Chemistry Final Exam Review Guide 2014
Mr. Bitar and Mr. Zandonella
Unit
Matter
Atomic
Structure and
Nuclear
Chemistry
Scientific
Measurement
Electrons in
Atoms
Periodicity
Ionic Bonding
Formula
Math
Covalent
Bonding and
Molecular
Shapes
States of
Matter
Topics
Chemical vs. Physical: Properties, Changes.
states of matter, elements and compounds, mixtures, heterogeneous
vs. homogeneous
Atom: Nucleus, electron cloud, protons, neutrons, electrons, atomic
number, mass number, isotopes, calculating atomic mass, ions,
nuclear stability, Half-life, transmutation reactions, fission and fusion
Math: Qualitative and quantitative measurements, scientific
notation, significant digits, SI units, metric conversions, density,
dimensional analysis (factor-label),
Electrons: Valence electrons, configurations, orbital notation,
excited state/ ground state, energy levels, light, waves
Classifications: Groups, periods, ionization energy,
electronegativity, atomic size, ionic size, metals, nonmetals, transition
elements, representative elements
Types of Bonds: ionic bonds, metallic bonds, electronegativity,
octet rule, drawing ionic bonds,
Naming and Writing Formulas: cations, anions, polyatomic
ions, roman numerals, hydrates-prefixes
Mole: Avogadro’s number, mole conversions (mass and particle),
molar mass (formula mass), % composition
Lewis Dot Structures: Octet rule, duet rule, single bonds, double
bonds, triple bonds, shapes (linear, bent, triangular pyramid,
tetrahedral), VSEPR Theory, Bond Angles (109.5, 107, 104.5, 180),
AXE number, lone pair (nonbinding) electrons, bonding electrons.
Polarity: Electronegativity, partial charges, bond polarity (polar
bond, nonpolar bond), molecule polarity (polar molecule, nonpolar
molecule).
Nomenclature: Naming, prefixes
Skills: Drawing & interpreting dot structures, determining polarity,
bond dissociation energy, bond length, empirical formula, molecular
formulas
Intermolecular Forces: London dispersion, dipole-dipole,
hydrogen bonding (relative strengths, evaporation rate, boiling point,
melting point, vapor pressure).
3 States of Matter: Solid, Liquid, Gas (differences in density,
changes in volume, changes in shape, intermolecular forces)
Phase Changes: Sublimation, deposition, condensation,
vaporization, freezing, fusion
Heating/Cooling Curves: Phases and changes in energy
Phase Diagrams: critical point, triple point
Temperature: what it measures, evaporation rate, evaporation
temperature
Pressure: Pressure conversions, vapor pressure
Gases: Ideal Gases, Ideal Gas Law calculations, Kinetic Molecular
Theory (KMT), Real gases
Energy: Unit, Law of Conservation of Energy.
Properties of Liquids: Surface tension, IMF, surfactants, viscosity,
adhesion and cohesion.
Text Book
Sections
3.1 – 3.4
4.1 – 4.4
24.1 – 24.4
2.1 – 2.4
5.1 – 5.3
6.1 – 6.3
7.1 -7.4
10.1 – 10.3,
10.5
8.1 – 8.5
(omit
Resonance
and
hybridization)
12.1 – 12.4,
13.2
Solutions
Chemical
Changes and
Stoichiometry
Reaction
Rates,
Equilibrium
and Entropy
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Solutions: solution, solute, solvent, solvation, hydration,
dissociation
Solubility: soluble, insoluble, solubility rules, factors that affect
solubility, immiscible, miscible
Types of Solutions: saturated solution, unsaturated,
supersaturated
Concentration: Molarity, Molality, Concentrated/Dilute solution.
Skills/Calculations: Dissociation reactions, solubility curves,
molarity and molality calculations, Like dissolves Like
Acids/Bases: pH, acidic vs. basic solutions, calculating pH and pOH
Chemical Equations: Reactants, products, yields/produces
Balancing: Law of Conservation of Mass (atoms), balancing
chemical reactions, word equations (ionic bonds, covalent bonds,
pure elements, diatomics)
Types of Reactions: Composition/Synthesis/Combination,
Decomposition, Single Replacement/Displacement, Double
Replacement/Displacement, Combustion, Oxidation-Reduction,
Acid-base neutralization
Stoichiometry: Mole-Mole, Mass-Mass, Volume Calculations
Redox: oxidation and reduction reactions
Potential Energy Diagram: Labeling (Reactants, Products,
Activated Complex, Activation Energy, Energy [Enthalpy] Changes)
Endothermic, Exothermic, Catalyst
Factors Affecting Reaction Rates: Temperature, Concentration,
Particle Size, Catalysts
Equilibrium: Reversible Reactions, Chemical Equilibrium,
LeChatelier’s Principle, Equilibrium Constant Expression
Entropy/Enthalpy: ∆H, ∆S, spontaneous reactions, changes in
state, gas, dissolving, temperature
14.1 – 14.3,
18.1 (p. 634 –
637), 18.3,
18.4 (p. 659 –
664)
9.1 – 9.3, 11.1,
11.2, 13.3, 19.1
15.1 (p. 516 –
518), 16.1 ,
16.2, 17.1,
17.2, 15.5
Study your notes.
Use your book for reference and sample problems.
Study homework worksheets and problems from the text.
Review the material you found the most difficult first.
Be sure to do some Chemistry, don’t just look at it!
Don’t do all of your studying in one night. Review one unit a night. Spread out your studying.
Form study groups with your friends or ask parents to quiz you.
Take advantage of extra-help and study sessions
Good Luck on the Exam!!!