The chemical compound PF5 is additionally known as Phosphorus Pentafluoride. It is one of the most important phosphorus halides. PF5 is a colorless gas toxicity in nature and form fumes in the air. It is very dangerous because that the eyes and likewise causes sickness ~ above inhalation. In this article, us will examine out the price to whether PF5 is a polar or nonpolar compound.

You are watching: Determine the molecular geometry of pf5.

So, is PF5 polar or nonpolar? Phosphorus pentafluoride or PF5 is a nonpolar compound since of its symmetrical geometry ie; Trigonal Bipyramidal. Back the P-F shortcut is polar together the F atom is more electronegative than the p atom, the entire PF5 molecule is nonpolar because the dipole the the P-F bond gets canceled out by every other leading to the zero net dipole moment making the a nonpolar molecule.

It exists together a compound v an irritating odor and forms highly toxic fumes in the air. It violently reacts when the hydrolysis reaction takes place.

PF5 is extremely reactive come water by nature and forms phosphoric and also hydrofluoric acid, phosphoric mountain as an end result of an exothermic reaction producing heat.

This PF5 compound can be easily acquired by fluorination that phosphorus pentachloride through the help of arsenic trifluoride.

3PCl5 + 5AsF3 ——> 3PF5 + 5AsCl

PF5 can also be synthesized by the procedure of fluorination that PCl3 through anhydrous hydrofluoric acid through the presence of Chlorine. This process ensures a high PF5 conversation rate.

Why PF5 is nonpolar?

The electron traction balances out electronegativity, in both the vertical and also horizontal axis of the Phosphorous Pentafluoride molecule.

One of the axis of the PF5 molecule drops to be linear while the various other one forms a triangular shape which outcomes in a no network dipole moment.

The molecule tote no dipole charge since of the cancellation of the dipole moment produced by each P-F bond.

The molecule geometry the Phosphorous Pentafluoride (PF5 ) is trigonal bipyramidal.

PF5 has symmetric charge circulation of Fluorine atoms approximately the main atom Phosphorous.

As charge circulation is equal and also there is no net dipole minute therefore, this molecule is nonpolar.

Although the P-F shortcut is polar in nature due to distinctions in your electronegativity, the dipole that P-F bonds gets canceled the end by each other as result of the symmetric framework of the whole PF5 molecule.

Points to determine the polarity of PF5

Generally, a nonpolar molecule has the bond sharing equal electronegativity in participating atoms.

Though if atoms are arranged such the polar bonds vector sum cancels out itself then also a molecule i do not care nonpolar.

Here, in PF5 the bonds room symmetric however due come the electronegativity of fluorine being higher than phosphorus atom, the molecule has actually polar bond canceling your vector sum.

This cancellation is responsible because that nonpolar nature together there is no dipole moment and also lone pair that electrons.

Due come this, PF5 develops a trigonal bipyramidal geometry consists of a pair the equatorial and also axial bonds.

As this horizontal and vertical bond cancel the end their charges, the molecule has actually no network charge.

Due to no network charge, the entirety molecule has actually a nonpolar nature creating polar covalent bonds.

Hybridization the Phosphorus Pentafluoride (PF5)

If we check out the lewis structure of this molecule!


In PF5, the Phosphorus atom has a full of 5 valence electrons and fluorine has actually 7 electrons in that is outermost shell. One electron is common by every fluorine atom to complete its octet.

The facets present in the third period comprise that d orbitals together with s and p orbitals in the regular table.

It is prominent that every bond angle of 90 degrees and also 120 degrees formed in trigonal bipyramidal geometry room not identical.

So, the 5 sp3d orbitals that phosphorus overlap v the ns orbitals the fluorine atoms. These ns orbitals space singularly occupied and together they form all the 5 P–F sigma bonds in PF5.

Hence, the PF5 molecule has a sp3d hybridization and also a trigonal bipyramidal geometry shape.

The Dipole moment of Phosphorus Pentafluoride

Both atom ie; Phosphorus and also fluorine differ in your electronegativity. Electronegativity of the fluorine atom is 3.98 and also that the phosphorus is 2.19.

Thus, the P-F bond is polar in nature.

The polarity that the P-F polar binding cancels the end each other because of the trigonal bipyramidal geometry that the molecule.

Since the molecule Phosphorus Pentafluoride (PF5) is symmetrically arranged around the main (P) atom, over there is no charge dispersed unevenly.

So, PF5 has no network (i.e. Zero) dipole moment.

CBr4 (Carbon tetrabromide) is likewise a comparable compound having actually polar C-Br bonds with some dipole moment value yet the whole molecule is nonpolar due to the fact that of the net-zero dipole.

Check out the article regarding the polarity that CBr4.

Why PF5 is nonpolar even with an odd variety of vectors approximately the central atom?

This is due to the fact that of the 3-dimensional arrangement (i.e. Ball and also stick diagram) the PF5.

We know that F is much more electronegative 보다 P, thus the bonds developed in PF5 space polar, but the molecule as as whole is nonpolar. Why?

Due to the arrangement of F atom in PF5 such the it develops a trigonal bipyramidal molecular geometry wherein electrons are mutual equally.

Thus, no dipole charge is produced and hence the link PF5 is nonpolar even with an odd number of vectors.

One such element with an odd variety of vectors about a main atom is BCl3 that also lies under the group of the nonpolar compound.

Read the end the short article for the polarity of BCl3.

Below is the picture of the PF5 Ball and also Stick Model


Why does PF5 exist together gas (covalent) conversely, PCl5 exists as ionic solid?

In both the molecules, Phosphorus is a usual atom yet both compounds different in the halogen.

Chlorine and fluorine have actually the exact same valence electrons however the size of the fluorine atom is smaller sized as compared to chlorine.

As a result, the electron density in fluorine is much more than chlorine because of which PCl5 has actually a lower polarizing aspect resulting in a an ext ionic character.

Whereas fluorine being a smaller-sized atom has an ext electron thickness brings the end a much more polarising nature and an ext covalent character and it exists in gas form.

Why PF5 is dubbed a attention or toxic substance?

This colorless Phosphorus Pentafluoride is thought about to be an very dangerous substance, as result of its violent reactivity through water.

It is corrosive to human skin and highly toxic as soon as inhaled. That is corrosive come eyes and also skin and damage eyes.

Hence, Phosphorus Pentafluoride (PF5) should be stored in sealed stole cylinders to stop its contact with water or even humidity.

If the substance it s okay in contact with water, one exothermic reaction bring away place developing poisonous fumes and sufficient heat to burn any combustible substance.

Hence, that is a danger compound the reacts violent to hydrolysis.

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Phosphorus Pentafluoride is supplied as a fluorinating agent provided in various commercial chemical reactions. The compound is nonpolar in nature because of the symmetric geometrical structure. All the 5 fluorine atom lie symmetric come the main phosphorus atom. The is toxic to inhale. PF5 has zero dipole moment. That is a totally nonpolar compound creating polar covalent bonds.