Firstly, here's the question,
When the cyclohexanone shown is dissolved in d6-benzene, 3JAB = 3.0 Hz. When the same molecule is dissolved in d4-methanol, 3JAB = 11.0 Hz. What are the conformations in these two solvents and why do the conformations differ. *Structure attached*
This is what i'm thinking so far,
So when methanol is the solvent, the coupling constant is 11Hz, thus the bond angle between Ha and Hb is 180, thus they are each in axial positions. The CHMe2 group is in the equatorial possie. We'll call this structure A.
When benzene is the solvent, the coupling constant is 3Hz, thus the bond angle between Ha and Hb is ~60, thus they are each in equatorial positions. The CHMe2 group is in the axial possie. We'll call this structure B.
So ring flip causes the coupling constant to change from 3 to 11, or vice versa. Obviously this has something to do with the solvent. One of the major differences between benzene and methanol is methanols ability to form hydrogen bonds. Does forming hydrogen bonds somehow allow the conversion from B to A? This would explain the change in coupling constants when methanol is used over benzene.
However as you may know, the CHMe2 group is much more stable in the equatorial possie, due to a number of reasons. So wouldn't structure B just flip into structure A automatically, given the added stability associated with structure A? Thus not needing the methanol?
I think i'm either a/ missing something basic here, or b/ looking too far into the question.
Any assistance is appreciated.