sp³ hybridization | AP Chemistry | Khan Academy

In sp³ hybridization, one s orbital and three p orbitals hybridize to form four sp³ orbitals, each consisting of 25% s character and 75% p character. This type of hybridization is required whenever an atom is surrounded by four groups of electrons. View more lessons or practice this subject at www.khanacademy.org/science/a...
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[@christinamccarthy7659]

Finally someone who explained this in SIMPLE terms beginning with our knowledge of orbital filling diagrams than showing us how these are hybridized

[@TheMotherOfBambi]

Khan academy is honestly a life saver i cannot thank you enough for making these amazing videos available to anyone on youtube 🙌🏿🙌🏿🙌🏿🙌🏿

[@KH-ey3ce]

I have actually never understood this until now! Thank you so much :D

[@ravinduwijayarathna6238]

this explained EVERY .....SINGLE . .QUESTION i had with hybridization.. Thank you so much 😘😘😘

[@musicspeaks0101]

THANK YOU SO MUCH this was so helpful!!!! I've watched so many videos about hybridization and I didn't understand it fully until now!

[@LeeKiseok]

wow just wow!!!! starting to like the subject a little more!

[@esmeraldaelhamzawy9114]

wow what a great video it was really helpful and informative, it cleared up everything to me

[@xXHyperDucksXx]

I love u :D It cleared up everything. Now I can ace my test tommorow! :D

[@Wolfeywolf16]

Thank you so much!!! I was so confused leaving organic chemistry

[@ahil5975]

i had watched like 10 videos prior to this regarding hybridization , none of which actually explained how hybridization takes place except this one

[@cortezvalle5613]

Finally makes sense. Thanks!

[@cholponzhakshylykova4099]

thank you very much :) , I start to understand about Hybridisation :)

[@lEmiliee]

you saved my life so many time wow

[@hafsawaseem3942]

I have an exam next wednesday and i wasn't understanding anything until I found this video wich is incredibly simple and understable , saying thanks is really not enough but i really mean it let me give you some hearts and flowers too 💜🌸💕💖💗💞💝💟💙💚💛🌷🥀🌹🌼

[@suzannanelson7290]

Thanks so much . so much easier to understand.

[@solaly9874]

Stupid question but how is the 2s promoted in energy it remains on the same level

[@alejandrosantos1879]

Kahn academy has saved me many times back in high school and currently last year of college

[@jonyjoyjoy437]

khaan acadamy is very useful for any educational information

[@therealsan9949]

best explanation i have seen so far

[@persona7506]

this helped so much

[@claireerialc7917]

Why can you promote an s2 electron to a p electron?

[@donnaezhukattil6310]

so good!!!!

[@sofiastortigajani4462]

thank you for this youtube channel, seriously

[@nirgunkaur3161]

thank you so much for this!

[@beckseamons]

Thanks Khan Academy. Super helpful

[@rhodaronke78]

It even same thing our textbook dat my text book offer me dat u still make example. There are lot of compound dat exist apart from d hydrocarbons eg AL2O3. More complex compound like dis dat should b use to explained for beta understanding

[@nitink3364]

The brand new hybrid orbitals formed have new/different electron densities and directions from the hybridising orbitals.But the electron densities and directions of the new hybrid orbitals formed DEPEND UPON the electron densities and directions of the hybridising orbitals.

[@fhdfba007]

Thank you, you're the best

[@yannickelbaj1970]

shoueldnt there be a 109° angele in between the top sp3 orbital and the bottom left and right

[@geerrooo]

thaaaaank youuuuuu very mmmmmmmmuch

[@yaramarwan6601]

bless ur soul

[@sciencenerd7639]

thank you

[@tangor6793]

doesnt carbon have 1s2 2s2 2p2 ? instead of 1s2 2s1 2p3

[@nooriaalihassani]

carbon 252p2 haw can it 4 bounds. why dose it form 4 bounds?

[@Geezweez788]

Hybridisation is intra atomic ressonance wouldnt you say.

[@ngwaimeng123]

Thk u saved my life🤣

[@sathyanarayanan9190]

what is a pi bond

[@neptune-metro]

in single bonds, its considered a sigma bond..... in double, one is considered a sigma while the other is considered a pi bond..... in triple, one is considered a sigma while the other two are considered pi bonds.... we can get out of this that the first bond is sigma while the rest (if there is any left) are pi

[@pawansapkota8181]

remember this when a bond forms in a covalent compounds especially in the carbon if the overlaping of the orbiatal is in the line joining the nucleus of the two atoms then they are called the sigma bond which is the strongest bond while if the overlap laterally not in the direction of the line joing the two nucleus of the two overlapping atoms then it is called a pi bond . Generally a Pi bond cannot be formed without a sigma bond . Check out the Video from the Salman Khan (Sal Khan) of the Khan Academy which he has described it very beautifully.

[@element4element4]

As a physicist trying to learn basics of chemistry, all this makes little sense to me. There is so much information missing, and everything is unjustified claims. The answer is assumed, not argued or derived. All sources (books/videos) just repeat the same logic. Maybe somebody can answer the points of my confusion. 1) Why do 2s and 2p orbitals have different energy? In the non-relativistic and non-interacting limit (essentially Hydrogen atom orbitals), these have the same symmetry. Energy is proportional to 1/n^2 and independent of j and m quantum numbers. And n=2 for 2p and 2s orbitals. Is the split between 2s and 2p orbitals due to relativistic effects (like spin-orbit coupling) or electron-electron interactions? Or something else? 2) It is claimed these orbitals hybridize with no argument for why. This implies that the orbitals are not exact orbitals and there is some coupling (off-diagonal term in the Hamiltonian in this orbital basis). The diagonalization of the Hamiltonian then gives us the new eigenstates, sp3. My guess is that the solution to 1) is: the 2s and 2p split is due to relativistic spin-orbit effects. These are very tiny and the split very tiny, much less than the coulomb energy scale. So if one adds (approximately) electron-electron interactions to the effective Hamiltonian in the subspace of 2s, and 2p orbitals (4-dimensional), then coulomb interactions are the off-diagonal terms. This is the source of hyberdization. Is my picture correct? Or is the mechanism behind hyberdization different from electron-electron interactions?

[@RonShenkar]

this shit, is freakin' cool.

[@rhodaronke78]

Y will he use two similar example, and he never even show d electronic configuration of d C2H4, he just assumed we know it just like our teachers here too do. Of wat importance do I waste such lot of data downloading dis. Teacher don't assume u will give reason for every step that being taken.

[@annikapanda]

anyone else see the green?

[@catkit86]

:D

[@damcross2308]

I hate this.