HADDONFIELD PUBLIC SCHOOLS Curriculum Map for AP Chemistry

Transcription

1 Curriculum Map for AP Chemistry Targeted Standard(s): NJCCCS Interdisciplinary: NJCCCS Technological Literacy 8.1A, 8.1B Enduring Understandings (The big ideas): Sept.-Nov. Essential Questions: What is the basic structure of matter? How can a chemical equation represent chemical reactions quantitatively and qualitatively? How can chemical quantities be manipulated? What are the fundamental qualitative and quantitative principles governing electrochemistry? What are the qualitative and quantitative principles governing equilibrium reactions? Core Content/Objectives Instructional Actions Math Concepts What students will know Lab Safety Atomic Structure, History of the atom Stoichiometry, Identifying, describing, writing and balancing equations, including redox equations Galvanic cells Standard Reduction potentials Line notation Crash course in thermochemistry: though thermochemistry is taught later in the year, Gibbs free energy, enthalpy and entropy are introduced early so that students can understand electrochemistry Work and free energy Dependence of cell potential on concentration (Nernst equation) and operation of a ph meter Electrolytic cells Skills What students will be able to do Application of lab safety principles Explain atomic structure and historical experimental evidence (Dalton, Thomson, Rutherford, Millikan, Bohr, Compton,Einstein) Converting stoichiometric quantities including molar volume,mole ratio, molar mass, molarity, and thermochemical stoichiometric relationships Applying concepts of limiting reagents, percent composition, molecular and empirical formula determination, average atomic mass, relative mass. Demonstrate knowledge of solution stoichiometry including strong, weak and non electrolytes, molarity calculations Application of memorized solubility rules in writingprecipitation reactions Calculations involving acid-base titration Balancing redox equations by the half-reaction method anddescribing oxidation and reduction Identifying and explaining the changes in precipitation, acidbase, and redox reactions. Activities/Strategies Learning Activities/ Differentiation Interdisciplinary Connections Lab: Chromatography of felt-tip pens in various solvent systems, separating components of a mixture Lab: standardization and redox titration using KMnO4 solution and determination of the molar mass of an unknown oxalate Lab: Classifying reactions as precipitation, oxidationreduction, acid-bases and identifying ions present in a solution based on solubility rules Lab: Gravimetric determination of the identify and formula of an unknown halide salt Lab: Creation, operation, and measurement of a galvanic cell and of an electrolytic cell and measurement of effect of concentration and temperature change on E (Nernst equation) Assessment How learning will be assessed Safety quiz Quizzes, tests, lab reports (formal and informal) Authentic AP multiple choice and free response questions Law of mass action Equilibrium characteristics KP, KC (KC is commonly called just K) definitions and applications Manipulating K after adding, subtracting, multiplying, or reversing equations Le Chatelier s principle Heterogeneous equilibria Reaction quotient (Q) Use ΔG = -nfe Define conditions for standard cell potentials Calculate Eo for any reaction at standard conditions Use E = Eo RT/nF (lnq) Describe corrosion Explain the operation of and predict the products resulting from an electrolytic cell Explain the concept of overvoltage and account for the production of Cl2 in aqueous electrolytic cells Lab: Spectrophotometric determination of Keq using the FeSCN2+ ion Reviewed 9-09 Page 1

2 Define equilibrium Write equilibrium expressions and solve equilibrium problems using an ICE chart Use KP = KC(RT)Δn Distinguish equilibrium constant and equilibrium position Qualitatively and quantitatively describe the effect on the position of changing concentrations, pressure (due to a change in volume)), and temperature. Recognize that only temperature changes change the K constant Recognize that adding an inert gas, adding a catalyst, andadding a solid or liquid reagent or product does not shift theposition or change K Write equilibrium expressions for heterogeneous equilibria Resources/Technology: Computers/Lab/ Probleware/MS Word and Excel Textbook technology resources: CDs, simulation software, laserdiscs, videos, etc. Reviewed 9-09 Page 2

3 Targeted Standard(s): NJCCCS Interdisciplinary: NJCCCS Technological Literacy 8.1A, 8.1B Enduring Understandings (The big ideas): Dec. Feb. Essential Questions: What are the qualitative and quantitative principles governing acid/base equilibria? What are the underlying chemical principles that control a substance s acidity or basicity? What are the fundamental reasons for buffers resistance to changes in ph? What changes occur during a titration? What are the quantitative and qualitative principles governing precipitation reactions? What are the properties of complex ions? What are the quantitative and qualitative principles that govern a reaction s rate? What fundamental principles govern nuclear reactions? What are the quantitative and qualitative principles that govern the heat change in chemical reactions? Core Content/Objectives Instructional Actions Math Concepts What students will know ph and poh scale Kw Acid strength vs. concentration (review strong and weak electrolytes) ph of weak acid solutions Percent dissociation Bases Polyprotic acids (exception for sulfuric acid) Acid-base properties of salts Oxides, structure, Lewis acids and bases Common ion effect in buffers and precipitation reactions Buffers Buffering capacity Titrations and ph curves Ksp calculations and relation to solubility and selective precipitation Complex ion equilibria Types of rate laws (integrated and differential) Method of initial rates Writing rate laws Half-life Plots of kinetic data Determining reaction order by graphical method Reaction mechanism Nuclear reactions: alpha, beta decay/bombardment Isotope notation Nature of energy Skills What students will be able to do ph = - log[h+] pk = - log K KaKb = Kw Use and ICE chart to solve acid-base equilibria problems for both Ka and Kb problems Describe the major species in solution Calculate percent dissociation from Ka and vice versa Describe K qualitatively in terms of acid strength Differentiate the definitions of Arrhenius, Bronsted-Lowry and Lewis Recognize and use amines in Kb problems Calculate the ph of a solution of an acidic or basic salt Use electron-withdrawing effects to predict changes in acid strength within a series of oxyacids Calculate the concentration of all species in a buffer solution,including H+ and ph Account for a resistance to change in ph in buffer systems qualitatively and quantitatively. Henderson-Hasselbalch equation (ph = pka + log ([A-]/[HA]) Calculate ph throughout the course of a titration Choice of buffering system based on pka Choice of acid-base indicator based on ph at equivalence point Explain the common ion effect qualitatively and quantitatively Account for the structure and equilibrium behavior of ion complexes. Devise a scheme for the separation of mixtures Activities/Strategies Learning Activities/ Differentiation Interdisciplinary Connections Lab: acid and base standardization, titration, and determinationof the molar mass of an unknown solid acid Lab: ph of solutions of strong, weak, and non acids and basesand salts Lab: titration curves of strong and weak acids and bases anddetermination of an appropriate indicator Lab: creation of a buffer system, measurement of ph, andevaluating resistance of a buffer to ph change Lab: determination of Ka using a ph meter and evaluatingconstancy of Ka after perturbing the system Lab: determination of the rate law of the decomposition ofcrystal violet using both the method of initial rates andgraphical analysis Lab: determination of the heat of combustion of magnesium using Hess Law and calorimetry Assessment How learning will be assessed Safety quiz ; Quizzes, tests, lab reports (formal and informal); Authentic AP multiple choice and free response questions Reviewed 9-09 Page 3

4 Enthalpy and Calorimetry Hess Law Enthalpy of Formation/Combustion Energy Sources Spontaneity, Enthalpy and Entropy Temperature effects on free energy Free energy and chemical reactions (K and Eo dependence) HADDONFIELD PUBLIC SCHOOLS of ions based on selective precipitation and ion complexation Recognize ion complexation, write balanced equations for it, and use it to account for changes in solubility Define rate of reaction in words and graphically for average and instantaneous rate; Writing rate laws from experimental data; Evaluating zero, first and second order rate lawsmathematically and graphically; Determining reaction order and rate constant from experimental data; Half-life determination for first and second order reactions Construct and interpret plots of zero, first, and second order rate laws; Determining rate determining step (RDS), the slow step; Constructing plausible reaction mechanisms from experimental data; Describe collision theory qualitatively, including effects of temperature and entropy ;Describing the effect of catalysts on rate; Write balanced nuclear equations for alpha, beta, positron emission or bombardment ;Describe relative penetration power of different radiation, includinggamma rays; Explain the band of stability; Describe enthalpy change qualitatively and quantitatively; Use calorimetry to determine enthalpy change for a reaction; Use given data (heats of formation/combustion, bond energies, enthalpies of other reactions) to solve for enthalpy change of a reaction.; Describe current and future energy sources.; Explain the qualitativelyand quantitatively the relationship between spontaneity, enthalpy and entropy Resources/Technology: Computers/Lab Probeware/MS Word and Excel; Textbook technology resources: CDs, simulation software, laserdiscs, videos etc. Reviewed 9-09 Page 4

5 Targeted Standard(s): NJCCCS Interdisciplinary: NJCCCS Technological Literacy 8.1A, 8.1B Enduring Understandings (The big ideas): March - June Essential Questions: What is the structure of the atom? How and why do atoms bond to each other? How and why do atoms bond to each other? What are the qualitative principles that govern covalent bonding? What qualitative and quantitative principles affect the study of gases? What forces bond molecules, atoms, and ions in solids, liquids,and gases? What are the properties of gases? What are the properties of condensed states (solids and liquids)? What are the properties of solutions? What are the structures and properties of organic compounds? What are the fundamental principles of experimental design? Core Content/Objectives Instructional Actions Math Concepts What students will know Electromagnetic radiation; Bohr vs. Quantum Mechanical model of the atom; Wave equations; Quantum numbers and electron configuration; Orbital shapes and energies; Periodicity Types of chemical bonds (Ionic vs. covalent character); Bond polarity and dipole moment; Ionic size; Bond energy Lewis structures, including valence shell expansion, formal charge, and resonance structures; VSEPR theory: molecular shape, geometry and molecular polarity; Pi and sigma bonding Ion complexation; Organic chemistry Kinetic molecular theory (KMT) Charles Law, Boyles Law, Gay-Lussac s Law, Dalton s Law, Avogadro s Law, Combined Gas Law, Ideal Gas Law Avogadro s hypothesis Gas stoichiometry Intermolecular forces Heat of vaporization, heat of fusion, heat capacity (also covered in heat changes section) Interparticle forces in crystals Vapor pressure Phase diagrams Colligative properties: boiling point elevation, freezing point depression, vapor pressure lowering and osmotic pressure Organic nomenclature Organic functional groups Basic organic reactions Experimental design Skills What students will be able to do Use E = hv and λ = c/v; Account qualitatively andquantitatively for Planck s discoveries of energy quantization Describe the Bohr model; Give relative energies and shapes for all orbitals; Give quantum numbers for any electron in a ground or excited state.; Give the Aufbau rule and its exceptions (Cr, Cu, etc.); Account qualitatively for wave equations Describe the photoelectric effect qualitatively and quantitatively; Give the fundamental principles controlling periodic trends in ionization energy (first and successive) atomic radius, electron affinity, and electronegativity. Account for exceptions to the expected trend; Predict Bond polarity and dipole moment; Predict Ionic size; Use bond energy to calculate enthalpy of a reaction; Draw Lewis structures, including valence shell expansion, formal charge, and resonance structures; Use VSEPR theory: to predict and draw molecular shape, geometry, and molecular polarity; Calculate lattice energy; Predict hybridization; Explain the concept of molecular orbitals; Recognize ion complexation reactions; Identify basic organic functional groups; Explain paramagnetism and diamagnetism Solve problems for any of the gas laws mentioned above Interconvert moles, grams, and atoms/molecules Describe the KMT qualitatively Explain the a and b factors of the Van der Waals equation and write (but not solve!) the Van der Waals equation for the behavior of Activities/Strategies Learning Activities/ Differentiation Interdisciplinary Connections Lab: modeling compounds (This is a dry lab) Lab: using flame tests and Geissler tubes to determine spectral emission lines and to calculate energy levels using the Bohr equation Lab: Determination of the molar mass of a gas from vapordensity Lab: Determination of the molar volume of hydrogen Lab: Using freezing point depression to determine molar mass of an unknown compound Lab: Constructing a heating curve for water and for an unknown organic solid Lab: modeling organic compounds (Dry lab) Lab: Student-designed lab on a topic of their choice. In thisindependent study, students choose a topic they would like toknow more about and then construct a lab to test or exemplify the principle under consideration Assessment How learning will be assessed Safety quiz ; Quizzes, tests, lab reports (formal and informal) Authentic AP multiple choice and free response questions Reviewed 9-09 Page 5

6 real gases Describe the differences between real and ideal gases Interpret a phase diagram Interpret a heating curve qualitatively and quantitatively Use any colligative property to find the molar mass of a substance Explain colligative effects quantitatively and qualitatively Give all interparticle forces (covalent network, ionic, metallic, and intermolecular), explain how their bonding works and how viscosity, boiling point and surface tension are affected Name all compounds in a homologous series Identify and draw ketone, alcohol, ether, ester, amine, acid, alkane, alkene, alkyne, and halocarbon functional groups Give products for some simple organic reactions (Sn2 reactions, addition reactions etc.) Students will choose a chemical principle that they have studied or which they wish to study and create a laboratory experiment to investigate that concept. Resources/Technology: Computers/Lab Probeware/MS Word and Excel Textbook technology resources: CDs, simulation software, laserdiscs, videos etc Reviewed 9-09 Page 6

7 AP Chemistry Course Syllabus & Timeline Text: Chemistry 6 th edition, Zumdahl Please note that durations and dates are estimated. Chapter(s) and Topics Duration Start Date Test/Quiz Summer Quiz Sep 3 Ch 1, Ch 2 Foundations 1.5 Wks Sep 8 Sep 17 Ch 3 Stoichiometry 1.5 Wks Sep 18 Oct 2 (Fri) Ch 4 Reactions 2 Wks Oct 5 Oct 22 Ch 17 Electrochemistry 1.5 Wks Oct 23 Nov 12 Professional Development week Ch 13 Equilibrium 2 Wks Nov 13 Nov 30 Includes Spirit Week/Thanksgiving Ch 14 Acid/Base Equilibrium 2.5 Wks Dec 1 Dec 21 Ch 15 Solution Equilibrium 2.5 Wks Dec 22 Jan 21 Includes Winter Break Ch 12, 18 Kinetics and Nuclear Chem 2.5 Wks Jan 22 Feb 8 Includes Midterms Ch 6, Ch 16 Thermochemistry 1.5 Wks Feb 9 Feb 22 Ch 7 Atomic Structure 2 Wks Feb 23 Mar 8 Includes HSPA testing. Take home assignments will be given during this time period because of missed instructional time Ch 8, 9, 21, 22 Bonding 2 Wks Mar 9 Mar 22 Ch 5 Gases 1.5 weeks Mar 23 Apr 12 Reviewed 9-09 Page 7

8 Includes Spring Break HADDONFIELD PUBLIC SCHOOLS Ch 10, 11 Solids and Liquids 1 Wk Apr 13 Apr 19 Practice/Review 3 Wks Apr 20 AP Chemistry Exam Tuesday, May 11, 2010, 7:30am By Marking Period: Ch 1, Ch 2 Foundations Ch 3 Stoichiometry Ch 4 Reactions 1 st Marking Period Ch 17 Electrochemistry Ch 13 Equilibrium Ch 14 Acid/Base Equilibrium Ch 15 Applications of Aqueous Equilibria 2 nd Marking Period Ch 12, 18 Kinetics and Nuclear Chemistry Ch 6, Ch 16 Thermochemistry Ch 7 Atomic Structure 3 rd Marking Period Ch 8, 9, 21, 22 Bonding Reviewed 9-09 Page 8

9 Ch 5 Gases Ch 10, 11 Solids and Liquids Review and Practice HADDONFIELD PUBLIC SCHOOLS 4 th Marking Period Reviewed 9-09 Page 9