Syllabus Chemistry 101 Fall 2008
Sec. 501 (MWF 8:00-8:50) Sec 505 (MWF 12:40-1:30) RM 100 HELD
Professor: Dr. Earle G. Stone
Office: Room 123E Heldenfels (HELD)
Telephone: 845-3010 (no voice mail) or leave a message at 845-2356
email: estone@tamu.edu
(put CHEM 101-Sec. # + subject in subject line of your email)
Office Hours: HELD 123E: Tue. And Thur. 8:00-10:50 AM
I.A. TBA
S.I. Leader: TBA
CHEM 101 and 102 are the first-year chemistry sequence in the core curriculum.
These are 3-credit courses. All lecture sections strive to cover common content.
The lecture component of Chemistry 101 covers stoichiometry, atomic and
molecular structure, inorganic and organic nomenclature and structure, chemical
bonding, fundamental acid/base chemistry, solution chemistry, properties of
liquids and solids, and the gas laws. Additionally, it is the goal of my lecture
section to help you develop the skill set to successfully complete your
undergraduate degree and as most in this class are pre-something to prepare you
for your professional school entrance exam.
All
College
BIMS
Science
GEST
Ag BICH, NUSC, GENE
Engineering
Education
Geosciences
Liberal Arts
Agriculture other
Architecture
Business
501
College
BIMS
Science
Ag BICH, NUSC, GENE
GEST
Engineering
Education
Geosciences
Liberal Arts
Agriculture other
Architecture
Business
498
176
126
64
28
21
30
5
10
25
7
6
100%
35%
25%
13%
6%
4%
6%
1%
2%
5%
1%
1%
2012
2011
2010
2009
2008
399
77
16
4
1
78% Science or Pre-something
22% This is a great way to learn how to survive college
505
249
60
80
20
32
14
15
2
5
11
6
4
100%
24%
32%
13%
8%
6%
6%
1%
2%
4%
2%
2%
College
BIMS
Science
Ag BICH, NUSC, GENE
GEST
Engineering
Education
Geosciences
Liberal Arts
Agriculture other
Architecture
Business
249
116
46
8
32
7
15
3
10
8
1
2
100%
47%
18%
3%
13%
3%
6%
1%
4%
3%
0%
1%
Top Ten Most Repeated Comments
1. But I did not have to study in High School.
2. The instructor places too much responsibility on the student by not requiring
homework which I feel would have helped me if I had done it promptly. Give a
few quizzes to make sure we are doing the required work outside of class
3. Tell us what to know and don’t expect us to figure it out on our own. Teach how to
do the problems in class not just theory. Actually work through the problems,
rather than say the rest is math.
4. Used material from tests earlier in the semester on later exams. The Free
Response was very random and not at all like the problems worked in class. The
material in class was simpler than the material on the exam.
5. I felt like I was seeing much of the material for the first time on the tests. The
instructor should relate class to exams to encourage attendance.
6. The information covered did not pertain to my major as much as BIMS or others.
7. Very good at concentrating on important material and concepts and explaining
them, while spending little time on extraneous issues.
8a. Well organized notes with the problems available online.
8b. (Wish the material was available so I did not have to write down the problems.)
9. His teaching methods make it easy to learn.
10. He needs to take a class in teaching.
http://slc.tamu.edu/
Tutoring
Supplemental Instruction
Courses
Texas Success Initiative
About Us
Contact Us
118 Hotard North of Sbisa, between
Neeley Hall and the Northside Post Office
(979) 845-2724
The Student Learning Center has won the 2008 National College Learning Center Association
Frank L. Christ Outstanding Learning Center Award!
The award recognizes the center's commitment to supporting and strengthening the
Academic experience of students at Texas A&M University by providing a variety of programs and
services that promote retention and success. Read more...
The Student Learning Center provides Supplemental Instruction and tutoring free of charge to all
Texas A&M University students. The SLC oversees the STLC courses (formerly CAEN), which teach
students how to improve their study skills and prepare for the job market. The SLC manages
Developmental programs for students who have not yet passed the assessment tests required by the state.
Study Tips
•General
•Time Management
•Reading Textbooks
•Setting Goals
•Preparing for Exams
•Success Tips from Fellow Aggies
Tutoring
During the Fall 2008 semester, drop-in tutoring will be offered Sunday nights 5-8pm and Monday through Thursday
nights from 5-10pm. Tutoring will begin on Monday, September 1st. Tutor Zones are currently planned for Studio 12 of The
Commons. Look for our table and tutors and just ask for help! See the schedule...
Drop-in tutoring is available for most lower level math and science courses on the first floor of Hotard Hall. Tutors
are also available to help out with many other courses. If you need help in a particular course and would like to check to see if
a tutor is available for that course, you can contact our tutor coordinator, Linda Callen, at 845-2724.
Suggested Course Materials:
“Chemistry and Chemical Reactivity,
Any Edition”, by Kotz, Treichel, and Weaver
or Mastering the Fundamental Skills –
General Chemistry I as a Second Language
Ebook includes
Online tutorial
Solution manual
$45 per semester
Hardbound ~$150
Solution Manual ~$40
Online Tutor ~$45
Helpful
Dictionary of Chemistry
Useful
As A Second Language
Organic Chemistry I
(There is a O-chem II also
for those who will have to
take the class.
Week
1
2
3
4
5
6
7
8
9
Date
25-Aug
27-Aug
29-Aug
1-Sept
3-Sept
5-Sept
End of Chapter Questions
Syllabus Chapter 1–11,13,30,43,45,78,80 Chapters 1,
2, 9
Chapter 2 – 1,27,29,57
Chapter 3 – 7, 8, 19, 21, 23, 27,
29, 31, 33, 39, 47, 51, 56, 61, 85
Chapter 4 – 5, 6, 7, 17, 19, 23,
29, 41, 53, 83
8-Sept Exam #1 Chapters 1,2,3,4
10-Sept 7,8,9 Chapter 7 – 49, 65, 69, 79
Chapters 3,6
12-Sept
Chapter 8 – 1, 3, 5, 7, 17, 31,
15-Sept
39, 47, 71
17-Sept
Chapter 9 – 19, 23, 27, 29, 33,
19-Sept
43, 55, 95
10
Chapter 10 – 5, 7, 11, 13, 23,
22-Sept
29, 33, 51, 53
24-Sept Exam #2 Chapters 7,8,9,10
26-Sept 11
Chapter 11 – 5, 7, 12, 15, 19, Klein Organic
29-Sept
25
Chapters 5, 7;
1-Oct
Traynham
1,2,3
3
3,4
4
3-Oct
6-Oct 22.38-Oct 22.6
10-Oct
13-Oct 5
15-Oct
17-Oct
20-Oct
22-Oct
24-Oct
Chapter 22 - 13,15, 17,19,21
Chapter 5 – 3, 7, 11, 15, 19, Chapters 7,8;
29, 31, 35, 37, 39, 41, 47, 49, Organic 3,4
55, 57, 59, 61, 67, 69, 73, 83,
85, 103, 115, 125
10
11
12
27-Oct
29-Oct
31-Oct
3-Nov
5-Nov
7-Nov
10-Nov
12-Nov
14-Nov
17-Nov
19-Nov
21-Nov
Exam # 3 Chapters 5,11,22
6
Chapter 6 – 9, 27, 33, Chapter 5
39, 43, 45, 47, 51, 59,
61, 71, 79, 83, 89
13
12
Chapter 13 – 1, 3, 7, 13,
19, 33, 35, 37
Chapter 12 - 3, 5, 7, 9, Chapter 4
13
15, 19, 25, 31, 37, 59,
63, 75, 77, 81, 91, 99
24-Nov Exam # 4 Chapter 6,12,13
14 26-Nov Reading Day
28-Nov Thanksgiving Holiday
1-Dec Reading Day
15 2-Dec Reading Day
5-Dec Final morning Sec 501 10 a.m. - Noon
16 8-Dec Final afternoon Sec 504 10:30AM-12:30 PM
Grading:
Your grade will be based on
•Four one-hour examinations (each worth 200 points)
•A final examination (400 points)
There are no bonuses, no extra credit, no soft points
Major Examination Schedule Fall 2005:
Mon. Sept. 8 Major Exam No.1
Wed. Sept. 24 Major Exam No.2
Mon. Oct. 27 Major Exam No.3
Mon. Nov. 24 Major Exam No. 4
Fri. Dec. 5 Section 501 Final Exam 10:00 to 12:00
Mon. Dec. 8 Section 505 Final Exam 10:30 to 12:30
What you are used to
The way the real world works
80%
63%
+3%
70%
90%
46%
80%
60%
100%
97%
29%
D,F,Q,W
after Exam 1
after Exam 2
after Exam 3
after Exam 4
after Final
100%
200
400
600
800
1200
C
B
A
approximate points needed for letter grade
A
B
C
D
150
120
90
60
300
240
180
120
450
360
270
180
600
480
360
240
900
720
540
360
Problem - A situation that presents difficulty, uncertainty, or perplexity:
The mere formulation of a problem is far more often essential than its solution, which
may be merely a matter of mathematical or experimental skill. To raise new questions,
new possibilities, to regard old problems from a new angle requires creative
imagination and marks real advances in science. Albert Einstein
Question - A request for data: inquiry, interrogation, query.
Answer - A spoken or written reply, as to a question.
Solution - Something worked out to explain, resolve, or provide a method for dealing
with and settling a problem.
1. Numbers – Significant Figures, Rounding Rules, Accuracy, Precision, Statistical
Treatment of the Data
2. Units – 5 of the 7
1.
2.
3.
4.
5.
Time – seconds
Length – Meters
Mass – grams
Amount – Moles
Temperature – Kelvins
Density?
Molecular Weight (Mass)
Mole Ratio, Molarity, molality
3. Vocabulary – Approximately 100 new terms or words and applying new or more
rigid definitions to words you may already own.
4. Principles (Theories and Laws) – Stoichiometry, Quantum Theory, Bonding,
Chemical Periodicity, Solutions, Thermodynamics, Intermolecular Forces, Gas Laws
cp = q/mDT
DG = DH – TDS
PV = nRT
DT = Kmi
rate = k[A]m[B]n
Eocell = Ecathode = Eanode
%yield = actual/theoretical * 100%
c (ms-1)
E = n =
l (m)
∆E = q + w
[C]c[D]d
K =[A]a[D]b
Use of Numbers
• Exact numbers
– 1 dozen = 12 things for example
• Accuracy
– how closely measured values agree with the correct value
• Precision
– how closely individual measurements agree with each other
• Significant Figures – start at the left and proceed to the right
– If the number does not have a decimal point count until there are no
more non zero numbers
– If the number has a decimal point start counting at the first non-zero
number and continue counting until you run out of decimal places
• Scientific notation – use it.
Use of Numbers
•
•
Multiplication & Division rule
Easier of the two rules
Product has the smallest number of significant figures of multipliers
4.242
x 1.23
2.7832
x 1.4
5.21766
round off to 5.22
3.89648
round off to 3.9
Addition & Subtraction rule
More subtle than the multiplication rule
Answer contains smallest decimal place of the addends.
3.6923
 1.234
 2.02
6.9463
round off to 6.95
8.7937
 2.123
6.6707
round off to 6.671
When a 5 appears. Is there anything to the right of the 5 greater than zero?
Is the number to the left of the 5 odd?
Is the number to the left of the 5 even? (Treat 0 as even.)
How many sig figs?
0.0713200
7843000
1.4800
100
100.0
894.003
89400
0.03000
74.000
How many sig figs in the answer?
472x101
4600x0.005
36.0x4752
45.08/36.2
1.003/8500
0.003/472x12
3.003/475.0x0.30/524
0.3005x4.1
23.56+24.983
4.78-2.892
46.83-0.03
34.892+5.0
134.033-0.02
48.2-46
[
]
23.56 – 2.3
=
(1.68)
3
1.248 x 10
Round off to two sig figs
34.78
17.51
48.50
45.50001
24.33
17.50
20.5
45.5000
Scientific Method
1.
2.
3.
4.
5.
Observation
Hypothesis
Experiment
Theory
Law
1
2
3
4
http://museum.nist.gov/exhibits/adx2/index.htm
http://museum.nist.gov/exhibits/adx2/index.htm
http://www.batteryequaliser.com/behome.html
http://www.patentstorm.us/patents/5945236-description.html
5
Matter and Energy - Vocabulary
•
•
•
•
•
•
•
•
Chemistry
– Science that describes matter – its properties-composition-structure, the changes
it undergoes, and the energy changes that accompany those processes
Matter
– Anything that has mass and occupies space.
Energy
– The capacity to do work or transfer heat.
Chemical Properties - chemical changes
– rusting or oxidation
– chemical reactions
Physical Properties - physical changes
– changes of state
– density, color, solubility
Extensive Properties - depend on quantity
Intensive Properties - do not depend on quantity
Scientific (natural) law
– A general statement based the observed behavior of matter to which no
exceptions are known.
Natural Laws
• Law of Conservation of Mass – The notion that mass, or matter, can be
neither created nor destroyed.
• Law of Conservation of Energy – A law that states that in any system not
involving nuclear reactions or velocities approaching the velocity of light, energy cannot be
created or destroyed. The First Law of Thermodynamics.
• Law of Conservation of Mass – Energy - Einstein’s Relativity
- E=mc2 – The special theory of relativity, which has been verified by experiment, has
shown that the mass of a body changes as the energy possessed by the body changes. Such
changes in mass are too small to be detected except in subatomic phenomena. Matter may
be created by the materialization of a photon into an electron-positron pair; or it may be
destroyed, by the annihilation of this pair of elementary particles to produce a pair of
photons.
• Law of Definite Proportions – When two or more elements combine to form
a compound, their masses in that compound are in a fixed and definite ratio. This data
helps justify an atomic view of matter.
• Law of Multiple Proportions – When two elements combine to form more
than one compound, the mass of element A which combines in the first compound with a
given amount of element B has a simple whole number ratio with the mass of element A
which combines in the second compound with the same given mass of element B.
Dr. Stone’s patent pending chemistry problem solver
1. Write down everything you are given
•Vocabulary
•Numbers
•Units
2. Write down what you want to know
•Vocabulary
•Numbers
•Units
3. Write down mathematical equation(s) that include(s)
these values and units
•Principles
4. Write a balanced stoichiometric equation
•Mole concept
5. Convert everything to moles
•Dimensional analysis
6. Convert everything to the unknown’s units
•Rounding, significant figures, accuracy and precision
Compounds & Molecules
• COMPOUNDS are a combination of 2 or more elements in
definite ratios by mass.
• The character of each element is lost when forming a
compound.
• MOLECULES are the smallest unit of a compound that
retains the characteristics of the compound.
Composition of molecules is given by a
CHEMICAL FORMULA
C8H10N4O2 - caffeine
H2O
MOLECULAR FORMULAS
• Formula for glycine is C2H5NO2
• In one molecule there are
–2 C atoms
–5 H atoms
–1 N atom
–2 O atoms
WRITING FORMULAS
Chemical Formula – chemical symbols and number of each representing composition
Empirical Formula – simplest ratio of elements that does not represent the actual
number and is non-positional
Molecular Formula – chemical symbols and number of each representing
composition representing actual number but not position
Structural Formula - chemical symbols and number of each representing
composition representing actual number and position
• Can write glycine chemical formula as
– H2NCH2COOH
to show atom ordering
• or in the bond-line structural formula
H H O
H N C C O H
H
MOLECULAR MODELING
H H O
H N C C O H
H
Ball & stick
Bond-line Structural
formula of glycine
Space-filling
STRUCTURAL
FORMULA
BOND-LINE
FORMULA
IONS are atoms or groups of atoms with a positive or negative charge.
Taking away an electron from an atom gives a CATION with a positive charge
Adding an electron to an atom gives an ANION with a negative charge.
PREDICTING ION CHARGES
In general
•
metals (Mg) lose electrons ---> cations
•
nonmetals (F) gain electrons ---> anions
• Charges on Common Ions
• CATION + ANION → COMPOUND
• A neutral compound requires equal number of + and - charges.
Table of Common Ions
Common Positive Ions (Cations)
Monovalent
Hydronium
(or hydrogen)
Lithium
Sodium
Potassium
Rubidium
Cesium
Francium
Silver
Ammonium
Thalium
Copper I
O+
H3
H+
Li+
Na+
K+
Rb+
Cs+
Fr+
Ag+
NH4+
Tl+
Cu+
Divalent
Magnesium
Calcium
Strontium
Beryllium
Manganese II
Barium
Zinc
Cadmium
Nickel II
Palladium II
Platinum II
Copper II
Mercury II
Mercury I
Iron II
Cobalt II
Chromium II
Lead II
Tin II
Mg2+
Ca2+
Sr2+
Be2+
Mn2+
Ba2+
Zn2+
Cd2+
Ni2+
Pd2+
Pt2+
Cu2+
Hg2+
Hg22+
Fe2+
Co2+
Cr2+
Pb2+
Sn2+
Trivalent
Aluminium
Antimony III
Bismuth III
Al3+
Sb3+
Bi3+
Iron III
Cobalt III
Chromium III
Fe3+
Co3+
Cr3+
Table of Common Ions
Common Negative Ions (Anions)
Monovalent
Hydride
Fluoride
Chloride
Bromide
Iodide
Hydroxide
Permangante
Cyanide
Thiocynate
Acetate
Nitrate
Bisulfite
Bisulfate
Bicarbonate
Dihydrogen phosphate
Nitrite
Amide
Hypochlorite
Chlorite
Chlorate
Perchlorate
HFlClBrIOHMnO4CNSCNC2H3O2NO3HSO3HSO4HCO3H2PO4NO2NH2ClOClO2ClO3ClO4-
Divalent
Oxide
Peroxide
Sulfide
Selenide
Oxalate
Chromate
Dichromate
Tungstate
Molybdate
tetrathionate
Thiosulfate
Sulfite
Sulfate
Carbonate
Hydrogen phosphate
O2O22S2Se2C2O42CrO42Cr2O72WO42MoO42S4O62S2O32SO32SO42CO32HPO42-
Trivalent
Nitride
N3-
Phosphate
PO43-