1. (1) Atomic Structure and Interatomic Bonding

2. BOHR ATOM Nucleus: Z = # protons = 1 for hydrogen to 94 for plutonium
Adapted from Fig. 2.1, Callister 6e.
Nucleus: Z = # protons
= 1 for hydrogen to 94 for plutonium
N = # neutrons
Atomic mass A ≈ Z + N 2

3. ELECTRON ENERGY STATES
Electrons...
• have discrete energy states
• tend to occupy lowest available energy state.
Adapted from Fig. 2.5, Callister 6e. 3

4. STABLE ELECTRON CONFIGURATIONS
• have complete s and p subshells
• tend to be unreactive.
Adapted from Table 2.2, Callister 6e. 4

5. SURVEY OF ELEMENTS • Most elements: Electron configuration not stable.
Adapted from Table 2.2, Callister 6e.
• Why? Valence (outer) shell usually not filled completely. 5

6. THE PERIODIC TABLE • Columns: Similar Valence Structure
Adapted from Fig. 2.6, Callister 6e.
Electropositive elements:
Readily give up electrons
to become + ions.
Electronegative elements:
Readily acquire electrons
to become - ions. 6

7. METALS

8. CERAMICS

9. POLYMERS

10. SEMICONDUCTOR

12. ELECTRONEGATIVITY • Ranges from 0.7 to 4.0,
• Large values: tendency to acquire electrons.
Smaller electronegativity
Larger electronegativity
Adapted from Fig. 2.7, Callister 6e. (Fig. 2.7 is adapted from Linus Pauling, The Nature of the Chemical Bond, 3rd edition, Copyright 1939 and 1940, 3rd edition. Copyright 1960 by Cornell
University. 7

13. IONIC BONDING • Occurs between + and - ions.
• Requires electron transfer.
• Large difference in electronegativity required.
• Example: NaCl 8

14. EXAMPLES: IONIC BONDING
• Predominant bonding in Ceramics
Give up electrons
Acquire electrons
Adapted from Fig. 2.7, Callister 6e. (Fig. 2.7 is adapted from Linus Pauling, The Nature of the Chemical Bond, 3rd edition, Copyright 1939 and 1940, 3rd edition. Copyright 1960 by Cornell
University. 9

15. COVALENT BONDING • Requires shared electrons • Example: CH4
C: has 4 valence e,
needs 4 more
H: has 1 valence e,
needs 1 more
Electronegativities
are comparable.
Adapted from Fig. 2.10, Callister 6e. 10

16. EXAMPLES: COVALENT BONDING
Adapted from Fig. 2.7, Callister 6e. (Fig. 2.7 is
adapted from Linus Pauling, The Nature of the Chemical Bond, 3rd edition, Copyright 1939 and 1940, 3rd edition. Copyright 1960 by Cornell University.
• Molecules with nonmetals
• Molecules with metals and nonmetals
• Elemental solids
• Compound solids (about column IVA) 11

17. METALLIC BONDING • Arises from a sea of donated valence electrons
(1, 2, or 3 from each atom).
Adapted from Fig. 2.11, Callister 6e.
• Primary bond for metals and their alloys 12

18. SECONDARY BONDING Arises from interaction between dipoles
• Fluctuating dipoles
Adapted from Fig. 2.13, Callister 6e.
• Permanent dipoles-molecule induced
Adapted from Fig. 2.14,
Callister 6e.
-general case:
-ex: liquid HCl
Adapted from Fig. 2.14,
Callister 6e.
-ex: polymer 13

19. SUMMARY: BONDING Type Bond Energy Comments Ionic Large!
Nondirectional (ceramics)
Variable
Directional
Covalent
large-Diamond
semiconductors, ceramics
small-Bismuth
polymer chains)
Variable
Metallic
large-Tungsten
Nondirectional (metals)
small-Mercury
Directional
Secondary
smallest
inter-chain (polymer)
inter-molecular 14

20. PROPERTIES FROM BONDING: TM
• Bond length, r
• Melting Temperature, Tm
• Bond energy, Eo
Tm is larger if Eo is larger. 15

21. PROPERTIES FROM BONDING: E
• Elastic modulus, E
• E ~ curvature at ro
E is larger if Eo is larger. 16

22. PROPERTIES FROM BONDING: a
• Coefficient of thermal expansion, a
• a ~ symmetry at ro
a is larger if Eo is smaller. 17

23. SUMMARY: PRIMARY BONDS
Ceramics
Large bond energy
large Tm
large E
small a
(Ionic & covalent bonding):
Metals
Variable bond energy
moderate Tm
moderate E
moderate a
(Metallic bonding):
Polymers
Directional Properties
Secondary bonding dominates
small T
small E
large a
(Covalent & Secondary): 18

24. ENERGY AND PACKING • Non dense, random packing
• Dense, regular packing
Dense, regular-packed structures tend to have
lower energy. 2

25. MATERIALS AND PACKING Crystalline materials...
• atoms pack in periodic, 3D arrays
• typical of:
-metals
-many ceramics
-some polymers
crystalline SiO2
Adapted from Fig. 3.18(a),
Callister 6e.
Noncrystalline materials...
• atoms have no periodic packing
• occurs for:
-complex structures
-rapid cooling
"Amorphous" = Noncrystalline
noncrystalline SiO2
Adapted from Fig. 3.18(b),
Callister 6e. 3

26. METALLIC CRYSTALS • tend to be densely packed.
• have several reasons for dense packing:
-Typically, only one element is present, so all atomic
radii are the same.
-Metallic bonding is not directional.
-Nearest neighbor distances tend to be small in
order to lower bond energy.
• have the simplest crystal structures.
We will look at three such structures... 4

27. SIMPLE CUBIC STRUCTURE (SC)
• Rare due to poor packing (only Po has this structure)
• Close-packed directions are cube edges.
• Coordination # = 6
(# nearest neighbors)
(Courtesy P.M. Anderson) 5

28. ATOMIC PACKING FACTOR • APF for a simple cubic structure = 0.52
Adapted from Fig. 3.19,
Callister 6e. 6

29. BODY CENTERED CUBIC STRUCTURE (BCC)
• Close packed directions are cube diagonals.
--Note: All atoms are identical; the center atom is shaded
differently only for ease of viewing.
• Coordination # = 8
Adapted from Fig. 3.2,
Callister 6e.
(Courtesy P.M. Anderson) 7

30. ATOMIC PACKING FACTOR: BCC
• APF for a body-centered cubic structure = 0.68
Adapted from
Fig. 3.2,
Callister 6e. 8

31. FACE CENTERED CUBIC STRUCTURE (FCC)
• Close packed directions are face diagonals.
--Note: All atoms are identical; the face-centered atoms are shaded
differently only for ease of viewing.
• Coordination # = 12
Adapted from Fig. 3.1(a),
Callister 6e.
(Courtesy P.M. Anderson) 9

32. ATOMIC PACKING FACTOR: FCC
• APF for a body-centered cubic structure = 0.74
Adapted from
Fig. 3.1(a),
Callister 6e. 10

33. FCC STACKING SEQUENCE • ABCABC... Stacking Sequence • 2D Projection
• FCC Unit Cell 11

34. HEXAGONAL CLOSE-PACKED STRUCTURE (HCP)
• ABAB... Stacking Sequence
• 3D Projection
• 2D Projection
Adapted from Fig. 3.3,
Callister 6e.
• Coordination # = 12
• APF = 0.74 12

35. STRUCTURE OF COMPOUNDS: NaCl
• Compounds: Often have similar close-packed structures.
• Structure of NaCl
• Close-packed directions
--along cube edges.
(Courtesy P.M. Anderson)
(Courtesy P.M. Anderson) 13

36. THEORETICAL DENSITY, r Example: Copper
Data from Table inside front cover of Callister (see next slide):
• crystal structure = FCC: 4 atoms/unit cell
• atomic weight = g/mol (1 amu = 1 g/mol)
• atomic radius R = nm (1 nm = 10 cm) -7 14

37. Characteristics of Selected Elements at 20C
Adapted from
Table, "Charac-
teristics of
Selected
Elements",
inside front
cover,
Callister 6e. 15

38. DENSITIES OF MATERIAL CLASSES
Why?
Metals have...
• close-packing
(metallic bonding)
• large atomic mass
Ceramics have...
• less dense packing
(covalent bonding)
• often lighter elements
Polymers have...
• poor packing
(often amorphous)
• lighter elements (C,H,O)
Composites have...
• intermediate values
Data from Table B1, Callister 6e. 16

39. CRYSTALS AS BUILDING BLOCKS
• Some engineering applications require single crystals:
--diamond single
crystals for abrasives
--turbine blades
Fig. 8.30(c), Callister 6e.
(Fig. 8.30(c) courtesy
of Pratt and Whitney).
(Courtesy Martin Deakins,
GE Superabrasives, Worthington, OH. Used with permission.)
• Crystal properties reveal features
of atomic structure.
--Ex: Certain crystal planes in quartz
fracture more easily than others.
(Courtesy P.M. Anderson) 17

40. POLYCRYSTALS • Most engineering materials are polycrystals. 1 mm
Adapted from Fig. K, color inset pages of Callister 6e.
(Fig. K is courtesy of Paul E. Danielson, Teledyne Wah Chang Albany)
1 mm
• Nb-Hf-W plate with an electron beam weld.
• Each "grain" is a single crystal.
• If crystals are randomly oriented,
overall component properties are not directional.
• Crystal sizes typ. range from 1 nm to 2 cm
(i.e., from a few to millions of atomic layers). 18

41. SINGLE VS POLYCRYSTALS
• Single Crystals
-Properties vary with
direction: anisotropic.
Data from Table 3.3, Callister 6e.
(Source of data is R.W. Hertzberg, Deformation and Fracture Mechanics of Engineering Materials, 3rd ed., John Wiley and Sons, 1989.)
-Example: the modulus
of elasticity (E) in BCC iron:
• Polycrystals
200 mm
-Properties may/may not
vary with direction.
-If grains are randomly
oriented: isotropic.
(Epoly iron = 210 GPa)
-If grains are textured,
anisotropic.
Adapted from Fig. 4.12(b), Callister 6e.
(Fig. 4.12(b) is courtesy of L.C. Smith and C. Brady, the National Bureau of Standards, Washington, DC [now the National Institute of Standards and Technology, Gaithersburg, MD].) 19

42. X-RAYS TO CONFIRM CRYSTAL STRUCTURE
• Incoming X-rays diffract from crystal planes.
Adapted from Fig. 3.2W, Callister 6e.
• Measurement of:
Critical angles, qc,
for X-rays provide
atomic spacing, d. 20

43. SCANNING TUNNELING MICROSCOPY
• Atoms can be arranged and imaged!
Photos produced from the work of C.P. Lutz, Zeppenfeld, and D.M. Eigler. Reprinted with permission from International Business Machines Corporation, copyright 1995.
Carbon monoxide molecules arranged on a platinum (111) surface.
Iron atoms arranged on a copper (111) surface. These Kanji characters represent the word “atom”. 21

44. DEMO: HEATING AND COOLING OF AN IRON WIRE
The same atoms can have more than one crystal structure.
• Demonstrates "polymorphism" 22

45. SUMMARY • Atoms may assemble into crystalline or amorphous structures.
• We can predict the density of a material,
provided we know the atomic weight, atomic
radius, and crystal geometry (e.g., FCC,
BCC, HCP).
• Material properties generally vary with single
crystal orientation (i.e., they are anisotropic),
but properties are generally non-directional
(i.e., they are isotropic) in polycrystals with
randomly oriented grains. 23