What is the molecular geometry of a molecule with a central atom that has 4 bonding pairs and no lone pairs?

The molecular geometry of a molecule with a central atom that has four bonding pairs and no lone pairs is tetrahedral. This geometry arises because the four bonding pairs are arranged to minimize repulsion between them, following VSEPR (Valence Shell Electron Pair Repulsion) theory. In a tetrahedral arrangement, the bonding pairs are positioned at the corners of a tetrahedron, with bond angles of approximately 109.5 degrees, which is optimal for minimizing electron pair repulsions.

In contrast, the other geometries listed would not be suitable for a molecule with this specific combination of bonding and lone pairs. For instance, a trigonal planar geometry would typically be associated with three bonding pairs and no lone pairs, while a linear geometry applies to two bonding pairs with angles of 180 degrees. An octahedral arrangement involves six bonding pairs, which does not apply here. Thus, the presence of four bonding pairs distinctly indicates a tetrahedral molecular shape.