Final answer:
The relationship between potential energy and orbital overlap is key in molecular bonding, with greater overlap leading to a more stable system with lower potential energy. This concept is exemplified by the formation of bonding molecular orbitals when atomic orbitals, such as p or s orbitals, overlap effectively.
Step-by-step explanation:
The relationship between potential energy and orbital overlap is fundamental to understanding molecular bonding. In chemistry, as the overlap between two atomic orbitals increases, so does the difference in energy between the resulting bonding and antibonding molecular orbitals.
This concept is also evident in molecular orbitals formed by the overlap of two atomic s orbitals on adjacent atoms. An in-phase combination of these orbitals results in a lower energy bonding orbital, which translates to a more stable arrangement with lower potential energy.