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Chapter 3:Interatomic Potential
3.1 Introduction to interatomic potentials
In Molecular Dynamics (MD) and Monte Carlo (MC) simulation we must have some
rules, which governs the interactions between the atoms. In classical simulation these
rules are expressed in terms of potential functions. Interatomic potential describes how
the atoms interact with each other.For example, in case of ionic solids the main source of
cohesion is Columbic attraction force. Ions with the opposite charge attract each other. In
the absence of any repulsive force all the atoms will collapse into one point. But this does
not happen in real case so there must be some repulsive force, which prevents the atoms
to collapse into one point. There are two types of repulsive forces in ionic solids. One is
due to Columbic interaction. Ions with the same charge repulse ease other. Also when the
ions comes very close to each other a strong repulsive force due to Paulis exclusion
principle acts which is a very strong function of distance between the ions. There is one
more kind of interaction between the ions is van der Waals interaction. Which is the
weakest interaction among all. Similarly in case of metals the main source of cohesion is
free electrons. In case of metallic solids it is assumed that there is a pool of free electrons
and positive ions are submerged in the pool. So more the density of free electrons
stronger will be the attractive force. Similar to the ionic case a strong repulsive force, due
to Paulis exclusion principle, acts when the atoms comes very close to each other. The
potential function U(r1, r2, , rN) describes how the potential energy of a system of N
atoms depends on the coordinates of the atoms, r1, r2, , rN. In classical MD or MC
simulation electrons comes nowhere in the calculations. It is assumed the electrons adjust
to new atomic positions much faster than the motion of the atomic nuclei (Born-
Oppenheimer approximation). The behavior of the electrons is approximated in thepotential itself.
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3.2 How to obtain the potential function for a particular system?
3.2.1 Empirical potential function: A functional form is assumed for the
potential function and then we fit the parameters to reproduce a set of experimental data
like lattice parameter, elastic constants, thermal expansion coefficient etc. This gives
empirical potential functions (e.g. Lennard-Jones, Morse, Born-Mayer). These potentials
have no direct physical basis but still widely used in many types of problems because of
their simplicity, computationally less expensive and reasonable accuracy.
3.2.2 Semi-empirical Potentials:The electronic wave function can be calculated
for fixed atomic positions. But for a system consist of many atoms this type of calculation
is very difficult. Different approximations are used and analytic semiempirical potentials
are derived from quantum-mechanical arguments (e.g. Embedded Atom Method (EAM)
by Foiles, Baskes, and Daw, Glue Model by Ercolessi et al., bondorder potentials by
Tersoff and Brenner, etc.). These are also called many body potential because the
potential depends on the density of surrounding atoms. These potentials are more
complex and computationally more expensive but provide good description of different
types of materials like metals and ceramics.
3.2.3 Potentials from Ab-initio calculations: Direct electronic-structure
(quantum-mechanics-based) calculations of forces can be performed during so-called ab-
initio MD simulation (e.g., Carr-Parrinello method using plane-wave psuedopotentials).
Potentials obtained from ab-initio method are most accurate because these are obtained
from electronic calculation using first principle and number of assumptions or
experimental parameters used is negligible. For more detailed and elaborated analysis
these types of potentials are used.
3.3 The Born-Oppenheimer approximation
In the MD and MC methods potential functions are used to describe the interactionamong the atoms. But in actual case atoms consist of a nucleus and electrons around it
and electrons play a vital role in defining the interactions and bonds between the atoms.
In the potential functions interaction of electrons with nuclei are not considered. Is the
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use of the potential function is justified. Hamiltonian of the real material is defined by the
presence of nuclei and electrons and can be written as follows:
+
++=i i
2i
2
ij ji
2ji
2
i i
2i
rR
eZ
2
1
rr
e
2
1
RR
eZZ
2
1
2m
p
2M
PH
3.3.1
where Pi, Mi, Ri and Zi are momentum, mass, coordinates and atomic number of the
nucleus i and p, m, r and e are momentum, mass, coordinates and charge on electron .
A Schrdinger equation H=E should be solve to get the total wavefunction (Ri, r),
which tells everything about the system. But this is impossible for any system of practical
use. In 1923 Born and Oppenheimer shown that the electrons (me=5.510-4 amu) are
much lighter than nuclei and are moving much faster. So it can be safely assumed that the
nucleus is fixed with respect to electrons and the total wavefunction is factorized as:
(Ri, r) = (Ri) (r;Ri) 3.3.2
where (Ri) describe the nuclei, and (r; Ri) depends parametrically on Ri and describes
electrons. The problem can be reformulated in terms of two separate Schrdinger
equations:
Hel(r;Ri) = U(Ri) (r;Ri) 3.3.3
Hi(Ri) = E (Ri) 3.3.4
Where
+
+=i ii
2i
2
ij ji
ji2
elrR
eZ
rr
e
2
1
RR
ZZ
2
1
m2
pH 3.3.5
and
)U(R2M
PH i
i i
ii += 3.3.6
the equation 3.3.3 for the electronic problem gives eigenvalue of the energy U(Ri) that
depends parametrically on the coordinates of the nuclei, Ri. After determining U(Ri) we
put it in equation 3.3.4, which describe the motion of nuclei. Equation 3.3.4 does notinclude any electronic degrees of freedom, all electronic effects are incorporated in U(Ri)
that is called interatomic potential.
Schrdinger equation is replaced with Newtonian equation in classical MD simulation.
This replacement is justified for most of the cases except for lightest atoms.
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3.4 Characteristics of potential
If we look into the literature will find different kinds of potential available for simulation
of different materials. Many things govern our choice of potential. Firstly, what type of
materials we are going to simulate? Second, what will be the size of our simulation
domain? Thirdly, what type of accuracy we want for our simulation. Fourthly, what types
of computational resources are available for simulation? Finally, up to what time we have
to simulate the problem (in molecular dynamics simulations). Typical time of these
problems vary form hundreds of femto-second (1x10-15 second) to few microsecond.
Potentials can be appropriate or inappropriate for a given problem. Following
characteristics should be considered while selecting a potential.
1.Accuracy potential is able to reproduce properties of interest as closely as possible.
High accuracy is typically required in Computational Chemistry. Computational domain
is typically very small in this case.
2. Transferability potential can be used to study a variety of properties for which it
was not fit. It is the most important characteristic of potential for empirical potential.
Empirical potential is fit using one set of parameters obtained from different experiments.
Transferability requires that the same potential must be able to reproduce other set of
parameters, which were not used to fit the potential.
3. Computational speed - calculations are fast with simple potentials. Most of empirical
potentials have simple form hence they are used extensively in different types of
problems. Computational speed is often critical in Materials Science where processes
have a collective character and big systems should be simulated for long times.
3.5 Pair potentials vs. many-body potentials
The total energy of a system of N atoms with interaction described by an empirical
potential can be expanded in a many-body expansion:
+++= > >> i ij jk
kji2i
jij
i2i
i1N21 )r,r,r(U)r,r(U)r(U)r,,r,rU( 3.5.1
where,1. U1 one-body term, due to an external field or boundary conditions (wall of a
container).
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2. U2 two-body term, or pair potential. The interaction of any pair of atoms
depends only on their spacing and is not effected by the presence of other atoms.
3. U3 three-body term arises when the interaction of a pair of atoms is modified by
the presence of a third atom.
Based on this expansion, we can loosely separate potentials into two classes:
1. Pair potentials (only U2 is present) and
2. Many-body potentials (U3 and higher terms are included).
In most of materials interaction of two atoms is affected by the presence of its neighbors.
In many body potentials we accounted the presence of its neighbors in the calculations
while in case of two body potentials we treat the interaction between the two atoms or
ions independently. Pair potentials are used for simulation of ionic solids and ideal gas.
Pair potential are computationally less expensive hence it is also used for other materialslike metals for simulating the general class effect with reasonable accuracy. MBP are
computationally more expensive but describes the materials like metals more elaborately.
We will also consider examples of many-potentials in which multi-body effects are
included implicitly, through an environment dependence of two-body terms
3.6 Short review of potentials used in MD and MC
Pair Potentials (hard spheres, Lennard-Jones, Morse) can be used :1. for inert gases, intermolecular van der Waals interaction in organic materials;
2. for investigation of general classes of effects (material non-specific).
The total potential energy of the system of N atoms interacting via pair potential is:
ijiji ij
ij2N21 rrrwhere)r(U)r,,r,rU(
== >
3.6.1
Commonly used examples of pair potentials:3.6.1 Hard/soft spheres potential It is the simplest potential without any
cohesive interaction i.e. there is no attractive force present. A very strong repulsive forceact when the spacing between the two atoms reaches below certain cutoff distance. It is
useful in theoretical investigations of some idealized problems. But it is difficult to
handle singularity in simulation. So we use a soft sphere model in which the
transformation of potential is gradual. Still it is not a realistic model for real materials.
We have very limited use of these potentials for real problems.
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potentialspherehardrrfor0
rrfor)U(r
0ij
0ij
ij
>
= 3.6.2
potentialspheresoft-r
r)U(r
n
0
ijij
= 3.6.3
3.6.2 Ionic potential In ionic solids the main source of cohesion is Coulomb
interaction of charges attraction.
ij
ji
ijr
qq)U(r = 3.6.4
These are very strong forces and have long range of influence i.e. the force dies out very
slowly. As we will see later that we can not use simply a cutoff radius and determine the
sum of total energy of forces as in case of other potentials. We have to give some specialtreatment to obtain the summation of the potential. Ions like O-- have a tendency to
polarize and form dipoles in presence of electric field. These dipoles also play an
important role in cohesive energy of the system. So the columbic potential is often added
to other functional forms to account polarization.
3.6.3 Lennard-Jones potential From computational point of view this potential
is very efficient. It describes the van der Waals interaction in inert gases and molecular
systems very accurately. Lennard-Jones potential can also be used to study the solid and
liquids. It is often used to model general effects (drop collision with surface, study of the
behavior of crack in fracture mechanics problems etc.) with very large system rather than
properties of a specific material.
=
6
ij
12
ij
ijrr
4)U(r
3.6.5
3.6.4 Morse potential It is similar to Lennard-Jones but is a more bonding-typepotential and is more suitable for cases when attractive interaction comes from the
formation of a chemical bond. This potential can be used for materials, which we
encounter in daily life like metals. It is proposed by P. M. Morse, Phys. Rev. 34, 57,
1930. It was a popular potential for simulation of metals that have fcc and hcp structures.
A fit for many metals is given by Girifalco and Weizer, Phys. Rev. 114, 687, 1959.
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=
)r-(r-e2
)r-(r2-e)U(r 0ij0ijij
3.6.6
3.6.5 6-exp (Buckingham) potential exp term (Born-Mayer) provides a better
description of strong repulsion due to the overlap of the closed shell electron clouds,
which is important in simulation of bombardment by energetic atoms or ions, etc.
6ij
BMijij rB
Rr-eA)U(r = 3.6.7
repulsion. Most of the potentials like Columbic potential and EAM potential (which
is a many body potential) use exp potential to describe the strong repulsive
3.7 Lennard Jones potential
3.7.1 IntroductionThe expression for Lennard Jones potential can be given by the following equation.
=
6
ij
12
ij
ij rr4)U(r
3.7.1
where rij is the distance between the atoms under consideration and and are material
specific constants. Values of constants and are determined by fitting the potential
for particular material. The potential is plotted below which describes different zones of
the potential like dipole-dipole attraction, equilibrium and Pauli repulsion. X-axis showsthe distance between the two atoms while y-axis represent the potential energy.
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distance between two atoms r
PotentialEnergy
4 6 8 10-0.02
-0.01
0
0.01
0.02
0.03
0.04
0.05
Pauli Repulsion
Equilibrium
Dipole-dipole attraction
Figure 1 plot of Lennard-Jones pair potential for Ar
When the spacing between the atoms is very large a week dipole-dipole attraction acts
between them. As the spacing between the atoms decreases the attractive force increases.
The term ~1/rij6, dominating at large distance, constitute the attractive part and describes
the cohesion to the system. A 1/r6 attraction describes van der Waals dispersion forces
(dipole-dipole interactions due to fluctuating dipoles). These are rather weak interactions,
which however are responsible for bonding in closed-shell systems, such as inert gases.
A strong repulsive force due to overlapping of close shell electrons counteracts the
attractive force before reach the equilibrium position. At equilibrium position resultant
force between the atoms is zero and potential energy is minimum at this position. If the
spacing between the atoms further decreases the repulsive force increases very rapidly.
The term ~1/rij12 represents the repulsion between atoms when they are brought close to
each other. Its physical origin is related to the Pauli principle: when the electronic cloudssurrounding the atoms starts to overlap, the energy of the system increases abruptly. The
exponent 12 was chosen on a practical basis: Lennard-Jones potential is particularly easy
to compute. In fact, on physical grounds an exponential behavior would be more
appropriate. Exponential term for repulsion (Born-Mayer potential) is typically used in
simulations where high-energy inter-atomic collisions are involved.
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3.7.2 Application of L-J potential:
1. The potential provides a good description of van der Waals interaction in inert gases
and molecular systems (Ar, Kr, CH4, O2, H2, C2H4, etc.). Parameters are given in [J.Chem. Phys. 104 8627 (1996)]. Parameters for inert gases can be also found in Ashcroft-
Mermin textbook. For example,
Ar ( = 0.0104 eV, = 3.40 )
Ne ( = 0.0031 eV, = 2.74 )
Kr ( = 0.0140 eV, = 3.65 )
Xe ( = 0.020 eV, = 3.98 ).
2. The main reason for popularity of Lennard-Jones potential is that it is used in
simulations when the objective is to model a general class of effects and the only
requirement is to have a physically reasonable potential.
Many studies on Lennard-Jones solids, liquids, surfaces, and clusters have been
performed. It is the potential of choice in studies when the focus is on fundamental
issues, rather than on properties of a specific material.
3.7.3 Derivation of the force for pair potential
In MD simulation we need forces that are acting on the atoms. The forces are given by
the gradient of the potential energy surface (the force on atom i is a vector pointing in the
direction of the steepest decent of the potential energy):
)r,,r,rU(rF N21ii
= 3.7.2
ir
operates on the position ri of atom i. Any change in the total potential energy that
results from a displacement of atom i contributes to the force acting on atom i.
For a pair potential:)r(U)r,,r,rU(
i ijij2N21
>
=
3.7.3
Where 222ij )()()(r jijijiji zzyyxxrr ++==
The force on atom i is:
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==ij
iji
N21ii)U(r
r)r,,r,rU(rF
3.7.4
ij
ij
ij i
ij
i
ij
i
ij
ijij iii dr
)dU(r
z
rz
y
ry
x
rx)U(r
zz
yy
xx
+
+
=
+
+
=
=
=
++=
ijij
ij
ij
ij ij
ji
ij
ij
ij ij
ij
ij
ij
ij
ij fdr
)dU(r
r
rr
dr
)dU(r
r
zz
r
yy
r
xx
3.7.5
for Lennard-Jones Potential:
=
612
4)(ijij
ijrr
rU
3.7.6
+= 7
612
6124
)(
ijijij
ij
rrdr
rd
=
6
8
6
21)(
24ijij ij
ji
irr
rrF
3.7.7
3.7.4 Potential cut-off
The potential functions like L-J have an infinite range of interaction i.e. whatever is the
value of r there is a corresponding value of potential. However as we increase value of rafter a certain value of r value of potential energy corresponding to this r is so small that
we can ignore the value for a practical problem. In practice a cutoff radius Rc is
established and interactions between atoms separated by more than Rc are ignored. There
are two reasons for this:
1. If we dont take a cutoff radius then the number of pair interactions grows as N 2.
Example: Consider system of 3000 atoms. If we dont tank a cutoff radius then the total
number of interactions (for force evaluation) in the simulation will be N2/2 = 45 lakhs.
While using a cutoff of 8-10 A we can reduce a number of interacting neighbors for each
atom to ~50 and we will have to evaluate force only ~50N = 150 thousand times for the
simulation. So with the introduction of a cutoff radius we can reduce the computational
requirement many times.
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2. The size of the system that can be simulated is finite. As we will see later with the help
of the finite size of the domain we evaluate the properties of the bulk materials using
periodic boundary conditions. And we will also see that these periodic boundary
conditions will require a cutoff radius.
But this introduction of cutoff radius also introduces some errors in the calculation as
explained below.
distance between two atoms r
PotentialEnergy
4 6 8 10-0.02
-0.01
0
0.01
0.02
0.03
0.04
0.05
Pauli Repulsion
Equilibrium
Dipole-dipole attraction
Jump in potential
Cutoff Radius
Figure 2 Plot of Lennard-Jones potential for Ar with the introduction of the cutoff radius
A simple truncation of the potential creates a jump in the potential at the cutoff distance.
This can spoil the energy conservation (i.e. energy of the system will not be remain
constant) or lead to unphysical behavior in simulations of the effects where contribution
of far-away molecules is important (surface tension, stacking faults, etc.). To avoid this
potential can be shifted to get potential energy zero at cutoff distance.
>
=cij
cijcij
ij RrRrRUrUrU
0)()()( 3.7.8
In the sifted potential value of potential at cutoff radius is subtracted from the potential
when the distance rij is less than or equal to cutoff radius andits value is zero when the
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distance rij is greater than cutoff radius. This arrangement smooth out the problem of
variation of energy.
distance between two atoms r
PotentialEnergy
4 6 8 10-0.02
-0.01
0
0.01
0.02
0.03
0.04
0.05
original potential
shifted potential
Pauli Repulsion
Equilibrium
Dipole-dipole attraction
Shiftd potential
origional potential
But for shifted potentials forces, which are derivative of potential energy, can have a
jump at the cutoff. To avoid this, a smooth transition function that brings potential to zero
can be added.
+
=
1973.8,1504,Phys.Rev.AJ.FordandstoddardS.D.byfunctionoff-cut
6122612612
47364)(ccc
ij
ccijij
ijRRR
r
RRrrrU
3.7.9
with cutoff function
0)( =cRU and 0)(
==
cijij
ij
Rrdr
rdU 3.7.10
In any case, physical quantities (cohesive energy, total pressure etc.) are affected by the
truncation and most modern potentials for real materials are designed with a cutoff radius
in mind, and go to zero at Rc together with several first derivatives of the potential
function.
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3.7.5 Limitations of pair potentials
1. Presence of other atoms affects the strength of bond between two atoms. It is called
many body effects and also known as environment dependence of bonds. Many body
effects are important in real materials. Pair potentials do not have environmental
dependence (e.g. atom in the bulk is too similar to the atom on the surface or near a
defect site). In reality, the strength of the individual bonds should decrease as the local
environment becomes too crowded due to the Paulis principle, but pair potentials do not
depend on the environment and cannot account for this decrease. Thus modeling of real
materials cannot be done accurately using only pair potentials.
2. Most of the ceramic materials have covalent bond. In covalent bonds the two or more
atoms share the valence electrons to complete their outer shell. And this sharing in turn
give rise to the directional nature of the bond i.e. the bond angle between the atoms
remains constant. Pair potentials do not account for directional nature of the bond. In
the same fashion covalent contributions (d orbitals) of the transition metals cannot be
described using pair potential. Pair potentials work better for metals in which cohesionis
provided bys andp electrons.
3. Energy required to remove an atom from its equilibrium position and thus form a
vacancy is called vacancy formation energy. The vacancy formation energy, Ev, is
significantly overestimated by pair potentials. Pair potential gives the estimation of Ev
equal to the cohesive energy per atom in the system Ec. In reality vacancy formation
energy is less then the cohesive energy per atom as in case of Cu Ev = 0.33 Ec and for Au
Ev = 0.25 Ec.
4. The ratio between the cohesive energy and the melting temperature, Tm, is
underestimated by as much as 2-3 times. Metals have some extra cohesion that is less
effective than pair potential in keeping the system in the crystalline state.
5. For cubic crystals (bcc, fcc) there exist a relation between the elastic constants (C12 =
C44), which is known as Cauchy relation. Ionic materials follow Cauchy relation, but
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metals show significant deviation from the Cauchy relation. Pair potentials do not
describe the deviations from the Cauchy relation for elastic constants in cubic crystals in
case of metals. (C12 = C44 or G = 3/5 B)
3.7.6 Relationship between pair potential and elastic constants
The bonding energy density of the system of N atoms interacting via pair potential is:
=ij
ij
a
b )U(r2N
1E 3.7.11
where a is the average volume per atom.
In equilibrium, when the force acting on any particle is zero, the structure must be stable
with respect to the application of a small homogeneous strain tensor . Then the
displacement vector for each interatomic distance, rij is uij = aij
where aij is
undeformed value of rij (uij = rij - aij). The elastic energy is expanded into a Taylor series
with respect to small displacements:
+
+
+=
ij
ij
ij
ij
ij
ij
ij
ij
ij
ij
a
b uurr
)U(ru
r
)U(r)U(r
NE
0
2
0
0 2
1
2
1 3.7.12
where the evaluation is at the undeformed values of rij and summation is implied byrepeated indices. Using uij
= aij we can rewrite this equation as
+++= CAEE bb2
1)0()( 3.7.13
where
=
ij
ij
ij
ij
a r
rU
NA
a
)(
2
1
0
3.7.14
is tensor of internal stress. First invariant of this tensor (Axx + Ayy + Azz) is the pressure.
In equilibrium A = 0, and
=
ij
ijij
ijij
ij
a rr
rU
NC
aa
)(
2
1
0
2
3.7.15
for pair potential
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ij
ij
ij
ij
ij
ij
dr
rdU
r
r
r
rU )()(
=
3.7.16
ij
ij
ijij
ij
ijij
ij
ij
ijij
ijij
ij
rd
rdU
rrd
rdU
rrd
rUd
r
rr
rr
rU )(1)(1)()(2
2
2
2
+
=
3.7.17
+
=
ij ij
ij
ijij
ij
ijij
ij
ija rd
rdU
rrd
rdU
rrd
rUd
rNC
ijijijijijij2
2
2aa
)(1aaaa
)(1)(1
2
1 3.7.18
C is symmetric with respect to all changes of indices and using Voigt notation (C11 =
C1111, C12 = C1122, C44 = C2323, C66 = C1212 etc.) we have Cauchy relation C12/C44=1
satisfied.
The Cauchy relation is often satisfied for van der Waals solids and ionic crystals. It is
never valid for metals (e.g. C12/C44 is 1.5 for Cu, 1.9 for Ag, 3.7 for Au). This means thatfor van der Waals and ionic solids the total energy may be reasonably well described by
the pair potential approximation. But for metals pair interaction may be used to represent
only part of the total energy.
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3.8 Embedded-atom and related methods for metallic systems
As we discussed above, pair potentials cannot provide an adequate description of metallic
systems. An alternative simple but rather realistic approach to the description of bondingin metallic systems is based on the concept of local densitythat is considered as the key
variable. This allows one to account for the dependence of the strength of individual
bonds on the local environment, which is especially important for simulation of surfaces
and defects. In metals the main source of cohesion is free electrons.
Many methods that have been proposed since early 1980s have different names (e.g.
embedded-atom method - EAM, effective medium theory, Finnis-Sinclair potential, the
glue model, corrected effective medium potential - CEM, etc.) and are based on different
physical arguments (e.g. tight-binding model, effective-medium theory), but result in a
similar expression for the total energy of the system of N atoms:
=+==ij
ijji
ij
ijijiii
i
itot rfrFEEE )()(2
1)( 3.8.1
Interpretation and functional form ofF,f, and depend on a particular method. From the
point of view of effective medium theory or the embedded-atom method, the energy of
the atom i is determined by the local electron density at the position of the atom and the
functionfdescribes the contribution to the electronic density at the site of the atom i from
all atomsj. The sum over function fis therefore a measure oflocal electron density i.
The embedding energyFis the energy associated with placing an atom in the electron
environment described by . The pair-potential term describes two-body contribution.
The general form of the potential can be considered as a generalization of the basic idea
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of the Density Functional Theory the local electron density can be used to calculate the
energy.
In addition to having different physical interpretations, the different methods differ in the
way function are determined. Some authors derive functions and parameters from first
principles calculations, others guess the functions and fit parameters to experimental
data Results are usually rather similar.
The main advantage of these methods over pair potentials is the ability to describe the
variation of the bond strength with coordination. Increase of coordination decreases the
strength of each of the individual bonds and increases the bond length.
+
=
ij
ijij
i
ij
ijjii rrfFE )(2
1)(
3.8.2
In order to use this potential in MD simulation we need to find the forces:
ij
ji
ijij
rr
ij
ijrr
i
j
j
ijrr
j
i
i
ij
ijij
ij
jjiiii
ii
toti
i
r
rr
r
r
r
rfF
r
rfF
rFFr
Er
Er
F
)()()()()()(
)()()(
+
+
=
++===
=====
3.8.3
Only inter-particles distances rij are needed to calculate energy and forces the
calculation is nearly as simple and efficient as with pair potentials.
The EAM potential can be called an environment-dependent pair potential. The lack
of explicit 3-body terms makes it challenging to design potentials for metals where
covalent effects are important.
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Chapter 4: Molecular Dynamics Simulations
4.1 Introduction
Molecular dynamics simulation is a technique for computing the equilibrium and
transport properties of a classical many-body system. In this context, the word classical
means that the nuclear motion of the constituent particles obeys the law of classical
mechanics. This is an excellent approximation for a wide range of materials. Molecular
dynamics simulations are in many respects very similar to real experiments. When we
perform a real experiment, we proceeded as follows. We prepare a sample of the material
that we wish to study. We connect this sample to a measuring instrument (e.g., a
thermometer, UTM, manometer), and we measure the property of interest during acertain time interval. If our measurements are subject to statistical noise then longer we
average the more accurate is our measurement becomes. In a Molecular Dynamics
simulation, we follow exactly the same approach. First, we prepare a sample: we select a
model system consisting of N particles and we solve Newtons equation of motion for
this system until the properties of the system no longer change with time. After
equilibration, we perform actual measurement. In fact, some of the most common
mistake that can be made when performing a computer experiment are very similar to the
mistakes that can be made in real experiments.(e.g. the sample is not prepared correctly,
the measurement is too short, or we do not measure what we think.)
4.2 Molecular Dynamics: A program
The best introduction to Molecular Dynamics simulations is to consider a simple
program. The program we consider is kept as simple as possible to illustrate a number of
important features of Molecular Dynamics simulations.
The program constructed as follows:
1. We read in the parameters that specify the condition of the run (e.g. initial
temperature, number of particle, density, time step).
2. We initialize the system (i.e. we select the initial positions and velocities).
3. We compute the forces on all particles.
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4. We integrate Newtons equations of motion. This step and the previous one make
up the core of the simulation. They are repeated until we have computed the time
evolution of the system for the desired length of time.
5. After completion of the central loop we compute and print the averages of the
measured quantities, and stop.
a flow chart for Molecular Dynamics algorithm isshown below:
no
Initialize coordinates,Temperature, velocity etc.
Compute force between the
Integrate the Newtonsequation of motion and find
new coordinate and velocities
System reached
Production runMeasurement of properties
progr am md simple MD program
cal l i ni t initializationt = 0do whi l e ( t . l t . t max) MD loop
cal l f orce( f , en) determine forcescal l i nt egr at e( f , en) integrate equation of motion
t = t + del tcal l sampl e sample averageend dostopend
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4.2.1 Initialization
To start the simulation, one must assign positions and velocities to all the particles in thesystem. The particle position should be chosen compatible with the structure that we are
aiming to simulate. The particle should not be placed in positions that result in anappreciable overlap of the atomic or molecular cores. In the present case, we put eachparticle on its lattice site and then we assign each velocity component a value that isdrawn from random distribution in the interval [-0.5, 0.5]. Subsequently, the velocitiesare shifted such that the total momentum is zero and the velocities are scaled to adjust themean kinetic energy to the desired value. In thermal equilibrium, the following relationshould hold:
,/2 mTkv B= 4.2.1
where vis the component of the velocity of a given particle. We can use this relation
to define an instantaneous temperature at time t, T(t):
=
N
i f
i
BN
tmvtTk
1
2, )()( 4.2.2
Algorithm for initialization of a Molecular Dynamics program
Subr out i ne i ni t Initialization of MD programsumv = 0sumv2 = 0do i = 1, npart
x( i ) = l at t i ce_pos( i ) place the particles on a latticev( i ) = ( r anf ( ) - 0. 5) give random velocitiessumv = sumv + v( i ) velocity of center of masssumv2= sumv2 + v( i ) **2 kinetic energy
enddosumv = sumv/ npar t velocity of center of mass
sumv2 = sumv2/ npar t mean square velocitiesf s = sqr t ( 3 * t emp/ sumv2) scale factor of velocitiesdo i = 1, npart set desired kinetic energy and set
v( i ) = ( v( i ) - sumv) * f s velocity of center of mass to zeroxm( i ) = x( i ) v( i ) * dt position at previous time step
enddoreturnstop
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The instantaneous temperature T(t) can be adjusted to match the desired temperature Tby
scaling all velocities with a factor (T/T(t))1/2. This initial setting of temperature is not
particularly critical, as the temperature will change during equilibration. The approximate
previous position can be obtained by the use of initial velocities byxm(i)= x(i) . v(i) . dt,
wherex is present position v is initial velocity and dtis time step for Molecular Dynamics
simulation.
4.2.2 Force Calculation
The calculation of forces on every particle is the most time consuming part of Molecular
Dynamics simulation. If we consider a model system with pair wise additive interactions
we have to consider the contribution to the force on particle i due to all its neighbors. If
we consider only interaction between a particle and the nearest image of another particle,
this implies that, for a system ofN particles, we must evaluate N (N -1)/2 pair
distances.
Algorithm for calculation of force
subr out i ne f or ce ( f , en) determine the forceen = 0 and energydo i = 1, npart
f ( i ) = 0 set force to zero
end dodo i = 1, npar t 1 loop over all pairdo j = i + 1, npart
xr = x( i ) x( j )xr = xr box*ni nt ( xr / box) periodic boundary conditionr 2 = xr **2i f ( r 2. l t . r c2) t hen test cutoff
r 2i = 1/ r 2r 6i = r 2i **3f f = 48*r2i *r6i *( r 6i - 0. 5) Lennard-Jones potentialf ( i )= f ( i ) + f f * xr update forces
f ( j ) = f ( j ) - f f * xren = en+4*r 6i *( r 6i - 1) - ecut update energy
endi fenddo
enddoreturn
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This implies that, if we use no tricks, the time needed for the evaluation of the forces
scales as N2. There exist different techniques to speed up the evaluation of both short
range and long-range forces in such a way that computing time scales as N, rather than
N2.
4.2.3Integrating the Equations of Motion
After computing all forces between the particles, we integrate Newtons equations of
motion. Algorithms have been designed to do this. Verlet algorithm is not only one the
simplest, but also usually the best.
The Taylor series expansion of the coordinate of the particle, around time t,
),(!32
)()()()( 43
2 tOrttmtfttvtrttr ++++=+ 4.2.3
similarly,
).(!32
)()()()( 4
32 tOr
tt
m
tfttvtrttr +
+= 4.2.4
Summing the two equations, we obtain
)(2
)()(2)()( 42 tOt
m
tftrttrttr ++=++
or2
2
)()()(2)( t
m
tfttrtrttr ++ 4.2.5
The estimate of the new position contains an error that is of the ordert4, where tis the
time step of our Molecular Dynamics scheme. Verlet algorithm does not use the velocity
Algorithm for integrating the equation of motionsubr out i ne i nt egr at e( f , en) integrate equation of motionsumv = 0
sumv2 = 0do i = 1, npar t MD loop
xx = 2 * x( i ) xm( i ) + del t **2 * f ( i ) Verlet algorithmvi = ( xx - xm( i ) ) / ( 2*del t ) velocitysumv = sumv + vi velocity of center of masssumv2 = sumv2 + vi **2 total kinetic energyxm( i ) = x( i ) update positions previous time stepx( i ) = xx update positions current time
end dot emp = sumv2/ ( 3*npar t ) instantaneous temperature
et ot = ( en + 0. 5*sumv2) / npar t total energy per particlereturnend
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to compute new position. The velocity can be derived from the knowledge of the
trajectory, using
)()(2)()( 3tOttvttrttr +=+
or
)(2
)()()( 2tO
t
ttrttrtv +
+
= 4.2.6
It is possible to cast Verlet algorithm in a form that uses positions and velocities
computed at equal times. This velocity Verlet algorithm looks like a Taylor series
expansion for the coordinates:
.2
)()()()( 2t
m
tfttvtrttr ++=+ 4.2.7
where the update of the velocities is given by
.2
)()()()( t
m
tfttftvttv
+++=+ 4.2.8
Note that, in this algorithm, we can compute the new velocities only after we have
computed the new positions and, from these the new forces. Now that we have computed
the new positions, we discard the positions at time (t - t). The current positions become
the old positions and the new positions become the current positions. After each time step
we compute the current temperature, the current potential energy and the total energy.
The total energy should be conserved. This completes the introduction to Molecular
Dynamics method.
4.5 Boundary Conditions
The length-scale of MD is limited a large fraction of atoms is therefore on the surface
or near the surface. This is not the case with most of the physical systems. How to
reproduce interaction of atoms in the MD computational cell with the surrounding
materials?
4.5.1 Free boundaries (or no boundaries):
this works for a molecule, a cluster or aerosol particle in vacuum. Free boundary can also
be appropriate for ultra-fast processes when the effect of boundary is not important due to
the short time scale of the involved processes, e.g. fast ion/atom bombardment, etc.
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Figure 3Free boundary condtion
4.5.2 Rigid Boundaries (atoms at the boundaries are fixed). In most
cases the rigid boundaries are unphysical and introduce artifacts into the simulation
results. Sometimes used in combination with other boundary conditions.
Figure 4 Rigid boundary condition
4.5.3. Periodic Boundary condition (eliminates surfaces the most popular
choice of boundary conditions) this boundary conditions are used to simulate processes
in a small part of a large system. all atoms in the computational cell (dark box) are
replicated throughout the space to form an infinite lattice. That is, if atoms in the
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computational cell have positions ri, the periodic boundary condition also produces
mirror images of the atoms at the positions defined as
Figure 5 Periodic boundary condition
cnbmalrr iimage
i
+++= , where a, b, c are vectors that correspond to the edges of the
box, l, m, n are any integers from - to +.
Each particle in the computational cell is interacting not only with other particles in the
computational box, but also with their images in the adjacent boxes. The choice of the
position of the original box (computational cell) has no effect on forces or behavior of the
systems.
Limitations of periodic boundary condition:
The size of the computational cell should be larger than 2Rcut, where Rcut is the cutoff
distance of the integration potential. In this case any atom i interact with only one image
of any atom j. it does not interact with its own image. This condition is called minimum
image criterion
The characteristic size of any structural feature in the system of interest or the
characteristic length-scale of any important effect should be smaller than the size of thecomputational cell. For example, low frequency parts of the phonon spectrum can be
affected, stress fields of the different images of the same dislocation can interact etc. to
check if there are any artifacts due to the size of the computational cell perform
simulation with different sizes and check if the result converge.
Calculation of distances between atoms with periodic boundary conditions:
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When the minimum image criterion is satisfied, a particle can interact only with the
closest image of any other particle.
Figure 6 Minimum image criteria
The closest image may or may not belong to the computational cell. Therefore, in the
code, if a particle j is beyond the range of interaction with particle i (Rij > Rcut), we have
to check the closest images. For example, an algorithm for checking the closest image is:
do i = 1, N ! loop over total number of atomsdo j = 1, nei ghbor ! loop up to number of neighbors
xr = x( i ) x( j )i f ( xr . gt . hbox) t hen ! half of the length of box = hbox
xr = xr box ! length of box = boxel sei f ( xr . l t . hbox) t hen
xr = xr + box
endi f. ! Other calculations.
end doend do
4.3 An Illustration
In this section we will look into the approach for a typical atomistic calculation problem.
Suppose we want to find out total energy and resultant force on an atom in a system of
Argon atoms having some initial positions with potential function for the Argon is given.
To simplify the problem let us consider a two-dimensional problem by assuming
that atoms can move only in x and y direction only.
Also we assume free boundary for the sake of simplicity.
We will use no cutoff radius in the calculation i.e. all atom will interact with all
other atoms.
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Let us assume that atoms are nicely sitting on the corners of a grid having equal spacing
in x and y direction. The potential energy of atom due to atom j can be obtained using the
following equation. (Eq. 3.7.1)
=
6
ij
12
ij
ij rr4)U(r
Figure 7 Arrangement of atoms in 2-D planefrom the above equation it is clear that if we have values of rij can determine the potential
energy of atom 1 due to j. we can obtain the total potential energy of atom 1 by taking
summation of all the U(r1j) over j. similarly we can determine the force due to atom j on
atom using the equation below
=
6
8
6
21)(
24ijij
ji
ijrr
rrF
the resultant force is the summation of the individual forces due all neighboring atoms.
parameters for potential of Argon are = 0.0104 eV, = 3.40
Suppose we want to evaluate total energy and total force on atom 1. First we have to find
the distance jr1 to determine potential energy as well as force due to atom j . The values
are tabulated as follows
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Atom no 1
interacts withR1j U(rij)
F(rij)in x-
direction
F(rij)in y-
direction
2 2.0 23.23 0.0 -142.4
3 4.0 -0.9722e-2 0.0 0.5782e-2
4 6.0 -0.1332e-2 0.0 0.1286e-2
5 2.0 23.23 -142.4 0.0
6 2.282 0.2523 -0.9478 -0.9478
7 4.472 -0.6482e-2 0.2958e-2 0.5917e-2
8 6.325 -0.9799e-3 0.2867e-3 0.8601e-3
9 4.000 -0.9772e-2 0.5782e-2 0.0
10 4.472 -0.6482e-2 0.5917e-2 0.2958e-2
11 5.657 -0.1869e-2 0.1332e-2 0.1332e-2
12 7.211 -0.4520e-3 0.2063e-3 0.3095e-3
13 6.000 -0.1332e-2 0.1286e-2 0.0
14 6.325 -0.9799e-3 0.8601e-3 0.2867e-3
15 7.211 -0.4520e-3 0.3095e-3 0.2063e-3
16 8.485 -0.1715e-3 0.8537e-4 0.8537e-4
total 46.679 -143.339 -143.339
It is clear from the table that total potential energy is positive and resultant force is not
zero, which shows that atom 1 is not at equilibrium position and the rest of the atoms
repels it collectively. It is also evident that the atoms beyond 4 A are pulling the atom 1
towards them i.e. an attraction force is acting between them. Also notice that energy due
to these atoms is negative. Atoms situated at less than or equal to 4 A are trying to push
away atom 1 i.e. repulsive force is acting and also notice that energy due to these atoms is
positive.
4.4 Ensembles
Ensemble is a set of all states, which a system can acquire with keeping some
macroscopic parameter constants. For example in constant energy and constant volume
ensemble (NVE) is a set of all states, which the system can acquire with keeping the
volume and total energy (KE + PE) constant. A typical MD simulation with periodic
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boundary condition is constant energy and constant volume ensemble (NVE), which is
also known as micro-canonical ensemble. Consider a many-body system with energy E
that is capable of occupying every quantum state. If we take an average of some property
of the system over all possible quantum states of is called an ensemble average of the
property. However, this is not the way one think about the average behavior of a system.
In most experiments we perform a series of measurements during a certain period of time
and then determine the average of these measurements. The idea behind Molecular
Dynamics is precisely that we can study the average behavior of the many-body particle
system simply by computing the natural time evolution of that system numerically and
averaging the quantity of interest over a sufficiently long period of time.
4.5 Computer ExperimentsAfter formulating and implementing the Molecular Dynamics program, we wish to use it
to measure the interesting properties of many body systems. These quantities can be
compared with the real experiments. Simplest among these are the thermodynamic
properties of the system under consideration, such as the temperature T, the pressureP,
and the heat capacity Cv. As mentioned earlier, the temperature is measured by
computing the average kinetic energy per degree of freedom. For a system offdegrees of
freedom, the temperature T is given by
f
KTkB
2= 4.5.1
whereKis kinetic energy.
There are several ways to measure the pressure of a classical N-body system. The most
common among these is based on the virial equation for pressure. For pair-wise
interactions, we can write
,).rf(r1
ijij