(c) It turns out that the difference in energies between the valence atomic orbitals of H and F are sufficiently different that we can neglect the interaction of the 1s orbital of hydrogen with the 2s orbital of fluorine.
The 1s orbital of hydrogen will mix only with one 2p orbital of fluorine. Draw pictures showing the proper orientation of all three 2p orbitals on F interacting with a 1s orbital on H. Which of the 2p orbitals can actually make a bond with a 1s orbital, assuming that the atoms lie on the z-axis?

Verified step by step guidance

1. Identify the atomic orbitals involved: The hydrogen atom has a 1s orbital, and the fluorine atom has three 2p orbitals (2p_x, 2p_y, and 2p_z).
2. Understand the orientation: Since the atoms lie on the z-axis, the 2p_z orbital of fluorine is aligned along this axis, making it the most likely candidate to interact with the 1s orbital of hydrogen.
3. Visualize the orbitals: Draw the 1s orbital of hydrogen as a sphere centered on the z-axis. For fluorine, draw the 2p_x and 2p_y orbitals as dumbbell-shaped lobes perpendicular to the z-axis, and the 2p_z orbital as a dumbbell-shaped lobe along the z-axis.
4. Determine the interaction: The 1s orbital of hydrogen can overlap with the 2p_z orbital of fluorine because they are both aligned along the z-axis, allowing for effective overlap and bond formation.
5. Conclude the bonding: The 2p_x and 2p_y orbitals of fluorine do not align with the 1s orbital of hydrogen along the z-axis, so they do not participate in bonding. Only the 2p_z orbital of fluorine can form a sigma bond with the 1s orbital of hydrogen.

Key Concepts

Atomic Orbitals

Atomic orbitals are regions in an atom where there is a high probability of finding electrons. The 1s orbital is spherical and closest to the nucleus, while p orbitals (like the 2p) have a dumbbell shape and are oriented along specific axes (x, y, z). Understanding the shapes and orientations of these orbitals is crucial for predicting how atoms will interact and bond with each other.

Orbital Hybridization

Orbital hybridization is the concept where atomic orbitals mix to form new hybrid orbitals that can form bonds. In this case, the 1s orbital of hydrogen can interact with the 2p orbitals of fluorine, but only certain orientations will allow for effective overlap and bonding. This concept helps explain the geometry and strength of chemical bonds formed between atoms.

Molecular Orbital Theory

Molecular orbital theory describes how atomic orbitals combine to form molecular orbitals, which can be occupied by electrons from the bonded atoms. The interaction between the 1s orbital of hydrogen and the 2p orbitals of fluorine leads to the formation of bonding and antibonding molecular orbitals. This theory is essential for understanding the stability and properties of the resulting molecule.