Classify each species as either a Lewis acid or a Lewis base. d. CN^–

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. Examine the chemical species CN⁻: The cyanide ion (CN⁻) has a negative charge, indicating it has an extra electron pair.
3. Consider the electron configuration of CN⁻: The negative charge suggests that CN⁻ has a lone pair of electrons that it can donate.
4. Determine the role of CN⁻: Since CN⁻ can donate an electron pair, it acts as a Lewis base.
5. Conclude the classification: CN⁻ is classified 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 classification is based on the ability of a species to either accept or donate a pair of electrons during a chemical reaction, expanding the traditional definitions of acids and bases beyond just protons.

Electron Pair Donation

A Lewis base donates an electron pair to form a covalent bond with a Lewis acid. This process is crucial in many chemical reactions, as it allows for the formation of new compounds and the stabilization of reactive intermediates. Understanding which species can donate electron pairs is essential for classifying them correctly.

Cyanide Ion (CN-)

The cyanide ion (CN-) is a well-known example of a Lewis base because it has a lone pair of electrons on the carbon atom that can be donated to a Lewis acid. This property allows CN- to participate in various chemical reactions, including coordination complexes and nucleophilic substitutions.