I’m super excited to teach you the lewis structure of N2 in just 6 simple steps.
Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of N2 molecule.
So, if you are ready to go with these 6 simple steps, then let’s dive right into it!
Lewis structure of N2 (nitrogen gas) contains one triple bond between both the Nitrogen (N) atoms. And both the Nitrogen atoms have one lone pair on it.
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 N2).
6 Steps to Draw the Lewis Structure of N2
Step #1: Calculate the total number of valence electrons
Here, the given molecule is N2 (Nitrogen gas). In order to draw the lewis structure of N2, first of all you have to find the total number of valence electrons present in the N2 molecule.
(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 N2
- For Nitrogen:
Nitrogen is a group 15 element on the periodic table.
Hence, the valence electrons present in nitrogen is 5 (see below image).
Hence, total number of Valence electrons in N2 molecule = 5(2) = 10
Step #2: Select the center atom
While selecting the atom, you have to put the least electronegative atom at the center.
But here in the N2 molecule, both the atoms are same. So you can consider any of the atoms as a center atom.
So, let’s assume that the nitrogen which is on the right side is the central atom.
Step #3: Put two electrons between the atoms to represent a chemical bond
Now in the above sketch of N2 molecule, put the two electrons (i.e electron pair) between both the nitrogen atoms to represent a chemical bond between them.
These pair of electrons present between the Nitrogen (N) atoms form a chemical bond, which bonds both the nitrogen atoms with each other in a N2 molecule.
Step #4: Complete the octet (or duplet) on outside atom. 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 N2, we have just assumed the right side nitrogen atom as a central atom and so the left side nitrogen atom is an outer atom.
So now, we have to complete the octet on this left side nitrogen atom.
Now, you can see in the above image that the outer nitrogen atom forms an octet.
Also, only 8 valence electrons of N2 molecule are used in the above structure.
But there are total 10 valence electrons in N2 molecule (as calculated in step #1).
So the number of electrons left to be kept on the central atom = 10 – 8 = 2.
So let’s keep these two electrons (i.e electron pair) on the central atom (i.e right side nitrogen atom).
Now, 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 right side nitrogen atom) has an octet or not.
In simple words, we have to check whether this Nitrogen (N) atom is having 8 electrons or not.
As you can see from the above image, this right side nitrogen atom has only 4 electrons. So it does not fulfill the octet rule.
Now, in order to fulfill the octet of this nitrogen atom, we have to move the electron pair from the outer atom (i.e left side nitrogen atom) to form a double bond.
Still, the octet of nitrogen atom is not fulfilled as it has only 6 electrons.
So again moving the electron pair from the outer nitrogen atom, we will get the following structure.
Now you can see from the above image that the nitrogen atom has 8 electrons. So it fulfills the octet rule and it 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 the nitrogen atoms (N).
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 = 2
Bonding electrons = 6
|Formal charge||=||Valence electrons||–||Nonbonding electrons||–||(Bonding electrons)/2|
So you can see above that the formal charge on both the nitrogen atoms are “zero”.
Hence, there will not be any change in the above structure and the above lewis structure of N2 is the final stable structure only.
Each electron pair (:) in the lewis dot structure of N2 represents the single bond ( | ). So the above lewis dot structure of N2 can also be represented as shown below.