Final Exam Review
Chemistry 11 University – SCH 3U1
UNIT 1: Matter & Bonding
1. Discuss the periodic trends as you go across a period or down a group within the periodic
table. (Atomic radius, Ionization Energy, Electron Affinty, Electronegativity)
2. Discuss the make up and the formation of the four types of bonds discussed in class. (Ionic,
Covalent, Polar covalent, Hydrogen)
3. Be able to name each of the following types of substances:
 Binary Ionic Compounds
 Binary Covalent Compounds
 Polyatomic Ionic Compounds
 Binary Acids
 Hydrated Salts
 Ternary Acids
UNIT 2: Chemical Quantities
1. What is a chemical reaction? What are the five signs of a chemical reaction? (4 + 1)
2. What are reactants and products?
3. What is the difference between a word equation, skeleton equation and a balanced chemical
equation?
4. What is the Law of Conservation of Matter?
5. Be able to balance a chemical equation.
6. Synthesis Reactions? How do you identify them?
7. Decomposition Reactions? How do you identify them?
8. (A) Single Displacement Reactions? How do you identify them?
(B) How do you use the activity series in a single displacement reaction?
9. (A) Double Displacement Reactions? How do you identify them?
(B) Do you know how to use the solubility rules?
(C) What is a neutralization reaction?
10. (A) Combustion Reactions? How do you identify them?
(B) What is the difference between a complete and an incomplete combustion reaction?
Final Exam Review
Chemistry 11 University – SCH 3U1
UNIT 3: Chemical Quantities
1. What is the “mole”? Why is it such a useful concept for everyday chemistry?
2. What is Avogadro’s number? How does it relate to the mole concept?
3. What is a “molar mass” for a compound?
4. How many atoms of carbon are there in a 12mol?
5. How many molecules of sulfur trioxide are there in 0.75mol?
6. How many moles of potassium are in 5.75 x 1024 atoms?
7. How any moles of hydrochloric acid are in 750g?
8. How many lead atoms are there in a 5kg pipe? If the pipe were made of aluminum, how
many atoms would there be (still 5kg pipe)?
9. How many molecules of carbon dioxide are there in 500g? How many oxygen atoms are in
the same sample?
10. What is the mass of 7.23 x 1022 molecules of carbonic acid?
11. What is the molar mass of glucose? What is the molecular mass of sodium phosphate?
12. What is the formula mass of aluminum nitrate?
13. What is the average atomic mass of oxygen given the information below?
Abundance
Mass
99.759
15.995
0.037
16.995
0.204
17.999
14. What is the percent composition of ammonium oxide? Iron (III) sulfide?
15. What is the empirical formula of a compound that is 69.9% iron and 30.1% oxygen?
16. What is the empirical formula of a compound that is 26.6% K, 35.4% Cr with the
remaining percent being oxygen?
17. The analysis of a compound shows that it is made up of 21.9% Na, 45.7%C, 1.9% H and
30.5% O. What is the molecular formula of the compound if the molecular mass is 210?
18. An unknown compound is found to have a molecular mass of 70 and to contain 32.0% C,
6.7% H, and 18.7% N, with the rest of the molecule consisting of oxygen. What is the
molecular formula of the compound?
Final Exam Review
Chemistry 11 University – SCH 3U1
CHEMICAL QUATITIES (CONT’D)
19. After a 4.626g sample of silver oxide is heated, 4.306g of silver metal remains. What is the
empirical formula of the silver oxide?
20. When 3.62g of anhydrous calcium chloride is left open to the air, 1.17g of water is
absorbed. Determine the formula of the hydrated salt that is formed?
21. What mass of H2SO4 can be prepared from 50.0g of SO2 given the equation below? We
assume the other reagents are in excess?
2SO2 + O2 + 2H2O  H2SO4
22. What mass of carbon dioxide is produced when 50g of ethyne are combusted in an
abundance of oxygen?
2C2H2 + 5O2  4CO2 + 2H2O
23. If 8.76g of PbF2 precipitate is obtained when 4.50g of KF is added to PbNO3, what is the
percent yield?
2KF + Pb(NO3)2  PbF2 + 2KNO3
24. A solution containing 5.00g of sodium phosphate is mixed with 10.90g of barium nitrate. If
7.69g of Ba3(PO4)2 precipitate is recovered from the reaction, what is the percent yield?
2Na3PO4 + 3Ba(NO3)2  Ba3(PO4)2 + 6NaNO3
25. The most common ore of arsenic, mispickel, can be heated to produce arsenic. How many
grams of mispickel are required to produce 1kg of arsenic?
FeSAs  FeS + As
26. If you have 20g of NaCl and 30g of MgO and you run the reaction below, what will the
limiting reagent be and how many grams of Na2O will you be able to produce?
2NaCl + MgO  Na2O + MgCl2
27. 50g of iron (III) chloride and 50g of potassium sulfide react as per the following equation.
What is the limiting reagent and how many grams of iron (III) sulfide will be able to be
produced? How many gram of KCl will be produced?
2FeCl3 + 3K2SO4  Fe2(SO4)3 + 6KCl
28. The previous reaction (#22) was performed in a lab and produced 7.5g of iron (III) sulfide.
What is the percent yield for this reaction?
29. Write the names, formulas and charges of the eight polyatomic ions you should know for
this course.
30. What is the formula for percent yield? Can you ever have a percent yield of 100%?
Final Exam Review
Chemistry 11 University – SCH 3U1
UNIT 4: Solutions
1. Define the following terms:
 Soluble/Insoluble
 Solution
 Solute
 Solvent
 Aqueous




Miscible/Immiscible
Solid/Liquid/Gas
Saturated solution
Polar/Nonpolar
2. How does a detergent get your clothes clean?
3. A solution contains 15g of sodium chloride in 500g of solution. Calculate the
concentration of the saline solution.
4. How many grams of calcium carbonate must be added to 2 litres of water if I want to
make up a solution with a concentration of 5.75mol/L?
5. How much water is needed if I have 50g of lithium chloride and want to make a
solution with a concentration of 2.5mol/L?
6. How much water must I add to a 1L container of 3.5mol/L saline solution in order to
dilute it to a concentration of 0.50mol/L?
7. The concentration of a hydrochloric acid sample is 8.50mol/L. If the density of the
acid is 1.20g/ml, what is the volume percent of hydrochloric acid in the sample?
8. A solution contains 7.5g of potassium fluoride in 250g of water. Calculate the mass
percent of this solution.
9. A solution contains 50g of sodium phosphate in 3.5L of solution. What is the
concentration of the sodium ions in the solution?
10. A solution contains 100g of copper (II) chloride in 5.35L of solution. What is the
concentration of the copper ions in the solution?
11. What are the two theories concerning the identification of acids and bases? How does
each recognize an acid and a base?
12. What is the difference between a strong acid and a weak acid? Strong base and a
weak base?
Final Exam Review
Chemistry 11 University – SCH 3U1
SOLUTIONS (CONT’D)
13. What is “pH”? What does it measure? What is “pOH”? How are they related?
14. Calculate the hydronium ion concentration of a solution with a pH of:
(A) 3.5
(C) 10.2
(B) 6
(D) 13.7
15. Calculate the pH of a solution that contains:
(A) 3.5x10-4 mol/L of hydronium ions.
(B) 2.3x10-11 mol/L of hydronium ions.
(C) 7.1x10-9 mol/L of hydroxide ions.
(D) 5.6x10-3 mol/L of hydroxide ions.
16. What are the net ionic equations for the following reactions?
(A) K2CO3 (aq) + BaCl2 (aq)  2KCl (aq) + BaCO3 (s)
(B) Na2CO3 (aq) + Ca(NO3)2 (aq)  2NaNO3 (aq) + CaCO3 (s)
17. How do you perform a titration experiment to find the concentration of an unknown
base? You have an entire lab to use at your disposal.
18. In a titration, 10ml of sodium hydroxide solution was neutralized by 16.36ml of
sulfuric acid (c = 0.158mol/L). Determine the concentration of the sodium hydroxide
solution.
19. In a titration, 10ml of hydrochloric acid solution was neutralized by 8.35ml of lithium
hydroxide solution (c = 0.235mol/L). Determine the concentration of the hydrochloric
acid sample.
Final Exam Review
Chemistry 11 University – SCH 3U1
UNIT 5: Gaseous Chemistry
1. Discuss the difference between a solid, liquid and gas using the kinetic molecular
theory to explain.
2. What are the values for STP and SATP?
3. What are the relationships for the three ideal gas laws? Formulas?
4. What are the formulas for the ideal gas law and the combined gas law?
5. What are the molar volumes for any gas at STP and/or SATP?
6. What is the ideal gas constant? Show correct units.
7. How do you find the temperature of a gas measured using Kelvins?
8. A gas that occupies a volume of 3.5L and a pressure of 100kPa is kept under a
constant temperature. What would happen to the pressure of the gas if the container
were to be doubled in size?
9. A gas occupies a volume of 750ml and is 23°C. What would happen to the
temperature of that gas if the volume were reduced to 500ml? The pressure is kept
constant.
10. A gas is at 50°C and 100kPa. What will the new temperature be if the pressure is
raised to 101.3kPa?
11. A gas occupies 12L at 32°C. If the pressure is kept constant, what will the new
temperature be if the volume is reduced to 3L?
12. A gas is at 30°C and a pressure 200kPa – the volume is kept constant. What would
the new pressure of the gas be if the temperature is raised to 75°C?
13. If a given mass of gas occupies a volume of 8.50L at a pressure of 95kPa and 35°C,
what volume will it occupy at a pressure of 75kPa and a temperature of 35°C?
14. A 5L volume gas is kept at -20°C and a pressure of 100kPa. What would happen to
the pressure of that gas if the temperature were to be raised to 30°C and the volume
was doubled?
15. How many grams of oxygen are there in a 25L tank of oxygen at 20°C when the
pressure is 1500kPa?
Final Exam Review
Chemistry 11 University – SCH 3U1
GASES (CONT’D)
16. What will the temperature be of 500g of sulfur trioxide gas that is held in a 2L tank at
250kPa?
17. What volume is occupied by 0.023mol of oxygen gas at 27°C and 107kPa?
18. What is the pressure in a 50L tank that contains 2530g of carbon dioxide at 22°C?
19. Silicon burns in fluorine gas to produce silicon tetrafluoride as per the following
equation:
Si + 2F2  SiF4
Calculate the minimum volume of fluorine gas needed to completely react with 12g
of silicon powder at STP.
20. Nitrogen and oxygen gases combine to produce a nitrogen oxide (undetermined
formula). What is the formula of the nitrogen oxide if it requires 20ml of nitrogen and
60ml of oxygen to produce 40ml of the unknown gas?
21. (A) How many grams of propane are needed to react with 15kg of oxygen according
to the combustion reaction shown below?
(B) How many moles of carbon dioxide will be produced?
(C) What volume will that carbon dioxide gas occupy if the temperature is 200°C and
the pressure is 102kPa?
C3H8 + 5O2  3CO2 + 4H2O
22. Carbon dioxide is commonly prepared by reacting calcium carbonate with dilute
hydrochloric acid (3mol/L) according to the following reaction:
CaCO3 + 2HCl  CaCl2 + CO2 + H2O
(A) Calculate the maximum mass of calcium carbonate that will react with 0.200L of
hydrochloric acid?
(B) Calculate the volume of carbon dioxide that will be produced at 18°C and 104kPa
from the quantities used in part (A).