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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Intermolecular Forces**
**3.38** What types of intermolecular forces are exhibited by each compound?
a. \[ \text{Cyclohexanecarboxylic acid} \]
Structure: A cyclohexane ring with a carboxylic acid group (COOH).
b. \[ \text{Methyl cyclohexanecarboxylate} \]
Structure: A cyclohexane ring with a methoxycarbonyl group (COOCH\(_3\)).
c. \[ \text{Pyridine} \]
Structure: A six-membered ring with five carbon atoms and one nitrogen atom, containing one double bond between each pair of carbon atoms adjacent to the nitrogen.
d. \[ \text{Naphthalene} \]
Structure: Two fused benzene rings with alternating double bonds.
**Explanation of Intermolecular Forces:**
- **Hydrogen Bonding**: Occurs in molecules with N-H, O-H, or F-H bonds. This force can be identified in compound (a) due to the presence of the OH group.
- **Dipole-Dipole Interactions**: Present in polar molecules, where there’s an uneven distribution of electrons. Compounds (a) and (b) may exhibit these interactions due to their polar functional groups.
- **London Dispersion Forces**: Found in all molecules, particularly nonpolar ones. Compounds (c) and (d) would primarily exhibit these forces due to their lack of polar functional groups.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbde2315f-a470-4d06-8b12-e68693b99b71%2Fcea0f4f6-8d0f-4d5c-8a4d-2b5cf7e340a2%2F2pprxyk_processed.png&w=3840&q=75)
Transcribed Image Text:**Intermolecular Forces**
**3.38** What types of intermolecular forces are exhibited by each compound?
a. \[ \text{Cyclohexanecarboxylic acid} \]
Structure: A cyclohexane ring with a carboxylic acid group (COOH).
b. \[ \text{Methyl cyclohexanecarboxylate} \]
Structure: A cyclohexane ring with a methoxycarbonyl group (COOCH\(_3\)).
c. \[ \text{Pyridine} \]
Structure: A six-membered ring with five carbon atoms and one nitrogen atom, containing one double bond between each pair of carbon atoms adjacent to the nitrogen.
d. \[ \text{Naphthalene} \]
Structure: Two fused benzene rings with alternating double bonds.
**Explanation of Intermolecular Forces:**
- **Hydrogen Bonding**: Occurs in molecules with N-H, O-H, or F-H bonds. This force can be identified in compound (a) due to the presence of the OH group.
- **Dipole-Dipole Interactions**: Present in polar molecules, where there’s an uneven distribution of electrons. Compounds (a) and (b) may exhibit these interactions due to their polar functional groups.
- **London Dispersion Forces**: Found in all molecules, particularly nonpolar ones. Compounds (c) and (d) would primarily exhibit these forces due to their lack of polar functional groups.
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