IF2- Lewis Structure in 6 Steps (With Images)

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

Let me explain the above image in short.

IF2- lewis structure has an Iodine atom (I) at the center which is surrounded by two Fluorine atoms (F). There is a single bond between the Iodine atom (I) and each Fluorine atom (F). There is a -1 formal charge on the Iodine atom (I).

If you haven’t understood anything from the above image of IF2- lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of IF2- ion.

So let’s move to the steps of drawing the lewis structure of IF2- ion.

Steps of drawing IF2- lewis structure

Step 1: Find the total valence electrons in IF2- ion

In order to find the total valence electrons in IF2- ion, first of all you should know the valence electrons present in the iodine atom as well as fluorine 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 iodine as well as fluorine using a periodic table.

Total valence electrons in IF2- ion

→ Valence electrons given by iodine atom:

Iodine is a group 17 element on the periodic table. ^[1] Hence the valence electrons present in iodine is 7.

You can see the 7 valence electrons present in the iodine atom as shown in the above image.

→ Valence electrons given by fluorine atom:

Fluorine is group 17 element on the periodic table. ^[2] Hence the valence electron present in fluorine is 7.

You can see the 7 valence electrons present in the fluorine atom as shown in the above image.

Hence, 

Total valence electrons in IF2- ion = valence electrons given by 1 iodine atom + valence electrons given by 2 fluorine atoms + 1 more electron is added due to 1 negative charge = 7 + 7(2) + 1 = 22.

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 ion is IF2- ion and it contains iodine atom (I) and fluorine atoms (F).

You can see the electronegativity values of iodine atom (I) and fluorine atom (F) in the above periodic table.

If we compare the electronegativity values of iodine (I) and fluorine (F) then the iodine atom is less electronegative.

So here the iodine atom (I) is the center atom and the fluorine atoms (F) are the outside atoms.

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

Now in the IF2 molecule, you have to put the electron pairs between the iodine atom (I) and fluorine atoms (F).

This indicates that the iodine (I) and fluorine (F) are chemically bonded with each other in a IF2 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 atoms.

Here in the sketch of IF2 molecule, you can see that the outer atoms are fluorine atoms.

These outer fluorine atoms are forming an octet and hence they are stable.

Also, in step 1 we have calculated the total number of valence electrons present in the IF2- ion.

The IF2- ion has a total 22 valence electrons and out of these, only 16 valence electrons are used in the above sketch.

So the number of electrons which are left = 22 – 16 = 6.

You have to put these 6 electrons on the central iodine atom in the above sketch of IF2 molecule.

Now let’s proceed to the next step.

Step 5: 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 IF2.

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 iodine atom (I) as well as fluorine atoms (F) present in the IF2 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 for each atom of IF2 molecule in the image given below.

For Iodine (I) atom:
Valence electrons = 7 (because iodine is in group 17)
Bonding electrons = 4
Nonbonding electrons = 6

For Fluorine (F) atom:
Valence electrons = 7 (because fluorine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
I	=	7	–	4/2	–	6	=	-1
F	=	7	–	2/2	–	6	=	0

From the above calculations of formal charge, you can see that the iodine (I) atom has -1 charge and the fluorine atoms have 0 charges.

So let’s keep these charges on the respective atoms in the IF2 molecule.

This overall -1 charge on the IF2 molecule is represented in the image given below.

In the above lewis dot structure of IF2- ion, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of IF2- ion.

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:

P2 Lewis Structure	IBr2- Lewis Structure
PI3 Lewis Structure	NOBr Lewis Structure
ClF2- Lewis Structure	ClF4- Lewis Structure