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Metallic Bonds• Metals can only bond to themselves (same
element)
• Don’t transfer or share electrons (need to lose)
• Do form lattices in solid state
• 8-12 metal atoms surround a single atom
• Crowded so outer energy levels overlap
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Electron Sea Model
• Valence electrons form a “sea” of electrons
• Free to move = delocalized electrons
• Forms a metallic cation (+ nucleus)
• Metallic Bond = cation + delocalized e-
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Metallic Properties
• Moderately high MP – really varies from mercury (-38.9) to tungsten (3422 celsius)
• High BP • Malleable & ductile• Durable• Good conductors –both heat & electricity• Luster (easily absorb & release light)• Transition metals = really hard & strong
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WHY?
• Mobile electrons = metal’s properties
• d electrons = make transitions metals even harder & stronger like chromium, iron and nickel
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Alloys
• Mixture of elements that has metallic properties – usually 2 or more metals
• Ex: brass, bronze, pewter, stainless steel
• Why – get good qualities of both elements
• 2 kinds that are easy to form: substitutional and interstitial
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Substitutional Alloys
• Occur when atoms of different elements are similar in size
• Atoms of one element are substituted for atoms of another element
• Ex: copper atoms replace silver atoms to form sterling silver
• Brass, pewter and 10 carat gold are other examples
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Interstitial alloys
• Occur when one atom is much bigger than the other atom
• A smaller atom is than used to fill in the spaces or interstices of the bigger atom – like pouring sand into a bucket of gravel
• Ex: carbon is added to iron and forms carbon steel which makes it harder, stronger and less ductile