Potential Energy of London interactions
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Potential Energy of London interactions
The equation for the potential energy of London interactions is -(alpha1*alpha2)/r^6. The concept that the potential energy increases with increasing polarizability of the molecules involved makes sense to me. However, for highly polarizable molecules, we would expect for them to have a larger radius since the outer electrons are farther from the nucleus and therefore more easily distorted. If this is case and the radius increases with polarizability, then wouldn't it make since for the potential energy of the London interaction to decrease (since the equation divides by the sixth power of the radius)?
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Re: Potential Energy of London interactions
In terms of bond strength: type of bond is more important than size of molecule
A larger radius, as you said, implies greater electron distortion
Greater distortion of electrons means that the atom is more easily polarizable: will more easily form a dipole
Since LDF forces are based on the formation of a dipole, an increased likelihood of dipole formation corresponds more to increased bond strength, rather than radius size.
A larger radius, as you said, implies greater electron distortion
Greater distortion of electrons means that the atom is more easily polarizable: will more easily form a dipole
Since LDF forces are based on the formation of a dipole, an increased likelihood of dipole formation corresponds more to increased bond strength, rather than radius size.
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Re: Potential Energy of London interactions
London Forces are the weakest forms of bonds created by instances moments of ionization, therefore bond length does not necessarily matter when discussing these bonds as their potential energy Is more influenced on the type of bond rather than distance.
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