Answer :
Final answer:
The second ionization enthalpy of nitrogen is lower than oxygen due to the stable electronic configuration of nitrogen. Nitrogen's half-filled 2p orbital is difficult to ionize, hence requiring more energy. On the other hand, the ionization of oxygen results in a similar stable configuration and less electron-electron repulsion, therefore needing less energy.
Explanation:
The second ionization enthalpy of nitrogen is lower than that of oxygen primarily due to the stable electronic configuration of nitrogen. This is connected with the factor that ionization energy increases with the increase in stability of an atom's electronic configuration. In nitrogen's case, it exhibits a half-filled stable configuration in the 2p orbitals. Therefore, it's harder to remove an electron from nitrogen's stable half-filled orbital, consequently requiring more energy.
Meanwhile, when oxygen is ionized, it achieves a similar half-filled configuration, which is relatively more stable and thus, less energy is needed for the second ionization. It's important to mention electron-electron repulsion as well. In the case of oxygen, before the second ionization, there are two electrons in one of its 2p orbitals. The removal of one electron reduces this electron-electron repulsion, which also contributes to a lower ionization energy.
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