So any data sheet will tell you;

Group 1: methane boils at: -164 deg C
         methanol boils at: 65 deg C 

Group 2: decane boils at: 174 deg C
         1-decanol boils at 229 deg C 

that being said; why is the difference in boiling point so much greater between methanol and methane than it is between 1 decanol and decane ?

As well is there anything else other than difference in non-polarity and IMF's that contribute to differences between molecules in individual groups (i.e. between methane and methanol; between decane and 1-decanol)

| improve this question | | | | |

The difference in boiling point, between methanol and methane on one hand and between 1-decanol and decane on the other hand, is primary due to the presence of hydrogen bonds (HB) in methanol and 1-decanol and not in methane and decane. The density of these intermolecular forces (HB) is higher in methanol than in 1-decanol (In 1-decanol, for every ten atoms of carbon there's one possibility to have HB. While in methanol for every atom of carbon there's one possibility to have HB.

| improve this answer | | | | |

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.