Lewis Structure of SeF6 (With 5 Simple Steps to Draw!)

I’m super excited to teach you the lewis structure of SeF6 in just 5 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of SeF6 molecule.

So, if you are ready to go with these 5 simple steps, then let’s dive right into it!

Lewis structure of SeF6 contains six single bonds between the Selenium (Se) atom and each Fluorine (F) atom. The Selenium atom (Se) is at the center and it is surrounded by 6 Fluorine atoms (F). The Selenium atom does not have a lone pair while all the 6 Fluorine atoms have 3 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 SeF6).

5 Steps to Draw the Lewis Structure of SeF6

Step #1: Calculate the total number of valence electrons

Here, the given molecule is SeF6. In order to draw the lewis structure of SeF6, first of all you have to find the total number of valence electrons present in the SeF6 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 SeF6

For Selenium:

Selenium is a group 16 element on the periodic table. ^[1]

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

For Fluorine:

Fluorine is a group 17 element on the periodic table. ^[2]

Hence, the valence electrons present in fluorine is 7 (see below image).

Hence in a SeF6 molecule,

Valence electrons given by Selenium (Se) atom = 6
Valence electrons given by each Fluorine (F) atom = 7
So, total number of Valence electrons in SeF6 molecule = 6 + 7(6) = 48

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). ^[3]

Here in the SeF6 molecule, if we compare the selenium atom (Se) and fluorine atom (F), then the selenium is less electronegative than fluorine.

So, selenium should be placed in the center and the remaining 6 fluorine atoms will surround it.

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

Now in the above sketch of SeF6 molecule, put the two electrons (i.e electron pair) between each selenium atom and fluorine atom to represent a chemical bond between them.

These pairs of electrons present between the Selenium (Se) and Fluorine (F) atoms form a chemical bond, which bonds the selenium and fluorine atoms with each other in a SeF6 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 SeF6, the outer atoms are fluorine atoms.

So now, you have to complete the octet on these fluorine atoms (because fluorine requires 8 electrons to have a complete outer shell).

Now, you can see in the above image that all the fluorine atoms form an octet.

Also, all the 48 valence electrons of SeF6 molecule (as calculated in step #1) are used in the above structure. So there are no remaining electron pairs.

Hence there is no change in the above sketch of SeF6.

Let’s move to the next step.

Step #5: 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 selenium atom (Se) as well as each fluorine atom (F).

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

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

For Selenium:
Valence electrons = 6 (as it is in group 16)
Nonbonding electrons = 0
Bonding electrons = 12
For Fluorine:
Valence electron = 7 (as it is in group 17)
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge	=	Valence electrons	–	Nonbonding electrons	–	(Bonding electrons)/2
Se	=	6	–	0	–	12/2	=	0
F	=	7	–	6	–	2/2	=	0

So you can see above that the formal charges on selenium as well as fluorine are “zero”.

Hence, there will not be any change in the above structure and the above lewis structure of SeF6 is the final stable structure only.

Each electron pair (:) in the lewis dot structure of SeF6 represents the single bond ( | ). So the above lewis dot structure of SeF6 can also be represented as shown below.

Article by;

Jay Rana

Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. With a desire to make learning accessible for everyone, he founded Knords Learning, an online learning platform that provides students with easily understandable explanations. Read more about our Editorial process.

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