(a) Interpretation: Products of each possible proton transfer reaction are to be written. Concept introduction: A proton transfer reaction is the one in which a Bronsted Lowry base reacts with a Bronsted Lowry acid. A Bronsted Lowry base is a proton acceptor while a Bronsted Lowry acid is a proton donor. The proton is transferred from the acid to the base. The formal charge of the base increases by 1 and that for the acid decreases by 1. The conjugate acid is the species that the base becomes after picking up a proton, and the conjugate base is the species that the acid becomes after losing a proton. A proton transfer reaction is a concerted reaction – that is single step.

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Answer 1

Question

Chapter 6, Problem 6.83P

Interpretation Introduction

(a)

Interpretation:

Products of each possible proton transfer reaction are to be written.

Concept introduction:

A proton transfer reaction is the one in which a Bronsted Lowry base reacts with a Bronsted Lowry acid. A Bronsted Lowry base is a proton acceptor while a Bronsted Lowry acid is a proton donor. The proton is transferred from the acid to the base. The formal charge of the base increases by 1 and that for the acid decreases by 1. The conjugate acid is the species that the base becomes after picking up a proton, and the conjugate base is the species that the acid becomes after losing a proton. A proton transfer reaction is a concerted reaction – that is single step.

Interpretation Introduction

(b)

Interpretation:

Among the two possible proton transfer reactions, the reaction that is more energetically favorable is to be determined.

Concept introduction:

Proton transfer reactions favor the side opposite the stronger acid (i.e., opposite the lower pKa). When comparing two uncharged acids, the stronger acid is the one whose negatively charged conjugate base is more stable. If the conjugate base formed is more stable, then the acid will be stronger. An anion becomes more stable as the electronegativity of the atom bearing the negative charge increases. When comparing two positively charged acids, the stronger acid is the one that is less stable.

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For each reaction below, decide if the first stable organic product that forms in solution will create a new CC bond, and check the appropriate box. Next, for each reaction to which you answered "Yes" to in the table, draw this product in the drawing area below. Note for advanced students: for this problem, don't worry if you think this product will continue to react under the current conditions - just focus on the first stable product you expect to form in solution. ? NH2 MgBr Will the first product that forms in this reaction create a new CC bond? ○ Yes ○ No MgBr ? Will the first product that forms in this reaction create a new CC bond? O Yes O No Click and drag to start drawing a structure. :☐ G x c olo Ar HE

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Answer 2

Question

Chapter 6, Problem 6.83P

Interpretation Introduction

(a)

Interpretation:

Products of each possible proton transfer reaction are to be written.

Concept introduction:

A proton transfer reaction is the one in which a Bronsted Lowry base reacts with a Bronsted Lowry acid. A Bronsted Lowry base is a proton acceptor while a Bronsted Lowry acid is a proton donor. The proton is transferred from the acid to the base. The formal charge of the base increases by 1 and that for the acid decreases by 1. The conjugate acid is the species that the base becomes after picking up a proton, and the conjugate base is the species that the acid becomes after losing a proton. A proton transfer reaction is a concerted reaction – that is single step.

Interpretation Introduction

(b)

Interpretation:

Among the two possible proton transfer reactions, the reaction that is more energetically favorable is to be determined.

Concept introduction:

Proton transfer reactions favor the side opposite the stronger acid (i.e., opposite the lower pKa). When comparing two uncharged acids, the stronger acid is the one whose negatively charged conjugate base is more stable. If the conjugate base formed is more stable, then the acid will be stronger. An anion becomes more stable as the electronegativity of the atom bearing the negative charge increases. When comparing two positively charged acids, the stronger acid is the one that is less stable.

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Answer 3

Question

Chapter 6, Problem 6.83P

Interpretation Introduction

(a)

Interpretation:

Products of each possible proton transfer reaction are to be written.

Concept introduction:

A proton transfer reaction is the one in which a Bronsted Lowry base reacts with a Bronsted Lowry acid. A Bronsted Lowry base is a proton acceptor while a Bronsted Lowry acid is a proton donor. The proton is transferred from the acid to the base. The formal charge of the base increases by 1 and that for the acid decreases by 1. The conjugate acid is the species that the base becomes after picking up a proton, and the conjugate base is the species that the acid becomes after losing a proton. A proton transfer reaction is a concerted reaction – that is single step.

Interpretation Introduction

(b)

Interpretation:

Among the two possible proton transfer reactions, the reaction that is more energetically favorable is to be determined.

Concept introduction:

Proton transfer reactions favor the side opposite the stronger acid (i.e., opposite the lower pKa). When comparing two uncharged acids, the stronger acid is the one whose negatively charged conjugate base is more stable. If the conjugate base formed is more stable, then the acid will be stronger. An anion becomes more stable as the electronegativity of the atom bearing the negative charge increases. When comparing two positively charged acids, the stronger acid is the one that is less stable.

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Answer 4

Question

Chapter 6, Problem 6.83P

Interpretation Introduction

(a)

Interpretation:

Products of each possible proton transfer reaction are to be written.

Concept introduction:

A proton transfer reaction is the one in which a Bronsted Lowry base reacts with a Bronsted Lowry acid. A Bronsted Lowry base is a proton acceptor while a Bronsted Lowry acid is a proton donor. The proton is transferred from the acid to the base. The formal charge of the base increases by 1 and that for the acid decreases by 1. The conjugate acid is the species that the base becomes after picking up a proton, and the conjugate base is the species that the acid becomes after losing a proton. A proton transfer reaction is a concerted reaction – that is single step.

Interpretation Introduction

(b)

Interpretation:

Among the two possible proton transfer reactions, the reaction that is more energetically favorable is to be determined.

Concept introduction:

Proton transfer reactions favor the side opposite the stronger acid (i.e., opposite the lower pKa). When comparing two uncharged acids, the stronger acid is the one whose negatively charged conjugate base is more stable. If the conjugate base formed is more stable, then the acid will be stronger. An anion becomes more stable as the electronegativity of the atom bearing the negative charge increases. When comparing two positively charged acids, the stronger acid is the one that is less stable.

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Answer 5

Chapter 6, Problem 6.83P

Interpretation Introduction

(a)

Interpretation:

Products of each possible proton transfer reaction are to be written.

Concept introduction:

A proton transfer reaction is the one in which a Bronsted Lowry base reacts with a Bronsted Lowry acid. A Bronsted Lowry base is a proton acceptor while a Bronsted Lowry acid is a proton donor. The proton is transferred from the acid to the base. The formal charge of the base increases by 1 and that for the acid decreases by 1. The conjugate acid is the species that the base becomes after picking up a proton, and the conjugate base is the species that the acid becomes after losing a proton. A proton transfer reaction is a concerted reaction – that is single step.

Interpretation Introduction

(b)

Interpretation:

Among the two possible proton transfer reactions, the reaction that is more energetically favorable is to be determined.

Concept introduction:

Proton transfer reactions favor the side opposite the stronger acid (i.e., opposite the lower pKa). When comparing two uncharged acids, the stronger acid is the one whose negatively charged conjugate base is more stable. If the conjugate base formed is more stable, then the acid will be stronger. An anion becomes more stable as the electronegativity of the atom bearing the negative charge increases. When comparing two positively charged acids, the stronger acid is the one that is less stable.

Answer 6

Chapter 6, Problem 6.83P

Interpretation Introduction

(a)

Interpretation:

Products of each possible proton transfer reaction are to be written.

Concept introduction:

A proton transfer reaction is the one in which a Bronsted Lowry base reacts with a Bronsted Lowry acid. A Bronsted Lowry base is a proton acceptor while a Bronsted Lowry acid is a proton donor. The proton is transferred from the acid to the base. The formal charge of the base increases by 1 and that for the acid decreases by 1. The conjugate acid is the species that the base becomes after picking up a proton, and the conjugate base is the species that the acid becomes after losing a proton. A proton transfer reaction is a concerted reaction – that is single step.

Answer 7

Chapter 6, Problem 6.83P

Interpretation Introduction

(a)

Interpretation:

Products of each possible proton transfer reaction are to be written.

Concept introduction:

A proton transfer reaction is the one in which a Bronsted Lowry base reacts with a Bronsted Lowry acid. A Bronsted Lowry base is a proton acceptor while a Bronsted Lowry acid is a proton donor. The proton is transferred from the acid to the base. The formal charge of the base increases by 1 and that for the acid decreases by 1. The conjugate acid is the species that the base becomes after picking up a proton, and the conjugate base is the species that the acid becomes after losing a proton. A proton transfer reaction is a concerted reaction – that is single step.

Answer 8

Interpretation Introduction

(b)

Interpretation:

Among the two possible proton transfer reactions, the reaction that is more energetically favorable is to be determined.

Concept introduction:

Proton transfer reactions favor the side opposite the stronger acid (i.e., opposite the lower pKa). When comparing two uncharged acids, the stronger acid is the one whose negatively charged conjugate base is more stable. If the conjugate base formed is more stable, then the acid will be stronger. An anion becomes more stable as the electronegativity of the atom bearing the negative charge increases. When comparing two positively charged acids, the stronger acid is the one that is less stable.

Answer 9

Interpretation Introduction

(b)

Interpretation:

Among the two possible proton transfer reactions, the reaction that is more energetically favorable is to be determined.

Concept introduction:

Proton transfer reactions favor the side opposite the stronger acid (i.e., opposite the lower pKa). When comparing two uncharged acids, the stronger acid is the one whose negatively charged conjugate base is more stable. If the conjugate base formed is more stable, then the acid will be stronger. An anion becomes more stable as the electronegativity of the atom bearing the negative charge increases. When comparing two positively charged acids, the stronger acid is the one that is less stable.

Answer 10

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Answer 13

Ch. 6 - Prob. 6.1P Ch. 6 - Prob. 6.2P Ch. 6 - Prob. 6.3P Ch. 6 - Prob. 6.4P Ch. 6 - Prob. 6.5P Ch. 6 - Prob. 6.6P Ch. 6 - Prob. 6.7P Ch. 6 - Prob. 6.8P Ch. 6 - Prob. 6.9P Ch. 6 - Prob. 6.10P

Solution Summary: The author explains that proton transfer reactions favor the side opposite the stronger acid.

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