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N2 has greater dissociation energy then N2+, where as O2 has a lower dissociation energy than O2+ because:
Dear Abhay,
Bond order = (#electrons in bonding orbitals - #electrons in antibonding orbitals)/2In N2, bond order is (8-2)/2 = 3In N2+, it is (7-2)/2 = 2.5 (lower, weaker bond)Your textbook should have MO pictures for N2, O2Do a similar calculation for O2, you should see why O2+ has a higher bond order.
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Dear Abhay ,
write the molecular orbital formula for both O2+ and O2
similarly do for N2 and N2+
according to aufbau principle , the energies of orbitals increases as 1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p
so note if the electrons are completely are partially filled.
if electrons are partially filled, then it is easier to break so it has higher dissociation enthalpy and
if electrons are completely filled in the orbitals , then it is harder to break them , so they have lower dissociation enthalpy.
The Molecular Oribitals filling will be given in the Chemical Bonding Chapter of your NCERT class XI Textbook
Hope that helps,
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