Final answer:
The statement that Boron trifluoride has a trigonal planar electron domain and molecular geometry is true due to the VSEPR theory and sp² hybridization.
Step-by-step explanation:
The statement that Boron trifluoride has three bonding domains and its electron domain geometry is trigonal planar is true. Boron trifluoride (BF3) consists of a central boron atom with three single bonds to fluorine atoms. This geometry is a direct consequence of the VSEPR (Valence Shell Electron Pair Repulsion) theory, which predicts the arrangement around a central atom based on the repulsion between electron pairs.
Boron (B) has three valence electrons and forms three bonds with fluorine (F) atoms, with no lone pairs of electrons on the boron. The arrangement of these three bond pairs around the boron atom is in a single plane, with 120° angles between them, resulting in a trigonal planar shape. Additionally, the BF3 molecule is highly symmetrical, which means that it also adopts a trigonal planar molecular structure. This corresponds to sp² hybridization of the boron atom, where the s orbital mixes with two p orbitals to create three equal sp² hybrid orbitals that are used for bonding with the fluorine atoms.