List all the intermolecular forces available for methylamine, CH3NH2, and indicate the predominant intermolecular force. H H-C-N-H H H dipole-dipole forces and dispersion forces, with dipole-dipole forces being the predominant intermolecular force. dispersion forces, with dispersion forces being the predominant intermolecular force. hydrogen bonds, dipole-dipole forces and dispersion forces, with dipole-dipole forces being the predominant intermolecular force. dipole-dipole forces and dispersion forces, with dispersion forces being the predominant intermolecular force. hydrogen bonds, dipole-dipole forces and dispersion forces, with hydrogen bonds being the predominant intermolecular force.

List all the intermolecular forces available for methylamine, CH3NH2, and indicate the predominant intermolecular force. H H-C-N-H H H dipole-dipole forces and dispersion forces, with dipole-dipole forces being the predominant intermolecular force. dispersion forces, with dispersion forces being the predominant intermolecular force. hydrogen bonds, dipole-dipole forces and dispersion forces, with dipole-dipole forces being the predominant intermolecular force. dipole-dipole forces and dispersion forces, with dispersion forces being the predominant intermolecular force. hydrogen bonds, dipole-dipole forces and dispersion forces, with hydrogen bonds being the predominant intermolecular force.

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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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.
Intermolecular Forces The following picture represents atoms of hypothetical, nonmetallic, monatomic elements A, B, and C in a container at a temperature of 4 K (the piston maintains the pressure at 1 atm). None of these elements reacts with the others. a What is the state (solid, liquid, or gas) of each of the elements represented in the container? b Rank the elements in the container from greatest to least, in terms of intermolecular interactions. Explain your answer. c What type(s) of intermolecular attractions are present in each of these elements? d Explain which element has the greatest atomic mass. e One of the elements in the container has a normal boiling point of 2 K. Which element would that be (A, B, or C)? How do you know? f One of the elements has a melting point of 50 K. Which element would that be (A, B, or C)? Why? g The remaining element (the one you have yet to choose) has a normal boiling point of 25 K. Identify the element. Could this element have a freezing point of 7 K? Explain. h If you started heating the sample to 20 K, explain what you would observe with regard to the container and its contents during the heating. i Describe the container and its contents at 20 K. Describe (include a drawing) how the container and its contents look at 20 K. j Now you increase the temperature of the container to 30 K. Describe (include a drawing) how the container and its contents look at 30 K. Be sure to note any changes in going from 20 K to 30 K. k Finally, you heat the container to 60 K. Describe (include a drawing) how the container and its contents look at this temperature. Be sure to note any changes in going from 30K to 60k
A solution of benzoic acid in benzene has a freezing point of 3.1 C and a boiling point of 82.6 C. (The freezing point of pure benzene is 5.50 C, and its boiling point is 80.1 C) The structure of benzoic acid is Benzoic acid, C6H5CO2H What can you conclude about the state of the benzoic acid molecules at the two different temperatures? Recall the discussion of hydrogen bonding in Section 11.3.
Define the following and give an example of each: (a) dispersion force (b) dipole-dipole attraction (c) hydrogen bond
When a doughnut is placed on a napkin, the napkin will often absorb a liquid and appear moist. What is most likely the nature of the liquid?
Methane, CH4, reacts with chlorine, Cl2, to produce a series of chlorinated hydrocarbons: methyl chloride (CH3Cl), methylene chloride (CH2Cl3), chloroform (CHCl3), and carbon tetrachloride (CCl4). Which compound has the highest vapor pressure at room temperature? Explain.
Describe the formation of hydrogen bonds in propanol, CH3CH2CH2OH. Represent possible hydrogen bonding structures in propanol by using structural formulas and the conventional notation for a hydrogen bond.
Substance A is composed of molecules that have stronger intermolecular forces than the molecules that compose substance B. Which substance has a lower boiling point? a. substance A b. substance B c. cannot be determined without more information.
The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.
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
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.
The vapor pressure of ethanol, C2H5OH, at 50.0 C is 233 mmHg, and its normal boiling point at 1 atm is 78.3 C. Calculate the vapH of ethanol.