Lewis Structure of SbF6- (With 5 Simple Steps to Draw!)

Ready to learn how to draw the lewis structure of SbF6- ion?

Awesome!

Here, I have explained 5 simple steps to draw the lewis dot structure of SbF6- ion (along with images).

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

Lewis structure of SbF6- ion contains six single bonds between the Antimony (Sb) atom and each Fluorine (F) atom. The Antimony atom (Sb) is at the center and it is surrounded by 6 Fluorine atoms (F). All the six Fluorine atoms have 3 lone pairs. The Antimony atom has -1 formal charge.

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 SbF6- ion).

5 Steps to Draw the Lewis Structure of SbF6- ion

Step #1: Calculate the total number of valence electrons

Here, the given ion is SbF6- ion. In order to draw the lewis structure of SbF6- ion, first of all you have to find the total number of valence electrons present in the SbF6- ion.
(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 SbF6- ion

• For Antimony: 

Antimony is a group 15 element on the periodic table.

Hence, the valence electrons present in antimony is 5 (see below image).

• For Fluorine: 

Fluorine is a group 17 element on the periodic table.

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

Hence in a SbF6- ion, 

Valence electrons given by Antimony (Sb) atom = 5
Valence electrons given by each Fluorine (F) atom = 7
Electron due to -1 charge, 1 more electron is added
So, total number of Valence electrons in SbF6- ion = 5 + 7(6) + 1 = 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). ^[1]

Here in the SbF6 molecule, if we compare the antimony atom (Sb) and fluorine atom (F), then the antimony is less electronegative than fluorine.

So, antimony 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 a SbF6 molecule, put the two electrons (i.e electron pair) between each antimony atom and fluorine atom to represent a chemical bond between them.

These pairs of electrons present between the Antimony (Sb) and Fluorine (F) atoms form a chemical bond, which bonds the antimony and fluorine atoms with each other in a SbF6 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 SbF6- ion, 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 SbF6- ion (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.

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 antimony atom (Sb) 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 Antimony:
  Valence electrons = 5 (as it is in group 15)
  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
Sb	=	5	–	0	–	12/2	=	-1
F	=	7	–	6	–	2/2	=	0

Let’s keep these charges on the atoms in the above lewis structure of SbF6- ion.

As you can see in the above sketch, there is one -ve charge on the antimony atom, which indicates the -1 formal charge on the SbF6- molecule.

Hence, the above lewis structure of SbF6- ion is the stable lewis structure.

Each electron pair (:) in the lewis dot structure of SbF6- ion represents the single bond ( | ). So the above lewis dot structure of SbF6- ion can also be represented as shown below.

Related lewis structures for your practice:
Lewis Structure of SbCl3
Lewis Structure of C2H4F2
Lewis Structure of Br2O
Lewis Structure of SiH2Cl2
Lewis Structure of NF5 

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