Question

According to the VSEPR theory, what is the shape of a molecule that has a central atom bound to three other atoms with no lone pairs of electrons?

Answer 1

Triangular planar structure

Answer 2

Step-by-step 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 =
`(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 =
`(1)/(2)[V+N-C+A]`

=
`(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.