Scale-free network

A graph of strength versus distance for the 12-6 Lennard-Jones potential.

Template:Computational physics The Lennard-Jones potential (also referred to as the L-J potential, 6-12 potential, or 12-6 potential) is a mathematically simple model that approximates the interaction between a pair of neutral atoms or molecules. A form of the potential was first proposed in 1924 by John Lennard-Jones. The most common expressions of the L-J potential are

${\begin{alignedat}{3}V_{LJ}&=4\varepsilon &\left[\left({\frac {\sigma }{r}}\right)^{12}-\left({\frac {\sigma }{r}}\right)^{6}\right]\\&=\varepsilon &\left[\left({\frac {r_{m}}{r}}\right)^{12}-2\left({\frac {r_{m}}{r}}\right)^{6}\right]\end{alignedat}}$

where ε is the depth of the potential well, σ is the finite distance at which the inter-particle potential is zero, r is the distance between the particles, and r_m is the distance at which the potential reaches its minimum. At r_m, the potential function has the value −ε. The distances are related as r_m = 2^1/6σ. These parameters can be fitted to reproduce experimental data or accurate quantum chemistry calculations. Due to its computational simplicity, the Lennard-Jones potential is used extensively in computer simulations even though more accurate potentials exist.

Explanation

The r⁻¹² term, which is the repulsive term, describes Pauli repulsion at short ranges due to overlapping electron orbitals and the r⁻⁶ term, which is the attractive long-range term, describes attraction at long ranges (van der Waals force, or dispersion force). Whereas the functional form of the attractive term has a clear physical justification, the repulsive term has no theoretical justification. It is used because it approximates the Pauli repulsion well, and is more convenient due to the relative computational efficiency of calculating r¹² as the square of r⁶.

The Lennard-Jones (12,6) potential can be further approximated by the (exp-6) potential later proposed by R. A. Buckingham, in which the repulsive part is exponential:

$V_{B}=\gamma \left[e^{-r/r_{0}}-\left({\frac {r_{0}}{r}}\right)^{6}\right].$

The L-J potential is a relatively good approximation and due to its simplicity is often used to describe the properties of gases, and to model dispersion and overlap interactions in molecular models. It is particularly accurate for noble gas atoms and is a good approximation at long and short distances for neutral atoms and molecules.

The lowest energy arrangement of an infinite number of atoms described by a Lennard-Jones potential is a hexagonal close-packing. On raising temperature, the lowest free energy arrangement becomes cubic close packing and then liquid. Under pressure the lowest energy structure switches between cubic and hexagonal close packing. Real materials include BCC structures as well.

Other more recent methods, such as the Stockmayer potential, describe the interaction of molecules more accurately. Quantum chemistry methods, Møller–Plesset perturbation theory, coupled cluster method or full configuration interaction can give extremely accurate results, but require large computational cost.

Alternative expressions

There are many different ways of formulating the Lennard-Jones potential The following are some common forms.

AB form

This form is a simplified formulation that is used by some simulation software packages:

$V_{LJ}(r)={\frac {A}{r^{12}}}-{\frac {B}{r^{6}}},$

where, $A=4\varepsilon \sigma ^{12}$ and $B=4\varepsilon \sigma ^{6}$. Conversely, $\sigma ={\sqrt[{6}]{\frac {A}{B}}}$ and $\varepsilon ={\frac {B^{2}}{4A}}$. This is the form in which Lennard-Jones wrote the 12-6 potential.

Truncated Lennard-Jones potential

To save computational time, the Lennard-Jones potential is often truncated at a cut-off distance of r_c = 2.5σ, where

$\displaystyle V_{LJ}(r_{c})=V_{LJ}(2.5\sigma )=4\varepsilon \left[\left({\frac {\sigma }{2.5\sigma }}\right)^{12}-\left({\frac {\sigma }{2.5\sigma }}\right)^{6}\right]\approx -0.0163\varepsilon$

(1)

i.e., at r_c = 2.5σ, the Lennard-Jones potential, V_LJ, is about 1/60th of its minimum value, ε (the depth of the potential well). Beyond $\displaystyle r_{c}$, the truncated potential is set to zero.

To avoid a jump discontinuity at $\displaystyle r_{c}$, the LJ potential must be shifted upward a little so that the truncated potential would be zero exactly at the cut-off distance, $\displaystyle r_{c}$.

For clarity, let $\displaystyle V_{LJ}$ denote the LJ potential as defined above, i.e.,

$\displaystyle V_{LJ}(r)=4\varepsilon \left[\left({\frac {\sigma }{r}}\right)^{12}-\left({\frac {\sigma }{r}}\right)^{6}\right].$

(2)

Then the truncated Lennard-Jones potential $\displaystyle V_{{LJ}_{trunc}}$ is defined as follows

$\displaystyle V_{{LJ}_{trunc}}(r):={\begin{cases}V_{LJ}(r)-V_{LJ}(r_{c})&{\text{for }}r\leq r_{c}\\0&{\text{for }}r>r_{c}.\end{cases}}$

(3)

It can be easily verified that V_LJtrunc(r_c) = 0, thus eliminating the jump discontinuity at r = r_c. Although the value of the (unshifted) Lennard Jones potential at r = r_c = 2.5σ is rather small, the effect of the truncation can be significant, for instance on the gas–liquid critical point. Fortunately, the potential energy can be corrected for this effect in a mean field manner by adding so-called tail corrections.

Limitations of the Lennard-Jones Potential

• The L-J Potential has only two parameters (A and B) and so can be fit to a maximum of two physical quantities. It may be necessary to match three different properties (for example, a length scale, an energy scale and elasticity). It is impossible to match all three properties together with the Lennard-Jones potential.

• With the L-J potential, the number of atoms bonded to an atom does not affect the bond strength. The bond energy per atom therefore increases linearly with the number of bonds per atom. Experiments show instead that the bond energy per atom increases quadratically with the number of bonds Template:Cn.

• Bonding has no directionality: the potential is spherically symmetric. Directional bonding is important for many systems.

• The sixth-power term models dipole-dipole interactions due to electron dispersion in noble gasses (London dispersion forces), but it does not represent other kinds of bonding well. The twelfth-power term appearing in the potential is chosen for its ease of calculation for simulations (by squaring the sixth-power term) and is not physically based.

• The potential diverges when two atoms approach one another. This may create instabilities that require special treatment in molecular dynamics simulations.

See also

• Morse/Long-range Potential
• Molecular mechanics
• Embedded atom model
• Morse potential
• Force field (chemistry)
• Force field implementation
• Lennard-Jones model on SklogWiki.

References

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