AP Chemistry Course and Exam Topics

AP Chemistry Course and Exam Topics This is an outline of the chemistry topics covered by the AP (Advanced Placement) Chemistry course and exam, as described by the College Board. The percentage given after the topic is the approximate percentage of multiple-choice questions on the AP Chemistry Exam about that topic. Structure of Matter (20%)States of Matter (20%)Reactions (35–40%)Descriptive Chemistry (10–15%)Laboratory (5–10%) I. Structure of Matter (20%) Atomic Theory and Atomic Structure Evidence for the atomic theoryAtomic masses; determination by chemical and physical meansAtomic number and mass number; isotopesElectron energy levels: atomic spectra, quantum numbers, atomic orbitalsPeriodic relationships including atomic radii, ionization energies, electron affinities, oxidation states Chemical Bonding Binding forcesa. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces)b. Relationships to states, structure, and properties of matterc. Polarity of bonds, electronegativitiesMolecular modelsa. Lewis structuresb. Valence bond: hybridization of orbitals, resonance, sigma and pi bondsc. VSEPRGeometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure Nuclear Chemistry Nuclear equations, half-lives, and radioactivity; chemical applications. II. States of Matter (20%) Gases Laws of ideal gasesa. Equation of state for an ideal gasb. Partial pressuresKinetic-molecular theorya. Interpretation of ideal gas laws on the basis of this theoryb. Avogadros hypothesis and the mole conceptc. Dependence of kinetic energy of molecules on temperatured. Deviations from ideal gas laws Liquids and Solids Liquids and solids from the kinetic-molecular viewpointPhase diagrams of one-component systemsChanges of state, including critical points and triple pointsStructure of solids; lattice energies Solutions Types of solutions and factors affecting solubilityMethods of expressing concentration (The use of normalities is not tested.)Raoults law and colligative properties (nonvolatile solutes); osmosisNon-ideal behavior (qualitative aspects) III. Reactions (35–40%) Reaction Types Acid-base reactions; concepts of Arrhenius, Brà ¶nsted-Lowry, and Lewis; coordination complexes; amphoterismPrecipitation reactionsOxidation-reduction reactionsa. Oxidation numberb. The role of the electron in oxidation-reductionc. Electrochemistry: electrolytic and galvanic cells; Faradays laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions Stoichiometry Ionic and molecular species present in chemical systems: net ionic equationsBalancing of equations including those for redox reactionsMass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants Equilibrium Concept of dynamic equilibrium, physical and chemical; Le Chateliers principle; equilibrium constantsQuantitative treatmenta. Equilibrium constants for gaseous reactions: Kp, Kcb. Equilibrium constants for reactions in solution(1) Constants for acids and bases; pK; pH(2) Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds(3) Common ion effect; buffers; hydrolysis Kinetics Concept of rate of reactionUse of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate lawsEffect of temperature change on ratesEnergy of activation; the role of catalystsThe relationship between the rate-determining step and a mechanism Thermodynamics State functionsFirst law: change in enthalpy; heat of formation; heat of reaction; Hesss law; heats of vaporization and fusion; calorimetrySecond law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changesRelationship of change in free energy to equilibrium constants and electrode potentials IV. Descriptive Chemistry (10–15%) A. Chemical reactivity and products of chemical reactions. B. Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements. C. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties). Physical and chemical properties of simple organic compounds should also be included as exemplary material for the study of other areas such as bonding, equilibria involving weak acids, kinetics, colligative properties, and stoichiometric determinations of empirical and molecular formulas. V. Laboratory (5–10%) The AP Chemistry Exam includes some questions based on experiences and skills students acquire in the laboratory: making observations of chemical reactions and substances; recording data; calculating and interpreting results based on the quantitative data obtained, and communicating effectively the results of experimental work. AP Chemistry coursework and the AP Chemistry Exam also include working some specific types of chemistry problems. AP Chemistry Calculations When performing chemistry calculations, students will be expected to pay attention to significant figures, precision of measured values, and the use of logarithmic and exponential relationships. Students should be able to determine whether or not a calculation is reasonable. According to the College Board, the following types of chemical calculations may appear on the AP Chemistry Exam: Percentage compositionEmpirical and molecular formulas from experimental dataMolar masses from gas density, freezing-point, and boiling-point measurementsGas laws, including the ideal gas law, Daltons law, and Grahams lawStoichiometric relations using the concept of the mole; titration calculationsMole fractions; molar and molal solutionsFaradays law of electrolysisEquilibrium constants and their applications, including their use for simultaneous equilibriaStandard electrode potentials and their use; Nernst equationThermodynamic and thermochemical calculationsKinetics calculations