Metallic Bond the force that holds metal atoms together Metals do not form covalent bonds with one another because they do not have enough electrons in their outer shells to form stable octets ID: 1024199
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1. Metallic Bonding
2. Metallic BondingMetallic Bond – the force that holds metal atoms togetherMetals do not form covalent bonds with one another because they do not have enough electrons in their outer shells to form stable octets.Even though they do not form covalent bonds, they do share electrons.They release their electrons to a shared pool of electrons.Imagine a metal as a non-rigid arrangement of metal ions in a sea of free electrons.
3. Sea of electronsThe valence electrons delocalize from the positive atoms.
4. Melting pointAccording to the strength of the bondDepends on the number of electrons the atom can delocalize to its “sea”Group 1 metals have the lowest m.p. since they only have one valence electron to contribute; also they have the largest radius so the positive nucleus is further from the seaTransition metals have particularly high melting points because they can involve the d electrons in their delocalization in addition to the s e’s.
5. ConductivityElectricalMetals conduct electricity well because the electrons can flow in the sea.ThermalMetals also conduct heat well because the freely moving electrons have kinetic energy.
6. Strength and WorkabilityMalleable – can be beaten into sheetsDuctile – can be stretched into wiresBECAUSE the atoms are able to roll over each other without breaking bondsStress can be put on the metal and released and the atoms will go back to normal because metals are ELASTIC.
7. Animation Websiteshttp://cd1.edb.hkedcity.net/cd/science/chemistry/resource/animations/metallic_bond/metallic.htmlhttp://www.ausetute.com.au/metallic.htmlhttp://www.drkstreet.com/resources/metallic-bonding-animation.swf