Why does the maximum oxidation state peak at +7 and then fall by one to Cu? I understand how Mn is able to lose 7 electrons but Fe technically has 8 electrons to be ionised.
@@MSJChem yes but the rules of empty, half-filled or filled subshells being stable don't seem to apply here as the electrons are able to be ionised easily within Mn. Would the reason be simply outside the scope of the course?
@@derrickmah3565 I believe to find the maximum oxidation state of a transition metal, u have to find the no.of unpaired electrons in the 'd' sub shell and then add 2, eg: manganese has 5 unpaired electrons in the 'd' subshell and then we add two and that's why it has a max oxidation of state 7
![S3.1.8/9 Why do Transition Metals Have Variable Oxidation States? [HL IB Chemistry]](http://i.ytimg.com/vi/0FPYIB9_fPY/mqdefault.jpg)
How do V, Cr, Mn, Fe, Co and Ni have +1 ? I thought those start from +2. That's what my book and my teacher says
Good video with well explanation 👍🏼
Why does the maximum oxidation state peak at +7 and then fall by one to Cu? I understand how Mn is able to lose 7 electrons but Fe technically has 8 electrons to be ionised.
I would guess it has something to do with ionization energy or the stability of the ion formed.
@@MSJChem yes but the rules of empty, half-filled or filled subshells being stable don't seem to apply here as the electrons are able to be ionised easily within Mn. Would the reason be simply outside the scope of the course?
@@derrickmah3565 I believe to find the maximum oxidation state of a transition metal, u have to find the no.of unpaired electrons in the 'd' sub shell and then add 2, eg: manganese has 5 unpaired electrons in the 'd' subshell and then we add two and that's why it has a max oxidation of state 7
@@barcaboy8264 ok but why does that formula work?
@@derrickmah3565 sorry but idk, that's just how we're learning it, but the plus 2 that we add is from 2s subshell.thats all I know
Hi , do i have to know the oxidation states?
Of the transition metals? There is a list of them in the data booklet but it wouldn’t hurt to know the common ones such as for copper and iron.
@@MSJChem thank you soo much
Why can't Sc lose 2e from 4s orbital to have +2 oxidation state?
Probably because the Sc2+ ion would not be stable with only one electron in the 3d sub-level.
No it's because the energy too remove that third electron from 3d is so similar to the ines on 4s
Doesn't the 29Cu has maximum oxidation state +2 ????
Copper in compounds with +3 oxidation state does exist but it is not common. The +1 and +2 oxidation states are the common ones.
Why nickle does not show 5 oxidation state
To be honest I don’t really know. I’m sure with a bit googling you’d find the answer.
Why is oxidation state important, what does it tell?
good video
Hi sir 👋