Unit 4 Objectives
(Chapters 11 and 12)
At the conclusion of this unit of study, you should know and/or be able to do the
following:
Chapter 11:
Intermolecular Forces and Liquids and Solids
1.
List and/or describe the characteristic properties of the three primary states (phases) of matter:
solids, liquids, and gases in terms of the Kinetic Molecular Theory.
2.
List and/or describe the three types of van der Waals forces (intermolecular attractive forces)
found in neutral molecules: dipole-diole, London dispersion, and hydrogen-bonding.
3.
Describe ion-dipole forces that are found in solutions.
4.
Describe the formation of each of these various intermolecular forces.
5.
Compare the relative strengths of these intermolecular forces in different sizes and types of
molecules.
6.
Describe how each of these intermolecular forces effects a substance’s properties, i.e., boiling
point.
7.
List the elements that exhibit significant hydrogen bonding and/or describe their characteristics.
8.
Identify the predominate type of intermolecular force for a given compound.
9.
Describe viscosity, surface tension (including cohesive and adhesive forces), and capillary action
in terms of the intermolecular forces.
10.
Describe phase changes (melting/freezing, vaporization/condensation, and
sublimation/deposition) in terms of the substance’s intermolecular forces.
11.
Describe, draw, and/or interpret a heating curve for a substance.
12.
Calculate the enthalpy changes associated with a substance’s phase change(s).
13.
Define and/or describe the relationship between critical temperature and critical pressure.
14.
Define vapor pressure and/or describe the factors that effect it.
15.
Describe the relationship between intermolecular forces and volatility.
16.
Discuss the boiling process in terms of intermolecular forces, pressure, and kinetic energy
(temperature).
17.
Interpret phase diagrams for substances and predict what effect pressure and temperature
changes have on a substance.
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Unit 4 Objectives
(Chapters 11 and 12)
18.
Describe and/or compare the characteristics of crystalline and amorphous solids.
19.
Define unit cell and describe and/or identify examples of simple unit cells: primitive cubic,
body-centered cubic, and/or face-centered cubic.
20.
Determine the number of cations and anions present in a unit cell.
21.
List and/or describe various “close packing” arrangements and their coordination number.
22.
Describe the relationship between packing arrangements and the amount of empty space in a
unit cell. Describe how X-ray diffraction is used to determine crystal structure.
23.
Describe various bonding types in solids: molecular, covalent-network, ionic, and metallic.
24.
Compare various physical properties (i.e., boiling point, conductivity, etc.) for solids based on
the predominate bond types and/or identify examples of substances that exhibit a particular bond
type.
25.
Describe the formation of amorphous solids and list examples.
Chapter 12:
Physical Properties of Solutions
25.
Define solution and describe its components – solute and solvent.
26.
Describe the solvation (hydration for aqueous solutions) process and the enthalpies associated
with its various steps.
27.
Describe the relationship between solution formation, spontaneity, and disorder.
28.
Discuss the importance of solutions in chemical reactions.
29.
Define and/or identify examples of crystallization.
30.
Define the terms: unsaturated, saturated and supersaturated. Using a solubility table, determine
a substance’s solubility at various temperatures.
31.
Describe the relationship between a substance’s predominant intermolecular force(s) and its
solubility.
32.
Describe how pressure effects solubility. Use Henry’s law (Cg = kPg) to determine a substance’s
solubility at a given pressure.
33.
Describe how temperature effects solubility … especially for gaseous solutes.
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Unit 4 Objectives
(Chapters 11 and 12)
34.
Determine a solute’s concentration in various units:
mass percent =
mass solute
x 100
masssolution
parts per million (ppm) =
parts per billion (ppb) =
mole fraction () =
molarity (M ) =
molality (m) =
mass solute
x 106
masssolution
mass solute
x 109
masssolution
molcomponent
total moles of all components
mol solute
L solution
mol solute
kg solvent
35.
Define and/or list examples of colligative properties.
36.
Describe and/or calculate the effect of vapor pressure on solubility
Raoult’s law: PA = A PAo
37.
Describe and/or calculate the effect of concentration on a substance’s boiling and freezing
points:
Tb = Kb m
Tf = K f m
38.
Describe and/or calculate the effect of concentration on osmotic pressure
n
= RT = MRT
V
39.
Determine a substance’s molar mass based on its colligative properties.
40.
Describe colloidal dispersions (collids), common types, (hydrophilic and hydrophobic) and their
properties.
41.
Describe various colloidal particle removal processes.
42.
Describe fractional crystallization.
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