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.
C₂H₂, 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,
C₂H₂, 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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