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Bonding, Polarity, Lewis Test Review

Total questions: 137

Worksheet time: 2hrs 2mins

Name
Class
Date
1.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

d)

2 Adams

2.

SO2

a)

ionic

b)

covalent

c)

metallic

d)

missing sock

3.

Ca(OH)2

a)

ionic

b)

covalent

c)

metallic

d)

Autotune has ruined "popular" music.

4.

Cations have a _____________ charge.

a)

positive

b)

negative

c)

neutral

d)

"Charge? Huh?"

5.

Anions have a ____ charge.

a)

positive

b)

negative

c)

neutral

d)

Union was not the band Yes's worst album.

6.

Cations, because they are positive, tend to be ________.

a)

metals

b)

nonmetals

c)

irrelevant

d)

nothing but a good time

7.

Anions tend to be _______

a)

metals

b)

nonmetals

c)

lachrymal

d)

impossible to control

8.

Identify the charge for a chloride anion (Cl-)

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

9.

Identify the charge for an oxide ion (O2-).

a)

1+

b)

2+

c)

2-

d)

3-

e)

3+

10.

Identify the charge for nitride ion (N3-).

a)

1+

b)

2+

c)

3+

d)

3-

e)

2-

11.

Identify the charge for a potassium ion (K+).

a)

1-

b)

1+

c)

2+

d)

2-

12.

In ionic bonding, valence electrons are _______.

a)

shared between atoms

b)

transferred from one atom to another

c)

destroyed by the force

d)

absorbed by the nucleus

13.

In covalent bonding, valence electrons are ______.

a)

shared between atoms

b)

transferred from one atom to another

c)

destroyed by the nonbelievers

d)

hanging out in the excited state

14.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

c)

Valentine

15.

Generally, atoms form covalent bonds so that _______________.

a)

each atom loses its electrons to become cations

b)

each atom "feels like" it has a full valence electron shell

c)

each atom feel like part of the greater atomic community

d)

each atom gains electrons to become anions

16.

______________ generally have low melting and boiling points.

a)

Ionic compounds such as NaCl

b)

Covalent compounds such as C6H12O6 (that's sugar, y'all)

c)

Metallic elements

d)

The tropical regions of earth

17.

________________ generally have high melting and boiling points.

a)

Ionic compounds

b)

Covalent compounds

c)

Metalloidic compounds

d)

Molecules from planets close to the sun

18.

____________ do not conduct electricity in solution.

a)

Ionic compounds

b)

Covalent compounds

c)

Old music composers

19.

____________ conduct electricity well when either melted or dissolved in water.

a)

Ionic compounds

b)

Covalent compounds

c)

Plastics

20.

MgO is held together by

a)

Ionic bonds

b)

Covalent bonds

c)

Metallic bonds

d)

Slayer bonds

21.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
d)

I forgot to color where they actually are.

22.

If Sodium and Bromine react, they will form a(n) _______ bond.

a)

ionic

b)

covalent

c)

metallic

d)

inseparable

23.

Carbon and Oxygen will form a(n) ___________ bond.

a)

ionic

b)

covalent

c)

metallic

d)

fake

24.

Why do covalent bonds form?

a)

filling the outermost energy level to be stable (i.e., have an octet except H or B)

b)

to make all atoms exactly the same

c)

to make other atoms in other molecules unstable

d)

to make all atoms different from each other

25.

Why don't noble gases form bonds?

a)

They already have a full valence shell.

b)

What? Noble gases form bonds with all kinds of other atoms.

c)

They only bond when with each other, and that doesn't count.

d)

Everything else except this choice is wrong.

26.

How many valence electrons are shown in the diagram?

a)

16

b)

7

c)

6

d)

2

27.

This refers to the tendency of atoms to prefer to have eight electrons in the valence shell

a)

Octet rule

b)

Valence electron

c)

Electronegativity

d)

Lewis symbol

28.

Electron that is located on the outermost shell

a)

proton

b)

neutron

c)

electron

d)

valence electron

29.

Which element is most likely to form only 2 covalent bonds?

a)

Carbon

b)

Fluorine

c)

Nitrogen

d)

Sulfur

30.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
31.

How many valence electrons does Oxygen (O) have?

a)

6

b)

8

c)

15

d)

16

32.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
33.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
34.

PCl3

a)

Polar

b)

Nonpolar

c)

Superpolar

d)

Subpolar

35.

H2O

a)

Polar

b)

Nonpolar

c)

Arctic Monkeys

d)

Baroness

36.

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
37.
In this Lewis structure, the symbol above F means...
a)

electrons are being completely 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 an anion

38.

Hydrogen "wants" (or needs) __ electrons in its valence shell to be stable.

a)
4
b)
6
c)
8
d)
2
39.

According to the octet rule most elements are stable with __ valence electrons.

a)
2
b)
8
c)
6
d)
18
40.

How many valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

12

d)

6

41.

NH3 has how many nonbonding (or lone) pairs of electrons?

a)

0

b)

1

c)

2

d)

3

e)

4

42.

Dihydrogen monosulfide, H2S

a)

nonpolar

b)

unintelligent

c)

polar

d)

grizzly bear

43.

CCl4

a)

made of polar covalent bonds but overall nonpolar

b)

made of polar covalent bonds and overall polar

c)

made of nonpolar covalent bonds and nonpolar

d)

made of nonpolar covalent bonds but is somehow polar

44.

Sulfur dioxide (cough, cough), SO2

a)

polar molecule because of its shape

b)

polar molecule because every atom has a full octet

c)

nonpolar molecule because there are no dipoles

d)

nonpolar molecule because there are dipoles that cancel each other out

45.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
46.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
47.

Although sulfur has more than an octet here, this actually happens.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

48.

Boron does not form an octet because it only has 3 valence electrons to share.

Is this molecule polar or non-polar? [Hint: shape]

a)

Non-polar

b)

Polar

49.

Bromine has more than an octet. This actually happens because ... well, it's bromine.

Considering its shape, is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

50.

Which molecule contains bonds that are the most polar?

a)

H2O

b)

OF2

c)

CH4

d)

CH2S

51.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
52.

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

a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
53.
If Boron bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
54.

If chlorine (Cl) bonds with Hydrogen, a ____________ bond forms.

a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
55.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
56.
Electronegativity is a measurement of the ability of a nucleus to...
a)
attract bonding electrons
b)
attract other nuclei
c)

attract electrons in the lower energy levels

d)

how many negative charges an electron has

57.
How many electrons are represented by a single straight line in a Lewis structure?
a)
1
b)
2
c)
4
d)
6
58.

The most electronegative atom on the periodic table is:

a)
Fluorine
b)
Helium
c)
Neon
d)
Francium
59.
Which molecule contains bonds with a GREATER polarity?
a)
HCl
b)

CCl4

60.

The electronegativity difference in the bonds of CH4 (methane) is:

a)

small enough to be nonpolar

b)

small enough to be irrelevant

c)

large enough to be polar

d)

large enough to be important enough for you to learn everything about it

61.

The electronegativity difference in the bonds of CCl4 (carbon tetrachloride) is:

a)
0.4
b)

0.6

c)

5.7

d)

Numbers

62.

Use the molecular model's shape to predict the most likely type of molecule shown.

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

63.

The molecule (CCl4) shown is ___________-.

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

64.

What type of bond would form between calcium and fluorine?

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

65.

Water which is polar likes to dissolve what stuff? Pick as many options that apply.

a)

ionic compounds

b)

polar molecules

c)

nonpolar molecules

d)

metallic compounds

66.

What is the correct Lewis Dot Structure for ammonia NH3

a)

b)

c)

d)

67.

Which is the correct Lewis diagram for carbon dioxide, CO2?

a)

b)

c)

d)

68.

What causes a partial charge (a dipole) to develop across a molecule with 2 atoms?

a)

unequal sharing of electrons

b)

an electronegativity difference between 0.4 and 1.7

c)

electron spends more time around one of the atoms

d)

all of the above

69.

Which has the greater Electronegativity:

N or C?

You shouldn't need a chart for this ... !!!

a)

C

b)

N

70.

Based on their location on the periodic table, which has the greater Electronegativity:

H or F?

a)

H

b)

F

71.

Put these in increasing order of electronegativity:

F, N, B (smallest on left; largest on right)

a)

B < N < F

b)

B < F < N

c)

N < F < B

d)

F < N < B

72.

Put these in increasing order of electronegativity:

C, H, and O (smallest on left; largest on right)

a)

H < C < O

b)

H < O < C

c)

O < C < H

d)

C < H < O

73.

Which has the greater electronegativity:

Cl or Al?

a)

Cl

b)

Al

74.

Electronegativity is...

a)

how much an atom wants electrons in a bond

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.

75.

Which of the following is the least electronegative element?

a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
76.

How many bonds does chlorine typically make?

[Huh? Draw its single element dot diagram showing its valence electrons.]

a)

1

b)

2

c)

3

d)

4

e)

7

77.

How many bonds does nitrogen typically make?

a)

1

b)

2

c)

3

d)

4

e)

5

78.

How many bonds does carbon typically make?

a)

1

b)

2

c)

3

d)

4

e)

5

79.

How many bonds does hydrogen typically make?

a)

1

b)

2

c)

3

d)

4

e)

5

80.

The octet rule says that most atoms want to have ____ valence electrons?

a)

1

b)

2

c)

3

d)

4

e)

8

81.

How many valence electrons does nitrogen have?

a)

1

b)

2

c)

3

d)

4

e)

5

82.

Which atom would likely be the central atom if H, C, and O are in a molecule? (choose the one that makes the most bonds)

a)

H

b)

C

c)

O

d)

all of these

e)

the center? where we hang out?

83.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
84.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
85.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
86.

The formation of which type of bond usually releases the most energy?

a)

polar covalent

b)

nonpolar covalent

c)

metallic

d)

ionic

87.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
88.
How would you describe this structure?
a)
diatomic, linear, polar
b)
diatomic, linear, nonpolar
c)
monatomic,nonpolar, linear
d)
monatomic, polar, linear
89.

Which compound would have a high melting point?

a)

CaCl2

b)

CO2

c)

PI3

d)

SO3

90.
Which substance would be polar?
a)
O2
b)
HCl
c)
CO2
d)
CH4
91.
Which substance is nonpolar?
a)
water
b)
N2
c)
NH3
d)
HCl
92.
What is the shape of this molecule?
a)
linear
b)
bent
c)
triognal planar
d)
tetrahedral
93.
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
94.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
95.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
96.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
97.
Multiple bonds are possible if _______, ______, and ________ are present in a molecule.
a)
C,H,O
b)
H,O,N
c)
H,N,Cl
d)
C,N,O
98.
After drawing in your bonds, what do you do if you don't have enough electrons to get each atom to its octet?
a)
Place dots until everything has eight
b)
Place dots only around the outer atoms
c)
Make a double bond
d)
Have eight only around the central atom
99.
Which molecule below would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
100.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
101.

2. The first step to creating a Lewis structure is going to be finding the total number of valence electrons. What is the total number of valence electrons for the compound HNO2?

a)

19

b)

16

c)

18

d)

20

102.

Except for hydrogen (H), the least electronegative element should be the central atom in a Lewis diagram. Out of the atoms listed, which should be in the center?

a)

Nitrogen

b)

Oxygen

c)

Hydrogen

d)

Fluorine

103.

10. The proper structure of the HNO2 molecule is seen here. It has four bonds, two single and one double, and nitrogen is the central atom that the oxygens are bonded to. Looking at this final structure, is this molecule polar or nonpolar? Describe how you know.

a)

nonpolar

b)

polar

104.

Conductivity in a metal results from the metal atoms having

a)

high electronegativity

b)

high ionization energy

c)

highly mobile protons in the nucleus

d)

highly mobile electrons in the valence shell

105.

Which type of substance is soft, has a low melting point and is a poor conductor of heat and electricity?

a)

network solid

b)

molecular solid

c)

metallic solid

d)

ionic solid

106.

Which compound contains both ionic and covalent bonds?

a)

CaCO3

b)

CH2Cl2

c)

NaCl

d)

C6H12O6

107.

Molecules:

a)

have covalent bonds and are always polar

b)

have covalent bonds and are always non-polar

c)

have covalent bonds and can be polar or non-polar

d)

have ionic bonds and are always polar

108.

The following properties are all characteristics of ionic compounds EXCEPT

a)

solid at room temperature

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

109.

Which types of elements become cations?

a)

non-metals

b)

metals

c)

metalloids

110.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
111.

Ionic bonds could be best described as:

a)

A bond formed when 2 atoms share electrons

b)

A firm handshake

c)

An electrostatic attraction between oppositely charged ions

d)

An electrostatic attraction between anions

112.

Which type of bond is formed from the sharing of electrons?

a)

ionic bond

b)

covalent bond

113.

What set of elements is most likely to form a covalent compound?

a)

Na and O

b)

Na and K

c)

O and C

114.

Which set of elements is most likely to form an ionic compound?

a)

Na and O

b)

C and O

c)

Na and K

115.

Molten or dissolved compound conducts electricity.

a)

ionic compound

b)

covalent compound

116.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
117.

Which of the following is a molecular compound?

a)

CaO

b)

NaCl

c)

MgCl2

d)

CH4

118.

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

119.

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

120.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

121.

Which bond is the most polar of the group?

a)

H--H

b)

H--C

c)

H--N

d)

H--O

122.

Which bond is LEAST polar?

a)

O=O

b)

O-H

c)

O-N

d)

O=C

123.

Which bond is the most polar?

a)

C--O

b)

C--F

c)

C--N

d)

C--P

124.
Which is the correct structure for ammonia?
(Top picture is A, bottom picture is D.)
a)
Option A
b)
Option B
c)
Option C
d)
Option D
125.
This could be the dot diagram of
a)
P
b)
Ar
c)
Na
d)
B
126.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
127.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
128.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
129.

Which type of bond involves sharing electrons?

a)

Metallic

b)

Ionic

c)

Nuclear

d)

Covalent

130.

Molten or dissolved compound conducts electricity.

a)

ionic compound

b)

covalent compound

131.

Which three of the following are features of ionic compounds? (click 3 boxes)

a)

They have bonds between metals and non-metals.

b)

They have bonds between two non-metals.

c)

They form simple molecular structures.

d)

They form giant ionic lattices.

e)

They involve the transfer of electrons.

132.

True or false? Ionic compounds have high melting points.

a)

true

b)

false

133.

Why do ionic compounds conduct electricity when they are molten or dissolved?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

134.

Why do ionic compounds NOT conduct electricity when they are in their solid state?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

135.

The bond between two chlorine atoms in Cl2 molecule is ...

a)

Ionic

b)

Covalent polar

c)

Covalent nonpolar

d)

metallic

136.

NH3 is a ... molecule

a)

Polar

b)

Nonpolar

137.

A polar bond happens between ...

a)

metal and non metal

b)

Two non metals of the same electronegativity

c)

Two non metals, one is more electronegative than the other

d)

Two metals

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