AP chemistry multiple-choice topics  [source:  college board (pdf; 2.3 MB); accessed July 2008]

I.  Structure of matter  [20%]

A.  atomic theory & atomic structure

1.  evidence for the atomic structure

2.  atomic masses; determination by chemical and physical means

3.  atomic number and mass number; isotopes

4.  electron energy levels:  atomic spectra, quantum numbers, atomic orbitals

5.  periodic relationships including, e.g. atomic radii, ionization energy, electron affinity, oxidation states

B.  chemcial bonding

1.  binding forces

a.  types:  ionic, covalent, metallic; hydrogen bonding, van der Waals (include London dispersion forces)

b.  relationships to states, structure, and properties of matter

c.  polarity of bonds, electronegativity

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 prpoperties to structure

C.  nuclear chemistry:  nuclear equations, half-lives, and radioactivity; chemical applications

II.  states of matter  [20%]

A.  gases

1.  laws of ideal gases

a.  equation of state for an ideal  gas

b.  partial pressure

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 moleculres on temperature

d. deviations from ideal gas laws

B.  liquids & solids

1.  liquids and solids from teh kinetic molecular viewpoint

2.  phase diagrams of 1-component systems

3.  changes of state, including critical points and triple points

4.  structure of solids; littice energy

C.  solutions

1.  types of solutions and factors affecting solubility

2.  methods of expressing concentration

3.  Raoult's law and colligative propeties (nonvolatile solutes); osmosis

4.  nonideal behavior (qualitative)

III.  reactions  [35 - 40%]

A.  reaction types

1.  acid-base reaction; concepts of Arrenius, Bronsted-Lewis, and Lewis; coordination complexes; ampjoterism

2.  precipitation reactions

3.  redox reaction

a.  oxidation number

b.  role of the electron in redox reactions

c.  electrochemistry:   electrolytic and galvanci cells; Faraday's laws; standard half-cell potentials; NErnst equation; prediction of hte directo of redox reactions

B.  stoichiometry

1.  ionic and molecular species present in chemical systems; net ionic equation

2.  balancing of equations including those for redox reactions

3.  mass and volume relations wti hemphasis on teh mole concept; including empirical formulas and limiting reactants

C.  equilibrium

1.  concept of dynamic equilibrium, physical and chemical; Le Chatelier's principle; equilibrium constant

2.  quantitative treatment

a.  equilibrium constants for gaseous reactions;  K_p & K_c

b.  equilibrium constants for reactions in solution

(1)  constants for acid and bases; pK, pH

(2)  solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds

(3)  common ion effect; buffer; hydrolysis

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.  relationship between the rate-determining step and a mechanism

E.  thermodynamics

1.  state functions

2.1^st law:  change in enthalpy; heat of formation; heat of reaction; Hess' law; heats of vaporization and fgusion; calorimetry

3.  2^nd law:  entropy; free energy of formation; free energy of reaction; dependence of chane in free energy on enthalpy and entropy changes

4.  relationship of change in free energy to equilibrium constatnts and electrode potential

IV.  descriptive chemistry  [10 - 15%]

A.  chemical reactivity and products of chemical reactions

B.  relationships in the periodic table:  horizontal, vertical, and diagonal wiht exampels from alkali metals, alkaline earth metals, halogens, and the first series of transition elements

C.  introduction to organic chemistry:  hydrocarbons and funtional groups (structure, nomenclature, chemcial properties)

V.  laboratory  [5 - 10%]

A.  making observations of chemical reactions and substances

B.  recording data

C.  calculating and interpreating results based on the quantitative data obtained

D.  communicating effectively the results of experimental work

 

i.e.  "you're responsible for everything"