Identify the Lewis acid and Lewis base in each of the following reactions: (b) FeBr31s2 + Br-1aq2 Δ FeBr4-1aq2

Verified step by step guidance

1. Identify the species involved in the reaction: FeBr3(s) and Br^-(aq).
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 species is accepting an electron pair: FeBr3 is accepting an electron pair from Br^- to form FeBr4^-.
5. Determine which species is donating an electron pair: Br^- is donating an electron pair to FeBr3, making Br^- the Lewis base.

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. Understanding this concept is crucial for identifying the roles of reactants in chemical reactions.

Electron Pair Donation

In the context of Lewis acid-base 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, which is essential in many chemical reactions. Recognizing which species donates and which accepts electrons is key to determining the acid-base roles in a reaction.

Coordination Complexes

Coordination complexes are formed when a central metal atom or ion binds to surrounding ligands through coordinate covalent bonds. In the given reaction, the formation of FeBr4- involves the coordination of bromide ions to the iron center. Understanding how these complexes form helps in identifying the Lewis acid and base in the reaction.