Name: ____KEY______________________ Section: ___________
Chapter 10 Worksheet Spring 2007 page 1 of 3
Chapter 10 Practice Worksheet:
Liquids, Solids, and Phase Changes
1. Circle all of the molecules below that are polar:
a. CH
3
Cl
b. CH
4
c. CCl
4
d. SO
2
e. CO
2
f. H
2
O
g. NH
3
h. CH
3
–CH
3
i. CH
2
=CH
2
j. CH
3
OH
k. CH
3
NH
2
2. Define each type of intermolecular force below. Give an example of each and describe what
characteristic that example has that results in each type of intermolecular force.
a. Ion-dipole: _attractive forces between an ion and a polar molecule _____
b. Dipole-dipole: _attractive forces between polar molecules (pure substance or mixture)___
c. London dispersion forces: _attractive forces between all molecules (induced dipoles uneven
electron distribution _
d. Hydrogen bonding: _ attractive forces between hydrogen and nitrogen, oxygen, or fluorine __
3. List the intermolecular forces that exist between molecules (or formula units) in each of the following.
Circle the strongest force that will determine physical properties (e.g., boiling points) for each substance.
CH
3
Cl __London, dipole-dipole________________________________________
H
2
_London_________________________________________
HCl __London, dipole-dipole________________________________________
Ne __London________________________________________
NH
3
___London, dipole-dipole, hydrogen_______________________________________
HF __London, dipole-dipole, hydrogen________________________________________
CH
3
OH __London, dipole-dipole, hydrogen________________________________________
C
2
H
4
___London_______________________________________
CO
2
___London_______________________________________
CO ___London, dipole-dipole_______________________________________
4. Explain the intermolecular forces that compete to determine whether or not an ionic substance will
dissolve in water. Which force must be strongest in order for an ionic substance to dissolve?
In order for an ionic solid to dissolve, there is competition between the ion-ion forces within the compound
and ion-dipole forces between ions and water molecules. If the ion-dipole forces are stronger, the solid will
dissolve in water.
