Question

Predict the number of unpaired electrons in pt cn 4 2- ion

Answer 1

Hey.

In this complex, Pt is in the +2 state. It forms a square planar structure. This means that it undergoes dsp2 hybridization. Now, the electronic configuration of Pd(+2) is 5d8.

CN - being a strong field ligand causes the pairing of unpaired electrons.

Hence, there are no unpaired electrons in [Pt(CN)4]2-

Thanks.

Answer 2

Answer:

Zero unpaired electron

Explanation:

As the compound will be dsp2 hybridised having one empty orbital in 5D leaving zero unpaired electron in 5D .

Hence it become diamagnetic having zero dipole moment.

Hope it's clear

Mark me brainliest