Chapter 1, Problem 51P

(a)

Interpretation Introduction

Interpretation:

The direction of the dipole moment in ${\text{CH}}_{\text{3}}\text{-Br}$ bond should be shown.

Concept introduction:

Polar molecule: It has net dipole as a result of the opposing charges.

For example:  A molecule has partially positive charge and partially negative charge. It has slight positive charge on one side and a slight negative charge on the other side.  

Electronegativity:

It’s a tendency of an atom to attract bond pair of electron of a molecule towards itself.

Fluorine has the highest electronegative value.

i.e. 4.

The Cesium and Francium has the least electronegative value .i.e. 0.7

Dipole moment:

Dipole moment occurs when there is a separation of charge.

Dipole moment arises due to difference in electronegativity.

The larger the difference of electronegativity, larger is the dipole moment.

The dipole moment is the measure of the polarity of the molecule.

$\text{Dipole moment of a bond = size of the charge × the distance between the charges}$

Dipole moment can be denoted by the Unit called Debye (D) only.

(b)

Interpretation Introduction

Interpretation:

The direction of the dipole moment in ${\text{CH}}_{\text{3}}\text{-Li}$ bonds should be shown.

Concept introduction:

Polar molecule: It has net dipole as a result of the opposing charges.

For example:  A molecule has partially positive charge and partially negative charge. It has slight positive charge on one side and a slight negative charge on the other side.  

Electronegativity:

It’s a tendency of an atom to attract bond pair of electron of a molecule towards itself.

Fluorine has the highest electronegative value.

i.e. 4.

The Cesium and Francium has the least electronegative value .i.e. 0.7

Dipole moment:

Dipole moment occurs when there is a separation of charge.

Dipole moment arises due to difference in electronegativity.

The larger the difference of electronegativity, larger is the dipole moment.

The dipole moment is the measure of the polarity of the molecule.

$\text{Dipole moment of a bond = size of the charge × the distance between the charges}$

Dipole moment can be denoted by the Unit called Debye (D) only.

(c)

Interpretation Introduction

Interpretation:

The direction of the dipole moment in ${\text{OH-NH}}_2$ bonds should be shown.

Concept introduction:

Polar molecule: It has net dipole as a result of the opposing charges.

For example:  A molecule has partially positive charge and partially negative charge. It has slight positive charge on one side and a slight negative charge on the other side.  

Electronegativity:

It’s a tendency of an atom to attract bond pair of electron of a molecule towards itself.

Fluorine has the highest electronegative value.

i.e. 4.

The Cesium and Francium has the least electronegative value .i.e. 0.7

Dipole moment:

Dipole moment occurs when there is a separation of charge.

Dipole moment arises due to difference in electronegativity.

The larger the difference of electronegativity, larger is the dipole moment.

The dipole moment is the measure of the polarity of the molecule.

$\text{Dipole moment of a bond = size of the charge × the distance between the charges}$

Dipole moment can be denoted by the Unit called Debye (D) only.

(d)

Interpretation Introduction

Interpretation:

The direction of the dipole moment in $\text{I-Br}$ bonds should be shown.

Concept introduction:

Polar molecule: It has net dipole as a result of the opposing charges.

For example:  A molecule has partially positive charge and partially negative charge. It has slight positive charge on one side and a slight negative charge on the other side.  

Electronegativity:

It’s a tendency of an atom to attract bond pair of electron of a molecule towards itself.

Fluorine has the highest electronegative value.

i.e. 4.

The Cesium and Francium has the least electronegative value .i.e. 0.7

Dipole moment:

Dipole moment occurs when there is a separation of charge.

Dipole moment arises due to difference in electronegativity.

The larger the difference of electronegativity, larger is the dipole moment.

The dipole moment is the measure of the polarity of the molecule.

$\text{Dipole moment of a bond = size of the charge × the distance between the charges}$

Dipole moment can be denoted by the Unit called Debye (D) only.

(e)

Interpretation Introduction

Interpretation:

The direction of the dipole moment in ${\text{CH}}_3\text{-OH }$ bonds should be shown.

Concept introduction:

Polar molecule: It has net dipole as a result of the opposing charges.

For example:  A molecule has partially positive charge and partially negative charge. It has slight positive charge on one side and a slight negative charge on the other side.  

Electronegativity:

It’s a tendency of an atom to attract bond pair of electron of a molecule towards itself.

Fluorine has the highest electronegative value.

i.e. 4.

The Cesium and Francium has the least electronegative value .i.e. 0.7

Dipole moment:

Dipole moment occurs when there is a separation of charge.

Dipole moment arises due to difference in electronegativity.

The larger the difference of electronegativity, larger is the dipole moment.

The dipole moment is the measure of the polarity of the molecule.

$\text{Dipole moment of a bond = size of the charge × the distance between the charges}$

Dipole moment can be denoted by the Unit called Debye (D) only.

(f)

Interpretation Introduction

Interpretation:

The direction of the dipole moment in ${{\text{(CH}}_3\text{)}}_2\text{-NH}$ bonds should be shown.

Concept introduction:

Polar molecule: It has net dipole as a result of the opposing charges.

For example:  A molecule has partially positive charge and partially negative charge. It has slight positive charge on one side and a slight negative charge on the other side.  

Electronegativity:

It’s a tendency of an atom to attract bond pair of electron of a molecule towards itself.

Fluorine has the highest electronegative value.

i.e. 4.

The Cesium and Francium has the least electronegative value .i.e. 0.7

Dipole moment:

Dipole moment occurs when there is a separation of charge.

Dipole moment arises due to difference in electronegativity.

The larger the difference of electronegativity, larger is the dipole moment.

The dipole moment is the measure of the polarity of the molecule.

$\text{Dipole moment of a bond = size of the charge × the distance between the charges}$

Dipole moment can be denoted by the Unit called Debye (D) only.