CHAPTER 7 – IONIC AND
METALLIC BONDING
QUESTION 1
The electron configuration of nitrogen is
1s22s2
2p3. How many more electrons does nitrogen need to
satisfy the octet rule?
a.
1
b.
3
c.
5
d.
8
QUESTION 2
What group of elements satisfies the octet rule without
forming compounds?
a.
halogen
b.
noble gas
c.
alkali metal
d.
alkaline-earth metal
QUESTION 3
To draw a Lewis structure, one must know the
a.
number of valence electrons in each atom.
b.
atomic mass of each atom.
c.
bond length of each atom.
d.
ionization energy of each atom.
QUESTION 4
The chemical formula for an ionic compound represents
the
a.
number of atoms in each molecule.
b.
number of ions in each molecule.
c.
ratio of the combined ions present in a
sample.
d.
total number of ions in the crystal lattice.
QUESTION 5
The ions in most ionic compounds are organized into a
a.
molecule.
b.
Lewis structure.
c.
polyatomic ion.
d.
crystal.
QUESTION 6
Ionic compounds are brittle because the strong attractive
forces
a.
allow the layers to shift easily.
b.
cause the compound to vaporize easily.
c.
keep the surface dull.
d.
hold the layers in relatively fixed positions.
QUESTION 7
A chemical bond formed by the attraction between positive
ions and surrounding mobile electrons is a(n)
a.
nonpolar covalent bond.
b.
ionic bond.
c.
polar covalent bond.
d.
metallic bond.
QUESTION 8
Compared with nonmetals, the number of valence electrons
in metals is generally
a.
smaller.
b.
greater.
c.
about the same.
d.
almost triple.
QUESTION 9
In metals, the valence electrons
a.
are attached to particular positive ions.
b.
are shared by all of the atoms.
c.
are immobile.
d.
form covalent bonds.
QUESTION 10
In metallic bonds, the mobile electrons surrounding the
positive ions are called a(n)
a.
Lewis structure.
b.
electron sea.
c.
electron cloud.
d.
dipole.
QUESTION 11
Metals are malleable because the metallic bonding
a.
holds the layers of ions in rigid positions.
b.
maximizes the repulsive forces within the metal.
c.
allows one plane of ions to slide past another.
d.
is easily broken.
QUESTION 12
Malleability and ductility are characteristic of substances
with
a.
covalent bonds.
b.
ionic bonds.
c.
Lewis structures.
d.
metallic bonds.
QUESTION 13
Shifting the layers of an ionic crystal causes the crystal to
a.
be drawn into a wire.
b.
shatter.
c.
become metallic.
d.
emit light.
QUESTION 14
A chemical formula includes the symbols of the elements
in the compound and subscripts that indicate
a.
atomic mass of each element.
b.
number of atoms or ions of each element
that
are combined in the compound.
c.
formula mass.
d.
charges on the elements or ions.
QUESTION 15
What is the formula for zinc fluoride?
a.
ZnF
b.
ZnF2
c.
Zn2F
d.
Zn2F3
QUESTION 16
What is the formula for the compound formed by calcium
ions and chloride ions?
a.
CaCl
b.
Ca2Cl
c.
CaCl3
d.
CaCl2
QUESTION 17
Name the compound Al2S3.
a.
aluminum sulfate
b.
aluminum sulfur
c.
aluminum(II) sulfate
d.
aluminum sulfide
QUESTION 18
How many valence electrons are in a silicon atom?
a.
2
b.
4
c.
6
d.
8
QUESTION 19
How does calcium obey the octet rule when reacting to
form compounds?
a.
It gains electrons.
b.
It gives up electrons.
c.
It does not change its number of electrons.
d.
Calcium does not obey the octet rule.
QUESTION 20
What is the electron configuration of the calcium ion?
a.
1s22s22p63s23p6
b.
1s22s22p63s23p44s2
c.
1s22s22p63s23p54s1
d.
1s22s22p63s2
QUESTION 21
The octet rule states that, in chemical compounds, atoms
tend to have ____.
a.
the electron configuration of a noble gas
b.
more protons than electrons
c.
eight electrons in their principal energy
level
d.
more electrons than protons
QUESTION 22
What is the formula of the ion formed when potassium
achieves noble-gas electron configuration?
a.
K2+
b.
K+
c.
K1d.
K2-
QUESTION 23
What is the charge on the cation in the ionic compound
sodium sulfide?
a.
0
b.
1+
c.
2+
d.
3+
QUESTION 24
What is the net charge of the ionic compound calcium
fluoride?
a.
2–
b.
1–
c.
0
d.
1+
QUESTION 25
What is the formula unit of aluminum oxide?
a.
AlO
b.
Al3O
c.
AlO3
d.
Al2O3
QUESTION 26
What does the term coordination number in ionic crystals
refer to?
a.
the total number of valence electrons in an
atom
b.
the number of oppositely charged ions
surrounding a particular ion
c.
the number of atoms in a particular formula unit
d.
the number of like-charged ions surrounding
a particular ion
QUESTION 27
How many electrons does silver have to give up in order to
achieve a pseudo-noble-gas electron configuration?
a.
1
b.
2
c.
3
d.
4
QUESTION 28
Which of the following elements does NOT form an ion
with a charge of 1+?
a.
fluorine
b.
hydrogen
c.
potassium
d.
sodium
QUESTION 29
What is the formula of the ion formed when tin achieves a
stable electron configuration?
a.
Sn4+
b.
Sn3+
c.
Sn2d.
Sn4-
QUESTION 30
The electron configuration of a fluoride ion, F-1, is ____.
a.
1s22s22p5
b.
the same as that of a neon atom
c.
1s22s22p63s1
d.
the same as that of a potassium ion
QUESTION 31
Which of the following occurs in an ionic bond?
a.
Oppositely charged ions attract.
b.
Two atoms share two electrons.
c.
Two atoms share more than two electrons.
d.
Like-charged ions attract.
QUESTION 32
A compound held together by ionic bonds is called a ____.
a.
diatomic molecule
b.
polar compound
c.
covalent molecule
d.
salt
QUESTION 33
What is the formula for potassium sulfide?
a.
KS
b.
K2S
c.
KS2
d.
K2S2
QUESTION 34
Ionic compounds are normally in which physical state at
room temperature?
a.
solid
b.
liquid
c.
gas
d.
plasma
QUESTION 35
Which of the following is true about the melting
temperature of potassium chloride?
a.
The melting temperature is relatively high.
b.
The melting temperature is variable and
unpredictable.
c.
The melting temperature is relatively low.
d.
Potassium chloride does not melt.
QUESTION 36
Under what conditions can potassium bromide conduct
electricity?
a.
only when melted
b.
only when dissolved
c.
only when it is in crystal form
d.
only when melted or dissolved in water
QUESTION 37
Which of the following particles are free to drift in metals?
a.
protons
b.
electrons
c.
neutrons
d.
cations