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Ionic, covalent, metallic review questions

Total questions: 115

Worksheet time: 2hrs 10mins

Name
Class
Date
1.

Why do atoms form bonds with other atoms?

a)

To become more stable.

b)

To achieve a noble gas electron arrangement.

c)

To lower their energy.

d)

To raise their energy.

2.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
3.
Are the atoms more stable when they are bonded together or when they are apart? 
a)
Bonded Together
b)
Apart
4.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
5.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
6.
What happens when the sodium atom loses an electron?
a)
It become negatively charged 
b)
It become positively charged
c)
none
7.
What usually forms the negative ion?
a)
nonmetals
b)
metal
c)
none
8.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
9.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
10.
What charges attract?
a)
Opposite
b)
Same
11.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
12.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
13.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
14.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
15.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
16.
How many valence electrons does Lithium have?
a)
1
b)
2
c)
3
d)
4
17.
How many valence electrons does Carbon have?
a)
4
b)
12
c)
6
d)
14
18.
How many valence electrons does Hydrogen have?
a)
1
b)
2
c)
3
d)
4
19.
How many valence electrons does Argon (Ar) have?
a)
2
b)
8
c)
18
d)
40
20.
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
21.
How many valence electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
22.
This is a correct dot diagram for magnesium (Mg)
a)
true
b)
false
23.

Describe how cations form.

a)

The atom loses one or more electrons, leaving it with a positive charge, to become more stable like the nearest noble gas.

b)

The atom loses one or more electrons, leaving it with a negative charge, to become more stable like the nearest noble gas.

c)

The atom gains one or more electrons, leaving it with a positive charge, to become more stable like the nearest noble gas.

d)

The atom gains one or more electrons, leaving it with a negative charge, to become more stable like the nearest noble gas.

24.

If you make an ion out of an element in group 13, what will it's charge likely be?

a)

1+

b)

2+

c)

1-

d)

2-

e)

3+

25.

If you make an ion out of an element in group 1, what will it's charge likely be?

a)

1+

b)

2+

c)

1-

d)

2-

e)

3+

26.

If you make an ion out of an element in group 2, what will it's charge likely be?

a)

1+

b)

2+

c)

1-

d)

2-

e)

3+

27.

If you make an ion out of an element in group 16, what will it's charge likely be?

a)

1+

b)

2+

c)

1-

d)

2-

e)

3-

28.

If you make an ion out of an element in group 15, what will it's charge likely be?

a)

1+

b)

2+

c)

1-

d)

2-

e)

3-

29.
What is the formula for lithium oxide?
a)
LiO
b)
LiO2
c)
Li2O
d)
Li2O3
30.
What is the formula for copper(II) sulfate?
a)
CuSO4
b)
Cu2SO8
c)
CuS
d)
Cu(SO4)2
31.
Which of the following could form an ionic bond with sulfur?
a)
Oxygen
b)
Iodine
c)
Arsenic
d)
Magnesium
32.
Element X is from Group 13 and Element Y is from Group 16.  What is the formula of the compound formed?
a)
X2Y3
b)
X3Y2
c)
Y3X2
d)
X2Y
33.
What is the charge on the ion of P, and it has the same number of electrons as which noble gas?
a)
-3, Ar
b)
+3, Ne
c)
-3, Ne
d)
-4, Ar
34.
Why do elements bond to form compounds?
a)
To become stable
b)
To lower their energy
c)
To achieve an octet of valence electrons
d)
all of these
35.
The polyatomic ion:  SO42- has the name
a)
Phosphate
b)
Sulfate
c)
Sulfite
d)
Sulfur tetra oxide
36.
What formula results when Ca+2 and Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
37.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
38.
What is the formula for lithium acetate?
a)
LiAc
b)
LiCHO
c)
LiC2H3O2
d)
LiClO3
39.
Name NH4Cl
a)
Nitrogen Hydrogen Chloride
b)
Nitrogen Tetrahydrogen Chloride
c)
Ammonium Chloride
d)
Ammounium Calcide
40.
Name Fe(NO3)3
a)
Iron (III) Nitrate
b)
Iron (III) Nitride
c)
Iron (VI) Nitrate
d)
Iron Nitrate
41.
Name Al(CN)3
a)
Aluminum Cyanide
b)
Aluminum Carbon Nitrogen
c)
Aluminum Tricarbon trinitride
d)
Aluminum Tricarbonitride
42.
Name MgO
a)
Magnesium Oxygen
b)
Magnesium Oxide
c)
Magnesium Monoxide
d)
Magnesium Dioxide
43.
What is the formula of ammonium phosphide?
a)
NH4PO3
b)
NH3P
c)
(NH4)3PO4
d)
(NH4)3P
44.
What is the formula for copper (II) hydroxide?
a)
CuOH
b)
Cu(OH)2
c)
Cu2OH
d)
Cu2O
45.
MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)
magnesium(III) fluoride
d)
magnesium fluoride(II)
46.
What is the formula for potassium carbonate?
a)
P2CO3
b)
PCO3
c)
KCO3
d)
K2CO3
47.
What is the name of ZnSO4?
a)
zinc sulfide
b)
zinc sulfate
c)
zinc (II) sulfate
d)
zinc sulfite
48.
What is the name of the compound KClO3
a)
potassium chlorate
b)
potassium chlorine
c)
Potassium chlorine trioxygen
49.
What is the formula for the phosphate ion?
a)
PO32-
b)
PO3-
c)
PO2-
d)
PO43-
50.
What is the formula for the carbonate ion?
a)
CO32-
b)
CO3-
c)
CO2-
d)
CO42-
51.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
52.

When the element aluminum (Al) bonds with a nonmetal, then the compound formed is ionic. In this case,

a)

Aluminum loses three electrons to become a cation

b)

Aluminum loses three electrons to become an anion.

c)

Aluminum gains electrons to become a cation

d)

Aluminum gains electrons to become an anion

53.

Which of the following ions have the same electron configuration as neon (Ne)?

a)

Na+

b)

Mg2+

c)

N3-

d)

Cl-

e)

Li+

54.
a)

A

b)

B

c)

C

d)

D

55.
a)

A

b)

B

c)

C

d)

D

56.
a)

A

b)

B

c)

C

d)

D

57.
a)

A

b)

B

c)

C

d)

D

58.
a)

Li

b)

C

c)

P

d)

Br

e)

H

59.
a)

A

b)

B

c)

C

d)

D

60.

In the compound Al2(CO3)3, what is the cation in this formula?

a)

A

b)

B

c)

C

d)

D

61.

In the compound Al2(CO3)3, what is the charge on the anion?

a)

1-

b)

2-

c)

3-

d)

1+

e)

3+

62.

What is the formula of nitride?

a)

N2-

b)

N-

c)

NO2-

d)

N3-

e)

N5+

63.

What is the formula of zinc ion?

a)

Zn+

b)

Zn3+

c)

Zn2+

d)

Zn4-

e)

ZnO3-

64.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

65.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
66.
Metallic bonding occurs between atoms of 
a)
Iron (Fe)
b)
Argon (Ar)
c)
 Helium (He)
d)
Boron (B)
67.
Electrons that are free to move in a metal are referred to as...
a)
localized electrons
b)
delocalized electrons
c)
electrostatic electrons
d)
cations
68.

How many electrons does aluminum (Al) ion have?

a)

3

b)

10

c)

13

d)

18

69.

An atom with 6 valence electrons,

a)

Is a non-metal.

b)

Is in group 16.

c)

Will make an ion with a 2+ charge.

d)

Forms ionic compounds with metals.

70.

Element X has 2 valence electrons. Element Z has 7 valence electrons. What is the formula of the compound made from X and Z?

a)

XZ2

b)

XZ

c)

X2Z

d)

X2Z7

71.

Which compound is NOT ionic?

a)

MgCO3

b)

NO2

c)

NH4NO3

d)

K2O

72.

In the compound Co(NO3)2 what is the cation?

a)

cobalt (I) ion

b)

cobalt (II) ion

c)

Cobalt ion

d)

nitrate ion

73.

NaOH is called

a)

sodium oxide hydride

b)

sodium oxygen hydride

c)

sodium hydroxide

d)

sodium oxohydride

74.

Potassium acetate

a)

KC2H3O2

b)

K2O

c)

K2C2H3O2

d)

K2C2O4

e)

KAc

75.

iron (III) oxide

a)

Fe2O3

b)

Fe3O

c)

FeO

d)

Fe3O2

e)

Fe(OH)3

76.

barium sulfide

a)

BaS

b)

Ba2S

c)

BaSO4

d)

BaSO3

e)

BaS2

77.

Rubidium phosphate

a)

RbPO4

b)

Rb3PO4

c)

Rb2PO4

d)

Rb3PO3

e)

Rb2PO3

78.

This image shows two atoms connected with a ____.

a)

Single covalent bond

b)

Double covalent bond

c)

Triple covalent bond

d)

Ionic bond

79.

Which does this represent?

a)

ionic structure

b)

metallic structure

c)

covalent structure

d)

octet rule

80.

Which of the following apply to metallic solids?

a)

Delocalized electrons.

b)

Fixed cations surrounded by mobile electrons

c)

Mobile valence electrons

d)

Weak intermolecular forces

e)

Regular repeating pattern of positive and negative ions.

81.

Which of the following apply to ionic compounds?

a)

Delocalized electrons.

b)

Charged particles

c)

Weak intermolecular forces

d)

Regular repeating pattern of alternating charges.

82.

What type of bonding between these two elements? What happens to the valence electrons? Mg and F

a)

ionic bonding, valence electrons are transferred

b)

ionic bonding, valence electrons are shared

c)

covalent bonding, valence electrons are transferred

d)

covalent bonding, valence electrons are shared

83.

What type of bonding between these two elements? What happens to the valence electrons? H and N

a)

ionic bonding, valence electrons are transferred

b)

ionic bonding, valence electrons are shared

c)

covalent bonding, valence electrons are transferred

d)

covalent bonding, valence electrons are shared

84.

What type of bonding between these two elements? What happens to the valence electrons? Al and Br

a)

ionic bonding, valence electrons are transferred

b)

ionic bonding, valence electrons are shared

c)

covalent bonding, valence electrons are transferred

d)

covalent bonding, valence electrons are shared

85.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
86.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
87.
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.
88.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
89.

triple covalent occurs when two atoms share____

a)

one pair of electrons

b)

two pairs of electrons

c)

three pairs of electrons

d)

three pair of protons

90.

This image shows two atoms connected with a ____.

a)

Single covalent bond

b)

Double covalent bond

c)

Triple covalent bond

d)

Ionic bond

91.

This image shows two atoms connected with a ____.

a)

Single covalent bond

b)

Double covalent bond

c)

Triple covalent bond

d)

Ionic bond

92.

This image shows two atoms connected with a ____.

a)

Single covalent bond

b)

Double covalent bond

c)

Triple covalent bond

d)

Ionic bond

93.

This image shows two atoms connected with a ____.

a)

Single covalent bond

b)

Double covalent bond

c)

Triple covalent bond

d)

Ionic bond

94.

What is the correct Lewis Structure for the bond between Mg and Cl?

a)

A

b)

B

c)

C

d)

D

95.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
96.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
97.

What is the correct Lewis Structure and chemical formula for an ionic bond between Aluminum and Oxygen?

a)

A

b)

B

c)

C

d)

D

98.

What is the correct Lewis structure of ion NO3- ?

a)

b)

c)

d)

99.
How many electrons can be used in the Lewis Structure for : NO3 -
a)
23
b)
20
c)
18
d)
24
100.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
101.
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
102.
In the correct Lewis structure for CH4, how many unshared electron pairs surround the carbon?
a)
2
b)
8
c)
0
d)
4
103.
In CO2, how many UNSHARED pairs of electrons does each oxygen have?
a)
2
b)
1
c)
4
d)
6
104.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
105.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
106.

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

a)

8

b)

4

c)

2

d)

3

107.

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

a)

Single

b)

Double

c)

Triple

108.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
109.

The central S atom in this structure has which of the following?

a)

achieved octet

b)

incomplete octet

c)

expanded octet

d)

odd number electrons

110.

What do we call electrons that move freely in a metallic bond?

a)

sea of electrons

b)

lone electrons

c)

unpaired electrons

d)

covalent electrons

111.

What do electrons do in a metallic bond?

a)

They stay on the metal atom.

b)

They are transferred from atom to atom.

c)

They form a covalent bond with another atom.

d)

They float around freely.

112.

What is meant by the term "sea of electrons"?

a)

It's what we call all the free floating electrons in a metal.

b)

It's what we call electrons that are floating in a liquid.

c)

It's the total number of electrons in a metal atom.

d)

It's the total number of electrons in the ocean.

113.

What kind of bonding is pictured here?

a)

ionic

b)

metallic

c)

covalent

114.

What kind of bonding is pictured here?

a)

ionic

b)

metallic

c)

covalent

115.

What kind of bonding is pictured here?

a)

ionic

b)

metallic

c)

covalent

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