07 - Chemistry 2000 Lecture 7 Delocalized molecular...

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Chemistry 2000 Lecture 7: Delocalized molecular orbitals Marc R. Roussel
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Back to MO theory The MOs of ozone I Ozone is planar, so there will be one p orbital from each oxygen atom perpendicular to the plane of the molecule. I These are the p orbitals that can be used for π bonding. (Why?) I With three p orbitals, we can make three MOs. I These MOs should have some of the symmetry of the molecule. I Represent the orientation of the MO by a + or - (e.g. + if the phase of the lobe of the p orbital sticking up is positive). I Possible arrangements: O O O + + + O O O + 0 + O O O - - + Type: bonding nonbonding antibonding
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Important: The π molecular orbitals are delocalized over the whole molecule.
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I MO diagram: O A O C O B I We can figure out how many electrons occupy the π orbitals from the Lewis diagram: O O O O O: :O .. .. .. .. .. .. .. .. .. .. I The four π electrons go into the 1 π and 2 π orbitals. I This gives us one two-electron bond shared between two “bonds”.
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