Which of the following reactions represents and acid-base reaction according to Lewis theory but not according to Bronsted-Lowry theory?

Which of the following reactions represents and acid-base reaction according to Lewis theory but not according to Bronsted-Lowry theory?

a) NH3 + HCl --> NH4Cl
b) 2H2O <--> H3O+ + OH-
c) Cu2+ + 4NH3 <--> [Cu(NH3)4]2+
d) BaO + H2O <--> Ba2+ + 2OH-


Answer: c) Cu2+ + 4NH3 <--> [Cu(NH3)4]2+

as there is no exchange of H+

Which of the following could not act as a ligand in a complex ion with a transition metal?

Which of the following could not act as a ligand in a complex ion with a transition metal?

a) Cl-
b) NCl3
c) PCl3
d) CH4


Answer: d) CH4 because it does not possess a lone pair

For each of the following, identify the lewis acid and the Lewis base:

For each of the following, identify the lewis acid and the Lewis base:

a) 4NH3 + Zn2+ --> [Zn[NH3)4]2+
b) 2Cl- + BeCl2 --> [BeCl4]2-
c) Mg2+ + 6H2O --> [Mg(H2O)6]2+


a) acid = Zn2+ base = NH3
b) acid = BeCl2 base = Cl-
c) acid = Mg2+ base = H2O

How can all Bronsted-Lowry acid-base reactions be classified under Lewis, but Lewis cannot be classified under Bronsted Lowry?

How can all Bronsted-Lowry acid-base reactions be classified under Lewis, but Lewis cannot be classified under Bronsted Lowry?

Answer: All Bronsted-Lowry involves a transfer of lone pairs of electrons.

However, reactions according to Lewis where no transfer of H+ occurs does not fall under Bronsted-Lowry