Chapter 1, Problem 74CP

(a)

Interpretation Introduction

Interpretation:

To identify the formal charges that are missing from structure 1 and 2.  To determine which of the two compound will be more soluble in polar solvent.  To determine the amount of increase in bond angle $\text{C-C-N}$ when 1 is converted to 2.

Concept introduction:

Formal charge on a atom is the charge that is associated with the atom that does not have appropriate number of valence electrons.  To find the formal charge on an atom in a compound the total number of valence electrons of the atom must be known.

To identify: To identify whether the two given compounds possess any formal charge.

(b)

Interpretation Introduction

Interpretation:

To identify the formal charges that are missing from structure 1 and 2.  To determine which of the two compound will be more soluble in polar solvent.  To determine the amount of increase in bond angle $\text{C-C-N}$ when 1 is converted to 2.

Concept introduction:

Formal charge on a atom is the charge that is associated with the atom that does not have appropriate number of valence electrons.  To find the formal charge on an atom in a compound the total number of valence electrons of the atom must be known.

(c)

Interpretation Introduction

Interpretation:

To identify the formal charges that are missing from structure 1 and 2.  To determine which of the two compound will be more soluble in polar solvent.  To determine the amount of increase in bond angle $\text{C-C-N}$ when 1 is converted to 2.

Concept introduction:

The atomic orbitals mix together to form a hybrid orbital which is suitable for forming bonds between the atoms to form a compound.  This mixing of hybrid orbitals is known as hybridization.  The hybridization determines the geometry of the particular atom in the compound.  Shortly to say

$s{p}^{3}hybridized$ =tetrahedral

trigonal pyramidal(if one lone pair of electron is present)

bent geometry (if two lone pair of electrons are present)

$s{p}^{2}hybridized$ =trigonal planar

$sp$ $hybridized$ =linear

Each and every hybridized orbital has its own bond angle,

$s{p}^{3}hybridized$ = $109.5°$

$s{p}^{2}hybridized$ = $120°$

$sp$ $hybridized$ = $180°$