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CHM 1010A - Chemistry I4 lecture hours 2 lab hours 4 credits
Course Description
This is a first-term general chemistry course designed for students who did not take chemistry in high school or who took high school chemistry more than five years ago. Students will design and conduct experiments, analyze and interpret data, and relate experimental results to theoretical understandings of chemical phenomena. Specifically, students will more thoroughly understand such subjects as atomic structure, periodic properties, basic chemical calculations, bonding, intermolecular forces, properties of gases, solutions, and types of chemical reactions (oxidation-reduction, acid-base, and precipitation). A brief overview of pH, chemical equilibria, corrosion, and rates of chemical reactions is included. These topics will be discussed with respect to real-world applications. This course meets the following Raider Core CLO requirement: Think Critically. (prereq: no high school chemistry or high school chemistry more than five years ago)
Course Learning Outcomes
Upon successful completion of this course, the student will be able to:
- Plan and create structured experiments
- Write proficiently in technical communications
- In a laboratory experiment, identify potential procedural errors
- Differentiate between precision and accuracy
- Interpret data to isolate trends
- Use the periodic table to determine electron configurations, trends in atomic radii, trends in ionic radii, ionization energy, electron affinity, and electronegativity
- Describe the formation and properties of ionic, covalent, and metallic bonding, including Lewis dot structures
- Predict Lewis dot structures, molecular geometry, and molecular polarity for molecules and polyatomic ions
- Compare melting points, solubility, and other physical properties for molecules using intermolecular forces
- Apply the law of conservation of mass to solve stoichiometric problems, including limited reagent problems
- Employ the gas laws, the kinetic theory of gases, and gas stoichiometry
- Explain the energy considerations in material changes, both physical and chemical
- Use solution chemistry, including molarity, dilutions, pH, and acid-base properties
- Qualitatively describe chemical equilibria and reaction rates
- Recognize acid-base, oxidation-reduction, and precipitation reactions
Prerequisites by Topic
Course Topics
- Classification and properties of matter, atomic structure, and periodic relationships
- Chemical bonding, Lewis dot structure, molecular geometry and polarity, and intermolecular forces
- Gases
- Mass and enthalpy relationships in chemical reactions
- Solutions, molarity, pH
- Types of chemical reactions (acid-base, oxidation-reduction and precipitation)
- Qualitative overview of chemical equilibrium, corrosion and reaction rates
Laboratory Topics
- Physical and chemical changes
- Density
- Properties of solids (ionic, molecular, metallic)
- Solution concentration and Beer’s law
- Molecular geometry and bonding
- Stoichiometry and limiting reactants
- Identification of a molecular unknown (intermolecular forces)
- Determination of the enthalpy of a reaction
- Determination of the atomic mass of aluminum (gas laws)
- Soaps and surfactants
- Types of chemical reactions
- Solubility
- Analysis of ions
Coordinator
Dr. Anne Alexander
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