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The Lewis structure for the ammonium ion (NH4+) can be drawn by counting a total of 8 valence electrons after accounting for the positive charge. Nitrogen is at the center, bonded to four hydrogen atoms with single bonds. This structure shows that ammonium has no lone pairs and a tetrahedral shape.


Explanation:

Drawing the Lewis Structure for Ammonium Ion (NH4+)

The ammonium ion, represented as NH4+, is a cation formed when ammonia (NH3) accepts a proton (H+). In order to draw its Lewis structure, we need to consider the total number of valence electrons available for bonding.

Here are the steps to construct the Lewis structure for NH4+:

  1. Count the Valence Electrons: Nitrogen (N) has five valence electrons, and each hydrogen (H) has one valence electron. Therefore, for NH4, we calculate:

5 (from N) + 4 (from 4 Hydrogens) = 9 valence electrons.

  1. Since NH4+ has a positive charge, it means that it has lost one electron. Thus, we subtract one electron from the total count:

Total = 9 - 1 = 8 valence electrons.

  1. Arrange the Atoms: Place nitrogen in the center, and surround it with the four hydrogen atoms.

This gives us:

H
  |
N - H
  |
H - H

  1. Distribute Electrons: Each N-H bond consists of two electrons (1 pair). As there are four N-H bonds, the total accounted for is 8 electrons:

Thus, the Lewis structure for NH4+ has nitrogen at the center with four single bonds connecting it to four hydrogen atoms. Since all 8 electrons are used up in bonding, there are no lone pairs on the nitrogen.

Final Representation

The final Lewis structure can be written as:

  H
    |
N - H
    |
H - H

Overall, the ammonium ion is tetrahedral in shape, and the bonding electrons are evenly spread out around the nitrogen atom.


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