ChemistryChemistry 102A/E102A/E

Dr. Christine Yerkes

207 Chem Annex

333-6353

cyerkes@illinois.edu

Mon. and Wed. 11:00 - 12:00

Tues. and Thurs. 2:00 - 3:00

or by appointment

Chemistry, 7th ed., Zumdahl

Quiz sections begin: Wed., Aug. 27

Required Texts:

On-line Homework: 75 pts.Exam Correction 10 pts.Quiz score: 150 pts.Participation 15 pts.Hour Exams (3 x 150) 450 pts.Final Exam 300 pts.

1000 pts.No make-up quizzes or exams

Grading Policy:

Grades

97-100% (970 - 1000) = A+93 - 96% (930 - 969) = A90 - 92% (900 - 929) = A-87 - 89% (870 - 899) = B+83 - 86% (830 - 869) = B80 - 82% (800 - 829) = B-etc., etc., etc.

1000 points total

weekly quizzes - material from Lecture andQuiz section

each quiz worth 15 points - keep 10 highest

Quiz scores:

175 points

TA evaluation - 15 points

After H.E. I and II – correct errors 10 points

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

Course Homepagehttp://www.chem.uiuc.edu

Lon-Capa = net i.d. Password = AD password

Chem 102A/ECourse Web Sites

homepage

Chemistry understand nature atomic or molecular level

observation

hypothesis

prediction

experiment

observation

measurement of physical phenomena

number units

charge of an electron

- coulombs00000000000000000160

Scientific Notation

0.

Scientific Notation

0.000000000000000000160

number x 10n

1-9

integer

1.60 x 10 = 1.601.60 x 101 = 16.01.60 x 10-1 = 0.1601.60 x 10-19

1.60 or 1.6 or 1.600

Significant figures

0

Significant figuresuncertainty in last digit

5.08 x 104 5.0800 x 104

3 sig.fig.5.07

50,700 50,900

5 sig.fig5.0799 50,799 50,801

1. All non zero digits are significant2. Zeros between digits are significant3. Zeros to left of digits are not significant 4. Zeros to right of digits and decimals are significant

5.09 5.0801

Significant figures(47.03) x (0.00540) =

sig.fig(5.40 x 10-3)

sig.fig

0.253962sig.fig

= 0.254

rounding 5 round up< 5 round down

round at end ofcalculations

45.6 0.369+ 83.51

1 decimal place

3 decimal places

2 decimal places

limiting

129.47900 129.5

4 3

3 limiting

Significant figures

732.11 + 6.3760.00

=

do addition (subtraction) first

732.11+ 6.3 =2 decimal 1 decimal 1 decimal

738.41 (738.4)

do multiplication (division) last738.4760.00

4 sig fig

5 sig fig

738.41760.00

= 0.9715921054 sig fig

0.9716

unitsSI

mass kilogram kglength meter mtime second stemperature kelvin Kamount mole mol

TK = TC + 273.15

mole = 6.02 x 1023

unitsSI

mass kilogram kglength meter mtime second stemperature kelvin Kamount mole mol

volume = length3

1 liter (L)1 cm3

= (1 dm)3 = (10 cm)3 = 1000 cm3

= 1 mL

Dimensional Analysis

1. Start with data given, including units.2. Determine the units in the answer3. Find conversion factors

What is the mass, in grams, of 1.00 gallon of water? The density of water is 1 g/mL.

1.00 gal = g

1 gal = 4 qt

4 qts

1 gal

1.057 qt = 1 L

1 L

1.057 qt

1 g = 1 mL 1000 mL = 1 L

1000 mL

1 L

1 g

1 mL

3

3780 g3.78 x 103 g

3784.295