VSEPR calculation for boron trifluoride, BF3

Boron trifluoride only has six valence electrons and is one of the relatively rare second period covalent molecules that disobeys the octet rule. There are three bonded groups and so no lone pairs. Six electrons implies three electron pairs and therefore a trigonal geometry.

I will check into that. Thanks

The answer to this question is incorrect on the practice study.com quiz

The molecular geometry of BF3 is trigonal planar with symmetric charge distribution on the central atom.