(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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Will NBS (and heat or light) work for this reaction, or do we have to use Br2?

HAND DRAW

Predict the major products of the following organic reaction: Some important notes: Δ CN ? • Draw the major product, or products, of the reaction in the drawing area below. • If there aren't any products, because no reaction will take place, check the box below the drawing area instead. Be sure to use wedge and dash bonds when necessary, for example to distinguish between major products that are enantiomers. ONO reaction. Click and drag to start drawing a structure.

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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