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Why is graphite said to be thermodynamically more stable than diamond?

Why is graphite said to be thermodynamically more stable than diamond?

Grade:12th pass

1 Answers

Umakant biswal
5359 Points
5 years ago
Graphite is sp2 hybridized, and the sp2 hybrid orbitals participate in covalent bond formation, the unhybridized p-orbital participates in pi-bonding. 
Graphite has delocalized pi-electrons over the entire sheet 
This delocalization lowers the energy of the system, leading to greater thermodynamic stability. 
Delocalization of electrons or greater conjugation - enhances the thermodynamic stability..
In diamond the interaction is only between neighbouring carbon atoms. 

In Graphite the delocalization of pi-electrons is over the entire 2-dim layer >
although u can say graphite have an extra electron but diamond donot have that . 
thats the reason behind it . 
ALL THE BEST ..

 

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