Metallic bonding


GCSE Chemistry (Atoms) Flashcards on Metallic bonding, created by anna.a.graysmith on 13/05/2014.
Flashcards by anna.a.graysmith, updated more than 1 year ago
Created by anna.a.graysmith almost 10 years ago

Resource summary

Question Answer
describe the atoms in a pure metal the atoms in a pure metal are in tightly - packed layers which form a regular lattice structure
what 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
describe the final stage of metallic bonding the 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
why do metals have high boiling and melting points they have a very strong bond so they need a lot of energy to break the bonds meaning they have high boiling and melting points
what does the sea of electrons do the sea of electrons allow the metals to conduct electricity
what is the definition of metallic bonding? Metallic bonding is the strong attraction between closely packed positive metal ions and a 'sea' of delocalised electrons
why are metals malleable and ductile? because the layers slide over eachother
how 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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