STANDARD COURSE OF STUDY

1.01 Design, conduct and analyze investigations to answer questions related to chemistry.

• Identify questions and suggest hypotheses.
• Identify variables.
• Use a control when appropriate.
• Select and use appropriate measurement tools.
• Collect and organize data in tables, charts and graphs.
• Analyze and interpret data.
• Explain observations.
• Make inferences and predictions.
• Explain the relationship between evidence and explanation.
• Identify how scientists share findings.

1.02 Analyze reports of scientific investigations from an informed scientifically-literate viewpoint including considerations of:

• Appropriate sample.
• Adequacy of experimental controls.
• Replication of findings.
• Alternative interpretations of the data

1.03 Analyze experimental designs with regard to safety and use safe procedures in laboratory investigations:

• Identify and avoid potential safety hazards given a scenario.
• Differentiate between safe and unsafe procedures.
• Use information from the MSDS (Material Safety Data Sheets) to assess chemical hazards.

2.01 Analyze the structure of matter at the atomic level

• Evidence for the atomic theory.
• Atomic masses; determination by chemical and physical means.
• Atomic number and mass number; isotopes.
• Electron energy levels: atomic spectra, quantum numbers, atomic orbitals.
• Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states.

2.02 Examine the types of chemical bonds and the nature of each

• Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces).
• Relationships to states, structure, and properties of matter.
• Polarity of bonds, electronegativities.

2.03 Analyze conceptual models of bonding and molecular shape and the relation to chemical and physical properties of matter.

• Lewis structures.
• VSEPR.
• Valence bond: hybridization of orbitals, resonance, sigma and pi bonds.
• Geometry of molecules and ions, structural isomerism of simple organic. molecules and coordination complexes; dipole moments of molecules; relation of properties to structure.

2.04. Assess the impact of nuclear chemistry

• Nuclear decay equations.
• Half-life and radioactivity.
• Chemical applications.
  

3.01 Examine the relationships between pressure, volume and temperature of ideal gases

• Laws of ideal gases: Boyle's, Charles'.
• The ideal gas equation.
• Partial pressures and Dalton's Law.

3.02. Analyze kinetic-molecular theory

• Interpretation of ideal gas laws on the basis of this theory.
• Avogadro's hypothesis and the mole concept.
• Dependence of kinetic energy of molecules on temperature.
• Deviations from ideal gas laws.

3.03. Assess the nature of liquids and solids

• Liquids and solids from the kinetic-molecular viewpoint.
• Phase diagrams of one-component systems.
• Changes of state, including critical points and triple points.
• Structure of solids; lattice energies.

3.04 Examine the nature of solutions

• Types of solutions and factors affecting solubility.
• Methods of expressing concentration (The use of normalities is not tested.).
• Raoult's law and colligative properties (nonvolatile solutes); osmosis.
• Non-ideal behavior (qualitative aspects).

4.01 Analyze the various types of common chemical reactions

• Acid-base reactions; concepts of Arrhenius, Brönsted-Lowry, and Lewis;
• Coordination complexes; amphoterism.
• Precipitation reactions.
• Oxidation-reduction reactions.
  Oxidation number.
  The role of the electron in oxidation-reduction.
  Electrochemistry: electrolytic and galvanic cells; Faraday's laws; standard half-cell potentials; Nernst equation; prediction of the direction redox reactions.

4.02 Apply the principles of stoichiometry

• Ionic and molecular species present in chemical systems: net ionic equations.
• Balancing of equations including those for redox reactions.
• Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants.

4.03 Analyze systems in dynamic equilibrium

• Concept of dynamic equilibrium, both physical and chemical; Le Chatelier's principle; equilibrium constants.
• Quantitative treatment for gaseous reactions using Kp and Kc.
• Quantitative treatment for reactions in solution Kc.
• Quantitative treatment of for acids and bases; using Ka and Kb, pKa and pKb and pH.
• Quantitative treatment for precipitation reactions and the dissolution of slightly soluble compounds using the solubility product constant, Ksp.
• Common ion effect; buffers; hydrolysis.

4.04 Analyze chemical kinetics

• Concept of rate of reaction.
• Use of differential rate laws to determine order of reaction and rate constant from experimental data.
• Effect of temperature change on rates.
• Energy of activation; the role of catalysts.
• The relationship between the rate-determining step and a mechanism.

4.05 Analyze chemical thermodynamics

• State functions.
• First law: change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry.
• Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes.
• Relationship of change in free energy to equilibrium constants and electrode potentials.
  

5.01 Examine chemical reactivity and predict the products of chemical reactions.

5.02 Analyze the relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements.

5.03. Explore organic chemistry on an introductory level

• Hydrocarbons and functional groups (structure, nomenclature, chemical properties).
• Physical and chemical properties of simple organic compounds should also be included as exemplary material for the study of other areas such as bonding, equilibria involving weak acids, kinetics, colligative properties, and stoichiometric determinations of empirical and molecular formulas.