1. about the properties of ionic and metallic substances
What can we learn
about the properties of
ionic and metallic substances
by looking at their
atomic structure?

3. etc
etc
The sodium chloride
crystal stays together
due to (+) and (-)
electrostatic attractions.

4. Here is an example of a metallic crystal.
Note its similarity to the
organization of an ionic
crystal.
Here, however, all the
ions are positive.
HOW CAN THAT BE?
How can (+) ions
stick together?

5. As an example metal, Let’s take a look at aluminum’s
subatomic structure
ALUMINUM

6. The aluminum particles are arranged in an orderly repeating pattern.

7. However the valence electrons are not localized to any one
particle. They are
free to move and
occupy the space
between the (+) ions.
ALUMINUM

8. The large attraction of the (+) ions for the (-) delocalized
valence electrons
are what holds the
crystal together.
ALUMINUM

9. cations (+ ions) The large attraction of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
cations
(+ ions)
ALUMINUM

10. cations (+ ions) The large attraction of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
cations
(+ ions)
ALUMINUM

11. cations (+ ions) The large attraction of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
cations
(+ ions)
ALUMINUM

12. freely moving valence electrons The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
freely moving
valence
electrons
ALUMINUM

13. freely moving valence electrons The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
freely moving
valence
electrons
ALUMINUM

14. freely moving valence electrons The large attraction
of the (+) ions for
the (-) delocalized
valence electrons
are what holds the
crystal together.
freely moving
valence
electrons
ALUMINUM

15. ALUMINUM

16. ALUMINUM

17. 3+
ALUMINUM

18. Our example of aluminum metal consists of Al3+ ions, with each Al atom
giving up
3 electrons
to the delocalized
‘sea’ of electrons.
ALUMINUM

19. 3+
How does this
arrangement
account
for metallic
properties?

20. 3+
Let’s look at
malleability.

21. 3+

22. 3+

23. 3+

24. 3+

25. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

26. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

27. 3+

28. 3+

29. 3+

30. 3+

31. 3+

32. 3+

33. 3+

34. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

35. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

36. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

37. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

38. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

39. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

40. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

41. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

42. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

43. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

44. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

45. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

46. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

47. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

48. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

49. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

50. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

51. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

52. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

53. The delocalized electrons are a constant presence, always holding3+
The delocalized
electrons are a
constant presence,
always holding
together any
shifting (+) ions. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+

54. This is malleability. The delocalized electrons are a3+
The delocalized
electrons are a
constant presence,
always holding
together any
shifting (+) ions. 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+ 3+
This is
malleability. 3+ 3+

55. Why aren’t ionic crystals malleable?

85. Ionic crystals cleave
because the like charges
of shifted ions repel each
other.
The cleavage often results
in a shear, smooth face
between the split crystals.

86. Back to metallic crystals!

87. The strong attraction between the (+) ions in the crystal for the3+
The strong
attraction
between the
(+) ions in the
crystal for the
delocalized
electrons
results not only
in malleability:

88. This structure makes metals hard and strong, with a high3+
This structure
makes metals
hard and strong,
with a high
melting point:

89. This structure makes metals hard and strong, with a high3+
This structure
makes metals
hard and strong,
with a high
melting point:
The particles
want to stay
together!

90. In general, the more delocalized electrons, the tougher the metal.3+
In general, the
more delocalized
electrons, the
tougher the metal.
Transition metals
have the most
delocalized
electrons and are
the strongest.

91. Delocalized electrons also carry electric current and heat3+
Delocalized
electrons also
carry electric
current and heat
due to their
ability to move
through the
crystal.

92. characteristic luster.3+
AND delocalized
electrons readily
absorb and re-emit
visible frequency
photons, giving
metals their
characteristic luster.

93. TOO COOL!!
The “Bean” in Chicago: 100% stainless steel—why so shiny?