Chemistry I

Unit 1 - Basic Concepts, Atoms, Molecules, & Ions -

1.1. Convert units (e.g., length, mass, volume, temperature) within a unit system

1.2. Convert units (e.g. length, mass, volume, temperature) between unit systems.

1.3. Combine measurements to calculate properties (e.g. density).

1.4. Express measured and calculated quantities in exponential form.

1.5. Express measured quantities in the proper number of significant figures.

1.6. Express calculated quantities in the proper number of significant figures.

1.7. Trace the historical development of theories of matter.

1.8. State the name and symbol for the elements and their ions.

1.9. Characterize the important subatomic particles.

1.10. Determine the subatomic structure of atoms, ions, and isotopes. Use AZX charge notation.

1.11. Characterize the various parts of the periodic table.

1.12. Name and write formulas for simple compounds.

Unit 2 - Stoichiometry -

2.1. Determine atomic weights from isotope abundance.

2.2. Relate formula weights and moles to weights and numbers of particles in a chemical formula.

2.3. Determine the % composition of compounds.

2.4. Determine molecular formulas from experimental analysis data.

2.5. Write and balance simple chemical equations.

2.6. Relate numbers of moles, grams, and particles in a chemical equation. (including limiting reagents)

2.7. Determine and use molar concentration units.

2.8. Use the MAVA = MBVB relationship to do dilution determinations.

Unit 3 - Thermochemistry -

3.1. Utilize and convert different forms of energy.

3.2. Determine the heat produced by a chemical or physical process from experimental data

(calorimetry).

3.3. Determine the heat produced during changes in state from experimental data.

3.4. Given a thermochemical equation, calculate Æ H for a given amount of reactant or product.

3.5. Apply Hess’ Laws to determine Æ H for reactions.

3.6. Apply standard Æ Hf to determine Æ Hrxn of reactions.

3.7. Use bond energies to predict Æ Hrxn.

Unit 4 - Atomic Structure & Periodicity -

4.2. Interpret the line spectrum of an atom in terms of quantum mechanics.

4.3. Describe the location and nature of electrons in an atom or ion in terms of: (a) quantum numbers, (b) energy level diagrams, (c) electron configuration, and (d) orbital shape.

4.4. Relate the periodic table to electron configurations.

4.5. Predict trends; similarities, and differences of physical and chemical properties of elements using the periodic table and electron configuration. (e.g. ionization energy, radius, formulas, reactivity)

Unit 5 - Molecular Structure & Bonding -

5.1. Predict the relative polarity and ionic/covalent character of bonds and molecules.

5.2. Identify simple bonding types.

5.3. Draw Lewis structures of ions and molecules.

5.4. Identify resonance structures for molecules.

5.5. Determine the geometric arrangement of atoms in a molecule.

5.6. Predict the types of orbitals (including hybrids) involved in bonding and resulting bond types (sigma, pi).

Unit 6 - Properties of Gases -

6.1. Describe measuring gas pressures using barometers and manometers. Relate pressure units.

6.2. Apply the ideal gas law to relate and calculate values for pressure, volume, temperature,

and amount of a gas.

6.3. Apply Dalton’s Law of partial pressure to calculate the pressure of combined gases and to calculate the partial pressures of gases in mixtures.

6.4. Describe gases in terms of KMT.

6.5. Relate MW and speeds of molecules using Graham’s law.

6.6. Distinguish between ideal and real gases.

Unit 7 - Properties of Liquids, Solids, & Solutions -

7.1. Use KMT to explain the general properties of liquids and solids and to explain phase changes.

7.2. Classify intermolecular bonds and predict relative properties of chemical substances.

7.3. Describe the structure and properties of liquids.

7.4. Describe the structure and properties of solids.

7.5. Interpret phase diagrams.

7.6. Identify the composition of a solution.

7.7. Characterize the dissolving process. Characterize hydrolysis.

7.8. Predict products of precipitation reactions.

7.9. Characterize solutions as strong electrolytes, weak electrolytes, and nonelectrolytes.

Unit 8 - Organic Chemistry

8.1. Describe the bonds associated with organic molecules.

8.2. Use IUPAC system to name simple organic compounds.

8.3. Identify types of organic molecules according to functional group.

8.4. Characterize the simple reactions of organic molecules.

8.5. Identify isomers of simple organic compounds.

8.6. Characterize the formation of polymers.

Chemistry II

Unit I - Kinetics -

1.1. Express and compare rates of chemical reactions in terms of the concentration changes of the reactants and products (or factors proportional to concentration) per unit time.

1.2. Use collision theory to explain how chemical reactions occur and how rates are affected.

1.3. From experimental kinetics data, derive the rate law, order, and rate constant for a chemical reaction.

1.4. For a zero, first or second order reaction, determine the exact rate constant and half-life for a chemical reaction from time/concentration data.

1.5. From a reaction profile, determine ÆH & E_a for a chemical reaction. [Readings 16.6 Problem 62]

1.6. Explain the role of catalysts, what they are, how they work, and how they affect a reaction profile.

1.7. From kinetic data, determine the relationship between E_a, k, and the temperature of both catalyzed and uncatalyzed chemical reactions.

1.8. Determine the relationship between the rate law and the mechanism of a simple chemical reaction.

Unit II - Equilibrium -

2.1. Characterize chemical reactions in terms of reversibility and relative concentrations of reactants and products.

2.2. Determine equilibrium expressions for homogeneous and heterogeneous chemical reactions from stoichiometry.

2.3. Determine the stoichiometric relationship between initial and equilibrium concentrations of reactants and products.

2.4. Determine the relationship between Kold and Knew when a chemical reaction is reversed or multiplied by a constant factor of n.

2.5. Determine the relationship between KC and KP for a chemical reaction involving gaseous components.

2.6. Determine value for K from equilibrium concentrations of reactants and products in a chemical reaction.

2.7. Determine the equilibrium concentrations of reactants and products of a chemical reaction from initial concentrations and value of K.

2.8. Determine if equilibrium has been reached in a chemical reaction; determine the direction the reaction will shift if equilibrium has not been reached.

2.9. Use Le Châtelier’s Principle to predict the direction a reaction at equilibrium will shift as a result of changes in concentration, pressure/volume, and temperature as it approaches a new equilibrium.

Unit III - Acid/Base -

3.1. Relate [H⁺], [OH^-], and K_W in an aqueous solution.

3.2. Determine the pH and/or pOH of an aqueous solution from the [H⁺] (or [OH^-]) and v.

3.3 Define acids and bases in terms of Arrhenius, and Brönsted-Lowry theories.

3.4. Recognize and construct conjugates of acids or bases.

3.5. Determine the [H⁺], [OH^-], pH and/or pOH of a strong acid or strong base solution.

3.6. Determine and relate equilibrium concentrations, [H⁺], [OH^-], pH and/or pOH with K_a values for weak acids (also, same for K_b values for weak bases).

3.7. Determine the [H⁺], [OH^-], pH and/or pOH for weak acids or weak bases from initial concentrations.

3.8. Construct an ordered list of strongest to weakest (or v.v.) for acids or bases.

3.9. Determine the K_b for a weak base, given the K_a value of its conjugate acid (v.v.).

3.10. Determine the [H⁺], [OH^-], pH and/or pOH of a salt solution.

3.11. Qualitatively determine the acidic, basic, or neutral properties of a salt.

3.12. Identify acids and bases using Lewis theory.

3.13. Determine the [H⁺], [OH^-], pH and/or pOH of weak and strong polyprotic acids.

Unit IV - Aqueous Equilibrium -

4.1. Define and make buffer solutions from (1) a weak acid and its conjugate base, (2) a weak base and its conjugate acid, (3) a weak acid and a strong base, and (4) a weak base and a strong acid.

4.2. Determine the pH of a buffer solution from concentrations and v.v.

4.3. Make a buffer with a specific pH. [Readings 19.1 Problems 23,25]

4.4. Determine the conjugate pair best suited to make a buffer of desired pH.

4.5. Analyze a strong acid/strong base titration (including polyprotic) (determine end point location and entire pH curve, including pH at beginning, pH at end point, and pH at all other points).

4.6. Analyze a titration of a weak acid or base with a strong base or acid (determine end point location and entire pH curve, including pH at beginning, pH at end point, and pH at all other points).

4.7. Determine the K_SP equilibrium expression for a partially soluble salt.

4.8. Determine the K_SP value, given the solubility of a salt (v.v.).

4.9. Determine the effect of a common ion on the solubility of a partially soluble salt.

Unit V - Chemical Thermodynamics -

5.1. Apply Hess’ Laws to thermodynamic quantities.

5.2. Determine ÆH° for a chemical reaction from ÆH_f° values of reactants and products.

5.3. Predict the qualitative change in enthalpy for various chemical reactions.

5.4. Predict and compare the qualitative change in entropy for various chemical reactions and physical processes.

5.5. Determine ÆS° for a chemical reaction from S° values of reactants and products.

5.6. Determine ÆG° for a chemical reaction from the Gibbs equation.

5.7. Determine ÆG° for a chemical reaction from ÆG_f° values of reactants and products.

5.8. Determine ÆG for a chemical reaction from ÆG° and the reaction quotient, Q.

5.9. Predict whether a chemical reaction, as written, is spontaneous, non-spontaneous, or at equilibrium.

5.10. Calculate the standard free energy for a chemical reaction from the equilibrium constant (v.v.).

5.11. Determine the equilibrium temperature, T_e, for a chemical reaction from ÆH° and ÆS° (v.v.).

Unit VI - Electrochemistry -

6.1. Assign oxidation numbers (oxidation states) to individual elements in a chemical compound or complex ion.

6.2. Recognize redox reactions; distinguish from reactions not involving oxidation/reduction.

6.3. Stoichiometrically balance both half-reactions and cell reactions involving redox.

6.4. Draw a diagram of a voltaic (galvanic, spontaneous) cell and explain how it works, predicting changes that will occur during discharge.

6.5. Define and identify anode, cathode, oxidation process, reduction process, oxidizing agent, and reducing agent for a redox reaction.

6.6. Calculate E° for a chemical reaction using a standard reduction potential table.

6.7. Predict the products of a redox reaction.

6.8. Calculate and relate values of E°, ÆG°, and K for an oxidation-reduction reaction.

6.9. Calculate E for a redox reaction under non-standard conditions of constituent concentrations and/or pressures.

6.10. Draw a diagram of an electrolytic (non-spontaneous) cell and explain how it works, predicting changes that will occur during operation.

6.11. Construct a line notation for an electrochemical cell from information concerning the anode, cathode, oxidation process, reduction process, oxidizing agent, and/or reducing agent (v.v.).

6.12. Relate the amount of product(s) produced and/or reactant consumed in an electrolytic cell to the current used, time involved, and moles of electrons associated with the corresponding half-reaction.

Unit VII - Nuclear Chemistry -

7.1. Identify the number of protons and neutrons found in the nucleus of any atom.

7.2. Identify the symbols representing various subatomic particles.

7.3. Using N and Z relationships for individual nuclides, predict stability/instability (non-radioactivity/radioactivity).

7.4. Write balanced equations for nuclear reactions including decay, transmutation, fission, & fusion.

7.5. Identify missing nuclear particles in a nuclear reaction.

7.6. Determine the half-life, beginning amount, final amount, or elapsed time in a radioactive decay reaction.

7.7. Use radioactive (e.g. carbon-14) dating techniques to calculate the age of a substance.

7.8. Determine the mass defect, binding energy, and binding energy per nucleon for a nuclear particle.

7.9. Determine the energy absorbed or released in a nuclear reaction.

Unit VIII - Coordination Chemistry -

8.1. Determine the electronic configurations of transition metals and metal ions.

8.2. Recognize and identify coordination compounds and their components.

8.3. Determine oxidation number, coordination number, orbitals used in bonding, and geometry of the central metal atom in coordination compounds and complexes.

8.4. Describe the bonding effects of polydentate ligands.

8.5. Given their formulas, name coordination compounds and complexes (and v.v.).

8.6. Recognize, describe, and identify structural isomers (coordination & linkage) and stereoisomers (geometrical and optical) of coordination complexes.

8.7. Explain spin state and the magnetic and color properties of transition elements.

8.8. Relate and predict electronic structure, field strength (Æ), spin state, and magnetic and color properties of coordination complexes in octahedral, tetrahedral, and square planar environments.

8.9. Relate and predict electronic structure, field strength (Æ), spin state, and magnetic and color properties of coordination complexes based on ligand strength.