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Bonding Basics Review

Total questions: 59

Worksheet time: 5hrs 43mins

Name
Class
Date
1.

This image shows the bonding between Lithium and Fluorine. What does the red arrow show?

a)

electrons being shared

b)

electrons being transferred to Fluorine

c)

electrons being transferred to Lithium

d)

electrons being destroyed

2.

Which of the following is NOT a step in forming an ionic bond?

a)

One atom shares its electrons with another one

b)

Opposite charged ions form due to the transfer of electrons

c)

One atom gives electrons to another one

d)

Oppositely charged ions attract

3.

An ionic bond is the attraction between: (Select ALL that apply)

a)

oppositely charged ions

b)

similarly charged ions

c)

metals and nonmetals

d)

neutral atoms

e)

cations and anions

4.

If I had a cation with a charge of 2+ how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 4 electrons

d)

lost 4 electrons

5.

If I had an anion with a charge of 3- how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 3 electrons

d)

lost 3 electrons

6.

Looking at the periodic table, when the alkali metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

7.

Looking at the periodic table, when the alkaline earth metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

8.

Looking at the periodic table, when the halogens form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

9.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

10.

In the compound aluminum oxide, which is the cation?

a)

[ Al ] +3

b)

Al

c)

[ O ] -2

d)

O

11.

When ionic compounds form what is the overall charge?

a)

neutral

b)

positive

c)

negative

12.

What is responsible for bringing cations and anions together?

a)

the size of the ions

b)

the opposite charges are attracted to one another

c)

the similar charges are attracted to one another

d)

depends on what period they're in

13.

When assigning ionic charge it is always written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

14.

When assigning the number of individual atoms in a chemical formula it is written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

15.
What is the charge on a Hydrogen ion?
a)
+1
b)
1
c)
2
16.
What is the charge on an Aluminium ion?
a)
3
b)
+3
c)
+2
d)
+1
17.
What is the charge on a Hydrogen ion?
a)
+1
b)
1
c)
2
18.
What is the charge on an Aluminium ion?
a)
3
b)
+3
c)
+2
d)
+1
19.
What is the charge on a chloride ion?
a)
-1
b)
1
c)
+2
d)
+1
20.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
21.
A charged particle that has gained at least one electron is called a(n) _____.
a)
Anion
b)
Cation
c)
Anonion
d)
chemistry cat
22.
What is the ionic compound formed between K and F?
a)
KF
b)
K2F
c)
KF2
d)
K2F2
23.
What is the ionic compound formed between Ba and P?
a)
Ba2P3
b)
Ba3P2
c)
BaP
d)
Ba2P2
24.
What is the ionic compound formed between Ca and O?
a)
CaO
b)
Ca2O
c)
Ca2O2
d)
CaO2
25.
The compound formed by Mn (IV) and S would be which of these choices?
a)
Mn4S2
b)
MnS
c)
MnS4
d)
MnS2
26.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
27.
Which of the following describes covalent bonds?
a)
Bonds form because of opposite charges
b)
Bonds form to fill outer electron shells
c)
Electrons are transferred between atoms
d)
Covalent bonds are magical
28.
Protons have a charge of:
a)
-1
b)
+1
c)
-2
d)
+2
29.
Electrons have a charge of:
a)
-1
b)
-2
c)
+1
d)
+2
30.
Most atoms have no net charge because they have....
a)
an equal number of charged and non-charged particles
b)
neutrons in their nuclei
c)
an equal number of electrons and protons
d)
an equal number of neutrons and protons
31.
What would you name this molecule?
a)
SNa3
b)
H3O
c)
NaCl
d)
H2O
32.
What molecule is this?
a)
CO
b)
CO2
c)
C2O
d)
C2O2
33.
If a you saw the following, K+; what does it tell you about the  the ion.
a)
it has lost one electron 
b)
it has lost one proton 
c)
it has lost two electrons 
d)
it is a negative ion 
34.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
35.
What does a sodium atom become when it loses its only valence electron?
a)
sodium compound
b)
sodium atom
c)
ionic compound
d)
sodium ion
36.
What is the charge of a sodium ion with 11 protons and 10 electrons?
a)
1+
b)
1-
c)
2+
d)
2-
37.

If an atom has no charge, which of the following must be true?

a)

It has more neutrons than protons or electrons.

b)

There are only neutrons inside the atom.

c)

Its number of protons is equal to its number of electrons.

d)

The neutrons in the atom outnumber the electrons and protons.

38.

Which of these are an ion?

a)

3 protons, 3 neutrons, 3 electrons.

b)

8 protons, 8 neutrons, 8 electrons

c)

2 protons, 3 neutrons, 2 electrons

d)

6 protons, 6 neutrons, 7 electrons

39.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
None
d)
conduct electricity
40.
If a potassium atom loses one electron, a positive ion results.
a)
TRUE
b)
FALSE
41.
What is an atom or group of atoms that has an electric charge?
a)
ion
b)
metal
c)
nonmetal
d)
ionic compound
42.
If an atom of nitrogen gains 3 electrons, what is its overall charge?
a)
Neutral - No charge
b)
+3
c)
-3
d)
-1
43.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
44.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
45.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
46.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
47.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
48.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
49.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
50.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
51.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
52.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
53.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
54.
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
55.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
56.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
57.

Which of the following compounds has only single bonds?

a)

I only

b)

II only

c)

III only

d)

I and III

e)

III and IV

58.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

59.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

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