Explanation:
A molecule which contains three bond pairs but no lone pair of electrons will have a trigonal planar geometry.
Hybridization of such a geometry is \(sp^{2}\).
For example, \(BF_{3}\) is a trigonal planar molecule.
As, hybridization of \(BF_{3}\) will be calculated as follows.
Hybridization = \(\frac{1}{2}[V+N-C+A]\)
where,
V = number of valence electrons present in central atom
N = number of monovalent atoms bonded to central atom
C = charge of cation
A = charge of anion
Hybridization = \(\frac{1}{2}[V+N-C+A]\)
= \(\frac{1}{2}[3 + 3]\)
= 3
So, the hybridization of \(BF_{3}\) will be \(sp^{2}\). As there are 3 bond pairs and no lone pair of electrons. Hence, the geometry of \(BF_{3}\) is trigonal planar.
Thus, we can conclude that according to the VSEPR theory, the shape of a molecule that has a central atom bound to three other atoms with no lone pairs of electrons is trigonal planar.
