Which intermolecular forces are present in a pure sample of the compound below? O dipole-dipole and hydrogen bonding O London-dispersion forces only O hydrogen-bonding, dipole-dipole, and London-dispersion O dipole-dipole and London-dispersion forces
Which intermolecular forces are present in a pure sample of the compound below? O dipole-dipole and hydrogen bonding O London-dispersion forces only O hydrogen-bonding, dipole-dipole, and London-dispersion O dipole-dipole and London-dispersion forces
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter10: Liquids And Solids
Section: Chapter Questions
Problem 1RQ: What are intermolecular forces? How do they differ from intramolecular forces? What are...
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![### Question 7
**Which intermolecular forces are present in a pure sample of the compound below?**
![Molecular Structure](data:image/png;base64,iVBORw0KGgoAAAANSUhEUgAAAAUA...kSuQmCC)
1. Dipole-dipole and hydrogen bonding
2. London-dispersion forces only
3. Hydrogen-bonding, dipole-dipole, and London-dispersion
4. Dipole-dipole and London-dispersion forces
**Explanation:**
The diagram shows the molecular structure of a compound with a carbon (C) atom and a fluorine (F) atom. The fluorine atom is electronegative and creates a polar bond with carbon, resulting in dipole-dipole interactions. There are no hydrogen atoms bonded to highly electronegative atoms (O, N, or F), so hydrogen bonding is not present. Both dipole-dipole and London-dispersion forces are applicable.
**Correct Answer:** Dipole-dipole and London-dispersion forces](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F277ae00b-d056-42ed-a729-386f4fca5973%2Fd9ca44e9-9a0a-4769-b98d-8e1bbb2750b4%2F2mbj83d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Question 7
**Which intermolecular forces are present in a pure sample of the compound below?**
![Molecular Structure](data:image/png;base64,iVBORw0KGgoAAAANSUhEUgAAAAUA...kSuQmCC)
1. Dipole-dipole and hydrogen bonding
2. London-dispersion forces only
3. Hydrogen-bonding, dipole-dipole, and London-dispersion
4. Dipole-dipole and London-dispersion forces
**Explanation:**
The diagram shows the molecular structure of a compound with a carbon (C) atom and a fluorine (F) atom. The fluorine atom is electronegative and creates a polar bond with carbon, resulting in dipole-dipole interactions. There are no hydrogen atoms bonded to highly electronegative atoms (O, N, or F), so hydrogen bonding is not present. Both dipole-dipole and London-dispersion forces are applicable.
**Correct Answer:** Dipole-dipole and London-dispersion forces
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