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Electron Configuration Test Review

Total questions: 50

Worksheet time: 25mins

Name
Class
Date
1.

1s2 2s2 is which element?

a)

Lithium

b)

Beryllium

c)

Helium

d)

Boron

2.

What is the configuration for Carbon?

a)

1s2 2p2

b)

1s2 2s2 2p2

c)

1s1 1s2 2s2 2p2

3.

Iron (Fe) configuration is

a)

1s2 2s2 2p6 3s2 3p3

b)

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

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d6

4.

Write the configuration for Oxygen

a)

1s2 2s2 1p4

b)

2s2 2p4

c)

1s2 2s2 3p4

d)

1s2 2s2 2p4

5.

Write the configuration for Phosphorus

a)

2s2 2p6 3s2 3p3

b)

1s2 2s3 2p6 3p3

c)

1s2 2s2 2p6 3s2 3p3

6.

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

a)

Sodium (Na)

b)

Lithium (Li)

c)

Potassium (K)

d)

Calcium (Ca)

7.

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

a)

Chlorine

b)

Bromine

c)

Krypton

d)

Sulfur

8.

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

9.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

10.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
11.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
12.

There are 4 different types of subshells(orbitals) s,p,d,f

a)

true

b)

false

13.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
14.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

15.

Energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

16.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
17.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
18.
Which element is depicted from this atomic orbital diagram?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Phosphorus
19.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
20.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
21.

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

22.
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
23.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

e)

None of these

24.

Which orbital shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

e)

None of these

25.
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
26.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
27.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
28.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
29.
What is the noble gas configuration for phosphorus?
a)
[Ar] 3p5
b)
[He] 3s2 3p5
c)
[Ne] 3s2 3p3
d)
[Na] 3s2 3p5
30.
What is the noble gas configuration for boron?
a)
[He]1s22s2
b)
[He]2s22p2
c)
[He]2s22p1
d)
[Li]2s22p1
31.
[Ne]3s23p5 is the noble gas configuration for which element?
a)
chlorine
b)
fluorine
c)
sulfur
d)
aluminum
32.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

33.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
34.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
35.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

36.

Light is emitted when electrons ...

a)

return from high energy state to low energy state

b)

jump from low energy state to high energy state

c)

either of these

d)

none of these

37.
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
38.

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

39.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
40.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

set state

d)

ground state

41.

Which part of the electromagnetic spectrum has the shortest wavelength?

a)

Radio waves

b)

Microwaves

c)

X-rays

d)

Gamma rays

42.

The number of waves that pass a given point every second

a)

Frequency

b)

Wavelength

c)

Energy

d)

Electromagnetic Spectrum

43.

The distance between the crests of two waves

a)

Frequency

b)

Wavelength

c)

Energy

d)

Electromagnetic Spectrum

44.

As wavelength increases: frequency,_____________ and energy ______________.

a)

Increases; decrease

b)

Increases; increases

c)

Decreases; decreases

d)

Decrease; increases

45.

Based on the picture, which of the following types of electromagnetic radiation has the LOWEST energy?

a)

microwave

b)

ultraviolet

c)

infrared

d)

x-rays

46.

On the electromagnetic spectrum, radio waves are found on the end of the spectrum considered to possess a low amount of energy. Which statement most accurately describes the wavelength/frequency relationship present in radio waves?

a)

Radio waves possess both low frequencies and small wavelengths.

b)

Radio waves possess both high frequencies and large wavelengths.

c)

Radio waves possess high frequencies and small wavelengths.

d)

Radio waves possess low frequencies and large wavelengths.

47.

The visible light that we can see travels in waves. Blue light has a wavelength of 450 nm and orange light has a wavelength of 600 nm. Based on this information, what is true about the energies of blue and orange light?

a)

Energy of blue light will be higher than that of orange light.

b)

Energy of blue light will be lower than that of orange light.

c)

Energy of blue light and orange light will be the same.

d)

Wavelengths of light and energy of light are independent of each other.

48.

What is the noble gas configuration for Neon?

a)

[Ne]

b)

[He]2s22p6

c)

[F]2p1

d)

[Ne]2s21p6

49.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
50.
Identify the element for
[Xe] 6s2 4f14 5d4
a)
Cobalt
b)
Iron
c)
Tungstun

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