Every Lewis acid is a Brønsted-Lowry acid, but not every Brønsted-Lowry acid is a Lewis acid.

Every Brønsted-Lowry acid is a Lewis acid, but not every Lewis acid is a Brønsted-Lowry acid.

The two theories are completely independent and have no overlap.

The Lewis theory is a specific case of the Brønsted-Lowry theory.

$H_3O^+$

$NH_3$

$HSO_4^-$

$BF_3$

${\rm{O}}{{\rm{H}}^ - }$

${\rm{N}}{{\rm{a}}_2}{\rm{C}}{{\rm{O}}_3}$

${\rm{N}}{{\rm{H}}_3}$

${\rm{HSO}}_4^ -$

${H_3}P{O_4}\,and\,P{O^{3 - }}_4$

${H_3}{O^ + }\,and\,P{O^{3 - }}_4$

${H_3}P{O_4}\,and\,HP{O^{2 - }}_4$

${H_3}P{O_4}\,and\,O{H^ - }$

${{\rm{H}}_2}{\rm{PO}}_2^ -$

${\rm{HPO}}_3^{2 - }$

${\rm{HPO}}_4^{2 - }$

All of these

A conjugate base

A non-polar solvent

An acid

A base

$HF$

${{\rm{H}}_2}{\rm{S}}$

${{\rm{H}}_2}{\rm{O}}$

${\rm{HCl}}$

${{\rm{H}}_2}{\rm{PO}}_4^ -$

${\rm{PO}}_4^{3 - }$

${{\rm{H}}_3}{\rm{P}}{{\rm{O}}_4}$

${{\rm{H}}_3}{\rm{P}}{{\rm{O}}_3}$

1.3 x 10^-2%

1.3 x 10^-3%

1.7 x 10^-2%

1.7 x 10^-8%

${\rm{C}}{{\rm{H}}_3}-{\rm{CH}}_2^ - > N{\rm{H}}_2^ - > H-C \equiv {{\rm{C}}^ - } > O{{\rm{H}}^ - }$

${\rm{H}}-{\rm{C}} \equiv {{\rm{C}}^ - } > C{{\rm{H}}_3}-{\rm{CH}}_2^ - > N{\rm{H}}_2^ - > O{{\rm{H}}^ - }$

${\rm{O}}{{\rm{H}}^ - } > N{\rm{H}}_2^ - > H-C \equiv {{\rm{C}}^ - } > C{{\rm{H}}_3}-{\rm{CH}}_2^ -$

${\rm{NH}}_2^ - > H-C \equiv {{\rm{C}}^ - } > O{{\rm{H}}^ - } > C{{\rm{H}}_3}-{\rm{CH}}_2^ -$

Lewis acids

Lewis bases

Bronsted acids

Bronsted bases