Hybridization of BF₃

Boron trifluoride (BF₃) undergoes sp² hybridization. Hybridization is a concept used to describe the mixing of atomic orbitals to form new hybrid orbitals that are involved in bonding.

1.0Hybridization in BF₃ 

2.0Boron's Atomic Structure

• Boron has an atomic number of 5, and its electron configuration is 1s² 2s² 2p¹.
• The outermost shell of boron, the valence shell, has only three electrons.
• Lewis structure represents the bonding in BF₃, showing how boron and fluorine share electrons to achieve a more stable arrangement.

3.0Hybridization Process

• In BF₃, boron forms three sigma (σ) bonds with three fluorine atoms. Each bond involves the overlap of an atomic orbital from boron with an atomic orbital from fluorine.
• To explain this bonding, boron undergoes hybridization to form three equivalent sp²  hybrid orbitals.

4.0sp²  Hybridization

• In sp² hybridization, one 2s orbital and two 2p orbitals of boron combine to create three equivalent sp²  hybrid orbitals.
• The 2s orbital and two 2p orbitals undergo mathematical combinations to yield three hybrid orbitals with a trigonal planar arrangement.

5.0Formation of Sigma Bonds

• Each sp² hybrid orbital of boron overlaps with a 2p orbital from a fluorine atom, resulting in the formation of three sigma (σ) bonds.
• Sigma bonds are formed by the head-on overlap of orbitals along the internuclear axis.

6.0Molecular Geometry

• The three sigma bonds and the absence of lone pairs on boron lead to a trigonal planar molecular geometry for BF₃. Which is shared below:
  
• The bond angles in BF₃ are approximately 120 degrees, reflecting the equilateral triangular arrangement of the three sigma bonds around boron.