Why is the carbon fluorine bond stronger than the carbon oxygen bond?

From [this wiredchemist.com](http://www.wiredchemist.com/chemistry/data/bond_energies_lengths.html), I obtained values of the bond dissociation energies of the $\ce{C-O}$ and $\ce{C-F}$ bonds:


\begin{align}
D\_0(\ce{C-F}) &= \pu{485 KJ mol-1}\\
D\_0(\ce{C-O}) &= \pu{358 KJ mol-1}
\end{align}


I have read an explanation saying that is because of fluorine being more electronegative than oxygen, consequently the dipole moment across the bond is greater. As a result the delta negative on $\ce{F}$ and delta positive on $\ce{C}$ attracts each other more compared to the situation in $\ce{C-O}$.


There is another explanation of better overlap resulting in stronger bond. However in this case the orbital overlap seems quite similar and if not $\ce{C-O}$ has better overlap than $\ce{C-F}$, so this explanation doesn't apply.


However, if this is the case, then why in many organic reaction mechanisms, the polar bonds are more prone to break when the atom with delta positive on is attacked by a nucleophile? Would you give examples for nucleophilic addition-elimination and for nucleophilic substitution?


