Free Printable Final Review 2022

1.

Define accuracy.

a)

How close multiple measurements are to each other.

b)

How close multiple measurements are to a prior measurement.

c)

How close a measurement is to a repeating value.

d)

How close a measurement is to an accepted value.

2.

Define precision.

a)

How many times a measurement matches a possible value.

b)

How close multiple measurements are to each other.

c)

How close a measurement is to the true or accepted value.

d)

How many times the exact same measurement repeats.

3.

Draw a target that is accurate but not precise.

4.

Draw a target that is precise but not accurate.

5.

Draw a target that is both accurate and precise.

6.

Which of the following would be precise but not accurate measurement of a 50 gram mass?

a)

49.35 g

b)

50.01 g

50.00 g

49.99 g

c)

50.00 g

d)

49.38 g

49.69 g

49.21 g

7.

Which of the following would be an accurate but not precise measurement of a 50 gram mass?

a)

49.35 g

b)

50.01 g

50.00 g

49.99 g

c)

49.75 g

49.86 g

50.74 g

d)

50.00 g

8.

Which of the following would be accurate and precise measurement of a 50 gram mass?

a)

50.00 g

b)

50.00 g

50.01 g

49.99 g

c)

49.68 g

d)

49.99 g

49.21 g

50.09 g

9.

Which of the following are significant figures?

a)

Leading Zeroes

ex: 0.0023

b)

Non-zeroes

ex: 241

c)

Captive Zeroes

ex: 30002

d)

Zeroes after Decimals

ex: 0.800

10.

How many significant figures are in 0.00340?

a)

5

b)

3

c)

2

d)

6

11.

How many significant figures are in 2.40007 x $10^{-3}$ ?

a)

3

b)

2

c)

6

d)

5

12.

Round 0.24503 to 2 significant figures.

a)

0.24

b)

0.25

c)

0.30

d)

0.3

13.

Round 405930 to 2 significant figures.

a)

410,000

b)

41,000

c)

40,500

d)

405,000

14.

Which of the following is NOT a chemical property?

a)

Bonding

b)

Boiling Point

c)

Reactivity

d)

Oxidation

15.

Which of the following is a chemical property?

a)

Flammability

b)

Boiling Point

c)

Malleability

d)

Melting Point

16.

Which of the following is a physical property?

a)

Oxidation

b)

Ductility

c)

Flammability

d)

Reactivity

17.

Which of the following is NOT a physical property?

a)

Malleability

b)

Luster

c)

Color

d)

Flammability

18.

Which of the following is a physical change?

a)

Melting ice

b)

Iron rusting

c)

Burning paper

d)

Molecules bonding

19.

Which of the following is a chemical change?

a)

Melting ice

b)

Iron rusting

c)

Cutting paper

d)

Mushing playdoh

20.

Melting and Boiling Point are

a)

Chemical Changes

b)

Chemical Properties

c)

Physical Changes

d)

Physical Properties

21.

Intensive physical properties are...

a)

Dependent on the amount of matter.

b)

Independent of the chemical properties.

c)

Independent of the amount of matter.

d)

Dependent on the number of atoms.

22.

Extensive physical properties are...

a)

Independent of the chemical reactions.

b)

Dependent of the amount of matter.

c)

Independent of the amount of matter.

d)

Dependent on chemical reactions.

23.

Melting and boiling point are ....

a)

Extensive chemical properties

b)

Intensive chemical properties

c)

Intensive physical properties

d)

Extensive physical properties

24.

Color and luster are

a)

Extensive chemical properties

b)

Intensive chemical properties

c)

Extensive physical properties

d)

Intensive physical properties

25.

Mass and volume are...

a)

Extensive physical properties

b)

Intensive physical properties

c)

Extensive chemical properties

d)

Intensive chemical properties

26.

Density is an...

a)

Extensive physical property

b)

Intensive physical property

c)

Extensive chemical property

d)

Intensive chemical property

27.

Which state of matter has the most kinetic energy?

a)

Solids

b)

Liquids

c)

Gases

28.

Which state of matter is the most easily compressed (smushed)?

a)

Solids

b)

Liquids

c)

Gases

29.

Which state of matter has particles that are tightly packed together?

a)

Solids

b)

Liquids

c)

Gases

30.

Which state of matter has particles that 'flow' past each other?

a)

Solids

b)

Liquids

c)

Gases

31.

Which state of matter has the least amount of kinetic energy?

a)

Solids

b)

Liquids

c)

Gases

32.

Name the phase change labeled Number 1.

a)

Sublimation

b)

Condensation

c)

Deposition

d)

Vaporization

33.

Name the phase change labeled Number 2.

a)

Sublimation

b)

Condensation

c)

Deposition

d)

Vaporization

34.

Name the phase change labeled Number 3.

a)

Sublimation

b)

Vaporization

c)

Condensation

d)

Melting

35.

Name the phase change labeled Number 4.

a)

Deposition

b)

Condensation

c)

Freezing

d)

Vaporization

36.

Name the phase change labeled Number 5.

a)

Deposition

b)

Melting

c)

Freezing

d)

Vaporization

37.

Name the phase change labeled Number 6.

a)

Freezing

b)

Deposition

c)

Melting

d)

Vaporization

38.

Identify if this is an element, compound, or mixture.

a)

Elements

b)

Compounds

c)

Mixture of Elements

d)

Mixture of Compounds

39.

Identify if this is an element, compound, or mixture.

a)

Elements

b)

Compounds

c)

Mixture of Elements

d)

Mixture of Elements and Compounds

40.

Identify if this is an element, compound, or mixture.

a)

Elements

b)

Compounds

c)

Mixture of Elements

d)

Mixture of Elements and Compounds

41.

Identify if this is an element, compound, or mixture.

a)

Compounds

b)

Elements

c)

Mixture of Compounds

d)

Mixture of Elements

42.

Identify if this is an element, compound, or mixture.

a)

Mixture of Elements

b)

Elements

c)

Mixture of Compounds

d)

Compounds

43.

Identify if this is an element, compound, or mixture.

a)

Elements

b)

Mixture of Elements

c)

Compounds

d)

Mixture of Compounds

44.

Identify if this is an element, compound, or mixture.

a)

Mixture of Elements

b)

Mixture of Compounds

c)

Mixture of Elements and Compounds

d)

Compounds

45.

Identify if this is an element, compound, or mixture.

a)

Elements

b)

Compounds

c)

Mixture of Elements

d)

Mixture of Compounds

46.

Identify if this is an element, compound, or mixture.

a)

Elements

b)

Mixture of Elements

c)

Compounds

d)

Mixture of Compounds

47.

Which scientist used a cathode ray tube to discover the electron?

a)

Bohr

b)

Rutherford

c)

Thompson

d)

Schrodinger

48.

Which scientist stated that electrons could be found in energy levels that orbit the nucleus like planets?

a)

Democritus

b)

Rutherford

c)

Thompson

d)

Bohr

49.

Which scientist stated that electrons are located in a 'cloud' around the nucleus?

a)

Dalton

b)

Democritus

c)

Rutherford

d)

Schrodinger

50.

Which scientist stated that all matter is made of 'atomos'?

a)

Dalton

b)

Democritus

c)

Rutherford

d)

Thompson

51.

Which scientist discovered the nucleus and protons using the gold foil experiment?

a)

Rutherford

b)

Thompson

c)

Dalton

d)

Bohr

52.

Which scientist came up with 4 ideas about atoms, including that all matter is made up of indivisible atoms.

a)

Democritus

b)

Rutherford

c)

Dalton

d)

Thompson

53.

What does atomic number equal?

a)

Number of Neutrons (n)

b)

Number of Electrons (e-)

c)

Number of Protons and Electrons (p+ + e-)

d)

Number of Protons (p+)

54.

What does mass number equal?

a)

Number of Neutrons (n)

b)

Number of Electrons (e-)

c)

Number of Protons and Neutrons (p+ + n)

d)

Number of Protons (p+)

55.

If an element is neutral, then it has the same number of ...

a)

Protons (p+) and Electrons (e-)

b)

Protons (p+) and Neutrons (n)

c)

Neutrons (n) and Electrons (e-)

d)

Electrons (e-) and Positrons (p++)

56.

Isotopes have a different number of ....

a)

Protons (p+)

b)

Electrons (e-)

c)

Neutrons (n)

d)

Charge (+/-)

57.

Ions have a different number of ...

a)

Electrons (e-)

b)

Neutrons (n)

c)

Protons (p+)

d)

Atoms

58.

Which part of this image represents the atomic number?

a)

Au

b)

Gold

c)

196.967

d)

79

59.

Which part of this image represents the element symbol?

a)

Au

b)

Gold

c)

196.967

d)

79

60.

Which part of this image represents the number of protons?

a)

Au

b)

Gold

c)

196.967

d)

79

61.

Which part of this image represents the average atomic mass?

a)

Au

b)

Gold

c)

196.967

d)

79

62.

What would the mass number for this element be?

a)

79

b)

80

c)

196.967

d)

197

63.

How many neutrons would this element have?

a)

79

b)

197

c)

118

d)

80

64.

How many electrons would this element have?

a)

79

b)

197

c)

118

d)

80

65.

How many protons does this element have?

a)

6

b)

12.011

c)

12

d)

7

66.

How many electrons does this element have?

a)

6

b)

12.011

c)

12

d)

7

67.

How many neutrons does this element have?

a)

12

b)

12.011

c)

6

d)

7

68.

What is the mass number of this element?

a)

12

b)

12.011

c)

6

d)

7

69.

What is the atomic number of this element?

a)

12

b)

12.011

c)

6

d)

7

70.

What is the average atomic mass of this element?

a)

12

b)

12.011

c)

6

d)

7

71.

Which number here represents the atomic number?

a)

23

b)

11

c)

12

d)

34

72.

Which number here represents the mass number?

a)

23

b)

11

c)

12

d)

34

73.

Which number here represents the number of protons?

a)

23

b)

11

c)

12

d)

34

74.

Which number here represents the number of neutrons?

a)

23

b)

12

c)

11

d)

34

75.

What is the charge of this element?

a)

0

b)

+1

c)

-1

d)

+2

76.

Which number here represents the average atomic mass?

a)

39.96259098

b)

39.96

c)

40

d)

20

77.

Which number here represents the mass number?

a)

39.96259098

b)

39.96

c)

40

d)

20

78.

Which number here represents the atomic number?

a)

39.96259098

b)

39.96

c)

40

d)

20

79.

Which number here represents the number of neutrons?

a)

39.96259098

b)

39.96

c)

40

d)

20

80.

Which number here represents the number of protons and neutrons?

a)

39.96259098

b)

39.96

c)

40

d)

20

81.

Which number here would you round to make the mass number?

a)

39.96

b)

40

c)

20

82.

How many electrons does this element have?

a)

40

b)

20

c)

39.96

d)

41

83.

How many electrons does this element have?

a)

40

b)

20

c)

39.96

d)

41

84.

What is the mass number of this element?

a)

26

b)

59

c)

3

d)

33

85.

What is the atomic number of this element?

a)

26

b)

59

c)

3

d)

33

86.

What is the charge of this element?

a)

26

b)

59

c)

3+

d)

3-

87.

How many electrons does this element have?

a)

26

b)

59

c)

29

d)

23

88.

How many protons does this element have?

a)

26

b)

59

c)

29

d)

23

89.

How many neutrons does this element have?

a)

26

b)

59

c)

33

d)

23

90.

What subatomic particle is changed in isotopes?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Protons and Electrons

91.

What subatomic particle is changed in ions?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Protons and Electrons

92.

What subatomic particle is changed in ions?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Protons and Electrons

93.

Cations are ________ ions formed by metals ______ electrons.

a)

Positive

Gaining

b)

Negative

Gaining

c)

Positive

Losing

d)

Negative

Losing

94.

Anions are ________ ions formed by nonmetals ______ electrons.

a)

Positive

Gaining

b)

Negative

Gaining

c)

Positive

Losing

d)

Negative

Losing

95.

Which form of radioactive decay penetrates the most and is the most dangerous?

a)

Alpha

b)

Beta

c)

Gamma

96.

Which form of radioactive decay penetrates the least and is the least dangerous?

a)

Alpha

b)

Beta

c)

Gamma

97.

What would be the product of the alpha decay of Uranium-238

$_{92}^{238\ }U\ \rightarrow\ _2^4\ He\ +\$

a)

$_{90}^{238}\ U$

b)

$_{94}^{242}\ U$

c)

$_{92}^{234}\ Th$

d)

$_{90}^{234}\ Th$

98.

What would be the product of the alpha decay of Plutonium-239?

$_{94}^{239\ }Pu\ \rightarrow\ _2^4\ He\ +\$

a)

$_{92}^{235}\ U$

b)

$_{96}^{235}\ U$

c)

$_{92}^{239}\ U$

d)

$_{96}^{235}\ Cm$

99.

What would be the product of the beta decay of Carbon-14?

$_6^{14\ }C\ \rightarrow\ _{-1}^0\ e\ +\$

a)

$_5^{14}\ B$

b)

$_6^{14}\ C$

c)

$_7^{14}\ N$

d)

$_{-1}^{14}\ H$

100.

What would be the product of the beta decay of Carbon-14?

$_{19}^{40\ }K\ \rightarrow\ _{-1}^0\ e\ +\$

a)

$_{18}^{40}\ Ar$

b)

$_{20}^{40}\ Ca$

c)

$_{19}^{40}\ K$

d)

$_{20}^{40}\ Ca$

101.

What would be the product of the beta decay of Carbon-14?

$_{19}^{40\ }K\ \rightarrow\ _{-1}^0\ e\ +\$

a)

$_{18}^{40}\ Ar$

b)

$_{20}^{40}\ Ca$

c)

$_{19}^{40}\ K$

d)

$_{20}^{40}\ Ca$

102.

What form of radioactive decay is represented here?

$_{92}^{238\ }U\ \rightarrow\ _{93}^{238}\ Np\ +\$

a)

Alpha

b)

Beta

c)

Gamma

103.

What does Group Number represent on the Periodic Table?

a)

The reactivity of an element

b)

The number of valence electrons

c)

The energy levels

d)

The family of elements

104.

What does Period Number on the Periodic Table represent?

a)

The orbitals of electrons

b)

The energy levels

c)

The number of valence electrons

d)

The number of neutrons

105.

What scientist first attempted to arrange the Periodic Table by atomic mass?

a)

Democritus

b)

Mendeleev

c)

Moseley

d)

Thompson

106.

What scientist finalized the arrangement of the Periodic Table using atomic number?

a)

Mendeleev

b)

Dalton

c)

Schrodinger

d)

Moseley

107.

What family is located in Group 1?

a)

Alkaline Earth Metals

b)

Transition Metals

c)

Alkali Metals

d)

Halogens

108.

What family is located in Group 18?

a)

Alkali Metalsx

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble Gases

109.

What family is located in Group 2?

a)

Alkali Metalsx

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble Gases

110.

What family of elements is located in the top row of f-block?

a)

Lanthanides

b)

Alkali Metals

c)

Transition Metals

d)

Actinides

111.

What family is located in Group 17?

a)

Alkali Metalsx

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble Gases

112.

What family of elements is located in the top row of f-block?

a)

Lanthanides

b)

Alkali Metals

c)

Transition Metals

d)

Actinides

113.

Where are the metalloids located on the Periodic Table?

a)

Left Side

b)

Middle

c)

Zigzag

d)

Right Side

114.

Where are the metals located on the Periodic Table?

a)

Left Side

b)

Middle

c)

Zigzag

d)

Right Side

115.

Where are the nonmetals located on the Periodic Table?

a)

Left Side

b)

Middle

c)

Zigzag

d)

Right Side

116.

What is the name of the red block on the Periodic Table?

a)

s-block

b)

d-block

c)

p-block

d)

f-block

117.

What is the name of the blue block on the Periodic Table?

a)

s-block

b)

d-block

c)

p-block

d)

f-block

118.

What is the name of the green block on the Periodic Table?

a)

s-block

b)

d-block

c)

p-block

d)

f-block

119.

What is the name of the yellow block on the Periodic Table?

a)

s-block

b)

d-block

c)

p-block

d)

f-block

120.

How many electrons can be held by s-block (spots)?

a)

2

b)

10

c)

6

d)

14

121.

How many electrons can be held by f-block (spots)?

a)

2

b)

10

c)

6

d)

14

122.

How many electrons can be held by d-block (spots)?

a)

2

b)

10

c)

6

d)

14

123.

How many electrons can be held by p-block (spots)?

a)

2

b)

10

c)

6

d)

14

124.

Atomic radius ________ down a group and _______ across a period.

a)

Increases

b)

Increases

Decreases

c)

Decreases

d)

Decreases Increases

125.

Which of these elements has the largest atomic radius?

a)

Fr

b)

F

c)

O

d)

Ca

126.

Which one of these elements has the smallest atomic radius?

a)

Fe

b)

Rb

c)

Se

d)

S

127.

Ionization energy ________ down a group and _______ across a period.

a)

Increases

b)

Increases

Decreases

c)

Decreases

d)

Decreases Increases

128.

Which of these elements has the smallest ionization energy?

a)

Fr

b)

F

c)

O

d)

Ca

129.

Which one of these elements has the greatest ionization energy?

a)

Fe

b)

Rb

c)

Se

d)

S

130.

Electronegativity ________ down a group and _______ across a period.

a)

Increases

b)

Increases

Decreases

c)

Decreases

d)

Decreases Increases

131.

Which one of these elements is the most electronegative?

a)

B

b)

Mg

c)

F

d)

He

132.

Reactivity in METALS ________ down a group and _______ across a period.

a)

Increases

b)

Increases

Decreases

c)

Decreases

d)

Decreases Increases

133.

Reactivity in NONMETALS ________ down a group and _______ across a period.

a)

Increases

b)

Increases

Decreases

c)

Decreases

d)

Decreases Increases

134.

How are the sublevels of energy levels represented on the Periodic Table?

a)

Block

b)

Period Number

c)

Atomic Number

d)

Group Number

135.

How many electrons can one orbital hold?

a)

1000000000

b)

6

c)

10

d)

2

136.

What is the electron configuration of Lithium?

a)

$1s^2$

b)

$1s^22s^1$

c)

$1s^21p^1$

d)

$1s^3$

137.

What is the electron configuration of Potassium?

a)

$1s^22s^22p^63s^23p^64s^1$

b)

$1s^22s^23s^24s^12p^63p^6$

c)

$4s^1$

d)

$1s^22s^22p^{10}3s^23p^{10}4s^1$

138.

What is the electron configuration of Potassium?

$1s^22s^22p^63s^23p^64s^1$

a)

$1$

b)

2

c)

3

d)

4

139.

How many valence electrons does Neon have?

$1s^22s^22p^6$

a)

2

b)

8

c)

6

d)

10

140.

How many total electrons does Neon have?

$1s^22s^22p^6$

a)

2

b)

8

c)

6

d)

10

141.

What would the Noble Gas configuration for Silver?

a)

[Kr] $5s^2$

b)

[Xe] $5s^2$

c)

[Kr] $5s^24d^{10}$

d)

[Xe] $5s^25d^{10}$

142.

Ionic bonding happens between a ________ and a __________.

a)

Nonmetal

b)

Nonmetal

Metal

c)

Metal

143.

Covalent bonding happens between a ________ and a __________.

a)

Nonmetal

b)

Nonmetal

Metal

c)

Metal

144.

Metallic bonding happens between a ________ and a __________.

a)

Nonmetal

b)

Nonmetal

Metal

c)

Metal

145.

Metallic bonding involves a _____ of electrons

a)

Sea

b)

Transfer

c)

Sharing

146.

Ionic bonding involves a _____ of electrons

a)

Sea

b)

Transfer

c)

Sharing

147.

Covalent bonding involves a _____ of electrons

a)

Sea

b)

Transfer

c)

Sharing

148.

What would the name of $N_2Cl_3$ ?

a)

Nitrogen trihydride

b)

Nitrogen trichloride

c)

Dinitrogen trihydride

d)

Dinitrogen trichloride

149.

How would you name $B_2Si$ ?

a)

Boron silicon

b)

Boron silicide

c)

Diboron silicide

d)

Boride silicide

150.

How would you name $N_2O_5$ ?

a)

Nitrogen oxide

b)

Dinitrogen pentoxide

c)

Dinitrogen pentaoxygen

d)

Nitrogen pentoxide

151.

How would you name $P_4S_3$ ?

a)

Phosphorous trisulfide

b)

Tetraphosphide sulfur

c)

Tetraphosphorous sulfide

d)

Tetraphosphorus trisulfide

152.

Write the formula for triphosphorus octabromide.

a)

$P_3Br_8$

b)

$P_3Br_9$

c)

$P_2Br_8$

d)

$PBr_8$

153.

Write the formula for hexaboron monosilicide.

a)

$B_9Si$

b)

$B_6Si$

c)

$B_5Si$

d)

$B_7Si$

154.

Write the formula of iodine pentafluoride.

a)

$I_1F_5$

b)

$IF_5$

c)

$IF_7$

d)

$IF_6$

155.

Write the formula for phosphorus triiodide.

a)

$PI_2$

b)

$PI_{ }$

c)

$PI_3$

d)

$PI_4$

156.

Write the formula for hydrogen monoiodide.

a)

$HSi$

b)

$HI_2$

c)

$H_1I_1$

d)

HI

157.

Draw the Lewis Structure for PCl3.

158.

Draw the Lewis Structure for SiF4.

159.

Polar covalent bonds have _______ sharing of electrons.

a)

Equal

b)

Unequal

160.

Nonpolar covalent bonds have _______ sharing of electrons.

a)

Equal

b)

Unequal

161.

Select the polar molecules from below.

a)

b)

c)

d)

162.

Select the nonpolar molecules from below.

a)

b)

c)

d)

163.

Which compound below is a molecule (covalent bond)?

a)

$CaCl_2$

b)

$NaBr$

c)

$CO_2$

d)

$FeBr_3$

164.

Which compound below is ionic?

a)

$NaCl$

b)

$HBr_3$

c)

$CO_2$

d)

$N_2Cl_5$

165.

Draw the Lewis Structure and predict the molecule shape of $CH_4$ .

a)

Trigonal pyramidal

b)

Linear

c)

Tetrahedral

d)

Trigonal Planar

166.

Draw the Lewis Structure to predict the molecule shape of $SO_2$ .

a)

Tetrahedral

b)

Bent

c)

Linear

d)

Trigonal planar

167.

How many electrons are in a single bond?

a)

1

b)

2

c)

4

d)

6

168.

How many electrons are in a double bond?

a)

1

b)

2

c)

4

d)

6

169.

How many electrons are in a triple bond?

a)

1

b)

2

c)

4

d)

6

170.

What two elements are the exceptions to the Octet Rule?

a)

Hydrogen

b)

Argon

c)

Helium

d)

Beryllium

171.

What is the Octet Rule?

a)

Elements want to have 8 energy levels.

b)

Elements want to have 8 total electrons.

c)

Elements want to have 8 valence electrons.

d)

Elements want to have 8 total bonds.

172.

How are you going to be successful on your finals this semester?

4 lines

Final Review 2022

Total questions: 172

Worksheet time: 2hrs 42mins