AnswersNY-Chemistry Term 1 HillcrestMetallic Bonding

Metallic Bonding Answers

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1
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Which combination of factors is most suitable for increasing the electrical conductivity of metals?

A
more valence electrons and larger atomic radius
B
fewer valence electrons and larger atomic radius
C
more valence electrons and smaller atomic radius
D
fewer valence electrons and smaller atomic radius
2
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Which is a characteristic of the electron sea model for metallic bonding?

A
Molecular orbitals overlap to produce bands.
B
Electrons flow easily between metal nuclei.
C
Electrons are in fixed positions in the orbitals.
D
Atomic nuclei are arranged in an irregular pattern.
3

Which statement best describes the basis of the band theory of metallic bonding?

A
Molecular orbitals overlap to form atomic orbitals in which the valence electrons of the atoms travel.
B
Molecular orbitals overlap to form atomic orbitals in which all electrons of the atoms travel.
C
Atomic orbitals overlap to form molecular orbitals in which the valence electrons of the atoms travel.
D
Atomic orbitals overlap to form molecular orbitals in which all electrons of the atoms travel.
4

Which statement is true when a crystal is formed from many metal atoms?

A
There are no bands being formed.
B
There are many molecular orbitals.
C
There are only unshared atomic orbitals.
D
There are many electrons lost to other atoms.
5

In a piece of metal, what holds the atoms together?

A
the positive charges of the nuclei and the localized electrons around them
B
the negative charges of the nuclei and the localized electrons around them
C
the positive charges of the nuclei and the negative charges of delocalized electrons
D
the negative charges of the nuclei and the positive charges of delocalized electrons
6

Which element is likely to be the best conductor of electricity?

A
copper
B
lithium
C
iodine
D
silicon
7

Which reason best explains why metals are ductile instead of brittle?

A
because they have rigid bonds
B
because they have flexible bonds
C
because they easily lose electrons
D
because they easily gain electrons
8

Which property is true for metals?

A
localized electrons
B
high electronegativity
C
low ionization energies
D
tightly held valence electrons
9

Which is the best metal to use in an alloy to increase its electrical conductivity?

A
Al
B
Cu
C
Li
D
Sb
10

What is another name for the molecular orbital theory of bonding in metals?

A
band theory
B
ionic bond theory
C
covalent bond theory
D
electron bond theory
11

Which property does a metal with a large number of free-flowing electrons most likely have?

A
very hard
B
very brittle
C
poor conductivity
D
good conductivity
12

The diagram is a representation of the electron sea model. Which statement best describes what is happening in this model?

Question illustration
A
The electrons are transferred to the innermost nuclei of metal atoms.
B
The electrons are transferred to the outermost nuclei of metal atoms.
C
The electrons are moving easily between the nuclei of metal atoms.
D
The electrons are in fixed positions between the nuclei of metal atoms.
13

Which of the following metal atoms would have the highest conductivity?

A
the atom with the smallest radius and the fewest valence electrons
B
the atom with the smallest radius and the most valence electrons
C
the atom with the largest radius and the fewest valence electrons
D
the atom with the largest radius and the most valence electrons
14

Which property is better explained by the band theory than by the sea-of-electrons model?

A
ductility
B
thermal conductivity
C
luster
D
electrical conductivity
15

Which is most likely the result of millions of metal atoms crowding together so that molecular orbitals become combined?

A
the loss of metallic properties
B
the formation of bands in a crystal
C
the loss of valence electrons to other atoms
D
the formation of localized valence electrons

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