Solution

The given statement is False.
$$\displaystyle O_2$$ and $$\displaystyle O_2^-$$ are paramagnetic while $$\displaystyle O_2^{2-}$$ is diamagnetic.

If unpaired electrons are present in an ion/molecule, then it is paramagnetic.
If all electrons are paired, then the ion/molecule is diamagnetic

The MO electronic configurations are given.
$$\displaystyle O_2 : KK (\sigma 2s)^2(\sigma * 2s)^2 (\sigma 2px)^2 (\pi 2py)^2 (\pi 2pz)^2 (\pi * 2py)^1 (\pi * 2pz)^1 $$ 2 unpaired electrons.

$$\displaystyle O_2^- : KK (\sigma 2s)^2(\sigma * 2s)^2 (\sigma 2px)^2 (\pi 2py)^2 (\pi 2pz)^2 (\pi * 2py)^2 (\pi * 2pz)^1 $$ 1 unpaired electron.

$$\displaystyle O_2^{2-} : KK (\sigma 2s)^2(\sigma * 2s)^2 (\sigma 2px)^2 (\pi 2py)^2 (\pi 2pz)^2 (\pi * 2py)^2 (\pi * 2pz)^2 $$ 0 unpaired electrons.