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Dissociation energy

  1. Feb 7, 2008 #1
    I am having some trouble understanding this concept. I get that the dissociation energy for N2 is much greater than N2+ because of the triple bond, which makes a stronger bond, and therefore it is harder to remove one bond, compared to N2+ where it is easier to remove the bond because of one less electron. My professor today though was saying that for oxygen, the dissociation energy of O2+ is higher than just O2. She explained why with orbital theory, but I was having trouble keeping up Can someone tell me why?

    thanks
     
  2. jcsd
  3. Feb 8, 2008 #2
    bond order = (#electrons in bonding orbitals - #electrons in antibonding orbitals)/2

    In N2, bond order is (8-2)/2 = 3
    In N2+, it is (7-2)/2 = 2.5 (lower, weaker bond)

    Your textbook should have MO pictures for N2, O2

    Do a similar calculation for O2, you should see why O2+ has a higher bond order
     
  4. Feb 8, 2008 #3
    thank you for your help
     
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