1. Bonding in Metals Section 15.3
All of the metals on the periodic table are cations (positively charged ions)
Metallic bonds consist of metals ions held together by free- floating valence electrons

2. Metallic properties & why
Ductile – can be drawn into a thin wire
Malleable – can be hammered into differing shapes
A sea of floating valence electrons insulate the metal ions, so when they are under pressure, the metal ions slide past each other instead of shattering
Good conductors of electricity
Because electrons can flow freely between the metal ions, which causes them hold and transfer a current

3. Alloys – a mixture of metals
Metals are mixed to improve their individual properties
Examples:
Steel = mixture of iron, carbon, boron, chromium, manganese, molybdenum, nickel, tungsten and vanadium
24, 22, 18 or 10 Karat Gold = gold, copper, silver or palladium
Sterling Silver = silver and copper
Bronze = copper and nickel

4. After reading Section 15.3, you should know:
How a metallic bond compares to an ionic bond
At least 3 properties of metallic bonds
Why metallic bonds demonstrate these properties