General Chemistry Final Review
The final will consist of:
100 Multiple choice questions (can cover topics from the entire year)
1 problem sheet front and back (only the second semester topics)
You may use a 3”x5” notecard on your exam provided that notecard is turned before to
the end of last class day before exams start. No cards will be accepted once your last
class period ends.
Major topics covered
Chapter 1 Chemistry an Introduction
Theory
Law
Scientific Method
Lab safety
Chapter 2 Measurements and Calculations
Sig figs
Dimensional analysis (field goals)
Metric system
Density
Chapter 3 Matter
Elements
Compounds
Mixture
Homogeneous/heterogeneous
Chapter 4 Chemical Foundations
Subatomic particles
Proton
Neutrons
Electrons
Nucleus
Orbitals
Rutherford
Thomson
Periodic Table
Periodic trends
Metals
Nonmetals
Metalloids
Alkali metals
Alkaline Earth Metals
Transition metals
Halogens
Noble gases
Chapter 5 Nomeclature
Ions
Cations
Anions
Ionic bonding
Polyatomic ions
Naming ionic compounds
Determining ionic formulas
Ionic dissociation
Molar mass
Covalent Naming
Covalent Prefixes
Naming Acids
Chapter 6 Chemical Reactions
Products
Reactants
Energy
Exothermic
Endothermic
Balancing Equations
Chapter 7 Reactions in an aqueous solution
Preciptiate
Redox reaction
Combustion Reaction
Single Replacement Reaction
Double Replacement reaction
Synthesis Reaction
Double Replacement Reaction
Net Ionic Equation
Spectator Ions
Acid Base Reactions
Chapter 8 Chemical Composition
Mole
Molar Mass
Mole gram conversion
Mole atom conversion
Chapter 9 Chemical Quantities
Stoichiometry
Limiting reactants
Percent Yield
Mole atom conversion
Chapter 11 Modern Atomic Theory
Bohr
Heisenberg
Orbitals
Energy levels
Electron configuration
Quantum numbers
Chapter 12 Chemical Bonding
Covalent bonding
Electronegativity
Polar Covalent Bond
Nonpolar covalent bond
Determining the type of bond
Lewis dot structures
VSEPR
Shapes of Molecules
Chapter 13 Gases
Boyle’s Law
Charles’ Law
Avagadro’s Law
Gay Lussac’s Law
Pressure
Combined Gas Law
Ideal Gas Law
Diffusion
Effusion
Graham’s Law of Effusion
Chapter 14 Liquids and Solids
Kinetic Molecular Theory
Solid
Liquid
Gas
Evaporation
Volatility
Phase Changes
Chapter 15 Solutions
Suspensions
Colloids
Tyndall Effect
Solutions
Solute
Solvent
Polarity of solvent (like dissolves like)
Concentration
Molarity
Saturated
Supersaturated
Chapter 16 Acids and Bases
Acids
Bases
Hydronium
Hydroxide
pH
Dilution
Neutralization
Salts
Chapter 17 Equilibrium
Equilibrium
Le Châtelier’s Principle
Shifting of equilibrium
Buffers
Acidosis/alkanosis
Chapter 19 Nuclear Chemistry
Radiation
Alpha () Radiation
Beta () Radiation
Gamma () Radiation
Showing  decay
Showing  decay
Half life
Determining the age using half life
Fission
Fusion
Transmutation
Meltdown
Nuclear Winter
Nuclear Medicine
X Rays
CT Scan/MRI
Practice Problems for the Chemistry Final
Given the balanced equation
Mg + 2 HNO3  Mg(NO3)2 + H2
1. Calculate how many grams of Magnesium nitrate Mg(NO3)2 will be made from
32.1 g of HNO3 and 15.4 g of Mg.
2. Given the balanced equation
CH4 + 2 O2  2 H2O + CO2
How many grams of water will be produced from 18 g of CH4 (methane) and 49 g of O2?
Balance the equation and do the following problem
O2 +
C4H10 
CO2 +
H2O
3. How much carbon dioxide can be produced from 32 g of oxygen and 45 g of
butane (C4H10) assuming a 39% yield?
Balance the equation and do the following problem
CH3COOH +
NaHCO3 
NaCH3COO +
H2O +
CO2
4. If 25.1 g of sodium acetate is produced from 43.6 g of CH3COOH and 79.6 g of
NaHCO3 what is the percent yield?
PV = nRT
VP/T = VP/T
5. If you collected 120 mL of gas at 25o C and 711 mm Hg, what volume will it
occupy at STP?
6. A chemical reaction will create 17.1 moles of gas, what volume will this occupy
at 19o C and 125 kPa?
7. If you have 32 g of CH4 gas, what volume will it occupy at 19o C and a pressure
of 1.3 atm?
8. Balance the equation ____ Al + ___ HCl  ____ AlCl3 + ____ H2?
If you have 29.5 g of aluminum and react it completely, what volume of H2 gas will you
have at 15o C, and 124 kPa?
M = mol/L
MV = MV
pH = -log[H3O+]
[H3O+] [OH-] = 1 x10-14
9. A solution of vinegar has a [H3O+] of 1.45 x10-5, what is its pH, what is its [OH-]?
10. A solution of milk of magnesia has a pH of 10.6, what is its [H3O+], what is its
[OH-]?
11. A solution of ammonia has a [OH-] of 5.87 x10-4, what is its [H3O+], what is its
pH?
12. If 27 g of HNO3 are dissolved in 1.2 L, what concentration will the solution be?
13. Show the beta decay C-14
14. Show the alpha decay followed by the beta decay of Ra-230
15. Show the alpha decay followed by another alpha decay of W-186
16. Show the beta decay followed by another beta followed by the alpha decay of
decay of K-40.
17. If you originally had 125 g of K-40, you now have 32 g left. How much time has
passed?
18. If you originally had 37 g of Na-22 and you now have 14 g left. How much time
has passed?