Southern State Community College
Curriculum Committee – February 2012
CHEM 1151 – First Year Chemistry I
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I.
OTM: 14989
COURSE TITLE: First Year Chemistry I
COURSE NUMBER: 1151
II.
TAG: OSC008
CATALOGUE PREFIX: CHEM
PREREQUISITES: CHEM 1120 or one year of high school chemistry and high school algebra,
or its equivalents
COREQUISITE: CHEM 1161
III.
CREDIT HOURS: 4
LABORATORY HOURS: 0
IV.
COURSE DESCRIPTION
LECTURE HOURS: 4
OBSERVATION HOURS: 0
A college level chemistry course covering measurement, significant figures, moles, chemical
formulas, chemical equations, stoichiometry, acids and bases, oxidation-reduction,
thermochemistry, quantum mechanics, atomic orbitals, and bonding theories.
V.
ADOPTED TEXT:
Chemistry & Chemical Reactivity,
8th Edition,
By: Kotz, Treichel, and Townsend
Cengage Learning, 2010
ISBN: 1-111-57498-7
VI.
COURSE OBJECTIVES:
Upon completion of this course the student should be able to:
1.
2.
3.
4.
5.
Read, write and talk about chemistry using a basic chemistry vocabulary.
Express measurements and calculated values in the correct number of significant figures.
Solve problems pertaining to
a. unit conversions,
b. density,
c. moles,
d. the determination of empirical and molecular formulas,
e. reaction stoichiometry, and
f. solution concentration.
Demonstrate a fundamental understanding of atomic and molecular structure and the
periodic table.
Name and write chemical formulas for compounds.
CHEM 1151: First Year Chemistry I
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6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
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18.
19.
VII.
Balance the chemical equations associated with exchange reactions and oxidationreduction reactions.
Classify chemical reactions.
Demonstrate a basic understanding of aqueous solutions including acids and bases.
Demonstrate a fundamental understanding of the Bohr model of the atom, the wave
mechanical view of the atom, and the scientific developments that led to each.
Apply the Pauli exclusion principle and orbital energies to the writing of electron
configurations of atoms and ions.
List and explain the periodic trends.
Draw Lewis structures to represent bonding in molecules. Use electronegativities to
evaluate bond polarities.
Predict electron-pair and molecular geometries.
Discuss and compare the valence bond and molecular orbital theories.
Determine orbital hybridization from electron pair geometries.
Explain the advantages and disadvantages of molecular orbital theory.
Use molecular orbital theory to predict the stability of molecules
Discuss and apply the concepts of thermochemistry, the heat involved in chemical and
physical changes.
Solve problems pertaining to specific heat, heat capacity, enthalpy, and calorimetry.
COURSE METHODOLOGY:
This course will use lecture, Power Point, discussion, home work assignments, computer
assignments, and written exams and quizzes as deemed appropriate by instructor.
VIII. GRADING:
The following grading scale will be used:
A = 90 - 100
B = 80 – 89
C = 70 - 79
D = 60 - 69
F = < 60
IX. COURSE OUTLINE:
1.
The Tools of Chemistry
a. The definition of chemistry
b. The scientific method
c. The language of chemistry
d. Units of measurement
CHEM 1151: First Year Chemistry I
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e. Significant figures
f. Unit conversions
2.
Atoms and Elements
a. Elements
b. Atomic structure
c. Atomic weight
d. An introduction to the periodic table
e. Moles
3.
Compounds and Molecules
a. Molecular compounds and molecular formulas
b. Diatomic elements
c. Ions and ionic compounds
d. Nomenclature
e. Moles and molar mass
f. Laws of composition
g. Determination of a formula
4.
Chemical Reactions
a. Balancing chemical equations
b. Types of chemical reactions
c. Reaction stoichiometry
d. Limiting reagents
5.
Reactions in Aqueous Solutions
a. Properties of aqueous solutions
b. Acid-Base Theory
c. Balancing chemical equations for reactions in aqueous solution
d. Exchange reactions
e. Solution concentrations
f. Solution stoichiometry
g. Oxidation-reduction reactions
6.
Atomic Structure
a. Electromagnetic radiation
b. Quantization of energy
c. Atomic line spectra
d. The Bohr model of the atom
e. The quantum mechanical view of the atom
f. Atomic orbitals
7.
Atomic Electron Configurations and Periodicity
a. Electron spin and the Pauli exclusion principle
b. Orbital energies and electron assignments
CHEM 1151: First Year Chemistry I
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c. Electron configurations
d. Ion electron configurations
e. Periodic trends
8.
Chemical Bonding
a. Valence electrons
b. Chemical bond formation
c. Ionic and covalent bonding
d. Lewis structures
e. Bond properties
f. Electron-pair and molecular geometry
g. Molecular polarity
h. Valence bond and orbital hybridization theories
i. Molecular orbital theory
9.
Thermochemistry
a. Energy
b. Heat capacity and specific heat
c. Enthalpy
d. Calorimetry
COURSE CALENDAR:
Week #
1
Chapter
1
2
2
3
2
Topics/Assignments
1.1 Fundamental Definitions and Scientific Method
1.2 Units of measurement
1.3 Measurement
1.4 Mathematics of Chemistry – Dimensional Analysis, Significant
Figures, Scientific Notation
2.1 Atomic structure
2.2 Atomic number and atomic mass
2.3 Isotopes
2.4 Atomic Weight,
2.5 Periodic Table
2.6 Molecules, Compounds and Formulas
2.7 Ionic compounds
2.9 Mole concept
2.10 Percent composition, empirical and molecular formulas,
hydrates
CHEM 1151: First Year Chemistry I
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4
3
5
3 and 4
6
4
7
5
8
5
9
6
10
7
11
7
12
8
13
8
14
9
3.2 Balancing chemical reactions
3.4 Reactions in aqueous solutions
3.5 Ions and molecules in aqueous solutions
3.6 Precipitation reactions
3.7 Acids and Bases
3.8 Gas forming reactions
3.9 Oxidation reduction reactions
3.10 Classifying reactions in aqueous solutions
4.1 Mass relations in chemical reactions
4.2 Limiting reagents
4.3 Percent Yield
4.4 Chemical Equations and Chemical Analysis
4.5 Concentration of compounds in solutions
4.7 Stoichiometry of reactions in aqueous solution
4.8 Spectrophotometry
5.1 Energy-basic principles
5.2 Specific heat capacity
5.3 Changes of state
5.4 First Law of Thermodynamics
5.5 Enthalpy changes for chemical reactions
5.7 Enthalpy calculations – Hess’s Law
5.8 Calorimetry
6.1 Electromagnetic radiation
6.2 Quantization
6.3 Atomic line spectra – Bohr model
6.4 Particle-Wave Duality
6.5 Quantum Mechanics
6.6 Atomic orbitals
6.7 Electron spin
7.1 Pauli Exclusion principle
7.2-7.4 Electron Configurations of atoms and ions
7.5 Periodic Trends and Chemical properties
Applications of Periodic Table to Industry
8.1 Chemical Bond Formation
8.2 Lewis structures
8.3 Formal Charges
8.4 Resonance
8.5 Exceptions to the Octet Rule
8.6 Molecular Shapes – VSEPR
8.7 Bond polarity and Electronegativity
8.8 Bonds and Molecular Polarity
8.9 Bond Properties
DNA Revisited
9.1 Orbitals and Theories of Bonding
9.2 Valence Bond Theory
CHEM 1151: First Year Chemistry I
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15
9
16
9.3 Molecular Orbital Theory
Final
X. OTHER REQUIRED BOOKS AND MATERIALS:
A calculator is required.
XI. EVALUATION
Discretion of instructor
XII.
SPECIFIC MANAGEMENT REQUIREMENTS:

You may not use programmable calculators or cell phone calculators for tests.

Please understand that your work may be seen by others. Others may see your work when
being distributed, during group project work, or if it is chosen for demonstration purposes.
There is also a possibility that your papers may be submitted electronically to other entities,
for reasons such as for plagiarism checks.

ACADEMIC MISCONDUCT: Any student who commits any type of academic misconduct
as stated in the current college catalogue will receive an "F" for the exam, quiz, or evaluated
project.
XIII. OTHER INFORMATION
FERPA: Students need to understand that your work may be seen by others. Others may see
your work when being distributed, during group project work, or if it is chosen for
demonstration purposes. Students also need to know that there is a strong possibility that your
work may be submitted to other entities for the purpose of plagiarism checks.
DISABILITIES: Students with disabilities may contact the Disabilities Service Office,
Central Campus, at 800-628-7722 or 937-393-3431.