madhav makkena Thanks very much. Please spread the word about these videos. If you are on twitter follow me @allerytutors to hear about what videos are being made before everyone else.
Your videos are AMAZING so thank you very much for this!! Do you have a playlist of videos for 'Organic synthesis and analysis' for A2 chemistry (AQA)?? do you also know of any online Biology tutors like your self? thanks
+iram khan Thanks for your kind words! Organic synthesis is something I am working on. It's a tricky one to do due to the vast scale of reactions. I quite like Mr Pollock Biology channel. Very clear and concise. Hope this helps!
+A Level Chemistry by Allery Tutors thank you :) I was looking at the podcasts on the allery tutors website but I couldn't find any for A2; only for AS?
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.
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! ☺
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?
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?
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.
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.
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?
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.
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.
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
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.
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
This man has godly powers to make anything easy....
Heh! Pleased I have made this easy for you! Chemistry doesn't have to be difficult.
Soo helpful, wish you could've been my Chemistry teacher! I have probably learned more in this 12 minute than I've in an hour of lesson time.
+KaBoom Thanks very much! Pleased it helpers, share the vid with people who you know will also find it helpful. 🙂
8 years later and just as useful!!
I am more than grateful for your existence right now. What a blessing!😩
+Kamara E. Thanks! Please share this channel to others who may benefit too!
You have just saved my whole chemistry a level!! Thank you for the great videos :) already shared them with others who are struggling!
You're very welcome! Hope your exams are going well and thanks for sharing!
Brilliant for self study. Thank you for your great posts.
Well done on self studying! Glad they are helping you.
Thank you soo much sir i never knew an angel like you exist but now i know !!!!!!!
Heh cheers. I'm no angel but I do like teaching chemistry! 😀
you are the singular reason why im make it out of chemistry alive
your videos are very helpful . thanks allery tutor
+Shakeel Ahmed Thanks!
thank you..... your videos are helping me so much...
madhav makkena Thanks very much. Please spread the word about these videos. If you are on twitter follow me @allerytutors to hear about what videos are being made before everyone else.
Your videos are AMAZING so thank you very much for this!! Do you have a playlist of videos for 'Organic synthesis and analysis' for A2 chemistry (AQA)?? do you also know of any online Biology tutors like your self? thanks
+iram khan Thanks for your kind words! Organic synthesis is something I am working on. It's a tricky one to do due to the vast scale of reactions. I quite like Mr Pollock Biology channel. Very clear and concise. Hope this helps!
+A Level Chemistry by Allery Tutors thank you :) I was looking at the podcasts on the allery tutors website but I couldn't find any for A2; only for AS?
+iram khan Yes I have only done them for AS to reflect the new specifications. The A2 new spec will be released next academic year.
Finally! Someone who also says the word 'Haber' correctly! (People usually say it like 'Harber')
Your videos are awesome!!!!! Thank you so much!
+Esther Jose Thanks very much! Glad they are helping. Please help by spreading the word about these videos.
A Level Chemistry Revision Videos by Allery Tutors Sure! :)
I love this guy.When my teacher teaches me i think im an idiot but now i feel smart bcs i understand
Awesome Sir...
+kalim Khan Thanks very much! Please spread the word about these vids! ☺
very helpful presentation
Thanks!
whys the quality so good when its been 5 years
Thank you, your videos has been very very very helpful :)
+Dr Spinz No problem. Please spread the word!
+A Level Chemistry Revision Videos by Allery Tutors I will!
Absolute don. Cheers mate
a great video brother..thanks..keep going.
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.
really impressive, thank you
Ur videos are soo good thank you soo much
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.
Which orbotal has higher energy s/d?
1s < 2s < 2p < 3s < 3p < 4s < 3d
so is the electronic configuration of scandium [Ar]4s23d1??
Yes
thank you. thank you so much. I wish I could meet you and give you the world.
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?
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?
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.
A Level Chemistry Revision Videos Thank you.
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! :)
+fatima khan Don't worry about it. It happens to us all.
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 ..
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.
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.
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.
thank you, your videos are so helpful!
You are one great teacher. Thank you so much for these videos. Please can you write just a little bigger... Please
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.
This was so helpful thanks a lot
Thank you, this really helped me.
Great video btw! :)
Sonil Zaki Thanks!
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
great video but in the ocr textbook it says Fe2 = pale green Fe3+ = yellow
Wah thank you so much for the video!!
Thanks this helped me a lot
Thank you!
Great video
Thank you
thanks
+Shah. F no probs!
helpful video but i wish the audio was better
PFFT who needs school when we have you lol
Thank you so much!!!
You're welcome!
Thank you sir
Welcome
Thank you.
thank you :)
You're welcome!
thank you
you the best ALLERY keep it up nigga u videos are th realest
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