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Describe the hybridization in case of Pci_(5) Why are the axial bonds longer as compared to equtiorial bonds ? OR Explain sp^(3)dhybridization by suitable example. Discuss about hybridization and shape of PCl_(5) . |
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Answer» Solution :Electron CONFIGURATION of phosphorus [Ne] `3s^(2) 3p^(3)` : Electron configuration of ground and exicted state (P = 15).  Hybridization in Phosphorous: In excited state of phoshorous one 3s, and three3p orbitals and one 3d orbitals having less DIFFERENCE in their energies mix together and form `sp^(3)`d HYBRID orbitals forms. Five new `sp^(3)`d hybride orbitals forms. All these five orbitals. has trigonal bipyamidal geometr which has `120^(@) and 90^(@)` bond angle.  Corners of pentagonal bipyramidal ARRANGEMENT. Bond formation in `PCl_(5)` : Each `sp^(3)` d hybrid orbital overlap with half filled p orbital of chlorine and form five P-Cl covalent bond.  Shape : In `PCl_(5)` like `sp^(3)` d hybridization all five bonding orbitals are arrange in trigonal bipyramidal shape.  Bond angle : From five P - Cl bonds three P - Cl bond are in same plane remain in planar trigonal & bond angle between them is `120^(@)`. All these three bonds are equational. Remaining two P- Cl one bond is above the plane and other is below the plane. So these two P-CI bond from `90^(@)` angle with plane. these two bonds are called axial bonds. Bond length : P - Cl axial bonds elector pair experiences more repulsion than equatorial bonds. So these are slightly longer them equatorial bonds. As the bond length of axial bonds is more so these bonds are WEAK and hence those bonds are highly reacitve. |
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