3
4
5
6
7
8
9
10
11
Week Date
1
2
Jan 9-13
16-20 no M
23-27
Jan 30-Feb 3
Feb 6-10
13-17 no R
20-24
Feb 27-Mar 2
Mar 12-16
19-23
Mar 26-30
Lecture
Ch 1-2
Ch 2
Ch 3
Ch 4
Ch 4-5
Ch 5
Ch 6
Ch 7
Ch 7,14
Ch 14
Ch 14-15
Experiment
MG2005: Toledo exam, paperwork, film
MG2005: Excel & lab info
Check-in; Determination of Density
Preparation of Alum
Gravimetric Analysis of Alum
University Conference
Colorimetric Determination of Al
Hydrolysis of Oil of Wintergreen
Determination of Molar Mass by Titration
Determination of Vitamin C
Enthalpies of Hydration
12
13
14
15
16
Apr 2- 6
9-13 no M
Ch 15,10
Ch 10
Reaction of Crystal Violet
Determination of Equilibrium Constant
16-20 no Tu
Apr 23-27
Ch 19
Ch 19
Molecular Models & Student Research Conference
Diffusion; Polymer Properties
May 1, Tuesday, at 1:30pm Final Exam http://academics.truman.edu/Spring2011FinalsSchedule.pdf
Lecture: MWF 1:30-2:20pm in MG 1000
Lab: T at 11:30-14:20, R at 8:30-11:20 and 11:30-14:20, all in MG 1029
Petrucci/Harwood/Herring/Madura, General Chemistry: Principles and Modern Applications , 9th ed,
©2007
Most of the laboratory experiments are at http://chemlab.truman.edu/ChemicalPrinciples.htm
but the Excel exercise, Molecular Models, Diffusion, and Polymer Properties are at U:\_SC Student File Area\Pultz\
Laboratory notebook (with carbon or carbonless copies)
Scientific calculator is required in lecture and lab (except when we use Excel)
Goggles are required in lab
The Solutions Manual is good.
Grades : The nominal cut-offs for letter grades are 90%, 80%, etc., but I will look for natural breaks at or below the nominal cut-offs
Approximate point distribution:
5 tests (~80 points each) every three weeks daily lecture quizzes + assignments lab final exam
400
200
200
200
Tentative test schedule: Jan 27, Feb 17, March 18, April 8 & 29
Attendance is expected. Contact me before missing any test so that you can take it early. If you are sick, contact me before I post the answer key. Experiments are set up for one week usually, and coming to a different lab section is subject to a maximum of 24 students per lab section. If you miss an experiment or test or assignment, the lost points may result in a lower letter grade for this course. Remember, however, that you can miss at least 100 points and still earn an A in this course. But it would be prudent to reserve those 100 points for incorrect answers rather than skipping opportunities to earn points.

I expect you to study the textbook. First skim each chapter or section to gain an overall impression or framework. Then reread slowly several times until you understand everything. Bring the textbook to class.
In order to be successful, the average student will spend 2 hours outside of class for each hour in class. You should be working on CHEM 130 for 8 hours per week outside of class time. Be effective in your studying: if you get stuck on a problem, do not just keep working on it but go to another problem or get help. This strategy of not getting stuck on a problem is also one to remember when taking a test.
Office hours : MWF 9:30-11:20am and M 2:30-4:20pm and Tu 8:30-9:20am
If you need help in this course, come see me during office hours or take advantage of the Chemistry Contact
Center in MG 3155 which is 28 feet south of my office. The Chemistry Contact Center is staffed by professors who are experts in chemistry and is generally open 9:30-12:30 and 1:30-4:30 Monday through
Friday, but see the schedule by the door for exact times. There is also tutoring by students in the evening and I will provide details as I receive the information.
Academic Integrity: Students are expected to work alone on quizzes and tests and the final exam without the use of any outside resources; I will provide a periodic table and any necessary constants. If I allow you to make up a test late, you may not consult with students who have already taken the test.
If you have a disability for which you wish to receive an accommodation, contact Disability Services in the
Student Health Center. The contact person is Vicky Wehner at 660-785-4478 or vwehner@truman.edu
CHEM 130 fulfills the physical science mode of inquiry in the Liberal Studies Program at Truman State
University. Modern chemistry began with quantitative experiments, and quantitative measurements continue to be essential for many applications of chemistry. This aspect of chemistry is emphasized in your textbook and in most laboratory experiments. The Vitamin C experiment introduces you to experimental design and serves as a capstone experience in scientific research.
This course emphasizes the technical language and basic theories of chemistry with a goal of assisting you in making informed decisions about many public policy issues. You should be empowered to locate information and to address technical issues, preparing for lifelong learning.
The LSP outcome statements are available on-line at http://academics.truman.edu/modesInquiry.asp
Detailed outcome statements are at http://chemlab.truman.edu/Assessment/CHEM130Outcomes.asp and http://chemlab.truman.edu/Assessment/laboutcomes.htm
Old minitests at U:\_SC Student File Area\Pultz\CHEM 120
I will send some announcements to your Truman e-mail address.
Assignment due F Jan 14 by 13:30
Go to www.epa.gov and explore the web site. Find a useful and interesting document. Turn in individually the information listed below.
+1 Name of EPA document
+1
+3
URL
Summary of information provided
+1 Something interesting that you learned
----------------------------------------------------------------------------

Week 1
WHAT IS CHEMISTRY?
M 10 Jan 2011
"The material world consists of an enormous variety of substances. Chemistry is concerned with the nature of these substances and with the changes that they undergo when they interact with each other.
We call these changes chemical reactions."[Ronald J. Gillespie et al.
, Chemistry , 2nd, ©1989, xxi]
Chemistry is also interested in the synthesis and characterization of new substances.
"Chemistry is the science that concerns the composition, structure, and properties of matter and changes that matter undergoes. Matter is anything that occupies space."[Umland and Bellama, General
Chemistry , 2nd, ©1996 p1]
Chemistry is the study of atoms and compounds, and their transformations.
The most important idea in chemistry is that matter consists of enormous numbers of incredibly small atoms. Elements consist of atoms characterized by a certain number of protons. Most substances are compounds that contain atoms of two or more different elements. The remarkable transformations that accompany chemical reactions--such as the burning of gasoline in air in an automobile engine to give carbon dioxide and water or the conversion of carbon dioxide and water into the complex molecules from which plants are composed in the process of photosynthesis--are simply a consequence of the reshuffling of the atoms of the reacting substances to form new combinations. Making new materials by combining atoms in new ways--whether they are for manufacturing integrated circuits for computers, building new space vehicles, or for making new types of batteries, new fuels, or new drugs--is one of the primary activities of chemists.
Chemistry is not just a collection of a large number of experimental observations--facts--about substances and their reactions. Chemists are constantly striving to understand the facts better in terms of general principles and theories. So the facts about substances and their reactions have been organized into a coherent body of knowledge by the principles and theories that have been developed over the years.
Chemistry is the central science!
U:\_SC Student File Area\Pultz\Beauty and the quest for beauty in science by Chandrasekhar - Physics
Today December 2010.mht http://ptonline.aip.org/journals/doc/PHTOAD-ft/vol_63/iss_12/57_1.shtml p. 1 "no chemicals added"
§1-1 Scientific Method (Figure 1-1) vs
C&EN 10 Nov 2008 Letters p4 & Physics Today July 2009 p8
U:\_SC Student File Area\Pultz\Petrucci_Harwood_Herring_Madura_9th\Harwood*
1. Make observations qualitative quantitative
Measurements have a number and almost always a unit.
Distinguish from conclusions. Observations should be reproducible; conclusions or explanations can change due to new information or biases. If we see a colorless liquid in a beaker we might jump to the conclusion that it is water, but if the liquid quickly evaporates from our finger, then we would need to revise our conclusion.
2. Formulate a hypothesis (possible explanation for the observation)
3. Use the hypothesis to make a prediction that can be tested by experiment
4. Perform experiments, gathering new observations.

Mendeleev took observed chemical and physical properties of the elements ( step 1 ) to develop the periodic table. He arranged the elements according to increasing atomic mass in a periodic fashion ( step 2 ).
He predicted properties of Sc, Ga, and Ge ( ekasilicon ) ( step 3 )
Table 9.1 on p342 (slide 6) ( step 4 )
This example also illustrates that scientists build on work done by other scientists.
Theories or models are our attempt to generalize rather than deal with zillions of independent observations.
Mendeleev developed the periodic table as a way to help his students remember a vast amount of observations on the elements.
"A natural law is a summary of observed behavior, whereas a theory is an explanation of behavior."[Zumdahl, 4th, p7]
This section contrasts deduction (done by the ancient Greeks; postulates of Quantum Mechanics) and induction (starting with experimental observations).
Real problem solving is trial and error. But to get to that level you need a basic understanding of chemistry, and at this basic level you will learn terminology and use applications of algebra.
"Chance favors the prepared mind."
Separate components of petroleum and chemically modify them to produce gasoline, diesel fuel, polymers, drugs, etc. As petroleum price increases, look for alternative sources, perhaps from coal, but also from living plant matter. Dow Chemical Company and Cargill (an agricultural products company) are collaborating to make biodegradable polymers.
────────────────────────────────────────────────────────────────────
Week 1
§1-3 Classification of Matter (Figure 1-4; slide 7)
§1-2 physical vs chemical properties & changes
W 12 Jan 2011
Polymers and mixtures
Undergraduate chemistry focuses on pure substances with relatively few atoms because such substances are easiest to understand. But most substances which we use are mixtures, usually because that is how we obtain desired properties: steel, concrete, rubber tires, gasoline, paper, paint, ...
And many materials contain polymers or macromolecules where the molecules contain thousands of atoms. also show slides 8-10 (Figures 1-5, 1-6, 1-7)
§1-4 SI base units used in General Chemistry: m, kg, s, K, mol Table 1.1; slide 11 mass vs weight
Prefixes for metric units: G, M, k, deci, c, m, μ, n, p, f Table 1.2; slide 12

Assignment due W 19 Jan 2011
Go to http://physics.nist.gov/cuu/Units/units.html
Click on Definitions of the SI base units. Give the precise definition of your assigned base unit, then click on its Go to historical context button and give a short summary.
First letter of last name Assigned base unit
A-E meter
F-J
K-N
O-S
T-Z kilogram second kelvin mole

temperature scales (Figure 1-8; slide 14)
§1-5 density = mass/volume intensive extensive
Solid and liquid densities should be around 1 g/cm
3
which is the approximate density of liquid water.
PHHM9 lists typical density ranges: solids 0.2 - 20 g/cm
3 liquids gases
0.5 - 4 g/cm
3
~0.001 g/cm
3
Substance
Li(
Al( s s
)
)
Fe( s )
Pb( s )
Density (g/cm
0.5
2.7
7.9
11.3
22.4
22.5
3
) at room temperature
Ir( s )
Os( s )
Hg( l )
CH
3
CH
2
CH
2
CH
2
CH
3
CH
3
CH
2
CH
2
CH
2
CH
2
CH
2
CH
3
CCl
4
0.63
0.68
1.6
13.5
Concept Assessment on page 14: mass water displaced = mass of block = 1.00 x 10
3 g
Answers for these questions are in Appendix H specify significant figures; k = 10
3
Since d = m/V, V = m/d
Volume of block = 1.00 x 10 3 g = 1.4
0.68 g/cm 3
7
x 10 3 cm 3 density of water  1.0 g/cm 3
Volume of water displaced = 1.00 x 10 3 g = 1.0 x 10 3 cm 3
1.0 g/cm 3 fraction of wood under water = Volume of water displaced
Volume of block
= 1.00 x 10
1.4
7
x 10
Note other appendices, esp. A-1, A-5, and G
Problems not covered in lab:
Density of Al is 2.70 g/cm
3
. Convert to kg/m
3
.
A vehicle consumes 11.7 L per 100 km. What is the mpg?
Use 1 inch

2.54 cm and 1 L = 1.0567 quarts mm to km, kg to ng, mm
2
to cm
2
7 L gasoline per 100 km: convert to miles/gal
3
3
cm
cm
3
3
= 0.68
34 mpg

Week 1
Toledo exam : 55 min + prep
T&R lab time
The Periodic Table : QD 467 P47 1980
24 min VHS video film produced by BBC-TV/Open University; distributed by The Media Guild.
"Does S ring a bell?"
Xe is a lead balloon.
Alkali metals are soft. Cs is very reactive.
Aluminium is
Group 0 (Noble gases): Compare to current numbering such as at webelements.com
"=" in chemical reaction is currently replaced by

or
⇄ macroscopic vs microscopic (particulate) vs symbolic water is most dense at 3.98

C
Physical vs chemical changes phase: sample of matter that is uniform in composition and physical state
Figure 1-7; slide 10 change state vs change identity
Blackboard SP11:CHEM130 Combined Lab Paperwork due this Friday

Week 1
Appendix A-1: Scientific or Exponential Notation
TR lab 11 & 13 Jan 2011
There are 100 cm in a meter; convert to exponential notation:
There are 6.02 x 10
23
molecules in 18.0 mL of water; write without using exponents:
The mass of an electron is 9.10939 x 10
-31 kg; write without using exponents:
Other examples of conversions ...
Remember: 10 raised to a positive number is greater than one
10 raised to a negative number is less than one
Multiplication and division: Your calculator should do this automatically. But let's do two examples by hand:
(5.4 x 10
3
)(2.0 x 10
-7
) = (5.4
x 2.0) x 10
3-7
= 10.8
x 10
-4
or 1.1 x 10
-3
(5.4 x 10
3
)/(2.0 x 10
-7
) = (5.4/2.0) x 10
3-(-7)
= 2.7 x 10
10
Add exponents for multiplication; subtract exponents for division!
Powers and roots: Again your calculator should do this, but we will do two examples by hand:
A cube has an edge length of 2.0 x 10
-2 m. Its volume is
(2.0 x 10
-2 m)
3
= (2.0)
3
x (10
-2
A square has an area of 1.6 x 10
5
km
2
)
3
= 8.0 x 10
-6 m
3
. The edge length is
(1.6 x 10
5 km
2
)
1/2
= (16 x 10
4
)
1/2
= 4.0 x 10
2 km
Addition and subtraction: Although your calculator should do this automatically, you may need to do it at least partially by hand so that you get the correct significant figures. When we add or subtract numbers, the exponents of the numbers must be the same.
1.356 x 10
- 1.287 x 10 -8 - 0.01287 x 10 -6
-6 1.356 x 10 -6
1.34313 x 10 -6 which rounds to 1.343 x 10 -6
§1-6&7 Uncertainties in Measurements and Significant Figures
All measurements have uncertainty, except when small #s of objects are counted.
Significant Figures: those digits which are certain plus one which is uncertain
DEMO: Put a little water in a beaker and report the amount.
Pour all the water into a graduated cylinder and report your new measurement. Note difference in significant figures!
Precision (reproducibility) vs accuracy (correctness) of measurements
U:\_SC Student File Area\Pultz\Petrucci_Harwood_Herring_Madura_9th\Zumdahl3_Fig1-7_Precision_vs_accuracy
Figure 1.7a indicates a large random or indeterminate error, probably due to poor technique.
Figure 1.7b indicates a large systematic or determinate error, but small random error.
Significant figures: Figure 1-12; slide 23
Ex.: 0.0008060
Significant figures in calculations often easier to see with exponential notation
Addition/Subtraction examples
Multiplication/Division examples 2.52 x 3.4
Rationale (Worst-case method for estimating experimental uncertainty) see U:\_SC Student File Area\Pultz\Petrucci_Harwood_Herring_Madura_9th/Worst-case_method.xls
Round only at end of multistep calculations!

Exact numbers: 4 in CH
4
, 12 in = 1 ft, 1 in = 2.54 cm, 1 m = 100 cm
A rule of thumb in designing experiments is to avoid using a result that is the small difference between two large measured quantities. In terms of uncertainties in measurement, why is this good advice?Zumdahl, 3rd, 1.73
A-5 & pp 14-17: Conversion factors (dimensional analysis)
PHHM9: Conversion relationships can be constructed from either intensive properties (such as density or % composition) or unit equivalencies.
Convert 2 Å to nm, given 1 Å = 10 -8 cm
Density of Al is 2.70 g/cm
3
. Convert to kg/m
3
.
A vehicle consumes 11.7 L per 100 km. What is the mpg?
Use 1 inch

2.54 cm and 1 L = 1.0567 quarts mm to km, kg to ng, mm
2
to cm
2
7 L gasoline per 100 km: convert to miles/gal 34 mpg

Class procedures:
Assignments will have due dates and they are to be turned in on paper individually unless specified otherwise.

Read chapters thoroughly and understand Concept Assessments and Examples within chapters. Work
Practice Examples.
Problems to work on as you prepare for the first test:
Chapter 1 Exercises: 1, 7, 9, 11, 13, 17, 19-23, 27-32, 37, 40, 42, 47, 51, 53, 57, 67, 78
Chapter 2 Exercises: 1-5, 7-9, 13, 19, 23, 37-39, 46-48, 51-53, 55
1. Which is the largest? 1 fs 1 ns 1 ks 1 Gs
2. Convert 5.05
x 10
7 m to the SI unit that will give the smallest number greater than 1. U&B2.56
3. Classify each of the following as a qualitative observation, quantitative observation, or conclusion:
(a) The gas is reddish-brown.
(b) The gas is nitrogen dioxide.
(c) The liquid boils at 100

C.
(d) Putting a burning match to the mouth of a test tube containing the gas produces a loud pop.
(e) Adding the solid to the liquid produces bubbles.
4. Observation or conclusion? This is a piece of chalk.
5. Liquid nitrogen boils at 77 K. What is this temperature in

C? 77 - 273 = -196

C
6. In my section of CHEM 120 in Spring 2007, the final grade distribution was 12 A's, 22 B's, 24 C's, 7 D's, and 2 F's. What was the percent distribution of grades, that is, % A's, etc.?