Cyclopentane adopts two puckered conformations, as well as a planar conformation. Name the two puckered forms...

Cyclopentane adopts two puckered conformations, as well as a planar conformation. Name the two puckered forms and explain why they are lower in energy than the planar form of cyclopentane.

Expert Solution

2nd-If one takes one end of the cyclopentane and “pulls” it up, then we will have a “envelope” conformation of cyclopentane. If you try this with a model you will note that there will be rotations about 2 different C-C bonds, and this will result in them no longer being completely eclipsed.This results in significantly less torsional strain

3rd-The “TWIST BOAT”. A significant portion of Van Der Waals strain of the boat can be relieved by a slight rotation of the bonds, resulting in a conformation known as the “twist boat”. Drawings don’t do it adequate justice – for this one you really need to build a model to see how a slight twisting of the structure can result in less strain. There is still significant torsional strain since there are two C-C bonds about which the hydrogens are not perfectly staggered.

queen_honey_blossom answered 4 months ago

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Cyclopentane adopts two puckered conformations, as well as a planar conformation. Name the two puckered forms...

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