wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemistry Final Exam Review 2023

Total questions: 110

Worksheet time: 2hrs 21mins

Name
Class
Date
1.

Which particles are responsible for creating chemical bonds between atoms? (a)  

Choose from the below words
Neutrons
Protons
Electrons
2.

An atom's valence electrons are located where? (a)  

Choose from the below words
Innermost electron shell
Nucleus
Second electron shell
Outermost electron shell
3.

Which particles are responsible for preventing the protons of an atom's nucleus from repelling each other and flying into space? (a)  

Choose from the below words
Protons
Neutrons
Electrons
4.

How many bonds can Nitrogen make?

5.

What is the mass of the Chlorine gas?

2NaCl + F2 ➜ 2NaF + Cl2

​​ (a)   g

Choose from the below words
70.906
35.453
17.727
6.

Which characteristics describe an acid? (a)  

Choose from the below words
tastes sour, pH is lower than 7
tastes bitter, pH is higher than 7
has no taste and, has pH of 7
tastes sour and bitter, Has no pH
7.

Which characteristics describe a base?

a)

tastes sour, Has a pH lower than 7

b)

tastes bitter, Has a pH greater than 7

c)

tastes bitter sour, lHas a pH of 7

d)

tastes bitter sour, Has no pH

8.

HCl reacts with Zn giving off heat. This reaction must be (a)   .

Choose from the below words
endothermic
exothermic
9.

Energy in fuel is stored where in the molecules?

a)

Protons

b)

Electrons

c)

Bonds

d)

Light

10.

Increasing temperature has what effect on reaction rate?

a)

No effect

b)

Increasing temperature lowers reaction rate

c)

Increasing temperature increases reaction rate

d)

What are you talking about?

11.
Combustion is another word for
a)
burning
b)
melting
c)
exploding
d)
incinerating 
12.
Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
13.

Balance the following equation.

__Na + __Cl2 --> __NaCl

a)

1,1,2

b)

2,1,2

c)

2,1,1

d)

already balanced

14.

Which type of reaction is:

2 NH3 + H2SO4 → (NH4)2SO4

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
15.

The two sides of a chemical equation are called?

a)

Reactants (left) and Products (right)

b)

Ingredients (left) and Product (right)

c)

Cations and Anions

d)

Reactants (left) and Results (right)

16.

How many HCl molecules do you need to balance this equation? 
Mg +   (a)   HCl --->  MgCl2 + H2

17.

What are the columns referred to on the Periodic Table of Elements?

a)

Families or groups

b)

Periods

18.

Elements on the Periodic Table of the Elements are classified into categories such as

a)

rocks and minerals

b)

molecules and atoms

c)

metals and nonmetals

19.

The majority (most) of the elements are:

a)

metals

b)

nonmetals

c)

metalloids

20.

What is formula when calcium and chlorine combine?

a)

CaCl

b)

CaCl2

c)

ClClO3

d)

CaC2

21.
What is found in the nucleus of atoms?
a)
Protons and electrons.
b)
Protons, neutrons, and electrons.
c)
Protons and neutrons.
d)
Neutrons and electrons.
22.

An atom of carbon has 6 protons and 7 neutrons in its nucleus. If the atom is neutral, how many electrons does it have?

a)

0

b)

7

c)

6

d)

13

23.

What type of bond is formed when atoms share electrons?

a)

Covalent

b)

Ionic

c)

Hydrogen

d)

Polyatomic

24.

A substance with a pH of 8 is a

a)

acid

b)

base

c)

neutral

25.

Carbon has 4 valence electrons which means

a)

it can only form bonds with carbon

b)

it is stable

c)

it can make ionic bonds

d)

it wants to make 4 covalent bonds

26.

Acids have more ______ ions than bases

a)

OH-

b)

H-

c)

OH+

d)

H+

27.

The atomic number of oxygen is

a)

8

b)

15.9994

c)

16

d)

O

28.

The molar volume of a gas at STP occupies _____________.

a)

22.4 L

b)

0˚C

c)

1 kiloPascal

d)

12 grams

29.

If 2.00 L of a gas in a container at room temperature exerts a pressure of 4.00 atm. If the pressure doubles and the temperature remains the same, the volume would become ________.

a)

16.0 L

b)

2.00 L

c)

4.00 L

d)

1.00 L

30.

If 7.00 grams of nitrogen gas are contained in a 5.00 L flask at 4.62 kPa. What is the temperature of the gas?

a)

11.1 K

b)

1.00 K

c)

4.12 K

d)

9.07 K

31.

Chemical equations must be balanced to satisfy ____.

a)

The law of definite proportions

b)

The law of multiple proportions

c)

The law of conservation of mass

d)

Avogadro's principle

32.

What are the coefficients that will balance the skeleton equation below?

AlCl3 + NaOH → Al(OH)3 + NaCl

a)

1,3,1,3

b)

3,1,3,1

c)

1,1,1,3

d)

1,3,3,1

33.

A sample of gas occupies 52.0 mL at 20℃ and 1.00 atm. What volume will it occupy at 40℃ and 1.00 atm?

a)

62.4 mL

b)

44.8 mL

c)

55.5 mL

d)

48.7 mL

34.

How many moles of aluminum are needed to react completely with 1.2 mol of FeO?

2Al(s) + 3FeO(s) → 3Fe(s) + Al2O3(s)

a)

1.2 mol

b)

0.8 mol

c)

1.6 mol

d)

2.4 mol

35.

What is the name of H2SO4?

a)

hyposulfuric acid

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

36.

When an equation is used to calculate the amount of product that could form during a reaction, then the value obtained is called the ____.

a)

Actual yield

b)

Percent yield

c)

Minimum yield

d)

Theoretical yield

37.

The equation 2C3H7OH + 9O2 → 6CO2 + 8H2O is an example of which type of reaction?

a)

Combustion reaction

b)

Single replacement reaction

c)

Double replacement reaction

d)

Decomposition reaction

38.

A process that absorbs heat is a(n) _________.

a)

Exothermic process

b)

Polythermic process

c)

Endothermic process

d)

Ectothermic process

39.

The reaction shown is an ________________ reaction because it has a _____________ enthalpy.

a)

Exothermic; negative

b)

Exothermic; positive

c)

Endothermic; negative

d)

Endothermic; positive

40.

Water and methane molecules are roughly the same size and the same mass but water boils at a much higher temperature. What can we conclude about the intermolecular forces between water and methane?

a)

water has stronger intermolecular forces than methane

b)

water has weaker intermolecular forces than methane

c)

methane has stronger intermolecular forces than water

d)

methane and water have similar intermolecular forces

41.

The diagram provided here shows the reactants and the products of a common chemical reaction. The line on the graph behind them represents the energy of the system as the reaction progresses. Which of the following conclusions is best supported by the information provided?

a)

This is a fast reaction.

b)

This is a slow reaction.

c)

This reaction is endothermic.

d)

This reaction is exothermic.

42.

If a reaction is endothermic

a)

the energy required to break bonds is less than the energy released when new bonds are formed.

b)

the energy required to break bonds is more than the energy released when new bonds are formed.

c)

the energy required to form bonds is less than the energy released when bonds are broken.

d)

the energy required to form bonds is more than the energy released when bonds are broken.

43.
Which state of matter is represented here?
a)
Solid
b)
Liquid
c)
Gas
44.
Describe how particles in a gas behave.
a)
They don't move at all.
b)
They vibrate.
c)
They move rapidly.
d)
They move moderately and vibrate
45.
Which of the following solutions is more concentrated?
a)
A
b)
B
c)
Cannot determine
d)
They are equal
46.
What are the units of molarity?
a)
mol/L
b)
g/L
c)
mol/g
d)
g/mol
47.

Two of anything means a "pair". What quantity does 6.02x1023 represent?

a)

a mole

b)

a ream

c)

an Avagadro

d)

a score

48.

A reaction was predicted to produce 50 grams of a compound. When the product was measured, there were only 45 grams made. What is the percent yield of this reaction?

a)

90%

b)

95%

c)

10%

d)

5%

49.

A 12 mL balloon is heated from 200 K to 300 K. Which of the following is a likely volume after the balloon is heated?

a)

18 mL

b)

10 mL

c)

12 mL

d)

4 mL

50.

What color do acids turn litmus paper?

a)

Blue

b)

Pink

c)

Clear

d)

Red

51.

A(an) __________ bond exists between two nonmetals.

a)

ionic

b)

covalent

52.
What is a positivly charge atom called?
a)
cation
b)
anion
53.

What is a negatively charged atom called?

a)

Anion

b)

Cation

c)

Ion

54.

What is a valence electron?

a)

an electron that is found in the outermost shell of an atom.

b)

an electron found in the innermost shell of an atom.

c)

an electron found in the middle shell.

55.

Determine the number of moles of AlNO3 that are in 264 g of the compound.

a)

2.97 mol

b)

3.45 mol

c)

2.73 mol

d)

1.86 mol

56.

A baker needs 6 g of baking soda for a recipe. The chemical formula for baking soda is NaHCO3. How many moles of baking soda is needed?

a)

0.071 mol

b)

0.167 mol

c)

0.273 mol

d)

0.214 mol

57.
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
58.

What is the name for this group of elements?

a)

Alkali

b)

Halogens

c)

Noble Gases

d)

Alkali-Earth

59.

What are isotopes?

a)

different element with the same number of electrons

b)

same element with a different number of electrons

c)

same element with a different number of neutrons

d)

different element with the same number of neutrons

60.

The modern periodic table is arranged in order of increasing atomic ____.

a)

mass

b)

charge

c)

number

d)

radius

61.

How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?

a)

1

b)

2

c)

3

d)

4

62.

What is the net charge of the ionic compound calcium fluoride?

a)

2-

b)

1-

c)

0

d)

1+

63.
Name the acid: HC2H3O2
a)
Acetic Acid
b)
Acetous Acid
c)
Hydrogen Acetate
d)
Hydrogen Dicarbon Trihydrogen Dioxygen
64.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
65.
Which element has the greatest electronegativity: Nitrogen (N) or Arsenic (As)?
a)
Nitrogen (N)
b)
Arsenic (As)
66.
What kelvin temperature is equivalent to -24 0C?
a)
a. 226 K
b)
b. 249 K
c)
c. 273 K
d)
d. 297 K
67.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

68.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

69.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

70.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
71.

What does pH measure?

a)

the amount of hydrogen (H+) ions

b)

the amount of hydroxide (OH-) ions

c)

amount of water

d)

all of the above

72.
A solution has a pH of 7.0.  What would happen to the pH if H ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
73.

For a solution at 25oC, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

74.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

75.
If 200 mL of a gas at 27°C is cooled to -33°C at a constant pressure, the volume will be
a)
250 mL
b)
204 mL
c)
196 mL
d)
160 mL
76.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
77.

Which will dissolve faster? Crushed table salt or a cube of table salt. Assume they have an equal mass.

a)

crushed table salt

b)

crystal of table salt

78.

When no more solute dissolves the solution is _________

a)

supersaturated

b)

unsaturated

c)

saturated

d)

extra saturated

79.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
80.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
81.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
82.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
83.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
84.
Elements in the same ____________ tend to have similar properties
a)
group
b)
period
85.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
86.
The subatomic particle with a negative charge is the
a)
electron
b)
proton
c)
neutron
d)
nucleus 
87.
In which region would the nonmentals be found?
a)
1
b)
4
c)
3
d)
5
88.
Are the atoms more stable when they are bonded together or when they are apart? 
a)
Bonded Together
b)
Apart
89.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
90.
How many significant figures does the following number have: 100.3
a)
4
b)
3
c)
5
d)
2
91.
How many sig figs are in 0.0045670?
a)
8
b)
4
c)
5
d)
7
92.

What is the volume of the fluid in the graduated cylinder shown?

a)

12.0 ml

b)

13.0 ml

c)

13.5 ml

d)

12.5 ml

93.

_______ are substances made of only one type of atom.

a)

Compounds

b)

Elements

c)

Mixtures

d)

Solutions

94.

If you have 15 grams of Baking Soda and 20 grams of Vinegar as products, what would you expect the mass of your reactants to be?

a)

15 grams

b)

20 grams

c)

5 grams

d)

35 grams

95.

What is a substance produced during a chemical reaction?

a)

product

b)

reactant

c)

law of conservation of mass

d)

chemical reaction

96.

Which name represents the formula Fe2O3Fe_2O_3  ?

a)

Iron (III) oxide

b)

Iron (II) oxide

97.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
98.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
99.
Which container will have lower pressure?
a)
left
b)
right
c)
they both have the same pressure
100.
When a solvent contains as much of the solute as it can hold, the solution is said to be
a)
supersaturated
b)
diluted
c)
saturated
d)
unsaturated
101.
What is a solvent
a)
the liquid in which a solute is dissolved to form a solution.
b)
Another word for solution
c)
A thing that make drinks turn colors
d)
Its a metal molecole
102.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Supersaturated
d)
Homogeneous solution
103.

In general as temperature decreases, the solubility...

a)

increases

b)

decreases

c)

stays the same

104.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
105.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
106.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
107.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
108.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
109.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
110.

Define: Solubility

a)

What is dissolved

b)

What does the dissolving

c)

A measure of how much solute can dissolve in solvent

d)

a charged ion

Similar Resources on Wayground

07 - IMFs - Polarity and IMFs

111 questions

07 - IMFs - Polarity and IMFs

quiz

Worksheet

•

10th Grade

BIOLOGY EOC Review Part 1

112 questions

BIOLOGY EOC Review Part 1

quiz

Worksheet

•

9th - 12th Grade

NCFE Earth Science Review

107 questions

NCFE Earth Science Review

quiz

Worksheet

•

9th - 12th Grade

Fall Final Review

105 questions

Fall Final Review

quiz

Worksheet

•

10th Grade

Biology Final Exam 2022-2023

110 questions

Biology Final Exam 2022-2023

quiz

Worksheet

•

10th Grade

Cell Structure and Function Review

107 questions

Cell Structure and Function Review

quiz

Worksheet

•

9th - 12th Grade

AICE MARINE EXTRA Exam REVIEW PT 1

110 questions

AICE MARINE EXTRA Exam REVIEW PT 1

quiz

Worksheet

•

9th - 12th Grade

Chemistry Unit 2

111 questions

Chemistry Unit 2

quiz

Worksheet

•

9th - 12th Grade