Pls help asap on all asked questions. pls show all work and steps. 7. Which of the following is not an example of an intermolecular force?a. dipole-dipole interactionsb. London dispersion forcesc. hydrogen bondingd. sigma bonding8. What experimental evidence led J.J. Thomson to the development of the Raisin bun model?a. The discovery of the atomic nucleusb. The discovery of the electronc. The discovery of the neutrond. All of the above

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Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter8: Molecules And Materials

Section: Chapter Questions

Problem 8.92PAE

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8.45 Describe how interactions between molecules affect the vapor pressure of a liquid.
Why do liquids have a vapor pressure? Do all liquids have vapor pressures? Explain. Do solids exhibit vapor pressure? Explain. How does vapor pressure change with changing temperature? Explain.
8.41 What is the specific feature of N, O, and F that causes them to play a role in hydrogen bonding?
An amorphous solid can sometimes be converted to a crystalline solid by a process called annealing. Annealing consists of heating the substance to a temperature just below the melting point of the crystalline form and then cooling it slowly. Explain why this process helps produce a crystalline solid.
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.
What types of liquids typically form amorphous solids?
8.81 Carbon tetrachloride (CCl4) is a liquid at room temperature and pressure, whereas ammonia (NH3) is a gas. How can these observations be rationalized in terms of intermolecular forces?
8.103 In previous chapters, we have noted that cryolite is used in refining aluminum. Use the web to look up what this addition does for the process, and relate it to the concepts of intermolecular forces from this chapter.
8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
Which of the following statements about intermolecular forces is( are) true? a. London dispersion forces are the only type of intermolecular force that nonpolar molecules exhibit. b. Molecules that have only London dispersion forces will always be gases at room temperature (25C). c. The hydrogen-bonding forces in NH3 are stronger than those in H2O. d. The molecules in SO2(g) exhibit dipole-dipole intermolecular interactions. e. CH3CH2CH3 has stronger London dispersion forces than does CH4.
8.36 Why are dispersion forces attractive?
Identify the intermolecular forces present in the following solids: (a) CH3CH2OH (b) CH3CH2CH3 (c) CH3CH2Cl

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