Question

What is the hybridisation of [PtCl4]2- and how?

Answer 1

Electrons in valence shell of Pt i.e 4d is eight and 5s is 2. Here valency of Pt is +2.
So electrons of 5s becomes zero.
For 4d and 5d series all ligands act as strong ligands hence pairing occur. The 2 unpaired electron in 4d of Pt get paired and hence there is one vacant orbital.
Hence one orbital of 4d, 5s and two orbitals of 5p participates in hybridization,
-> resulting in dsp2 type of hybridization and square planar geometry.

Hope it helps.

Answer 2

The Hybridisation of $(PtCl_4)^{-2}$ is $dsp^{2}$ and it has structure of square planar .

Reason - See the attach file for reason , there are only 4 atoms of ligand i.e cl which get attach to Pt at last 4 position and also it pairs the electrons of Pt since it is strong ligand.

Hope it will help u ....

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Best of luck ;)
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