Hybridization of BrF3 (Bromine Trifluoride)

The hybridization that takes place in BrF₃ is sp³d. We will understand how hybridization of BrF₃ occurs in the molecules as well as its molecular geometry and the bond angles below.

What is the Hybridization of Bromine Trifluoride?

To determine the hybridization of bromine trifluoride we will first take the bromine atom which is the central atom and look at its electron configuration. It is represented as;

1s² 2s²2p⁶ 3s²3p⁶3d¹⁰4s²4p⁵. However, in order to form bonds with the fluorine atom some electrons in Bromine are shifted to 4d-orbitals. Besides, fluorine has a higher oxidative capacity and therefore it forces bromine to promote electrons to the said level. Now, bromine can use the d-orbitals for hybridization.

BrF₃ will consist of seven electrons in its outermost shell. After the bond formation, it will further have 2 lone pairs and 3 Br—F covalent bonds. As the hybridization value or the electron pair is equal to 5 it gives rise to sp³d hybrid orbitals.

Important Points To Remember

• The central atom bromine uses the d-orbitals for hybridization.
• In BrF₃, it will have 2 lone pairs and 3 Br—F covalent bonds.
• Lone pairs take part in hybridization.

BrF₃ Molecular Geometry And Bond Angles

BrF₃ molecular geometry is said to be T-shaped or Trigonal Bipyramidal with a bond angle of 86.2^o which is slightly smaller than the usual 90°.

This angle formed due to the repulsion generated by the electron pairs which is greater than that of the Br-F bonds.

Read More About Hybridization of Other Chemical Compounds

• Hybridization Of XeF4
• Hybridization Of SF4
• Hybridization Of PCl3
• Hybridization Of Graphite
• Hybridization Of SO3