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Electron Configuration

Total questions: 52

Worksheet time: 1hrs 18mins

Name
Class
Date
1.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
2.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
3.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
4.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
5.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
6.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
7.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
8.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
9.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
10.
What element has the valence shell configuration
3s2 3p2
a)
Al
b)
B
c)
Si
d)
Ga
11.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
12.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
13.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
14.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
15.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
16.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
17.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
18.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
19.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
20.
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
21.
What does Hund's rule states ?
a)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
22.

Write the configuration for Phosphorus

a)

2s2 2p6 3s2 3p3

b)

1s2 2s3 2p6 3p3

c)

1s2 2s2 2p6 3s2 3p3

d)

1s2 2s2 2p5 3s2 3p3

23.

Which element is 1s2 2s2 2p6 3s2 3p6 4s1?

a)

Sodium (Na)

b)

Lithium (Li)

c)

Potassium (K)

d)

Calcium (Ca)

24.

Choose the correct configuration for Zinc

a)

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

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d9

c)

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

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

25.

Choose the correct element for 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

a)

Chlorine

b)

Bromine

c)

Krypton

d)

Sulfur

26.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
27.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
28.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
29.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
30.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
31.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
32.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

33.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
34.

Identify the Electron Configuration for Aluminum (Al)

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3p3

c)

1s2 2s2 2p6 3s2 4p1

35.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
36.

What is the noble gas notation electron for Sulfur?

a)

[Ne] 3p4

b)

[He] 3s2 3p4

c)

[Ne] 3s2 3p4

d)

[Na] 3s2 3p4

37.

Whta is the noble gas notation for V?

a)

[Ar] 4s2 4d2

b)

[Kr] 4s2 3d3

c)

[Ar] 4s2 4d3

d)

[Ar] 4s2 3d3

38.

What is the noble gas configuration for silicon?

a)

[Ne] 3s2 3p1

b)

[Ar] 4s1

c)

[Kr] 5s1

d)

[Ne] 3s2 3p2

39.
Question Image

Match the parts of the electron configuration to what it represents.

a)

1

1.

Energy Level

b)

s

2.

Sublevel

c)

2

3.

# of electrons

40.

Finish the electron configuration for chlorine:

1s2 2s2 (a)   3s2 3p5

41.

What is the missing piece?

1s2 2s2 ___ 3s1

a)

2p6

b)

2p4

c)

3p6

d)

3s2

42.

What are the missing pieces?

1s2 2s2 2p6 ___ 3p6 4s2 ___ 4p2

a)

3s2 , 4d10

b)

2p4 , 3d10

c)

3p6 , 3d10

d)

3s2 , 3d10

43.

Match the element to it's noble gas notation:

a)

krypton

1.

[Kr]

b)

silicon

2.

[Ne] 3s2 3p2

c)

strontium

3.

[Kr] 5s2

d)

copper

4.

[Ar] 4s2 3d9

44.

Reorder these from shortest electron configuration to the longest:

a)

hydrogen

b)

boron

c)

argon

d)

calcium

e)

xenon

1)
2)
3)
4)
5)
45.

Explain the significance of valence electrons in an atom.

a)

Valence electrons have no impact on the behavior of the atom.

b)

Valence electrons determine the atomic weight of the atom.

c)

Valence electrons are responsible for the color of the atom.

d)

Valence electrons determine the reactivity and bonding behavior of an atom.

46.

Valence electrons are located...

a)

inside the nucleus

b)

in outer space

c)

on the outermost orbit of an atom

47.
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.
48.
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
49.
Which element is depicted from this atomic orbital diagram?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Phosphorus
50.
What is the correct configuration for uranium?
a)
[Xe] 6s2 4d 3
b)
[Rn] 7s2 5f3 6d1
c)
[Rn] 7s2 5f4 
d)
[Rn] 7s2 6d1 6f3
51.
What is the correct configuration for lead?
a)
[Rn] 6s2  4f14 5d10 6p2
b)
[Xe] 6s2 6d10 6p2
c)
[Xe] 6s2 5d10 6p2
d)
[Xe] 6s2  4f14 5d10 6p2
52.
In an orbital diagram,  an arrow represents: 
a)
an electron
b)
an orbital
c)
an element

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