The molecular orbital theory supports paramag | vedclass

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(D) The molecular orbital electronic configuration of $Be_2$ is: $\sigma 1s^2 < \sigma^* 1s^2 < \sigma 2s^2 < \sigma^* 2s^2$. The molecular orbital el

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$O_2$

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(D) The molecular orbital electronic configuration of $Be_2$ is: $\sigma 1s^2 The molecular orbital electronic configuration of $C_2$ is: $\sigma 1s^2 The molecular orbital electronic configuration of $N_2$ is: $\sigma 1s^2 The molecular orbital electronic configuration of $O_2$ is: $\sigma 1s^2 Molecules having unpaired electrons are paramagnetic,and those without unpaired electrons are diamagnetic. Since $O_2$ has $2$ unpaired electrons in its antibonding molecular orbitals,it is paramagnetic. Conversely,$Be_2$,$C_2$,and $N_2$ have no unpaired electrons,making them diamagnetic.

The molecular orbital theory supports paramagnetic behaviour of:

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