Classify each of the following as a Lewis acid or a Lewis base. (e) OH-

Verified step by step guidance

1. Step 1: Recall the definition of a Lewis acid and a Lewis base. A Lewis acid is a substance that can accept a pair of electrons, while a Lewis base is a substance that can donate a pair of electrons.
2. Step 2: Consider the chemical species given in the problem, which is the hydroxide ion, \( \text{OH}^- \).
3. Step 3: Analyze the electron configuration of \( \text{OH}^- \). The hydroxide ion has a lone pair of electrons on the oxygen atom.
4. Step 4: Determine whether \( \text{OH}^- \) can donate or accept a pair of electrons. Since it has a lone pair, it can donate electrons.
5. Step 5: Conclude that \( \text{OH}^- \) is a Lewis base because it can donate a pair of electrons.

Key Concepts

Lewis Acids and Bases

Lewis acids are substances that can accept an electron pair, while Lewis bases are those that can donate an electron pair. This definition expands the traditional Brønsted-Lowry concept of acids and bases, which focuses on proton transfer. Understanding this distinction is crucial for classifying chemical species based on their electron pair interactions.

Electron Pair Donation

A Lewis base is characterized by its ability to donate a pair of electrons to form a covalent bond. In the case of hydroxide ion (OH-), it has a lone pair of electrons that it can readily donate, making it a strong Lewis base. This property is essential for predicting how OH- will interact with Lewis acids in chemical reactions.

Hydroxide Ion (OH-)

The hydroxide ion (OH-) is a negatively charged ion consisting of one oxygen atom covalently bonded to one hydrogen atom. It is commonly encountered in aqueous solutions and is known for its basic properties. Recognizing OH- as a Lewis base is important for understanding its role in acid-base chemistry and its interactions with various Lewis acids.