| |
Jul 01, 2025
|
|
|
|
|
2021-2022 Catalog [ARCHIVED CATALOG]
|
CHEM 105 - General Chemistry I
PREREQUISITES: MATH 136 - College Algebra and demonstrated competency through appropriate assessment or earning a grade of “C” or better in ENGL 093 - Introduction to College Writing and ENGL 083 - Reading Strategies for College e or ENGL 095 - Integrated Reading and Writing , or ENGL 075 - Co-Requisite Integrated Reading & Writing
PROGRAM: Physical Sciences
CREDIT HOURS: 5
LECTURE HOURS: 3
LAB HOURS: 4
DATE OF LAST REVISION: Fall, 2019
The first in a series of two courses designed to cover general chemistry including measurement, atoms, molecules and ions, stoichiometry, chemical reactions, solids, liquids, and gases thermochemistry, atomic structure, and molecular bonding. One year of high school chemistry or one semester of college introductory chemistry is recommended. Includes lab.
MAJOR COURSE LEARNING OBJECTIVES: Upon successful completion of this course the student will be expected to:
- Explain and use measurement techniques including correct unit conversions, dimensional analysis, and significant figures.
- List the parts of an atom, classify matter, name those substances and discuss their place on the periodic table.
- Apply the concepts of stoichiometry including molar mass, percent composition, balancing equations and limiting reagents.
- Categorize chemical reactions and predict the products of common chemical reactions
- Describe the kinetic molecular theory of gases and apply the knowledge using accepted gas laws.
- Explain the basics of thermochemistry including enthalpy, calorimetry, Hess’s law, and standard enthalpies of formation.
- Interpret the quantum mechanical model of the atom including quantum numbers, orbital shapes, orbital energies, electron spin and the Pauli Principle as well as the periodicity, which rises from this model.
- Illustrate the basic concepts of ionic bonding and polar covalent bonding and their relationship to electron configuration, as related to the concepts of electronegativity, bond polarity and dipole moment.
- Compare the VSEPR model, the hybridization model and the molecular orbital model for covalent bonding.
- Identify intermolecular forces in the liquid state and relate how they affect solution formation, vapor pressure, boiling point and other colligative properties.
- Relate the general structure of solids especially molecular solids and ionic solids.
COURSE CONTENT: Topical areas of study include -
Scientific method
Measurements and Units
Significant figures
Density
Elements
Compounds
Mixtures
Nomenclature
Chemical reactions
Chemical equations
Precipitation reactions
Redox reactions
The mole
Molar mass
Stoichiometry
Limiting reagents
Properties of gases
Gas laws
Molecular motion
Energy, heat, enthalpy
Enthalpy of chemical reactions
Atomic structure
Orbital theory
Electron configurations
Periodicity
Ionic bonding
Covalent bonding
Lewis structures
Molecular structure
VSEPR model
Polarity
Bond strength and lengths
Valence bond theory
Molecular orbital theory
Intermolecular forces
Liquid structure
Solid structure
Phase changes
Solutions
Solubility
Colligative properties
Course Addendum - Syllabus (Click to expand)
|
|
