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

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

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

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