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anonymous
 4 years ago
Hey,
I'm having trouble understanding a result of a chemist lab which involved computing the energies of molecules using software. I found the energies of (Z) 1,1 diisopropyl ethene, (E) 1,1 diisopropyl ethene and 1,1 diisopropyl ethane to be 102.10 , 102.17, and 89.49 kJ/mol, respectively. I understand why the E isomer is more stable than the Z isomer, but why is the 1,1 diisopropyl ethane less stable than both of the others?
anonymous
 4 years ago
Hey, I'm having trouble understanding a result of a chemist lab which involved computing the energies of molecules using software. I found the energies of (Z) 1,1 diisopropyl ethene, (E) 1,1 diisopropyl ethene and 1,1 diisopropyl ethane to be 102.10 , 102.17, and 89.49 kJ/mol, respectively. I understand why the E isomer is more stable than the Z isomer, but why is the 1,1 diisopropyl ethane less stable than both of the others?

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anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0I was thinking that the ability to rotate around the single bond would allow it to reduce any steric stress, but this isn't reflected in the software. Why is this?
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