AP Course Topics

Listed Below are the Chapters and Topics that will be covered in AP Chemistry and the order the topics will be covered.

 

Course Outline:

Nomenclature and Dimensional Analysis (Chapters 1 & 2)

-Standard inorganic IUPAC

-Coordination complexes

-Metric/English conversion

-Significant figures

-Density / specific gravity

-Classification of matter

-Relationships in the Periodic Table

 

Mole Concept and Stoichiometry (Chapter 3)

-Empirical & molecular formulas

-Percent composition

-Avogadro’s Law and number

-Mass-mass, mass-vol, vol-vol calculations

-Concentration of ions, spectator ions

-Limiting reactants and % yield

-Atomic, molecular, and molar masses

 

Reaction Prediction (Chapter 4)

-Basic Reaction types: acid-base, precipitation, oxidation-reduction

-Anhydrous acid / base reactions

-Redox, complexes, combustion, precipitation

-Balancing by standard, half-cell, and change-in-oxidation state methods

-Ionic and molecular species present in chemical systems: net ionic equations

-Chemical reactivity and the products of chemical reactions

 

Thermo chemistry / Thermodynamics (Chapters 5, 8.8, 19)

-State functions

-First law: change in enthalpy, heat of formation, heat of reaction, Hess’ law, heat of vaporization and heat of fusion, calorimetry

-Second law: entropy, free energy of formation, free energy of reaction, dependence of change in free energy on enthalpy and entropy changes

-Quantitative relationships between ΔG°, E° , and K

 

Atomic Theory / Nuclear Chemistry

-Standard Model of Fundamental Particles

-Decay kinetics

-Atomic structure, atomic mass, atomic number, isotopes

-Evidence for the atomic theory

-Nuclear equations, half-lives, and radioactivity

-Applications of nuclear chemistry

 

EM Radiation / Electron Configurations. / Quantum Numbers

-Relationships with frequency, wavelength, and energy

-Hund’s Rule, Aufbau, Pauli exclusion, Heisenberg

-Periodic relationships

-Paramagnetism

-Historic development of atomic theory

-Electron energy levels: atomic spectra, quantum numbers, atomic orbitals

 

 

 

Bonding, Geometry, and Organic Structures

-Intermolecular and intramolecular forces: types, relationships to states and properties of matter, and electronegativities

-VSEPR Theory

-Lewis Dot Structures

-Bond types and energies

-Hybridization of orbitals, resonance, sigma and pi bonds

-Introductory organic chemistry: basic hydrocarbon nomenclature, functional groups, structure, and properties

-Polymers

 

Solids, Liquids, and Solutions

-Energy of phase changes

-Structure of solids, lattice energies

-Kinetic-molecular theory relationships

-Phase diagrams

-Types of solutions and factors affecting solubility

-Concentration units

-Colligative properties, Raoult’s law, osmosis

-Electrolytes

-Non-ideal behavior

 

Gas Laws

-Kinetic molecular theory

-Deviations from ideal gas laws

-Avogadro’s hypothesis

-Ideal gas laws and interpretations

-Partial pressures

 

Kinetics

-Concept of rate of reaction

-Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws

-Effect of temperature changes on rates

-Activation energy and catalysts

-Reaction mechanisms and rate-determining steps

 

Gaseous Equilibrium

-Concept of dynamic equilibrium: LeChatelier’s principle and equilibrium constants

-Quantitative treatment: Kc , KP, and ICE calculations

 

Limited Solubility Equilibrium

-Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds, common ion effect

-Molar solubility & Ksp

-pH & solubility

 

Acid – Base Equilibrium

-Concepts of Arrhenius, Bronsted-Lowry, and Lewis

-Percent ionization

-Quantitative treatment of constants for acids and bases: pH, pOH, Kw, Ka, Kb

-Titration and titration curves

-Buffering and salt hydrolysis calculations

-Indicators

 

Electrochemistry

-Predicting spontaneity and E°

-Electrolytic and galvanic cells

-Faraday’s laws

-Standard half-cell potentials, prediction and direction of half-cell reactions

-Nernst equation

 

Review Until Exam

 

5/6/13 AP Chemistry Exam

 

 

AP Exam:

 

The AP Exam is broken into two parts:

 

Section 1: Multiple Choice

This section is 90 minutes long and contains 75 multiple-choice which covers a broad range of topics. Calculators are NOT permitted during this section.

 

Section 2: Free Response

This section is 95 minutes long and is broken into two parts. One question in this section is based on laboratory experiments

 

     Part A: (55 Minutes) There will be three comprehensive problems. Calculators are permitted.

 

     Part B: (40 Minutes) This part has one question requiring the writing of balanced chemical                       

                                           reactions, and two essay questions. Calculator is not permitted.