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.