Chapter 3, Problem 96AP

(a)

Interpretation Introduction

Interpretation: The Lewis structure of ${\text{BeCl}}_{\text{2}}$ in which all atoms have octet configuration needs to be drawn and formal charge to all bonded atoms needs to be assigned.

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 existing 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. The formula for the formal charge can be written as:

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

(b)

Interpretation Introduction

Interpretation: The correct Lewis structures of ${\text{BeCl}}_{\text{2}}$ by relaxing the requirement of octet for Be atom needs to be drawn.

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 existing 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. The formula for the formal charge can be written as:

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