Electron affinity of nitrogen is lower than that of its neighbouring elements, carbon and oxygen. Explain.
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since nitrogen has half filled p orbital in its valence shell so it does not tend to accept another electron as half filled configuration is more stable . but in order to add one more electron energy has to be supplied and thus it's E. A. is lower than C and O.
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To answer this question, we should first know about Electron Affinity.
What is Electron Affinity?
Electron affinity is the amount of energy that is released when an atom is added to an atom.
Why Electron Affinity of Nitrogen is lower than Carbon and Oxygen?
- If we look at the electronic configuration of nitrogen that is 1s² 2s² 2px¹ 2py¹ 2pz¹. Nitrogen has a stable half-filled P orbital so the atom will face repulsion which will result in more release of energy.
- That is why Nitrogen electron affinity is Negative. On the other hand, In carbon, electron is added in one of the empty p orbital and that is why less energy is released.
- In case of Oxygen, the electron will be added to an orbital that already has an electron. Electron affinity will be positive in this case because nuclear charge will over power the repulsion.
That is why Nitrogen has less electron affinity than carbon and oxygen.
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Learn more about electron affinity
What is electron affinity
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