Lewis Structure of SeO (With 6 Simple Steps to Draw!)

I’m super excited to teach you the lewis structure of SeO in just 6 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of SeO molecule.

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

Lewis structure of SeO contains one double bond between the Selenium (Se) and Oxygen (O) atom. The Selenium and Oxygen atoms have two lone pairs on them.

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 SeO).

6 Steps to Draw the Lewis Structure of SeO

Step #1: Calculate the total number of valence electrons

Here, the given molecule is SeO. In order to draw the lewis structure of SeO, first of all you have to find the total number of valence electrons present in the SeO 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 SeO

• For Selenium: 

Selenium is a group 16 element on the periodic table.

Hence, the valence electrons present in selenium is 6 (see below image).

• For Oxygen:

Oxygen is a group 16 element on the periodic table.

Hence, the valence electron present in oxygen is 6 (see below image).

Hence in a SeO molecule, 

Valence electrons given by Selenium (Se) atom = 6
Valence electrons given by Oxygen (O) atom = 6
So, total number of Valence electrons in SeO molecule = 6 + 6 = 12

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 SeO molecule, there are only two atoms. So you can consider any of the atoms as a center atom.

So, let’s assume that the oxygen atom is a central atom.

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

Now in the above sketch of SeO molecule, put the two electrons (i.e electron pair) between the selenium atom and oxygen atom to represent a chemical bond between them.

This pair of electrons present between the Selenium (Se) atom and Oxygen (O) atom forms a chemical bond, which bonds both the selenium atom and oxygen atom with each other in a SeO 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 SeO, we have just assumed the oxygen atom as a central atom and so the selenium atom is an outer atom.

So now, we have to complete the octet on this selenium atom.

Now, you can see in the above image that the selenium atom forms an octet.

Also, only 8 valence electrons of SeO molecule are used in the above structure.

But there are total 12 valence electrons in SeO molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 12 – 8 = 4.

So let’s keep these four electrons (i.e 2 electron pairs) on the central atom (i.e oxygen 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 oxygen atom) has an octet or not.

In simple words, we have to check whether this Oxygen (O) atom is having 8 electrons or not.

As you can see from the above image, this oxygen atom has only 6 electrons. So it does not fulfill the octet rule.

Now, in order to fulfill the octet of this oxygen atom, we have to move the electron pair from the outer atom (i.e selenium atom) to form a double bond.

Now you can see from the above image that the oxygen 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 selenium and oxygen atom.

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

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

• For Selenium:
  Valence electron = 6 (as it is in group 16)
  Nonbonding electrons = 4
  Bonding electrons = 4
• For Oxygen:
  Valence electron = 6 (as it is in group 16)
  Nonbonding electrons = 4
  Bonding electrons = 4

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

So you can see above that the formal charge on selenium and oxygen atoms are “zero”.

Hence, there will not be any change in the above structure and the above lewis structure of SeO is the final stable structure only.

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

Related lewis structures for your practice:
Lewis Structure of ICN
Lewis Structure of P2H4
Lewis Structure of SI6
Lewis Structure of CBr2F2
Lewis Structure of SiH3- 

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