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Quantum Theory Bank

Total questions: 104

Worksheet time: 2hrs 47mins

Name
Class
Date
1.

Which atomic model uses atomic orbitals to describe the probable location of any electron in a three-dimensional space?

a)

A. the cubic model

b)

B. the plum-pudding model

c)

C. the planetary model

d)

D. the quantum mechanical model

2.

This shape is that of

a)

s-orbital

b)

d-orbital

c)

p-orbital

d)

f-orbital

3.

The figure is a 3-dimensional representation of an atomic orbital. Which orbital does it represent?

a)

A. an s-orbital

b)

B. a single p-orbital

c)

C. three d-orbitals

d)

D. three p-orbitals

4.
A three-dimensional region around a nucleus where an electron may be found is called a(n
a)
orbit
b)
circle
c)
orbital
d)
circuit
5.

How many orbitals are there in the p sublevel?

a)

1

b)

3

c)

5

d)

7

6.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
7.

Match the following

a)

  • transition metals

1.

  • d-block

b)

  • actinide series

2.

  • f-block

c)

  • alkali metals

3.

  • s-block

d)

  • noble gases

4.

  • p-block

8.

Reorder these representative elements from fewest valence electrons to most valence electrons.

a)

Hydrogen (H)

b)

Boron (B)

c)

Sulfur (S)

d)

Bromine (Br)

1)
2)
3)
4)
9.

An element's electron configuration and number of valence electrons can be determined by its ______.

a)

atomic mass

b)

position on the periodic table

c)

melting and boiling points

d)

chemical symbol

10.

How many electrons can the d sublevel (the d orbitals) hold?

a)

14

b)

10

c)

2

d)

6

11.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

12.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

There is nothing incorrect with this diagram

c)

In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box pointing in the same direction.

d)

All the arrows should be pointing up.

13.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
14.

What orbital is shown in the picture?

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

15.

The Pauli exclusion principle requires electrons that are in the same orbital must have

a)

opposite charges.

b)

the same spin.

c)

opposite spins.

d)

good hygiene.

16.

According to Pauli Exclusion Principle, how many electrons may occupy a single orbital?

a)

1

b)

2

c)

4

d)

8

17.

“An electron should occupy the lowest energy level first before the higher energy level” is stated in what rule?

a)

Hund's rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

All of the above.

18.

What rule states that single electrons must occupy each equal-energy orbital before additional electrons can occupy the same orbitals.

a)

Hund's rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

None of the choices.

19.

How many energy levels are currently present on the periodic table?

a)

18

b)

7

c)

6

d)

4

20.

How many orbitals are there in a p-sublevel?

a)

1

b)

3

c)

5

d)

7

21.

How many electrons can the d sublevel hold?

a)

14

b)

10

c)

2

d)

6

22.

How many electrons can the s sublevel hold?

a)

14

b)

10

c)

2

d)

6

23.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

24.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

25.

Which of the following sub-levels is correctly designated?

a)

1p5

b)

3f9

c)

2p6

d)

3d11

26.

According to Pauli Exclusion Principle, how many electrons may occupy a single orbital?

a)

1

b)

2

c)

4

d)

8

27.

“An electron should occupy the lowest energy level first before the higher energy level” is stated in what rule?

a)

Hund's rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

All of the above.

28.

What rule states that single electrons must occupy each equal-energy orbital before additional electrons can occupy the same orbitals.

a)

Hund's rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

None of the choices.

29.

What is the electron configuration of Argon?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s1

c)

1s2 2s2 2p6 3s2

d)

1s2 2s2 2p6 3s2 3p6

30.

What model of the atom replaced Bohr's model?

a)

Heisenberg's model

b)

Thomson's model

c)

Rutherford's model

d)

Quantum Mechanical model

31.

How many energy levels are currently present on the periodic table?

a)

18

b)

7

c)

6

d)

4

32.

How many orbitals are there in a p-sublevel?

a)

1

b)

3

c)

5

d)

7

33.

What atom matches this electron configuration?
1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

34.

What atom matches this electron configuration?
1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

35.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

36.

The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 

a)

3

b)

6

c)

8

d)

10

37.

Which electron configuration belongs to Chlorine (Cl)?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

38.

How many electrons can the d sublevel hold?

a)

14

b)

10

c)

2

d)

6

39.

How many electrons can the s sublevel hold?

a)

14

b)

10

c)

2

d)

6

40.

What atom matches this electron configuration?
1s22s22p63s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

41.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

42.

What atom matches this electron configuration?
1s22s22p63s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

43.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

44.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

45.

What is the noble gas shorthand electron for Sulfur atom?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p4

46.

What is the electron configuration for this atom?

a)

1s22s22p6

b)

1s22s22p5

c)

1s22s22p3

d)

2s22p3

47.

What atom matches this electron configuration?
1s22s22p63s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

48.

Which element is depicted from this orbital diagram

a)

Fluorine

b)

Neon

c)

Chlorine

d)

Argon

49.

Which is associated with more energy? 

a)

2p

b)

2s

c)

3p

d)

1s

50.

What is the electronic configuration of sodium?

a)

1s22s22p63s1

b)

[Ne]3s1

c)

1s22s22p7

d)

Both A and B are correct

51.

Which of the following is the correct electron configuration for a phosphorus  atom?

a)

1s2 2s2 2p6 3s2 3p3

b)

1s2   2s2   3p3 

c)

1s2 2s2 2p6 3s2 3p6 

d)

1s2 2s2  3s2 2p6 3p3

52.

Which of the following is the correct electron configuration for a carbon atom?

a)

1s2 2s2 2p6 3s2 3p2

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p2

d)

1s2 2s2 2p6 3s2 3p6 4s2 4p2

53.

Which of the following is the correct electron configuration for a neon atom?

a)

1s2 2s2 2p3

b)

1s2 2s2 2p6 3s1

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

d)

1s2 2s2 2p6 

54.

Which of the following elements is a noble gas?

a)

1s2 2s2

b)

1s2 2s2 2p5

c)

1s2 2s2 2p6 3s2 3p6

d)

1s2 2s2 2p6 3s1

55.

Which of the following elements is a transition metal?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

b)

1s2 2s2 2p6 3s2 3p6 

c)

1s2 2s2 2p6 3s2 3p6 4s2 

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d4

56.

Which group of the periodic table has an electron configuration of ns2 np5?

a)

Metalloids

b)

Nobel Gases

c)

Halogens

d)

Alkaline Metals

57.

What is the abbreviated electron configuration for silver?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9

b)

[Kr] 5s2 4d9

c)

[Ar] 4s2 3d9

d)

[Ag]

58.

What is the abbreviated electron configuration for barium?

a)

[Xe] 6s2

b)

[Rn] 6s2

c)

[Ar] 4s2 3d10 4p5

d)

[He] 2s2 3p1

59.

How many electrons can the first energy level hold?

a)

1

b)

2

c)

8

d)

0

60.

The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 

a)

3

b)

6

c)

8

d)

10

61.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

62.

Which of the following is the electron configuration for an alkali earth metal?

a)

1s22s1

b)

1s22s22p1

c)

1s22s22p5

d)

1s22s22p63s2

63.

How many electrons at most are in the 4f sublevel?

a)

10

b)

8

c)

18

d)

14

64.

The following electron configuration is for which element?

1s22s22p63s23p64s23d10

a)

Cu

b)

Zn

c)

Cd

d)

Ga

65.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

66.

How many valence electrons are in this element? AND identify the element.

1s22s22p63s23p64s23d104p65s24d105p66s25d14f145d2

a)

11; Hf

b)

2; Ba

c)

3; La

d)

2; Ta

67.

What is this element?
1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

68.

What is this element? 
[Ne] 3s23p64s2

a)

Calcium

b)

Sodium

c)

Scandium

d)

Titanium

69.

What is the electron configuration for Bromine (Br)

a)

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1

b)

1s2, 2s2, 2p4

c)

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p5

d)

1s2, 2s2, 2p6

70.

What is the noble gas configuration for Sulfur?

a)

[Ar] 3p4

b)

[He] 3s2 3p4

c)

[Ne] 3s2 3p4

d)

[Na] 3s2 3p4

71.

How many orbitals are available to hold electrons in the 6th energy level (n=6)?

a)

9

b)

16

c)

26

d)

36

72.

According to the Aufbau Principle, which sublevel should starting filling with electrons after 5s?

a)

6s

b)

5p

c)

4d

d)

3f

73.

How many electrons can the d sublevel hold?

a)

14

b)

10

c)

2

d)

6

74.

Which of the following is the noble gas (shorthand) configuration for iodine?

a)

[Ar] 4s24d104p5

b)

[Kr] 5s24d105p5

c)

[Xe] 5s25d105p5

75.

Each row of the periodic table represents a(n)

a)

Energy level

b)

Sublevel

c)

Electron

d)

Orbital

76.

Which of the following is the electron configuration for iron?

a)

1s22s22p63s23p64s23d6

b)

1s22s22p63s23p63d8

c)

1s22p63s23p64s23d6

d)

1s22s22p63s23p64s13d6

77.

Which of the following is the noble gas configuration for boron?

a)

[He] 1s22s2

b)

[He] 2s22p2

c)

[He] 2s22p1

d)

[Ne] 2s22p1

78.

What atom matches this electron configuration?

1s22s22p63s23p64s23d3

a)

Vanadium

b)

Copper

c)

Nickel

d)

Germanium

79.
What is the electron configuration for this atom?
a)
1s22s22p6
b)
1s22s22p5
c)
1s22s22p3
d)
2s22p3
80.

Identify the following element:

1s22s22p63s23p64s23d104p65s24d9

a)

Silver

b)

Copper

c)

Cadmium

d)

Cobalt

81.
Identify the element whose electron configurations ends with 5p3
a)
As
b)
Te
c)
Sb
d)
Sn
82.
According to the Aufbau Principle, which sublevel should starting filling with electrons before the 3p sublevel?
a)
3s
b)
2p
c)
4s
d)
4p
83.

What is the next orbital filled after 4d?

a)

6p

b)

5d

c)

5p

d)

4f

84.

What is the correct electron configuration for Titanium (22)?

a)

1s22s22p63s23p4

b)

1s22s22p63s23p64s23d2

c)

1s22s22p63s23p64s24p2

d)

1s22s22p63s23p64s24d2

85.

Which of the following subshells holds the least electrons?

a)

s

b)

p

c)

d

d)

f

86.

Which of the following subshells holds the most electrons?

a)

s

b)

p

c)

d

d)

f

87.

Which of the following elements is located in the 5p subshell?

a)

Pb

b)

Sb

c)

Ag

d)

Au

88.

What is the correct electron configuration for strontium (Sr)?

a)

1s2 2s2 2p6 3s2 3p6 4s1

b)

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

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 5s2

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2

89.

What is written at the beginning of a condensed electron configuration?

a)

In brackets, the noble gas located at the far right of the same horizontal row on the table.

b)

In brackets, the noble gas located at the far right of the preceding horizontal row on the table.

90.

What is the correct condensed electron configuration for potassium (K)?

a)

[Ar] 4s1

b)

[Kr] 4s1

c)

[Ar] 4s2

d)

[Kr] 4s2

91.

How many energy levels does Rb have? Just give me the number.

(a)  

92.

How many energy levels does He have? Just give me the number.

(a)  

93.

P and Po have the same number of energy levels.

a)

True

b)

False

94.

Mg and Ga have the same number of energy levels?

a)

True

b)

False

95.

Where would the electrons be located?

A
B
C
D
E
96.

Label the three parts of an electron configuration:

a)

protons

b)

section

c)

family

d)

period (row)

e)

block (orbital)

f)

electrons

g)

group

1
2
3
1)
2)
3)
97.

The image shows the partial electron configuration of manganese (Mn). Below there are two empty boxes. Correctly drag the final two answers in the correct order to finish its electron configuration.​

​ ​ (a)   ​ (b)  

Choose from the below words
4s²
3d⁵
1p⁶
2s³
3d⁹
2d⁹
98.

Match the following

a)

1s2 2s2 2p4

1.

oxygen

b)

1s2 2s2 2p6 3s2 3p6 4s1

2.

potassium

c)

1s2 2s2 2p6

3.

neon

d)

1s2 2s2 2p6 3s2 3p2

4.

silicon

e)

1s2 2s2 2p6 3s2

5.

magnesium

99.

The 2,8,8 rule means the first shell is filled with ​ (a)   electrons, the second is filled with 8 ​ (b)   , and the third is filled with 8.

Choose from the below words
2
8
electrons
protons
100.

Which element is represented by each configuration?
1s22s22p5 ​ (a)  
[Xe]6s24f4 ​ (b)  

[Kr]5s14d5 ​ (c)  

Choose from the below words
F
Nd
Mo
101.

Match the following

a)

1s2 2s2 2p4

1.

oxygen

b)

1s2 2s2 2p6 3s2 3p6 4s1

2.

potassium

c)

1s2 2s2 2p6

3.

neon

d)

1s2 2s2 2p6 3s2 3p2

4.

silicon

e)

1s2 2s2 2p6 3s2

5.

magnesium

102.

Which element is represented by each configuration?
1s22s22p5 ​ (a)  
[Xe]6s24f4 ​ (b)  

[Kr]5s14d5 ​ (c)  

Choose from the below words
F
Nd
Mo
103.

For each ​square that you move ​ (a)   on the ​ (b)   , an ​ (c)   is ​ (d)   making the atom ​ (e)   .

Choose from the below words
downward
periodic table
electron shell
added
larger
104.

Label the three parts of an electron configuration:

a)

protons

b)

section

c)

family

d)

period (row)

e)

block (orbital)

f)

electrons

g)

group

1
2
3
1)
2)
3)

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