wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Orbitals, Electrons, Electron Configuration

Total questions: 112

Worksheet time: 5hrs 54mins

Name
Class
Date
1.

Choose the correct electron configuration for Beryllium (Be).

a)

1s1

b)

1s2 2s2

c)

1s2 2s2 2p1

2.

Choose the correct electron configuration for Chlorine (Cl).

a)

1s2 2s2 2p1

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s2 3p5

3.

Choose the correct electron configuration for Nickel (Ni).

a)

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

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d2

c)

1s2 2s2 2p6 3s2 3p6 4s10

4.

Choose the correct electron configuration for Krypton (Kr).

a)

1s2 2s2 2p6 3s2 3p6 4s8 3d8

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d8 4p3

c)

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

5.

Choose the correct electron configuration for Terbium (Tb).

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d19 5p6 6s2

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f9

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f5

6.
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
7.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)

Zinc (Zn)

b)

Copper (Cu)

c)

Nickel (Ni)

d)

Germanium (Ge)

8.

What electron configuration matches an oxygen (O) atom?

a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
9.
What atom matches this electron configuration?
1s22s22p63s2
a)

Neon (Ne)

b)

Magnesium (Mg)

c)

Aluminum (Al)

d)

Potassium (K)

10.

Write the configuration for Phosphorus (P)

a)

2s2 2p6 3s2 3p3

b)

1s2 2s3 2p6 3p3

c)

1s2 2s2 2p6 3s2 3p3

d)

1s2 2s2 2p5 3s2 3p3

11.

Choose the correct configuration for Neon (Ne).

a)

1s2 2s2 2p6 3s2 3p6

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6

d)

1s2 2s1 2p6

12.
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
13.

What is the electronic configuration of iron (Fe)?

a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
14.

What element has the following electron configuration?

1s22s22p63s23p64s23d104p65s1

a)

Rubidium (Rb)

b)

Halfnium (Hf)

c)

Aluminum (Al)

d)

Potassium (K)

15.

What element has the following electron configuration:

1s22s22p63s23p64s23d104p5

a)

Bromine (Br)

b)

Chlorine (Cl)

c)

Calcium (Ca)

d)

Manganese (Mn)

16.

Look carefully at the picture. It shows an electron in the excited state on the left, and the electron returning to its ground state on the right. When the electron return to the ground state it emits a_______________________.

a)

blast of cold air

b)

electrostatic charge

c)

proton

d)

photon (light)

17.

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

a)

Ground State

b)

Excited State

18.

Take a close look at the picture. What is this called?

a)

the color of life

b)

lucky charms

c)

spectral line

d)

electron cloud

19.

Line emission spectra is produced from atoms when

a)

electrons release energy as they move to their excited state.

b)

electrons absorb energy as they move to their excited state.

c)

electrons release energy as they return to the ground state.

d)

electrons absorb energy as they return to the ground state.

20.

The color of emitted light with lowest energy is

a)

violet

b)

green

c)

red

d)

indigo

21.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
22.

When an electron moves from n=2 (energy level 2) to n=4 (energy level 4)

MULTIPLE ANSWERS: CHECK ALL CORRECT ANSWERS

a)

it must absorb light

b)

it will release light

c)

it will move farther from the nucleus

d)

it will move closer to the nucleus

23.

High frequency waves have _________ wavelengths.

a)

varying

b)

long

c)

the same

d)

short

24.
There is an emission spectrum and absoption spectrum shown here. What is the bottom spectrum?
a)
an emission spectrum
b)
an absoption spectrum
c)
neither
d)
both 
25.
The splitting of white light into a spectrum is called...
a)
diffraction
b)
dispersion
c)
divergence
d)
refraction
26.
The type of spectrum generated here is called...
a)
absoption
b)
continuous
c)
constant
d)
emission
27.
The arrows pointing down represents...
a)
photon absorption
b)
proton emission
c)
electron absorption
d)
electron transition
28.
The parallel lines represents...
a)
energy levels of the atom
b)
energy levels of the electrons
c)
energy levels of the photons
d)
energy levels of the nucleus
29.
Light is emitted when electrons ...
a)
jump from high to low 
b)
jump from low to high 
c)
either of these
d)
none of these
30.
As the energy level increases the difference in the energy level ...
a)
increases
b)
decreases
c)
stays the same
d)
none of these
31.
There are seven arrows shown. Which would correspond to the longest wavelength?
a)
the left Lyman arrow
b)
the right Lyman arrow
c)
the left Balmer arrow
d)
the Paschen arrow
32.

What evidence did you observe that proves that elements give off their own unique color spectrum?

a)

All of the gas tubes produced a full spectrum. (A rainbow.)

b)

When we looked at white light through a prism, we saw the rainbow.

c)

Each gas tube gave off its own unique color and color spectrum when we looked at the light through the spectroscope. None of them were the exact same.

d)

Each gas tube gave off the same color and color spectrum when we looked at the light through a spectroscope.

33.

A ground state electron is

a)

freshly crushed into a fine powder.

b)

in the highest possible energy level.

c)

in the lowest possible energy level.

d)

constantly emitting light.

34.
A line spectrum is produced when an electron moves from one energy level
a)
into the nucleus.
b)
to another position in the same sublevel.
c)
to a higher energy level.
d)
to a lower energy level.
35.

What type of spectrum is shown?

a)

emission

b)

absorption

c)

visible

d)

photon

36.
Which type of orbital is shaped like a sphere?
a)
s orbital
b)
p orbital
c)
d orbital
d)
f orbital
37.

There are _____ types of atomic orbitals.

a)

1

b)

2

c)

3

d)

4

38.

Which of the following are TRUE of atomic orbitals?

a)

There is 1 s orbital

b)

There are 3 p orbitals

c)

There are 5 d orbitals

d)

There are 7 f orbitals

39.

How many electrons can fit in one orbital?

a)

1

b)

2

c)

3

d)

4

40.

Look at a periodic table. Count how many columns on the periodic table are in the "p" block. How many columns did you find?

a)

2

b)

6

c)

10

d)

14

41.

If the f block contains 14 columns, then it would make sense that an f orbital can hold up to _____ electrons.

a)

2

b)

5

c)

7

d)

14

42.

Using your orbital filling cheat sheet, tell me which orbital fills after the 2 p orbital is full.

a)

3p

b)

3s

c)

2s

d)

1p

43.

Using your orbital filling cheat sheet, which orbital fills after the 4s orbital?

a)

4p

b)

5s

c)

3d

d)

4f

44.
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
45.
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
46.
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
47.
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
48.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
49.
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.
50.
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
51.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
52.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
53.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
54.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
55.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
56.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
57.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
58.
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.
59.
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
60.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
61.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
62.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
63.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
64.
Which element is depicted from this atomic orbital diagram?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Phosphorus
65.
What is the name of this element?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
66.
How many electrons should Carbon have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
67.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
68.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
None of these
69.
What group does this element belong to?
a)
Group 1: Alkali metals
b)
Group 18: Noble Gases
c)
Group 2: Alkaline-Earth Metals
d)
Group 17: Halogens
70.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
71.
What is the shape of a p orbital?
a)
sphere
b)
it's just too complex to thing about it
c)
dumbbell
d)
pyramidal
72.

This orbital diagram represents:

a)

C

b)

B

c)

N

d)

O

73.
Maximum number of electrons that can be placed in an s orbital.  
a)
2
b)
6
c)
10
d)
14
74.

The maximum number of electrons that can be placed in the p subshell.

a)

2

b)

6

c)

10

d)

14

75.

How many orbitals inhabit the d subshell?

a)

1

b)

3

c)

5

d)

7

76.

How many electrons can inhabit the f subshell?

a)

6

b)

7

c)

10

d)

14

77.

What atom matches this electron configuration?

1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

78.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
79.

Which orbital shows a violation of the Aufbau Principle?

a)

A

b)

B

c)

C

d)

D

80.

What is the Electron Configuration of Helium?

a)

1s2

b)

1s1

c)

2s1

d)

1s22s1

81.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
82.

Choose the correct electron configuration for Nitrogen:

a)

1s2 2s2 2p6

b)

1s2 2s2 2p8

c)

1s2 2s2 2p1

d)

1s2 2s2 2p3

83.

In the Quantum Mechanic Model of the atom there are four orbital present and they are named --> s, p, d, f

a)

true

b)

false

84.

How many electrons can the "d" orbital hold at maximum?

a)

14

b)

10

c)

2

d)

6

85.

How many electrons can the "s" orbital hold at maximum?

a)

14

b)

10

c)

2

d)

6

86.

How many electrons can the "p" orbital hold at maximum?

a)

14

b)

10

c)

2

d)

6

87.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
88.

Which part of the orbital diagram has the highest energy?

a)

2p

b)

2s

c)

3p

d)

1s

89.

Which element does this orbital diagram represents?


** You need to look these element symbols up on a periodic table and determine the number of electrons.

a)

C

b)

B

c)

N

d)

O

90.

Which element does this orbital diagram represents?


** You need to look these element symbols up on a periodic table and determine the number of electrons.

a)

C

b)

B

c)

N

d)

O

91.
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 there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
92.

Which element is pictured in this orbital diagram?


** You need to look these elements up on a periodic table and determine the number of electrons.

a)

neon

b)

fluorine

c)

magnesium

d)

argon

93.
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
94.

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 electrons 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

95.

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 electrons have opposite spins

96.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
97.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
98.

What atom matches this electron configuration?

1s22s22p63s23p64s23d10


** You need to look these elements up on a periodic table and determine the number of electrons and use the Electron Fill Order Chart (from orbital diagram activities).

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

99.

Which electron configuration belongs to Chlorine (Cl)?


** You need to look these elements up on a periodic table and determine the number of electrons and use the Electron Fill Order Chart (from orbital diagram activities).

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

100.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
101.

What electron configuration matches an oxygen atom?


** You need to look these elements up on a periodic table and determine the number of electrons and use the Electron Fill Order Chart (from orbital diagram activities).

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

102.

Identify the Electron Configuration for Aluminum (Al)


** You need to look these elements up on a periodic table and determine the number of electrons and use the Electron Fill Order Chart (from orbital diagram activities).

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3p3

c)

1s2 2s2 2p6 3s2 4p1

103.

The number of arrows placed in an orbital diagram = the number of...

a)

atoms

b)

electrons

c)

protons

d)

neutrons

104.

electron configuration tells us the ____ of the electron whereas the orbital configuration tells us the _____ of the electrons.

a)

spin, location

b)

size, location

c)

location, size

d)

location, spin

105.

How many electrons can be held at most in the p subshell?

a)

2

b)

6

c)

10

d)

14

106.

Which rule said that orbitals get one arrow(electron) first then get paired up by getting a second electron?

a)

Aufbau

b)

Hund's

c)

Pauli

107.

Which element has this orbital configuration?

a)

Hydrogen (Atomic # = 1)

b)

Helium (Atomic # = 2)

c)

Lithium (Atomic # = 3)

d)

Beryllium (Atomic # = 4)

108.

Which is the correct orbital notation for nitrogen (atomic # = 7)

a)
b)
c)
d)
109.

Which rule is described as opposite and paired?

a)

Aufbau

b)

Pauli

c)

Hund's

110.

Which rule is violated in this orbital diagram?

a)

Aufbau

b)

Pauli

c)

Hund's

111.

Which rule is violated in this orbital diagram?

a)

Aufbau

b)

Pauli

c)

Hund's

112.

each orbital (box) can hold a max of __ electrons

a)

1

b)

2

c)

6

d)

depends

Similar Resources on Wayground

List of -ectomies

111 questions

List of -ectomies

quiz

Worksheet

•

1st Grade - Professio...