Acid Bases Venn Diagram

[Jennifer Downey]

Fromcategorizing molecules to ranking their strength without pKa or pKb values. This isn't terrible if/when you learn it correctly, however, your professor will assume you already know this.

The key here is to recognize that while each classification has a specific definition, any given molecule can fall into more than one category, some into all 3. Again, something we'll look at later in this article.

An acid dissociating in water does not form a free-floating proton. Instead one of the water molecules in solution will grab the H+ yielding a hydronium or H3O+ ion. Here's what happens when nitric acid dissociates in water.

An Arrhenius base is a molecule that when dissolved in water will break down to yield an OH- or hydroxide in solution. To recognize the Arrhenius base look for a molecule ending in OH, but not following CHx which refers to an alcohol.

The Arrhenius definition for acids and bases only refers to compounds dissolved in water. Does this mean that acids and bases cannot exist out of water? Not quite, that's where the Bronsted-Lowry definition comes in.

A Bronsted-Lowry acid, like an Arrhenius acid, is a compound that breaks down to give an H+ in solution. The only difference is that the solution does not have to be water. We can still refer to the exact same acids as listed for the Arrhenius acid examples, but this time we'll change the solvent to ammonia, alcohol, or anything else.

This is where we start to see the difference between the Bronsted-Lowry and Arrhenius definitions. While the Arrhenius base referred specifically to the hydroxide (OH-) ion, the Bronsted-Lowry base refers to any atom or ion capable of accepting or bonding to a free proton in solution.

The drawing below is part of the EAS Aromatic Halogenation reaction which you'll see in late Orgo 1 or Orgo 2. Notice how the Fe gets attacked by a lone pair of electrons. By accepting those electrons Fe acts as a Lewis acid

Since the Lewis definition has to do with the transfer of electrons, you can guess by now that a Lewis Base is an electron pair donor. Once again think back to your reaction mechanisms. The molecule using its electrons to attack another atom is an electron pair donor and a Lewis Base.

The definitions above evolved slowly as scientists were starting to understand more and more details about chemical reactions. The first is a basic (no pun intended) definition, but the last 2 simply expand to fit more complex solvents and situations.

Now that you understand the similarities/difference between Arrhenius, Bronsted-Lowry, and Lewis acids and bases, how do you tell which is the stronger or weaker acid? Which molecule is more reactive? Which side of a reaction will be favored at equilibrium?

As an organic chemistry student you will be required to recognize and classify 3 different types of acids and bases. Arrhenius, Bronsted-Lowry, and Lewis. While the technical definitions vary, once you get the logic behind their definitions you'll be able to quickly and easily identify the different types of acids and bases.

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Even though this doesnt answer your question completely. I thought that this will be useful for other people looking to plot Venn Diagram.One can use the venn() function from the gplots package: -r.org/packages/cran/gplots/docs/venn

I know that the OP asks about a solution in R but I would like to point to a web-based solution called BioVenn. It takes up to 3 lists of elements and draws a Venn diagram so that each surface is proportional to the number of elements - like this one:

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