N₂ (Nitrogen molecule)
- Total electrons = 14
- Orbital filling: all electrons get paired.
- Bond order = 3 → triple bond
- Magnetism: Diamagnetic (no unpaired electrons).
O₂ (Oxygen molecule)
- Total electrons = 16
- Orbital filling: two electrons remain unpaired in higher orbitals.
- Bond order = 2 → double bond
- Magnetism: Paramagnetic (because of unpaired electrons).
Key difference:
- N₂ has a triple bond and is diamagnetic.
- O₂ has a double bond and is paramagnetic.