Paramagnetic or diamagnetic
Started by anteater85
That's what I thought but both are diamagnetic
Isn't paramagnetic one arrow and diamagnetic 2 arrow in an orbital?
3 see up/down, up/down, up/down, up, up
I think this is paramagnetic.
3 see up/down, up/down, up/down, up, up
I think this is paramagnetic.
If all the electrons are paired, then it is diamagnetic (i.e. a noble gas). however, if not all the elctrons are paired (i.e. Fe+2), then ti is paramagnetic.
Sorry forgot ot finish haha: http://www.britannica.com/EBchecked/topic/442927/paramagnetism
according ot encyclopeida brittanica, Pd and Pt are paramagnetic.
according ot encyclopeida brittanica, Pd and Pt are paramagnetic.
Here is what it says in the AP cliff book about the Pd, it has 46 electrons and an electron configuration [46]4d^10. Since the d orbitals are completely filled, Pd would be diamagnetic..
wth...how many exceptions are there?
There is no charge
Acutally, read this: http://chemed.chem.purdue.edu/demos/demosheets/6.3.html
Apparently, if an element has an even number of electrons, there is a possibility thatall the electrons could pair up, so it is diamagnetic.
Ok thx dude.....I don't know how i'm gonna remember all these rules for the test
I think this is about 5s2 4d8 vs. 4d10.
I guess 4D10 is more stable because it has D orbitals completely filled.
But I wonder why Ni would still have 4s2 3d8 instead of 3d10.
I guess 4D10 is more stable because it has D orbitals completely filled.
But I wonder why Ni would still have 4s2 3d8 instead of 3d10.
When you're filling up orbitals, you'll always fill up s first then go to d (two exceptions are when you get both of them to be half full like 4s13d5 instead of 4s23d4 and 4s13d10 instead of 4s24d9.
When taking electrons out, you will always remove s first (whether you have one or two), then head to taking out the d electrons.
I meant to post this on the other thread and not here, but whatevz.
When taking electrons out, you will always remove s first (whether you have one or two), then head to taking out the d electrons.
I meant to post this on the other thread and not here, but whatevz.
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The same reason oxygen is 2s2 2p4 and not just just 2p6. First of all Aufbau's rule, and conceptually, the energy between the s and p sub-shells is larger than the stabilizaiton energy u would get if you just had a "FULL" orbital of higher energy.
