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Explain hybridization and bond structure of ethane (C_(2) H_(6)) molecule. |
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Answer» Solution :`sp^(3)` HYBRIDIZATION of carbon: The ground state of carbon [He] `2s^(2) 2p^(2) 2s^(2)` the one electron of `2s^(2)` is go in empty ORBITAL of 2p and form exicted carbon (C*).C* [He] `2s^(1) 2p_(x)^(1) 2p_(y)^(1) 2p_(z)^(1)` The four half filled orbitals of excited carbon overlap & form `sp^(3)` hybrid orbital arrange in tertahydron at `109.5^(@)`ANGLE so repulsion between them remain minimum.  Bonding in `C_(2)H_(6)`: From the four `sp^(3)` hybrid orbitals of the carbon and form an C- H sigma bond still both carbon has three half filled `sp^(3)` orbital which axially overlap with ls orbital of hydrogen and form C-H 6 sigma bond. In this way total SIX C- H sigma bond and one C- C sigma bond total seven sigma bond from in `C_(2)H_(6)`. In ethane all carbon has tetrahedral geometry.  In ethane all carbon has tetrahedral geometry . |
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