Wallingford Public Schools - HIGH SCHOOL COURSE OUTLINE. Department: Science Grade(s): 11-12

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1 Wallingford Public Schools - HIGH SCHOOL COURSE OUTLINE Course Title: Advanced Placement Chemistry Course Number: 2352 Department: Science Grade(s): Level(s): Advanced Placement Credit: 1.5 Course Description AP Chemistry is the equivalent of the general chemistry course usually taken during the first years of college and is designed to follow the successful completion of a high school chemistry course, such as Academic or Honors Chemistry. Topics covered include the structure of matter, kinetic theory of gases, chemical equilibria, chemical kinetics, and the basic concepts of thermodynamics. Strong emphasis is placed on chemical calculations and the mathematical formulations of principles. The course should contribute to the development of the students abilities to think clearly and to express their ideas, orally and in writing, with clarity and logic. This rigorous course is intended for students who have demonstrated a willingness to commit considerable time to studying and completing assignments outside of the classroom. (Prerequisite: Chemistry A or H) Required Instructional Materials Brown LeMay, Bursten, Chemistry the Central Science, Brown, LeMay, Bursten, Preparing for the Chemistry AP Exam, Current and sufficient laboratory materials and equipment for each of the learning strands Appropriate safety equipment goggles, aprons, eyewash, safety shower, etc. Information technologies internet and library resources Completion/Revision Date Revisions Approved by Board of Education on July 17, 2006 Mission Statement of the Curriculum Management Team The mission statement of the Science Curriculum Management Team is to promote scientific literacy emphasizing the process, content, and interdisciplinary nature of science. Enduring Understandings for the Course Inquiry is the integration of process skills, the application of scientific content and critical thinking to solve problems. Science is the method of observation and investigation used to understand our world. AP Chemistry involves many fundamental terms that are use in daily life, examples: solution, mixture, element and compound, etc. Accuracy and precision are essential tools for careers such as medical, pharmaceutical, engineering, etc. AP Chemistry Page 1 of 26

2 Technological tools have helped scientists to update theories that describe the nature of atoms. The Periodic Table is arranged in a logical sequence that can be used to predict the properties of elements. Atoms gain or lose electrons to form ions which can be used to predict the empirical formulas of ionic compounds. There is a systematic nomenclature for naming inorganic compounds. Chemistry has rules that govern how to express chemical formulas and equations, similar to the rules of grammar. The mole concept can be applied to predict the outcome of chemical reactions. One of the most important properties of water is its ability to dissolve a wide variety of substances. Many chemical reactions occur while in aqueous solutions. The study of energy is applicable to chemical and biological reaction such as metabolism, respiration, photosynthesis, and various industrial applications such as the automobile engine. Wave-like properties of electromagnetic radiation are used to demonstrate electron placement in the atom. Our knowledge of electronic structure is directly related to understanding the Quantum Mechanical Model, a twentieth century development. Many properties of atoms depend on both the net attraction between the nucleus and the outer electrons and on the average distance of those electrons from the nucleus. There are periodic trends that demonstrate several key properties of atoms electron affinity, electronegativity, atomic radius, ionization energy and metallic character. The periodic table is useful in predicting periodic trends and periodic properties. Different kinds of chemical bonding occur based on the electron arrangement of elements. Intricate diagrams can be used to pictorially represent microscopic molecular structures. Molecular shapes and geometry can be predicted by electron placement around individually bonded atoms. Lewis structures provide explanations for multiple bonds and bond shape. Gases present different physical and chemical properties from solids and liquids. Pressure and temperature are important factors in viewing the kinetic molecular theory with gases. Intermolecular forces between neutral molecules depend on their molecular polarity, size, and shape. Solids, liquids, and gases display vastly different kinetic behavior at different temperatures. Arrangements of atoms within the individual states of solid, liquid, and gas can be visualized through an understanding of the forces that hold them together. Aqueous solutions of ionic substances are very important to our daily lives (i.e. air, ocean, fuels, living fluids, etc.) Colligative properties of solutions provide insight into the physical nature of their solute molecules. Reactions are dynamic and their rate can be influenced by different variables. Chemical equilibrium occurs when opposing reactions are proceeding at equal rates. Acids and bases are ubiquitous and important in innumerable chemical processes in industry, biology, and the environment. AP Chemistry Page 2 of 26

3 A large part of the chemical industry can be understood in terms of acid-base reactions. The physical and chemical characteristics of water make it uniquely important in almost all chemical reactions that take place in or on this planet. Spontaneous thermochemical processes are closely tied to energy and equilibrium. There is a systematic process for balancing redox reactions by the half reaction method. Oxidation-reduction reactions are very common and truly important chemical reactions in our everyday lives. There is a distinctive difference between a chemical reaction and a nuclear reaction. Nuclear chemistry affects our lives in a variety of ways. Genetic information provides both similarities and differences between two organisms and is transferred from one generation to the next by the replication of molecules of DNA. AP Chemistry Page 3 of 26

4 1.0 Scientific Reasoning and Communication Skills NOTE: This learning strand should be taught through the integration of the other learning strands. This learning strand is not meant to be taught in isolation as a separate unit. Inquiry is the integration of process skills, the application of scientific content and critical thinking to solve problems. Science is the method of observation and investigation used to understand our world. LEARNING OBJECTIVES The student will: 1.1 Generate scientific questions to be investigated. 1.2 Read, interpret and examine the credibility and validity of scientific claims in different sources of information. 1.3 Formulate a testable hypothesis in the If then because form that demonstrates logical connections between the scientific concepts guiding the hypothesis and the design of the experiment. 1.4 Design and conduct appropriate types of scientific investigations to answer different questions. 1.5 Identify independent and dependent variables, including those that are kept constant and those used as controls. 1.6 Apply appropriate instruments needed to make observations and collect data precisely. 1.7 Analyze experimental design and data to question validity/reliability, identify variables, and improve experimental design. 1.8 Develop conclusions based on critical data analysis identifying further investigations and/or questions based on the results. 1.9 Use mathematical operations to analyze and interpret data, and present relationships between variables in appropriate forms (tables, graphs, etc.) 1.10 Utilize graphs in order to determine How is inquiry used to solve problems or gather data to better understand a situation? How do you evaluate data and conclusions to determine its validity? How do prior knowledge, bias, and opinion affect inquiry? How does new knowledge gained create new questions? Sufficient laboratory instrumentation Laboratory Exercise: Methods and Measurement in the Laboratory Inquiry Hands-on, minds-on lab activities See other learning strands for integration Lab reports Open-ended questions Teacher observations Essays and/or compositions Research based projects See other learning strands for integration AP Chemistry Page 4 of 26

5 patterns and make predictions Apply computer-based tools to present and research information Gather information using a variety of print and non-print sources Support scientific arguments using a variety of print and non-print sources Communicate about science in different formats using relevant science vocabulary, supporting evidence and clear logic. AP Chemistry Page 5 of 26

6 2.0 Matter and Measurement AP Chemistry involves many fundamental terms that are used in daily life, examples: solution, mixture, element and compound, etc. Accuracy and precision are essential tools for careers such as medical, pharmaceutical, engineering, etc. Technological tools have helped scientists to update theories that describe the nature of atoms. The Periodic Table is arranged in a logical sequence that can be used to predict the properties of elements. Atoms gain or lose electrons to form ions which can be used to predict the empirical formulas of ionic compounds. There is a systematic nomenclature for naming inorganic compounds. 2.1 Examine ways to classify materials pure substances and mixtures elements and.compounds. 2.2 Separate and characterize substances based on their properties. 2.3 Choose appropriate measurement tools and units for a specific purpose. 2.4 Measure accurately using metric units and SI units. Why do many chemical properties rely on quantitative measurements, involving both numbers and units? How do we characterize, identify, and separate chemical substances? Laboratory materials Problem solving Group work Laboratory Exercise: Determination of the formula of a compound Analytical gravimetric determination AP Chemistry Page 6 of 26

7 AP Chemistry Page 7 of 26

8 3.0 Atoms, Molecules, and Ions Technological tools have helped scientists to update theories that describe the nature of atoms. The Periodic Table is arranged in a logical sequence that can be used to predict the properties of elements. Atoms gain or lose electrons to form ions which can be used to predict the empirical formulas of ionic compounds. There is a systematic nomenclature for naming inorganic compounds. 3.1 Understand the discovery and development of the modern nuclear model of the atom 3.2 Name and assemble ionic, molecular, and empirical formulas. 3.3 Discuss the development behind the organization of the modern periodic table. 3.4 Write correct nomenclature to ionic and molecular compounds. 3.5 Differentiate between an atom, ion, isotope and molecule. How do all the materials in the world exhibit striking and seemingly infinite variety of properties, including different colors, textures, solubilities, and chemical reactivities? Laboratory materials Problem solving Group work Laboratory investigation: Determination of the water of hydration in a hydrated salt AP Chemistry Page 8 of 26

9 4.0 Stoichiometry: Calculations with Chemical Formulas and Equations Chemistry has rules that govern how to express chemical formulas and equations, similar to the rules of grammar. The mole concept can be applied to predict the outcome of chemical reactions. 4.1 Use chemical formulas to write chemical equations that represent chemical reactions 4.2 Develop a facility with the mole concept and apply it to chemical reactions 4.3 Predict the amounts of substances consumed and/or produced in a chemical reaction 4.4 Determine which reactant is in excess and which is the limiting reactant How does the chemical formula and chemical equation provide important quantitative information about the substances that it represents? What rules do scientists follow when writing chemical equations? Laboratory materials Problem solving Group work Laboratory investigation: Determination of mass and mole relationships in chemical reactions AP Chemistry Page 9 of 26

10 5.0 Aqueous Reactions and Solution Stoichiometry One of the most important properties of water is its ability to dissolve a wide variety of substances. Many chemical reactions occur while in aqueous solutions. Why is water so unusual in its ability to dissolve so many other substances? Why are many of the chemical reactions that take place within us and around us occurring in water solutions? How can the concentrations of solutions be expressed quantitatively and be used to predict the outcome of aqueous chemical reactions? 5.1 Differentiate between the three basic types of chemical processes that occur in aqueous solutions: Precipitation reactions Acid-base reactions Oxidation-reduction reactions 5.2 Demonstrate how to write net ionic equations. 5.3 Consider how the concentration of a solution is determined. 5.4 Solve for an unknown solution concentration by using a known solution concentration. Laboratory materials Laboratory Exercise: Redox titration Separation and qualitative analysis of cations and anions Thermite demonstration AP Chemistry Page 10 of 26

11 6.0 Thermochemistry The study of energy is applicable to chemical and biological reaction such as metabolism, respiration, photosynthesis, and various industrial applications such as the automobile engine. 6.1 Recognize the nature of energy and its changes supporting the first law of thermodynamics. 6.2 Relate enthalpy as a state function to determine heat lost or gained by a system in a process such as a chemical reaction. 6.3 Demonstrate how calorimetry is related to foods and fuels. Why does modern society depend so much on energy for its existence? What chemical and thermal reactions occur daily that determine human well-being and comfort? Laboratory materials Laboratory Exercise: Calorimetry and specific heat Hess s Law Determination of enthalpy change associated with a reaction Review of sample and practice problems AP Chemistry Page 11 of 26

12 7.0 Electron Structure in Atoms Wave-like properties of electromagnetic radiation are used to demonstrate electron placement in the atom. Our knowledge of electronic structure is directly related to understanding the Quantum Mechanical Model, a twentieth century development. 7.1 Recognize the numerous types of electromagnetic radiation. 7.2 Characterize the type of electromagnetic radiation using wavelength, frequency, and speed of light. 7.3 Realize that the colors of fireworks are based upon the arrangements of electrons in atoms of certain elements. 7.4 Construct a model of electron configuration, orbital notation, and suggest how atoms might bond. What are the fundamental reasons for the periodic table being arranged the way it is? How does light relate to matter? Laboratory materials Spectroscope Gas discharge apparatus Bright line spectral chart Lab exercise: Hydrogen spectrum AP Chemistry Page 12 of 26

13 8.0 Periodic Properties of the Elements Many properties of atoms depend on both the net attraction between the nucleus and the outer electrons and on the average distance of those electrons from the nucleus. There are periodic trends that demonstrate several key properties of atoms electron affinity, electronegativity, atomic radius, ionization energy and metallic character. The periodic table is useful in predicting periodic trends and periodic properties. 8.1 Use the periodic table to predict bond formation 8.2 Compare periodic trends and the relationship to energy associated with electrons 8.3 Differentiate between physical and chemical properties of metals and nonmetals 8.4 Identify the importance of metals, nonmetals, metalloids, and the inert gases. Why is the Periodic Table the most significant tool that chemists use for organizing and remembering chemical facts? Why is the most striking feature of different elements, their electron configurations? Periodic Puzzle Card Activity AP Chemistry Page 13 of 26

14 9.0 Chemical Bonding Different kinds of chemical bonding occur based on the electron arrangement of elements. Intricate diagrams can be used to pictorially represent microscopic molecular structures. Why are the properties of substances determined in large part by the chemical bonds that hold their atoms together? What incredible forces hold atoms together in specific ratios to create the wide array of chemical compounds on this planet? 9.1 Diagram valence electrons with Lewis structures and relate bonding characteristics to the periodic table. 9.2 Determine bond type using the electronegativity. 9.3 Demonstrate how to use formal charge to suggest a model for the molecule or ion. 9.4 Provide an understanding of resonance and exceptions to the octet rule. 9.5 Estimate the enthalpies of reactions using average bond energy tables. Laboratory Exercise: Molecular model kit Bond type and VSEPR Theory AP Chemistry Page 14 of 26

15 10.0 Molecular Geometry Molecular shapes and geometry can be predicted by electron placement around individually bonded atoms. Lewis structures provide explanations for multiple bonds and bond shape Discover that the shape of a molecule is determined by electron placement and bond angles of the atoms within Recognize that Lewis structures tell the student which atoms are physically connected to which Predict the best arrangement of electron domains using the VSEPR model Demonstrate with the molecular model kit the shapes of larger molecules, multiple bonds, and molecular polarity Expand student knowledge of valence bond theory by investigating sp hybrid orbitals, orbital overlap, bond order, and electron configuration. How do molecules exist in a 3D presentation? How does electron arrangement predict molecular geometry through VSEPR theory? Why are the sensations of smell and vision dependent upon the molecular shape of the substances viewed or inhaled? How does the shape and size of a molecule partly determine the properties of that substance? Molecular model kit Laboratory activity Molecular model kit AP Chemistry Page 15 of 26

16 11.0 Gases Gases present different physical and chemical properties from solids and liquids. Pressure and temperature are important factors in viewing the kinetic molecular theory with gases Compare and contrast the molecular properties of solids, liquids, and gases Recognize the factors that temperature and pressure play in chemical reactions involving gases Explain the pressure, volume, temperature relationships of the four basic gas laws: Boyles, Charles, Gay-Lussac, Avogadro Solve reaction stoichiomety problems using the ideal gas law equation Explain gas behavior according to the kinetic molecular theory. How are gases different in their physical and chemical properties from solids and liquids during chemical reactions? How do pressure and temperature relate to the kinetic molecular theory of gases? Why does the relative simplicity of the gas state afford such a good starting point to understand the properties of matter in terms of its atomic and molecular constitution? Absolute Zero Demonstration Kit Laboratory activity: Molar volume of a gas Molar mass of a gas Effusion vs diffusion Collection of gas over water AP Chemistry Page 16 of 26

17 12.0 Intermolecular Forces, Liquids and Solids Intermolecular forces between neutral molecules depend on their molecular polarity, size, and shape. Solids, liquids, and gases display vastly different kinetic behavior at different temperatures. Arrangements of atoms within the individual states of solid, liquid, and gas can be visualized through an understanding of the forces that hold them together Explain how solids and liquids exist because of their intermolecular forces 12.2 Identify the different types of intermolecular forces and compare their effects on specific molecules 12.3 Summarize how viscosity, surface tension, and capillary action in liquids relate to intermolecular forces Provide examples of a crystalline solids and amorphous solids and relate this to the unit cell and crystal packing theory. Why are virtually all substances that exist in the liquid state at room temperature molecular? What incredible forces within molecules give rise to covalent bonds that influence molecular shape, bond energy, and many aspects of chemical behavior? Molecular model kit/styrofoam spheres Overhead transparencies of crystal packing Laboratory activity: NaCl diamonds Separation by chromatography Laboratory Demonstration: Crystal packing efficiency with iron wire Carbon and graphite models AP Chemistry Page 17 of 26

18 13.0 Properties of Solutions Aqueous solutions of ionic substances are very important to our daily lives (i.e. air, ocean, fuels, living fluids, etc.). Colligative properties of solutions provide insight into the physical nature of their solute molecules Explain the solution process with the role of intermolecular forces Recognize dilute and concentrated solutions Identify the forces that allow gases to be dissolved in aqueous solution Calculate and prepare a solution concentration Relate how colligative properties allow for such phenomenon as vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. Why are aqueous solutions of ionic substances so important in chemistry and our daily lives? Why is it that most of the materials that we encounter in everyday life are mixtures? How are the concentrations of solutions quantitatively determined? Appropriate laboratory equipment Overhead transparencies Phase diagrams Solution process Solubility table of salts Laboratory activity: Freezing point depression Determination of molecular mass Precipitation of an insoluble salt Standardization of a solution as a primary standard Demonstration: Super saturation of sodium acetate Laboratory investigations, reports, and AP Chemistry Page 18 of 26

19 14.0 Chemical Kinetics Reactions are dynamic and their rate can be influenced by different variables. Chemical kinetics helps society to research and explain technological advances related to: medicines and how they work, environmental issues, development of new materials, digestion of food Explain how concentration, physical states of reactants, temperature, and catalysts affect reaction rate Derive and express reaction rates and use stoichiometry of reaction Examine how rate laws are determined experimentally Identify rate laws Recognize activation energy and consider reactions that require a minimum of input energy Demonstrate the step-by-step molecular pathways that are the mechanisms by which reactions take place Discuss how catalysts and enzymes can speed up chemical reactions. Why do chemical reactions convert substances with well-defined properties into other materials with different properties? What factors determine the rates at which chemical reactions occur? Laboratory activity: Determination of reaction rate and reaction order Laboratory investigation, reports, and AP Chemistry Page 19 of 26

20 15.0 Chemical Equilibrium Chemical equilibrium occurs when opposing reactions are proceeding at equal rates. 8.1 Explain the concept of equilibrium in a chemical reaction. 8.2 Identify how to use an equilibrium constant in a chemical equilibrium constant expression. 8.3 Calculate equilibrium constants from known or given values of reaction kinetics. 8.4 Predict, using equilibrium expressions, the concentrations of reactants and products needed in a chemical reaction done in a laboratory setting. 8.5 Understand the implications of Le Chatelier s Principle and predict how a system responds to situations where concentration, temperature, volume, pressure, and temperature change. How can a scientist predict and calculate the amounts of products formed in a chemical reaction? Why do chemical systems respond differently to changes in concentration, volume, pressure, and temperature? Lab Activity Determination of the equilibrium constant for a chemical reaction Inquiry Hands-on, minds-on lab activities See other learning strands for integration AP Chemistry Page 20 of 26

21 16.0 Acid-Base Equilibria Acids and bases are ubiquitous and important in innumerable chemical processes in industry, biology, and the environment. A large part of the chemical industry can be understood in terms of acid-base reactions Clearly define an acid or a base in terms of the following accepted modern theories: Arrhenius Theory Bronsted-Lowry Theory Lewis Theory 16.2 Demonstrate the idea of proton donation in defining a species of ion as acidic Explain conjugate acid-base pairs Recognize the autoionization of water that may be used to establish the equilibrium constant for specific acidbase reactions Describe and use the ph scale in a mathematical application Differentiate between strong and weak acids on the level of ionization Explain Ka and Kb in the equilibrium process and use it to calculate not only ph, but other stoichiometric factors Identify the limitations and uses of each of the three acid-base theories. What particular factors make a substance behave as an acid or a base? Why are acids and bases so important in so many chemical processes that occur around or inside us? Lab Exercise: Determination of concentration by acid base titration Determination of weak acid/strong acid, weak base/strong base Determination of appropriate indicators used in various acid/base titrations ph determination Inquiry Hands-on, minds-on lab activities See other learning strands for integration AP Chemistry Page 21 of 26

22 17.0 Additional Aspects of Aqueous Equilibria The physical and chemical characteristics of water make it uniquely important in almost all chemical reactions that take place in or on this planet. What special types of equilibria occur in aqueous solutions found in nature such as biological fluids and seawater? What forces are understood with the formation of solutions with slightly soluble salts and those involving the formation of metal complexes in solution? Why does water occupy such an important position in chemical, environmental, and biological settings? 17.1 Discover the common-ion effect related to Le Chatelier Recognize the unusual characteristics of a buffer Use the solubility-product-constant to determine the solubility of a salt in aqueous solution Learn how ions are precipitated selectively by use of particular chemicals in specific reactions Use the principles of solubility and complexation equilibria to identify ions qualitatively in solution. Lab Exercise: Preparation and properties of a buffer solution Inquiry Hands-on, minds-on lab activities See other learning strands for integration AP Chemistry Page 22 of 26

23 18.0 Chemical Thermodynamics Spontaneous thermochemical processes are closely tied to energy and equilibrium Discuss the spontaneous process and energy relationships related to the first law of thermodynamics Recognize that many chemical reactions are reversible and that there are methods to determine their spontaneity Reflect upon the nature of gases and how they demonstrate special situations to consider when working with thermodynamic data Explain how the term entropy applies to thermodynamic principles Relate the second and third laws of thermodynamics to chemical reactions Calculate energy changes for chemical reactions from experimental and theoretical data. How does society recognize and afford the enormous amounts of energy that prepare synthetic and naturally-occurring materials? Thermodynamic data table Inquiry Hands-on, minds-on lab activities See other learning strands for integration AP Chemistry Page 23 of 26

24 19.0 Electrochemistry There is a systematic process for balancing redox reactions by the half reaction method. Oxidation-reduction reactions are very common and truly important chemical reactions in our everyday lives Calculate loss and gain of electrons to balance redox reactions Explain how a voltaic cell works Calculate the voltage of cells and the relative strengths of oxidizing and reducing agents using the standard reduction potential tables Recognize that batteries are based on voltaic cells Discuss the spontaneous nature of corrosion and how it relates to oxidationreduction Examine electrolytic cells which use electricity and then explain the relationship between the quantity of current flowing through a cell and the amounts of products obtained. How does the corrosion of iron metal and the production of electricity in batteries demonstrate the electrochemical processes that occur daily in our lives? Standard Reduction Potential Tables Lab Exercise: Determination of electrochemical series Inquiry Hands-on, minds-on lab activities See other learning strands for integration AP Chemistry Page 24 of 26

25 20.0 Nuclear Chemistry There is a distinctive difference between a chemical reaction and a nuclear reaction. Nuclear chemistry affects our lives in a variety of ways Describe nuclear reactions by equations analogous to chemical equations Explain the difference between alpha and beta particles and gamma radiation Recognize how nuclear stability is established Identify the mechanisms of nuclear transmutations Calculate half-life and how radioisotopes decay Discuss how energy changes in nuclear reactions are related to mass changes via the famous Einstein equation, E=mc Compare the energy and processes of fusion and fission Summarize how radiation in nuclear reactions has the potential to cause damage to biological materials. How are chemical reactions different from reactions that originate in the nucleus of an atom? Inquiry Hands-on, minds-on lab activities See other learning strands for integration AP Chemistry Page 25 of 26

26 21.0 The Chemistry of Life: Organic and Biological Chemistry Genetic information provides both similarities and differences between two organisms and is transferred from one generation to the next by the replication of molecules of DNA Review the structures and reactivity of simple carbon-containing compounds Categorize the several classes of hydrocarbons Apply the nomenclature essential to communicating organic chemicals effectively Recognize how isomerism permits the vast number of organic compounds Identify the different functional groups and demonstrate how these allow specific organic reactions to occur Consider the array of biochemically important molecules proteins, carbohydrates, and nucleic acids. How does the element carbon form such a vast number of compounds? Molecular Model Kit Lab Exercise: Preparation and analysis of aspirin Preparation of an ester Colorimetric or spectrophotometric analysis Inquiry Hands-on, minds-on lab activities See other learning strands for integration AP Chemistry Page 26 of 26