AP CHEMISTRY CURRICULUM
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1 AP CHEMISTRY CURRICULUM Goals of AP Chemistry: 1. To understand the fundamental concepts and principles of chemistry through the investigation of chemical phenomena, theories and experimental methods. 2. To develop problem solving skills, and mathematical reasoning, through the active asking and answering of testable questions, and employing the components of a well-designed experimental investigation. 3. To foster scientific habits of mind including curiosity, creativity, and objectivity. 4. To understand the interconnections of chemistry to the other sciences, society, culture, and technology. Science Practices as Big Ideas: The student can use representations and models to communicate scientific phenomena and solve scientific problems. The student can use mathematics appropriately. The student can engage in scientific questioning to extend thinking or to guide investigations within the context of the AP course. The student can plan and implement data collection strategies in relation to a particular scientific question. The student can perform data analysis and evaluation of evidence. The student can work with scientific explanations and theories. The student is able to connect and relate knowledge across various scales, concepts, and representations in and across domains. Big Idea 1: 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. Enduring Understandings: 1
2 All matter is made of atoms. There are a limited number of types of atoms; these are atoms. The atoms of each element have unique structures arising from interactions between electrons and nuclei. Elements display trends with their properties when arranged by atomic number. Atoms are so small they are difficult to study directly, and there fore we learn through macroscopic data collected during experimentation. Atoms are conserved during physical and chemical changes. Essential Questions: How is the position of an element on the Periodic Table related to that element s chemical and physical properties? How does the arrangement of subatomic particles dictate an element s chemical properties? How do we know so much about something (the atom) that we can t see? (history & interactions of matter) What information can be gleaned about an atom/element from its box on the Periodic Table? Do atoms exist or are they just concepts invented by scientists? What evidence is there in your everyday life for the existence of atoms? What is a mole and why do chemists use the mole concept? Why is the location of the electrons so important? How is the location of electrons related to chemistry/chemical reaction? What does light and the electromagnetic spectrum have to do with electrons and energy? Topics: Classification of matter Properties of matter States of matter Physical vs. chemical change SI units and prefixes 2
3 Significant figures and rounding Accuracy vs. precision and percent error Dimensional analysis and unit conversion Atomic theory Atomic structure Atomic weights Periodic table Molecules/molecular compounds/empirical formulas Line spectra & Bohr model Wave-particle duality Energy, wavelength, and frequency Quantum mechanics & atomic orbitals Representations of orbitals Many-electron atoms Electron configurations, Electron configs & periodic table Paramagnetic vs. diamagnetic Labs: Identification of Substances by Physical Properties Determining the empirical formula of a compound Big Idea 2: 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. Matter can be described by its physical properties. The physical properties of the substance generally depend on the distance between the particles. 3
4 Forces of attraction between particles are important in determining macroscopic properties. The strong electrostatic forces holding atoms together are called chemical bonds. The type of bond in the solid state can be deduced from the properties of the solid state. Essential Questions: What makes something a solid, liquid, or gas? How are the types of forces different from each other? Topics: Chemical bonds, Lewis symbols & octet rule, Ionic bonding, Covalent bonding, Bond polarity & electronegativity, Drawing Lewis structures, Resonance structures, Exceptions to the octet rule, Strengths of covalent bonds Molecular Shapes, VSEPR, Shape & molecular polarity, Covalent bonding & orbital Big Idea 3: Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons. Enduring Understandings 4
5 Chemical changes are represented by a balanced chemical equation that identifies the ratios with which reactants react and products form. Chemical reactions can be classified by considering what the reactants are, what the products are, or how they change from one into the other. Chemical and physical transformations may be observed in several ways and typically involve a change in energy. Essential Questions: How do you know a chemical reaction took place? What are the qualitative and quantitative observations I can make during a chemical reaction? Topics: Chemical equations, Patterns of chemical reactivity, Formula weights, Mole, Empirical formulas from analyses, Quantitative info from balanced equations, Limiting reactants Labs: Analysis of Hydrate Compound Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions. Enduring Understandings: Reaction rates that depend on temperature and other environmental factors are determined by measuring changes in concentration of reactants or products over time. 5
6 Elementary reactions are mediated by collisions between molecules. Only collisions having sufficient energy and proper relative orientation of reactants lead to products. Many reactions proceed via a series of elementary reactions. Reaction rates may be increased by the presence of a catalyst. Big Idea 5: The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter. Enduring Understandings: Two systems with different temperature that are in thermal contact will exchange energy. The quantity of thermal energy transferred from one system to another is called heat. Energy is neither created nor destroyed, but only transformed from on form to another. Breaking bonds requires energy, while forming bonds releases energy. Electrostatic forces exist between molecules, as well as between atoms or ions, and breaking the resultant intermolecular interactions requires energy. Chemical or physical processes are driven by a decrease in enthalpy or an increase in enthalpy, or both. Big Idea 6: 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. 6
7 Enduring Understandings: Chemical equilibrium is a dynamic, reversible state in which rates of opposing processes are equal. Systems at equilibrium are responsive to external changes, with the response changing the composition of the system. Chemical equilibrium plays an important role in acid base chemistry as well as solubility. The equilibrium constant is related to temperature and the difference in Gibbs Free Energy between reactants and products. Essential Questions: Topics: Properties of aqueous solutions Precipitation reactions Acid-base reactions Oxidation-reduction reactions Concentrations of solutions Solution stoichiometry and chemical analysis Coordination chemistry (complex ions) 7
8 Course Content Outline: Unit 1-2 Matter, Measureme nt, Atoms, Molecules and Ions (Review of 1 st year Chemistry) 3 Electronic Structure of Atoms Big Idea and EU 1.A, 1.B, 1.E, 2.C, 3.B 1.B, 1.C, 1.D, 5.E Week Topics Laboratory Major Assessments 1-2 Classification of matter, Properties of matter, States of matter, Physical vs. chemical change, SI units and prefixes, Significant figures and rounding, Accuracy vs. precision and percent error, Dimensional analysis and unit conversion, Atomic theory, Atomic structure, Atomic weights, Periodic table, Molecules/molecular compounds/empirical formulas, Ions and ionic compounds, Naming inorganic compounds, Simple organic compounds 3-4 Line spectra & Bohr model, Wave-particle duality, Energy, wavelength, and frequency Quantum mechanics & atomic orbitals, Representations of orbitals, Many-electron atoms, Identification of Substances by Physical Properties Determining the empirical formula of a compound Atomic Spectra and Atomic Structure In-class Quiz Test 1: Units 1-2 (Multiple Choice, Problems, Constructed Response) Test 2: Unit 3 (Multiple Choice, Problems, Constructed Response) 8
9 4 Unit Stoichiome try 5 Qualitative and Quantitativ e Chemistry (Reaction and Equation Writing) Big Idea and EU 1.A, 1.D, 1.E, 3.A, 3.B 1.A, 1.E, 2.A, 2.B, 2.D, 3.A, 3.B, 3.C, 5.D, 6.C Week Topics Laboratory Major Assessments Electron configurations, Electron configs & periodic table Paramagnetic vs. diamagnetic 4-5 Chemical equations, Patterns of chemical reactivity, Formula weights, Mole, Empirical formulas from analyses, Quantitative info from balanced equations, Limiting reactants 6-8 Properties of aqueous solutions, Precipitation reactions, Acid-base reactions, Oxidation-reduction reactions, Concentrations of solutions, Solution stoichiometry and chemical analysis Coordination chemistry (complex ions) Analysis of Hydrate Compound Analysis of Bleach Test 3: Unit 4 (Multiple Choice, Problems, Constructed Response) Test 4: Unit 5 (Multiple Choice, Problems, Constructed Response) In-class Quiz 6 Gases 1.A, 2.A, 2.B, 3.A, 5.A 9-10 Characteristics of gases, Pressure, Gas laws, Ideal-gas equation, Applications of ideal-gas equation, Gas mixtures & partial pressures, Kinetic-molecular theory, Behavior of Gases: Molar Mass Test 5: Unit 6 (Multiple Choice, Problems, Constructed Response) In-class Quiz 9
10 Unit 7 Periodic Properties of the Elements 8 Chemical Bonding Big Idea and EU 1.B, 1.C, 1.D, 5.E 1.B, 1.C, 1.D, 2.C, 2.D, 5.C, 2.A, 2.B, 5.B, 5.D, 6.A, 6.C Week Topics Laboratory Major Assessments Molecular effusion & diffusion, Real gases: deviation from ideal 11 Development of periodic table, Effective nuclear charge, Sizes of atoms & ions, Ionization energy, Electron affinities, Metals, nonmetals, & metalloids, Group trends for the active metals, Group trends for some nonmetals Chemical bonds, Lewis symbols & octet rule, Ionic bonding, Covalent bonding, Bond polarity & electronegativity, Drawing Lewis structures, Resonance structures, Exceptions to the octet rule, Strengths of covalent bonds Molecular Shapes, VSEPR, Shape & molecular polarity, Covalent bonding & orbital overlap, Hybrid orbitals, Multiple bonds, Molecular orbitals, 2 nd -row diatomic molecules Molecular comparison Molecular Geometries of Covalent Molecules: Lewis Structures and VSEPR Theory In-class Quiz Test 6: Units 7-8 (Multiple Choice, Problems, Constructed Response) 10
11 Unit Big Idea and EU Week Topics Laboratory Major Assessments liquids/solids, Intermolecular forces 9 Thermochemistry 10 Chemical Kinetics 3.C, 5.A, 5.B, 5.C, 5.E, 2.B, 6.D 4.A, 4.B, 4.C, 4.D Energy, First law of thermodynamics, Enthalpy, Enthalpies of reaction, Calorimetry, Hess s law, Enthalpies of formation, Spontaneous processes, Entropy & 2 nd law of thermodynamics, Molecular interpretation of entropy, Entropy changes in chemical reactions, Gibbs free energy, Free energy & temperature, Free energy & equilibrium constant Factors affect reaction rates, Reaction rates, Concentration & rate, Change of concentration with time, Temperature & rate, Reaction mechanisms, Catalysis Hot/Cold Pack Rates of Chemical Reactions I: A Clock Reaction Test 7: Unit 10 (Multiple Choice, Problems, Constructed Response) Test 9: Unit 12 (Multiple Choice, Problems, Constructed Response) 11
12 Unit 11 Chemical Equilibriu m 12 Acid-Base Equilibria Big Idea and EU Week Topics Laboratory Major Assessments 6.A, 6.B 21 Concept of equilibrium, Reactions of Aqueous Equilibrium constant, Solutions: Metathesis Heterogeneous equilibria, Reactions and Net Ionic In-class Quiz Calculating equilibrium constants, Equations Applications of equilibrium constants, Determination of the Le Châtelier s principle Solubility-Product Constant for a Sparingly Soluble Salt 1.E, 3.A, Determination of Test 10: Units (Multiple 3.B, 6.A, Dissociation Constant of Choice, Problems, Constructed 6.C a Weak Acid Response) Acids & bases, Brønsted-Lowery acids & bases, Autoionization of water, ph scale, Strong acids & bases, Weak acids, Weak bases, Relationship between K a & K b, Acid-base properties of salt solutions, Acid-base behavior & chemical structure, Lewis acids & bases Common ion effect, Buffered solutions, Acid-base titrations, Solubility equilibria, Factors that affect solubility, Precipitation & separation ions Introduction to Qualitative Analysis Titration of Acids and Bases Hydrolysis of Salts and ph of Buffer Solutions 12
13 Unit 13 Electrochemistry 14 Properties of Solutions 15 Review for the AP Exam Big Idea and EU Week Topics Laboratory Major Assessments 3,4,5, Oxidation-reduction reactions, Electrochemical Cell Test 11: Units 15 (Multiple Balancing redox equations, Choice, Problems, Constructed Voltaic cells, Response) Cell EMF, Spontaneity of redox reactions, Effect of conc. on Cell EMF, Batteries, Corrosion, Electrolysis 2.A, 2.B 28 Solution process, Colligative Properties: Take-home Quiz Saturated solutions & solubility, Freezing-Point Factors affecting solubility, Depression and Molar Expressing concentration, Mass Colligative properties, Colloids ALL BIG IDEAS Topics that students feel weak in Test 12: Units 1-18 (Multiple Choice, Problems, Constructed Response) 16 Scientific Investigatio n ALL BIG IDEAS Students chose an open-ended question to investigate and research. Student-designed and conducted experiment to test their hypotheses Semester 2 Assessment (Multiple Choice, Problems, Constructed Response) Long Term Student Inquiry Project (Written formal report and PowerPoint presentation) 13
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