What is the definition of perfection??? Thisss🙌🙌🙌🙌🙌 Honestly, NOBODY explained it with such detail as well as precision. This channel was THE eye opener for me in organic chemistry. THANK YOU
@@chemistry.student bro you are so damn good in explaining. Im from india and preparing for the Jee exam. Your videos are extremely good and many top faculties cannot explain like this. Thank you brother! ❤😊
If anyone is wondering, one of the 2sp² electron jumps over to the p orbital during the first excited state when external energy is provided. This energy could be in the form of heat etc.
7:53 if u think about it because each unhybridised p orbital has single electro and for a bond to be formed 2 electrons are needed that means an ovarlap well form only on one side(at Top maybe ) the bottom orbitals won't overlap as they are no electrons And bottom one wouldn't be a dative bond in case of ethene because each p orbital only has 1 electron not 2 So would that mean a pi bond is not formed as the is only 1 overlap and not 2 Edit : if I would answer myself I would say the top and bottom (pi bond) is just a probability of were electron pair could be either up or down.. we can never know we're the would be up or down. So its just a region of probability of finding the electron pair
Question when an atom hybridsise it's orbitals does the orbitals always have to be half filled, Which would make sense if it's true because it would allow a covalent bond to form But I guess it's not always true because even if u hybridsise an orbital with 2 electrons a covalent bond can form through dative bonds
Really good question! No, orbitals don’t have to be half-filled for hybridisation to occur. Hybridisation is just the mixing of atomic orbitals to form new hybrid orbitals, which can happen regardless of whether those orbitals are fully filled, half-filled, or empty. As long as the new orbital formed contains a pair of electrons, it doesn't matter where they came from. However, for bonding (especially in typical covalent bonds), it’s more common for half-filled orbitals to participate since they can pair up with electrons from other atoms. But when forming dative (coordinate) bonds, a fully filled orbital from one atom can overlap with an empty orbital from another atom, and this bond can still involve hybridised orbitals. Hope that helps :)
What is the definition of perfection??? Thisss🙌🙌🙌🙌🙌
Honestly, NOBODY explained it with such detail as well as precision. This channel was THE eye opener for me in organic chemistry. THANK YOU
Wow, thank you! Glad it's helped :)
@@chemistry.student bro you are so damn good in explaining. Im from india and preparing for the Jee exam. Your videos are extremely good and many top faculties cannot explain like this. Thank you brother! ❤😊
extreme! the recap-lesson-summary structure really helps!
your videos are so helpful! please keep making more videos
Thank you! Great idea
If anyone is wondering, one of the 2sp² electron jumps over to the p orbital during the first excited state when external energy is provided. This energy could be in the form of heat etc.
extremely helpful! can't thank you enough!
indeed very helpful video keep going more power to you
Thank you!
Thank you! I finally understand what sp2 and sp3 hybridisation mean ^w^
Thank you! Glad it helped :)
7:53 if u think about it because each unhybridised p orbital has single electro and for a bond to be formed 2 electrons are needed that means an ovarlap well form only on one side(at Top maybe ) the bottom orbitals won't overlap as they are no electrons
And bottom one wouldn't be a dative bond in case of ethene because each p orbital only has 1 electron not 2
So would that mean a pi bond is not formed as the is only 1 overlap and not 2
Edit : if I would answer myself I would say the top and bottom (pi bond) is just a probability of were electron pair could be either up or down.. we can never know we're the would be up or down. So its just a region of probability of finding the electron pair
Super helpful!!! Thank you so much!!
Thank you! Glad it helped :)
Best on yt 🎉
Wow - thank you!
ur vids are amzinggg
Thanks it’s really helpful 😊
Thank you! Good luck with your studies :)
this really helped thank youuuuu
U a beast bruh
Question when an atom hybridsise it's orbitals does the orbitals always have to be half filled,
Which would make sense if it's true because it would allow a covalent bond to form
But I guess it's not always true because even if u hybridsise an orbital with 2 electrons a covalent bond can form through dative bonds
Really good question! No, orbitals don’t have to be half-filled for hybridisation to occur. Hybridisation is just the mixing of atomic orbitals to form new hybrid orbitals, which can happen regardless of whether those orbitals are fully filled, half-filled, or empty. As long as the new orbital formed contains a pair of electrons, it doesn't matter where they came from.
However, for bonding (especially in typical covalent bonds), it’s more common for half-filled orbitals to participate since they can pair up with electrons from other atoms. But when forming dative (coordinate) bonds, a fully filled orbital from one atom can overlap with an empty orbital from another atom, and this bond can still involve hybridised orbitals.
Hope that helps :)
Just perfect the only problem am having the models are making stuff hard for me to conceptualise
Models can be frustrating - thank you for watching!
Thanks
Thank you :)
Can I speak to you in private? I couldn’t find an email or a phone number anywhere..
Hello, for any video based comments you can contact me at site@chemistrystudent.com :)
@@chemistry.student Hey, I’ve tried to send an email but it says it’s an invalid recipient, can you make sure the email address is correct? Thanks 😊
Hello, should be working now! site@chemistrystudent.com :)