Final answer:
The statement is true; nonbonding pairs, or lone pairs, are larger than bonding pairs due to increased electrostatic repulsion, affecting molecular shape and stability.
Step-by-step explanation:
The statement that nonbonding pairs are physically larger than bonding pairs is true. Nonbonding pairs, also known as lone pairs, occupy more space around the central atom than bonding pairs due to increased electrostatic repulsions. This differences in space occupation is important when considering the shape and geometry of molecules, as represented by VSEPR theory. Lone pairs have a greater repulsive effect on adjacent electron pairs, thus affecting the overall molecular shape.
Bonding pairs, on the other hand, are shared between two nuclei and help to stabilize the system through lowering the energy. As the overlap between two atomic orbitals increases, we see that the difference in energy between the bonding and antibonding molecular orbitals also increases.