1. New AP Chemistry Cirriculum What’s In What’s Out

2. The 6 Big Ideas 1.Atomic Structure 2.Bonding and Properties 3.Reactions (including Electrochemistry) 4.Kinetics 5.Thermodynamics 6.Chemical Equilibrium

3. Big Idea 1 Atomic Structure The chemical elements are fundamental building materials of matter, and all matter can be understood in terms of arrangements of atoms. These atoms retain their identity in chemical reactions Includes atomic theory, mole-mass calculations, electronic configuration, periodicity Lab-wise: gravimetric analysis, titrations, Beer’s law

4. Big Idea 1 (Cont.) Atomic Structure Exclusions: Memorization of exceptions to Aufbau principle, i.e., Cr and Cu, Mo and Ag Assignment of quantum numbers to electrons

5. What’s Out: Content Quantum Numbers

6. Big Idea 1 (Cont.) Atomic Structure New or emphasized: LO 1.5, 1.6, 1.7: Photoelectron Spectroscopy LO 1.7, 1.8: Coulomb’s Law – attractive force due to opposite charges vs distance LO 1.13: Refining models LO 1.14: Mass spectrometry for isotopes LO 1.15: Vibration (IR) vs Electronic transition (UV- Vis)

7. Big Idea 2 Bonding and Properties Chemical and physical properties of materials can be explained by the structure and the arrangement of atoms, ions, or molecules and the forces between them Includes solids, liquids, gases, solutions, inter-particulate forces, electronegativity, Lewis structures, VSEPR theory, bonding, properties Lab-wise: LO 2.7, 2.10: separation techniques especially chromatography and distillation; and LO 2.22: type of bonding

8. Big Idea 2 (Cont.) Bonding and Properties Exclusions: Phase Diagram (prior knowledge) Colligative properties (prior knowledge) Molality, percent by mass and by volume (prior knowledge) Weaker H-bonding with H not bonded to N, O, or F Specific types of crystal structures, e.g. ABC, ABA, etc.

9. Big Idea 2 (Cont.) Bonding and Properties Exclusions (Cont.): The use of formal charge to explain exception to octet rule – but the use of formal charge calculation is still in Learning how to defend the Lewis model, e.g. with odd number of electrons Hybridization beyond sp 3 Filling molecular orbital diagrams Specific varieties of crystal lattices for ionic compound

10. What’s Out: Content Hybridization beyond sp, sp2, and sp3

11. What’s Out: Content Phase Diagram

12. Big Idea 2 (Cont.) Bonding and Properties New or emphasized: LO 2.19, 2.21, 2.26: Macroscopic properties such as viscosity, surface tension, capillary action, vapor pressure, boiling point, volumes of mixing for liquids, hardness LO 2.14: Coulombic forces as IMFs in biological systems and in hydrogen PE vs. nuclear distance LO 2.25, 2.26: Alloys LO 2.30: Semi-conductors using Si

13. Big Idea 3 Chemical Reactions Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons Equation writing, stoichiometric calculations, Bronsted- Lowry acid-base theory, oxidation numbers, redox reactions, energies involved, electrochemistry Lab-wise: LO 3.5, 3.6: synthesis and decomposition reactions; LO 3.9: redox reactions; acid-base reactions

14. Big Idea 3 (Cont.) Chemical Reactions Exclusions: Lewis acid-base concepts (prior knowledge) but complex ions and related solubility are included Language of reducing agent and oxidizing agent Labeling an electrode as positive or negative Calculations using the Nernst equation is excluded but qualitative reasoning about effects of concentration on cell potential is in

15. What’s Out: Content Lewis definition of acids and bases Also no more 5 choice multiple choice, only 4 choices!

16. Big Idea 3 (Cont.) Chemical Reactions New or emphasized: LO 3.1: Pictorial representation at the particulate level LO 3.10: Classify physical change, chemical change, or ambiguous change based on macroscopic observation and microscopic theory regarding bonding and interactions of particles LO 3.11: Graphical depiction of energy diagrams

17. Big Idea 4 Kinetics Rates of chemical reactions are determined by details of the molecular collisions Includes factors affecting reaction rates, rate laws (both differential and integrated), collision theory, reaction mechanism, catalysis Lab-wise: LO 4.1: Exploration of factors affecting rate of reaction; Beer’s Law

18. Big Idea 4 (Cont.) Kinetics Exclusions: Arrhenius equation in calculations is out, but conceptual aspects of the equation and graphical interpretation are still in Collection of data pertaining to experimental detection of a reaction intermediate

19. Big Idea 4 (Cont.) Kinetics New or emphasized: LO 4.7, 4.8: Catalysts function either by lowering activation energy and keeping the same mechanism, or by altering the mechanism by forming an intermediate LO 4.9: Catalysis includes Acid-base catalysis, surface catalysis, enzyme catalysis

20. Big Idea 5 Thermodynamics The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter Includes kinetic theory, specific heat, heating curve, calorimetry and enthalpy changes, intermolecular forces, entropy, Gibb’s free energy, relation between ΔG and K Lab-wise: LO 5.7: calorimetry

21. Big Idea 5 (Cont.) Thermodynamics Exclusions: None New or emphasized: LO 5.1 Create or use graphical representations to connect the dependence of potential energy to distance between atoms, and factors such as bond order and polarity that influence the interaction strength LO 5.2: Drawing of arrows to indicate particle velocities to relate temperature and motion

22. Big Idea 5 (Cont.) Thermodynamics New or emphasized (Cont.): LO 5.3: Heat transfer to establish equilibrium LO 5.6: Heat and PV work in gas expansion and contraction LO 5.9, 5.10, 5.11: IMF in small and large molecules, polymers, enzymes, biological molecules LO 5.13, 5.14: The phrase “thermodynamically favored” in place of “spontaneous”

23. Big Idea 5 (Cont.) Thermodynamics New or emphasized (Cont.): LO 5.15, 5.16, 5.17: External energy source or coupling to make non-TF reactions occur, e.g. electrochemistry, light requirement in photosynthesis, ionization

24. Big Idea 6 Chemical Equilibrium Any bond or intermolecular attraction that can be formed can be broken. These two processes are in a dynamic competition, sensitive to initial conditions and external perturbations Includes equilibrium, Le Chatelier’s principle, acid- base equilibria, pH, pOH, Kw, Ka, Kb, titration, buffers, Ksp, ΔG and K Lab-wise: LO 6.13: acid-base titration; LO 6.18: preparing a buffer

25. Big Idea 6 (Cont.) Chemical Equilibrium Exclusions: Numerical computation of concentrations of species in titration of polyprotic acids Computing the change in pH resulting from addition of acid or base to a buffer Production (derivation) of Henderson-Hasselbalch equation from equilibrium constant expression

26. Big Idea 6 (Cont.) Chemical Equilibrium Exclusions (Cont.): Memorization of solubility rules beyond Na, K, NH 4, and nitrates salts Calculating solubility of salts as a function of pH Calculating solubility of salts in pH-sensitive solutions

27. Big Idea 6 (Cont.) Chemical Equilibrium New or emphasized: LO 6.11 Generate or use a particulate representation of an acid (strong, weak, polyprotic) and a strong base to explain the major species at equilibrium LO 6.24 Analyze the enthalpic and entropic changes during dissolution of a salt, using particulate level interactions and representations LO 6.25: “Exergonic/endergonic”distinction in biological systems involving relationship of K and ΔG

28. Additional Content Deletion Organic Chemistry Nomenclature Nuclear Chemistry Complex Ion / Coordination Chemistry

29. Science Practices 7 Science Practices, p.185-189 Enable students to establish lines of evidence and to develop and refine testable explanations and predictions Require students to think and conduct scientific investigations like working scientists

30. Science Practices The Student Can … SP1: Use representations and models to communicate scientific phenomena and solve scientific problems SP2: Use mathematics appropriately SP3: Engage in scientific questioning to extend thinking or to guide investigations SP4: Plan and implement data collection strategies for a scientific question

31. Science Practices The Student Can … SP5: Perform data analysis and evaluation of evidence SP6: Work with scientific explanation and theories SP7: Connect and relate knowledge across various scales, concepts, and representations in and across domains

32. Activity: Science Practices Example on Handbook p.7 Answer questions on p.8 in your group

33. Science Practices Not Emphasized in Textbooks 1.3: The student can refine representations and models of natural or man-made phenomena and systems in the domain 1.4:The student can use representations and models to analyze situations or solve problems qualitatively and quantitatively 2.1:The student can justify the selection of a mathematical routine to solve problems 3.1-3.3:The student can pose, refine, and evaluate scientific questions

34. Science Practices Not Emphasized in Textbooks 4.1:The student can justify the selection of the kind of data needed to answer a particular scientific question 4.2:The student can design a plan for collecting data to answer a particular scientific question 5.3:The student can evaluate the evidence provided by data sets in relation to a particular scientific question 6.5:The student can evaluate alternative scientific explanations 7.1:The student can connect phenomena and models across spatial and temporal scales

35. What’s Out: Content Nuclear reactions Flame Colors

36. What’s Out: Content Memorization of Conclusions

37. What’s Out: Question Type

39. What’s Out: Content & Question Type Correct statements about alpha particles include which of the following? I.They have a mass number of 4 and a charge of +2. II.They are more penetrating than beta particles. III.They are helium nuclei. (A) I only(B) III only(C)I and II (D) I and III(E) II and III