Riverdale Collegiate Institute
June Examination 2016
Chemistry, Grade 12, University Preparation
(SCH4U1)
STUDENT’S NAME:_________________________________ HOME FORM: ______
Circle the name of your teacher
Mr. Dermer
Ms. Likins
Friday, June 17th, 2016
9:00 – 11:00 am
2 hours
13 (including this one)
85
Date:
Time:
Duration of Exam:
Total Number of Pages:
Total Number of Marks:
SPECIAL INSTRUCTIONS:

PART A: Using only PENCIL, record the best answer in the SCANTRON sheet
provided. Additional time will not be given to complete the Scantron card.

PART B: Complete each question in the space provided.

Non-programmable calculators may be used, but may not be shared.

Tabular values are located at the BACK of the exam paper and may be detached for
convenience.

Should you require additional space to answer a question from PART B, use the back
side of the page containing that particular question. Be sure to make a clear
indication that the back side of the page is to be marked.
Examination Breakdown:
EXAM PART
TOTAL
MARKS
PART A
Multiple Choice (40 questions)
40 MARKS
50 MINUTES
PART B
Full Solutions (9 questions)
45 MARKS
65 MINUTES
REVIEW EXAM
SUGGESTED
TIME
5 MINUTES
85 MARKS
TOTAL
120 MINUTES
Mark breakdown by unit
Part A: Multiple
Choice
Part B: Short Answers
Total
Unit 1
7
Unit 2
12
Unit 3
6
Unit 4
10
Unit 5
5
Total
40
9
10
5
14
8
14
18
29
5
21
45
85
Unit 1: Electrochemistry
Unit 2:
Unit 3:
Unit 4:
Unit 5:
Atomic Structure and Bonding
Organic Chemistry
Thermodynamics and Kinetics
Chemical Equilibrium
Periodic Table
1
1
H
1.01
18
2
He
2
4
Be
13
5
B
14
6
C
15
7
N
16
8
O
17
9
F
4.00
3
Li
6.94
9.01
10.81
12.01
14.01
16.00
18.99
20.18
11
Na
12
Mg
13
Al
14
Si
15
P
16
S
17
Cl
18
Ar
22.99
24.31
3
4
5
6
7
8
9
10
11
12
26.98
28.09
30.97
32.06
35.45
39.95
19
K
20
Ca
21
Sc
22
Ti
23
V
24
Cr
25
Mn
26
Fe
27
Co
28
Ni
29
Cu
30
Zn
31
Ga
32
Ge
33
As
34
Se
35
Br
36
Kr
39.10
40.08
44.96
47.90
50.94
51.99
54.94
55.85
58.93
58.71
63.55
65.37
69.72
72.59
74.92
78.96
79.90
83.80
37
Rb
38
Sr
39
Y
40
Zr
41
Nb
42
Mo
43
Tc
44
Ru
45
Rh
46
Pd
47
Ag
48
Cd
49
In
50
Sn
51
Sb
52
Te
53
I
54
Xe
85.47
87.62
88.91
91.22
92.91
95.94
99
101.07
102.91
106.4
107.87
112.40
114.82
118.69
121.75
127.60
126.90
131.30
55
Cs
56
Ba
57
La
72
Hf
73
Ta
74
W
75
Re
76
Os
77
Ir
78
Pt
79
Au
80
Hg
81
Tl
82
Pb
83
Bi
84
Po
85
At
86
Rn
132.91
137.34
138.91
178.49
180.95
183.85
186.2
190.2
192.2
195.09
196.97
200.59
204.37
207.19
208.98
210
210
222
87
Fr
88
Ra
89
Ac
104
Unq
105
Unp
106
Unh
107
Uns
223
226
227
261.11
262.11
263.12
262.12
58
Ce
59
Pr
60
Nd
61
Pm
62
Sm
63
Eu
64
Gd
65
Tb
66
Dy
67
Ho
68
Er
69
Tm
70
Yb
71
Lu
140.12
140.91
144.24
147
150.35
151.96
157.25
158.92
162.50
164.93
167.26
168.93
173.04
174.97
90
Th
91
Pa
92
U
93
Np
94
Pu
95
Am
96
Cm
97
Bk
98
Cf
99
Es
100
Fm
101
Md
102
No
103
Lw
232.04
231
238.03
237
242
243
247
249
251
254
253
256
254
257
10
Ne
SCH4U1 – Review
Riverdale Collegiate Institute
SCH4U1 – Review
Standard Reduction Potentials
Riverdale Collegiate Institute
SCH4U1 – Review
Riverdale Collegiate Institute
Exam Review: Breakdown of topics by unit
Unit 1: Redox
Oxidation number
Oxidation
Reduction
Galvanic cells
Balancing Redox Equations
Oxidizing / Reducing agent
Labs
Electrolytic cells
Unit 2: Structure and Properties
Nuclear Atomic model
Quantum model
Electron configuration
Orbitals
Explaining multiple valences
Periodicity
Bonding models
VSEPR
Molecular shape and polarity
Intra/intermolecular forces
Labs
Unit 3: Organic Chemistry
Hydrocarbons
Alcohols
Carboxylic acids
Aldehydes / Ketones
Ethers
Properties
Reactions
Organic halides
Aromatics
Esters
Amines
Amides
Labs
Unit 4: Energy Changes and Rates of Reaction
Heat / Thermal Energy
Measuring the rate of reaction
Factors that affect the rate of a reaction
Q=mcT
Calorimetry
Collision Theory
Heats of Formation
Reaction mechanism
Hess’s Law
Activation energy
Enthalpy diagrams
Potential energy diagrams
Entropy
Gibbs Free Energy
Labs
Unit 5: Equilibrium and Acid/Base Chemistry
Closed systems
Approximation method
Equilibrium expression
Le Chatelier’s Principle
SCH4U1 – Review
Riverdale Collegiate Institute
Review questions from Chemistry 12,McGraw-Hill
Unit 1(pg. 112): 1,2,5,10, 13, 14, 15, 16, 17, 22, 26, 27
Unit 2 (pg. 214): 1-56
Unit 3(pg. 112): 1-45 (Skip 10,12,13,16,17,22,23,27,35,36,37,38,39,41,44)
Unit 4 (pg 316): 1- 38 (Skip 34)
Unit 5 (pg 458): 1- 43 (Skip 10,11,28,33,35,38,39,41)
Additional Questions
1. Compare and contrast the following forces by filling in the table below
Type of force
Intramolecular
Intermolecular
London / Van
der Waals
Particles
involved
Model
Individual
strength
(kJ/mol)
0.05-40
Dipole-Dipole
5-25
Hydrogen Bond
10-40
Ion-dipole
40-600
Metallic
75-1000
Electrostatic
150-1100
Covalent
400-4000
2. Using knowledge from the organic chemistry, and structure and properties unit
predict the relative boiling points of the following molecules. Justify your
answer.
Butanoic acid
Ethoxyethane
2-butanone
2-butanol
Ethyl ethanoate
butanamine
N-ethyl butanamide 2-butene
Butane
2-methylpropane
Example
SCH4U1 – Review
Riverdale Collegiate Institute
SCH4U June Exam Review Package (Chapter 1 – Chapter 10 (inclusive))
Unit 1 - Organic Chemistry - Chapter 1 & 2:
1. Name and draw the isomers of C5H12
2. a) Which of the following formulas correspond with an alkane?
i) C2H4
ii) C6H14
iii) CH3
iv) C4H10
b) Which of the following formulas correspond with a cycloalkane?
i) C2H4
ii) C3H6
iii) C4H8
iv) C5H10
v) C10H22
v) C8H18
3. Circle and identify the functional groups in the molecule below. If it is an alcohol or amine, then
indicate if it is primary, secondary, or tertiary:
H2N
N
O
O
NH
O
O
O
O
OH
H2N
HO
OH
O
HO
4. Rank the following molecules according to their boiling point (from lowest to highest):
butan-1-ol, butanoic acid, butane, cis-but-2-ene, butan-1-amine, butanone, methyl propanoate, 1methoxypropane
5. For the following reactions, draw the product(s) using any structural diagram, provide their IUPAC
names, and identify the type of reaction
a)
b)
c)
d)
e)
f)
g)
ethanol + propan-2-ol
methanol + butanoic acid
ethanamine + ethanoic acid
butan-2-ol + [O]
2-methylpent-2-ene + H2O
hept-3-ene + HCl
propan-1-amine + chloroethane
6. Name the following molecules using IUPAC:
a)
b)
c)
F
OH
OH
Br
O
d)
e)
f)
O
HO
O
OH
O
OH
7. Draw the following compounds:
a) 4-amino-2-chlorohex-1-en-5-yn-3-ol
c) cycloocta-1,7-dien-1-ol
e) propyl 2-hydroxypropanoate
b) 2-amino-3-methylcyclohexanone
d) 5-tert-butyl-8-hydroxy-7-oxodecanal
f) butoxymethanol
SCH4U1 – Review
Riverdale Collegiate Institute
Unit 2: Structure and Properties - Chapter 3 & 4:
1)
Complete the table below:
Molecule
Lewis Structure
VSEPR Notation
Name of Molecular
Shape
Polar Molecule?
(Yes or No)
SCl2
NSF3
H3O+
SF6
FCl22. State the n, l, and ml values for these orbitals:
n
M
ml (all values)
4s
3d
5f
3. In each case, name the element with the following valence electron configuration
a) 1s2
b) 6s24f145d1
c) 3s23p4
d) 4s13d10
4. Explain what n, l, ml, and ms represent
5. Define ionization energy (I.E.) and electron affinity (E.A.). Explain the periodic trends for each.
Suggested Text Questions:
Chapter 3 Review:
pg. 159-160 #4, 5, 7, 9, 10, 13, 14, 16, 19
Chapter 4 Review:
pg. 209-210 #2, 3, 5-7, 9, 15, 16, 19, 29, 30
Unit Review:
pg. 214 – 216 #1, 2, 3, 5-9, 15-17, 20, 30-32, 36-40, 42, 51
Unit 3: Energy Changes and Rates of Reaction
Chapter 5:
1) Two reactions are given by the following equations:
X(g) + W (g) → Z(g) + Y(g) + 30.0 kJ
Z(g) + Y(g) + 25 kJ → P(g)
Find the ∆Hº value for the reaction P(g) → X(g) + W (g).
2) Use the data table of standard enthalpies of formation to help determine the enthalpy of reaction for each of
the following reactions.
(a) N2O4(g) + 3CO(g) → N2O(g) + 3CO2(g)
(b) 4FeS2(s) + 11O2(g) → 8SO2(g) + 2Fe2O3(s)
3)
a) Write the balanced equation for the complete combustion of glucose, C6H12O6(s), to form
carbon dioxide gas and water.
b) When a 2.000 g sample of glucose is burned in a calorimeter, the temperature of 200.00 g
of water rises by 37.3ºC. What is the molar enthalpy of combustion of glucose?
4) Using the data table on standard enthalpies of formation, determine the heat absorbed when a 5.00
g sample of Fe2O3(s) undergoes the following reaction.
6Fe2O3(s) → 4Fe3O4(s) + O2(g)
Recommended Textbook Review Questions:
Page 235 #5-8
Page 238-9 #9 – 12
Page 247 #13-16
Page 254 #21-24 (for #24a also answer using bond enthalpies: answer: -751 kJ/mol
Page 333 #3,4
Chapter 6:
1) Given the following reaction:
D+E F+G
Assume that this reaction has a two step mechanisms. Draw the potential energy diagram for the
reaction that correctly incorporates each of the following labels:


Potential Energy
Reaction Progress
SCH4U1 – Review






Riverdale Collegiate Institute
ΔH = -75 kJ
Ea(rev) = 100 kJ
Transition State
Intermediate A + B
D+E
F+G
a) Is this reaction exo- or endothermic?
b) Determine Ea(fwd) for this reaction. Add this value to your diagram
c) Show how your diagram would change if a catalyst was present.
2) An investigation is carried out in which evidence is collected for the following hypothetical chemical
reaction:
W + 2X + 2Y  Z
(W, X, and Y could be either elements or compounds, but Z is a compound)
a) What is the rate law equation for the reaction?
b) What is the rate-determining step?
c) What is a possible mechanism, including the slow step?
d) Determine the instantaneous rate when [W] = 0.05 mol/L; [X] = 0.1 mol/L; [Y] = 0.002 mol/L
Text questions:
Pg 284 # 5 – 8
Pg 288 # 1 – 7
Pg 301 # 17 – 20
Pg 309 #6, 7, 9
SCH4U1 – Review
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Unit 4: Equilibrium
Chapter 7:
1)
Scientists and technologists are particularly interested in the use of hydrogen as a fuel:
2 H2(g) + O2(g)
2 H2O(g)
K = 1 x 1080 at SATP
What interpretation can be made about the relative proportions of reactants and products in this
system at equilibrium?
2)
Predict the shift in the following equilibrium system resulting from each of the following changes.
4 HCl(g) + O2(g)
2 H2O(g) + 2 Cl2(g) + 113 kJ
(a) an increase in the temperature of the system
(b) an increase in the volume of the container
(c) an increase in the concentration of oxygen
(d) the addition of a catalyst
(e) addition of Ne(g) at constant volume
3) For each example, predict whether, and in which direction, the equilibrium is shifted by the change
imposed. Explain any shift in terms of changes in forward and reverse reaction rates.
4)
In a container at high temperature, ethyne (acetylene) and hydrogen react to produce ethene
(ethylene).
The equilibrium constant is 0.072.At a specific time, the substance concentrations are [C2H2(g)] = 0.40
mol/L, [H2(g)] = 0.020 mol/L, and [C2H4(g)] = 3.2 x10–4 mol/L. Predict the direction of the reaction shift.
5) For the reaction: H2(g) + Br2(g)
2 HBr(g) K = 12.0 at t°C
calculate the concentrations of all three substances at equilibrium, if the following amounts of reactants
are mixed in a 2.00-L reaction container.
(a) 8.00 mol of hydrogen and 8.00 mol of bromine
(b) 12.0 mol of hydrogen and 12.0 mol of bromine
(c) 12.0 mol of hydrogen and 8.00 mol of bromine
6)
CO(g) + H2O(g)
CO2(g) + H2(g)
K = 4.00 at 900°C
In a container, carbon monoxide and water vapour are in the process of reacting to produce carbon
dioxide and hydrogen. The concentrations are: [CO(g)] = 4.00 mol/L, [H2O(g)] = 2.00 mol/L,
[CO2(g)] = 4.00 mol/L, and [H2(g)] = 2.00 mol/L. Determine the direction in which the reaction proceeds
to establish equilibrium.
7) Predict the algebraic sign of the entropy change for each of the following reactions:
8) Calculate the value of ΔG0 for the following reactions and interpret the results:
Text Questions
Pg 333 #2-4
Pg 347 #11-14
Pg 349 - 350 #16 – 20
Pg 352 #21-25
SCH4U1 – Review
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Chapter 10
1) Determine the oxidation number of
a. S in SO2
b. Cl in HClO4
c. S in SO42d. Cr in Cr2O72e. I in MgI2
f. H in CaH2
2) For each of the following chemical reactions, assign oxidation number of each atom/ion
and indicate whether the equation represents a redox reaction. If it does, identify the
oxidation and reduction
3) Write a pair a balanced half-reaction equations for each of the following reactions. Label
each half reaction as either oxidation or reduction.
4) For each of the following, complete the half-reaction equation and classify it as an
oxidation or a reduction:
5) Balance the following equations representing reactions that occur in an acidic solution:
6) Balance the following equations representing reactions that occur in a basic solution:
SCH4U1 – Review
Riverdale Collegiate Institute
SCH4U Final Exam Review Solutions
Chapter 1/2
1.
pentane
2.
2-methylbutane
a) ii, iv, & v
b) ii, iii, & iv
2,2-dimethylpropane
primary amine
tertiary
amine
H2N
N
ketone
3.
ester
O
O
secondary amine
NH
O
aldehyde
ether
O
O
O
tertiary alcohol
OH
amide
H2N
HO
OH
tertiary alcohol
O
carboxylic acid
HO
primary alcohol
4. butane, cis-but-2-ene, 1-methoxypropane, butanone, methyl propanoate, butan-1-amine, butan-1-ol, butanoic
acid
5. a)
b)
c)
d)
O
O
O
O
NH
O
2-ethoxypropane + water
(condensation)
methyl butanoate + water
(condensation/exterification)
e)
N-ethylethanamide + water
(condensation)
f)
butan-2-one
(oxidation)
g)
Cl
NH
Cl
OH
2-methylpentan-2-ol
(hydration)
3-chloroheptane + 4-chloroheptane
(hydrohalogenation)
6. a) 4-isopropylheptane
c) 4-bromo-5-fluorohexane-1,3-diol
e) 5-hydroxy-4-oxooct-7-en-2-ynal
7. a)
Cl
N-ethylpropan-1-amine + hydrogen chloride
(substitution)
b) trans-4-ethylhept-2-ene
d) 2-methylbutyl 2-hydroxypropanoate
f) 2-methylcyclohex-3-en-1-ol
NH2
b)
H2N
OH
c)
d)
O
O
HO
O
OH
e)
OH
f)
HO
O
O
O
Chapter 3/4
State the n, l, and ml values for these orbitals:
4s
3d
5f
n
4
3
5
l
0
2
3
ml (all values)
0
-2, -1, -, 0, 1, 2
-3, -2, -1, 0, 1, 2, 3
SCH4U1 – Review
Riverdale Collegiate Institute
2. In each case, name the element with the following valence electron configuration
a) 1s2
He
b) 6s24f145d1
Lu
c) 3s23p4
S
d) 4s13d10 Cu
3.
n = the main electron energy levels or shells
l = the electron sublevels or subshells
ml = the orientation of a sublevel
ms = the electron spin
4. I.E. = the energy needed to completely remove one electron from a ground state. I.E. increases as one moves
across a period, and decreases as one moves down a group.
E.A. = the change in energy that occurs when an electron is added to an atom. E.A. increases as one moves
across a period and decreases as one moves down a group
Chapter 5
1) 5 kJ
2)a) –778.5 kJ
b) –3310kJ
3) a) C6H12O6(s) + 6 O2(g)  6 CO2(g) + 6 H2O(g)
b)
H0f  -2.81 x 103 kJ/mol
4) 2.46 kJ
5) -92.4 kJ/mol
Chapter 6
1 a. exo b. 25 kJ
2) a. r = 1.2 x 104 L2 smol-2[X][Y]2
b. X + 2Y  product(s)
c.
X + 2Y  B (slow)
answers may vary
B + X + W  Z (fast)
d) 48 molL-1s-1
3) 6.25 %
Chapter 7
1. [products]>>[reactants]
2 a) left
b) left
c) right
d) no effect
3 a) right
b) left
c) no effect
d) left
4. Q = 0.04 (shift right)
5. a. [H2]eq = [Br2]eq = 1.5 mol/L
[HBr]eq = 5.0 mol/L
b. [H2]eq = [Br2]eq = 2.2 mol/L
[HBr]eq = 7.6 mol/L
c. [H2]eq = 3.0 mol/L [Br2]eq = 1.0 mol/L [HBr]eq = 6.0 mol/L
6. Q = 1 (shifts right)
7. a) positive
b) negative
c) negative
8. a. G = -208.05 kJ/mol b. G = 739.2 kJ
Chapter 10
1) a. 4 b) +7 c) +^ d) +6 e) -1 f) -1
2)
3)
4)
e) no effect
e) right
f) no change
SCH4U1 – Review
Riverdale Collegiate Institute
5)
6)
SCH4U1 – Review
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Appendix
SCH4U1 – Review
Riverdale Collegiate Institute
SCH4U1 – Review
Riverdale Collegiate Institute
Periodic Table
1
1
H
1.01
18
2
He
2
4
Be
13
5
B
14
6
C
15
7
N
16
8
O
17
9
F
4.00
3
Li
6.94
9.01
10.81
12.01
14.01
16.00
18.99
20.18
11
Na
12
Mg
13
Al
14
Si
15
P
16
S
17
Cl
18
Ar
22.99
24.31
3
4
5
6
7
8
9
10
11
12
26.98
28.09
30.97
32.06
35.45
39.95
19
K
20
Ca
21
Sc
22
Ti
23
V
24
Cr
25
Mn
26
Fe
27
Co
28
Ni
29
Cu
30
Zn
31
Ga
32
Ge
33
As
34
Se
35
Br
36
Kr
39.10
40.08
44.96
47.90
50.94
51.99
54.94
55.85
58.93
58.71
63.55
65.37
69.72
72.59
74.92
78.96
79.90
83.80
37
Rb
38
Sr
39
Y
40
Zr
41
Nb
42
Mo
43
Tc
44
Ru
45
Rh
46
Pd
47
Ag
48
Cd
49
In
50
Sn
51
Sb
52
Te
53
I
54
Xe
85.47
87.62
88.91
91.22
92.91
95.94
99
101.07
102.91
106.4
107.87
112.40
114.82
118.69
121.75
127.60
126.90
131.30
55
Cs
56
Ba
57
La
72
Hf
73
Ta
74
W
75
Re
76
Os
77
Ir
78
Pt
79
Au
80
Hg
81
Tl
82
Pb
83
Bi
84
Po
85
At
86
Rn
132.91
137.34
138.91
178.49
180.95
183.85
186.2
190.2
192.2
195.09
196.97
200.59
204.37
207.19
208.98
210
210
222
87
Fr
88
Ra
89
Ac
104
Unq
105
Unp
106
Unh
107
Uns
223
226
227
261.11
262.11
263.12
262.12
58
Ce
59
Pr
60
Nd
61
Pm
62
Sm
63
Eu
64
Gd
65
Tb
66
Dy
67
Ho
68
Er
69
Tm
70
Yb
71
Lu
140.12
140.91
144.24
147
150.35
151.96
157.25
158.92
162.50
164.93
167.26
168.93
173.04
174.97
90
Th
91
Pa
92
U
93
Np
94
Pu
95
Am
96
Cm
97
Bk
98
Cf
99
Es
100
Fm
101
Md
102
No
103
Lw
232.04
231
238.03
237
242
243
247
249
251
254
253
256
254
257
10
Ne