Identify the Lewis acid and Lewis base among the reactants in each of the following reactions: (a) Fe(ClO 4 ) 3 (s) + 6 H 2 O(l) ⇌ [Fe(H 2 O) 6 ] 3+ (aq) + 3 ClO 4 - (aq) (b) CN - (aq) + H 2 O(l) ⇌ HCN(aq) + OH - (aq) (c) (CH 3 ) 3 N(g) + BF 3 (g) ⇌ (CH 3 )NBF 3 (s) (d) HIO(lq) + NH 2 - (lq) ⇌ NH 3 (lq) + IO - (lq) (lq denotes liquid ammonia as solvent)

Hello everyone. So in this video we're looking at this reaction right here and we're trying to identify the lewis acid and Lewis base among the reactant. So that's going to be our starting materials on the left side of our equilibrium era. Alright, so let's go ahead and refresh our memory of what a lewis acid and lewis bases. So by definition our lewis acid is going to be our electron paris sectors. As for our louis space, that's going to be our electron pair donors. So we can go ahead and draw out the lewis dot structure to clearly see it visually. However, we can also use our knowledge given the definitions and just background of chemistry to go ahead and find our lewis acid and Lewis space. So we can see here that we have our H B R and we have our p H two minus. So one thing that I recognize really quickly is our Hbr that's one of our known six strong acids. And of course that means this has to be our lewis acid. But let's say I don't have that list memorized and I want to go ahead and look at this one right here. It's the only one with the charge we have a neutral molecule and a negatively charged molecule. If we have this negative here, this means that this is going to be very electron dance. It's gonna go wanna go ahead and give up some of his electrons. This just means that it will donate or share electrons never donate electrons. That fits our very definition of a Lewis base. And just by default, then the other, the only other reactant is going to be our acid because we have to have a lewis acid and louis space. Right, So here is our Lewis base. Here is our Lewis acid. And to write this more formally, Our final answer is that our Lewis acid, it's going to be our h b R and the Lewis space. It's going to be our PH two negative. And this, right here is going to be my final answer for this problem.

Ch.16 - Acid-Base Equilibria

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Brown 14th Edition

Ch.16 - Acid-Base Equilibria

Problem 95

Chapter 16, Problem 95

Identify the Lewis acid and Lewis base among the reactants in each of the following reactions:
(a) Fe(ClO₄)₃(s) + 6 H₂O(l) ⇌ [Fe(H₂O)₆]³⁺(aq) + 3 ClO₄^-(aq)
(b) CN^-(aq) + H₂O(l) ⇌ HCN(aq) + OH^-(aq)
(c) (CH₃)₃N(g) + BF₃(g) ⇌ (CH₃)NBF₃(s)
(d) HIO(lq) + NH₂^-(lq) ⇌ NH₃(lq) + IO^-(lq) (lq denotes liquid ammonia as solvent)

Verified step by step guidance

Identify the Lewis acid and Lewis base by understanding their definitions: A Lewis acid is an electron pair acceptor, and a Lewis base is an electron pair donor.

Examine the reactants: HIO and NH2-. Consider which species can donate an electron pair and which can accept an electron pair.

Recognize that NH2- has a lone pair of electrons that it can donate, making it a potential Lewis base.

Consider HIO, which can accept an electron pair to form a bond, making it a potential Lewis acid.

Conclude that in the reaction, NH2- acts as the Lewis base (electron pair donor) and HIO acts as the Lewis acid (electron pair acceptor).

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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 concept of acids and bases beyond protons (H+) to include electron pair interactions, making it applicable to a wider range of chemical reactions.

Electron Pair Donation and Acceptance

In a Lewis acid-base reaction, the Lewis base donates an electron pair to the Lewis acid, forming a coordinate covalent bond. Understanding this interaction is crucial for identifying which reactant acts as the acid and which as the base in a given reaction.

Solvent Effects

The solvent can influence the behavior of acids and bases in a reaction. In this case, liquid ammonia serves as a solvent, which can stabilize certain ions and affect the reactivity of the reactants, thereby impacting the identification of Lewis acids and bases in the reaction.