Binary Acids vs Oxyacids
Acids are defined in several ways by various scientists. Arrhenius defines an acid as a substance that donates H3O+ ions in the solution. Bronsted- Lowry defines a base
Binary Acids vs Oxyacids
Acids are defined in several ways by various scientists. Arrhenius defines an acid as a substance that donates H3O+ ions in the solution. Bronsted- Lowry defines a base as a substance that can accept a proton. Lewis acid definition is far common than the above two. According to it, any electron pair donator is a base. According to the Arrhenius or Bronsted-Lowry definition, a compound should have a hydrogen and the ability to donate it as a proton to be an acid. But according to Lewis, there can be molecules, which don’t possess hydrogen, but can act as an acid. For example, BCl3 is a Lewis acid, because it can accept an electron pair. An alcohol can be a Bronsted-Lowry acid, because it can donate a proton; however, according to Lewis, it will be a base. Regardless of the above types of acids which are defined differently, acids can be described and classified in many other ways. For example, acids are classified as inorganic and organic acids depending on the elements they have. In this article, we are going to focus on another way of classifying acids, which is as binary acids and oxyacids.
Binary acids are molecules, which contain two elements; one element is hydrogen, and the other one is a nonmetal element, which is more electronegative than hydrogen. Therefore, binary acids can donate H+ ions in aqueous media. HCl, HF, HBr, and H2S are some of the examples for binary acids. These show different properties when they are in pure form and when they are in aqueous media. In the nomenclature of