Answer :

To draw a Lewis structure for the ammonium ion ([tex]NH4^+[/tex]), we need to consider the valence electrons of each atom. The formal charge on [tex]NH4^+[/tex] is zero.

Nitrogen (N) is in Group 5 of the periodic table and has 5 valence electrons. Hydrogen (H) is in Group 1 and has 1 valence electron. Additionally, the ammonium ion has a positive charge of +1.

The Lewis structure for the ammonium ion is as follows:

H H

\ /

N+

/ \

H H

In this structure, nitrogen (N) is surrounded by four hydrogen (H) atoms. Each hydrogen atom shares one electron with nitrogen, resulting in a total of 8 electrons around nitrogen (4 from hydrogen and 4 from its own valence electrons).

To determine the formal charge on the nitrogen atom, we calculate the difference between the number of valence electrons of nitrogen in the Lewis structure and its usual number of valence electrons (5).

Number of valence electrons of nitrogen in the Lewis structure = 5

Usual number of valence electrons for nitrogen = 5

Formal charge on nitrogen = Valence electrons - Usual number of valence electron

= 5 - 5

= 0

Therefore, the formal charge on the nitrogen atom in the ammonium ion ([tex]NH4^+[/tex]) is 0.

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