What is the Bronsted-Lowry acid and base versus Lewis?

Here’s how I understand it. We will look at some straight definitions and then we will put them into context right afterwards.
A Brnsted-Lowry acid is a proton donor while a Lewis base is an electron donor.
When a proton (##H^(+)##) accepts electrons donated from a Lewis base (like ##OH^(-)##) it exceeds its valency and must break its bond with a given atom on a Brnsted-Lowry acid (like the nitrogen on ##NH_4^(+)##).
If a bond between a Brnsted-Lowry acid and a proton breaks the Brnsted-Lowry acid donates the proton.
Thus a Lewis base can donate electrons to acquire a proton while the Brnsted-Lowry acid had donated that proton. They can work together!
From the other perspective a Brnsted-Lowry base is a proton acceptor while a Lewis acid is an electron acceptor.
If a Brnsted-Lowry acid (like ##NH_4^(+)##) accepts electrons from a Lewis base (like water in this case) then it is also a Lewis acid by definition.
Furthermore if that proton donates itself onto the Lewis base (water in this case) that base is also a Brnsted-Lowry base (water in this case) because it accepted the proton.
Thus a Lewis acid that possesses a proton can accept electrons to donate a proton while the Brnsted-Lowry base accepts that proton. Again they work together!