Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Problem 47

Hydrogen peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) is a syrupy liquid with a relatively low vapor pressure and a normal boiling point of \(152.2^{\circ} \mathrm{C}\) . Rationalize the differences of these physical properties from those of water.

Short Answer

Expert verified
The differences in physical properties, such as boiling point and vapor pressure, between hydrogen peroxide (H2O2) and water (H2O) are a result of their different molecular structures and the presence or absence of strong intermolecular forces like hydrogen bonding. Water has stronger hydrogen bonds than hydrogen peroxide due to its overall dipole moment and more electronegative oxygen atoms, leading to a higher boiling point (\(100^{\circ} \mathrm{C}\)) and a lower vapor pressure. In contrast, the reduced dipole moment and weaker hydrogen bonding in hydrogen peroxide yield a lower boiling point (\(152.2^{\circ} \mathrm{C}\)) and higher vapor pressure.

Step by step solution

01

Understanding the chemical structures of H2O and H2O2

First, we need to understand the chemical structures of both compounds. Water, or H2O, is a simple molecule consisting of a single oxygen atom bonded to two hydrogen atoms. Hydrogen peroxide, or H2O2, is a larger molecule consisting of two oxygen atoms and two hydrogen atoms with a single bond connecting the two oxygen atoms. Although these molecules share similar elements, the arrangements and the types of bonds connecting the atoms are different.
02

Analyzing intermolecular forces in H2O

In water, the oxygen atom is more electronegative than the hydrogen atoms, leading to a polar covalent bond between oxygen and hydrogen atoms. This difference in electronegativity creates a dipole moment in the molecule, making water a polar molecule. Consequently,water molecules are attracted to each other through hydrogen bonding, which is a strong type of intermolecular force specifically between hydrogen atoms and highly electronegative atoms like oxygen.
03

Analyzing intermolecular forces in H2O2

Hydrogen peroxide also possesses polar covalent bonds between the oxygen and hydrogen atoms. However, the oxygen-oxygen single bond reduces the overall dipole moment of the H2O2 molecule. Consequently, hydrogen peroxide does not exhibit a strong dipole moment like water, and its capability to form hydrogen bonds is less than that of water.
04

Comparing boiling points

The boiling point of a substance is related to the strength of its intermolecular forces. Since hydrogen bonding is significantly stronger in water than in hydrogen peroxide, water molecules require more energy to break away from each other than the H2O2 molecules. This leads to water having a higher boiling point (\(100^{\circ} \mathrm{C}\)) than hydrogen peroxide (\(152.2^{\circ} \mathrm{C}\)).
05

Comparing vapor pressures

Vapor pressure is a measure of the tendency of a substance to evaporate. Substances with stronger intermolecular forces have lower vapor pressures because more energy is required to break the intermolecular forces holding the molecules together. Since water has stronger hydrogen bonds than hydrogen peroxide, water has a lower vapor pressure compared to H2O2.
06

Conclusion:

The differences in physical properties such as boiling point and vapor pressure between hydrogen peroxide and water are a result of the different molecular structures and the presence or absence of strong intermolecular forces like hydrogen bonding. Since hydrogen bonds are stronger in water than in hydrogen peroxide, water exhibits a higher boiling point and a lower vapor pressure than hydrogen peroxide.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

What type of solid will each of the following substances form? a. diamond b. \(\mathrm{PH}_{3}\) c. \(\mathrm{H}_{2}\) d. \(\mathrm{Mg}\) e. \(\mathrm{KCl}\) f. quartz g. \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) h. \(\mathrm{SF}_{2}\) i. Ar j. \(\mathrm{Cu}\) k. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

X rays from a copper \(\mathrm{X}\) -ray tube \((\lambda=154 \mathrm{pm})\) were diffracted at an angle of 14.22 degrees by a crystal of silicon. Assuming first-order diffraction \((n=1 \text { in the Bragg equation), what is }\) the interplanar spacing in silicon?

Consider the following melting point data: Account for the trends in melting points in terms of interparticle forces

The conductivity of silicon is enhanced by doping. What is doping?

You and a friend each synthesize a compound with the formula \(\mathrm{XeCl}_{2} \mathrm{F}_{2} .\) Your compound is a liquid and your friend's compound is a gas (at the same conditions of temperature and pressure). Explain how the two compounds with the same formulas can exist in different phases at the same conditions of pressure and temperature.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free