Fundamentals of Materials Science and Engineering: An Integrated Approach, 3e

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22 • Chapter 2 / Atomic Structure and Interatomic Bonding

Table 2.2 A Listing of the Expected Electron Configurations for Some of the

Common Elementsa

Element Symbol Atomic Number Electron Configuration

Hydrogen H 1 1 s^1

Helium He 2 1 s^2

Lithium Li 3 1 s^22 s^1

Beryllium Be 4 1 s^22 s^2

Boron B 5 1 s^22 s^22 p^1

Carbon C 6 1 s^22 s^22 p^2

Nitrogen N 7 1 s^22 s^22 p^3

Oxygen O 8 1 s^22 s^22 p^4

Fluorine F 9 1 s^22 s^22 p^5

Neon Ne 10 1 s^22 s^22 p^6

Sodium Na 11 1 s^22 s^22 p^63 s^1

Magnesium Mg 12 1 s^22 s^22 p^63 s^2

Aluminum Al 13 1 s^22 s^22 p^63 s^23 p^1

Silicon Si 14 1 s^22 s^22 p^63 s^23 p^2

Phosphorus P 15 1 s^22 s^22 p^63 s^23 p^3

Sulfur S 16 1 s^22 s^22 p^63 s^23 p^4

Chlorine Cl 17 1 s^22 s^22 p^63 s^23 p^5

Argon Ar 18 1 s^22 s^22 p^63 s^23 p^6

Potassium K 19 1 s^22 s^22 p^63 s^23 p^64 s^1

Calcium Ca 20 1 s^22 s^22 p^63 s^23 p^64 s^2

Scandium Sc 21 1 s^22 s^22 p^63 s^23 p^63 d^14 s^2

Titanium Ti 22 1 s^22 s^22 p^63 s^23 p^63 d^24 s^2

Vanadium V 23 1 s^22 s^22 p^63 s^23 p^63 d^34 s^2

Chromium Cr 24 1 s^22 s^22 p^63 s^23 p^63 d^54 s^1

Manganese Mn 25 1 s^22 s^22 p^63 s^23 p^63 d^54 s^2

Iron Fe 26 1 s^22 s^22 p^63 s^23 p^63 d^64 s^2

Cobalt Co 27 1 s^22 s^22 p^63 s^23 p^63 d^74 s^2

Nickel Ni 28 1 s^22 s^22 p^63 s^23 p^63 d^84 s^2

Copper Cu 29 1 s^22 s^22 p^63 s^23 p^63 d^104 s^1

Zinc Zn 30 1 s^22 s^22 p^63 s^23 p^63 d^104 s^2

Gallium Ga 31 1 s^22 s^22 p^63 s^23 p^63 d^104 s^24 p^1

Germanium Ge 32 1 s^22 s^22 p^63 s^23 p^63 d^104 s^24 p^2

Arsenic As 33 1 s^22 s^22 p^63 s^23 p^63 d^104 s^24 p^3

Selenium Se 34 1 s^22 s^22 p^63 s^23 p^63 d^104 s^24 p^4

Bromine Br 35 1 s^22 s^22 p^63 s^23 p^63 d^104 s^24 p^5

Krypton Kr 36 1 s^22 s^22 p^63 s^23 p^63 d^104 s^24 p^6

aWhen some elements covalently bond, they formsphybrid bonds. This is especially true

for C, Si, and Ge.

configurations by gaining or losing electrons to form charged ions, or by sharing

electrons with other atoms. This is the basis for some chemical reactions and also for

atomic bonding in solids, as explained in Section 2.6.

Under special circumstances, thesandporbitals combine to form hybridspn

orbitals, wherenindicates the number ofporbitals involved, which may have a

value of 1, 2, or 3. The 3A, 4A, and 5A group elements of the periodic table (Figure

2.6) are those that most often form these hybrids. The driving force for the formation

of hybrid orbitals is a lower energy state for the valence electrons. For carbon the

sp^3 hybrid is of primary importance in organic and polymer chemistries. The shape