Based on their compositions and structures and on conjugate acid–base relationships, select the stronger base in each of the following pairs: (b) BrO- or BrO2-

Verified step by step guidance

1. Identify the conjugate acids for each base: BrO^- and BrO_2^-.
2. Recall that the strength of a base is inversely related to the strength of its conjugate acid.
3. Determine the conjugate acids: HBrO for BrO^- and HBrO_2 for BrO_2^-.
4. Compare the acid strengths: HBrO is a weaker acid than HBrO_2 because it has fewer oxygen atoms, which means less electron-withdrawing effect.
5. Conclude that BrO^- is the stronger base because its conjugate acid (HBrO) is weaker than the conjugate acid of BrO_2^- (HBrO_2).

Key Concepts

Conjugate Acid-Base Pairs

In acid-base chemistry, a conjugate acid-base pair consists of two species that differ by the presence of a proton (H+). The strength of a base is often determined by its ability to accept protons, while the strength of an acid is determined by its ability to donate protons. Understanding these relationships helps in predicting which species will act as a stronger base in a given context.

Oxidation States and Stability

The oxidation state of an element in a compound can influence its chemical behavior, including its acidity or basicity. In the case of bromine oxoanions like BrO- and BrO2-, the oxidation state of bromine affects the stability of the anions. Generally, higher oxidation states can lead to greater acidity, which inversely affects the basicity of the conjugate base.

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 can stabilize negative charge better, which can influence the strength of a base. For the bromine oxoanions, the presence of additional oxygen atoms in BrO2- increases the electronegativity effect, making BrO- a stronger base due to less stabilization of the negative charge.