Question

What is the hybridization of Boron in $BF_3$ molecules?

Answer 1

Hint: Hybridization is that the concept of atomic orbitals fuse to form newly hybridized orbitals, which successively influences molecular geometry and bonding properties. Hybridization is additionally an expansion of the valence bond theory.

Complete answer:
Total no. of bonds formed in $BF_3$ molecules are 3 and each one among them are sigma bonds and there exist no lone pair of electrons in Boron.
 So, hybridization involving 3 sigma bonds and 0 lone pair of electrons is $sp_2$.
Hence, hybridization of Boron in the $BF_3$ molecule is $sp_2$.
Boron trifluoride is the compound with the formula $BF_3$. This pungent colourless toxic gas forms white fumes in moist air. It is a useful Lewis acid and a versatile building block for other boron compounds.
The geometry of the $BF_3$ molecule is known as trigonal planar. The fluorine atoms are positioned at the vertices of an equilateral triangle. The F-B-F angle is $120^o$ and each one four atoms dwell in the same plane.
$BF_3$ (Boron trifluoride) is Non-Polar thanks to its highly symmetric shape. It is a Trigonal Planar geometry which cancels out the dipole moments of the three BF bonds making the resultant moment of the compound capable 0 (Zero).

Note:
$BF_3$ is an $sp_2$ hybridization. It's $sp_2$ for this molecule because one π bond is required for the chemical bond between the Boron, and just three σ bonds are produced per Boron atom. The atomic S and P – orbitals in Boron outer shell mix to form three equivalent hybrid orbitals of $sp_2$.