Consider the molecule BF3. (c) What hybrid orbitals should be constructed on the B atom to make the B–F bonds in BF3?

Key Concepts

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that can accommodate bonding. In BF3, the boron atom undergoes sp2 hybridization, which involves mixing one s orbital and two p orbitals to create three equivalent sp2 hybrid orbitals. This allows boron to form three sigma bonds with fluorine atoms.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. In the case of BF3, the sp2 hybridization leads to a trigonal planar geometry, where the three B–F bonds are arranged at 120-degree angles around the boron atom. Understanding molecular geometry is crucial for predicting the shape and reactivity of molecules.

Bonding and Lone Pairs

In covalent bonding, atoms share electrons to achieve stability. In BF3, boron forms three bonds with fluorine atoms, utilizing its sp2 hybrid orbitals. Importantly, boron has an incomplete octet, as it does not have any lone pairs of electrons, which influences its reactivity and the overall electron deficiency of the molecule.