Chapter 10 and 11 Logs
1. Which compound is most likely to form intermolecular hydrogen bonds?
a. C4H10
b. NaH
c. C2H5OH
d. C2H5SH
2. Which bests explains why bromine is soluble in mineral oil?
a. both substances are liquids
b. both substances have similar densities
c. both substances are made up of nonpolar molecules
d. both substances dissolve in water
3. Generally, the strongest interaction with water molecules in aqueous solution is for ions that have
a. large charge and large size
b. large charge and small size
c. small charge and large size
d. small charge and small size
e. zero charge and small size
For questions 4-6, consider the following intermolecular forces of attraction. Choose which type of
interaction best explains each statement. You may use a response once, more than once, or not at all.
a. London Dispersion b. dipole-dipole interactions c. hydrogen bonds
d. covalent bonds
4. This force is the strongest interaction between hexane and iodine.
5. Water and ethanol are completely miscible.
6. Dry ice sublimes endothermically.
7. Which factor(s) affect the vapor pressure of a liquid at equilibrium?
I. Intermolecular forces of attraction within the liquid
II. The volume and/or surface area of the liquid present
III. The temperature of the liquid.
a. I only
b. II only
c. III only
d. I and II
e. I and III
Questions 8-11 refer to the following information: A solid that is a poor conductor of electricity, is very
hard, and has a high melting point.
8. The solid probably is
a. metallic
b. an alloy
c. ionic
d. molecular
e. network covalent
9. The solid could be
a. quartz
b. tin
c. brass
d. table sugar
e. rock salt
10. The chemical formula of this solid is
a. CaSO4
b. Pb
c C20H42
d. SiC
11. The properties of this solid can be attributed to
a. interlocking pattern of atoms
b. intermolecular hydrogen bonding
c. the electron sea model
d. interstitial atoms occupying the spaces between them
e. P2O5
12. The aqueous solution of which salt will have the strongest cation-dipole interaction?
a. NaCl
b. MgCl2
c. K2SO4
d. Cr(NO3)3
e. CaSO4
13. Enough water is added to 11.5 g of ethanol to make 2.00 L of solution. What is the molarity of the
ethanol?
a. 0.125 M
b. 0.250 M
c. 0.500 M
d. 5.75 M
e. 0.333 M
14. Which pair of substances will dissolve in each other?
I. CH3OH
II. C6H6
a. I and II
b. II and III
c. I and III
15. All the following will dissolve in water except:
a. ethanol
b. aluminum chloride
III. CH3CH3
d. I and II, II and III
c. calcium nitrate
d. hexane
Problem Solving
1. Use concepts of chemical bonding and/or intermolecular forces to account for each of the
following observations. List the type of intermolecular force for each substance.
a. The boiling points of water, ammonia, and methane are 100oC, -33oC, and -134oC,
respectively.
b. At STP, chlorine is a gas, bromine is a liquid, and iodine is a solid.
2. Solid Ammonium chloride dissolves in water with a marked decrease in temperature. Calcium
chloride dissolves in water with a marked increase in temperature. Little or no temperature change
is observed when solid sodium chloride dissolves in water.
a. Write an equation that describes the dissolving process of ammonium chloride.
b. Is the dissolving of calcium chloride endothermic or exothermic?
c. Describe the opposing forces of attraction that are at work in the dissolution of calcium
chloride. Which are greater? Why?
3. Using some common laboratory equipment and materials, devise a plan to deduce the type of
bonding in a sample of unknown solid. Specify the tests you would perform and discuss what the
results mean.