activation energy, 8.1, 12.1

alcohols

aldehydes

alkali metal salts, solubility of

alkanes

alkenes

alkynes

alpha emission, 14.1, 14.2

amines

amino group

ammonia, Haber process

ammonium salts, solubility of

amphoteric substances

aromatic hydrocarbons

Arrhenius, S. A.

Arrhenius constant, 12.1, 12.2

Arrhenius equation

atomic number

atomic radius

atomic structure and the periodic table

balancing chemical equations

Beer’s law

beta emission, 14.1, 14.2

binding energy

Bohr, Niels

Bohr model

boiling-point, elevation of

bonding

bonds between molecules

bonds within molecules

Coulomb’s law

covalent bonds, 4.1, 4.2

hydrogen bonds

ionic bonds, 4.1, 4.2

Lewis dot structures

metallic bonds

molecular geometry

van der Waals forces, 4.1, 6.1

bonds, breaking

Boyle’s law

bromide salts, solubility of

calculations, showing them on the test paper

calculators

carbon compounds

catalysts

in energy diagrams

and kinetics (rate of reactions)

and calculation of products

writing, 1.1, 17.1

colligative properties

collision theory

colored solutions

combustion, of carbon compounds

common ion effect

compounds, heat of formation of

concentration of a reactant

and equilibrium

and rate laws

concentration of a solution, measuring, 9.1, 15.1

condensation

conduction

conductivity, of ions in solution

conductors of electricity

conjugate pairs

Coulomb’s law

covalent bonds, 4.1, 4.2

de Broglie hypothesis

density

of a gas

of a solution

descriptive chemistry

dissociation constant

electrochemistry. See also oxidation-reduction and electrochemistry

electrolytes

electrolytic cells

electromagnetic radiation

electron affinity

electron capture (as nuclear decay), 14.1, 14.2

electronegativity

electrons

as beta particles

and energy, 3.1, 3.2

Hund’s rule

odd number of, in molecules

and the periodic table

electrostatic attraction

elements

Dalton’s theory

oxidation state of

in the periodic table

symbols of

uncombined

endothermic reactions, 8.1, 8.2

energy

electrons and, 3.1, 3.2

energy (reaction) diagrams

enthalpy, 8.1, 8.2

enthalpy change

entropy, 8.1, 8.2

entropy change

equations. See chemical equations

equilibrium

concentration, volume, temperature and

kinetics and

Le Châtelier’s law

voltage and

equilibrium constant, 8.1, 10.1

and gases

equilibrium expression

equivalence point, 11.1, 15.1

Erlenmeyer flask

essays on the AP Chemistry Exam

about the essays, to keep in mind

acids and bases, 11.1, 11.2

atomic structure and the periodic table

bonding, 4.1, 4.2

gases, 6.1, 6.2

kinetics, 12.1, 12.2

laboratory, 15.1, 15.2

nuclear decay

organic chemistry, 16.1, 16.2

oxidation-reduction and electrochemistry, 13.1, 13.2

phase changes, 7.1, 7.2

solutions, 9.1, 9.2

thermodynamics, 8.1, 8.2

exothermic reactions, 8.1, 8.2

first-order rate laws

flame tests

freezing-point, depression of

equilibrium constant and

Graham’s law

ideal gas equation, for pressure, volume, moles, and temperature

kinetic molecular theory

moles and, 5.1, 6.1

standard temperature and pressure (STP)

van der Waals equation

Group 3A, oxidation state of

group of periodic table

guessing, in multiple-choice section

Haber process

half-equivalence point

Heisenberg uncertainty principle

helium

Henderson-Hasselbalch equation

hydroxide ion, charge of

hydroxide salts, solubility of

hydroxyl group

ideal gas equation

intermediates in a reaction

Internet, for test preparation

iodide salts, solubility of

ionic bonds, 4.1, 4.2

ionic equations

ionization energy

first, second, and greater

ions

conductivity of, in solution

oxidation state of

isomers

isotopes

mass number related to atomic weight of

Le Châtelier’s law, 10.1, 13.1

liquids

London dispersion forces

Lowry, T. M.

mass action, law of

mass defect

mass number, nuclear decay and

measuring concentrations

metals, 3.1, 4.1

molarity, 9.1, 15.1

molecules

and gases, 5.1, 6.1

multistep processes, equilibrium constant and

neon

Nernst equation

network (covalent) bonds

neutralization reactions

neutrons

nitrate ion, charge of

nitrate salts, solubility of

nonmetals

nuclear decay

and atomic number and mass number

mass defect and binding energy

vs. nuclear stability

octets

odor, identifying chemicals by

oxidation-reduction and electrochemistry

voltage and equilibrium

voltage and spontaneity

oxidation state (number)

oxidizing agents (oxidants)

oxoacids

oxygen, oxidation state of

paramagnetism

Pauli exclusion principle

perchlorate ion, charge of

perchlorate salts, solubility of

periodic table, 3.1, 3.2, 3.3

periodic trends

summary of

period of periodic table

pH, 11.1, 11.2

phosphate ion, charge of

phosphate salts, solubility of

pi (double and triple) bond

pipette bulb

Planck, Max

platform balance (triple beam)

positive and negative charges, in atoms

positron emission, 14.1, 14.2

precipitation

precision of laboratory experiments

pressure, and phase changes

problems on the AP Chemistry Exam

about the problems, to keep in mind

acids and bases, 11.1, 11.2

equilibrium, 1.1, 10.1, 10.2

gases, 6.1, 6.2

kinetics, 12.1, 12.2

oxidation-reduction and electrochemistry, 13.1, 13.2

solutions, 9.1, 9.2

stoichiometry and chemical equations, 5.1, 5.2

thermodynamics, 8.1, 8.2

processes, multistep, equilibrium constant and

using the periodic table to determine

quantum theory

Raoult’s law

rate constant, 12.1, 12.2

rate-determining step of a reaction

rate laws

first-, second- and zero-order

related to concentration and time

rate of chemical reactions. See kinetics

reactants

concentration of, 10.1, 12.1

energy of

single

water as a reactant, 16.1, 17.1

reactions

spontaneity of, 8.1, 13.1

the rate law

reducing agents (reductants)

solubility of, 9.1, 9.2

saturated hydrocarbons

Second Law of Thermodynamics

second-order rate laws

separation, methods of

shells (of atoms), 3.1, 3.2

sigma (single) bond

significant figures, 5.1, 15.1

solids

solubility, 9.1, 9.2

transition metal ions in

spontaneity of a reaction

voltage and

standard state conditions

standard temperature and pressure (STP)

state functions

strong acids and bases

sublimation

subshells (of atoms), 3.1, 3.2

substitution reaction

sulfate ion, charge of

temperature

titration, 11.1, 15.1

transition metal ions, in solution

transition metals

oxidation state of

in solution

trigonal bipyramidal shapes

trigonal planar shapes

triple point

unsaturated hydrocarbons

valence electrons

valence shell electron-pair repulsion (VSEPR) model

van der Waals equation

van der Waals forces, 4.1, 6.1

voltage

volume, and equilibrium

volumetric pipette

water

equilibrium for ionization of

gas, liquid, solid phases of

phase diagram for

as a reactant, 16.1, 17.1

weak acids and bases

zero-order rate laws

Index