/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 25 (a) What atoms must a molecule c... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 11: Problem 25

(a) What atoms must a molecule contain to participate in hydrogen bonding with other molecules of the same kind? (b) Which of the following molecules can form hydrogen bonds with other molecules of the same kind: \(\mathrm{CH}_{3} \mathrm{~F}, \mathrm{CH}_{3} \mathrm{NH}_{2}, \mathrm{CH}_{3} \mathrm{OH}, \mathrm{CH}_{3} \mathrm{Br} ?\)

Short Answer

Expert verified
A molecule must have a hydrogen atom bonded to nitrogen (N), oxygen (O), or fluorine (F) to participate in hydrogen bonding with other molecules of the same kind. Out of the given molecules, \(\mathrm{CH}_{3}\mathrm{NH}_{2}\) and \(\mathrm{CH}_{3}\mathrm{OH}\) can form hydrogen bonds with other molecules of the same kind, while \(\mathrm{CH}_{3}\mathrm{F}\) and \(\mathrm{CH}_{3}\mathrm{Br}\) cannot.

Step by step solution

01

Identify conditions for hydrogen bonding

To participate in hydrogen bonding, a molecule must have a hydrogen atom bonded to a highly electronegative element, usually nitrogen (N), oxygen (O), or fluorine (F). This creates a highly polar bond, enabling the positive hydrogen end to attract the negative end of another molecule containing N, O, or F.
02

Examine each molecule

Now, let's examine each of the given molecules and determine if they can form hydrogen bonds with other molecules of the same kind. 1. \(\mathrm{CH}_{3}\mathrm{F}\): This molecule has a hydrogen atom, but it is not bonded to the highly electronegative fluorine (F) atom. The hydrogen atoms are bonded to carbon (C), which is less electronegative. Therefore, this molecule cannot form hydrogen bonds with other molecules of the same kind. 2. \(\mathrm{CH}_{3}\mathrm{NH}_{2}\): Here, the hydrogen atoms are bonded to a highly electronegative nitrogen (N) atom. As a result, this molecule can participate in hydrogen bonding with other molecules of the same kind. 3. \(\mathrm{CH}_{3}\mathrm{OH}\): In this case, the hydrogen atom is bonded to a highly electronegative oxygen (O) atom, allowing this molecule to form hydrogen bonds with other molecules of the same kind. 4. \(\mathrm{CH}_{3}\mathrm{Br}\): This molecule has a hydrogen atom, but it is not bonded to a highly electronegative atom. The hydrogen atoms are bonded to carbon (C), and bromine (Br) is less electronegative than N, O, or F. Therefore, this molecule cannot form hydrogen bonds with other molecules of the same kind.
03

Conclusion

In summary, a molecule must have a hydrogen atom bonded to nitrogen (N), oxygen (O), or fluorine (F) to participate in hydrogen bonding with other molecules of the same kind. Out of the given molecules, \(\mathrm{CH}_{3}\mathrm{NH}_{2}\) and \(\mathrm{CH}_{3}\mathrm{OH}\) can form hydrogen bonds with other molecules of the same kind, while \(\mathrm{CH}_{3}\mathrm{F}\) and \(\mathrm{CH}_{3}\mathrm{Br}\) cannot.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electronegativity
Electronegativity is a fundamental concept in chemistry that refers to the ability of an atom to attract electrons towards itself in a chemical bond. This property can vary significantly across different elements. Generally, electronegativity increases across a period from left to right in the periodic table and decreases down a group.

When it comes to hydrogen bonding, the key elements involved are nitrogen (N), oxygen (O), and fluorine (F). These atoms are highly electronegative:
  • Fluorine is the most electronegative element, which makes it a strong hydrogen bond acceptor.
  • Oxygen comes next, known for its strong electron-pulling capabilities, often found in water molecules.
  • Nitrogen, while slightly less electronegative than oxygen, still readily participates in hydrogen bonds.
Understanding electronegativity helps us predict the behavior of molecules and their ability to form hydrogen bonds, particularly by assessing which atoms in a molecule might "pull" electrons and create polar bonds.
Hydrogen Bond Donor
A hydrogen bond donor is an atom within a molecule that provides the hydrogen atom needed for hydrogen bonding. For this to occur, the hydrogen must be bonded to an electronegative atom, creating a scenario where the hydrogen has a partial positive charge.

In the context of hydrogen bonding, typical hydrogen bond donors include:
  • Nitrogen (as in amines like CH3NH2)
  • Oxygen (such as in alcohols like CH3OH)
These atoms not only contribute to high polarity in the bond with hydrogen but also make the hydrogen available to interact with an electronegative atom from another molecule, thereby forming a strong intermolecular attraction known as a hydrogen bond. Without such donors, molecules cannot effectively participate in hydrogen bonding, as seen in less electronegative pairings like hydrogen bonded to carbon.
Intermolecular Forces
Intermolecular forces are forces of attraction or repulsion between neighboring particles (molecules, atoms, or ions). These forces are crucial in determining the physical properties of substances such as boiling points and solubility.

Hydrogen bonds are a specific type of intermolecular force. They are particularly strong dipole-dipole attractions that occur when a hydrogen atom bonded to a highly electronegative atom (like N, O, or F) attracts an electronegative atom on a neighboring molecule. This allows molecules to cling to each other more tightly:
  • Hydrogen bonds give water its unique properties, such as a high boiling point.
  • Such bonds also make hydrogen bonding participants, like CH3OH and CH3NH2, have higher boiling points compared to non-hydrogen bonding molecules.
Overall, understanding these interactions helps explain why some liquids, like water and alcohols, remain liquid at room temperature, while others, like methane, do not.

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

(a) Which is generally stronger, intermolecular interactions or intramolecular interactions? (b) Which of these kinds of interactions are broken when a liquid is converted to a gas?

You are high up in the mountains and boil water to make some tea. However, when you drink your tea, it is not as hot as it should be. You try again and again, but the water is just not hot enough to make a hot cup of tea. Which is the best explanation for this result? (a) High in the mountains, it is probably very dry, and so the water is rapidly evaporating from your cup and cooling it. (b) High in the mountains, it is probably very windy, and so the water is rapidly evaporating from your cup and cooling it. (c) High in the mountains, the air pressure is significantly less than \(101.3 \mathrm{kPa}\), so the boiling point of water is much lower than at sea level. (d) High in the mountains, the air pressure is significantly less than \(101.3 \mathrm{kPa}\), so the boiling point of water is much higher than at sea level.

Rubbing alcohol is the common name for 2 -propanol (isopropanol), \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}\). (a) Draw the three-dimensional structure of the 2 -propanol molecule and predict the geometry around each carbon atom. (b) Is the 2 -propanol molecule polar or nonpolar? (c) What kinds of intermolecular attractive forces exist between the 2 -propanol molecules? (d) The isomer 1-propanol has the same molecular weight as 2 -propanol, yet 2 -propanol boils at \(82.6^{\circ} \mathrm{C}\) and 1 -propanol boils at \(97.2^{\circ} \mathrm{C}\). Explain the difference.

As a metal such as lead melts, what happens to (a) the average kinetic energy of the atoms and (b) the average distance between the atoms?

(a) Which type of intermolecular attractive force operates between all molecules? (b) Which type of intermolecular attractive force operates only between polar molecules? (c) Which type of intermolecular attractive force operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

Kinetics

Read Explanation

Organic Chemistry

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.