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Bonding and Lewis structures

Total questions: 50

Worksheet time: 2hrs 35mins

Name
Class
Date
1.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
2.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
3.

Which type of bond has a transfer of an electron from a metal to a non-metal atom?

a)

Polar Covalent

b)

Non Polar Covalent

c)

Ionic

d)

Metallic

4.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
5.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
6.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
7.

Which type of bond creates a "sea" of electrons between atoms?

a)

Ionic Bonds

b)

Covalent Bonds

c)

Metallic Bonds

d)

Saving Bonds

8.
What type of bond forms between two or more atoms that are charged (+/-)?
a)
Covalent bond
b)
Incomplete bond
c)
Ionic bond
d)
Metallic bond
9.
Which of the following is an example of an IONIC COMPOUND?
a)
NaCl
b)
H2O
c)
CO2
d)
NO
10.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
11.
Which category of elements have the property of being malleable and ductile?
a)
gases
b)
metals
c)
metalloids
d)
nonmetals
12.
Ionic bonds are between _______ and ________. 
a)
nonmetals and nonmetals 
b)
metals and metals 
c)
metals and nonmetals
d)
none
13.
The compound formed between lithium and chlorine is _________.
a)
ionic
b)
covalent
14.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
15.

Which of the following descriptions of ionic compounds will NOT conduct electricity because the ions cannot move?

a)

when dissolved in water

b)

as a solid

c)

molten state

16.

The bonds in Na2O are best described as

a)

covalent, because valence electrons are shared.

b)

covalent, because valence electrons are transferred

c)

ionic, because valence electrons are shared.

d)

ionic, because valence electrons are transferred.

17.

Determine the type of bond in a nitrogen molecule (N2).

a)

Double covalent

b)

Single covalent

c)

Ionic

d)

Triple covalent

18.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
19.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
20.
How many electrons can be used in the Lewis Structure for : NO3 -
a)
23
b)
20
c)
18
d)
24
21.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
22.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
23.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
24.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
25.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
26.

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

a)

8

b)

4

c)

2

d)

3

27.

NBr3 has how many lone pairs on the central atom?

a)

0

b)

1

c)

2

d)

3

28.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

29.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

30.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

31.

CHCl3 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

32.

CH2O has which of the following?

a)

Multiple double bonds

b)

Multiple single bonds

c)

One double bond

d)

One single bond

e)

A lone pair

33.

Which of the following elements are an exception to the octet rule and require less than 8 valence electrons?

a)

H

b)

P

c)

B

d)

C

34.
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
35.
Which of the following is an ionic bond?
a)
H3N
b)
CaCl2
c)
NO2
d)
SCl
36.
Choose the structure that forms a double bond.
a)

Carbon tetrachloride (CCl4)

b)
Carbon dioxide (CO2)
c)
Water (H2O)
d)
Cyanic Acid (HCN)
37.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
38.

The Lewis dot structure for a boron atom has?

a)

1 lone electron

b)

3 lone electrons

c)

1 pair and 1 lone electron

d)

two pairs of electrons

39.

How many lone pairs are on the central atom of ClF₃?

a)

3

b)

0

c)

4

d)

2

40.

Atoms that are bonded with an electronegativity difference of 0.3 to 1.5 are generally considered to be

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

41.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
42.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
43.
If Boron bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
44.
If Bromine bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
45.

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

46.

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

47.

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

48.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number of electrons

49.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number electrons

50.
a)

achieved octet

b)

incomplete octet

c)

expended octet

d)

odd number electrons

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