Due to the presence of these unpaired electrons, O2 was found to be paramagnetic in nature. This explains why liquid oxygen is attracted in an external magnetic field. The bond order was also calculated to be equal to 2, signifying that it has a double bond between 2 oxygen atoms.
Oxygen (O2) is paramagnetic due to the presence of two unpaired electrons in its molecular orbital, which causes it to be weakly attracted to a magnetic field.
Here's a more detailed explanation:
Paramagnetism:
Paramagnetic substances are weakly attracted to a magnetic field because they contain unpaired electrons.
Molecular Orbital Theory:
The standard Lewis structure of O2 suggests all electrons are paired, implying diamagnetism. However, molecular orbital theory reveals that the last two electrons occupy separate, degenerate π orbitals, resulting in two unpaired electrons.
Unpaired Electrons:
These unpaired electrons are responsible for the paramagnetic behaviour of O2.
Experiment:
Liquid oxygen, when poured between the poles of a magnet, is attracted to the magnet, demonstrating its paramagnetic nature.
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