Free Printable Chemistry Final Exam

1.

The mole is a...

a)

Unit to measure the amount of atoms in a substance

b)

Unit to measure distance

c)

Unit to measure time of atomic decay

d)

Unit used to measure the size of each atom in a substance

2.

How many particles are in 13.5 grams of Beryllium, Be?

a)

1.5 particles

b)

9 particles

c)

4x10²³ particles

d)

9x10²³ particles

3.

What is the molar mass of calcium hydroxide, Ca(OH)₂?

a)

74.1 g/mole

b)

57.1 g/mole

c)

58.1 g/mole

d)

57.1 u

4.

What is the molar mass of AuCl₃?

a)

96 g

b)

130 g

c)

232.5 g

d)

303.3 g

5.

Determine the mass of 2.40 moles of C₆H₁₂

a)

201 g

b)

115 g

c)

230 g

d)

353 g

6.

What is the total mass, in grams, of a 0.75 mole sample of SO₂?

a)

16 g

b)

24 g

c)

32 g

d)

48 g

7.

Find the molar mass of calcium carbonate (CaCO₃) to the nearest gram.

a)

100 g

b)

68 g

c)

84 g

d)

112 g

8.

What is the mass number of an atom with 6 protons and 8 neutrons?

a)

12

b)

16

c)

10

d)

14

9.

How many neutrons are in an atom with mass number 35 and atomic number 17?

a)

18

b)

22

c)

16

d)

20

10.

Calculate the number of neutrons in an atom with a mass number of 56 and atomic number of 26.

a)

56

b)

6

c)

30

d)

26

11.

What is the mass number of an atom with 6 protons and 8 neutrons?

a)

12

b)

16

c)

10

d)

14

12.

Calculate the mass number of an atom with 20 protons and 20 neutrons.

a)

39

b)

41

c)

40

d)

38

13.

How many neutrons are present in an atom with a mass number of 35 and atomic number of 17?

a)

18

b)

22

c)

16

d)

20

14.

What is the mass number of an atom with 47 protons and 61 neutrons?

a)

108

b)

107

c)

105

d)

108.5

15.

Calculate the number of neutrons in an atom with a mass number of 56 and atomic number of 26.

a)

56

b)

6

c)

30

d)

26

16.

How many protons are there in an atom with a mass number of 40 and 20 neutrons?

a)

40

b)

80

c)

60

d)

20

17.

Determine the atomic number of an atom that has 79 protons.

a)

197

b)

83

c)

118

d)

79

18.

Calculate the atomic number of an atom with 82 neutrons and a mass number of 207.

a)

125

b)

82

c)

164

d)

207

19.

How many neutrons are present in an atom with an atomic number of 14 and mass number of 28?

a)

14

b)

28

c)

56

d)

42

20.

Determine the mass number of an atom with 6 protons, 6 neutrons, and 6 electrons.

a)

24

b)

12

c)

6

d)

18

21.

How many electrons are there in an atom with an atomic number of 82?

a)

125

b)

82

c)

207

d)

0

22.

How many neutrons would you expect the average gold atom to have?

a)

79

b)

118

c)

197

d)

276

23.

The section labeled D is known as the?

a)

Electron cloud

b)

Neutron

c)

Nucleus

d)

Electron

24.

What is the atomic number of this atom?

a)

2

b)

4

c)

6

d)

none of the above

25.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

26.

Name this element.

a)

Neon

b)

Magnesium

c)

Sodium

d)

Manganese

27.

What is the correct name for the covalent compound $N_2O_5$ ?

a)

Nitrogen oxide

b)

Dinitrogen pentoxide

c)

Nitrogen pentaoxide

d)

Dinitrogen oxide

28.

What is the correct Lewis structure for methane, $CH_4$ ?

a)

C surrounded by 4 H, with no lone pairs on carbon

b)

C double bonded to 2 H, with 2 lone pairs on carbon

c)

C triple bonded to H, with 1 lone pair on carbon

d)

C surrounded by 2 H, with 2 lone pairs on carbon

29.

What is the correct name for the covalent compound $PCl_5$ ?

a)

Phosphorus pentachloride

b)

Phosphorus chloride

c)

Monophosphorus pentachloride

d)

Phosphorus chlorate

30.

Which of the following is the correct Lewis structure for ammonia, $NH_3$ ?

a)

N with 3 H attached and 1 lone pair on nitrogen

b)

N with 3 H attached and no lone pairs on nitrogen

c)

N triple bonded to 3 H with no lone pairs

d)

N double bonded to 3 H with 1 lone pair

31.

How is the covalent compound $SO_3$ named?

a)

Sulfur trioxide

b)

Sulfur oxide

c)

Monosulfur trioxide

d)

Sulfur monoxide

32.

What is the correct name for the covalent compound $SF_6$ ?

a)

Sulfur hexafluoride

b)

Sulfur fluoride

c)

Monosulfur hexafluoride

d)

Sulfur hexachloride

33.

Which of the following is the correct Lewis structure for ethylene, $C_2H_4$ ?

a)

Two C atoms double bonded, each C bonded to 2 H

b)

Two C atoms single bonded, each C bonded to 3 H

c)

Two C atoms triple bonded, each C bonded to 1 H

d)

Two C atoms double bonded, each C bonded to 1 H

34.

How is the covalent compound $P_2O_5$ named?

a)

Diphosphorus pentoxide

b)

Phosphorus oxide

c)

Phosphorus pentaoxide

d)

Diphosphorus oxide

35.

What is the correct Lewis structure for nitrogen trifluoride, $NF_3$ ?

a)

N with 3 F attached and 1 lone pair on nitrogen

b)

N with 3 F attached and no lone pairs on nitrogen

c)

N triple bonded to 3 F with no lone pairs

d)

N double bonded to 3 F with 1 lone pair

36.

What is the correct name for the compound $Cl_2O_7$ ?

a)

Dichlorine heptoxide

b)

Chlorine oxide

c)

Dichlorine oxide

d)

Chlorine heptoxide

37.

Which of the following is the correct Lewis structure for sulfuric acid, $H_2SO_4$ ?

a)

S double bonded to 2 O and single bonded to 2 OH groups

b)

S single bonded to 4 O, each O bonded to an H

c)

S double bonded to 4 O, no H attached

d)

S surrounded by 4 O, each O bonded to an H

38.

How is the covalent compound $ClO_2$ named?

a)

Chlorine dioxide

b)

Chlorine oxide

c)

Monochlorine dioxide

d)

Dichlorine oxide

39.

What is the correct name for the covalent compound $SiO_2$ ?

a)

Silicon dioxide

b)

Silicon oxide

c)

Disilicon oxide

d)

Monosilicon dioxide

40.

How is the covalent compound $N_2O$ named?

a)

Dinitrogen monoxide

b)

Nitrogen oxide

c)

Nitrogen monoxide

d)

Dinitrogen oxide

41.

The chemical bond formed when two atoms share electrons is called a(n) _______.

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Electron bond

42.

How many electrons are shared within a single bond?

a)

0

b)

1

c)

2

d)

4

43.

Which atoms are most likely to form covalent bonds?

a)

Metal atoms that share electrons

b)

Metal atoms that share protons

c)

Nonmetal atoms that share electrons

d)

Nonmetal atoms that share protons

44.

The electrons that are lost, gained, or shared in chemical bonds are called _______.

a)

Valence electrons

b)

Chemical electrons

c)

Lewis electrons

d)

None of the above

45.

How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable?

a)

2

b)

4

c)

6

d)

8

46.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

47.

How many valence electrons does an atom of oxygen have?

a)

8

b)

4

c)

2

d)

6

48.

How many energy shells does an atom of sodium have?

a)

7

b)

3

c)

5

d)

1

49.

What is the maximum number of electrons that can be present in the first energy shell?

a)

2

b)

8

c)

6

d)

4

50.

What is the maximum number of electrons that can be present in the third energy shell? [Hint: #e- = 2n^2, where n= # of shells]

a)

8

b)

2

c)

18

d)

32

51.

What is the trend of valence electrons across a period in the periodic table?

a)

Decrease

b)

Stay the same

c)

Increase

d)

Random

52.

What is the trend of energy shells across a period in the periodic table?

a)

Number of energy shells decreases

b)

Number of energy shells increases

c)

Number of energy shells remains the same

d)

Number of energy shells varies randomly

53.

What is the trend of valence electrons down a group in the periodic table?

a)

Valence electrons increase

b)

Valence electrons remain constant

c)

Valence electrons fluctuate randomly

d)

Valence electrons decrease

54.

The period for Bromine is ___________.

a)

3

b)

2

c)

4

55.

Beryllium is in group number______.

a)

Group 2

b)

Group 3

c)

Group 4

d)

Group 7

56.

Name group 1A on the periodic table.

a)

alkali metals

b)

alkaline earth metals

c)

noble gases
noble gases

d)

halogens

57.

Elements in group 18 are called ___.

a)

Alkali metals

b)

Alkaline Earth metals

c)

Halogens

d)

Noble gases

58.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

59.

Which element is located in period 3 and group 16 of the periodic table?

a)

Sulfur

b)

Oxygen

c)

Chlorine

d)

Argon

60.

What is the electron configuration of chlorine?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p5

d)

1s2 2s2 2p6

61.

Which element is located in period 2 and group 14 of the periodic table?

a)

Carbon

b)

Nitrogen

c)

Oxygen

d)

Boron

62.

What is the trend of atomic radius across a period in the periodic table?

a)

Increases

b)

Decreases

c)

Remains constant

d)

Fluctuates randomly

63.

What type of reaction involves one element replacing another element in a compound?

a)

Single Displacement Reaction

b)

Double Displacement Reaction

c)

Decomposition Reaction

64.

What are the products of the chemical reaction pictured?

a)

CH₄ and CO₂

b)

CH₄ and O₂

c)

CO₂ and H₂O

d)

O₂ and H₂O

65.

What type of reaction involves 2 substances combining to form 1 new compound?

a)

Single Displacement Reaction

b)

Double Displacement Reaction

c)

Synthesis Reaction

66.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

67.

What is the general form of a combustion reaction?

a)

A single reactant breaks down into multiple products.

b)

Two or more reactants combine to form a single product.

c)

A hydrocarbon reacts with oxygen to produce carbon dioxide and water.

d)

An element displaces another in a compound.

68.

Which of the following is an example of a synthesis reaction?

a)

$2KClO_3 \rightarrow 2KCl + 3O_2$

b)

$2Mg + O_2 \rightarrow 2MgO$

c)

$Zn + 2HCl \rightarrow ZnCl_2 + H_2$

d)

$AgNO_3 + NaCl \rightarrow AgCl + NaNO_3$

69.

What occurs during a decomposition reaction?

a)

Two compounds exchange partners.

b)

A single compound breaks down into two or more simpler substances.

c)

Two elements combine to form a compound.

d)

An element replaces another in a compound.

70.

Identify the type of reaction: $CuSO_4 + Zn \rightarrow ZnSO_4 + Cu$

a)

Combustion

b)

Synthesis

c)

Decomposition

d)

Single displacement

71.

Which reaction is an example of a double displacement reaction?

a)

$2Na + Cl_2 \rightarrow 2NaCl$

b)

$CaCO_3 \rightarrow CaO + CO_2$

c)

$Na_2S + Cd(NO_3)_2 \rightarrow CdS + 2NaNO_3$

d)

$C + O_2 \rightarrow CO_2$

72.

What is a key characteristic of a combustion reaction?

a)

It always involves oxygen as a reactant.

b)

It results in the formation of a single product.

c)

It only occurs with organic compounds.

d)

It is a type of synthesis reaction.

73.

Choose the correct example of a decomposition reaction:

a)

$H_2 + Cl_2 \rightarrow 2HCl$

b)

$2HgO \rightarrow 2Hg + O_2$

c)

$Fe + CuSO_4 \rightarrow FeSO_4 + Cu$

d)

$NaCl + AgNO_3 \rightarrow AgCl + NaNO_3$

74.

What is typically produced in a combustion reaction involving a hydrocarbon?

a)

Hydrogen gas and carbon monoxide

b)

Water and carbon dioxide

c)

Oxygen and carbon

d)

Hydrogen peroxide and carbon

75.

Which of the following is a possible product of a reaction between Hydrogen (H) and Oxygen (O)?

a)

$Fe_2O_3$

b)

$CO_2$

c)

$H_2O$

d)

HF

76.

Which of the following is a possible product of a reaction between Iron(Fe) and Oxygen (O)?

a)

$Fe_2O_3$

b)

$CO_2$

c)

$H_2O$

d)

HF

77.

Balance the equation below

_ WO₃ + _H₂ → _W + _H₂O

_{Note: Write the coefficient "1" to avoid ambiguity}

(a)

78.

Balance this equation.
_SnO₂+_H₂-->_Sn +_H₂O

a)

1,1,2,1

b)

1,2,1,1

c)

1,2,1,2

d)

1,2,2,1

79.

Balance this equation.
_CF₄+ _Br₂-- _CBr₄+ _F₂

a)

2,1,2,1

b)

1,2,2,1

c)

1,2,1,2

d)

2,2,2,2

80.

An unbalanced equation is given below. After balancing the equation, what is the coefficient in front of H_2(g)?

Al_(s) + HCl_(aq) ---> AlCl_3(aq) + H_2(g)

a)

2

b)

3

c)

1

d)

6

81.

An unbalanced equation is given below. After balancing the equation, what is the coefficient in front of Cu_(s)?

Al_(s) + CuSO_4(aq) ---> Al₂(SO₄)_3(aq) + Cu_(s)

a)

2

b)

3

c)

1

d)

6

82.

What is the number of particles in one mole of any substance?

a)

3.01 x 10^23 particles

b)

6.02 x 10^23 particles

c)

6.02 x 10^22 particles

d)

6.02 x 10^24 particles

83.

How many moles of magnesium are there in 3.01 x 10^22 atoms of magnesium?

a)

0.05 mol Mg

b)

0.5 mol Mg

c)

5 mol Mg

d)

0.005 mol Mg

84.

What is the number of formula units in 12.5 moles of calcium phosphate?

a)

7.53 x 10^24 formula units

b)

75.3 x 10^23 formula units

c)

7.53 x 10^23 formula units

d)

75.3 x 10^24 formula units

85.

How many moles are in 28 grams of CO2?

a)

0.64 mol CO2

b)

6.4 mol CO2

c)

0.064 mol CO2

d)

64 mol CO2

86.

What is the mass of 5 moles of Fe2O3?

a)

798.5 g

b)

79.85 g

c)

7.985 g

d)

7985 g

87.

What is the molar mass of argon used in the calculation to find the number of moles of argon in 452 g of argon?

a)

39.95 g/mol

b)

40.08 g/mol

c)

18.00 g/mol

d)

28.02 g/mol

88.

How many grams of CO2 are present in 3.45 moles of CO2?

a)

151.8 g

b)

44 g

c)

100 g

d)

200 g

89.

How many molecules are there in 3.36 g of oxygen (O2)?

a)

6.02 x 10^23 molecules

b)

6.32 x 10^22 molecules

c)

1.00 x 10^23 molecules

d)

2.00 x 10^23 molecules

90.

What is the result of the calculation for the mass of 2.00 x 10^23 molecules of F2?

a)

12.0 g

b)

37.92 g

c)

12.6 g

d)

50.0 g

91.

How many molecules of aspartame are present in 10.5 g of aspartame?

a)

2.15 x 10^22 molecules

b)

6.02 x 10^23 molecules

c)

1.00 x 10^23 molecules

d)

3.57 x 10^21 molecules

92.

How many atoms of nitrogen are there in 1.2 grams of aspartame?

a)

4.91 x 10^21 atoms

b)

6.02 x 10^23 atoms

c)

1.00 x 10^23 atoms

d)

2.00 x 10^22 atoms

93.

What is the mass of 2 moles of NaCl?

a)

117 g

b)

58.5 g

c)

234 g

d)

29.25 g

94.

How many moles of carbon dioxide are there in 4.4 x 10^24 molecules of CO2?

a)

7.3 mol CO2

b)

0.73 mol CO2

c)

73 mol CO2

d)

0.073 mol CO2

95.

What is the molar mass of calcium carbonate used in the calculation to find the number of moles in 500 g of CaCO3?

a)

100.09 g/mol

b)

200.18 g/mol

c)

50.05 g/mol

d)

150.14 g/mol

96.

What is the mass of 3 moles of sulfuric acid (H2SO4)?

a)

294 g

b)

98 g

c)

196 g

d)

588 g

97.

How many formula units are there in 0.25 moles of sodium chloride (NaCl)?

a)

1.51 x 10^23 formula units

b)

1.51 x 10^24 formula units

c)

1.51 x 10^22 formula units

d)

1.51 x 10^21 formula units

98.

What is the number of moles in 22 grams of carbon dioxide (CO2)?

a)

0.5 mol CO2

b)

0.05 mol CO2

c)

5 mol CO2

d)

0.005 mol CO2

99.

What is the mass of 4 moles of H2O?

a)

72 g

b)

36 g

c)

18 g

d)

144 g

100.

How many moles are there in 44 grams of nitrogen gas (N2)?

a)

1.57 mol N2

b)

3.14 mol N2

c)

0.785 mol N2

d)

6.28 mol N2

Chemistry Final Exam

Total questions: 100

Worksheet time: 2hrs 55mins

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