AP Chemistry Syllabus 2015
Text used: Chemistry by Zumdahl and Zumdahl, 9th ed., Houghton Mifflin Company, 2013.
ISBN: 1133611095.
Course Overview
AP Chemistry meets five times per week for 50 minutes. Prerequisites for this course include general level
physical and biological sciences, 2nd year algebra, honors chemistry, as well, pre-calculus or higher math course
taken concurrently. This is a second year chemistry course for motivated students who intend to pursue a career
in science. The structure, properties, and behavior of matter are examined theoretically and in the laboratory.
College level text and labs are used. This course poses intellectual and laboratory challenges to all students and
is equivalent rigor of college level general chemistry and chemistry lab, and many college’s honors level
chemistry courses.
Course Goals and Philosophy
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Develop students’ ability to think critically to solve problems in science.
Allow students to attain an in depth knowledge of chemical phenomena.
To produce individuals who have mastered the use of various chemical equipment and techniques.
To gain the ability to make relevant observations and to analyze collected data qualitatively and quantitatively.
Effectively communicate results of various investigations verbally as well as in a formal written report.
To compile evidence of knowledge gain through experimentation and problem solving.
Course Grading Policy
Tests are given at the end of each unit. Quizzes and other formative assessments are given during the units.
Labs are assessed mainly through lab reports while part of the grade depends on technique and lab conduct.
Select homework problems are checked for completeness but not graded. Quarter grades are NOT rounded,
however, the test scores are curved based on all students’ performance. If you have incomplete homework
checks during a unit then your test score will not be curved for that unit.
Student’s grade is based on the following weighted categories:
Assessments (tests, quizzes) 85%
Labs & Projects 15%
Additional Help
Material in this class is covered at a fast pace. Do not wait for help to be given; be proactive in asking questions and seeking additional
assistance.
Review
Additional time before the AP Chemistry Exam is used for reviewing and assessing knowledge
AP Chemistry Labs
This course stresses hands-on laboratory experiments with emphasis on lab safety. This becomes one of the most
important safety precautions, knowledge of intention in the laboratory. A pre-lab assignment is a requirement of each
student to complete and understand before each lab is conducted. This is especially important for safety and also allows
the students to foresee and predict potential errors. All of the experiments conducted in the laboratory require
collaboration with other students (typically with a partner). Not only collaboration to complete the experimental procedure
in the allotted time but to also to interpret and analyze data obtained. Following each experiment, a debrief session is
conducted. This is typically conducted in larger groups or as an entire class to share results with others and to aid in
interpreting the data properly. Additionally, each lab is required to have a formal write-up presenting materials, procedure,
data/analysis, and conclusion. The students are required to neatly organize data and manipulate it using Microsoft Excel.
Conclusions should reflect students’ understanding of their results verses expected results, as well as detailed insight and
explanation of sources of error. Lab reports are graded and returned to students in sheet protectors. Students are
additionally required to compile the lab reports in a separate lab binder. This binder allows students to reflect on
laboratory experiments conducted as well as serve as evidence of having conducted the experiments.
Schedule & Summary of Course
Topics:
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Unit 1 & 2: Foundations of Chemistry and The Atom (8
days)
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Observations
Uncertainty in measurements
Basic calculations and significant figures (conversions,
temperature, density, etc.)
Atomic theory (from early ideas to new)
Chemical Laws
Modern atomic structure
Isotopes and average atomic mass
Basic organization of the periodic table
Naming all compounds
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Unit 3: Stoichiometry (5 days)
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Mole, molar ratios, atomic masses, % composition
Determining molecular formula of compounds
Components of chemical equations
Balancing reactions
Stoichiometric relations
Limiting reactants
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Unit 10: Properties of solutions (7 days)
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Unit 4: Chemical Reactions (6 days)
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Aqueous solution reactions
Details on all types of chemical reactions, including special
emphasis:
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Unit 5: Gases (6 days)
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Acid base reactions
Precipitation reactions
Oxidation reduction reactions
Balancing Redox reactions note: 5 days will be spent later in the
course after student have a deeper understanding of chemical
relations
Gas laws and their originators
Combined gas law
Ideal gas law
Gas stoichiometry
Kinetic Molecular Theory
Diffusion and Effusion
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Unit 7: Quantum Mechanics and Periodicity (7 days)
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Electromagnetic Radiation and Atomic Spectrum
Electron Configurations: Quantum Numbers, orbital shapes, and
Aufbau Principle
Valence electrons, core electrons, and shielding
Modern Periodic Trends in atomic properties, including:
Reaction Rates
Rate Law
Integrated Rate Law
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Order of reactions
Catalysts
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Heterogeneous
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Homogeneous
Unit 12: Chemical Equilibrium (24 days)
Nature of energy
Enthalpy and Calorimetry
Hess’s Law
Standard Enthalpies of formation
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Solution formation energies
Effects on solubility, including
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Pressure effects
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Temperature effects
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Structural effects
Colligative Properties
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Vapor pressure of solutions and non-ideal solutions
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Boiling point elevation
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Freezing point depression
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Osmotic pressure
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Electrolyte solutions and van’t Hoff factor
Colloids and their properties, including
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Coagulation
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Tyndall effect
Unit 11: Kinetics (9 days)
Unit 6: Intro to Thermochemistry (8 days)
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Instantaneous dipoles
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polarizability
Liquids and their properties, including:
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Surface tension
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Capillary action
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Viscosity
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Vapor pressure and its relation to temperature
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Enthalpy of vaporization
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Phase changes and phase diagrams including allotropic
states
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Heating curves
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Enthalpy of fusion
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Supercooling
Molecular and Ionic Solids
Metallic bonding structure
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Equilibrium Expression and Reaction Quotient
Le Chatelier’s Principle
Gaseous Equilibrium Kc, Kp
Acid-Base Equilibrium – Kw, Ka, Kb
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Calculating pH
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Polyprotic Acids
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Properties of Salts
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Properties of Oxides
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Buffers
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Titrations
Solubility Equilibrium – Ksp
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Qualitative Analysis
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Common ion effect
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Complex Ion formation and equilibrium
Unit 13: Spontaneity, Entropy, and Free Energy (12 days)
Unit 8: Chemical Bonds (15 days)
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Types of Bonding
Bond Polarity
Lewis-dot Structures
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Octet rule and its exceptions
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Resonance
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Formal Charge
VSEPR Theory – Molecular Shapes
Hybridization of orbitals in bonding
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Spontaneous processes and entropy
2nd Law of Thermodynamics
Effect of Temperature
Free Energy and chemical reactions
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Pressure effects
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Temperature effects
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Relation to K
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Relation to work
Unit 14: Electrochemistry (11 days)
Unit 9: States of Matter (6 days)
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Intermolecular Forces of liquids and solids, including:
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Dipole-Dipole interactions
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Hydrogen bonding
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London Dispersion forces
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Cell Potential
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Nernst Equation
Standard Reduction Potential
Electrolysis