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Quantum number

Total questions: 45

Worksheet time: 4hrs 45mins

Name
Class
Date
1.

Select ways to show the the arrangement of electrons in the quantum mechanical model.

a)

Energy Level Diagram (Orbital Diagram)

b)

Orbits

c)

Electron Configurations

d)

Heisenberg Uncertainty Principle

2.

Electrons are arranged so that the element has...

a)

...the lowest amount of energy, which is called the excited state configuration

b)

...the lowest amount of energy, which is called the ground state configuration

c)

...the highest amount of energy, which is called the excited state configuration

d)

...the highest amount of energy, which is called the ground state configuration

3.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
4.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
5.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
6.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
7.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
8.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
9.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
10.
Why do we use the three electron configuration rules: Hund's Rule, Aufbau Principle, and Pauli Exclusion Principle?
a)
to know where electrons are located
b)
to know how electrons are oriented in space
c)
to know how electrons are used in chemical reactions
d)
all of these
11.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
12.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
13.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
14.
Why do we not use Bohr's planetary model today?
a)
it is too specific; we are not allowed to know the electron's specific location
b)
it represented the nucleus far too largely
c)
it is too vague; we have more specific information to use now
d)
it placed the electrons too close to the nucleus
15.
represents the distance the electrons are from the nucleus
a)
energy level 
b)
sublevel
16.
represents an area of probability of the electron's location, called s, p, d, or f
a)
energy level 
b)
sublevel
17.
"Electrons in the same orbital have opposite spin."
a)
aufbau principle
b)
Hund's Rule
c)
Pauli Exclusion Principle
d)
Uncertainty Principle
18.
"Electrons fill equal energy orbitals singly before pairing."
a)
aufbau principle
b)
Hund's Rule
c)
Pauli Exclusion Principle
d)
Uncertainty Principle
19.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
20.

Which electron configuration belongs to Chlorine (17Cl)?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

21.

The second shell from the center of an atom can hold how many electrons?

a)

2

b)

6

c)

8

d)

18

22.
According to _______, an electron occupies the lowest-energy orbital that can receive it.
a)
the Aufbau principle
b)
the Pauli exclusion principle
c)
Hund's rule
d)
Conservation of Energy
23.

Which rule is broken by this electron configuration?

a)

the Aufbau principle

b)

the Pauli exclusion principle

c)

Hund's rule

d)

Conservation of Energy

24.

Which rule is broken by this electron configuration?

a)

the Aufbau principle

b)

the Pauli exclusion principle

c)

Hund's rule

d)

Conservation of Energy

25.
How many unpaired electrons does sulfur have ( 1s22s22p63s23p4 ) ?
a)
0
b)
1
c)
2
d)
3
26.

What's the electron configuration for 14S?

a)

1s22s22p63s23p2

b)

1s22s22p63s4

c)

1s22s22p63p4

d)

1s22s22p63s23p4

27.

What's the electron configuration for 23V?

a)

1s22s22p63s23p64s23d3

b)

1s22s22p63s23p63d5

c)

1s22s22p63p64s24p3

28.

What is the atomic number?

a)

the number of protons

b)

the number of protons and neutrons

c)

the number of neutrons

d)

the number of protons and electrons

29.
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.
30.
The atomic sublevel with the next hightest energy after 4p is
a)
5s
b)
4f
c)
5p
d)
4d
31.

Write the full electronic structure for Na with 11 electrons.

a)

1s22s22p63s1

b)

1s22s23p63s1

c)

[Ne]3s2

d)

1s22s22p63p1

32.
Write the full electronic structure for Ca with 20 electrons.
a)
1s22s22p63s23p6
b)
1s22s22p63s23p64s0
c)
1s22s22p63s23p64s1
d)
1s22s22p63s23p64s2
33.
How many quantum numbers are needed to describe the energy state of an electron in an atom?
a)
1
b)
2
c)
3
d)
4
34.

Which values can (n) be?

a)

only 0

b)

0, 1, 2, 3...

c)

1,2,3,4...

d)

-2 < n < +2

35.

What values of ml can there be is l = 0 (s orbital)?

a)

0

b)

-1 to +1

c)

-2 to +2

d)

-3 to +3

36.

What values of ml can there be is l = 1 (p orbital)?

a)

0

b)

-1 to +1

c)

-2 to +2

d)

-3 to +3

37.

What values of ml can there be is l = 2 (d orbital)?

a)

0

b)

-1 to +1

c)

-2 to +2

d)

-3 to +3

38.

What values of ml can there be is l = 3 (f orbital)?

a)

0

b)

-1 to +1

c)

-2 to +2

d)

-3 to +3

39.

What two values can ms be?

a)

-1 and +1

b)

-1/2 and +1/2

c)

-2 and +2

d)

+1 and +2

40.

What is the maximum number of electrons that can be present in each principal energy level of hydrogen?

a)

n

b)

n2

c)

2n

d)

2n2

41.

What is the lowest energy state of an atom called?

a)

the ground state

b)

the excited state

c)

the solid state

d)

the chaotic state

42.

How many electrons can fit into a d- orbital?

a)

6

b)

2

c)

8

d)

10

43.

for each set of quantum numbers, which set is correct

a)

n = 1 ℓ = 1 mℓ = 0 ms = +1/2

b)

n = 2 ℓ = 0 mℓ = -1 ms = +1/2

c)

n = 3 ℓ = 2 mℓ = -1 ms = -1/2

d)

n = 2 ℓ = 1 mℓ = -2 ms = +1/2

44.

when n= 3

a)

ℓ = 3

b)

m ℓ = 4

c)

ℓ =0

d)

ms= +1

45.

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

a)

n= 2

b)

ℓ = 2

c)

3 orbitals

d)

spherical shape

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