Interhalogen compounds oxoacids of halogens

Elements like fluorine, iodine, chlorine, bromine, and astatine are “halogens.” The members of this group share several characteristics. The physical and chemical characteristics of these molecules follow a predictable pattern. Many individuals aren’t aware that astatine is the group’s lone radioactive element. These elements contain seven electrons in their valence shell in their most common form. The electrical configuration of this pair is ns²np⁵.

They’ve moved one electron away from the closest noble gas or octet configuration. Because of their large effective nuclear charge, these elements have a tiny physical size. As a result, they have no inclination to lose electrons when heated. They may acquire one electron and complete their octet structure with relative ease. Halogens produce oxoacids in various forms. These are the acids in the acidic group of the periodic table that include oxygen

The suffixes –ous and –ic are used again to signify the lower and larger amount of oxygens in the acid formula if the acid includes oxygen (referred to as an oxoacid). Hydrogen, oxygen, and a few more elements make up oxyacids. Oxoacids are acids that include hydrogen, oxygen, plus another element besides hydrogen and oxygen.

Halogen Oxoacids and Their Properties

Fluorine is an excellent electrical conductor owing to its tiny size and high electronegativity. It only produces one oxoacid, HOF, which is known as fluoric(I) acid or hypofluorous acid in the presence of water. Other halogen family members combine to generate a variety of oxoacids. In their natural nature, they can’t be separated. 

Hypohalous acids (one oxidation state), halous acids (+three oxidation states), halic acids (+five oxidation states), and perhalic acids are the four types of oxoacids produced by halogens (with seven oxidation states).

Oxoacids of halogens structure

The core atom of oxoacids is sp³ hybridized, which means it has three electrons. One X-OH bond makes up the majority of each oxoacid. On the other hand, most oxoacids have X=O linkages in their structure. In nature, this double bond between oxygen and halogen is referred to as d⫪-p⫪ . The oxoacid series’ initial member has a strong acidic strength that distinguishes it from the rest. This is the only explanation given the halogen atom’s strong electronegativity and short size. The acidic strength increases as the number of halogen oxidations increases. This page discusses the oxoacid of halogen. 

Order of acidic strength of oxoacids of halogens (X) is as follows –

HOX <  HXO2  < HXO3  < HXO4

Conclusion

We have seen that the closest noble gas or octet configuration is one electron away from the halogen group elements. The tiny size of these elements is due to their high nuclear charge. Since they do not lose electrons, they do not incline to do so. They’re able to pick up one electron with ease, completing their octet structure. Halogens are responsible for the production of a wide range of oxoacids. These are only the acids that include oxygen.