Chapter 7, Problem 7.110MP

Interpretation Introduction

(a)

Interpretation:

The formula of compound A is to be determined that is formed by the reaction of sulfur with ammonia and contains 69.6 % by mass S and 30.4% by mass with a molar mass of 184.3 g.

Concept introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom.

Lewis dot structure is also known as Lewis dot formula or electron dot structure. The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

$\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Interpretation Introduction

(b)

Interpretation:

The possible electron dot structures of compound A with molecular formula ${\text{S}}_{\text{4}}{\text{N}}_{\text{4}}$ in which S and N are bonded in an alternate way in a ring structure with half of the atoms having some formal charge are to be determined.

Concept introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom.

Lewis dot structure is also known as Lewis dot formula or electron dot structure. The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

$\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Interpretation Introduction

(c)

Interpretation:

Two possible electron dot structures of compound Bare to be determined which are formed when the compound A; ${\text{S}}_{\text{4}}{\text{N}}_{\text{4}}$ is heated with metallic silver at 250^o C. The product B has the same percent composition as A; ${\text{S}}_{\text{4}}{\text{N}}_{\text{4}}$ with molar mass 92.2 g.

Concept introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom.

Lewis dot structure is also known as Lewis dot formula or electron dot structure. The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Formal charge on each atom can be determined with the help of a number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

$\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$