A Hydrogen bonding between acetone molecules is stronger than the hydrogen bonding between ethylene glycol molecules. Hydrogen bonding between ethylene glycol molecules is stronger than the dipole-dipole interactions between acetone molecules. London dispersion forces between acetone molecules are stronger than the London dispersion forces between ethylene glycol molecules. London dispersion forces between ethylene glycol molecules are stronger than the dipole-dipole interactions between acetone molecules. 쁘 Sav

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Enema nuclear forces determine many physical properties for organic chemicals. What is the reason ethylene glycol  has a much higher boiling main point than acetone?
A
Hydrogen bonding between acetone molecules is stronger than the hydrogen bonding between ethylene glycol molecules.
Hydrogen bonding between ethylene glycol molecules is stronger than the dipole-dipole interactions between acetone molecules.
C
London dispersion forces between acetone molecules are stronger than the London dispersion forces between ethylene glycol molecules.
London dispersion forces between ethylene glycol molecules are stronger than the dipole-dipole interactions between acetone molecules.
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Transcribed Image Text:A Hydrogen bonding between acetone molecules is stronger than the hydrogen bonding between ethylene glycol molecules. Hydrogen bonding between ethylene glycol molecules is stronger than the dipole-dipole interactions between acetone molecules. C London dispersion forces between acetone molecules are stronger than the London dispersion forces between ethylene glycol molecules. London dispersion forces between ethylene glycol molecules are stronger than the dipole-dipole interactions between acetone molecules. Save
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