Chapter 8.1, Problem 6PP

Interpretation Introduction

Interpretation:

The Lewis structure of molecule formed with group 1 and group 16 elements needs to be drawn.

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 6PP

After sharing the electrons between the group $1$ and group $16$, the stable valence shell configuration or stable structure can be obtained.

Explanation of Solution

Write general electron configuration of group $1$ and group 16 as follows:

In group $1\to n{s}^1$

Group $16\to n{s}^{2}n{p}^4$

Group $1$ has $1$ electron and group $16$ has $6$ electron in their outer most shell.

For the valence shell configuration or stable structure formation group $1$ requires $1$ electron and group $16$ element requires $2$ electron to achieve octet configuration.

Thus, there will be 2 atoms of group 1 element combined with 1 atom of group 16. The number of lone pair of electrons on group 16 element will be 2.

Let the group 1 element be A and group 16 element be B thus, the general Lewis structure will be as follows:

For example $Hydrogen$ is from group $1$ and $Oxygen$ is from group $16.$ The formula of compound will be H₂O.

$\begin{array}{l}{H}_{2}O\\ H\to 1s^1\\ O\to 1s^{2}2s^{2}2p^4\end{array}$

Conclusion

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