From a first year honours biomed student at uOttawa (Ontario, Canada): I much appreciate the analogy with the two bottles at the beginning. Very easy way for students to immediately have a general understanding of the concept. I also like the way you lecture, Sir; I don't doubt the knowledge of any of my chemistry professors, but the choice of wording and grammar in lectures can make a huge difference. I found the video beneficial and I thank you for that.
I do have a question, though: why is it that the distance between bonding and anti-bonding sigma orbitals decrease as the bond strength increases? To my knowledge, the stronger a bond is, the more stable it is. The more stable a bond is, the less energy its bonding molecular orbital(s) will have. Following that logic, shouldn't stabler bonds have bonding MO with less energy (which therefore means the anti bonding MO would have more energy)?
Good start with the bottle example. Question... with the pi bonded structure, how would you remove electrons to increase the polarizabilty? Polymer within + charged carbon ions? That doesn't seem very convincing. If it was metal (Ag for your example), I would understand better but with carbon, I am not too sure. Please enlighten me with example. Thank you.
The idea of explaining with bottles at first really helped my understanding. Thanks from an IB student :D
From a first year honours biomed student at uOttawa (Ontario, Canada):
I much appreciate the analogy with the two bottles at the beginning. Very easy way for students to immediately have a general understanding of the concept. I also like the way you lecture, Sir; I don't doubt the knowledge of any of my chemistry professors, but the choice of wording and grammar in lectures can make a huge difference. I found the video beneficial and I thank you for that.
Oh man He's sooo intelligent!!!! So fast thinking!
Big ups David
👍👍👍👍👍👍👍
I do have a question, though: why is it that the distance between bonding and anti-bonding sigma orbitals decrease as the bond strength increases? To my knowledge, the stronger a bond is, the more stable it is. The more stable a bond is, the less energy its bonding molecular orbital(s) will have. Following that logic, shouldn't stabler bonds have bonding MO with less energy (which therefore means the anti bonding MO would have more energy)?
Good start with the bottle example.
Question... with the pi bonded structure, how would you remove electrons to increase the polarizabilty? Polymer within + charged carbon ions? That doesn't seem very convincing. If it was metal (Ag for your example), I would understand better but with carbon, I am not too sure. Please enlighten me with example. Thank you.
Great analogy!
whats the name of the second compound???? Dude... I can't understand it ;)
+Vera Maria Ahh... its acetylen!
I love you so much lifesaver
Thank you so much
thank you so much