wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Review for Interim #2 (2025)

Total questions: 125

Worksheet time: 4hrs 10mins

Name
Class
Date
1.

Which type of bond is formed when electrons are transferred from one atom to another?

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Hydrogen bond

2.

What is the chemical formula for sodium chloride?

a)

NaCl

b)

NaCl 2_2

c)

Na 2_2 Cl

d)

Na 2_2 Cl 2_2

3.

What is the IUPAC name for H 2_2 O?

a)

Hydrogen oxide

b)

Dihydrogen monoxide

c)

Water

d)

Hydrogen dioxide

4.

Which law states that mass is conserved during a chemical reaction?

a)

Law of Definite Proportions

b)

Law of Conservation of Mass

c)

Law of Multiple Proportions

d)

Law of Constant Composition

5.

In the reaction 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O , how many hydrogen atoms are present on each side of the equation?

a)

2

b)

4

c)

1

d)

8

6.

Which of the following compounds is most likely to be ionic?

a)

CO 2_2

b)

NaF

c)

H 2_2 O

d)

CH 4_4

7.

Given magnesium (Mg) and chlorine (Cl), predict the formula for the stable binary ionic compound they form.

a)

MgCl

b)

MgCl 2_2

c)

Mg 2_2 Cl

d)

Mg 2_2 Cl 2_2

8.

Translate the chemical name "calcium oxide" into its chemical formula using IUPAC nomenclature.

a)

CaO

b)

CaO 2_2

c)

Ca 2_2 O

d)

Ca 2_2 O 2_2

9.

A student mixes 10 g of reactant A with 15 g of reactant B. After the reaction, 25 g of product C is formed. What does this demonstrate?

a)

Mass is not conserved

b)

Mass is conserved

c)

Mass increases

d)

Mass decreases

10.

Which chemical equation correctly shows conservation of atoms for the reaction between hydrogen and oxygen to form water?

a)

H2+O2→H2OH_2 + O_2 \rightarrow H_2O

b)

2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O

c)

H2+2O2→2H2OH_2 + 2O_2 \rightarrow 2H_2O

d)

2H2+2O2→2H2O2H_2 + 2O_2 \rightarrow 2H_2O

11.

Does NaCl or H 2_2 O have a higher melting point and why?

a)

NaCl, because it is ionic

b)

H 2_2 O, because it is covalent

c)

NaCl, because it is covalent

d)

H 2_2 O, because it is ionic

12.

What is the chemical formula for the ionic compound formed between aluminum (Al) and oxygen (O)?

a)

AlO

b)

Al 2_2 O 3_3

c)

AlO 2_2

d)

Al 3_3 O 2_2

13.

Given the chemical formula K 2_2 S, use IUPAC nomenclature to determine the name of the compound.

a)

Potassium sulfide

b)

Potassium sulfate

c)

Potassium sulfur

d)

Dipotassium monosulfide

14.

Plan an investigation to show that mass is conserved when copper reacts with sulfur to form copper(II) sulfide.

a)

Weigh reactants and products before and after the reaction

b)

Only measure the reactants

c)

Only measure the products

d)

Do not measure anything

15.

Use a model of the chemical equation 2Na+Cl2→2NaCl2Na + Cl_2 \rightarrow 2NaCl to illustrate how the total number of atoms is conserved.

a)

2 Na atoms and 2 Cl atoms on both sides

b)

1 Na atom and 2 Cl atoms on both sides

c)

2 Na atoms and 1 Cl atom on both sides

d)

1 Na atom and 1 Cl atom on both sides

16.

Which of the following is a property of covalent compounds?

a)

High melting point

b)

Conducts electricity in solution

c)

Low melting point

d)

Forms crystals

17.

What is the formula for the ionic compound formed between potassium (K) and bromine (Br)?

a)

KBr

b)

K 2_2 Br

c)

KBr 2_2

d)

K 2_2 Br 2_2

18.

What is the IUPAC name for Na 2_2 O?

a)

Sodium oxide

b)

Disodium oxide

c)

Sodium dioxide

d)

Sodium monoxide

19.

During a chemical reaction, if the total mass of reactants is 50 g and the total mass of products is 50 g, what does this indicate?

a)

Mass is lost

b)

Mass is gained

c)

Mass is conserved

d)

Mass is destroyed

20.

In the equation C+O2→CO2C + O_2 \rightarrow CO_2 , how many oxygen atoms are present on each side?

a)

1

b)

2

c)

3

d)

4

21.

Which compound is most likely to be covalent?

a)

NaCl

b)

MgO

c)

CO 2_2

d)

KBr

22.

Predict the formula for the stable binary ionic compound formed between calcium (Ca) and fluorine (F).

a)

CaF

b)

CaF 2_2

c)

Ca 2_2 F

d)

Ca 2_2 F 2_2

23.

Translate the chemical name "magnesium chloride" into its chemical formula using IUPAC nomenclature.

a)

MgCl

b)

MgCl 2_2

c)

Mg 2_2 Cl

d)

Mg 2_2 Cl 2_2

24.

A student combines 20 g of reactant X with 30 g of reactant Y. After the reaction, 50 g of product Z is obtained. What principle does this support?

a)

Law of Conservation of Mass

b)

Law of Definite Proportions

c)

Law of Multiple Proportions

d)

Law of Constant Composition

25.

Which chemical equation shows conservation of atoms for the reaction between nitrogen and hydrogen to form ammonia?

a)

N2+H2→NH3N_2 + H_2 \rightarrow NH_3

b)

N2+3H2→2NH3N_2 + 3H_2 \rightarrow 2NH_3

c)

2N2+3H2→2NH32N_2 + 3H_2 \rightarrow 2NH_3

d)

N2+2H2→2NH3N_2 + 2H_2 \rightarrow 2NH_3

26.

Compare the electrical conductivity of NaCl and CH 4_4 in water. Which compound conducts electricity and why?

a)

NaCl, because it forms ions in water

b)

CH 4_4 , because it forms ions in water

c)

NaCl, because it is covalent

d)

CH 4_4 , because it is ionic

27.

Develop a model to predict the formula for the ionic compound formed between barium (Ba) and chlorine (Cl).

a)

BaCl

b)

BaCl 2_2

c)

Ba 2_2 Cl

d)

Ba 2_2 Cl 2_2

28.

Plan an investigation to demonstrate mass conservation when zinc reacts with hydrochloric acid to produce hydrogen gas and zinc chloride.

a)

Measure the mass of all reactants and products before and after the reaction

b)

Only measure the mass of zinc

c)

Only measure the mass of hydrogen gas

d)

Do not measure anything

29.

Use a model of the chemical equation 2K+2H2O→2KOH+H22K + 2H_2O \rightarrow 2KOH + H_2 to illustrate how the total number of atoms is conserved.

a)

2 K, 4 H, and 2 O atoms on both sides

b)

2 K, 2 H, and 2 O atoms on both sides

c)

4 K, 4 H, and 2 O atoms on both sides

d)

2 K, 2 H, and 4 O atoms on both sides

30.

Which of the following best explains why ionic compounds generally have higher melting points than covalent compounds?

a)

Weak forces between molecules

b)

Strong electrostatic forces between ions

c)

Presence of hydrogen bonds

d)

Low atomic mass

31.

In the reaction 2Mg+O2→2MgO2Mg + O_2 \rightarrow 2MgO , how many magnesium atoms are present on each side of the equation?

a)

4

b)

3

c)

2

d)

1

32.

What is the IUPAC name for the compound with the formula KBr?

a)

Potassium bromide

b)

Potassium bromine

c)

Potassium bromate

d)

Potassium dibromide

33.

Valence electrons are transferred

a)

Ionic bonds

b)

Covalent bonds

34.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

35.

Conducts electricity well when melted or dissolved

a)

Ionic compounds

b)

Covalent compounds

36.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

37.

Always a solid at room temperature

a)

Ionic compounds

b)

Covalent compounds

38.

Can be a solid, liquid, or gas at room temperature

a)

Ionic compounds

b)

Covalent compounds

39.

Generally high melting & boiling points

a)

Ionic compounds

b)

Covalent compounds

40.

Generally low melting and boiling points

a)

Ionic compounds

b)

Covalent compounds

41.

Generally, atoms form bonds so that _______________.

a)

Each atom loses its electrons

b)

Each atom has a stable electron configuration

c)

Each atom has an unstable electron configuration

d)

Each atom gains electrons

42.

What kind of bond does this show?

a)

Ionic

b)

Covalent

43.

What kind of bonds are shown here?

a)

Covalent

b)

Ionic

44.

What happens when you put an ionic compound in water?

a)

The ions separate

b)

The ions pack more closely together

c)

Nothing happens

45.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

46.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

47.

Cations are ​ (a)   ​ charged metal ion because the metals ​ (b)   electrons

Choose from the below words
positively
lose
negatively
gain
48.

Anions are ​​ (a)   charged metal ion because the metals ​ (b)   ​electrons

Choose from the below words
negatively
gain
positvely
lose
49.

Which of the following could form a covalent bond?

a)

Two or More Nonmetals

b)

Metal and Nonmetal

c)

Two or More Metals

d)

Metal and Polyatomic Ion

e)

All Provided Options

50.

How many valence electrons do most atoms need to be stable?

a)

8

b)

6

c)

4

d)

2

51.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
52.

Where are the metals located on the periodic table? 

a)
Blue
b)
Red
c)
Green
53.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

54.

The chemical bond between a metal and a non-metal will be a _____ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

55.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

56.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

57.

MgO

a)

ionic

b)

covalent

c)

metallic

58.

If two fluorine atoms bond they will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

59.

Hydrogen and Chlorine will from a _________ bond

a)

ionic

b)

covalent

c)

metallic

60.

Why don't noble gases form bonds?

a)

They all have a full octet

b)

Noble gases do form bonds

c)

They only bond when with eachother

d)

none of these answers are correct

61.

A sodium ion has a charge of

a)

-1

b)

-2

c)

+1

d)

+2

62.

An example of a covalent compound is

a)

sodium floride

b)

calcium chloride

c)

carbon dioxide

d)

all of the above

63.

What is the chemical formula for the compound containing one nitrogen atom and two oxygen atoms?

a)

O2N

b)

N2O

c)

NO

d)

NO2

64.

True or False: An oxygen atom has eight valence electrons

a)

True

b)

False

65.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
66.

Valence electrons are found

a)

outermost energy level

b)

innermost energy level

c)

some where in the electron cloud

67.

How many valence electrons does Boron have?

a)

1

b)

2

c)

3

d)

4

68.

Group numbers on the periodic table help us determine

a)

number of valence electrons

b)

state of the element (solid, liquid, gas)

69.

What does the number 3 represent in 4NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

70.

What does the number 4 represent in 4NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

71.

How many Nitrogen (N) atoms are in 4NH3?

a)

4

b)

1

c)

3

d)

12

72.

How many Hydrogen (H) atoms are in 4NH3?

a)

4

b)

1

c)

3

d)

12

73.

In the equation shown, what are the reactant(s)?

a)

N2 + H2

b)

NH3

74.

In the equation shown, what are the product(s)?

a)

N2 + H2

b)

NH3

75.

Is this equation balanced?

a)

Yes

b)

No

76.

Is this equation balanced?

a)

Yes

b)

No

77.

Is this equation balanced?

a)

Yes

b)

No

78.

To balance an equation you should:

a)

ONLY change subscripts.

b)

ONLY change coefficients.

c)

Change BOTH subscripts and coefficients.

79.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
80.

88 g of strontium reacts with 160 g of bromine to produce _______ g of strontium bromide.

a)

72

b)

240

c)

248

d)

80

81.

24 g of magnesium reacts with 38 g of fluorine to produce ______ g of magnesium fluoride.

a)

10

b)

24

c)

14

d)

62

82.

14 g of lithium reacts with _____ g of sulfur to produce 46 g of lithium sulfide.

a)

32

b)

60

c)

25

d)

10

83.

40 grams of calcium reacts with 71 grams of chlorine to produce _______ g of calcium chloride.

a)

31

b)

101

c)

100

d)

111

84.

In the chemical formula C12H22O11C_{12}H_{22}O_{11}  , how many elements are there?

a)

1

b)

2

c)

3

d)

4

85.

In the chemical formula C12H22O11C_{12}H_{22}O_{11}  , how many C atoms are there?

a)

12

b)

22

c)

11

d)

45

86.

In the chemical formula C12H22O11C_{12}H_{22}O_{11}  , how many O atoms are there?

a)

12

b)

22

c)

11

d)

45

87.

In the chemical formula C12H22O11C_{12}H_{22}O_{11}  , how many H atoms are there?

a)

12

b)

22

c)

11

d)

45

88.

What is the TOTAL number of atoms in the chemical formula C12H22O11C_{12}H_{22}O_{11}  ?

a)

12

b)

22

c)

11

d)

45

89.

How does a balanced chemical equation satisfy the Law of Conservation of Mass?

a)

During a chemical reaction, matter is destroyed.

b)

During a chemical reaction, the total number of atoms increases.

c)

 During a chemical reaction, one or more new substances are formed.

d)

During a chemical reaction, the total amount of matter stays the same.

90.

What happens to the total mass of the substances after a chemical reaction?

a)

It decreases.

b)

It increases.

c)

 It remains the same.

d)

It increases then decreases.

91.

Jin bought a heat pack that weighs 15 g. He shook it so it would release heat to warm his hands. The release of heat indicates a chemical reaction took place in a closed system. What would be the mass of the heat pack after the chemical reaction?

a)

5 g

b)

10 g

c)

12 g

d)

15 g

92.
Matter can not be created nor destroyed: it can only be
a)
Destroyed a little bit
b)
Invisible
c)
Transformed, changed
d)
None of the above
93.
The number to the lower side of an element is a 
a)
Subscript
b)
Superscript
c)
Coefficient
d)
Charge
94.
The number in front of a compound or element is a 
a)
Subscript
b)
Coefficient
c)
Superscript
d)
Charge
95.
A chemical reaction is balanced when
a)
both sides have the same elements
b)
Both sides have the same  number of atoms
c)
Same subscripts
d)
Same coefficients
96.
If reaction starts with 20g of reactants it should produce 
a)
a total of 40g of products
b)
a total of 10g of products
c)
a total of 80 g of products
d)
a total of 20g of products
97.
In a reaction A + B ----> C,  reactant A has 5g and product  C has 9g. How many grams does reactant B should have? 
a)
4g
b)
5g
c)
9g
d)
14g
98.
Bob puts 200 grams of ice into a pitcher with 900 grams of water. He gets distracted and comes back later to find that the ice has melted in the water. How many grams of water does Bob now have in the pitcher?
a)
200 g
b)
700 g
c)
1,100 g
99.

According to the law of conservation of mass, how much zinc was present in the zinc carbonate?

a)

256 g

b)

88 g

c)

104 g

d)

40 g

100.
A 55-gram egg is placed in a pot. After the egg is boiled, which is most likely the mass of the egg?
a)
50 
b)
55 
101.
Rodney tears a piece of paper weighing 1 oz into small pieces. What most likelyhappens to the weight of the sheet of paper after Rodney tears it into pieces?
a)
The 
b)
The weight is cut in half.
c)
The weight stays the same.
102.

So, the Law of Conservation of Mass would tell us that the mass of all the REACTANTS must __________ the mass of all PRODUCTS in a chemical reaction.

a)

equal

b)

be greater than

c)

be less than

103.

Which of the following equations does not demonstrate the law of conservation of mass?

a)

2Na + Cl2 ➡️ 2NaCl

b)

NaOH + HCl ➡️ NaCl + H20

c)

P4 + 5O2 ➡️ 2P4O10

104.
How many Oxygen (O) atoms are in 2C2HO8Cl2
a)
2
b)
16
c)
8
d)
5
105.

The reactants in the image above are:

a)

CH4 and 2 O2

b)

2 H2O and CO2

c)

All of these are reactants

d)

All of these are products

106.

Aria and David are studying chemistry and they come across the elements magnesium (Mg) and bromine (Br) in the Periodic Table. Avery joins them and asks, 'What would be a characteristic of the compound MgBr2 that we could observe if we had it in our lab?'.

a)

It has a high melting point.

b)

It is formed by covalent bonds.

c)

It is a gas at room temperature.

d)

It does not conduct electricity when dissolved in water.

107.

An unbalanced chemical equation is shown below.

CH4 + O2  → CO2 + H2O


Which is the correctly balanced equation for the expression?

a)

CH4 + 2O2 → CO2 + H2O

b)

CH4 + 3O2 → CO2 + H2O

c)

2CH4 + O2 → CO2 + H2O

d)

CH4 + 2O2 → CO2 + 2H2O

108.

Potassium chloride can be produced from potassium metal and chlorine gas. Which of the following is the correct, balanced equation for the production of potassium chloride?

a)

4K(s) + Cl2(g) → 2K2Cl(s)

b)

K(s) + Cl2(g) → KCl(s)

c)

2K(s) + Cl2(g) → 2KCl(s)

d)

K(s) + Cl2(g) → KCl2(s)

109.

An unbalanced chemical equation is shown below.

NO + O2 → NO2


Which is the correctly balanced equation for the expression?

a)

NO + O2 → 3NO2

b)

NO + 2O2 → 2NO2

c)

2NO + O2 → 2NO2

d)

2NO + O2 → NO2

110.

During combustion, methane yields carbon dioxide and water. The unbalanced equation for this reaction is:

CH4 + O2 CO2 + H2O


What coefficients are needed in order to balance this equation?

a)

1, 1, 1, 2

b)

1, 2, 1, 2

c)

5, 4, 3, 6

d)

1, 1, 2, 1

111.

An unbalanced chemical equation is shown below.

Al + O2 → Al2O3


Which is the correctly balanced equation for the expression?

a)

4Al + O2 → 2Al2O3

b)

4Al + 3O2 → 2Al2O3

c)

3Al + 2O2 → Al2O3

d)

2Al + 3O2 → Al2O3

112.

An unbalanced chemical equation is shown below.
CH4 + O2  CO2 + H2O

Which of the following particle diagrams correctly represents the balanced form of the equation?

a)

b)

c)

d)

113.
This pictures simulates what type of reaction?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
114.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
115.
Pb(NO3)2 --> PbO + NO2 + O2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
116.

3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2

a)

Synthesis (or combination)

b)

Decomposition

c)

Single replacement

d)

Double replacement

117.

What reaction has the following general formula:

A + CD --> C + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

118.

What reaction has the following general formula:

AB + CD --> CB + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

119.

What reaction has the following general formula:
CxHy + O2 −>CO2 + H2OC_xH_y\ +\ O_2\ ->CO_{2\ }+\ H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

120.

What is the general reaction scheme for a decomposition reaction?

a)

A + B --> AB

b)

AB --> A + B

c)

A + CD --> C + AD

d)

AB + CD --> CB + AD

e)

CxHy+O2 −> CO2+H2OC_xH_y+O_2\ ->\ CO_2+H_2O

121.

Which of the following atomic models of chemical reactions correctly demonstrates the Law of Conservation of Matter?

a)

b)

c)

d)

122.

Students want to gather evidence for the claim that the number of atoms present before a chemical reaction is equal to the number of atoms present after the chemical reaction.  They decide to react vinegar and baking soda in a sealed plastic bag.  Which of the following would provide the evidence the students need?

a)

The mass of the plastic bag, baking soda, and vinegar before the reaction was equal to the mass after the reaction

b)

Bubbles were produced during the reaction, which meant that a gas was being produced

c)

The plastic bag did not change in any way, indicating that it was not involved in the reaction

d)

The mass of the baking soda was exactly equal ot the mass of the vinegar used to create the chemical reaction

123.

True or False: The mass of the reactants is equal to the mass of the products?

a)

True

b)

False

124.

Which of the models of a chemical reaction best represents the Law of Conservation of Mass?

a)

A

b)

B

c)

C

d)

D

125.

Which of the models of a chemical reaction best represents the Law of Conservation of Mass?

a)

A

b)

B

c)

C

d)

D

Similar Resources on Wayground

Atoms, elements, and compounds

120 questions

Atoms, elements, and compounds

quiz

Worksheet

•

9th - 10th Grade

Semester 2 Exam Review

123 questions

Semester 2 Exam Review

quiz

Worksheet

•

9th - 12th Grade

B1 AQA Cell biology

122 questions

B1 AQA Cell biology

quiz

Worksheet

•

KG - 12th Grade

Spring Semester Final Review

120 questions

Spring Semester Final Review

quiz

Worksheet

•

9th - 10th Grade

Unit 1 Chemistry of Life Practice Test

127 questions

Unit 1 Chemistry of Life Practice Test

quiz

Worksheet

•

9th - 12th Grade

N4 Chapter Review

124 questions

N4 Chapter Review

quiz

Worksheet

•

9th Grade - University

Aquatics Summer Final Exam

130 questions

Aquatics Summer Final Exam

quiz

Worksheet

•

9th Grade - University

Earth Systems Midterm Review

120 questions

Earth Systems Midterm Review

quiz

Worksheet

•

9th - 12th Grade