The discussion centers on the existence of various oxyanions, specifically ClO-, ClO2-, ClO3-, and ClO4-, compared to the absence of FO3- and the limited presence of IO3- and BrO3-. The primary reason for these differences is attributed to the electronegativity and size of the elements involved. Fluorine, being the most electronegative element, cannot be oxidized by oxygen, which explains the lack of FO3-. The behavior of pnictides, particularly nitrogen and phosphorus, is also highlighted; phosphorus can form more complex oxyanions like H3PO4 due to having more electrons available for oxidation compared to nitrogen. The discussion touches on the ability of elements to form stable compounds based on their electron configurations, emphasizing that while the number of outer shell electrons is important, other factors like electronegativity and atomic size also play crucial roles in determining the formation of these compounds.