Examples of Lewis Acids and Lewis Bases

We’re going take a look at Lewis acids and bases. A Lewis acid is a substance that accepts electron pairs. A Lewis base that is just the opposite, a substance that donates electron pairs. Look at this reaction right here. We have hydrogen and ammonia and a reaction to form this product.

Here, the Lewis acid is going to be the hydrogen right here, because it accepts an electron pair from ammonia. Ammonia is obviously the Lewis base, because it’s what’s donating the electron pair to hydrogen over here on the product side.

In a reaction like this it’s very easy, because as soon as you identify the Lewis acid or base, you know the other element or compound must be the other one, either the Lewis acid or the Lewis base. Now, there are three main points about Lewis acids and bases that is helpful if you understand.

First of all, understand that the Lewis acid, or the concept of Lewis acid and Lewis bases, is the broadest definition of acids and bases. Lewis acids and bases do not depend upon any particular ion. Finally, Lewis acids and bases can occur in any state, not just the liquid phase.

Again, a Lewis acid is a substance that accepts electron pairs. A Lewis base donates electron pairs. The concept of Lewis acids and bases is the broadest definition. They do not depend upon any particular ion, and they can occur in any state.