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CHEM | Orbital Diagrams + Electron Configurations

Total questions: 70

Worksheet time: 6hrs 50mins

Name
Class
Date
1.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
2.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
3.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
4.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
5.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
6.
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
d)
All the arrows should be pointing up.
7.
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
8.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
9.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
10.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
11.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
12.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
13.
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
14.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
15.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
16.

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)

There should be 1 electron (arrow) in the first 2p box and one in the 2nd 2p box

d)

All the arrows should be pointing up.

17.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
18.

How many electrons can a d orbital hold?

a)
14
b)
10
c)
2
d)
6
19.

Which rule is being violated in the following orbital diagram?

a)

Hund's

b)

Aufbau's

c)

Pauli's Exclusive

20.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
21.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
22.

This shape is that of a/n:

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

23.

How many orbitals are there in the d sublevel?

a)

1

b)

3

c)

5

d)

7

24.

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

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

25.

Which of the following is the electron configuration for Fluorine

a)
b)
c)
d)
26.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
27.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
28.

What element has this electron configuration?

a)

hydrogen

b)

helium

c)

lithium

d)

beryllium

29.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

30.

What element has this electron configuration?

a)

helium

b)

lithium

c)

beryllium

d)

boron

31.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

32.

Which element is represented by this electron configuration?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

33.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

34.

Which of the following is the electron configuration for neon?

a)
b)
c)
d)
35.

Which of the following is the electron configuration for silicon?

a)
b)
c)
d)
36.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
37.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
38.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
39.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
40.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
41.

What is the element?

a)

Neon

b)

Chlorine

c)

Aluminum

d)

Argon

42.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
43.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
44.

Elements in the same ___ have the same number of Valence electrons.

a)

period

b)

group

45.

Elements in the same ___ have the same number of energy levels.

a)

period

b)

group

46.

How many energy levels does element #2 have ?

a)

6

b)

7

c)

3

d)

4

e)

5

47.

How many energy levels does element #3 have ?

a)

6

b)

7

c)

3

d)

4

e)

5

48.

How many energy levels does element #1 have ?

a)

6

b)

2

c)

3

d)

4

e)

5

49.

How many energy levels does element #4 have ?

a)

6

b)

2

c)

3

d)

4

e)

5

50.

How many valence electrons does element #3 have?

a)

5

b)

17

c)

7

d)

1

e)

3

51.

How many valence electrons does element #1 have?

a)

14

b)

4

c)

6

d)

5

e)

8

52.

How many valence electrons does element #4 have?

a)

14

b)

4

c)

6

d)

5

e)

8

53.

How many valence electrons does the element #1 have?

a)

15

b)

2

c)

7

d)

4

e)

5

54.

How many valence electrons does the element #2 have?

a)

1

b)

2

c)

3

d)

4

e)

5

55.

Which letter represents an element in the f-block of the periodic table ?

a)

1

b)

2

c)

3

d)

4

56.

Which letter represents an element in the d-block of the periodic table  ?

a)

1

b)

2

c)

3

d)

4

57.

Which letter represents an element in the p-block of the periodic table  ?

a)

1

b)

2

c)

3

d)

4

58.

Which letter represents an element in the s-block of the periodic table  ?

a)

1

b)

2

c)

3

d)

4

59.

Which number on the periodic table would represent an element with an electron configuration ending in 3p63p^6  ?

a)

1

b)

2

c)

3

d)

4

60.

Which number on the periodic table would represent an element with an electron configuration ending in 2p22p^2  ?

a)

1

b)

2

c)

3

d)

4

61.

Which number on the periodic table would represent an element with an electron configuration ending in 3d53d^5  ?

a)

1

b)

2

c)

3

d)

4

62.

Which number on the periodic table would represent an element with an electron configuration ending in 4s24s^2  ?

a)

1

b)

2

c)

3

d)

4

63.

Which number on the periodic table would represent an element with an electron configuration ending in 3p53p^5  ?

a)

1

b)

2

c)

3

d)

4

64.

Which number on the periodic table would represent an element with an electron configuration ending in 4d94d^9  ?

a)

1

b)

2

c)

3

d)

4

65.

Which number on the periodic table would represent an element with an electron configuration ending in 4f104f^{10}  ?

a)

1

b)

2

c)

3

d)

4

66.

Which number on the periodic table would represent an element with an electron configuration ending in 7s17s^1  ?

a)

1

b)

2

c)

3

d)

4

67.

Which number on the periodic table would represent an element with an electron configuration ending in 4p34p^3  ?

a)

1

b)

2

c)

3

d)

4

68.

Which number on the periodic table would represent an element with an electron configuration ending in 5f75f^7  ?

a)

1

b)

2

c)

3

d)

4

69.

Which number on the periodic table would represent an element with an electron configuration ending in 5s15s^1  ?

a)

1

b)

2

c)

3

d)

4

70.

This is the shape of ____ orbital

a)

s

b)

d

c)

p

d)

d

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