Lewis Structure of NH4+ (Ammonium ion) (With 6 Simple Steps)

Ready to learn how to draw the lewis structure of NH4+ ion?

Awesome!

Here, I have explained 6 simple steps to draw the lewis dot structure of NH4+ ion (along with images).

So, if you are ready to go with these 6 simple steps, then let’s dive right into it!

Lewis structure of NH4+ ion (or Ammonium ion) contains four single bonds between each Nitrogen (N) and Hydrogen (H) atoms. The Nitrogen atom (N) is at the center and it is surrounded by 4 Hydrogen atoms (H). The Nitrogen atom has +1 formal charge.

Let’s draw and understand this lewis dot structure step by step.

(Note: Take a pen and paper with you and try to draw this lewis structure along with me. I am sure you will definitely learn how to draw lewis structure of NH4+ ion).

6 Steps to Draw the Lewis Structure of NH4+

Step #1: Calculate the total number of valence electrons

Here, the given ion is NH4+ (ammonium ion). In order to draw the lewis structure of NH4+ ion, first of all you have to find the total number of valence electrons present in the NH4+ ion.
(Valence electrons are the number of electrons present in the outermost shell of an atom).

So, let’s calculate this first.

Calculation of valence electrons in NH4+

• For Nitrogen:

Nitrogen is a group 15 element on the periodic table. ^[1]

Hence, the valence electrons present in nitrogen is 5 (see below image).

• For Hydrogen: 

Hydrogen is a group 1 element on the periodic table. ^[2]

Hence, the valence electron present in hydrogen is 1 (see below image).

Hence in a NH4+ ion, 

Valence electrons given by Nitrogen (N) atom = 5
Valence electron given by each Hydrogen (H) atom = 1
The +1 charge indicates that one electron is less
So, total number of Valence electrons in NH4+ ion = 5 + 1(4) -1 = 8

Step #2: Select the center atom (H is always outside)

While selecting the center atom, always put the least electronegative atom at the center.

(Remember: Fluorine is the most electronegative element on the periodic table and the electronegativity decreases as we move right to left in the periodic table as well as top to bottom in the periodic table). ^[3]

Here in the NH4 molecule, if we compare the nitrogen atom (N) and hydrogen atom (H), then hydrogen is less electronegative than nitrogen. But as per the rule, we have to keep hydrogen outside.

So, nitrogen should be placed in the center and the remaining 4 hydrogen atoms will surround it.

Step #3: Put two electrons between the atoms to represent a chemical bond

Now in the above sketch of NH4 molecule, put the two electrons (i.e electron pair) between each nitrogen atom and hydrogen atom to represent a chemical bond between them.

These pairs of electrons present between the Nitrogen (N) and Hydrogen (H) atoms form a chemical bond, which bonds the nitrogen and hydrogen atoms with each other in a NH4 molecule.

Step #4: Complete the octet (or duplet) on outside atoms. If the valence electrons are left, then put the valence electrons pair on the central atom

Don’t worry, I’ll explain!

In the Lewis structure of NH4+, the outer atoms are hydrogen atoms.

So now, you have to check whether these hydrogen atoms are forming a duplet or not! (because hydrogen requires only 2 electrons to have a complete outer shell).

You can see in the above image that all the hydrogen atoms form a duplet.

Also, all the 8 valence electrons of NH4+ ion (as calculated in step #1) are used in the above structure. So there are no remaining electron pairs.

Hence there is no change in the above sketch of NH4.

Let’s move to the next step.

Step #5: Check whether the central atom has octet or not. If it does not have an octet, then move the electron pair from the outer atom to form a double bond or triple bond

In this step, we have to check whether the central atom (i.e nitrogen) has an octet or not. 

In simple words, we have to check whether the central Nitrogen (N) atom is having 8 electrons or not.

As you can see from the above image, the central atom (i.e nitrogen), is having 8 electrons. So it fulfills the octet rule and the nitrogen atom is stable.

Step #6: Final step – Check the stability of lewis structure by calculating the formal charge on each atom

Now, you have come to the final step and here you have to check the formal charge on nitrogen atom (N) as well as each hydrogen atom (H).

For that, you need to remember the formula of formal charge;

Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2

• For Nitrogen:
  Valence electrons = 5 (as it is in group 15)
  Nonbonding electrons = 0
  Bonding electrons = 8
• For Hydrogen:
  Valence electron = 1 (as it is in group 1)
  Nonbonding electrons = 0
  Bonding electrons = 2

Formal charge	=	Valence electrons	–	Nonbonding electrons	–	(Bonding electrons)/2
N	=	5	–	0	–	8/2	=	+1
H	=	1	–	0	–	2/2	=	0

Let’s keep this charge on the nitrogen atom in the above lewis structure of NH4 molecule.

As you can see in the above sketch, there is one +ve charge on the nitrogen atom, which indicates the +1 formal charge on the NH4 molecule.

Hence, the above lewis structure of NH4+ ion is the stable lewis structure.

Each electron pair (:) in the lewis dot structure of NH4+ ion represents the single bond ( | ). So the above lewis dot structure of NH4+ ion can also be represented as shown below.

Related lewis structures for your practice:
Lewis structure of NH2-
Lewis structure of AlCl3
Lewis structure of BeH2
Lewis structure of HNO
Lewis structure of NI3

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