|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