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The bond dissociation energy of B-F in B...

The bond dissociation energy of `B-F` in `BF_(3)` is `"646 kJ mol"^(-1)` whereas that of `C-F` in `CF_(4)` is `"515 kJ mol"^(-1)`. The correct reason for higher `B-F` bond dissociation energy as compared to that of `C-F` is

A

Smaller size of B -atom as compared to that of C - atom

B

Stronger `sigma` bond between B and F in `BF_3` as compared to that between C and F in `CF_4`

C

Significant `ppi - ppi` interaction between B and F in BF3 whereas there is no possibility of such interaction between C and F in `CF_4`

D

Lower degree of `ppi - ppi` interaction between Band F in `BF_3` than that between C and F in `CF_4`

Text Solution

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The correct Answer is:
C

Decrease in B - F bond length which results in the higher bond dissociation energy of B - F in `BF_3` is due to delocalised `ppi- ppi` bonding between filled p-orbital of F -atom and vacant p -orbital of B atom.
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