In this video we're going to take a look at a mean reactions through the prism of acid based reactions. Now under this type of reaction, an acid reacts with an amine, which represents a weak base. Now recall when a base accepts an H+, it transforms into a conjugate acid. This conjugate acid of an amine is called the ammonium ion.
Now here we're going to say for the ammonium ion we modify the ending of a mean, which is the neutral form of our mean to ammonium ion. So if we take a look here at this generic amino reaction, we have methylamine as our starting amine. It's reacting with hydrochloric acid, which is an acid. We know, following the Bronsted-Lowry definition, that the acid donate to an H+ to the base.
So when it accepts that H+, it's now accepting H+. So now nitrogen is making four bonds. So it's going to be positively charged. And we're going to say when a nitrogen is possibly charged by making four bonds, that's when the moniker of ammonium ion comes into play. So we're going from methylamine to methyl ammonia ion. So this would be the name of our newly created ammonium ion product.