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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?
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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