Identify the Lewis acids and bases in the following reactions.a) H+ + OH– ⇌ H2Ob) Cl– + BCl3 ⇋ BCl4–c) SO3 + H2O ⇌ H2SO4

a) H + :acid, OH - :base; b) Cl - :base, BCl 3 :acid; c)SO 3 :acid, H 2 O:base

Identify the Lewis acids and bases in the following reactions. a) H + + OH – ⇌ H 2 O b) Cl – + BCl 3 ⇋ BCl 4 – c) SO 3 + H 2 O ⇌ H 2 SO 4

Hey, guys, we're not gonna attempt to do the practice question that was left on the bottom of the page. So here, the question says, identify the Lewis acids and bases in the following reactions. If we take a look at the first one, we have a positive hydrogen there with a negative Ohh! Again. Remember, if you're positive or partially positive, you're going to attract electrons, which are negatively charged. So this would be our acid. The O. H. Has a negative charge. Negative charges implying that you have lone pairs available to share. So O H minus would be our base. And again they combined together. Since we're adding them together, H 20 is our ad ukt. For the next one, we have again, uh, compound with the negative charge, which means that it has lone pairs available to share, So this would be our base. Here we have boron, which is a Group three element connected to three Corinne's. So it has less than eight electrons around it, so it's gonna be our acid. The last one was tricky because here we have s 03 and here we have Htoo now, Really, This required a little bit of skills in terms of drawing. If you wanted to see what s 03 looks like it would look like this, the sulfur there would be positively charged. That's tricky. Most students would know how to draw that, but then again, you know that water the oxygen has lone pairs. Water is a basic kind, the most simplest kind of Louis space that exists out there. If you see water, it's most likely going to behave as a Lewis base. And if that's the base and sulfur here has a positive charge, then it's going to be the acid. So again, the last one was tricky. But if you could remember that water acts as a Louis space because of the lone pairs on oxygen, and that would have helped you figure out what to do for this question here, and we'll realize here that later on when we talk about this more now we have water, and here we have eso three, which is a Covalin compound. So we're gonna say here that this non metal oxide we say that this is called a non metal oxide because it's a non metal with oxygen. When it combines with water. It gives us an acid, and this acid is called an oxy acid. So to make oxy acids, which is a type of acid, we use water and a non metal oxide. Another common example. You could have co two plus water, which would give me H two c l three. So hopefully you were able to get the first to the third one was a little bit tricky, so just remember, water normally asked acts as a Lewis base here.

Identify the Lewis acids and bases in the following reactions. a) H + + OH – ⇌ H 2 O b) Cl – + BCl 3 ⇋ BCl 4 – c) SO 3 + H 2 O ⇌ H 2 SO 4

a) H + :acid, OH - :base; b) Cl - :base, BCl 3 :acid; c)SO 3 :acid, H 2 O:base

a) H + :acid, OH - :base; b) Cl - :acid, BCl 3 :base; c)SO 3 :acid, H 2 O:base

a) H + :base, OH - :acid; b) Cl - :acid, BCl 3 :base; c)SO 3 :base, H 2 O:acid

a) H + :acid, OH - :base; b) Cl - :base, BCl 3 :acid; c)SO 3 :base, H 2 O:acid

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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
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13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

17. Acid and Base Equilibrium

Lewis Acids and Bases

General Chemistry

17. Acid and Base Equilibrium

Lewis Acids and Bases

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Multiple Choice

Identify the Lewis acids and bases in the following reactions.
a) H⁺ + OH^– ⇌ H₂O
b) Cl^– + BCl₃ ⇋ BCl₄^–
c) SO₃ + H₂O ⇌ H₂SO₄

a) H⁺:acid, OH^-:base; b) Cl^-:acid, BCl₃:base; c)SO₃:acid, H₂O:base

a) H⁺:base, OH^-:acid; b) Cl^-:acid, BCl₃:base; c)SO₃:base, H₂O:acid

a) H⁺:acid, OH^-:base; b) Cl^-:base, BCl₃:acid; c)SO₃:acid, H₂O:base

a) H⁺:acid, OH^-:base; b) Cl^-:base, BCl₃:acid; c)SO₃:base, H₂O:acid

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Verified step by step guidance

Step 1: Understand the concept of Lewis acids and bases. A Lewis acid is a substance that can accept a pair of electrons, while a Lewis base is a substance that can donate a pair of electrons.

Step 2: Analyze reaction (a) H+ + OH– ⇌ H2O. Here, H+ is a proton that can accept a pair of electrons from OH–, making H+ the Lewis acid and OH– the Lewis base.

Step 3: Analyze reaction (b) Cl– + BCl3 ⇋ BCl4–. In this reaction, BCl3 has an empty orbital and can accept a pair of electrons from Cl–, making BCl3 the Lewis acid and Cl– the Lewis base.

Step 4: Analyze reaction (c) SO3 + H2O ⇌ H2SO4. SO3 can accept a pair of electrons from H2O to form H2SO4, making SO3 the Lewis acid and H2O the Lewis base.

Step 5: Review the correct identifications: a) H+ is the acid, OH– is the base; b) Cl– is the base, BCl3 is the acid; c) SO3 is the acid, H2O is the base.