Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter20: Organic Chemistry
Section: Chapter Questions
Problem 4QAP: How many electron pairs are shared when a triple bond exists between two carbon atoms? What must he...
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![### Question 10 of 20
#### Determine the type of alcohol the molecule shown here.
**Diagram:**
The diagram depicts a chemical structure of an alcohol molecule. The molecule consists of a carbon chain where the second carbon atom is attached to a hydroxyl group (-OH). The structure can be described as follows:
- The first carbon is bonded to two hydrogen atoms and one methyl group (-CH3).
- The second carbon, which is attached to the hydroxyl group (-OH), is also bonded to one hydrogen atom and one other carbon atom.
- The third and fourth carbons each are bonded to three hydrogen atoms.
**Options:**
A) primary
B) secondary
C) tertiary
D) quaternary
**Detailed Description:**
- **Primary alcohols** have the hydroxyl group (-OH) connected to a carbon atom that is attached to only one other carbon.
- **Secondary alcohols** have the hydroxyl group (-OH) attached to a carbon atom that is connected to two other carbon atoms.
- **Tertiary alcohols** have the hydroxyl group (-OH) attached to a carbon atom that is connected to three other carbon atoms.
- **Quaternary alcohols** do not exist, as a quaternary carbon cannot have a hydroxyl group due to having four carbon bonds.
The molecule shown in the diagram has the hydroxyl group (-OH) connected to a secondary carbon atom, which is bonded to two other carbon atoms. Therefore, the molecule is a **secondary alcohol**.
**Correct Answer: B) secondary**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5707f817-26ef-49f8-a626-ee896014d672%2F88d58e3e-0d0e-4c46-b1d8-605bf1d23e48%2Fh8fuy1t_processed.png&w=3840&q=75)
Transcribed Image Text:### Question 10 of 20
#### Determine the type of alcohol the molecule shown here.
**Diagram:**
The diagram depicts a chemical structure of an alcohol molecule. The molecule consists of a carbon chain where the second carbon atom is attached to a hydroxyl group (-OH). The structure can be described as follows:
- The first carbon is bonded to two hydrogen atoms and one methyl group (-CH3).
- The second carbon, which is attached to the hydroxyl group (-OH), is also bonded to one hydrogen atom and one other carbon atom.
- The third and fourth carbons each are bonded to three hydrogen atoms.
**Options:**
A) primary
B) secondary
C) tertiary
D) quaternary
**Detailed Description:**
- **Primary alcohols** have the hydroxyl group (-OH) connected to a carbon atom that is attached to only one other carbon.
- **Secondary alcohols** have the hydroxyl group (-OH) attached to a carbon atom that is connected to two other carbon atoms.
- **Tertiary alcohols** have the hydroxyl group (-OH) attached to a carbon atom that is connected to three other carbon atoms.
- **Quaternary alcohols** do not exist, as a quaternary carbon cannot have a hydroxyl group due to having four carbon bonds.
The molecule shown in the diagram has the hydroxyl group (-OH) connected to a secondary carbon atom, which is bonded to two other carbon atoms. Therefore, the molecule is a **secondary alcohol**.
**Correct Answer: B) secondary**
![### Question 11 of 20
**Compare the following two isomers. Which is more soluble in water? Why?**
#### Diagram of Isomers:
- **Compound 1:** Structural formula is a chain of four carbons (butane) with an -OH (hydroxyl) group attached to the fourth carbon.
- **Compound 2:** Structural formula is a chain of four carbons (butane) with an oxygen atom linking the second and third carbons, forming an ether.
#### Answer Choices:
- **A) Compound 1 is more soluble because it has greater ability to hydrogen bond with water.**
- **B) Compound 2 is more soluble because it has greater ability to hydrogen bond with water.**
- **C) Neither of these compounds are water soluble.**
- **D) Compound 1 is more soluble because it will have more dipole-dipole interactions with water.**
- **E) Compound 2 is more soluble because it will have more dipole-dipole interactions with water.**
### Explanation:
The exercise at hand requires evaluating the solubility of two isomers in water. Both compounds have the same molecular formula but different functional groups, resulting in distinct chemical properties.
**Compound 1** has a hydroxyl group (-OH), which is known for its strong ability to form hydrogen bonds with water molecules. This significantly enhances its solubility in water.
**Compound 2** features an ether functional group (C-O-C). While ethers do interact with water through dipole-dipole interactions, they are generally less effective at forming hydrogen bonds compared to hydroxyl groups.
Considering the capacity of hydrogen bonding as a significant factor in determining water solubility, **Compound 1** is expected to be more soluble in water than **Compound 2**.
### Conclusion:
The correct answer is:
- **A) Compound 1 is more soluble because it has greater ability to hydrogen bond with water.**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5707f817-26ef-49f8-a626-ee896014d672%2F88d58e3e-0d0e-4c46-b1d8-605bf1d23e48%2Fe89av1_processed.png&w=3840&q=75)
Transcribed Image Text:### Question 11 of 20
**Compare the following two isomers. Which is more soluble in water? Why?**
#### Diagram of Isomers:
- **Compound 1:** Structural formula is a chain of four carbons (butane) with an -OH (hydroxyl) group attached to the fourth carbon.
- **Compound 2:** Structural formula is a chain of four carbons (butane) with an oxygen atom linking the second and third carbons, forming an ether.
#### Answer Choices:
- **A) Compound 1 is more soluble because it has greater ability to hydrogen bond with water.**
- **B) Compound 2 is more soluble because it has greater ability to hydrogen bond with water.**
- **C) Neither of these compounds are water soluble.**
- **D) Compound 1 is more soluble because it will have more dipole-dipole interactions with water.**
- **E) Compound 2 is more soluble because it will have more dipole-dipole interactions with water.**
### Explanation:
The exercise at hand requires evaluating the solubility of two isomers in water. Both compounds have the same molecular formula but different functional groups, resulting in distinct chemical properties.
**Compound 1** has a hydroxyl group (-OH), which is known for its strong ability to form hydrogen bonds with water molecules. This significantly enhances its solubility in water.
**Compound 2** features an ether functional group (C-O-C). While ethers do interact with water through dipole-dipole interactions, they are generally less effective at forming hydrogen bonds compared to hydroxyl groups.
Considering the capacity of hydrogen bonding as a significant factor in determining water solubility, **Compound 1** is expected to be more soluble in water than **Compound 2**.
### Conclusion:
The correct answer is:
- **A) Compound 1 is more soluble because it has greater ability to hydrogen bond with water.**
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