Question

Explain the formation of sf6 and pcl5 molecules with their hybridisation structures

Answer 1

Answer:

Formation of PCl  

5

​  

 (sp  

3

d hybridization): The ground state and the excited state outer electronic configurations of phosphorus (Z=15) are represented in Figure 1.

Three P—Cl bond lie in one plane and make an angle of 120  

o

 with each other; these bonds are termed as equatorial bonds. The remaining two P—Cl bonds—one lying above and the other lying below the equatorial plane, make an angle of 90  

o

 with the plane. These bonds are called axial bonds. As the axial bond pairs suffer more repulsive interaction than the equatorial bond pairs, therefore axial bonds have been found to be slightly longer and hence slightly weaker than the equatorial bonds; which makes PCl  

5

​  

 molecule more reactive.

Hope this will help you

Answer 2

The hybridization of the P

$PCl_5 \: is \: sp³d$

and the hybridization of the S in

$SF_6 \: is \: sp³d²$

• Phosphorus Penta chloride has trigonal bipyramidal geometry. In this case, the axial bonds are slightly longer than the equatorial bonds. This is because the axial bonds experience greater repulsion from other bonds than the equatorial bonds which makes PCl_5 molecule more reactive and geometry as shown in Figure.
• Formation of Sulphur Hexafluoride Molecule has a regular octahedral geometry . It is a type of greenhouse gas which is colourless, odourless, non-toxic and non-flammable. It is also an inorganic and non-polar gas as shown in Figure.

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