Chemistry Exam Notes

Unit 1

  • Nuclear Chemistry
  • Differentiate between physical and chemical changes and properties.
  • Compare solids, liquids, and gasses in terms of:
    • Compressibility
    • Structure
    • Shape
    • Volume
  • Classify matter as pure substances or mixtures through investigation of their properties.
  • Explain everyday examples that illustrate the four laws of thermodynamics.
  • Investigate the process of heat transfer using calorimetry.
  • Classify processes as:
    • Exothermic
    • Endothermic
  • Represent energy changes that occur in chemical reactions using:
    • Thermochemical equations
    • Graphical analysis
  • Perform calculations involving:
    • Heat
    • Mass
    • Temperature change
    • Specific heat

Unit 2

  • Construct an argument to support how periodic trends such as electronegativity can predict bonding between elements.
  • Name and write the chemical formulas for ionic and covalent compounds using International Union of Pure and Applied Chemistry (IUPAC) nomenclature rules.
  • Classify and draw electron dot structures for molecules with:
    • Linear
    • Bent
    • Trigonal planar
    • Trigonal pyramidal
    • Tetrahedral molecular geometries as explained by Valence Shell Electron Pair Repulsion (VSEPR) theory
  • Analyze the properties of ionic, covalent, and metallic substances in terms of intramolecular and intermolecular forces.

Unit 3

  • Describe the characteristics of alpha, beta, and gamma radioactive decay processes in terms of balanced nuclear equations.
  • Compare fission and fusion reactions.
  • Give examples of applications of nuclear phenomena such as:
    • Nuclear stability
    • Radiation therapy
    • Diagnostic imaging
    • Solar cells
    • Nuclear power

Unit 4

  • The Moles and The Solutions
  • Define mole and apply the concept of molar mass to convert between moles and grams.
  • Calculate the number of atoms or molecules in a sample of material using Avogadro’s number.
  • Calculate percent composition of compounds.
  • Differentiate between empirical and molecular formulas.
  • Describe the unique role of water in solutions in terms of polarity.
  • Distinguish among types of solutions, including:
    • Electrolytes and nonelectrolytes
    • Unsaturated, saturated, and supersaturated solutions
  • Investigate how solid and gas solubilities are influenced by temperature using solubility curves and how rates of dissolution are influenced by temperature, agitation, and surface area.
  • Investigate the general rules regarding solubility and predict the solubility of the products of a double replacement reaction.
  • Calculate the concentration of solutions in units of molarity.
  • Calculate the dilutions of solutions using molarity.

Unit 5

  • Chemical Reactions & Stoichiometry
  • Interpret, write, and balance chemical equations, including:
    • Synthesis
    • Decomposition
    • Single replacement
    • Double replacement
    • Combustion reactions using the law of conservation of mass
  • Perform stoichiometric calculations, including determination of:
    • Mass relationships
    • Gas volume relationships
    • Percent yield
  • Describe the concept of limiting reactants in a balanced chemical equation.

Unit 6

  • Gas Laws
  • Describe the postulates of the kinetic molecular theory.
  • Describe and calculate the relationships among volume, pressure, number of moles, and temperature for an ideal gas.
  • Define and apply Dalton’s law of partial pressure.

Unit 7

  • Acids & Bases
  • Name and write the chemical formulas for acids and bases using IUPAC nomenclature rules.
  • Define acids and bases and distinguish between Arrhenius and Bronsted‐Lowry definitions.
  • Differentiate between strong and weak acids and bases.
  • Predict products in acid‐base reactions that form water.
  • Define pH and calculate the pH of a solution using the hydrogen ion concentration.

Unit 8

  • Redox & Thermal Chemistry
  • Differentiate among:
    • Acid‐base reactions
    • Precipitation reactions
    • Oxidation‐reduction reactions
  • Explain everyday examples that illustrate the four laws of thermodynamics.
  • Investigate the process of heat transfer using calorimetry.
  • Classify processes as exothermic or endothermic and represent energy changes that occur in chemical reactions using thermochemical equations or graphical analysis.
  • Perform calculations involving heat, mass, temperature change, and specific heat.