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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
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