I’m super excited to teach you the lewis structure of NS2 in just 5 simple steps.
Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of NS2 molecule.
So, if you are ready to go with these 5 simple steps, then let’s dive right into it!
Lewis structure of NS2 contains one double bond and one single bond between the Nitrogen (N) atom and Sulfur (S) atoms. The Nitrogen atom (N) is at the center and it is surrounded by 2 Sulfur atoms (S). The Nitrogen atom has 1 unpaired electron, one Sulfur atom has 3 lone pairs and the other Sulfur atom has 2 lone pairs.
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 NS2).
5 Steps to Draw the Lewis Structure of NS2
Step #1: Calculate the total number of valence electrons
Here, the given molecule is NS2. In order to draw the lewis structure of NS2, first of all you have to find the total number of valence electrons present in the NS2 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 NS2
- For Nitrogen:
Nitrogen is a group 15 element on the periodic table.
Hence, the valence electrons present in nitrogen is 5 (see below image).
- For Sulfur:
Sulfur is a group 16 element on the periodic table.
Hence, the valence electrons present in sulfur is 6 (see below image).
Hence in a NS2 molecule,
Valence electrons given by Nitrogen (N) atom = 5
Valence electrons given by each Sulfur (S) atom = 6
So, total number of Valence electrons in NS2 molecule = 5 + 6(2) = 17
Step #2: Select the center atom
While selecting the 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).
Here in the NS2 molecule, if we compare the nitrogen atom (N) and sulfur atom (S), then the nitrogen is less electronegative than sulfur.
So, nitrogen should be placed in the center and the remaining 2 sulfur atoms will surround it.
Step #3: Put two electrons between the atoms to represent a chemical bond
Now in the above sketch of NS2 molecule, put the two electrons (i.e electron pair) between each nitrogen atom and sulfur atom to represent a chemical bond between them.
These pairs of electrons present between the Nitrogen (N) and Sulfur (S) atoms form a chemical bond, which bonds the nitrogen and sulfur atoms with each other in a NS2 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 NS2, the outer atoms are sulfur atoms.
So now, you have to complete the octet on these sulfur atoms (because sulfur requires 8 electrons to have a complete outer shell).
Now, you can see in the above image that all the sulfur atoms form an octet.
Also, only 16 valence electrons of NS2 molecule are used in the above structure.
But there are total 17 valence electrons in NS2 molecule (as calculated in step #1).
So the number of electrons left to be kept on the central atom = 17 – 16 = 1.
So let’s keep this electron (i.e unpaired electron) on the central atom.
(Note: In most cases, you will see that the pair of electrons are left. But here, only one electron is left. So we have to put this unpaired electron on the central 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 nitrogen) has an octet or not.
In simple words, we have to check whether the central Nitrogen (N) atom has 8 electrons or not.
As you can see from the above image, the central atom (i.e nitrogen) has only 5 electrons. So it does not fulfill the octet rule.
Now, in order to fulfill the octet of nitrogen atom, we have to move the electron pair from the outer atom (i.e sulfur atom) to form a double bond.
Now you can see from the above image that the central atom (i.e nitrogen), is having 7 electrons.
If we try to add one more electron pair on the nitrogen atom, then there will be 7+2=9 electrons in its outermost orbit. And nitrogen atom does not have the capacity to hold 9 electrons in its outermost orbit.
Because of this reason, the above lewis dot structure of NS2 (having 7 electrons on central atom) is a stable structure.
Each electron pair (:) in the lewis dot structure of NS2 represents the single bond ( | ). So the above lewis dot structure of NS2 can also be represented as shown below.