You are so important to me and others, thank you!! I lose track of time watching your videos and learning, and everything sticks with me and it is easy to note-take along. I'm glad to have found you.
I was absolutely dreading organic chemistry because of how unorganized the information was but your channel has sorted out that problem for me and made this semester so much more manageable. You have done a great service to your fellow man. Thank you for your time, knowledge and generosity Sir.
Bro been having multiple panic attacks and the semester hasn't even started. My OG teacher isn't the best so I now I have to result to TH-cam University. Thanks so much Chad, you're the best!
Thank you for your content. I'm finally "in person" with my classes so I'm managing a little better, but I still use your videos for review. When I was forced to do online classes you were basically my substitute professor! Have a good day.
Thank God I found your channel! This is the clearest and most understandable explanation of this topic I've ever seen, and it has clarified the confusion I’ve held for more than 2 years!
Valence Bond Theory Concept: Valence bond theory explains covalent bonding through the overlap of atomic orbitals. Electrons are shared in these overlapping regions. Atomic Orbitals: 1s Orbital: Spherical shape. 2p Orbital: Dumbbell shape with a node at the nucleus. Overlap Types: Sigma (σ) Overlap: Occurs along the internuclear axis (the line connecting the two nuclei). Pi (π) Overlap: Occurs side-to-side and involves p orbitals only. Examples of Sigma and Pi Overlap H2 Molecule: Sigma overlap of two 1s orbitals. HF Molecule: Sigma overlap of hydrogen’s 1s orbital with fluorine’s 2p orbital. F2 Molecule: Sigma overlap of two 2p orbitals. Pi Overlap: Only involves p orbitals and occurs above and below the internuclear axis. Hybridization Concept: Hybridization is the mixing of atomic orbitals to form new hybrid orbitals that can form stronger, more stable bonds. Determining Hybridization: Electron Domains: The number of atoms bonded to and lone pairs around an atom. Types: sp3 Hybridization: Four electron domains, bond angles of 109.5°. sp2 Hybridization: Three electron domains, bond angles of 120°. sp Hybridization: Two electron domains, bond angles of 180°. Examples of Hybridization Methane (CH4): Carbon is sp3 hybridized with four sigma bonds, bond angles of 109.5°. Ammonia (NH3): Nitrogen is sp3 hybridized with three sigma bonds and one lone pair, bond angles slightly less than 109.5° due to lone pair repulsion. Formaldehyde (H2CO): Carbon is sp2 hybridized with three sigma bonds and one pi bond, bond angles approximately 120°. Acetylene (C2H2): Carbons are sp hybridized with a triple bond (one sigma and two pi bonds), bond angles of 180°. Practical Applications Sigma Bonds: Formed by overlapping hybrid orbitals or atomic orbitals. Pi Bonds: Formed by the sideways overlap of unhybridized p orbitals. Lone Pairs: Reside in hybrid orbitals if the atom is hybridized.
I better be smiling in that Prometric centre like an hyena ...just cause professor Chad is my YT tutor. Can’t wait to ace that DAT and come back with my testimony.
Awesome Christianah! And have you seen my DAT Practice Exams? They're still available free of charge for a little while longer! courses.chadsprep.com/courses/chads-dat-practice-exams
I have a question. Towards the beginning of the video, in the H-F and F-F bonds, would it not be overlap between s (for H) and sp3 (for F), instead of p for F? I thought F would have sp3 hybridization, and thus it would be an sp3 hybridized orbital overlapping with the s orbital from H as opposed to a pure p orbital from F overlapping with the s from H. And then F-F would have overlap between two sp3 hybridized orbitals, instead of overlap of two p orbitals.
Great question Laura! It turns out that only atoms that are making more than one bond experience hybridization. With F only making one bond, it simply used the atomic orbital where we find its unpaired electron, a 'p' orbital. So while you might look at the Lewis structure and see 4 electron domains and think sp3, F is not hybridized and is just using a 'p' orbital. The worst part of all of this is that when you get to molecular orbital theory, you'll learn that while the idea of hybrid orbitals has great utility in predicting bond angles and molecular geometry, it isn't an accurate reflection of reality in other ways (predicting energy levels of orbitals). So the theory does have some explanatory power, but molecular orbital theory has even greater explanatory power and is 'more' correct. So hybrid orbitals may not even really exist :( Hope this helps!
@chad, concerned about the idea of a carbon atom ‘investing’. It cant do that, so what’s the mechanism? Dont need to explain, just give me the buzzwords and I’ll research it myself. Thanks for great content.
I'm not sure I understand overlapping orbitals. In methane, for example, each H shares a pair of electrons with the C. In one of those pairs, do the two electrons have identical wave functions (except for spin)?
Hey Fred! First of all, keep in mind that Valence Bond Theory has its shortcomings...it's an incomplete theory but still has its utility. But it sets the stage for molecular orbital theory (the next lesson I'll be releasing later today). The main idea was that when two atoms bond together their electron clouds overlap to form a giant electron cloud that encompasses both atoms. Note my use of the word cloud instead of orbital just to give it a little different feel. In Molecular Orbital theory we'll find out the when two orbitals (which are depictions of wave functions) overlap they actually combine to form a new orbital (a new wavefunction). So we could say that the overlap of the Atomic Orbitals leads to the creation of a new Molecular orbital. But you'll see that even this explanation is too simplistic as the overlapping atomic orbitals will actually result in the creation of TWO molecular orbitals: one bonding and one antibonding. And if you get to molecules having more than two atoms it gets even more complicated, but we will largely ignore that in organic chemistry with one exception when we study conjugated systems (usually in the 2nd semester). Hope this helps!
Hi Pablo! I go into that in greater detail in the very next lesson on Molecular Orbital Theory: th-cam.com/video/PZCsJH1taYA/w-d-xo.html Take a look and let me know if I didn't answer your question to your satisfaction there. Happy Studying!
Yes - briefly, anything that increases the disorder of a system increases entropy. When a solute dissolves it increases the disorder of the system because solute particles separate and become dispersed in the solution. So dissolving increases entropy.
You re indeed a teacher.. thanks for your efforts
Thank you! 😃
You are so important to me and others, thank you!! I lose track of time watching your videos and learning, and everything sticks with me and it is easy to note-take along. I'm glad to have found you.
Glad you did!
I was absolutely dreading organic chemistry because of how unorganized the information was but your channel has sorted out that problem for me and made this semester so much more manageable. You have done a great service to your fellow man. Thank you for your time, knowledge and generosity Sir.
Glad the channel is helping you - Happy Studying!
Bro been having multiple panic attacks and the semester hasn't even started. My OG teacher isn't the best so I now I have to result to TH-cam University. Thanks so much Chad, you're the best!
Glad the channel is helping you - Happy Studying!
I have faith that this will get me through my class 😭🥲
Chad, you make learning so enjoyable and the content easy to digest. It's incredibly refreshing. Thank you!!!
Always glad to hear that, Maryam - Glad you enjoy!
You just earned a new sub ! Thank you,I was really confused with my professor's lessons,but now I have more understanding on it !
Excellent - thanks for the sub!
I am grateful for this man standing there make college kids' life better.
😄
This man is a literal angel. I should probably watch your vids BEFORE class, I'd avoid so much confusion!
Glad the channel is helping you - Happy Studying!
Thank you for your content. I'm finally "in person" with my classes so I'm managing a little better, but I still use your videos for review. When I was forced to do online classes you were basically my substitute professor! Have a good day.
You're welcome, Ava C - glad you found the channel and it has been a useful tool for you!
Thank God I found your channel! This is the clearest and most understandable explanation of this topic I've ever seen, and it has clarified the confusion I’ve held for more than 2 years!
Glad you found us, too - Happy Studying!
Chad you saved my life in gen chem and you're saving me now in organic. Thank you for your commitment, God bless you!!!!!
Glad the channel has helped and will continue to do so - Happy Studying!
Thank you Chad!!! I'm retaking organic chem right now and your videos are definitely giving me the information I need to ace this second try!
Awesome! Best of luck in your studies - you got this!
Wonderful lessons. I wanted to point out a mistake @ 5:57: Should be "p orbital" and not "s orbital".
Valence Bond Theory
Concept: Valence bond theory explains covalent bonding through the overlap of atomic orbitals. Electrons are shared in these overlapping regions.
Atomic Orbitals:
1s Orbital: Spherical shape.
2p Orbital: Dumbbell shape with a node at the nucleus.
Overlap Types:
Sigma (σ) Overlap: Occurs along the internuclear axis (the line connecting the two nuclei).
Pi (π) Overlap: Occurs side-to-side and involves p orbitals only.
Examples of Sigma and Pi Overlap
H2 Molecule: Sigma overlap of two 1s orbitals.
HF Molecule: Sigma overlap of hydrogen’s 1s orbital with fluorine’s 2p orbital.
F2 Molecule: Sigma overlap of two 2p orbitals.
Pi Overlap: Only involves p orbitals and occurs above and below the internuclear axis.
Hybridization
Concept: Hybridization is the mixing of atomic orbitals to form new hybrid orbitals that can form stronger, more stable bonds.
Determining Hybridization:
Electron Domains: The number of atoms bonded to and lone pairs around an atom.
Types:
sp3 Hybridization: Four electron domains, bond angles of 109.5°.
sp2 Hybridization: Three electron domains, bond angles of 120°.
sp Hybridization: Two electron domains, bond angles of 180°.
Examples of Hybridization
Methane (CH4): Carbon is sp3 hybridized with four sigma bonds, bond angles of 109.5°.
Ammonia (NH3): Nitrogen is sp3 hybridized with three sigma bonds and one lone pair, bond angles slightly less than 109.5° due to lone pair repulsion.
Formaldehyde (H2CO): Carbon is sp2 hybridized with three sigma bonds and one pi bond, bond angles approximately 120°.
Acetylene (C2H2): Carbons are sp hybridized with a triple bond (one sigma and two pi bonds), bond angles of 180°.
Practical Applications
Sigma Bonds: Formed by overlapping hybrid orbitals or atomic orbitals.
Pi Bonds: Formed by the sideways overlap of unhybridized p orbitals.
Lone Pairs: Reside in hybrid orbitals if the atom is hybridized.
You explain this better than my chemistry professor
Glad you found us, Toker!
This was so incredibly helpful, thank you!
You're very welcome!
Thanks you so much Mr lecture,you made me understand this topic very well rather than before ,otherwise be bless
You're welcome, Daniel - thanks for saying so!
You're so helpful 🙂 youre pretty much my substitute teacher rn ❤❤
Glad the channel is helping you.
I better be smiling in that Prometric centre like an hyena ...just cause professor Chad is my YT tutor. Can’t wait to ace that DAT and come back with my testimony.
Awesome Christianah! And have you seen my DAT Practice Exams? They're still available free of charge for a little while longer!
courses.chadsprep.com/courses/chads-dat-practice-exams
That was super informative and clearly and simply explained so thanks a lot!
You're welcome and Thank You.
This is an incredible video.
Thank you
Great videos! great explanations!
Glad you like them - thanks for the comment!
Thank you so much! You seriously are helping a lot of students and reducing stress:))
Glad to hear it - thank you!
most amazing teacher ever!
Thank you!
Chad you are my king
King? I certainly hope not!😜 How about short, bald, helpful YT instructor? But I appreciate the sentiment!😊
Kinda crazy that I pay to go to college when chad literally teaches me everything online for free
Glad the channel is helping you.
omg thank you so much i dont know why i didn't found this before my exams but i hope i can get a good grade on the final exam so i can pass:C
You're welcome - glad you found the channel!
For the F2 example did you mean their valence electrons are in the P orbital not S?
I think so, I came here to say the same thing 😂
You are literally Awesome. Thank you so much . God bless you
You're welcome and thank you.
I have a question. Towards the beginning of the video, in the H-F and F-F bonds, would it not be overlap between s (for H) and sp3 (for F), instead of p for F? I thought F would have sp3 hybridization, and thus it would be an sp3 hybridized orbital overlapping with the s orbital from H as opposed to a pure p orbital from F overlapping with the s from H. And then F-F would have overlap between two sp3 hybridized orbitals, instead of overlap of two p orbitals.
Great question Laura! It turns out that only atoms that are making more than one bond experience hybridization. With F only making one bond, it simply used the atomic orbital where we find its unpaired electron, a 'p' orbital. So while you might look at the Lewis structure and see 4 electron domains and think sp3, F is not hybridized and is just using a 'p' orbital.
The worst part of all of this is that when you get to molecular orbital theory, you'll learn that while the idea of hybrid orbitals has great utility in predicting bond angles and molecular geometry, it isn't an accurate reflection of reality in other ways (predicting energy levels of orbitals). So the theory does have some explanatory power, but molecular orbital theory has even greater explanatory power and is 'more' correct. So hybrid orbitals may not even really exist :(
Hope this helps!
@@ChadsPrep Good to know, thank you very much for your reply!
@@lauraj2815 👍👍👍
Chad goated for this one
Thanks, Luke!
Thank you so much❤️❤️❤️
You're very welcome Imanish! Glad you're finding these helpful!🙂
you're amazing. thanks a ton.
You're welcome!
Amazing thanks a lot
Most welcome 😊
@chad, concerned about the idea of a carbon atom ‘investing’. It cant do that, so what’s the mechanism? Dont need to explain, just give me the buzzwords and I’ll research it myself. Thanks for great content.
thankyou sirrr
You're welcome!
I'm not sure I understand overlapping orbitals. In methane, for example, each H shares a pair of electrons with the C. In one of those pairs, do the two electrons have identical wave functions (except for spin)?
Hey Fred! First of all, keep in mind that Valence Bond Theory has its shortcomings...it's an incomplete theory but still has its utility. But it sets the stage for molecular orbital theory (the next lesson I'll be releasing later today). The main idea was that when two atoms bond together their electron clouds overlap to form a giant electron cloud that encompasses both atoms. Note my use of the word cloud instead of orbital just to give it a little different feel.
In Molecular Orbital theory we'll find out the when two orbitals (which are depictions of wave functions) overlap they actually combine to form a new orbital (a new wavefunction). So we could say that the overlap of the Atomic Orbitals leads to the creation of a new Molecular orbital. But you'll see that even this explanation is too simplistic as the overlapping atomic orbitals will actually result in the creation of TWO molecular orbitals: one bonding and one antibonding.
And if you get to molecules having more than two atoms it gets even more complicated, but we will largely ignore that in organic chemistry with one exception when we study conjugated systems (usually in the 2nd semester).
Hope this helps!
If the negative side of the orbital hits the positive side of the other orbital then they don't form a bond? What makes it positive or negative?
Hi Pablo! I go into that in greater detail in the very next lesson on Molecular Orbital Theory: th-cam.com/video/PZCsJH1taYA/w-d-xo.html
Take a look and let me know if I didn't answer your question to your satisfaction there. Happy Studying!
Sir if there are two hybrid orbitals in one molecule what happens
A lot of molecules have 2+ hybrid orbitals, can you be more specific when you say "what happens?"
God bless you Sir
Thank you.
I will donate My grade in "shekels", man you are the greatest!!! I owe you more than i can pay.
Thank you - Happy Studying!
I love you
Glad the channel is helping!
is it me or does he have radio voice?
Sir can you explain me about the role of entropy in dissolving process? It is not relevant to your videos 😶
Yes - briefly, anything that increases the disorder of a system increases entropy. When a solute dissolves it increases the disorder of the system because solute particles separate and become dispersed in the solution. So dissolving increases entropy.
if i get a 20 on the ochem section on the dat i''ll donate a 1000 to you
😁😁😁 Good luck!
We love when people love our videos - thanks!
@@ChadsPrep We students love when teachers actually know how to educate and not just school kids!