SCH4U
Name: ________________________________
SCH4U EXTRA REVIEW QUESTIONS
Naming of Organic Compounds
1. Fill in the following table:
Family of compounds
Structure of functional group.
Alkanes
Alkenes
Alcohols
Aldehydes
Ketones
COOH
or
2. Number the following families (from 1 to 8) in order of lowest to highest IUPAC
naming priority:
___alcohols, ___aldehydes, ___halides, ___alkanes, ___alkenes,
___carboxylic acids, ___ketones, ___alkynes
.
Extra exam review questions page 1
SCH4U
Name: ________________________________
3. In the following pairs of hydroxyl groups, circle the functional group that has
the higher priority and determines the root (family) of the IUPAC name:
Hydroxyl group or halide group
Aldehyde or C-C double bond
C-C double bond or C-C triple bond
Ketone or aldehyde group
Alkyl group or C-C double bond
Carbonyl group or hydroxyl group
4. How many carbon atoms are in the parent chain of the following structures?
5. Identify any cyclic structure(s) above. What prefix do cyclic structures use?
Properties of organic compounds
1. Circle the compound with the higher boiling point in the following pairs:
ethane or ethanol
butanoic acid or propanoic acid
heptan-1-ol or heptan-2-one
pentan-1-ol or butan-1-ol
methane or ethane
propanone or propanoic acid
Extra exam review questions page 2
SCH4U
Name: ________________________________
Electron configurations
1. Fill in the following table using only the periodic table as reference:
Element
Electron configuration
Noble gas
shorthand
Sr
[Xe] 6s1
1s22s22p63s23p64s23d104p65s24d105p6
2. Circle the ions below that have the same electronic configuration as argon:
Ca2+
Cl-
Mg2+
Br-
S2-
K+
VESPR theory
1. Determine the geometry and bond angles (about the central atom) of the
following compounds:
a)
b)
c)
d)
e)
CO2
H2
CH4
H2O
Cl2
2. Draw the Lewis structure for CH3OH. Determine the geometry about the
central atom. What is the ΔEN for the C-O bond? Is the molecule polar?
Hess’s Law problems
Questions are slightly rewritten versions of #1 – 5 from online page (solutions
available on site): http://www.chemteam.info/Thermochem/HessLawIntro1b.html
Extra exam review questions page 3
SCH4U
Name: ________________________________
1. Calculate the value of ΔH° for the formation of Cl3PO(g) from the reaction of
P4O10(s) and PCl5(g) using the following four equations:
a) P4(s) + 6Cl2(g)  4PCl3(g)
ΔH° = -1225.6 kJ
b) P4(s) + 5O2(g)  P4O10(s)
ΔH° = -2967.3 kJ
c) PCl3(g) + Cl2(g)  PCl5(g)
ΔH° = -84.2 kJ
d) PCl3(g) + (1/2)O2(g)  Cl3PO(g)
ΔH° = -285.7 kJ
2. Calculate the reaction enthalpy for the formation of solid anhydrous
aluminum chloride from aluminum metal Al(s) and chlorine gas from the
following data:
2Al(s) + 6HCl(aq)  2AlCl3(aq) + 3H2 (g)
ΔH° = -1049 kJ
HCl(g)  HCl(aq)
ΔH° = -74.8 kJ
H2(g) + Cl2(g)  2HCl (g)
ΔH° = -185 kJ
AlCl3(s)  AlCl3(aq)
ΔH° = -323 kJ
3. Using only the equations below, calculate the molar heat of formation of
nitrous acid HNO2(aq).
NH4NO2(aq)  N2(g) + 2H2O(l)
ΔH° = -320.1 kJ
NH3(aq) + HNO2(aq)  NH4NO2(aq)
ΔH° = -37.7 kJ
2NH3(aq)  N2(g) + 3H2(g)
ΔH° = +169.9 kJ
2H2(g) + O2(g)  2H2O(l)
ΔH° = -571.6 kJ
4. Calculate the ΔH in kilojoules for the preparation of nitrous acid HNO2
from hydrochloric acid and sodium nitrite (NaNO2) using the following
thermochemical equations:
2NaCl(s) + H2O(l)  2HCl(g) + Na2O(s)
ΔH = +507.31 kJ
NO(g) + NO2(g) + Na2O(s)  2NaNO2(s)
ΔH = -427.14 kJ
NO(g) + NO2(g)  N2O(g) + O2(g)
ΔH = -42.68 kJ
2HNO2(l)  N2O(g) + O2(g) + H2O(l)
ΔH = +34.35 kJ
Extra exam review questions page 4
SCH4U
Name: ________________________________
5. Determine the heat of reaction (in kJ) at 298 K for the reaction:
N2H4(l) + O2(g)  N2(g) + 2H2O(l)
given the following equations and ΔH values at the same temperature:
2NH3(g) + 3N2O(g)  4N2(g) + 3H2O(l)
ΔH = -1013 kJ
N2O(g) + 3H2(g)  N2H4(l) + H2O(l)
ΔH = -317 kJ
2NH3(g) + ½O2(g)  N2H4(l) + H2O(l)
ΔH = -142.9 kJ
H2(g) + ½O2(g)  H2O(l)
ΔH = -285.8 kJ
Specific Heat Capacity Questions
Table of Specific Heat Capacities
Substance
Water
Air
Copper
Iron
Specific Heat Capacity J/g⋅°C
4.20
0.990
0.390
0.450
1. What is the unit for energy?
2. What are the units for specific heat capacity?
3. Which of the materials above has the highest specific heat capacity?
4. If 5 g of each of the above materials was exposed to 256J of energy in a
closed system, which would be at the highest temperature afterwards?
5. How much energy is needed to heat up 1 kg of water by 15°C?
6. How much energy would be needed to raise the temperature of a 0.2 moles of
Copper from 11°C to 21°C?
7. Calculate the energy needed to increase the temperature of 150 mL of water
by 30°C. Note: 1 mL of water weighs 1 gram.
8. The molar heat of formation of nitrous acid HNO2(aq) is -129 kJ. How many
kilograms of nitrogen gas do you need to react in the presence of excess oxygen
gas to generate enough heat to raise the temperature of 300 mL of water from
19.0°C to 72.0°C? The equation for the reaction is given below:
½H2(g) + ½N2(g) + O2(g)  HNO2(aq)
Extra exam review questions page 5
SCH4U
Name: ________________________________
Rates of reactions questions.
When hydrogen peroxide solution reacts with iodide ions in aqueous
acid, iodine is liberated.
[H2O2]
0.10
0.20
0.30
0.30
0.30
Initial Concentrations
(mol / L)
[I-]
0.10
0.10
0.10
0.20
0.20
[H+]
0.10
0.10
0.10
0.10
0.20
Initial Rate of Formation
of I2
(mol / L•s)
1.75x10-6
3.50x10-6
5.25x10-6
1.05 x 10-5
1.05 x 10-5
1. Write the balanced equation for this reaction.
2. Use the results to deduce the order of reaction with respect to H2O2(aq). Explain
how you arrived at your answer.
3. Use the results to deduce the order of reaction with respect to I–(aq), giving an
explanation as in #2.
4. Use the results to deduce the order of reaction with respect to H+(aq), giving an
explanation as before.
5. What is the rate equation for the reaction?
6. Calculate the rate constant for the reaction (please give answer in scientific
notation and include proper units).
Rate-determining step
1. The proposed mechanism for the overall reaction
H2O2 + 2H3O+ 2 I-  I2 + 4H2O
involves the following three elementary steps:
Step 1
Step 2
Step 3
H2O2 + I-  IO- + H2O
IO- + H3O+  HIO + H2O
HIO + H3O+ + I-  I2 + 2H2O
(SLOW)
(FAST)
(FAST)
Come up with a rate equation that is consistent with the observed rates of each
step.
2. For the reaction 2N2O5  4NO2 + O2 , a mechanism has been proposed
involving the following elementary steps:
Extra exam review questions page 6
SCH4U
Step 1
Step 2
Step 3
Name: ________________________________
N2O5  NO2 + NO3
NO2 + NO3  NO + NO2 + O2
NO + NO3  2NO2
If it was determined that the rate equation is rate=k[N2O5], which step must be
the rate-determining step? Explain your reasoning.
Solubility
1. What is the solubility product expression for tin(II) hydroxide?
2. The solubility product constant for MgF2 is 6.4 × 10-9. How many grams of
MgF2 will dissolve in 150 mL of H2O at 25°C?
3. The solubility of silver sulfate in water at 100°C is approximately 1.4 g/100mL.
What is the solubility product of this salt at 100°C?
4. For Cu(OH)2, Ksp = 1.6 x 10-19.
(a) What is the molar solubility of Cu(OH)2?
(b) What is the pH of a saturated solution of Cu(OH)2?
5. In which of the following solutions would the solubility of Cu(OH)2 be lower
than in water?
(a) HCl
(b) NaOH
(c) CuSO4 (d) KOH
(e) NaCl
Equilibrium problems
At 448°C the equilibrium constant for the following reaction is 50.0.
H2(g) + I2(g) ⇌ 2HI(g)
a) How many moles of HI will be present at equilibrium when 1.0 mol of H 2(g) and
1.0 mol of I2(g) are allowed to reacted in a 1.0 L container?
b) How many moles of H2 and I2 remain unreacted?
Extra exam review questions page 7
SCH4U
Name: ________________________________
3. A 1.0 L container contains 0.750 mol of CO and 0.275 mol of H2O. After one
hour, equilibrium is reached according the following equation:
CO(g) + H2O(g) ⇌ CO2(g) + H2(g)
Analysis shows that 0.25 mol of CO2 is present. What is the equilibrium constant
for the reaction?
4. Consider the equilibrium:
3I2(g) + 6F2(g) ⇌ 2IF5(g) + I4F2(g)
a) At a certain temperature, 3.0 mol of F2 and 2.0 mol of I2 are placed into a 10.0
L container. At equilibrium, the concentration of IF5 is 0.020 mol/L. Calculate Keq
for the reaction.
Acid Base problems
1. Calculate the pH of a solution prepared by adding 60.0 mL of 0.100 M NaOH
to 100 mL of 0.100 M CH3COOH solution. Ka for acetic acid is 1.8 x 10-5.
2. Circle the ions that would have an effect on the pH of a solution:
CH3COO-
Be2+
Fe2+
NO3-
Fe3+
K+
Cl-
Br-
Mg2+
NO2-
Mn2+
Ni3+
Extra exam review questions page 8