SNC2D1 – Chemistry Review Package
Study tips:
 Read through your notes (labs & demos too)
 Make point form notes to summarize the topics
 Complete the attached review sheets
 For extra practice . . .
Do the following textbook review questions:
p. 151 – Q. 1, 2, 3, 5, 6, 7
p. 158 – Q. 1, 2, 3, 5, 6, 7
p.168 – Q. 3, 7, 8
Chap. Review p.174-175 – Q.9, 10, 11, 12, 13, 16, 20
p. 189 – Q. 1, 4, 5, 7, 8
p. 198 – Q. 1, 4, 6, 7
p.206 – Q. 1, 4, 7
Chap. Review p.214-215 – Q.1-7, 8, 10, 11, 12, 13, 15, 17
p. 228 – Q. 1, 3, 4, 5, 6, 7, 8
p. 235 – Q. 1, 2, 3, 4, 6, 7, 8
p.246 – Q. 1, 2, 4
Chap. Review p.252-253 – Q.1-7, 8, 9, 10, 11, 12, 13, 16,
18, 19, 20, 21, 22, 26, 28
Chemistry Topics Review
1
1. Safety Symbols
2. Matter, Physical and chemical properties/changes
3. The Periodic Table – Classifications
 Metals/non-metals/metalloids
 Groups & periods
 Name of groups
4.
Drawing Bohr-Rutherford Diagrams & Lewis Dot Structures
 Atoms/ions
5. Ionic Compounds (Textbook p. 139-146; 148-149)
 Terminology (ion, cation, anion, ionic charge/combining capacity, valence electron,
stable octet, polyatomic ion, binary compound, ternary compound, ionic bond)
 Draw Bohr-Rutherford diagrams/Lewis Dot structures to show the formation of ionic
compounds
 Naming & writing formula
o binary ionic compounds
o ionic compounds with polyatomic ions
6. Molecular Compounds (Textbook p. 152-158)
 Terminology (covalent bond, molecule, binary covalent compound)
 Draw Bohr-Rutherford diagrams/Lewis Dot structures to show the formation of
molecular compounds
 Diatomic molecules (H2, N2, O2, Cl2, Br2, I2, and F2)
 Naming & writing formula - binary molecular compounds
7. Conservation of Mass & Chemical Equations (Textbook p. 159-168)
 Terminology (reactant, product, chemical reaction, chemical equation, coefficient)
 Law of Conservation of Mass
 Writing word equations, skeleton equations, balanced chemical equations
8. Classifying chemical Reactions (Textbook p. 179-198)
 Synthesis, Decomposition, Single displacement, Double displacement
 Combustion, Acid-base reaction
 Predicting products for the different types of reactions
9. Acids and Bases (Textbook p. 179-234; 236-245)
 Terminology (acid, base, ionization, dissociation, pH scale, neutralization)
 Naming and writing formula- Binary acids, Oxyacids
 pH scale
 Differences in pH values
 pH indicators
 Reactions of acids and bases - neutralization
Chemistry Unit Review
2
1) What are the four clues of a chemical change?
a)
b)
c)
d)
2) Elements with similar properties are grouped into ____________________ called groups. Complete
the following chart for each group.
Group
Location in periodic
table
Number of valence
electrons
Type of compound
usually formed
Halogens
Noble gases
Alkali metals
Alkaline earth metals
3) Where are the non-metals and metals located in the periodic table?
4) Complete the following chart, using your periodic table to help you.
# of
Symbol Element name Atomic
Atomic
# of
neutrons
number
mass
protons
Calcium
# of
electrons
Electron
configuration
Sulphur
Carbon
Fluorine
Sodium
Helium
Aluminum
phosphorus
5) A(n) ______________________ is a positively charged ion formed by ___________________ electrons.
A(n) _____________________ is a negatively charged ion formed by ___________________ electrons.
6) Draw a Bohr-Rutherford diagram for the atom of the following 3 elements:
Mg
P
Ne
3
7) Draw a Bohr-Rutherford/Lewis diagram for the stable ions formed by each of the
following atom:
a) State the number of electrons gained or lost to form each ion.
b) State the ionic charge on each of the ions.
c) Name the noble gas that is isoelectric with each of the stable ions.
Ca
F
K
8) For each of the following:
(i) Classifying the type of bond that will form between the two elements as ionic or
covalent.
(ii) Use Bohr-Rutherford/Lewis diagrams to show how electrons are shared or
transferred to form the bonds. Show resulting charges for ionic binding.
(iii) Write the chemical formula.
Calcium combines with fluorine
Nitrogen combines with hydrogen
9) Complete the following chart:
Type of bond
Strategy for getting
stable octet
Types of
elements
involved
Type of
particles
formed
Ionic
Molecular
10) Show the bonding for the following compounds:
Compound Formula
Type of Compound
Lewis Dot Diagram
4
(Ionic or Molecular)
(Show sharing or Transfer)
CaCl2
H2O
Al3P3
NH3
11) Write the chemical formulas for the following compounds:
a) Sodium iodide
b) Carbon monoxide
c) Nitrogen triiodide
d) Hydrochloric acid
e) Sodium phosphate
f) Nitrogen gas
g) Magnesium oxide
h) Phosphoric acid
i) Potassium chlorate
j) Beryllium nitrate
k) Sulphuric acid
l) Aluminum sulphide
m)Hydrofluoric acid
n) Magnesium carbonate
o) Nitric acid
p) Nitrogen and hydrogen
q) Phosphorus and chlorine
r) Sulphur and bromine
s) Oxygen and fluorine
t) Carbon and chlorine
12) Write the names for the following compounds:
a) KCl
5
b) Al2(CO3)3
c) CBr4
d) Na3P
e) SiCl4
f) NI3
g) HF (aq)
h) K2CO3
i) KOH (aq)
j) Na2SO4
k) H3PO4 (aq)
l) SCl2
m)CCl4
n) H2SO4 (aq)
o) NH4OH (aq)
p) I2
q) CaF2
r) NH3
s) HNO3 (aq)
t) CH4
u) OF2
v) Ca(OH)2 (aq)
w) CaCO3
x) H2
y) RaI2
13) There are different types of compounds that are formed when atoms bond together.
Complete the following chart to show the difference between these types.
Characteristics
Ionic Compound
Molecular Compound
Types of atoms involved
Types of bond (ionic or
covalent)
Electrons (shared or
transferred)
Dissolve in water (yes or no)
Conducts electricity
Example:
14) Some elements exist in the form of diatomic molecules. What are these elements?
15) Vinegar is a compound. The chemical formula for vinegar is H3C2O2H
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Type of elements present
Number of atoms of each element
16) a) State the law of conservation of mass.
b) What are the implications of this law during a chemical reaction?
c) What does this law force us to have to do to our equations when we write them?
17) Examine the following word equation:
Propane + oxygen → carbon dioxide + water
a) List all reactants in this reaction.
b) List all the products in this reaction.
18) The products of neutralization reactions are always __________________ and _____________________.
Predict the products and balance the equations.
a) ____NaOH (aq) + ____HCl (aq) →
b) ____Mg(OH)2 (aq) + ____H2SO4 (aq) →
c) ____Al(OH)3 (aq) + ____H2S (aq) →
d) ____Ca(OH)2 (aq) + ____H3P (aq) →
e) ___H2SO4 (aq) + ___NaOH (aq) →
7
19) For each of the following word equations, write the balanced chemical equation (with
states) and classify the reaction.
a) Calcium metal reacts with hydrobromic acid to form aqueous calcium bromide and
hydrogen gas.
b) Solid aluminum oxide is formed when aluminum metal reacts with oxygen gas.
c) Sodium metal reacts with aqueous calcium oxide to produce aqueous sodium oxide and
calcium metal.
d) Nitrogen gas and liquid iodine are formed from nitrogen triiodide gas.
e) Butane (C4H10) gas reacts with oxygen gas to produce liquid water and carbon dioxide
gas.
20) Write a word equation to represent combustion of propane, a fuel used in stoves and home
heating. Then write a balanced chemical equation for this reaction.
21) Classify each of the following reactions, and write skeleton and balanced equations.
a) gallium + hydrochloric acid → hydrogen + gallium chloride
b) Calcium carbonate + hydrochloric acid → carbonic acid + calcium chloride
c) Aluminum + strontium chloride → strontium + aluminum chloride
d) Barium + sulphur → barium sulphide
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e) Bromine + sodium iodide → iodine + sodium bromide
f) Barium nitrate + sodium sulphide → barium sulphide + sodium nitrate
g) Lithium carbonate → carbon dioxide + lithium oxide
h) Calcium + water → hydrogen + calcium hydroxide
i) Sulfur trioxide + water → sulfuric acid
22) What happens when a metal is added to the solution of an ionic compound? Explain with an
example.
23) Predict the products, and write balanced chemical equations.
a) Magnesium is added to hydrochloric acid.
b) Bromine is added to sodium iodide solution.
24) Explain the differences between acids and bases.
Property
Acids
Ion that is present in solution
Bases
Reactivity with metals
Electrical conductivity
Taste
Touch
pH range
Chemical indicators:
Phenolphthalein will turn?
Bromothymol blue will turn?
Litmus paper will turn?
9
25) What does pH measure?
26) a) If apple juice has a pH of 5 and vinegar has a pH of 3, which is more acidic? __________________
b) How many more hydrogen ions are there in the more acidic substance? ____________________
27) How much more acidic is a solution with a pH of 4.5 than a solution with a pH of
a) 5.5?
b) 6.5?
28) How much more basic is a solution with a pH of 12.5 than a solution with a pH of
a) 10.5?
b) 8.5?
29) Write word and chemical equations for the reactions that occur when the following
elements react with oxygen.
a) Barium
b) Chlorine
c) Potassium
d) Carbon
30) Use the physical or chemical properties identified below to classify each solution as acidic,
basic, or neutral.
a) Reacts with magnesium to produce bubbles and conducts electricity
b) Blue litmus stays blue and red litmus stays red
c) Has a pH of 10 and blue litmus stays blue
d) Taste bitter and does not react with magnesium
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31) Predict the products of the following reactions, then balance the equations:
a) Ca + N2 →
b) K + O2 →
c) CsCl →
d) MgS + HCl →
e) KCl + H2SO4 →
f) AlN + Li →
g) BCl3 →
h) CaCl2 + NaOH →
i) Cl2 + HBr →
j) HF(aq) + Al(OH)3 →
k) Ca + O2 →
l) BaCl2 + Na2O →
32) For each of the following questions, do the following:
i. Complete the following word equations,
ii. Write the balanced chemical equation
iii. Type of reaction
a) Silicon + chlorine →
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b) Calcium oxide →
c) Sodium chloride + barium →
d) Aluminum oxide + potassium fluoride →
e) Iodine gas + sodium nitride →
f) Potassium + oxygen →
g) Sodium bromide →
h) Lithium bromide + chlorine →
i) Sodium hydroxide + phosphoric acid →
j) Beryllium chloride + magnesium nitride →
k) Methane + oxygen gas →
l) Ammonia →
m) Propane (C3H8) + oxygen gas →
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