[o1ocups]

I know that a Lewis acid is an electron-pair acceptor, and a Lewis base is an electron-pair donor. So in this case: CH₃NH₂(g)+HBr(g)  CH₃NH₄Br(s), HBr is the Lewis acid and the other one is the base, right? But do they have to form a covalent bond at the end?

In this reaction: Al(NO₃)₃(s)+6H₂O(l)  Al(H2O)₆³⁺(aq)+NO3^-(aq), can the reactants still be classified as Lewis acid and base?

I am just not sure if the electron pair donor and the electron pair acceptor have to form a covalent bond.

Thanks!!

[Loyal]

Someone can correct me if I am missing something.

The H forms a covalent bond with the N, but the Br itself is not covalently bonded as it became an ion.   Since the CH3NH3 is now a positive ion the bromine likes to hang around unless they are in solution.

[o1ocups]

But does the product of Lewis acid and base always contain a covalent bond (even if the bond doesn't include all the elements involved)?

[o1ocups]

I have another related question: are all Brønsted-Lowry acids/bases Lewis acids/bases ?
All the examples of Lewis acids/bases that are given in my book have one single product that is the compound of the two reactants bonded by a covalent bond. Is that the standard form of Lewis acid/base reactions?

[Loyal]

But does the product of Lewis acid and base always contain a covalent bond (even if the bond doesn't include all the elements involved)?

In most of the examples I can think of I will say yes, but just because of that don't assume that it is only possible for it to form a covalent bond.   

I have another related question: are all Brønsted-Lowry acids/bases Lewis acids/bases ?
All the examples of Lewis acids/bases that are given in my book have one single product that is the compound of the two reactants bonded by a covalent bond. Is that the standard form of Lewis acid/base reactions?

The since a Brønsted-Lowry acid/base involves the transfer of protons(H+) most if not all can be considered Lewis acids.   Lewis took it one step further to explain the fact that not all acids or bases have an OH or a H. 

[o1ocups]

So Brønsted-Lowry acids/bases also form covalent bonds? I thought they are separate ions.
(for example NH₃ +H₂O NH₄⁺ + OH^-, do NH₄⁺ and OH^- form covalent bonds?)

[o1ocups]

Al(NO₃)₃(s)+6H₂O(l) Al(H₂O)₆³⁺(aq)+NO^3-(aq)

So in this reaction, is Al(NO₃)₃ the Lewis base since it's the electron-pair donor, and is H₂O the Lewis acid because it's the electron-pair acceptor?

[o1ocups]

Al(NO₃)₃(s)+6H₂O(l) Al(H₂O)₆³⁺(aq)+NO^3-(aq)

So in this reaction, is Al(NO₃)₃ the Lewis base since it's the electron-pair donor, and is H₂O the Lewis acid because it's the electron-pair acceptor?

Even if they are not stuck together at the product side?

[Loyal]

So Brønsted-Lowry acids/bases also form covalent bonds? I thought they are separate ions.
(for example NH₃ +H₂O NH₄⁺ + OH^-, do NH₄⁺ and OH^- form covalent bonds?)

The H itself forms a covalent bond.   Any other bonds are usually ionic.