Question

To illustrate the bonding in the ammonium ion (NH4+), you need to represent the arrangement of atoms and the sharing of electrons. Ammonium ion consists of one nitrogen atom (N) bonded to four hydrogen atoms (H). Each hydrogen atom contributes one electron, while the nitrogen atom shares its lone pair of electrons. Here's the structural formula for the ammonium ion (NH4+):

a. H
b. |
c. H-N-H
d. |
e. H

Answer 1

The ammonium ion (NH4+) features a nitrogen atom bonded to four hydrogen atoms with no lone pairs, resulting in a tetrahedral molecular structure.

Step-by-step explanation:

To illustrate the bonding in the ammonium ion (NH4+), consider a central nitrogen atom surrounded by four hydrogen atoms. A neutral nitrogen atom has five valence electrons, but in an ammonium ion, the nitrogen shares this valence with the four hydrogens, forming four covalent bonds. No lone pairs are present on the nitrogen in NH4+.

The bonding results from the nitrogen's lone pair in NH3 forming a coordinate covalent bond with an additional hydrogen ion (H+). This results in a tetrahedral electron-pair geometry as well as a tetrahedral molecular structure, meaning the areas of high electron density (the bonds) orient themselves as far apart as possible, forming a three-dimensional shape resembling a pyramid with a triangular base.

In summary, when drawing the Lewis structure for the ammonium ion, keep in mind it should reflect four bonds from the nitrogen to the hydrogen atoms, leading to a tetrahedral shape, without any lone pairs on the nitrogen.