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3. Circle all of the following molecules that would be considered highly water soluble O → Na o *H₂N. Na OH

3. Circle all of the following molecules that would be considered highly water soluble O → Na o *H₂N. Na OH

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
Section: Chapter Questions
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**Title: Understanding Water Solubility of Molecules** **Question: Circle all of the following molecules that would be considered highly water soluble.** In the given image, there are six different molecular structures. The task is to determine which of these molecules are highly water soluble and circle them. Here is a description of each molecule from left to right: 1. **Structure 1:** A molecule with an ammonium ion (\[H3N]+) attached to a carbon chain. 2. **Structure 2:** A pentane ring, also known as cyclopentane. 3. **Structure 3:** A sulfonate ion with the sodium counterions (Na+). 4. **Structure 4:** A carbon chain attached to a carbonyl group (a carbon double-bonded to oxygen). 5. **Structure 5:** A carbon chain with a hydroxyl group (OH) at the end. **Explanation:** - Molecules that are polar or ionic are more likely to be water soluble because water is a polar solvent. - Presence of functional groups like hydroxyl (OH), ammonium ions (\[H3N]+), and sulfonate groups increases solubility due to their ability to form hydrogen bonds or ionic interactions with water molecules. **Molecules With Higher Water Solubility:** - The first structure with the ammonium ion (\[H3N]+) should be water soluble due to its ionic nature. - The third structure, sodium sulfonate (NaO3S\), is highly water soluble due to its ionic nature. - The last structure containing a hydroxyl group (OH) at the end of a carbon chain is also likely to be water soluble because of the polar hydroxyl group. **Molecules With Lower Water Solubility:** - The second structure (cyclopentane) is non-polar and would be relatively insoluble in water. - The fourth structure (carbon chain with a carbonyl group) is somewhat polar but less so compared to the other structures with ionic or hydroxyl groups. By understanding the molecular structure and the presence of specific functional groups, we can predict the water solubility of these molecules.
Transcribed Image Text:**Title: Understanding Water Solubility of Molecules** **Question: Circle all of the following molecules that would be considered highly water soluble.** In the given image, there are six different molecular structures. The task is to determine which of these molecules are highly water soluble and circle them. Here is a description of each molecule from left to right: 1. **Structure 1:** A molecule with an ammonium ion (\[H3N]+) attached to a carbon chain. 2. **Structure 2:** A pentane ring, also known as cyclopentane. 3. **Structure 3:** A sulfonate ion with the sodium counterions (Na+). 4. **Structure 4:** A carbon chain attached to a carbonyl group (a carbon double-bonded to oxygen). 5. **Structure 5:** A carbon chain with a hydroxyl group (OH) at the end. **Explanation:** - Molecules that are polar or ionic are more likely to be water soluble because water is a polar solvent. - Presence of functional groups like hydroxyl (OH), ammonium ions (\[H3N]+), and sulfonate groups increases solubility due to their ability to form hydrogen bonds or ionic interactions with water molecules. **Molecules With Higher Water Solubility:** - The first structure with the ammonium ion (\[H3N]+) should be water soluble due to its ionic nature. - The third structure, sodium sulfonate (NaO3S\), is highly water soluble due to its ionic nature. - The last structure containing a hydroxyl group (OH) at the end of a carbon chain is also likely to be water soluble because of the polar hydroxyl group. **Molecules With Lower Water Solubility:** - The second structure (cyclopentane) is non-polar and would be relatively insoluble in water. - The fourth structure (carbon chain with a carbonyl group) is somewhat polar but less so compared to the other structures with ionic or hydroxyl groups. By understanding the molecular structure and the presence of specific functional groups, we can predict the water solubility of these molecules.
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