Represent th eformation of an ammonium ion with the aid of Lewis structures
The formation of an ammonium ion (NH4+) can be shown using Lewis structures.
First, we start with the Lewis structure of ammonia (NH3), which has a central nitrogen atom bonded to three hydrogen atoms. The nitrogen atom also has one lone pair of electrons.
NH3:
H - N - H
|
H
To form the ammonium ion, one hydrogen atom undergoes ionization and transfers its lone pair of electrons to the nitrogen atom. This creates a positive charge on the nitrogen atom and forms a coordinate covalent bond between the hydrogen and nitrogen.
NH4+:
H - N+
|
H
H
To represent the formation of an ammonium ion (NH4+), we need to consider the Lewis structures of its individual components, nitrogen (N), and hydrogen (H).
1. Start by considering the Lewis structure of nitrogen (N):
- Nitrogen has five valence electrons.
- Place one electron around nitrogen as a lone pair (represented as a pair of dots).
- Now, connect the remaining three valence electrons around nitrogen with single bonds (represented as lines) to represent the three hydrogen atoms.
H
|
H - N - H
|
2. Next, discuss the formation of ammonium ion (NH4+):
- The ammonium ion is formed when a hydrogen ion (H+) attaches to the nitrogen atom, bonding with the lone pair of nitrogen.
- Hydrogen ion (H+) only has one proton, so no electrons are present.
- Remove one electron from the nitrogen atom to form a positive charge, allowing it to bond with the hydrogen ion.
H
|
H - N - H
|
H+
Please note that the Lewis structure represents the valence shell electrons in an atom or ion and focuses on bonding and lone pair electrons.