Examination Outline & Review
Chemistry, Grade 12 University (SCH4U)
Examination Date:
Exam Duration:
2.0 Hours
Equipment Required:
pencils, pens, eraser, liquid paper, calculator
Exam format:
Part A: Multiple Choice (50 marks, ~ 60 minutes)
Part B: Written Responses/Calculations (30 Marks)
(Choice – Do 5 out of 7)
Topics & Sections to Review in preparation for exam
Chapter/Sections
Topics/concepts
Chapter 4 Î
♦ Intermolecular Forces
Chapter 5 Î
5.1 – 5.5 (inclusive)
♦ Distinguishing between a Chemical system and the
Surroundings
♦ Comparing different types of systems (open vs closed vs
isolated)
♦ Measuring/Calculating heat Changes Î Calorimetry: q =
mc∆T
♦ Recognizing exothermic and endothermic changes
♦ Relating enthalpy (∆H) with heat changesÆ
∆Hsystem = +/- |qsurroundings|
♦ Calculating Enthalpy changes I: ∆H = n∆Hx = q
♦ Representing Enthalpy Changes:
- Thermochemical Equations with energy terms
- Thermochemical Equations with ∆H values
- Molar enthalpies of Reaction (∆Hr)
- Potential energy diagrams
♦ Calculating Enthalpy Changes II: Hess’s Law Æ
∆Htarget = ∑∆Hknown
♦ Calculating Enthalpy Changes III: Standard Enthalpies of
Formation
Chapter 6 Î
6.1 – 6.5 (inclusive)
Chapter 7 Î
7.1 – 7.7 (inclusive)
Chapter 8 Î
8.1, 8.2, 8.3, 8.4, 8.5
♦ Calculating Reaction Rates
♦ Measuring Reaction Rates (changes in pressure/volume;
changes in conductivity; changes in colour (colorimetry
analysis)
♦ Identifying and Explaining the factors that affect Reaction
Rates
♦ Calculating Rate Law
♦ Determining the order of reactants and reaction
♦ Explaining Reaction Rates using Collision Theory & Theory
of the Activated complex
♦ Drawing and analyzing potential energy diagrams
♦ Writing Reaction mechanisms for multi-step processes
♦ Explaining the properties of a system @ equilibrium
♦ Comparing solubility, phase and chemical equilibrium
♦ Writing Equilibrium Law/expression for various systems
♦ Performing Calculations pertaining to systems @
equilibrium: Î ICE Table
- Calculating Keq
- Calculating equilibrium concentrations
- (Remember 100 rule)
• Interpreting the magnitude of Keq
• Comparing Q with Keq to assess the direction an system
will shift in order to reach equilibrium
• Using Le Chatelier’s Principle to predict the adjustments a
system will make in order to re-establish equilibrium after it
has experience a “stress”
• Using the Solubility Chart to predict which ionic salts will
have low/high solubility
• Writing Solubility Equilibrium Law
• Calculating Ksp, given the Solubility
• Calculating Solubility, given Ksp
• Predicting the fomation of precipitates
• Perfoming calculations which involve a common ion.
• Predicting Spontaneity using ∆H, ∆S, & ∆G
♦
♦
♦
♦
Identifying Bronsted-Lowry acids and bases
Recognizing amphoteric (amphiprotic) substances
Identifying conjugate acid-base pairs
Comparing the strength of the conjugate acid-base
pairs..eg. the conjugate base of a strong acid is a very
weak base
♦ Distinguishing between strong acids/strong bases and
weak acids/bases (% ionization; value of Ka/Kb)
♦ Properties of acids and bases
♦ Kw – writing the expression; its value @ SATP?
♦ Calculating the pH, pOH, [H+] and [OH-] of strong
acids/bases Æ pH = -log [H+]; [H+] = 10-pH
♦ Remember pH + pOH = pKw Î 14 @ SATP
♦ Calculating Ka/Kb for weak acids/weak bases
♦ Calculating % ionization for weak acids/weak bases
♦ Illustrating that for conjugate acid/base pairs:
Ka x Kb = Kw
♦ Calculating the pH/pOH for weak acids and weak bases Î
use ICE table to show ionization then use and pH/pOH
equations
♦ Comparing the K values for polyprotic acids
♦ Predicting the acid-base properties of salts
♦ Performing calculations pertaining to acid-base titration
♦ Sketching titration curves for different combinations of acids
and bases (e.g. can you sketch the typical titration curve
which results when a strong acid is titrated with a strong
base?
♦ How can one select an appropriate Indicator for a particular
titration?
♦ Lewis Model of Acids/Bases
♦ Buffers Î
What are they? How do we make them? How do we
calculate their pH after a small amount of acid or base is
added? Can you use Le Chatelier’s principle to explain the
outcome when a small amount of acid or base is added to a
solution that is buffered?
Chapter 9Î
9.1, 9.2
♦
♦
♦
♦
♦
Defining Oxidation & Reduction
Identifying Reducing & Oxidizing Agents’
Knowing how to use the Activity Series of Metals
Determining Oxidation Numbers
Balancing Redox Reactions using: The oxidation number
Method and Half-reaction method