Download ap chemistry – 2013-2014

AP CHEMISTRY – 2013-2014
Course Description:
This AP Chemistry course is designed to be the equivalent of the general chemistry
course usually taken during the first year of college. This course is structured around six
big ideas that include: Structure of matter, properties of matter-characteristics, states,
and forces of attraction, chemical reactions, rates of chemical reactions,
thermodynamics and equilibrium. Your PCDS grade for this course in both semesters will
be based on three tests per semester, regular quizzes, homework and lab work. Please
note that quizzes may be administered on either an ‘open’ or ‘closed’ book basis,
depending upon the topic/activity.
Course Objectives:
Through active participation in this revised AP Chemistry course, students will be able
to:
1. Develop attitudes of curiosity about and appreciate chemical occurrences in their
daily experiences.
2. Appreciate the importance of contributions of the history of chemistry.
3. Understand and apply basic and advanced chemical concepts to daily life
4. Recognize the value of solving problems using the scientific method.
5. Develop intellectual processes of inquiry by which scientific occurrences are
explained, predicted and/or controlled.
6. Develop a fundamental and advanced knowledge of Chemistry to include
understandings of atoms, molecules, and ions, chemical and physical changes, and
chemical formulas and equations.
7. Understand energy changes, thermodynamics, physical and chemical behavior of
gases.
8. Be able to use and understand the Periodic Table, predict general patterns from the
table, and the electronic structure of atoms.
9. Build an understanding of ionic, covalent, network covalent, and intermolecular
forces of attraction.
10. Learn the physical behavior of solutions, solids, and liquids.
11. Explain and use the factors that determine reaction rates, mechanisms, chemical
equilibrium, and acid/base theories.
12. Balance and use oxidation - reduction reactions as well as electrochemistry.
13. Be able to safely and efficiently perform numerous laboratory procedures using a
wide variety of materials and equipment.
14. Learn essential descriptive chemistry of numerous elements and compounds.
Textbook:
Zumdahl, Steven and Susan Zumdahl, Chemistry, 9th edition.
The Six Big Ideas:
Big Idea 1: Structure of matter
Big Idea 2: Properties of matter-characteristics, states, and forces of attraction
Big Idea 3: Chemical reactions
Big Idea 4: Rates of chemical reactions
Big Idea 5: Thermodynamics
Big Idea 6: Equilibrium
Labs:
The labs in AP Chemistry require following or developing processes and procedures,
taking observations and data manipulation. Students are to communicate and
collaborate in lab groups (ideally working in pairs); however, each student writes a
laboratory report in a lab notebook for every lab they perform. It is important that
students do not procrastinate when doing pre-lab and post-lab work. Late labs will not
be accepted for full credit. Any practical (lab) work not completed in the allocated class
time must be done at lunch or before/after school by appointment. The AP Board
request that six of the labs you complete are ‘guided-inquiry’ based labs.
Each of the 13 units of work and topic titles are listed below:
Unit 1: Chemistry Fundamentals
Scientific Method
Classification of Matter
a. pure substances vs. mixtures
b. law of definite proportions
c. law of multiple proportions
d. chemical and physical changes
Nomenclature and formula of binary compounds
Polyatomic ions and other compounds
Determination of atomic masses
Mole concept
Percent composition
Empirical and molecular formula
Writing chemical equations and drawn representations
Balancing chemical equations
Applying mole concept to chemical equations (Stoichiometry)
Determine limiting reagent, theoretical and % yield.
Unit 2: Types of Chemical Equations
Electrolytes and properties of water
Molarity and preparation of solutions
Precipitation reactions and solubility rules
Acid Base reactions and formation of a salt by titration
Balancing redox
Simple redox titrations
Gravimetric calculations
Unit 3: AP Style Net Ionic Equations
Redox and single replacement reactions
Double replacement reactions
Combustion reactions
Addition reactions
Decomposition reactions
Unit 4: Gas Laws
Measurement of gases
General gas laws - Boyle, Charles, Combined, and Ideal
Dalton’s Law of partial pressure
Molar volume of gases and Stoichiometry
Graham’s Law
Kinetic Molecular Theory
Real Gases and deviation from ideal gas law
Graham’s Law
Unit 5: Thermochemistry
Law of conservation of energy, work, and internal energy
Endothermic and exothermic reactions
Potential energy diagrams
Calorimetry, heat capacity, and specific heat
Hess’s law
Heat of formation/combustion
Bond energies
Unit 6: Atomic Structure and Periodicity
Electron configuration and the Aufbau principle
Valence electrons and Lewis dot structures
Periodic trends
Table arrangement based on electronic properties
Properties of light and study of waves
Atomic spectra of hydrogen and energy levels
Quantum mechanical model
Quantum theory and electron orbitals
Orbital shape and energies
Spectroscopy
Unit 7: Chemical Bonding
Lewis Dot structures
Resonance structures and formal charge
Bond polarity and dipole moments
VSEPR models and molecular shape
Polarity of molecules
Lattice energies
Hybridization
Molecular orbitals and diagrams
Unit 8: Liquids, Solids, and Solutions
Structure and bonding
a. metals, network, and molecular
b. ionic, hydrogen, London, van der Waals
Vapor pressure and changes in state
Heating and cooling curves
Composition of solutions
Colloids and suspensions
Separation techniques
Effect on biological systems
Unit 9: Kinetics
Rates of reactions
Factors that effect rates of reactions collision theory
Reaction Pathways
Rate equation determination
a. rate constants
b. mechanisms
c. method of initial rates
d. integrated rate laws
Activation energy and Boltzmann distribution
Unit 10: General Equilibrium
Characteristics and conditions of chemical equilibrium
Equilibrium expression derived from rates
Factors that affect equilibrium
Le Chatelier’s principle
Unit 11: Acids and Bases
Definition and nature of acids and bases
Kw and the pH scale
pH of strong and weak acids and bases
Polyprotic acids
pH of salts
Structure of Acids and Bases
Unit 12: Buffers, Ksp, and Titrations
Characteristics and capacity of buffers
Titrations and pH curves
Choosing Acid Base Indicators
pH and solubility
Ksp Calculations and Solubility Product
Unit 13: Thermodynamics
Laws of thermodynamics
Spontaneous process and entropy
Spontaneity, enthalpy, and free energy
Free energy