Chemistry Why does Hexane have higher intermolecular force than Propylamine?

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Hexane exhibits higher intermolecular forces than propylamine despite propylamine's ability to form hydrogen bonds due to its lower molecular weight and larger surface area, which enhances van der Waals forces in hexane. The discussion highlights the importance of considering molecular structure and functional groups when comparing intermolecular forces. While propylamine can form hydrogen bonds, its overall molecular interactions may be weaker than those of larger alkanes like heptane or octane. Additionally, the comparison with butylamine suggests that molecular size and structure significantly influence intermolecular forces. Understanding these concepts is crucial for analyzing the behavior of different organic compounds.
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< Moderator Note -- thread moved to Homework Help forums >[/color]

Shouldn't Propylamine (C3H7NH2) be able to form hydrogen bonds with alike molecules?
Hexane (c6h14) doesn't seem to have hydrogen bonding capability.
 
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This is homework and in the future, should be posted in HW Help. What functional groups are you comparing between the two molecules?
 
Bystander said:
This is homework and in the future, should be posted in HW Help.
No it's not HW. I'm asking to explain the answer. Not to solve it.
Bystander said:
What functional groups are you comparing between the two molecules?
If I say "hexane" I clearly mean the whole molecule.
So, why does hexane have higher intermolecular force than propylamine, if the latter has the hydrogen bonding capability (since its Hydrogen is bonded to Nitrogen).
 
Why do heptane, octane, nonane, decane, undecane, ad nausea have higher intermolecular forces than propylamine. Why does butylamine have higher intermolecular forces than propylamine?
 
How do I know? That's why I'm asking!
 
What is the structure of propylamine, and how does it differ from that of butylamine?
 

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