Chemistry P106 Final Fact Sheet
Important Stuff:
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Bring a pencil.
Bring a scientific calculator.
Bring a card no larger than 3”x5” filled with any desired information
Bring a green scantron sheet with your name written on it.
Use the restroom before you begin taking the final exam.
Turn your cell phone off and put it in your bag before you begin taking the final exam.
Optional Review 8 – 9:30 a.m. Monday, Dec 5
Final Exam 7:30 – 9:30 a.m. Thursday, Dec 8
Majority of Topics Covered on the Final Exam:
Chapter 1
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– Introduction to Chemistry
Terminology
Scientific Method
Physical and chemical change
Physical and chemical properties
Chapter 2
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- Measurement
Metric System
Conversions
Significant Digits (Figures)
Temperature Conversions
Density
Just the
facts, ma’am!
Chapter 3 – Matter
 Classify matter: Elements, compounds, substances, homogeneous or heterogeneous
mixtures
 Physical vs Chemical Change/Properties
Chapter 4
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– Elements, Atoms, Ions
The 3 subatomic particles and their properties (mass, charge)
Atomic number (= number of protons)
Isotopes (same atomic number, different numbers of neutrons)
Periodic Table classification (alkali metal, alkaline earth metals, etc)
Chapter 5 – Nomenclature
 Responsible for naming compounds that contain the following anions: sulfate, sulfite,
nitrate, nitrite, chlorate, chlorite, and halides (e.g. bromide)
 Name binary molecular (2 non-metals; uses Greek prefixes)
Chapter 6
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& 7 – Chemical Equations
Principles, descriptors, coefficients
Balancing equations
Determine reaction type: combustion, double replacement (precipitation or acid/base),
combination (synthesis), decomposition, redox
Chapter 8
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– Chemical Composition
Avogadro’s number : 6.022 X 1023 = 1 mole
Convert between any of the following: grams, moles, atoms, molecules
Molar mass
Percent composition
Empirical formula calc
Chapter 9
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– Chemical Reaction Quantities (Stoichiometry)
Convert moles A  Moles B
Convert grams A Moles B
Convert grams A grams B
Theoretical yield vs. actual yield
Limiting Reactant
Chapter 11 – Modern Atomic Theory
 Orbitals defined
 Electronic configuration of the elements
 Valence electrons
 Periodic Table – Classification by electron config / valence electrons
 Trends: atomic radius, ionization energy
Chapter 12 – Chemical Bonding
 Covalent vs. ionic bonding (electronegativity trend)
 Draw Lewis structures: polyatomic ions, molecules
 Single, double, triple bonds
 Unpaired (non-bonding) electrons
 Resonance Structures
 3D Structures (VSEPR theory—geometries, bond angles, sketch structure)
 Bond and molecular polarity
Chapter 13 – Gases
 Gas Laws:
 Boyle’s Law (P1V1 = P2V2)
 Charles’ Law (V1/T1 = V2/T2)
 Avogadro’s Law (V1/n1 = V2/n2)
 Ideal Gas Law: PV = nRT
 Dalton’s Law of PP: Ptot = P1 + P2 + P3 +…
 Gas Stoichiometry
Chapter 14 – Solids, Liquids
 Heating/Cooling curve (sketch & label)
 Intramolecular vs intermolecular forces
 Intermolecular forces: (DD, HB, LD), and predict properties trends
 Vapor Pressure
 Types of solids (Ionic, Molecular, Atomic)
Chapter 15 – Solutions
 Solution = solute + solvent (definitions)
 Calculate mass percent solution
 Calculate molarity from (grams or moles) solute, and volume solution
 Calculate moles from molarity and volume, and convert to grams if needed.
Also, know what each of these scientists contributed to chemistry: Dalton,
J.J. Thomson, Mendeleev, Rutherford, Bohr, Schrödinger
The Final Exam is worth 22.5% of
your grade. Don’t forget to study!