giant covalent structures and Fullerenes

Question 1

giant covalent structures

Answer 1

similar to giant ionic lattices except there are no charged ions
atoms are bonded through strong covalent bonds
so they have high melting and boiling points
carbon atoms are giant covalent structures

Question 2

carbon

Answer 2

carbon atoms are giant covalent structures
can form different types of molecules cause carbon atoms can form up to 4 covalent bonds and easily bond to eachother

Question 3

diamond

Answer 3

pure diamonds are sparkly and colourless
each carbon atom forms 4 covalent bonds in very rigid giant covalent structures which make diamond hard
very high melting point
doesnt conduct electricity as it has no free electrons

Question 4

graphite

Answer 4

here the carbon atoms only make 3 covalent bonds creating sheets of carbon able to slide over each other
the layers are held together weakly so they are rubbed off onto paper(pencils)
high melting point
many delocalised electrons so it conducts electricity

Question 5

graphene

Answer 5

a single sheet of of graphite is graphene.
the covalent bonds make it strong but its so thin it is transparent and light
all its electrons are delocalised so it conducts electricity really well

Question 6

fullerenes

Answer 6

they are large molecules shaped like hollow balls. the atoms are arranged like rings
they have delocalised electrons so they can conduct electricity
have high melting and boiling points as they big molecules (bigger molecules have more intermolecular forces)