According to the molecular orbital energy-level diagram below, which one of the following statements is not correct about NO, NO+, and NO−? These molecular orbitals are formed from the 2s and 2p atomic orbitals.

The untrue statement among the options is that only one of the species is paramagnetic.

In the molecular orbital model, electrons could be filled into molecular orbitals according to the Aufbau principle in the same way electrons can be filled into atomic orbitals.

The molecular orbital configuration of the species listed are as follows;

NO = (σ2s)2 (σ⋆2s)2 (π2px)2 (π2pz)2 (σ2pz)2 (π2p⋆x)1

NO+ =  (σ2s)2 (σ⋆2s)2 (π2px)2 (π2p)2 (σ2pz)2

NO− = (σ2s)2 (σ⋆2s)2 (π2px)2 (π2p)2 (σ2pz)2 (π2p⋆x)1 (π2p⋆y)1

From this information, the untrue among the options is that only one of the species is paramagnetic. This is because both NO and NO- are paramagnetic.

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None of the statement is not correct about NO, NO+, and NO−.

Explanation:

Those molecules whose all subshells are completely filled are diamagnetic.

Those molecules whose any sub-shell is incomplete is termed paramagnetic.

Let us check the magnetism in all three molecules based on molecular orbital theory and Lewis structure

NO= number of electrons 11

It form N=O having configuration 1s2,2s2,2p6,3s1, it has 1 unpaired electron so it is paramagnetic.

Now NO-, number of electrons 12 having configuration 1s2,2s2,2p6,3s2, no unpaired electron hence dimagnetic.

Now NO+, number of electrons is 10 having configuration 1s2,2s2,2p6,3s2, dimagnetic

Let us calculate the bond order of NO-

N0- have 12 electrons as 5 of nitrogen, 6 of oxygen and 1 of - charge on oxygen.

So, bond order =

                          = 2 double bonds

bond order of NO+, Number of electrons is 10

bond order=

bond order = 3

bond order of NO, number of electrons 11

bond order=

bond order=2.5

Larger the bond order shorter the bond.

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