SCH4U Exam Review
Unit 1 Organic Chemistry
1. Draw the following organic molecules:
a. propane-1,2-diol
b. 2,5,7,-trimethylnon-3-yne
c. 1-ethyl-3-isopropylcyclohexane
d. 4,4-diethylhexanal
e. 4,4,-diethylhexane-2,3-dione
f. 3-methyl-4-phenylhexanoic acid
g.
h. N-ethylpentan-2-amine
i.
Ethyl 2-cyclobutylpropanoate
N-ethyl-N-propyl-2-methylbutanamide
2. Draw and name the products of the following organic reactions:
a. Hex-3-ene + H2O 
b. 4,4-dimethylpent-2-yne + excess H2 
c. Propane + Cl2 
d. Pentan-1-ol + [O] 
e. Benzene + I2 
f.
Ethanol + propanoic acid 
g. butanal [O] 
h. Propanone +[H] 
i.
Tert-butyl pentanoate + H2O 
3. Draw and name all the constitutional isomers of C6H14, of C2H2Cl2.
4. Draw and name the cis-trans isomers of C4H8 .
5. Identify any errors in the following structures by drawing them. Rename them
correctly:
a. 2-ethyl-2,4,4,-trimethylpentane
b. 2,2,2-trimethylethane
c. 2-ethyl-2,4,4,-trimethylpentane
Unit 2 Structure and Properties of Matter
1. Draw an energy level diagram, complete electron configuration and
condensed electron configuration for the following atoms and ions:
Sb, K+, Au
2. Draw Lewis structures and 3-d diagrams for the following molecules or
ions: SO3, ClO31-, PF5. State the AXE formula, shape, type of bond, bond
angle and determine whether the molecule is polar or not.
3. Rank the following molecules in order of increasing solubility in water and
explain their ranking: 2-chloropropane, propan-1-ol, propanone, propane.
Unit 3 Energy and Rates of Reaction
1. In a laboratory investigation into the neutralization reaction: HNO3 (aq) + KOH (s) 
H2O (l) + KNO3 (aq). A researcher adds solid potassium hydroxide to nitric acid solution
in a calorimeter. The mass of KOH added was 5.2 g. The volume of nitric acid solution
is 200mL. The initial temp was 21.0oC and the final temp was 28.1oC. Calculate the
molar enthalpy of neutralization of potassium hydroxide. (ans -64 kJ/mol)
2. The standard enthalpy of combustion of liquid cyclohexane to carbon dioxide and liquid
water is -3824 kJ/mol. What is the standard enthalpy of formation of cyclohexane
C6H12 (l)? (ans. -251.8 kJ/mol)
3. In a student lab, 60.0 mL of a 0.700 mol/L sodium hydroxide solution was neutralized
with 40.0 mL of excess sulfuric acid solution. The temperature increased by 5.60oC.
Calculate the molar enthalpy of neutralization for sodium hydroxide. (ans -55.7 KJ/mol)
4. Nitromethane is a rapid-burning fuel often used in dragsters where rate, not energy
yield, is important.
4 CH3NO2 (g) + 3 O2 (g)  4 CO2 (g) + 2 N2(aq) + 6 H2O (g)
Use Hess’s law to calculate the enthalpy change for the combustion of one mole of
nitromethane.
C(s) + O2 (g)  CO2 (g) ∆H = -393.5 kJ
2 H2 (g) + O2 (g)  2 H2O (g) ∆H = -483.6 kJ
2 C(s) + 3 H2 (g) + N2 (g) + 2 O2 (g)  2 CH3NO2(g) ∆H = -226.2 kJ (ans -643.0 kJ/mol)
Unit 4 Chemical Systems in Equilibrium
1. If 1.00mol
of each carbon dioxide and hydrogen is initially injected into a 10.0L
reaction chamber at 986OC, what are the concentrations of each entity at equilibrium?
(ans [CO]=[H2O]=0.0559 mol/L, [CO2 ]=[H2]=0.0441 mol/L)
CO2 (g) + H2 (g)
CO (g) + H2O (g)
K = 1.60 at 986 oC
2. If 0.20 mol of hydrogen and 0.50 mol of iodine are initially introduced into a 0.500L
reaction chamber, calculate the concentrations of all entities at equilibrium.
H2 (g) + I2 (g)
2 HI (g)
K = 46.0 at 490 oC
(ans [HI]=0.75 mol/L, [H2]=0.03 mol/L,
[I2]=0.63 mol/L)
3. Given that 2.5 mol of carbonyl chloride gas, COCl2 (g) is initially introduced into a 10.00
L rigid container and the following reaction is allowed to reach equilibrium:
CO2 (g) + Cl2 (g)
COCl2 (g)
K = 8.2 x 10
-2
at 626oC
Find the equilibrium concentrations of CO2 and Cl2. (ans [CO2]=[Cl2]=0.25 mol/L)
4.
Calculate the molar solubility of iron II carbonate at 25 oC. The Ksp of FeCO3 is
3.5 x 10
-11
at 25 oC. (ans 5.9 x 10-6 mol/L)
5.
Calculate the molar solubility of zinc hydroxide at 25 oC. The Ksp of Zn(OH)2 (s) is 4.5 x
10
-17
at 25 oC. (ans 2.2 x 10-6 mol/L)
6. Methanoic acid, HCO2H also known are formic acid is partially responsible for the
characteristic itchy rash produced by the leaves od the stinging nettle plant, Calculate
the pH of 0.150 mol/L methanoic acid. The Ka for methanoic acid is 1.8 x 10-4 (ans
2.28)
7. Calculate the pH and [H+] of a 0.30 mol/L solution of butanoic acid, HC4H7O2 . The Ka of
butanoic acid is 1.52 x 10-5 (ans 2.67)
8. Codeine, a weak base has a Kb of 1.73 x 10-6 . Calculate the pH of a 0.02 mol/L solution
of codeine. (ans pH = 10.27)
Unit 5 Electrochemistry
1. Calculate the standard cell potential of a galvanic cell that uses Ag(s) /Ag+(aq) and
Al(s) /Al3+(aq) half-cell reactions. State which half-cell is the oxidation half-cell and
which is the reduction half-cell. (ans Eo =+2.46v oxidation Al/Al3+, reduction Ag/Ag1+)
2. Write the half reactions and calculate the standard cell potential for each reaction.
a.
Zn (s) + Fe
b.
Cr (s) + AlCl3 (aq)  CrCl3 (aq) + Al(s) (ans Cr anode, Al cathode Eo =-0.92v)
c.
2 AgNO3 (aq) + H2O2 (aq)  2 Ag (s) + 2 HNO3 (aq) + O2 (g) (ans H2O anode, Ag
2+
(aq)  Zn2+ (aq) + Fe (s) (ans Zn anode, Fe cathode, Eo =+0.31v)
cathode Eo =+0.10v)
3. Balance the following redox reactions using the half-reaction method:
a.
b.
Zn (s) + NO31- (aq)  Zn2+ (aq) + NH4
CN (aq) +
-
CrO4 2-
1-(aq)
+
I1-
(aq) 
c.
BrO3
d.
ClO1-(aq) + CrO21-(aq)
(aq) 
CNO1-
Br1-
→
1+(aq)
(acidic)
(aq) + Cr(OH)3 (s) (basic)
(aq) + I2 (s) (acidic)
CrO42-(aq) + Cl2(g)
4. Balance the following using the oxidation number method.
a.
MnO4 1-(aq) + Fe2+ (aq)  Mn2+ (aq) + Fe3+(aq) (acidic)
b.
Cr3+(aq) + ClO3
c.
NO31- (aq) + Bi (s)  Bi3+ (aq) + NO2 (aq) (basic)
1-
(aq)  ClO2 (aq) + Cr2O7 2-(aq) (acidic)