Molecular orbital theory and Lewis structure for dioxygen

I am a bit confused about how molecular bond theory predicts pairings of unbounded electrons. For example, in $\ce{O2}$ there are two pairs of electrons on each oxygen along with the double bond. However, in the molecular orbital diagram, there are two unpaired electrons in degenerate $\pi$ antibonding orbitals. Obviously, bond order predicts the double bond. But how can one "predict" the two pairs of non-bonded electrons in $\ce{O2}$ from this?


[![enter image description here](https://i.stack.imgur.com/FirrO.jpg)](https://i.stack.imgur.com/FirrO.jpg)


Source: <https://commons.wikimedia.org/wiki/File:Oxygen_molecule_orbitals_diagram.JPG>


Pairs of non bounded electron refer to these -> ++++++++++++ooooo++++++++++ooooo++++
[![enter image description here](https://i.stack.imgur.com/byrjg.jpg)](https://i.stack.imgur.com/byrjg.jpg)


