Chapter 2.4, Problem 13CC

(a)

Interpretation Introduction

Interpretation:

The formal charges on Oxygen atom has to be determined.

Concept Introduction:

Lone pair:

A lone pair is given by a pair of outer most electrons that are not shared with another atom, otherwise called as non-bonding pair. These are generally found in the valence shell of atom and are identified by Lewis structure. Pairs of electrons are considered as lone pairs when two electrons are paired and are not participated in chemical bonding. The sum of number of lone pairs and number of bonding electrons equals the total number of outermost electrons around an atom.

Delocalized lone pair:

The lone pair that participates in resonance is called as delocalized lone pair. The presence of lone pair affects the geometry of the atom.

Localized lone pair:

The lone pair that doesn’t participate in the resonance is called localized lone pair. The lone pair is not allylic to $\text{π}$ bond.

(b)

Interpretation Introduction

Interpretation:

The formal charges on Oxygen atom has to be determined.

Concept Introduction:

Lone pair:

A lone pair is given by a pair of outer most electrons that are not shared with another atom, otherwise called as non bonding pair. These are generally found in the valence shell of atom and are identified by Lewis structure. Pairs of electrons are considered as lone pairs when two electrons are paired and are not participated in chemical bonding. The sum of number of lone pairs and number of bonding electrons equals the total number of outermost electrons around an atom.

Delocalized lone pair:

The lone pair that participates in resonance is called as delocalized lone pair. The presence of lone pair affects the geometry of the atom.

Localized lone pair:

The lone pair that doesn’t participate in the resonance is called localized lone pair. The lone pair is not allylic to $\text{π}$ bond.

(c)

Interpretation Introduction

Interpretation:

The formal charges on Oxygen atom has to be determined.

Concept Introduction:

Lone pair:

A lone pair is given by a pair of outer most electrons that are not shared with another atom, otherwise called as non bonding pair. These are generally found in the valence shell of atom and are identified by Lewis structure. Pairs of electrons are considered as lone pairs when two electrons are paired and are not participated in chemical bonding. The sum of number of lone pairs and number of bonding electrons equals the total number of outermost electrons around an atom.

Delocalized lone pair:

The lone pair that participates in resonance is called as delocalized lone pair. The presence of lone pair affects the geometry of the atom.

Localized lone pair:

The lone pair that doesn’t participate in the resonance is called localized lone pair. The lone pair is not allylic to $\text{π}$ bond.

(d)

Interpretation Introduction

Interpretation:

The formal charges on Oxygen atom has to be determined.

Concept Introduction:

Lone pair:

A lone pair is given by a pair of outer most electrons that are not shared with another atom, otherwise called as non bonding pair. These are generally found in the valence shell of atom and are identified by Lewis structure. Pairs of electrons are considered as lone pairs when two electrons are paired and are not participated in chemical bonding. The sum of number of lone pairs and number of bonding electrons equals the total number of outermost electrons around an atom.

Delocalized lone pair:

The lone pair that participates in resonance is called as delocalized lone pair. The presence of lone pair affects the geometry of the atom.

Localized lone pair:

The lone pair that doesn’t participate in the resonance is called localized lone pair. The lone pair is not allylic to $\text{π}$ bond.