AP Chemistry Scope and Sequence
Overview of AP Chemistry
Course Structure:
Class meets 5 days per week, alternating single and double periods (42 minutes) each day
providing for 270 periods in the school year.
Resources:
Text
Zumdahl, Steven. Chemistry 6th edition
Study Guide
Zumdahl, Steven. Chemistry 6th edition
Laboratory Guide
Holmquist, Randall & Volz, Chemistry with Calculators (Computers), 3rd edition, 2000
Various Internet Resources
Tutorial Guides
Ohio State University Chemistry (http://chemunder.chemistry.ohiostate.edu/under/chemed/qbank/quizmain.htm)
Demonstration Resources
Shakhashiri, Bassam. Chemical Demonstrations: A Handbook for Teachers of Chemistry,
Volumes 1,2 and 3
Methodology:
Course notes, homework, and laboratory activities are online for students to access.
Homework corresponds to chapter topics and should be completed by the end of each topic.
Homework assignments are guides for students to assess their ability to complete the
work as it is presented in class.
Weekly take-home quizzes are given on Friday (due Tuesday AM) which test the students’
ability to master the work and to foster the formation of study groups.
Group effort is expected on these quizzes as they are AP caliber in their difficulty.
Reaction quizzes are given on Tuesdays (due Friday AM) starting in January, to allow students
to master the various types of reactions required on the AP exam.
Tests are given twice per quarter which would correspond with 3 tests per semester in a college
course.
Laboratory Work is a hands on experience (wet labs), with students working collaboratively in
pairs. Utilizing various laboratory techniques in conjunction with Vernier probeware, the labs
are written following a standard write-up and submitted electronically. Laboratory work
corresponds with classroom topics and requires a standard laboratory write-up including
hypothesis, procedure, analysis of data, conclusion and further study. Total laboratory time is 30
hours during the course of the year.
Submission of the laboratory write-up constitutes the laboratory notebook in electronic
form, making it accessible to colleges for evaluation of credit in their chemistry curricula.
Demonstrations – Students carry out demonstrations of various chemistry concepts and present
the relationships of these concepts to the class.
All course work can be observed at:
http://www.sachem.edu/schools/east/departments/_level3sites/science/ChemistryDept/index
.htm
Curriculum:
Chapter 1 – Chemical Foundations (3 days)
The Metric System
Unit Analysis
Significant Figures – rules for counting significant figures
Significant Figures in Calculations
Precision and Accuracy
Temperature
Classification of Matter
Phases of Matter
Substance
Mixture
Chapter 2 – Atoms, Molecules, & Ions (4 days)
Fundamental Chemical Laws
Nuclear Atom
Electrons
Modern Atomic Theory
Isotopes
The Periodic Table
Periodic Law
Metals
Nonmetals
Two Fundamental Types of Chemical Bonds
Covalent Bonds
Ionic Bonds
Writing Chemical Formulas
Naming Compounds
1. Binary Compounds
2. Ternary Comounds
3. Acids
Chapter 3 – Stoichiometry (10 days)
Atomic Mass (or atomic weight)
Mole
Mole Conversions
Molar Mass
Percent Composition of Compounds
Determining Formulas from Percent Composition
Chemical Equations
Problems Involving Equations
Limiting Reagent (Limiter)
Theoretical Yield
Chapter 4 – Solution Stoichiometry & Chemical Analysis (15 days)
Water as a Solvent
Molarity (M)
Standard Solution
Equations:
1. Molecular Equation
2. Ionic Equation
3. Net Ionic Equation
Precipitation Reactions
Qualitative Analysis
Quantitative Analysis
Acid-Base Reactions
Titrations
Oxidation Reduction Reactions
Redox Reactions in Acidic or Basic Solutions
Chapter 5 – Gases (10 days)
The Gas Laws
Avogadro’s Law
Molar Mass of a Gas
Dalton’s Law of Partial Pressure
Mole Fraction
Kinetic Molecular Theory of Gases
Van der Waals Equation
Root Mean Square Velocity
Graham’s Law of Diffusion
Chapter 6 – Thermochemistry (10 days)
Thermodynamics
Exothermic Reactions
Endothermic Reactions
The First Law of Thermodynamics
Enthalpy (H)
Calorimetry
Heat Capacity
Hess’s Law
Standard Enthalpy of Formation
Chapter 7 – Atomic Structure and Periodicity (10 days)
Electromagnetic Radiation
Wavelength
Frequency C = λ v
Planck’s constant = 6.626x10-34Js
ΔE = nhv
The deBroglie Equation (on formula sheet)
The Bohr Model
Heisenberg Uncertainty Principle (Werner Heisenberg)
Modern Day Atomic Theory
Electron Configurations
Hund’s Rule
Quantum Numbers
Pauli Exclusion Principle
Valence Electrons
Ionization Energy
Effective Nuclear Charge (Zeff)
Electron Affinity
Atomic Radius
Chapter 8 & 9 – Bonding Concepts (10 days)
Chemical Bonds
Ionic Bonds
Size of Ions
Lattice Energy
Covalent Bonds
Electronegativity
Nonpolar Covalent Bonds
Polar Covalent Bonds
Polar Molecules
Nonpolar Molecules
Bond Energy
Lewis Structures
Resonance
Molecular Structure: The VSEPR Model
Localized Electron Model (Hybridization)
Molecular Orbital Model
Bond Order
Paramagnetism and Diamagentism
AP Reactions (5 days)
Organic Reactions
Synthesis Reactions
Decomposition Reactions
Single Replacement Reactions
Double Replacement Reactions
Redox Reactions
Acidified
Basic
Complex Ions
Chapter 10 – Liquids & Solids (7days)
Ionic Solids
Molecular Substances
Dipole-Dipole Forces
Hydrogen Bonds
London Dispersion Forces (Fritz London)
Liquid State
Surface Tension
Capillary Action
Viscosity
Vaporization – evaporation
Heat of Vaporization (ΔHvap) – Enthalpy of Vaporization
Vapor Pressure
Solid State
Types of Crystalline Solids
Metals
Network Solids
Molecular Solids
Ionic Solid
Heating Curve
Heat of Fusion (Hfus)
Sublimation
Phase Diagrams
Triple Points
Critical Point
Critical Temperature
Critical Pressure
Chapter 11 – Properties of Solutions (6 days)
Molarity
Mass Percent
Mole Fraction (χ, chi)
Molality (m)
Solubility
Factors Affecting Solubility
Colligative Properties
Raoult’s Law
Henry’s Law
Van’t Hoff factor – (Jacobus Van’t Hoff) 1901 first Nobel Prize for Chemistry.
Boiling Point Elevation
Freezing Point Depression
Osmotic Pressure
Colloids (also called colloidal dispersions)
Chapter 12 – Kinetics (10 days)
Collision Theory
Rate of Reactions
Differential Rate Law (Rate Law)
Rate Determining Step (Calculating)
Calculating the Rate Constant (k)
Reaction Mechanisms
Catalysts
Intermediates
Integrated Rate Laws
Recognizing Reaction order graphically
Calculations of Integrated Rate Laws
Activation Energy
Chapter 13 – Chemical Equilibrium (5 days)
Equilibrium
Equilibrium Expressions
Reaction Quotient (Q)
Calculating Equilibrium Concentrations (& Pressures)
LeChatlier’s Principle
Chapter 14 – Acids & Bases (5 days)
Arrhenius
Brönsted-Lowry
Structure of Acids
Acid Strength
pH Scale
Calculating the pH of Strong Acid Solutions
Calculating the pH of Weak Acid Solutions
Percent Dissociation
Base Strength
Calculating the pH of Strong Base Solutions
Calculating the pH of Weak Base Solutions
Nonhydroxide Bases
Salts – Hydrolysis
Acid – Base Properties of Oxides
Lewis Acid – Base Model
Chapter 15 – Applications of Aqueous Equilibria (5 days)
Buffered Solutions
The Henderson Hasselbach Equation
Titration (or pH curve)
Equivalence Point
Acid – Base Indicators
Solubility Product Constant (Ksp)
Relative Solubilities
Common Ion Effect
Precipitation
Complex Ions
Chapter 16 – Spontaneity, Entropy, & Free Energy (5 days)
Spontaneous Change
Second Law of Thermodynamics
Entropy (S)
Third Law of Thermodynamics
Entropy vs. Structure
Gibbs Free Energy (G)
Standard Free Energy Change (ΔG0)
Standard Free Energy of Formation (ΔG0f)
Free Energy and Equilibrium Δ G0 = -RTlnK
Chapter 17 – Electrochemistry (5 days)
Electrochemistry
Galvanic Cell
Cell Potential
Standard Reduction Potential (E0)
Faraday (Ʒ)
ΔG= -n ƷE
Dependence of E on Solution Concentration
Nernst Equation
Electrolysis
Chapter 22 – Organic Chemistry (3 days)
Hydrocarbons
Alkanes, Alkenes, Alkynes, Aromatics
Isomers
Functional Groups
Alcohols, Aldehyde, Acid, Ketone, Ether, Ester, Amine, Amide
Organic Reactions
Additions, Substitution, Esterification, Polymerization, Saponification
AP Exam Review (10 days)
Total Time = 138 days
Time after the AP exam is spent in laboratory and student demonstrations.
Laboratory Activities:
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Lab 1: Molar Volume
Lab 2: Precipitation Reactions - Solution Stoichiometry
Lab 3: Endothermic & Exothermic Reactions
Lab 4: Heat of Combustion of Magnesium
Lab 5: Hess' Law
Lab 6: Evaporatiotn & Intermolecular Forces of Attraction
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Lab 7: Molal Idendification of a Binary Salt
Lab 8: Beer's Law
Lab 9: Rate Law of Crystal Violet Reaction
Lab 10: Determining the Equilibrium Constant
Lab 11: Titration Curves for Various Acids & Bases
Lab 12: Determining the Ka of a Weak Acid
Lab 13: Phosphoric Acid
Lab 14: Solution Properties of Electrolytes
Lab 15: Conductivity of Various Solutions
In addition, students complete 30 laboratory exercises in Regents Chemistry
Time allotted is 30 lab hours during the course of the year.