2.2 Structure & bonding of carbon
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Describe and explain the properties of diamond
● Four, strong covalent bonds for each carbon atom ● Very hard (strong bonds) ● Very high melting point (strong bonds) ● Does not conduct heat / electricity (no delocalised electrons)
Describe and explain the properties of graphite
● Three covalent bonds for each carbon atom ● Layers of hexagonal rings ● High melting point ● Layers free to slide as weak intermolecular forces between layers; soft, can be used as a lubricant ● Conducts heat and electricity due to one delocalised electron per carbon atom
Describe and explain the properties of fullerenes
● Hollow shaped molecules ● Based on hexagonal rings but may have 5/7-carbon rings ● C60 has spherical shape, simple molecular structure (Buckminsterfullerene)
Describe and explain the properties of nanotubes
● Cylindrical fullerene with high length to diameter ratio ● High tensile strength (strong bonds) ● Electrical/thermal conductivity (delocalised electrons) ● Large surface area to volume ratio
Describe and explain the properties of graphene
● A single layer of graphite. ● High tensile strength (strong bonds) ● Electrical/thermal conductivity (delocalised electrons) ● Large surface area to volume ratio
What are giant covalent structures? Give examples
● Solids, atoms covalently bonded together in a giant lattice. ● High melting/boiling points – strong covalent bonds. ● Mostly don’t conduct electricity (no delocalised e−) ● Diamond, graphite, silicon dioxide.