Which of the following molecules will have the highest boiling point? (Hint: assume similar MW) a. CHỊCH,CH,CHINH, b. CH₂CH₂CH₂CH₂CH₂ CH₂ I Ẹ CHỊCHCHỊCH, d. NF₁ What intermolecular forces affect the following molecule? a. London Dispersion Forces Only b. Dipole-Dipole Forces Only c. Hydrogen-Bonding Only d. e. London Dispersion and Dipole-Dipole Forces London Dispersion, Dipole-Dipole, and Hydrogen-Bonding Forces

Which of the following molecules will have the highest boiling point? (Hint: assume similar MW) a. CHỊCH,CH,CHINH, b. CH₂CH₂CH₂CH₂CH₂ CH₂ I Ẹ CHỊCHCHỊCH, d. NF₁ What intermolecular forces affect the following molecule? a. London Dispersion Forces Only b. Dipole-Dipole Forces Only c. Hydrogen-Bonding Only d. e. London Dispersion and Dipole-Dipole Forces London Dispersion, Dipole-Dipole, and Hydrogen-Bonding Forces

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 121CWP: Which of the following compound(s) exhibit only London dispersion intermolecular forces? Which...

See similar textbooks

Similar questions

8.45 Describe how interactions between molecules affect the vapor pressure of a liquid.
Consider the following data for xenon: Triple point: 121C, 280 torr Normal melting point: 112C Normal boiling point: 107C Which is more dense, Xe(s) or Xe(l)? How do the melting point and boiling point of xenon depend on pressure?
8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
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.
The following data are given for CC14: normalmeltingpoint=23Cnormalboilingpoint=77Cdensityofliquid=1.59g/mLvaporpressureat25C=110mmHg How much heat is required to vaporize 20.0 L of CCl4 at its normal boiling point?
Rubidium chloride has the sodium chloride structure at normal pressures but assumes the cesium chloride structure at high pressures. (See Exercise 69.) What ratio of densities is expected for these two forms? Does this change in structure make sense on the basis of simple models? The ionic radius is 148 pm for Rb+ and 181 pm for CI.
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?
ou seal a container half-filled with water. Which best describes what occurs in the container? Water evaporates until the air becomes saturated with water vapor; at this point, no more water evaporates. Water evaporates until the air becomes overly saturated (supersaturated) with water, and most of this water recondenses; this cycle continues until a certain amount of water vapor is present, and then the cycle ceases. The water does not evaporate because the container sealed. Water evaporates, and thou water evaporates and recondenses simultaneously and continuously. The water evaporates until it is eventually all in vapor form. stify your choice, and for choices you did not pick, explain what is wrong with them.
8.39 Under what circumstances are ion-dipole forces important?
Referring to Figure 9.7, state what phase(s) is (are) present at (a) 1 atm, 10C. (b) 3 mm Hg, 20C. (c) 1000 mm Hg, 75C.
8.87 Use the vapor pressure curves illustrated here to answer the questions that follow. (a) What is the vapor pressure of ethanol (C2H5OH) at 60°C? (b) Considering only carbon disulfide (CS2) and ethanol, which has the stranger intermolecular forces in the liquid state? (c) At what temperature does heptane (C7H16) have a vapor pressure of 500 mm Hg? (d) What are the approximate normal boiling pains of each of the three substances? (e) At a pressure of 400 mm Hg and a temperature of 70°C, is each substance a liquid, a gas, or a mixture of liquid and gas?