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WorksheetsElectron Configurations
Total questions: 55
Worksheet time: 2hrs 54mins
Name
Class
Date
1.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
2.
What atom matches this electron configuration?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
3.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
4.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
5.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
6.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
7.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
8.
What is this element?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
9.
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
10.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
11.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
12.
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
13.
What is the electron configuration of sodium?
a)
2.8
b)
2.8.2
c)
2.8.1
d)
11
14.
What is the electron configuration of calcium?
a)
2.8.8.2
b)
2.8.10
c)
20
d)
2.18.2
15.
What is the electron configuration of Aluminium?
a)
2.8.3
b)
2.11
c)
13
d)
2.8.2
16.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
17.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
18.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
19.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
20.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
21.
What is this element?
1s22s22p63s23p6
4s23d104p6
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
22.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
23.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
24.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
25.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
26.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
27.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
28.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
29.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
30.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
31.
What is the electron configuration of Iodine?
a)
[Kr]5s24d105p6
b)
[Kr]5s24d106p6
c)
[Kr]5s25d106p6
d)
None of the above
32.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
33.
What atom matches this electron configuration?
[Xe] 6s24f145d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
34.
There are __ energy levels
a)
1
b)
2
c)
7
d)
8
35.
How many atomic orbitals are there in the p sublevel?
a)
2
b)
3
c)
4
d)
5
36.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
37.
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
38.
[Ne]3s23p5 is the noble gas configuration for which element?
a)
chlorine
b)
fluorine
c)
sulfur
d)
aluminum
39.
Is the following electron configuration correct? Why or why not?
1s22s22p63s23p64s24d104p65s1
a)
No. 4p6 should be after 5s1.
b)
No. It should be 3d10 not 4d10
c)
Yes. All electrons are represented properly.
d)
Yes.
40.
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
41.
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
42.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that -no two electrons in the same orbital can have the same spin
c)
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
43.
What is the maximum number of electrons that an S orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
44.
How many electrons can the d sublevel(orbital) hold?
a)
8
b)
10
c)
2
d)
4
45.
What is this element?
1s22s22p63s23p64s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
46.
There are 4 different types of subshells(orbitals) s,p,d,f
a)
true
b)
false
47.
Which area on the periodic table represents the electrons in the "d" sublevel?
a)
representative elements
b)
columns 3-8
c)
rare earth elements
d)
transition elements
48.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
49.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
50.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
c)
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
51.
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
52.
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
53.
What atom matches this electron configuration?
[Xe] 6s25d9
[Xe] 6s25d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
54.
What atom is represented here?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Fluorine
55.
Which element is depicted from this atomic orbital diagram?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Phosphorus
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