SCH3U
Practice Exam
Formulas:
pH = -log[H+]
[H+] = 10-pH
P1V1 = P2V2
V1T2 = V2T1
P1T2 = P2T1
P1V1T2 = P2V2T1

PV = nRT
% yield =
experimental
x 100%
theoretical
Constants
R = 0.08206 Latm/Kmol
= 8.3145 LkPa/Kmol
= 62.4 LmmHg/Kmol
m
V
% error =
experimental-theoretical
x 100%
theoretical
760 mm Hg = 1 atm = 101.3 kPa
STP = 1 atm, 0oC
Multiple choice and true or false questions
(1 mark each)
1.
Which of the following is NOT a property of oxygen?
a)
colourless
b)
does not support combustion
c)
expands when heated
d)
forms an oxide when reacting with mercury
e)
gaseous at room temperature
2.
What must be done to classify elements?
a)
consider colour only
b)
consider one property for all elements
c)
group together those with different melting points
d)
group together those with similar properties
e)
measure their mass
3.
Which of the following statements best describes the metalloids? They:
a)
are chemically stable
b)
have metallic and non-metallic properties
c)
are not elements
d)
are good insulators
e)
are not used in transistors
4.
A bottle contains 5 L of air. You separate the constituents and find a volume of 4
L of nitrogen. What is the percentage, volume-wise, of nitrogen in air?
a)
20%
b)
44%
c)
50%
d)
56%
e)
80%
5.
Which of the following properties best applies to the elements of the noble gas
family?
a)
great reactivity of the elements
b)
rarest of all elements
c)
are gases at room temperature
d)
form negative ions
e)
are solids at room temperature
6.
Under constant pressure, an increase in temperature will:
a)
increase the volume
b)
decrease the volume
c)
not change the volume
d)
increase, then decrease the volume
e)
decrease, then increase the volume
7.
What is the maximum number of electrons in energy level n=2?
a)
8
b)
2
c)
32
d)
18
e)
50
8.
How many valence electrons does a magnesium atom have?
a)
1
b)
2
c)
8
d)
12
e)
24
9.
The atomic number of an element is 31 and the mass number of one of its atoms
is 65. This atom contains:
a)
31 neutrons
b)
34 electrons
c)
65 protons
d)
34 neutrons
e)
34 protons
10.
A temperature of 400K corresponds to:
a)
27oC
b)
127oC
c)
227oC
d)
327oC
e)
427oC
11.
Identify the anion.
a)
He
b)
Ca2+
c)
F
d)
Na
e)
F-
12.
A gas is heated in a closed rigid container. The molecules:
a)
move faster
b)
move slower
c)
get closer to one another
d)
occupy more space
e)
exert less pressure
13.
Identify the particle that must receive 2 electrons to acquire a charge of +1.
a)
O2b)
Al3+
c)
Fe2+
d)
K
e)
Ne
14.
An ionic bond is the transfer of an electron from a:
a)
metal to a non-metal
b)
non-metal to metal
c)
metal to another metal
d)
non-metal to another non-metal
e)
metal to a noble gas
15.
The piece of lab equipment that is used in a titration is:
a)
burette
b)
beaker
c)
test tube brush
d)
volumetric flask
e)
watch glass
16.
According to the solubility graph, what is the solubility of potassium nitrate at 50oC?
a) 35 g/100 g H2O
b) 50 g/100 g H2O
c) 55 g/100 g H2O
d) 60 g/100 g H2O
e) 80 g/100 g H2O
17.
Which of the following are polar molecules?
i)
CH4
ii)
iii) Br2
iv)
a)
1 and 2
b)
1 and 4
c)
2 and 4
d)
2 and 3
e)
3 and 4
H2O
H-F
18.
17- Which of the following is an element?
a)
air
b)
milk
c)
mercury
d)
salt
19.
An example of a mixture is:
a)
water
b)
sulphur
c)
carbon dioxide
d)
soil
20.
A substance is homogeneous if:
a)
all its particles have the same colour
b)
it is made of particles which are small
c)
all its particles are soluble in water
d)
all samples of this substance look identical
21.
In a chemical reaction, the mass of the reactants compared to the mass of the
products is:
a)
always different
b)
always the same
c)
smaller
d)
larger
22.
The percentage of sulphur in H2SO4 is:
a)
2%
b)
16%
c)
33%
d)
50%
e)
83%
23.
At STP, 1 mole of a gas corresponds to:
a)
0.224 L
b)
2.24 L
c)
4.24L
d)
22.4 L
e)
24.2 L
24.
215 K is equivalent to:
a)
–85 oC
b)
–58 oC
c)
58 oC
d)
85 oC
e)
245 oC
25.
Which of the following is considered to be an air pollutant?
a) oxygen
b) nitrogen oxides
c) water vapour
d) nitrogen
26.
A substance formed of two or more elements bonded chemically is a:
a)
solution
b)
compound
c)
pure substance
d)
mixture
27.
Pure substances:
a)
have a variable composition
b)
have three visible phases
c)
have constant physical properties
d)
are heterogeneous
28.
Solutions of barium hydroxide and calcium nitrate are mixed. What precipitate will
form?
a) barium nitrate
b) calcium hydroxide
c) barium nitrate and calcium hydroxide
d) there will be no precipitate formed
29.
The vapour pressure of water at 65oC is:
a) 6 kPa
b) 19 kPa
c) 25 kPa
d) 31 kPa
e) 65 kPa
30.
A glass cylinder contains 2 gases at a pressure of 106 kPa. If one gas is at 7
kPa, what is the pressure of attributed to the other gas?
a) 2 kPa
b) 7 kPa
c)
9 kPa
d) 99 kPa
e) 113 kPa
31.
What is the [H+] of a solution that has a pH of 12?
a) 12 x 101 M
b) 1 x 1012 M
c) 1 x 10-12 M
d) 1 x 10-2 M
e) 1 x 10-1.2 M
32.
A hydrochloric acid solution contains a concentration of hydrogen ions of 5.8 x
10-4 M. What is the solution's pH?
a) -3.2
b) -1
c) 0.8
d) 3.2
e) 4.8
33.
A rotting apple is an example of a chemical change.
a) true
b) false
34.
Relish is an example of a heterogeneous mixture.
a) true
b) false
35.
Gadolinium is an element.
a) true
b) false
36.
According to the activity series, if you place a piece of zinc in a solution of copper
(II) chloride, it will dissolve.
a) true
b) false
37.
An element's atomic number represents the element's atomic mass.
a) true
b) false
38.
A neutral element has an equal number of protons and neutrons.
a) true
b) false
39.
There is a maximum of 4 electrons which can occupy an atom's first energy level.
a) true
b) false
40.
25oC corresponds to 298.15 K
a) true
b) false
41.
One mole corresponds to 2.07 x 10-23
a) true
b) false
42.
H2SO3 is called sulphurous acid.
a) true
b) false
43.
The molar mass of KOH is 17 g/mol.
a) true
b) false
44.
The difference in electronegativity from calcium to iodine is 3.66
a) true
b) false
45.
The bond between copper and fluorine is ionic.
a) true
b) false
46.
BCl3 has polar covalent bonds.
a) true
b) false
Fill in the Blanks
0
1
7
101.3
-273
blue
alkali
red
atom
1.
(1 mark each)
bromine
carbon
cation
electronegativity
exothermic
alloys
indicator
ionic
larger
lower
litre
manometer
mercury
moles
rare gas
oxidation
precipitate
are characterized by their high chemical stability.
2.
is the only metal element which is a liquid at room
temperature.
3.
is the only non-metal element which is a liquid at room
temperature.
4.
In the ideal gas law formula, 'n' stands for
5.
Rusting iron is an example of an
.
.
6.
Positive ions are also called
7.
The elements of family 1 are also named
8.
Alkali metals all have
9.
The attractions of a nucleus for the electrons that bond it to another nucleus is
its
.
10.
Lithium fluoride is an example of an
11.
An
is the smallest particle of a substance that can exist
freely and have the properties of the substance.
12.
The pressure exerted by a gas in a closed container is measured with a
.
13.
In the Celsius scale, absolute zero corresponds to
oC.
14.
STP corresponds to a temperature of
oC
15.
STP corresponds to a pressure of
kPa.
16.
The molar concentration of a solution is the number of moles of solute per
of solvent.
17.
Steel and brass are examples of
18.
Litmus paper is
in an acidic solution
19.
Litmus paper is
in a basic solution.
20.
Phenolphthalein is a chemical
.
21.
The pH of distilled water is
.
22.
The pH of an acid is
23.
A
24.
In a positive ion, the number of protons is
electrons.
25.
The element which has 6 electrons is
26.
A reaction which releases energy is called
.
.
valence electron(s).
compound.
.
than 7.
is a solid that can form when two solutions are mixed.
than the number of
.
.
Definitions
(1 mark each)
Define six of the following terms.
a)
covalent bond
b)
isotope
c)
ionization energy
d)
molecule
e)
molar volume
f)
solubility
g)
molarity
h)
absolute zero
Short answer questions
Make sure you show ALL your work, including formulas,
to get full marks.
1.
Balance the following equations
a)
Fe + H2O 
 Fe3O4 + H2
b)
Al  O2 
 Al2O3
c)
C8H16  O2 
 CO2  H2O
(6 marks)
2.
Use dots to represent the valence electrons in the ionic bonds between the
following elements.
(2 marks)
Mg and Cl
3.
What difference is there between polar covalent bonds and non–polar covalent
bonds?
(2 marks)
4.
Use Lewis diagrams to show the covalent bonds in the following compounds.
(2 marks)
a)
Carbon dioxide
b)
Hydrogen fluoride
5.
The atomic number of an atom is 11 and its mass number is 23. Determine its:
(4 marks)
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
the charge of its ion
6.
Write a balanced equation for each of the following reactions.
(4 marks each)
a)
hydrochloric acid and sodium hydroxide
b)
potassium iodide and lead (II) nitrate
c)
calcium sulphate and iron (III) oxide
7.
Give the chemical formulas for the following compounds:
(2 marks each)
a)
b)
c)
d)
e)
f)
barium oxide
bromic acid
potassium chloride
magnesium hydroxide
sodium nitrite
lithium percarbonate
8.
9a)
b)
c)
d)
e)
f)
Name the following chemicals.
SrSO4
NaBr
K2S
LiCH3COO
AlPO2
Cu(BrO2)2
9.
Give an example of the following types of reactions:
a)
synthesis
b)
oxidation
c)
double displacement
d)
endothermic
(2 marks each)
(1 mark each)
Calculations
1.
How many grams of potassium dichromate (K2Cr2O7) must be used to prepare
0.75 L of a 0.01 M solution?
(3 marks)
2.
Calculate the density, in g/L, of nitrogen dioxide gas at STP. (4 marks)
3.
If the pressure is kept constant, what will the new volume of gas be at 80 oC if it
initially occupied 25 L at 15oC?
(4 marks)
4.
a)
A sample of carbon dioxide gas occupies a volume of 950 mL at 60oC and
under a pressure of 150 kPa. What volume will this sample of gas occupy at
STP?
(4 marks)
b)
What is the mass of the sample of carbon dioxide?
(3 marks)
5.
Propane, C3H8, reacts with oxygen. Write the balanced chemical equation.
(4 marks)
6.
Given the equation
a)
b)
c)
C5H12(g) + O2(g)  CO2(g) + H2O(g)
Balance the equation.
(3 marks)
What mass of oxygen is needed to completely burn 150 g of C5H12?
(3 marks)
Calculate the volume of CO2 produced when 50 L of C5H12 reacts with
excess oxygen at STP.
(3 marks)
7.
How many moles are there in 200 g of water?
(3 marks)
8.
In order to form CO2, what mass of carbon will combine with 6.2 g of oxygen?
(3 marks)
9.
Copper reacts with silver nitrate and the reaction is a single displacement. In
the lab, Antonio produced 1.7 g Ag from 5 g of copper and excess silver
nitrate.
a) Write the balanced chemical equation.
(3 marks)
b) What is the theoretical yield of Ag?
(3 marks)
c) What is the actual yield of silver?
(1 mark)
d) What is the percentage yield of Ag?
(2 marks)