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Hexane has stronger IMF's than cyclohexane since it has more hydrogen atoms to hydrogen bond with. Hexane has stronger IMF's than cyclohexane due to its higher molar mass. Cyclohexane has stronger IMF's than hexane due to its shape. The IMF's are the same strength since they both have weak dispersion forces.

Hexane has stronger IMF's than cyclohexane since it has more hydrogen atoms to hydrogen bond with. Hexane has stronger IMF's than cyclohexane due to its higher molar mass. Cyclohexane has stronger IMF's than hexane due to its shape. The IMF's are the same strength since they both have weak dispersion forces.

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Intermolecular Forces in Cyclohexane and Hexane** When comparing intermolecular forces (IMFs) of cyclohexane and hexane, it's important to consider their molecular structures and the forces at play. **Molecular Representations:** - **Cyclohexane**: Shown as a hexagonal ring in three representations, illustrating its cyclic structure with single bonds connecting the carbon atoms, each bonded to two hydrogen atoms. - **Hexane**: Displayed as a straight chain with six carbon atoms, each bonded to enough hydrogen atoms to satisfy the tetravalency of carbon. **Statements to Evaluate:** 1. **Hexane has stronger IMFs than cyclohexane since it has more hydrogen atoms to hydrogen bond with.** 2. **Hexane has stronger IMFs than cyclohexane due to its higher molar mass.** 3. **Cyclohexane has stronger IMFs than hexane due to its shape.** 4. **The IMFs are the same strength since they both have weak dispersion forces.** **Evaluation and Explanation:** - **Correct Statement**: Both molecules are nonpolar, and primarily exhibit London dispersion forces. Since dispersion forces increase with molar mass and surface contact, hexane's linear structure provides greater surface area contact in liquid state than cyclohexane's cyclic structure, potentially making its dispersion forces slightly stronger. It's incorrect to consider hydrogen bonding as neither compound has hydrogen atoms bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine needed for hydrogen bonds. Understanding the properties of these compounds involves not just looking at their chemical formulae but appreciating their structural differences and how these influence their physical interactions in a given state.
Transcribed Image Text:**Intermolecular Forces in Cyclohexane and Hexane** When comparing intermolecular forces (IMFs) of cyclohexane and hexane, it's important to consider their molecular structures and the forces at play. **Molecular Representations:** - **Cyclohexane**: Shown as a hexagonal ring in three representations, illustrating its cyclic structure with single bonds connecting the carbon atoms, each bonded to two hydrogen atoms. - **Hexane**: Displayed as a straight chain with six carbon atoms, each bonded to enough hydrogen atoms to satisfy the tetravalency of carbon. **Statements to Evaluate:** 1. **Hexane has stronger IMFs than cyclohexane since it has more hydrogen atoms to hydrogen bond with.** 2. **Hexane has stronger IMFs than cyclohexane due to its higher molar mass.** 3. **Cyclohexane has stronger IMFs than hexane due to its shape.** 4. **The IMFs are the same strength since they both have weak dispersion forces.** **Evaluation and Explanation:** - **Correct Statement**: Both molecules are nonpolar, and primarily exhibit London dispersion forces. Since dispersion forces increase with molar mass and surface contact, hexane's linear structure provides greater surface area contact in liquid state than cyclohexane's cyclic structure, potentially making its dispersion forces slightly stronger. It's incorrect to consider hydrogen bonding as neither compound has hydrogen atoms bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine needed for hydrogen bonds. Understanding the properties of these compounds involves not just looking at their chemical formulae but appreciating their structural differences and how these influence their physical interactions in a given state.
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