Just finished the IB exams a few days ago. I want to thank you for making these videos. They're a godsend for me who is never good at Chem. Thank you Mr. Thornley.
Hi Mr. Thornley, at min 4:01, you mention (and is already written in the video) that Ti3+ has an electron configuration of: (Ar) 3d2, but shouldn't it be 3d1? And for V2+, shouldn't the electron configuration be: (Ar) 3d3, as V only lost 2 electrons - the 4s2 (due to the V electron config. which is: (Ar) 4s2 3d3)? Thanks :))
Why does iron have a bigger split? Since it has more protons, doesn't that mean it'll pull the electrons closer to the nucleus making the split smaller?
@@rohinikayal4440 I’m not 100% sure about this answer but maybe it’s because difference of energy level is not correlated with the physical distance between the shells
I would think that because there are more protons, there is more pull on the electrons offered by the ligands and thus, as these electrons come closer to the nucleus, the repulsion between ligand electrons and 3d electrons of the central metal ion increases, which increases the split.
The fourth reason is the shape of complex, also sometimes the solvent, temperature, and the concentration will change the complex colour, particularly with main group complexes. Thanks for your fundmental vedio
Does the difference in protons outweigh the relevance of ligands in what colour the complex will absorb? Like if two complexes have different Ligands but also different metals, will the higher proton metal absorb more energy?
@@ibchemvids Ya I mean how is the blue light in the case of Copper Sulphate for instance getting re-radiated perpetually? Are the valence electrons jumping all the time?
Hello, first of all thank you for the videos they are extremally useful. i would like to know if we have to memorise the complex examples for Chemistry HL?
+katei m. From the syllabus:"Students are not expected to recall the colour of specific complex ions. " The syllabus is unclear about memorizing examples. I would memories the Cu2+ ions with water being replaced by ammonia.
You would need to know the charge of the ligands to get the OS of chromium. eg [Cr(CN)6]4-, each CN is really CN-, so this accounts for -6, when this is added to the OS of Chromium you need to get -4. So chromium must be +2
Hi Mr. Thornley, just a quick question. Is it the binding of the ligand to the transition metal that causes the electron to be promoted or is it the absorption of the specific colour?
Thankyou! That's was very helpful indeed. But there is one thing I'm still confused on: will a metal with a higher or lower oxidation state produce a larger d-orbital split? And why?
Thanks a lot for the video, however there is a small error. At around 6.54 you transferred the electron from the s-sub shell whereas I think you are supposed to transfer the excited electron from the d-sub shell. Great video anyways!
more protons means bigger gap, it absorbs light with bigger energy. (the color you see, it's the light it did not absorbs.) With only this information, we don't know what color it will be, unless we have a complex with information to compare with. ( I hope it helps, even it's one year later)
![S3.1.10 Why are Complexes Coloured? [HL IB Chemistry]](http://i.ytimg.com/vi/Kq_tKki1syE/mqdefault.jpg)
![S3.1.10 Why are Complexes Coloured? [HL IB Chemistry]](/img/tr.png)
![S3.1.6 How do I Assign Oxidation States? [SL IB Chemistry]](/img/n.gif)
Just finished the IB exams a few days ago. I want to thank you for making these videos. They're a godsend for me who is never good at Chem. Thank you Mr. Thornley.
The 6 dislike are the bad chem teachers who wish to teach this well
It helps a lot, thank you! I WILL SMASH THE TEST!
Hi Mr. Thornley, at min 4:01, you mention (and is already written in the video) that Ti3+ has an electron configuration of: (Ar) 3d2, but shouldn't it be 3d1? And for V2+, shouldn't the electron configuration be: (Ar) 3d3, as V only lost 2 electrons - the 4s2 (due to the V electron config. which is: (Ar) 4s2 3d3)? Thanks :))
Yes I think he accidentally swapped the charges for Ti and V.
Why does iron have a bigger split? Since it has more protons, doesn't that mean it'll pull the electrons closer to the nucleus making the split smaller?
I have the same question, can you please explain this question @Mr. Thornley ???
@@rohinikayal4440 I’m not 100% sure about this answer but maybe it’s because difference of energy level is not correlated with the physical distance between the shells
I would think that because there are more protons, there is more pull on the electrons offered by the ligands and thus, as these electrons come closer to the nucleus, the repulsion between ligand electrons and 3d electrons of the central metal ion increases, which increases the split.
Messiah of Chemistry
The fourth reason is the shape of complex, also sometimes the solvent, temperature, and the concentration will change the complex colour, particularly with main group complexes.
Thanks for your fundmental vedio
Hi! Very very goooooooood
Thank you so much for this video, it really cleared my concept on this topic!
Does the difference in protons outweigh the relevance of ligands in what colour the complex will absorb? Like if two complexes have different Ligands but also different metals, will the higher proton metal absorb more energy?
But why does the light keep getting emitted perpetually?
No light is emitted, just selectively absorbed (then reradiated as IR as the electron takes small jumps back down).
@@ibchemvids Ya I mean how is the blue light in the case of Copper Sulphate for instance getting re-radiated perpetually? Are the valence electrons jumping all the time?
Hello, first of all thank you for the videos they are extremally useful. i would like to know if we have to memorise the complex examples for Chemistry HL?
+katei m. From the syllabus:"Students are not expected to recall the colour of specific complex ions. " The syllabus is unclear about memorizing examples. I would memories the Cu2+ ions with water being replaced by ammonia.
Thanks, this video was amazing
Why does the [V(H2O)6]2+ absorb yellow light but [Cr(H2O)6]3+ absorb red light even though Cr(III) has larger proton number ?
I have a question 7:55 how did you know the oxidation state of the Chrominum. Thanks Anyways Your Videos are good!!!
You would need to know the charge of the ligands to get the OS of chromium.
eg [Cr(CN)6]4-, each CN is really CN-, so this accounts for -6, when this is added to the OS of Chromium you need to get -4. So chromium must be +2
how do we know that the Protons indicate which colour?
Hi Mr. Thornley, just a quick question. Is it the binding of the ligand to the transition metal that causes the electron to be promoted or is it the absorption of the specific colour?
The ligand binding causes the electrons orbitals to split apart. The absorption of light then promotes the electron.
that video rather makes me listen to wasted years!!
im not sure but i think you mixed up the electron config of titanium co titanium 3+ only has one electron left in the d subshell
good
yeahh exactly i was confused as well
thanks....an extremely useful video
I just am confused on how do I know which color is absorbed
the colour absorbed is the complementary colour of the one that you see
very helpful
Thankyou! That's was very helpful indeed. But there is one thing I'm still confused on: will a metal with a higher or lower oxidation state produce a larger d-orbital split? And why?
the lower the oxidation state, the smaller the split (and vice versa). You can just search up the reason on google :)
because the less interaction with the ligands
he says it in the video haha 6:49
Hi sir, is always "one" electron promoted towards upper energy level after ligand attatched?
In HL IB Chemistry - yes. In real life I would think that more than one is possible if there is space and enough electrons and energy to excite.
ti+2 and V+3 are isomeric .
ti+3 and V+2 are not isomeric
Thanks a lot for the video, however there is a small error.
At around 6.54 you transferred the electron from the s-sub shell whereas I think you are supposed to transfer the excited electron from the d-sub shell. Great video anyways!
@Shaurya LEEKHA My bad, thanks for the clarification
wait ti3+ and V2+ are not isoelecrtonic what are you talking about.
I added a "card" a while back to correct the error - but it does not show on the video if watched on a mobile device
can you plz explain that how
more protons means bigger gap, it absorbs light with bigger energy. (the color you see, it's the light it did not absorbs.) With only this information, we don't know what color it will be, unless we have a complex with information to compare with. ( I hope it helps, even it's one year later)
thank you
I dont know why but this @7:36 creeped me out
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