Which of the following can be inferred from the diagram above that shows the dependence of potential — Bonding Chemistry Question

STEPS:

1. Understand how potential energy relates to atomic interactions: When two isolated atoms are far apart, they do not interact, and the potential energy of the system is close to zero. As they approach each other, electrostatic attractions between the nucleus of one atom and the electrons of the other pull them closer, which lowers the potential energy of the system.
2. Identify the stable bond configuration (energy minimum): The lowest point (the absolute minimum) on the potential energy curve represents the most stable state for the two-atom system. At this position, the attractive forces and repulsive forces between the atoms are perfectly balanced, making the net force between them exactly zero. This stable state corresponds directly to the formation of a chemical bond.
3. Locate the bond length on the graph: By examining the provided potential energy diagram, the minimum potential energy (the bottom of the well) corresponds to an internuclear distance of exactly $75\text{ pm}$ on the horizontal axis. Therefore, the atoms form a stable bond with a bond length of $75\text{ pm}$, which identifies Option B as the correct answer.
4. Determine the nature of the forces at other distances:
* Internuclear distances shorter than the minimum (e.g., $25\text{ pm}$): If the atoms are pushed closer than the stable bond length, the positively charged nuclei and negative electron clouds repel one another strongly. The potential energy rises sharply, meaning the net force between the atoms is highly repulsive.
* Internuclear distances longer than the minimum (e.g., greater than $75\text{ pm}$): If the atoms are pulled farther apart than the stable bond length, the electrostatic attractions pull them back together, meaning the net force between the atoms is attractive.

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WHY_OTHERS_WRONG:

• Option A is incorrect: At an internuclear distance of $25\text{ pm}$, the potential energy is extremely high and positive. A stable bond is not formed at this distance because the strong repulsive forces make the configuration highly unstable.
• Option C is incorrect: At $25\text{ pm}$, the atoms are forced too close together, well to the left of the energy minimum. In this region of the graph, the net force between the atoms is repulsive, not attractive.
• Option D is incorrect: At the stable bond length of $75\text{ pm}$ (the minimum of the curve), the attractive forces are exactly balanced by the repulsive forces. As a result, the net force between the two atoms is zero, not attractive.