Office  3109 Newman and Wolfrom Lab
Office Hours  2:30-3:30 M, T, W, R
E-mail  woodward@chemistry.ohio-state.edu
Phone  688-8274
Web Site  www.chemistry.ohio-state.edu/~woodward/chem_121.htm

Text  “Chemistry, The Central Science” by Brown,
Lemay and Bursten 9 th Edition
Lab Manual  “General Chemistry Laboratory
Experiments, Volume 1” by Casey & Tatz
Lab Notebook  “Student Laboratory Notebook”
Calculator  TI-30, Sharp EL-509, Sharp EL-531,
Casio FX-250 www.chemistry.ohio-state.edu/~woodward/chem_121.htm

Midterm 1 (Tues, Feb 3 rd )
Midterm 2 (Tues, Feb 24 th )
Final Exam (Tues, Mar 16 th )
Laboratory (10 labs)
Quizzes
(6 Quizzes, drop the lowest)
Total
175 pts
175 pts
300 pts
200 pts
150 pts
1000 pts
Opportunities to do problems
 Take home quizzes
 Recitation Exercises
 Homework Problems (at the end of the chapter)
 Web Material (Old exams, sample quizzes, CD exercises)

5. This class is a weed out class.
For example consider the final grade distribution from
Autumn 2002 (beginning with ~300 students):
21 Dropped 20 Failed
29 D/D+
59 B-/B/B+
126 C-/C/C+
46 A-/A

4. It’s OK to blow off lab, because it’s only 20% of your grade.
If you don’t get 50% in lab, you will be given a failing grade. Extra time will not be given to make up missed labs.

3. The curve will save me.
If you get below 600 points (60%) the best grade you can hope for is C-, and your likely to get a D or D+.
If you get below 500 points (50%) you’re almost certain to fail the class.

2. There are so many students that office hours will be very crowded, plus professors don’t want to be bothered.
Office hours are usually only crowded before the exams. I set aside time to see you during office hours so it’s boring when no one comes. I’m also happy to make appointments for other times if you have conflicts with my office hours.

1. Knowledge of chemistry will make you more attractive to the opposite sex and enhance your love life.
Unfortunately based on personal experience I see no evidence for this kind of cause and effect relationship.

Keep in mind though that generally hypotheses and even theories are based on an incomplete set of experiments, so that later experiments or advances may provide further information that shows the theory or hypothesis to be incorrect.

Matter – Anything that has mass and occupies space.
Atom – The smallest stable building block of matter. Made up of protons, neutrons & electrons.
Molecule – Groups of atoms held together with a specific connectivity and shape.
Composition tells us the types of atoms that are present in a compound and the ratio of these atoms (for example H
2 etc.).
O, C
2
H
6
O,
Structure tells us which atoms are connected (bonded) to each other, how far apart they are, and the shape of the molecule.

Pure Substance  Matter that has a fixed composition and distinct properties. All substances are either elements or compounds.
Elements  All atoms are the same, i.e. Oxygen (O
Silicon (Si) and Diamond (C).
2
), Gold (Au),
You should memorize the elemental symbols in Table 1.2
Compounds  Contains more than one type of atom, but all molecules (or repeat units) are the same, i.e. Water (H
2
(C
2
H
6
O), Quartz (SiO
2
O), Ethanol
), Sodium Chloride (NaCl). All compounds follow the law of constant composition.
Mixture  Have variable composition and can be separated into component parts by physical methods. Mixtures contain more than one kind of molecule, and their properties depend on the relative amount of each component present in the mixture.

Periodic Table

Ne
SO
3
N
2
Homogeneous
Mixture

Homogeneous Mixture  Composition and properties are uniform. Sometimes called a solution.
Air – principle components include O
2
, N
2
& CO
2
Vodka – principle components are ethanol and water
Brass – solid solution of Cu and Zn
Ruby – solid solution of Al
2
O
3 and Cr
2
O
3
Heterogeneous Mixture  Composition and properties are non-uniform.
Chocolate Chip Cookie – Chocolate, Dough, etc.
Concrete – Cement, Rocks, etc.
Vomit – Depends upon previous intake of food and drink

Physical Properties  The identifying characteristics of matter. Some properties can be readily measured with our senses, such as odor and color, instruments are needed to measure other properties, such as electrical resistivity, compressibility, hardness, melting point, etc.
Chemical Properties  Describe the reactivity of a substance toward other substances. Examples include:
Ethanol burns in air (reacts with oxygen in the air)
Sodium reacts vigorously with water,
Corrosion of metal parts (rust),
Trinitrotoluene (TNT) is explosive,
Lysergic acid diethylamide (LSD) is a hallucinogenic drug.

Ethanol
Stoichiometry = C
2
H
6
O
Melting Point = -115 ºC
Boiling Point = 78 ºC
Density = 0.79 g/cm 3
Chemical Prop. = Intoxicating
Dimethyl Ether
Stoichiometry = C
2
H
6
O
Melting Point = -140 ºC
Boiling Point = -24 ºC
Density = Gas
Chemical Prop. = Intermediate
Ethylene Glycol
Stoichiometry = C
2
H
6
Melting Point = -16 ºC
O
2
Boiling Point = 197 ºC
Density = 1.11 g/cm 3
Chemical Prop. = Toxic

You will be expected to know these prefixes from memory.

1. Non-zero numbers are always significant.
2. Zeros between non-zero numbers are always significant.
3. Zeros before the first non-zero digit are not significant. (Example: 0.0003 has one significant figure.)
4. Zeros at the end of the number after a decimal place are significant.
5. Zeros at the end of a number before a decimal place are ambiguous (e.g. 10,300 g).

Addition and Subtraction
Line up the numbers at the decimal point and the answer cannot have more decimal places than the measurement with the fewest number of decimal places.
Multiplication and Division
The answer cannot have more significant figures than the measurement with the fewest number of significant figures.

1 m 3  (100 3 cm 3 )/(1 m 3 ) = 1,000,000 cm 3
1,000,000 cm 3 = 1  10 6 cm 3

2H
2
(g) + O
2
(g)  2H
2
O(g)