First, the remarks are made, not about boron itself, but boron
compounds or (boron
in a compound). For example, alkylboranes are said to be susceptible to oxidation. As B is more electropositive than C, in an oxidation reaction like R
3B
(RO)
3B it is formally C, not B, that undergoes an increase in oxidation number. (The mechanism involves transfer of R
- from B to O, so the electropositivity of B favours this.)
Boron has 3 valence electrons, therefore tends to form compounds with an incomplete octet. This is the reason for B compounds undergoing electrophilic reactions, as the octet can be made up by donation of a lone pair from a Lewis base into the empty orbital on B, e.g. BF
3 + F
- BF
4-. But this can be reversed; tetrafluoroborates can often be heated to give the fluoride and BF
3. Whereas you wouldn't get CF
4 giving CF
3+ + F
-, because CF
3+ isn't a stable compound.
You can also get dative delocalisation, e.g. >N:-B<
>N
+=B
-<. Note that this puts a negative charge on B, though it is electropositive. This is the reverse of the familiar phenomenon that O or Cl is inductively electron-withdrawing but mesomerically electron-donating. In principle this could happen on pyridine, deactivating it to electrophilic attack, though I'm not sure from your description whether B is directly attached to pyridine, and if so whether as a C substituent or an N adduct.