3:49 why does the *2s* combine with the *2p* since the former is already filled and will not be able to form any bonds? Why does it still combine with the 2p to form a hybrid orbital?
@@adithyapatil4346 No, it's *indeed* hybridised. The assumption that only partially filled orbitals can hybridise is what's wrong here. If it was unhybridised, ammonia wouldn't have a tetrahedral shape. Learn more about this somewhere else.......
Looking at NH3, are those bondings between N and Hs really sigma bondings? N has got 2s22p3, does it really rearrange its outer orbitals to be the same? Also, how same are those new orbitals? Because the three bondings with hydrogen has two electrons that are compelled by hydrogen but the lone electron pair does not have any other nuclei to be attracted to so that is not the same as the other three bondings. So can we really approximate them as same bondings?
One mistake: it's not the number of single bonds. For example, CO2 has 2 double bonds, and the steric number is.. 2 (www.chem.ucla.edu/~harding/IGOC/S/steric_number.html )
Khan academy always have a great impact in my life! Thank you....
3:49 why does the *2s* combine with the *2p* since the former is already filled and will not be able to form any bonds?
Why does it still combine with the 2p to form a hybrid orbital?
Do you know the answer to this now?
It doesn't. It's in unhybridized. That's why it has two electrons.
@@adithyapatil4346 No, it's *indeed* hybridised. The assumption that only partially filled orbitals can hybridise is what's wrong here. If it was unhybridised, ammonia wouldn't have a tetrahedral shape. Learn more about this somewhere else.......
Great Video! Thank you.
Wonderful! Nothing more to say🙇
You're awesome!!
very conceptual
how can you tell which orbital excited electrons go to so that they single to form hybrid orbitals
Thank you very much I am very grateful for your help
.Do you have another video on drawing Lewis structure for Ions that have resonance
They must have a video on that, you can go search on www.khanacademy.org 👍
Thanks
Forget He saying "single" bond. Remember only "sigma" bond" .For example, the steric number of C2H4 is 5 and NOT 4.
Don't reply please I'm speaking with myself.
@@nitink3364 mood
Looking at NH3, are those bondings between N and Hs really sigma bondings? N has got 2s22p3, does it really rearrange its outer orbitals to be the same? Also, how same are those new orbitals? Because the three bondings with hydrogen has two electrons that are compelled by hydrogen but the lone electron pair does not have any other nuclei to be attracted to so that is not the same as the other three bondings. So can we really approximate them as same bondings?
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One mistake: it's not the number of single bonds. For example, CO2 has 2 double bonds, and the steric number is.. 2 (www.chem.ucla.edu/~harding/IGOC/S/steric_number.html )
thank you