With the help of molecular orbital energy level diagram compare the stability, magnetic behave of $O_{2}^{2 -}, N O$ .

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Solution

1)The molecular orbital diagram of $O_{2}^{2 -}$ is given in the diagram

The bond order of $O_{2}^{2 -}$ can be calculated as,
$\frac{1}{2} (N u m b e r o f b o n d i n g e l e c t r o n s - N u m b e r o f a n t i b o n d i n g e l e c t r o n s)$
$\frac{1}{2} (10 - 8)$
$1$
Hence with an increase in the number of electrons in the antibonding orbital the stability of the bond order decreases.
2)The molecular orbital diagram of $N O$ is shown in the diagram:
$N O$ which has 11 valence electrons in that 8 are bonding electrons and 3 are antibonding electrons.

The bond order of $N O$ can be calculated as:
$\frac{1}{2} (8 - 3)$
$2.5$
On comparing to the bond orders of $O_{2}^{2 -}$ and $N O$ the stability of the molecule can be defined.
Stronger the bonds will have higher bond energy and higher in the stability

In this case the $N O$ having high stability due to the high bond order.This is because when bond order is increased the molecule is more tightly bonded so that the bond length is decreased results in the more stability of the molecule.

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With the help of molecular orbital energy level diagram compare the stability, magnetic behave of O2−2,NO.

With the help of molecular orbital energy level diagram compare the stability, magnetic behave of $O_{2}^{2 -}, N O$ .