SCH 3U9 – Chemistry 11 Advanced Placement
Final Examination - Millcreek Secondary School
Student Number: ________________
Full Name: ______________________
Time: 2.5 hours
Teacher’s Name: Dr. McNally
Course Code and Section: SCH 3U9 -
Total Pages: 14
Number of Sections: 4
Period: 3
Instructions:
1. Print your full name and student number on the title page and of the
examination booklet along with every additional sheet you hand in to the
teacher.
2. Ensure to check that no pages are missing from the examination booklet.
3. Read all the instructions and questions carefully.
4. Scientific calculators and reference sheets are permitted, however, cannot
be shared during the examination.
5. Do not separate the examination booklet unless given permission.
Evaluation:
SECTION/PART
STUDENT
SCORE
TOTAL
Section A – Chemical Foundations and Matter
[
]
30
Section B – Atomic Structure and Properties
[
]
30
Section C – Quantities in Chemical Reactions
[
]
20
Section D – Solutions and Solubility
[
]
20
TOTAL:
100
For Exam Review Day Only: I, _____________________, have reviewed the exam and results.
Student Signature: _______________________________
Name: _______________
FINAL EXAMINATION – SCH 3U9
SECTION A: Chemical Foundations and Matter
1. Examine the following reactants. Predict the product(s) and type of
reaction that will occur (S, D, C, DD, SD). Write a balanced chemical
equation for each reaction. If no reaction occurs, write “N.R”. States of
products and reactants are only required for double displacement
reactions. [9]
a. ___ MgCl2 + ___ K2SO4 
b. ___ Li
+ ___ N2

Type: ________
Type: ________
c. ___ Na + ___ Al(NO3)3 
Type: ________
d. ___ CH6 + ___ O2 
Type: ________
e. ___H2SO4
+ ___ RbOH 
Type: ________
f. ___ CaCO3 
Type: ________
g. ___ Mg + ___ CaCl2 
Type: ________
h. ___ AgBr 
Type: ________
i. ___Na2O + ___ HCL 
Type: ________
2. A chemistry professor conducts an experiment for his students. He mixes
sodium chloride and ammonium sulfate. [5]
a. Predict the type of reaction and write a balanced chemical equation
for this reaction.
b. Write the total ionic equation for this reaction.
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Name: _______________
FINAL EXAMINATION – SCH 3U9
c. Write the net ionic equation for this reaction. Ensure to include the
states.
d. What were the spectator ions for this reaction?
e. Briefly describe the difference between a total ionic equation, and a
net ionic equation. Describe the importance of both in your
explanation.
3. Why is selective precipitation important? What compound could be added
to precipitate the sodium ions in a solution of NaCH3COO and
Mg(CH3COO)2? [4]
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Name: _______________
FINAL EXAMINATION – SCH 3U9
4. Fill in the table by describing the three fundamental laws of chemistry. [9]
Law Name/ Person
Who Invented the Law
Law Explanation
Example of Law
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Name: _______________
FINAL EXAMINATION – SCH 3U9
5. Using a balance that is +/- 0.02 g and a graduated cylinder that is +/- 0.04
mL, the following measurements were made for an object. Mass = 30.20 g,
V1 = 15.2 mL, V2 = 16.3 mL. Using these observations, calculate the density
of the object and indicate the +/- uncertainty. Remember to number your
steps and round your answer to significant digits. [3]
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Name: _______________
FINAL EXAMINATION – SCH 3U9
SECTION B: Atomic Structure and Properties
1. Determine if CH3Cl is a polar molecule. Ensure to include a Lewis structure
diagram, bond angles, AXE code, VSPER shape, and a few words of
explanation in your answer. [4]
2. Write formulas or names for the following compounds. [10]
a. CuClO3
f. TiO2
b. sodium nitrate trihydrate
g. chromium (II) hydroxide
c. HCLO2
h. Al2(SO4)3
d. P2S5
i. manganese (III) sulfite
e. iron (III) carbonate
j. Mg3PO4 . 8H2O
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Name: _______________
FINAL EXAMINATION – SCH 3U9
3. What amount of energy is contained in a photon of blue light with a
wavelength of 450 nm? How many of these photons are required to
produce 0.75 J of energy? [4]
4. Using the following diagram sketch and label the type of intermolecular
forces you would expect to find between the two molecules. Would you
expect this molecule to have a high or low boiling point? Explain. [4]
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Name: _______________
FINAL EXAMINATION – SCH 3U9
5. Bromine (atomic weight 79.90 u) has two stable isotopes with isotopic
weights 78.918 u and 80.916 u. [8]
a. What is the percentage abundance of the heavier isotope?
b. Draw the energy level diagram for Bromine.
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Name: _______________
FINAL EXAMINATION – SCH 3U9
SECTION C: Quantities in Chemical Reactions
1. A hydrate of CaCO3 has a mass of 8.45 g before heating. After heating,
the anhydrous compound’s mass is found to be 5.20 g. Determine the
formula of the hydrate. [3]
2. A compound’s percentage composition is 30.0 % carbon, 8.6 % oxygen
and the remainder is hydrogen. If the compound’s molar mass was
determined to be 110.5 g/mol, what is the compound’s molecular
formula? [3]
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Name: _______________
FINAL EXAMINATION – SCH 3U9
3. When 0.85 g of sodium hydroxide reacts with 1.13 g of barium chloride,
0.23 g of sodium chloride is collected.
BaCl2 + 2NaOH  Ba(OH)2 + 2NaCl
a. Determine the limiting reagent [2]
b. Determine the theoretical yield in grams of NaCl [2]
c. What was the percent yield of this reaction? [1]
d. Why is it important to balance equations in stoichiometric
calculations? [2]
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Name: _______________
FINAL EXAMINATION – SCH 3U9
4. An impure sample of MgCO3 has a mass of 2.68 grams and is dissolved in
water. Addition of NH3 solution produced a precipitate of magnesium
hydride with mass 2.32 g. What is the percentage of MgCO3 in the
impure sample? [3]
3MgCO3 + 2NH3  3MgH2 + N2(CO3)3
5. A 0.585 g sample containing carbon, hydrogen and oxygen is burned and
analyzed using a carbon hydrogen analyzer from which 0.358 g of H2O
and 5.357 g of CO2 are collected. The compound’s molar mass is 286
g/mol. If the sample contains carbon, hydrogen and oxygen, determine
its molecular formula. [4]
11
Name: _______________
FINAL EXAMINATION – SCH 3U9
SECTION D: Solutions & Solubility
1. Several 10.00 mL samples of HNO2 (aq) of unknown concentration are
titrated with a 0.300 mol/L solution of KOH (aq). The results for three trials
are shown below.
Trial
Final Burette Volume Reading (mL)
Initial Burette Volume Reading (mL)
Volume of Titrant KOH Added (mL)
1
11.66
00.10
11.56
2
24.97
13.45
11.52
3
30.47
18.93
11.54
a. Balanced Equation:
________________________________________________________
b. What is the concentration of HNO2 (aq)?
c. What is the significance of running multiple titration trials?
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Name: _______________
FINAL EXAMINATION – SCH 3U9
2. Using square arrows, identify the acid, base, conjugate acid and conjugate
base for the following reactions. [5]
a. HF
H2O 
+
b. HNO2
+
F-
H2O 
+
H3O+
H3O+
+
NO2-
c. HCLO4
+
OH-

CLO4-
+
H2O
d. HSO4-
+
PO43- 
SO42-
+
HPO42-
e. HCN
+
NH3

CN-
+
NH4+
3. The World Health Organization’s guideline for safe levels of arsenic in water
is 0.01 ppm (0.01 mg/L). When 1.3 L of water from the Hudson River was
tested, it was found to contain 0.4 mg of arsenic. Is the water safe to drink?
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Name: _______________
FINAL EXAMINATION – SCH 3U9
4. How would you prepare 3.2 L of 0.4 mol/L solution of HCL (aq) starting from
a 15 mol/L stock solution purchased from a chemical company?
5. How much water should be added to 400.0 mL of a solution of HCL with a
pOH of 11.00 to raise the pH to 5.00?
14