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Worksheets

HM4 Bonding Exam Review

Total questions: 220

Worksheet time: 4hrs 34mins

Name
Class
Date
1.

What is the shape of this molecule?

a)

Linear

b)

Bent

c)

Trigonal planar

d)

Trigonal Pyramidal

e)

Tetrahedral

2.

What is the shape of this molecule?

a)

Linear

b)

Bent

c)

Trigonal planar

d)

Trigonal Pyramidal

e)

Tetrahedral

3.

What is the shape of this molecule?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Trigonal pyramidal

e)

Trigonal planar

4.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
5.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
6.

Will this molecule be polar or nonpolar?

a)

polar

b)

nonpolar

c)

no way to tell

7.

Will this molecule be polar or nonpolar?

a)

polar

b)

nonpolar

c)

no way to tell

8.

What is the shape of this molecule?

a)

Linear

b)

Bent

c)

Tetrahedral

d)

Trigonal Pyramidal

e)

Trigonal Planar

9.

Is this molecule polar?

a)

No

b)

Yes

10.

What shape is this?

a)

linear

b)

bent

c)

trigonal planar

d)

trigonal pyramidal

e)

tetrahedral

11.

What shape is this?

a)

linear

b)

bent

c)

trigonal planar

d)

trigonal pyramidal

e)

tetrahedral

12.

What shape is this?

a)

linear

b)

bent

c)

trigonal planar

d)

trigonal pyramidal

e)

tetrahedral

13.

What shape is this?

a)

linear

b)

bent

c)

trigonal planar

d)

trigonal pyramidal

e)

tetrahedral

14.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
15.

Which of the following images represents a Trigonal Planar molecular geometry?

a)
b)
c)
d)
16.
The ability of an atom to attract electrons to itself is called
a)
geometry
b)
conductivity
c)
electronegativity
d)
ionization energy
17.

Is this molecule polar?

a)

yes

b)

no

c)

no way to tell

18.

Is this molecule polar?

a)

yes

b)

no

c)

no way to tell

19.

Why is this molecule polar, even though it doesn't have electrons on the central atom?

a)

It's trigonal planar.

b)

It's asymmetrical.

c)

It's not polar.

d)

It's trigonal pyramidal.

20.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Bent

d)

Tetrahedral

21.

Which type(s) of intermolecular force(s) applies to this molecule? H2OH_2O

a)

London Dispersion Forces (LDF)

b)

London Dispersion Forces (LDF) and Dipole-Dipole Forces (DD)

c)

Hydrogen bonding (HB), Dipole-Dipole (DD) and London Dispersion Forces (LDF)

22.

Which type(s) of intermolecular force(s) applies to this molecule?

a)

London Dispersion Forces (LDF)

b)

London Dispersion Forces (LDF) and Dipole-Dipole Forces (DD)

c)

Hydrogen bonding (HB), Dipole-Dipole (DD) and London Dispersion Forces (LDF)

23.

Which type(s) of intermolecular force(s) applies to this molecule?

a)

London Dispersion Forces (LDF)

b)

London Dispersion Forces (LDF) and Dipole-Dipole Forces (DD)

c)

Hydrogen bonding (HB), Dipole-Dipole (DD) and London Dispersion Forces (LDF)

24.

Which type(s) of intermolecular force(s) applies to this molecule?

a)

London Dispersion Forces (LDF)

b)

London Dispersion Forces (LDF) and Dipole-Dipole Forces (DD)

c)

Hydrogen bonding (HB), Dipole-Dipole (DD) and London Dispersion Forces (LDF)

25.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
26.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
27.

Which noble gas has the highest boiling point because it has the strongest London dispersion forces due to its high number of electrons?

a)

Xe

b)

Kr

c)

Ar

d)

He

28.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
29.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

30.

Which have relatively low melting points and boiling points?

a)

ionic compounds

b)

molecular compounds

c)

both

d)

no such generalization can be made

31.

If two covalently bonded atoms are identical (the same element bonded to itself), what sort of bond is holding them together?

a)

ionic bond

b)

polar covalent bond

c)

nonpolar covalent bond

d)

metallic bond

32.

How are polyatomic ions held together?

a)

ionic bonds

b)

covalent bonds

c)

metallic bonds

33.

Which of these is the strongest?

a)

single covalent bond

b)

double covalent bond

c)

triple covalent bond

d)

ionic bond

34.

Which of the following is not naturally found as a diatomic molecule?

a)

hydrogen

b)

helium

c)

oxygen

d)

iodine

35.

Which of the following is not a diatomic molecule?

a)

N2

b)

O2

c)

I2

d)

S2

36.

Which category of elements have the property of being malleable and ductile?

a)

gases

b)

metalloids

c)

nonmetals

d)

metals

37.

What type of forces attract one molecule to another

a)

intramolecular forces

b)

ionic bonds

c)

intermolecular forces

d)

covalent bonds

38.

Which of these has only dispersion forces?

a)

I2

b)

NH3

c)

OCl2

d)

SH2

39.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
40.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)

bond order

b)

density

c)

solubility

d)

molecular polarity
(lone pairs)

41.

Which of the following will have the lowest melting point because it has the weakest intermolecular forces?

a)
b)
c)
d)
42.

Which type(s) of intermolecular force(s) applies to this molecule?

a)

London Dispersion Forces (LDF)

b)

London Dispersion Forces (LDF) and Dipole-Dipole Forces (DD)

c)

Hydrogen bonding (HB), Dipole-Dipole (DD) and London Dispersion Forces (LDF)

43.

Which shapes have lone pairs of electrons on their central atom?

a)

Bent and Trigonal Pyramidal

b)
Trigonal Planar and Bent
c)

Tetrahedral and Trigonal Pyramidal

d)

Trigonal Pyramidal and Linear

44.

How many unshared pairs of electrons can a bent molecule have?

a)

0

b)

2

c)

3

d)

1

45.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
46.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
47.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
48.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
49.
Will this molecule be polar or nonpolar? CS2
a)
polar
b)
nonpolar
50.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
51.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
52.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
53.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
54.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
55.
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
56.

By replacing the element symbol, this could be a diagram of which element?

a)

Li

b)

Al

c)

C

d)

Be

57.

NH3 has how many lone pairs on the central atom?

a)

0

b)

1

c)

2

d)

3

58.

What is the central atom in nitrate ion (NO3- )

a)

3

b)

O

c)

N

d)

none

59.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
60.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
61.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
62.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
63.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
64.

3. Which is a correct Lewis structure for hydrogen cyanide, HCN?

a)
b)
c)
d)
65.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
66.

To draw a Lewis structure, we need to find the --

a)

number of valence electrons in each atom.

b)

atomic mass of each atom.

c)

bond length of each atom.

d)

ionization energy of each atom.

67.

Which picture is the correct Lewis Dot Structure for HCl?

a)
b)
c)
d)
68.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
69.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
70.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
71.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

72.

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

a)

Single

b)

Double

c)

Triple

73.

Hydrogen being an exception to the octet rule, needs _____ electrons in its outer energy level to be stable.

a)

4

b)

6

c)

8

d)

2

74.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
75.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
76.

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

a)

8

b)

4

c)

2

d)

3

77.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
78.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

79.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
80.

How many connection points does carbon have to bond?

a)

2

b)

4

c)

6

d)

8

81.

How many valence electrons does Oxygen have?

a)

8

b)

5

c)

6

d)

1

82.

How many valence electrons should boron (B) have around its lewis dot structure?

a)

5

b)

6

c)

4

d)

3

83.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
84.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
85.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
86.

dinitrogen pentoxide

a)

N2O5

b)

NO5

c)

N5O2

d)

N2O6

87.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
88.

P₄S₁₀

a)

tetrapotassium decasulfide

b)

phosphorus decasulfide

c)

tetraphosphorus decasulfide

d)

phosphorus (X) sulfide

89.

SO₃

a)

sulfate

b)

sulfur oxide

c)

sulfur trioxide

d)

monosulfur trioxide

90.

tetraphosphorus heptoxide

a)

K₄O₁₀

b)

P₄O7

c)

KO

d)

P₁₀O₄

91.

chlorine dioxide

a)

ClO2

b)

ClO

c)

ClO3

d)

HClO2

92.

hexaboron monosilicide

a)

B6Si

b)

BSi

c)

BSi6

d)

B6Si6

93.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

94.
The chemical formula of carbon tetrachloride is
a)
CCl
b)
C₄Cl
c)
CCl₄
d)
C(IV)Cl
95.
The name of P₄S₁₀ is
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
96.
What is the formula for Hexaboron Monosilicide
a)
B6Si
b)
BSi
c)
BSi6
d)
B6Si6
97.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
98.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
99.
P3F4
a)
Phosphorous fluoride
b)
Triphosphorous tetrafluoride
c)
Phosphate Fluoride
d)
Trifluoride hexafluoride
100.
NO
a)
Mononitrogen monoxide
b)
nitrogen oxide
c)
nitrogen monoxide
d)
nitrate monoxide
101.
SiCl6
a)
Monosilicon hexachloride
b)
Silicon hexachloride
c)

Silicon heptachloride

d)
Monosilicon heptachloride
102.
Tribromine nonoxide
a)
Br3O9
b)
Br3O10
c)
Br3O6
d)
Br3O4
103.
Octanitrogen tetraoxide
a)
N8O3
b)
N7O3
c)
N8O3
d)
N8O4
104.
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.
105.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
106.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
107.
PBr5
a)
Phosphorus Bromide
b)
Phosphorus Pentabromide
c)
Pentaphosphorus bromide
d)
Phosphorus Bromine
108.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
109.

Match the following

a)

CF4

1.

Carbon Tetrafluoride

b)

CH4

2.

Carbon Tetrahydride

c)

SCl2

3.

Sulfur Dichloride

d)

NBr3

4.

Nitrogen TriBromide

e)

CO2

5.

Carbon Dioxide

110.

Antimony tribromide

a)

AnBr3

b)

AtBr3

c)

Sb1Br3

d)

SbBr3

111.

Hexaboron monosilicide

a)

B5S

b)

B6S

c)

B6Si

d)

Br6Si1

e)

Br6Si

112.

Chlorine dioxide

a)

Cl1O2

b)

CO2

c)

ClO2

d)

CrO2

113.

Hydrogen iodide

a)

H1I1

b)

HI

c)

HyIo

d)

HIo1

114.

Si2Br6

a)

silicon bromide

b)

disilicide bromide

c)

disilicon hexabromide

d)

disilicide hexabromide

115.

SF4

a)

sulfur quadchloride

b)

sulfur tetrafluoride

c)

monosulfur tetrafluoride

d)

sulfide tetrafluoride

116.

B2Si

a)

dibromine silicon

b)

diboron monosilicide

c)

diboron monosulfide

d)

dibromine monosilicide

117.

Se5I9

a)

hexasilicon nonaiodide

b)

pentaselenium noniodide

c)

heptaselenium noniodine

d)

pentasilicon noniodide

118.

Mg and Cl create...

a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
119.

H and S create...

a)
H2S
b)
HS2
c)
H2S2
d)
HS
120.

Ca and N create...

a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
121.

Li and P create...

a)
Li3P
b)
LiP3
c)
LiP
d)
Li2P
122.

Na and Cl create...

a)

Na2Cl

b)

NaCl2

c)

Na2Cl2

d)

NaCl

123.

K and S create...

a)

K2S

b)

KS2

c)

K2S2

d)

KS

124.

Mg and O create...

a)

Mg2O3

b)

MgO2

c)

MgO

d)

Mg2O

125.

Ca and F create...

a)

Ca2F2

b)

Ca3F

c)

CaF2

d)

Ca2F

126.

Al and P create...

a)

Al3P

b)

AlP3

c)

AlP

d)

Al2P

127.

Ba and Cl create...

a)

Ba2Cl

b)

BaCl2

c)

Ba2Cl2

d)

BaCl

128.
What is the formula for the compound formed by magnesium ions and nitrogen ions?
a)
MgN
b)
Mg2N3
c)
Mg3N2
d)
MgN3
129.
Which of the following will form an ion with a 2- charge?
a)
Ca
b)
Se
c)
Ge
d)
N
130.
What charge does a calcium (Ca) ion have?
a)
+1
b)
+2
c)
+3
d)
+4
131.
A phosphorus atom needs to gain ___ electrons to achieve a full octet.
a)
3
b)
4
c)
6
d)
5
132.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
133.

K + and N-3 form...

a)

KN

b)

KN3

c)

K3N3

d)

K3N

134.
Cations are
a)
positive
b)
negative
c)
on the right side of the periodic table.
d)
nonmetals
135.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
136.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
137.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
138.

Which of the following is an ionic compound:

a)

CH4

b)

I2

c)

LiBr2

d)

CO

139.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
140.
What is the FORMULA for...
calcium arsenide
a)
Ca3As2
b)
CaAs2
c)
Ca3As
d)
Ca3Ar2
141.

Write the formula for barium + nitrogen

a)

Ba2N3

b)

Ba3N2

c)

BaN

d)

BaN3

142.

Na+ and Cl- create...

a)

Na2Cl

b)

NaCl2

c)

Na2Cl2

d)

NaCl

143.
Ca2+ and N3- create...
a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
144.

The formula of calcium and phosphate is

a)

CaPO4

b)

Ca2(PO4)3

c)

Ca3PO4

d)

Ca3(PO4)2

145.

The chemical formula of Iron (III) and bromine is

a)

FeBr

b)

Fe(III)Br

c)

FeBr₃

d)

Fe₂Br₃

146.
Fe +2  and  SO4 -2
a)
FeSO4
b)
Fe4(SO4)2
c)
FeSO2
d)
correct answer is not given
147.
Ca +2  and  OH -
a)
Ca2OH
b)
CaOH2
c)
Ca(OH)2
d)
correct answer is not given
148.

What is the formula for copper(I) and sulfate?

a)

CuSO3

b)

CuSO4

c)

Cu2SO3

d)

Cu2SO4

149.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
150.
The formula of calcium phosphate is 
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
151.

Pb4+ and O2- create...

a)

Pb2O

b)

PbO2

c)

Pb2O2

d)

PbO

152.

Rb+ and P3- create...

a)

Rb3P

b)

RbP3

c)

RbP

d)

Rb2P

153.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
154.
If copper (II) and phosphate bond together, the resulting chemical formula would be:
a)
Cu2(PO4)3
b)
CuPO4
c)
Cu3(PO4)2
d)
Cu3PO4
155.
What is the formula for iron(II) carbonate?
a)
Fe2CO3
b)
FeCO3
c)
Fe2CO2
d)
FeCO4
156.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
157.

Which two elements would NOT form an ionic bond?

a)

calcium and lithium

b)

calcium and oxygen

c)

lithium and oxygen

d)

calcium and carbon

158.

A sodium ion has a charge of

a)

-1

b)

-2

c)

+1

d)

+2

159.

What is the correct molecular formula of Calcium Chloride?

a)

CaCl

b)

Ca2Cl

c)

CaCl2

d)

Ca3Cl2

160.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

161.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

162.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

163.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

164.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

165.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

166.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

167.

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

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

168.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

169.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

170.
name the following ionic compound: NaF
a)
nitrogen fluorine
b)
sodium fluoride
c)
nitrogen fluoride
d)
sodium fluorine
171.
Name this compound: 
KF
a)
Potassium fluoride
b)
Potassium fluorite
c)
Fluorine potasside 
d)
Potassium fluorate
172.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
173.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
174.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
175.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
176.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
177.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
178.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
179.
The chemical formula of iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
180.
What is the formula for calcium phosphide?
a)
CaP
b)
Ca2P3
c)
Ca3P2
d)
Ca2P
181.

If a sulfate ion has a charge of 2-, how many sodium ions will combine with one sulfate ion?

a)

1

b)

2

c)

3

d)

2.5

182.

The chemical formula for CaS is

a)

Cerium sulfide

b)

Carbon sulfur

c)

Calcium sulfide

d)

Calcium sulfur

183.

Which of these is NOT a polyatomic ion?

a)

OH-

b)

CO32-

c)

PO43-

d)

Cl-

e)

ClO4-

184.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

185.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

186.

electrons are transferred

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

187.

electrons are shared

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

188.

delocalized electrons

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

189.

nonconductors

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

190.

good conductors when solid

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

191.

good conductors when liquid (molten) or dissolved in water

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

192.

lustrous, malleable and ductile

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

193.

soft and easy to crush

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

194.

low melting and boiling points

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

195.

high melting and boiling points

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

196.

hard and brittle

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

197.

liquids and gases at room temperature

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

198.

strong forces

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

199.

usually solid at room temperature

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

200.

are volatile liquids

a)

Covalent Bonding

b)

Ionic Bonding

c)

Metallic Bonding

201.

electrons are shared equally
(there are no partial charges)

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

202.

electrons are shared unequally
(there are partial positive and negative charges)

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

203.

The difference between the electronegativities are so large that the electron is stolen by the more electronegative atom.

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

204.

What type of bonding will occur between:
oxygen and carbon

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

205.

What type of bonding will occur between:
gold and silver

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

206.

What type of bonding will occur between:
aluminum and titanium

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

207.

What type of bonding will occur between:
lead and tin

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

208.

What type of bonding will occur between:
mercury and silver

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

209.

What type of bonding will occur between:
silicon and phosphorus

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

210.

What type of bonding will occur between:
carbon and boron

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

211.

What type of bonding will occur between:
germanium and arsenic

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

212.

What type of bonding will occur between:
iodine and astatine

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

213.

What type of bonding will occur between:
chlorine and bromine

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

214.

What type of bonding will occur between:
arsenic and phosphorus

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

215.

What type of bonding will occur between:
oxygen and sylfur

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

216.

What type of bonding will occur between:
carbon and bromine

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

217.

What type of bonding will occur between:
nitrogen and iodine

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

218.

What type of bonding will occur between:
selenium and boron

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

219.

What type of bonding will occur between:
phosphorus and iodine

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

220.

What type of bonding will occur between:
oxygen and bromine

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

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9th - 12th Grade