1.35 Recall that graphite and diamond are different forms of carbon and that they are examples of giant covalent substances 1.36 Describe the structures of graphite and diamond Flashcards
What is the structure of diamond?
In diamond, each carbon is joined to 4 other carbons covalently.
What are the properties of diamond?
Diamond is very hard, has a very high melting point, and does not conduct electricity.
What is the bonding structure of carbon in graphite?
In graphite, each carbon is covalently bonded to 3 other carbons, forming layers of hexagonal rings, with no covalent bonds between the layers.
What allows the layers of graphite to slide over each other?
The layers can slide over each other due to no covalent bonds between the layers, but weak intermolecular forces. This means that graphite is soft and slippery.
What happens to one electron from each carbon atom in graphite?
One electron from each carbon atom is delocalised.
How do graphite and diamond differ?
Graphite and diamond are different forms of carbon and are examples of giant covalent substances.
What is a key structural similarity between graphite and metals?
Graphite is similar to metals because of its delocalised electrons.
Can graphite conduct electricity?
Yes, graphite can conduct electricity, unlike diamond.
