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Periodic table stuff

Total questions: 96

Worksheet time: 3hrs 57mins

Name
Class
Date
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 Alkali metals?

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

4.

Which of the following elements have 5 valence electrons?

a)

C

b)

N

c)

O

d)

Sb

e)

Pb

5.

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

a)

Ag

b)

Cu

c)

Au

d)

Rg

6.

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

7.

Which of the following elements has 8 valence electrons?

a)

He

b)

Ne

c)

Ar

d)

F

e)

Cl

8.

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

a)

P3-

b)

O2-

c)

Cl1-

d)

K1+

e)

Al3+

9.

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

a)

1s22s22p6

b)

1s12s22p6

c)

1s22s22p4

d)

1s22s22p5

10.

Which of the following has the smallest atomic radius?

a)

Cl

b)

F

c)

O

d)

Br

e)

Ar

11.

Which of the following would have the biggest Atomic radius?

a)

K

b)

Cu

c)

Mg

d)

Fr

e)

Rb

12.

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

13.

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

14.

Who discovered the Electron?

a)

Thompson

b)

Rutherford

c)

Dalton

d)

Bohr

15.

Who discovered the nucleus?

a)

Dalton

b)

Bohr

c)

Thompson

d)

Rutherford

16.

Who discovered the Energy levels in the atom?

a)

Schodinger

b)

Bohr

c)

Rutherford

d)

Thompson

17.

Who mathematically predicted the electron clouds?

a)

Bohr

b)

Thompson

c)

Schrodinger

d)

Dalton

18.

How many neutrons would Ca-45 have?

a)

45

b)

5

c)

20

d)

25

19.

How many protons would Al- 27 have?

a)

13

b)

27

c)

14

d)

26

e)

12

20.

How many electrons does O2- have

a)

6

b)

8

c)

10

d)

12

21.

How many electrons does Na1+ have?

a)

9

b)

10

c)

11

d)

12

22.

What does electron configuration of P3- end with?

a)

3d6

b)

3p6

c)

3d3

d)

3p3

23.

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

24.

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

a)

1

b)

2

c)

3

d)

4

e)

5

25.

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

a)

Down

b)

Up

c)

Left

d)

right

26.

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

a)

up

b)

down

c)

left

d)

right

27.

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

28.

Which family would be considered the least reactive?

a)

Noble gases

b)

Carbon group

c)

Halogens

d)

Boron group

e)

Alkali metals

29.

How many neutrons would Carbon-14 have?

a)

14

b)

6

c)

12

d)

8

30.

How many neutrons would be in the isotope 23692U?

a)

92

b)

236

c)

144

d)

146

31.

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

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

32.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

33.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

34.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

35.

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

a)

Ag

b)

Cu

c)

Au

d)

Rg

36.

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

(a)  

37.

Name an element has 6 valence electrons?

(a)  

38.

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

a)

Ar

b)

O2-

c)

F1-

d)

K1+

e)

Ga3+

39.

How many electrons would Al3+ have?

a)

10

b)

13

c)

16

d)

24

e)

12

40.

How many electrons does Zn1+ have?

a)

30

b)

31

c)

29

d)

65

41.

How many electrons does S2- have?

a)

19

b)

18

c)

16

d)

17

42.

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

a)

3d6

b)

3p6

c)

3d3

d)

3p3

43.

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

a)

1

b)

2

c)

3

d)

4

e)

5

44.

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

a)

Down

b)

Up

c)

Left

d)

right

45.

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

a)

up

b)

down

c)

left

d)

right

46.

Which family would be considered the least reactive?

a)

Noble gases

b)

Oxygen group

c)

Lanthanide series

d)

Transition metals

e)

Alkaline earth metals

47.

How many neutrons would Rutherium-105 have?

a)

44

b)

61

c)

105

d)

78

48.

How many neutrons would be in the isotope 9139Y?

a)

52

b)

39

c)

91

d)

55

49.

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

50.

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

51.

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

52.

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

53.

Which subatomic particles are responsible for atomic mass?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Positrons

54.

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

a)

Electrons

b)

Neutrons

c)

Nucleus

d)

Protons

55.

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

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

56.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

57.

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

a)

Ag

b)

Cu

c)

Au

d)

Rg

58.

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

59.

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

60.

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

61.

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

62.

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

a)

Ar

b)

O2-

c)

F1-

d)

K1+

e)

Ga3+

63.

Match the following atoms with the correct Orbital diagram.

a)

1.

Magnesium

b)

2.

Neon

c)

3.

Oxygen

d)

4.

Sodium

e)

5.

Carbon

64.

Which of the following orbital diagrams is correct for Aluminum?

a)

b)

c)

d)

65.

What is the electron configuration for Krypton?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

b)

[Ar] 4s2 3d10 4p6

c)

1s2 2s2 3s2 2p6 4s2 3p6 4p6 3d10

d)

[Ne] 4s2 3d10 4p6

66.

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)
67.

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)
68.

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)
69.

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)
70.

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)
71.

How many valence electrons does Helium have?

a)

1

b)

2

c)

6

d)

7

e)

4

72.

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

a)
2
b)

3

c)

1

d)

4

73.

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

a)
2
b)

3

c)

1

d)

4

74.

Who discovered the Electron?

a)

Thompson

b)

Rutherford

c)

Dalton

d)

Bohr

75.

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

76.

Who discovered the nucleus?

a)

Dalton

b)

Bohr

c)

Thompson

d)

Rutherford

77.

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.

78.

Who discovered the Energy levels in the atom?

a)

Schodinger

b)

Bohr

c)

Rutherford

d)

Thompson

79.

Who mathematically predicted the electron clouds?

a)

Bohr

b)

Thompson

c)

Schrodinger

d)

Dalton

80.

How many neutrons would Ca-45 have?

a)

45

b)

5

c)

20

d)

25

81.

How many electrons would Al3+ have?

a)

10

b)

13

c)

16

d)

24

e)

12

82.

How many electrons does Zn1+ have?

a)

30

b)

31

c)

29

d)

65

83.

How many electrons does S2- have?

a)

19

b)

18

c)

16

d)

17

84.

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

a)

3d6

b)

3p6

c)

3d3

d)

3p3

85.

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

86.

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

a)

1

b)

2

c)

3

d)

4

e)

5

87.

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.

88.

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

a)

Down

b)

Up

c)

Left

d)

right

89.

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

a)

up

b)

down

c)

left

d)

right

90.

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

91.

Which family would be considered the least reactive?

a)

Noble gases

b)

Oxygen group

c)

Lanthanide series

d)

Transition metals

e)

Alkaline earth metals

92.

How many neutrons would Rutherium-105 have?

a)

44

b)

61

c)

105

d)

78

93.

How many neutrons would be in the isotope 9139Y?

a)

52

b)

39

c)

91

d)

55

94.

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

95.

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

96.

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

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