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May 07, 2024
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2022-2023 Catalog [ARCHIVED CATALOG]
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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 MIN: 5
LECTURE HOURS MIN: 3
LAB HOURS MIN: 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)
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