Why nitrogen has a higher first ionisation enthalpy than oxygen atom?
Answers
Answer:
In reality, the first ionisation energy of nitrogen is greater than the first ionisation energy of oxygen, because nitrogen, in a stable half filled orbital state, is comparatively more stable than oxygen.
Explanation:
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Answer:
(1) The electronic configuration of nitrogen (N, Z = 7) is 1s², 2s², 2p³ and that of oxygen (O, Z=8) is 1s², 2s² 2p^4.
(2) Nitrogen atom acquires extra stability due to half- filled 2p-orbitals while oxygen can acquire half-filled orbital and extra stability by losing one electron. Thus, oxygen can easily lose one electron.
(3) Nitrogen requires more energy to remove an electron due to extra stability. Therefore, first ionisation enthalpy of oxygen is less than that of nitrogen.