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Unit 3 Test Review

Total questions: 88

Worksheet time: 3hrs 38mins

Name
Class
Date
1.

Label Parts of wave

a)

Crest

b)

Trough

c)

Wavelength

d)

Amplitude

2.

Label parts of wave

a)

Wavelength

b)

Crest

c)

Amplitude

d)

The top

3.

Label parts of wave

a)

Bottom

b)

Crest

c)

Low

d)

Trough

4.

Label parts of the wave

a)

Amplitude

b)

Space

c)

Trough

d)

Length

5.

As frequency increases, what happens to the energy of the light?

a)

The energy decreases

b)

It goes down

c)

The energy increases

d)

The light fades

6.

What happens to the wavelength of the light as it’s frequency decreases?

a)

The energy increases

b)

It gets longer

c)

The energy decreases

d)

It gets shorter

7.

What is the speed of light?

a)

3.0x108 ms

b)

3.0x108 m/s

c)

6.626x10-34 Js

d)

6.626x10-34 J/s

8.
Which wave in the diagram has the greatest wavelength?
a)
1
b)
2
c)
3
d)
4
9.

Ground state means that an electron is...

a)

at its lowest possible potential energy

b)

in the first shell of an atom

c)

laying low for the weekend

d)

removed from an atom

10.

In order to go from ground state to an excited state, an electron must

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

11.

When an electron returns to ground state from an excited state, the atom will

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

12.

What is the ground state electron configuration of Sodium, Na

a)

1

b)

2-8-1

c)

2-7-1

d)

2-7-2

13.

Which is a possible excited state for an element?

a)

2-8-8-2

b)

2-8-18-8-2

c)

2-7-8-3

d)

2-8-18-8-3

14.

What happens when an electron gains energy?

a)

The electron goes to an excited state, and electrons move to an outer shell

b)

The electron goes to an excited state, and electrons move to an inner shell

c)

The electron goes to the ground state, and electrons move to an outer shell

d)

The electron goes to the ground state, and electrons move to an inner shell

15.

What is the maximum amount of electrons in the 3rd period, or 3rd principal energy level?

a)

2

b)

8

c)

18

d)

32

16.

What is the maximum amount of electrons in the 3rd period, or 2nd principal energy level?

a)

2

b)

8

c)

18

d)

32

17.

Which elements are present in the mixture?

SELECT ALL THAT APPLY

a)

Lithium

b)

Cadmium

c)

Strontium

d)

None

18.

What elements are in the mixture?

SELECT ALL THAT APPLY

a)

A

b)

D

c)

Z

d)

None of them

19.

What element is in the unknown?

a)

He

b)

O2

c)

Ne

d)

Ar

e)

Xe

20.

What element is in the unknown?

a)

H2

b)

He

c)

O2

d)

None of them

21.
What is the electron configuration for this atom?
a)
1s22s22p6
b)
1s22s22p5
c)
1s22s22p3
d)
2s22p3
22.

This orbital diagram represents:

a)

Carbon

b)

Boron

c)

Nitrogen

d)

Oxygen

23.

Which atom matches this shorthand electron configuration?

[Xe] 6s24f145d9

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

24.

Which example shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

25.
How many electrons can the p sublevel hold?
a)
14
b)
10
c)
2
d)
6
26.
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
27.
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
28.

Which of the following is written correctly?

a)

A

b)

B

c)

C

d)

D

29.

An aluminium ion would have which electron configuration?

a)

1s2 2s2 2p6 3s2

b)

1s2 2s2 2p6 3s2 3p1

c)

1s2 2s2 2p6 3s2 3p6

d)

1s2 2s2 2p6

30.
What atom is represented here?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Fluorine
31.
How many valence electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
32.

This orbital diagram represents

a)

Nitrogen

b)

Oxygen

c)

Carbon

d)

Neon

33.
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
34.
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
35.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
36.
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
37.
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
38.
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
39.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
40.
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.
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.
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
43.

What is the purpose of using noble-gas notation in electron configurations?

a)

To simplify the representation of electron configurations

b)

To show the exact number of electrons in the noble gas

c)

To represent the atomic mass of an the noble gas

d)

To indicate the chemical reactivity of an element

44.

Which elements are represented by noble gases in the periodic table?

a)

Elements in the first column

b)

Elements in the last column

c)

Elements in the middle of the table

d)

Elements with the highest atomic number

45.

What does the bracketed noble gas represent in noble-gas notation?

a)

The outermost electrons

b)

The inner levels or first levels filled up to the location of that noble gas

c)

the inner levels plus the electron configuration that follows it

d)

The chemical properties of the element

46.

What are valence electrons?

a)

Electrons in the innermost shell

b)

Electrons in the atom's outermost s and p orbitals

c)

electrons in all the orbitals available of that element

d)

electrons that live in the 1st and 2nd energy level

47.

Which rule states that each atom wants to attain 8 valence electrons?

a)

Hund's Rule

b)

Pauli Exclusion Principle

c)

Octet Rule

d)

Aufbau Principle

48.

For which groups does the number of valence electrons correspond to the group number on the periodic table?

a)

Groups 1, 2, and 3-8

b)

Groups 1, 2, and 3-12

c)

Groups 1, 2, and 3-18

d)

Groups 1, 2, and 3-6

49.

How many valence electrons does Helium have in group 8?

a)

8

b)

2

c)

4

d)

6

50.

How many valence electrons do neutral atoms of sulfur have?

a)

4

b)

6

c)

8

d)

2

51.

What is the maximum number of dots used in electron dot notation?

a)

6

b)

8

c)

10

d)

12

52.

In electron dot notation, how are electrons typically placed around the element symbol?

a)

As single dots on each side

b)

As pairs around the element symbol

c)

As a circle around the symbol

d)

As a line above the symbol

53.

What does the electron dot structure represent?

a)

The atomic nucleus and inner level electrons

b)

The atomic mass

c)

The atomic number

d)

The atomic weight

54.

What is the electron configuration for Carbon?

a)

1s²2s²2p²

b)

1s²2s²2p⁴

c)

1s²2s²

d)

1s²2s²2p⁵

55.

How many valence electrons does Fluorine have according to its electron-dot structure?

a)

7

b)

5

c)

6

d)

8

56.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
57.

Whta is the noble gas notation for V?

a)

[Ar] 4s2 4d2

b)

[Kr] 4s2 3d3

c)

[Ar] 4s2 4d3

d)

[Ar] 4s2 3d3

58.

What is the noble gas notation electron for Sulfur?

a)

[Ne] 3p4

b)

[He] 3s2 3p4

c)

[Ne] 3s2 3p4

d)

[Na] 3s2 3p4

59.

There may be a maximum of ____ p orbitals at a given energy level.

a)

2

b)

6

c)

3

d)

8

60.

This shape is that of

a)

s-orbital

b)

d-orbital

c)

p-orbital

d)

f-orbital

61.

This is the shape of ____ orbital

a)

s

b)

d

c)

p

d)

d

62.

Orbital sublevels, or l, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

63.

How many electrons total are found in the f orbital?

a)

2

b)

6

c)

10

d)

14

64.

What does the 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

65.

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

a)

high level

b)

base line

c)

set state

d)

ground state

66.

This shape is that of a...

a)

s orbital

b)

d orbital

c)

p orbital

d)

f orbital

67.

The spin of an electron is represented by this variable:

a)

n

b)

m

c)

L

d)

s, ms

68.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

69.

Hydrogen

a)

Hy

b)

Hi

c)

Hd

d)

H

70.

Helium

a)

H

b)

He

c)

Hi

d)

Hm

71.

Carbon

a)

C

b)

Ca

c)

Cr

d)

Cn

72.

Sodium

a)

S

b)

Sd

c)

Na

d)

K

73.

Ca

a)

Cesium

b)

Cerium

c)

Calcium

d)

Kalium

74.

Iron

a)

Fe

b)

Ir

c)

On

d)

Li

75.

Copper

a)

Co

b)

Cp

c)

Cr

d)

Cu

76.

Zinc

a)

Zn

b)

Zi

c)

Zc

d)

Ak

77.

O

a)

Oron

b)

Oxygen

c)

Oblivium

d)

Osmium

78.

Silver

a)

Si

b)

Au

c)

K

d)

Ag

79.

Nitrogen

a)

N

b)

Ni

c)

Nt

d)

Nr

80.

Fluorine

a)

F

b)

Fl

c)

Fo

81.
Cl is the chemical symbol for...
a)
Chlorine
b)
Carbon
c)
Copper
d)
Silicon
82.
K is the chemical symbol for...
a)
Potassium
b)
Krypton
c)
Chromium
d)
Phosphorus
83.
Lead
a)
Le
b)
La
c)
L
d)
Pb
84.
Mg
a)
Magnesium
b)
Manganesse
c)
Iron
d)
Germanium
85.

Al

a)

aluminum

b)

antimony

c)

argon

d)

silver

86.

Au

a)

Tin

b)

Sulfur

c)

Gold

d)

sliver

87.

Iodine

a)

Ie

b)

Io

c)

ID

d)

I

88.

Br

a)

beryllium

b)

boron

c)

bromine

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