Name
Date
Class
IONIC AND METALLIC BONDING
Chapter Test A
A. Matching
Match each description in Column B with the correct term in Column A. Write the letter of the correct description on
the line.
Column A
Column B
E
1. electron dot structure
a. a mixture of two or more elements, at least one of which is
a metal
F
2. ionic compound
b. the number of ions of opposite charge surrounding each ion
in a crystal
H
3. valence electron
c. the force of attraction binding oppositely charged ions
together
C
4. ionic bond
J
5. chemical formula
d. the attraction of valence electrons for positive metal ions
e. a depiction of valence electrons around the symbol of an
element
f. compound of cations and anions
G
6. halide ion
A
7. alloy
I
8. octet rule
K
9. formula unit
g. an anion of a halogen
h. an electron in the highest occupied energy level of an atom
i. Atoms in most compounds tend to achieve the electron
configuration of a noble gas.
j. shows the kinds and numbers of atoms in the smallest
representative unit of a substance
B
10. coordination number
k. lowest whole-number ratio of ions in an ionic compound
D
11. metallic bond
B. Multiple Choice
Choose the best answer and write its letter on the line.
C 12. How many valence electrons does an atom of any element in Group 6A have?
a. 2
b. 4
c. 6
d. 8
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Core Teaching Resources
Name
B
Date
Class
13. The electron dot structure for an atom of phosphorus is
a.
b.
P
P
c.
P
d.
P
C
14. When an aluminum atom loses its valence electrons, what is the charge on the resulting ion?
a. 2+
c. 3+
b. 2–
d. 1+
B
15. The electron configuration of a fluoride ion, F–, is
a. 1s2 2s2 2p5.
b. the same as that of the neon atom.
c. 1s2 2s2 2p6 3s1.
d. the same as that of a potassium ion.
C
16. Metals are good conductors of electricity because they
a. form crystal lattices.
b. contain positive ions.
c. contain mobile valence electrons.
d. form ionic bonds.
B
17. In forming chemical bonds, atoms tend to attain an element is the
a. a state of higher energy.
b. the electron configuration of noble gas atoms.
c. the electron configuration of halogen atoms.
d. all of the above
D
18. An ionic compound is
a. electrically neutral.
b. held together by ionic bonds.
c. composed of anions and cations.
d. all of the above
B
19. Which of these is not a characteristic of most ionic compounds?
a. solid at room temperature
b. has a low melting point
c. conducts an electric current when melted
d. produced by reaction between metallic and nonmetallic elements
A
20. A metallic bond is a bond between
a. valence electrons and positively charged metal ions.
b. the ions of two different metals.
c. a metal and nonmetal.
d. none of the above
A
21. Which element when combined with chlorine would most likely form an ionic compound?
a. lithium
c. phosphorus
b. carbon
d. bromine
A
22. A cation is any atom or group of atoms with
a. a positive charge.
b. no charge.
c. a negative charge.
d. more electrons than the corresponding atoms.
Chapter 7 Ionic and Metallic Bonding
169
Name
Date
Class
23. The cation Fe3+ is formed when
a. an atom of iron loses two electrons.
b. an atom of zinc loses two electrons.
c. an atom of iron loses three electrons.
d. an atom of iron gains three electrons.
C
C. True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
AT
24. The chemical properties of an element are largely determined by the number of valence electrons the
element has.
NT
25. Fluorine and chlorine each have one valence electron.
NT
26. The coordination number gives the total number of ions in a crystal.
ST
27. Atoms acquire the stable electron structure of a noble gas by losing electrons.
AT
28. An alloy is a mixture of two or more elements, of which at least one is a metal.
NT
29. The crystal structure of ionic compounds such as sodium chloride is very unstable.
AT
30. When melted, ionic compounds conduct electricity.
AT
31. Metals are ductile because the cations in a piece of pure metal are insulated from one another by a sea of
electrons.
ST
32. Metal atoms are arranged in a face-centered cubic structure.
AT
33. During the formation of ionic compounds, electrons are transferred from one atom to another.
D. Questions
Answer the following in the space provided.
34. Write electron dot structures for the atoms and ions of each of the following elements.
Atoms
Ions(all ions will have the nearest inert gas configuration and
the charge on it.)
a. Ca xCax
b. Br Br with 7 valence electrons
c. Al Al with 3 valence electrons
35. Write the formulas obtained when each of these atoms loses or gains valence electrons and becomes anion. Tell
whether each is a cation or an anion.
a. Cl
b. Be
Cl-, anion
Be 2+, cation
c. Na Na+, cation
d. O O2-, anion
170
Core Teaching Resources
Name
Date
Class
36. Write the complete electron configurations for the ions in problem 35.
a. Cl- 1s2 2s2 2p6 3s2 3p6
b. Be2+ 1s2
c. Na+ 1s2 2s2 2p6
d. O2- 1s2 2s2 2p6
Na+ and O2- are called isoelectronic as they have the same electronic configuration
37. Use electron dot structures to predict the structure of the ionic compound composed of aluminum and chlorine.
Al: 1s2 2s2 2p6 3s2 3p1, valence e=1, Al-3e=Al+
Cl: 1s2 2s2 2p6 3s2 3p6, valence e=7, Cl + 1e =ClSince Al can give 3 e and Cl can accept only 1e, so 3 atoms of Cl are required. Predicted Formula
AlCl3
38. Write the electron configuration diagram that shows the transfer of electrons that takes place to form the compound
sodium fluoride. Include the electron configurations of the ions formed. Which noble gas configuration does each
ion have?
Na: 1s2 2s2 2p6 3s1, Na-1e=Na+
F: 1s2 2s2 2p5, F +1e=FBoth ions have noble gas configuration of ions
E. Essay
Write a short essay for the following.
39. Explain how scientists have used the concept of metallic bonding to account for many of the physical properties of
metals, such as electrical conductivity and malleability.
Metallic bonds are the result of the attraction of free-flowing valence electrons for positively
charged metal ions.
An electric current is a flow of electrons.
As electrons enter one end of a piece of metal, some of the free flowing electrons leave the other
end. So metals are good conductors of electricity.
The cations in a piece of metals are insulated from each other by the free electrons. Thus, when a
metal is struck, the cations slide past each other easily. This makes the metal malleable.
Chapter 7 Ionic and Metallic Bonding
171