Observe the following molecules / ions H_2, N | vedclass

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Question

(B) Based on Molecular Orbital Theory $(MOT)$: $H_2$ $(1s^2)$: No unpaired electrons $\rightarrow$ Diamagnetic $N_2$ $(KK(\sigma 2s)^2(\sigma^* 2s)^2(

Vedclass · Accepted Answer

$O_2, O_2^+, O_2^-, N_2^+$ show paramagnetic property

Vedclass · Answer

(B) Based on Molecular Orbital Theory $(MOT)$: $H_2$ $(1s^2)$: No unpaired electrons $\rightarrow$ Diamagnetic $N_2$ $(KK(\sigma 2s)^2(\sigma^* 2s)^2(\pi 2p_x)^2(\pi 2p_y)^2(\sigma 2p_z)^2)$: No unpaired electrons $\rightarrow$ Diamagnetic $O_2$ $(KK(\sigma 2s)^2(\sigma^* 2s)^2(\sigma 2p_z)^2(\pi 2p_x)^2(\pi 2p_y)^2(\pi^* 2p_x)^1(\pi^* 2p_y)^1)$: $2$ unpaired electrons $\rightarrow$ Paramagnetic $N_2^+$: $1$ unpaired electron $\rightarrow$ Paramagnetic $O_2^+$: $1$ unpaired electron $\rightarrow$ Paramagnetic $O_2^-$: $1$ unpaired electron $\rightarrow$ Paramagnetic $F_2$: No unpaired electrons $\rightarrow$ Diamagnetic Thus,$O_2, O_2^+, O_2^-, N_2^+$ are all paramagnetic.

Observe the following molecules / ions $H_2, N_2, O_2, N_2^+, O_2^+, O_2^-, F_2$. Identify the correct statement.

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