Jul 25, 2025  
Catalog 2025-2026 
    
Catalog 2025-2026

CH 221Z General Chemistry 1


Lecture Hours: 3 Lecture and 1 Recitation
Credits: 4

 Explores and applies principles and applications of chemistry. Emphasis on measurement, components of matter, atomic and molecular structure, quantitative relationships including foundational stoichiometry, and major classes of chemical reactions. CH 221Z is a lecture course; CH 227Z is the laboratory component. 

Prerequisite: Placement into WR 115  (or higher), or completion of WR 090  (or higher); and placement into MTH 112Z  (or higher); or completion of MTH 111Z  (or higher); or consent of instructor. (All prerequisites must be completed with a grade of C or better.).
Concurrent: Concurrent enrollment in CH 227Z  
Differential Fee YES
Student Learning Outcomes:
Common Course Number Outcomes

  1. Describe the phases and classifications of matter and differentiate between physical and chemical properties.
  2. Represent physical measurements using SI and derived units and demonstrate systematic problem-solving including unit conversion.
  3. Use the periodic table to solve problems in chemistry.
  4. Describe the principles of electromagnetic energy, the Bohr model and quantum theory, and use electron configurations to identify periodic variations in chemical properties.
  5. Interpret and apply ionic and covalent bonding theories including Lewis structures, formal charges, resonance, molecular structure, and polarity.
  6. Quantify the composition of substances and solutions.
  7. Identify and name a variety of elements, ions, ionic compounds, and covalent compounds.
  8. Write, balance, and classify chemical reactions and solve foundational stoichiometry calculations.

Statewide General Education Outcomes:

  1. Gather, comprehend, and communicate scientific and technical information in order to explore ideas, models, and solutions and generate further questions.
  2. Apply scientific and technical modes of inquiry, individually, and collaboratively, to critically evaluate existing or alternative explanations, solve problems, and make evidence-based decisions in an ethical manner.
  3. Assess the strengths and weaknesses of scientific studies and critically examine the influence of scientific and technical knowledge on human society and the environment.


Content Outline
  • Keys to the Study of Chemistry
    • Properties of matter
    • Chemical arts and the origins of modern chemistry
    • Scientific approach: developing a model
    • Chemical problem solving
    • Measurements, uncertainty and significant figures
  • Components of Matter
    • Elements, compounds and mixtures: an atomic overview
    • Observations that led to an atomic view of matter
    • Dalton’s Atomic Theory
    • Compounds: Bonding, formulas, names and masses
    • Classification and Separation of Mixtures
  • Quantum Theory and Atomic Structure
    • Wave-Particle Duality of Matter and Energy
    • Atomic Spectra and the Bohr Model of the Hydrogen Atom
    • Quantum-Mechanical Model of the Atom
  • Models of Chemical Bonding
    • Atomic Properties and Chemical Bonds
    • Ionic and Covalent Bonding Models
    • Between the Extremes: Electronegativity and Bond Polarity
    • Molecular Shape and Polarity
    • Valence Bond Theory and Orbital Hybridization
    • Orbital Overlap and Types of Covalent Bonds
  • Stoichiometry: Mole-Mass-Number Relationships in Chemical Systems
    • The mole
    • Determining the formula of an unknown compound
    • Writing and balancing chemical equations and calculating the amounts of reactants and products
  • Electron Configuration and Chemical Periodicity
    • Development of the Periodic Table Using the Quantum-Mechanical Model
    • Characteristics of Many-Electron Atoms
    • Trends in Some Key Periodic Atomic Properties
    • The Connection Between Atomic Structure and Chemical Reactivity
  • Intermolecular Forces: Liquids, Solids and Phase Changes
    • Qualitative and Quantitative Aspects of Phase Changes: Phase Diagrams
    • Types of Intermolecular Forces
    • IM Forces and Predicting Solubility
    • Properties of the Liquid State: The Uniqueness of Water
  • Laboratory Experiments
    • Laboratory Basics
    • Volumes of Liquids
    • Spectrophotometry of Solutions
    • Reaction Cycles of a Metal
    • Properties and Formula of a Hydrate
    • Lewis Structures and Molecular Models
    • Determination of an Empirical Formula
    • Rates of Evaporation and Intermolecular Forces
    • Chromatography