Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
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Intermolecular Forces, Liquids, and Solids (Chapter 11)
Very brief review of Lewis structures and molecular geometry
Draw Lewis structures for and determine polarity of molecules through sp3 8.45 – 8.64, 9.31 – 9.38
hybridization (8.5-8.7, 9.1-9.6)
The kinetic-molecular description of gases, liquids and solids
State assumptions of kinetic-molecular theory of gases (10.7)
10.71 – 10.74
Describe molecular level differences between gases, liquids, and solids (11.1)
11.1, 11.9 – 11.12
Intermolecular forces and their effect on properties
Given a substance identify its intermolecular forces (11.2)
11.13 – 11.20
Properties of liquids and solids
Define surface tension and viscosity and predict trends based on intermolecular
11.29-11.31
forces (11.3)
Arrange a series of compounds in order of increasing or decreasing
11.5, 11.21-11.27,
boiling/freezing point (11.3)
11.79 – 11.83, 11.100,
11.110
Interpret a phase diagram and locate the triple point and critical points (11.4, 11.6)
11.6, 11.41-11.42,
11.51 – 11.56
Define vapor pressure and relate it to boiling point (11.5)
11.43– 11.50, 11.91
Identify the three basic types of unit cell – cubic, body-centered cubic, and face11.59 – 11.68
centered cubic (11.7)
Identify the bonding types – molecular, covalent network, ionic, and metallic - in
11.69 – 11.78
various solids (11.8)
Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
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Properties of Solutions (Chapter 13)
The solution process - energetics
Identify the endothermicity and exothermicity of steps in the solution process
13.13-13.14
(13.1)
Identify the role of entropy in the solution process (13.1)
13.3
Define the terms unsaturated, saturated, and supersaturated (13.2)
13.5, 13.21-13.26
Predict solubilities based on intermolecular forces (13.3)
13.7, 13.15-13.16,
13.29-13.30, 13.87
State and predict effects of temperature and pressure on
13.8, 13.31-13.33,
solubility (13.3)
13.89-13.90
Methods of expressing concentrations
Work numerically with the expressions of mass percentage, ppm, ppb, molarity,
13.9, 13.35-13.56
molality, and mole fraction (4.5, 13.4)
Colligative properties
Describe the four colligative properties of solutions and write the mathematical
relationships that apply to each (13.5)
Apply Raoult’s Law and the relationships between concentration and freezing
13.10-13.11, 13.57point, boiling point, and osmosis to a variety of problem situations (13.5)
13.80, 13.96, 13.10013.103
Colloids
Qualitatively describe colloids (13.6)
13.83-13.86
Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
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Needs work
Chemical Kinetics (Chapter 14)
Methods of expressing rates
Given a chemical reaction, express the rate in terms of the stoichiometry (14.2)
14.1-14.4
Factors that affect reaction rates
Identify factors that affect a reaction rate and their effect (14.1)
Given experimental initial rate information, determine the rate law for a reaction
14.13-14.34
(14.3)
Given sufficient concentration/time information, find missing information for
14.35-14.46
first- and second- order reactions (14.4)
Use half-life relationships for first- and second-order reactions to find missing
14.6
information (14.4)
Describe molecularly the effect of temperature on reaction rate (14.5)
14.5,14.7
Apply the Arrhenius equation (14.5)
14.47-14.60
Qualitatively describe the mechanisms of homogeneous, heterogeneous, and
enzyme catalysis (14.7)
Mechanisms and molecularity
Identify the molecularity of an elementary step
14.61-14.64
Combine given chemical equations to result in a desired chemical equation
14.67, 14.70
Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
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Needs work
Chemical Equilibrium (Chapter 15)
The concept of equilibrium
Describe the concept of a dynamic equilibrium (15.1)
The equilibrium constant
Write Kc and Kp for a given system to include heterogeneous systems (15.3-15.4)
15.11-15.14
Relate Kc and Kp (15.2)
15.17-15.18
Interpreting and working with equilibrium constants
Relate chemical equations and equilibrium constants (reverse, take reciprocal,
15.19-15.26
etc.) (15.3)
Given sufficient information, determine whether or not a system is at equilibrium
15.2-15.7
(15.2)
Predict direction of equilibrium (to the left, to the right) based on value of
15.15-15.16
equilibrium constant (15.3)
Calculating equilibrium constants
Find the value of the equilibrium constant given equilibrium concentrations or
15.27-15.34
missing equilibrium concentrations given sufficient information (15.5)
Use the equilibrium constant and given concentrations to predict the direction of
15.35 – 15.38
reaction (reaction quotient) (15.6)
Calculate equilibrium concentrations given starting concentrations and the
15.39-15.50
equilibrium constant (15.6)
LeChâtelier's Principle
Predict shifts in equilibrium due to changes in concentration, volume, temperature,
15.8-15.9, 15.51-15.56
pressure, or the addition of catalyst (15.7)
(in 15.50, CaCrO4
should be a solid)
Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
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Acid-base equilibria (Chapter 16)
Review of current acid-base concepts
Arrhenius Theory (16.1)
16.15-16.16
Identify substances as Bronsted-Lowry acids or bases (16.2)
Identify conjugate acid-base pairs (16.2)
16.17-16.24
Determine relative acidity or basicity of substances (16.2)
16.25-16.28, 16.107
The autoionization of water
Given hydronium or hydroxide concentration, determine the other (16.3)
16.29-16.34
The pH scale
Given hydronium, hydroxide, pH, and/or pOH determine the other values (16.4)
16.35-16.42, 16.111
Calculations involving strong acids and bases
Determine hydronium, hydroxide, pH, and/or pOH values given a concentration of
16.43-16.50, 16.110,
a strong acid or base (16.5)
16.112, 16.122-16.123
Calculations involving weak acids
Given sufficient information, determine hydronium, hydroxide, pH, pOH, Ka,
16.51-16.70, 16.105and/or percent ionization for a weak acid solution (16.6) 16.106, 16.113-16.115,
16.130
Calculations involving weak bases
Given sufficient information, determine hydronium, hydroxide, pH, pOH, Ka,
16.71-16.78, 16.118and/or percent ionization for a weak base solution (16.7)
16.119,16.127
Relationship between Ka and Kb
Determine Ka and Kb for a conjugate acid/base pair given one of them (16.8)
16.79-16.82
Acid-base properties of salt solutions
Given sufficient information, determine hydronium, hydroxide, pH, pOH, Ka,
16.83-16.90, 16.116
and/or percent ionization for a salt solution (16.9)
Acid-base behavior and chemical structure
Identify factors that affect acid and base strengths (16.10)
16.91-16.92
Evaluate the relative acidity or basicity of a series of compounds (16.10)
16.93-16.98, 16.120
Lewis acids and bases
Identify materials as Lewis acids or bases (16.11)
16.99-16.104, 16.125
Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
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Other Aspects of Aqueous Equilibria (Chapter 17)
The Common Ion Effect
Identify “common ions” in a given solution (17.1)
Calculate the pH and associated quantities in systems made with compounds
containing common ions (17.1)
Buffered solutions
Define and identify buffer systems (17.2)
Calculate the pH and associated quantities in buffer systems (17.2)
Calculate changes in pH when acids and bases are added to buffer solutions (17.2)
Acid-base titrations
Generate titration curves for strong acid-strong base, weak acid-strong base,
polyprotic acid titrations (17.3)
Solubility equilibria
Given any chemical equation expressing the dissolution of a solid, write the
mathematical expression for the Ksp (17.4)
Given sufficient information, calculate missing information related to a solubility
situation (17.4-17..5)
Predict solubility based on the introduction of common ions (17.5)
17.13-17.14
17.15-17.18
17.19-17.20
17.21-17.26
17.27-17.28
17.29-17.32
17.33-17.38
17.39-17.46
17.49-17.50, 17.5317.56, 17.59-17.62
17.57-17.58
Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
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Electrochemistry (Chapter 20)
Oxidation States and Oxidation-Reduction Reactions
Use oxidation number to identify the species oxidized, reduced, the oxidizing
20.11-20.16
agent and reducing agent in a redox reaction (20.1)
Balancing Oxidation-Reduction Equations
Use the half-reaction method to balance redox reactions in neutral, acidic, and
20.17-20.22
basic solution (20.2)
Voltaic Cells
Identify the anode and cathode in a voltaic cell (20.3)
20.25-20.26
Find the standard cell potential of a voltaic cell (20.4)
20.27-20.40
Identify the relative strengths of oxidizing agents and reducing agents from
20.41-20.48
standard reduction half-cell potentials (20.4)
Determine the cell potential of a cell under nonstandard conditions using the
20.37-20.68
Nernst equation (20.6)
Electrolysis
Manipulate equations relating current, time, moles of electrons, and mass to
20.87-20.89, 20.91determine missing information (20.9)
20.92
Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
Got it?
Needs work
Chemical Thermodynamics (Chapter 19)
Spontaneous Processes
Distinguish between the terms spontaneous process and nonspontaneous process
(19.1)
Distinguish between reversible and irreversible processes (19.1)
Entropy and the Second Law of Thermodynamics
Describe the role of entropy in determining the spontaneity of a process (19.2)
State and apply the Second Law of Thermodynamics (19.2)
Given sufficient information, determine the entropy change in a chemical or
physical process (19.2, 19.4)
Gibbs Free Energy
Given sufficient information, calculate the Gibbs Free Energy change for a
reaction (19.5)
Determine temperature ranges of spontaneity based on enthalpy and entropy
changes (19.6)
Free Energy and the Equilibrium Constant
Manipulate the relationships between ΔG and K and E° (19.7)
19.9-19.20
19.25-19.26
19.21-19.24, 19.2719.28, 19.43-19.50
19.53-19.60, 19.6919.72
19.61-19.68
19.73-19.82