$$$ Quiz $$$ Ionic and Metallic Bonding/Naming Ionic Compounds.
Metallic and Ionic Bonding and Properties
93
What can we learn about the properties of ionic and metallic substances by looking at their atomic structure?
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Transcript of Metallic and Ionic Bonding and Properties
8/8/2019 Metallic and Ionic Bonding and Properties
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What can we learn
about the properties of
ionic and metallic substances
by looking at their
atomic structure?
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The sodium chloride
crystal stays together
due to (+) and (-)electrostatic attractions.
etcetc
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Here is an example of a metallic crystal.
Note its similarity to the
organization of an ionic
crystal.
Here, however, all theions are positive.
HOW CAN THAT BE?
How can (+) ions
stick together?
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As an example metal,Let¶s take a look
at aluminum¶s
subatomic structure
ALUMINUM
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The aluminum
particles are
arranged in an
orderly repeating
pattern.
ALUMINUM
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However the valence
electrons are not
localized to any one
particle.They are
free to move and
occupy the space
between the (+) ions.
ALUMINUM
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The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
ALUMINUM
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The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
ALUMINUM
cations
(+ ions)
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The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
ALUMINUM
cations
(+ ions)
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The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
ALUMINUM
cations
(+ ions)
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The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
ALUMINUM
freely moving
valenceelectrons
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The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
ALUMINUM
freely moving
valenceelectrons
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The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
ALUMINUM
freely moving
valenceelectrons
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ALUMINUM
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ALUMINUM
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ALUMINUM
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ALUMINUM
Our example of
aluminum metalconsists of
Al3+ ions,
with eachAl atom
giving up
3 electrons
to the delocalized
µsea¶ of electrons.
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How does this
arrangement
account
for metallic
properties?
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Let¶s look at
malleability.
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The delocalized
electrons are aconstant presence,
always holding
together any
shifting (+) ions.
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The delocalized
electrons are aconstant presence,
always holding
together any
shifting (+) ions.
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This is
malleability.
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Why aren¶t ionic crystals malleable?
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Ionic crystals cleave
because the like chargesof shifted ions repel each
other.
The cleavage often resultsin a shear, smooth face
between the split crystals.
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Back to metallic crystals!
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The strong
attraction
between the
(+) ions in the
crystal for the
delocalizedelectrons
results not only
in malleability:
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This structure
makes metals
hard and strong,
with a high
melting point:3+
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This structure
makes metals
hard and strong,
with a high
melting point:
The particles
want to stay
together!
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In general, the
more delocalized
electrons, the
tougher the metal.
Transition metals
have the mostdelocalized
electrons and are
the strongest.
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Delocalized
electrons alsocarry electric
current and heat
due to their
ability to movethrough the
crystal.
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AND delocalized
electrons readilyabsorb and re-emit
visible frequency
photons, giving
metals their characteristic luster.
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TOO COOL!!
The ³Bean´ in Chicago: 100% stainless steel²why so shiny?
