SeS2 Lewis Structure in 6 Steps (With Images)

So you have seen the above image by now, right?

Let me explain the above image in short.

SeS2 lewis structure has a Selenium atom (Se) at the center which is surrounded by two Sulfur atoms (S). There are 2 double bonds between the Selenium atom (Se) and each Sulfur atom (S). There are 2 lone pairs on both the Sulfur atoms (S) and 1 lone pair on the Selenium atom (Se).

If you haven’t understood anything from the above image of SeS2 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of SeS2.

So let’s move to the steps of drawing the lewis structure of SeS2.

Steps of drawing SeS2 lewis structure

Step 1: Find the total valence electrons in SeS2 molecule

In order to find the total valence electrons in a SeS2 molecule, first of all you should know the valence electrons present in selenium atom as well as sulfur atom.
(Valence electrons are the electrons that are present in the outermost orbit of any atom.)

Here, I’ll tell you how you can easily find the valence electrons of selenium as well as sulfur using a periodic table.

Total valence electrons in SeS2 molecule

→ Valence electrons given by selenium atom:

Selenium is a group 16 element on the periodic table. ^[1] Hence the valence electrons present in selenium is 6.

You can see the 6 valence electrons present in the selenium atom as shown in the above image.

→ Valence electrons given by sulfur atom:

Sulfur is a group 16 element on the periodic table. ^[2] Hence the valence electrons present in sulfur is 6.

You can see the 6 valence electrons present in the sulfur atom as shown in the above image.

Hence, 

Total valence electrons in SeS2 molecule = valence electrons given by 1 selenium atom + valence electrons given by 2 sulfur atoms = 6 + 6(2) = 18.

Step 2: Select the central atom

For selecting the center atom, you have to remember that the atom which is less electronegative remains at the center.

Now here the given molecule is SeS2 and it contains selenium atom (Se) and sulfur atoms (S).

You can see the electronegativity values of selenium atom (Se) and sulfur atom (S) in the above periodic table.

If we compare the electronegativity values of selenium (Se) and sulfur (S) then the selenium atom is less electronegative.

So here the selenium atom (Se) is the center atom and the sulfur atoms (S) are the outside atoms.

Step 3: Connect each atoms by putting an electron pair between them

Now in the SeS2 molecule, you have to put the electron pairs between the selenium atom (Se) and sulfur atoms (S).

This indicates that the selenium (Se) and sulfur (S) are chemically bonded with each other in a SeS2 molecule.

Step 4: Make the outer atoms stable. Place the remaining valence electrons pair on the central atom.

Now in this step, you have to check the stability of the outer atoms.

Here in the sketch of SeS2 molecule, you can see that the outer atoms are sulfur atoms.

These outer sulfur atoms are forming an octet and hence they are stable. 

Also, in step 1 we have calculated the total number of valence electrons present in the SeS2 molecule.

The SeS2 molecule has a total 18 valence electrons and out of these, only 16 valence electrons are used in the above sketch.

So the number of electrons which are left = 18 – 16 = 2.

You have to put these 2 electrons on the central selenium atom in the above sketch of SeS2 molecule.

Now let’s proceed to the next step.

Step 5: Check the octet on the central atom. If it does not have octet, then shift the lone pair to form a double bond or triple bond.

In this step, you have to check whether the central selenium atom (Se) is stable or not.

In order to check the stability of the central selenium (Se) atom, we have to check whether it is forming an octet or not.

Unfortunately, the selenium atom is not forming an octet here. Selenium has only 6 electrons and it is unstable.

Now to make this selenium atom stable, you have to shift the electron pair from the outer sulfur atom so that the selenium atom can have 8 electrons (i.e octet).

After shifting this electron pair, the central selenium atom will get 2 more electrons and thus its total electrons will become 8.

You can see from the above picture that the selenium atom is forming an octet as it has 8 electrons.

Now let’s proceed to the final step to check whether the lewis structure of SeS2 is stable or not.

Step 6: Check the stability of lewis structure

Now you have come to the final step in which you have to check the stability of lewis structure of SeS2.

The stability of lewis structure can be checked by using a concept of formal charge.

In short, now you have to find the formal charge on selenium (Se) atom as well as sulfur (S) atoms present in the SeS2 molecule.

For calculating the formal charge, you have to use the following formula;

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

You can see the number of bonding electrons and nonbonding electrons for each atom of SeS2 molecule in the image given below.

For Selenium (Se) atom:
Valence electrons = 6 (because selenium is in group 16)
Bonding electrons = 6
Nonbonding electrons = 2

For double bonded Sulfur (S) atom:
Valence electrons = 6 (because sulfur is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4

For single bonded Sulfur (S) atom:
Valence electrons = 6 (because sulfur is in group 16)
Bonding electrons = 2
Nonbonding electrons = 6

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
Se	=	6	–	6/2	–	2	=	+1
S (double bonded)	=	6	–	4/2	–	4	=	0
S (single bonded)	=	6	–	2/2	–	6	=	-1

From the above calculations of formal charge, you can see that the selenium (Se) atom has +1 charge and the single bonded sulfur (S) atom has -1 charge.

Because of this reason, the above obtained lewis structure of SeS2 is not stable. 

So we have to minimize these charges by shifting the electron pairs towards the selenium atom.

After shifting the electron pair from sulfur atom to selenium atom, the lewis structure of SeS2 becomes more stable.

In the above lewis dot structure of SeS2, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of SeS2.

I hope you have completely understood all the above steps.

For more practice and better understanding, you can try other lewis structures listed below.

Try (or at least See) these lewis structures for better understanding:

TeBr4 Lewis Structure	NO4 3- Lewis Structure
C2H2F2 Lewis Structure	C2Br2 Lewis Structure
GeCl4 Lewis Structure	P2O5 Lewis Structure