Identify the Lewis acid and Lewis base from among the reactants in each equation. a. Fe 3+ (aq) + 6 H 2 O(l) ⇌ Fe(H 2 O) 6 3+ (aq) b. Zn 2+ (aq) + 4 NH 3 (aq) ⇌ Zn(NH 3 ) 4 2+ (aq) c. (CH 3 ) 3 N(g) + BF 3 (g) ⇌ (CH 3 ) 3 NBF 3 (s)

Hey everyone. So today we are asked to identify which of the reactant in the following reaction between silver and ammonia are the lewis acid and Lewis base. Now recalling our definitions, a Lewis acid, Let's sort this out. A Lewis acid is any compound that can freely accept electrons. It is an electron except her. And conversely a Lewis base is an electron donor. It can donate electrons into solution. With this in mind we can go ahead and take a look at our to react ints. We have a G plus, A G plus or silver plus and we have ammonia, N H three. So right off the bat we can see that silver is a cat ion. In this case it has a charge of plus one. So as a positively charged metal, that means that it can accept electron pairs. So by that definition that means that this is a Lewis acid. We have to look no further. Similarly, by that same logic, if silver is the lewis acid, then ammonia has to be the Lewis base. However, just to double check this, we can go ahead and draw the Lewis structure for ammonia. To see if there are any lone pairs that can be donated, which signifies that electrons can be donated by ammonia. So ammonia nitrogen has five valence electrons. Remember we need to find out how many valence electrons we have in a molecule to draw out it's loose structure. So we have five valence electrons from the nitrogen. We have three hydrogen, each of which have one valence electron each. So one times three which will give you eight valence electrons. Now, ammonia will be our central atom. It will be bonded to three hydrogen, Which gives us six total electrons present in single bonds And the remaining two of the total eight valence electrons present in Ammonia can be added as a lone pair on these nitrogen as such. Because there's this nitrogen because there's this lone pair on the nitrogen. Sorry, that means that it can be donated into solution, thus solidifying the fact that ammonia is our louis base space. Therefore once again, silver pluses are loose, acid and ammonia is our lewis base. I hope this helps. And I look forward to seeing you in the next one.

Ch.16 - Acids and Bases

Tro - Chemistry: A Molecular Approach 4th Edition

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Ch.16 - Acids and Bases

Problem 125

Chapter 16, Problem 125

Identify the Lewis acid and Lewis base from among the reactants in each equation. a. Fe³⁺(aq) + 6 H₂O(l) ⇌ Fe(H₂O)₆³⁺(aq) b. Zn²⁺(aq) + 4 NH₃(aq) ⇌ Zn(NH₃)₄²⁺(aq) c. (CH₃)₃N(g) + BF₃(g) ⇌ (CH₃)₃NBF₃(s)

Verified step by step guidance

Identify the reactants in the equation: Fe^{3+} (aq) and H_2O (l).

Recall that a Lewis acid is a species that can accept an electron pair, while a Lewis base is a species that can donate an electron pair.

Consider the role of Fe^{3+} in the reaction. As a positively charged ion, it is likely to accept electron pairs from other species, making it a Lewis acid.

Consider the role of H_2O in the reaction. Water molecules have lone pairs of electrons that can be donated to form coordinate covalent bonds, making H_2O a Lewis base.

Conclude that in the reaction, Fe^{3+} acts as the Lewis acid and H_2O acts as the Lewis base.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 traditional Brønsted-Lowry concept of acids and bases, allowing for a broader range of chemical reactions to be analyzed. In the given reaction, identifying which species donates and which accepts electron pairs is crucial for determining the Lewis acid and base.

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, Fe3+ acts as the central metal ion, and H2O molecules serve as ligands. Understanding how these complexes form helps in identifying the roles of different species 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 a new bond, resulting in a more stable complex. Recognizing which reactant donates the electron pair is essential for correctly identifying the Lewis base in the reaction.