vankessel et al (2003). Chapter 3. Zumdahl & Zumdahl (2000). Chapter 7.

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1 TOPIC 1: ATOMIC STRUCTURE AND PERIODICITY vankessel et al (2003). Chapter 3. Zumdahl & Zumdahl (2000). Chapter 7. Part I: Wave-Particle Theory a) Description and calculations based on wave nature of matter, including frequency, wavelength, amplitude, and speed using c = λν b) Quantization of energy and quantifying Planck and Einstein s contributions using E = hν and h m = λ c h c) de Broglie s equation and calculations using λ = mv d) Atomic spectra and the atomic spectrum of hydrogen Lab: Identification of an unknown gas using a gas discharge tube and a diffraction grating Part II: Quantum Numbers a) Description and meaning of each of the quantum numbers n, l, m l, ms b) Sketch of p subshells c) Pauli exclusion principle, Aufbau principle, orbital diagrams and Hund s rule d) Atomic orbital energy diagrams, atomic orbital diagrams, the periodic table of orbitals, and first row transition element exceptions e) Electron configurations of atoms Activity: Review and reinforcement of assigning quantum numbers using the Quantum Numbers Card Game Part III: Periodic Trends f) Explaining first ionization energies of elements in the first three periods g) Trends in atomic radii, ionic radii, and isoelectronic atoms and ions TOPIC 2: KINETICS vankessel et al (2003). Chapter 6. Zumdahl & Zumdahl (2000). Chapter 12. Part I: Reaction Rates & Rate Laws a) Types of data that may be collected to calculate reaction rates

2 b) Representing and interpreting rates using concentration versus time graphs c) Measuring rates, factors affecting rates, and stoichiometry of reaction rates Lab: Investigating the relationship between the average rate of appearance of iodine and changes in concentration of iodate ion and temperature in the Landolt reaction d) Determining differential rate laws from data obtained by method of initial rates e) Specific rate constant calculations and units Part II: Potential Energy Diagrams, Reaction Mechanisms & Collision Theory f) Potential energy, kinetic energy, and enthalpy g) Activation energy and the activated complex h) Difference between activated complexes and intermediates i) Endothermic and exothermic reactions j) Sketching and labelling potential energy diagrams, including enthalpy of reactants, products, enthalpy of reaction, intermediates, activation energy, location of activated complexes, and catalysts k) Writing balanced overall reactions, distinguishing between intermediates and catalysts, and identifying the slowest step given a reaction mechanism consisting of two or more elementary reactions l) Explaining the four factors affecting rates concentration, surface area, temperature, addition of a catalyst, nature of reactant in terms of frequency of collisions and fraction of effective collisions with supporting diagrams, such as a potential energy diagram or a Maxwell Boltzmann energy distribution curve TOPIC 3: GASEOUS EQUILIBRIUM vankessel et al (2003). Chapter 7. Zumdahl & Zumdahl (2000). Chapter 13. a) Phase equilibrium, conditions of equilibrium, and the dynamic nature of equilibrium Simulation Activity: Graphical analysis of equilibrium concentrations using glass straws and changes in volume as a metaphor for chemical equilibrium b) Identifying equilibrium on concentration versus time graphs c) Guldberg and Waage s equilibrium law expression, called the mass action expression d) The Law of chemical equilibrium and writing equilibrium law constant expressions, K c e) Altering the K c expression given heterogeneous equilibrium systems f) Calculating equilibrium concentrations from ICE tables and percent reaction.

3 g) Comparing the reaction quotient, Q, to the equilibrium constant, K c and predicting the direction of the reaction h) Solving ICE tables resulting in a quadratic, or a reducible square i) Simplifying ICE table solutions using the Rule of 100 j) Using Le Châtelier s Principle to interpret concentration versus time graphs, and explaining temperature, concentration, volume, pressure, inert gas, and catalyst stresses on a system and the system s response TOPIC 4: SOLUBILITY EQUILIBRIUM vankessel et al (2003). Chapter 7. Zumdahl & Zumdahl (2000). Chapter 15. a) Review of saturated solutions and heterogeneous equilibrium b) Writing balanced equilibrium equations and equilibrium constant expressions for the dissociation of ionic compounds with low solubility c) Calculating molar solubility (in units of mol/l) or solubility in other units such as mg/l, g/ml given the solubility product, K sp d) Calculating K sp from solubility data Lab: Determination of the solubility product constant of PbCl 2 through quantitative analysis of the precipitate formed between a saturated solution of PbCl 2 and excess K 2 CrO 4 solution e) Review of solubility rules for double displacement reactions in aqueous solution f) Predicting precipitation of a slightly soluble ionic salt after mixing two solutions with known volumes and concentrations g) Calculating solubility in various units mol/l, or g/l or mg/ml when a solution containing a common ion is added to a solution of a sparingly soluble ionic salt (called the common ion effect) TOPIC 5: ACIDS & BASES AND AQUEOUS EQUILIBRIUM vankessel et al (2003). Chapter 8. Zumdahl & Zumdahl (2000). Chapter 13. Part I: Introduction to Acids and Bases a) Investigating properties of acids, and writing chemical formulas and naming binary and ternary acids b) Distinguishing between monoprotic, diprotic, and polyprotic acids and bases c) Development of 6 ph equations from the autoionization of water H 2 O(l) H 3 O + (aq) + OH + (aq) and K W = [ H 3 O ][ OH ] d) Calculating ph, poh, [H 3 O + ], [H + ], and [OH ] in solutions of strong acids or strong bases.

4 Part II: Strong Acid with Strong Base Titrations e) Writing balanced neutralization equations (molecular form) f) Performing stoichiometric calculations g) Introduction to titration as a technique and laboratory equipment used for titrations Lab: Determination of the concentration of acetic acid in household vinegar via titration with sodium hydroxide solution h) Calculating ph before titrant is added, before equivalence, at equivalence (ph = 7.0 for a strong acid/strong base reaction), and after equivalence i) Constructing and interpreting ph titration curves, including labeling endpoint given specific indicators, ph and titrant volume at equivalence, and regions where acid and base limits j) Explaining the difference between endpoint and equivalence Part III: Aqueous Equilibrium k) Writing balanced acid ionization equations and acid ionization constant expressions l) Interpreting acid ionization constants at 25 C from K a tables m) Examining acids as strong or weak electrolytes, and identifying the six common strong acids HCl, HNO 3, HClO 4, HI, HBr, H 2 SO 4 n) Calculating percent ionization of acids o) Performing equilibrium ph stoichiometry calculations for solutions of weak acids in aqueous solution Lab: Dilution of 1.0 M solution of acetic acid and calculating the acid ionization constant of a 0.10 M solution of acetic acid from ph data TOPIC 6: ELECTROCHEMISTRY vankessel et al (2003). Chapters 9 & 10. Zumdahl & Zumdahl (2000). Chapter 17. Part I: Redox Reactions a) Assigning oxidation numbers, identifying redox reactions, and the role of the electron b) Identifying oxidation, reducing agents, reduction, and oxidizing agents c) Balancing redox reactions using the half-cell method d) Determining the strongest oxidizing agent and strongest reducing agent from experimental evidence and constructing a table of balanced reduction half-reactions, ordered from strongest oxidizing agent to weakest oxidizing agent e) Predicting spontaneity from standard redox tables

5 Lab: Constructing a redox table of balanced half reactions from the reaction of four metals with the appropriate solutions of metallic ions Part II: Galvanic Cells and Electrolytic Cells f) Galvanic cells and spontaneous reactions, including inert electrodes g) Cell notation h) Sketching labelled Galvanic cell diagrams from cell notation, including direction of electron flow, charge of anode and cathode, movement of ions in solution, sites of oxidation and reduction, and voltmeter i) Using redox tables to determine the anode, cathode, and direction of electron movement through metals, and ion movement through solution Lab: Constructing functional galvanic cells and determining their overall cell potential, including labelled diagrams, balanced half-reactions, overall reactions, and predicted standard cell potentials from SRP tables j) Sketching labelled aqueous and molten electrolytic cells, including charge of anode and cathode, movement of ions in solution, power source, balanced half-reactions, overall reaction, and emf Lab: Aqueous electrolysis of potassium iodide, including labelled diagrams, balanced half-reactions, overall reactions, identification of strongest oxidizing agent and strongest reducing agent and minimum emf required to drive the reaction k) Faradays laws and electrolysis stoichiometry using It q = l) Similarities and differences between electrochemical cells and electrolytic cells m) Applications of electrochemistry, including cathodic protection, electrorefining and electroplating