Editing Lewis acids and bases (section)

===Simple Lewis acids===
Some of the most studied examples of such Lewis acids are the boron trihalides and [[organoboranes]]:<ref>{{cite journal |doi=10.1021/ic990713m|title=Ligand Close-Packing and the Lewis Acidity of BF3 and BCl3 |year=1999 |last1=Rowsell |first1=Bryan D. |last2=Gillespie |first2=Ronald J. |last3=Heard |first3=George L. |journal=Inorganic Chemistry |volume=38 |issue=21 |pages=4659–4662 |pmid=11671188 }}</ref>
:BF<sub>3</sub> + F<sup>−</sup> → {{chem2|BF4-}}
In this adduct, all four fluoride centres (or more accurately, [[ligand]]s) are equivalent.
:BF<sub>3</sub> + OMe<sub>2</sub> → BF<sub>3</sub>OMe<sub>2</sub>
Both BF<sub>4</sub><sup>−</sup> and BF<sub>3</sub>OMe<sub>2</sub> are Lewis base adducts of boron trifluoride.

Many adducts violate the [[octet rule]], such as the [[triiodide]] anion:
:I<sub>2</sub> + I<sup>−</sup> → {{chem2|I3-}}
The variability of the colors of iodine solutions reflects the variable abilities of the solvent to form adducts with the Lewis acid I<sub>2</sub>.

Some Lewis acids bind with two Lewis bases, a famous example being the formation of [[hexafluorosilicate]]:
:SiF<sub>4</sub> + 2 F<sup>−</sup> → {{chem2|SiF6(2-)}}