Diamond vs graphite by a conductivity?

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SUMMARY

Diamond is an electrical insulator due to its sp3 hybridization, where each carbon atom forms four covalent bonds, leaving no free electrons for conductivity. In contrast, graphite is a good conductor because it features sp2 hybridization, allowing for the formation of pi-bonds between carbon atoms. These pi-bonds create an unfilled conduction band, enabling the flow of electric current. Understanding the molecular orbital (MO) diagrams for both materials is crucial for grasping their distinct conductive properties.

PREREQUISITES
  • Understanding of hybridization types: sp3 and sp2
  • Knowledge of covalent bonding in carbon compounds
  • Familiarity with molecular orbital (MO) theory
  • Basic concepts of electrical conductivity in materials
NEXT STEPS
  • Study the molecular orbital diagrams for sp3 and sp2 hybridized carbon
  • Research the electrical properties of diamond and graphite
  • Learn about the implications of hybridization on material properties
  • Explore the concept of conduction bands and their role in electrical conductivity
USEFUL FOR

Students and professionals in materials science, chemistry, and electrical engineering who are interested in the conductive properties of carbon allotropes like diamond and graphite.

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Diamond vs graphite by a conductivity?

Hello. This is the last question on HW.

Q) Diamond and graphite are both made of carbon atoms. Explain why diamond is elecrically insulationg while graphite is a good conductor in terms of type(s) of hybridization of atomic orbitals and bonds in each material. Draw relevant molecular orbital (MO) diagrams for two canbons forming bonds fro each material and schemetically show these MOs leading to energy bands. (Consider only p-orbitals that form pi bonding, anti-bonding, or non-bonding MOs ---Only graphite)


I knew that no one electron is free to pass an electric current through the Diamond, since each atom's valence electron is taken up in covalent bonding. Other than that I have no clue... Is there MOs for a dimond or graphite? Are they consisted of only carbon, right? Please help me out.


Thanks,

Ryan.
 
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In a nutshell, diamond is sp3 hybrid and graphite is sp2 hybrid bonded. p orbitals perpendicular to the plane overlap to form pi-bonds between the layers, effectively an unfilled conduction band
 

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