Free Printable More Practice for unit 1

1.

Which subatomic particles are responsible for atomic mass?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Positrons

2.

Which subatomic particles are responsible for the charge of an atom?

a)

Electrons

b)

Neutrons

c)

Nucleus

d)

Protons

3.

Which of the follow elements are in the Alkaline Earth metals?

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

4.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

5.

Which element's electron configuration is 1s² 2s² ...7s² 5f¹⁴ 6d⁹?

a)

Ag

b)

Cu

c)

Au

d)

Rg

6.

Match the element to the group name?

a)

Transition Metal

1.

Iron

b)

Halogen

2.

Bromine

c)

Alkali Metal

3.

Sodium

d)

Noble Gas

4.

Argon

e)

Alkaline Earth Metal

5.

Calcium

7.

Match the element to the group name?

a)

Transition Metal

1.

Tungsten

b)

Halogen

2.

Chlorine

c)

Alkali Metal

3.

Potassium

d)

Noble Gas

4.

Krypton

e)

Alkaline Earth Metal

5.

Magnesium

8.

Match the number of valence electrons to the correct element

a)

Oxygen

1.

6

b)

Chlorine

2.

7

c)

Phosphorus

3.

5

d)

Magnesium

4.

2

e)

Sodium

5.

1

9.

Match the number of valence electrons with the correct element

a)

Sulfur

1.

6

b)

Bromine

2.

7

c)

Aluminum

3.

3

d)

Calcium

4.

2

e)

Argon

5.

8

10.

Which of the following atoms could be represented by the orbital diagram above?

a)

Ar

b)

O^2-

c)

F^1-

d)

K¹⁺

e)

Ga³⁺

11.

What is the electron configuration for Krypton?

a)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s²3d¹⁰ 4p⁶

b)

[Ar] 4s² 3d¹⁰ 4p⁶

c)

1s² 2s² 3s² 2p⁶4s² 3p⁶ 4p⁶ 3d¹⁰

d)

[Ne] 4s² 3d¹⁰ 4p⁶

12.

Reorder the following from the smallest atomic radius to the largest atomic radius.

a)

Fluorine

b)

Nitrogen

c)

Sulfur

d)

Copper

e)

Francium

1)

2)

3)

4)

5)

13.

Reorder the following from the smallest electronegativity to the largest electronegativity.

a)

Boron

b)

Carbon

c)

Nitrogen

d)

Oxygen

e)

Fluorine

1)

2)

3)

4)

5)

14.

How many valence electrons does Helium have?

a)

1

b)

2

c)

6

d)

7

e)

4

15.

The Alkaline earth metals need to lose how many electrons to look like the noble gases?

a)

2

b)

3

c)

1

d)

4

16.

Who discovered the Electron?

a)

Thompson

b)

Rutherford

c)

Dalton

d)

Bohr

17.

Who discovered the nucleus?

a)

Dalton

b)

Bohr

c)

Thompson

d)

Rutherford

18.

What was the problem with Rutherford's model?

a)

Electrons freely floating around the nucleus

b)

Nucleus was a small dense positively charges object

c)

The atom was made up of mostly empty space

d)

Most of the atom's mass must be in the nucleus.

19.

Who discovered the Energy levels in the atom?

a)

Schodinger

b)

Bohr

c)

Rutherford

d)

Thompson

20.

Who mathematically predicted the electron clouds?

a)

Bohr

b)

Thompson

c)

Schrodinger

d)

Dalton

21.

How many neutrons would Ca-45 have?

a)

45

b)

5

c)

20

d)

25

22.

How many electrons would Al³⁺ have?

a)

10

b)

13

c)

16

d)

24

e)

12

23.

How many electrons does Zn¹⁺have?

a)

30

b)

31

c)

29

d)

65

24.

How many electrons does S^2- have?

a)

19

b)

18

c)

16

d)

17

25.

What does the electron configuration of Vandium-53 end with?

a)

3d⁶

b)

3p⁶

c)

3d³

d)

3p³

26.

Which of the following was the conclusion of the gold foil experiment by Rutherford

a)

Atom is mostly empty space

b)

Atom has a dense center

c)

The center is positively charged

d)

The center is negatively charged

e)

The atom is a solid sphere

27.

How many electrons does selenium need to complete the octet rule?

a)

1

b)

2

c)

3

d)

4

e)

5

28.

Which ways do the atomic radius decrease on the periodic table?

a)

Down

b)

Up

c)

Left

d)

right

29.

Which way does the electron affinity decrease across the periodic table?

a)

up

b)

down

c)

left

d)

right

30.

Which families would be considered to be the most reactive?

a)

Alkali metals

b)

alkaline earth metals

c)

Oxygen group

d)

Halogens

e)

Noble gases

31.

Which family would be considered the least reactive?

a)

Noble gases

b)

Oxygen group

c)

Lanthanide series

d)

Transition metals

e)

Alkaline earth metals

32.

How many neutrons would Rutherium-105 have?

a)

44

b)

61

c)

105

d)

78

33.

How many neutrons would be in the isotope ⁹¹₃₉Y?

a)

52

b)

39

c)

91

d)

55

34.

If Copper-65 naturally occurred 55% of the time and Copper-63 naturally occurred 25% of the time and Copper-61 occurred 20 % of the time, What would Copper's average atomic weight be calculated as?

a)

63 g/mol

b)

63.7 g/mol

c)

63.1 g/mol

d)

63.5 g/mol

35.

If Tin-120 occurred at 73.6% of the time and Tin-116 occurred at 26.4% of the time, What would be Tin's average atomic weight?

a)

120.144 g/mol

b)

118.71 g/mol

c)

118.944 g/mol

d)

115.753 g/mol

36.

What did Bohr base his atomic model on?

a)

Electrons emitting light when they jumped to higher energy levels

b)

Electrons emitting light when they jumped to lower energy levels

c)

The amount, or type, of light produced when electrons jumped multiple energy levels

d)

He concluded that each energy level had an set amount of energy that electrons had absorb and emit to change to that energy level

37.

Aluminum would have to (a) 3 electrons to be stable.

38.

What did Rutherford use to design a new model of the atom?

a)

The amount of energy an electron needs to jump to the higher energy levels

b)

The bombardment of Beryllium by alpha particles

c)

Gold foil and alpha particles

d)

Cathode ray tubes Maxwell's equations

e)

Maxwell's equations

39.

What did Chadwick use to design a new model of the atom?

a)

The amount of energy an electron needs to jump to the higher energy levels

b)

The bombardment of Beryllium by alpha particles

c)

Gold foil and alpha particles

d)

Cathode ray tubes Maxwell's equations

e)

Maxwell's equations

40.

How many protons would Al- 27 have?

a)

13

b)

27

c)

14

d)

26

e)

12

41.

How many electrons does O^2- have

a)

6

b)

8

c)

10

d)

12

42.

What does electron configuration of P^3- end with?

a)

3d⁶

b)

3p⁶

c)

3d³

d)

3p³

43.

Which of the following was the conclusion of the gold foil experiment by Rutherford

a)

Atom is mostly empty space

b)

Atom has a dense center

c)

The center is positively charged

d)

The center is negatively charged

e)

The atom is a solid sphere

44.

How many electrons does C need to complete the octet rule?

a)

1

b)

2

c)

3

d)

4

e)

5

45.

Which ways do the atomic radius increase on the periodic table?

a)

Down

b)

Up

c)

Left

d)

right

46.

Which way does the electron affinity increase across the periodic table?

a)

up

b)

down

c)

left

d)

right

47.

Which families would be considered to be the most reactive?

a)

Alkali metals

b)

alkaline earth metals

c)

Oxygen group

d)

Halogens

e)

Noble gases

48.

Which family would be considered the least reactive?

a)

Noble gases

b)

Carbon group

c)

Halogens

d)

Boron group

e)

Alkali metals

49.

How many neutrons would Carbon-14 have?

a)

14

b)

6

c)

12

d)

8

50.

How many neutrons would be in the isotope ²³⁶₉₂U?

a)

92

b)

236

c)

144

d)

146

51.

What is the section of the periodic table where elements have electrons in the d orbitals called?

a)

Transition metals

b)

Translation metals

c)

Transistor metals

d)

Translator metals

52.

Which of the following elements has 8 valence electrons?

a)

He

b)

Ne

c)

Ar

d)

F

e)

Cl

53.

Which of the following would have the biggest Atomic radius?

a)

K

b)

Cu

c)

Mg

d)

Fr

e)

Rb

54.

Which group needs only 2 electrons to complete the Octet rule?

a)

Carbon group

b)

Oxygen group

c)

Noble gases

d)

Lanthanide series

e)

Halogens

55.

How many electrons would the Alkaline earth metals need to lose to look like the noble gases?

a)

1

b)

2

c)

3

d)

4

e)

None, they have to gain electrons

56.

Who discovered the Electron?

a)

Thompson

b)

Rutherford

c)

Dalton

d)

Bohr

57.

Who discovered the nucleus?

a)

Dalton

b)

Bohr

c)

Thompson

d)

Rutherford

58.

Who discovered the Energy levels in the atom?

a)

Schodinger

b)

Bohr

c)

Rutherford

d)

Thompson

59.

Who mathematically predicted the electron clouds?

a)

Bohr

b)

Thompson

c)

Schrodinger

d)

Dalton

60.

How many neutrons would Ca-45 have?

a)

45

b)

5

c)

20

d)

25

61.

How many protons would Al- 27 have?

a)

13

b)

27

c)

14

d)

26

e)

12

62.

How many electrons does O^2- have

a)

6

b)

8

c)

10

d)

12

63.

Which subatomic particles are responsible for atomic mass?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Positrons

64.

Which subatomic particles are responsible for the charge of an atom?

a)

Electrons

b)

Neutrons

c)

Nucleus

d)

Protons

65.

Which of the follow elements are in the Alkali metals?

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

66.

Which of the following elements have 5 valence electrons?

a)

C

b)

N

c)

O

d)

Sb

e)

Pb

67.

Which element's electron configuration would end in 3d⁹?

a)

Ag

b)

Cu

c)

Au

d)

Rg

68.

What is the section of the periodic table where elements have electrons in the d orbitals called?

a)

Transition metals

b)

Translation metals

c)

Transistor metals

d)

Translator metals

69.

Which of the following elements has 8 valence electrons?

a)

He

b)

Ne

c)

Ar

d)

F

e)

Cl

70.

Which of the following atoms could be represented by the orbital diagram above?

a)

P^3-

b)

S^2-

c)

^Cl1-

d)

K¹⁺

e)

Ga³⁺

71.

Which of the following could be the electron configuration for an ion of Oxygen?

a)

1s²2s²2p⁶

b)

1s¹2s²2p⁶

c)

1s²2s²2p⁴

d)

1s²2s²2p⁵

72.

Which of the following has the smallest atomic radius?

a)

Cl

b)

F

c)

O

d)

Br

e)

Ar

73.

Which subatomic particles are responsible for atomic mass?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Positrons

74.

Which subatomic particles are responsible for the charge of an atom?

a)

Electrons

b)

Neutrons

c)

Nucleus

d)

Protons

75.

Which of the follow elements are in the Alkali metals?

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

76.

Which of the following elements have 5 valence electrons?

a)

C

b)

N

c)

O

d)

Sb

e)

Pb

77.

Which element's electron configuration would end in 3d⁹?

a)

Ag

b)

Cu

c)

Au

d)

Rg

78.

What is the section of the periodic table where elements have electrons in the d orbitals called?

a)

Transition metals

b)

Translation metals

c)

Transistor metals

d)

Translator metals

79.

Which of the following elements has 8 valence electrons?

a)

He

b)

Ne

c)

Ar

d)

F

e)

Cl

80.

Which of the following atoms could be represented by the orbital diagram above?

a)

P^3-

b)

O^2-

c)

Cl^1-

d)

K¹⁺

e)

Al³⁺

81.

Which of the following could be the electron configuration for an ion of Oxygen?

a)

1s²2s²2p⁶

b)

1s¹2s²2p⁶

c)

1s²2s²2p⁴

d)

1s²2s²2p⁵

82.

Which of the following has the smallest atomic radius?

a)

Cl

b)

F

c)

O

d)

Br

e)

Ar

83.

Which of the following would have the biggest Atomic radius?

a)

K

b)

Cu

c)

Mg

d)

Fr

e)

Rb

84.

Which group needs only 2 electrons to complete the Octet rule?

a)

Carbon group

b)

Oxygen group

c)

Noble gases

d)

Lanthanide series

e)

Halogens

85.

How many electrons would the Alkaline earth metals need to lose to look like the noble gases?

a)

1

b)

2

c)

3

d)

4

e)

None, they have to gain electrons

86.

Who discovered the Electron?

a)

Thompson

b)

Rutherford

c)

Dalton

d)

Bohr

87.

Who discovered the nucleus?

a)

Dalton

b)

Bohr

c)

Thompson

d)

Rutherford

88.

Who discovered the Energy levels in the atom?

a)

Schodinger

b)

Bohr

c)

Rutherford

d)

Thompson

89.

Who mathematically predicted the electron clouds?

a)

Bohr

b)

Thompson

c)

Schrodinger

d)

Dalton

90.

How many neutrons would Ca-45 have?

a)

45

b)

5

c)

20

d)

25

91.

How many protons would Al- 27 have?

a)

13

b)

27

c)

14

d)

26

e)

12

92.

How many electrons does O^2- have

a)

6

b)

8

c)

10

d)

12

93.

How many electrons does Na¹⁺ have?

a)

9

b)

10

c)

11

d)

12

94.

What does electron configuration of P^3- end with?

a)

3d⁶

b)

3p⁶

c)

3d³

d)

3p³

95.

Which of the following was the conclusion of the gold foil experiment by Rutherford

a)

Atom is mostly empty space

b)

Atom has a dense center

c)

The center is positively charged

d)

The center is negatively charged

e)

The atom is a solid sphere

96.

How many electrons does C need to complete the octet rule?

a)

1

b)

2

c)

3

d)

4

e)

5

97.

Which ways do the atomic radius increase on the periodic table?

a)

Down

b)

Up

c)

Left

d)

right

98.

Which way does the electron affinity increase across the periodic table?

a)

up

b)

down

c)

left

d)

right

99.

Which families would be considered to be the most reactive?

a)

Alkali metals

b)

alkaline earth metals

c)

Oxygen group

d)

Halogens

e)

Noble gases

100.

Which family would be considered the least reactive?

a)

Noble gases

b)

Carbon group

c)

Halogens

d)

Boron group

e)

Alkali metals

101.

How many neutrons would Carbon-14 have?

a)

14

b)

6

c)

12

d)

8

102.

How many neutrons would be in the isotope ²³⁶₉₂U?

a)

92

b)

236

c)

144

d)

146

103.

Which of the follow elements are in the Alkaline Earth metals?

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

104.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

105.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

106.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

107.

Which element's electron configuration would end in 6d⁹?

a)

Ag

b)

Cu

c)

Au

d)

Rg

108.

What is the section of the periodic table where elements have electrons in the d orbitals called?

(a)

109.

Name an element has 6 valence electrons?

(a)

110.

Which of the following atoms could be represented by the orbital diagram above?

a)

Ar

b)

O^2-

c)

F^1-

d)

K¹⁺

e)

Ga³⁺

111.

How many electrons would Al³⁺ have?

a)

10

b)

13

c)

16

d)

24

e)

12

112.

How many electrons does Zn¹⁺have?

a)

30

b)

31

c)

29

d)

65

113.

How many electrons does S^2- have?

a)

19

b)

18

c)

16

d)

17

114.

What does the electron configuration of Vandium-53 end with?

a)

3d⁶

b)

3p⁶

c)

3d³

d)

3p³

115.

How many electrons does selenium need to complete the octet rule?

a)

1

b)

2

c)

3

d)

4

e)

5

116.

Which ways do the atomic radius decrease on the periodic table?

a)

Down

b)

Up

c)

Left

d)

right

117.

Which way does the electron affinity decrease across the periodic table?

a)

up

b)

down

c)

left

d)

right

118.

Which family would be considered the least reactive?

a)

Noble gases

b)

Oxygen group

c)

Lanthanide series

d)

Transition metals

e)

Alkaline earth metals

119.

How many neutrons would Rutherium-105 have?

a)

44

b)

61

c)

105

d)

78

120.

How many neutrons would be in the isotope ⁹¹₃₉Y?

a)

52

b)

39

c)

91

d)

55

121.

If Copper-65 naturally occurred 55% of the time and Copper-63 naturally occurred 25% of the time and Copper-61 occurred 20 % of the time, What would Copper's average atomic weight be calculated as?

a)

63 g/mol

b)

63.7 g/mol

c)

63.1 g/mol

d)

63.5 g/mol

122.

If Tin-120 occurred at 73.6% of the time and Tin-116 occurred at 26.4% of the time, What would be Tin's average atomic weight?

a)

120.144 g/mol

b)

118.71 g/mol

c)

118.944 g/mol

d)

115.753 g/mol

123.

What did Bohr base his atomic model on?

a)

Electrons emitting light when they jumped to higher energy levels

b)

Electrons emitting light when they jumped to lower energy levels

c)

The amount, or type, of light produced when electrons jumped multiple energy levels

d)

He concluded that each energy level had an set amount of energy that electrons had absorb and emit to change to that energy level

124.

Aluminum would have to (a) 3 electrons to be stable.

125.

Which subatomic particles are responsible for atomic mass?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Positrons

126.

Which subatomic particles are responsible for the charge of an atom?

a)

Electrons

b)

Neutrons

c)

Nucleus

d)

Protons

127.

Which of the follow elements are in the Alkaline Earth metals?

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

128.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

129.

Which element's electron configuration is 1s² 2s² ...7s² 5f¹⁴ 6d⁹?

a)

Ag

b)

Cu

c)

Au

d)

Rg

130.

Match the element to the group name?

a)

Transition Metal

1.

Iron

b)

Halogen

2.

Bromine

c)

Alkali Metal

3.

Sodium

d)

Noble Gas

4.

Argon

e)

Alkaline Earth Metal

5.

Calcium

131.

Match the element to the group name?

a)

Transition Metal

1.

Tungsten

b)

Halogen

2.

Chlorine

c)

Alkali Metal

3.

Potassium

d)

Noble Gas

4.

Krypton

e)

Alkaline Earth Metal

5.

Magnesium

132.

Match the number of valence electrons to the correct element

a)

Oxygen

1.

6

b)

Chlorine

2.

7

c)

Phosphorus

3.

5

d)

Magnesium

4.

2

e)

Sodium

5.

1

133.

Match the number of valence electrons with the correct element

a)

Sulfur

1.

6

b)

Bromine

2.

7

c)

Aluminum

3.

3

d)

Calcium

4.

2

e)

Argon

5.

8

134.

Which of the following atoms could be represented by the orbital diagram above?

a)

Ar

b)

O^2-

c)

F^1-

d)

K¹⁺

e)

Ga³⁺

135.

Match the following atoms with the correct Orbital diagram.

a)

1.

Magnesium

b)

2.

Neon

c)

3.

Oxygen

d)

4.

Sodium

e)

5.

Carbon

136.

Which of the following orbital diagrams is correct for Aluminum?

a)

b)

c)

d)

137.

What is the electron configuration for Krypton?

a)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s²3d¹⁰ 4p⁶

b)

[Ar] 4s² 3d¹⁰ 4p⁶

c)

1s² 2s² 3s² 2p⁶4s² 3p⁶ 4p⁶ 3d¹⁰

d)

[Ne] 4s² 3d¹⁰ 4p⁶

138.

Reorder the following from the smallest atomic radius to the largest atomic radius.

a)

Fluorine

b)

Nitrogen

c)

Sulfur

d)

Copper

e)

Francium

1)

2)

3)

4)

5)

139.

Reorder the following from the smallest atomic radius to the largest atomic radius.

a)

Nitrogen

b)

Phosphorus

c)

Arsenic

d)

Antimony

e)

Bismuth

1)

2)

3)

4)

5)

140.

Reorder the following from the smallest electronegativity to the largest electronegativity.

a)

Boron

b)

Carbon

c)

Nitrogen

d)

Oxygen

e)

Fluorine

1)

2)

3)

4)

5)

141.

Reorder the following that has the least ionization energy to the most ionization energy.

a)

Astatine

b)

Bromine

c)

Iodine

d)

Chlorine

e)

Fluorine

1)

2)

3)

4)

5)

142.

Reorder the following that has the least ionization energy to the most ionization energy.

a)

Boron

b)

Carbon

c)

Oxygen

d)

Fluorine

e)

Neon

1)

2)

3)

4)

5)

143.

How many valence electrons does Helium have?

a)

1

b)

2

c)

6

d)

7

e)

4

144.

The Alkaline earth metals need to lose how many electrons to look like the noble gases?

a)

2

b)

3

c)

1

d)

4

145.

How many electrons do the alkali metals need to lose to look like noble gases?

a)

2

b)

3

c)

1

d)

4

146.

Who discovered the Electron?

a)

Thompson

b)

Rutherford

c)

Dalton

d)

Bohr

147.

Who disproved Dalton's theory of the atom saying that all atoms must have positive and negative charges?

a)

Thompson

b)

Rutherford

c)

Dalton

d)

Bohr

148.

Who discovered the nucleus?

a)

Dalton

b)

Bohr

c)

Thompson

d)

Rutherford

149.

What was the problem with Rutherford's model?

a)

Electrons freely floating around the nucleus

b)

Nucleus was a small dense positively charges object

c)

The atom was made up of mostly empty space

d)

Most of the atom's mass must be in the nucleus.

150.

Who discovered the Energy levels in the atom?

a)

Schodinger

b)

Bohr

c)

Rutherford

d)

Thompson

151.

Who mathematically predicted the electron clouds?

a)

Bohr

b)

Thompson

c)

Schrodinger

d)

Dalton

152.

How many neutrons would Ca-45 have?

a)

45

b)

5

c)

20

d)

25

153.

How many electrons would Al³⁺ have?

a)

10

b)

13

c)

16

d)

24

e)

12

154.

How many electrons does Zn¹⁺have?

a)

30

b)

31

c)

29

d)

65

155.

How many electrons does S^2- have?

a)

19

b)

18

c)

16

d)

17

156.

What does the electron configuration of Vandium-53 end with?

a)

3d⁶

b)

3p⁶

c)

3d³

d)

3p³

157.

Which of the following was the conclusion of the gold foil experiment by Rutherford

a)

Atom is mostly empty space

b)

Atom has a dense center

c)

The center is positively charged

d)

The center is negatively charged

e)

The atom is a solid sphere

158.

How many electrons does selenium need to complete the octet rule?

a)

1

b)

2

c)

3

d)

4

e)

5

159.

What is the octet rule?

a)

It is the number of valence electrons it takes to be an ion

b)

It is the number of valence electrons that will make most atoms stable.

c)

It is the number of neutrons in a nucleus to match oxygen

d)

It is a rule of 8 atoms that are stable.

160.

Which ways do the atomic radius decrease on the periodic table?

a)

Down

b)

Up

c)

Left

d)

right

161.

Which way does the electron affinity decrease across the periodic table?

a)

up

b)

down

c)

left

d)

right

162.

Which families would be considered to be the most reactive?

a)

Alkali metals

b)

alkaline earth metals

c)

Oxygen group

d)

Halogens

e)

Noble gases

163.

Which family would be considered the least reactive?

a)

Noble gases

b)

Oxygen group

c)

Lanthanide series

d)

Transition metals

e)

Alkaline earth metals

164.

How many neutrons would Rutherium-105 have?

a)

44

b)

61

c)

105

d)

78

165.

How many neutrons would be in the isotope ⁹¹₃₉Y?

a)

52

b)

39

c)

91

d)

55

166.

If Copper-65 naturally occurred 55% of the time and Copper-63 naturally occurred 25% of the time and Copper-61 occurred 20 % of the time, What would Copper's average atomic weight be calculated as?

a)

63 g/mol

b)

63.7 g/mol

c)

63.1 g/mol

d)

63.5 g/mol

167.

If Tin-120 occurred at 73.6% of the time and Tin-116 occurred at 26.4% of the time, What would be Tin's average atomic weight?

a)

120.144 g/mol

b)

118.71 g/mol

c)

118.944 g/mol

d)

115.753 g/mol

168.

What did Bohr base his atomic model on?

a)

Electrons emitting light when they jumped to higher energy levels

b)

Electrons emitting light when they jumped to lower energy levels

c)

The amount, or type, of light produced when electrons jumped multiple energy levels

d)

He concluded that each energy level had an set amount of energy that electrons had absorb and emit to change to that energy level

169.

Match the following Elements with the Family or group they are in

a)

Chlorine

1.

Halogens

b)

Phosphorus

2.

Nitrogen Group

c)

Selenium

3.

Oxygen Group

d)

Cobalt

4.

Transition Metal

e)

Lead

5.

Carbon Group

170.

Match the following Elements with the Family or group they are in

a)

Iodine

1.

Halogens

b)

Magnesium

2.

Alkaline Earth Metals

c)

Potassium

3.

Alkali metals

d)

Tungsten

4.

Transition Metal

e)

Aluminum

5.

Boron Group

171.

Match the following Elements with the Family or group they are in

a)

Promethium

1.

Lanthanide series

b)

Calcium

2.

Alkaline Earth Metals

c)

Sodium

3.

Alkali metals

d)

Silver

4.

Transition Metal

e)

Gallium

5.

Boron Group

172.

Match the following Elements with the Family or group they are in

a)

Plutonium

1.

Actinide series

b)

Barium

2.

Alkaline Earth Metals

c)

Cesium

3.

Alkali metals

d)

Mercury

4.

Transition Metal

e)

Tin

5.

Carbon Group

173.

Match the following Elements with the Family or group they are in

a)

Unranium

1.

Actinide series

b)

Strontium

2.

Alkaline Earth Metals

c)

Lithium

3.

Alkali metals

d)

Iron

4.

Transition Metal

e)

Argon

5.

Noble Gasses

174.

Match the following Elements with the Family or group they are in

a)

Helium

1.

Noble Gasses

b)

Beryllium

2.

Alkaline Earth Metals

c)

Rubidium

3.

Alkali metals

d)

Gold

4.

Transition Metal

e)

Bromine

5.

Halogens

175.

Match the following about the isotopic notation

a)

AMU's

1.

197

b)

Element Name

2.

Gold

c)

Number of Protons

3.

79

d)

Number of neutrons

4.

118

e)

Charge

5.

0

176.

Match the following about the isotopic notation

a)

AMU's

1.

27

b)

Element Name

2.

Aluminum

c)

Number of Protons

3.

13

d)

Number of neutrons

4.

14

e)

Number of Electrons

5.

10

177.

Match the following about the isotopic notation

a)

AMU's

1.

23

b)

Element Name

2.

Sodium

c)

Number of Protons

3.

11

d)

Number of neutrons

4.

12

e)

Number of Electrons

5.

10

178.

Match the following about the isotopic notation

a)

AMU's

1.

56

b)

Element Name

2.

Iron

c)

Number of Protons

3.

26

d)

Number of neutrons

4.

30

e)

Number of Electrons

5.

23

179.

Organize these options into the right categories

Categorize the following

Discovered the Proton

Discovered the Nucleus

Performed the Gold Foil Experiment

Developed the Planetary Model of the Atom

Developed the Plum Pudding Model of the Atom

Conducted the Cathode Ray Experiment

Identified the First Subatomic Particle

Developed the Electron Cloud model

Contributed to the development of Quantum Mechanics

Worked on Wave Mechanics

Discovered the Enery Levels of the electrons around the nucleus

Discovered that when electrons absorb energy they jump to a higher energy level

Discovered that when electrons release energy they fall to a lower energy level

Discovered light is produced from electrons that fall from higher lenergy levels to lower energy

Showed the atom was made up of mostly space

Showed the nucleus was a small dense positively charged area

Rutherford

Bohr

Thompson

Schodinger

180.

Reorder the following

a)

1s²

b)

2s²

c)

2p⁶

d)

3s²

e)

3p⁶

1)

2)

3)

4)

5)

181.

Match the following number of sub orbitals for each type

a)

s

1.

1

b)

p

2.

3

c)

d

3.

5

d)

f

4.

7

182.

Match the following number of electrons that be housed in each orbital type

a)

2

1.

s

b)

6

2.

p

c)

10

3.

d

d)

14

4.

f

183.

Rank the following elements in order of increasing electronegativity

a)

Calcium

b)

Iron

c)

Arsenic

d)

Selenium

e)

Bromine

1)

2)

3)

4)

5)

184.

Rank the following elements in order of increasing Ionization energy

a)

Lead

b)

Tin

c)

Germanium

d)

Silicon

e)

Carbon

1)

2)

3)

4)

5)

185.

Rank the following elements in order of decreasing Atomic Radii

a)

Lead

b)

Tin

c)

Germanium

d)

Silicon

e)

Carbon

1)

2)

3)

4)

5)

186.

Rank the following elements in order of increasing Atomic Radii

a)

Magnesium

b)

Aluminum

c)

Phosphorus

d)

Sulfur

e)

Chlorine

1)

2)

3)

4)

5)

187.

Rank the following elements in order of decreasing electron affinity

a)

Hydrogen

b)

Lithium

c)

Sodium

d)

Potassium

e)

Rubidium

1)

2)

3)

4)

5)

188.

What did Thompson model of the atom (the plum pudding model) change Dalton's atomic theory?

a)

Showed that atoms had things that negative things called electrons

b)

Showed that atoms of different elements had similar parts

c)

Discovered the nucleus

d)

Showed electrons produce light by releasing energy

More Practice for unit 1

Total questions: 188

Worksheet time: 6hrs 40mins

Similar Resources on Wayground