (in red) 1, 2, and 3?arrow_forwardIn the molecular orbital mode l, compare and contrast bonds with bonds. What orbitals form the bonds and what orbitals form the bonds? Assume the z-axis is the internuclear axis.arrow_forwardTrue or false: Boron contains 2s22p1 valence electrons, so only one p orbital is needed to form molecular orbitals.arrow_forward
- When is it desirable to use MO theory rather than valence bond theory?arrow_forwardElectrons in bonding molecular orbitals are most likely to be found in the region between the two bonded atoms. Why does this arrangement favor bonding? In a antibonding orbital, where are the electrons most likely to be found in relation to the nuclei in a bond?arrow_forward
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