Octane (CH,3) is a straight chain of carbon atoms with no dipole moment and a boiling point of 125°C. Water has a dipole moment, has hydrogen bonds and has a boiling point of 100°C. The difference between these two boiling points can best be rationalized by: A. Intermolecular forces between molecules with dipole moments are greater than between molecules with no dipole moment B. Hydrogen bonding is a strong intermolecular force C. London dispersion forces are weak but there are many LDFS in octane so the net IMF in CH18 is greater than the net IMF in H,0 D. London dispersion forces are strong and so the boiling point of octane is greater than the boiling point of water E. There is no trend, this is a magical mystery of science

Octane (CH,3) is a straight chain of carbon atoms with no dipole moment and a boiling point of 125°C. Water has a dipole moment, has hydrogen bonds and has a boiling point of 100°C. The difference between these two boiling points can best be rationalized by: A. Intermolecular forces between molecules with dipole moments are greater than between molecules with no dipole moment B. Hydrogen bonding is a strong intermolecular force C. London dispersion forces are weak but there are many LDFS in octane so the net IMF in CH18 is greater than the net IMF in H,0 D. London dispersion forces are strong and so the boiling point of octane is greater than the boiling point of water E. There is no trend, this is a magical mystery of science

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

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 1RQ: What are intermolecular forces? How do they differ from intramolecular forces? What are...

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