1 dishing out the dirt on reaxff force field subgroup meeting 29/9/2003
TRANSCRIPT
2
Contents
- ReaxFF: general principles and potential functions
-All-carbon compounds: Training set
- Sample simulation: Ethylene+O2 reactive NVE
3
ReaxFF: general principles and potential functions
Tim
e
DistanceÅngstrom Kilometres
10-15
years
QC
ab initio,DFT,HF
ElectronsBond formation
MD
Empiricalforce fields
AtomsMolecular
conformations
MESO
FEA
Design
Grains
Grids
Hierarchy of computational chemical methods
ReaxFF Simulate bond formationin larger molecular systems
Empirical methods:- Allow large systems- Rigid connectivity
QC methods:- Allow reactions- Expensive, only small systems
4
Current status of ReaxFF program and force fields
Program:
- 18,000 lines of fortran-77 code; currently being integrated into CMDF- MD-engine (NVT/NVE/limited NPT), MM-engine- Force field optimization methods: single parameter search, anneal- Can handle periodic and non-periodic systems- User manual (under development) available online
Force fields
Published: hydrocarbons, nitramines, Si/SiO/SiH, Al/AlOAdvanced: proteins/CH/CN/CO/NO/NN/NH/OH/OO, MoOx, all-carbon, Mg/MgHIn development: SiN/SiC, Pt/PtO/PtN/PtC/PtCo/PtCl, Ni/NiAl/NiC, Co/CoC, Cu/CuC, Zr/ZrO, Y/YO, Ba/BaO, Y-BaZrOH, BH/BB/BN/BC, Fe/FeO
Method seems universally available; has been tested now for covalent, ceramic, metallic and ionic materials.
5
MM or MD routine
Connection table
1: 2 3 42: 1 5 63: 14: 15: 26: 2
Non-reactive force field
Atom positions
1: x1 y1 z1
2: x2 y2 z2
3: x3 y3 z3
4: x4 y4 z4
5: x5 y5 z5
6: x6 y6 z6
Fix
ed
MM or MD routine
Determineconnections
Reactive force field
Atom positions
1: x1 y1 z1
2: x2 y2 z2
3: x3 y3 z3
4: x4 y4 z4
5: x5 y5 z5
6: x6 y6 z6
Program structureB
ond
orde
r
Interatomic distance (Angstrom)
)( ijij rfBO =
1 2
3
4
5
6
6
ReaxFF: General rules
- MD-force field; no discontinuities in energy or forces
- User should not have to pre-define reactive sites or reactionpathways; potential functions should be able to automatically handlecoordination changes associated with reactions
- Each element is represented by only 1 atom type in force field;force field should be able to determine equilibrium bond lengths,valence angles etc. from chemical environment
7
underover
torsvalCoulombvdWaalsbondsystem
EE
EEEEEE
++
++++=
conjpen EE ++ ReaxFFCH
ReaxFFSiO: System energy description
2-body
multibody
3-body 4-body
8
Sigma bond
Pi bond
Double pi bond
Bond energy 1. Calculation of bond orders from interatomic distances
0
1
2
3
1 1.5 2 2.5 3
Interatomic distance (Å)
Bond order
Bond order (uncorrected)
Sigma bond
Pi bond
Double pi bond
9
Bond energy 2. Bond order correction for 1-3 bond orders
H
HH
HH
H
0.950.
97
0.97
0.97
0.97
0.97
0.97
0.10
0.10 0.10
0.10
0.10
0.10
BOC=4.16
BOH=1.17
Uncorrected bond orders
0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1
0 0.2 0.4 0.6 0.8 1
3.5
3.7
4.1
4.5
5
6
BO
Uncorrected bond order
Cor
rect
ed b
ond
orde
r
- Unphysical- Puts strain on angle and overcoordination potentials
BOC=3.88
BOH=0.98
H
HH
HH
H
0.94
0.97
0.97
0.97
0.97
0.97
0.97
0.01
0.01 0.01
0.01
0.01
0.01
Corrected bond orders
- Correction removes unrealistic weak bonds but leaves strong bonds intact- Increases computational expense as bond orders become multibody interactions
10
Bond energy 3. Calculate bond energy from corrected bond orders
€
Ebond = −Deσ ⋅BOij
σ ⋅exp pbe,1 1− BOijσ
( )pbe,2
( ){ }
− Deπ ⋅BOij
π − Deππ ⋅BOij
ππ
0
1
2
3
1 1.5 2 2.5 3
Interatomic distance (Å)
Bond order
Bond order (uncorrected)
Sigma bond
Pi bond
Double pi bond
-500
-400
-300
-200
-100
0
100
1 1.5 2 2.5 3
Interatomic distance (Å)
Bond energy (kcal/mol)
Sigma energy
Pi energy
Double pi energy
Total bond energy
11
Nonbonded interactions
- Nonbonded interactions are calculated between every atom pair, including bonded atoms; this avoids having to switch off interactions due to changes in connectivity- To avoid excessive repulsive/attractive nonbonded interactions at short distances both Coulomb and van der Waals interactions are shielded
( ){ } 3/133 /1 ijij
jiCoulomb
r
qqCE
γ+
⋅⋅=
Shielded Coulomb potential
0
250
500
750
1000
0 0.5 1 1.5 2 2.5 3
Unshielded Coulomb
Shielded Coulomb
Unshielded vdWaals
Shielded vdWaals
+0.5 +0.5
Interatomic distance (Å)
Ene
rgy
(kca
l/mol
)
vdWaals: Shielded Morse potential
12
Charge calculation method
- ReaxFF uses the EEM-method to calculate geometry-dependent, polarizable point charges
- 1 point charge for each atom, no separation between electron and nucleus
- Long-range Coulomb interactions are handled using a 7th-order polynomal (Taper function), fitted to reproduce continuous energy derivatives. Taper function converges to Ewald sum much faster than simple spline cutoff.
NaCl-crystal (33.84x33.84x33.84 Å)
-200000
-190000
-180000
-170000
-160000
0 5 10 15 20 25 30 35
Outer cutoff
Coulomb energy
Taper 7
Ewald (12.5 Å innerspace cutoff)Spline 3
13
Interatomic distance (Å)
Ene
rgy
(kca
l/mol
)- Summation of the nonbonded and the bonded interactions gives the two-body interactions- Bond energies overcome van der Waals-repulsions to form stable bonds
-500
-250
0
250
500
750
0 1 2 3
Bond energy
Shielded vdWaals energy
Total pair energy
Total two-body interaction
14
Valence angle energy1. General shape
i
j
k
ba
( )( )ππbaoijkbaval BOBOfBOfBOfE ,)()( Θ−Θ⋅⋅=General shape:
Ensures valenceangle energy contributiondisappears when bond a
or bond b dissociates
Modifies equilibriumangle o according
to π-bond order in bond a andbond b
15
0 0.5 1 1.5 2
Valence angle energy2. Bond order/valence angle energy
i
j
k
ba
( )( )ππbaoijkbaval BOBOfBOfBOfE ,)()( Θ−Θ⋅⋅=
( )21exp1)( λλ aa BOBOf ⋅−−=
Bond order bond a
Eval,max
Eva
l
0
16
Valence angle energy3. π-Bond order/equilibrium angle
i
j
k
ba
( )( )ππbaoijkbaval BOBOfBOfBOfE ,)()( Θ−Θ⋅⋅=
( )21exp1)( λλ aa BOBOf ⋅−−=
⎟⎟⎠
⎞⎜⎜⎝
⎛
⎭⎬⎫
⎩⎨⎧
⎟⎟⎠
⎞⎜⎜⎝
⎛−⋅−−⋅−= ∑
=
)(
13, 2exp1180),(
jneighbours
njnoobao BOBOBO πππ λ
∑=
)(
1
jneighbours
njnBOπ
Equ
ilibr
ium
ang
le(d
egre
es)
17
Torsion angle energy1. General shape
( ) ( ) ( )⎭⎬⎫
⎩⎨⎧ +⋅+⋅−⋅⋅⋅⋅= ijklbijklcbators VBOfVBOfBOfBOfE ωω π 3cos1
2
12cos1
2
1)()()( 32
General shape:
Ensures torsion angle energy contribution
disappears when bond a, b or cdissociates
(similar to valence angle)
i
j
k
bac
l
Controls V2-contributionas a function of the
π-bond order in bond b
18
Torsion angle energy2. π-bond order influence on V2-term
( ) ( ) ( )⎭⎬⎫
⎩⎨⎧ +⋅+⋅−⋅⋅⋅⋅= ijklbijklcbators VBOfVBOfBOfBOfE ωω π 3cos1
2
12cos1
2
1)()()( 32
i
j
k
bac
l
( ) ( )( )24 1exp ππ λ bb BOBOf −−=
0 0.25 0.5 0.75 1
πbBO
eff
V2
V2,max
0
19
Avoid unrealistically high amounts of bond orders on atoms
3 3.5 4 4.5A
tom
ene
rgy
BOi ji
nbonds
,
1
BO (C)=4i ji
nbonds
,
1BO (C)=3i j
i
nbonds
,
1BO (C)=5i j
i
nbonds
,
1
∑=
−=Δ
Δ⋅+⋅Δ⋅=
neighbours
jijii
iiijover
BOValency
BOfE
1
)exp(1
1)(
λ
Overcoordination energy
20
0.01
0.1
1
10
100
1000
10000
100000
1000000
0 100 200 300 400
ReaxFF
QM (DFT)
Nr. of atoms
Tim
e/ite
ratio
n (s
econ
ds)
Computational expense
x 1000,000
21
All-carbon compounds: training set
Strategy for parameterizing reactive force fields
- Pick an appropriate QC-method - Determine a set of cluster/crystal cases; perform QC- Fit ReaxFF-parameters to QC-data
Interatomic distance (Angstroms)
Bonds
Valence/Torsions
Nonbonded
Non-reactive force field
Interatomic distance (Angstroms)
Bonds
Valence/Torsions
Nonbonded
Overcoordination
ReaxFF
Complications
22
Binding energies in all-carbon compounds relative to Graphite
0
20
40
60
80
100
120
Acyclic C2Acyclic C3Cyclic C3Acyclic C4Cyclic C4C4 pyramidAcyclic C5Cyclic C5Acyclic C62_C3Cyclic C6Acyclic C7Cyclic C7Acyclic C8C8 3ringC8 3ringIIC8 cubeCyclic C8Acyclic C9Cyclic C9Acyclic C10Cyclic C10Tricyclic C10Acyclic C12Acyclic C13Cyclic C13Tricyclic C13Acyclic C14Cyclic C15Cyclic C17Bicyclic C17Acyclic C20Hexacyclic C20C20-dodecaC60-buckyballDiamond
Relative binding energy (kcal/atom)
Reax
QC
- Even-carbon acyclic compounds are more stable in the triplet state; odd-carbon, mono and polycyclic compounds are singlet states- Small acyclic rings have low symmetry ground states (both QC and ReaxFF)- ReaxFF reproduces the relative energies well for the larger (>C6) compounds; bigger deviations (but right trends) for smaller compounds- Also tested for the entire hydrocarbon training set (van Duin et al. JPC-A, 2001); ReaxFF can describe both hydro- and all-carbon compounds
23
0
50
100
1.5 2 2.5
DFTReaxFF
0
50
100
1.5 2 2.5
DFTReaxFF
C-C distance (Å)
Ene
rgy
(kca
l/m
ol)
Ene
rgy
(kca
l/m
ol)
Bond formation between two C20-dodecahedrons
- ReaxFF properly describes the coalescence reactions between C20-dodecahedrons
24
Angle bending in C9
- ReaxFF properly describes angle bending, all the way towards the cyclization limit
25
C6+C5 to C11 reaction
- ReaxFF properly predicts the dissociation energy but shows a significantly reduced reaction barrier compared to QC
26
3-ring formation in tricyclic C13
-ReaxFF describes the right overall behaviour but deviates for both the barrier height and the relative stabilities of the tetra- and tricyclic compounds
27
0
0.05
0.1
0.15
0.2
10 15 20
c-axis (Å)
ΔE (
eV/a
tom
)
diamond
graphite
Diamond to graphite conversionCalculated by expanding a 144 diamond supercell in the c-direction and relaxing
the a- and c axes
QC-data: barrier 0.165 eV/atom(LDA-DFT, Fahy et al., PRB 1986, Vol. 34, 1191)
-ReaxFF gives a good description of the diamond-to-graphite reaction path
28
Relative stabilities of graphite, diamond, buckyball and nanotubes
Compound ERef (kcal/atom) EReaxFF
Graphite 0.00a 0.00
Diamond 0.8a 0.52
Graphene 1.3a 1.56
10_10 nanotube 2.8b 2.83
17_0 nanotube 2.84b 2.83
12_8 nanotube 2.78b 2.81
16_2 nanotube 2.82b 2.82
C60-buckyball 11.5a 11.3
a: Experimental data; b: data generated using graphite force field (Guo et al. Nature 1991)
- ReaxFF gives a good description of the relative stabilities of these structures
29
Ongoing all-carbon projects
- Nanotube failure, buckyball collision (Claudio)
- Si-tip/nanotube interactions (Santiago)
- Nanotube growth, buckyball polymerization (Weiqiao)
- Buckyball/nanotube nucleation (Kevin)
- Buckyball/nanotube oscillator (Haibin)
- Diamond surface interactions (Sue Melnik)
30
Sample simulation: Ethylene+O2 reactive NVE
-12 Ethylene, 36 O2
- Pre-equilibrated at 4000K. Switched off C-O and H-O bonds during equilibration to avoid reactions
- Time-step: 0.025 fs.; cannot go much higher due to high temperature + reactive potential
- Should react; main expected products H2O, CO2 and CO
32MD-iteration
- Fast reaction after initiation
- Exothermic; temperature rises to 7000K
- Energy is not perfectly conserved at elevated temperatures.
- Future work: investigate potential; see if energy conservation can be improved.