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SCH 4C
EXAM REVIEW
UNIT 1
1. Study the WHMIS symbols on page 479.
2. What does the term qualitative analysis refer to? Give an example of a time
where you carried out a qualitative analysis in class.
3. Distinguish between physical properties and chemical properties. Give an
example of each.
4. Distinguish between physical changes and chemical changes. Give an
example of each.
5. Define and give an example of each of the four classes of matter: elements,
compounds, solutions, and mechanical mixtures.
6. What are the three subatomic particles? For each of these particles give its
relative mass, relative charge, and location in the atom.
7. Give the group number from the periodic table for each of the following:
halogens, alkali metals, noble gases, alkaline earth metals. Where on the
periodic table are the metals and the nonmetals? How do the properties of
metals compare to those of nonmetals, state at least 3 properties?
8. Give the numbers of protons, neutrons and electrons found in each of the
following.
168O
199F
9. Draw Bohr-Rutherford diagrams for the atoms in number 9.
10. Define the following terms: conductivity, electrolyte, and non electrolyte.
11. What are valence electrons? State the octet rule.
12. What is an ion? What is the difference between an anion and a cation?
13. Draw Lewis symbols for the following atoms: H, F, Ar.
14. How does an ionic bond form? What type of elements do ionic bonds form
between? Show what happens to the valence electrons during the formation
of an ionic bond between (a ) Mg and Cl (b) Ca and O
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15. How does a covalent bond form? What type of elements do covalent bonds
form between? Draw Lewis structures for the following molecules: (a) H2O (b)
NH3
16. Use the charts on pages 493 and 494 to help answer these questions
(a) Give the correct formula for: iron(11) oxide, sodium carbonate,
magnesium chloride, copper(11) sulphate, potassium nitrate
(b) Give the correct names for: Ca(NO3)2, K2SO4, Cu(OH)2, HCl, MgCO3
17. Identify each of the following as synthesis, decomposition, single displacement,
or double displacement. Balance each of the equations.
(a) HCl + Zn  ZnCl2 + H2
(b) Mg(NO3)2 + Na2CO3  NaNO3 + MgCO3
(c) H2O  H2 + O2
(d) Na + Cl2  NaCl
(e) H2SO4 + Mg  MgSO4
+ H2
18. Which one of the following two substances would be ionic? Give reasons for
your answer.
SUBSTANCE
MELTING POINT
BOILING POINT
CONDUCTIVITY
A
850ºC
1600ºC
Good
B
43ºC
125ºC
does not
conduct
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UNIT 2 - SCH 4C
1. Define the term mole.
2. Calculate the molar mass of each of the following: (a) C6H6 (b) Ba(NO3)2
(c) K3PO4
ANS: (a) 78.12 g
(b) 261.36 g
(c) 212.27 g
3. What is the mass of 2.4 mol of H2O?
ANS: 43 g
4. How many CO2 molecules do you have if you have 0.0052 mol of CO2?
3.13 X 1021 molecules
ANS:
5. How many moles of Mg do you have if you have 50.0 g of Mg? ANS: 2.06 mol
6. How many moles of Na do you have if you have 8.74 X 1025 atoms of Na?
ANS: 145 mol
7. What is the mass of 4.33 X 10 22molecules of SO2?
ANS: 4.61 g
8. A compound is 38.71 % C, 9.71 % H and 51.58 % O. What is the empirical formula
of this compound?
ANS: CH3O
9. If the actual molar mass of the compound in number 8 is 93.12 g/mol, what is
the molecular formula of this compound?
ANS: C3H9O3
10. Propane reacts with oxygen according to the following equation:
C3H8 + 5 O2  3 CO2 + + 4 H2O
What mass of O2 is needed to react completely with 40.0 g of C3H8? ANS: 145 g
11. Determine the mass of Cu that can be obtained from a reaction between 286.2
g of Cu2O and 318.3 g of Cu2S. They react according to the following equation:
2 Cu2O + Cu2S  6 Cu + SO2
ANS: 381 g
12. Zinc reacts with HCl as shown in the following equation:
Zn + 2 HCl  ZnCl2 + H2
ANS: 82.%
13. In an experiment 16.1 g of FeS is added to an excess of oxygen and the
following reaction occurs:
4 FeS + 7 O2  2 Fe2O3 + 4 SO2
(a) What is the theoretical yield of Fe2O3?
(b) What is the percentage yield if 14.1 g of FeO3 is collected in the lab?
ANS: (a) 14.6 g (b) 96.6%
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UNIT 3 – SCH4C
1. What is a hydrocarbon?
2. (a) What is the difference between a saturated hydrocarbon and an unsaturated
hydrocarbon?
(b) Which type of hydrocarbons are saturated?
(c) Which types of hydrocarbons are unsaturated?
(d) Which are more reactive chemically, saturated hydrocarbons of unsaturated
hydrocarbons?
3. What type of chemical reaction do all hydrocarbons undergo?
4. Write the balanced chemical equation for the complete combustion of the
following hydrocarbons.
(a) ethane
(b) 1 – butene
5. What type of reaction will unsaturated hydrocarbons undergo that saturated
hydrocarbons will not?
6. Write a complete balanced equation for the following addition reactions.
(a)
H
C
CH3
H2C
+ Cl2 
(b)
H3C
H2
C
C
C
CH3
+ 2 Br2 
(c)
H3C
H
C
C
H
CH3
+ H2O 
7. (a) How does the length of the carbon chain effect the melting points and boiling
points of hydrocarbons?
(b) Which of the following would you expect to have the highest boiling point?
(1) CH3CH2CH2CH2CH3
(2) CH4
(3) CH3CH3
8. Are hydrocarbons soluble in water? Why or why not?
9. What are isomers?
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10. Which of the following pairs represents pairs of isomers?
(a)
(b)
H2C CH2
H3C CH3
H
C
H2C
H
C
H2C
(c)
CH3
C
H2
H3C
H
C CH
2
CH3
H3C
H
C
C
H
CH3
11. Classify each of the following as an alkane, an alkene or an alkyne.
(a) propane
(b)
CH2
H2C
(c) ethyne
(d)
H3C
H2
C
C
C
C
H2
H2
C
C
H2
H2
C
CH3
12. Give the correct name for each of the following hydrocarbons.
(a)
H2
H2
H2
C
C
C
C
CH3
C
C
C
H3C
H2
H2
H2C
(b)
(c)
H3C C
CH2
C CH3
(d)
H3C
CH
HC
CH2
H3C
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13. Draw the structural formula and give the molecular formula for:
(a) butane
(b) 1 – hexene
(c) 2 – pentyne
(d) ethyne
(e) 4- nonene
14. Why is no number used in the names “ethene” and “propene”?
15. Why is the name 3 - pentyne incorrect?
16. Describe and explain the relationship between the sizes of hydrocarbon molecules
and their boiling points.
20 What is a functional group?
21. What type of functional group does an alcohol contain?
22. Give the physical properties of alcohols.
23. Write the equation for the complete combustion of methanol.
24. (a) Name the following:
(1) CH3CH2OH
(2) CH3CH2CH(OH)CH3
(3) CH3 CH2 CH2CH(OH) CH2 CH2CH3
(b) Draw the structural formula for each of the following:
(1) 1 – propanol
(2) ethanol
(3) 3 – hexanol
25. What type of functional group does an ether contain?
26. Describe the physical properties of ethers.
27. Explain why methanol has a higher melting point than methane.
29. Consider the following two compounds: CH3CH2CH2CH2CH2CH2OH and
CH3CH2CH2OCH2CH2CH3.
(a) Which is an ether and which is an alcohol?
(b) Which will evaporate at the lower temperature?
(c) Which has the higher solubility in a polar solvent?
30. What type of functional group does a carboxylic acid have?
31. What type of chemical reaction is common for carboxylic acids?
32. What is the functional group for an ester?
34. What are the products and the reactants in an esterification reaction?
41. What is a polymer?
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UNIT 4 – SCH4C
1. What is an electrolyte? What evidence do we have that acids and bases are
electrolytes?
2. List three properties of bases.
3. List three properties of acids.
4. What colour is litmus in acid? In base?
6. Give the Arrhenius definition of an acid.
7. Give the Arrhenius definition of a base.
8. Classify each of the following as an acid, a base, or a salt.
(a) HCl (b) Mg(OH)2 (c) MgCl2 (d) HC2H3O2 (e) NaNO3 (f) KOH
(g) BaBr2 (h) Ca(OH)2 (i) H2SO4 (j) NaOH
10. Show the dissociation or ionization reactions for each of the following:
(a) Ba(OH)2
(b) HNO3
(c) Ca(NO3)2
11. What does pH stand for?
12. Determine the pH of each of the following given the hydrogen ion concentration in
the solution.
(a) [H+] = 10-5 mol/L
(b) [H+] = 10-14 mol/L
(c) [H+] = 10-2 mol/L
(d) [H+] = 10-7 mol/L
(e) [H+] = 10-6 mol/L
13. State whether each of the solutions in number 12 is acidic, basic, or neutral.
14. Find the [H+] in solutions with each of the following pH values.
(a) pH = 5
(b) pH = 10
(c) pH = 13
(d) pH = 4
15. State whether each of the solutions in number 14 is acidic, basic, or neutral.
16. If the pH of one solution is 4 and the pH of another solution is 7, which solution is
more acidic? How many times greater is the [H+] in the more acidic solution?
17. Define the term salt.
18. What are the three characteristic reactions that acids undergo? Write the general
equation for each one.
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