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SCH3U Final Mock Exam

Total questions: 140

Worksheet time: 2hrs 45mins

Name
Class
Date
1.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
2.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
3.

A solution that is considered dilute would ....

a)

Be dark in color

b)

Have a strong scent

c)

Have a large amount of solute

d)

Have a small amount of solute

4.

How many L of a 14 mol/L solution must be used to make 250 mL of a 1.75 mol/L solution? C1V1=C2V2

a)

0.031 L

b)

31.3 L

c)

2000 L

d)

10.2 L

5.
Which of the following bonds are soluble in water?
a)
polar & nonpolar covalent
b)
polar covalent & ionic
c)
nonpolar covalent & ionic
d)
Only ionic
6.

Calculate the concentration of 25.0 grams of KBr dissolved in 0.750 L (hint: convert grams to moles)

a)

0.280 mol/L

b)

0.210 mol/L

c)

33.3 mol/L

7.

What is the concentration of a solution containing 8.0 moles of solute in 500. mL of solution?

a)

0.016 mol/L

b)

16 mol/L

c)

62.5 mol/L

d)

0.063 mol/L

8.
Which solution is more concentrated?
a)
1 mole of solute in 1 liter of solvent
b)
3 moles of solute in 6 liters of solvent
c)
4 moles of solute in 2 liters of solvent
9.

When ions separate in an ionic compound it is called:

a)

Ionization

b)

Separation

c)

Dissociation

d)

Polymerization

10.

A weak acid:

a)

Ionizes completely

b)

Ionizes partially

c)

Does not ionize

d)

Dissociates

11.

What is the net ionic equation for the following neutralization reaction?


HCl(aq) + NaOH(aq) --> NaCl(aq) + H2O(l)

a)

Na+(aq) + Cl-(aq) --> NaCl(aq)

b)

NaCl(aq) --> Na+(aq) + Cl-(aq)

c)

H2O (l) --> H+(aq) + OH-(aq)

d)

H+(aq) + OH-(aq) --> H2O (l)

12.

What volume of 0.500 mol/L NaOH would you need to completely react with 0.750 L of 2.00 mol/L H2SO4 in the following reaction?


2NaOH(aq) + H2SO4(aq) --> Na2SO4(aq) + 2H2O(l)

a)

1.50 L

b)

0.750 L

c)

6.00 L

d)

1.33 L

13.

Which of the following would be considered a base?

a)

NaOH

b)

H2SO4

c)

NaCl

d)

H2O

14.

What is the name of the positively charged subatomic particle in the nucleus of an atom?

a)

Electron

b)

Neutron

c)

Proton

d)

Turtleon

15.

What is the name of the negatively charged subatomic particle that orbits the nucleus?

a)

Electron

b)

Neutron

c)

Proton

d)

Flamingon

16.

What is the subatomic particle that does not have a charge and that can be found in the nucleus of an atom?

a)

Electron

b)

Neutron

c)

Proton

d)

Pigeon

17.

Which of the following is a heterogeneous mixture?

a)

Apple juice

b)

Salt water

c)

Clean Air

d)

Fruit Loops cereal

18.

The ability of a substance to dissolve is called:

a)

Lustre

b)

Malleability

c)

Ductility

d)

Solubility

19.

An atom that gains or loses electrons is called a(n):

a)

Element

b)

Neutron

c)

Ion

d)

Atomizer

20.

Which element is represented by the Bohr-Rutherford diagram in the picture?

a)

Sodium

b)

Hydrogen

c)

Helium

d)

Lithium

21.

Rows (going from left to right) on the periodic table are called:

a)

Groups

b)

Periods

c)

Elementals

d)

Trumpets

22.

Columns (going from up to down) on the periodic table are called:

a)

Groups (or Families)

b)

Periods

c)

Elementals

d)

Trumpets

23.

The atomic # of an element on the periodic table tells you:

a)

The number of electrons in the atom

b)

The number of protons in the atom

c)

The number of neutron in the atom

d)

Both the number of electrons and protons in the atom

24.

Which of the following compounds would have a covalent bond?

a)

NaCl

b)

MgO

c)

CO

d)

KBr

25.

Which of the following is not an acid?

a)

HCl

b)

H2S

c)

H2CO3

d)

Mg(OH)2

26.

The term used to describe the quantity of solute that is dissolved in a defined quantity of solution is called:

a)

density

b)

concentration

c)

malleability

d)

dissociation

27.

The name of metals that have more than one ion form and that have more than one charge listed on the periodic table is:

a)

Electrolyte metals

b)

Soluble metals

c)

Multivalent metals

d)

Wild metals

28.

The most reactive nonmetal on the periodic table is:

a)

Bromine

b)

Fluorine

c)

Sulfur

d)

Helium

29.

The most reactive metal on the periodic table is:

a)

Lithium

b)

Copper

c)

Gold

d)

Francium

30.

The term used to describe the outermost electron shell of an atom is:

a)

Valence

b)

Respute

c)

Orbital

d)

Universal

31.

A solution which has water as the solvent is called a(n):

a)

Watery solution

b)

Translucent solution

c)

Aqueous solution

d)

Molar solution

32.

Atoms that have the same number of protons but different numbers of neutrons are called:

a)

Isotopes

b)

Ions

c)

Quarks

d)

Polyatomics

33.

The amount of energy required to remove an electron from an atom is called:

a)

Electron affinity

b)

Electronegativity

c)

Atomic radius

d)

Ionization energy

34.

The amount of energy required for atoms to gain electrons is called:

a)

Ionization energy

b)

Atomic radius

c)

Electronegativity

d)

Electron affinity

35.

The amount of substance containing 6.02 x 1023 entities:

a)

Molarity

b)

Molar ratio

c)

Mole

d)

Mouse

36.

A chemical compound that does NOT contain water as part of its structure is called:

a)

Hydrate

b)

Anhydrous

c)

Anaerobic

d)

Polar

37.

A substance that does the dissolving in a solution and is often the liquid component of a solution (e.g. water) is called:

a)

Solute

b)

Solvent

c)

Soluble

d)

Insoluble

38.

The amount of mass product expected based on stoichiometry (math) of the chemical equation is called:

a)

Actual yield

b)

Theoretical yield

c)

Percentage yield

d)

Imveryconfused yield

39.

The distance from the nucleus to the valence shell of an atom is called:

a)

Atomic diameter

b)

Atomic circumference

c)

Atomic distance

d)

Atomic radius

40.

A type of chemical bond where a pair of electrons is unequally shared between two atoms is called a:

a)

Non-polar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

James bond

41.

How many valence electrons does Selenium have?

a)

1

b)

2

c)

6

d)

7

42.

How many electrons phosphorous gain when participating in a ionic bond?

a)

1

b)

2

c)

3

d)

4

43.

Which element is diatomic

a)

Sodium

b)

Carbon

c)

Bromine

d)

Magnesium

44.

Which element is a halogen?

a)

Sulfur

b)

Nitrogen

c)

Lithium

d)

Iodine

45.

If neon has 10 electrons, which element has the same number of electrons as an ion?

a)

Chlorine (Cl, charge of -1)

b)

Nitrogen (N, charge of -3)

c)

Zinc (Zn, charge of 2+)

d)

Iron (Fe, charge of 2+)

46.

What is the name of the following compound?

Mg(NO3)2

a)

Magnesium nitrate

b)

Magnesium (II) nitrate

c)

Magnesium nitride

d)

Magnesium (II) nitride

47.

What is the name of the following compound?

PBr3

a)

Phosphorous bromide

b)

Monophosphorous tribrimide

c)

Phosphorous tribromide

d)

Phosphorous tetrabromide

48.

What is the chemical formula for Potassium iodide

a)

K2I

b)

KI2

c)

KI

d)

KI3

49.

What is the chemical formula for Copper (I) phosphide

a)

Cu3P

b)

CoP3

c)

CuP3

d)

CuP

50.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
51.
The following is what type of reaction:
NH3 + HCl  → NH4Cl
a)
Synthesis
b)
Decomposition
c)
Single Replacement Replacement
d)
Double Replacement Replacement
52.
What is decomposition?
a)
putting substances together
b)
breaking substances apart
c)
element replacing another element in a compoud
d)
burning of a subtance
53.
Ions in two compounds switch. 
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
54.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
55.
Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
56.
C4H12 + O2 → CO2 + H2O
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
57.
2Pb(NO3)2   -->   2PbO +  4NO2  +  O2
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
58.

Which metal is the least reactive

(i.e. the most easily displaced/reduced)?

a)

aluminum

b)

tin

c)

mercury

d)

silver

59.

How many moles of aluminum will react with 15 mol of copper (II) chloride?

2 Al + 3 CuCl2 --> 2 AlCl3 + 3 Cu

a)

2 mol

b)

10 mol

c)

12 mol

d)

15 mol

60.

A strong Arrhenius acid _________ dissociates to release ___ ions.

a)

partially ; H+

b)

fully ; H+

c)

partially ; OH-

d)

fully ; OH-

61.

The mass number of an element that has 18 protons, 18 electrons, and 19 neutrons is _____.

a)

12.5

b)

13

c)

25

d)

37

62.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
63.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
64.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
65.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
66.
Carbon dioxide
a)
C2O2
b)
C20
c)
CO
d)
CO2
67.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
68.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
69.
How many valence electrons does nitrogen have?
a)
3
b)

2

c)
5
d)
1
70.
A covalent bond involves a __________ of electrons.
a)
sharing
b)
borrowing
c)
exchanging
d)
switching
71.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

72.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

73.
Name this compound:
Li2SO3
a)
Lithium sulfate
b)
Lithium sulfite
c)
Lithite sulfide
d)
Sulfur lithite
74.
What is the formula for silver nitrate?
a)
Ag3NO
b)
AgNO3
c)
Ag(NO3)2
d)
Ag2NO3
75.
Which of the following elements has the most "shielding" electrons?
a)
Nitrogen
b)
Phosphorus
c)
Arsenic
d)
Bismuth
76.
As you go down a group, the amount of shielding....
a)
increases
b)
decreases
c)
stays the same
77.

when atom gain an electron (negative) the size of atom

a)

Increase

b)

Decrease

c)

No change

d)

Small

78.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
79.
Which of the following will have the highest electronegativity?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
80.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
81.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
82.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
83.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
84.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
85.
Molecular compounds do not conduct electricity because they:
a)
break up into ions
b)
do not break up into ions
c)
do not dissolve in water
d)
have high melting points
86.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
87.
Which of these molecules is nonpolar?
a)
O2
b)
H2O
c)
HBr
d)
NI3
88.
Of these 3 molecules, which has polar covalent bonding?
a)
O2
b)
NaI2
c)
HBr
d)
MgO
89.
Which of these molecules is polar?
a)
H2O
b)
BBr3
c)
I2
d)
MgI2
90.
In the HCl molecule which atom would have a slightly negative charge?
a)
H
b)
Both
c)
Cl
d)
Neither
91.
The following all contain polar bonds, which one is a polar molecule?
a)
CBr4
b)
PCl3
c)
BCl3
d)
BeCl2
92.
Why does H2O have a higher boiling point than H2Se?
a)
It has stronger bonding
b)
it has dipole-dipole forces
c)
it has london dispersion forces
d)
it has hydrogen bonding
93.
Which of these forces applies to all molecules
a)
London Dispersion
b)
Dipole dipole
c)
Hydrogen Bonding
d)
Covalent bonding
94.
What is the molar mass of fluorine gas?
(beware!)
a)
18.998 g/mol
b)
38 g/mol
c)
9 g/mol
d)
18 g/mol
95.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
96.

How many molecules are in 3 moles of oxygen gas?

a)

3.612 x 10^24 molecules

b)

6.02 x 10^23 molecules

c)

1.806 x 10^24 molecules

d)

1.204 x 10^24 molecules

97.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
98.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
99.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
100.
When 12 moles of O2 reacts with 6 moles of C10H8, what is the limiting reactant?  
1 C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
101.

6Na + Fe2O3 --> 3Na2O + 2Fe


If you are provided 200g of sodium and 250 grams of iron(III) oxide, how much of excess reagent is left?

a)

232 g

b)

18 g

c)

250 g

102.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
103.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

104.

2Fe2O3 + C → Fe + 3CO2

You add 28 grams of carbon. You find the actual yield to be 181.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)

a)

58.83%

b)

308%

c)

6435%

d)

15.5

105.

11.

LiOH + KCl → LiCl + KOH


b) I actually produced 6 grams of lithium chloride and I began this reaction with 20.0 grams of lithium hydroxide. What is my percent yield?

a)

16.9%

b)

5.91%

c)

1.88%

d)

12.3%

106.

In the combustion of methane gas reaction, what is the mole ratio of methane to water?

a)

2:2

b)

1:2

c)

2:4

d)

1:1

107.

In the synthesis reaction between nitrogen gas and hydrogen gas, ammonia is formed. What is the mole ratio between hydrogen and ammonia?

a)

1:1

b)

2:1

c)

3:2

d)

6:8

108.

SATP - Standard Ambient Temperature and Pressure, the temperature is:

a)

22.5oC

b)

273.15 OC

c)

0 K

d)

298.15 K

109.

The pressure of a sample of helium is 2.00 atm in a 200.0 mL container. If the container is compressed to 10.0 mL without changing the temperature, what is the new pressure?

a)

200 atm

b)

40.0 atm

c)

0.10 atm

d)

100 atm

110.

A sample of oxygen occupies 560.0 mL when the pressure is 1.05 atm. At a constant temperature, what volume does the gas occupy when the pressure decreases to 0.921 atm.

a)

0.080 L

b)

0.490 L

c)

0.600 L

d)

0.638 L

111.

The volume of gas is 5.0 L when the temperature is 1.0 oC. If the temperature is increased to 10.0oC without changing the pressure, what is the new volume?

a)

4.8 L

b)

5.2 L

c)

2.5 L

d)

10.0 L

112.

On a cold winter morning when the temperature is -13oC, the air pressure in a car tire is 1.5 atm. If the volume does not change, what is the pressure after the tire has warmed to 15 oC?

a)

19.5 atm

b)

3.0 atm

c)

-1.5 atm

d)

1.7 atm

113.

The pressure of a 1000.0 mL sample of gas at 283 K increases from 0.921 atm to 1.18 atm. If the volume is unchanged, what is the new temperature?

a)

308 K

b)

373 K

c)

130 K

d)

275 K

114.

A 70.0 L sample of gas at 20.0oC and 0.789 atm expands to 90.0 L at 15.0oC. What is the new gas pressure?

a)

0.934 atm

b)

0.767 atm

c)

0.603 atm

d)

0.418 atm

115.

What is the volume occupied by 1 mol of oxygen at STP?

a)

22.4 L

b)

16.0 L

c)

11.2 L

d)

32.0 L

116.

Which is a common unit for the ideal gas constant R?

a)

atm L

b)

atm L / mol K

c)

mol k

d)

atm/K

117.

What is the pressure exerted by 1.2 mol of a gas with a temperature of 20.0 oC and a volume of 9.5L? (R for atm is 0.082057)

a)

3.0 atm

b)

1.0 atm

c)

0.030 atm

d)

30 atm

118.

What is the volume of as gas in a 1.50 mol sample that exerts a pressure of 0.922 atm and has a temperature of 10.0oC? (R for atm is 0.082057)

a)

14.2 L

b)

37.8 L

c)

13 L

d)

378 L

119.

A gas sample with a mass of 12.8 g exerts a pressure of 1.2 atm at 15.0oC and a volume of 3.94 L. What is the molar mass of the sample? (R for atm is 0.082057)

a)

128 g/mol

b)

19 g/mol

c)

64 g/mol

d)

32 g/mol

120.

Chlorine is produced by the reaction

2 HCl(g) --> H2(g) + Cl2(g).

How many grams of HCl (MM 36.46 g/mol) must be used to produce 10.0 L of Chlorine at SATP? (R for atm is 0.082057)

a)

36.5 g

b)

32.6 g

c)

30.2 g

d)

15.8 g

121.

The combustion of iron produces iron (III) oxide.

4 Fe(s) + 3 O2(g)--> 2 Fe2O3(s)

How many grams of Fe2O3 (MM 159.70 g/mol) can be produced from 50.0 L of O2 at 1.00 atm and 298.15 K? (r for atm is 0.082057)

a)

37.8 g

b)

196 g

c)

217 g

d)

50 g

122.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
123.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
124.

How many grams are in 1.00 mol of Oxygen gas, O2

a)

16.0 g

b)

32.0 g

c)

15.99 g

d)

31.98 g

125.

Fe2O3 + 3H2 → 2Fe + 3H2O

About how many grams of H2O will be produced from 150 grams of Fe2O3?

a)

51 grams H2O

b)

2.8 grams H2O

c)

0.17 grams H2O

d)

9001 grams H2O

126.

CH4 + 2 O2 → CO2 + 2 H2O

How many moles of carbon dioxide are produced from the combustion of 110. g of CH4?

a)

13.7 mol

b)

2.75 mol

c)

6.11 mol

d)

6.85 mol

127.

How many atoms are in 13.5 grams of Beryllium?

a)

1.5 atoms

b)

9 atoms

c)

4x1023 atoms

d)

9x1023 atoms

128.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
129.

When you use a balanced chemical equation to calculate the amount of a product on paper it is referred to as the

a)

experimental value

b)

theoretical yield

c)

actual yield

d)

percent yield

130.

If 15 grams of copper (II) chloride react with 20. grams of sodium nitrate, how much sodium chloride can be formed?

a)

13 g

b)

130 moles

c)

130 g

d)

13 moles

131.
P4 + 3O2 --> P4O6 
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6 
d)
none of the above
132.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
133.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
134.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
135.

Silver nitrate and sodium phosphate are reacted in equal amounts of 200. g each. How many grams of silver phosphate are produced?

3AgNO3 + Na3(PO4) ---> Ag3(PO4) + 3NaNO3

a)

164 g

b)

64.0 g

c)

146 g

d)

164 moles

136.
When reacting Na with Cl2, we calculated that the theoretical yield should be 12.5 grams. Our actual yield was 13.0 grams. What is the percent yield?
a)
100%
b)
104%
c)
96%
d)
1.04
137.

P4 + 6Cl2 --> 4PCl3

In an experiment, the reaction of 75.0g P4 with excess chlorine gas produced 110g PCl3. Find the theoretical yield and calculate percent yield for the reaction.

a)

78%

b)

64%

c)

27%

d)

33%

138.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
139.
What is the empirical formula of the following molecular formula:  C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
140.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8

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