Bonding in MetalsSection 15.3All 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

Metallic properties & whyDuctile – can be drawn into a thin wireMalleable – can be hammered into differing

shapesA 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 electricityBecause electrons can flow freely between the

metal ions, which causes them hold and transfer a current

Alloys – a mixture of metalsMetals 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 copperBronze = copper and nickel

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