Respuesta :
Answer:
C₂H₂ > C₂H₄ > C₂H₆
Explanation:
Greater the number of bonds, greater is the bond strength and lesser is the bond length. Sigma bonds are stronger than pi bonds.
Câ‚‚Hâ‚‚, ethyne has 1 sigma and 2 pi bonds with sp- hybridization.
The sp orbitals of carbon atoms overlap to give sigma bond and the other two p-orbitals of carbons overlap to give 2 pi bonds.
C₂H₄, ethene has 1 sigma and 1 pi bond with sp²- hybridization.
The sp² orbitals of carbon atoms overlap to give sigma bond and p-orbitals of carbons overlap to give 2 pi bonds.
C₂H₆ , ethane has 1 sigma and 0 pi bond with sp³- hybridization.
The sp³ orbitals of carbon atoms overlap to give sigma bond and there are no p-orbitals left for pi bond to be formed.
Decreasing bond strength order is
C₂H₂ > C₂H₄ > C₂H₆
The ranking is C₂H₂ > C₂H₄ > C₂H₆
Relation of bond and bond strength & length:
The greater the number of bonds, the greater is the bond strength and the lesser is the bond length. Sigma bonds should be stronger as compared to pi bonds.
So,
Câ‚‚Hâ‚‚, ethyne has 1 sigma and 2 pi bonds with sp- hybridization.
C₂H₄, ethene has 1 sigma and 1 pi bond with sp²- hybridization.
C₂H₆ , ethane has 1 sigma and 0 pi bond with sp³- hybridization.
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