4.2.3 Structure and bonding of carbon Flashcards
What is the structure of diamond?
Each carbon atom forms four covalent bonds in a giant covalent structure.
What are the properties of diamond?
Very hard.
Very high melting point.
Does not conduct electricity (no free electrons).
Why is diamond so hard and has a high melting point?
The strong covalent bonds throughout the structure make diamond extremely durable and heat-resistant.
What is the structure of graphite?
Each carbon atom forms three covalent bonds, creating layers of hexagonal rings.
There are no covalent bonds between the layers.
One electron per carbon atom is delocalised.
What are the properties of graphite?
Soft and slippery (layers can slide over each other).
Good conductor of electricity (delocalised electrons).
High melting point (strong covalent bonds within layers).
How is graphite similar to metals?
Both graphite and metals have delocalised electrons, allowing them to conduct electricity.
What is graphene, and what is its structure?
Graphene is a single layer of graphite, consisting of hexagonal rings of carbon atoms.
What are the properties of graphene?
Strong and lightweight.
Excellent conductor of electricity and heat.
Useful in electronics and composites.
What are fullerenes, and what is their structure?
Fullerenes are molecules of carbon atoms with hollow shapes.
They are based on hexagonal rings but can also contain rings with five or seven carbon atoms.
What are the types of fullerenes?
Buckminsterfullerene (C60): Spherical shape.
Carbon Nanotubes: Cylindrical fullerenes with high length-to-diameter ratios.
What are the uses of fullerenes?
Nanotechnology.
Electronics.
Materials science.
Why can carbon nanotubes and graphene conduct electricity?
Both have delocalised electrons that are free to move and carry electrical charge.
