Classify each species as either a Lewis acid or a Lewis base. a. BeCl₂

Verified step by step guidance

1. Identify 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 electronic structure of BeCl2: Beryllium (Be) is in group 2 of the periodic table and typically forms compounds where it has a +2 oxidation state, resulting in an electron-deficient central atom.
3. Consider the molecular geometry of BeCl2: It is a linear molecule with beryllium at the center bonded to two chlorine atoms, which are more electronegative and pull electron density away from beryllium.
4. Determine the electron pair availability: Since Be in BeCl2 is electron-deficient, it has empty orbitals that can accept electron pairs, making it a potential Lewis acid.
5. Classify BeCl2: Based on its ability to accept electron pairs due to its electron-deficient nature, BeCl2 is classified as a Lewis acid.

Key Concepts

Lewis Acids and Bases

Lewis acids are species that can accept an electron pair, while Lewis bases are species that can donate an electron pair. This definition expands the concept of acids and bases beyond protons (H+) to include electron pair interactions, making it applicable to a wider range of chemical reactions.

Electron Pair Donation

In the context of Lewis theory, a Lewis base donates an electron pair to form a covalent bond with a Lewis acid. This donation is crucial in understanding how different chemical species interact, as it determines the direction of electron flow and the formation of new compounds.

Molecular Geometry and Hybridization

The molecular geometry and hybridization of a species influence its ability to act as a Lewis acid or base. For example, BeCl2 has a linear geometry and does not have a lone pair of electrons, which makes it a Lewis acid as it can accept electron pairs from bases during chemical reactions.