Don't used hand raiting and don't used Ai solution Macmillan LearningIdentify the predominant intermolecular force in each of these substances.Hydrogen bondingH₂ONH3OHCH3CCH3OHCH3COCH3Dipole-dipoleDispersion (London) forcesAnswer BankCH

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Answered: Macmillan Learning Identify the…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter14: Liquids And Solids

Section: Chapter Questions

Problem 23QAP

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8.39 Under what circumstances are ion-dipole forces important?
Silane SiH4, phosphine (PH3), and hydrogen sulfide (H2S) melt at 185 C, 133 C, and 85 C, respectively. What does this suggest about the polar character and intermolecular attractions of the three compounds?
Which of the following compounds would be expected to form intermolecular hydrogen bonds in the liquid state? (a) H2Se (b) HCO2H (formic acid) (c) HI (d) acetone, (CH3)2CO
8.43 Identify the kinds of intermolecular forces (London dispersion, dipoledipole, or hydrogen bonding) that are the most important in each of the following substances. (a) methane (CH4) , (b) methanol (CH4OH) , (c) chloroform (CHCl3) , (d) benzene (C6H6) , (e) ammonia (NH3) , (f) sulfur dioxide (SO2)
The types of intermolecular forces in a substance are identical whether it is a solid, a liquid, or a gas. Why then does a substance change phase from a gas to a liquid or to a solid?
Liquid ethylene glycol, HOCH2CH2OH, is one of the main ingredients in commercial antifreeze. Would you predict its viscosity to be greater or less than that of ethanol, CH3CH2OH?
8.36 Why are dispersion forces attractive?
Identify the kinds of forces that are most important in holding the particles together in a crystalline solid sample of each of the following substances. (a) Kr (b) HF (c) K2O (d) CO2 (e) Zn (f) NH3
Define the following terms and describe how each depends on the strength of the intermolecular forces. a. surface tension b. viscosity c. melting point d. boiling point e. vapor pressure
What are intermolecular forces? How do they differ from intramolecular forces? What are dipole-dipole forces? How do typical dipole-dipole forces differ from hydrogen bonding interactions? In what ways are they similar? What are London dispersion forces? How do typical London dispersion forces differ from dipole-dipole forces? In what ways are they similar? Describe the relationship between molecular size and strength of London dispersion forces. Place the major types of intermolecular forces in order of increasing strength. Is there some overlap? That is, can the strongest London dispersion forces be greater than some dipole-dipole forces? Give an example of such an instance.

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Macmillan Learning Identify the predominant intermolecular force in each of these substances. Hydrogen bonding H₂O NH3 OH CH3CCH3 OH CH3COCH3 Dipole-dipole Dispersion (London) forces Answer Bank CH