The Concepts in Chemistry course at JAHS is a collaboration with the University of Pitt at Bradford, through the College in High School program.

Its purpose is to provide the opportunity to earn college credits while in high school for a small fraction of the cost of regular tuition. The course syllabus is derived from the UPB course. It may not follow the order or timeline of the actual UPB course due to scheduling differences and instructor preferences.

UPB Course syllabus:

UPB example tests and answers.

Unit 1: Introduction and Laboratory Safety
chem lab.jpeg
chem lab.jpeg

  1. Course introduction: fields and uses for chemistry
  2. Classroom tour of lab safety devices
  3. Review of Rules, Safety Contract
  4. General Equipment usage and care: see this online quiz.





Unit 2: Properties of Matter
  1. Observations: qualitative vs. quantitative; direct vs. indirect
  2. Classification of matterphysical versus chemical properties
  3. metals and alloys: properties of metals and nonmetals
  4. The Scientific Method


Unit 3: Measurement and Uncertainty
measure.jpeg
measure.jpeg

  1. base units and prefixes
  2. metric system conversions
  3. English-metric conversions
  4. accuracy versus precision
  5. proper measurement
  6. significant figures
  7. calculations using significant figures




Unit 4: Discovery of Atomic Structure
nucleus.jpeg
nucleus.jpeg

  1. Dalton's Atomic Theory (Democritus was first!)
  2. Discovering electricity, radiation, and isotopes
  3. J. J. Thomson and electrons: his CRT, plum pudding model
  4. Rutherford and his gold foil experiment
  5. Bohr and his planetary model, emission theory
  6. The nucleus: atomic symbols
  7. Modern atomic structure





Unit 5: The Electronic Structure of the Elements
spectra.jpeg
spectra.jpeg

  1. the wave-particle theory and quantization
  2. predictions using electronic structure:



Unit 6: The Ionic Bond
salts.jpeg
salts.jpeg

  1. ionic compound nomenclature
  2. crystalline structures
  3. hydrates
  4. solubility of ionic compounds
  5. ionic compounds in chemical reactions (double replacement)
    • how to write and balance a chemical equation
  6. predicting products of double replacement reactions:
    • precipitate reactions
    • acid-base reactions
  7. precipitate and titration reactions


Unit 7: Periodic Trends
trends.jpeg
trends.jpeg

  1. chemical activity
  2. atomic radius
  3. electronegativity trends
  4. ionization energy (oxidation) and electron affinity (reduction)


Unit 8: Covalent Bonding
covalent.jpeg
covalent.jpeg

  1. covalent compound nomenclature
  2. Lewis diagrams and a view into combustion reactions
  3. VSEPR and 3D models of compounds - a look at
  4. Polarity of bonds
  5. intermolecular forces - relating structure to physical properties
  6. solubility of covalent compounds


Unit 9: Gases
gases.jpeg
gases.jpeg

  1. Phlogiston Theory
  2. the Kinetic Molecular Theory
  3. pressure and temperature units, conversions
  4. Boyle's, Charles' and Avogadro's Laws
  5. the Ideal Gas Law
  6. Dalton's Law of Partial Pressures






Unit 10: Chemical Formulas and the mole unit
mole.jpeg
mole.jpeg

  1. formula weights
  2. percent composition (decomposition reactions)
  3. empirical formulas
  4. Avogadro's Number
  5. mass to mole to number of conversions
  6. solution concentrations








Unit 11: Stoichiometry
  1. mole ratios in chemical formulas and equations
    stoich.jpeg
    stoich.jpeg
  2. using mass conversions with the mole ratio
  3. using stoichiometry to determine:
    • theoretical yields (thus percent yields) - synthesis reactions
    • limiting reactants (thus excess reactants)
  4. solution and gas stoichiometry
  5. practice problems in stoichiometry


Unit 12: Solutions
  1. notes on solutions
  2. calculating solution concentrations
  3. performing dilutions
  4. colligiative properties of solutions