Identify the Lewis acid and Lewis base in each reaction: (a) \(\mathrm{Na}^{+}+6 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{Na}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{+}\) (b) \(\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}\) (c) \(\mathrm{F}^{-}+\mathrm{BF}_{3} \rightleftharpoons \mathrm{BF}_{4}^{-}\)

Short Answer

Expert verified
(a) \(\mathrm{Na}^{+}\) is the Lewis acid; \(\mathrm{H}_{2} \mathrm{O}\) is the Lewis base. (b) \(\mathrm{CO}_{2}\) is the Lewis acid; \(\mathrm{H}_{2} \mathrm{O}\) is the Lewis base. (c) \(\mathrm{BF}_{3}\) is the Lewis acid; \(\mathrm{F}^{-}\) is the Lewis base.

Step by step solution

01

Title - Define Lewis Acid and Lewis Base

A Lewis acid is a substance that can accept an electron pair, while a Lewis base is a substance that can donate an electron pair.
02

Title - Analyze Reaction (a)

In the reaction (a) \(\mathrm{Na}^{+}+6 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{Na}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{+}\), \(\mathrm{Na}^{+}\) is accepting electron pairs from \(\mathrm{H}_{2} \mathrm{O}\), making \(\mathrm{Na}^{+}\) the Lewis acid. \(\mathrm{H}_{2} \mathrm{O}\) is donating electron pairs, making it the Lewis base.
03

Title - Analyze Reaction (b)

In the reaction (b) \(\mathrm{CO}_{2} + \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}\), \(\mathrm{CO}_{2}\) is accepting electron pairs from \(\mathrm{H}_{2} \mathrm{O}\), making \(\mathrm{CO}_{2}\) the Lewis acid. \(\mathrm{H}_{2} \mathrm{O}\) is donating electron pairs, making it the Lewis base.
04

Title - Analyze Reaction (c)

In the reaction (c) \(\mathrm{F}^{-} + \mathrm{BF}_{3} \rightleftharpoons \mathrm{BF}_{4}^{-}\), \(\mathrm{BF}_{3}\) is accepting electron pairs from \(\mathrm{F}^{-}\), making \(\mathrm{BF}_{3}\) the Lewis acid. \(\mathrm{F}^{-}\) is donating electron pairs, making it the Lewis base.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Lewis acid definition
A Lewis acid is a substance that can accept an electron pair from a donor during a chemical reaction. This concept was introduced by Gilbert N. Lewis in 1923 and offers a broad definition of acids beyond the familiar hydrogen-ion donors (Brønsted acids). Lewis acids can be cations like \(\text{Na}^{+}\), neutral molecules with vacant orbitals like \(\text{BF}_{3}\), or even molecules like \(\text{CO}_{2}\). By understanding electron pair acceptance, we can analyze many chemical reactions, observe stability, and predict the formation of complexes.
Lewis base definition
A Lewis base is a substance that can donate an electron pair to an electron pair acceptor (the Lewis acid) to form a covalent bond. Some common examples of Lewis bases include water (\(\text{H}_{2}\text{O}\)), fluoride ions (\(\text{F}^{-}\)), and ammonia (\(\text{NH}_{3}\)). It's important to note that Lewis bases are not limited to neutral molecules; anions are often effective Lewis bases due to their extra electron pairs. Understanding Lewis bases allows for deeper insight into complexation reactions and mechanisms in organic and inorganic chemistry.
electron pair acceptance
The process of electron pair acceptance is a defining feature of a Lewis acid. When a Lewis acid encounters a Lewis base in a chemical reaction, it accepts an electron pair from the Lewis base. For instance, in reaction (a) \(\text{Na}^{+} + 6 \text{H}_{2}\text{O} \rightleftharpoons \text{Na}(\text{H}_{2}\text{O})_{6}^{+}\), the \(\text{Na}^{+}\) ion accepts electron pairs from water molecules. This process stabilizes the \(\text{Na}^{+}\) ion and forms a complex ion. Similarly, in reactions (b) and (c), the electron pair acceptors are \(\text{CO}_{2}\) and \(\text{BF}_{3}\), respectively.
electron pair donation
Electron pair donation is the act performed by a Lewis base during a reaction. In this process, the Lewis base donates a pair of electrons to a Lewis acid, creating a new covalent bond. In the reactions we analyzed, water (\(\text{H}_{2}\text{O}\)) donates electron pairs to \(\text{Na}^{+}\) and \(\text{CO}_{2}\), while fluoride ions (\(\text{F}^{-}\)) donate electron pairs to \(\text{BF}_{3}\). This electron donation is crucial in forming stable product complexes and driving the reaction towards equilibrium.
chemical reaction analysis
Analyzing chemical reactions through the lens of Lewis acids and bases provides a clearer understanding of the reaction mechanisms. When examining reactions like (a) \(\text{Na}^{+} + 6 \text{H}_{2}\text{O} \rightleftharpoons \text{Na}(\text{H}_{2}\text{O})_{6}^{+}\), (b) \(\text{CO}_{2} + \text{H}_{2}\text{O} \rightleftharpoons \text{H}_{2}\text{CO}_{3}\), and (c) \(\text{F}^{-} + \text{BF}_{3} \rightleftharpoons \text{BF}_{4}^{-}\), we identify the key role of electron pair transfer. This transfer not only signifies the formation of products but also influences factors like reaction rate and stability. By understanding which species acts as a Lewis acid or base, students can predict the course of many chemical reactions and propose plausible reaction mechanisms.

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Most popular questions from this chapter

The following aqueous species constitute two conjugate acid-base pairs. Use them to write one acid-base reaction with \(K_{c}>1\) and another with \(K_{c}<1: \mathrm{NO}_{3}^{-}, \mathrm{F}^{-}, \mathrm{HF}, \mathrm{HNO}_{3}\)

The antimalarial properties of quinine \(\left(\mathrm{C}_{20} \mathrm{H}_{24} \mathrm{~N}_{2} \mathrm{O}_{2}\right)\) saved thousands of lives during the construction of the Panama Canal. This substance is a classic example of the medicinal wealth that tropical forests hold. Both \(\mathrm{N}\) atoms are basic, but the \(\mathrm{N}\) (colored) of the \(3^{\circ}\) amine group is far more basic \(\left(p K_{b}=5.1\right)\) than the \(N\) within the aromatic ring system \(\left(p K_{b}=9.7\right)\) (a) A saturated solution of quinine in water is only \(1.6 \times 10^{-3} M\). What is the pH of this solution? (b) Show that the aromatic N contributes negligibly to the pH of the solution. (c) Because of its low solubility, quinine is given as the salt quinine hydrochloride \(\left(\mathrm{C}_{20} \mathrm{H}_{24} \mathrm{~N}_{2} \mathrm{O}_{2} \cdot \mathrm{HCl}\right),\) which is 120 times more soluble than quinine. What is the pH of \(0.33 M\) quinine hydrochloride? (d) An antimalarial concentration in water is \(1.5 \%\) quinine hydrochloride by mass \((d=1.0 \mathrm{~g} / \mathrm{mL}) .\) What is the \(\mathrm{pH} ?\)

Write balanced net ionic equations for the following reactions, and label the conjugate acid-base pairs: (a) \(\mathrm{NaOH}(a q)+\mathrm{NaH}_{2} \mathrm{PO}_{4}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Na}_{2} \mathrm{HPO}_{4}(a q)\) (b) \(\mathrm{KHSO}_{4}(a q)+\mathrm{K}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons \mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{KHCO}_{3}(a q)\)

Perchloric acid, \(\mathrm{HClO}_{4},\) is the strongest of the halogen oxoacids, and hypoiodous acid, \(\mathrm{HIO}\), is the weakest. What two factors govern this difference in acid strength?

(a) Is a weak Bronsted-Lowry base necessarily a weak Lewis base? Explain with an example. (b) Identify the Lewis bases in the following reaction: $$ \mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}^{2+}(a q)+4 \mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{Cu}(\mathrm{CN})_{4}^{2-}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l) $$ (c) Given that \(K_{c}>1\) for the reaction in part (b), which Lewis base is stronger?

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