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WorksheetsSpring Final Exam Chemistry 2025
Total questions: 90
Worksheet time: 52mins
Name
Class
Date
1.
What is the name of Sr(NO₃)₂ ?
a)
strontium nitrite
b)
strontium dinitrate
c)
strontium (II) nitrate
d)
strontium nitrate
2.
What is the chemical formula for Tin (IV) carbonate ?
a)
Sn(CO₃)₂
b)
Sn(CO₂)₂
c)
Sn₄(CO₃)₂
d)
SnCO₃
3.
What is the bond angle for a tetrahedral molecule?
a)
90
b)
120.4
c)
180
d)
109.5
4.
What is the Lewis diagram for BF₃?
a)
A
b)
B
c)
C
d)
D
5.
Which is a correct Lewis structure for carbonic acid, H₂CO₃?
a)
A
b)
B
c)
C
d)
D
6.
Which of the following is an acceptable Lewis structure for the diatomic nitrogen molecule?
a)
A
b)
B
c)
C
d)
D
7.
Horseplay or practical jokes in the laboratory are
a)
okay if you are working alone
b)
not dangerous
c)
okay
d)
always against the rules
8.
Which of the following is the correct Lewis structure for phosphorus tribromide, PBr3?
a)
A
b)
B
c)
C
d)
D
9.
What is the name of the molecular geometry for this Lewis Structure?
a)
trigonal planar
b)
tetrahedral
c)
trigonal pyramid
d)
bent
10.
What is the name of the molecular geometry of this Lewis Structure?
a)
linear
b)
bent
c)
tetrahedral
d)
planar
11.
How many electrons can be used in the Lewis Structure for : NO₃⁻¹
a)
23
b)
18
c)
20
d)
24
12.
What shape is the following molecule?
a)
T-shaped
b)
Trigonal bipyramidal
c)
See Saw
d)
Pentahedral
13.
What shape is this structure?
a)
trigonal planar
b)
angular or bent
c)
trigonal pyramid
d)
tetrahedral
14.
Calculate the Formal Charge for the Oxygen Labeled 2
a)
-1
b)
+1
c)
-2
d)
0
15.
Considering formal charge as well as the octet rule, what is the best electron dot structure for the polyatomic ion NCO-? (Note: three of these structures are correct but one is "best")
a)
1
b)
2
c)
3
d)
4
e)
5
16.
Which is a correct Lewis structure for nitric acid, HNO₃?
a)
A
b)
B
c)
C
d)
D
17.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
18.
Balance and identify the type of reaction: ___Pb(NO₃)₂ + ___H₂S --> ___PbS + ___HNO₃
a)
3,2,3,2 single replacement
b)
1,2,2,1 double replacement
c)
2,1,1,1 single replacement
d)
1,1,1,2 double replacement
19.
When a solid produced by a chemical reaction separates from the solution it is called
a)
a reactant
b)
a precipitate
c)
a molecule
d)
the mass of the product
20.
The reaction represented by the equation Mg(s) + 2HCl(aq) --> H₂(g) + MgCl₂(aq) is a
a)
composition reaction
b)
decomposition reaction
c)
single replacement reaction
d)
double replacement reaction
21.
The reaction represented by the equation Pb(NO₃) (aq) + 2 KI(aq) -- PbI₂(s) + 2KNO₃(aq) is a
a)
double replacement reaction
b)
synthesis reaction
c)
decomposition reaction
d)
combustion reaction
22.
How many moles of zinc are in 4.22 x 10²⁷ atoms of zinc?
a)
5.25 x 10³ moles Zn
b)
7.01 x 10³ moles Zn
c)
8.57 x 10³ moles Zn
d)
8.35 x 10³ moles Zn
23.
When a metal chlorate is heated, it decomposes to yield a metal chloride and
a)
a metal oxide
b)
a metal hydroxide
c)
hydrogen gas
d)
oxygen gas
24.
An element in the activity series can replace any element __.
a)
in the periodic table
b)
below it on the list
c)
above it on the list
d)
in its group
25.
Which is the balanced equation for the above reaction?
a)
2 NH₄NO₃ + 2 Na₃PO₄--> 2 (NH₄)₃PO₄ + 6 NaNO₃
b)
3 NH₄NO₃ + Na₃PO₄--> (NH₄)₃PO₄ + 3 NaNO₃
c)
NH₄NO₃ + Na₃PO₄--> (NH₄)₃PO₄ + NaNO₃
d)
NH₄NO₃ + Na₃PO₄--> (NH₄)₃PO₄ + 3 NaNO₃
26.
How many grams of ammonium phosphate can be made starting with 30 grams of ammonium nitrate?
a)
10 g
b)
20 g
c)
30 g
d)
40 g
27.
What is the limiting reagent?
a)
sodium nitrate
b)
sodium phosphate
c)
ammonium phosphate
d)
ammonium nitrate
28.
According to the chemical equation, which compound would form a precipitate?
a)
Co(NO₃)₂
b)
Co(OH)₂
c)
NaOH
d)
NaNO₃
29.
Potassium chlorate solid when heated produces potassium chloride solid and oxygen gas.
a)
2 KClO₃ + heat --> 2 KCl + 3O₂
b)
2 PClO₃ + heat --> 2 PCl + 3 O₂
c)
2 KClO₃ + heat --> 2 KCl + 3 O
d)
2 KCl + heat --> 2 KCl + 3 O₂
30.
How many grams are there in 4.5 x 10²² molecules of molecules of Ba(NO₂)₂?
a)
27.1g Ba(NO₂)₂
b)
19.8g Ba(NO₂)₂
c)
1.7g Ba(NO₂)₂
d)
17.1g Ba(NO₂)₂
31.
A balanced chemical equation allows one to determine the
a)
mole ratio of any two substances in the reaction.
b)
energy released in the reaction.
c)
electron configuration of all elements in the reaction.
d)
mechanism involved in the reaction.
32.
If one knows the mole ratio of a reactant and product in a chemical reaction, one can
a)
estimate the energy released in the reaction.
b)
calculate the speed of the reaction.
c)
calculate the mass of the product produced from a known mass of reactant.
d)
decide whether the reaction is reversible.
33.
The units of molar mass are
a)
g/mol
b)
amu/mol
c)
mol/g
d)
amu/g
34.
Name the type of reaction, the products, balanced coefficients. 3KOH + H₃PO₄--->
a)
Synthesis, K₃PO₄ & H₂O, 3,1,1,2
b)
Decomposition, K₃PO₄ + 3H₂O, 3,1,1,3
c)
Single displacement, K₃PO₄ & H₂O, 3,1,1,2
d)
Double displacement, K₃PO₄ + 3H₂O, 3,1,1,3
35.
Which type of reaction is: C₂H₄ + 3 O₂ → 2 CO₂ + 2 H₂O
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
36.
What are the coefficients for this reaction: Ca + N₂ --> Ca₃N₂
a)
1,2,1
b)
3,1,1
c)
1,1,2
d)
1,1,3
37.
For the reaction represented by the equation 2HNO₃ + Mg(OH)₂ --> Mg(NO₃)₂ + 2H₂0, how many grams of magnesium nitrate are produced from 8.00 mol of nitric acid, HNO₃ , and an excess of Mg(OH)₂?
a)
148g
b)
445g
c)
593g
d)
818g
38.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the __.
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
39.
Aqueous barium chloride reacts with aqueous potassium carbonate to produce solid barium carbonate and aqueous potassium chloride. What is the correct balanced equation?
a)
Ba₂Cl(aq) + KCO₃(aq) --> BaCO₃(s) + KCl(aq)
b)
BaCl(aq) + K₂CO₃(aq) --> BaCO₃(s) + K₂Cl(aq)
c)
Ba₂Cl₂(aq) + KCO₃(aq) --> Ba₂CO₃(s) + KCl₂(aq)
d)
BaCl₂(aq) + K₂CO₃(aq) --> BaCO₃(s) + 2KCl(aq)
40.
According to the activity series, which of the following single replacement reactions can occur?
a)
Fe + NaOH
b)
Ni + MgSO₄
c)
Ca + Al₂(SO₄)₃
d)
Al + KOH
41.
Which types of reactions are essentially opposites of one another?
a)
synthesis and decomposition
b)
combustion and synthesis
c)
single replacement and double replacement
d)
synthesis and single replacement
42.
What is the mole ratio of H₂O to H₃PO₄ in the following chemical equation? P₄O₁₀ + 6 H₂O → 4 H₃PO₄
a)
3:1
b)
1:3
c)
4:6
d)
6:4
43.
How many water molecules are in 5.2 moles of water?
a)
5.2
b)
6.02 x 10²³
c)
8.638 x 10⁻²⁴
d)
3.1 x 10²⁴
44.
Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g) How many moles of HCl are consumed in the production of 7.5 moles of MgCl₂?
a)
3.8 moles
b)
15 moles
c)
7.5 moles
d)
23 moles
45.
How many particles are in a mole?
a)
602
b)
602 moles
c)
602 million
d)
6.02 x 10²³
46.
1 mole of any gas at STP has a volume of __.
a)
22.4 liters
b)
44.2 liters
c)
6.02 x 10²³ liters
d)
2.4 liters
47.
How many liters of NH₃ are needed to react completely with 30.0 L of NO? 4NH₃+6NO --> 5N₂ + 6H₂O
a)
5.0 L
b)
7.5 L
c)
20.0L
d)
120.0L
48.
You are heating a substance in a test tube. Always point the open end of the tube __.
a)
away from all people
b)
toward another classmate
c)
toward your lab partner
d)
toward yourself
49.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Write an Unbalanced Equation
c)
Panic
d)
Avogadro's Number
50.
What is the percent composition of nitrogen in AgNO₃?
a)
63.6%
b)
8.3%
c)
28.2%
d)
42.3%
51.
A 3.585 g sample contains 1.388 g of C, 0.345 g of H, 1.850 g O and its molar mass is 62 g. What is molecular formula of this substance?
a)
C₂H₄O₂
b)
C₄H₆O₂
c)
C₂H₆O₂
d)
C₂H₅O₄
52.
How many representative particles are in 34.0 mol SO₃?
a)
2.05 x 10²⁵ molecules SO₃
b)
1.10 x 10²⁵ molecules SO₃
c)
7.78 x 10²⁵ molecules SO₃
d)
3.23 x 10²⁵ molecules SO₃
53.
If you start with 5.5 grams of both lithium chloride and calcium hydroxide, how many grams of aqueous calcium chloride will be produced?
a)
11 g CaCl₂
b)
68.2 g CaCl₂
c)
72.2 g CaCl₂
d)
56.1 g CaCl₂
54.
The volume of a gas collected when the temperature is 11.0°C and the pressure is 710 mmHg measures 14.8mL. What is the calculated volume of the gas at 20.0°C and 740 mmHg?
a)
7.8 mL
b)
13.7 mL
c)
14.6 mL
d)
15 mL
55.
What is the pressure exerted by 1.2 mol of a gas with a temperature of 20.°C and a volume of 9.5 L?
a)
0.030 atm
b)
1.0 atm
c)
3.0 atm
d)
30. atm
56.
According to the kinetic-molecular theory, particles of matter
a)
are in constant motion
b)
have different shapes
c)
have different colors
d)
are always fluid
57.
A sample of neon is at 89°C and 123 kPa. If the pressure changes to 145 kPa and the volume remains constant, find the new temperature, in °C.
a)
150°C
b)
154°C
c)
158°C
d)
161°C
58.
At 350°C, nitrogen has a velocity of 800 m/s. Find the velocity of hydrogen at the same temperature.
a)
2190 m/s
b)
2235 m/s
c)
2697 m/s
d)
3000 m/s
59.
The spontaneous disintegration of a nucleus into a slightly lighter and more stable nucleus, accompanied by emission of particles, electromagnetic radiation, or both, is
a)
nuclear fusion
b)
nuclear radiation
c)
radioactive decay
d)
nuclear fission
60.
Alpha particles have a _____ charge.
a)
+2
b)
0
c)
+1
d)
-1
61.
Who coined the term "radioactivity"?
a)
Ernest Rutherford
b)
Henri Becquerel
c)
Marie Curie
d)
James Chadwick
62.
Which of the following nuclear emissions has the greatest penetrating power?
a)
alpha
b)
gamma
c)
beta
d)
positron
63.
This is the symbol for a(n)
a)
alpha particle
b)
beta particle
c)
gamma particle
64.
If an acid is splashed on your skin, wash at once with __.
a)
weak base
b)
soap
c)
plenty of water
d)
oil
65.
Which type of nuclear radiation is being emitted here?
a)
alpha
b)
beta
c)
gamma
d)
none
66.
Which type of nuclear radiation is being emitted here along with Rn?
a)
alpha
b)
beta
c)
gamma
d)
none
67.
Which of the illustrations below represents a fission reaction?
a)
A
b)
B
c)
C
d)
D
68.
The three types of nuclear radiation in increasing order of penetrating power.
a)
alpha, beta, gamma
b)
alpha, gamma, beta
c)
x-ray, beta, gamma
d)
x-ray, gamma, beta
69.
You accidentally break some glassware you should __.
a)
Clean it up immediately
b)
Leave it
c)
Tell the teacher
d)
Tell you lab partner to clean it up
70.
Nuclear equations differ from chemical equations by
a)
using new and different elements
b)
having to balance the numbers on each side
c)
different elements being on the reactant and product side of the equation due to transmutation
d)
gluing elements together
71.
__ the amount of mass required to sustain a chain reaction.
a)
chain reaction
b)
critical mass
c)
fusion
72.
Which process puts 2 very small nuclei together?
a)
nuclear fission
b)
nuclear fusion
73.
Which type of reaction does the diagram illustrate?
a)
Fission
b)
Fusion
c)
Alpha Decay
d)
Beta Decay
74.
What is one benefit associated with a nuclear fission reaction?
a)
The products are not radioactive.
b)
Stable isotopes are used as reactants.
c)
There is no chance of biological exposure.
d)
A large amount of energy is produced.
75.
What is the name of the location where the nuclear meltdown that took place in Japan?
a)
Chernobyl
b)
Pripyat
c)
Fukishima
76.
What is the name of the power plant that melted down in the former Soviet Union?
a)
Chernobyl
b)
Pripyat
c)
Fukishima
77.
Explain what you discovered concerning hydrogen gas and how its presence can be tested for during the "Hydrogen, What a Bang" Lab?
4 lines
78.
What is the chemical formula of Sulfuric acid?
a)
HS
b)
H2SO4
c)
H2SO3
d)
H2S
79.
What is the chemical formula of Diiodine heptaselenide
a)
I2Se7
b)
I2Se6
c)
I2Se
d)
ISe2
80.
Write the name of Mg(MnO4)2 ?
a)
magnesium manganate
b)
magnesium dimanganate
c)
magnesium permanganate
d)
magnesium manganide
81.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
82.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
83.
Considering formal charge as well as the octet rule, what is the best electron dot structure for the polyatomic ion NCO-? (Note: three of these structures are correct but one is "best")
a)
1
b)
2
c)
3
d)
4
e)
5
84.
Classify this reaction
4Fe + 3O2 --> 2Fe2O3
a)
Synthesis
b)
Decomposition
c)
Double Replacemnt
d)
Single Replacement
85.
What does aq mean in a chemical reaction?
a)
aqua dancing
b)
aqua lungs
c)
aqualirious
d)
aqueous
86.
Write a complete reaction for the following.
Solid iron (III) oxide decomposes.
Solid iron (III) oxide decomposes.
a)
2 Fe2O3 (s) → 4 Fe (s) + 3 O2 (g)
b)
Fe2O3 (s) → 2 Fe (s) + 3 O (g)
c)
2 FeO (s) → 2 Fe (s) + O2
d)
Fe3O2 (s) → 3 Fe (s) + O2
87.
When zinc oxide is produced from the reaction of zinc and oxygen gas, how many grams of zinc oxide can be produced if 100g of each reactant is used?
a)
50 g ZnO
b)
65 g ZnO
c)
80 g ZnO
d)
100 g ZnO
88.
A gas at STP occupies 28 cm3 of space. If the pressure changes to a 3.8 atm and the temperature increases to 203oC, find the new volume.
a)
6.7 cm3
b)
9.8 cm3
c)
13 cm3
d)
17.7 cm3
89.
____ is when unstable atoms break down by emitting radiation until they become stable.
a)
Radiation
b)
Chemical Reaction
c)
Radioactive Decay
d)
Isotopes
90.
Oxidation is the _________ of electrons.
a)
loss
b)
gain
c)
sharing
d)
transfer
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