OCR AS Chemistry Unit F321, Module 2 - Shells, sub shells and orbitals

This is an OCR AS Chemistry Unit 1, Module 2 Shells, subshells and orbitals video.
1.2.2 - Shells and orbitals
1.2.4 - Electrons and the periodic table

Sorry about the blunder in the middle - I can get distracted at times.

[Arya-sxnz]

this is actually one of the best explanation i could find on youtube. i was getting so confused between sub-shells and orbitals. but now it's all good, Thanks to you. Keep making these videos.

[zannatul]

LOOOL @ 8:27 Mary is online 
He went proper quiet 

[ThatChiickChrissy]

ahhhh thank you SO much for making this video i've been so confused cos i was away when my teacher taught it to the class. Finally understanding. :))

[Limz]

mrowner100 , A full outer shell in the d block is more stable (energy-wise) than a full s block so an electron drops down into the D block giving it a full sub-shell. This also occurs with copper and with chromium for similar reasons

[ANDYtheGAFFER]

This was really helpful, I didn't understand in lesson, thanks mate :)

[SiddiQah]

I missed the lesson on this!
Thank you so much! I simply read the text book before this, and quite frankly - understood NOTHING.

[enamul]

This is really is fantastic and helped me a lot. Thanks man!

[michelle]

the website is really useful! THANK YOU SO MUCH for ur tutorial! :) now i can understand what my teacher taught... :D pls make more tutorials!!

[Jsouassou]

Why thank you :D ... More videos will be on its way through the half term.

[alaaal-dibouni]

omg i actually understand this now, thank you :)

[harryws]

Just a little thing - I'd call the 'rows' in the periodic table periods. Thanks for the tips though!

[Jsouassou]

@mahsun9898 haha... that won't happen again, I'll assure you. and yeah, there will be more videos soon. Thanks for your support!

[Jsouassou]

Also, I have a theory for the question you're asking but that just requires another video. Again, you do not need to worry about that because if you think about Rubidium in terms of orbitals, it will look VERY messy, but still, you should most definitely ask your teacher about that, or a university professor.

[Jsouassou]

@michelle4869 Of course, there will be more videos throughout the term as I learn the stuff.

[Combustious]

It should be 4d9 instead of 5d9 because the d block starts at a lower number than the s and p blocks.

[Jsouassou]

Hi,
10:31 - There are 5 individual orbitals there; all 5 of them is a single orbital. What there isn't is a picture on how it would look like all joined up. The same with 11:33 . There are 7 individual orbitals there. Anyways, even still, you do NOT need to learn how they look like for the exam.

[Jsouassou]

Thanks! Watch my other videos... More are coming up over this week.

[jameshayes]

8:24 . You seemed a bit flustered when Mary came online Dude

[sejadlol]

Haha nice videos man helping me alot :)

[lithiumsapphire]

you said there is 5 d and 7 f orbitals but in picture there is 4 d and 6 f orbitals?where are the missing orbitals then? and i wonder why don't these electrons hit each other because if we look at p orbital for example, it has a part which is inner s orbital, so for example an s orbital electron can hit to the p orbital?or why p orbital electrons dont hit the protons because their subshell is at the core of the electron.i am so confused please help.i need a pic with every orbitals on the same e-