ap chemistry curriculum - st. ignatius college … · ap chemistry curriculum goals of ap...

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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:

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• 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

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• 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.

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• 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

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• 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.

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• 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.


• 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.

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• 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)

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Course Content Outline:

Unit Big Idea and EU

Week Topics Laboratory Major Assessments

1-2 Matter, Measurement, Atoms, Molecules and Ions (Review of 1st year Chemistry)

1.A, 1.B, 1.E, 2.C,

3.B

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

Identification of Substances by Physical Properties Determining the empirical formula of a compound

Laboratory Notebook In-class Quiz Test 1: Units 1-2 (Multiple Choice, Problems, Constructed Response)

3 Electronic Structure of Atoms

1.B, 1.C, 1.D, 5.E

3-4 Line spectra & Bohr model, Wave-particle duality, Energy, wavelength, and frequency Quantum mechanics & atomic orbitals, Representations of orbitals, Many-electron atoms,

Atomic Spectra and Atomic Structure

Test 2: Unit 3 (Multiple Choice, Problems, Constructed Response)

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Electron configurations, Electron configs & periodic table Paramagnetic vs. diamagnetic

4 Stoichiometry

1.A, 1.D, 1.E, 3.A,

3.B

4-5 Chemical equations, Patterns of chemical reactivity, Formula weights, Mole, Empirical formulas from analyses, Quantitative info from balanced equations, Limiting reactants

Analysis of Hydrate Compound

Test 3: Unit 4 (Multiple Choice, Problems, Constructed Response) Laboratory Notebook

5 Qualitative and Quantitative Chemistry (Reaction and Equation Writing)

1.A, 1.E, 2.A, 2.B, 2.D, 3.A, 3.B, 3.C, 5.D, 6.C

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 Bleach Test 4: Unit 5 (Multiple Choice, Problems, Constructed Response) In-class Quiz Laboratory Notebook

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 Laboratory Notebook

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Molecular effusion & diffusion, Real gases: deviation from ideal

7 Periodic Properties of the Elements

1.B, 1.C, 1.D, 5.E

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

In-class Quiz

8 Chemical Bonding

1.B, 1.C, 1.D, 2.C, 2.D, 5.C, 2.A, 2.B, 5.B, 5.D, 6.A, 6.C

12-13 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, 2nd-row diatomic molecules Molecular comparison

Molecular Geometries of Covalent Molecules: Lewis Structures and VSEPR Theory

Test 6: Units 7-8 (Multiple Choice, Problems, Constructed Response) Laboratory Notebook

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liquids/solids, Intermolecular forces

9 Thermo-chemistry

3.C, 5.A, 5.B, 5.C, 5.E, 2.B,

6.D

15-17 Energy, First law of thermodynamics, Enthalpy, Enthalpies of reaction, Calorimetry, Hess’s law, Enthalpies of formation, Spontaneous processes, Entropy & 2nd law of thermodynamics, Molecular interpretation of entropy, Entropy changes in chemical reactions, Gibbs free energy, Free energy & temperature, Free energy & equilibrium constant

Hot/Cold Pack Test 7: Unit 10 (Multiple Choice, Problems, Constructed Response) Laboratory Notebook

10 Chemical Kinetics

4.A, 4.B, 4.C, 4.D

19-20 Factors affect reaction rates, Reaction rates, Concentration & rate, Change of concentration with time, Temperature & rate, Reaction mechanisms, Catalysis

Rates of Chemical Reactions I: A Clock Reaction

Test 9: Unit 12 (Multiple Choice, Problems, Constructed Response) Laboratory Notebook

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11 Chemical Equilibrium

6.A, 6.B 21 Concept of equilibrium, Equilibrium constant, Heterogeneous equilibria, Calculating equilibrium constants, Applications of equilibrium constants, Le Châtelier’s principle

Reactions of Aqueous Solutions: Metathesis Reactions and Net Ionic Equations Determination of the Solubility-Product Constant for a Sparingly Soluble Salt

Laboratory Notebook In-class Quiz

12 Acid-Base Equilibria

1.E, 3.A, 3.B, 6.A,

6.C

22-24 Acids & bases, Brønsted-Lowery acids & bases, Autoionization of water, pH scale, Strong acids & bases, Weak acids, Weak bases, Relationship between Ka & Kb, 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

Determination of Dissociation Constant of a Weak Acid Introduction to Qualitative Analysis Titration of Acids and Bases Hydrolysis of Salts and pH of Buffer Solutions

Test 10: Units 13-14 (Multiple Choice, Problems, Constructed Response) Laboratory Notebook

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13 Electro-chemistry

3,4,5,6 25-27 Oxidation-reduction reactions, Balancing redox equations, Voltaic cells, Cell EMF, Spontaneity of redox reactions, Effect of conc. on Cell EMF, Batteries, Corrosion, Electrolysis

Electrochemical Cell Test 11: Units 15 (Multiple Choice, Problems, Constructed Response) Laboratory Notebook

14 Properties of Solutions

2.A, 2.B 28 Solution process, Saturated solutions & solubility, Factors affecting solubility, Expressing concentration, Colligative properties, Colloids

Colligative Properties: Freezing-Point Depression and Molar Mass

Take-home Quiz Laboratory Notebook

15 Review for the AP Exam

ALL BIG IDEAS

30-33 Topics that students feel weak in Test 12: Units 1-18 (Multiple Choice, Problems, Constructed Response) Laboratory Notebook

16 Scientific Investigation

ALL BIG IDEAS

34-36 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)

ap chemistry curriculum - st. ignatius college … · ap chemistry curriculum goals of ap...

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