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How would the Molecular orbitals of a theoretical BF (boron fluoride) look like?

How would the Molecular orbitals of a theoretical BF (boron fluoride) look like?
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When considering the amount of electrons per atom, remember boron has 5 in total, and fluorine has 9. From which, three from boron are considered as valence electrons, and seven from fluorine. Three different fluorine atoms will react with one boron to create the molecule in question.

Now, as the molecule will involve three sp2 orbitals when joined, it will be a flat molecule in the form of a triangle. Normally, this particular shape has angles between each orbital of around 120º. And it would look as:

It would then be a triangular plane, mainly.

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