1.3 Valence Bond Theory and Hybridization | Organic Chemistry 

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 RU-vid University. Thanks so much Chad, you're the best!

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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 explain this better than my chemistry professor

That was super informative and clearly and simply explained so thanks a lot!

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.

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Great videos! great explanations!

Thanks you so much Mr lecture,you made me understand this topic very well rather than before ,otherwise be bless

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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!

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For the F2 example did you mean their valence electrons are in the P orbital not S?

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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.

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Chad goated for this one

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)?

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.

@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.

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

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?

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Sir can you explain me about the role of entropy in dissolving process? It is not relevant to your videos 😶

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