SeO Lewis Structure in 5 Steps (With Images)

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

Let me explain the above image in short.

SeO lewis structure has one Selenium atom (Se) and one Oxygen atom (O) which contain a double bond between them. There are 2 lone pairs on the Selenium atom (Se) as well as Oxygen atom (O).

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

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

Steps of drawing SeO lewis structure

Step 1: Find the total valence electrons in SeO molecule

In order to find the total valence electrons in SeO molecule, first of all you should know the valence electrons present in a selenium atom as well as oxygen 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 oxygen using a periodic table.

Total valence electrons in SeO 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 oxygen atom:

Oxygen is group 16 element on the periodic table. ^[2] Hence the valence electrons present in oxygen is 6.

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

Hence, 

Total valence electrons in SeO molecule = valence electrons given by 1 selenium atom + valence electrons given by 1 oxygen atom = 6 + 6 = 12.

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 SeO. It has only two atoms, so you can select any of the atoms as a center atom.

Let’s assume the oxygen atom as a central atom.

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

Now in the SeO molecule, you have to put the electron pairs between the selenium atom (Se) and oxygen atom (O).

This indicates that the selenium (Se) atom and oxygen (O) atom are chemically bonded with each other in a SeO 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 atom.

Here in the sketch of SeO molecule, we have assumed the oxygen atom as a center atom. So the selenium is the outer atom.

Hence you have to make the selenium atom stable.

You can see in the below image that the selenium atom is forming an octet and hence it is stable.

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

The SeO molecule has a total 12 valence electrons and out of these, only 8 valence electrons are used in the above sketch.

So the number of electrons which are left = 12 – 8 = 4.

You have to put these 4 electrons on the oxygen atom in the above sketch of SeO 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 oxygen atom (O) is stable or not.

In order to check the stability of this oxygen (O) atom, we have to check whether it is forming an octet or not.

Unfortunately, this oxygen atom is not forming an octet here. Oxygen has only 6 electrons and it is unstable.

Now to make this oxygen atom stable, you have to shift the electron pair from the selenium atom.

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

You can see from the above picture that the oxygen atom is forming an octet.

And hence this oxygen atom is stable.

Now let’s proceed to the final step to check whether the lewis structure of SeO 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 SeO.

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 the selenium atom (Se) and oxygen atom (O) present in the SeO 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 in the image given below.

For Selenium (Se) atom:
Valence electrons = 6 (because selenium is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4

For Oxygen (O) atom:
Valence electrons = 6 (because oxygen is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
Se	=	6	–	4/2	–	4	=	0
O	=	6	–	4/2	–	4	=	0

From the above calculations of formal charge, you can see that the selenium (Se) atom and oxygen (O) atoms have a “zero” formal charge.

This indicates that the above lewis structure of SeO is stable and there is no further change in the above structure of SeO.

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

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:

ICN Lewis Structure	P2H4 Lewis Structure
SI6 Lewis Structure	CBr2F2 Lewis Structure
SiH3- Lewis Structure	AsBr3 Lewis Structure