(a) Interpretation: The most polar bond of methanol should be identified and polarity described with symbols δ − and δ + Concept Introduction: Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

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Answer 1

Question

Chapter 10, Problem 10.49P

Interpretation Introduction

(a)

Interpretation:

The most polar bond of methanol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methanol, most polar bond is O-H bond with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 1

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methanol, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-O bond have 1.0 electronegativity but it is less polar when compare to O-H bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 2

Interpretation Introduction

(b)

Interpretation:

The most polar bond of methylamine should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methylamine, most polar bond is N-H bond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 3

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methylamine, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-H bond is nonpolar because of electronegativity of 0.4 only.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 4

Interpretation Introduction

(c)

Interpretation:

The most polar bond of 2-aminoethathiol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In 2-aminoethathiol, most polar bond is N-Hbond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 5

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In 2-aminoethanethiol, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The bonds S-H, C-C and C-H have electronegativity difference are 0.4, 0, and 0.4 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 6

Interpretation Introduction

(d)

Interpretation:

The most polar bond of acetone should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 7

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

Other bonds present in acetone are C-H and C-C with electronegativity of 0.4 and 0 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 8

Interpretation Introduction

(e)

Interpretation:

The most polar bond of formaldehyde should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 9

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

The bond C-H has electronegativity difference of 0.4 and it is a nonpolar bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 10

Interpretation Introduction

(f)

Interpretation:

The most polar bond of acetic acid should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 11

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The other bonds are C-C, C=O and C-H with electronegativity of 0, 1.0 and 0.4 but bond O-H has more electronegativity as compared to other bonds.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 12

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Answer 2

Question

Chapter 10, Problem 10.49P

Interpretation Introduction

(a)

Interpretation:

The most polar bond of methanol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methanol, most polar bond is O-H bond with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 1

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methanol, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-O bond have 1.0 electronegativity but it is less polar when compare to O-H bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 2

Interpretation Introduction

(b)

Interpretation:

The most polar bond of methylamine should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methylamine, most polar bond is N-H bond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 3

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methylamine, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-H bond is nonpolar because of electronegativity of 0.4 only.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 4

Interpretation Introduction

(c)

Interpretation:

The most polar bond of 2-aminoethathiol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In 2-aminoethathiol, most polar bond is N-Hbond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 5

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In 2-aminoethanethiol, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The bonds S-H, C-C and C-H have electronegativity difference are 0.4, 0, and 0.4 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 6

Interpretation Introduction

(d)

Interpretation:

The most polar bond of acetone should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 7

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

Other bonds present in acetone are C-H and C-C with electronegativity of 0.4 and 0 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 8

Interpretation Introduction

(e)

Interpretation:

The most polar bond of formaldehyde should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 9

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

The bond C-H has electronegativity difference of 0.4 and it is a nonpolar bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 10

Interpretation Introduction

(f)

Interpretation:

The most polar bond of acetic acid should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 11

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The other bonds are C-C, C=O and C-H with electronegativity of 0, 1.0 and 0.4 but bond O-H has more electronegativity as compared to other bonds.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 12

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Answer 3

Question

Chapter 10, Problem 10.49P

Interpretation Introduction

(a)

Interpretation:

The most polar bond of methanol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methanol, most polar bond is O-H bond with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 1

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methanol, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-O bond have 1.0 electronegativity but it is less polar when compare to O-H bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 2

Interpretation Introduction

(b)

Interpretation:

The most polar bond of methylamine should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methylamine, most polar bond is N-H bond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 3

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methylamine, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-H bond is nonpolar because of electronegativity of 0.4 only.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 4

Interpretation Introduction

(c)

Interpretation:

The most polar bond of 2-aminoethathiol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In 2-aminoethathiol, most polar bond is N-Hbond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 5

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In 2-aminoethanethiol, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The bonds S-H, C-C and C-H have electronegativity difference are 0.4, 0, and 0.4 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 6

Interpretation Introduction

(d)

Interpretation:

The most polar bond of acetone should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 7

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

Other bonds present in acetone are C-H and C-C with electronegativity of 0.4 and 0 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 8

Interpretation Introduction

(e)

Interpretation:

The most polar bond of formaldehyde should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 9

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

The bond C-H has electronegativity difference of 0.4 and it is a nonpolar bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 10

Interpretation Introduction

(f)

Interpretation:

The most polar bond of acetic acid should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 11

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The other bonds are C-C, C=O and C-H with electronegativity of 0, 1.0 and 0.4 but bond O-H has more electronegativity as compared to other bonds.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 12

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Answer 4

Question

Chapter 10, Problem 10.49P

Interpretation Introduction

(a)

Interpretation:

The most polar bond of methanol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methanol, most polar bond is O-H bond with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 1

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methanol, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-O bond have 1.0 electronegativity but it is less polar when compare to O-H bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 2

Interpretation Introduction

(b)

Interpretation:

The most polar bond of methylamine should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methylamine, most polar bond is N-H bond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 3

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methylamine, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-H bond is nonpolar because of electronegativity of 0.4 only.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 4

Interpretation Introduction

(c)

Interpretation:

The most polar bond of 2-aminoethathiol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In 2-aminoethathiol, most polar bond is N-Hbond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 5

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In 2-aminoethanethiol, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The bonds S-H, C-C and C-H have electronegativity difference are 0.4, 0, and 0.4 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 6

Interpretation Introduction

(d)

Interpretation:

The most polar bond of acetone should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 7

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

Other bonds present in acetone are C-H and C-C with electronegativity of 0.4 and 0 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 8

Interpretation Introduction

(e)

Interpretation:

The most polar bond of formaldehyde should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 9

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

The bond C-H has electronegativity difference of 0.4 and it is a nonpolar bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 10

Interpretation Introduction

(f)

Interpretation:

The most polar bond of acetic acid should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 11

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The other bonds are C-C, C=O and C-H with electronegativity of 0, 1.0 and 0.4 but bond O-H has more electronegativity as compared to other bonds.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 12

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Answer 5

Chapter 10, Problem 10.49P

Interpretation Introduction

(a)

Interpretation:

The most polar bond of methanol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methanol, most polar bond is O-H bond with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 1

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methanol, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-O bond have 1.0 electronegativity but it is less polar when compare to O-H bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 2

Interpretation Introduction

(b)

Interpretation:

The most polar bond of methylamine should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methylamine, most polar bond is N-H bond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 3

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methylamine, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-H bond is nonpolar because of electronegativity of 0.4 only.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 4

Interpretation Introduction

(c)

Interpretation:

The most polar bond of 2-aminoethathiol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In 2-aminoethathiol, most polar bond is N-Hbond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 5

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In 2-aminoethanethiol, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The bonds S-H, C-C and C-H have electronegativity difference are 0.4, 0, and 0.4 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 6

Interpretation Introduction

(d)

Interpretation:

The most polar bond of acetone should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 7

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

Other bonds present in acetone are C-H and C-C with electronegativity of 0.4 and 0 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 8

Interpretation Introduction

(e)

Interpretation:

The most polar bond of formaldehyde should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 9

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

The bond C-H has electronegativity difference of 0.4 and it is a nonpolar bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 10

Interpretation Introduction

(f)

Interpretation:

The most polar bond of acetic acid should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 11

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The other bonds are C-C, C=O and C-H with electronegativity of 0, 1.0 and 0.4 but bond O-H has more electronegativity as compared to other bonds.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 12

Answer 6

Chapter 10, Problem 10.49P

Interpretation Introduction

(a)

Interpretation:

The most polar bond of methanol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methanol, most polar bond is O-H bond with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 1

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methanol, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-O bond have 1.0 electronegativity but it is less polar when compare to O-H bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 2

Answer 7

Chapter 10, Problem 10.49P

Interpretation Introduction

(a)

Interpretation:

The most polar bond of methanol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Answer 8

Expert Solution

Answer to Problem 10.49P

In methanol, most polar bond is O-H bond with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 1

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methanol, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-O bond have 1.0 electronegativity but it is less polar when compare to O-H bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 2

Answer 13

Interpretation Introduction

(b)

Interpretation:

The most polar bond of methylamine should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In methylamine, most polar bond is N-H bond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 3

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methylamine, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-H bond is nonpolar because of electronegativity of 0.4 only.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 4

Answer 14

Interpretation Introduction

(b)

Interpretation:

The most polar bond of methylamine should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Answer 15

Expert Solution

Answer to Problem 10.49P

In methylamine, most polar bond is N-H bond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 3

Answer 16

Expert Solution

Answer 17

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In methylamine, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

C-H bond is nonpolar because of electronegativity of 0.4 only.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 4

Answer 20

Interpretation Introduction

(c)

Interpretation:

The most polar bond of 2-aminoethathiol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In 2-aminoethathiol, most polar bond is N-Hbond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 5

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In 2-aminoethanethiol, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The bonds S-H, C-C and C-H have electronegativity difference are 0.4, 0, and 0.4 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 6

Answer 21

Interpretation Introduction

(c)

Interpretation:

The most polar bond of 2-aminoethathiol should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Answer 22

Expert Solution

Answer to Problem 10.49P

In 2-aminoethathiol, most polar bond is N-Hbond with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 5

Answer 23

Expert Solution

Answer 24

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In 2-aminoethanethiol, most polar bond is N-H with electronegativity difference of 0.9 and nitrogen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The bonds S-H, C-C and C-H have electronegativity difference are 0.4, 0, and 0.4 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 6

Answer 27

Interpretation Introduction

(d)

Interpretation:

The most polar bond of acetone should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 7

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

Other bonds present in acetone are C-H and C-C with electronegativity of 0.4 and 0 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 8

Answer 28

Interpretation Introduction

(d)

Interpretation:

The most polar bond of acetone should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Answer 29

Expert Solution

Answer to Problem 10.49P

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 7

Answer 30

Expert Solution

Answer 31

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetone, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

Other bonds present in acetone are C-H and C-C with electronegativity of 0.4 and 0 respectively.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 8

Answer 34

Interpretation Introduction

(e)

Interpretation:

The most polar bond of formaldehyde should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 9

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

The bond C-H has electronegativity difference of 0.4 and it is a nonpolar bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 10

Answer 35

Interpretation Introduction

(e)

Interpretation:

The most polar bond of formaldehyde should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Answer 36

Expert Solution

Answer to Problem 10.49P

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 9

Answer 37

Expert Solution

Answer 38

Expert Solution

Answer 39

Expert Solution

Answer 40

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In formaldehyde, most polar bond is C=O with electronegativity difference of 1.0 and oxygen atom becomes partial negative charge atom whereas carbon becomes partial positive charge atom.

The bond C-H has electronegativity difference of 0.4 and it is a nonpolar bond.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 10

Answer 41

Interpretation Introduction

(f)

Interpretation:

The most polar bond of acetic acid should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Expert Solution

Answer to Problem 10.49P

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 11

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The other bonds are C-C, C=O and C-H with electronegativity of 0, 1.0 and 0.4 but bond O-H has more electronegativity as compared to other bonds.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 12

Answer 42

Interpretation Introduction

(f)

Interpretation:

The most polar bond of acetic acid should be identified and polarity described with symbols δ− and δ+

Concept Introduction:

Polarity of any molecule depends on electronegativity of atoms that forms covalent bonds. Depending upon the difference in electronegativity of atoms, polar or nonpolar molecule is determined. Polar molecule has electronegativity between 0.5 and 1.4 whereas in nonpolar molecule, it is less than 0.5.

Answer 43

Expert Solution

Answer to Problem 10.49P

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 11

Answer 44

Expert Solution

Answer 45

Expert Solution

Answer 46

Expert Solution

Answer 47

Explanation of Solution

Polar covalent bonds contains more atoms with high electronegativity and acquire more partial negative charge represented as delta minus δ− and atoms with less electronegativity gets partial positive charge represented as delta plus δ+

In acetic acid, most polar bond is O-H with electronegativity difference of 1.4 and oxygen atom becomes partial negative charge atom whereas hydrogen becomes partial positive charge atom.

The other bonds are C-C, C=O and C-H with electronegativity of 0, 1.0 and 0.4 but bond O-H has more electronegativity as compared to other bonds.

OWLv2 for Bettelheim/Brown/Campbell/Farrell/Torres' Introduction to General, Organic and Biochemistry, 11th Edition, [Instant Access], 1 term (6 months), Chapter 10, Problem 10.49P , additional homework tip 12