In a pure sample of HF, what forces of attraction exist between the molecules? A) dispersion forces only B) dipole-dipole interactions only C) Both dispersion forces and dipole-dipole interactions D) dispersion forces, dipole-dipole interactions and hydrogen bonds
In a pure sample of HF, what forces of attraction exist between the molecules? A) dispersion forces only B) dipole-dipole interactions only C) Both dispersion forces and dipole-dipole interactions D) dispersion forces, dipole-dipole interactions and hydrogen bonds
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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
Transcribed Image Text:**Question 22 of 34**
**Topic: Intermolecular Forces in Hydrogen Fluoride (HF)**
**Question:**
In a pure sample of HF, what forces of attraction exist between the molecules?
**Options:**
A) Dispersion forces only
B) Dipole-dipole interactions only
C) Both dispersion forces and dipole-dipole interactions
D) Dispersion forces, dipole-dipole interactions, and hydrogen bonds
**Explanation:**
This question explores the types of intermolecular forces present in hydrogen fluoride (HF). In a pure sample of HF, the molecules exhibit several types of intermolecular attractions:
- **Dispersion Forces:** Also known as London dispersion forces, these are present in all molecules, including nonpolar ones, due to momentary dipoles created by the motion of electrons.
- **Dipole-Dipole Interactions:** These forces occur between polar molecules like HF, where there is a permanent dipole moment due to the electronegativity difference between hydrogen and fluorine.
- **Hydrogen Bonds:** Particularly strong dipole-dipole interactions, hydrogen bonds occur when hydrogen is covalently bonded to a highly electronegative atom (such as fluorine). HF is a classic example of a molecule capable of hydrogen bonding.
**Answer:** D) Dispersion forces, dipole-dipole interactions, and hydrogen bonds.
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