Answer
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Step 1: Determine the total number of valence electrons in the NH^4 + ion.
5 \ \text{valence electrons (N)} + 4 \ \text{valence electrons (H)} - 1 \ \text{positive charge} = 8 \ \text{valence electrons}
The nitrogen atom (N) is in the 5th period of the periodic table and has 5 valence electrons. Each hydrogen atom (H) in the 1st period has 1 valence electron. Since there are 4 hydrogen atoms and one nitrogen atom, and the charge is + 1, we have:
Step 2: Place the atoms in their positions and distribute the valence electrons.
Place nitrogen in the center with hydrogen atoms surrounding it. Draw a single bond between the nitrogen and each hydrogen atom, using 2 electrons from the nitrogen for each bond.
Final Answer
The Lewis structure for NH^4 + is shown above, with the nitrogen atom in the center and single bonds to each hydrogen atom. The nitrogen atom has 2 lone pairs of electrons and a positive charge, representing the + 1 charge on the ion.
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