Download AP CHEMISTRY COURSE SYLLABUS

AP CHEMISTRY COURSE SYLLABUS
COURSE OVERVIEW
This course is a college-level chemistry course for competent and highly motivated high
school students and is designed to be the equivalent of a college-level introductory
chemistry course. The course is a second year chemistry course where general chemistry
is a prerequisite. The overall curriculum follows the guidelines of the Collegeboard for
AP Chemistry. AP chemistry differs significantly from your general chemistry course
with respect to the kind of textbook used, the range and depth of topics covered, the kind
of laboratory work done, and the time and effort required. The aim of this course is to
provide you with the conceptual framework, factual knowledge, and analytical skills
necessary to deal critically with the theoretical and practical applications of chemistry.
MEETING TIMES:
This course meets every other day for 90 minutes. This provides adequate time to
perform laboratory activities on any given day.
THEMES:
This course is centered on the 4 major themes, Structure of Matter, States of Matter,
Chemical Reactions, and Descriptive Chemistry, listed in the AP Chemistry description.
Within each of these themes, there will be topics that are extensions of subject matter
learned in general chemistry as well some completely new topics that will be discussed in
detail.
LAB COMPONENT
Students work in small groups to complete the labs. Labs involve setting up the lab,
answering a series of pre-lab questions, performing the experiment, analyzing results and
formalize their conclusion which we then discuss at the beginning of the next class
period. Labs write-ups are completed in a lab notebook and turned in for grading
following the discussion. Many of the labs are interfaced with computers and labquest
sensors to accurately collect and analyze data using temperature, pressure, pH, and
colorimeters. Statistical analysis of data is emphasized. .
Text: Chemistry – Zumdahl 5th Edition Chapters 1-17.
Theme
AP Required Topics
Coursework/ Text Resource
Laboratory Work
Review
Topics covered in General
Chemistry
(summer)
Scientific Method, hypotheses, laws, theories,
significant figures, Classification of Matter,
Writing Ionic and covalent compounds, solve
problems involving basic stoichiometry, basic
gas laws, basic periodic table relationships
Lab: Vernier: “Find the
relationship”
(transposing graphical
data to linear
relationships to
determine relationships
between x and y.
Atomic theory and atomic structure
1. Evidence for the atomic theory
2. Atomic masses; determination by
chemical and physical means
3. Atomic number and mass number;
isotopes
Structure of
4. Electron energy levels: atomic
Matter
spectra, quantum numbers, atomic
orbitals
Work and solve basic stoichiometry problems
using the mole concept and basic gas law
problems using the ideal and combination gas
law equations.
Chapter 2: Atoms, Molecules and Ions. (1
lesson)
History of AtomDalton, Thomson,
Rutherford,
Atomic Mass, Mass Number, Isotopes, Ions,
Protons, Neutrons, Electrons
Chapter 7: Atomic Structure and
Periodicity (2wk)
Electromagnetic Radiation, Bohr Model,
Quantum Model, Quantum Numbers and
orbital shapes
Work and solve problems using Atomic
Structure Equations.
Lab: “Beer’s Law
Mechanical Universe:
Models of the Atom
Video.
Lab: Bohr Model
Energy Levels of
Hydrogen (Spectral
Lines)
Theme
Structure of
Matter
(cont)
AP Required Topics
Coursework/ Text Resource
5. Periodic relationships including, for
example, atomic radii, ionization
energies,
electron affinities, oxidation states
Periodic Trends for Ionization energy, Atomic
radii, Ionic radii, electron affinities. Reasons
for oxidation numbers based on Quantum
model
B. Chemical bonding
1. Binding forces
a. Types: ionic, covalent, metallic,
hydrogen bonding, van der Waals
(including
London dispersion forces)
b. Relationships to states, structure, and
properties of matter
c. Polarity of bonds, electronegativities
2. Molecular models
a. Lewis structures
b. Valence bond: hybridization of
orbitals, resonance, sigma and pi bonds
c. VSEPR
3. Geometry of molecules and ions,
structural isomerism of simple organic
molecules and coordination complexes;
dipole moments of molecules; relation
of properties to structure
Chapter 8-9: Bonding: General Concepts
And Orbital Bonding. (3 lessons)
C. Nuclear chemistry: nuclear equations,
half-lives, and radioactivity; chemical
Applications
Types: ionic, covalent, metallic, hydrogen bonding,
van der Waals (including London dispersion forces)
Polarity of bonds via electronegativity.
Polarity of molecules based on Lone-pair electrons
and VSPER
Lewis structures.
Hybridization, Resonance, sigma and pi bonds.
Laboratory Work
Lab: Bonds, Polarity
and Solubility
Lab: “Liquid
Chromatography”
Chapter 20: Sec 1-7 (1 lesson)
Isomerism and Coordination Complex Compounds
Chapter 21: The Nuclear Atom (2 lessons)
Types of Decay: Alpha, Beta, Gamma.
Nuclear Reactions, Half-lives. Fission, fusion
Lab: Radioactive decay
and half life
Lab: Shielding (alpha,
beta, gamma)
Theme
States of
Matter
AP Required Topics
Coursework/ Text Resource
Laboratory Work
A. Gases
1. Laws of ideal gases
a. Equation of state for an ideal gas
b. Partial pressures
2. Kinetic molecular theory
a. Interpretation of ideal gas laws on the
basis of this theory
b. Avogadro’s hypothesis and the mole
concept
c. Dependence of kinetic energy of
molecules on temperature
d. Deviations from ideal gas laws
Chapter 5: Gases (Conceptual and
mathematical relationships) (3 lessons)
Boyles, Charles, Avagadro’s Laws,
Combination Law, Ideal Gas law.
Dalton’s Law of partial Pressure
Gas Stoichiometry
Kinetic Theory of Gases
Root mean square velocity
Deviations from the ideal gas law
Work and solve problems using Gas Law
equations:
Labs:
1)“Gas laws
relationships”
2) Molar Mass of
Butane Lab
3) Diffusion Lab
Theme
States of
Matter
(cont)
AP Required Topics
Coursework/ Text Resource
B. Liquids and solids
1. Liquids and solids from the kineticmolecular viewpoint
2. Phase diagrams of one-component
systems
3. Changes of state, including critical
points and triple points
4. Structure of solids; lattice energies
Chapter 10: Liquids and Solids: (3 lessons )
Explanation of boiling pts based on molar mass
and types of bonding (London, dipole-dipole,
hydrogen bonding)
Structure of water in all three phases including
relative number of hydrogen bonds in each
phase. Connection to surface tension in liquid
phase.
Ionic solids, molecular solids, metallic solids,
network solids and their lattice structures.
Phase change vs time diagrams for substances.
Pressure vs. temp. phase change diagrams for
substances and descriptions of critical points
and triple points.
Laboratory Work
Lab: Freezing and
Melting pt of water.
Theme
States of
Matter
(cont)
AP Required Topics
Coursework/ Text Resource
Laboratory Work
C. Solutions
1. Types of solutions and factors
affecting solubility
2. Methods of expressing concentration
(use of normalities is not tested)
3. Raoult’s law and colligative
properties (nonvolatile solutes); osmosis
4. Nonideal behavior (qualitative
aspects)
Chapter 11: Solutions (2 lessons)
Molality and Molarity conceptual and
mathematical
Mole fraction (math)
Lab: Mixing Solutions
Structure, pressure, temp effects on solubility
Lab: Freezing pt
depression
Raoult’s Law concepts and mathematical
Freezing pt depression, Boiling pt Elevation
(math)
Osmotic Pressure
Non-ideal Solutions (math)
Work and solve problems using solutions
equations:
Theme
Reactions
AP Required Topics
Coursework/ Text Resource
Laboratory Work
A. Reaction types
1. Acid-base reactions; concepts of
Arrhenius, Brønsted-Lowry, and Lewis;
coordination complexes; amphoterism
Chapter 4: Reactions and Solution
Stoichiometry
(3 lessons)
1.Predicting and balancing reactions by
recognizing, composition, decomposition,
single replacement, double replacement
reactions (review Gen Chem)
2. Balancing Molecular, Ionic and net ionic
reactions
Predicting precipitation reactions based on
solubility rules. (review Gen Chem)
3. Balancing Redox reactions including halfreaction method.
Lab: “Deterinining the
Mole ratio in a
chemical reaction”
Lab: “Conductimetric
Titration and
Gravimetric
determination of a
precipitatie
2. Precipitation reactions
3. Oxidation-reduction reactions
a. Oxidation number
b. The role of the electron in oxidationreduction
4. Acid-Base definitions based on Arrhenius,
Bronstead-Lowry and Lewis Concepts.
5. Acid-Base Reactions including
Stoichiometry
Lab: OxidationReduction Titration:
Reaction of Fe2+ and
Ce4+
Lab: Acid-Base
Titration (Determining
concentration of
unknown acid)
Lab: “Investigating
Indicators”
Theme
AP Required Topics
Coursework/ Text Resource
Laboratory Work
Reactions
(cont)
c. Electrochemistry: electrolytic and
galvanic cells; Faraday’s laws; standard
half-cell potentials; Nernst equation;
prediction of the direction of redox
reactions
Chapter 17: Electrochemistry (3 lessons)
Galvanic and Electrolytic Cells
Faraday’s Law
Standard Cell Potential,
Calculating Cell potential using Nernst
Equation (math) and predicting direction of
redox half reactions.
Lab:“Electrochemistry:
Voltaic Cells”
Lab: ”Electroplating”
Work and solve problems using
Electrochemistry equations:
B. Stoichiometry
1. Ionic and molecular species present in
chemical systems: net ionic equations
2. Balancing of equations including
those for redox reactions
3. Mass and volume relations with
emphasis on the mole concept, including
empirical formulas and limiting
reactants
C. Equilibrium
1. Concept of dynamic equilibrium,
physical and chemical; Le Chatelier’s
Chapter 3: Stoichiometry (2 lessons) (80%
review from Gen Chemistry)
1. Predicting and balancing reactions by
recognizing, composition, decomposition,
single replacement, double replacement
reactions and net ionic reactions.
2. Mole concept with reactions. Determining
Mass, moles, volume @STP and non-STP
values.
3. Calculate empirical, molecular formulas, and
percent yield for reactions and or lab activities.
Empirical formula labs
Lab: “Tin(II) or Tin
(IV)Oxide”
Lab: “Formula of a
hydrate”
Lab: “%Yield of a
chem. Reaction”
Theme
AP Required Topics
Coursework/ Text Resource
principle;
equilibrium constants
2. Quantitative treatment
a. Equilibrium constants for gaseous
reactions: Kp, Kc
Chapter 13: Chemical Equilibrium (3
lessons)
1. Equilibrium Constant and concepts
2. Le Chatelier’s Principle and direction of
equilibrium shift based on changes in
conditions.
3. Equilibrium expressions in terms of
Pressure and concentration Kp, Kc (math)
4. Using ICE method to determine
concentrations at equilibrium.
b. Equilibrium constants for reactions in
solution
(1) Constants for acids and bases; pK;
pH
Reactions
(cont)
(2) Solubility product constants and their
application to precipitation and the
dissolution of slightly soluble
compounds
(3) Common ion effect; buffers;
hydrolysis
Chapter 14: Acids and Bases (2 lessons)
Determining equilibrium constants for weak
acids and bases.
Chapter 15: Solubility Products (2 lessons)
Apply equilibrium concepts to Solubility.
Determine solubility product for chemical
reactions
Chapter 15: Applications of Aqueous
Equilibrium
(3 lessons)
1. Calculating pK for acids and bases (math)
2. Calculating pH of strong, weak and Buffer
solutions including math.
3. Acid-Base properties of Salts…neutral pH,
acidic pH, basic pH conceptual and
mathematical
4. Titration curves for strong-strong, weakstrong, and weak-weak acid base reactions.
5. Hydrolysis applications
Laboratory Work
Lab: “Determination of
the equilibrium
constant”
Lab: Determining Ksp
Lab: pH titration
Curves
Lab: Buffers
Theme
AP Required Topics
Coursework/ Text Resource
Work and solve problems using Equilibrium
equations:
Reactions
(cont)
Laboratory Work
Theme
Reactions
(cont)
AP Required Topics
Coursework/ Text Resource
Laboratory Work
D. Kinetics
1. Concept of rate of reaction
2. Use of experimental data and
graphical analysis to determine reactant
order,
rate constants, and reaction rate laws
3. Effect of temperature change on rates
4. Energy of activation; the role of
catalysts
5. The relationship between the ratedetermining step and a mechanism
Chapter 12: Chemical Kinetics (3 lessons)
1. Rate law concepts and equation
2. Conceptual understanding of how temp
effect the rate of reaction.
3. Determine the order of reactions (0,1,2)
based on concentration vs. time graphs and
based on tables of initial concentrations and
rates or graphs of concentration vs. time
4. Concepts of catalysts
5. Determining half-life based on rate
equations
6. Determining activation energy based on
concentration data.
Work and solve kinetics problems using
Kinetics equations:
Lab:“Rate and Order of
a Chemcial Reaction”
Lab: “Rate
determination and
Activation energy”
Theme
AP Required Topics
Coursework/ Text Resource
Laboratory Work
E. Thermodynamics
1. State functions
2. First law: change in enthalpy; heat of
formation; heat of reaction; Hess’s law;
heats of vaporization and fusion;
calorimetry
Chapter 6: Thermochemistry (2 lessons)
1. Explain each of the 3 laws of
thermodynamics and their consequences
and connections.
2. Enthalpy concepts and calculations.
3. Hess’s Law (enthalphy calculations)
4. Heats of vaporization and Fusion.
5. Calorimetry within one phase.
6. Multiple phase calorimetry
Lab: Determining the
Enthalpy of a chemical
Reaction
Work and solve problems using Thermo
equations.
Reactions
(cont)
3. Second law: entropy; free energy of
formation; free energy of reaction;
dependence of change in free energy on
enthalpy and entropy changes
4. Relationship of change in free energy
to equilibrium constants and electrode
Potentials
Chapter 16: Spontaneity, Entropy, and Free
Energy (2 lessons)
1. Spontaneity and change in Entropy
2. Entropy change in chemical reactions
3. Free Energy and Chemical reactions
4. Relationship between entropy, Enthalpy
and Free energy (math)
5. Free energy and electric potential (math)
Lab: Heat of
Vaporization of liquid
Nitrogen
Lab: Melting/Freezing
of water.
Theme
AP Required Topics
Coursework/ Text Resource
Laboratory Work
Work and solve problems using the
Thermodynamic equations
Reactions
(cont)
Descriptive
Chemistry
1. Chemical Reactivity
After students have completed the first nine weeks of
coursework which includes the atomic structure and
chemical reactions every Monday begins with a series
of reactions that they must identify and complete.
(similar to net ionic reactions free response from AP
Exam). This process requires them to formalize their
understanding of solubility rules, redox, Oxide
reactions etc. As the course progresses additional
reaction types are added such as Acid-Base reactions
until they are very comfortable with the reaction and
reactivity relationships.
Lab: “Seperation and
Qualitative Analysis of
Cations”
Lab: “Seperation and
Qualitative Analysis of
Anions”
Theme
AP Required Topics
2. Relationships in periodic table
Descriptive
Chemistry
(cont)
3. Organic Chemistry
Coursework/ Text Resource
Laboratory Work
These topics are built into the atomic structure section
and referred to throughout the course to provide the
atomic level understanding of each topic covered
throughout the course. Students will:
1. Apply periodic law to predit reaction
products
2. Discuss activity series
3. Distinguish between metals and nonmetals
4. Use periodic table to predict common
oxidation states.
5. Predict single replacement reactions based on
activity series.
6. Predict products of aqueous double
replacement reactions based on solubility
rules.
Chapter 22: Organic Chemistry Sec 1-5 (1 lessons)
Alkenes, Alkanes, Alkynes Structures
Lab: Synthesis and
Analysis of Aspirin