AP Chemistry 2012-2013
Syllabus
AP CHEM TEST MAY 6, 2013 @ 8:00 am
Text
Chemistry, The Central Science by Brown Theodore L, et al. Tenth Edition.
Suplemental Handbook
The Ultimate Chemical Equation by George R. Hague, Jr and Jane D. Smith
Laboratory Manual
Laboratory Experiments for AP Chemistry by Vonderbrink Sally Ann, Second Edition
Brief description of the course
AP Chemistry meets daily for a double- 43 minute period.
Labs are conducted approximately every two weeks for a double period. Students work in groups of two
or three. In each laboratory experiment, students will physically manipulate equipment and materials in
order to make relevant observations and collect data; use the collected data to form conclusions and
verify hypotheses; and communicate and compare results and procedures.
Each student is responsible to submit a formal report that includes a hypothesis, procedure,
observations/data, calculations and a conclusion. The reports are to be kept in a Laboratory Notebook.
This notebook is graded with each lab and is mandatory. The notebook goes with the student to the
university to evaluate their placement in a college laboratory program.
The laboratory manual should be brought to class the day before and the day of the laboratory
experiment.
Students in AP Chemistry are expected to take the AP Chemistry Exam in May.
Goals of the course
Students are prepared to be critical and independent thinkers who are able to function effectively
in a scientific and technological society.
Conceptual learning and problem solving is emphasized throughout the course.
Students will be able to analyze scientific and societal issues using scientific problem solving.
Students will be able to make an acceptable score on the AP Chemistry Examination in May
Fall 2012
Introduction and review concepts - Chapters 1-3
(1 and 1/2 weeks) 9/6-9/21
These topics were covered in Regents Chemistry which is a requisite to the AP class.
I. Measurement topics
II. Atomic theory
III. Symbols and formulas
IV. Periodic table
V. Ionic and covalent bonds
VI. Nomenclature
VII. Reactions
VIII. Stoichiometry: Percent composition-Empirical formulas-Solutions
Mole relationships-Percent (%) yield-Limiting reagents-Titrations and other analyses
Laboratory
*Determination of the Empirical Formula of Silver Oxide
Aqueous Reactions and Solution Stoichiometry Chapter 4
(2 weeks) 9/24-10/5
I Reaction Types: Acid base reactions: concepts of Arrhenius, Bronsted-Lowry, Lewis - Precipitation
Reactions - Redox Reactions: oxidation number-electron transport-activity series-electrochemistry
II Stoichiometry
III Net ionic equations
IV Balancing equations including redox
V Mass-volume relationships with emphasis on the mole
Laboratory
*Finding the Ratio of Moles of Reactants in a Chemical Reaction
The Kinetic-Molecular Theory and States of Matter - Chapters 10 and 11
(2 weeks ) 10/9-10/22
I. Gases Laws: Ideal gases-Boyles-‘s Law- Charles Law- Dalton’s
Law of partial pressureGraham’s Law-Henry’s Law-Van der Waals Equation
II. Kinetic-Molecular Theory: Avogadro’s Hypothesis and mole concept-Kinetics Energy of moleculesDeviation from Ideality
III. Liquids and Solids: Intermolecular Forces- Phase Changes – Vapor Pressure – Phase Diagrams of
one-component system- Structure of solids including lattice energies
Laboratory
*Determining the Molar Volume of a gas
Atomic Structure and Periodicity - Chapters 6 and 7
(2 weeks) 10/23 to11/8
I. Electronic Structure: Atomic Theory- Atomic Masses- Atomic Number and Mass Number- Electron
Energy Levels - Atomic Spectra –Wave behavior of Matter – Quantum Numbers – Atomic Orbitals –
Electron Configurations and the periodic Table
II. Periodic trends-Types of elements- Group trends: Alkali, Alkaline Earth Metals, Halogens, Oxygen
Group, Noble Gases
Laboratory
*Spectrophotometric Analysis – Hydrogen Spectrum
Bonding and Molecular Structure - Chapters 8 and 9
(2 weeks) 11/9 to 11/27
I Binding Forces: Ionic – Covalent – Metallic – Hydrogen Bonding – Van der Waals
II Relationship to States, structure and properties of matter
III Bonds Polarity and electronegativity
IV Molecular Models: Lewis Structures – Resonance Structures- Exceptions to the octet rule
V Strength of covalent bonds – Bond enthalpies and enthalpies of reactions
VI Molecular Shapes
V The VSERP model: Hybridization of orbitals-Molecular orbitals- Geometry of molecules and ions
VI Structural, geometric, optical and conformational isomerism of organic molecules and coordination
complexes.
VII Polarity of molecules
VII Relation of molecular structure to physical properties
Laboratory
*Chromatography
Solutions and Colloids - Chapter 13
(2 weeks ) 11/29 to 12/7
I. Types of solution
II. Factors affecting solubility
III. Concentration Problems
IV. Roult’s law and colligative properties
V. Colloids: Hydrophilic-Hydrophobic Colloids – Removal of colloidal particles
Laboratory
*Molar Mass by freezing point depression
Thermochemistry - Chapter 5
(1 ½ weeks) 12/10 to 12/21
I Thermal energy, heat and temperature
II Calorimetry
III Enthalpy changes
IV Hess’s Law
Laboratory
* Thermodynamics –Enthalpy of Reaction and Hess’s Law
Chemical Kinetics - Chapter 14
(2 1/2 weeks) 1/2 to 1/14
I. Factors that affect reaction rates: temperature-concentration-nature of substance-catalyst
III Rate law expressions
III. Order of reaction
IV Reaction Mechanism
V Catalyst
Laboratory
*Kinetics of a reaction
Nuclear Chemistry - Chapter 21
(1/2 Week) 1/15 to 1/18
Nuclear Structure: Radioactivity –Nuclear Stability - Nuclear Equations- Half lives- Energy changes in
Nuclear Reactions
Spring 2013
Chemical Equilibrium -Chapter 15
(2 weeks) 1/29 to 2/12
I. Equilibrium Concept
II. Equilibrium Constants: problems-magnitud of equilibrium constants-direction of chemical
equilibrium-calculating concentrations at equilibrium
III Le Chatelier’s Principle: problems predicting how equilibrium is shifted by temperature,
concentration, pressure.
Laboratory
*The determination of Keq for FeSCN2+
Acid-Base Equilibria - Chapter 16
(2 weeks) 2/13 to 3/6
I. Arrhenius Theory
II. Bronsted-Lowry
III pH Scale – Kw expression
IV. Strong acids and bases
V. Weak acids and bases
VI. Relationship between Ka and Kb
VII. Salt Hydrolysis
Laboratory
*Determination of Ka of Weak Acids
Additional Aspects of Aqueous Equilibria - Chapter 17
(1 1/2 weeks) 3/7 to 3/15
I. Common ion effect
II Buffered solutions
III. Acid-Base titrations
IV. Solubility equilibria
V. Factors that affect solubility
VI Precipitation and Separation of ions
Laboratory
*Acid-Base Titrations
*pH properties of buffer solutions
*Hydrolysis of salt
Chemical Thermodynamics - Chapter 19
(1 weeks) 3/18 to 3/22
I. State Functions
II. Laws of thermodynamics
III. Relationship of change of free energy to equilibrium constants
Electrochemistry - Chapter 20
(2 weeks) 4/3 to 4/17
I. Galvanic cells and cell potentials- Nernst equation- EMF
II. Electrolytic Cells
III Redox equations: half cells-balancing equations in acid/base solutions
Laboratory
*Redox Titration
*An activity series Determining the E0 of several ions
*Electroplating
*Separation and quantitative determination of cations and anions
Review for the AP Exam
(2 weeks) 4/18 to 5/3