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Consider the intermolecular forces present in a pure sample of each of the following compounds: CH3OH and CF4. Identify the intermolecular forces that these compounds have in common. A) Dispersion forces, dipole-dipole forces, and hydrogen bonding. B) Dispersion forces only. C) Dispersion forces and dipole- dipole forces. D) Dipole-dipole forces only.

Consider the intermolecular forces present in a pure sample of each of the following compounds: CH3OH and CF4. Identify the intermolecular forces that these compounds have in common. A) Dispersion forces, dipole-dipole forces, and hydrogen bonding. B) Dispersion forces only. C) Dispersion forces and dipole- dipole forces. D) Dipole-dipole forces only.

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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**Understanding Intermolecular Forces in CH3OH and CF4** When studying the properties of different compounds, one important aspect to consider is the type of intermolecular forces present. These forces, which occur between molecules, significantly influence the physical properties of a substance, such as boiling point, melting point, and solubility. In this exercise, we will examine the intermolecular forces in pure samples of methanol (CH₃OH) and carbon tetrafluoride (CF₄), and identify which types of intermolecular forces these two compounds have in common. ### Question: Consider the intermolecular forces present in a pure sample of each of the following compounds: CH₃OH and CF₄. Identify the intermolecular forces that these compounds have in common. A) Dispersion forces, dipole-dipole forces, and hydrogen bonding. B) Dispersion forces only. C) Dispersion forces and dipole-dipole forces. D) Dipole-dipole forces only. ### Explanation: - **Methanol (CH₃OH)**: Methanol is a polar molecule with an O-H bond, which allows for hydrogen bonding. In addition to hydrogen bonding, it also has dipole-dipole interactions due to its polar nature. Lastly, like all molecules, methanol exhibits London dispersion forces. - **Carbon Tetrafluoride (CF₄)**: Carbon tetrafluoride is a nonpolar molecule because of its symmetrical tetrahedral shape, which causes the dipoles to cancel each other out. Therefore, the only intermolecular force present in CF₄ is London dispersion forces. Considering these properties: - Both CH₃OH and CF₄ have dispersion forces. - Only CH₃OH has dipole-dipole forces and hydrogen bonding. Thus, the intermolecular forces these compounds have in common are **dispersion forces only**. ### Correct Answer: B) Dispersion forces only.
Transcribed Image Text:**Understanding Intermolecular Forces in CH3OH and CF4** When studying the properties of different compounds, one important aspect to consider is the type of intermolecular forces present. These forces, which occur between molecules, significantly influence the physical properties of a substance, such as boiling point, melting point, and solubility. In this exercise, we will examine the intermolecular forces in pure samples of methanol (CH₃OH) and carbon tetrafluoride (CF₄), and identify which types of intermolecular forces these two compounds have in common. ### Question: Consider the intermolecular forces present in a pure sample of each of the following compounds: CH₃OH and CF₄. Identify the intermolecular forces that these compounds have in common. A) Dispersion forces, dipole-dipole forces, and hydrogen bonding. B) Dispersion forces only. C) Dispersion forces and dipole-dipole forces. D) Dipole-dipole forces only. ### Explanation: - **Methanol (CH₃OH)**: Methanol is a polar molecule with an O-H bond, which allows for hydrogen bonding. In addition to hydrogen bonding, it also has dipole-dipole interactions due to its polar nature. Lastly, like all molecules, methanol exhibits London dispersion forces. - **Carbon Tetrafluoride (CF₄)**: Carbon tetrafluoride is a nonpolar molecule because of its symmetrical tetrahedral shape, which causes the dipoles to cancel each other out. Therefore, the only intermolecular force present in CF₄ is London dispersion forces. Considering these properties: - Both CH₃OH and CF₄ have dispersion forces. - Only CH₃OH has dipole-dipole forces and hydrogen bonding. Thus, the intermolecular forces these compounds have in common are **dispersion forces only**. ### Correct Answer: B) Dispersion forces only.
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