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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
Intermolecular Forces, Liquids, and Solids (Chapter 11)
Very brief review of Lewis structures and molecular geometry
Sample Exercises
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Draw Lewis structures for and determine polarity of molecules through sp 8.45 – 8.64, 9.31 –
hybridization (8.5-8.7, 9.1-9.6) 9.38
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 face- 11.59 – 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)
Properties of Solutions (Chapter 13)
Chapter Exercises
The solution process – a review of electrolytes
Identify substances as acids, bases, or salts in aqueous
solutions (4.3, handout)
Identify substances as strong or weak/non electrolytes in
aqueous solution (4.3, handout)
Determine whether substances are soluble or insoluble in
aqueous solution (4.2, handout)
Write total ionic and net ionic equations for a variety of
acid/base/salt reactions (4.2)
Methods of expressing concentrations
Work numerically with the expressions of mass percentage,
ppm, ppb, molarity, molality, and mole fraction (4.5, 13.4)
Factors affecting solubility
Predict solubilities based on intermolecular forces (13.3)
State and predict effects of temperature and pressure on
solubility (13.3)
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 point, boiling point, and osmosis
(13.5)
Colloids
Qualitatively describe colloids (13.6)
4.29 – 4.36
4.1 - 4.18, 4.37 – 4.38,
4.19 – 4.22
4.23 – 4.28, 4.39 – 4.44,
4.59 – 4.76, 13.33 – 13.54, 13.85, 13.87 –
13.91, 13.114 – 13.116
13.11 – 13.14, 13.83
13.19 – 13.32
13.55
13.55 – 13.76, 13.92 – 13.98, 13.99 –
13.100, 13.104 – 13.105, 13.107, 13.112 –
13.113, 13.117 – 13.121
13.77 – 13.82
Chemical Kinetics (Chapter 14)
Methods of expressing rates
Given a chemical reaction, express the rate in terms of the
stoichiometry (14.2)
Factors that affect reaction rates
Identify factors that affect a reaction rate and their effect
(14.1)
i. Dependence of rate on concentration
Given experimental initial rate information, determine the rate
law for a reaction (14.3)
Given sufficient concentration/time information, find missing
information for first- and second- order reactions (14.4)
Use half-life relationships for first- and second-order reactions
to find missing information (14.4)
ii. Dependence on temperature
Describe molecularly the effect of temperature on reaction rate
(14.5)
Apply the Arrhenius equation (14.5)
iii. Catalysis
Qualitatively describe the mechanisms of homogeneous,
heterogeneous, and enzyme catalysis (14.7)
Mechanisms and molecularity
Given a mechanism, write the anticipated rate law (14.6)
Simplify a rate law for a given mechanism given the rate
determining step (14.6)
Chemical Equilibrium (Chapter 15)
The concept of equilibrium
Describe the concept of a dynamic equilibrium (15.1)
The equilibrium constant and its link to thermodynamics
Given sufficient information, determine whether or not a
system is at equilibrium (15.2)
Relate Kc and Kp (15.2)
Relate the equilibrium constant to the free energy (19.7)
Interpreting and working with equilibrium constants
Predict direction of equilibrium based on value of equilibrium
constant (15.3)
Given a chemical equilibrium write the expression for the
equilibrium constant (15.3-15.4)
Calculating equilibrium constants
Use the equilibrium constant expression to find missing
information (15.5)
Use the equilibrium constant and given concentrations to
predict the direction of reaction (15.6)
Calculate equilibrium concentrations given starting
concentrations and the equilibrium constant (15.6)
LeChâtelier's Principle
Predict shifts in equilibrium due to changes in concentration,
volume, temperature, pressure, or the addition of catalyst
(15.7)
Acid-base equilibria (Chapter 16)
Review of current acid-base concepts (4.3, 16.1)
Bronsted-Lowry acids and bases
Identify substances as Bronsted-Lowry acids or bases (16.2)
Identify conjugate acid-base pairs (16.2)
Determine relative acidity or basicity of substances (16.2)
The autoionization of water
Given hydronium or hydroxide concentration, determine the
other (16.3)
The pH scale
Given hydronium, hydroxide, pH, and/or pOH determine the
other values (16.4)
Calculations involving strong acids and bases
Determine hydronium, hydroxide, pH, and/or pOH values
given a concentration of a strong acid or base (16.5)
Calculations involving weak acids, weak bases, and salts
Determine hydronium, hydroxide, pH, and/or pOH values
given a concentration of a weak acid, weak base, or salt
solution and the appropriate equilibrium constant (16.6-16.9)
Acid-base behavior and chemical structure
Identify factors that affect acid and base strengths (16.10)
Lewis acids and bases
Identify materials as Lewis acids or bases (16.11)
Other Aspects of Aqueous Equilibria (Chapter 17)
Common ion effect
Identify “common ions” in a given solution
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)
Qualitative analysis for metallic elements
Given results of particular steps in Figure 17.22, state
conclusions regarding the presence or absence of specific ions
(17.7)
Thermochemistry and Thermodynamics (Chapter 5 and 19)
The nature of energy and its importance in chemistry
Distinguish between kinetic and potential energy (5.1)
Convert between energy units (5.1)
Identify system and surroundings (5.1)
Work with energy conversions, particularly heat and work
(5.1)
The First Law of Thermodynamics
Relate internal energy to heat and work (5.2)
Identify endothermic and exothermic changes (5.2)
Identify properties as a state function or path function (5.2)
Chemical applications of enthalpy
Define enthalpy (5.3)
Draw an enthalpy diagram for a reaction (5.4)
Determine heat requirements for heating, cooling, and phase
changes in physical changes (5.5)
Given calorimetry data, determine enthalpies of change and
reaction (5.5)
Given sufficient information, apply Hess’ Law to determine
enthalpies of reaction (5.6)
Enthalpies of formation
Use enthalpies of formation to determine enthalpies of
reaction (5.7)
Spontaneous processes
Distinguish between the terms spontaneous and
nonspontaneous process (19.1
Distinguish between reversible and irreversible processes
(19.1)
Entropy
5.1, 5.9-5.12, 5.16
5.13, 5.14
5.15, 5.17-5.18
5.3, 5.19-5.22
5.2, 5.5, 5.6
5.4
5.7
5.8
Describe the role of entropy in determining the spontaneity of
a process (19.2)
State and apply the Second Law of Thermodynamics (19.2)
Free energy and
its application to
spontaneity
Given sufficient information, calculate the Gibbs Free Energy
for a reaction (19.5)
Determine temperature ranges of spontaneity (19.5)
Complete a nuclear transmutation equation given sufficient
information (21.3)
Describe the process of nuclear fission and the basic principles
behind a nuclear fission reactor (21.7)
Describe biological effects of radiation (21.9)