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Report (any type)/Brief report
22/09/2021
Because of the lone pairs of electrons present on the oxygen atom.
Oxygen difluoride, ##”OF”_2##, is a polar molecule because it has a bent .
This ensures that the dipole moments associated with the oxygen – fluoride bonds do not cancel each other out to produce a nonpolar molecule.
To see why this is the case, draw the molecule’s . The molecule will have a total of ##20##
The oxygen atom will take the role of central atom, forming single bonds with the two fluoride atoms. These bonds will account for ##4## of the molecule’s ##20## .
The resulting ##16## electrons will be placed as lone pairs
Now, it is very important to realize the Lewis structures are not meant to to convey molecular geometry!
In order to find the molecule’s geometry, you count the regions of electron that surround the central atom – these will give you the atom’s steric number.
Regions of electron density are bonds to other atoms (here single, double, or triple bonds count as one region) and lone pairs of electrons.
In your case, the central oxygen atom is bonded to two other atoms and is surrounded by two lone pairs ##->## it has a steric number equal to ##4##.
According to , this corresponds to an ##”AX”_2″E”_2## molecular geometry, which is characteristic of a bent molecule.
Now, the difference in between fluorine and oxygen ensures that the two ##”O”-“F”## bond are polar. The bent molecular geometry will cause the two dipole moments to add to each other.
The result will be the formation of a permanent dipole moment, and thus a polar molecule
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I want to thank your team (Jeff) for finding a new writer when you were unable to reach my existing writer to revise my paper. I appreciate your professionalism and efforts. Thanks
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