JIC MME 323 Materials Science Teaching Slide Week 2

1. MME 323: MATERIALS SCIENCE
WEEK 2 :
ATOMIC STRUCTURE & INTERATOMIC
BONDING*
Adhi Primartomo, PhD
Email: primartomo_a@jic.edu.sa
Office: Room 191 – JIC Academic Building
* Source: Materials Science and Engineering; 9th Edition; W.D.Callister;
Wiley; 2011
https://sites.google.com/site/primartomo/file-cabinet

2. ~ LECTURE OUTLINE ~
Chapter 2: Atomic Structure & Interatomic
Bonding (page 17 - 43)
• Why Study Atomic Structure & Interatomic
Bonding?
• Fundamental Concepts,
• Electrons in Atoms,
• Quantum Numbers,
• Electron Configuration,
• The Periodic Table,
• Primary Atomic Bonding,
• Secondary Atomic Bonding.
2

3. ~ Week 2 Learning Objective ~
After studying this chapter, you should be able to:
• Define atomic number, atomic mass, isotope, atomic
weight and atomic mass unit,
• Name the two atomic models and note the differences
between them,
• Give the atomic configurations for the atoms based on
Pauli exclusion principle,
• Briefly describe the ionic, covalent, metallic, hydrogen
and Van der Waals bonds,
• Mention which atoms/molecules exhibit each of these
bonding types mentioned above.
3

4. WHY STUDY ATOMIC STRUCTURE & INTERATOMIC
BONDING?
(page 18)
The atomic structures and interatomic bonding directly
define the properties of materials
4
Pic Source:
http://www.auburn.edu/~blumeri
/diamond/diamond.htm
Example: Carbon as graphite
and diamond

5. FUNDAMENTAL CONCEPTS
(page 18-19)
Atom consist of:
 Nucleus (core): protons + neutrons
 Electrons (e-)
5
• Atomic Number (Z):
?
• Atomic Mass (A):
?
• Atomic Weight:
?
• Atomic Mass Unit (amu):
?
• Isotope:
?

6. ELECTRONS in ATOMS – ATOMIC MODELS
(page 20-21)
Bohr Atomic Model:
 Electrons revolve around
nucleus in certain orbitals
6
Wave Mechanical/Quantum
Mechanics Model:
 Electrons is at various
locations around nucleus
 The locations/regions
shapes is described by
complex mathematical
equations

7. ELECTRONS in ATOMS – QUANTUM NUMBERS
(page 21-23)
7
• Every electron in an atom is characterized by 4 parameters 
Quantum Numbers (n, l, m, no. of electrons)
• ‘n’  no. of shells
Value of ‘n’ = 1 ,2 ,3 & 4
• ‘l’  no. of sub-shells
Value of ‘l’ = 0 ,1 ,2 & 3 or s, p, d & f
value of 'n' value of 'l' Name of Subshell
1 0 (s) 1s
2
0 (s) 2s
1 (p) 2p
3
0 (s) 3s
1 (p) 3p
2 (d) 3d
4
0 (s) 4s
1 (p) 4p
2 (d) 4d
3 (f) 4f

8. ELECTRONS in ATOMS – QUANTUM NUMBERS
(page 21-23)
8
• ‘m’  no. of electron orbitals in each sub-shell
• Each electron orbital  max 2 electrons
Subshell No. of Orbitals (m) Max No. of Electrons
s 1 2
p 3 6
d 5 10
f 7 14
Shell No.: Name of Subshell + Max Electrons
1 1s2
2
2s2
2p6
3
3s2
3p6
3d10
4
4s2
4p6
4d10
4f14

9. ELECTRONS in ATOMS – ELECTRON CONFIGURATIONS
(page 24-26)
9
• Pauli Exclusion Principle  each electron state/electron orbital
max 2 electrons
Subshell No. of Orbitals (m) Max No. of Electrons
s 1 2
p 3 6
d 5 10
f 7 14
Shell No.: Name of Subshell + Max Electrons
1 1s2
2
2s2
2p6
3
3s2
3p6
3d10
4
4s2
4p6
4d10
4f12

10. 10
1s
2s
2p
K-shell n = 1
L-shell n = 2
3s
3p M-shell n = 3
3d
4s
4p
4d
Energy
N-shell n = 4
• have discrete energy states
• tend to occupy lowest available energy
state.
Electrons:
ELECTRONS in ATOMS – ELECTRON CONFIGURATIONS
(page 24-26)

11. 11
Hafnium Diagonal Rule for Electron Configuration:
ELECTRONS in ATOMS – ELECTRON CONFIGURATIONS
(page 24-26)

12. ELECTRONS in ATOMS – ELECTRON CONFIGURATIONS
(page 24-26)
12
• Electron Configuration  represents the way in which the
electron states/electron orbitals are occupied.
• Notation (how to write) : No. of electrons in each subshell
indicate by a script after shell-subshell designation:
1s2
Shell Subshell
No. of electron
• Examples: - Hydrogen (H), Z=1  1s1
- Helium (He), Z=2  1s2
- Lithium (Li), Z=3  1s2 2s1

13. ELECTRONS in ATOMS – ELECTRON CONFIGURATIONS
(page 24-26)
13
Valence electron:
• Electrons that occupy outermost shell,
• Involve in bonding between atoms to form molecules,
• Physical & chemical properties of solids based on valence
electron.
Stable electron configuration:
• Valence electron shell completely filled,
• Max no. of electron in outermost shell  8 (as in Ne, Ar, Kr)
• Basic for chemical reactions & atomic bonding in solids  ?

14. THE PERIODIC TABLE of ELEMENTS
(page 26-27)
14

15. • Element  Type of Atom that is distinguishes by Its Atomic
Number
• Periodic Table of Elements  Tabular Method of Displaying
Elements
• Same Column  Same valence electron and similar properties
 Alkali Metal –> Group 1 (Li, Na, K, Rb, Cs): Soft, Low Density,
Has 1 valence electron  Very Reactive (React with halogen)
 Halogen –> Group VIIA (F, Cl, Br, I): Has 7 valence electrons
 Highly Reactive Gas (React with Alkali Metal)
 Noble Gas –> Group VIIIA (He, Ne, Ar, Kr, Xe): Odorless, Has 8
valence electrons  Great Chemical Stability
 Electropositive  ?
 Electonegative  ?
15
THE PERIODIC TABLE of ELEMENTS
(page 26-27)

16. PRIMARY INTERATOMIC BONDINGS
(page 30-37)
Atom-to-Atom bonding that involves the exchange of valence
electrons to assume stable electrons structure (as inert gases – 8
valence electrons
16
1. Ionic Bonding
• metal + non-metal, electropositive + electronegative
• ?

17. PRIMARY INTERATOMIC BONDS
(page 30-37)
17
2. Covalent Bonding
• Non-metal + non-metal,
• ?

18. PRIMARY INTERATOMIC BONDS
(page 30-37)
18
3. Metallic Bonding
• metal + metal,
• ?

19. SECONDARY BONDING
(page 30-37)
Arise due to atomic or molecular dipoles
19
1. Van der Waals bonding:

20. SECONDARY BONDING
(page 30-37)
Arise due to atomic or molecular dipoles
20
2. Hydrogen Bonding:

21. 21