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What makes the cyclic structure of glucose more stable than the open chain structure?
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Justin Harper
What makes the cyclic structure of glucose more stable than the open chain structure?
You get to form a C-O $\mathrm{\sigma}$ bond at the expense of a C-O $\mathrm{\pi}$ bond. The single bond has a higher bond energy, even though it is somewhat de-stabilized by the anomeric effect. It's still an overall win, despite taking the entropic hit to confine your molecule into a ring.
You get to form a C-O $\mathrm{\sigma}$ bond at the expense of a C-O $\mathrm{\pi}$ bond. The single bond has a higher bond energy, even though it is somewhat de-stabilized by the anomeric effect. It's still an overall win, despite taking the entropic hit to confine your molecule into a ring.
Irrelevant was the wrong word. I meant to say that taking into account the entropic effect, it becomes temperature-dependent, and no temperature was specified.More
@Karl Thats not correct. The free energy difference between the open-chain and ring forms has a entropic component because the open-chain has more degrees of freedom.More
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The carbon atoms in the gulucose ring each have four covalent bonds ......it follows,therefore,that the gulucose molecule will be at its most stable when all carbon atoms can arrange themselves , so that their bond angles are all close to 109.5 degree .
The carbon atoms in the gulucose ring each have four covalent bonds ......it follows,therefore,that the gulucose molecule will be at its most stable when all carbon atoms can arrange themselves , so that their bond angles are all close to 109.5 degree .
You get to form a C-O $\mathrm{\sigma}$ bond at the expense of a C-O $\mathrm{\pi}$ bond. The single bond has a higher bond energy, even though it is somewhat de-stabilized by the anomeric effect. It's still an overall win, despite taking the entropic hit to confine your molecule into a ring.
You get to form a C-O $\mathrm{\sigma}$ bond at the expense of a C-O $\mathrm{\pi}$ bond. The single bond has a higher bond energy, even though it is somewhat de-stabilized by the anomeric effect. It's still an overall win, despite taking the entropic hit to confine your molecule into a ring.
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The carbon atoms in the gulucose ring each have four covalent bonds ......it follows,therefore,that the gulucose molecule will be at its most stable when all carbon atoms can arrange themselves , so that their bond angles are all close to 109.5 degree .
The carbon atoms in the gulucose ring each have four covalent bonds ......it follows,therefore,that the gulucose molecule will be at its most stable when all carbon atoms can arrange themselves , so that their bond angles are all close to 109.5 degree .
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