Download 1 AP CHEMISTRY CURRICULUM Goals of AP Chemistry: 1. To

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.
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The student can use mathematics appropriately.
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The student can engage in scientific questioning to extend thinking or to guide investigations within the context of the AP
course.
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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.
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The student can work with scientific explanations and theories.
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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
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All matter is made of atoms. There are a limited number of types of atoms; these are atoms.
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The atoms of each element have unique structures arising from interactions between electrons and nuclei.
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Elements display trends with their properties when arranged by atomic number.
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Atoms are so small they are difficult to study directly, and there fore we learn through macroscopic data collected
during experimentation.
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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.
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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.
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The strong electrostatic forces holding atoms together are called chemical bonds.
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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
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Chemical changes are represented by a balanced chemical equation that identifies the ratios with which reactants react
and products form.
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Chemical reactions can be classified by considering what the reactants are, what the products are, or how they change
from one into the other.
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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.
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Many reactions proceed via a series of elementary reactions.
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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:
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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.
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Energy is neither created nor destroyed, but only transformed from on form to another.
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Breaking bonds requires energy, while forming bonds releases energy.
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Electrostatic forces exist between molecules, as well as between atoms or ions, and breaking the resultant
intermolecular interactions requires energy.
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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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Enduring Understandings:
•
Chemical equilibrium is a dynamic, reversible state in which rates of opposing processes are equal.
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Systems at equilibrium are responsive to external changes, with the response changing the composition of the
system.
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Chemical equilibrium plays an important role in acid base chemistry as well as solubility.
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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
1-2
Matter,
Measureme
nt, Atoms,
Molecules
and Ions
(Review of
1st 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
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
Line spectra & Bohr model,
Wave-particle duality,
Energy, wavelength, and
frequency
Quantum mechanics & atomic
orbitals,
Representations of orbitals,
Many-electron atoms,
3-4
Laboratory
Major Assessments
Identification of
Substances by Physical
Properties
Laboratory Notebook
Determining the
empirical formula of a
compound
Test 1: Units 1-2 (Multiple
Choice, Problems, Constructed
Response)
Atomic Spectra and
Atomic Structure
Test 2: Unit 3 (Multiple Choice,
Problems, Constructed Response)
In-class Quiz
8
Unit
4
Stoichiome
try
Big Idea
and EU
1.A, 1.D,
1.E, 3.A,
3.B
5
Qualitative
and
Quantitativ
e
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
Gases
1.A, 2.A,
2.B, 3.A,
5.A
Week
4-5
6-8
9-10
Topics
Electron configurations,
Electron configs & periodic table
Paramagnetic vs. diamagnetic
Chemical equations,
Patterns of chemical reactivity,
Formula weights,
Mole,
Empirical formulas from analyses,
Quantitative info from balanced
equations,
Limiting reactants
Properties of aqueous solutions,
Precipitation reactions,
Acid-base reactions,
Oxidation-reduction reactions,
Concentrations of solutions,
Solution stoichiometry and
chemical analysis
Coordination chemistry (complex
ions)
Characteristics of gases,
Pressure,
Gas laws,
Ideal-gas equation,
Applications of ideal-gas equation,
Gas mixtures & partial pressures,
Kinetic-molecular theory,
Laboratory
Analysis of Hydrate
Compound
Major Assessments
Test 3: Unit 4 (Multiple Choice,
Problems, Constructed Response)
Laboratory Notebook
Analysis of Bleach
Test 4: Unit 5 (Multiple Choice,
Problems, Constructed Response)
In-class Quiz
Laboratory Notebook
Behavior of Gases:
Molar Mass
Test 5: Unit 6 (Multiple Choice,
Problems, Constructed Response)
In-class Quiz
Laboratory Notebook
9
Unit
Big Idea
and EU
7
Periodic
Properties
of the
Elements
1.B, 1.C,
1.D, 5.E
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
Week
Topics
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
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
Laboratory
Major Assessments
In-class Quiz
Molecular Geometries
of Covalent Molecules:
Lewis Structures and
VSEPR Theory
Test 6: Units 7-8 (Multiple
Choice, Problems, Constructed
Response)
Laboratory Notebook
10
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
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
19-20 Factors affect reaction rates,
Reaction rates,
Concentration & rate,
Change of concentration with
time,
Temperature & rate,
Reaction mechanisms,
Catalysis
Hot/Cold Pack
Test 7: Unit 10 (Multiple Choice,
Problems, Constructed Response)
Laboratory Notebook
Rates of Chemical
Reactions I: A Clock
Reaction
Test 9: Unit 12 (Multiple Choice,
Problems, Constructed Response)
Laboratory Notebook
11
Unit
11
Chemical
Equilibriu
m
12
Acid-Base
Equilibria
Big Idea
and EU
6.A, 6.B
1.E, 3.A,
3.B, 6.A,
6.C
Week
Topics
Laboratory
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
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
Major Assessments
Laboratory Notebook
In-class Quiz
Determination of the
Solubility-Product
Constant for a Sparingly
Soluble Salt
Determination of
Test 10: Units 13-14 (Multiple
Dissociation Constant of Choice, Problems, Constructed
a Weak Acid
Response)
Introduction to
Qualitative Analysis
Laboratory Notebook
Titration of Acids and
Bases
Hydrolysis of Salts and
pH of Buffer Solutions
12
Unit
13
Electrochemistry
Big Idea
and EU
3,4,5,6
14
Properties
of
Solutions
2.A, 2.B
15
Review for
the AP
Exam
ALL BIG
IDEAS
Week
Topics
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
28
Solution process,
Saturated solutions & solubility,
Factors affecting solubility,
Expressing concentration,
Colligative properties,
Colloids
30-33 Topics that students feel weak in
Laboratory
Electrochemical Cell
Major Assessments
Test 11: Units 15 (Multiple
Choice, Problems, Constructed
Response)
Laboratory Notebook
Colligative Properties:
Freezing-Point
Depression and Molar
Mass
Take-home Quiz
Laboratory Notebook
Test 12: Units 1-18 (Multiple
Choice, Problems, Constructed
Response)
Laboratory Notebook
16
ALL BIG
Scientific
IDEAS
Investigatio
n
34-36 Students chose an open-ended
question to investigate and
research.
Student-designed and
Semester 2 Assessment (Multiple
conducted experiment to Choice, Problems, Constructed
test their hypotheses
Response)
Long Term Student Inquiry
Project (Written formal report and
PowerPoint presentation)
13