Identify the Lewis acid and Lewis base from among the reactants in each equation. a. Ag⁺(aq) + 2 NH₃(aq) ⇌ Ag(NH₃)₂⁺(aq)

Verified step by step guidance

1. Identify the reactants in the given chemical equation: Ag^+(aq) and NH_3(aq).
2. Recall the definition of a Lewis acid: a species that can accept a pair of electrons.
3. Recall the definition of a Lewis base: a species that can donate a pair of electrons.
4. Determine which reactant is the Lewis acid: Ag^+ is the Lewis acid because it can accept a pair of electrons from NH_3.
5. Determine which reactant is the Lewis base: NH_3 is the Lewis base because it can donate a pair of electrons to Ag^+.

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 theory expands the definition of acids and bases beyond protons, focusing instead on electron pair interactions. In the given reaction, identifying which species donates and which accepts electron pairs is crucial for determining the roles of the reactants.

Coordination Complexes

Coordination complexes are formed when a central metal atom or ion binds to surrounding molecules or ions, known as ligands. In the provided equation, Ag+ acts as a central metal ion, and NH3 serves as a ligand. Understanding how these complexes form helps in identifying the Lewis acid-base interactions in the reaction.

Electron Pair Donation

Electron pair donation is a key process in Lewis acid-base chemistry, where a Lewis base donates a pair of electrons to a Lewis acid. This interaction leads to the formation of new bonds and complexes. Recognizing which reactant donates the electron pair is essential for correctly identifying the Lewis base in the reaction.