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Metallic bonding
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- 1describe the atoms in a pure metalthe atoms in a pure metal are in tightly - packed layers which form a regular lattice structure
- 2what do the outer electrons of metal atoms do?they separate from the atoms and create a sea of electrons, these atoms then delocalize and so are free to move through the whole structure
- 3describe the final stage of metallic bondingthe delocalised atoms that can move through the structure become positively charged ions and are attracted to the sea of electrons, this attraction is called metallic bonding
- 4why do metals have high boiling and melting pointsthey have a very strong bond so they need a lot of energy to break the bonds meaning they have high boiling and melting points
- 5what does the sea of electrons dothe sea of electrons allow the metals to conduct electricity
- 6what is the definition of metallic bonding?Metallic bonding is the strong attraction between closely packed positive metal ions and a 'sea' of delocalised electrons
- 7why are metals malleable and ductile?because the layers slide over eachother
- 8how do delocalized electrons in metallic bonding allow metals to conduct heat and electricity?for example, when a metal is heated, the delocalised electrons gain kinetic energy, these electrons then move faster so they gain energy throughout the metal, this makes the hear transfer in metals very efficient
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- El usuario ha eliminado su información de asignaturas Fichas sobre Metallic bonding, creado por Usuario eliminado el 10/06/2021.
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- Usuario eliminado · jun 2021
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- 10 jun 2021
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- Creado por anna.a.graysmith · 13 may 2014
- Copiado por Francesca gore · 10 jun 2021
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