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Chemistry Exam #5 Review: Electron Configurations

Total questions: 100

Worksheet time: 2hrs 36mins

Name
Class
Date
1.

The distance between the crests of two waves

a)

Frequency

b)

Wavelength

c)

Energy

d)

Electromagnetic Spectrum

2.

Broad range of radiation that carries energy as waves

a)

Frequency

b)

Wavelength

c)

Energy

d)

Electromagnetic Spectrum

3.

As wavelength increases: frequency,_____________ and energy ______________.

a)

Increases; decrease

b)

Increases; increases

c)

Decreases; decreases

d)

Decrease; increases

4.

As wavelength decreases: frequency,_____________ and energy ______________.

a)

Increases; decrease

b)

Increases; increases

c)

Decreases; decreases

d)

Decrease; increases

5.

The number of waves that pass a given point every second

a)

Frequency

b)

Wavelength

c)

Energy

d)

Electromagnetic Spectrum

6.

The highest point of a wave is called:

a)

Wave Height

b)

Trough

c)

Amplitude

d)

Crest

7.

The lowest point of a wave is called:

a)

Wave Height

b)

Trough

c)

Amplitude

d)

Crest

8.

Which wave has the highest energy?

a)

A

b)

B

c)

C

d)

You cannot tell from this diagram.

9.

Which color waves have the lowest frequency?

a)

red

b)

yellow

c)

green

d)

violet

10.

Which color waves have the shortest wavelength?

a)

red

b)

yellow

c)

green

d)

violet

11.

Which EM waves are have the highest energy & are the most dangerous?

a)

radio

b)

gamma rays

c)

infrared

d)

x-rays

12.

Which EM waves are have the lowest frequency?

a)

radio

b)

none

c)

infrared

d)

x-rays

13.

Which EM waves are invisible? (more than one correct answer)

a)

radio

b)

visible

c)

ultraviolet

d)

gamma rays

14.

Which EM waves have the longest wavelength?

a)

radio

b)

x-rays

c)

ultraviolet

d)

gamma rays

15.

Which EM waves have the shortest wavelength?

a)

radio

b)

x-rays

c)

ultraviolet

d)

gamma rays

16.

Which electromagnetic waves are used in devices such as heat lamps & TV remote controls?

a)

Ultraviolet Rays

b)

Microwaves

c)

Infrared Rays

d)

Gamma Rays

17.

Which of the following is arranged in decreasing frequency?

a)

radio waves, microwaves, x-rays, gamma rays

b)

gamma rays, x-rays, infrared, visible light

c)

microwaves, infrared, ultraviolet waves, gamma rays

d)

x-ray, ultraviolet waves, microwaves, radiowaves

18.

The following are uses in radiowaves EXCEPT:

a)

Magnetic Resonance Imaging

b)

Heat Lamps

c)

Television

d)

Universal Product Code

19.

What do all forms of electromagnetic radiation have in common?

a)

Their strength

b)

Their speed

c)

Their wavelength

d)

Their frequency

20.

What produces electromagnetic radiation?

a)

Electrons changing energy levels

b)

Electrons bonding with other atoms

c)

Electrons leaving the atomic nucleus

d)

Electrons becoming protons or neutrons

21.
Radar uses which type of electromagnetic waves to detect objects & measure their distance and speed?
a)
microwaves
b)
infrared rays
c)
x-rays
d)

Visible Light

22.

What block is represented by the colour green?

a)

p-block

b)

d-block

c)

s-block

d)

f-block

23.

What block is represented by the colour yellow?

a)

p-block

b)

d-block

c)

s-block

d)

f-block

24.

What block is represented by the colour blue?

a)

p-block

b)

d-block

c)

s-block

d)

f-block

25.

What block is represented by the colour red?

a)

p-block

b)

d-block

c)

s-block

d)

f-block

26.

Period 1 has which blocks present? Choose all that apply

a)

S Block

b)

P Block

c)

D Block

d)

F Block

27.

Period 2 has which blocks present? Choose all that apply

a)

S Block

b)

P Block

c)

D Block

d)

F Block

28.

Period 3 has which blocks present? Choose all that apply

a)

S Block

b)

P Block

c)

D Block

d)

F Block

29.

Period 4 has which blocks present? Choose all that apply

a)

S Block

b)

P Block

c)

D Block

d)

F Block

30.

Period 5 has which blocks present? Choose all that apply

a)

S Block

b)

P Block

c)

D Block

d)

F Block

31.

Period 6 has which blocks present? Choose all that apply

a)

S Block

b)

P Block

c)

D Block

d)

F Block

32.

Period 7 has which blocks present? Choose all that apply

a)

S Block

b)

P Block

c)

D Block

d)

F Block

33.

Energy Level 1 (Period 1) holds how many electrons

a)

2 Electrons

b)

8 electrons

c)

18 electrons

d)

32 Electrons

34.

Energy Level 2 (Period 2) holds how many electrons

a)

2 Electrons

b)

8 electrons

c)

18 electrons

d)

32 Electrons

35.

Energy Level 3 (Period 3) holds how many electrons

a)

2 Electrons

b)

8 electrons

c)

18 electrons

d)

32 Electrons

36.

Energy Level 4 (Period 4) holds how many electrons

a)

2 Electrons

b)

8 electrons

c)

18 electrons

d)

32 Electrons

37.

Energy Level 5 (Period 5) holds how many electrons

a)

2 Electrons

b)

8 electrons

c)

18 electrons

d)

32 Electrons

38.

Energy Level 6 (Period 6) holds how many electrons

a)

2 Electrons

b)

8 electrons

c)

18 electrons

d)

32 Electrons

39.

Energy Level 7 (Period 7) holds how many electrons

a)

2 Electrons

b)

8 electrons

c)

18 electrons

d)

32 Electrons

40.

S-Block Elements are found in which groups?

a)

Groups 1 and 2

b)

Groups 3-12

c)

Groups 13-18

d)

Lanthanide and Actinide Series

41.

P-Block Elements are found in which groups?

a)

Groups 1 and 2

b)

Groups 3-12

c)

Groups 13-18

d)

Lanthanide and Actinide Series

42.

D-Block Elements are found in which groups?

a)

Groups 1 and 2

b)

Groups 3-12

c)

Groups 13-18

d)

Lanthanide and Actinide Series

43.

F-Block Elements are found in which groups?

a)

Groups 1 and 2

b)

Groups 3-12

c)

Groups 13-18

d)

Lanthanide and Actinide Series

44.

S-Block holds ____ electrons

a)

32

b)

18

c)

8

d)

2

45.

P-Block holds ____ electrons

a)

14

b)

10

c)

6

d)

2

46.

D-Block holds ____ electrons

a)

14

b)

10

c)

6

d)

2

47.

F-Block holds ____ electrons

a)

14

b)

10

c)

6

d)

2

48.

S-Block has ________ sublevels

a)

7

b)

5

c)

3

d)

1

49.

P-Block has ________ sublevels

a)

7

b)

5

c)

3

d)

1

50.

D-Block has ________ sublevels

a)

7

b)

5

c)

3

d)

1

51.

F-Block has ________ sublevels

a)

7

b)

5

c)

3

d)

1

52.

What element does this Lewis Dot Digram represent?

a)

Li

b)

Al

c)

C

d)

Be

53.
How many electrons should Lithium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
54.
This is a correct dot diagram for carbon (C)
a)
true
b)
false
55.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
56.
This could be the dot diagram of
a)
O
b)
B
c)
Li
d)
Ne
57.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
58.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
59.

Which of these is correct?

a)
b)
c)
60.

Write out the periodic table position for Gold

a)

5d10

b)

5d10

c)

6d9

d)

5d9

61.

Write out the periodic table position for Californium

a)

5f10

b)

7f10

c)

6f10

d)

5f6

62.

Write out the periodic table position for Strontium

a)

4d1

b)

5s2

c)

4s2

d)

5s1

63.

Write out the periodic table position for Copper

a)

4d11

b)

3d8

c)

4d9

d)

3d9

64.

Write out the periodic table position for Radon

a)

6p6

b)

5p6

c)

6p5

d)

5f14

65.

Write out the periodic table position for Lawrencium

a)

6d2

b)

5f14

c)

6d1

d)

7d1

66.

Write out the periodic table position for Bismuth

a)

5p3

b)

6p3

c)

4f13

d)

7p3

67.
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
68.
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
69.
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
70.
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
71.
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
72.

What is the element?

a)

Neon

b)

Chlorine

c)

Aluminum

d)

Argon

73.

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

74.

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

a)

Sodium (Na)

b)

Lithium (Li)

c)

Potassium (K)

d)

Calcium (Ca)

75.

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

76.

Electron configuration of oxygen (O)

a)

1s1 2s2 2p41s^{1^{\ }}2s^2\ 2p^4  

b)

1s2 2s2 2p41s^2\ 2s^{2\ }2p^4  

c)

1s2 2s2 2p61s^2\ 2s^2\ 2p^{6^{ }}  

d)

1s1 2s1 2p41s^1\ 2s^1\ 2p^4  

77.

Electron configuration of boron (B)

a)

1s2 2s1 2p11s^{2^{\ }}2s^1\ 2p^1  

b)

1s2 2s2 2p11s^2\ 2s^{2\ }2p^1  

c)

1s2 2s11s^2\ 2s^1  

d)

1s1 2s1 2p11s^1\ 2s^1\ 2p^1  

78.
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
79.

The electron configuration 1s2 2s22p6 3s23p64s23d104p6 represents which noble gas?

a)

neon

b)

argon

c)

helium

d)

krypton

80.
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
d)

1s22s22p63s13p6

81.
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
82.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
83.

Which of the following is the noble gas (shorthand) configuration for iodine?

a)

[Ar] 4s24d104p5

b)

[Kr] 5s24d105p5

c)

[Xe] 5s25d105p5

84.

Which of the following is the noble gas (shorthand) configuration for sulfur?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Xe] 3s23p4

85.

What is the shorthand configuration for tin, Sn?

a)

[Xe]5s24d105p2

b)

[Xe]5s24d105p2

c)

[Kr]5p2

d)

[Kr]5s24d105p2

86.

What is the correct noble gas configuration for neon?

a)
[Ne]
b)
[He]2s22p6
c)
[F]2p1
d)
[Ne]2s21p6
87.

What is the shorthand configuration for lead (Pb)?

a)

[Xe]6s24f145d106p2

b)

[Xe]6s25d106p2

c)

[Rn]6s25d106p2

d)

[Rn]6s24f145d106p2

88.
What is the abbreviated electron configuration for barium?
a)
[Xe] 6s2
b)
[Rn] 6s2
c)
[Ar] 4s2 3d10 4p5
d)
[He] 2s2 3p1
89.
What is the noble gas configuration for phosphorus?
a)
[Ar] 3p5
b)
[He] 3s2 3p5
c)
[Ne] 3s2 3p3
d)
[Na] 3s2 3p5
90.

The shorthand configuration below is for which element?

[Ar] 4s2

a)

Calcium

b)

Sodium

c)

Scandium

d)

Potassium

91.

This shape is that of a/n:

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

92.

Region of high probability of finding an electron

a)

atomic orbital

b)

ground state

c)

Heisenberg uncertainty principle

d)

electron configuration

93.

Which of the following is NOT a possible pair of quantum numbers?

a)

2p

b)

2d

c)

4p

d)

4f

94.
Which type of orbital is shaped like a sphere?
a)
s orbital
b)
p orbital
c)
d orbital
d)
f orbital
95.
Which statement is true about orbital shapes in relation to the picture?
a)
S-orbital on the left, P-orbital on the right
b)
P-orbital on the left, S-orbital on the right
c)
D-orbital on the left, P-orbital on the right
d)
S-orbital on the left, D-orbital on the right
96.

The Alkali Earth Metals typically end with what configuration?

a)

S1

b)

s2

c)

p4

d)

p5

e)

p6

97.

The Alkaline Earth Metals typically end with what configuration?

a)

S1

b)

s2

c)

p4

d)

p5

e)

p6

98.

The Chalcogens (Group 16) typically end with what configuration?

a)

S1

b)

s2

c)

p4

d)

p5

e)

p6

99.

The Halogens typically end with what configuration?

a)

S1

b)

s2

c)

p4

d)

p5

e)

p6

100.

The Noble Gases typically end with what configuration?

a)

S1

b)

s2

c)

p4

d)

p5

e)

p6

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