Nitrogen has more first ionization energy than first ionization energy as electronic configuration of nitrogen is
The 2p orbital of nitrogen is half filled as it is considered as stable configuration because there is equal exchange of energies between the electrons of 2p orbital
Secondly the half filed orbital has a plane of symmetry thus it is considered as stable configuration.
When electron is being removed form a stable configuration the energy requires would be higher because a stable configuration is shifted to an unstable configuration.
But in case of Oxygen the configuration is one more than half filled configuration.
So oxygen would readily loose an electron to attain a stable configuration that is half filled configuration.
So first Ionization energy of nitrogen is more than first ionization energy of Oxygen.
The 2p orbital of nitrogen is half filled as it is considered as stable configuration because there is equal exchange of energies between the electrons of 2p orbital
Secondly the half filed orbital has a plane of symmetry thus it is considered as stable configuration.
When electron is being removed form a stable configuration the energy requires would be higher because a stable configuration is shifted to an unstable configuration.
But in case of Oxygen the configuration is one more than half filled configuration.
So oxygen would readily loose an electron to attain a stable configuration that is half filled configuration.
So first Ionization energy of nitrogen is more than first ionization energy of Oxygen.
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