ACS Chemistry Practice Exam 2026 – The All-in-One Guide to Exam Success!

The molecular geometry of a molecule with 4 bonding pairs and 0 nonbonding pairs is tetrahedral. In a tetrahedral arrangement, the central atom is surrounded by four atoms or groups of atoms that are spaced as far apart as possible. The angles between these bonds are approximately 109.5 degrees, which minimizes the repulsion between the bonded electron pairs in accordance with VSEPR (Valence Shell Electron Pair Repulsion) theory.

The tetrahedral geometry occurs specifically when there are no lone pairs on the central atom that would alter the shape by introducing repulsive forces that would compress bond angles. In this case, with 4 bonding pairs and no nonbonding pairs, the electron pairs orient themselves in a way that maximizes their distance from each other, leading to the characteristic tetrahedral shape.

The other geometries listed do not apply here; for instance, a square planar arrangement involves coordination of 4 atoms in a plane with 2 nonbonding pairs, which is not the scenario described. Similarly, pyramidal geometry typically includes one lone pair of electrons, leading to a shape that is not tetrahedral. Octahedral geometry involves 6 bonding pairs, which exceeds the number specified in the question. Thus, the identification