Diamond and graphite Flashcards
What element is diamond and graphite made of?
Carbon
What type of bonds are there between the carbon atoms in diamond and graphite?
Covalent
In diamond, how many covalent bonds does each carbon atom make to other carbon atoms?
4
Why does diamond have such a high melting point?
It takes a lot of energy to break the strong covalent bonds
Why is diamond so hard?
The covalent bonds between carbon atoms are very strong
Why does diamond not conduct electricity?
There are no free (delocalised) electrons
In graphite, how many covalent bonds does each carbon atom make to other carbon atoms?
3
Why does graphite have such a high melting point?
It takes a lot of energy to break the strong covalent bonds
Describe the bonding and structure of graphite
Each carbon forms 3 covalent bonds with other carbon atoms to form layers.
The layers have weak forces between them.
One electron from each carbon atom becomes delocalised.
Why is graphite soft and slippery (it is often used as a lubricant)?
The layers of carbon atoms can slide over each other easily.
Why does graphite conduct electricity?
One electron from each carbon atom becomes delocalised and can move through the structure
