Metallic bonding

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

Resource summary

	Created by anna.a.graysmith over 10 years ago

	Copied by Hannah McCafferty about 5 years ago