What is the geometry of a molecule with five bonded pairs of electrons and no lone pairs?

A molecule with five bonded pairs of electrons and no lone pairs exhibits trigonal bipyramidal geometry. This geometry arises from the arrangement of the five bonded pairs around a central atom to minimize electron pair repulsion, as described by the VSEPR (Valence Shell Electron Pair Repulsion) theory.

In a trigonal bipyramidal arrangement, there are three bonds in a plane (equatorial positions) and two bonds above and below this plane (axial positions). This arrangement maximizes the distance between the bonded pairs, which would result in the lowest energy configuration for the molecule.

For example, phosphorus pentachloride (PCl5) is a classic example of a molecule with this geometry, where phosphorus has five bonded pairs of chlorine atoms surrounding it. The lack of any lone pairs further supports the stability of this geometry, as lone pairs would create additional repulsion and change the shape of the molecule.

Thus, the geometry of a molecule with five bonded pairs and no lone pairs is indeed trigonal bipyramidal.