Lewis Structure of IF2- (With 5 Simple Steps to Draw!)

I’m super excited to teach you the lewis structure of IF2- ion in just 5 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of IF2- ion.

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

Lewis structure of IF2- ion contains two single bonds between the Iodine (I) atom and each Fluorine (F) atom. The Iodine atom (I) is at the center and it is surrounded by 2 Fluorine atoms (F). The Iodine atom as well as both the Fluorine atoms have 3 lone pairs. The Iodine 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 IF2- ion).

5 Steps to Draw the Lewis Structure of IF2- ion

Step #1: Calculate the total number of valence electrons

Here, the given ion is IF2- ion. In order to draw the lewis structure of IF2-, first of all you have to find the total number of valence electrons present in the IF2- 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 IF2- ion

• For Iodine:

Iodine is a group 17 element on the periodic table. ^[1]

Hence, the valence electrons present in iodine is 7 (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 IF2- ion, 

Valence electrons given by Iodine (I) atom = 7
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 IF2- ion = 7 + 7(2) + 1 = 22

Step #2: Select the center atom

While selecting the atom, always put the least electronegative atom at the center. 

Here in the IF2- ion, if we compare the iodine atom (I) and fluorine atom (F), then the iodine is less electronegative than fluorine.

So, iodine should be placed in the center and the remaining 2 fluorine atoms will surround it.

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

Now in the above sketch of IF2, put the two electrons (i.e electron pair) between each iodine atom and fluorine atom to represent a chemical bond between them.

These pairs of electrons present between the Iodine (I) and Fluorine (F) atoms form a chemical bond, which bonds the iodine and fluorine atoms with each other in a IF2 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 IF2, 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, only 16 valence electrons of IF2- ion are used in the above structure.

But there are total 22 valence electrons in IF2- ion (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 22 – 16 = 6.

So let’s keep these six electrons (i.e 3 electron pairs) on the central atom.

Now, 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 iodine atom (I) 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 Iodine:
  Valence electron = 7 (as it is in group 17)
  Nonbonding electrons = 6
  Bonding electrons = 4
• 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
I	=	7	–	6	–	4/2	=	-1
F	=	7	–	6	–	2/2	=	0

Let’s keep these charges on the atoms in the above lewis structure of IF2- ion.

As you can see in the above sketch, there is one -ve charge on the iodine atom, which indicates the -1 formal charge on the IF2 molecule.

Hence, the above lewis structure of IF2- ion is the stable lewis structure.

Each electron pair (:) in the lewis dot structure of IF2- ion represents the single bond ( | ). So the above lewis dot structure of IF2- ion can also be represented as shown below.

Related lewis structures for your practice:
Lewis Structure of BrF2-
Lewis Structure of P2
Lewis Structure of IBr2-
Lewis Structure of PI3
Lewis Structure of NOBr 

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