Presentation on theme: "Bonding in Metals Section 15.3"— Presentation transcript:
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 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 shatteringGood conductors of electricityBecause 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 propertiesExamples:Steel = mixture of iron, carbon, boron, chromium, manganese, molybdenum, nickel, tungsten and vanadium24, 22, 18 or 10 Karat Gold = gold, copper, silver or palladiumSterling Silver = silver and copperBronze = copper and nickel
4 After reading Section 15.3, you should know: How a metallic bond compares to an ionic bondAt least 3 properties of metallic bondsWhy metallic bonds demonstrate these properties
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