Step 1: Identify the central atom in BF3, which is boron (B).
Step 2: Count the number of bonds boron forms with fluorine (F) atoms. BF3 has three F atoms bonded to B.
Step 3: Determine the number of lone pairs on the central atom (B). In BF3, there are no lone pairs on boron.
Step 4: Use the VSEPR theory, which states that the shape of a molecule is determined by the number of bonding pairs and lone pairs around the central atom.
Step 5: Since there are three bonding pairs and no lone pairs, the molecular geometry is trigonal planar.
