Advanced Placement Chemistry. High School

Transcription

1 Planned Course of Study dvanced Placement Chemistry High School NORTHWESTERN LEHIGH SCHOOL DISTRICT 6493 ROUTE 309 NEW TRIPOLI, P 8066

2 NORTHWESTERN LEHIGH SCHOOL BORD 0 Gregory W. Snyder, President Sally Schoffstall, Esq., Vice President Donald Link, Secretary Willard Dellicker, Treasurer Camille S. Bartlett Todd Hernandez Christopher Ford Darryl S. Schafer Michael Marich John E. Freund III, Esq., Solicitor DMINISTRTION Dr. Mary nne Wright, Superintendent Jennifer Holman, ssistant Superintendent Dr. Mark Scott, Director of Pupil Services Luann E. Matika, Director of Human Resources Lenn M. Stitzel, Director of Curriculum and Technology ileen M. Yadush, High School Principal Donald llen, ssistant High School Principal Laurie Hoppes, Middle School Principal my Wahl, Middle School ssistant Principal Jill Berlet, Northwestern Elementary Principal Marc Dobbs, Weisenberg Elementary Principal

3 TBLE OF CONTENTS Introduction and 4 Description Course Outline 5-37

4 INTRODUCTION The dvanced Placement Chemistry curriculum guide contains planned course formats for the Northwestern Lehigh School District. The content of this document describes the objectives, activities, assessments, content, time frame, and standard alignment that serve as a guide to the specific units of study offered in dvanced Placement Chemistry. The dvanced Placement Chemistry curriculum guide is the product of much diligent work on the part of the following members of the Science department who contributed during the 00- school years: Stephen Gensits This document reflects their efforts to establish a well-defined and organized approach to teaching Science in the Northwestern Lehigh School District. pproved by Northwestern Lehigh School District Board of Education July 0 LEVEL OF MSTERY DESCRIPTIONS Recognition (R) pplication () Inference (I) Students will be able to recall concepts. Students will be able to apply ideas/skills to a curricular concept. Students will be able to evaluate and synthesize materials or concepts.

5 Curriculum Units. Introduction: Matter and Measurement. toms, Molecules, and Ions 3. Stoichiometry: Calculations with Chemical Formulas and Equations 4. queous Reactions and Solution Stoichiometry 5. Thermochemistry 6. Electronic Structure of toms 7. Periodic Properties of the Elements 8. Basic Concepts of Chemical Bonding 9. Molecular Geometry and Bonding Theories 0. Gases. Intermolecular Forces, Liquids, and Solids. Properties of Solutions 3. Chemical Kinetics 4. Chemical Equilibrium 5. cid-base Equilibria 6. dditional spects of queous Equilibria 7. Chemical Thermodynamics 8. Electrochemistry 9. Nuclear Chemistry 0. Preparation for the Chemistry dvanced Placement Examination. Individual Laboratory Experimentation and Demonstration

6 Introduction: Matter and Measurement - differentiate between physical properties and chemical properties - classify physical or chemical changes within a system in terms of matter and/or energy - differentiate between pure substances and mixtures; differentiate between heterogeneous and homogeneous mixtures - predict how combinations of substances can result in physical and/or chemical changes - make accurate and precise measurements of mass, length, volume and temperature using metric units - utilize significant figures to communicate the uncertainty in a quantitative observation 3..C. 3..C.5 3..C.5 3..C. S C.3 3..C.3 - determine percent error 3..C.3 - characterize data in terms of precision and accuracy 3..C.3 I Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Class ctivity: Why Does Popcorn Pop? - Chapter One Quiz - Lab: The Identity of an Unknown Compound from Qualitative Observations - Lab: Drano vs. Sani-Flush, What s the Difference s - Chapters - 3 Test - Class Lecture and Discussion - Reading ssignments and - Measurements Problem Set - Lab: The Laboratory and SI - Chapter One Quiz - Chapters - 3 Test - Class ctivity: Calculating Percent Error - Reading ssignments and - Measurements Problem Set - Chapter One Quiz - Chapters - 3 Test 3

7 - recall and convert metric system units - do unit conversions using the factor label method. 3..C.3 3..C.3 - Class Lecture - Reading ssignments and - Measurements Problem Set - Chapter One Quiz - Lab: The Laboratory and SI - Chapters - 3 Test 3

8 toms, Molecules, and Ions - describe the historical development of models of the atom and how each discovery contributed to modern theory - recognize discoveries from Dalton (atomic theory), Thomson (the electron), and Rutherford (the nucleus) - describe Rutherford s gold foil experiment that led to the discovery of the nuclear atom - identify the major components (protons, neutrons, and electrons) of the nuclear atom and explain how they interact - distinguish among the isotopic forms of elements C C C C C C.5 3..C.5 3..C.5 S C. 3..C R R Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Chapter Two Quiz - Chapters - 3 Test

9 - experimentally determine the composition of a substance using analytical gravimetric techniques - interpret and apply the laws of conservation of mass, constant composition (definite proportions), and multiple proportions - explain why compounds are composed of integer ratios of elements - predict chemical formulas based on the number of valence electrons - predict the chemical formulas for simple molecules and ionic compounds. - Lab: Gravimetric nalysis of a Chloride Salt - Lab Report I - Class Lecture and Discussion - Reading ssignments and - Chapter Two Quiz - Chapters - 3 Test - Class Lecture and Discussion - Reading ssignments and - Dry Lab : Oxidation Numbers - Dry Lab 3: Inorganic Nomenclature: Binary Compounds - Dry Lab 4: Inorganic Nomenclature: Ternary Compounds - Chapter Two Quiz - Chapter Two Quiz - Chapters - 3 Test - Periodic Table - Table of Polyatomic Ions 3

10 Stoichiometry: Calculations with Chemical Formulas and Equations - describe chemical reactions in terms of atomic rearrangement and/or electron transfer - balance chemical equations by applying the laws of conservation of mass - use the mole concept to determine the number of particles and molar mass for elements and compounds - determine percent compositions, empirical formulas, and molecular formulas - experimentally determine the chemical formula for a compound - experimentally determine the percentage of water in a hydrate S... S..3. S Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Class ctivity: How Large is a Mole? - Stoichiometry Problem Set - Chapter Three Quiz - Chapters 3 Test - Lab: Empirical Formula of a Compound - Lab: Formula of a Hydrate

11 - predict the amounts of products and reactants in a chemical reaction using mole relationships - experimentally determine the mass and mole relationships in a chemical reaction - use stoichiometry to predict quantitative relationships in a chemical reaction S S...3 I - Class Lecture and Discussion - Reading ssignments and - Chapter Three Quiz - Lab: Chemical Reactions of Copper and Percent Yield - Chapter Three Problem Set - Chapters 3 Test - Class Lecture and Discussion - Reading ssignments and - Lab: Synthesis of Barium Sulfate and Percent Yield - Chapters 3 Test

12 queous Reactions and Solution Stoichiometry - classify chemical reactions as synthesis (combination), decomposition, single displacement (replacement), double displacement (replacement), and composition - predict whether precipitation will occur as a result of a double displacement reaction - experimentally separate and analyze unknown solids and solutions of cations and anions - predict and identify the products of a chemical reaction S...3 Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Chapter Four Quiz - Chapters 4-6 Test - Class Lecture and Discussion - Reading ssignments and - Lab: Inorganic Compounds and Metathesis Reactions - Lab: Small-Scale One Pot Reactions of Copper, Iron, and Silver - Lab Reports - Chapter Four Quiz - Chapters 4-6 Test 6

13 Thermochemistry - explain the difference between endothermic and exothermic reactions - explain the high specific heat of water and its use in calorimetry - experimentally determine the enthalpy change associated with a chemical reaction - explain how energy, heat, and work are related - construct and use a calorimeter to measure heat flow Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and I - Chapter Five Quiz - Thermochemistry Problem Set - Chapters 4-6 Test - Lab: Determining the Heat of Reaction 3..0.B I - Class Lecture and Discussion - Reading ssignments and - Chapter Five Quiz - Chapters 4-6 Test Lab: Determining the Heat of Reaction - Minilab: Heat of Fusion of Water - Lab: Calorimetry: The Heat Capacity of Metals s 3

14 - solve for the enthalpy change that occurs when a substance melts, freezes, boils, condenses, or dissolves - solve for energy changes by using Hess s law of standard heats of formation Class Lecture and Discussion - Reading ssignments and - Chapter Five Quiz - Chapters 4-6 Test - Thermochemistry Problem Set - Minilab: Heat of Fusion of Water - Class Lecture and Discussion - Reading ssignments and - Chapter Five Quiz - Thermochemistry Problem Set - Chapters 4-6 Test

15 Electronic Structure of toms - recognize the discoveries of Thomson (the electron) and Bohr (planetary model of the atom), and how each discovery leads to modern theory - describe the historical development of models of the atom and how they contributed to modern atomic theory - compare the electron configurations for the elements found on the periodic table - state and apply the laws and rules by which electrons are added to atoms C C C C C C C C. I Suggested ctivity and ssessment - Classroom Lecture and Discussion - Reading ssignments and - Chapter Six Quiz - Chapters 4 6 Test - Minilab: Electron Configurations of toms - Classroom Lecture and Discussion - Reading ssignments and - Chapter Six Quiz - Chapter Six Quiz - Electronic Structure Problem Set - Chapters 4-6 Test - Periodic Table

16 - explain how light is absorbed or emitted by electron orbital transitions - explain how the frequencies of emitted light are related to changes in electron energies 3... S..3.3 I - Classroom Lecture and Discussion - Reading ssignments and - Chapter Six Quiz - Electronic Structure Problem Set - Chapters 4-6 Test - Lab: Spectrum of Hydrogen - Lab: Flame Tests s Classroom Lecture and Discussion - Reading ssignments and - Chapter Six Quiz - Electronic Structure Problem Set - Chapters 4-6 Test - Lab: Spectrum of Hydrogen - Lab: Flame Tests s 3

17 Periodic Properties of the Elements - predict properties of elements using trends of the periodic table - relate the position of an element on the periodic table to its electron configuration and compare its reactivity to other elements in the table - explain the relationship of an element s position on the periodic table to its atomic number, ionization energy, electronegativity, atomic size, and classification of elements - describe the group trends of the elements on the periodic table - write chemical equations describing the reactions of elements based upon their location on the periodic table S C. Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and I - Chapter Seven Quiz - Chapter Seven Quiz - Chapters 7-9 Test - Demo: lkali Metals - Lab: Periodic Table and Periodic Law I - Class Lecture and Discussion - Reading ssignments and - Chapter Seven Quiz - Chapter Seven Quiz - Chapters 7-9 Test - Lab: Periodic Table and Periodic Law - Class Lecture and Discussion - Reading ssignments and - Chapter Seven Quiz - Chapters 7-9 Test - Lab: Chemical Puzzle - Periodic Tables - Periodic Tables - Periodic Tables 4

18 - compare the properties of metals, nonmetals, metalloids, and noble gases. 3..C. I - Class Lecture and Discussion - Reading ssignments and - Chapter Seven Quiz - Chapters 7-9 Test - Periodic Tables

19 Basic Concepts of Chemical Bonding - draw Lewis (electron) dot structures for elements. - explain how atoms combine to form compounds through both ionic and covalent bonding - compare and contrast different bond types that result in the formation of molecules and compounds - explain the relationship of an element s position on the periodic table to its electronegativity - use electronegativity to explain the difference between polar and nonpolar covalent bonds S S... Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Chapter Eight Quiz - Chapters 7 9 Test - Class Lecture and Discussion - Reading ssignments and - Chapter Eight Quiz - Chapters 7 9 Test - Lab: Chemicals in Everyday Life 3..C. - Class Lecture and Discussion - Reading ssignments and Questions - Chapter Eight Quiz - Chapters 7 9 Test 3..C I - Class Lecture and Discussion - Reading ssignments and - Chapter Eight Quiz - Chapters 7 9 Test - Periodic Tables - Periodic Tables - Periodic Tables - Periodic Tables 3

20 Molecular Geometry and Bonding Theories - draw Lewis dot structures for simple molecules and ionic compounds - use VSEPR theory to predict the molecular geometry of simple molecules - describe the relationship between atomic and molecular orbitals - identify ways in which orbital hybridization is useful in describing molecules. 3..C S S I Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Lab: Molecular Geometries and Polarity - Chapter Nine Quiz - Chapters 7 9 Test - Class Lecture and Discussion - Reading ssignments and - Chapter Nine Quiz - Chapters 7 9 Test - Periodic Table - Table of Molecular Geometries 3

21 Gases - describe phases of matter according to the kinetic molecular theory - describe the three normal states of matter in terms of energy, particle motion, and phase transitions - relate Kelvin-scale and Celsiusscale temperatures - describe the relationship between the average kinetic molecular energy, temperature, and phase changes - predict the behavior of gases through the application of laws (i.e., Boyle s law, Charles law, or ideal gas law) - experimentally determine the molar mass of a volatile liquid S C.3 S C.3 S B C.3 S C.3 I Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Demo: Kinetic Molecular Theory - Chapter Ten Quiz - Chapters 0 3 Test - Gases Problem Set - Class Lecture and Discussion - Reading ssignments and - Chapter Ten Quiz # - Chapter Ten Quiz # - Chapters 0 3 Test - Gases Problem Set - Lab: Determining the Molar Mass of Butane - Lab: Formula Mass of a Volatile Liquid - Periodic Tables 3

22 - experimentally determine the molar volume of a gas under standard conditions - relate how volumes of gases react in terms of the kinetic theory of gases C.3 - Lab: KClO 3 Mixture and the Molar Volume of Oxygen I - Class Lecture and Discussion - Reading ssignments and - Chapter Ten Quiz # - Chapters 0 3 Test - Gases Problem Set - Periodic Tables

23 Intermolecular Forces, Liquids, and Solids - compare, using examples, the effect of covalent and ionic bonding on the physical properties of matter - explain the unique properties of water (polarity, high boiling point, and hydrogen bonding) that support life on Earth - compare and contrast the unique properties of water to other liquids - describe the three normal states of matter in terms of energy, particle motion, and phase transitions - describe the type(s) of intermolecular forces found between particles in a substance 3..C. 3..C.3 S C. 3..C C.3 3..C.3 S C I I I Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Chapter Eleven Quiz # - Chapters 0 3 Test R - Class Lecture and Discussion - Reading ssignments and - Chapter Eleven Quiz # - Chapters 0 3 Test - Minilab: The Triple Point of Carbon Dioxide - Class Lecture and Discussion - Reading ssignments and - Chapter Eleven Quiz # - Chapter Eleven Quiz # - Chapters 0 3 Test - Minilab: Intermolecular Forces s

24 - evaluate the strength of intermolecular attractions compared with the strength of ionic and covalent bonds - experimentally use chromatography to separate the components in a mixture Class Lecture and Discussion - Reading ssignments and - Chapter Eleven Quiz # - Chapters 0 3 Test - Lab: Thin-Layer Chromatography

25 Properties of Solutions - compare and contrast colligative properties of mixtures - describe the solution process on the molecular level - express the concentration of a solution using mass percentage, mole fraction, molarity, and molality - experimentally determine the molar mass of a solid by freezing point depression - describe the factors affecting the solubility of substances Suggested ctivity and ssessment Class Lecture and Discussion - Reading ssignments and - Chapter Thirteen Quiz - Chapters 0-3 Test 3..C C R - Class Lecture and Discussion - Reading ssignments and - Chapter Thirteen Quiz - Chapters 0-3 Test - Class Lecture and Discussion - Reading ssignments and - Chapter Thirteen Quiz - Chapters 0-3 Test - Lab: Molar Mass of a Solid - Class Lecture and Discussion - Reading ssignments and - Chapter Thirteen Quiz - Chapters 0-3 Test

26 Chemical Kinetics - identify the factors that affect the rates of reactions - describe how changes in energy affect the rate of chemical reactions - explain the difference between an endothermic process and an exothermic process C C.B3 - define the rate of reaction S determine the instantaneous rate S...3 of reaction - write the rate laws of reactions S...3 I and determine the overall order of the reaction - determine the order of reaction and value of the rate constant by the method of initial rates S...3 S... S experimentally determine the rate of a chemical reaction and its order S...3 S... S..3.3 Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Kinetics Problem Set - Chapter Fourteen Quiz - Lab: Rates of Chemical Reactions - Chapters 4 7 Test - Class Lecture and Discussion - Reading ssignments and - Kinetics Problem Set - Chapter Fourteen Quiz - Chapter Fourteen Quiz - Lab: Rates of Chemical Reactions - Chapters 4 7 Test - Lab: Hypokinetics 3

27 - relate the rate of chemical reactions to the frequency of molecular collisions and effectiveness of collisions - determine possible reaction mechanisms for a chemical reaction given its rate law S... S... S..3.3 S... S..3. I - Class Lecture and Discussion - Reading ssignments and - Kinetics Problem Set - Chapter Fourteen Quiz - Chapters 4-7 Test

28 Chemical Equilibrium - predict the shift in equilibrium when a system is subjected to a stress - describe how the amounts of reactants and products change in a chemical system at equilibrium - calculate the concentrations of all chemical species in a solution at equilibrium S...3 S..3. S..3. S...3 S..3. Suggested ctivity and ssessment I - Class Lecture and Discussion - Reading ssignments and - Chemical Equilibrium Problem Set - Chapter Fifteen Quiz - Chapters 4 7 Test - Class Lecture and Discussion - Reading ssignments and - Chemical Equilibrium Problem Set - Lab: LeChatelier s Principle - Chapter Fifteen Quiz - Chapters 4 7 Test S Class Lecture and Discussion - Reading ssignments and - Chemical Equilibrium Problem Set - Chapter Fifteen Quiz - Chapter Fifteen Quiz - Chapters 4 7 Test

29 - explain the relationship between the value of an equilibrium constant and the position of equilibrium - experimentally determine the equilibrium constant for a chemical reaction. S Class Lecture and Discussion - Reading ssignments and - Chemical Equilibrium Problem Set - Chapter Fifteen Quiz - Chapter Fifteen Quiz - Chapters 4 7 Test S...3 S... S... - Lab: Colorimetric Determination of an Equilibrium Constant in queous Solution

30 cid-base Equilibria - predict the shift in equilibrium when a system is subjected to a stress - calculate the ph of strong acid, strong base, weak acid, and weak base solutions - determine the equilibrium constants for weak basic and weak acid solutions from the concentration of species in the solution S...3 S..3. S..3. S...3 Suggested ctivity and ssessment I - Class Lecture and Discussion - Reading ssignments and - cid-base Equilibria Problem Set - Chapter Sixteen Quiz - Chapters 4 7 Test - Class Lecture and Discussion - Reading ssignments and - cid-base Equilibria Problem Set - Chapter Sixteen Quiz - Chapters 4 7 Test - Lab: Lewis cids S Class Lecture and Discussion - Reading ssignments and - cid-base Equilibria Problem Set - Chapter Sixteen Quiz - Chapters 4 7 Test

31 - calculate ph values for salts and polyprotic acids - experimentally standardize a solution using a primary standard - experimentally determine the concentration of a weak acid by acid-base titration - experimentally determine the appropriate indicators to use for various acid-base titrations and ph determination - experimentally prepare and describe the properties of buffer solutions S...3 S..3. S...3 S... S...3 S... S... S..3. S...3 S... S..3. S...3 S... - Class Lecture and Discussion - Reading ssignments and - cid-base Equilibria Problem Set - Chapter Sixteen Quiz - Chapters 4 7 Test - Lab: Titration of cids and Bases - Lab: cids, Bases, and Indicators - Lab: Buffers

32 dditional spects of queous Equilibria - predict the shift in equilibrium when a system is subjected to a stress - define the solubility constant and use it to compare the relative solubilities of compounds - calculate the equilibrium concentrations of substances using K eq - describe the common ion effect and calculate the equilibrium concentrations of ions when more than one source of an ion is present S...3 S..3. S..3. S...3 Suggested ctivity and ssessment I - Class Lecture and Discussion - Reading ssignments and - queous Equilibria Problem Set - Chapter Seventeen Quiz - Chapters 4 7 Test - Class Lecture and Discussion - Reading ssignments and - queous Equilibria Problem Set - Chapter Seventeen Quiz - Chapters 4 7 Test S Class Lecture and Discussion - Reading ssignments and - queous Equilibria Problem Set - Chapter Seventeen Quiz - Chapters 4 7 Test S...3 S..3. I - Class Lecture and Discussion - Reading ssignments and - queous Equilibria Problem Set - Chapter Seventeen Quiz - Chapters 4 7 Test

33 - experimentally synthesize and chemically analyze a coordination compound. S... S... - Lab: Preparation and Reactions of Coordination Compounds: Oxalate Complexes

34 Chemical Thermodynamics - explain the natural tendency for systems to move in a direction of disorder or randomness (entropy) - describe the law of conservation of energy - explain how the behavior of matter and energy follow predictable patterns that are defined by laws 3..C.B S... S...3 S..3. S..3. S C.B3 S...3 S..3.3 S.C B6 S...3 S..3. S..3.3 S.C.. - define a spontaneous process S...3 S determine the spontaneity of a chemical process using standard free energy - experimentally synthesize, purify, and chemically analyze an organic compound I Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Thermodynamics Problem Set - Chapter Nineteen Quiz - Chapters 9 Test - Demonstration: Endothermic Reaction S Class Lecture and Discussion - Reading ssignments and - Thermodynamics Problem Set - Chapter Nineteen Quiz - Chapters 9 Test S... S... - Lab: Preparation of spirin and Oil of Wintergreen - Lab: nalysis of spirin s 3

35 Electrochemistry - apply oxidation/reduction principles to electrochemical reactions. - identify the substance oxidized or reduced, the oxidizing agent and the reducing agent in a redox reaction Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Electrochemistry Problem Set - Chapter Twenty Quiz - Chapters 9 Test - Lab: Redox Reactions - balance redox equations - Class Lecture and Discussion - Reading ssignments and - Electrochemistry Problem Set - Chapter Twenty Quiz - Chapters 9 Test - Dry Lab Six: Balancing Redox Equations - calculate the standard emf for a voltaic cell - experimentally determine an electrochemical series S.C.. S... S...3 S.C.. - Class Lecture and Discussion - Reading ssignments and - Electrochemistry Problem Set - Chapter Twenty Quiz - Chapter Twenty Quiz - Chapters 9 Test - Lab: ctivity Series

36 - determine the spontaneity of an electrochemical process - draw a cell diagram describing an electrochemical process - experimentally determine the concentration of a solution by oxidation-reduction titration - experimentally use electrochemical cells and electroplating to make measurements. S.C.. S.C.. S... S...3 S.C.. S... S...3 S.C.. - Class Lecture and Discussion - Reading ssignments and - Electrochemistry Problem Set - Chapter Twenty Quiz - Chapters 9 Test - Class Lecture and Discussion - Reading ssignments and - Electrochemistry Problem Set - Chapter Twenty Quiz - Chapters 9 Test - Lab: Oxidation-Reduction Titration: Determination of Oxalate - Lab: Galvanic Cells

37 Nuclear Chemistry - identify the three main types of radioactive decay and compare their properties - explain the probabilistic nature of radioactive decay based on subatomic rearrangement in the atomic nucleus - explain how matter is transformed into energy in nuclear reactions according to the equation E = mc - describe the relationship between nuclear particles and nuclear stability - write nuclear equations describing various modes of nuclear decay - describe the processes of nuclear fission and nuclear fusion. 3..C S..3. S.C.. S.C.. S.C.. S.C.. R I Suggested ctivity and ssessment - Class Lecture and Discussion - Reading ssignments and - Chapter Twenty-One Quiz - Chapters 9 Test - Class Lecture and Discussion - Reading ssignments and - Chapter Twenty-One Quiz - Chapters 9 Test - Class Lecture and Discussion - Reading ssignments and - Chapter Twenty-One Quiz - Chapters 9 Test - Laptop