Could someone please explain the following?

These are the potential energy diagrams I discussed in Unit 2-2.2 | Intramolecular Forces and Potential Energy. Please review the accompanying notes as well.

On the Y-axis, we have potential energy (PE), while the X-axis represents the separation distance between atoms. At the far right of the graph, where the atoms are infinitely apart, there is no attraction or repulsion, and the potential energy is nearly zero.

As the atoms move closer to each other, attraction increases, causing the potential energy to decrease. The lowest point on the graph represents the equilibrium distance, or the bond length, where the attractive and repulsive forces between the atoms are balanced. This is the most stable configuration.

If the atoms are pushed even closer, repulsive forces dominate, causing the potential energy to rise sharply.
Graph A is with the above explanation.
However He never makes a bond so there is not potential energy curve for He atoms making a bond.

This is the answer that I wrote on my test but my teacher marked it wrong and said it was B. Any thoughts?

In He atom there is no bond formation so howcome this question is made.Even in graph B he is showing decreases in potentail energy may be small.But Noble element Helium never makes a bond.
I explained you the graph of formation of a covalent bond.He gave you He atoms and they do not make bonds by sharing.
B diagram is showing that He atoms are making bonds with very low bond energies.I dont think question frmaed by teacher is correct.