Why do Transition Metals Form Coloured Compounds?

[@tasnimghani2360]

Searched the entire internet for a proper perfect explanation didn't find one. This video is on point, I finally understand this complex concept. Wish I found this sooner. Thank you so very much

[@chemistry.student]

Thank you! Glad it helped :)

[@tokiwii]

Literally the best video. Describes and summarises everything perfectly, i‘m so happy

[@chemistry.student]

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[@360PLOWQUALITY]

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[@chemistry.student]

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[@potati4097]

You are the best yt channel for a-level chemistry ❤

[@chemistry.student]

Wow! Thank you :)

[@manuelread2283]

Amazing video, thank you!

[@chemistry.student]

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[@krushnamali6183]

Now I conceptually understood why this happes, THANKS

[@chemistry.student]

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[@quitekid2863]

Damn this was exactly what I wanted . Don’t stop making videos dude

[@chemistry.student]

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[@AndrewBleasdale-q7g]

This is well done.

[@chemistry.student]

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[@chunhochan7174]

then will the electron jump back from the high energy level to the low energy level? If yes, then I will still see that colour. If no, then there will be more and more electron in the high energy level? I don't understand about this. Can you please explain about it more? Thanks.

[@moonsoon199]

THANK YOU

[@chemistry.student]

Thank you :)

[@purusottamgoswami1830]

thnks.. great explanation

[@chemistry.student]

Thank you!

[@Dr1z.]

Brilliant video

[@chemistry.student]

Thank you :) Hope it helped!

[@naveensingh5787]

can u explain why Fe shows 3 plus ion , in case of Cu one electron goes from 4S to 3d , but in case of Fe it does not happen, then how it forms Fe 3 plus

[@chemistry.student]

Iron (Fe) forms Fe³⁺ because the resulting 3d⁵ half-filled configuration is (relatively) stable.
Copper (Cu) does not easily form Cu³⁺ because the electron configuration after removing two electrons (3d⁹) is not as favorable or stable as 3d¹⁰ (Cu⁺).
Hope that helps :)

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[@muhammada.muhammad6287]

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[@robertyates5919]

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