the first ionization energy of nitrogen atom
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Following are the electronic configurations of two elements:
N: 1s2, 2s2, 2p3
O: 1s2, 2s2, 2p4
As we can see that Nitrogen has half filled p orbitals which is relatively stable configuration as compared to 2p4 configuration of Oxygen atom so it is difficult to remove one electron from this stable configuration. Further, removal of one electron from Oxygen atom is relatively easy because it results in half filled stable p orbital configuration. That's why ionisation energy of Nitrogen is more than Oxygen.
N: 1s2, 2s2, 2p3
O: 1s2, 2s2, 2p4
As we can see that Nitrogen has half filled p orbitals which is relatively stable configuration as compared to 2p4 configuration of Oxygen atom so it is difficult to remove one electron from this stable configuration. Further, removal of one electron from Oxygen atom is relatively easy because it results in half filled stable p orbital configuration. That's why ionisation energy of Nitrogen is more than Oxygen.
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