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Electron Configuration Practice

Total questions: 60

Worksheet time: 2hrs 54mins

Name
Class
Date
1.

What is the electron configuration for Beryllium?

a)

1s2 2s2

b)

1s2 2s1 2p1

c)

1s2 2p2

d)

1s2 1p2

2.

Which element has the following electron configuration?

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1

a)

Krypton

b)

Rubidium

c)

Yttrium

d)

Potassium

3.

What is the electron configuration for Aluminum?

a)

1s2 2s2 2p6 3d10

b)

1s2 2s2 2p6

c)

1s2 2s2 2p3 3s2 3p1

d)

1s2 2s2 2p6 3s2 3p1

4.

Which of the following is the correct order of the levels for electron configuration?

a)

1s2s3s4s5s2p3p4p5p3d4d5d4f5f

b)

1s1p2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p

c)

1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p

d)

1s1p2s2p3s3d3p4s4d4p5s5d5p6s4f6d6p

5.

What is the electron configuration for phosphorus?

a)

1s2 2s2 2p6 3s2 3p3

b)

1s2 2s2 2p6 3p5

c)

1s2 2s2 2p6 3s1 3p4

d)

1s2 2s2 2p6 3s2 3d3

6.

Which neutral element has the following electron configuration?

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d7

a)

Cobalt

b)

Rhodium

c)

Manganese

d)

Technetium

7.

What is the electron configuration for magnesium?

a)

1s2 2s2 2p6 3s1 3p1

b)

1s2 2s2 2p6 3p2

c)

1s2 2s2 2p6 3d2

d)

1s2 2s2 2p6 3s2

8.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
9.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
10.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
11.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
12.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
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.

What is the noble gas configuration for Cobalt?

a)

[Kr] 4s2 3d7

b)

[Kr] 4s2 4d7

c)

[Ar] 4s2 3d7

d)

[Ar] 4s2 4d7

15.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
16.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
17.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
18.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
19.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
20.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
21.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
22.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
23.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
24.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
25.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
26.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
27.
1.  What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
28.

Which orbital shows a violation?

a)
A
b)
B
c)
C
d)
D
29.

What atom matches this electron configuration?

[Xe] 6s2 4f14 5d10

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

30.
[He]2s22p4 is the noble gas configuration for which element?
a)
oxygen
b)
sulfur
c)
phosphorus
d)
fluorine
31.
[Ne]3s23p1 is the noble gas configuration for which element?
a)
scandium
b)
boron
c)
nitrogen
d)
aluminum
32.

What is the noble gas shorthand electron for Phosphorus atom?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p3

d)

[Na] 3s23p4

33.
How many total electrons can be held in the third energy level of an atom?
a)
8
b)
18
c)
32
d)
12
34.

Which block of elements are known as transition elements?

a)

s block

b)

p block

c)

d block

d)

f block

35.

Which of the following states that electrons occupy orbitals of lowest energy first?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

36.

What does the Pauli Exclusion Principle state?

a)

An orbital can only hold a maximum of 2 electrons, each with opposite spins

b)

An orbital can hold a minimum of 6 electrons, each with opposite spins

c)

An orbital can hold a maximum of 6 electrons, each with the same spin

d)

An orbital can hold a maximum of 2 electrons, each with the same spin

37.

Which orbital diagram violates of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

38.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
39.
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.
40.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
41.
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
42.
The maximum number of electrons that can be placed in an f orbital.  
a)
2
b)
6
c)
10
d)
14
43.
In an orbital diagram,  an arrow represents: 
a)
an electron
b)
an orbital
c)
an element
44.

This orbital diagram represents

a)

Sodium

b)

Magnesium

c)

Aluminum

d)

Iron

45.

Which of the following is the electron configuration for silicon?

a)
b)
c)
d)
46.

What is incorrect about this electron configuration for calcium (Ca): 1s22s22p63s23p8

a)

There are not enough electrons in the 3p orbital. There should be 10 electrons in the 3p orbital.

b)

There are too many electrons in the 3p orbital. There should be 6 electrons in the 3 p orbital.

c)

There are too many electrons in the 3p orbital AND the electrons should be in the next orbital, 4s.

d)

There are too many total electrons.

47.

In an electron configuration, an exponent represents...

a)

the electrons

b)

the orbital location of an electron

c)

an element

d)

an energy level or row on the periodic table

48.
This orbital fill after the s,  the shape is a dumbbell. 
a)
s
b)
p
c)
d
d)
f
49.

This shape is that of

a)

s-orbital

b)

d-orbital

c)

p-orbital

d)

f-orbital

50.

How many orbitals does an s sublevel have?

a)

1

b)

3

c)

5

d)

7

51.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

52.

Which statement is true about "p" orbitals?

a)

A subshell that contains three "p" orbitals.

b)

These orbitals are shaped like dumbbells.

c)

A 3p orbital has a higher energy than a 2p orbital.

d)

All of these statements are true

53.

Which block (s, p, d, or f) contains the non-metals?

a)

s block

b)

p block

c)

d block

d)

f block

e)

both d and f

54.

Which of the following elements will have electrons in the d orbitals?

a)

silver

b)

sodium

c)

sulfur

d)

helium

55.
What is this element? 
[Ar]4s2
a)
Calcium
b)
Sodium
c)
Scandium
d)
Titanium
56.

What is the electronic configuration of sodium?

a)

1s22s22p63s1

b)

[Ne]3s1

c)

1s22s22p7

d)

Two of the choices are correct

57.

Which of the following is the correct electron configuration for cadmium?

a)

1s22s22p63s23p64s23d104p65s25d10

b)

1s22s22p63s23p64s24d104p65s24d10

c)

1s22s22p63s23p64s23d104p65s24d10

d)

1s22s22p63p64s23d104p65s24d10

58.

Which of the following is the correct electron configuration for Vanadium?

a)

1s22s22p63s23p64s24d3

b)

1s22s22p63s23p64s23d3

c)

1s22s22p63s23p64s2

d)

1s22s22p63s23p64s23d6

59.

Which of the following is the correct electron configuration for helium?

a)

1s1

b)

2s2

c)

2p6

d)

1s2

60.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons

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