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Worksheets

Ionic and Covalent Bonding Quiz

Total questions: 193

Worksheet time: 3hrs 50mins

Name
Class
Date
1.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
None of these
2.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
3.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
4.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
5.
How many dots would a Lewis Dot structure of Helium have?
a)
1
b)
2
c)
8
d)
0
6.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
7.
The majority of an atom's mass exists where?
a)
In the nucleus
b)
In the electron cloud
c)
In the space between the nucleus and the electrons
d)
In the neutrons
8.
How many electrons are in the outer shell of Sodium (Na)?
a)
3
b)
1
c)
2
d)
4
9.
?
a)
Boron
b)
Carbon
c)
Nitrogen
d)
Lithium
10.

What Element does this Bohr Model show?

a)

Helium

b)

Hydrogen

c)

Argon

d)

Silver

11.

What is a Bohr Model?

a)

a simplified representation of an atom

b)

vertical column in periodic table

c)

horizontal row in periodic table

d)

Only shows the element symbol and it's outer most electron shell

12.

What are the names of the 2 models that we have been using?

a)

Bohr and Newton Structures

b)

Lewis and Caroll Models

c)

Bohr Model & Lewis Dot Structure

d)

Element & Atom structures

13.

What is a Lewis Dot Structure?

a)

It shows all of the particles in the atom.

b)

Contains protons and neutrons

c)

Only shows the element symbol and it's outer most electron shell

d)

Contains protons and electrons

14.

What do we call many atoms of the same type; has unique properties such as melting and boiling points?

a)

Atoms

b)

Elements

c)

Isotope

d)

Ions

15.

Why do carbon, silicon, and tin all react similarly?

a)

They are located in the same period

b)

They have an even atomic number

c)

They have the same number of energy levels

d)

They are located in the same group

16.

Is this a correct dot diagram for fluorine (F)

a)

Yes

b)

No

17.

Is this a correct dot diagram for magnesium (Mg)

a)

Yes

b)

No

18.
How many electrons should Nitrogen have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
19.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
20.

Which of these is incorrect?

a)

b)

21.

These particles are found in the nucleus of the atom.

a)

protons only

b)

protons and electrons

c)

electrons only

d)

protons and neutrons

22.

The mass number is the total of the protons plus the neutrons in the atom.

a)

True

b)

False

23.

How many neutrons would you expect the average gold atom to have given the information shown?

a)

79

b)

118

c)

197

d)

276

24.

Which subatomic particle has a negative charge?

a)

proton

b)

electron

c)

neutron

d)

quark

25.
The section labeled D is known as the?
a)
Electron cloud
b)
Neutron
c)
Nucleus
d)
Electron
26.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
27.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
28.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
29.

Name this element.

a)

Neon

b)

Magnesium

c)

Sodium

d)

Manganese

30.

An element will always have the same number of 

a)
neutrons
b)
protons
c)
isotopes
d)
atoms
31.

Which subatomic particle has a positive charge and is found inside the nucleus?

a)

Electron

b)

Proton

c)

Neutron

d)

Nucleus

32.

Which subatomic particle has a neutral charge and is found inside the nucleus?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Nucleus

33.

What is the maximum number of electrons that can be found in the third shell (energy level)?

a)

2

b)

8

c)

18

34.

What is the maximum number of electrons that can be found in the second shell (energy level)?

a)

2

b)

8

c)

18

35.

What is the maximum number of electrons that can be found in the first shell (energy level)?

a)

2

b)

8

c)

18

36.

What is the atomic number of this element?

a)

17

b)

18

c)

35

d)

35.453

37.

Which element is this?

a)

Calcium

b)

Chlorine

c)

Silicon

d)

Potassium

38.

What element is this?

a)

Nitrogen

b)

Chlorine

c)

Argon

d)

Phosphorous

39.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

40.

Which element is this?

a)

Nickel

b)

Neon

c)

Sodium

d)

Nitrogen

41.

Use the periodic table below to determine the number of protons in Bromine (Br).

a)

35

b)

79.904

c)

36

d)

83.798

42.

How many valence electrons does this element have?

a)

12

b)

8

c)

2

d)

10

43.

Use your periodic table to determine the number of protons in Neon (Ne).

a)

18.998

b)

20.18

c)

10

d)

12

44.

What is the atomic mass for this element? (Round to the nearest WHOLE number.) (This information for this element can be found on the periodic table!)

a)

11

b)

19

c)

24

d)

23

45.

How many valence electrons does this element have?

a)

1

b)

2

c)

3

d)

4

46.

What element does this Bohr model represent?

a)

Carbon

b)

Boron

c)

Neon

d)

Nitrogen

47.

How many valence electrons does this element have?

a)

1

b)

2

c)

3

d)

4

48.

What is a Bohr Model?

a)

a simplified representation of an atom

b)

vertical column in periodic table

c)

horizontal row in periodic table

d)

Only shows the element symbol and it's outer most electron shell

49.

What are the names of the 2 models that we have been using?

a)

Bohr and Newton Structures

b)

Lewis and Caroll Models

c)

Bohr Model & Lewis Dot Structure

d)

Element & Atom structures

50.

What is a Lewis Dot Structure?

a)

It shows all of the particles in the atom.

b)

Contains protons and neutrons

c)

Only shows the element symbol and it's outer most electron shell

d)

Contains protons and electrons

51.

What is a drawing of an atom that shows all of the par;cles?

a)

Lewis Dot Model

b)

Dalton Model

c)

Thompson Model

d)

Bohr Model

52.

What is the the outermost shell with electrons?

a)

Shells

b)

Isotope

c)

Orbit

d)

Valence

53.

What is the atom called when there is adding or removing electrons creates atoms with (+) or (-) charges?

a)

isotopes

b)

ions

c)

neutral

d)

stable

54.

What is the drawing of an atom that only has the symbol and the valence electrons?

a)

Lewis Dot Diagram

b)

Bohr Diagram

c)

Thompson Diagram

d)

Dalton Diagram

55.

Each column of the Periodic Table are known by this number

a)

Period

b)

Group

c)

Family

d)

Transition Metals

56.

What is the atomic number of this element?

a)

17

b)

18

c)

35

d)

35.453

57.

What is the mass number of this atom of Chlorine?

a)

17

b)

18

c)

35

d)

35.453

58.

Which element is this?

a)

Calcium

b)

Chlorine

c)

Silicon

d)

Potassium

59.

What element is this?

a)

Na

b)

P

c)

N

d)

S

60.

What element is this?

a)

Nitrogen

b)

Chlorine

c)

Argon

d)

Phosphorous

61.

Which Bohr model represents Be?

a)
b)
c)
d)
62.

Which Bohr model represents Neon?

a)
b)
c)
d)
63.

___________ simplify the Bohr Model by showing only the outer valence electrons used for bonding.

a)

Lewis Dot Diagrams

b)

Bohr Models

c)

Electron Clouds

d)

Periodic Tables

64.

Is this a correct dot diagram for fluorine (F)

a)

Yes

b)

No

65.

Is this a correct dot diagram for magnesium (Mg)

a)

Yes

b)

No

66.
How many electrons should Nitrogen have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
67.
How many electrons should Chlorine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
68.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
69.

This is a Bohr Diagram of Aluminum. How many valence electrons does Aluminum have?

a)

3

b)

4

c)

5

70.

How many valence electrons does Tin (Sn) have?

a)

8

b)

7

c)

5

d)

4

71.

How many valence electrons does Lithium (Li) have?

a)

8

b)

1

c)

5

d)

2

72.

How many valence electrons does Bromine (Br) have?

a)

5

b)

6

c)

7

d)

8

73.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons in the second shell
74.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
75.

According to the diagram below, how many bonds will this atom be able to make?

a)
1
b)
2
c)
3
d)
4
76.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

77.

Which of these is incorrect?

a)

b)

78.
Most elements will gain or lose electrons so that they end up with _______ valence electrons.
a)
2
b)
6
c)
8
d)
10
79.

Which of these is correct?

a)
b)
c)
80.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
81.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
82.
Covalent bonds actually "share" electrons?
a)
true
b)
false
83.
How are covalent bonds formed?
a)
Sharing of electrons
b)
Transfer of electrons
84.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
85.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
86.
Is this ionic bond drawn correctly?
a)
Yes
b)
No
87.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
88.
Gain or lose electrons
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
89.
Share electrons
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
90.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
91.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
92.

Water molecules are held together by what type of bond?

a)

Hydrogen

b)

covalent

c)

ionic

d)

none

93.

Atoms in a water molecule are held together by what type of bond?

a)

Ionic

b)

hydrogen

c)

covalent

d)

none

94.

Covalent bonds are weak

a)

True

b)

False

95.

Metals ____________ valence electrons and form __________ ions.

a)

Lose, negative

b)

Lose, positive

c)

Gain, negative

d)

Gain, positive

96.

Nonmetals ______________ valence electrons and form ___________ ions.

a)

Lose, negative

b)

Lose, positive

c)

Gain, negative

d)

Gain, positive

97.

Ionic bonds are formed between

a)

Metal + nonmetal

b)

Metal + metal

c)

Nonmetal + nonmetal

d)

Metalloid + metalloid

98.

Covalent bonds are formed between

a)

Metal + nonmetal

b)

Metal + Metal

c)

Nonmetal + nonmetal

d)

Metalloid + metalloid

99.

When writing ionic compounds the _____________ always comes first

a)

Nonmetal

b)

Gibbs free energy

c)

Metal

d)

Constant

100.

Identify the compound below


NaCl

a)

Ionic

b)

Covalent

c)

Metallic

d)

Synthetic

101.

Identify the compound below


NH3

a)

Ionic

b)

Covalent

c)

Metallic

d)

Synthetic

102.

Identify the compound below


Ca3N2

a)

Ionic

b)

Covalent

c)

Metallic

d)

Synthetic

103.

Identify the compound below


P2O5

a)

Ionic

b)

Covalent

c)

Metallic

d)

Synthetic

104.

Prefixes are only used for covalent compounds

a)

True

b)

False

105.

What is the formula for sodium sulfide?

a)

NaS

b)

SS

c)

Na2S

d)

NaS2

106.

Is the following compound ionic or covalent? What is the name of the compound?


CaBr2

a)

Ionic, calcium dibromide

b)

Ionic, calcium bromide

c)

Covalent, calcium dibromide

d)

Covalent, calcium bromide

107.

Is the following compound ionic or covalent? What is the name of the compound?


CH4

a)

Ionic, carbon hydrogen

b)

Ionic, carbon tetrahydride

c)

Covalent, carbon hydrogen

d)

Covalent, carbon tetrahydride

108.

Write the formula for carbon dioxide

a)

CO2

b)

C2O

c)

CO

d)

COO

109.

What is the formula for magnesium fluoride?

a)

MgF

b)

FMg

c)

Mg2F

d)

MgF2

110.

What is the name of this compound?


P2O5

a)

Phosphorus oxide

b)

Phosphorus monoxide

c)

Diphosphorus pentoxide

d)

Pentaphosphorus Dioxide

111.

What is the formula for aluminum oxide?

a)

Al2O3

b)

AlO

c)

Al3O2

d)

Al3O

112.

What is the name of this compound?


AlN

a)

Aluminum nitrogen

b)

Aluminum nitride

c)

Aluminum mononitrogen

d)

Aluminum mononitride

113.

What is the name of this chemical compound Cl2O7

a)

Dichlorine sevenoxide

b)

Chlorine Oxide

c)

Chloride Oxide

d)

Dichlorine Heptoxide

114.

What is the formula for trisulfur decoxide

a)

Na2O2

b)

SO2

c)

S3O10

d)

S10O3

115.

What is the formula for calcium oxide?

a)

CaO

b)

CO

c)

Ca2O2

d)

C2O2

116.

A bond between a nonmetal and a nonmetal is called a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

117.

What is Covalent Bonding?

a)

Bonding that is the result of two nonmetals sharing electrons

b)

Bonding between two metals

c)

Bonding that is the result of a nonmetal and a metal exchanging electrons

d)

Bonding between more than two elements

118.

Which particle is responsible for bonding?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Nucleus

119.

Which of the following is true about Ionic Bonds? (select ALL TRUE options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

120.

Potassium Chloride is...

a)

Ionic

b)

Covalent

121.

Water (H2O) is...

a)

Ionic

b)

Covalent

122.

Ammonium (NH4) is...

a)

Ionic

b)

Covalent

123.
Share electrons
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
124.
Gain or lose electrons
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
125.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
126.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
127.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

128.
What happens when an atom loses an electron?
a)
It becomes Negatively Charged
b)
It remains neutral because the proton also leaves.
c)
It becomes Positively Charged
d)
It stays the same.
129.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
130.
Elements in Group 1 lose one electron to form ions with a(n) _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
131.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
132.
What type of bond is this?
a)
ionic
b)
covalent
133.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
134.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
135.
How are covalent bonds formed?
a)
Sharing of electrons
b)
Transfer of electrons
136.
Which is the charge that results when oxygen becomes an ion?
a)
+3
b)
+2
c)
-2
d)
-3
137.
LiF
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
138.
MgBr2
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
139.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

140.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

141.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

142.

Identify the following compound as ionic or covalent: CO

a)

ionic

b)

covalent

143.

Identify the following compound as ionic or covalent: Ca(OH)2

a)

ionic

b)

covalent

144.

When a metal loses an electron(s) it becomes a ...

a)

positive ion

b)

negative ion

c)

metalloid

d)

nonmetal

145.

In an ionic bond the metal wants to ______ electrons.

a)

lose

b)

gain

c)

share

146.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
147.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
148.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
149.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
150.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
151.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
152.
Where are the metalloids located on the periodic table?
a)
Blue
b)
Red
c)
Green
153.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
154.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
155.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
156.
Which of the following is an ionic bond?
a)
H3N
b)
CaCl2
c)
NO2
d)
SCl
157.

Which is the correct structure for ammonia NH3?

Pictures correspond with a-d.

a)

Option A.

b)

Option B.

c)

Option C.

d)

Option D.

158.

Choose the structure that forms a triple bond. You will need to write these down and/or look in your notes.

a)

Hydrogen

b)

Fluorine

c)

Oxygen

d)

Nitrogen

159.

Hydrogen needs _____ electrons in its valence shell to be stable or happy.

a)

4

b)

6

c)

8

d)

2

160.

Which is the correct molecular structure for carbon dioxide? Try working this one out before choosing.

a)
b)
c)
d)
161.

How many total valence electrons are participating in bonding in the molecule above? They ones that are not lone pairs.

a)

8

b)

4

c)

2

d)

3

162.

CO2 has how many lone pairs? You may need to write this one down to figure it out.

a)

0

b)

1

c)

2

d)

3

e)

4

163.

NH3 has how many lone pairs? You may need to write this one down to figure it out.

a)

0

b)

1

c)

2

d)

3

164.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

165.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
166.

An atom with 3 valence electrons "wants" a full shell, so it can either gain 5 or lose 3. Which is more likely to occur?

a)

Gain 5

b)

Lose 3

c)

Nothing

167.

When figuring out Lewis Dots for Covalent compounds what does "A" mean?

a)

A = the total available valence electrons of all the atoms

b)

A = the available valence electrons of one atom

c)

A = the total valence electrons the atoms wants to have in its outer shell

d)

A = the number of shared electrons

168.

What does the "N" mean when figuring out Lewis Dots for covalent compounds?

a)

N = the total number of valence electrons NEEDED in the outer shell

b)

N = how many more valence electrons are needed

c)

N = how many valence electrons are available to share

d)

N = nitrogen

169.

What would the "A" be for CH3F when figuring out the Lewis Dot?

a)

(1 x 8 ) + (3 x 2 ) + (1 x 8) = 22

b)

(1 x 4) + (3 x 1) + (1 x 7) = 14

170.

Which atom will never be in the middle of a Lewis Dot structure?

a)

N

b)

C

c)

H

d)

P

171.

Which atom goes in the middle of the Lewis Dot structure?

a)

The one the needs the least number of valence electrons

b)

The most electronegative element

c)

The one that needs the most or is less electronegative generally

172.

These conduct electricity well.

a)

Metallic bonds

b)

ionic bonds

c)

covalent bonds

173.

These only conduct electricity as molten substances or if dissolved in water.

a)

Metallic bonds

b)

ionic bonds

c)

covalent bonds

174.

These have super high melting points.

a)

Metallic bonds

b)

ionic bonds

c)

covalent bonds

175.

These have delocalized electrons.

a)

Metallic bonds

b)

covalent bonds

c)

ionic bonds

176.

These have very large electronegativity differences.

a)

Metallic bonds

b)

ionic bonds

c)

covalent bonds

177.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
178.
What type of bond is shown in this image?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
179.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
180.
A Nitrogen molecule (N2) has one triple bond. How many electrons do the nitrogen atoms share?
a)
1
1
b)
3
c)
4
d)
6
181.
Compared to ionic compounds, molecular compounds generally have...
a)
good conductivity
b)
greater densities
c)
more chemical bonds
d)
a low boiling point
182.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
183.
In a(an) POLAR bond, one atom pulls on the shared electrons more than the other atom. 
a)
True
b)
False
184.
Which has the greater EN: 
N or C?
a)
C
b)
N
185.
Choose the set that goes from lowest to highest electronegativity?
a)
Cu, Mg, Sr, Ca
b)
F, Cl, Br, Si
c)
Cs, Rb, Ca, Mg
d)
Zn, Cd, Ag, Cu
186.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
187.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
188.
Put these in order of increasing electronegativity:
Se, S, and O
a)
Se < S < O
b)
Se < O < S
c)
O < S < Se
d)
S < Se < O
189.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

190.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

191.

What must the difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

192.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

193.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

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