The paramagnetic nature of the oxygen molecul | vedclass

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(C) According to the Molecular Orbital Theory $(MOT)$,the electronic configuration of the oxygen molecule $(O_2)$ is: $\sigma 1s^2, \sigma^* 1s^2, \si

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Molecular orbital theory

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(C) According to the Molecular Orbital Theory $(MOT)$,the electronic configuration of the oxygen molecule $(O_2)$ is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$. Due to the presence of two unpaired electrons in the antibonding $\pi^*$ molecular orbitals,the oxygen molecule exhibits paramagnetic behavior. This phenomenon cannot be explained by the Valence Bond Theory or other classical models.

The paramagnetic nature of the oxygen molecule $(O_2)$ is best explained on the basis of:

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