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Module 4 Exam Review

Total questions: 75

Worksheet time: 1hrs 10mins

Name
Class
Date
1.

Determine if the following electron configuration is excited or unexcited: 1s22s22p63s23p4

a)

Excited

b)

Unexcited

2.

Determine if the following electron configuration is excited or unexcited: 1s22s22p63s23p64s23d9

a)

Excited

b)

Unexcited

3.

Determine if the following electron configuration is excited or unexcited: [Kr] 5s24d95p1

a)

Excited

b)

Unexcited

4.

Determine if the following electron configuration is excited or unexcited: [Ar] 4s23d104p5

a)

Excited

b)

Unexcited

5.

Determine if the following electron configuration is excited or unexcited: 1s22s22p63s13p1

a)

Excited

b)

Unexcited

6.

1s22s22p63s23p64s23d104p4

a)

Excited

b)

Unexcited

7.

The following quantum number combination IS possible: 1s

a)

True

b)

False

8.

The following quantum number combination IS possible: 1p

a)

True

b)

False

9.

The following quantum number combination IS possible: 3d

a)

True

b)

False

10.

The following quantum number combination IS possible: 2d

a)

True

b)

False

11.

The following quantum number combination IS possible: 3f

a)

True

b)

False

12.

The following quantum number combination IS possible: 5f

a)

True

b)

False

13.

How many electrons would be required to fill the 3rd energy level?

a)

2

b)

8

c)

18

d)

32

14.

How many electrons would be required to fill the 4th energy level?

a)

2

b)

8

c)

18

d)

32

15.

How many electrons would be required to fill the 5th energy level?

a)

2

b)

8

c)

18

d)

32

16.

How many electrons would be required to fill the 6th energy level?

a)

2

b)

8

c)

18

d)

32

17.

How many electrons would be required to fill the 7th energy level?

a)

2

b)

8

c)

18

d)

32

18.

How many electrons would be required to fill the 2nd energy level?

a)

2

b)

8

c)

18

d)

32

19.

How many electrons would be required to fill the 1st energy level?

a)

2

b)

8

c)

18

d)

32

20.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
21.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
22.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
23.

What is the electron configuration of Ag?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10

b)

[Kr] 5s2 4d9

c)

1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d9

d)

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4d10 4p6 5d10 5s2 4d9

24.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
25.

What atom matches this electron configuration?

[Xe] 6s24f145d9

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

26.
What is this element? 
[Ar]4s2
a)
Calcium
b)
Sodium
c)
Scandium
d)
Titanium
27.

The s orbital is generally composed of which elements on the periodic table:

a)

Alkali & Alkaline Earth Metals (Group 1 & 2)

b)

Transition Metals in the middle portion

c)

Metals & Nonmetals above and below the Metalloid "staircase"

d)

The Lanthanide & Actinide Series (typically shown below the periodic table)

28.

The p orbital is generally composed of which elements on the periodic table:

a)

Alkali & Alkaline Earth Metals (Group 1 & 2)

b)

Transition Metals in the middle portion

c)

Metals & Nonmetals above and below the Metalloid "staircase"

d)

The Lanthanide & Actinide Series (typically shown below the periodic table)

29.

The d orbital is generally composed of which elements on the periodic table:

a)

Alkali & Alkaline Earth Metals (Group 1 & 2)

b)

Transition Metals in the middle portion

c)

Metals & Nonmetals above and below the Metalloid "staircase"

d)

The Lanthanide & Actinide Series (typically shown below the periodic table)

30.

The f orbital is generally composed of which elements on the periodic table:

a)

Alkali & Alkaline Earth Metals (Group 1 & 2)

b)

Transition Metals in the middle portion

c)

Metals & Nonmetals above and below the Metalloid "staircase"

d)

The Lanthanide & Actinide Series (typically shown below the periodic table)

31.

Electron Configurations also help us identify the electrons involved in Valence Electrons. Valence electrons are the electrons found in the _____________________________ electron shell and are found in what 2 orbitals?

a)

inner

b)

outer

c)

middle

32.

_________ & __________ **hint: which two letter/orbitals are VALENCE ELECTRONS identified in when looking at the groups on the periodic table?

a)

s & p

b)

s & d

c)

d & f

d)

s & d

33.

Lewis Dot Diagrams are a way of representing the _____________________ electrons in atoms in a way that allows prediction of bonding patterns.

a)

total number of

b)

valence shell

c)

inner

d)

middle

34.
How many electrons should Carbon have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
35.
When chlorine reacts it wants to ______________ electron.
a)
gain 1
b)
lose 1
c)
gain 2
d)
lose 2
36.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
37.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
38.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
39.

Which of the following shows a correct Lewis dot structure?

a)
b)
c)
d)
40.

Which of these is correct?

a)
b)
c)
41.
This could be the dot diagram of
a)
Be
b)
B
c)
C
d)
Ne
42.
This could be the dot diagram of
a)
P
b)
Ar
c)
Na
d)
B
43.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
44.

What is the correct formula for this molecule?

a)

NH

b)

N3H

c)

NH3

d)

NH4

45.
How many electrons are shared between the carbon atoms in an ethyne molecule?
a)
2
b)
4
c)
6
d)
8
46.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
47.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
48.

By replacing the element symbol, this could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

49.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
50.

Ionic compounds are formed when one or more valence electrons are transferred from _____

a)

A nonmetal atom to a metal atom

b)

A nonmetal atom to a nonmetal atom

c)

A metal atom to a nonmetal atom

d)

A metal atom to a metal atom

51.

When an atom loses an electron, it becomes a:

a)

Positive ion

b)

Negative ion

c)

Neutral ion

d)

Neutral atom

52.

Negative ions form when atoms _________ valence electrons.

a)

Lose

b)

Gain

c)

Share

d)

Gain or Share

53.

What is the ONLY part of the atom that makes a chemical bond

a)

Nucleus

b)

Electrons

c)

Valence Electrons

d)

Protons

54.

A(n) _________ is an ion with a positive (+) charge.

a)

Anion

b)

Cation

c)

Ion

d)

Solute

55.
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
56.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
57.
Which element is depicted from this atomic orbital diagram?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Phosphorus
58.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
59.
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
60.

Which orbital shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

e)

None of these

61.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

e)

None of these

62.

Which orbital shows a violation of the Aufbau Principle?

a)

A

b)

B

c)

C

d)

D

e)

None of these

63.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

Nothing

c)

One of the electrons in the first 2p box should be placed in the second 2p box, still pointing down

d)

One of the electrons in the first 2p box should be placed in the second 2p box, pointing up

64.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
65.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
66.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
67.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
68.
Which of the following shapes has unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
69.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
70.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
71.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
72.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
73.
Which shapes are altered by unshared pairs of electrons? 
a)
Bent and Pyramidal
b)
Trigonal Planar and Bent
c)
Tetrahedram and Bipyramidal
d)
Pyramidal and Linear
74.
How many unshared pairs of electrons will a pyramidal molecule have? 
a)
1
b)
2
c)
3
d)
4
75.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3

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