diamond,graphite and graphene ,fullerenes

what bond is graphite?

graphite is a covalent bond

property of graphite

graphite is soft and slippery, high mp and bp,good conductor of electricity and heat

in graphite each carbon atom forms covalent bonds to how many other carbon atoms?

in graphite each carbon atom forms covalent bonds to 3 other carbon atoms

in graphite what do the carbon atoms form? which have … covalent bonds …………. the layers

carbon atoms form hexagonal rings which have no covalent bonds between the layers

in graphite what does no covalent bonds between the layers mean?

no covalent bonds between the layers means layers can slide over eachother making graphite soft and slippery

why does graphite have high mp and bp?

if we want to melt graphite,we need to break those bonds with lots of energy thats why graphite has a high mp and bp

why can graphite can conduct electricity?

graphite can conduct electricity as the delocalised electrons can move

what does one electron from each carbon atom is delocalised mean?

one electron from each carbon atom is delocalised makes graphite similar to metals because of its delocalised electrons

giant covalent substances are always solids at room temp because all giant covalent substances have high mp and bp

4 diamond properties

4 strong covalent bonds for each carbon atom,very hard,very high mp ,doesnt conduct electricity

to melt a diamond we need to break all the covalent bonds which takes a huge amount of energy so they have high mp and bp

why cant diamond conduct electricity?

diamond cant conduct electricity as it has no free electrons to carry electrical charge

silicon dixoide have high mp and bp?

silicone have a high mp and bp as they have a huge number of strong covalent bonds

to melt silicon dioxide,…… covalent bonds need to be broken with?

to melt silicon dioxide these covalent bonds need to be broken with lots of energy