2) As seen in the graph below, the boiling point of HF is higher than HCI, HBr, and HI. Which ofthe following intermolecular attractions is responsible for the high boiling point of HF?100H20HFH2TeSbHsNH3HASeHIH&SASH3SnH4HCHBr-100-PH3GeH4CH4-2003.PeriodA) Dipole-dipole bondingB) London dispersionC) Hydrogen bondingD) lon-dipole bondingE) Covalent bondingBoiling point (in C)

Boiling point of a given molecule depends on the intermolecular interactions. Higher the strength of…

2) As seen in the graph below, the boiling point of HF is higher than HCI, HBr, and HI. Which of the following intermolecular attractions is responsible for the high boiling point of HF? 100 H20 HF SbHs NH3 HASe H&S IH AsH3 SnH4 HC HBr -100 PH3 GeH4 SH CH -200 4 Period A) Dipole-dipole bonding B) London dispersion C) Hydrogen bonding D) lon-dipole bonding E) Covalent bonding Boiling point (in C)

2) As seen in the graph below, the boiling point of HF is higher than HCI, HBr, and HI. Which of the following intermolecular attractions is responsible for the high boiling point of HF? 100 H20 HF SbHs NH3 HASe H&S IH AsH3 SnH4 HC HBr -100 PH3 GeH4 SH CH -200 4 Period A) Dipole-dipole bonding B) London dispersion C) Hydrogen bonding D) lon-dipole bonding E) Covalent bonding Boiling point (in C)

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter14: Liquids And Solids

Section: Chapter Questions

Problem 6A

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Similar questions

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.
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?
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.
The heats of vaporization of liquid O2, liquid Ne, and liquid methanol, CH3OH, are 6.8 kJ/moL 1.8 kJ/mol, and 34.5 kJ/mol, respectively. Are the relative values as you would expect? Explain.
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A 1.50-g sample of methanol (CH3OH) is placed in an evacuated 1.00-L container at 30 C. (a) Calculate the pressure in the container if all of the methanol is vaporized. (Assume the ideal gas law, PV = nRT.) (b) The vapor pressure of methanol at 30 C is 158 torr. What mass of methanol actually evaporates? Is liquid in equilibrium with vapor in the vessel?
For each of the following pairs, choose the member with the lower boiling point. Explain your reason in each case. (a) NaCl or PCl3 (b) NH3 or AsH3 (c) C3H7OH or C2H5OCH3 (d) HI(g) or HCl(g)
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8.45 Describe how interactions between molecules affect the vapor pressure of a liquid.
Suppose that three unknown pure substances are liquids at room temperature. You make vapor pressure measurements and find that substance Q has a pressure of torr, substance R has a pressure of 42 torr, and substance S has a pressure of 330 torr. If you slowly increase the temperature, which substance will boil first and which will boil last?
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