Name ______pd______
Chapter 11 Assignment
Due Date:
Directions: Read Chapter 11, sections 1, 2, and 4 only (not section 3). Complete this assignment- it is worth 45 points and will be counted as a test. Once you have completed this assignment, please sign your name below, next to the x, to indicate you have not worked with a partner.
x______
(Signature)
Multiple Choice (1pt each)
Identify the choice that best completes the statement or answers the question.
____ 1. Because of dipole-dipole forces, the melting points of highly polar compounds are _____ those of less polar compounds.
a. / higher than / c. / equal tob. / lower than / d. / not comparable to
____ 2. A hydrogen bond is a special form of a(n)
a. / covalent bond. / c. / ionic bond.b. / dipole-dipole force. / d. / London dispersion force.
____ 3. A hydrogen bond forms between molecules that contain hydrogen bonded to
a. / a highly electronegative atom. / c. / another hydrogen atom.b. / an atom with a low electronegativity. / d. / a metal.
____ 4. London dispersion forces occur between molecules that are
a. / highly polar. / c. / nonpolar.b. / slightly polar / d. / None of the above
____ 5. A London dispersion force is considered a dipole-dipole force because it
a. / affects all types of compounds. / c. / affects polar molecules.b. / affects nonpolar molecules. / d. / results from a temporary dipole.
____ 6. In the above figure, point B represents the _____ of water, and point C represents the _____ of water.
(The boiling and freezing points occur at standard pressure which is 101kPa or 1atm).
a. / normal freezing point, normal boiling pointb. / normal boiling point, normal freezing point
c. / vapor pressure, atmospheric pressure
d. / critical point of the liquid, critical point of the vapor
____ 7. Point A in the figure represents the _____ point of water.
a. / boiling / c. / freezingb. / critical / d. / triple
____ 8. In the figure, water is a _____ at point D and a _____ at point G.
a. / solid, liquid / c. / solid, gasb. / liquid, gas / d. / gas, solid
Completion (1pt each)
Complete each statement.
1. The tendency of liquids to decrease their surface area to the smallest size possible is called ______. (Use a key term)
2. When a liquid is heated, the temperature stops rising at the liquid’s ______. (key term)
3. When a solid sublimes, it goes from a(n) ______to a(n) ______.
4. The type of bonding in a substance that is a liquid at room temperature will most likely be ______. (section 11-2)
5. The melting point of BaCl2 is ______than the melting point of CaCl2. Hint:p386
6. The greater the difference in electronegativities in a molecule, the ______the polarity of the molecule.
7. Weak dipole-dipole forces result in a(n) ______melting point.
8. A hydrogen bond is ______than a London dispersion force and ______than an ionic bond.
9. The base pairs on complementary strands of DNA are held together by ______.
10. If it were not for London dispersion forces, most nonpolar compounds would be ______at room temperature.
11. Large, flat molecules can come close together and the attractive forces have a______effect.
Section 11-4
12. A region that has the same composition and properties throughout is a(n) ______.(key term)
13. Sweetened iced tea contains ______phases.
14. Vapor pressure ______when temperature decreases.
15. At 630 K, the vapor pressure of mercury equals atmospheric pressure, so 630 K is the ______of mercury. (key term)
16. All three equilibrium lines on a phase diagram meet at the ______. (key term)
17. On a phase diagram, the liquid and vapor phases of a substance are impossible to tell apart above the ______point. (key term)
Short Answer (3pts each)
Answer in no more than 3 COMPLETE sentences. Grammar counts.
1. Explain the difference in adhesion and cohesion in terms of capillary action.
2. How do intermolecular forces differ from attraction between ions?
3. Why don’t dipole-dipole forces have much affect on a gas?
4. Explain how the size and shape of particles affect the attraction between them.
5. Explain what happens in an equilibrium that involves a liquid and a solid.
6. What does a phase diagram show for a substance?
7. What is a supercritical fluid?