The electron distribution in ${\text{O}}_2^{-}$ is :

${\mathrm{\sigma }}_{1\mathrm{s}}^2{\mathrm{ }\mathrm{\sigma }}_{2\mathrm{s}}^{\mathrm{*}2}\mathrm{ }{\mathrm{\sigma }}_{2\mathrm{s}\mathrm{ }}^2{\mathrm{\sigma }}_{2\mathrm{s}\mathrm{ }}^{\mathrm{*}2}{\mathrm{\sigma }}_{2\mathrm{p}\mathrm{x}\mathrm{ }}^2{\mathrm{\sigma }}_{2\mathrm{p}\mathrm{y}\mathrm{ }}^2{\mathrm{\sigma }}_{2\mathrm{p}\mathrm{z}\mathrm{ }}^2{\mathrm{\sigma }}_{2\mathrm{p}\mathrm{y}\mathrm{ }}^{\mathrm{*}2}{\mathrm{\sigma }}_{2\mathrm{p}\mathrm{z}\mathrm{ }}^{\mathrm{*}1}$

$\therefore \mathrm{ }{\mathrm{O}}_2^{2-}$ is diamagnetic and ${\mathrm{O}}_2^{-}$ is paramagnetic. In $\mathrm{A}\mathrm{l}{\mathrm{O}}_2^{-}$, oxide ions $\left({\mathrm{O}}^{2-}\right)$ are present

and oxide ion is diamagnetic.

${\mathrm{N}\mathrm{O}}_2$ has one unpair electron hence paramagnetic but $\mathrm{N}{\mathrm{O}}_2^{+}$ has no unpair electron therefore diamagnetic