Which of the following is diamagnetic?

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(D) The electronic configuration of $O_2$ 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 (\

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(D) The electronic configuration of $O_2$ is $(\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 (\sigma^* 2s)^2 (\sigma 2p_z)^2 (\pi 2p_x)^2 (\pi 2p_y)^2 (\pi^* 2p_x)^1 (\pi^* 2p_y)^1$,which contains two unpaired electrons,making it paramagnetic.$B_2$ has the configuration $(\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 (\sigma^* 2s)^2 (\pi 2p_x)^1 (\pi 2p_y)^1$,which contains two unpaired electrons,making it paramagnetic.$N_2^{+}$ has $13$ electrons with the configuration $(\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 (\sigma^* 2s)^2 (\pi 2p_x)^2 (\pi 2p_y)^2 (\sigma 2p_z)^1$,which contains one unpaired electron,making it paramagnetic.Since all the given species are paramagnetic,the correct option is $D$.

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