wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

IPC Unit 5 Review

Total questions: 127

Worksheet time: 2hrs 6mins

Name
Class
Date
1.

What is the correct formula for lithium bromide?

a)

LiBr

b)

Li2Br2

c)

BrLi

d)

LiBr2

2.

What is the correct name for CaS?

a)

calcium sulfate

b)

calcium sulfide

c)

calcium monosulfide

d)

calcium sulfite

3.

What is the correct formula for potassium oxide?

a)

KO2

b)

KO

c)

K2O

d)

OK2

4.

What is the correct name for SrF2?

a)

fluoride strontium

b)

strontium fluorine

c)

strontium diflluoride

d)

strontium fluoride

5.

What is the correct name for VBr3?

a)

vanadium(III) bromide

b)

vanadium bromide

c)

vanadium(III) bromate

d)

vanadium tribromide

6.

What is the correct name for CrO?

a)

chromium monoxide

b)

chromium(I) oxide

c)

chromium(II) oxide

d)

chromium oxide

7.

What is the name of Co2Se3?

a)

cobalt(III) selenide

b)

dicobalt triselenide

c)

cobalt(II) selenide

d)

cobalt selenide

8.

What is the formula for copper(II) phosphide?

a)

Cu2P3

b)

Cu3P2

c)

Cu3(PO4)2

d)

Cu2P

9.

What is the correct formula for silver chromate?

a)

Ag2CO3

b)

Ag2Cr2O7

c)

AgCrO4

d)

Ag2CrO4

10.

What is the correct name for Zn(CN)2?

a)

zinc cyanide

b)

zinc dicyanide

c)

zinc carbide

d)

zinc(I) cyanide

11.

What is the correct name for (NH4)2CO3?

a)

diammonium carbonate

b)

nitrogen hydrogen carbon oxide

c)

ammonium carbonate

d)

ammonium carbide

12.

What is the correct name for Al2(SO4)3?

a)

aluminum(II) sulfate

b)

dialuminum trisulfate

c)

aluminum sulfide

d)

aluminum sulfate

13.

What is the correct name for Rh(C2H3O2)4?

a)

rhodium(I) acetate

b)

rhodium(IV) acetate

c)

rhodium tetraacetate

d)

rhodium acetate

14.

What is the correct formula for iron(III) permanganate?

a)

FeMnO4

b)

Fe(MnO4)3

c)

Fe3MnO4

d)

FeMn3O12

15.

What is the correct name for NiSO3?

a)

nickel(I) sulfite

b)

nickel(II) sulfite

c)

nickel(II) sulfate

d)

nickel(I) sulfate

16.

Which of the following is the correct formula for tungsten(VI) phosphate?

a)

W6PO4

b)

W2PO4

c)

W(PO4)2

d)

WP2O8

17.
Magnesium ion would take a charge of
a)
1+
b)
2+
c)
3+
d)
0
18.
Nitride
a)
has gained e-
b)
has lost e-
c)
is a cation
d)
doesn't exist
19.
The charge of V in V2O5 is?
a)
2+
b)
3+
c)
4+
d)
5+
20.
Which of the following elements would require Roman Numerals when it is named?
a)
Ga
b)
Ca
c)
B
d)
Au
21.
The correct name for the compound between sodium and sulfur is
a)
sodium sulfuride
b)
sodiumide sulfuride
c)
sodium sulfide
d)
sodium(I) sulfide
22.
How many of the aluminum ion are needed to form an ionic compound with chlorine
a)
0
b)
1
c)
2
d)
3
23.
Copper and phosphorus form an ionic compound. Which could be a possible name for their compound?
a)
Copper phosphorus
b)
Copper(I) phosphorus
c)
copper phosphide
d)
Copper(II) phosphide
24.
The formula for iron(III) oxide is
a)
FeO
b)
Fe3O
c)
Fe2O3
d)
Fe3O2
25.
Which of the following is not an ionic compound?
a)
Rb2Se
b)
gold(I) chloride
c)
N2O5
d)
barium phosphide
26.
What is the formula for sodium sulfide?
a)
SSu
b)
NaS
c)
Na2S
d)
NaS2
27.
What is the formula for boron selenide?
a)
B2Se3
b)
BSe
c)
BoSe
d)
B3Se2
28.
What is the charge of Ni in NiBr3?
a)
+2
b)
+3
c)
-3
d)
+6
29.
Which of the following metals gets a roman numeral in its name?
a)
Gallium
b)
Sodium
c)
Strontium
d)
Lead
30.
What is the name of Li3P?
a)
Lithium potassium
b)
Lithium III Phosophide
c)
Lithium3 Phosphide
d)
Lithium Phosphide
31.
Which of these is CoCl4?
a)
cobalt chlorine IV
b)
cobalt chloride
c)
cobalt IV chlorine
d)
cobalt IV chloride
32.
What is the formula for scandium II phosphide?
a)
Sc3P2
b)
S3P2
c)
S2P
d)
ScP
33.
What is the formula for a compound made of Mg2+ and As3-?
a)
Mg3As2
b)
Mg2As3
c)
MgAs
d)
Mg6As4
34.
What is the name for MnO2?
a)
Manganese II oxide
b)
Manganese dioxide
c)
Manganese 2 oxide
d)
Manganese IV oxide
35.
The roman numeral in a compound name indicates ___________________.
a)
the number of metal ions
b)
the charge of the metal ion
c)
nothing
d)
the number of total ions
36.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
37.
Bromine monoflouride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
38.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
39.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
40.
SeF4
a)
Tetraselenium fluoride
b)
Selenium Fluoride
c)
Selenium tetraflouride
d)
Selenium (IV) Fluoride
41.
CO
a)
Carbon Oxide
b)
Carbon Oxygen
c)
Dicarbon dioxide
d)
Carbon Monoxide
42.
PBr5
a)
Phosphorus Bromide
b)
Phosphorus Pentabromide
c)
Pentaphosphorus bromide
d)
Phosphorus Bromine
43.
Name the following compound:
  BF3
a)
boron fluoride
b)
boron difluoride
c)
monoboron trifluoride
d)
boron trifluoride
44.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
45.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
46.
chlorine monoxide
a)
ClO
b)
ClO-
c)
ClO2
d)
CO
47.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
48.

What is the name of the following:Ca(NO3)2

a)

Calcium Nitrate

b)

Calcium Nitrite

c)

Calcium Nitride

d)

Calcium Manganate

49.

What type of bond is CF4?

a)

ionic

b)

covalent

c)

metallic

50.

What is the greek prefix for 7?

a)

tetra

b)

hexa

c)

nona

d)

hepta

51.
When two atoms share electrons, a chemical bond is formed.  This type of bond is called:
a)
covalent bond
b)
ionic bond
c)
crystal bond
d)
polyatomic bond
52.
What type of compound consists of molecules that made of atoms that are covalently bonded?
a)
ionic
b)
crystal
c)
noncovalent
d)
molecular
53.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
54.
Which is true about covalent bonds?
a)
they are between 2 nonmetals
b)
they are between 2 metals
c)
they are between 1 metal and 1 nonmetal
55.
How many valence electrons does oxygen have?
a)
2
b)
3
c)
6
d)
4
56.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
57.
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
58.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
59.
What usually forms the negative ion?
a)
nonmetals
b)
metal
c)
none
60.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
61.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
62.
What is the formula for ammonium sulfate?
a)
NH4SO4
b)
NH4(SO4)2
c)
(NH4)2SO4
d)
(NH4)2S
63.
What is the formula for lead II oxide?
a)
PbO
b)
PbO2
c)
Pb2O
d)
Pb2O2
64.
N2
a)
Polar 
b)
Nonpolar 
65.
F2
a)
Polar 
b)
Nonpolar 
66.
H2O
a)
Polar 
b)
Nonpolar 
67.
NH3
a)
Polar 
b)
Nonpolar 
68.
NF3
a)
Polar 
b)
Nonpolar 
69.
PH3
a)
Polar 
b)
Nonpolar 
70.
BF3
a)
Polar 
b)
Nonpolar 
71.
CH4
a)
Polar 
b)
Nonpolar 
72.
CF4
a)
Polar 
b)
Nonpolar 
73.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

74.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

75.
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
76.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
77.
If Boron bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
78.
If Bromine bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
79.
When naming ionic compounds, the cation is always named first and the anion is always named second.
a)
False
b)
True
80.
A negatively-charged ion.
a)
atom
b)
cation
c)
anion
d)
electron
81.
Which of these combinations is an ionic compound made of?
a)
Metal and Metal
b)
Nonmetal and Nonmetal
c)
Metal and Nonmetal
d)
Cation and Cation
82.
What is oxidation number of Fe in FeO ?
a)
+2
b)
-2
c)
0
d)
+1
83.
What is oxidation number of Ca in CaCl2 ?
a)
-1
b)
-2
c)
+1
d)
+2
84.
What is oxidation number of Na in Na+ ?
a)
0
b)
+1/2
c)
+1
d)
-1
85.
What is oxidation number of Mn in MnO2 ?
a)
0
b)
+2
c)
-2
d)
+4
86.
What are oxidation numbers?
a)
Number of electrons in the outer most energy level
b)
Number of protons
c)
Electrons gained or lost in chemical bonding
d)
Number of neutrons gained or lost
87.
What are valence electrons?
a)
Number of electrons in the outer most energy level
b)
Number of electrons gained or lost
c)
Number of electrons in the inner energy level
d)
Number of electrons 
88.
What element's don't have oxidation numbers?
a)
alkali metals
b)
noble gases
c)
halogens
d)
alkaline earth metals
89.
The sum of all oxidation numbers in a neutral compound is ___.
a)
0
b)
1
c)
-1
d)
depends on the compound
90.
What is the oxidation number of Magnesium (Mg)?
a)
+2
b)
-2
c)
whats an oxidation number
91.
What is the oxidation number for Flourine (F)?
a)
+1 
b)
-1
c)
17
d)
7
92.
All the elements in group 13 would have an oxidation number of ..
a)
+3
b)
-3
c)
0
93.
Ba +3 and  Cl-
a)
Ba3Cl
b)
Ba3Cl3
c)
BaCl3
d)
BaCl
94.
K +  and  N-3
a)
KN
b)
KN3
c)
K3N3
d)
K3N
95.
Na +  and  S -2
a)
Na2S
b)
NaS2
c)
Na2S2
d)
NaS
96.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
97.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
98.
If electrons are shared equally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
99.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
100.
Which of the following is the correct Lewis  structure for the molecule fluorine (F2) ? (click the image to enlarge)
a)
A
b)
B
c)
C
d)
D
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.
Which is the correct structure for NH3 ?
(click the image to enlarge)
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D. 
103.

Large differences in electronegativity result in __________ bonding between atoms.

a)

Covalent

b)

Mettalic

c)

Ionic

d)

Hydrogen

104.

Hydrogen has an electronegativity of 2.20, fluorine an electronegativity of 3.98. What sort of bond do they form?

0-0.4= nonpolar; 0.41-1.7 = polar covalent; 1.71+ = ionic

a)

mostly ionic

b)

polar covalent

c)

mostly covalent

d)

nonpolar covalent

105.

Which has the greater Electronegativity:

N or C?

a)

C

b)

N

106.

Which has the greater Electronegativity:

H or F?

a)

H

b)

F

107.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
108.
Some are solids, some are liquids, and some are gases at room temperature.
a)
ionic compounds
b)
covalent compounds
109.
Molten compound conducts electricity.
a)
ionic compound
b)
covalent compound
110.
Molten compound does NOT conduct electricity.
a)
ionic compound
b)
covalent compound
111.

Have a high melting point (1000°C-3000°C)

a)

ionic compounds

b)

covalent compounds

112.

Have a low melting point (< 200°C)

a)

ionic compounds

b)

covalent compounds

113.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
114.
When dissolved in water, the solution does NOT conduct electricity.
a)
ionic compounds
b)
covalent compounds
115.
usually hard but brittle
a)
ionic compounds
b)
covalent compounds
116.
usually soft
a)
ionic compounds
b)
covalent compounds
117.
forms ions in solution
a)
ionic compounds
b)
covalent compounds
118.

The closer the elements are on the periodic table, their electronegativities are more similar. (True or False)

a)

True

b)

False

c)

none of the above

d)

maybe

119.

Prefix Mono

a)

1

b)

2

c)

3

d)

4

120.

Prefix Tetra-

a)

1

b)

3

c)

2

d)

4

121.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
122.
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.
123.
Metallic bonding is...
a)
a type of covalent bond.
b)
a type of ionic bond.
c)
an attraction between positive ions and electrons.
124.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
125.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
126.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
127.
What is the ability of a substance to allow heat, sound, or electricity to flow through it?
a)
Malleability
b)
Ductility
c)
Solubility
d)
Conductivity

Similar Resources on Wayground

Get ready 2

127 questions

Get ready 2

quiz

Worksheet

•

11th Grade

Ib Chem: Ions to Memorize (without ions that don't exist)

132 questions

Ib Chem: Ions to Memorize (without ions that don't exist)

quiz

Worksheet

•

11th Grade

C05 Electrons, Protons, and Neutrons

126 questions

C05 Electrons, Protons, and Neutrons

quiz

Worksheet

•

10th Grade - University

Spring Final Exam Review

129 questions

Spring Final Exam Review

quiz

Worksheet

•

10th Grade

Fall Final Practice Test

125 questions

Fall Final Practice Test

quiz

Worksheet

•

10th Grade

Naming Covalent Compounds

128 questions

Naming Covalent Compounds

quiz

Worksheet

•

10th - 12th Grade

Chapter 4-7 Test Review

131 questions

Chapter 4-7 Test Review

quiz

Worksheet

•

10th - 12th Grade

Unit 1 Concept 1 Review Ant

132 questions

Unit 1 Concept 1 Review Ant

quiz

Worksheet

•

9th - 12th Grade