Chem I Final Exam
Review and Study Guide
The following guide is intended to be a study aid for the upcoming final exam in
Chem I. If you work to know the topic areas listed below you will be well
prepared for this test. The exam will cover the topics listed below, although all
information we went over in class may potentially be on the test. Good luck on the
Final!
Have a great summer!
Know the definitions of:
Chapter 9 – Chemical Reactions
Chemical reaction
Types of Reaction
Reactant
Synthesis
Product
Decomposition reaction
Chemical equation
Single-Replacement reaction
Coefficient
Double-Replacement reaction
Precipitate
Combustion Reaction
Solute
Complete ionic equation
Solvent
Net ionic equation
Aqueous Solution
Spectator ion
Chapter 17 – Chemical Equilibrium
Le Chatelier’s Law
Equilibrium
Chapter 10 – The Mole
Mole
Percent Composition
Avogadro’s Constant
Empirical formula
Molar mass
Molecular formula
Hydrate
Chapter 11 – Stoichiometry
Stoichiometry
Excess reactant
Mole ratio
Theoretical yield
Limiting reactant
Actual yield
Percent yield
Chapter 13 – Gases
Ideal Gas Law (PV = nRT)
Avogadro’s Principle
Ideal Gas Constant
STP
Gas Stoichiometry
Dalton’s Law of Partial Pressure
Chapter 14 – Solutions
Molarity
Solution
Mass-mass percent - %(m/m)
Soluble/Insoluble
Mass/volume percent - %(m/v)
Miscible/immiscible
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Chem I Final Exam
Review and Study Guide
Saturated/Unsaturated Solutions
Concentration (of a solution)
Parts per Million (ppm)
Molality
Kf and Kb
Acid
Base
Neutralization
Strong Electrolyte
Buffer
Weak base/strong base
Dissolve
Mole fraction
Colligative Properties
Freezing Point Depression
Boiling Point Elevation
Chapter 18 – Acid/Base
pH
pOH
[H+]
[OH-]
Weak acid/strong acid
Chapter 7 – Ionic Compounds/Chapter 8 Covalent Compounds
Know how to:
 Read the ion chart to identify elemental ions like oxide (O2-) and polyatomic
ions like carbonate (CO32-)
 Write out a formula from the name of the compound (Ex. Potassium nitrate
is KNO3), and what to do when you have a transition element (Ex. CoCl2 is
cobalt (II) chloride) and a hydrated compound (Ex. BaI2•2H2O is barium
iodide dihydrate).
 Write the formula for covalent compounds (e.g. carbon dioxide)
Chapter 9 – Chemical Reactions
Know how to:
 Balance simple reactions
 Identify simple reactions as decomposition, synthesis, single replacement,
double replacement or combustion.
 Know the seven diatomic elements (H2, N2, O2, F2, Cl2, Br2, I2)
 Decomposition of carbonates yields a metal oxide and carbon dioxide (eg.
CaCO3  CaO(s) + CO2(g))
 Decomposition of chlorates yields a metal chloride and oxygen gas (eg.
2Al(ClO3)3  2AlCl3(s) + 9O2(g))
 Identify the physical states of reactants and products (s= solid, aq=aqueous,
l=liquid, g=gas)
 Write the reaction using formulas if you are given the names and states of
the compounds
 Write the complete ionic equation and net ionic equation of a reaction
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Chem I Final Exam
Review and Study Guide
Chapter 10 – The Mole; Chapter 13.1 – 13.2 (Gases)
Know how to:
 Determine the molar mass of a substance (element or compound).
 Change grams to moles to number of atoms, molecules or formula units and
back
 Determine the empirical formula of a compound given the elemental mass
percentages (or masses) of the compound
 Determine the molecular formula of a compound given the elemental mass
percentages (or masses) and the molar mass
 Determine the empirical formula of a hydrated compound given the mass
percentages of salt and water in the compound
 Determine the number of moles (or mass) of gas given mass, T, & P
 Ideal Gas Law: PV = nRT; how to work with this formula
 Determine density or molar mass of a gas using M=dRT/P
 Determine the partial pressure of a gas given its mole fraction and viceversa.
Chapter 11 – Stoichiometry; Chapter 13.3 – Gas (Gas Stoichiometry)
Know how to:
 Perform mol-mol, mol-mass, mass-mol, and mass-mass stoichiometry
calculations
 Determine the limiting reactant in a reaction
 Determine the amount of product(s) (mass or moles) formed in a limiting
reactant problem
 Determine the mass (or moles) of excess reactant leftover in a limiting
reactant problem
 Use gas volumes like moles in a gas stoichiometry problem
 Determine the volume of gas produced in a reaction at STP or other
conditions
 Determine the percentage yield, theoretical yield, and actual yield of a
reaction
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Chem I Final Exam
Review and Study Guide
Chapter 14 – Solutions
Know how to:
 Calculate the mass percent %(m/m) of a solution
 Calculate the mass-volume percent %(m/v) of a solution
 Calculate the mole fraction of a solution
 Calculate the ppm concentration
 Calculate the molarity of a solution
 Convert between %(m/v) and molarity
 Prepare a solution of a certain molarity and volume (i.e. how many grams of
solute to weigh)
 Determine the new concentration %(m/v) of a solution if it is diluted
(CV=CV)
 Determine the new molarity of a solution if it is diluted (MV=MV)
 Determine the molality of a solution
 Determine the new boiling point or freezing point of a solution with a
nonvolatile solute (∆T=Kb*m*i or ∆T=Kf*m*i)
Chapter 18 – Acids and Bases
Know how to:
 Determine pH from [H+] or [OH-]; pH = -log[H+], pOH = -log[OH-]
 Determine [H+] from pH ([H+] = 10-pH)
 Determine an unknown molarity by titration (neutralization)
 Determine what part of the buffer system reacts with added acid or base
Remember for the final, I will give you:
 a periodic table
 a list of formulas and conversions
 a list of ions and oxidation numbers
 the prefixes and numbers (ex. mono- is one, di- is two, etc.)
 roadmap to change grams to moles to number of particles
 roadmap to change amount (in grams or moles) of Substance A to
amount (in g or moles) of Substance B
It is your responsibility to know how to use them.
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