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5) (20 Pts) a) Ni(II) tends to form a variety of complexes w square-planar geometries, while Pd(IID) and PtII) form predomina
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5) a) Nickel uses it's 3d orbital for complex formation , so not that much electron density can be stabilized by those d orbitals and due lower in energy of d orbital , the crystal field spilitting is not that much. For Pt(+2) or Pd(+2) , the size of the d orbitals is bigger than that of Nickel , which can stabilize much more electron density than Nickel.They use 4d orbitals for complexation.Moving from up to down across the periodic table , it is seen that the crystal field splitting gets higher up and so , due to Jahn Teller distotion , only square planar complexes are formed for Paladium and Plainum in comparison with Nickel though they all have d8 configufration.

b) We know , lower the size of atom and higher the charge , lesser the stability. Hence Nickel has lower size than that of Paladium or Platinum. Being bigger in size , Paladium and Platinum can afford higher charge._ dus az den du square-plorer cugtal iead sputing spliting

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