Giant Covalent Structures And Fullerenes Flashcards
What is the difference between giant covalent structures and giant ionic lattices?
There are no charged ions
How are atoms in giant covalent structures bonded to each other?
Strong covalent bonds
What are the melting and boiling points of giant covalent structures like?
Melting and boiling points are very high
Do giant covalent structures conduct electricity at all?
No, unless it is graphite and graphene
Describe the physical properties of diamond.
Sparkly, colourless, hard
Describe the carbon bonding pattern in diamonds.
Each carbon atoms forms 4 other covalent bonds in a very rigid covalent structure. This makes diamonds very hard.
What kind of melting and boiling point does diamond have and why?
Very high, this is because of all of the strong covalent bonds between the carbon atoms.
Does diamond conduct electricity? Why?
No, it does not have any free electrons or ions.
Describe the physical properties of graphite.
Black and opaque and shiny
Describe the bonding pattern in graphite.
Each carbon atom only has 3 covalent bonds creating sheets of carbon atoms which are free to slide over each other.
How are the layers of carbon atoms held together and what does this mean?
The layers are held on together weakly so that means they are slippery and slide over each other easily.
What is the melting and boiling point of graphite like?
High melting and boiling point
Given that only 3 out of 4 electrons in carbon’s outer shell are used in bonding, what is the final electron used for?
That electron become delocalised and so that means graphite can conduct electricity.
What is a single sheet of graphite called?
Graphene
Describe the physical properties of graphene.
Strong, thin, light
