Determine the hybridization of the central atom in BF3.

Determine the hybridization of the central atom in BF3.

Step 1: Identify the central atom in BF3, which is boron (B).
Step 2: Count the number of bonds boron forms with surrounding atoms. In BF3, boron forms three bonds with three fluorine (F) atoms.
Step 3: Determine the number of electron groups around the central atom. Boron has three bonding pairs and no lone pairs.
Step 4: Use the VSEPR theory to determine the geometry. Three bonding pairs result in a trigonal planar shape.
Step 5: Identify the hybridization that corresponds to a trigonal planar shape. This is sp2 hybridization.
Step 6: Conclude that boron in BF3 is sp2 hybridized, forming three equivalent sp2 hybrid orbitals.

Hybridization – The concept of hybridization involves the mixing of atomic orbitals to form new hybrid orbitals that can accommodate bonding.
Molecular Geometry – Understanding the molecular geometry of BF3 helps in determining the hybridization of the central atom.
Valence Bond Theory – This theory explains how atomic orbitals combine to form bonds in molecules, which is essential for determining hybridization.