Time Frame: First Grading Period
Pitt County Schools
305127 AP Chemistry
Instructional Guide
SCOS GOALS AND OBJECTIVES
/ ESSENTIAL QUESTIONS, BENCHMARKS, AND SKILLS / ESSENTIAL TASKS, STRATEGIES, PROJECTS, CONNECTIONS / RECOMMENDED RESOURCES AND ASSESSMENTCompetency Goal 4: The learner will develop an understanding of chemical 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. / 1. Why is a balanced equation important?
2. How do you calculate quantitative relationships? / Quantitative Relationships
LAB: Determination of a Copper Iodide / Textbook: Chapter 3
Lab Manual
Competency Goal 4: The learner will develop an understanding of chemical reactions.
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.
Competency Goal 3: The learner will build an understanding of the states of matter and the connection to chemical and physical properties.
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). / 1. What are the concentrations of various chemical species in solution? / Calculations involving chemical species in solution
LAB: Determination of Acetic Acid in Vinegar / Textbook: Chapter 3
Lab Manual
Competency Goal 3: The learner will build an understanding of the states of matter and the connection to chemical and physical properties.
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. / 1. How does the kinetic theory govern gas behavior?
2. How do real gases differ from ideal gases?
3. How do you calculate various parameters of gases under varying conditions?
4. How do you account for the deviations real gases present to the ideal gas equation? / Performing calculations involving gases.
LAB: Collection of Oxygen over Water / Textbook: Chapter 10
Lab Manual
Competency Goal 4: The learner will develop an understanding of chemical reactions.
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. / 1. How do you calculate an equilibrium constant?
2. How do you predict how a system at equilibrium will respond to a stress? / Calculations involving equilibrium constants.
LAB: LeChatelier’s Principle Involving Concentration and Temperature Stresses / Textbook: Chapter 15
Lab Manual
Competency Goal 4: The learner will develop an understanding of chemical reactions.
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. / 1. How do you calculate the pH of a solution containing either acids or bases?
2. How do you calculate the concentrations of conjugate species?
3. How do you calculate equilibrium concentrations?
4. How do you calculate the pH of a salt solution? / Calculations involving pH and equilibrium concentrations.
LAB: Determination of an Unknown Polyprotic Acid / Textbook: Chapter 15
Lab Manual
Time Frame: Second Grading Period
SCOS GOALS AND OBJECTIVES / ESSENTIAL QUESTIONS, BENCHMARKS, AND SKILLS / ESSENTIAL TASKS, STRATEGIES, PROJECTS, CONNECTIONS / RECOMMENDED RESOURCES AND ASSESSMENTCompetency Goal 4: The learner will develop an understanding of chemical reactions.
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. / 1. How do you identify and calculate the chemical species present during any of three types of titrations?
2. How do you calculate the solubility or the Ksp of a relatively insoluble salt?
3. How do you calculate the equilibrium concentrations based on either Ka or Kb?
4. How do you calculate the pH of a buffer? / Calculation involving pH and pOH based on Kw.
Plotting of pH vs. volume points for any of three types of titrations.
LAB: Buffers and Buffering Capacity / Textbook:
Chapters 15, 16, 17
Lab Manual
Competency Goal 2: The learner will develop an understanding of the composition and properties of matter.
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. / 1. How do you calculate the numbers of subatomic particles for different elements?
2. How do you account for the unique electronic arrangement of single ground state elements?
3. How do you relate the solutions to the Schroedinger Equation to the quantum numbers for a single electron?
4. How do you explain various periodic trends? / Assigning unique electronic arrangements for ground state atoms.
Assigning quantum numbers to single atoms. / Chapters 2, 6, 7
Competency Goal 5: The learner will build a knowledge of descriptive chemistry
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. / 1. How do you write net-ionic equations for various types of reactions?
2. How do you name inorganic compounds and coordination chemistry complexes? / Writing AP net-ionic equations.
Naming coordination compounds.
LAB: Qualitative Analysis of Anions / Chapters 2, 4, 6, 7, 24, 25
AP Resource Materials
Competency Goal 2: The learner will develop an understanding of the composition and properties of matter.
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. / 1. How do you differentiate between ionic, covalent, and metallic bonding?
2. Why are Lewis structures limited to simple compounds?
3. What is resonance?
4. How are polarity and miscibility related? / Drawing structures of and predicting geometry of simple compounds.
LAB: Redox Titration of an Oxalate Salt / Chapters 8, 9
Competency Goal 2: The learner will develop an understanding of the composition and properties of matter.
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. / 1. How do you explain the stability and the feasibility of homonuclear diatomic species?
2. How do you explain the importance of intermolecular forces? / Calculations of bond order using molecular orbital diagrams.
LAB: The Evaporative Cooling and Intermolecular Forces of Alcohols (CBL Lab) / Chapters 8, 9, 11
Lab Manual
Time Frame: Third Grading Period
SCOS GOALS AND OBJECTIVES / ESSENTIAL QUESTIONS, BENCHMARKS, AND SKILLS / ESSENTIAL TASKS, STRATEGIES, PROJECTS, CONNECTIONS / RECOMMENDED RESOURCES AND ASSESSMENTCompetency Goal 4: The learner will develop an understanding of chemical reactions.
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. / 1. What is enthalpy and entropy?
2. How do you determine the spontaneity of a process?
3. How do you calculate the total energy required for a phase change? / Calculations involving entropy and enthalpy.
Calculations involving the Gibbs Function.
LAB: Determination of Enthalpy and Entropy Based on the Solubility of Sodium Borate at Varying Temperatures / Textbook:
Chapters 5, 19Lab Manual
Competency Goal 4: The learner will develop an understanding of chemical reactions.
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. / 1. How do you quantitative various colligative properties?
2. How do you differentiate between ideal and nonideal solution behavior?
3. How do you interpret phase diagrams? / Calculations involving colligative properties.
Calculations involving Raoult’s Law.
LAB: Heats of Solution (CBL Lab) / Textbook:
Chapters 5, 17
Lab Manual
Competency Goal 4: The learner will develop an understanding of chemical reactions.
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. / 1. How do you calculate the voltage of various galvanic cells?
2. How do you associate spontaneity with cell voltage?
3. How do you compare the maximum cell voltage with real cell voltage? / Calculations involving cell voltage based on redox.
Calculation of Ecell using the Nernst equation. / Textbook:
Chapters 20
Competency Goal 4: The learner will develop an understanding of chemical reactions.
Competency Goal 4: The learner will develop an understanding of chemical reactions.
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. / 1. How do you determine the rate law of an equation using time versus concentration data?
2. How do you calculate the energy of activation given two k values and temperatures?
3. Is a mechanism feasible?
4. How do you write an integrated rate law? / Calculations involving rate versus concentration data.
Calculations involving the Arrhenius equation.
LAB: Spectrophotometric Determination of the Kinetics for the fading of Phenolphthalein in Alkaline Solution / Textbook:
Chapters 14
Lab Manual
Competency Goal 2: The learner will develop an understanding of the composition and properties of matter.
2.04. Assess the impact of nuclear chemistry
§ Nuclear decay equations.
§ Half-life and radioactivity.
§ Chemical applications. / 1. How do you identify various functional groups?
2. How do you explain isomerism?
What is radioactive decay? / Naming of functional groups.
Calculations involving half-life.
LAB: Organic Synthesis - The Synthesis of Aspirin
LAB: Inorganic Synthesis - The Synthesis of Alum / Textbook:
Chapters 21
Lab Manual
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