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WorksheetsCh6 Test Review (Covalent Compounds)
Total questions: 75
Worksheet time: 6hrs 7mins
Name
Class
Date
1.
Which will NOT form a diatomic molecule?
a)
fluorine
b)
nitrogen
c)
bromine
d)
boron
2.
Which type of bond has one pair of electrons shared between atoms?
a)
single covalent
b)
double covalent
c)
triple covalent
d)
ionic
3.
How many bonds can carbon form?
a)
1
b)
2
c)
3
d)
4
4.
How many bonds can halogens form?
a)
1
b)
2
c)
3
d)
4
5.
Covalent compounds display which of these properties?
a)
They are hard, brittle solids.
b)
They have high melting and boiling points.
c)
They display luster.
d)
They are usually insoluble in water.
6.
Which of these elements does NOT exist as a diatomic molecule?
a)
Ne
b)
F
c)
H
d)
I
7.
Which of the following elements can form diatomic molecules held together by triple covalent bonds?
a)
carbon
b)
oxygen
c)
nitrogen
d)
fluorine
8.
A molecule is formed when two or more atoms form a covalent bond. According to this definition, which of these is NOT a molecule?
a)
NaCl
b)
H2
c)
HCl
d)
NH3
9.
Which element can share only one pair of electrons?
a)
C
b)
H
c)
O
d)
N
10.
In forming a molecular structure, each atom should have ___ electrons around it unless there is some specific reason why this cannot be achieved.
a)
2
b)
4
c)
6
d)
8
11.
How many electrons does a nitrogen atom need to gain in order to attain stability?
a)
1
b)
2
c)
3
d)
4
12.
How many electrons are shared in a double bond?
a)
4
b)
2
c)
1
d)
0
13.
How many covalent bonds does phosphorus need to form in order to have a full octet?
a)
2
b)
3
c)
4
d)
5
14.
Which of the following will NOT be surrounded by an octet of electrons in a correctly drawn Lewis structure?
a)
C
b)
Cl
c)
O
d)
H
15.
Which of the following is NOT a property/characteristic of covalent compounds?
a)
May be a liquid at room temperature.
b)
Poor conductors of electricity.
c)
Have high melting points.
d)
Solid forms are soft or brittle.
16.
Which pair of elements is most likely to form a covalently bonded compound?
a)
Mg with Cl
b)
F with Cl
c)
Li with S
d)
Ni with Rn
17.
How many electrons are shared in a single bond?
a)
4
b)
2
c)
1
d)
0
18.
How many covalent bonds does carbon need to form in order to have a full octet?
a)
2
b)
3
c)
4
d)
5
19.
Which pair of elements is most likely to form a covalently bonded compound?
a)
Li with Cl
b)
S with O
c)
Ca with S
d)
Na with Br
20.
What kind of bond holds water molecules together?
a)
ionic
b)
metallic
c)
covalent
d)
hydrogen
21.
The bond that holds two fluorine atoms together in an F2 molecule would be classified as nonpolar covalent because
a)
both atoms are different and the difference in electronegativity is large.
b)
both atoms are different and the difference in electronegativity is zero.
c)
both atoms are the same and the difference in electronegativity is large.
d)
both atoms are the same and the difference in electronegativity is zero.
22.
In a water molecule, shared electrons spend more time around the oxygen atom than the hydrogen atoms. As a result, the oxygen atom is
a)
very positive.
b)
very negative.
c)
slightly positive.
d)
slightly negative.
23.
Which of the following is the correct formula for the compound dinitrogen hexaoxide?
a)
NO3
b)
NO2
c)
N2O6
d)
N2O5
24.
Which of the following is the correct formula for the compound dicarbon monosulfide?
a)
CS
b)
C2S2
c)
CS2
d)
C2S
25.
The common name of SiI4 is tetraiodosilane. What is its molecular compound name?
a)
silane tetraiodide
b)
silicon tetraiodide
c)
silicon iodide
d)
silane tetraiodine
26.
Which of the following is the correct name for the compound N2O3?
a)
dinitro trioxide
b)
nitrogen (II) oxide (III)
c)
trinitrogen dioxide
d)
dinitrogen trioxide
27.
Which of the following is the correct name for the compound N2O4?
a)
tetranitrogen dioxide
b)
dinitrogen tetroxide
c)
dinitrogen quadoxide
d)
nitrogen oxide
28.
Which of the following is the correct formula for the compound nitrogen dichloride?
a)
NBr
b)
NaCl
c)
NCl
d)
NCl2
29.
Which of the following prefixes mean four?
a)
mono-
b)
di-
c)
tri-
d)
tetra-
30.
Which of the following is the correct formula for the compound silicon tetrafluoride?
a)
SiF4
b)
SiF2
c)
SiF
d)
Si4F
31.
Which of the following is the correct formula for the compound dinitrogen monoxide?
a)
NO2
b)
(NO)2
c)
N2O1
d)
N2O
32.
Which of the following is the correct formula for the compound sulfur hexachloride?
a)
S6Cl
b)
SCl6
c)
SCl5
d)
S2Cl3
33.
Which of the following is the correct formula for the compound disulfur dibromide?
a)
SBr
b)
S2Br
c)
S2Br2
d)
SBr2
34.
What is the compound name for hydrazine, N2H4?
a)
trinitrogen quatrahydride
b)
dinitrogen tetrahydride
c)
trinitrogen pentahydride
d)
dinitrogen hydride
35.
How many lone pairs of electrons are in a molecule of hydrogen monoiodide?
a)
1
b)
2
c)
3
d)
4
36.
When drawing Lewis structures, a single line between 2 atoms represents
a)
a shared pair of electrons.
b)
an unshared pair of electrons.
c)
an octet of electrons.
d)
a donated electron.
37.
In the compound PCl3, how many total valence electrons are available?
a)
4
b)
8
c)
24
d)
26
38.
When drawing Lewis structures, which of the following is most likely the central atom?
a)
C
b)
N
c)
O
d)
H
39.
In the polyatomic ion (NO3)1-, how many total valence electrons are available?
a)
16
b)
9
c)
22
d)
24
40.
A molecule with a single covalent bond is ___.
a)
CO2
b)
Cl2
c)
CO
d)
N2
41.
Fluorine belongs to group 7A. How many covalent bonds are formed between two fluorine atoms?
a)
1
b)
2
c)
3
d)
4
42.
In the correct Lewis structure for water, how many lone (unshared) pairs of electrons will oxygen have?
a)
1
b)
2
c)
3
d)
4
43.
In the correct Lewis structure for ammonia (NH3), how many lone (unshared) pairs of electrons will nitrogen have?
a)
0
b)
1
c)
2
d)
3
44.
Which of the following compounds is an exception to the octet rule?
a)
BH3
b)
CH4
c)
NH3
d)
H2O
45.
In the compound CO2, how many total valence electrons are available?
a)
4
b)
6
c)
16
d)
18
46.
Which of the following diatomic elements has a double bond between its atoms?
a)
fluorine
b)
oxygen
c)
nitrogen
d)
hydrogen
47.
How many extra electrons are in the Lewis structure of the phosphate ion, (PO4)3-?
a)
0
b)
2
c)
3
d)
4
48.
Which of the following is the correct molecular shape of CF4?
a)
tetrahedral
b)
bent
c)
trigonal pyramidal
d)
linear
49.
The ammonia (NH3) molecule has a trigonal pyramidal shape. How do you know?
a)
N has 4 bonded atoms and 0 lone pairs
b)
N has 2 bonded atoms and 2 lone pairs
c)
N has 3 bonded atoms and 1 lone pair
d)
N has 6 bonded atoms and 0 lone pairs
50.
Which of the following is the correct molecular shape of water, H2O?
a)
linear
b)
trigonal pyramidal
c)
bent
d)
tetrahedral
51.
Which of the following is the correct molecular shape of CCl4?
a)
trigonal planar
b)
tetrahedral
c)
octahedral
d)
bent
52.
According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?
a)
pairs of valence electrons
b)
inner shell electrons
c)
mobile electrons
d)
the electrons closest to the nuclei
53.
Which of the following is the correct molecular shape of the methane molecule (CH4)?
a)
tetrahedral
b)
square
c)
trigonal planar
d)
trigonal pyramidal
54.
Which of the following is the correct molecular shape of BH3?
a)
trigonal planar
b)
trigonal pyramidal
c)
linear
d)
tetrahedral
55.
One can predict the shape of a molecule by drawing its Lewis structure and
a)
accounting for bonding and lone pairs of valence electrons.
b)
balancing the charges.
c)
determining the formula.
d)
identifying the presence of polyatomic ions.
56.
Which of the following prefixes mean six?
a)
hepta-
b)
tetra-
c)
penta-
d)
hexa-
57.
Which of the following is the correct name for the compound SiC?
a)
silicon carbide
b)
silicon monocarbide
c)
silver carbide
d)
silver monocarbide
58.
Which of the following is the correct name for the compound P2O5?
a)
dipotassium pentaoxide
b)
phosphorus oxide
c)
diphosphorus pentaoxide
d)
diphosphorus heptaoxide
59.
Which of the following is the correct Lewis structure for the compound dinitrogen monoxide?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
60.
Which of the following is the correct Lewis structure for the compound phosphorus tribromide?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
61.
An attraction between molecules of different substances.
a)
adhesion
b)
cohesion
c)
diatomic molecule
d)
lone pair
62.
The ability of a liquid to flow upward in narrow tubes.
a)
adhesion
b)
cohesion
c)
capillary action
d)
surface tension
63.
An attraction between molecules of the same substance.
a)
adhesion
b)
cohesion
c)
capillary action
d)
diatomic molecule
64.
The bond formed when electrons are shared between atoms.
a)
covalent bond
b)
hydrogen bond
c)
nonpolar covalent bond
d)
polar covalent bond
65.
The product that results from the sharing of electrons between two or more nonmetals.
a)
covalent compound
b)
hydrogen bond
c)
molecule
d)
diatomic molecule
66.
A molecule that consists of two atoms of the same element.
a)
lone pair
b)
molecule
c)
diatomic molecule
d)
covalent compound
67.
A weak bond between a hydrogen atom in one molecule to an atom in a second molecule.
a)
hydrogen bond
b)
covalent bond
c)
polar covalent bond
d)
nonpolar covalent bond
68.
A model that uses electron-dot structures to show how valence electrons are arranged in molecules.
a)
lone pair
b)
VSEPR theory
c)
ozone
d)
Lewis structure
69.
A pair of valence electrons not involved in bonding.
a)
lone pair
b)
molecule
c)
nonpolar covalent bond
d)
polar covalent bond
70.
A substance formed when two or more atoms covalently bond.
a)
covalent bond
b)
molecule
c)
hydrogen bond
d)
cohesion
71.
A bond in which the electrons are shared equally by two atoms.
a)
polar covalent bond
b)
hydrogen bond
c)
nonpolar covalent bond
d)
diatomic molecule
72.
A layer of naturally occurring gas in the Earth's stratosphere that serves as a shield from the harmful radiation emitted by the sun.
a)
ozone
b)
surface tension
c)
adhesion
d)
cohesion
73.
A bond in which the electrons are shared unequally by two atoms.
a)
polar covalent bond
b)
hydrogen bond
c)
nonpolar covalent bond
d)
molecule
74.
The ability of molecules at the surface of a liquid to resist an external force due to the cohesive nature of its molecules.
a)
cohesion
b)
adhesion
c)
surface tension
d)
capillary action
75.
A model for predicting the shapes of molecules.
a)
Lewis structures
b)
VSEPR theory
c)
ozone
d)
lone pair
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