Fall 2011
General Chemistry for Science Majors
(Prerequisite: MATH 1100 or equivalent)
Lecture: CHEM 1410.007: TR, 8:00-9:20 AM, Chemistry 109
Recitation CHEM 1410.271: T, 3:00 – 3:50, Chemistry 109
Recitation CHEM 1410.272: T, 11:00-11:50 AM, Chemistry 235
Professor:
E-mail:
Office:
Office hours:
FAX:
Dr. Diana Mason
[email protected]
Science Research Building (SRB) 240 (Walk-ins are welcome)
CHEM 235A, Tuesday and Thursday, 9:30 – 10:20 AM
(940) 565-4318
TA:
E-mail:
Office:
Office hours:
Carrie Moore
[email protected]
Chemistry Building (CHEM) 173
Wednesday, 1:00 – 2:00 PM and Thursday, 1:00 – 2:00 PM
Suggested:
Moore, Stanitski, and Jurs: Principles of Chemistry: The Molecular Science
There are several excellent online homework systems that you might like to
subscribe to. They are NOT FREE! Sapling, OWL and ALEKS are
suggestions of programs you should look at, if you need help. There
are no grades associated with doing online homework.
Sapling: http://www.saplinglearning.com/
OWL: http://www.cengage.com/owl/
ALEKS: http://www.aleks.com/
Web pages:
http://www.chem.unt.edu/faculty/mason.htm
https://ecampus.unt.edu/webct/entryPage.dowebct
REQUIRED: Internet access and Blackboard Vista access are required for this course.
(Homework from Sapling Learning is required.)
Exam Dates: Exam 1
Exam 2
Exam 3
Exam 4
Final Exam
September 22 (Thursday): Lessons 1-7
October 27 (Thursday): Lessons 8-14
November 10 (Thursday): Lessons 15-20
December 1 (Thursday): Lessons 21-24
December 15 (Thursday): 7–10 AM (Chapters 1-11)
No exam grades are dropped! If you miss an exam, the grade on your final exam replaces the missing grade!
Catalog Description
Fundamental concepts, states of matter, periodic table, structure and bonding, stoichiometry,
oxidation and reduction, solutions, and compounds of representative elements.
Grade Allocation
Keep all returned assignments in case there is any discrepancy regarding your final course grade!
Your average is based on the number of points you receive out of the total possible points.
Possible points will be obtained from your homework, exams, and other exercises when deemed
appropriate.
Your letter grade in this course will be based on the following scale:
A = 90-100%; B = 80 – 89%; C = 70 – 79%; D = 60 –69%; F < 60%.
Failure to turn in completed assignments by the due date and time will result in a zero for the
missing grade.
Important University Dates
August 31
Last day to add a class or change a schedule
September 5
Labor Day (no class)
September 8
Census Day/12th Class Day
Last day to drop a class without instructor approval
September 9
Instructor approval required to drop and receive W
October 4
Last day to change to pass/no pass status
October 5
WF for non-attendance may be given
October 28
Last day to drop (written consent of instructor required)
November 18
Last day of WF for non-attendance
Last day to withdraw from the university (5 PM deadline)
November 24-27
Thanksgiving Holidays
December 3-9
Pre-final exam week
December 9
Reading Day (no classes)
December 17
Fall Commencement
Course Objectives
(1)
Upon successful completion of Chem I, students should be able to adhere to the rules of significant digits and
express answers in both decimal and scientific notations.
(2)
Upon successful completion of Chem I, students should understand the underlying concepts associated with
the early and modern atomic theories and their applications to the periodic table and basic chemical reactions
along with how elements combine to form different structures.
(3)
Upon successful completion of Chem I, students should be able to name elements and compounds,
understand the connections between a balanced chemical equation and mass/molar quantities, and the
importance of chemistry as the central science.
(4)
Upon successful completion of Chem I, students should be able to solve problems related to the concepts of
density, heat, stoichiometric relationships, gas laws, and solubility.
Student Learning Objectives: General Chemistry (based on topics listed by the ACS Exams Institute)
1. Students will be able to apply measurements, scientific notation and significant figure rules to all
algorithmic-based problems.
2. Students will be able to perform all types of elementary conversions.
3. Students will be able to identify and describe matter and subatomic particles of isotopes.
4. Students will be able to write and be able to determine chemical/empirical formulas for most
inorganic compounds and select groups of organic compounds.
5. Students will be able to name most inorganic compounds and select groups of organic compounds.
6. Students will be able to balance chemical equations and identify the major types of chemical
reactions.
7. Students will be able to solve basic stoichiometry problems.
8. Students will be able to identify oxidation numbers of all atoms in common compounds.
9. Students will be able to identify the components contributing to the chemistry (solubility,
acids/bases, etc.) of most compounds.
10. Students will be able to determine concentrations of various solutions considering molarity and
molality with stoichiometric relationships.
11. Students will be able to solve thermochemical equations.
12. Students will be able to write electron configurations and understand basic quantum number rules.
13. Students will be able to differentiate between ionic and covalent bonding and know the identifying
factors of each.
14. Students will be able to explain the periodic trends including, but not limited to, atomic radius,
ionization energy, electron affinity, and electronegativity
15. Students will be able to draw Lewis structures, including isomers, resonance, and determine
formal charges.
16. Students will be able to apply VSEPR theory to determine the electronic and molecular topology
of simple compounds.
17. Student will be able to solve gas laws and gas stoichiometry problems.
18. Student will be able to describe common physical and chemical properties of solids, liquids, and
gases.
19. Students will assess the concepts of intermolecular forces and how these forces affect structure
and function of molecules.
Class Policies
1. You should enroll in both lecture (with recitation) and a lab (with lecture). CHEM 1430.00x (Lab Lecture) +
CHEM 1430.3xx (Lab) are separate courses form CHEM 1410.00x + CHEM 1410.2x1 (or 1410.2x2) Students
receive separate grades for the lecture and lab courses. Dropping either course does NOT automatically drop a
student from the other course.
2. Calculators are permitted for use in class and on exams. Calculators may never be shared during an exam.
3. By University regulations, a grade of “I” cannot be given as a substitute for a failing grade in a course.
4. There are no “extra credit” assignments given to an individual that are not available to the entire class.
5. Attend class—lectures and recitations, labs and lecture for labs. You are responsible for all information
presented in class regardless of your attendance. Some of the information discussed in class is not in your
textbook and you are still very much responsible for this information! No make-up work is provided. If you fail
to attend an exam (regardless of excuse), the same percentage as your final exam grade will be calculated in its
place.
Study Groups
You are strongly encouraged to form study groups. Practicing the language of chemistry by “talking” chemistry with
others is a very easy and painless way to help you understand the concepts covered in this course.
POLICY STATEMENTS
ADA COMPLIANCE: In cooperation with the Office of Disability Accommodation (ODA) reasonable
accommodations for qualified students with registered disabilities will be made. If applicable, please present your
request, with written verification from the ODA, prior to the first exam. See: http://policy.unt.edu/policy/18-1-14
o “The University of North Texas is on record as being committed to
both the spirit and letter of federal equal opportunity
legislation; reference Public Law 92-112 – The Rehabilitation Act
of 1973 as amended. With the passage of new federal legislation
entitled Americans with Disabilities Act (ADA), pursuant to
section 504 of the Rehabilitation Act, there is renewed focus on
providing this population with the same opportunities enjoyed by
all citizens.”
o The University of North Texas complies with Section 504 of the 1973 Rehabilitation Act
and with the Americans with Disabilities Act of 1990. The University of North Texas
provides academic adjustments and auxiliary aids to individuals with disabilities, as
defined under the law. Among other things, this legislation requires that all students with
disabilities be guaranteed a learning environment that provides for reasonable
accommodation of their disabilities. If you believe you have a disability requiring
accommodation, please see the instructor and/or contact the Office of Disability
Accommodation at 940-565-4323 during the first week of class.
SCHOLASTIC DISHONESTY: The University expects every student to maintain a high standard of individual
integrity for work done. Scholastic dishonesty is a serious offense, which includes, but is not limited to, cheating on
a test or other class work, plagiarism (the appropriation of another’s work and the unauthorized incorporation of that
work in one’s own work), and collusion (the unauthorized collaboration with another person in preparing college
work offered of credit). In cases of scholastic dishonesty, the faculty member responsible for the class may initiate
disciplinary proceedings against the student. In this class all UNT procedures will be followed and the necessary
paperwork will be filed with the Academic Integrity Office. In the case of an infraction, a penalty will be
recommended by the professor of this course to the Academic Integrity Officer, who may impose an additional
university penalty. (See: http://www.vpaa.unt.edu/academic‐integrity.htm)
DISCLAIMER: The professor of this course reserves the right to alter at any time any of the information
presented on this syllabus at her discretion. If you are not in class, you may miss important information that
directly affects your grade in this course!
Grades are not wages. They are not intended to reflect how hard you worked or how good your
intentions were. They are intended to reflect your mastery of the material relative to this class,
other classes (elsewhere and else-when), and to reflect what I believe you ought to have achieved
to attain a particular grade.
Lessons are available on Blackboard Vista!
Schedule of Events for Chemistry 1410.007 (Mason)
Fall 2011
Activity
L1
L2
R1
L3
L4
R2
L5
L6
R3
L7
L8
R4
E1
L9
R5
L10
L11
R6
L12
L13
R7
L14
L15
R8
L17
L16
R9
E2
L18
R10
L19
L20
R11
E3
L21
R12
L22
L23
R13
L24
R14
E4
L25
R15
L26
E5
Date
8/25
8/30
8/30
9/1
9/6
9/6
9/8
9/13
9/13
9/15
9/20
9/20
9/22
9/27
9/27
9/29
10/4
10/4
10/6
10/11
10/11
10/13
10/18
10/18
10/20
10/25
10/25
10/27
11/1
11/1
11/3
11/8
11/8
11/10
11/15
11/15
11/17
11/22
11/22
11/29
11/29
12/1
12/6
12/6
12/8
Chpts
1
1
12/15
1-11
2
2
3
3
3
4
1-3
4
4
5
5
6
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4-6
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10-11
12
Topics/Assignments:
Assessments
Matter (Lesson 01: Blackboard Vista)
Demographic Surveys*
History (Lesson 02: Blackboard Vista)
Pre-tests*
Week 01: Matter & Density
Atomic Structure
Significant Figures (Lesson 03: Blackboard Vista)
Week 02: Subatomics
Dimensional Analysis
Nomenclature (Lesson 04: Blackboard Vista)
Week 03: Problem Solving
Hydrocarbons
Moles (Lesson 05: Blackboard Vista)
Week 04: Naming
Exam 1
Balancing Equations
Week 05: Percent Composition
Stoichiometry (Lesson 06: Blackboard Vista)
Reactions
Week 06: Combustion Analysis
Solutions (Lesson 07: Blackboard Vista)
Energy and Heat
Week 07: Limiting Reactant
Thermochemistry (Lesson 08: Blackboard Vista)
Quantum (Lesson 09: Blackboard Vista)
Week 08: Hess's Law
Electron Configuration
Bonding
Week 09: Quantum Mechanics
Exam 2
Lewis Structures (Lesson 10: Blackboard Vista)
Week 10: Electron Behavior
Hydridization (Lesson 11: Blackboard Vista)
Special Bonding (Lesson 12: Blackboard Vista)
Week 11: Hybridization
Exam 3
Gas Laws
Week 12: Gas Laws
Partial Pressures
Phases and Changes (Lesson 13: Blackboard Vista)
Week 13: Partial Pressures & Heat Problems
Heat Curves
Practice for Final Exam
Exam 4
Applications (Lesson 14: Blackboard Vista)
Review for Final Exam
Post-tests**
Review for Final Exam
Post-tests**
Final Exam, 7-10 AM
*Pre-tests:
Demographic Survey
ACS California Chemistry Diagnostic Test (1997)
Group Assessment of Logical Thinking (GALT)
**Post-tests: Attitude Survey
GALT
ACS California Chemistry Diagnostic Test (1997)
Delayed post-test given in January 2012 semester to all students enrolled in General Chemistry II during
laboratory recitation: ACS Paired Questions Exams: First term (2005)
Daily Lesson Objectives as
Supported by the Texas College and Career Readiness Standards
II. Foundation Skills: Scientific Applications of Mathematics
VII. Chemistry: SCIENCE STANDARDS
Lecture 1: Matter
A. Matter and its properties
1. Know that physical and chemical properties can be used to describe
and classify matter.
a. Distinguish between physical properties (e.g., density, melting point) and
chemical properties (e.g., ability to react, combustibility). Know that
chemical changes create new substances (e.g., rusting), while physical
changes do not (e.g., boiling).
b. Understand that, as an intrinsic property, density does not change as
sample size is changed, and be able to perform density calculations.
2. Recognize and classify pure substances (elements, compounds) and
mixtures.
a. Describe separation techniques for both mixtures and compounds.
b. Distinguish between homogeneous and heterogeneous mixtures.
c. Understand that, as an intrinsic property, density does not change as
sample volume is changed, and be able to perform density calculations.
Lecture 2: History
B. Atomic structure
1. Summarize the development of atomic theory. Understand that models
of the atom are used to help us understand the properties of elements
and compounds.
a. Describe the discoveries of Dalton (atomic theory), Thomson (the
electron), Rutherford (the nucleus), and Bohr (planetary model of the
atom); understand how each discovery contributed to modern atomic
theory.
Lecture 3: Atomic Structure
B. Atomic structure
1. Summarize the development of atomic theory. Understand that models
of the atom are used to help us understand the properties of elements
and compounds.
b. Identify the masses, charges, and locations of the major components of
the atom (protons, neutrons, and electrons); describe Rutherfordʼs “gold
foil” experiment that led to the discovery of the atomic nucleus; describe
Millikanʼs “oil drop” experiment that led to determining the charge on an
electron
Lecture 4: Significant Figures
F. Scientific measurement
1. Select and use appropriate Standard International (SI) units and
prefixes to express measurements for real-world problems.
2. Use appropriate significant digits.
Lecture 5: Dimensional Analysis
B. Mathematics as a symbolic language
1. Carry out formal operations using standard algebraic symbols and
formulae.
2. Represent natural events, processes, and relationships with algebraic
expressions and algorithms.
D. Scientific problem solving
1. Use dimensional analysis in problem solving.
Lecture 6: Nomenclature
F. Chemical nomenclature
1
Know formulas for ionic compounds.
a. Name and write formulas for binary and ternary ionic compounds, using
Group A (representative) metals and Group B (transition) metals, including
those containing common polyatomic ions, (e.g., nitrate, sulfate,
carbonate, ammonium, phosphate, hydroxide).
2. Know formulas for molecular compounds.
a. Name and write formulas for binary molecular compounds and acids.
b. Categorize a compound as ionic or molecular.
Lecture 7: Periodic Table and Hydrocarbons
C. Periodic table
1. Know the organization of the periodic table.
a. Identify periods and groups on the periodic table.
b. Identify metals, metalloids, and nonmetals on the periodic table.
c. Distinguish between and describe patterns in electron configurations for
representative elements, transition elements, inner-transition elements,
and noble gases. Predict the common charges on the representative
elements from the periodic table.
J. Basic structure and function of biological molecules: proteins,
carbohydrates, lipids, and nucleic acids
1. Understand the major categories of biological molecules: proteins,
carbohydrates, lipids, and nucleic acids.
a. Recognize each type of biological molecule by its structural formula, and
describe simple chemical tests or procedures to detect, identify, or
characterize each type.
Lecture 8: Moles
G. The mole and stoichiometry
1. Understand the mole concept.
a. Use Avogadroʼs number and molar mass to convert to moles of a
substance. Determine the percent composition of a compound. Calculate
the empirical formula of a compound from mass or percent composition
data.
Lecture 9: Balancing Equations
E. Chemical reactions
3. Understand oxidation-reduction reactions.
a. Differentiate between oxidation and reduction, and between oxidizing
agent and reducing agent.
b. Understand the consequences of corrosion processes and define and
describe the electroplating process.
c. Determine the oxidation number of any atom in an element, ion, or
compound.
Lecture 10: Stoichiometry
G. The mole and stoichiometry
2. Understand molar relationships in reactions, stoichiometric
calculations, and percent yield.
a. Construct mole ratios for a reaction to calculate the reactant amounts
needed or product amounts formed in terms of moles or mass.
b. Calculate percent yield, theoretical yield, or actual yield for a reaction.
Lecture 11: Reactions
E. Chemical reactions
1. Classify chemical reactions by type. Describe the evidence that a
chemical reaction has occurred.
a. Write equations for chemical reactions using appropriate symbols and
balance the equations by applying the Law of Conservation of Mass. Write
net ionic equations.
b. Predict the products of a reaction that fall within the five general types of
chemical reactions (synthesis, decomposition, single replacement, double
replacement, and combustion).
c. Use an activity series to predict whether a single replacement reaction will
occur.
d. Use solubility rules to determine the precipitate formed in a double
replacement precipitation reaction.
Lecture 12: Solutions
E. Chemical reactions
1. Classify chemical reactions by type. Describe the evidence that a
chemical reaction has occurred.
c. Distinguish between the Arrhenius and Br∅nsted definitions of acids and
bases. Identify conjugate acid-base pairs.
d. Describe how a titration is performed and how this process can be used to
determine the concentration of an unknown acid or base solution.
Lecture 13: Energy and Heat
E. Chemical reactions
5. Understand energy changes in chemical reactions.
a. Distinguish between endothermic and exothermic reactions. Draw energy
diagrams for endothermic and exothermic reactions.
b. Describe the Law of Conservation of Energy.
Lecture 14: Thermochemistry
H. Thermochemistry
1. Understand the Law of Conservation of Energy and processes of heat
transfer.
a. Distinguish among radiation, convection, and conduction as means of heat
transfer.
b. Describe processes of heat transfer.
c. Perform calculations involving heat transfer, using specific heat and latent
heat (phase changes).
2. Understand energy changes and chemical reactions.
a. Describe and give examples of renewable and non-renewable energy
resources.
b. Describe endothermic and exothermic reactions.
Lecture 15: Quantum
B. Atomic structure
1. Summarize the development of atomic theory. Understand that models
of the atom are used to help us understand the properties of elements
and compounds.
c. Describe basic wave properties (calculate wavelength, frequency, or
energy of light) and understand that electrons can be described by the
physics of waves.
d. Explain the importance of quantized electron energy and its relationship to
atomic emission spectra.
e. Understand the electron configuration in atoms (Aufbau principle, the Pauli
exclusion principle, Hund's rule) and their connection with the periodic
table.
Lecture 16: Electron Configuration
C. Periodic table
2. Recognize the trends in physical and chemical properties as one moves
across a period or vertically through a group.
a. Define and describe the periodic trend: atomic radii, ionic radii, ionization
energy, electron affinity, and electronegativity.
b. Use the periodic trends to compare the size and behavior of atoms and
ions.
Lecture 17: Bonding
D. Chemical bonding
1. Characterize ionic bonds, metallic bonds, and covalent bonds. Describe
the properties of metals and ionic and covalent compounds.
c. Describe nonpolar and polar covalent bonds. Use a chart of
electronegativities to determine bond polarity.
d. Determine if a molecule is polar (contains a dipole moment).
Lecture 18: Lewis Structures
D. Chemical bonding
1. Characterize ionic bonds, metallic bonds, and covalent bonds. Describe
the properties of metals and ionic and covalent compounds.
a. Draw Lewis dot structures for simple molecules, including simple
hydrocarbons.
Lecture 19: Hybridization
D. Chemical bonding
1. Characterize ionic bonds, metallic bonds, and covalent bonds. Describe
the properties of metals and ionic and covalent compounds.
b. Use Valence Shell Electron Pair Repulsion (VSEPR) model to predict
molecular shapes.
Lecture 20: Special Bonding
C. Understand relationships among geometry, algebra, and
trigonometry
4. Understand basic geometric principles
Use geometric principles to predict molecular angles
Lecture 21: Gas Laws
I. Properties and behavior of gases, liquids, and solids
1. Understand the behavior of matter in its various states: solid, liquid,
gas.
a. Describe how gas pressure is affected by volume, temperature, and the
addition of gas.
3. Understand principles of ideal gas behavior and kinetic molecular
theory.
a. Use kinetic molecular theory to explain how gas pressure is affected by
volume, temperature, and the addition of gas.
b. Distinguish between real and ideal gas behavior, and identify the criteria in
the kinetic molecular theory that conflict with the properties of real gases.
Lecture 22: Partial Pressures
I. Properties and behavior of gases, liquids, and solids
4. Apply the concept of partial pressures in a mixture of gases.
a. Use Daltonʼs Law to determine the partial pressure of a gas in a mixture of
gases.
Lecture 23: Phases and Changes
I. Properties and behavior of gases, liquids, and solids
2. Understand properties of solutions.
b. Calculate the molarity and molality of solutions.
5. Know properties of liquids and solids.
a. Describe the properties of liquids (e.g., surface tension, capillary action).
b. Describe the structure of solids (e.g., crystal lattice structure, unit cell,
amorphous solids).
7. Describe intermolecular forces.
a. Distinguish between dispersion forces, dipole interactions, and hydrogen
bonding. Identify the most important intermolecular force acting on a
substance.
Lecture 24: Heat Curves
I. Properties and behavior of gases, liquids, and solids
6. Understand the effect of vapor pressure on changes in state; explain
heating curves and phase diagrams.
a. Define boiling, freezing, sublimation, etc.
b. Explain heating curves and phase diagrams.
Lecture 25: Applications
I. Properties and behavior of gases, liquids, and solids
2. Understand properties of solutions.
a. Describe factors affecting solubility, units of concentration, colligative
properties, and colloids.
c. Determine boiling point elevation and freezing point depression for a
solution.