CHEMISTRY 11 FINAL EXAM SUMMARY
Your Chemistry 11 Final Exam will consist of multiple choice & written response questions testing you
on the most important concepts that we learned this year that will prepare you for Chemistry 12.
1) UNIT CONVERSION
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Be able to setup and show all of your work, including units, for conversions
Example:
Silver has a density of 10.5 g/cm3. If you have a pure silver coin with a mass of 6.00 g (about
the same as a Canadian quarter), what is the volume of silver in the coin? Express your answer
in units of mL. (1 mL = 1 cm3)
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Pages 1 to 6 of Measurement Notes, Unit Conversion Worksheet #1 and Unit Conversion
Worksheet #2
2) SIGNIFICANT FIGURES
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Be able to count the number of significant figures in a measured number and perform
calculations to the correct number of significant figures
Be able to take measurements from equipment to the correct # of significant figures
Examples:
How many significant figures are in the following?
103.75 m
270 m
2.50 g
2.756 x 103 mole
15 books
104 mL
10 L
0.0023070 cm
1.57035 x 10-21 g
Perform the following operation to the appropriate number of significant figures:
3.75 + 2.314 + 1.1
3.75 x 2.2
1.36 x 10-2 / 7.202 x 10-4
243.76 – 35.12 – 101.9
Determine the volume reading of the following buret:
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Pages 11 to 20 of Measurement Notes, Determining Significant Figures Worksheet,
Experimental Uncertainty of Apparatus Worksheet and Calculations Involving Significant
Figures Worksheet
3) IONIC & COVALENT COMPOUNDS
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Be able to construct the formula of ionic and covalent compounds given their name
Be able to name ionic and covalent compounds given their formula
Examples:
Write the correct name for each of the following:
Al(ClO4)3
C3S2
N2 O
CuS
Write the chemical formula for each of the following:
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Magnesium hydroxide
Difluorine dioxide
Carbon tetrachloride
Lead (II) sulphate
Pages 5 to 8 and 11 to 12 of Compounds Notes, Ionic Compounds Worksheet #1, Ionic
Compounds Worksheet #2 and Covalent Compounds Worksheet
4) THE MOLE
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Be able to calculate the molar mass of a compound
Be able to use the molar mass of a compound to convert g
Examples:
mol
Calculate the molar mass of each of the following:
Ca(OH)2
(NH4)3PO4
How many moles are in 125 g of PbC2O4?
What is the mass of 2.5 x 10-8 mol of (NH4)2SO4?
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Pages 4 to 6 of The Mole Concept Notes, Molar Mass Worksheet and Mass
Volume
Moles &
Moles Worksheet
5) CHEMICAL REACTIONS
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Be able to balance chemical reaction equations
Be able to write chemical reaction equations, including phases, from the chemical word
equation
Be able to identify and predict the products for the 6 major types of chemical reactions
Examples:
Write a balanced chemical reaction equation, including phases, for the following:
Nitrogen gas reacts with lead (II) oxide powder to yield lead (II) nitride and oxygen gas
Complete, balance and classify the reaction type for each of the following:
_____ F2 + _____ K2S →
_____ Pb(NO3)2 + _____ NaCl →
_____ BaO →
_____ HNO3 + _____ Sr(OH)2 →
_____ C3H5OH + _____ O2 →
_____ Na + _____ N2 →
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Pages 3 to 9 of Chemical Reactions Notes, Balancing Chemical Reactions Worksheet and Word
Equations and Types of Chemical Reactions Worksheet
6) ENERGY CHANGES IN A REACTION
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Be able to define exothermic and endothermic reactions
Be able to write equations for chemical reactions including the energy term and draw their
respective energy diagrams
Examples:
Consider the following reaction:
H2 (g) + S (s) → H2S (g) + 20 kJ
Determine the ΔH
Is the reaction endothermic or exothermic?
Energy
Draw the energy diagram for the above reaction
Progress of the reaction
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Pages 10 to 14 of Chemical Reactions Notes and Energy Changes in Chemical Reactions
Worksheet
7) STOICHIOMETRY
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Be able to relate the coefficients in a balanced equation to the relative number of molecules or
moles (the mole ratio) of reactants and products in the chemical reaction
Be able to perform calculations involving reactions using stoichiometry
Example:
An organic compound, C14H10O3S (s), undergoes combustion according to the following
unbalanced chemical equation:
____ C14H10O3S (s) + ____ O2 (g) → ____ CO2 (g) + ____ H2O (l) + ____ SO2 (g)
What mass of H2O is produced when 0.410 g of CO2 is produced?
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Pages 15 to 17 of Chemical Reactions Notes and Stoichiometry Worksheet
8) SOLUTIONS
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Be able to explain the relationship between [ion] and conductivity of compounds
Be able to write dissociation equations for ionic compounds dissolving to give conducting
solutions
Be able to calculate concentration given appropriate information and perform calculations
converting concentration
moles
volume
Be able to calculate the molarity of each ion in a salt solution given the molarity of the solution
Be able to calculate the concentration of compounds & ions resulting when two solutions of
known concentration and volume are mixed (dilution calculations)
Be able to perform stoichiometry calculations involving molarity
Be able to explain the process by which solutions are prepared to a known concentration
Example:
Complete the following dissociation equation:
K2C2O4 (aq) →
Calculate the concentration of a 50.0 mL solution containing 0.0700 mol of NH4Cl.
What volume of 2.40 M HCl can be made from 100.0 g of HCl?
What is the [Cl-] when 15.0 g of AlCl3 is dissolved in enough water to make 100.0 mL of
solution?
What is the concentration of each ion present when 20.0 mL of 0.50 M FeCl3 is mixed with
80.0 mL of 0.15 M NH4Cl?
What mass of zinc would completely react with 10.0 mL of 0.45 M hydrochloric acid solution?
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Pages 2 to 5 & 12 to 22 of Solutions Notes, Dissociation & Molar Concentration Worksheet,
Dilution Calculations Worksheet, Molarity Stoichiometry Worksheet and [Ion] After Diluting
& Preparing Standard Solutions Worksheet