Chapter 8.3, Problem 41PP

Interpretation Introduction

Interpretation:

The structure of ${\text{NH}}_{\text{4}}{}^{\text{+}}$ ion needs to be drawn.

Concept introduction:

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

Answer to Problem 41PP

Explanation of Solution

Lewis structure of ${\text{NH}}_{\text{4}}{}^{\text{+}}$ :

First write the electron configuration of nitrogen and hydrogen as follows:

Nitrogen (N) ${\text{1s}}^{2}2s^{2}2p^3$

H ${\text{1s}}^1$

As ${\text{NH}}_{\text{4}}{}^{\text{+}}$ ion is the cation, N must have lost its one electron. So, nitrogen has $4$ valence electrons in their outermost shell and hydrogen has $1$ valence electron.

For the valence shell configuration nitrogen requires $4$ electrons and hydrogen requires $1$ electron to complete their octet configuration.

The structure is represented as follows:

After sharing the electron between the nitrogen and hydrogen atoms, the stable valance shell configuration can be obtained.

Conclusion

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