Question

ompare he orbital hybr re 7 Und e hylene

Answer 1

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(b) There is rigidity in the Ethene molecule due to the double-bonded carbons. In Ethane there are two carbons that share a single bond, this allows the two Methyl groups to rotate with respect to each other. These different conformations result in higher and lower energy forms of Ethane. In Ethene there is no free rotation about the carbon-carbon sigma bond. There is no rotation because there is also a ππ bond along with the sigma bond between the two carbons. A ππ bond is only formed when there is adequate overlap between both top and bottom p-orbitals. In order for there to be free rotation the p-orbitals would have to go through a phase where they are 90° from each other, which would break the ππ bond because there would be no overlap. Since the ππ bond is essential to the structure of Ethene it must not break, so there can be not free rotation about the carbon-carbon sigma bond.
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(c) In ethane there is single sigma bond where as there is double bond in ethylene between carbon carbon bond which consist of pi bond formed due to sideways overlap of 2p orbitals of carbon atoms in addition to sigma bonds. Pi and sigma bond together form a double bond which is stronger and shorter than a sigma bond.