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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?
 2 years ago
 2 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?
 2 years ago
 2 years ago

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ggrreeBest ResponseYou've already chosen the best response.0
I 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?
 2 years ago
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