---
title: "The potential energy curve for an isolated \\(\\text{HCl}\\) molecule as a function of internuclear distance is shown in the diagram. If a similar curve were plotted for an isolated \\(\\text{HBr}\\) molecule on the same axes, where would the minimum of the \\(\\text{HBr}\\) curve be located relative to the minimum of the \\(\\text{HCl}\\) curve?"
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url: "https://nerd-notes.com/ubq/123538/"
date_modified: "2026-09-28T12:00:04+00:00"
---

# The potential energy curve for an isolated \(\text{HCl}\) molecule as a function of internuclear distance is shown in the diagram. If a similar curve were plotted for an isolated \(\text{HBr}\) molecule on the same axes, where would the minimum of the \(\text{HBr}\) curve be located relative to the minimum of the \(\text{HCl}\) curve?

The potential energy curve for an isolated \(\text{HCl}\) molecule as a function of internuclear distance is shown in the diagram. If a similar curve were plotted for an isolated \(\text{HBr}\) molecule on the same axes, where would the minimum of the \(\text{HBr}\) curve be located relative to the minimum of the \(\text{HCl}\) curve?

![A 2D Cartesian graph with bare axes and no gridlines showing potential energy as a function of internuclear distance for a diatomic molecule. The horizontal x-axis is labeled Internuclear Distance (pm) and extends from zero to the right. The vertical y-axis is labeled Potential Energy (kJ/mol), with positive values above and negative values below a horizontal dashed line at zero potential energy. A single solid black curve represents an isolated HCl molecule. Starting at the top left at high positive potential energy, the curve drops steeply toward the right, reaches a distinct minimum well in the negative region, and then rises smoothly to asymptotically approach the zero potential energy line from below at large distances. The minimum of the curve is labeled HCl minimum. No other curves, data points, or text appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1790596804-6rX1TR.jpg)

- **A.** At a greater internuclear distance and a less negative potential energy, because \(\text{Br}\) has a larger atomic radius and forms a weaker bond with \(\text{H}\).
- **B.** At a greater internuclear distance and a more negative potential energy, because the larger electron cloud of \(\text{Br}\) leads to greater polarizability that strengthens the bond.
- **C.** At a shorter internuclear distance and a less negative potential energy, because the lower electronegativity of \(\text{Br}\) decreases the bond distance while weakening the bond.
- **D.** At a shorter internuclear distance and a more negative potential energy, because the higher nuclear charge of \(\text{Br}\) draws the \(\text{H}\) atom closer and forms a stronger bond.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123538/*