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bond dissociation energy of every c-h bond in methane is not 415 KJ /mole. why?
The first C-H bond break “sees” a CH3 group while the second C-H bond break “sees” a CH2 group and so on until all four C-H are broken. Each bond break sees a different electronic environment and so the energy required to break each successive C-H is slightly different.
DEAR FRIENDThe product of that dissociation is methyne () . The C-H bonds in methane do not have the same dissociation energy as C-H bonds in methyl radical, which in turn do not have the same dissociation energy as the C-H bonds in methylene, which are again different from the C-H bond in methyne.THANK U
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