SCH4C1: Unit One Review Assignment
Matter and Qualitative Analysis
Know the following terms:
Energy level:
Atomic number:
Mass number:
Isotope:
Emission spectrum:
Ionic bond:
Covalent bond:
Molecular compound:
Chemical reaction:
Chemical equation:
Synthesis reaction:
Decomposition reaction:
Single displacement reaction:
Double displacement reaction:
Precipitate:
Precipitation reaction:
Ionic equation:
Spectator ion:
Net ionic equation:
Name:
Assignment Value: 5% upon submission ON THE DAY OF
THE TEST, PRIOR TO THE START OF THE TEST. Late
assignments will NOT be accepted.
1. Identify the three subatomic particles, their charges and their location within an atom:
Subatomic Particle
Charge
Location
2. Use your knowledge of the periodic table to complete the following charts:
Element
Symbol
Atomic
Number
Mass
Number
No. of
protons
No. of
electrons
34
No. of
neutrons
45
137
Bi
81
83
3. What can the group number tell you about the atoms within that group?
4. What can the period number tell you about the atoms within that period?
5. What would be the ionic charge of the following atoms?
a) Phosphide ion
b) Calcium ion
c) Bromide ion
d) Aluminum ion
e) Helium
6. Use your knowledge of chemical nomenclature to provide the names or formulas of the given compounds.
Know the rules for ionic vs. molecular compounds.
Name
Formula
Ca3N2
Al2(SO3)3
FeCl3
Pb3(PO4)4
P2O5
CO
CCl4
Name
Formula
Magnesium oxide
Potassium nitrate
Cobalt (III) nitride
Mercury (II) bromate
Dinitrogen tetraiodide
Iodine heptafluoride
7. Draw the Lewis diagram for the formation of the following ionic compounds. Remember, FIRST determine the
formula of the ionic compound.
Ba & S
C&F
Ca & O
Mg & N
8. List three (3) things you must remember when drawing Lewis diagrams for ionic compounds.
9. Draw the Lewis diagram for the formation of the following molecular compounds. Remember, the atoms that
need the most electrons are often in the centre of the molecule.
HCN
PO4
SO3
CH2F2
10. List three (3) things you must remember when drawing Lewis diagrams for molecular compounds.
11. Complete the following chart comparing and contrasting ionic vs. molecular compounds.
Property
Ionic Compounds
Molecular Compounds
Types of elements involved
Transfer or sharing of valence
electrons?
Physical state at room temperature
Melting Point
Boiling Point
Solubility
Electrical Conductivity
12. Why are ionic compounds electrically neutral?
13. Write the word, skeleton and balanced chemical equation for the following reaction.
A solution of hydrogen chloride reacts with sodium carbonate to produce carbon dioxide, sodium chloride, and
water.
Word:
Skeleton:
Balanced:
14. What is the Law of Conservation of Mass?
15. What are the diatomic elements?
16. Balance the following chemical equations. If the reaction is already balanced, you do not need to write any
coefficients in the blanks. Also, identify the type of reaction as a Synthesis, Decomposition, Single Displacement,
Double Displacement or Combustion reaction.
Chemical Equation
Type of Reaction
a)
HgO →
Hg +
b)
NaCl +
AgNO3 →
c)
Cl2 +
d)
C2H6 +
O2 →
CO2 +
H2O
e)
H2O +
Fe →
Fe2O3 +
H2
f)
Al2S3 +
g)
S8 +
Fe →
FeS
h)
N2 +
H2 →
NH3
i)
KClO3 →
j)
Al2(SO4)3 +
Ca →
O2
NaNO3 +
AgCl
CaCl2
Ca(OH)2 →
KCl +
Al(OH)3 +
CaS
O2
Ca(OH)2 →
Al(OH)3 +
CaSO4
17. Use the activity series to determine whether the following single displacement reactions will proceed. If it will,
complete and balance the chemical equations. If will not proceed, simply write “No rxn.”
K+
Ag2S →
Br2 +
NaCl →
Pb4+ + NiCl2 →
Al +
SnO →
F2 +
KI →
Au2+ + PtBr2 →
Mg +
Cu(NO3)2 →
Cl2 +
CaF2 →
18. Use your solubility guidelines to write out the products of the following double displacement reactions. In this
exercise, write the symbol (s) beside any precipitates that will form and (aq) beside any soluble products.
Balance ALL OF THE EQUATIONS (For practice! ).
Al2(SO4)3 (aq) +
Na3PO4 (aq) →
BaCl2 (aq) +
H3PO4 (aq) →
K2SO4 (aq) +
MgF2 (aq)
AlCl3 (aq) +
BaSO4 (aq) →
→
19. Write the balanced, ionic and net ionic equations for the following double displacement reactions. Identify the
spectator ions and the precipitate in each reaction.
Reaction: Potassium chloride and lead (II) nitrate
Balanced:
Ionic:
Net Ionic:
Spectator Ions:
Precipitate:
Reaction: Ammonium phosphate and zinc nitrate
Balanced:
Ionic:
Net Ionic:
Spectator Ions:
Precipitate: