NH3 is sp3, as is the NH2 bonded to C. Nitrogen is group 5 and has five valence electrons and then 3 covalent bonds brings that up to 8 valence electrons = 4 pairs. 1 pair to H, 1 pair to H, 1 pair to C and one lone pair = 4 charge centers = sp3
Wow thank you!! I have watched so many videos and read so many books onto of all my lessons..... Thanks to you, I finally get it, just in time for my test tomorrow! :) :) :)
I know it's unrelated to hybridisation, but I don't understand how you knew to place the lone pairs of electrons in the N2H2 molecule (why is one above one of the nitrogens and the other below the other nitrogen)? Thank you!!
Damn this video is super helpful! It's the first time I've heard of this trick. Also, one question. Is this hybridization of a molecule always based on the central atom?
Hi Mr. Thornley! Quick questions - 1. When atoms are covalently bonded with one atom having hybridized valence orbitals (e.g. O), the rest having simple valence orbitals (e.g. H), and some lone pairs of electrons, how can a single electron be part of a hybridized atom (O) and non-hybridized atom (H) at the same time because they're of 2 different energy levels? 2. Can two covalently bonded atoms both be hybridized, but with different hybridizations? Are there any examples for this?
1) hmmm - beyond my pay grade (and IB) that question! I thought I understood this - now you make me doubt myself! I suppose the electron energy is the same in respect to the O and the H, or an average or the reality is the sp hybrid hybridizes again with the H orbital and that is were the electron is. If you find out from a smarter chemistry teacher ley me know.
1 lone pair = 1 charge center. In your case, it's two. So 2 lone pairs = 2 charge centers. Also you said that the atom is bonded to two other atoms. Hence 4 charge centers => sp3 :D
Sorry, just a quick question. For NH3 apparently it hybridizes and also forms an sp3 and has the shape tetrahedral. Can you please explain how? I'm mainly confused because the electron would not have anything to be promoted too... all the p orbitals already have an electron there --> they would want to simply bond, not hybridize then.
would you happen to know the ssciencevid people that make biology videos for the ib? you both appear to be from new york and your videos follow a, somewhat, similar syntax.
2p XX X X 2s XX 1s XX goes to sp3 XX X X X this has 4e since nitrogen has 1 more e than carbon 1s XX the sp3 has room for 3 more e now from the hydrogen
![S2.2.15 Explain hybridization as mixing of orbitals making new orbitals [HL IB Chemistry]](http://i.ytimg.com/vi/HKyobMewXBw/mqdefault.jpg)
![4.3 (Pre-Video) VSEPR and Charge Centers [SL IB Chemistry]](http://i.ytimg.com/vi/QzlKNs9VplY/mqdefault.jpg)
you have no idea how helpful this is Mr thornley!!
He has made the video bro so how he couldn't have the idea
You are such a legend! The best, most logical and most simple explanation I have come across. Thank you!
Wow.... i just learned more chemistry in 3 minutes than I have in my entire gen chem class. Thank you so much
NH3 is sp3, as is the NH2 bonded to C. Nitrogen is group 5 and has five valence electrons and then 3 covalent bonds brings that up to 8 valence electrons = 4 pairs.
1 pair to H, 1 pair to H, 1 pair to C and one lone pair = 4 charge centers = sp3
I did the IB program last year and i still watch these videos in my university years. Richard thornley. you are the hero we need.
I've had 3 difference professors teach hybridization and this is the first time I felt like I really clearly understood. Thank you so much!
Can’t believe it! I’ve understood it in less than 3 minutes! Thank you Mr Thornley 😊😊
This is easily the most clear explanation I have seen, thank you
I'm ready for my IB HL Chem quiz because of this! Thank you!
Thank you sooo much! It make sense how easily the teacher tells the hyb. from the structures
BEST DAMN VIDEO ON YOUR TUBE EXPLAINING THE DIFFERENCE
You have helped me SO much! i am so greatful, thank you sooo much. :D All my friends in the IB taking chemistry just love your videos!
Wow thank you!! I have watched so many videos and read so many books onto of all my lessons..... Thanks to you, I finally get it, just in time for my test tomorrow! :) :) :)
Excellent Mr. Thornley!! Best Chemistry Teacher!!! WOW!
This was soooo helpful!!! And the easiest to understand.. Thank you soo much sir!!
u r the best chem teacher woderful and amazingggggggggggggggg................
THANKS SIR I HAVE UNDERSTOOD IN VERY LESS TIME THANKS U SO MUCH SIR
You sir are a genius. greets from Swizerland.
hi, this video was amazing but just wondering, is a charge centre the same as an electron domain? thank you so much!!
amazing thanks helped so much for my test tomorrow
A helpful tip it to add up the number of electron domains than subtract 1 to get the type of hybridization
So much more helpful than my actual instructor
Thank you sir very much! Chemistry HL, here I come.
The position is not important but traditionally try to spread out the most repulsive (or the largest) parts of a molecule/atom.
I know it's unrelated to hybridisation, but I don't understand how you knew to place the lone pairs of electrons in the N2H2 molecule (why is one above one of the nitrogens and the other below the other nitrogen)? Thank you!!
Damn this video is super helpful! It's the first time I've heard of this trick.
Also, one question.
Is this hybridization of a molecule always based on the central atom?
you saved my life. thanks!
Danm ... Now that looks super easy from now on xD
Hi, just a quick question - if there are two lone pairs on an atom which is also bonded to two other atoms, would the hybridization be sp3 or sp2?
Hi Mr. Thornley! Quick questions -
1. When atoms are covalently bonded with one atom having hybridized valence orbitals (e.g. O), the rest having simple valence orbitals (e.g. H), and some lone pairs of electrons, how can a single electron be part of a hybridized atom (O) and non-hybridized atom (H) at the same time because they're of 2 different energy levels?
2. Can two covalently bonded atoms both be hybridized, but with different hybridizations? Are there any examples for this?
1) hmmm - beyond my pay grade (and IB) that question! I thought I understood this - now you make me doubt myself! I suppose the electron energy is the same in respect to the O and the H, or an average or the reality is the sp hybrid hybridizes again with the H orbital and that is were the electron is. If you find out from a smarter chemistry teacher ley me know.
1 lone pair = 1 charge center. In your case, it's two. So 2 lone pairs = 2 charge centers. Also you said that the atom is bonded to two other atoms. Hence 4 charge centers => sp3
:D
Oh my good lord thank you so much
Sorry, just a quick question. For NH3 apparently it hybridizes and also forms an sp3 and has the shape tetrahedral. Can you please explain how? I'm mainly confused because the electron would not have anything to be promoted too... all the p orbitals already have an electron there --> they would want to simply bond, not hybridize then.
It all makes sense now thank you very much :D
Thanks, it really help me
Thank You so much!!😁
great video..charge centers baby
Thanks so much. It was really helpful ☆
would you happen to know the ssciencevid people that make biology videos for the ib? you both appear to be from new york and your videos follow a, somewhat, similar syntax.
Is there one of you for physics
OH YES SO I WAS RIGHT! A person argued with me saying that two lone pairs count as one charge center, thus resulting in sp2 hybridization. :D :D
i didnt understand why you used sp2 in linear structured compound...
thank you :)
sp3 since there are 4 charge centers
yup, she works in the next cupboard to me
2p XX X X
2s XX
1s XX
goes to
sp3 XX X X X this has 4e since nitrogen has 1 more e than carbon
1s XX
the sp3 has room for 3 more e now from the hydrogen
2p X X X
2s XX
1s XX
just to clarify
no one bothered to know what the name of the structure is?
I love you!!
(No homo)
no