I/GCSE Chemistry – Giant Covalent Compounds

• Same things in different forms of carbon
• Graphite, charcoal, and diamond are all allotropes of carbon.

• 4 Covalent Bonds  - Carbon has 4 electrons in the outer shell so makes 4 covalent bonds.
• Rigid structure  - This makes diamond hard.
• High melting point  - Covalent bonds are strong so it takes a lot of energy to break them.
• Won't conduct electricity  - There are no free electrons or ions.

• Strong covalent bonds between carbon atoms. Weak intermolecular forces between the layers.
• 3 covalent bonds - 3 of 4 electrons are used in the covalent bond, the fourth one is delocalized (moving freely) so conducts electricity.
• High melting point - Lots of energy needed to break the strong bonds.
• Conducts electricity - The delocalized electron conducts electricity.
• Layers held by weak forces - The layers slide over each other so it is slippery and can be used as a lubricant

• A single layer of graphite.
• 1 atom thick - Makes it 2-dimensional atoms.
• Strong - Due to the strong covalent bonds.
• Light - Can be used to add strength without adding weight.
• Conducts electricity - Like graphite, it contains delocalized electrons so can conduct electricity through the whole structure. This means it has the potential to be used in electronics.

• Fullerenes are hollow molecules of carbon, shaped like tubes or balls.
• They're mainly made up of carbon atoms arranged in hexagons but can also contain pentagons (rings of five carbon atoms) or heptagons (rings of seven carbon atoms).

It's got the molecular formula C₆₀ forms a hollow sphere (cage-like shape) containing 20 hexagons and 12 pentagons.
 

• Tiny carbon cylinders.
• The ratio between the length and diameter is very high. 
• Good conductors of heat and electricity

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Written by Bryant Wong (Chemistry)

Photo reference

1. Wikipedia, https://tr.wikipedia.org/wiki/Fulleren