1.
In a Lewis structure, what do the dots represent?
2.
Draw the Lewis structure of the bromine atom.
3.
How many dots are shown in the Lewis structure for the sulfur atom?
4.
What are the two principal types of bonding called?
5.
Name the two classes of element which are most likely to form an ionic
compound if they are allowed to react with each other.
6.
Draw the Lewis structure of the Pb2+ ion.
7.
What constitutes a covalent bond between two atoms?
8.
In what way is a polar covalent bond similar to a nonpolar covalent
bond? In what way are they different?
9.
What does it mean if an atom is said to have a high electronegativity?
10.
The elements with the lowest electronegativities are found in the
_______ _______ region of the periodic table.
11.
Who first assigned electronegativity values to many of the elements?
12.
What do we call the three-dimensional arrangement of positive and
negative ions in an ionic solid?
13.
Predict the formula of the compound formed when ions of sodium and
sulfur combine.
14.
Predict the formula of the compound formed when ions of barium and
nitrogen combine.
15.
What is the name of Fe2+ in the Stock system?
16.
What does the suffix "-ous" on the common names of ions mean?
17.
What is the term used for ions that are composed of two or more atoms
bonded together?
18.
What is the formula of the sulfate ion?
19.
What is the name of the ion HCO3-?
20.
What is the name of the ion NH4+?
21.
Provide the name of Na3PO4.
22.
What is the name of Cu2O in the Stock system?
23.
Write the formula of sodium carbonate.
24.
What kind of compound results when two or more different nonmetals
share electrons?
25.
What kind of bonding exists in substances which consist of discrete
molecules?
Page 1
26.
Provide the formula of sulfur trioxide.
27.
Write the formula of ammonia.
28.
Provide the name of CCl4.
29.
Provide the name of the compound whose formula is N2O5.
30.
At what temperature is a liquid converted into a gas?
31.
What is the term that describes a solid with no regular structure?
32.
What is the term that describes a compound that, when dissolved in
water conducts an electric current?
33.
What is the term that describes a compound that, when dissolved in
water does not conduct an electric current?
34.
What kind of bonding is present in substances which are
nonelectrolytes?
35.
How many bonding electrons are shown in the Lewis structure for the
bicarbonate ion, HCO3-?
36.
Draw the Lewis structure of methylamine, CH3NH2.
37.
Draw the Lewis structure of hydrogen sulfide, H2S.
38.
What is wrong with the Lewis structure shown below for sulfur trioxide,
SO3?
O
O
S
O
39.
Ozone, O3, has two resonance forms. Draw them, given the skeletal
arrangement O-O-O
40.
What is defined as the amount of energy needed to break a bond holding
two atoms together?
41.
What is defined as the distance of separation of two nuclei in a
covalent bond?
42.
What do the letters VSEPR stand for?
43.
If the shape of a molecule is trigonal planar, what are the values of
the bond angles?
44.
In the molecule AX2, the central atom A has two lone pairs of electrons
in addition to the two bond pairs in the A-X bonds. What is the shape
of this molecule?
45.
The ammonia molecule, NH3, is polar. Why does this fact suggest that its
shape is trigonal pyramidal, rather than trigonal planar?
Page 2
46.
Which of the following Lewis structures of neutral atoms is correct?
A.
47.
K
Ba
Al
Sn
O
A
B
C
D
E
+
A
A.
2+
Sn
B
A
2+
N
C
B.
B
-
3-
I
D
C.
E
D.
C
D
E.
E
H
B.
Cl
C.
D.
O
F
E.
Na
Si
B.
P
C.
D.
Cl
Ar
E.
Br
B.
D.
intermolecular
nonpolar covalent
ionic
polar covalent
The atoms lose electrons in forming ions.
The elements are metals.
They are located to the left of the periodic table.
They have low ionization energies.
They have high electron affinities.
Assuming reactions between the following pairs of elements, which pair
is most likely to form an ionic compound?
A.
B.
C.
D.
E.
53.
Ca
Which one of the following is NOT true about elements that form
cations?
A.
B.
C.
D.
E.
52.
E
In the compound CH3Cl the bond between carbon and chlorine is
A.
C.
51.
E.
D
Which of the following has the greatest electronegativity?
A.
50.
D.
C
Which of the following has the greatest electronegativity?
A.
49.
C.
B
Which of the following Lewis structures of ions is incorrect?
Na
48.
B.
A
copper and tin
chlorine and oxygen
cesium and iodine
carbon and chlorine
fluorine and iodine
What kind of bond results when electron transfer occurs between atoms
of two different elements?
A.
B.
C.
D.
E.
ionic
covalent
nonpolar
single
double
Page 3
54.
What is the old name of Cu+?
A.
B.
C.
D.
E.
55.
Give the name of FeSO4 in the Stock system.
A.
B.
C.
D.
E.
56.
C.
D.
E.
PCl
B.
PCl3
C.
PCl5
D.
P2Cl5
E.
P5Cl
What term describes the temperature at which a solid is converted into
a liquid?
A.
B.
C.
D.
E.
60.
is longer than a single bond between the same two atoms
has a lower bond energy than a single bond between the same two
atoms
arises when two electrons are transferred from A to B
consists of two electrons shared between A and B
consists of four electrons shared between A and B
What is the correct formula of phosphorus pentachloride?
A.
59.
lithium and iodine
sodium and oxygen
calcium and chlorine
copper and tin
carbon and oxygen
A double bond between two atoms, A and B
A.
B.
58.
iron monosulfuric acid
iron(II) sulfate
iron(III) sulfate
ferrous sulfate
ferric sulfate
Assuming reactions between the following pairs of elements, which pair
is most likely to form a covalent compound?
A.
B.
C.
D.
E.
57.
cupric ion
cuprous ion
copper(I) ion
copper(II) ion
ferrous ion
critical point
flash point
sublimation point
melting point
boiling point
What term describes a solution of a compound in water that conducts an
electric current?
A.
B.
C.
D.
E.
amorphous solution
an electrolyte solution
a nonelectrolyte solution
superconducting solution
isoelectric solution
Page 4
61.
How many bonding electrons are in CO2?
A.
62.
2
C.
3
D.
4
E.
8
0
B.
1
C.
2
D.
3
E.
8
D.
12
E.
16
How many valence electrons are in SO42-?
A.
64.
B.
How many nonbonding electrons are in CH4?
A.
63.
1
2
B.
64
C.
32
According to VSEPR theory, if the valence electrons on a central atom
are 3 bond pairs and one nonbonding (lone) pair, the geometry (shape)
at this atom will be
A.
B.
C.
D.
E.
linear
bent (angular)
trigonal planar
trigonal pyramidal
tetrahedral
65.
T
F
In Lewis structures, the chemical symbol of an element represents
both the nucleus and the lower energy (nonvalence) electrons.
66.
T
F
The name of SnO2 is tin(I) oxide.
67.
T
F
The old name of iron(III) chloride is ferrous chloride.
68.
T
F
The are three atoms of iodine represented in the formula NaIO3.
69.
T
F
In solid NaCl, no molecules of NaCl exist.
70.
T
F
Ionic solids are amorphous.
71.
T
F
Molecular compounds usually involve ionic bonding.
72.
T
F
As a rule, ionic compounds tend to have lower melting and boiling
points than covalent compounds consisting of small molecules.
73.
T
F
In the water molecule, the oxygen atom is an exception to the
octet rule.
74.
T
F
The NO2 molecule can never satisfy the octet rule.
75.
T
F
Six electrons shared between two atoms corresponds to a bond
order of three.
76.
T
F
Resonance occurs when two or more different, valid Lewis
structures can be drawn for a molecule+.
77.
T
F
The existence of resonance makes a molecule less stable than
would otherwise be the case.
78.
T
F
Because the C-H bond in methane is polar, the CH4 molecule will
also be polar.
79.
T
F
Chemical bonds are intramolecular forces.
Page 5
80.
T
F
In determining properties such as solubility, melting point and
boiling point, intramolecular forces are more important than
intermolecular forces.
81.
T
F
As a rule, a polar substance will be a good solvent for nonpolar
solutes, and vice versa.
Page 6
Answer Key for Test "chapter4.tst", 8/17/04
No. in No. on
Q-Bank Test Correct Answer
4
1
1
valence electrons
4
2
2
Br
4
4
4
4
3
4
5
6
4
4
7
8
4
9
4
4
4
4
4
4
4
4
4
10
11
12
13
14
15
16
17
18
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
3
4
5
6
six
ionic bonding and covalent bonding
metal, nonmetal
Pb
2
a shared pair of electrons
7
8
In each case, the bond consists of an electron pair shared between the
bonded atoms. The difference is that the sharing is unequal in the case
of the polar covalent bond, equal in a nonpolar covalent bond.
The atom has a strong attraction for shared electron pairs
9
(electrons in covalent bonds).
bottom left
10
Pauling
11
crystal lattice
12
Na2S
13
14
Ba3N2
15
iron(II) ion
16
lower positive charge
17
polyatomic
18
SO42hydrogen carbonate
19
ammonium
20
sodium phosphate
21
copper(I) oxide
22
Na2CO3
23
covalent
24
Covalent
25
SO3
26
NH3
27
carbon tetrachloride
28
dinitrogen pentoxide
29
boiling point
30
amorphous
31
electrolyte
32
nonelectrolyte
33
covalent
34
ten
35
H
H
36
H
4
37
37
4
38
38
H
C
N
H
H
S
H
Page 1
Answer Key for Test "chapter4.tst", 8/17/04
No. in No. on
Q-Bank Test Correct Answer
The structure shows 26 valence electrons, but there should only be 24.
4 39
39
O
4
4
4
4
4
4
40
41
42
43
44
45
40
41
42
43
44
45
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
4
46
47
48
49
50
51
52
53
54
55
56
57
58
59
60
61
62
63
64
65
66
67
68
69
70
71
72
73
74
75
76
77
78
79
80
81
46
47
48
49
50
51
52
53
54
55
56
57
58
59
60
61
62
63
64
65
66
67
68
69
70
71
72
73
74
75
76
77
78
79
80
81
O
O
O
O
O
bond energy
bond length
Valence Shell Electron Pair Repulsion
120°
bent or angular
If the molecule were trigonal planar, the symmetry would result
in a nonpolar molecule. The centers of positive and negative
charge would coincide.
C
C
D
C
D
E
C
A
B
B
E
E
C
D
B
E
A
C
D
T
F
F
F
T
F
F
F
F
T
T
T
F
F
T
F
F
Page 2