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anonymous
 one year ago
For the substituted cyclohexane compound given below, highlight the groups – by clicking on atoms – that will sterically interact with the methyl group in a 1,3diaxial fashion.
anonymous
 one year ago
For the substituted cyclohexane compound given below, highlight the groups – by clicking on atoms – that will sterically interact with the methyl group in a 1,3diaxial fashion.

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greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2Well for starters, axial groups are those that point either directly up or directly down on our chair form of cyclohexane for example: dw:1441936471814:dw these are the positions of all our axial groups on the chair form of cyclohexane. infact, it is not advisable to have large groups at the axial position, because there is a phenomena called 13, di axial interactions, meaning that the electron clouds of certain groups will repel eachother making our chair conformation less stable. If possible, what will happen is something called a ring flip. the ring will flip to minimize some of the repulsion caused by the 13 di axial interaction and will stay in the more stable conformation more.

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2In your figure it translates to this dw:1441936710898:dw

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2All of the groups I circled groups are axial in this depiction; Well the CH3 should be also circled, i'm sorry for that. If I am correct, this molecule may under go a ring flip and when a ring flip happens all the groups that are axial become equatorial and all the equatorial groups become axial.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0How do I know which group will sterically interact?

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2For this i'm not too sure but I believe there are 2 interactions at most possibly 3. the atoms have to be at the 3 position. so look at the axial group and label that as carbon 1, then count until you find the third atom and then look at the group that's axial. dw:1441936984215:dw

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2Consequently, the molecule will naturally flip if it can to minimize these 1,3diaxial interactions, naturally this puts alot of strain on our molecule NOTE: These interactions only happen at groups that are in the axial positions. equatorial positions are irrelevant.

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2Just to show you how to do this and for anyone else who is reading this: dw:1441937554093:dw

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2Ring flips CAN and WILL happen but only if it results in fewer of these 1,3 diaxial interactions.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I understand what you are saying. Will the answer include the while group or just the carbon?

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2good question, I didn't specify. the 13 diaxial interaction will include only the group that is in the axial position bonded to the carbon on the ring, not the carbon itself. is that what you meant?

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2@sharmar25 the interactions will be between the two groups at the axial positions as shown, not necessarily the carbons in the ring. steric interaction implies repulsion between groups. Imagine each group as an electron cloud, two negative charges will repel, that's why the molecule tries to minimize this if it can. dw:1441938341493:dw

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2One last example: say if we had something like this: for instance an oxygen bonded to a hydrogen at one of the groups in the axial position. Say if we didn't have any other groups just hydrogen at the axial positions. This is also a 1,3 di axial interaction, although one of a different kind. it's possible that the lone pair of electrons on the oxygen will hydrogen bond to one of the nearby hydrogens. dw:1441938504189:dw

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Yes. Thats what I was asking. Thank so much for your help.

greatlife44
 one year ago
Best ResponseYou've already chosen the best response.2Absolutely, hope this helps you and anyone else reading this take care

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Yeah this was an awesome answer @greatlife44
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