Classify each species as either a Lewis acid or a Lewis base. b. OH^–

Verified step by step guidance

1. Understand the definition of a Lewis acid and a Lewis base. A Lewis acid is a species that can accept an electron pair, while a Lewis base is a species that can donate an electron pair.
2. Consider the chemical species in question: OH⁻ (hydroxide ion).
3. Analyze the electron configuration of OH⁻. The hydroxide ion has a lone pair of electrons on the oxygen atom.
4. Determine the ability of OH⁻ to donate or accept an electron pair. Since OH⁻ has a lone pair of electrons, it can donate this pair to another species.
5. Conclude that OH⁻ acts as a Lewis base because it donates an electron pair.

Key Concepts

Lewis Acids and Bases

Lewis acids are defined as electron pair acceptors, while Lewis bases are electron pair donors. This theory expands the traditional definitions of acids and bases beyond protons, focusing instead on the transfer of electron pairs. Understanding this concept is crucial for classifying chemical species based on their ability to donate or accept electrons.

Electron Pair Donation

A Lewis base donates an electron pair to form a covalent bond with a Lewis acid. This donation is a key characteristic of Lewis bases, which often contain lone pairs of electrons that can be shared. Recognizing the presence of these lone pairs in a species helps in identifying its role in chemical reactions.

Hydroxide Ion (OH⁻)

The hydroxide ion (OH⁻) is a common example of a Lewis base due to its ability to donate a lone pair of electrons from the oxygen atom. This characteristic allows it to interact with Lewis acids, facilitating various chemical reactions. Understanding the properties of hydroxide is essential for classifying it correctly in the context of Lewis acid-base theory.