Question #ed8c1

1 Answer
Jul 1, 2015

Answer:

The molecular geometry of this molecule is tetrahedral.

Explanation:

The molecular geometry of #POClBrF# is identical to that of the phosphoryl chloride molecule, #POCl_3#.

The only difference between the two molecules if the fact that phosphoryl chloride has three chlorine atoms bonded to the central phosphorus atom, instead of one chlorine, one bromine, and one fluorine atoms.

So, start by drawing the Lewis structure for your molecule. The molecule will have a total of 32 valence electrons, 5 from phosphorus, 6 from xoygen, and 7 from each of the three halogen atoms.

The central phosphorus atom will be bonded to the oxygen atom via a double bond. The three halogens will be bonded to the central atom via single bonds.

The bonds will account for 10 out of the 32 valence electrons.

https://en.wikipedia.org/wiki/Phosphoryl_chloride

The rest of the valence electrons will be placed as lone pairs, two on oxygen and three on each of the halogen atoms.

The central atom is surrounded by four regions of electron density, one double bond and three single bonds, which means that it has a steric number equal to 4.

Since it has no lone pairs present, the molecular geometry will be tetrahedral.

https://en.wikipedia.org/wiki/Phosphoryl_chloride