Identify the Lewis acid and Lewis base in each of the following reactions: (a) HNO 2 (aq) + OH - (aq) ⇌ NO 2 - (aq) + H 2 O(l) (b) FeBr 3 (s) + Br - (aq) ⇌ FeBr 4 - (aq) (c) Zn 2+ (aq) + 4 NH 3 (aq) ⇌ Zn(NH 3 ) 4 2+ (aq) (d) SO 2 (g) + H 2 O(l) ⇌ H 2 SO 3 (aq)

Hello. Everyone in this video we're trying to find the lewis acid and lewis base for this following reaction. And it's asking about the reactant only but that's going to be our starting materials on the left side of our arrow. So here let's go ahead and remind ourselves what the lewis acid and lewis based definition is. So just really simply our lewis acids are going to be our electron pair receptors and then our lewis base then is going to be our electron pair donors. Alright, of course these two, even though they are true, we also need to make sure that it does not break octet. So no breaking octet. All right. So we can go ahead and draw out the lewis dot structure if you want to go ahead and see it more clearly. But we can also use our knowledge to go ahead and find our lewis acid or louis space very quickly. So if we have a Lewis base and the definition is that it's an electron pair donor. Of course it has to be very electron dense in our reaction here we see a neutral molecule and this an island and I can have a negative charge. It means it's very electron dense. In that case it has electrons to give. So let's write that down. So it's very electron dense. So it has electrons to donate. So it's an electron pair donor. And that fits the very definition of our Lewis base. So if this line right here is a louis space than the only other reactant is going to be our acid. So then our final answer is that our lewis acid, It's going to be COCL two and our louis base, it's going to be c L minus. So this right here is going to be my final answer for this problem. Thank you all so much for watching.

Ch.16 - Acid-Base Equilibria

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Brown 14th Edition

Ch.16 - Acid-Base Equilibria

Problem 96

Chapter 16, Problem 96

Identify the Lewis acid and Lewis base in each of the following reactions:
(a) HNO₂(aq) + OH^-(aq) ⇌ NO₂^-(aq) + H₂O(l)
(b) FeBr₃(s) + Br^-(aq) ⇌ FeBr₄^-(aq)
(c) Zn²⁺(aq) + 4 NH₃(aq) ⇌ Zn(NH₃)₄²⁺(aq)
(d) SO₂(g) + H₂O(l) ⇌ H₂SO₃(aq)

Verified step by step guidance

Identify the species involved in the reaction: FeBr3(s) and Br^-(aq).

Recall the definition of a Lewis acid: a species that can accept an electron pair.

Recall the definition of a Lewis base: a species that can donate an electron pair.

Determine which species is accepting an electron pair: FeBr3 is accepting an electron pair from Br^- to form FeBr4^-.

Determine which species is donating an electron pair: Br^- is donating an electron pair to FeBr3, making Br^- 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 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.