Why does Hexane have higher intermolecular force than Propylamine?

In summary, the discussion is about the hydrogen bonding capabilities of propylamine and hexane. While propylamine has the ability to form hydrogen bonds due to its functional group of a nitrogen atom bonded to three hydrogen atoms, hexane does not have this capability. The question also raises the comparison of intermolecular forces between different molecules, such as heptane, octane, nonane, decane, undecane, and butylamine. The structure of propylamine is mentioned as a point of comparison with butylamine to understand the difference in intermolecular forces.
  • #1
dramadeur
19
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< Moderator Note -- thread moved to Homework Help forums >

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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  • #2
This is homework and in the future, should be posted in HW Help. What functional groups are you comparing between the two molecules?
 
  • #3
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).
 
  • #4
Why do heptane, octane, nonane, decane, undecane, ad nausea have higher intermolecular forces than propylamine. Why does butylamine have higher intermolecular forces than propylamine?
 
  • #5
How do I know? That's why I'm asking!
 
  • #6
What is the structure of propylamine, and how does it differ from that of butylamine?
 

1. Why does Hexane have higher intermolecular force than Propylamine?

Hexane has a higher intermolecular force than propylamine because it is a non-polar molecule, meaning it has a symmetrical distribution of charge. This allows for stronger dispersion forces between molecules, resulting in a higher intermolecular force.

2. What is the difference between intermolecular forces in Hexane and Propylamine?

The main difference between the intermolecular forces in hexane and propylamine is the type of force present. Hexane has only dispersion forces, while propylamine has both dispersion forces and dipole-dipole interactions. This results in a stronger overall intermolecular force in hexane.

3. How do the molecular structures of Hexane and Propylamine affect their intermolecular forces?

The molecular structure of hexane, with its long, linear carbon chain, allows for a greater surface area for dispersion forces to act upon. On the other hand, the polar nitrogen atom in propylamine allows for dipole-dipole interactions in addition to dispersion forces. These structural differences contribute to the difference in intermolecular forces between the two molecules.

4. Can the strength of intermolecular forces in Hexane and Propylamine be predicted based on their molecular formula?

Yes, the strength of intermolecular forces in hexane and propylamine can be predicted based on their molecular formula. Non-polar molecules, such as hexane, have stronger dispersion forces due to their symmetrical charge distribution. Polar molecules, like propylamine, have stronger dipole-dipole interactions in addition to dispersion forces.

5. How do intermolecular forces affect the physical properties of Hexane and Propylamine?

The intermolecular forces in hexane and propylamine contribute to their physical properties, such as boiling point and viscosity. Hexane has a lower boiling point and lower viscosity due to its weaker intermolecular forces, while propylamine has a higher boiling point and viscosity due to its stronger intermolecular forces.

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