1. Introduction to Bonding

2. Metallic Bonding: Metal-metal bonds
Valence electrons are mobile, moving easily from atom to atom

3. Ionic Bonding: Metals and Non-Metals
Metals lose electrons, become (+) ions
Non-metals gain electrons, become (-) ions
+ and – ions hold each other tightly in place

4. Covalent Bonding: Non-metals Sharing Electrons
A handful of non-metals (C, N, O, H) are extremely common
They tend to share their valence electrons with each other to gain noble gas configurations
Covalent bonded elements make molecules.

5. Metallic Bonding Valence Electrons are a mobile “sea”
Act as “lubrication”, allowing rows of atoms to slide past each other
Mobile electrons account for conductivity, malliability, ductility

6. Metallugy
The development of metallurgy has led to the rise and fall of civilizations, technological development

7. Important Metals

8. Properties of Metals Good conductors – mobile valence electrons
Malleable – can be bent into shapes
Ductile – can be drawn into wires
Good conductors of heat (low specific heat)
Shiny – has luster
Many metals are dense, with high melting points
Alloys (solutions of metals) have different properties than the pure metals

9. Alloys

10. Examples of Alloys Steel: Fe and C Stainless Steel: Fe, C and Cr
Bronze: Cu and Sn
Brass: Cu and Zn
Pewter: Sn, Sb, Bi, Pb
Dental Amalgam: Hg, Ag, Sn, Cu
Lead Solder: Sn, Pb
Lead-free Solder: Sn, Ag, Cu