CHEMISTRY 30 REVIEW PACKAGE
FOR THE FINAL EXAM
Unit 1: Review of Basic Principles
Unit 2: Solubility
Unit 3: Reaction Rates and Equilibrium
Unit 4: Acid/Base Equilibria
Unit 5: Oxidation and Reduction (Redox)
Unit 6: Molecular Geometry
Unit 1: Review of Basic Principles
This means know your PSC 20 backward and forward.
 Types of reactions
 Naming…You’d better not need to review this by now
 Mole conversions. Again, you better be able to do these.
 Using the Activity Series of Metals to determine if a single replacement reaction
would proceed.
 Using a solubility table to determine if a double replacement reaction would
proceed.
 Understanding that if the products of a double replacement reaction were a soluble,
liquid, precipitate or gas
 Making sure to include the states of chemicals in a chemical reaction
 Stoich
 Also, know limiting reagents and excess. Trust me, you should know this…
 Heat in chemical reactions. Endo, exothermic and how to write this in an equation
Unit 2: Solubility
 Understand the term molarity, and be able to calculate any of the three variables
from the formula M = moles ÷ litres.
 Use the formula m1v1 = m2v2 in order to perform dilutions.
 Determine the concentration of individual ions from a balanced dissociation
equation.
 Understand that only ionic substances dissociate…molecular substances can
dissolve, but they do not dissociate.
 Understand that increased temperature works to increase the solubility of a solid but
does the opposite for the solubility of a gas.
 Be able to interpret a solubility curve and use it to predict precipitation
o Super, Un, and plain ol’ saturated
 Define and describe titration.
 Perform titration calculations
Unit 3: Reaction Rates and Equilibrium
 Identify factors that affect the rate of a chemical reaction.
 Understand and explain collision theory.
 Define the term “activated complex.”
 Explain how a catalyst works to speed up a reaction.
 Calculate the rate of a chemical reaction
 Understand that we can never be sure that a proposed reaction mechanism represents
reality: reaction mechanisms are educated guesses!
 The slow step in a reaction mechanism is the rate determining step.
 Be able to create, interpret, and label graphs displaying a reaction mechanism
 Understand and be able to apply Le Chatelier’s Principle: know how changes of
pressure, temperature, and concentration affect the dynamics of an equilibrium.
 When given reaction aA + bB  cC + dD, then Keq = [C]c[D]d ÷[A]a[B]b.
Remember that only compounds that are gases or are aqueous are included in the
Keq expression.
 Be able to calculate Keq: be able to calculate any other variable in the expression for
Keq, given the remaining values.
o Remember there are basically 3 ways to calculate concentrations at
equilibrium using Keq
 Understand the concept of Ksp
 Be able to write a Ksp expression
 Calculate molar solubility of a saturated solution of a substance when we are given
Ksp.
 Calculate Ksp from molar solubility, or from any expression of concentration
 Understand the common ion effect
 Determine whether a precipitate will form by using Ksp – calculate Qsp.
Unit 6: Acid-Base Equilibria.
 State some physical properties of acids and bases
 Construct an operational definition of an acid and a base, using characteristic
properties of those substances
 Describe the Arrhenius and Bronsted-Lowry conceptual definition of acids and bases
 Identify the conjugate bases formed in an acid dissociation
 Identify the conjugate acid of any base
 Associate the acid or base strength with magnitudes of Ka and Kb
 Distinguish between strong and weak electrolytes (acids and bases)
 Recognize substances which are amphiprotic (amphoteric)
 Write dissociation series for a polyprotic acid
 Compare the strengths of the dissociation in the dissociation series for a polyprotic
acid
 Write the equation for the ionization of water
 Write the equilibrium constant expression for the ionization of water
 Show how the common ion effect influences the equilibrium of water’s ionization
when H+ ions or OH- ions are added to water
 State the value of Kw for pure water
 Recognize the relationship between [H+] and [OH-] in an aqueous system
 Calculate the [H+] in solution
 Express the [H+] as pH, determine [H+] given pH
 Recognize the relationship between the pH value and the [OH-]
 Convert values expressed as [H+] and [OH-] to pH and pOH.
 Determine [OH-] when given pH
 Recognize the pH at which various indicators undergo a change in colour using an
equilibrium reaction.
 State the general neutralization equation: acid + base  salt + water
 Write equations for neutralization reactions
 **Titration questions will be in the Unit 2 section**
Unit 7: Oxidation and Reduction
 Define oxidation and reduction in terms of transfer of electrons: LEO goes GER!
 Know how to assign oxidation numbers to elements in their pure form, and in
compounds
 Be able to distinguish redox reactions from non-redox reactions
 Balance redox equations (almost everyone needs to review this for sure)
 Compare reduction potentials for different half-reactions in a table
 Describe and diagram an electrochemical cell (this covers much detail! Think
about all the things you would need to know in order to do this)
 Calculate the voltage generated by any given electrochemical cell
 Be able to perform redox stoichiometry calculations
Unit 6: Molecular Geometry
 Be able to draw orbital diagrams and electron configurations for atoms
 Be able to draw the lewis structure for a molecule
 Be able to identify:
o The Electron group geometry
o Molecular geometry
o Bond angles
o Hybridization around the central atoms (only for sp, sp2, and sp3)
o Intermolecular forces experienced
o Dominant IMF
 Be able to discuss the effects of different intramolecular forces on properties
(ionic vs. covalent vs. metallic bonding)