Paramagnetic vs Diamagnetic Properties of NO2
Finding whether NO2 is paramagnetic or diamagnetic involves analyzing the electron configuration of the molecule.

Paramagnetic Molecules
- Paramagnetic molecules have unpaired electrons in their molecular orbitals.
- When a molecule has unpaired electrons, it is attracted to a magnetic field.
- This attraction causes the molecule to be paramagnetic.

Diamagnetic Molecules
- Diamagnetic molecules have all paired electrons in their molecular orbitals.
- These molecules are slightly repelled by a magnetic field.
- This repulsion makes the molecule diamagnetic.

Determining the Paramagnetic/Diamagnetic Nature of NO2
- The molecular formula for NO2 is N2O4.
- The electron configuration for NO2 is written as σ2,σ*2,π4.
- This configuration shows that NO2 has unpaired electrons in its π molecular orbitals.
- Since NO2 has unpaired electrons, it is considered paramagnetic.
In conclusion, NO2 is paramagnetic due to the presence of unpaired electrons in its molecular orbitals. This analysis helps in understanding the magnetic properties of molecules based on their electron configurations.

No2 is paramegnatic