Which of the following is diamagnetic?

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(D) To determine the magnetic property,we look at the Molecular Orbital $(MO)$ configuration of each species:$H_{2}^{+}$ ($1$ electron): $\sigma 1s^{1

Vedclass · Accepted Answer

$N_{2}$

Vedclass · Answer

(D) To determine the magnetic property,we look at the Molecular Orbital $(MO)$ configuration of each species:$H_{2}^{+}$ ($1$ electron): $\sigma 1s^{1}$ (Paramagnetic due to $1$ unpaired electron).$He_{2}^{+}$ ($3$ electrons): $\sigma 1s^{2}, \sigma^{*} 1s^{1}$ (Paramagnetic due to $1$ unpaired electron).$O_{2}$ ($16$ electrons): $\sigma 1s^{2}, \sigma^{*} 1s^{2}, \sigma 2s^{2}, \sigma^{*} 2s^{2}, \sigma 2p_{x}^{2}, \pi 2p_{y}^{2} = \pi 2p_{z}^{2}, \pi^{*} 2p_{y}^{1} = \pi^{*} 2p_{z}^{1}$ (Paramagnetic due to $2$ unpaired electrons).$N_{2}$ ($14$ electrons): $\sigma 1s^{2}, \sigma^{*} 1s^{2}, \sigma 2s^{2}, \sigma^{*} 2s^{2}, \pi 2p_{y}^{2} = \pi 2p_{z}^{2}, \sigma 2p_{x}^{2}$ (Diamagnetic as all electrons are paired).Therefore,$N_{2}$ is the correct answer.

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