Ethene CH2CH2 aka CH2=CH2 has a lower boiling point than Ethane CH2CH3. Why is this? The ethene has double bonds and the ethane has single bonds. Shouldnt the boiling point of ethene be the highest?
Why is it that the boiling point of ethyne is the lowest, followed by ethene and ethane when comparing the two carbon chains?
Why is it that the boiling point of ethyne is the lowest, followed by ethene and ethane when comparing the two carbon chains?
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See, Alkane(ethane) has only C-H bonds and C-C bonds(other than Meth-) so they are relatively stronger because they are more STABLE. Then Alkene(ethene) have and extra C=C bonds which are LESS Stable.
And alkyne has the lowest be cause it has much more Unstable C≡C bonds.
A way to explain this is a double bond is stronger than a single bond. However, it is not twice as strong as a single bond. In other words, two single bonds are stronger than one double bond, but in addition to being stronger it is more reactive too.
And alkyne has the lowest be cause it has much more Unstable C≡C bonds.
A way to explain this is a double bond is stronger than a single bond. However, it is not twice as strong as a single bond. In other words, two single bonds are stronger than one double bond, but in addition to being stronger it is more reactive too.