Engineering 45
Atomic Structure
and
InterAtomic Bonding
Bruce Mayer, PE
Registered Electrical & Mechanical Engineer
BMayer@ChabotCollege.edu
Engineering-45: Materials of Engineering
1
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Learning Goals
 Understand the Sources/Causes of
Atom-Level Bonding
 Understand The Number & Types of
Bonding
 Determine Which properties May be
inferred from bonding trends
Engineering-45: Materials of Engineering
2
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
The Nuclear Atom
 Current Best Model of
the Atomic Structure
• A Small & Dense
NUCLEUS surrounded
by an Electronic Cloud
 Nucleus Composition → Two Constituents
• PROTONS → POSITIVE Electronic Charge
• NEUTRONS → UNcharged
 Electronic Cloud Composed of
NEGATIVELY Charged ELECTRONS
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Atomic Facts
 ELEMENTS are Defined by
the Atomic Number, Z
• Z  Number of Protons
– For NATURALLY Occurring Elements Z Ranges
from 1 (H) to 92 (U)
 By the Electronic Neutrality Requirement
• [No. Protons] = [No. Electrons]
 Electronic Charge = 1.6x10-19 Amp•sec
• Note: 1 A•s = 1 Coulomb (C)
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
 Since The No. of NEUTRONS
Are not Constrained by Charge
Neutrality, Then The SAME Element
May Have Different No.s of Nuetrons, N
• Elemental Forms with Different Neutron
Counts are Called ISOTOPES
– e.g,; Consider Oxygen with Z = 8
O Isotope Neutrons, N Abundance
16
O
17
O
18
O
Engineering-45: Materials of Engineering
5
16-8 = 8
99.7620%
17-8 = 9
0.0383%
18-8 = 10
0.2001%
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
http://ie.lbl.gov/education/isotopes.htm
Atomic Facts cont
Recall the Periodic Table
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Atomic Facts cont.2
 Atomic Weight/Mass, A 
Weighted Average of Naturally
Occurring Isotopes
 SubAtomic Particle Masses
• Electron, e- = 9.11x10-31 kg
• Proton, p+ , and Neutron, n = 16 700x10-31 kg
 Since Mp+ & Mn >> Me• Then A  (Z+N)Mn
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
amu & gMol
 By SI DEFINITION 12.00000...
grams of 12C contains ONE
gram-Mol of Carbon
• 1 Mol of Any element Contains 6.023x1023
Protons and/or Electrons
– 6.023x1023  Avagrado’s Number
 Atomic Mass Unit, amu
• 1 amu/atom = 1 g/mol
– e.g.; Atomic Wt of Niobium = 92.91 amu/atom
= 92.91 g/mol
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Atomic Reactions
 Nuclear Reaction
• Change in the Number of Neutrons, N, or
Protons, Z, in an Atom
– Remember, Changing Z Changes the
ELEMENT TYPE
 e.g., a Nuclear Reaction can Change LEAD to GOLD
 Chemical Reaction
• Exchange or ReArrangement of
ELECTRONS
– VAST Majority of Matl Sci Done with Chem Rcns
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Electron Behavior → Quanta
 Electronic Behavior Governed by
Quantum (Energy) Mechanics (QE)
• QE Studied in Advanced
Physics/Chemistry, and
Some Branches of Engineering
 Basic Principle of QE as Applied to
Materials Science
• Electrons can have ONLY DISCRETE
Quantities (quanta) of Energy
– i.e., e- Energy Levels are QUANTIZED
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Bohr Atom

1st
Quantum
Model
orbital electrons:
n = principal
quantum number
1
2
n=3
• Electrons Revolve Around
Nucleus at Discrete Energy
Levels Called Orbitals
 A Refined Model Based on
Wave Mechanics
• e- Treated as Both a WAVE
and a PARTICLE
– Position is Determined STATISTICALLY,
not Physically
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Atom: Shells & Valence
VALENCE
Electron
Nucleus
INNER
Shell
Electron
Neutron
VALENCE
Shell/Orbit
Engineering-45: Materials of Engineering
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Proton
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Atom Structure - Valence
 Only the electrons
(e-) in the
OUTERmost
electron shell can
participate in
CHEMICAL
Reactions
 Adding or Removing
an e- creates a
CHARGED Atom
Called an ION
Engineering-45: Materials of Engineering
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 Valence e- Behavior
Governs the Atom’s
Ability to combine
with other elements
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Valence e- Importance
 A CHEMICAL reaction is the
restructuring of the VALENCE Electrons
in two or more Elements
 Valence electron structure determines
all of the following properties
 Composition
 Thermal
 Electrical
 Optical
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Electron Configuration of Atoms
3
M
d
p
s
2
L
p
s
6
2
1
n
K
s
2
1st
Shell
2nd
Sub-shell
10
6
2
 Four QUANTUM
NUMBERS Describe
the Electronic
Configuration of
Atoms
• 3rd Quantum No.
Describes the
Number of VALENCE
Electrons
3rd
# Electrons
4th
Spin 
Per Sub-shell
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Electron Energy States
 e- have DISCRETE energy states; tend to
occupy LOWEST available energy state.
4d
4p
N-shell n = 4
3d
4s
Energy
3p
3s
M-shell n = 3
2p
2s
L-shell n = 2
1s
K-shell n = 1
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Shell Filling Rules

Following Quantum Mechanics
1. Electrons Fill Shells/Orbitals to MINIMIZE
the Overall Atom Energy
2. Only TWO e- can Occupy a Single Orbital
– Must Have OPPOSITE “SPINS”: ↑ and ↓
3. Electrons Stay as Widely Separated in
physical space as Possible
– Favors EMPTY Orbitals as opposed to
Half-Filled Orbitals of the SAME Energy
 Leads to apparently “NONsequential” Filling;
e.g. Ca (20) and Sc (21)
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Electronic Configuration
 The Normal Fill Sequence
• 1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p
→ 5s → 6s → 4f → 5d → 6p → 7s → 5f →
6d → 7p
 For a Given Shell Structure We can
Write a ShortHand for an Element’s
Electronic Structure; e.g., Sulfur
S  1s 2s 2 p 3s 3 p
2
Principal
Quantum No.
SubShell
Engineering-45: Materials of Engineering
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2
6
2
4
Number of
VALENCE
Electrons
Electrons
Per SubShell
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Stable Electron Configurations
 Stable Electron Configurations
• Have COMPLETE s & p SubShells
– i.e., The VALENCE SubShell is FULL
• Are VERY Unreactive
Engineering-45: Materials of Engineering
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“OCTET”
RULE:
Ns2Np6
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Periodic
Table
Structure
Columns
Engineering-45: Materials of Engineering
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(valence shells)
Rows
(valence electron structure)
n=1
n=2
n=3
n=4
(1s1)
(2s1)
(3s1)
(4s1)
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Periodic Table Structure cont.
 Rows: Same OUTER Shell (Primary Quantum No.)
 Column: SAME Number Of Valence Electrons 
Similar Properties
 Trends: Atomic Radii, Electronegativity (tendency
to acquire electrons)
METALS
NONMETALS
Radii
Less ElectroNeg
Engineering-45: Materials of Engineering
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More ElectroNeg
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Periodic Table Structure
 Organized by Quantum No., Valence (or
Group), and SubShell
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Metals, SemiMetals, NonMetals
s
p
d
Quantum No.
Engineering-45: Materials of Engineering
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f
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Metals, SemiMetals, NonMetals
 METALS
• Solid at Room
Temperature
– Except Hg
• Maleable & Ductile
• Conduct Electricity
 SemiMetals
• 6 or 7 (Astatine
is the Wobbler)
• Have Some MetalLike Properties
 NonMetals (17)
– Solids at Rm Temp
– Can Conduct
Electricity
• Poor Heat
Conductors
• Have Some
NonMetal-Like Props
• Brittle and
Fracture Easily
Engineering-45: Materials of Engineering
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– Hard & Brittle
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
At
Refined Shell Model for Nitrogen
Valence
SHELL
(L or 2)
Valence
SUBShell
(2p)
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Molecular Bonding
 Molecules (2+ units of SAME atom) and
Compounds (2+ DIFFERENT atoms)
are Formed by CHEMICAL Bonding
 CHEMICAL Bonds Result from
ELECTRON Configuration
Rearrangement
• STRONG Bonds → Ionic, Metallic,
Covalent
• WEAK Bonds → Van Der Waals
– DiPole, Polar, H-Bond
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Bond-Energy
Curve
Force
 Balance Between Atoms’
REPULSIVE and
ATTRACTIVE Forces
• ZERO Net Force
• LOWEST System Energy
r0 - equilibrium
bond distance
“just right”:
Energy
too close → Repulsion
 Bond Distance  Equilibrium
InterAtomic Distance, or
LATTICE Constant
 Bond STRENGTH ↑
• Melting Temperature ↑
• Stiffness ↑
too far → Attaction
Engineering-45: Materials of Engineering
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Min U
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Ionic Bonding
 Ion  An Atom That Has Gained/Lost e-(s)
• Resulting Ion has +/- CHARGE
 Ionic Bonding Ocurrs Between + & - Ions
• Requires Electron TRANSFER; e.g. NaCl
X
Na (metal)
Unstable
1s22s22p63s1
Na (cation)
Stable
1s22s22p6
electron
+
Coulombic
Attraction
Engineering-45: Materials of Engineering
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Cl (nonmetal)
Unstable
1s22s22p63s23p5
-
Cl (anion)
Stable
1s22s22p63s23p6
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Ionic Bonding Examples
 Dominant Bonding Type for CERAMICS
H
2.1
Li
1.0
Na
0.9
K
0.8
Rb
0.8
Cs
0.7
Fr
0.7
NaCl
MgO
CaF 2
CsCl
Be
1.5
Mg
1.2
Ca
1.0
Sr
1.0
Ti
1.5
Cr
1.6
Ba
0.9
Fe
1.8
Ni
1.8
Zn
1.8
As
2.0
F
4.0
Cl
3.0
Br
2.8
I
2.5
At
2.2
Ra
0.9
Give up electrons
Engineering-45: Materials of Engineering
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O
3.5
Acquire electrons
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
He
Ne
Ar
Kr
Xe
Rn
-
CoValent Bonding
 Requires SHARED
Electrons (Co-Valent)
 Example is CH4
(methane)
• C: has 4 valence e-’s,
needs 4 more
• H: has 1 valence e-,
needs 1 more
 Characteristics
• If A compound, Then
Electronegativities are
comparable
• ≥4 valence e-’s
Cl2
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
CoValent Bonding Examples
 NonMetallic Elemental
Molecules; e.g. F2
 Elemental Solids; e.g.,
C, Si, Ge
col IVA
 Hydrogen Compounds;  Near Group-IVA Solid
e.g., HF, HNO3
Compounds; e.g. GaAs
H2O
H2
F2
C(diamond)
He
H
2.1
Cl2
SiC
Li
O
F
Ne
Be
C
1.0
Na
0.9
K
0.8
1.5
Mg
1.2
Rb
0.8
Cs
0.7
Sr
1.0
Ba
0.9
Ca
1.0
Ti
1.5
Cr
1.6
Fr
Ra
Engineering-45:
Materials of Engineering
0.7 0.9
31
2.0
2.5
Si
1.8
Fe
1.8
Ni
1.8
Zn
1.8
Ga
1.6
Ge
1.8
As
2.0
Sn
1.8
Pb
1.8
GaAs
4.0
Cl
3.0
-
Ar
-
Br
2.8
I
2.5
Kr
Xe
-
At
2.2
Rn
-
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Mixed Ionic+Covalent Bonding
 Many Compounds Exhibit
Ionic-Covalent Mixed Bonding

% - Ionic  1  e



X A  X B 2

4
 100%

 1

• where XA & XB are Pauling ElectroNegativities
 Example MgO: XMg = 1.3, XO = 3.5

% - Ionic  1  e


Engineering-45: Materials of Engineering
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
1.33.5 2

4
 100%

 70.2%
 1

Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Metallic Bonds
 Electrons Shared By
All Atoms
• “sea of electrons” around
“ion cores”
 Ion Cores
Ne config
• Atoms Give Up Valence-eto the “sea”, leaving
remaining Atoms with a
Positive Ionic Charge
– The Ion contains the Large
& Heavy Nucleus and is thus
FIXED in Space
 Generally Applies to
Electro-Positive Elements
• e.g.; Transition Metals such
as Ti, Ni, Zn, Cu
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Secondary Bonding
 Arises from Atomic or
Molecular DIPOLES
 What’s a DiPole?
• Separation of the + & Charge-Centers
 Fluctuating DiPoles
• Charge Centers Due to
SHORT-LIVED Charge
Asymmentry
– Generates an
ELECTRIC Field
within the Entity
E-Field
Engineering-45: Materials of Engineering
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 Liquifying Force for
Electrically Neutral and
Symetrical Molecules
such as H2, N2
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Secondary Bonding cont.
 Ionic Bonding in some
Molecules results in a
PERMANENT Dipole
 The +/- End of These
Polar Molecules can
Then Attract the -/+
Ends of Other Polar
Molecules
 General Case
 e.g.; HCl Liquid
 e.g.; Polymer
Solid
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Secondary Bonding, H Bond
 Recall that H has in
Only a Single Proton
and Electron
• NO Neutrons
 When H forms an Ionic
Bond, it Gives Up (for
the most part) the e-
 This Proton-Induced
Dipole is quite Strong
and Can Lead to
relatively powerful
Dipole Bonding
• Classic Example = H2O
to Form Liquid or Solid
• This Leaves the
Hydrogen’s p+ Ionic Core
Unscreened by any e-’s
• This Forms a Molecule
with a POSITIVE (and
Negative) end
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Summary: Chemical Bonding
Bond Type
Ionic
Bond Energy
Metallic
Large
Variable
• Large =>Diamond
• Small => Bismuth
Variable
• Large => Tungsten
• Small => Mercury
Secondary
Smallest
Covalent
Engineering-45: Materials of Engineering
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Notes
NonDirectional
e.g.; Ceramics
Directional
e.g.: SemiConductors, Ceramics,
Polymer-Chains
NonDirectional
e.g.; Metals
Directional
Interchain (PolyMer)
InterMolecular (Liq Water)
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Properties From Bonding: TMelt
 Bond Length
 Melting Temperature, TM
Energy (r)
r
 Bond Energy, E0
ro
r
Energy (r)
smaller TM
unstretched length
ro
r
Eo =
“bond energy”
Engineering-45: Materials of Engineering
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larger TM
 General Relationship:
|E0|↑  TM ↑
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Properties From Bonding: E
 Modulus of Elasticity
Defined
cross
sectional
area Ao
length, Lo
undeformed
unstretched length
ro
L
deformed
F
 Mathematically, E
Elastic modulus
F
L
=E
Ao
Lo
Engineering-45: Materials of Engineering
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 Modulus of Elasticity
Curvature of E vs r curve
Energy
r
Smaller E
larger E
 General Relationship:
|E0|↑  E ↑
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Properties From Bonding: 
 Coefficient of Thermal
Expansion, , Defined
Energy
length, L o
unheated, T1
  ~symmetry at r0
L
heated, T 2
 Mathematically, 
ro
r
Smaller 
Larger 
coeff. thermal expansion
L
=  (T2 -T1)
Lo
Engineering-45: Materials of Engineering
40
 General Relationship:
|E0|↑  ↑
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Summary: Primary Bonds
Ceramics
(Ionic & covalent bonding):
Metals
(Metallic bonding):
Polymers
(Covalent & Secondary):
Engineering-45: Materials of Engineering
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Large bond energy
large Tm
large E
small 
Variable bond energy
moderate Tm
moderate E
moderate 
Directional Properties
Secondary bonding dominates
small Tm
small E
large 
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
All Done for Today
α
Superimposed
On Periodic
Table
 GALLUIUM is the Tall Yellow one
 SODIUM is th Tall Blue one
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
WhiteBoard Work – P2.13
 K+ & O2-
dipotassium oxide = K2O
r0 = 1.5 nm
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
Problem Tutorial
Let’s Work
Text Problem
2.14
 Calcuim
Oxide →
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
P2.13
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
P2.13
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
P2.13
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
P2.14
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
P2.14
Engineering-45: Materials of Engineering
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Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
P2.15
% Program E45_Prob_2_15_1101.m:
% Plot EA and ER vs r * Verify r0 numerically
% Bruce Mayer, PE • ENGR45 • 24Jan11
%
% Calc r0 numerically using anonymous fcn for En
%* the eqn in text book is for r in nm
%
A = 1.436;
B = 5.86e-6;
En = @(r) B/r^9 - A/r
%
% find En,min at r = r0 us fminbnd command
[r0, Emin] = fminbnd(En, 0, 1);
disp('InterAtomic spacing for Min E, r0 in nm =')
disp (r0)
%
% Calc En,min = En(r0)
En_min = En(r0);
disp('Min E, En_min in eV =')
disp (En_min)%
% Set Plotting Vector as 300 points
r_plt = linspace (0.1, .4, 300); % in nm
%
% The Energy Functions
EA = -A./r_plt;
ER = B./r_plt.^8;
Etot = EA + ER;
%
% Plot on Same Graph
plot(r_plt,EA, r_plt,ER, r_plt, Etot), xlabel('r (InterAtom
Spacing)'),...
ylabel('Energy'), title('ENGR45 Problem 2.14'), grid,...
legend('EA', 'ER', 'Etot'), axis([.1 .4 -8 8])
%
% Compare to eqn 2.11 solution
n = 9;
disp('by eqn 2.11')
r0eqn = (A/(n*B))^(1/(1-n))
E0eqn = -A/(A/(n*B))^(1/(1-n)) + B/(A/(n*B))^(n/(1-n))
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
50
Bruce Mayer, PE
Engineering-45: Materials of Engineering
NaCl electron Exchange
Engineering-45: Materials of Engineering
51
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt
WhiteBoard Work – P2.13
 Ca2+ & O2-
Engineering-45: Materials of Engineering
52
Bruce Mayer, PE
BMayer@ChabotCollege.edu • ENGR-45_Lec-02_AtomicBonding.ppt