Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 60

Which of the following does not form hydrogen bonds? Justify your choice. (a) Methyl alcohol, \(\mathrm{CH}_{3} \mathrm{OH}\) (b) Hydrofluoric acid, HF (c) Ammonia, \(\mathrm{NH}_{3}\) (d) Methane, \(\mathrm{CH}_{4}\)

Short Answer

Expert verified
Methane (CH4) does not form hydrogen bonds, as its central carbon atom is not highly electronegative, unlike nitrogen, oxygen, and fluorine, which are necessary for hydrogen bonding.

Step by step solution

01

Analyze Methyl Alcohol (CH3OH)

Methyl alcohol, also known as methanol, has a hydroxyl (OH) group in its structure. Oxygen is highly electronegative, and hydrogen is bonded to it. When methanol interacts with another methanol molecule, hydrogen bonding can occur between the oxygen atom of one molecule and the hydrogen atom of the other.
02

Analyze Hydrofluoric Acid (HF)

Hydrofluoric acid (HF) consists of hydrogen bonded to fluorine. Fluorine is the most electronegative element in the periodic table. Therefore, the hydrogen in HF experiences a strong attraction to the fluorine atom in another HF molecule, leading to the formation of hydrogen bonds.
03

Analyze Ammonia (NH3)

The ammonia molecule has a nitrogen atom, which is highly electronegative, bonded to three hydrogen atoms. The hydrogen atoms in one ammonia molecule can form hydrogen bonds with the nitrogen atom in another ammonia molecule.
04

Analyze Methane (CH4)

Methane consists of a carbon atom bonded to four hydrogen atoms. Carbon is not considered a highly electronegative atom, as its electronegativity is lower than nitrogen, oxygen, and fluorine. Consequently, hydrogen bonding does not occur between methane molecules.
05

Conclusion

Methane (CH4) is the molecule among the given options that does not form hydrogen bonds. This is because carbon, the central atom in methane, does not have a high enough electronegativity to form hydrogen bonds between methane molecules.

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

Shown below are the structures for two isomers of hydroxy-benzaldehyde. Structure (a) is 2-hydroxy-benzaldehyde and structure (b) is 4 -hydroxy- benzaldehyde. The melting point for isomer (a), \(2{ }^{\circ} \mathrm{C}\), is significantly lower than the melting point of isomer (b), \(118^{\circ} \mathrm{C}\). Based on your knowledge of intermolecular forces, suggest a substantive reason for this difference in melting points. (Hint: Consider the intermolecular forces that must be overcome to melt each compound and postulate a reason for the difference in the strengths of those forces).

Based on the strength of their molecular dipole moments, which compound should have the higher boiling point, HF or HBr? Explain.

What is so special about hydrogen atoms that makes hydrogen bonding possible?

Explain what gives rise to London forces and when they occur.

Draw some molecules of ammonia, \(\mathrm{NH}_{3}\), and use dotted lines to show the hydrogen bonding between them.
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Chemistry Branches

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

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