Electronic Configuration:
* Nitrogen (N): 1s² 2s² 2p³
* Oxygen (O): 1s² 2s² 2p⁴
Key Factors:
1. Half-Filled p-Orbital: Nitrogen has a half-filled 2p orbital, meaning each of the three 2p orbitals contains a single electron. This configuration provides extra stability due to:
* Electron-electron repulsion: Having one electron in each orbital minimizes repulsion between electrons.
* Exchange energy: The ability of electrons with the same spin to exchange positions contributes to stability.
2. Electron-Electron Repulsion in Oxygen: Oxygen, with a 2p⁴ configuration, has two electrons in one of its 2p orbitals. This leads to increased electron-electron repulsion, making it slightly less stable than nitrogen.
Therefore:
Even though oxygen has one more electron than nitrogen, the half-filled p-orbital configuration in nitrogen provides a greater degree of stability. Removing an electron from this stable configuration requires more energy, leading to a higher ionization potential for nitrogen compared to oxygen.
In summary: The higher ionization potential of nitrogen is attributed to the enhanced stability of its half-filled p-orbital, which outweighs the extra electron in oxygen.
