Name: ______________________ Class: _________________ Date: _________
Final Prep #2: Ch 8-9
Matching
Match the terms below with their correct definitions.
a. alloy
j. ionic bond
b. anion
k. lattice energy
c. cation
l. metallic bond
d. chemical bond
m. monatomic ion
e. delocalized electrons
n. oxidation number
f. electrolyte
o. oxyanion
g. electron sea model
p. polyatomic ion
h. formula unit
q. salts
i. interstitial alloy
____
____
____
____
____
____
____
____
____
____
____
____
____
____
____
____
____
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
Electrons that are free to move in metals
For a monatomic ion, is equal to the charge
The force that holds two atoms together
A charged particle containing more than one atom
A positively charged ion
A negatively charged ion
An ionic compound whose aqueous solution conducts electricity
The name for most ionic compounds other than oxides
Represents the way electrons exist in metals
A charged particle containing only one atom
The energy needed to separate the ions of an ionic compound
The electrostatic force that holds oppositely charged particles together
A mixture of elements that has metallic properties
A mixture formed when small atoms fill holes in a metallic crystal
A polyatomic ion composed of an element bonded to at least one oxygen atom
Shows the simplest ratio of ions in an ionic compound
The attraction of a metallic cation for delocalized electrons
1
ID: A
Name: ______________________
ID: A
Short Answer
The diagram below represents a lithium atom (group 1 of the periodic table) and a fluorine atom (group
17). Use the diagram to answer the questions that follow.
18. What is the electron configuration of the neutral lithium atom?
19. What is the electron configuration of the neutral fluorine atom?
20. What happens to the lithium atom when it reacts with the fluorine atom? What is the electron
configuration of the lithium after the change?
21. In terms of the electron arrangement, why is this change favorable for the lithium atom?
22. What happens to the fluorine atom when it reacts with the lithium atom? What is the electron
configuration of the fluorine after the change?
23. In terms of the electron arrangement, why is this change favorable for the fluorine atom?
24. What kind of compound is formed in the reaction?
25. What are the formula and name of the product in this reaction?
Answer the following questions, which refer to the graph below. The graph shows the lattice energies of
the halide compounds of the group 1 metals sodium (atomic number 11) and potassium (atomic number
19).
26. How does lattice energy relate to the attraction between ions and the stability of an ionic compound?
27. What is the relationship between the lattice energy of the halides of sodium and the atomic number and
size of the halides? What is the relationship for the halides of potassium?
28. How does the plot of lattice energy for the potassium halides compare with that for the sodium
halides? What does this suggest about lattice energy and ionic size?
2
Name: ______________________
ID: A
29. Given what you know about lattice energy and the stability of a crystal, how would you expect the
melting point of NaBr to compare with that of NaI? How would you expect the melting point of NaBr
to compare with that of KBr? Explain your answer.
30. What effect on lattice energy would you expect the amount of charge on an ion to have? Explain.
Four students (A, B, C, and D) are given separate solid samples of the same unknown pure substance.
They are asked to determine whether the substance is a metallic element, a nonmetallic element, or an
ionic compound. In order to find out, they independently carry out experiments to determine some of
the properties of the substance. Student A observes the substance to determine its luster. Student B tests
the solid’s ability to conduct electricity. Student C determines whether the solid is malleable and ductile.
Student D determines its melting point and tests the melted liquid’s ability to conduct electricity. The
students do not communicate their separate findings to one another. The results of their experiments
are shown in the table below. Use the information to answer the questions that follow.
Student
Property Studied
Result
A
Luster
Nonlustrous
B
Ability of solid to conduct electricity
Nonconducting
C
Malleability and ductility
Nonmalleable and nonductile
(brittle)
D
Melting Point
Approximately 800ºC
D
Ability of melted liquid to conduct
Good
electricity
31. On the basis of his results, Student A concludes that the solid is a nonmetallic element rather than a
metallic element or an ionic compound. Comment on the soundness of his conclusion, given only what
he has determined about luster.
32. On the basis of her results, Student B also concludes that the unknown is a nonmetallic element.
Evaluate her conclusion.
33. On the basis of his results, Student C concludes that the unknown is a metallic element. Evaluate his
conclusion.
34. On the basis of her results, Student D states that she cannot conclude anything about whether the
unknown is a metallic element, nonmetallic element, or ionic solid. Evaluate her comment.
35. Suppose that Student B and Student C shared their results with each another. Should they then be able
to come to a definite conclusion as to the nature of the unknown? Explain.
36. Suppose that Student B and Student D shared their results with each other. Should they then be able to
come to a definite conclusion as to the nature of the unknown? Explain.
37. Would a test of a water solution of the unknown might also have been useful in determining the nature
of the unknown? Explain.
3
ID: A
Final Prep #2: Ch 8-9
Answer Section
MATCHING
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
E
N
D
P
C
B
F
Q
G
M
K
J
A
I
O
H
L
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
SHORT ANSWER
18. ANS:
1s2 2s1
PTS: 1
19. ANS:
1s2 2s2 2p5
PTS: 1
20. ANS:
The lithium atom loses one electron, to form an Li+ ion. The configuration is 1s2 .
PTS: 1
21. ANS:
The lithium has achieved the stable configuration of a noble gas.
PTS: 1
22. ANS:
The fluorine atom gains one electron, to form an F– ion. The configuration is 1s2 2s2 2p6 .
PTS:
1
1
ID: A
23. ANS:
The fluorine has achieved a stable octet configuration, like that of a noble gas.
PTS: 1
24. ANS:
ionic
PTS: 1
25. ANS:
LiF; lithium fluoride
PTS: 1
26. ANS:
The more negative the lattice energy is, the stronger is the attraction between ions and the more stable
is the ionic compound.
PTS: 1
27. ANS:
The lattice energy decreases (becomes less negative) as atomic number and size increase for the halides
of sodium. The same relationship exists for the potassium halides.
PTS: 1
28. ANS:
The lattice energy values are lower for the halides of potassium than they are for the corresponding
halides of sodium. As the ionic size increases, the lattice energy becomes less negative.
PTS: 1
29. ANS:
The melting point of NaBr should be higher than that of NaI because NaBr has higher lattice energy
and therefore more energy would be required to separate the ions. The melting point of NaBr should be
higher than that of KBr for the same reason.
PTS: 1
30. ANS:
The lattice energy should be greater (more negative) for ions of greater charge because the electrostatic
force of attraction would be higher.
PTS: 1
31. ANS:
His conclusion is questionable. Although it is correct that nonmetallic elements tend to be nonlustrous,
so do ionic compounds because both types of substances do not have delocalized electrons.
PTS: 1
32. ANS:
Her conclusion is questionable. Although it is true that most nonmetallic elements are poor conductors
of electricity, so are ionic compounds when in the solid state.
PTS:
1
2
ID: A
33. ANS:
His conclusion is almost definitely faulty. Metals tend to be malleable and ductile. On the basis of his
results, C should have concluded that the unknown is probably either a nonmetallic element or an ionic
compound.
PTS: 1
34. ANS:
A limited conclusion is possible. Nonmetallic elements tend to be poor conductors of electricity, even
when melted, so they can be ruled out. Metals and melted ionic solids both tend to conduct well. The
melting point is within the range of that of many metallic elements and ionic solids, so it is not very
useful in further narrowing the conclusion.
PTS: 1
35. ANS:
No; neither separate conclusion can rule out either nonmetals or ionic solids.
PTS: 1
36. ANS:
Yes; only ionic solids are nonconductors as solids but good conductors as liquids.
PTS: 1
37. ANS:
A test of conductivity of the solution would have been useful because dissolved ionic solids tend to
conduct electricity.
PTS:
1
3