---
title: "The potential energy curves for diatomic nitrogen, \\(\\text{N}_2\\), and diatomic oxygen, \\(\\text{O}_2\\), are represented in the graph as a function of internuclear distance.  Which of the following correctly identifies the curve corresponding to \\(\\text{N}_2\\) and provides the valid justification?"
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url: "https://nerd-notes.com/ubq/119644/"
date_modified: "2026-08-21T08:11:54+00:00"
---

# The potential energy curves for diatomic nitrogen, \(\text{N}_2\), and diatomic oxygen, \(\text{O}_2\), are represented in the graph as a function of internuclear distance.

Which of the following correctly identifies the curve corresponding to \(\text{N}_2\) and provides the valid justification?

The potential energy curves for diatomic nitrogen, \(\text{N}_2\), and diatomic oxygen, \(\text{O}_2\), are represented in the graph as a function of internuclear distance.

Which of the following correctly identifies the curve corresponding to \(\text{N}_2\) and provides the valid justification?

![A line graph plots potential energy in \(\text{kJ/mol}\) on the vertical axis against internuclear distance in \(\text{pm}\) on the horizontal axis. A horizontal dotted line represents zero potential energy. Two curves, labeled Curve 1 and Curve 2, start at very high positive potential energy at small internuclear distances, decrease sharply to a minimum below zero, and then rise asymptotically toward zero at large distances. Curve 1 is drawn as a solid black line with its minimum at a shorter internuclear distance and a deeper potential energy value. Curve 2 is drawn as a dashed black line with its minimum at a greater internuclear distance and a shallower potential energy value. No gridlines, shading, or additional annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787299914-DAWQ0K.jpg)

- **A.** Curve 2, because the triple bond in \(\text{N}_2\) has a lower bond order than the bond in \(\text{O}_2\), leading to a shallower potential energy minimum.
- **B.** Curve 2, because nitrogen has fewer total electrons than oxygen, resulting in weaker intermolecular forces and a longer equilibrium bond length.
- **C.** Curve 1, because nitrogen has a larger atomic radius than oxygen, which causes a deeper potential energy well and a shorter equilibrium bond distance.
- **D.** Curve 1, because the triple bond in \(\text{N}_2\) has a greater bond energy and a shorter bond length than the double bond in \(\text{O}_2\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119644/*