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 tape or internet slide shows available 
F = final exam 
1,2,3,4,5 
TBR General Ed learning outcomes 15  see
below 
CI = critical item question or lecture test 
item  Performance/Task: The student will:  text sections 
delivery method 
eval. method 
TBR learn objectives 
General  
1  Know the definitions and characteristics of "science" and "chemistry."  1.2  l/n/v  T  3 
2 
Be able to describe the scientific method
and the distinctions between "hypothesis", "theories" and "laws" 
1.3 
l/n/v 
T 
2,3 
3 
Know the definitions of: "substance"
, "homogeneous mixture", "heterogeneous mixture", "element" and
"compound" 
1.4 
l/n/v 
T 
3 
4 
Be able to distinguish between the three
major phases of matter, solids, liquids and gases by their specific
properties 
1.5 
l/n/v 
T 
3,4 
Unit Conversions  
5 
Know the SI base units and unit symbols for mass, length, temperature, amount, time and charge and the unit prefixes M, k, c, m, µ, and n  1.7  l/n/v  T/L2  3 
6 
Know and be able to apply the principles of quantity calculus (i.e. unit factor.)  1.9  l/n/v  T/L2  3 
7 
Know how to interconvert between temperature in degrees celcius and temperature in kelvins  1.8  l/n/v  T  3 
8 
Know the equation which defines density and be able to use it in calculations.  1.7  l/n/v  CI/L3  1,2,3 
Significant Figures  
9 
Know what is meant by significant figures (or digits) and how to express this properly in a written number.  1.8  l/n/v  T/L2  3 
10 
Know how to determine the correct number of significant figures when adding, subtracting, multiplying and dividing quantities.  1.8  l/n/v  T/L2  3 
Introduction to Atomic and Molecular Structure  
11 
Know the characteristics of charge and mass of protons, neutrons and electrons.  2.2  l/n/v  T  3 
12 
Know the composition and general construction of atoms and how in general atoms are related to elements, isotopes and compounds.  2.2  l/n/v  T/L4  3,4,5 
13  Be able to write and interpret the nuclear symbol conventions, eg. ^{2}H,  2.3  l/n/v  T  3 
14 
Be able to distinguish between
ionic and covalent compounds and be able to write their chemical symbolism 
2.5, 2.6 
l/n/v 
T 
3,4,5 
15 
Be able to describe and recognize an
acid or base by the Arrhenius definition 
2.7 
l/n/v 
T 
3,4,5 
16 
Be able to name simple common ionic and
covalent compounds . 
2.7  l/n/v 
T 
3 
Avogadro's Number, N_{A}, Molar Mass, M, and Moles, n  
17  Be able to obtaining the molar masses, M, from the periodic chart.  2.6, 3.1  l/n/v  CI/L4  3 
18  Be able to interconvert between moles and grams and numbers of atoms or molecules.  3.2, 3.3  l/n/v  CI/L4  3,4,5 
19  Be able to interconvert between a molecular or ionic formula and percent composition and from percent composition to empirical formula.  3.5, 3.6  l/n/v  T/L4  3,4,5 
20 
Know what is meant in chemistry by % and how to calculate or interconvert.  3.5  l/n/v  T/L2  3 
Reaction Stoichiometry  
21 
Know what is meant by a chemical reaction and the symbolism used to describe a reaction  3.7  l/n/v  CI/L4  3,4,5 
22 
Be able to do reaction stoichiometry problems if given a reaction.  3.8, 4.6  l/n/v  T/L5  4,5 
23 
Be able to do a limiting reactant stoichiometry problem.  3.9  l/n/v  T/L5  4,5 
24 
Know the definition of percent yield and be able to do problems involving percent yield  3.10  l/n/v  T/L5  4,5 
Solutions, Solution Reactions and Solution Stoichiometry  
25 
Be able to describe the properties of
solutions, both electrolytic and nonelectrolytic 
4.1 
l/n/v 
T 
3 
26 
Be able to recognize a precipitation
reaction 
4.2 
l/n/v 
T 
3,4,5 
27 
Know what spectator ions are and how to identify
them 
4.2  l/n/v 
T 
3,5 
28 
Be able to recognize an "overall reaction" and
be able to describe its usefulness for measurement purposes. 
4.2  l/n/v 
T 
3,4,5 
29 
Be able to write and recognize net ionic reactions
and be able to describe its usefulness for chemical reactions. 
4.2  l/n/v 
T 
2,5 
30 
Be able to describe the BronstedLowery
acidbase reaction and identify the conjugate pairs 
4.3, LM 
l/n/v 
T 
2,3,4,5 
33 
Know the definition of molarity and be able to interconvert from grams or moles of solute and liters of solvent to molarity  4.5  l/n/v  CI/L6 /L11 
1,2,3,4,5 
34  Be able to calculate concentrations in a solution dilution problem  4.5  l/n/v  CI/L6 /L11 
1,2,3,4,5 
35  Be able to do calculations involved with titrations.  4.7, 4.8  l/n/v  CI/L11 /L12 
1,2,3,4,5 
Naming
and Oxidation Numbers 

36 
Know the rules for determining oxidation numbers
and be able to apply them. 
4.4 
l/n/v 
T 
2,3,4 
37 
Know the definition of and be able to recognize
a redox reaction. 
4.4 
l/n/v 
T 
3,4,5 
38 
Know the rules for naming compounds by the
IUPAC convention and be able to apply them. 
L 
l/n/v 
T 
3 
The Perfect Gas Law 

4 
Be able to distinguish
the three major states of matter and know their properties (repeat) 
5.1 
l/n/v 
T 

39 
Know the definition of pressure 
5.2 
l/n/v 
T 
3 
40 
Be able to use the subset of gas laws:
Boyle's law, Charles' law, Amontons' law, GayLussac's law, Avogadro's
principle combined gas law and the Dumas method. 
5.3 
l/n/v 
L13/ L14/CI 
1,2,3,4,5 
41 
Be able to use the ideal gas law to solve
problems 
5.4 
l/n/v 
13/ L14/T 
1,2,3,4,5 
42 
Know the definition of STP and the significance/use
of the value 22.4 L/mol at STP. 
5.4 
l/n/v 
T/L13 
3,4 
Combining the Perfect Gas Law with Stoichiometry
Problems 

43 
Be able to use the ideal gas equation
in combination with reaction stoichiometry 
5.5 
l/n/v 
T/L13 /CI 
1,2,3,4,5 
Dalton's Law 

44 
Be able to derive Dalton's Law from the
ideal gas law. 
5.6 
l/n/v 
T/L13 /L14 
2 
45 
Know the definition of mole fraction
and be able to calculate it and interconvert it to other units. 
5.6 
l/n/v  T 
3,4,5 
46 
Be able to use Dalton's Law in problem
solving. 
5.6 
l/n/v 
T/L13 /L14 
1,3,4,5 
47 
Be able to work with vapor pressure together
with Dalton's Law. 
5.6 
l/n/v 
T/L13 
1,3,4,5 
Kinetic Molecular Theory 

48 
Be able to describe the situation where
there are independent particles as a gas and derive the expression for
the molecular kinetic energy. 
5.7 
l/n/v 
T/L9 
5 
Graham's
Law 

49 
Be able to derive Graham's law from kinetic
molecular theory, i. e. the relationship between kinetic energy and
temperature. 
5.7 
l/n/v 
T 
2 
50 
Be able to use Graham's law for various
practical examples. 
5.7 
l/n/v 
T/L10 
1,3,4,5 
van der Waal's Equation 

51 
Be able to perform calculations using
the van der Waal's equation and know the significance of the van der
Waal's constants. 
5.8 
l/n/v 
T 
2,3,4,5 
Theory of Atomic Structure  
52 
Know what is meant by "Quantum"
and be able to describe the fundamental differences between classical
and quantum physics 
7.1 
l/n/v 
T 

53 
Be able to describe the dual nature of
matter, giving some examples of this dual nature 
7.4 
l/n/v 
T 

54 
Be able describe and to give reasons for quantum numbers  7.5 
l/n/v 
T 

55 
Know what is meant by energy levels and the meaning of the four quantum numbers for an electron in an atom  7.6  l/n/v  T/L7  
56 
Know the selection rules for the quantum numbers of electrons in an atom.  7.6  l/n/v  T/L7  
57 
Know how to designate the quantum numbers by the letter designation, i. e. the electron configurations.  7.6, 7.7  l/n/v  T/L7  
58 
Be able to use the aufbau principle based on the hydrogen atom to give the electron configuration for any atom in its ground state..  7.8, 7.9  l/n/v  T/L7  
59 
Know the order of the high stability configurations and Hund's rule.  7.8  l/n/v  T/L7  
Periodic Trends 

60 
Know the periodic trends, the exceptions to the trends, and the logic behind both for inozation energy, electron affinity, atomic and ionic radius.  8.38.5  l/n/v  T  
61 
Know the definition of electronegativity and the periodic trends for it.  9.5  l/n/v  T  
62 
Be able to describe the peroxides and superoxides in terms of oxidation number and ions formed  8.6  l/n/v  T  
Bond Structure 

63 
Know the definition of valence electrons and how to tell how many there are for a particular atom  8.2  l/n/v  T/L7  
64 
Be able to use the Lewis dot structures
of ionic and covalent molecules and ions using valence electrons. Know and be able to apply the rules for Lewis dot formulas give in the lab manual 
9.29.9 
l/n/v 
T/L8 

65 
Know the definitions of an ionic and covalent compounds and how each is formed..  9.2, 9.4  l/n/v  T/L8  
66 
Be able to explain the reason for the formation
of ionic or covalent compounds based on the tendency to obtain highly
stable electron configuations 
9.3 
l/n/v 
T 

67 
Be able to describe the bonding
involved in a covalent compound including the possibility of double
and triple bonding. 
9.4, 10.5 
l/n/v 
T 

68 
Know the definition of lone or unshare electron pair and how to show this in the Lewis dot structure  9.4  l/n/v  T/L8  
69 
Be able to predict whether a compound is ionic or covalent based upon electronegativity and periodic table position.  9.5  l/n/v  T/L8  
70 
Be able to distinguish between hydrogen
compounds with H having an oxidation number 1 and those with +1 
9.5 
l/n/v 
T 

71 
Be able to recognize the presence of resonance
and symbolize it. 
9.8 
l/n/v 
T 



72 
Know the rules for creating hybrid orbials and be able to apply them to determine electron geometry  10.1  l/n/v  T/L8  
73 
From the molecular structure, be able to
determine if a molecule is polar and, if so, what the orientation of the
dipole is 
9.5, 10.2 
l/n/v 
T/L8 

74 
From the hybrid orbitals and the lone electron pairs, be able to predict the electronic and molecular geometry  10.3,10.4  l/n/v  T/L8  
75 
Know the definition of sigma and pi bonds and the physical appearance and how these might affect geometry (including hindered rotation)  10.5  l/n/v  T/L8  
Ionic Bonding 

76 
Know the definition of ionic compound formation and be able to describe what an ionic compound is  5.15.5  l/n/v  T  
77 
Be able to explain the reason for the formation of ionic or covalent compounds based on the tendency to obtain highly stable configurations.  ?  l/n/v  T  
78 
Be able to decide whether a compound is ionic or covalent; that is, know how to tell by electronegativity difference or Periodic Table positions.  5.10  l/n/v  T  
79 
Be able to distinguish between the hydrogen compounds with 1 oxidation number, the hydrides, and +1, the nonmetal hydrogen compounds.  5.3, 4.3  l/n/v  T  
80 
Be able to write combination reactions of nonmetals (including H) with metals to give principal oxidation number.  5.25.5  l/n/v  T  
81 
Be able to give the formula for the normal oxides for groups 1, 2, 3 and 13 metals.  5.6  l/n/v  T  
82 
Be able to describe the peroxides and superoxides in terms of oxidation number and the ions formed.  5.6  l/n/v  T  
Intermolecular
Forces and the Condensed Phases 

83 
Be able to describe the condences phases and be able to contrast between the three states of matter.  11.1  l/n/v  T  
84 
Be able to describe and rank the various interparticle forces. (London, dipole/ioncdipole/ionic, dipoleinduced dipole, "hydrogen bond")  11.2  l/n/v  T  
85 
Be able to describe and explain the relative boiling points and melting points from the interparticle forces  11.2  l/n/v  T  
Solid State 

86 
Be able to describe some simple crystal
structures for solids and do calculations based on these structures. 
11.4 
l/n/v 
T 

87 
Be able to identify types of solids and
describe the interparticle forces for each type. (ionic, metallic,
covalent, molecular) 
11.6 
l/n/v 
T 

Phase Diagrams 

88 
Know meaning and location of the regions,
boundaries and points in a phase diagram (including the supercritical
fluid.) 
11.8  l/n/v  T  
89 
Be able to describe the equalibria involved
for each phase boundary and point. 
11.8 
l/n/v 
T 

90 
Be able to do calculations based on the
ClausiusClapeyron equation and the associated van't Hoff plot 
11.8  l/n/v  T  
91 
Be able to do calculations to obtain the
total enthapy using heat capacities and heats of phase changes 
11.8  l/n/v  T  
92 
Be able to describe a system that is in
dynamic equilibrium. 
11.8  l/n/v  T  
Electrolytic Solutions 

93 
Know the general characteristic of electrolytic and nonelectrolytic solutions and the molecular dynamics involved  12.1,12.2  l/n/v  T  
94 
Given enthapies of solution, be able to describe the temperature effects involved in solubility.  12.4  l/n/v  T  
95 
Know the definitions of and be able to interconvert between molarity, percent concentration, molality and mole fraction.  12.3 
l/n/v  T/L1  
96 
Be able to do calculations based upon Henry's
law 
12.5 
l/n/v  T/L 

Colligative Properties and Mole Fraction 

97 
Know the definition of colligative properties and the dependence upon mole fraction.  12.6  l/n/v  T,L15  
98 
Be able to calculate mole fraction and molality (based upon particle concentrations.)  12.6 
l/n/v  T,L15  
99 
Be able use Raoult's law in calculations.  12.6 
l/n/v  T  
100 
Be able calculate freezing point depression and boilint point elevation.  12.6  l/n/v  T,L15  
101 
Be able calculate osmotic pressure.  12.6 
l/n/v  T  
102 
Know how to modify the colligative property
calculations with the total concentration for electrolytic solutions 
12.7 
l/n/v 
T 

Colloids 

103 
Be able to describe the various properties
of colloid systems 
12.8 
l/n/v 
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. 