Introduction to transition metals
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- เผยแพร่เมื่อ 8 ก.ค. 2024
- Transition into this! A quick look at what the difference is between a transition metal and d-block element. Also looking into electron configuration of ions and elements including Cr and Cu (the unusual elements).
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I'm confused about Zinc. Wouldn't the Zn2+ ion have the configuration [Ar] 4s2 3d8, therefore it would have a partially filled d sub shell and be classed as a transition metal? Do the 4s2 electrons move into the d sub shell to fill it?
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Hi
With scandium, can't you get a 2+ ion since by removing 2 electrons, you would still have that one electron in the 3d-subshell?
Wouldn't this be a partially filled 3d-subshell and hence a stable ion.
This was so helpful thanks a lot
Absolute don. Cheers mate
does it matter which order you write the 3d and 4s in when writing out electron configurations?
I noticed that, for example, you wrote the 4s before 3d in chromium and copper, but for manganate you did the opposite.
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Thank you.
With the new specification for AQA A- level Chemistry, are Scandium and Zinc still not transition metals because I saw a powerpoint which included them as Transition metals and I don't know whether to learn them or not?
The textbook says no so ..
very helpful presentation
Thanks!
so is the electronic configuration of scandium [Ar]4s23d1??
Yes
Thank you so much!!!
You're welcome!
In an exam do you write the electron configurations for copper and chromium with 4s1 going before the 3d sub level or after. Just a bit confused my teacher taught it differently, great video
Either to be honest. Normally it is numerical order though.
why is it that we remove the electrons from 4s orbital first, when we're told that 3d has a higher energy and is filled up after the 4s (when working out the electronic configuration for the atoms), so wouldn't it make more sense for the 3d electrons to be removed first since based on that logic they have the higher energy?
Excellent video, very helpful and concise. However i would suggest a better microphone or some sound proofing as the audio is a bit scratchy at some points. Hope this helps.
thank you
Which orbotal has higher energy s/d?
1s < 2s < 2p < 3s < 3p < 4s < 3d
Hi. Is there a difference between a transition metal and a transition element. Is a transition element not an element that has an incomplete d sub shell either in the element or in one of its stable ions?You mentioned that Scandium is not a transition metal. However, it does have a partially filled 3d sub shell right? Sorry a bit confused by this, Thanks for your videos btw! :)
+Rhea Jain No difference. Scandium is not a transition element as it's ion Sc3+ has an empty d orbital. Scandium is a d block element but not a transition metal. Hope this helps! ☺
+Allery Chemistry Great thanks for the quick reply :)
+Rhea Jain You're welcome.
You are one great teacher. Thank you so much for these videos. Please can you write just a little bigger... Please
I'm confused. You said that "d-block elements are any element that has its outer most electrons in a d-orbital". I'm looking at the electron configurations and it appears that the outer most electrons of d-block elements are in the 4s orbital as this is furthest from the nucleus and hence the highest energy level?
+John Lad When we fill up the orbitals we fill the 4s first as it is of slightly lower energy (closer to nucleus) when removing electrons the energy levels change and it becomes easier to remove from 4s than 3d as it is now highest energy level (by a whisker). What I am saying is that the 2 levels are so close to each other in terms of energy that they can swap places in an energy level diagram depending on what you are doing to it. d-block elements have electrons that sit in the d-orbital. In fact the electron config can be written as 3d,4s OR 4s,3d in the eyes of AQA. I suspect this may be the case for others too, that's how close they are in energy! Hope this helps.
thank you :)
You're welcome!
thanks
+Shah. F no probs!
Thank you sir
Welcome
Amazing content as always!
I have a confusion in this. as you stated anything with incomplete D orbital is a T.E
And then you said a complex is a compound with a transition element in the center with ligands joined by covalent bond and drew a compound with Cu.
what concept am i missing since to the best of my knowledge Cu shouldn't be a TE in the first place.
+fatima khan Cu is a transition element.
+Allery Chemistry I'm a special kind of stupid. Thankyou! :)
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Sonil Zaki Thanks!
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great video but in the ocr textbook it says Fe2 = pale green Fe3+ = yellow
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i don't understand what you mean by the configuration of Argon?are you saying all those elements and ions you showed have the configuration of argon because they don't so please help me please Chemistry God!!! Your videos are wow
Why is nickel [Ar] 4s2 3d8?
And not,
[Ar] 4s0 3d10
The D orbital can fill up 10 electron, so why doesnt it? It's slightly confusing.
Sonil Zaki A good question that thankfully you don't need to explain just recall. The explanation is complex and follows the Aufbau principle and governed by Hund's rule which states electrons will arrange themselves in orbital to have the lowest energy but occupying singly occupied orbital first. Briefly, the energy required to fill the 3d orbital by moving 2 electrons from the 4s is higher than the energy when only one electron is moved to form a complete d orbital.
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helpful video but i wish the audio was better
PFFT who needs school when we have you lol