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7.4 Bond Polarity Bank

Total questions: 110

Worksheet time: 56mins

Name
Class
Date
1.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
2.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
3.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
4.
Electronegativity is a measurement of the ability of a nucleus to...
a)
attract bonding electrons
b)
attract other nuclei
c)
attract elenece in the non-valence energy levels
5.
How many electrons are represented by a single straight line in a Lewis structure?
a)
1
b)
2
c)
4
d)
6
6.
The most electronegative atom in the periodic table is:
a)
Fluorine
b)
Helium
c)
Neon
d)
Francium
7.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
8.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
9.
Partial charges like the ones shown here are called:
a)
dipoles
b)
deltas
c)
ions
d)
magnetic poles
10.
Which molecule contains bonds of GREATER polarity?
a)
H2O
b)
OF2
11.
Which molecule contains bonds with a GREATER polarity?
a)
HCl
b)
CCl4
12.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
13.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
14.
If Boron bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
15.
If Bromine bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
16.
When you are asked to find bond polarity, compare EN values of each bonding atom to the central atom
a)
true
b)
false
17.
The electronegativity difference in the bonds of CH4 (methane) is:
a)
0.4
b)
5.9
c)
-0.4
d)
1.7
18.
The electronegativity difference in the bonds of CCl4 (carbon tetrachloride) is:
a)
0.4
b)
0.5
c)
9.5
d)
5.5
19.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

20.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

21.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

22.

In an ionic bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity Only

b)

The atom with the Lowest Electronegativity Only

c)

The atom with the Greatest Electronegativity Mostly

d)

The atom with the Lowest Electronegativity Mostly

23.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

24.

In a nonpolar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

25.

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

26.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

27.

Molecules that contain whole number charges on atoms (+1,-3, etc.) must be...

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

d)

Polar Covalent or Ionic

28.

In a polar covalent bond, which atom will have a partial positive charge? (choose 2 correct answers)

a)

The atom that attracts fewer electrons

b)

The atom with the greater electronegitivity

c)

The atom that attracts more electrons

d)

The atom with the lower electronegativity

29.

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

30.

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

31.

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

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

32.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

33.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
34.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
35.
Electronegativity is a measurement of the ability of a nucleus to...
a)
attract bonding electrons
b)
attract other nuclei
c)
attract elenece in the non-valence energy levels
36.
The most electronegative atom in the periodic table is:
a)
Fluorine
b)
Helium
c)
Neon
d)
Francium
37.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
38.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
39.
Partial charges like the ones shown here are called:
a)
dipoles
b)
deltas
c)
ions
d)
magnetic poles
40.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
41.
If Boron bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
42.
When you are asked to find bond polarity, compare EN values of each bonding atom to the central atom
a)
true
b)
false
43.
The electronegativity difference in the bonds of CCl4 (carbon tetrachloride) is:
a)
0.4
b)
0.5
c)
9.5
d)
5.5
44.

A diatomic molecule like O2 is always_______ because electrons are shared ________.

a)

nonpolar; equally

b)

polar; equally

c)

nonpolar; unequally

d)

nonpolar; unequally

45.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

46.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

47.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

48.

When you have Be-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

49.

When you have Si-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

50.

When you have F-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

51.

When you have C-H, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

52.

When you have Zn-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

53.

When you have Mn-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

54.

When you have Ga-Se, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

55.

What would solubility look like for nonpolar covalent bond in water?

a)

soluable

b)

nonsoluable

56.

What would solubility look like for polar covalent bond in water?

a)

soluable

b)

nonsoluable

57.

How would the melting point and boiling point for nonpolar covalent bond?

a)

High

b)

Low

58.

How would the melting point and boiling point for polar covalent bond?

a)

High

b)

Low

59.

Class Period

a)

1

b)

2

c)

3

d)

4

60.

The electrons in a POLAR covalent bond are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

61.

The electrons in a NONPOLAR covalent bond are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

62.

What type of bond is depicted in the image?

a)

Nonpolar Covalent

b)

Polar Covalent

c)

Ionic

63.

Electronegativity is...

a)

The ability for an atom to ATTRACT electrons

b)

the ability of an atom to LOSE electrons

c)

the energy required to remove an electron from an atom

d)

how easy it is to make friends.

64.

Which element is MORE electronegative?

a)

O

b)

Be

65.

What is the difference in electronegativity for HBr?

a)

0.7

b)

1.9

c)

2.0

d)

2.8

66.

HBr has a difference in electronegativity of 0.7. Based on the table, what kind of bond is HF?

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

67.

H2OH_2O  has a difference in electronegativity of 1.4. Based on the table, what kind of bond is 

H2OH_2O ? 

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

68.

NH3NH_3   is a polar covalent compound. Which atom, N or H, will electrons spend MORE time with?

a)

N

b)

H

69.

How are you feeling about this topic (polar covalent bonds, electronegativity)?

a)

I'm lost :(

b)

I need some more practice

c)

I'm almost there

d)

I'm an expert!

70.

What is the difference in electronegativity for 

SO2SO_2  ?

a)

0.5

b)

1.0

c)

2.0

d)

3.5

71.
Will this molecule be polar or nonpolar? CCl4
a)
polar
b)
nonpolar
72.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
73.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
74.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
75.
Partial charges like the ones shown here are called:
a)
dipoles
b)
deltas
c)
ions
d)
magnetic poles
76.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

77.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

78.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

79.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

80.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

81.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

82.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

83.

When you have F-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

84.

When you have C-H, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

85.

What would solubility look like for nonpolar covalent bond in water?

a)

soluable

b)

nonsoluable

86.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

87.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

88.

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

89.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

90.

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

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

91.

Lithium and Oxygen will form a(n) _____ bond

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

92.

Hydrogen and Chlorine will form a(n) _____ bond

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

93.

Which of the following represents an ionic molecule?

a)

BeO

b)

IF

c)

CO2

d)

SeBr2

94.

Manganese and Oxygen will form a(n) _____ bond

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

95.

Gallium and Selenium will form a(n) _____ bond

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

96.

Which of the following molecules will have one partially-negative charged atom?

a)

SF2

b)

H2O

c)

NaBr

d)

NCl3

97.

Which of the following molecules will have two partially-positive charged atoms?

a)

CO2

b)

PH3

c)

H2O

d)

C2H4

98.

Which of the following represents a polar molecule?

a)

H2

b)

H2O

c)

CH4

d)

CSe2

99.

Which of the following represents a nonpolar molecule?

a)

KCl

b)

Cl2

c)

HF

d)

CO2

100.

Sulfur and Oxygen (SO) will form a(n) _____ bond

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

101.

What is the electronegativity of Chlorine gas(Cl2)

a)

0

b)

1

c)

2

102.

Which refers to the unequally shared electrons of molecules?

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

103.

What is the electron difference of Hydrochloric acid (HCl)?

a)

0.5

b)

0.9

c)

1.7

104.

Who proposed the Pauling Scale?

a)

Carl Linnaeus

b)

Herbert Powell

c)

Linus Pauling

105.

What is the bond polarity of Hydrogen bromide if its electronegativity difference is 0.7?

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

106.

Which bond polarity refers to Nitrous oxide as the electrons are equally shared?

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

107.

Electronegativity increases from _______ of the period.

a)

left to right

b)

right to left

c)

top to bottom

108.

Electronegativity decreases from ____ of the group.

a)

left to right

b)

top to bottom

c)

bottom to top

109.

What is the bond polarity if the electronegativity difference ranges from 0 to 0.5?

a)

Nonpolar Covalent

b)

Polar Covalent

c)

Ionic

110.

A polar covalent bond should have an electronegativity difference ranges from _____?

a)

0-0.5

b)

0.6-1.8

c)

1.9 and up

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