Chapter 10, Problem 10.49P

Interpretation Introduction

(a)

Interpretation:

The most polar bond of methanol should be identified and polarity described with symbols $\delta -$ and $\delta +$

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 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.

Explanation of Solution

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

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.

Interpretation Introduction

(b)

Interpretation:

The most polar bond of methylamine should be identified and polarity described with symbols $\delta -$ and $\delta +$

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 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.

Explanation of Solution

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

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.

Interpretation Introduction

(c)

Interpretation:

The most polar bond of 2-aminoethathiol should be identified and polarity described with symbols $\delta -$ and $\delta +$

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 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.

Explanation of Solution

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

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.

Interpretation Introduction

(d)

Interpretation:

The most polar bond of acetone should be identified and polarity described with symbols $\delta -$ and $\delta +$

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 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.

Explanation of Solution

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

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.

Interpretation Introduction

(e)

Interpretation:

The most polar bond of formaldehyde should be identified and polarity described with symbols $\delta -$ and $\delta +$

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 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.

Explanation of Solution

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

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.

Interpretation Introduction

(f)

Interpretation:

The most polar bond of acetic acid should be identified and polarity described with symbols $\delta -$ and $\delta +$

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 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.

Explanation of Solution

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

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.