In the reaction between bromine (Br₂) and iron(III) bromide (FeBr₃), we can identify the Lewis acid and Lewis base. In this case, FeBr₃ acts as a Lewis acid because it can accept an electron pair, while Br₂ can act as a Lewis base by donating an electron pair.
The reaction can be represented by the following equation:
\[ \text{Br}_2 + \text{FeBr}_3 \rightarrow \text{Br}^+ + \text{FeBr}_4^- \]
In this reaction:
- FeBr₃ (Lewis acid) accepts a pair of electrons from one of the bromine atoms in Br₂, resulting in the formation of a bromide ion (Br⁻) and a positively charged bromine ion (Br⁺).
- The remaining FeBr₄⁻ is formed by the coordination of the Br⁻ to the FeBr₃.
This equation highlights the role of Br₂ as a Lewis base and FeBr₃ as a Lewis acid in this reaction.
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