What Determines the Dependence of Dipole-Dipole Interactions on Distance?

In summary, the sixth root dependency on the inverse of the distance between dipoles in any dipole-dipole interaction can be mathematically derived through the use of Coulomb's law and the binomial expansion. The potential energy falls as 1/r^6 due to the induced dipole moments between the two dipoles. The remaining orders in the denominator represent permutations for Coulomb forces, and the extra two orders of displacement are accounted for through the binomial expansion with dipole separation approaching zero.
  • #1
LeoYard
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What is the basis for the sixth root dependancy on the inverse of the distance between the dipoles (in any dipole-dipole interaction)? Is it empirical or can it be mathematically derived?
 
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  • #3
Though I should add that it is possible to derive the long distance attraction between dipoles theoretically. It's an elementary exercise in electrostatics -- if you get stuck, post your efforts here and I'm sure PF members will guide you.
 
  • #4
Thank you, genneth. Coulomb's law states that the electric field from a point charge drops as the square of the radius. Put two charges at the same place and you get zero electric field, so the two charges need to be slightly displaced. However, as you go to large radii, the separation between the two charges becomes irrelevant, so that starts to look more like a zero-charge object.
 
  • #5
Not quite. A dipole field falls off as 1/r^3 at large distances -- it's a tedious calculation, but you should learn to do it anyway, since it's quite typical of mathematical analysis of physics. Another dipole would feel 1/r^4 attraction. However, the usual law assumes induced dipole moments, so you get another 1/r^2 factor.

(I think -- all this is off the top of my head.)
 
  • #6
LeoYard said:
What is the basis for the sixth root dependancy on the inverse of the distance between the dipoles (in any dipole-dipole interaction)? Is it empirical or can it be mathematically derived?
I assume you mean the the potential energy falls like 1/r^6.
The interaction energy of a dipole in an electric field = -p.E.
E of a dipole varies like 1/r^3, so the energy of two permanent dipoles varies like 1/r^3.
The 1/r^6 results if the dipole moments are induced dipoles, that is each dipole moment is caused by the E field of the other dipole. This gives another factor of 1/r^3,
resulting in the 1/r^6 for the energy of two induced dipoles.
 
  • #7
Four of the six radial orders in the field's denominator represent the permutations for Coulomb forces between the charges in the two dipoles. Binomial expansion with dipole separation approaching zero accounts for the extra two orders of displacement.
 

Related to What Determines the Dependence of Dipole-Dipole Interactions on Distance?

What are dipole-dipole interactions?

Dipole-dipole interactions are a type of intermolecular force that occurs between molecules that have a permanent dipole moment. This means that the molecules have a slightly positive and negative end, and these charges can interact with each other.

How do dipole-dipole interactions differ from other intermolecular forces?

Dipole-dipole interactions are stronger than London dispersion forces, but weaker than hydrogen bonding. They also differ from ionic bonds, as they occur between neutral molecules rather than ions.

What causes dipole-dipole interactions?

Dipole-dipole interactions are caused by the attraction between the positive and negative ends of two polar molecules. This attraction is strongest when the molecules are in close proximity to each other.

How do dipole-dipole interactions affect the properties of a substance?

Dipole-dipole interactions can affect the melting and boiling points of a substance, as well as its solubility in polar solvents. They also play a role in determining the structure and stability of molecules in a substance.

Can dipole-dipole interactions be broken or disrupted?

Yes, dipole-dipole interactions can be disrupted by changes in temperature or pressure, as well as by the presence of other molecules or ions that can interact with the polar molecules. Additionally, molecular motion can also weaken or break dipole-dipole interactions.

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