Why ionization potential of nitrogen is higher than oxygen?
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The energy required to remove one electron from an atom called first ionization energy.
Usually, first ionization energy increases as we go across the period. As per trend oxygen should have higher first ionization energy than nitrogen. But this is not the reality.
Oxygen has smaller first ionization energy compared to nitrogen. We can explain by writing electronic configuration and valence orbital diagrams for both N and O below:(refer the attachment)
Nitrogen has three electrons in the p-orbital and each electron fill all the three p-orbital with aligned spins and stay farther apart. As the electrons in nitrogen p-orbital are half-filled and are stable and require more energy to remove one electron.
But in oxygen, there are four electrons in the p-orbital, as each electron fill the 3 p-orbital first and the fourth electron pairs up with already present electron in first p-orbital with opposite spins. This causes repulsion between electrons more than the ones in separate orbitals. This electron-electron repulsion causes this electron to get removed easily hence making oxygen to have lower than expected first ionization energy.
HOPE IT HELPS YOU AND MARK AS BRAINLIEST.......❤❤☺☺
The energy required to remove one electron from an atom called first ionization energy.
Usually, first ionization energy increases as we go across the period. As per trend oxygen should have higher first ionization energy than nitrogen. But this is not the reality.
Oxygen has smaller first ionization energy compared to nitrogen. We can explain by writing electronic configuration and valence orbital diagrams for both N and O below:(refer the attachment)
Nitrogen has three electrons in the p-orbital and each electron fill all the three p-orbital with aligned spins and stay farther apart. As the electrons in nitrogen p-orbital are half-filled and are stable and require more energy to remove one electron.
But in oxygen, there are four electrons in the p-orbital, as each electron fill the 3 p-orbital first and the fourth electron pairs up with already present electron in first p-orbital with opposite spins. This causes repulsion between electrons more than the ones in separate orbitals. This electron-electron repulsion causes this electron to get removed easily hence making oxygen to have lower than expected first ionization energy.
HOPE IT HELPS YOU AND MARK AS BRAINLIEST.......❤❤☺☺
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