Why the first ionization energy of nitrogen is the highest as compared to that of carbon and oxygen?

This is why one requires large amounts of energy to ionised the nitrogen atom. On the other hand, since Oxygen is already unstable relative to Nitrogen, by losing one electron it attains a stable half filled orbital. This is why nitrogen has a higher ionisation energy than oxygen.Click to see full answer. Beside this, which of the following has highest ionization enthalpy carbon nitrogen and oxygen and why?That’s why ionisation energy of Nitrogen is more than Oxygen. Answer: This is so because nitrogen has half filled electronic configuration. This energy will be higher for fully filled and half-filled electronic configuration than partially filled electronic configuration.Likewise, what is the first ionization energy of nitrogen? Ionization Energy is the Energy Required to Remove an Electron Element Electron Configuration First Ionization Energy IE1 Carbon (C) [He]2s22p2 1086 kJ/mol Nitrogen (N) [He]2s22p3 1400 kJ/mol Oxygen (O) [He]2s22p4 1314 kJ/mol Fluorine (F) [He]2s22p5 1680 kJ/mol One may also ask, why is the first ionization energy of beryllium greater than that of boron? the first ionization energy of beryllium is greater than that of boron because beryllium has a stable complete electronic configuration (1s2 2s2) so it requires more energy to remove the first electron from it.Why the ionization energy of nitrogen is more than oxygen?Nitrogen has a half filled orbital. On the other hand, since Oxygen is already unstable relative to Nitrogen, by losing one electron it attains a stable half filled orbital. So oxygen undergoes ionisation at a relatively lower energy. This is why nitrogen has a higher ionisation energy than oxygen.

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