Write the Lewis structure for the NH[latex]_{4}^{+}[/latex] ion.

Begin by writing the skeletal structure. Since hydrogen is always terminal, put the nitrogen atom in the central position. [latex] \begin{matrix} & H & \\ H & N & H \\ & H & \end{matrix} [/latex] Calculate the total number of electrons for the Lewis structure by summing the number of valence electrons for each atom and subtracting 1 for the 1+ charge. Place two bonding electrons between every two atoms. Since all of the atoms have complete octets (or duets for hydrogen), no double bonds are necessary. [latex] \begin{matrix} H \\ H : \overset{..}{\underset{..}{N}} : H \\ H \end{matrix} [/latex] (8 of 8 electrons used) Finally, write the Lewis structure in brackets with the charge of the ion in the upper right hand corner [latex] \begin{bmatrix}H\\ H-\overset{|}{\underset{|}{N}} -H\\H \end{bmatrix} ^+ [/latex]

Question 9.6: Write the Lewis structure for the NH4 + ion.

Principles of Chemistry: A Molecular Approach

Write the Lewis structure for the NH $_{4}^{+}$ ion.

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Begin by writing the skeletal structure. Since hydrogen is always terminal, put the nitrogen atom in the central position.	$\begin{matrix} & H & \\ H & N & H \\ & H & \end{matrix}$
Calculate the total number of electrons for the Lewis structure by summing the number of valence electrons for each atom and subtracting 1 for the 1+ charge.
Place two bonding electrons between every two atoms. Since all of the atoms have complete octets (or duets for hydrogen), no double bonds are necessary.	$\begin{matrix} H \\ H : \overset{..}{\underset{..}{N}} : H \\ H \end{matrix}$ (8 of 8 electrons used)
Finally, write the Lewis structure in brackets with the charge of the ion in the upper right hand corner	$\begin{bmatrix}H\\ H-\overset{\|}{\underset{\|}{N}} -H\\H \end{bmatrix} ^+$