This question is about different allotropic structures of carbon: diamond and Buckminsterfullerene (C60\text{C}_{60}C60).
Name the type of chemical bond that exists between the carbon atoms within both diamond and Buckminsterfullerene.
Explain, in terms of structure and bonding, why diamond has an extremely high melting point.
Buckminsterfullerene has a simple molecular structure. Explain why it sublimes at a much lower temperature than diamond melts.
Diamond and graphite are two different crystalline forms of carbon. They can be interconverted according to the equation:
C(diamond)⇌C(graphite)ΔH=−1.9 kJ/mol \text{C}(\text{diamond}) \rightleftharpoons \text{C}(\text{graphite}) \quad \Delta H = -1.9 \text{ kJ/mol} C(diamond)⇌C(graphite)ΔH=−1.9 kJ/molWould a low or a high temperature favour the conversion of diamond into graphite? Give a reason for your choice.
