Chemistry · Chemical Bonding

The correct answer is that the BF₃ molecule has a planar trigonal geometry. This is because the central boron atom forms three bonds with fluorine atoms, and there are no lone pairs on the boron atom. This arrangement leads to a 120-degree angle between the bonds, creating a planar triangular shape. Other options such as tetrahedral, linear, octahedral, and square planar do not fit the molecular structure of BF₃ because they involve different numbers and arrangements of surrounding atoms and lone pairs.

A tetrahedral geometry involves four atoms equidistant from each other around a central atom, which is not the case for BF₃.

A linear geometry involves two atoms at 180 degrees apart from the central atom, which does not match the structure of BF₃.

An octahedral geometry involves six atoms around a central atom, which is not applicable for BF₃.

BF₃ has a trigonal planar geometry due to three fluorine atoms symmetrically arranged around the central boron atom forming 120-degree angles.

A square planar geometry involves four atoms in a square around the central atom, which is not the structure of BF₃.