Free Printable Quantum number

1.

If n = 1, what are the allowed values of L? Tick all that apply:

a)

0

b)

1

c)

2

d)

3

2.

If n = 2, what are the allowed values of L? Tick all that apply:

a)

0

b)

1

c)

2

d)

3

3.

If n = 3, what are the allowed values of L? Tick all that apply:

a)

0

b)

1

c)

2

d)

3

4.

For L = 0, tick the possible values of m:

a)

-1

b)

1

c)

0

d)

-2

e)

2

5.

If L = 1, tick the possible values of m:

a)

1,0

b)

-1, 0, 1

c)

-2, 0, 1

d)

-2, -1, 0, 1,2,

6.

If L = 2, tick the possible values of m:

a)

-1,0,1

b)

-2,-1,0,1,2

c)

-3,-2,-1,0,1,2,3

d)

0

7.

What are the possible values of the spin number Ms?

pick all the options

a)

-1/2

b)

0

c)

- 1

d)

1

e)

1/2

8.

If n=4, and l=3

Which one is the configuration that represents these numbers?

a)

4d

b)

4f

c)

3d

d)

4p

9.

What is the correct electronic configuration for an orbital which has an "n" value of 4 and an "L" value of 2?

a)

4d

b)

4f

c)

4p

d)

4s

10.

Which of the following sets of quantum numbers (n, l, m_l, and m_s) describes the valence electron of Na?

Z=11

a)

2, 1, 0, -½

b)

3, 1, 1, +½

c)

2, 0, 0, -½

d)

3, 0, 0, +½

11.

Which one of the following sets of quantum numbers (n, l, m_l, and m_s) describes the valence electron of 4s¹?

a)

2, 0, 0, +1/2

b)

4, 0, 0, +1/2

c)

2, 1, 0, +1/2

d)

4, 1, 1, +1/2

12.

If we have

n = 2

l = 2

m = 0

s = +1/2

Which is the correct notation

a)

2p¹

b)

2s²

c)

2p²

d)

No correct answer

13.

What is the correct representation for an orbital which has an "n" value of 4 and an "L" value of 2?

a)

4d

b)

4s

c)

4f

d)

4p

14.

For a p sublevel, "L" equals ____.

a)

0

b)

1

c)

2

d)

3

15.

What is the correct representation for an orbital which has an "n" value of 3 and an "l" value of 1?

a)

3s

b)

3p

c)

3d

d)

3f

16.

For a principle quantum number, "n", equal to 2, what is the total electron capacity of that level?

a)

2

b)

4

c)

8

d)

16

17.

What quantum number describes the energy level of an orbital?

a)

l

b)

m

c)

s

d)

n

18.

Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

19.

Which of the following sets of quantum numbers (n, l, m_l, and m_s) describes the valence electron of Na?

a)

2, 1, 0, -½

b)

2, 0, 0, -½

c)

3, 1, 1, +½

d)

3, 0, 0, +½

20.

What atom matches this electron configuration?
1s²2s²2p⁶3s²

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

21.

Which values can (n) be?

a)

only 0

b)

0, 1, 2, 3...

c)

1,2,3,4...

d)

-2 < n < +2

22.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

set state

d)

ground state

23.

This is a ____ orbital

a)

s

b)

d

c)

p

d)

d

24.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

25.

Orbital sublevels, or L, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

26.

The proper pair of the L value with the orbital shape.

a)

0; f

b)

3; p

c)

1; s

d)

2; d

27.

How many electrons total are found in the f orbital?

a)

2

b)

6

c)

10

d)

14

28.

For a p sublevel, "L" equals ____.

a)

0

b)

1

c)

2

d)

3

29.

How many electrons can the first energy level hold?

a)

1

b)

2

c)

8

d)

0

30.

4. Below are the examples on how to fill the atomic quantum number, except... .

a)

n = 2, l =1, m = 0, s = -1/2

b)

n = 1, l =3, m = 0, s = +1/2

c)

n = 3, l =1, m = 0, s = -1/2

d)

n = 3, l = 2, m = +2, l = +1/2

31.

6. Primal quantum number (n) states that... .

a)

The direction of its spinning axis, when it rotates the core

b)

Sum of shells in an atom

c)

Orbital orientation of an electron

d)

The location of the outmost subshell in an atom

32.

7. The magnetic quantum number (m), has value within... .

a)

0 up to (n-1)

b)

0, 1, 2, 3, ...

c)

-l up to. +l

d)

-1/2 and +1/2

33.

12. A subshell that contains 5 orbitals is ... subshell.

a)

d

b)

s

c)

f

d)

p

34.

15. Orbital shape of an atom is characterized by ... quantum number.

a)

Spin projection

b)

Primal

c)

Magnetic

d)

Azimuthal

35.

Which of the following is NOT a possible pair of quantum numbers?

a)

2p

b)

2d

c)

4p

d)

4f

36.

What is the electron configuration for F?

a)

1s2 2s2 3p5

b)

1s2 2s2 3d5

c)

1s2 2s2 2p5

d)

1s2 2p5

37.

for each set of quantum numbers, which set is correct

a)

n = 1 ℓ = 1 mℓ = 0 m_s = +1/2

b)

n = 2 ℓ = 0 mℓ = -1 m_s = +1/2

c)

n = 3 ℓ = 2 mℓ = -1 m_s = -1/2

d)

n = 2 ℓ = 1 mℓ = -2 m_s = +1/2

38.

when n= 3

a)

ℓ = 3

b)

m ℓ = 4

c)

ℓ =0

d)

ms= +1

39.

3d sublevel has ------------

a)

n= 2

b)

ℓ = 2

c)

3 orbitals

d)

spherical shape

40.

This shape is that of a...

a)

s orbital

b)

d orbital

c)

p orbital

d)

f orbital

41.

The proper pair of the l value with the orbital shape.

a)

0; f

b)

3; p

c)

1; s

d)

2; d

42.

How many electrons total are found in the f orbital?

a)

2

b)

6

c)

10

d)

14

43.

n=4, l=3?

a)

4f

b)

4d

c)

3s

d)

3p

44.

Orbital sublevels, or L, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

45.

Which of the following is NOT a possible pair of quantum numbers?

a)

2p

b)

2d

c)

4p

d)

4f

46.

What does the 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

47.

What is the correct representation for an orbital which has an "n" value of 4 and an "L" value of 2?

a)

4d

b)

4s

c)

4f

d)

4p

48.

The major difference between a 1s orbital and a 2 s orbital is that

a)

the 2 s orbital is at a higher energy level.

b)

the 2s orbital has a slightly different shape.

c)

the 1 s orbital can have only one electron.

d)

the 2s orbital can hold more electrons.

49.

n=4, l=3?

a)

4f

b)

4d

c)

3s

d)

3p

50.

Which of the following sub levels does not exist

a)

2p

b)

3d

c)

2d

d)

5f

e)

4f

51.

What is the maximum number of electrons that contain the values

n=4 l=3

a)

2

b)

6

c)

10

d)

14

e)

18

52.

2. A quantum number determining orbital orientation around the atom’s core is called... .

a)

n

b)

l

c)

m

d)

s

53.

4. Below are the examples on how to fill the atomic quantum number, except... .

a)

n = 2, l =1, m = 0, s = -1/2

b)

n = 1, l =3, m = 0, s = +1/2

c)

n = 3, l =1, m = 0, s = -1/2

d)

n = 3, l = 2, m = +2, l = +1/2

54.

This is a ____ orbital

a)

s

b)

d

c)

p

d)

d

55.

Any given orbital may hold a maximum of __ electrons

a)

2

b)

8

c)

18

d)

32

56.

Which of the following elements is Paramagnetic?

look at the atomic numbers.

a)

Mg

b)

Ne

c)

P

d)

Ca

e)

Kr

57.

A paramagnetic atom is

a)

An atom with All paired electrons

b)

An atom with unpaired electrons

58.

An atom that is diamagnetic is

a)

An atom with all paired electrons

b)

An atom with unpaired electrons

59.

N=5 l=2

a)

3s

b)

4sp

c)

5d

d)

5p

60.

If L = 2, tick the possible values of m:

a)

-1,0,1

b)

-2,-1,0,1,2

c)

-3,-2,-1,0,1,2,3

d)

0

61.

If n=4, and l=3

Which one is the configuration that represents these numbers?

a)

4d

b)

4f

c)

3d

d)

4p

62.

Which one of the following sets of quantum numbers (n, l, m_l, and m_s) describes the valence electron of 4s¹?

a)

2, 0, 0, +1/2

b)

4, 0, 0, +1/2

c)

2, 1, 0, +1/2

d)

4, 1, 1, +1/2

63.

If we have

n = 2

l = 2

m = 0

s = +1/2

Which is the correct notation

a)

2p¹

b)

2s²

c)

2p²

d)

No correct answer

64.

There may be a maximum of ___ p orbitals at a given energy levle.

a)

2

b)

3

c)

6

d)

8

65.

The first energy level to have d-orbitals is:

a)

1

b)

2

c)

3

d)

4

66.

What is untrue about f orbitals?

a)

first found at energy level 4

b)

when all f orbitals of a given energy level are full, they may contain up to 14 electrons

c)

there are 5 different orientations, or axes

d)

each f orbital may hold an electron with a +1/2 spin and a -1/2 spin

67.

The spin of an electron is represented by this variable:

a)

n

b)

l

c)

m

d)

s, m_s

68.

3. A subshell containsing 7 orbitals is called ... subshell.

a)

s

b)

p

c)

d

d)

f

69.

2. A quantum number determining orbital orientation around the atom’s core is called... .

a)

n

b)

l

c)

m

d)

s

70.

1. Below are the quantum number classifications, except... .

a)

Primal quantum number (n)

b)

Azimuthal quantum number (a)

c)

Magnetic quantum number (m)

d)

Spin projection quantum number (s)

71.

5. The total amount of electrons that can be filled within p subshell are ... electrons.

a)

6

b)

10

c)

14

d)

18

72.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

set state

d)

ground state

73.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

74.

What is the electron configuration for F?

a)

1s2 2s2 3p5

b)

1s2 2s2 3d5

c)

1s2 2s2 2p5

d)

1s2 2p5

75.

What orbitals can you find on the 3rd energy level? (Check all that apply)

a)

s

b)

p

c)

d

d)

f

Quantum number

Total questions: 75

Worksheet time: 47mins

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