Identify the Lewis acid and Lewis base from among the reactants in each equation. b. AlBr₃ + NH₃ ⇌ H₃NAlBr₃ c. F^–(aq) + BF₃(aq) ⇌ BF₄^–(aq)

Verified step by step guidance

1. Identify the reactants in the equation: AlBr3 and NH3.
2. Recall the definition of a Lewis acid: a species that can accept an electron pair.
3. Recall the definition of a Lewis base: a species that can donate an electron pair.
4. Determine which reactant can accept an electron pair: AlBr3, as it has an empty orbital to accept electrons.
5. Determine which reactant can donate an electron pair: NH3, as it has a lone pair of electrons on the nitrogen atom.

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 concept of acids and bases beyond protons, focusing instead on electron pair interactions. Understanding this distinction is crucial for identifying the roles of reactants in chemical reactions.

Electron Pair Donation

In the context of Lewis theory, electron pair donation refers to the process by which a Lewis base donates a pair of electrons to a Lewis acid. This interaction forms a coordinate covalent bond, where both electrons in the bond originate from the base. Recognizing which reactant donates the electron pair is essential for determining the Lewis base in a reaction.

Coordination Complex Formation

Coordination complexes are formed when a Lewis acid and a Lewis base interact, resulting in a new compound where the acid accepts an electron pair from the base. This concept is fundamental in understanding many chemical reactions, particularly in transition metal chemistry, where such complexes play a significant role in reactivity and stability.