Polymers And Giant Covalent Structures-Paper 1 Flashcards
Properties of Giant covalent structures?
Very high melting and boiling points.
No charged particles (except graphite)
All atoms bonded to each other by strong covalent bonds.
Do giant covalent structures have high or low melting/boiling points? why?
Very high as lots of energy is required to break the covalent bonds between the atoms.
Do giant covalent structures conduct electricity?
No, they don’t contain charged particles so they don’t conduct electricity even when molten- EXCEPT GRAPHITE
How many covalent in diamond?
Each carbon atom forms 4 covalent bonds in s very rigid giant covalent structure.
How many covalent bonds does graphite bond to?
Each carbon atom forms 3 covalent bonds which creates layers of hexagons. Each carbon atom has one delocalised electron.
Why is diamond hard?
Due to the carbon atoms each forming four covalent bonds. They take lots of energy to break.
Why is graphite weak?
There aren’t any covalent bonds BETWEEN the layers, so they’re free to move over each other.
Why is graphite used in lead?
As there aren’t any covalent bonds between the layers, they’re feee to move other each other so it’s soft and slippery.
What is graphene?
One layer of graphite ( a sheet of carbon atoms joined together in hexagons, only one atom thick making it 2D)
Why could graphene be used in electronics?
It contains delocalised electrons so can conducts electricity through the whole structure.
What are fullerenes?
Molecules of carbon shaped like closed tubes or hollow balls.
What are fullerenes mainly made up of?
Carbon atoms arranged in hexagons, pentagons or heptagons.
Fullerenes can form…
Nanotubes- tint carbon cyclinders.
Nanotubes can co duct both ….. and …..
Electricity and thermal energy.
Give 3 uses of fullerenes?
Lubricants
Catalysts
Strengthen materials
Drug delivery
