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(D) The electronic configuration of the $O_2$ molecule ($16$ electrons) is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \p

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Unpaired electrons in the antibonding $\pi$ molecular orbital

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(D) The electronic configuration of the $O_2$ molecule ($16$ electrons) is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$. According to Hund's rule,the last two electrons enter the degenerate antibonding $\pi^*$ molecular orbitals singly. These two unpaired electrons in the $\pi^* 2p_x$ and $\pi^* 2p_y$ orbitals are responsible for the paramagnetic nature of the $O_2$ molecule.

According to molecular orbital theory,the paramagnetism of the $O_2$ molecule is due to the presence of

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