AP Correlations for Advanced Chemistry with Vernier
The College Board’s AP* Chemistry Curriculum Framework has undergone significant changes. The new standards will go into effect for the 2013-2014 school year.
Table 1 outlines the correlation of the Primary Learning Objective in the 16 lab investigations from AP® Chemistry Guided-Inquiry Experiments: Applying the Science Practices and the Vernier lab book Advanced Chemistry with Vernier.
Table 2 correlates Learning Objectives from the new Curriculum Framework to each lab experiment in the Vernier lab book Advanced Chemistry with Vernier.
Table 1
| College Board | Vernier Experiment | |
|---|---|---|
| Lab | Primary Learning Objective | |
| 1 | 1.15 | 17. Determining the Concentration of a Solution: Beer’s Law |
| 2 | 1.16 | 17. Determining the Concentration of a Solution: Beer’s Law |
| 3 | 1.19 | 1. The Determination of a Chemical Formula |
| 4 | 1.20 | 7. Acid-Base Titration |
| 7 | 3.5 | 1. The Determination of a Chemical Formula |
| 8 | 3.9 | 8. An Oxidation-Reduction Titration: The Reaction of Fe2+ and Ce4+ |
| 9 | 3.10 | 22. The Synthesis and Analysis of Aspirin |
| 10 | 4.1 | 12. The Decomposition of Hydrogen Peroxide 25. The Rate and Order of a Chemical Reaction |
| 11 | 4.2 | 35. Rate Determination and Activation Energy 25. The Rate and Order of a Chemical Reaction |
| 12 | 5.7 | 26. The Enthalpy of Neutralization of Phosphoric Acid |
| 13 | 6.9 | 10. The Determination of an Equilibrium Constant |
| 14 | 6.13 | 7. Acid-Base Titration |
| 15 | 6.20 | 19. Buffers 7. Acid-Base Titration |
| 16 | 6.18 |
19. Buffers 7. Acid-Base Titration |
Table 2
| Vernier Experiment | Learning Objective from the AP Chemistry 2013 Framework |
|---|---|
| 1. The Determination of a Chemical Formula |
1.19: The student can design, and/or interpret data from, an experiment that uses gravimetric analysis to determine the concentration of an analyte in a solution. 3.3: The student is able to use stoichiometric calculations to predict the results of performing a reaction in the laboratory and/or to analyze deviations from the expected results. 3.5: The student is able to design a plan in order to collect data on the synthesis or decomposition of a compound to confirm the conservation of matter and the law of definite proportions. |
| 2. The Determination of the Percent Water in a Compound | 3.3: The student is able to use stoichiometric calculations to predict the results of performing a reaction in the laboratory and/or to analyze deviations from the expected results. |
| 3. The Molar Mass of a Volatile Liquid | 1.4: The student is able to connect the number of particles, moles, mass, and volume of substances to one another, both qualitatively and quantitatively. |
| 4. Using Freezing-Point Depression to Find Molecular Weight | (No correlation, removed from the AP Chem curriculum) |
| 5. The Molar Volume of a Gas | 1.4: The student is able to connect the number of particles, moles, mass, and volume of substances to one another, both qualitatively and quantitatively. |
| 6. Standardizing a Solution of Sodium Hydroxide | 1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution. |
| 7. Acid-Base Titration | 1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution., 6.13: The student can interpret titration data for monoprotic or polyprotic acids involving titration of a weak or strong acid by a strong base (or a weak or strong base by a strong acid) to determine the concentration of the titrant and the pKa for a weak acid, or the pKb for a weak base. |
| 8. An Oxidation-Reduction Titration: The Reaction of Fe2+ and Ce4+ |
1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution. 3.9: The student is able to design and/or interpret the results of an experiment involving a redox titration. |
| 9. Determining the Mole Ratios in a Chemical Reaction | 3.3: The student is able to use stoichiometric calculations to predict the results of performing a reaction in the laboratory and/or to analyze deviations from the expected results. |
| 10. The Determination of an Equilibrium Constant |
6.5: The student can, given data (tabular, graphical, etc.) from which the state of a system at equilibrium can be obtained, calculate the equilibrium constant, K. 6.9: The student is able to use LeChatelier’s principle to design a set of conditions that will optimize a desired outcome, such as product yield. |
| 11. Investigating Indicators | (No match to a Learning Objective) |
| 12. The Decomposition of Hydrogen Peroxide |
4.1: The student is able to design and/or interpret the results of an experiment regarding the factors (i.e., temperature, concentration, surface area) that may influence the rate of a reaction. 4.2: The student is able to analyze concentration vs. time data to determine the rate law for a zeroth-, first-, or second-order reaction. |
| 13. Determining the Enthalpy of a Chemical Reaction | 3.11: The student is able to interpret observations regarding macroscopic energy changes associated with a reaction or process to generate a relevant symbolic and/or graphical representation of the energy changes. |
| 14 A&B. Separation and Qualitative Analysis of Cations and Anions | 3.10: The student is able to evaluate the classification of a process as a physical change, chemical change, or ambiguous change based on both macroscopic observations and the distinction between rearrangement of covalent interactions and noncovalent interactions. |
| 15 A&B. The Synthesis and Analysis of Alum | 3.10: The student is able to evaluate the classification of a process as a physical change, chemical change, or ambiguous change based on both macroscopic observations and the distinction between rearrangement of covalent interactions and noncovalent interactions. |
| 16. Conductimetric Titration and Gravimetric Determination of a Precipitate | 1.19: The student can design, and/or interpret data from, an experiment that uses gravimetric analysis to determine the concentration of an analyte in a solution. |
| 17. Determining the Concentration of a Solution: Beer’s Law | 1.15: The student can justify the selection of a particular type of spectroscopy to measure properties associated with vibrational or electronic motions of molecules. 1.16: The student can design and/or interpret the results of an experiment regarding the absorption of light to determine the concentration of an absorbing species in a solution. |
| 18. Liquid Chromatography | 2.10: The student can design and/or interpret the results of a separation experiment (filtration, paper chromatography, column chromatography, or distillation) in terms of the relative strength of interactions among and between the components. |
| 19. Buffers |
6.18: The student can design a buffer solution with a target pH and buffer capacity by selecting an appropriate conjugate acid-base pair and estimating the concentrations needed to achieve the desired capacity. 6.20: The student can identify a solution as being a buffer solution and explain the buffer mechanism in terms of the reactions that would occur on addition of acid or base. |
| 20. Electrochemistry: Voltaic Cells | 3.13: The student can analyze data regarding galvanic or electrolytic cells to identify properties of the underlying redox reactions. |
| 21. Electroplating |
3.12: The student can make qualitative or quantitative predictions about galvanic or electrolytic reactions based on half-cell reactions and potentials and/ or Faraday’s laws. 3.13: The student can analyze data regarding galvanic or electrolytic cells to identify properties of the underlying redox reactions. |
| 22. The Synthesis and Analysis of Aspirin | 3.10: The student is able to evaluate the classification of a process as a physical change, chemical change, or ambiguous change based on both macroscopic observations and the distinction between rearrangement of covalent interactions and noncovalent interactions. |
| 23. Determining the Ksp of Calcium Hydroxide | 1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution. |
| 24. Determining Ka by the Half-Titration of a Weak Acid | 1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution. |
| 25. The Rate and Order of a Chemical Reaction |
4.1: The student is able to design and/or interpret the results of an experiment regarding the factors (i.e., temperature, concentration, surface area) that may influence the rate of a reaction. 4.2: The student is able to analyze concentration vs. time data to determine the rate law for a zeroth-, first-, or second-order reaction. |
| 26. The Enthalpy of Neutralization of Phosphoric Acid |
3.11: The student is able to interpret observations regarding macroscopic energy changes associated with a reaction or process to generate a relevant symbolic and/or graphical representation of the energy changes. 5.7: The student is able to design and/or interpret the results of an experiment in which calorimetry is used to determine the change in enthalpy of a chemical process (heating/cooling, phase transition, or chemical reaction) at constant pressure. |
| 27. α, β, and γ | (No match to a Learning Objective) |
| 28. Radiation Shielding | (No match to a Learning Objective) |
| 29. The Base Hydrolysis of Ethyl Acetate | (No match to a Learning Objective) |
| 30. Exploring the Properties of Gases | 2.4: The student is able to use KMT and concepts of intermolecular forces to make predictions about the macroscopic properties of gases, including both ideal and nonideal behaviors. |
| 31. Determining Avogadro’s Number | 3.12: The student can make qualitative or quantitative predictions about galvanic or electrolytic reactions based on half-cell reactions and potentials and/ or Faraday’s laws. |
| 32. Potentiometric Titration of Hydrogen Peroxide | 3.9: The student is able to design and/or interpret the results of an experiment involving a redox titration. |
| 33. Determining the Half-Life of an Isotope | (No match to a Learning Objective) |
| 34. Vapor Pressure and Heat of Vaporization | 5.6: The student is able to use calculations or estimations to relate energy changes associated with heating/cooling a substance to the heat capacity, relate energy changes associated with a phase transition to the enthalpy of fusion/vaporization, relate energy changes associated with a chemical reaction to the enthalpy of the reaction, and relate energy changes to PΔV work. |
| 35. Rate Determination and Activation Energy |
4.1: The student is able to design and/or interpret the results of an experiment regarding the factors (i.e., temperature, concentration, surface area) that may influence the rate of a reaction. 4.2: The student is able to analyze concentration vs. time data to determine the rate law for a zeroth-, first-, or second-order reaction. |
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