Structure and bonding of carbon Flashcards
Explain the properties of diamond in terms of its structure and bonding
In diamond, the carbon atoms form FOUR strong covalent bonds (sharing electrons).
These bonds make the structure HARD.
The bonds are very strong and so require a great amount of energy to overcome, this means that they have a high melting and boiling point.
There are no delocalised electrons so diamond does NOT conduct electricity.
Explain the properties of Graphite in terms of its structure and bonding
In graphite, carbon atoms form THREE strong covalent bonds, forming layers of hexagonal rings with weak bonds between them.
The weak bonds between the layers mean that they can freely move over each other, this makes graphite SOFT and SLIPPERY, an IDEAL LUBRICATING MATERIAL.
The strong covalent bonds require a lot of energy to overcome, so graphite has a high boiling and melting point
Graphite can conduct electricity and thermal energy, as the carbon atoms have delocalised electrons.
Why is graphite similar to metals?
Because it has delocalised electrons and so can conduct electricity and thermal energy.
Explain the properties of Graphene in terms of its structure and bonding
Graphene is one layer of graphite. It is made of hexagonal rings joined together.
Graphene is only one atom thick so it is 2-dimensional and very light.
Because of strong covalent bonds, graphene can be added to composite materials to increase the strength without increasing the weight.
Explain the structure of fullerenes
Fullerene are molecules of carbon atoms with hollow shapes.
The structure of fullerenes are normally hexagonal but can be pentagonal or heptagonal.
What was the first fullerene ever discovered called?
Buckminsterfullerene (C60). It consisted of 60 carbon atoms in a spherical shape.
List some of the USES of fullerene
Lubricant
Industrial Catalyst ( because it has a large surface area)
Can be used to transmit drugs into the body (because fullerene can cage other molecules into it)
Why do Giant Covalent Structures have a high boiling and melting point?
In giant covalent structures the covalent bonds are very strong and require a great amount of energy to overcome so they have high melting and boiling points
Name 3 different Giant Covalent Structres
Diamond
Silica Dioxide (Silicon)
Graphite
Why does the structure of graphite make it useful as a lubricant?
Graphite consists of layers of hexagonal rings that are have no covalent bonds between them together.
Because of these weak forces between the layers, they can freely move over each other, this makes it soft and slippery and an ideal lubricating material.
Suggest why DIAMOND is useful as a cutting tool
In diamond, the carbon atoms form four strong covalent bonds. All of the electrons are bonded together, this makes diamond very hard and an d ideal for cutting.
Explain why graphite is able to conduct electricity
There are delocalised electrons, so the electrons can move through the structure and carry an electrical charge
Give a reason why a covalent structure may have a low boiling and melting point
The INTERMOLECULAR FORCES are weak
Explain why graphite is soft and slippery
In graphite the carbon atom form covalent bonds which form layers of hexagonal rings with no covalent bonds between the layers.
Due to the weak forces between the layers, the layers can freely move over each other, this makes them soft and slippery.
