Interesting article, but I wish OPs would give us a comment on what made it worth sharing to them.

As a Chem major it’s cool to see this, but not sure how it ended up on the front page?

Ah, Brønsted-Lewis. In defence of the OP:

People informed on Chemistry usually take "acid = you'll get H₃O⁺ in water" and "base = you'll get OH⁻ in water"; that is, the Arrhenius' definition, updated for modern times. Brønsted-Lewis actually makes you think about what's going on (the transference of H⁺), in order to generalise it to other situations.

For example, consider the following reaction:

H₂O + HF ←→ OH⁻ + H₂F⁺

You don't get H₃O⁺ so by Arrhenius' [updated] definition there wouldn't be an acid there. But there is one - H₂O.

And someone might say "but wait, Arrhenius talks about H⁺!" - well, go look for "bare" protons in nuclear fusion, not in chemical reactions.

Even more interesting is how some chemicals (like water or amino acids) are amphoteric and act as both acids and bases, depending on what environment they are in.

Gas phase Brønsted acids are kind of mind boggling, if I'm understanding them correctly. They are up to 10^(30) times more acidic than standard strong acids. The goal (I'm not sure if this has been reached) is a compound that in equilibrium has free protons, just bouncing around in space. (In solution, the free protons are always bound to something, for example H3O+ in water.)

Reminds me of one of the childhood book titles that I inexplicably remember even as I forget things from last week - "Acids, Bases and the Chemistry of the Covalent Bond". Which [1] tells me was written by Calvin A. VanderWerf, University of Kansas.

[1] https://pubs.acs.org/doi/10.1021/ed039p273.2

This is a random section from a chemistry course?

https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2....

Would be a more accessible document for the audience.