Polarity, Science

Is BrF5 Polar or Nonpolar?- Bromine Pentafluoride Polarity Explained

Is BrF5 Polar or Nonpolar- Bromine Pentafluoride Polarity Explained

The chemical formula BrF5 represents Bromine Pentafluoride. It is an interhalogen compound and a strong fluorination agent. Interhalogen compounds comprise two or more different halogen atoms and no atoms of elements from other groups. 

BrF5_Lewis-structure_

BrF5 is prepared by treating Bromine with large amounts of Fluorine at temperatures of over 150°C. It reacts violently with water but produces Bromic Acid and Hydrofluoric Acid upon dilution. 

It finds use in analytical studies and practical applications. Being a strong fluorinating agent, it reacts with Uranium to form Uranium Hexafluoride. This is then used to enrich Uranium.

We say that Bromine Pentafluoride is polar. Let’s see why that is the case.

To determine the polarity of BrF5, we must first account for its Lewis Structure and properties. These properties include its electronegativity, its molecular geometry, and its resulting dipole moment if any.

Electronegativity and Bond Nature

To determine if the bonds present in BrF5 are polar or non-polar, we look to the periodic table. The difference in charges between the Bromine and Fluorine atoms is 1.02

Now, in accordance with the Pauling scale, this tells us that the Bromine- Fluorine bond in the BrF5 ion is polar. 

Molecular Shape and Symmetry

BrF5 comprises Bromine as the central atom with 5 Fluorine atoms surrounding it. It also has two unpaired electrons which att

ach themselves to the central atom, Bromine, as a lone pair.

BrF5_structure

Bromine Pentafluoride has a square pyramidal molecular geometry. The presence of a lone pair creates a region of negative charge that remains unbalanced. Therefore, it is structurally unsymmetrical making it a polar molecule.

Net Dipole Moment in BrF5

There is a net dipole moment as there is asymmetric charge

 distribution due to the presence of the lone pair. 

BrF5polarity_

It’s asymmetrical square pyramidal structure also contributes to a net dipole moment. 

Conclusion

As shown above, due to its asymmetrical square pyramidal structure and the presence of a lone pair, BrF5 is considered a polar molecule.

The difference in electronegativity between the Bromine and Fluorine atoms also contributes to unequal charge distribution on the central Bromine atom.

Therefore, this proves that BrF5 is a polar molecule.

 

 

Priyanka

About Priyanka

To read, write and know something new everyday is the only way I see my day ! Well that rhymed. Hey folks, this is me, Priyanka, writer at Geometry of Molecules where I want to make Chemistry easy to learn and quick to understand. Having a MSc degree helps me explain these concepts better. I write all the blogs after thorough research, analysis and review of the topics. And if not writing you will find me reading a book in some cozy cafe !

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