Which of the following statements is correct?

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(A) According to Molecular Orbital Theory $(MOT)$: $1$. The electronic configuration of $O_2$ ($16$ electrons) is $\sigma 1s^2, \sigma^* 1s^2, \sigma

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Oxygen and nitric oxide molecules are both paramagnetic because both contain unpaired electrons.

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(A) According to Molecular Orbital Theory $(MOT)$: $1$. The electronic configuration of $O_2$ ($16$ electrons) is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$. It has two unpaired electrons in the antibonding $\pi^*$ orbitals,making it paramagnetic. $2$. The electronic configuration of $NO$ ($15$ electrons) is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1$. It has one unpaired electron in the antibonding $\pi^*$ orbital,making it paramagnetic. Therefore,both $O_2$ and $NO$ are paramagnetic due to the presence of unpaired electrons.

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