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