Determine the geometry and spin of the following complex ion. Alright, so if we take a look here, we have Palladium involved. Palladium would have to have a charge of two plus and that's because the bromide ion, there's four of them, which collectively is -4. But our overall charge is 2 minus. The Palladium would have to be two plus in order to secure this 2 minus overall charge.
Alright, so we have the ion. Remember, Palladium is one of those exceptions that exists. Palladium is a neutral atom is Krypton, and the thing with it is it cannot have any electrons in its 5S orbital. Those two electrons are promoted up to the 4D orbitals, so it's really 4D10. Two plus means we've lost electrons from our highest shell number here, so now it's going to be Krypton 4D8. So this is AD8 ion.
And remember, if your D8, that means your geometry is square planar. So we know that geometry is square planar, and then we have to talk about the spin. Here we'd say because it's square planar, they typically have high crystal field slitting energy, which means that they will result in a low spin complex. So here this is what we can say in terms of this particular complex ion.
Now if we were to fill this out, we would see that there would be some unpaired electrons which would actually give us a perimagnetic orientation. But remember, with square planar and basically with our tetrahedral species, we could talk about the spins of them and typically square planar should have a diamagnetic orientation, but that's not always certain as we can see here. And that's because Palladium is one of those elements. That's just an exception to the electron configuration setup. So it kind of throws everything out of whack.
So here in this particular case, all we need to know is that this is a square square planar species and that it has a low spin complex.