In which of the following ionization processe | vedclass

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(C) To determine the change in bond energy and magnetic behavior,we analyze the Molecular Orbital Theory $(MOT)$ configurations:$1$. For $NO$ ($15$ el

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$NO \rightarrow NO^+$

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(C) To determine the change in bond energy and magnetic behavior,we analyze the Molecular Orbital Theory $(MOT)$ configurations:$1$. For $NO$ ($15$ electrons): Configuration 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 is paramagnetic due to the unpaired electron in the $\pi^*$ orbital. Bond order = $(10-5)/2 = 2.5$.$2$. For $NO^+$ ($14$ electrons): Configuration is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2$. It is diamagnetic as all electrons are paired. Bond order = $(10-4)/2 = 3.0$.Since the bond order increases from $2.5$ to $3.0$,the bond energy increases,and the magnetic behavior changes from paramagnetic to diamagnetic.

In which of the following ionization processes does the bond energy increase and the magnetic behaviour change from paramagnetic to diamagnetic?

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