---
title: "A student analyzes the molecular structures of the chlorine oxoacids: \\(\\text{HClO}\\), \\(\\text{HClO}_2\\), \\(\\text{HClO}_3\\), and \\(\\text{HClO}_4\\). Which of the following correctly ranks the oxoacids in order of decreasing acid strength and provides the correct justification?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/119733/"
date_modified: "2026-08-21T08:12:10+00:00"
---

# A student analyzes the molecular structures of the chlorine oxoacids: \(\text{HClO}\), \(\text{HClO}_2\), \(\text{HClO}_3\), and \(\text{HClO}_4\). Which of the following correctly ranks the oxoacids in order of decreasing acid strength and provides the correct justification?

A student analyzes the molecular structures of the chlorine oxoacids: \(\text{HClO}\), \(\text{HClO}_2\), \(\text{HClO}_3\), and \(\text{HClO}_4\). Which of the following correctly ranks the oxoacids in order of decreasing acid strength and provides the correct justification?

- **A.** \(\text{HClO} > \text{HClO}_2 > \text{HClO}_3 > \text{HClO}_4\), because having fewer oxygen atoms bonded to the chlorine atom minimizes steric hindrance around the proton, allowing it to dissociate more readily.
- **B.** \(\text{HClO} > \text{HClO}_2 > \text{HClO}_3 > \text{HClO}_4\), because the lower oxidation state of the chlorine atom increases the polarity of the \(\text{O-H}\) bond, facilitating proton transfer.
- **C.** \(\text{HClO}_4 > \text{HClO}_3 > \text{HClO}_2 > \text{HClO}\), because the additional oxygen atoms increase the molar mass and London dispersion forces, which strengthens interactions with water to remove the proton.
- **D.** \(\text{HClO}_4 > \text{HClO}_3 > \text{HClO}_2 > \text{HClO}\), because the increasing number of electronegative oxygen atoms draws electron density away from the \(\text{O-H}\) bond, weakening the bond and stabilizing the conjugate base.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119733/*