Pick the stronger base from each pair. c. F^– or ClO^–

Key Concepts

Acid-Base Theory

Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry theory, an acid is a proton donor, while a base is a proton acceptor. Understanding this concept is crucial for determining the strength of bases, as it helps identify which species can effectively accept protons in a reaction.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs consist of two species that differ by the presence of a proton. When a base accepts a proton, it forms its conjugate acid. The strength of a base can often be inferred from the stability of its conjugate acid; a weaker conjugate acid indicates a stronger base. This concept is essential for comparing the basicity of F- and ClO-.

Electronegativity and Basicity

Electronegativity refers to the tendency of an atom to attract electrons in a bond. In the context of basicity, a more electronegative atom in a conjugate base can stabilize the negative charge, making it a weaker base. Comparing the electronegativities of fluorine and chlorine helps determine which anion, F- or ClO-, is the stronger base, as the less electronegative atom will generally be a stronger base.