Grade 9 Academic Science
Unit Chemistry Practice Test
Answers
Part A. Multiple Choice
1. Anything with mass and volume?
a. Element
b. Space
c. Matter
d. Subatomic Particles
2. If a substance remains the same, but its STATE changes, it is an example of
a. Physical Property
b. Physical Change
c. Chemical Property
d. Chemical Change
3. It has a negative change and virtually no mass.
a. Electron
b. Element
c. Neutron
d. Proton
4. What is the correct number of NEUTRONS in Sodium if it has a mass of 23 and an Atomic
Number of 11
a. 11
b. 12
c. 23
d. 34
5. What is a PURE SUBSTANCE made up of MORE THAN ONE element?
a. Element
b. Compound
c. Solution
d. Mechanical Mixture
e. Heterogeneous Mixture
6. What is the MAXIMUM number of electrons in Orbit #2?
a. Two
b. Four
c. Eight
d. Eighteen
7. Which element is a NOBLE GAS?
a. Hydrogen
b. Oxygen
c. Helium
d. Potassium
8. How many DIFFERENT ELEMENTS are in the chemical formula CH3COOH?
a. 3
b. 6
c. 8
d. 0
9. What does this WHMIS symbol represent?
a. Toxic
b. Biohazardous
c. Flammabl
d. Corrosive
10. What is the IONIC CHARGE of the nitrogen ion?
a. 1+
b. 2+
c. 3+
d. 3e. 2f. 1g. No charge
11. What is the correct chemical name of the following compound: Mg2Cl?
a. Magnesium chlorine
b. Magnesium II chorine
c. Magnesium chlorate
d. Magnesium chloride
12. What type of bond is used to create the ammonia compound NH4?
a. Covalent bond
b. Ionic bond
c. Electron bond
d. Electrical bond
13. What is the IONIC CHARGE of the polyatomic ion in the chemical formula for phosphoric acid
(H3PO4)?
a. No charge
b. 1c. 3
d. 314. “Total Mass of the Products must equal Total Mass of the Reactants” refers to what chemical
rule?
a. Rule of Mass
b. Law of Conservation of Mass
c. Law of Concentration of Mass
d. Equal Product-Reactant Mass Rule
15. What type of chemical reaction will occur in the following equation: Ca(OH)2 + HCl?
a. Decomposition
b. Double Displacement
c. Single Displacement
d. Synthesis
16. In an IONIC COMPOUND, the positive charge always comes first. What is it called?
a. Anion
b. Positive Ion
c. Cation
d. First Ion
17. What SUBATOMIC PARTICLES occur in the NUCLEUS of an atom?
a. Neutrons and Electrons
b. Only Protons
c. Protons and Electrons
d. Protons and Neutrons
Part B – Bohr Rutherford Diagrams
 Draw a Bohr-Rutherford Diagrams for the following elements
18. Calcium
19. Oxygen
Part C – Short Answer
20. There are many ways of changing the RATE of a chemical reaction. Name two.
 Add more reactant
 Heat
 Make more surface area
 Add a catalyst
21. There are four clues of chemical change. Name three
 A new colour will appear
 Heat or light is given off
 Bubbles of gas form
 A solid material forms from a liquid...called a PRECIPITATE
22. On the very first day of class, we learned that Lithium (Li), Sodium (Na) and Potassium (K) all
reacted with water. They all burned and produced a gas. We discovered these elements
were in the same GROUP (Column #1 of the Periodic Table, and as such, they have one
electron in their outer shell. We also learned that Potassium reacted MOST VIOLENTLY…it
burned and, if the gas was collected, exploded. Two reasons for the more violent reaction
was presented. Name ONE.
 Outer electron was further away from attracting + charge
 Other electrons cloudy the attraction
Part D – Fill in the Charts
 Use the Periodic Table to complete the chart
Chart 1 – 9 marks
Element
Element
Symbol
Atomic
Number
Number of
Protons
Number of
Electrons
Number of
Neutrons
Atomic
Mass
Cadmium
Cd
48
48
48
64
112
Mercury
Hg
80
80
80
121
201
Francium
Fr
87
87
87
136
223
Chart 2 – Ionic Charge
 Determine the Ionic Charge for each of the following
Element
Ionic Charge
Ca
+2
Br
-1
N
-3
Chart 3 – Name the Compound
2Al2O3
Mg
+
Chemical Formula
Chemical Name
NaCl
Sodium chloride
K2O
Potassium oxide

MgF2

+
3O2
F2 
2KCl
Ca
4Al +
2HCl
2K

+
CaCl2 + H2
Cl2
Decomposition
Synthesis
Decomposition
Single Displacement
Grade 9 Academic Science
Unit Chemistry – Practice Test
Part A. Multiple Choice
1.
Anything with mass and volume?
a. Element
b. Space
c. Matter
d. Subatomic Particles
2. If a substance remains the same, but its STATE changes, it is an example of
a. Physical Property
b. Physical Change
c. Chemical Property
d. Chemical Change
3. It has a negative change and virtually no mass.
a. Electron
b. Element
c. Neutron
d. Proton
4. What is the correct number of NEUTRONS in Sodium if it has a mass of 23 and an Atomic
Number of 11 and one electron in its outer shell?
a. 11
b. 12
c. 23
d. 34
5. What is a PURE SUBSTANCE made up of MORE THAN ONE element?
a. Element
b. Compound
c. Solution
d. Mechanical Mixture
e. Heterogeneous Mixture
6. What is the MAXIMUM number of electrons in Orbit #2?
a. Two
b. Four
c. Eight
d. Eighteen
7. Which element is a NOBLE GAS?
a. Hydrogen
b. Oxygen
c. Helium
d. Potassium
8. How many DIFFERENT ELEMENTS are in the chemical formula CH3COOH?
a. 3
b. 6
c. 8
d. 0
9. What does this WHMIS symbol represent? .
a. Toxic
b. Biohazardous
c. Flammable
d. Corrosive
10. What is the IONIC CHARGE of the nitrogen ion?
a. 1+
b. 2+
c. 3+
d. 3e. 2f. 1g. No charge
11. What is the correct chemical name of the following compound: Mg 2Cl?
a. Magnesium chlorine
b. Magnesium II chorine
c. Magnesium chlorate
d. Magnesium chloride
12. What type of bond is used to create the ammonia compound NH4?
a. Covalent bond
b. Ionic bond
c. Electron bond
d. Electrical bond
13. What is the IONIC CHARGE of the polyatomic ion in the chemical formula for phosphoric acid
(H3PO4)?
a. No charge
b. 1
c. 3+
d. 314. “Total Mass of the Products must equal Total Mass of the Reactants” refers to what chemical
rule?
a. Rule of Mass
b. Law of Conservation of Mass
c. Law of Concentration of Mass
d. Equal Product-Reactant Mass Rule
15. What type of chemical reaction will occur in the following equation: Ca(OH)2 + HCl?
a. Decomposition
b. Double Displacement
c. Single Displacement
d. Synthesis
16. In an IONIC COMPOUND, the positive charge always comes first. What is it called?
a. Anion
b. Positive Ion
c. Cation
d. First Ion
17. What SUBATOMIC PARTICLES occur in the NUCLEUS of an atom?
a. Neutrons and Electrons
b. Only Protons
c. Protons and Electrons
d. Protons and Neutrons
Part B – Bohr Rutherford Diagrams
 Draw a Bohr-Rutherford Diagrams for the following elements
18. Calcium
19. Oxygen
Part C – Short Answer
20. There are many ways of changing the RATE of a chemical reaction. Name two.
21. There are four clues of chemical change. Name three
22. On the very first day of class, we learned that Lithium (Li), Sodium (Na) and Potassium (K) all
reacted with water. They all burned and produced a gas. We discovered these elements
were in the same GROUP (Column #1 of the Periodic Table, and as such, they have one
electron in their outer shell. We also learned that Potassium reacted MOST VIOLENTLY…it
burned and, if the gas was collected, exploded. Two reasons for the more violent reaction
was presented. Name ONE.
Part D – Fill in the Charts
 Use the Periodic Table to complete the chart
Chart 1
Element
Element
Symbol
Atomic
Number
Number of
Protons
Cd
Number of
Electrons
Number of
Neutrons
48
80
Francium
Atomic
Mass
201
Fr
223
Chart 2 – Ionic Charge
 Determine the Ionic Charge for each of the following
Element
Ionic Charge
Ca
Br
N
Chart 3
Chemical Formula
Chemical Name
NaCl
K2O
PART E – Complete (if required), Balance AND Define the TYPE of chemical reaction for
the following chemical equations

Al2O3
Mg
+
HCl
____________________________
_____________________________

+
O2
F2 
KCl
Ca
Al +

K
+
Cl2
_____________________________
_____________________________