CH 221 General Chemistry 1

1. Estimate the uncertainties inherent in all scientific measurements and calculations and report answers to the correct number of significant figures 
2. Generate and test models in a logical and objective manner and use them to explain observed natural phenomena.
3. Collect, organize, analyze and interpret data and identify key trends and relationships.
4. Perform experiments safely, make clear observations, summarize data in tables, interface computers to chemical sensors, maintain a detailed laboratory notebook and write clear concise laboratory reports. 
5. Use units, conversion factors, formulas, balanced chemical equations, moles and mole ratios to solve many interesting, community-related and practical scientific problems. 
6. Explain the organization of the periodic table using electronic theory to predict the type of bonding (ionic, covalent or metallic) used by elements and compounds. 
7. Use VSEPR theory, hybridization concepts molecular orbital principles to assign the shape and polarity of molecules.
8. Critically think about periodic properties of the elements, energy flow in chemical systems and the role of intermolecular forces on the properties of liquids and solids. 

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.

• 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