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Which of the two molecules show below would have the higher boiling point? CI H X X H H H A B

Which of the two molecules show below would have the higher boiling point? CI H X X H H H A B

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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Boiling Point Comparison of Molecules #### Question: Which of the two molecules shown below would have the higher boiling point? #### Molecule Structures: - **Molecule A:** - Structure: Cl—C=C—Cl - Other atoms: H bonded to both Carbons - **Molecule B:** - Structure: Cl—C=C—Cl - Other atoms: H bonded to only one Carbon and H bonded to the other, forming a symmetrical structure. #### Choices: 1. A 2. Same boiling point for each 3. B **[Radio buttons for selection]** --- In this exercise, students are asked to determine which of the given molecules (A or B) would have a higher boiling point. By considering intermolecular forces and molecular symmetry, they can deduce that molecule A, having two chlorine atoms bonded to carbon atoms in a symmetrical fashion, is likely to have stronger intermolecular forces due to dipole interactions compared to molecule B. These concepts are crucial for understanding physical properties of compounds in chemistry. --- This problem encourages learners to apply knowledge of molecular structure and intermolecular forces to predict boiling points, a foundational topic in chemistry education.
Transcribed Image Text:### Boiling Point Comparison of Molecules #### Question: Which of the two molecules shown below would have the higher boiling point? #### Molecule Structures: - **Molecule A:** - Structure: Cl—C=C—Cl - Other atoms: H bonded to both Carbons - **Molecule B:** - Structure: Cl—C=C—Cl - Other atoms: H bonded to only one Carbon and H bonded to the other, forming a symmetrical structure. #### Choices: 1. A 2. Same boiling point for each 3. B **[Radio buttons for selection]** --- In this exercise, students are asked to determine which of the given molecules (A or B) would have a higher boiling point. By considering intermolecular forces and molecular symmetry, they can deduce that molecule A, having two chlorine atoms bonded to carbon atoms in a symmetrical fashion, is likely to have stronger intermolecular forces due to dipole interactions compared to molecule B. These concepts are crucial for understanding physical properties of compounds in chemistry. --- This problem encourages learners to apply knowledge of molecular structure and intermolecular forces to predict boiling points, a foundational topic in chemistry education.
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