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Homolytic fission of carbon-carbon bond of ethane produces an intermediate in which the carbon atom is in
- a)sp2 hybridized state
- b)sp3 hybridized state
- c)sp hybridized state
- d)dsp2 hybridized state
Correct answer is option 'A'. Can you explain this answer?
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Homolytic fission of carbon-carbon bond of ethane produces an intermed...
Explanation:
Homolytic fission of carbon-carbon bond of ethane refers to the process of breaking the bond between two carbon atoms in such a way that each carbon atom gets one electron from the bond. This leads to the formation of two carbon-centered free radicals.
The carbon atom in the intermediate is in sp2 hybridized state. This can be explained as follows:
- Before the bond fission, each carbon atom in ethane is sp3 hybridized, with four hybrid orbitals oriented in tetrahedral geometry.
- When the bond fission occurs, one of the four hybrid orbitals on each carbon atom participates in the bond formation with the other carbon atom, leaving behind three hybrid orbitals and one unhybridized p orbital on each carbon atom.
- The unhybridized p orbitals on each carbon atom overlap sideways with each other to form a pi bond, which is responsible for the double bond character of the C=C bond.
- The three remaining hybrid orbitals on each carbon atom now participate in the formation of sigma bonds with the hydrogen atoms attached to them. This leads to the formation of a planar molecule with each carbon atom in sp2 hybridized state, having three sigma bonds and one unhybridized p orbital perpendicular to the plane of the molecule.
Therefore, the carbon atom in the intermediate formed by homolytic fission of the C-C bond in ethane is also in sp2 hybridized state, having three sigma bonds and one unhybridized p orbital.
Homolytic fission of carbon-carbon bond of ethane refers to the process of breaking the bond between two carbon atoms in such a way that each carbon atom gets one electron from the bond. This leads to the formation of two carbon-centered free radicals.
The carbon atom in the intermediate is in sp2 hybridized state. This can be explained as follows:
- Before the bond fission, each carbon atom in ethane is sp3 hybridized, with four hybrid orbitals oriented in tetrahedral geometry.
- When the bond fission occurs, one of the four hybrid orbitals on each carbon atom participates in the bond formation with the other carbon atom, leaving behind three hybrid orbitals and one unhybridized p orbital on each carbon atom.
- The unhybridized p orbitals on each carbon atom overlap sideways with each other to form a pi bond, which is responsible for the double bond character of the C=C bond.
- The three remaining hybrid orbitals on each carbon atom now participate in the formation of sigma bonds with the hydrogen atoms attached to them. This leads to the formation of a planar molecule with each carbon atom in sp2 hybridized state, having three sigma bonds and one unhybridized p orbital perpendicular to the plane of the molecule.
Therefore, the carbon atom in the intermediate formed by homolytic fission of the C-C bond in ethane is also in sp2 hybridized state, having three sigma bonds and one unhybridized p orbital.
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Homolytic fission of carbon-carbon bond of ethane produces an intermediate in which the carbon atom is ina)sp2 hybridized stateb)sp3 hybridized statec)sp hybridized stated)dsp2 hybridized stateCorrect answer is option 'A'. Can you explain this answer?
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