KEY: 

text (Chang) 
delivery method  evaluation method 
x.y where 
l = lecture 
T = lecture test 
x = chapter 
n = notes 
Lx = lab number x (labs are also delivery methods)^{1} 
y = section 
v = video, slideshows, internet sources available 
F = final exam 
1,2,3,4,5 
TBR General Ed learning outcomes 15 
see below 
C = critical item question or lecture test 
Item 
Performance/Task: The student will:  text sections 
delivery method 
eval. method 
TBR learn objectives 
General Equilibria 

1 
Be able to write the expression
for any equilibrium if given a reaction using standard states 
14.114.3 
l, n 
T 

2 
Be able to solve for an unknown
quantity in an equailibrium problem when simple substitution is involved
(RSCC type 1 when the problem is presented at equilibrium). 
14.214.3 
l, v, L 
T, F, L 

3 
Be able to apply algebra to
problems that start out not at equilibrium and approach equilibrium (RSCC
type 2) 
14.4 
l, v, L 
T, F, L 

4 
Be able to apply Le Châtelier's
principle to shifts in equilibrium cause by changes in temperature, pressure
and concentrations. 
14.5 
l, v 
T 

5 
Be able to describe the role of a catalyst. 
14.5,(13.6) 
l 
T 

Acids and Bases and pH 

6 
Be able to write any BrønstedLowry
acidbase reaction (also review from CHEM 1110) 
15.1 
l, v, L 
T, L 

7 
Be able to describe autoionization
and be able to make calculations using the K_{w} 
15.2 
l, v, L 
T. F, L 

8 
Be able to calculate the pH given
either the [H_{3}O^{+}]} or the [OH^{}] 
15.3 
l, v, L 
T, C, L 

9 
Be able to calculate the pH of a strong acid
or a strong base 
15.4 
l, v, L 
T, C, L 

10 
Be able to calculate the pH of a weak acid or
a weak base (type 2) 
15.5, 15.6 
l, v, L 
T, C, L 

11 
Be able to calculate the equilibrium constant
for the conjugate of a weak acid or weak base. 
15.7 
l, v, L 
T, C, L 

12 
Be able to calculate pH of polyprotic acids
and know the convention for the 1st, 2nd, etc. ionization constant 
15.8 
l, v, L 
T, L 

Review item  know the strong and weak acids
and the strong, slightly soluble and weak soluble bases 
15.9 
l, v, L 
T, L 

13 
Be able to do salt hydrolysis problems to obtain
pH 
15.10 
l, v, L 
T, L 

Review item  Be able to write the reaction
between metal or nonmetal oxides and water. 
15.11 
l, v, L 
T, L 

14 
Know the definition of amphoteric (and amphiprotic)
and how it applies to slightly soluble polyprotic hydroxides. 
15.11 
l, v, L 
T, L 

15 
Know the definition of a Lewis acid and base
and be able to identify these in a reaction 
15.12 
l 
T 

Buffers, Titrations, K_{sp},
K_{f} and K_{d} 

16 
Be able to calculate the pH
of a buffer. 
16.2, 16.3 
l, v, L 
T, C, L 

17 
Be able to calculate the titration
curve for either a strong acid/weak base titration or a strong base/weak
acid titration 
16.4 
l, v, L 
T, L 

18 
Be able to calculate the pH
of an end point a determine the appropriate indicator 
16.5 
l, v, L 
T, L 

19 
Be able to calculate the common
ion effect for solubility using the K_{sp}_{ (type 1)} 
16.6, 16.8 
l, v, L 
T, L 

20 
Be able to calculate the molar solubility from any starting solution given the K_{sp}_{ (type 2) }  16.6, 16.8 
l, v, L 
T, L 

21 
Be able to combine solubility calculations with
pH 
16.9 
l, v, L 
T, L 

22 
Be able to do type 1 or type 2 problems involving
complex ions using either the K_{f} or K_{d} 
16.10 
l, v, L 
T, L 

23 
Be able to combine pH, complex ion and solubility
problems, especially to the qualitative analysis scheme 
16.11 
l, v, L 
T, L 

Thermochemistry* 

24 
Know the definition of energy
and the various forms it might assume. 
6.1 
l, v 
T 

25 
Know the definitions of the
following: open system, closed system, isolated system, surroundings,
a universe, exothermic, endothermic, state function, state of a system 
6.26.3 
l, v 
T 

26 
Be able to give the first law
of thermodynamics and make calculations base upon it. 
6.4 
l, v 
T, C 

27 
Be able to define work, heat,
internal energy and enthalpy 
6.26.4 
l, v 
T 

28 
Know the definition of molar heat capacity (at
either constant volume or pressure) and be able to do problems involving
heat capacity 
6.5 
l, v 
T 

29 
Be able to calculate the enthalpy of reaction
from the standard enthalpies of formation. 
6.6 
l, v 
T, C 

30 
Be able to calculate the enthalpy of solution
from the standard enthalpies of formation of compounds and ions. 
6.7+ 
l, v 
T, C 

Thermodynamics* 

31 
Be able to give an explanation
of the zeroth law of thermodynanics 
6.5 
l, v 
T 

32 
Be able to define what a spontaneous process
is. 
18.2 
l, v 
T, C 

33 
Be able to relate entropy to
microscopic randomness and how to calculate it give the number of microstates. 
18.3 
l, v 
T 

34 
Know what is meant by "standard
state" and standard (molar) state functions 
18.3 
l, v 
T 

35 
Be able to give the second law of thermodynamics
and make calculations based upon it 
18.4 
l, v 
T, C 

36 
Be able to tell what the third law of thermodynamic
is a reach conclusions based upon it. 
18.4 
l, v 
T 

37 
Be able to calculate the Gibbs' free energy
and know the importance of it in relation to equilibrium. 
18.5 
l, v, L 
T, C, L 

38 
Be able to derive the equation that relates
thermodynamics to the equilibrium constant and relate this to the van't
Hoff plot 
18.6 
l, v, L 
T, C, L 

39 
Be able to calculate the equilibrium constant
from the standard molar Gibbs' free energy 
18.6 
l, v, L 
T, C, L 

Electrochemistry 

40 
Be able to balance redox reactions
by the half reaction method. 
19.1 
l, v, L 
T, L 

41 
Be able to describe how an electrochemical cell works, with it various parts. Cells include: Galvanic, Leclanché, mercury, lead storage, NiCd, lithium , fuel cell, concentration cells, Downs cell,  19.2, 19.6 
l, v, L 
T, L 

42 
Know the definitions used in electrochemistry
including: anode, cathode, electrolyte, anolyte, catholyte, half cell reaction,
voltage, electromotive force or emf 
19.2 
l, v, L 
T, L 

43 
Be able to describe and use
standard (reduction) potentials and how they are derived from thermodynamics. 
19.3 
l, v, L 
T, C, L 

44 
Be able to interconvert from
standard molar Gibbs' free energy to standart potentials using the standard
hydrogen electrode 
l, v 
T, C 

45 
Be able to calculate standard potentials for
a cell. 
19.3 
l, v, L 
T, C, L 

46 
Be able to calculat nonstandard potentials
for a cell using the Nernst equation. 
19..5 
l, v, L 
T, C, L 

47 
Be able to recognize whether a radox reaction
is spontaneous or not and, related, whether a cells emf is positive or
negative. 
19.4 
l, v, L 
T, L 

48 
Be able to describe the principal mechanism
of aqueous corrosion 
19.7 
l 
T 

49 
Be able to calculate quantities of material
evolved (or used) in an electroplating (or galvanic) cell using Faraday's
law 
19.8 
l, v, L 
T, L 

Chemical Kinetics 

50 
Be able to define mathematically
the rate of a reaction and how this is related to other expressions of rate. 
13.1 
l, v, L 
T, C, L 

51 
Be able to determine a rate law and make calculations base upon a rate law.  13.2 
l, v, L 
T, L 

52 
Be able to express the simple
zero, first, and second order integrated rate laws and use them to make
calculations. 
13.3 
l, v, L 
T, L 

53 
Be able to utilize the concept
of "half life" for the first order integrated rate law to make calculations. 
13.3 
l, v 
T, C 

54 
Be able to explain the collision theory and
the transition state theory to calculate the temperature dependance (Arrhenius
equation both simple substitution and parametrically) of the rate constant. 
13.4 
l, v 
T 

55 
Be able to relate reaction mechanisms and elementary
steps to obtain the rate law 
13.5 
l, v 
T 

56 
Know the role of catylsts and be able to site
some examples and how it affects a reaction. 
13.6 
l 
T 

Organic Chemistry (instructor
option) 

57 
Be able to distinguish the various
classes of hydrocarbons and their properties. (aliphatic, aromatic,
alkanes, alkenes, alkynes, cyclic, etc.) 
24.1, 24.2 
l 
T 

58 
Be able to name the alkanes, alkenes, alkynes
and their (functional) substituted derivatives. 
24.2 
l 
T 

59 
Know the various types of isomers
and what the origin is of structural, geometrical and optical isomerism. 
24.2 
l 
T 

60 
Be able to tell if a molecule has a geometrical
isomer or an optical isome 
24.2 
l 
T 

61 
Be able to describe the substitution reaction
and how it is accomplished. 
24.2 
l 
T 

62 
Be able to describe and predict the addition reaction
to alkenes and alkynes 
24.2 
l 
T 

63 
Know the basic structure of the aromatic hydrocarbons
and the role of resonance. 
24.3 
l 
T 

64 
Be able to name some of the simple substituted
aromatics. 
24.3 
l 
T 

65 
Be able to describe the mechanism of the aromatic
substitution reaction. 
24.3 
l 
T 

66 
Be able to recognize the functional groups:
alcohols, carboxylic acids, esters, ethers, aldhydes, ketones,amines, amides,
halogens, nitryls 
24.4 
l 
T 

67 
Know the important reactions involving the functional
groups. 
24.4. 
l 
T 

Nuclear
Chemistry (instructor option) 

68 
Know the subatomic particles important in nuclear
chemistry and their symbols 
23.1 
l 
T 

69 
Be able to balance a nuclear reaction and fill
in unknown quantities 
23.1 
l 
T 

70 
Know what is meant by the belt (band, island)
of stability be able to predict the type of decay for a radioactive isotope
not on the belt 
23.2 
l 
T 

71 
Be able to calculate the energy released in a
nuclear reaction given the isotope masses 
23.2 
l 
T 

72 
Be able to describe the decay of unstable heavy
isotopes and the various decay series 
23.3 
l 
T 

73 
Be able to do halflife type calculations, include
dating techniques 
23.3 
l 
T 

74 
Be able to describe fusion reactions and know
some of the important ones. 
23.4, 23.6 
l 
T 

75 
Be able to describe fission reactions and know
some of the important ones. 
23.4, 23.5 
l 
T 

76 
Be able to describe some important applications
of radioactive isotopes 
23.7 
l 
T 
TBR General Education
Outcomes for Natural Sciences Learning Outcomes 

Item 
Students will demonstrate the ability to….. 
1 
Conduct an experiment, collect and analyze data,
and interpret results in a laboratory setting. 
2 
Analyze, evaluate and test a scientific hypothesis. 
3 
Use basic scientific language and processes, and
be able to distinguish between scientific and nonscientific explanations. 
4 
Identify unifying principles and repeatable patterns
in nature, the values of natural diversity, and apply them to problems or
issues of a scientific nature. 
5 
Analyze and discuss the impact of scientific discovery
on human thought and behavior. 