Chapter 8.1, Problem 4PP

Interpretation Introduction

Interpretation:

The Lewis dot structure for CCl₄ needs to be determined.

Concept introduction:

Lewis structure is shown by each atom in the molecule using the chemical symbol with the electron. The bond is formed by sharing of electron between the atoms and excess electrons are shown as lone pairs.

Answer to Problem 4PP

After sharing the electron between $Carbon\left(C\right)$ and $Chlorine\left(Cl\right)$, the stable valence shells configuration and stable structure is formed.

Explanation of Solution

Lewis structure of $CC{l}_4.$ :

First write the electron configuration $Carbon\left(C\right)$ and $Chlorine\left(Cl\right).$ as follows:

$C\to 1s^{2}2s^{2}2p^2$

$Cl\to 1s^{2}2s^{2}2p^{6}3s^{2}3p^5$

$Carbon\left(C\right)$ and $Chlorine\left(Cl\right)$ has $4$ electrons and $7$ electrons in their outer most shell respectively.

For the valence shell configuration or stable structure formation $C$ requires $4$ electrons and $Chlorine$ requires $1$ electron. Thus, each Cl will have 3 lone pair of electrons on them. The Lewis structure will be as follows:

After sharing the electron between $Carbon\left(C\right)$ and $Chlorine\left(Cl\right)$, the valence shells configuration and stable structure is formed.

Conclusion

The valence shell configuration can be achieved by sharing the electrons between the atoms.