According to VBT O2 will be diamagnetic and according to MOT O2 will be paramagnetic

Paramagnetic, Diamagnetic, or Ferromagnetic?

Introduction:
In order to determine whether O2 is paramagnetic, diamagnetic, or ferromagnetic, we need to understand the magnetic properties of these terms.

Diamagnetic:
Diamagnetic substances have all of their electrons paired up in their orbital shells, resulting in a net magnetic moment of zero. This means that diamagnetic substances are not attracted to a magnetic field.

Paramagnetic:
Paramagnetic substances have unpaired electrons in their orbital shells, resulting in a net magnetic moment greater than zero. This means that paramagnetic substances are weakly attracted to a magnetic field.

Ferromagnetic:
Ferromagnetic substances have unpaired electrons and exhibit a strong attraction to a magnetic field. They can be magnetized and retain their magnetization even after the external magnetic field is removed.

Analysis:
To determine the magnetic properties of O2, we need to examine its electron configuration.

Oxygen (O) has atomic number 8, which means it has 8 electrons. The electron configuration of oxygen is 1s2 2s2 2p4. We can see that there are two unpaired electrons in the 2p orbital. These unpaired electrons make oxygen paramagnetic.

Conclusion:
Based on the analysis of the electron configuration, we can conclude that O2 is paramagnetic because it has unpaired electrons in its orbital shells.