Chapter 5:
Liquids and Solids
1. Why do condensed phases form?
a. Because they have been cooled sufficiently.
b. Because they have a lack of kinetic energy.
c. Attractive forces between particles pull the particles together.
d. None of the above.
Answer:
C
2. In the process of hydration, to what is water attached?
a. Solute ions.
b. Neutral, solute particles.
c. Solvent ions.
d. Neutral particles.
Answer:
A
3. Dipole-dipole interactions require what electron arrangement occur within molecules?
a. Non-ionic regions within a molecule.
b. Ionic regions within a molecule.
c. Non-polar regions within each molecule.
d. Polar regions, positive and negative, within each molecule.
Answer:
D
4. What causes London forces?
a. Electric interactions between any ions in solution.
b. Attractions between instantaneous induced electric dipoles on adjacent molecules.
c. Electric interactions between solute ions dissolved in solution.
d. Attractions between permanent induced electric dipoles on adjacent molecules.
Answer:
B
5. What element or elements must H be bonded to for hydrogen bonding to occur?
a. Nitrogen, chlorine, or fluorine atoms.
b. Oxygen, nitrogen, or carbon atoms.
c. Oxygen, nitrogen, or fluorine atoms.
d. Nitrogen, carbon, or oxygen atoms.
Answer:
C
6.
a.
b.
c.
d.
What gives rise to surface tension?
The imbalance of intramolecular forces at a liquid’s surface.
The imbalance of intermolecular forces at a liquid’s surface.
The favorable attraction of solvent molecules to each other at a liquid’s surface.
The favorable attraction of solute molecules in a solution to each other at a liquid’s
surface.
Answer:
B
7. How are the atoms or ions of a crystalline solid arranged in comparison to those of a
cooled liquid?
a. They are less ordered within a two dimensional plane than the cooled liquid structure.
b. They display less short range three dimensional order than the cooled liquid structure.
c. They are more ordered and regularly arranged in three dimensions than the cooled
liquid structure.
d. None of the above.
Answer:
C
8. What coordination number of adjacent (nearest neighbor) atoms does any cubic
closest-packed structure have (another name for cubic closest-packed is face centered
cubic)?
a. 6.
b. 8.
c. 10.
d. 12.
Answer:
D
9. A unit cell represents atoms in what type of array?
a. The smallest unit of an amorphous solid.
b. The smallest unit of a non-crystalline solid, one that can stack repeatedly without
gaps.
c. The smallest unit that can represent a crystal, when stacked together repeatedly
without gaps.
d. The smallest unit that can represent any solid, when stacked together repeatedly
without gaps.
Answer:
C
10. Upon what factor does an ionic structure always depend?
a. The radius ratio between cation and anion.
b. The charge ratio between the cation and anion.
c. The covalent character of polyatomic ions within the unit cell.
d. The ionic character of charged ions within the unit cell
Answer:
A
11. Upon what do the physical properties of molecular solids depend?
a. The covalent character of polyatomic ions within them.
b. The strength of their intermolecular forces.
c. The charges of the ions within them.
d. The radius ratio of the ions that make up the molecules.
Answer:
B
12. What is the primary binding force within network solids?
a. Dipole-Dipole forces.
b. Ionic bonds.
c. Covalent bonds.
d. Hydrogen bonds.
Answer:
C
13. How does the fixed, localized character of valence electrons in metals produce its
luster and malleability?
a. By providing slip planes within the material.
b. By oscillating in similar frequencies to light reflected off a metal’s surface.
c. By providing a flexible, electron sea throughout the material.
d. It does not; rather, the mobility of valence electrons produces metal luster and
malleability.
Answer:
D
14. What is an interstitial alloy?
a. One in which one type of atom replaces another atom within the lattice.
b. One in which an atom fits into the holes made by the lattice of another type of atom.
c. One in which one type of atom is inserted into another atom’s space within the lattice.
d. One in which a smaller atomic type makes up the lattice of an alloy.
Answer:
B
15. How do properties differ in anisotropic materials versus in crystalline materials?
a. Properties depend upon the direction of measurement in anisotropic materials.
b. Properties depend upon the size of the material sample in anisotropic materials.
c. Properties depend upon the charge density within anisotropic materials.
d. Properties depend upon the radius ratio of ions within anisotropic materials.
Answer:
A