The $B-F$ bond dissociation energy in $BF_3$ is $646 \, kJ \, mol^{-1}$,whereas the $C-F$ bond dissociation energy in $CF_4$ is $515 \, kJ \, mol^{-1}$. Which of the following is the correct reason for the $B-F$ bond dissociation energy being higher than the $C-F$ bond dissociation energy?

• A
  Smaller size of $B$ atom compared to $C$ atom.
• B
  Stronger bond between $B$ and $F$ in $BF_3$ compared to the weaker bond between $C$ and $F$ in $CF_4$.
• C
  Presence of $p\pi - p\pi$ interaction between $B$ and $F$ in $BF_3$,which is not possible between $C$ and $F$ in $CF_4$.
• D
  Less interaction between $C$ and $F$ in $CF_4$ compared to $p\pi - p\pi$ interaction between $B$ and $F$ in $BF_3$.