Final answer:
The overlap of Py and s orbitals does not form typical bonding or antibonding molecular orbitals since their symmetries and spatial orientations are different. Instead, sigma and pi molecular orbitals are formed by end-to-end and side-to-side overlaps of s and p orbitals along the internuclear axis, respectively.
Step-by-step explanation:
The student is asking about the formation of non-bonding molecular orbitals with respect to the internuclear axis in the context of molecular orbital theory. If the z-axis is considered as the internuclear axis, the overlap of Py and s orbitals does not directly lead to the formation of bonding or antibonding molecular orbitals; instead, such interactions are more complex and typically less significant in molecular bonding compared to the direct overlaps forming sigma or pi bonds.
For example, a pi (π) bonding molecular orbital is formed by the side-to-side overlap of two p orbitals, which results in the electron density being found on opposite sides of the internuclear axis. Similarly, a sigma (σ) bond is produced by the end-to-end overlap of p orbitals or s orbitals along the internuclear axis. The py orbitals are oriented perpendicular to the z-axis and their side-to-side overlap can lead to the formation of pi (π) molecular orbitals.
Nonetheless, in the specific case of the overlap of Py + s, it doesn't conform to the typical bonding interactions due to the differing symmetries and spatial orientations of the s and p orbitals, and such combination does not correspond straightforwardly to the formation of typical σ or π molecular orbitals.