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Based only on intermolecular forces, which of the following would be the least soluble in CH3CH(OH)CH3? A) CH3OCH3 B) CH3CH₂CH3 C) H₂O D) CH3CH2CH₂OH

Based only on intermolecular forces, which of the following would be the least soluble in CH3CH(OH)CH3? A) CH3OCH3 B) CH3CH₂CH3 C) H₂O D) CH3CH2CH₂OH

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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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**Question:** Based only on intermolecular forces, which of the following would be the least soluble in CH₃CH(OH)CH₃? **Options:** A) CH₃OCH₃ B) CH₃CH₂CH₃ C) H₂O D) CH₃CH₂CH₂OH --- **Explanation:** This question is asking about solubility based on intermolecular forces such as hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Understanding these forces is crucial in determining the solubility properties of different compounds. - **CH₃OCH₃ (Dimethyl Ether):** This molecule has an ether functional group, which means it can engage in dipole-dipole interactions, but it cannot form hydrogen bonds with itself. - **CH₃CH₂CH₃ (Propane):** This molecule is nonpolar and only experiences London dispersion forces, the weakest of the intermolecular forces. - **H₂O (Water):** This molecule is highly polar and can form hydrogen bonds with itself and with other molecules that have hydrogen-bonding capability. - **CH₃CH₂CH₂OH (Propanol):** This molecule contains an alcohol functional group, allowing it to form hydrogen bonds, making it quite soluble in other hydrogen-bonding solvents. Based on intermolecular forces, CH₃CH₂CH₃ (Propane) would be the least soluble in isopropanol (CH₃CH(OH)CH₃), primarily due to its inability to participate in strong intermolecular interactions such as hydrogen bonding or dipole-dipole interactions as effectively as the other molecules listed.
Transcribed Image Text:**Question:** Based only on intermolecular forces, which of the following would be the least soluble in CH₃CH(OH)CH₃? **Options:** A) CH₃OCH₃ B) CH₃CH₂CH₃ C) H₂O D) CH₃CH₂CH₂OH --- **Explanation:** This question is asking about solubility based on intermolecular forces such as hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Understanding these forces is crucial in determining the solubility properties of different compounds. - **CH₃OCH₃ (Dimethyl Ether):** This molecule has an ether functional group, which means it can engage in dipole-dipole interactions, but it cannot form hydrogen bonds with itself. - **CH₃CH₂CH₃ (Propane):** This molecule is nonpolar and only experiences London dispersion forces, the weakest of the intermolecular forces. - **H₂O (Water):** This molecule is highly polar and can form hydrogen bonds with itself and with other molecules that have hydrogen-bonding capability. - **CH₃CH₂CH₂OH (Propanol):** This molecule contains an alcohol functional group, allowing it to form hydrogen bonds, making it quite soluble in other hydrogen-bonding solvents. Based on intermolecular forces, CH₃CH₂CH₃ (Propane) would be the least soluble in isopropanol (CH₃CH(OH)CH₃), primarily due to its inability to participate in strong intermolecular interactions such as hydrogen bonding or dipole-dipole interactions as effectively as the other molecules listed.
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