1. Chemistry 102A/E Dr. Christine Yerkes 207 Chem Annex 333-6353
Mon. and Wed. 1:00 - 2:00
Tues. and Thurs.2:00 - 3:00
or by appointment

2. Required Texts:
Chemistry, 7th ed., Zumdahl
Quiz sections begin: Wed., Aug. 29
Merit sections begin tomorrow

3. Grading Policy: On-line Homework: 75 pts. Exam Correction 10 pts.
Quiz score: pts.
Participation pts.
Hour Exams (3 x 150) 450 pts.
Final Exam pts.
1000 pts.
No make-up quizzes or exams

4. Grades 1000 points total 97-100% (970 - 1000) = A+
% ( ) = B+
% ( ) = B
% ( ) = B-
etc., etc., etc.

5. 175 points Quiz scores: weekly quizzes - material from Lecture and
Quiz section
each quiz worth 15 points -
keep 10 highest
After H.E. I and II – correct errors 10 points
TA evaluation - 15 points
175 points

6. On-line Homework: 13 Homework assignments on Lon-Capa
due dates in the on-line Syllabus and calendar
credit for all problems completed by deadline
normalized to 75 points

7. Course Homepage Course Web Sites Chem 102A/E Lon-Capa = net i.d.
www.
chem.uiuc.edu
Course Web Sites
Chem 102A/E
Lon-Capa = net i.d.
Password = AD password
homepage

8. Chemistry
understand nature
atomic or molecular level
observation
experiment
hypothesis
prediction

9. observation
measurement of physical phenomena
number
units
charge of an electron - 0. 1 6
coulombs
Scientific Notation

10. Scientific Notation
integer
number x
10n
1.60 x 10 =
1.60
1-9
1.60 x 101 =
16.0
1.60 x 10-1 =
0.160
1.60 x 10
-19
1.60 or
1.6 or
1.600
Significant figures

11. Significant figures uncertainty in last digit 5.08 x 104 5.0800 x 104
3 sig.fig.
5 sig.fig
5.07
5.09
5.0799
5.0801
50,700
50,800
50,799
50,801
1. All non zero digits are significant
2. Zeros between digits are significant
3. Zeros to left of digits are not significant
Zeros to right of digits and decimals are
significant

12. Significant figures (47.03) x (0.00540) = 0.253962 = 0.254
sig.fig 3
sig.fig
(5.40 x 10-3) 3
limiting
sig.fig
rounding
 5
round up
round at end of
calculations
< 5
round down
45.6
0.369
limiting
1 decimal place
3 decimal places
2 decimal places
129.5

13. Significant figures 732.11 + 6.3 = 760.00
do addition (subtraction) first =
738.41
(738.4)
2 decimal
1 decimal
1 decimal
do multiplication (division) last
738.4
738.41
4 sig fig =
760.00
760.00
5 sig fig
4 sig fig
0.9716

14. SI
units
mass
kilogram kg
length
meter m
time
second s
temperature
kelvin K
amount
mole
mol
TK = TC
mole =
6.02 x 1023

15. SI
units
mass
kilogram kg
length
meter m
time
second s
temperature
kelvin K
amount
mole
mol
volume
= length3
1 liter (L)
= (1 dm)3
= (10 cm)3
= 1000 cm3
1 cm3
= 1 mL

16. Start with data given, including units.
Dimensional Analysis
Start with data given, including units.
Determine the units in the answer
3. Find conversion factors
What is the mass, in grams, of 1.00 gallon
of water? The density of water is 1 g/mL. 3    
1.00 gal
4 qts
1 L
1000 mL
1 g
= g
1 gal
1.057 qt
1 L
1 mL
3780 g
3.78 x 103 g
1 gal = 4 qt
1.057 qt = 1 L
1 g = 1 mL
1000 mL = 1 L