IF5 is vital molecule in the soil of chemistry. Questions about the molecule have been asked in various exams. Some of the typical questions that space asked encompass – how is the formed? Is this molecule stable? space there any uses the this compound? draw the shape of this molecule etc. There are a lot of facts the make that an exception in many cases.

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I am right here to discuss all those facts and to teach girlfriend all the is there to know about this molecule including its structure, hybridization, shape, etc.

I hope by the finish of this article, you will certainly be well versed come answer any kind of question around IF5 that comes her way!

IF5 (Iodine pentafluoride) is a colorless liquid, though part impure samples may show up yellowish. That was discovered in 1891 by Henri Moissan by burning solid Iodine in fluorine gas. The reaction is together follows:

I2 + 5F2 ——> 2IF5

It is an interhalogen compound that is used as a fluorination reagent in essential synthesis. Iodine pentafluoride (IF5) is extensively utilized in the creation of alkyl iodides comprise fluoride, which act together an intermediary in the synthetic of perfluoro-organic mixtures.

These are then used to develop water and also oil repellent emulsions for the therapy of textiles and also for fire extinguishing froths.

The molar massive of IF5 is 221.89 g/mol and its density is 3.250 g/cm3.

Boiling Point- 97.85 °C

Melting Point- 9.43 °C

IF5 Lewis Structure

Before we start making the Lewis framework for IF5, there room a few things to keep in mind.

A Lewis structure basically represents the number of valence electrons of one atom.

The easiest means to recognize the variety of valence electrons of one atom is by counting the number of columns of a periodic table left to appropriate excluding the change elements.

For example, Carbon (C) has actually 4 valence electrons, when Fluorine (F) has 7 valence electrons.

The just exception, in this case, is Helium (He) which has actually 2 valence electrons. Atoms shot to accomplish stability through the octet dominion i.e every atom should have 8 electrons approximately it.

In lewis diagrams, valence electron are represented by dots. So when we draw the Lewis diagram for the Cl atom we attract 7 dots about it.

Now we relocate on to the actions of drawing a Lewis diagram:-

1. The first step is to counting all the valence electrons of each molecule.

In the situation of IF5,

The Iodine atom has 7 valence electrons. F also has 7 valence electrons. But due to the fact that there room 5 atom of F, us multiply 7×5= 35 valence electrons.

Adding both we get 35+7= 42.

Hence, a total variety of valence electrons of IF5= 42.

2. Determining the central atom.

A central atom is typically the one come which every atom is bound to. Over there is typically only one of it in a molecule. In the situation of IF5, i (Iodine) is the central atom.

3. Draw solitary bonds come the main atom. A single bond represents 2 electrons gift shared.

4. Put every the remaining valence electron on the atoms together lone bag (2 dots).

5. Turn the lone pairs right into a dual or a triple bond so the each atom has actually its finish octet.

As a last resort, examine the formal fee of each atom. It have to be the lowest possible and have the right to be calculated by the formula offered below.


Now in the situation of IF5, we deserve to see that I no only had actually completed that is octet yet had gone beyond it by 2 electrons. We will pertained to that component in a bit.

Now us arrange the continuing to be valence electrons roughly all the atom to finish their octet. After ~ this, we observe that us still have 2 valence electron remaining.

We ar these on the main atom I together lone pairs. Hence we have completed the Lewis framework of IF5. Now notice that the Iodine atom has 12 valence electrons around it.

This is an exception to the rule of octet recognized as expanded octet’s dominance which claims that main atoms that are found in the third duration or listed below which space bound to highly electronegative terminal atoms (F) deserve to have an increased octet containing as much as 12 valence electrons.

Hence I have the right to hold approximately 12 valence electrons. Currently if you check the formal charge of each atom the comes out to it is in 0, i m sorry is the lowest value possible.

Thus the Lewis structure of any kind of compound deserve to be developed using these an easy steps!


IF5 Hybridization


The Hybridization of IF5 is Sp3d2

The hybridization the a molecule can be taken in 2 ways:-

The Theoretical part – The central atom Iodine atom has actually 7 valence electrons. Its electronic configuration in the ground state is –

I = 5s2, 5p5, 5d10

All the 7 valence electron are dispersed in the s and also p orbitals.

Now in that is excited state, since I has actually to form 5 bonds through F, 2 valence electron from the ns orbital jump (promoted) to the d orbital hence making 5 bonds v F and the electrons staying in the s orbit acting together lone pair(non-bonding), for this reason making every electrons hybridized.

Hence the Hybridization is figured out by count the number of bonds made and also the lone pair.

This contains the lone pair in the s orbital, 3 sigma binding in the ns orbital, and also 2 sigma binding in the p orbital making that Sp3d2 hybridized.

The formula to discover the Hybridization is as follows:-

H= 1/2

H= HybridizationV= variety of Valence electronsC= charge on cation or more electropositive element.A= charge on anion or an ext electronegative element.

Now if H =2, climate it reflects Sp hybridization.

H= 3, it to represent Sp2 hybridization.

H= 4, that will present Sp3 hybridization

H=5 method it isSp3d hybridized.

H=6, the molecule will have actually Sp3d2 hybridization.

In the instance of IF5,

V = 7 (valence electron of central atom)

M= 5 (5 monovalent atom of F)

Since the total charge of IF5 is 0, C and also A will certainly be zero.



H=6, indicating the its Sp3d2 hybridized. Hence, we deserve to easily discover the hybridization of IF5 using these two methods.

IF5 molecule Geometry

The molecule geometry that IF5 is Square Pyramidal. The shortcut angles formed are close come 90°.

The molecular geometry the IF5 have the right to be established using the VSEPR theory. Given listed below is the chart of VSEPR.


From the graph it is clear that IF5 is AX5E, wherein A to represent the number of the main atoms, X to represent the number of atom bonded come the central atom (5) and E represents the non-bonding electrons (lone pair).

Hence its molecular shape is square Pyramidal and electron geometry is Octahedral.

Molecular form depicts just the atom when illustration the shape whereas electron geometry depicts all electron pairs as well, hence making the octahedral.

If us deeply check, then us will notification that because of the existence of lone pair, the form of IF5 is small bent square pyramidal as shown in the listed below image.


IF5 Polarity

IF5 is a Polar Molecule.

Polarity occurs once there is a distinction in the electronegativity that the two bonded atoms the induces an electric dipole moment.

This deserve to be seen as soon as we take a look at its molecule Geometry. IF5 has actually a bending square Pyramidal shape since of lone pair and bond pair repulsion.

Notice that the 4 bonds of IF5 cancel each other out, yet there is tho one shortcut remaining.

Due come Fluorine being an ext electronegative than I, a dipole moment is induced for this reason making IF5 a polar molecule.

For more detailed information, you can refer come IF5 Polarity.

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As ns had stated in the beginning, come answer any question related to IF5, we need to know around its Lewis Structure, Hybridisation, Polarity, and also Molecular Shape. Every one of these topics have been questioned in a simple and concise manner.

Now, you should feel confident around answering any type of questions around IF5 the come her way!

I expect all her queries have been answered and if girlfriend have any doubts about any that the above concepts, feel complimentary to ask me. Happy Learning!