---
title: "The graph below shows the potential energy of a system of two isolated oxygen atoms as a function of the internuclear distance between them as they form an \\(\\text{O}_2\\text{(g)}\\) molecule.  Which of the following best predicts and explains how the potential energy curve for two isolated nitrogen atoms forming an \\(\\text{N}_2\\text{(g)}\\) molecule would compare to the curve shown for \\(\\text{O}_2\\text{(g)}\\)?"
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url: "https://nerd-notes.com/ubq/119936/"
date_modified: "2026-08-21T08:18:30+00:00"
---

# The graph below shows the potential energy of a system of two isolated oxygen atoms as a function of the internuclear distance between them as they form an \(\text{O}_2\text{(g)}\) molecule.

Which of the following best predicts and explains how the potential energy curve for two isolated nitrogen atoms forming an \(\text{N}_2\text{(g)}\) molecule would compare to the curve shown for \(\text{O}_2\text{(g)}\)?

The graph below shows the potential energy of a system of two isolated oxygen atoms as a function of the internuclear distance between them as they form an \(\text{O}_2\text{(g)}\) molecule.

Which of the following best predicts and explains how the potential energy curve for two isolated nitrogen atoms forming an \(\text{N}_2\text{(g)}\) molecule would compare to the curve shown for \(\text{O}_2\text{(g)}\)?

![A 2D line graph drawn on bare axes without gridlines. The horizontal axis is labeled Internuclear distance (\(\text{pm}\)), and the vertical axis is labeled Potential energy (\(\text{kJ/mol}\)). A horizontal dashed reference line extends across the plot marking zero potential energy. A single solid black curve represents the \(\text{O}_2\) molecule. At very small internuclear distances on the left, the curve begins high in the positive energy region, slopes steeply downward, passes through zero energy, reaches a single potential energy minimum in the negative region, and then curves smoothly upward to approach the dashed zero-energy line asymptotically at large distances. The minimum point represents the equilibrium bond length and bond energy of \(\text{O}_2\). No other curves, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787300310-FM8ij7.jpg)

- **A.** The minimum would be shifted to the right and be shallower, because nitrogen atoms have fewer valence electrons, resulting in weaker attractive forces and a longer bond.
- **B.** The minimum would be shifted to the left and be deeper, because the triple bond in \(\text{N}_2\) has a higher bond order and greater bond energy than the double bond in \(\text{O}_2\), resulting in a shorter, stronger bond.
- **C.** The minimum would be shifted to the left and be shallower, because nitrogen has a lower effective nuclear charge than oxygen, which weakens the bond despite having a shorter internuclear distance.
- **D.** The minimum would be shifted to the right and be deeper, because the greater number of shared electron pairs in \(\text{N}_2\) increases electron-electron repulsion, requiring a larger internuclear distance to achieve a stable bond.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119936/*