Please, like, share, and comment to help promote this video! If you would like to support the channel, you can do so by either donating or becoming a member: Donate: www.organicchemistrytutor.com/donate/ Membership www.organicchemistrytutor.com/membership/
Remember that solvent is a facilitator of the reaction. It won’t usually determine the mechanism. So, first look at the nature of the reagent, then the position of your leaving group, and only then at the temperature and solvent. I’ve got more on that in the substitution and elimination playlist.
Is it though? It has a dipole moment of 0.45, it's not as polar as THF or DCM for instance, but it's polar enough and fulfills the same function of creating a solvation shell around cations. Edit: yes, it is technically non-polar if we stick to the strict definition and polarity cutoffs for polar solvents. I base my list on the "Solvents and Solvent Effects in Organic Chemistry" which is a commonly referenced publication for such comparisons.
@@rockubabe No worries, I suspected you might've misinterpreted something. But you did make me go over my videos and materials on the website wondering if I brainfarted that bad 😂
Please, like, share, and comment to help promote this video!
If you would like to support the channel, you can do so by either donating or becoming a member:
Donate: www.organicchemistrytutor.com/donate/
Membership www.organicchemistrytutor.com/membership/
Helpful ❤
Thanks!! My all questions are almost solved
Which has greater nucleophilicity in each case
Cyclohexanol and cyclohexanamine in polar protic and polar aprotic solvents
How did you read my mind? I was going over Sn1 and Sn2. The solvents kept messing up my questions!
Remember that solvent is a facilitator of the reaction. It won’t usually determine the mechanism. So, first look at the nature of the reagent, then the position of your leaving group, and only then at the temperature and solvent. I’ve got more on that in the substitution and elimination playlist.
1,4 dioxane is non-polar though
Is it though? It has a dipole moment of 0.45, it's not as polar as THF or DCM for instance, but it's polar enough and fulfills the same function of creating a solvation shell around cations.
Edit: yes, it is technically non-polar if we stick to the strict definition and polarity cutoffs for polar solvents. I base my list on the "Solvents and Solvent Effects in Organic Chemistry" which is a commonly referenced publication for such comparisons.
I'm not sure why ethanol is classified as poor nucleophile/base according to my instructor, but base+nucleophile according to your system?...
What are you talking about? I've never classified ethanol as a base/nucleophile.
@@VictortheOrganicChemistryTutor Omg..I'm dumb. EtO. That's not Ethanol. Sorry, my bad.
@@rockubabe No worries, I suspected you might've misinterpreted something. But you did make me go over my videos and materials on the website wondering if I brainfarted that bad 😂