AP Chemistry Final Exam Review

Chapter 1Matter and Measurements

Atom

Element

Law Of Definite Proportions

Important Terms

Mixture

Solution

Physical Properties

Chemical Properties

Intensive Property

Extensive Property

SI units

Precision

Accuracy

Significant figures

Dimensional Analysis

Density = m/v

K = oC + 273

Equations

Solve simple problems using dimensional analysis.

Convert between Celsius and Kelvin

Things You Should Be Able To Do

Chapter 2Atoms, Molecules, and Ions

Nucleus

Proton, Neutron, Electron

Atomic Mass Unit

Important Terms

Isotope

Group

Period

Metal, nonmetal, metalloid

Molecule

Compound

Empirical Formula

Molecular Formula

Ion

Ionic Compound

Polyatomic Ion

None

Equations

Calculate number of subatomic particles in an atom based on basic information about AMU’s and the type of element the atom is.

Work with empirical and molecular formulas.

Name ionic compounds. Determine the formula of an ionic

compound when given the name.

Things You Should Be Able To Do

20, 22, 47, 53, 69

Example Problems

Chapters 3 and 4Stoichiometry

Chemical Equation

Reactants

Products

Important Words

Formula Weight

Mole

Molar Mass

Limiting Reactant

Theoretical Yield

Percent Yield

Aqueous solution

Sovlent

Solute

Electrolyte

nonelectrolyte

Strong and weak electrolyte

Precipitation Reaction

Molecular Equation

Complete Ionic Equation

Net Ionic Equation

Acid

Base

Neutralization Reaction

Oxidation

Oxidation state

Reduction

Concentration

Titration

Equivalence Point

Molarity = moles/L

M1V1 = M2V2

Equations

Balance Equations Calculate Molar Masses Convert between moles and mass Convert between Mass, moles, and number

of particles. Determine percent composition Determine empirical and molecular

formulas from percent composition data. Calculate percent yeild

Things You Should Be Able To Do

1, 8, 9, 21, 25, 41, 44, 63,

Example Problems

Chapter 5 and 19Thermodynamics and Thermochemistry

Thermodynamics

Thermochemistry

Kinetic Energy

Important Terms

Potential Energy

Joule

Calorie

System

Surroundings

Heat

First Law Of Thermodynamics

Endothermic

Exothermic

Enthalpy

Calorimetry

Heat Capacity

Molar Heat Capacity

Specific Heat

Hess’s Law

Enthalpy Of Formation

Standard Enthalpy of Reaction

Standard Enthalpy of Formation

Spontaneous

Isothermal

Second Law Of Thermodynamics

Third Law Of Thermodynamics

Gibbs Free Energy

Standard Free Energy of Formation

q = C x m x ΔT ΔHorxn = sum(nΔHo

f products) – sum(ΔHof

reactants) Δso = sum(nΔS products) – sum(nΔS

reactants) ΔG = ΔH - TΔS ΔGorxn = sum(nΔGo

f products) – sum(ΔGof

reactants) ΔG = ΔGo + RT lnQ ΔGo =- RT ln k

Equations

Understand the mathematical signs associated with thermodynamics.

Use Hess’s law to determine the heat energy transfer during a chemical reaction.

Calculate the heat transferred in a process using calorimetry.

Use standard enthalpies of formation to determine the standard enthalpy of a reaction.

Qualitatively describe entropy and entropy changes.

Things You Should Be Able To Do

Calculate the standard entropy change for a process using standard molar entropies.

Calculate gibbs free energy from the enthalpy and entropy changes at a given temperature.

Predict the effect of temperature on spontaneity given ΔH and ΔS.

Calculate ΔG under nonstandard conditions. Relate Δgo and equilibrium constants.

29, 37, 46, 52,

Example Problems

Chapter 6Electronic Structure Of Matter

Electron Configuration

Ground State

Excited State

Pauli exclusion principle

Important Terms

Hunds Rule

Valance Electrons

None

Equations

Be able to interpret electron energy level diagrams.

Be able to write electron configurations.

Things You Should Be Able To Do

23

Example Problems

Chapter 7Periodic Properties Of The Elements

Effective Nuclear Charge

Atomic Radius

Isoelectronic

Important Terms

Ionization Energy

Electron Affinity

Metallic Character

None

Equations

Understand how effective nuclear charge affects first ionization energy.

Use the periodic table to predict atomic radii, ionic radii, ionization energy, and electron affinity.

Understand how the ionization energy changes as we remove successive electrons.

What You Should Be Able To Do

18, 57

Example Problems

Chemical Bonds

Ionic Bonds

Covalent Bonds

Important Terms

Metallic Bonds

Lewis Symbol

Octet Rule

Lattice Energy

Lewis Structure

Sigma Bond

Pi Bond

Bond Polarity

Nonpolar Covalent Bond

Polar Covalent Bond

Electronegativity

Polar Molecule

Formal Charge

Resonance Structure

Bond Enthalpy

ΔHrxn = Sum(bond enthalpies of bonds broken) – Sum(Bond enthalpies of bonds formed)

Equations

Write Lewis symbols for atoms and ions. Understand lattice energy and arrange compounds

in order of lattice energy. Draw Lewis structures for molecules and

compounds. Calculate formal charges. Use formal charges to select the best possible

Lewis structure. Understand the relationship between bond type,

bond strength, and bond length. Use bond enthalpies to determine the enthalpy of a

reaction.

Things You Should Be Able To Do