10.1 Intermolecular Forces
Dispersion, dipole-dipole, and hydrogen bonding ranked by strength, matched to molecular structure, and tied to melting and boiling points.
10 exercises
10.1 Exercise 1
In terms of their bulk properties, how do liquids and solids differ? How are they similar?
10.1 Exercise 3
In terms of the kinetic molecular theory, in what ways are liquids similar to gases? In what ways are liquids different from gases?
10.1 Exercise 5
What is the evidence that all neutral atoms and molecules exert attractive forces on each other?
10.1 Exercise 7
Define the following and give an example of each:
(a) dispersion force
(b) dipole-dipole attraction
(c) hydrogen bond
10.1 Exercise 9
Why do the boiling points of the noble gases increase in the order He < Ne < Ar < Kr < Xe?
10.1 Exercise 11
Arrange each of the following sets of compounds in order of increasing boiling point temperature:
(a) HCl, H2O, SiH4
(b) F2, Cl2, Br2
(c) CH4, C2H6, C3H8
(d) O2, NO, N2
10.1 Exercise 13
On the basis of intermolecular attractions, explain the differences in the boiling points of n–butane (−1 °C) and chloroethane (12 °C), which have similar molar masses.
10.1 Exercise 15
The melting point of H2O(s) is 0 °C. Would you expect the melting point of H2S(s) to be −85 °C, 0 °C, or 185 °C? Explain your answer.
10.1 Exercise 17
Explain why a hydrogen bond between two water molecules is weaker than a hydrogen bond between two hydrogen fluoride molecules.
10.1 Exercise 21
Identify the intermolecular forces present in the following solids:
(a) CH3CH2OH
(b) CH3CH2CH3
(c) CH3CH2Cl
Adapted from General Chemistry © 2019 Rice University. Licensed under CC BY 4.0. Sources: Chemistry 2e, Chemistry: Atoms First 2e. Imported at revision 32c7196.