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Molecular dynamic simulations of DMPC lipid bilayer along with ab initio calculations have been presented.
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Molecular Dynamic Simulations to
Probe Interactions of Buffer Molecules
with Lipid Bilayers
A PROJECT REPORT
SUBMITTED IN PARTIAL FULFILLMENT OF THE
REQUIREMENTS FOR THE DEGREE OF
MASTER OF ENGINEERING
BY
MOHAMMAD SIRAJUDDIN
DEPARTMENT OF CHEMICAL ENGINEERING,
INDIAN INSTITUTE SCIENCE, BANGALORE
JUNE-2015
i
Declaration
I verify that all chapters in the report were written by myself, and during the course of
writing the report:
i. Simulations results presented have been obtained by me without any bias,
modification and alteration. One can obtain the identical results using the
information provided in the report to draw similar conclusion.
ii. I have not copied or edited any form of content or chapter from published or
unpublished sources. However figures, theory or any other material which was
essential during report writing and was not derived, obtained or written by me
was given due credit by citing it in text of the report and details have been shared
in the reference section.
iii. Ethical issues have been taken into consideration while formatting and shaping
the report so as to accord with the departmental guidelines.
Mohammad Sirajuddin
ii
Acknowledgements
Research work presented in this report is the outcome of invaluable guidance, suggestions
and kind support of many adroit and elite peoples from my department. First and foremost
I express sincere and enormous gratitude to my advisor Prof. K Ganapathy Ayappa, whose
adept knowledge and dexterous advice enabled me to relish and explore the diverse aspects
of my project. His affable and cheerful personality attest instrumental during my project
course to outreach a trite milestone. I further extend my appreciation to astounding lab
members Ayush, Pradeep, Vadhana, Rajshekhran, Subbarao and Rajat for pleasant and
informal conversation during numerous lunches and meetings. My special thanks to Rajat
for his continuous assessment and umpteen support during my project in the form of
discussion, chats and constructive critics which sculpted my project to its final shape in
due time.
I am grateful to all the faculty members from my department for their enlightenment and
professionalism during entire program. Many thanks to my class mates for their
cooperation and amity which moulded the meticulous and burdensome Master’s program
into adorable and zealous environment. Extra special thanks to my camaraderie
Satyaghosh, Shubhashish and Jitendra for nurturing and weaving golden memories during
my stay at IISc. Jitendra’s companionship from my very first question “where is chemical
engineering department?” till leaving department has imprinted unexplainable memories.
Innocence of Satyaghosh with crazy Subhashish’s quest for haunting new restaurants on
iii
every weekend added blend of flavours and textures to my M.E. tenure. I owe my every
achievements to you nutty guys!
I’d like to convey my heartfelt thanks to all colleagues in the department for wonderful
trips and peaceful stay. My acknowledgement to AICTE for scholarship during M.E.
program, adequate to pay off my bills and hunger. Finally, I express intense gratitude
towards the hallowed portals of IISc, which manifested sheer and obscure arena, buzzing
with soothing sound of birds and breezing through the shadows of green garment, entitled
my inner self to invoke “Yes… Heaven in here!”
To the end, I express deepest appreciation to all my near and dear who believed this naive
person with uttermost encouragement which propelled my research project to fruition.
iv
Abstract
Buffers are very widely used in biophysical and biochemical studies to maintain a desired
pH. The effect of buffers on the lipid bilayers is often ignored or assumed to be negligible,
since buffers which are generally hydrophilic are not expected to interact strongly with the
membranes. However recent literature has shown that buffers in presence of other salt
molecules can interact with lipid bilayers through van der Waals forces, electrostatic and
hydration forces and alter the bending rigidity of the bilayer membrane [4, 5].
In order to obtain a molecular understanding of these interactions and their influence on
membrane properties, we carried out a molecular dynamic simulation of Hydroxy ethyl
piperazine ethane sulfonic acid (HEPES) buffer on a 1,2-dimyristoyl-sn-glycero-3-
phosphocholine (DMPC) lipid bilayer. Initially we carried out ab-initio calculations at the
Hartree–Fock (HF) level of theory to construct an electrostatic potential map and derived
charges using the restrained electrostatic potential (RESP) fitting procedure. These charges
are used in classical force fields to carry out molecular dynamic simulations. The structural
properties like radial distribution function, density distribution are presented at different
buffer concentrations.
iii
Contents
Chapter 1 ........................................................................................................................... 1
Introduction ....................................................................................................................... 1
1.1 Cell ............................................................................................................................ 1
1.2 Cell Membrane.......................................................................................................... 2
1.3 Lipid Bilayer ............................................................................................................. 3
1.4 Role of buffers in cell membrane.............................................................................. 5
1.4 Problem definition .................................................................................................... 6
Chapter 2 ........................................................................................................................... 8
Molecular Dynamics ......................................................................................................... 8
2.1 Introduction ............................................................................................................... 8
2.2 Simulations … How it works? .................................................................................. 8
Chapter 3 ......................................................................................................................... 14
Molecular dynamics simulations of DMPC .................................................................. 14
3.1 Introduction ............................................................................................................. 14
3.2 Simulation methods and details .............................................................................. 16
3.3 Results and discussion ............................................................................................ 17
Chapter 4 ......................................................................................................................... 22
Ab-initio calculations and simulation of HEPES .......................................................... 22
4.1 Introduction ............................................................................................................. 22
4.1.1 HEPES ................................................................................................................. 23
4.1.2 Charge derivation for HEPES .............................................................................. 24
4.1.3 Molecular geometry optimization and partial charge .......................................... 29
4.2 Simulation of HEPES in water ............................................................................... 33
4.2.1 Analysis................................................................................................................ 34
Chapter 5 ......................................................................................................................... 37
Simulation of DMPC in presence of buffer molecules ................................................. 37
5.1 Introduction ............................................................................................................. 37
5.2 Simulation Method.................................................................................................. 37
5.3 Results and Discussion ........................................................................................... 38
5.3.1 Mass density......................................................................................................... 38
5.3.2 Hydrogen bonds ................................................................................................... 41
5.3.3. Area per lipid ...................................................................................................... 46
5.3.4 Radial distribution function ................................................................................. 48
Chapter 6 ......................................................................................................................... 50
Umbrella sampling .......................................................................................................... 50
6.1 Introduction ............................................................................................................. 50
6.2 Steps in Umbrella techniques.................................................................................. 53
6.3 Results and discussion ........................................................................................... 54
Chapter 7 ......................................................................................................................... 59
Conclusions and suggestions for future work .............................................................. 59
7.1 Conclusions ............................................................................................................. 59
7.2 Future work ............................................................................................................. 60
References………………………………………………………………………………61
Appendix A…………………………………………………………………………….64
Appendix B……………………………………………………………………………65
Appendix C……………………………………………………………………………...70
List of Figures
1.1 Description of typical eukaryotic cell .....................................................................2
1.2 Structure of phospholipids ......................................................................................4
2.1 Bonded and non-bonded interaction terms in force field .......................................10
3.1 Structure of Dimyristoyl phosphatidylcholine (DMPC) ........................................15
3.2 Snapshot of DMPC in VMD .................................................................................18
3.3 Membrane thickness variation as a function of simulation time ...........................19
3.4 Order parameter comparision from simulations and experiments .........................20
4.1 Chemical structure of HEPES ................................................................................24
4.2 Comparison of optimised and experimental bond length,angles and dihedrals for
HEPES molecule ................................................................................................................33
4.2 HEPES structure after geometry optimisation .....................................................33
5.3 Density distribution of the buffer molecules at different concentrations .............41
6.3.1 Snapshots from the simulation showing the pulling of HEPES molecule ............54
6.3.2 Umbrella histograms .............................................................................................56
6.3.3 Free energy profile for insertion of HEPES from aqueous phase to lipid phase .57
List of Tables
3.1 Physical properties of DMPC obtained from Avanti polar lipid………………......15
4.1 Physical properties of HEPES………...…………………………………………...24
4.2 List of some commonly used Good’s buffers……………………………………..26
5.3.2 Average number of different hydrogen bonds in the system ……………………45
5.3.3 Area per lipid and bilayer thickness of DMPC ……….……...………………….47
5.3.4 Coordination number at different buffer concentrations………………………....49
1
iv
Chapter 1
Introduction
1.1 Cell
Cells are the primary building blocks of living organisms. Biologists have divided cells
into two primary types: eukaryotic and prokaryotic cells. Eukaryotic cells are characterised
by the presence of a well-defined nucleus. The nucleus, which houses DNA, is contained
within a membrane, separated from other cellular structures. Prokaryotic cells however
have no true nucleus. DNA in a prokaryotic cell is not separated from the rest of the cell
but coiled up in a region called the nucleoid. Nevertheless independent of its type, cells are
the basic structural, functional and biological unit of all known living organisms including
viruses which can replicate independently.
Every cell is enclosed by a membrane which gives structure to the cell and allows for the
passage of nutrients and metabolic wastes into and out of the cell. The cell membrane is
made up of the bilayer which is predominantly made up of lipids with their hydrocarbon
tails facing inwards. The cell membrane typically contains other molecules such as
carbohydrates and proteins, which serve as receptor sites for other messenger molecules.
Interactions with the cell membrane allows molecular signalling events which
communicate with processes that occur within the cell [5].
1.2 Cell Membrane
Cell membranes are rich in two classes of molecules: lipids and proteins. Proteins serve as
enzymes, transport molecules, and provide the membrane with distinctive functional
properties while lipids provide the structural integrity to the cell as discussed in Figure 1.1.
Lipids found in the cell membrane consist of two parts: hydrophilic (water soluble) and
hydrophobic (water insoluble). The hydrophobic portion of the lipids is the non-polar long
Figure 1.1: Structure of eukaryotic cell membrane showing different types of proteins and phospholipids.
Both the exterior and interior region of the cell membrane are multicomponent made up of a large number
of different types of molecules. [1]
hydrocarbon chains of two fatty acids. The fatty acids are present as esters bonded to
glycerol. The third-OH group on glycerol is ester bonded to phosphate hence the term
phospholipid. The phosphate ester portion of the molecule is polar or even ionic and hence
is water soluble.
1.3 Lipid Bilayer
At the macroscopic (cellular) level, the membrane are modelled as two dimensional layers,
covering a cell and appears as a “fluid mosaic model”, rich in complexity along with a
heterogeneous distribution of lipids forming a matrix in which proteins are embedded.
The bilayer structure which has a thickness of 3-4 nm results spontaneously from lipid self-
assembly, driven by the hydrophobic effect. Arrangement of lipid bilayers in cell
membranes can be derived from X-Ray diffraction data. Fig 1.2 shows the chemical
structure of phospholipids in the lipid bilayer. Animal cells are arranged as a bilayer
stacked with the non-polar hydrocarbon chains pointed inward while the polar ends act as
the external surface facing the surrounding aqueous environment. The hydrophobic layer
of the cell membrane acts as a barrier for ionic and polar molecules from directly entering
inside of the cell.
Eukaryotic cell are characterised by the presence of sterol (eg. cholesterol), inserted
between the non-polar chains, and makes up about 20% of the molecules of the membrane.
This helps to make the membrane more rigid and adds to its physical strength. Apart from
this, sterols and glycerophospholipids account for about 85-90% of the total lipids in
membrane with sphingolipids (eg. sphingomyelin) accounts for majority of the remaining
fraction.
Figure 1.2: Structure of a typical phospholipid in the lipid bilayer. Figure shows chemical structure of
hydrophilic and hydrophobic tail which is produced from esterification of fatty acids and glycerol [2] .
The prominent function played by lipids can be categorised into three parts [6]. First they
provide the barrier for passive diffusional motion of small polar solutes like ions, sugar and
low molecular weight metabolites as well as all macromolecules such as proteins, nucleic
acid and other poly saccharides.
Secondly they provide a unique solvation environment for trans membrane protein. Finally
third and less studied is their role in the internal organisation of the cell, which accounts
the major fraction of cell function. Thus regulating various chemical processes that occur
in the cell.
1.4 Role of buffers in cell membrane
Buffers plays a crucial role in maintaining pH of a medium by resisting changes in H+ ions
and OH- ions concentrations. In the human body, blood plasma has a buffer mixture of
carbonic acid and hydrogen carbonate ions which keeps the pH constant and avoid acidosis
or alkalosis, a condition resulting due to an increase or decrease in the pH. Moreover in
the laboratory, buffers are used to maintain the pH during cell culture or bacterial growth.
In biophysical and biochemical studies of lipid bilayers the influence of buffer is often
ignored or assumed to be negligible on membrane structure, elasticity, or other physical
properties. However, experimental observations on giant unilamellar vesicles [7] suggest
that buffering molecules may considerably affect the bending rigidity of
phosphatidylcholine bilayers. Furthermore, a synergistic effect on the bending modulus is
observed in the presence of both salt and buffer molecules, which serves as a warning to
experimentalists while data interpretation of their studies, since typical lipid bilayer studies
contain buffer and ion molecules.
1.4 Problem definition
In this project work we focused our attention towards the specific buffer molecules and
their interactions with the lipid bilayers by using atomistic molecular dynamic simulations.
We choose zwitterionic buffer molecules that are commonly used as buffering agents while
carrying out experiments and the DMPC lipid bilayer as a prototypical lipid bilayer. All
atom molecular dynamics simulations are performed to study effect of the buffer on bilayer
structural properties such as radial distribution functions and density distribution as a
function of buffer concentrations In addition we also carry out potential of mean force
calculations to investigate the binding affinity of the buffer molecules with the bilayer
membrane. All simulations were performed using GROMACS molecular dynamics
simulation package which is an open source molecular dynamics code under GNU Public
License (GPL).
The chapters in the report are organized in the following manner. Chapter 1 introduce
reader with the cell and its role in our body followed by research problem definition. In
Chapter 2, we describe molecular dynamics simulation methods and introduce the different
methods for solving Newton’s equation of motion. In Chapter 3, we simulate the pure
DMPC lipid bilayers in order to test our simulation protocols. Preliminary results of these
simulations are presented to validate our method. In Chapter 5 we present simulations of
the DMPC lipid bilayer in presence of different buffer molecules at various concentrations.
Density distribution at different buffer concentration, hydrogen bonding and radial
distribution functions are also presented. In Chapter 6, we performed free energy
calculation for the penetration of buffer molecules inside the lipid bilayers. A brief theory
for biased umbrella sampling is presented in this chapter. Free energy profile along bilayer
normal (z-direction) is computed to obtain the free energy landscape of the buffer-bilayer
interactions, enabling us to comment on the thermodynamically most favourable state.
Chapter 2
Molecular Dynamics
2.1 Introduction
Lipid bilayers dynamics vary over large length and time scale. A typical bilayer thickness
in cell membrane ranges from 3 to 4 nm with bilayer undulations ranging from 4 Å to 0.25
mm. Bond vibrations occur on the femtosecond time scales and lipid lateral diffusion
occurs on the nanosecond time scale. Various undulation modes range from nanoseconds
to milliseconds time scales. Hence the lipid dynamics occurring at these length and time
scale not only elude bare eyes but also ordinary microscope. Therefore power of molecular
dynamics simulation comes into picture, which has an ability to scan out the atomic level
description and orientations of atoms and their interaction. In this chapter the method of
molecular dynamics is described along with some commonly used force fields which are
used in all atom molecular dynamic simulations.
2.2 Simulations … How it works?
Molecular dynamics simulations involves numerically integrating Newton’s equation of
motion [8] thereby generating trajectories obtained from solving forces derived from an
appropriate interaction potential, assuming that the molecules follow classical mechanics.
The equations of motion for an assembly of N particles with positions 𝑟𝑖, momenta 𝑝𝑖 and
masses 𝑚𝑖 can be expressed as follows:
𝜕𝑟𝑖
𝜕𝑡=
𝑝𝑖
𝑚𝑖= 𝑣𝑖 (2.1)
𝜕𝑝𝑖
𝜕𝑡= 𝐹𝑖 = −
𝜕𝑈(𝑟𝑖)
𝜕𝑟𝑖 𝑤ℎ𝑒𝑟𝑒 𝑖 = 1,2 … . . 𝑁 (2.2),
and 𝐹i is the total conservative force on 𝑖th particle due to all other particles.
The non-bonded interaction potential for soft spheres is the Lennard-Jones 12-6 potential,
𝑢(𝑟𝑖𝑗) = 4휀 [(𝜎
𝑟)
12
− (𝜎
𝑟)
6
] (2.3)
The total potential energy 𝑈 can be written as
𝑈 = ∑ ∑ 𝑢(𝑟𝑖𝑗) (2.4)
𝑁
𝑗=1𝑖>𝑗
which is the sum of interaction energies on the 𝑖th particle due to all other particles, 𝑟𝑖𝑗 is
the distance between the two particles, ε and σ are the depth of the potential well and
distance at which the inter-particle potential is zero respectively. 𝐹𝑖 is related to 𝑈 by the
equation 2.2. The interaction potential 𝑈 contains parameters which are taken from
experiments and/or quantum mechanical calculations.
There are various algorithms for solving these equations of motion including Verlet, leap-
frog, Velocity-Verlet algorithms etc. One of the popular methods for the numerical
integration is the Velocity-Verlet algorithms, which is described below,
𝑟𝑖(𝑡 + 𝛿𝑡) = 𝑟𝑖(𝑡) + 𝛿𝑡𝑣𝑖(𝑡) +𝛿𝑡2
2𝑚𝑖 𝐹𝑖(𝑡) (2.5)
𝑣𝑖(𝑡 + 𝛿𝑡) = 𝑣𝑖(𝑡) +𝛿𝑡
2𝑚𝑖 [𝐹𝑖(𝑡) + 𝐹𝑖(𝑡 + 𝛿𝑡)] (2.6)
Figure 3.1: Bonded and non-bonded interaction terms in the force field. Right figure
shows the non-bonded interaction potential and consist of columbic interaction (bottom
right) and Lennard-Jones potential (top right). Left figure shows the bonded interaction
which consist of bond angle, length (bottom left) and dihedral terms (top left) [4] .
Here 𝑣𝑖(𝑡) is the velocity of the ith particle and a trajectory of velocities is obtained with an
increment of 𝛿𝑡 time interval. For more complex molecules and environments, like lipid
bilayer with embedded proteins in addition to intermolecular forces there will be
intramolecular force as well. Figure 3.1 shows the potential energy for bonded and non-
bonded interactions which can be written as a sum of different interaction energies as
follows:
𝐸 = 𝐸𝐿𝐽 + 𝐸𝑐𝑜𝑢𝑙𝑜𝑚𝑏 + 𝐸𝑏𝑜𝑛𝑑𝑙𝑒𝑛𝑔𝑡ℎ + 𝐸𝑏𝑜𝑛𝑑𝑎𝑛𝑔𝑙𝑒 + 𝐸𝑡𝑜𝑟𝑠𝑖𝑜𝑛𝑎𝑙 (2.7)
𝐸𝐿𝐽 is the soft sphere Lennard-Jones non bonded interaction potential and 𝐸𝑐𝑜𝑢𝑙𝑜𝑚𝑏 is the
electrostatic non bonded interaction between fixed charges.
The functional form can be described as follows:
𝐸𝐿𝐽 = 4 ∑ 휀𝑖𝑗
𝑖,𝑗
[(𝜎𝑖𝑗
𝑟𝑖𝑗)
12
− (𝜎𝑖𝑗
𝑟𝑖𝑗)
6
] (2.8)
where, in this equation 휀𝑖𝑗 gives the strength of interaction between non bonded
atoms and 𝜎𝑖𝑗 is a distance parameter at which potential is zero and 𝑟𝑖𝑗 is the distance
between atoms i and j.
𝐸𝑐𝑜𝑢𝑙𝑢𝑚𝑏 = ∑𝑞𝑖𝑞𝑗
4ᴨ휀0𝑟𝑖𝑗 (2.9)
𝑖,𝑗
where 𝑞𝑖 and 𝑞𝑗 are the effective charges on the atoms and 휀0 is the free space permittivity
Similarly the functional form of the bonded interaction can be described as follows:-
𝐸𝑏𝑜𝑛𝑑𝑙𝑒𝑛𝑔𝑡ℎ = ∑𝑘𝑏
2(𝑟𝑖𝑗−𝑙𝑖𝑗)2
𝑖,𝑗
(2.10)
where, 𝑘𝑏 is spring constant and 𝑙𝑖𝑗 is a equilibrium value of length between atoms
i and j which are bonded.
The bond-angle term is a three body potential and can be written as a sum of harmonic
potentials between three atoms.
𝐸𝑏𝑜𝑛𝑑𝑎𝑛𝑔𝑙𝑒 = ∑𝑘𝛩
2(𝛩𝑖𝑗𝑘−𝛩0
𝑖𝑗𝑘)2
𝑖,𝑗,𝑘
(2.11)
where 𝛩𝑖𝑗𝑘 is the angle formed by i,j and k atoms and 𝛩0𝑖𝑗𝑘 is the equilibrium value of
angle.
Torsional or dihedral angle potential describes the rotational flexibility of the chains and
one of the popular functional form is given below.
𝐸𝑡𝑜𝑟𝑠𝑖𝑜𝑛𝑎𝑙 = ∑ ∑𝑣𝑛
2(1 ± cos (𝑛𝜏𝑖𝑗𝑘𝑙))2 (2.12)
𝑛𝑖𝑗𝑘𝑙
where 𝜏𝑖𝑗𝑘𝑙 is the angle between the planes formed by atoms i, j and k and atoms j, k and l.
The first sum is over all dihedral angles. Integer n is typically a value between one and
three.
It is worth mentioning that there are no unique force fields describing all kinds of lipids
bilayer systems. In fact depending on our working environment and the types of lipids we
need to carefully select the force fields for our system. To name some of the well-known
atomistic force fields in literature are CHARMM, AMBER, OPLS-AA, OPLS,
GROMACS87, GROMACS96, GROMOS.
In these CHARMM, AMBER and OPLS-AA are all-atom force fields and consider
hydrogen atoms explicitly in the simulations. Others are united atom force fields and do
not consider non-polar hydrogen’s attached to aliphatic carbon atoms due to their light
weight. Both types of force fields are known as atomistic force fields and are used
depending on the nature of problem.
To eliminate edge effects and mimic a macroscopic system, we take a help of a simulation
box having a fixed number of molecules replicated by using three-dimensional periodic
boundary conditions (PBCs). In the case of a membrane simulation, application of PBCs
to a small membrane portion generates an infinite multi lamellar system. The constant
pressure and temperature (NPT) or isothermal-isobaric ensemble is particularly useful for
membranes because it gives the possibility for validating simulations results by checking
some experimentally reported parameters. For example the phase behaviour can be
analysed from order parameters and dynamic structure factors which can then be compared
with published literature results.
Chapter 3
Molecular dynamics simulations of
DMPC
3.1 Introduction
For decades, biophysicists have used dimyristoyl phosphatidylcholine (DMPC) bilayers as
model system to study the structural and dynamics of the lipid membrane as well as
understanding the interaction of small molecules and proteins with the lipid membrane. For
the most part, DMPC’s popularity as a model membrane system can be attributed to the
fact that it is stable, inexpensive, and easy to obtain. Importantly, the bilayers that it forms
have physical properties not dissimilar to those found in biological membranes (e.g., liquid
crystalline order, hydrophobic thickness, etc.). In this chapter our focus is to perform
molecular dynamic simulations with pure DMPC lipid bilayers and to compare the results
with the experimental studies.
DMPC lipid bilayers have a net zero charge with a positive charge on nitrogen atom and a
negative charge on phosphate group. The zwitterionic structure of DMPC molecule is
shown in Figure 3.1 and its physical properties are given in table 3.1. In this study we have
simulated DMPC bilayer at 370C which is well above its transition temperature of 240C. In
order to confirm it liquid crystalline phase (Lα) we have computed structural properties
like acyl tail order parameter and the area per head group which shows good agreement
with experimental values.
Figure 3.1: Chemical structure of dimyristoyl phosphatidylcholine (DMPC)
Molecular formula C36H72NO8P
Molar mass 677.933 g mol−1
Transition Temperature 24oC
Percent composition (w/w%) C-63.78%,H-10.70%,N-2.07%,O-18.88%,P 4.57%
Table 3.1 Physical properties of DMPC lipid bilayers obtained from Avanti polar lipid
3.2 Simulation methods and details
Simulations were carried out in the constant pressure, temperature and number of
molecules (NPT) ensemble with periodic boundary condition in all the three direction using
the GROMACS molecular simulation package [9].
The DMPC bilayer was taken from Stockholm Lipids (S-Lipid) [10]website which consist
of 128 lipid molecules. We have maintained 30 waters per lipid so as to mimic fully
hydrated system. Hydration was carried out using the TIP3P (transferable intermolecular
potential 3P) water model. The total system size was 63.2 × 63.2 × 63.6 Å. Dynamics were
propagated using a leapfrog integrator with time steps of 2 femtoseconds and the
coordinates were saved after every 2 ps. MD Simulation were performed in three stages:
first energy minimisation in order to avoid any repulsive or steric contacts followed by
NVT and NPT ensemble. We have chosen a temperature of 310 K to ensure system
temperature is well above its transition temperature of 297 K. The system temperature was
maintained at 310 K using the Nosé-Hoover thermostat and pressure was maintained at 1
atm using Parrinello-Rahman barostat with semi isotropic pressure coupling. Particle mesh
Ewald summation was used to account for the conditionally convergent long-range
electrostatic interactions. During simulations all bonds were constrained using LINKS
algorithms [11] in order to achieve longer run.
3.3 Results and discussion
Figure 3.2 shows snapshot of simulation box which consists of 128 DMPC lipid molecules
and 3840 water molecules. We have maintained 30waters per lipid molecules in order to
confirm bilayer is well above its critical hydration number of 18 water per lipid [12]. In a
simulation box with three dimensional periodic boundary conditions, bilayer d-spacing is
simply the box dimension in the direction perpendicular to the bilayer membrane. As the
system under study contain single lipid bilayers in a box, the total length of box in the
direction of bilayer normal can be considered as the d-spacing. Thus 𝐿𝑧 is the d-spacing in
our study.
The properties of a lipid bilayer are commonly described using the area per lipid, bilayer
thickness and acyl chain order parameters. These properties also help us understand the
phase of the lipid at a given temperature.
The average area per lipid is computed by taking mean value of the XY box vectors and
dividing by the total number of lipids. This is found to be 61.58 Å2 which is in good
Figure 3.2 Snapshot of simulation box which is drawn from VMD (Virtual Molecular
dynamics) simulation package. The simulation is carried out with 128 DMPC lipid
molecules with 64 in the upper leaflet and 64 in the bottom leaflet. Total number of water
molecules in a box are 3840 in order to ensure bilayer is well above its critical hydration
number. Figure illustrate the d-spacing (Lz) which is length of z-coordinate in a
simulation box with periodic system.
agreement with experimental value of 60.6 Å2 obtained from X-ray diffraction experiments
at 310 K [13]
Thickness of the bilayer is not uniform and shows thermal fluctuations in XY plane of
bilayer. In GROMACS membrane thickness is obtain by tagging a reference atom in the
head group usually phosphorus atom both in upper and lower leaflet and using the script
g_dist tool to obtain the distance between them. Figure 3.3 shows the variation of bilayer
thickness with average value of 3.016 nm which is in good agreement of reported value of
3.67 nm [13].
Figure 3.3: Membrane thickness variation as a function of simulation time with a mean
value of 3.016 nm.
Lipids in a fluid bilayer are highly dynamic. Many movements on different timescales take
place: rotation around chemical bonds and Trans/gauche isomerisation (picoseconds),
rotation (axial diffusion) around the lipid axis (nanoseconds), lateral diffusion
(microseconds), flip-flop across the bilayer (millisecond) and undulation of the membrane
(milliseconds to seconds). Most of these movements influence the order parameters of the
acyl chains
Lipid acyl chain order parameters are obtained easily from deuterium NMR experiments
and can be compared with simulation. In simulation lipid order parameters are a defined as
Figure 3.4: figure 3.4(a) shows the experimentally measured order parameter and figure
3.4(b) to the right shows corresponding results for simulati on. Series1 and Series2 are
values for SN1 and SN2 tails of DMPC respectively.
𝑆 = ⟨3 cos 𝜃2 − 1
2⟩ (3.1)
where 𝜃 is the (time dependent) angle between the C–H bond vector and a reference axis
which Z coordinate in our case. Figure 3.4 shows both simulated and reported values for
order parameter. S = 1 means perfect alignment with the bilayer normal, S= −0.5 anti-
alignment, and S = 0 random orientation.
Chapter 4
Ab-initio calculations and simulation of
HEPES
4.1 Introduction
Buffer solutions are essential to maintain the desire pH in organisms to function properly.
Many enzymes and proteins work only under very precise pH conditions; if the pH moves
outside a narrow range, enzyme activity can be slowed or stopped completely, protein
unfolding can occur leading to denaturing the cell. In many studies pH is adjusted outside
the working range in order to bring denaturation or cell-lysis. Until 1966 biologists used
buffers made up of carbonic acid (H2CO3) and bicarbonate (HCO3−) which were not very
effective in maintaining a neutral pH due to their low pKa values [14].
The rapid development of molecular biology prompted biologists to search for effective
buffering agents, which resulted in synthesis of a number of different buffer compounds
that can effectively maintain the physiological pH range of 7.0–8.0. A set of 12 of them
were described by Norman Good and co-workers in 1966 as suitable for biological
applications and since then have been described as the ‘Good’ buffers. Table 5.2 describes
a set of some commonly used Good’s buffesr. Good’s buffers apart from maintaining
desired pH, exhibit other experimentally useful properties like resistance to enzymatic
degradation, lack of UV absorbance, lack of interference with biological assays and very
limited cell-wall permeability. In our study we have first chosen HEPES buffer and
monitored its effect on a DMPC lipid bilayer[14].
In this Chapter we will discuss the derivation of partial charges for HEPES molecule from
ab-initio calculations. We have validated the molecular structure of the HEPES molecule
from experimental data and carry out molecular dynamic simulations in order to check its
stability in water.
4.1.1 HEPES
HEPES (HydroxyEthylPiperazineEthaneSulfonic acid) is a zwitterionic organic buffering
agent and included in one of the twenty mentioned Good's buffers. HEPES is commonly
used in cell culture because of its ability in maintaining physiological pH during cellular
respiration as a result of the variation in carbon dioxide concentration. Figure 4.1 and table
4.1 describes the chemical structure and physical properties of HEPES. During simulations
we have maintained a neutral pH in order to keep pKa and pH corresponding to
experimental conditions where the buffer performance is optimal.
4.1.2 Charge derivation for HEPES
In order to perform simulations on any given molecule, it is necessary to obtain values for
partial charges on each atom, its geometrical parameters such as bond lengths, angles and
dihedrals. Moreover a reliable force field has to be selected which involves bond, angle,
dihedrals, bonded and non-bonded interaction parameters. In what follows we briefly
describe the quantum mechanical basis for the charge derivation procedure.
Molecular formula C8H18N2O4S
Molar mass 238.30 gmol−1
Melting point 238oC
Appearance White crystalline powder
pKa (250C) 7.5
pH range 6.8 to 8.2
Table 4.1 Physical properties of HEPES
Figure 4.1 Chemical structure of HEPES
Matter is composed of atomic nuclei and electrons, and complex interaction of these atomic
particles is responsible for all intrinsic characteristics of the material. To explain electronic
structure of the material we need to perform quantum mechanics calculations and it was
known more than hundred years ago that solving the many body Schrodinger wave
equation can in principle yield all the material properties. The general form of time-
independent Schrödinger wave equation is,
Buffer Effective
pH range Molecular structure
MES
(MorpholinoEthaneSulfonic acid)
5.5–7.7
BES
(Bis2-hydroxyethyl)-2-
aminoEthaneSulfonic acid)
6.4–7.8
MOPS
(MorpholinoPropanSulfonic acid)
6.5–7.9
TES
(Trishydroxymethyl]-2-
aminoEthaneSulfonic acid)
6.8–8.2
HEPES (2-Hydroxyethyl)-1-
PiperazineEthaneSulfonic acid) 6.8–8.2
Table 4.2 List of some commonly used Good’s buffers.
𝐸𝜓 = Ĥ𝜓 (4.1)
where 𝜓 is the wave function and 𝐸 is the total energy of the system corresponding to that
wave function and Ĥ is the Hamiltonian operator which characterises the total energy of
any given wave function. The total Hamiltonian of a system containing NI atomic nuclei
and Ne electrons can be written as,
Ĥ = Ĥ𝑛𝑛+ Ĥ𝑒𝑒+ Ĥ𝑛𝑒
= {− ∑ ħ2
2𝑀𝐼𝛻𝐼
2 + 𝑉𝑛𝑛 𝑁𝐼
𝐼=1} + {− ∑
ħ2
2𝑚𝛻𝑖
2 + 𝑉𝑒𝑒 𝑁𝑒
𝑖=1} (4.2)
where the subscript ‘I’ indicates ions and the subscript ‘i’ indicates electrons, 𝑀𝐼 is the
ionic mass, m is the electron mass, ħ =h/2π where h is the Planck’s constant. The first term
in Eq. 4.2 represent the Hamiltonian Ĥ𝑛𝑛 for the nuclear coordinates, the second term
corresponds to the Hamiltonian for the electronic coordinates Ĥ𝑒𝑒 and the last term Ĥ𝑛𝑒
corresponds to the interactions between the nuclei and the electrons. 𝐻𝑛𝑒 describes the
interactions between electrons and nuclei. Once the Hamiltonian is known one can write
the many body Schrodinger wave equation as,
{Ĥ𝑛𝑛+ Ĥ𝑒𝑒+ Ĥ𝑛𝑒} 𝜓𝑡𝑜𝑡 = 𝐸𝜓𝑡𝑜𝑡 , (4.3)
where 𝜓𝑡𝑜𝑡 is the wave function of the total system comprising of nuclei and associated
electrons and E is the corresponding energy.
The apparent simplicity of the equations however belies the actual complexity involved in
solving the problem. It is generally impossible to find the true solution for many body total
wave function𝜓𝑡𝑜𝑡, even for very small system involving few ions and electrons. Hence in
order to obtain the solution involving a large number of ions and electrons it is often
necessary to introduce suitable approximations and reformulations of the above equations.
Here we state three simplifications in order to handle three contribution to the Hamiltonian
accurately and efficiently.
1. The Born-Oppenheimer approximation for separating nuclear degrees of freedom from
the electronic degrees of freedom
2. The density functional theory for handling ground state electronic interactions.
3. Mean field approximation where the system comprising of large number of small
interacting individuals components in which the effect of all other individuals on any given
individual is approximated by a single averaged effect, thus reducing a many body problem
to one body problem.
We will not go in details and functional form of the above equations and restrict ourselves
at this point. Next part of this chapter is concerned with calculating partial charges on
molecule. Various quantum mechanical packages are available for carrying out these
calculations; GAMESS, Gaussian, Jaguar, and Quantum ESPRESSO. We use Guassian-
09 package for our calculations.
Initial structure for HEPES molecule was built using GUASSVIEW and the energy
minimisation and optimisation of the structure was carried out in Gaussian using the
B3LYP basis set. Details are provided in the Appendix A.
4.1.3 Molecular geometry optimization and partial charge
Geometry optimization for HEPES has been achieved by energy minimization, using DFT
at the B3LYP level, employing the split valence basis set 6-311G (d). Initial structure of
the molecule was built using the Gauss view program then optimized in steps to obtain
local minima on the potential energy surface. The optimized molecular structures thus
obtained along with the numbering scheme of the atoms are shown in Fig. 4.1. We
compared the values for bond length, bond angle, and dihedrals from CIF (Crystallographic
Information File) file for HEPES molecule and found the results to be in good agreement
as shown in fig 4.2 and 4.3.
In second step we perform HF (Hartree-Fock) calculations employing 6-311G (d) basis set
to get electrostostatic points (ESP) for molecule. Since we are using GAFF (Generalized
Amber Force Field) for HEPES, we need to obtain RESP (Restrained electrostatic
potential) charges as discussed in the GAFF computational procedure [15]. Hence we input
ESP data into Antechamber package which is design to perform two main task; first assign
the atom types from GAFF and find any missing force field parameters of the molecule.
Second to calculate and assign partial charges based on the RESP procedure. Finally we
use ACPYPE tool to generate topologies for the molecule based on GAFF as a necessary
input requirement to GROMACS. Fig 4.2 shows RESP partial charges on atoms (hydrogen
atoms are not shown for visual simplicity).
Figure 4.2 (b)
Figure 4.2 (a)
Figure 4.2 (c)
Figure 4.2: Comparison of optimized bond length with experimental values (a) for all
thirty three bonds in HEPES molecule. Figure 4.2(b) and 4.2(c) shows comparison of
some selected bond angle and dihedra ls with experimental values . Experimental data are
obtained from crystallographic information file for HEPES.
4.2 Simulation of HEPES in water
Initial structure for HEPES molecule which is generated in Section 4.1.3; is simulated in a
cubic box in presence of water molecules under constant pressure, temperature and number
of molecules (NPT ensemble) for 10 nanoseconds. Protonated structure of HEPES was
hydrated using TIP3P water model in GROMACS with genbox tool. The total system size
is 3.0 × 3.0 × 3.0 Å. Leap frog integrator with a time step of 2 femtoseconds is used for
integrating equations of motion and the coordinates are saved after every 2 picosecond.
Fig 4.3 HEPES structure after geometry optimization. Numbers on each atom shows
RESP (Restrained Electrostatic Potential) partial charges whic h are derived from
Hartree-Fock basis set. (Hydrogen atoms are not shown for visual simplicity)
The system temperature is maintained at 310 K using the Nosé-Hoover thermostat and
pressure is maintained at 1 atm using Parrinello-Rahman barostat with isotropic pressure
coupling.
4.2.1 Analysis
The average number of hydrogen bonds ⟨NHB ⟩ per molecule for each saved frame was
determined based on a geometrical criterion with a cut-off donor−acceptor (DA) distance
of 0.35 nm and a cut-off donor−hydrogen−acceptor (DHA) angle of 30°.The donor-
acceptor (DA) criteria adopted here gives the simulated DHA angle distribution and the
Figure 4.4: Hydrogen bond distribution for HEPES in water (a) after 10 nanoseconds of simulation. Total
11.11 number of hydrogen bonds are formed using donor acceptor distance of 0.35 nm and
donor−hydrogen−acceptor (DHA) cut off angle of 30°. Figure 4.4(b) shows RMSD plot for HEPES
molecule with respect to simulation time. HEPES molecule shows the structure stability during simulation
time of 10 ns with fluctuations around 0.1 nm.
Figure 4.4 (a) Figure 4.4 (b)
Nu
mb
er o
f h
yd
rogen
bond
DA distance in water similar to the experimental values [16]. Average number of hydrogen
bond ⟨NHB ⟩ are reproduced by using the standard tool g_hbond implemented in
GROMACS.
In the protonated form HEPES buffer has two pKa. The first dissociation constant (pKa1)
refers to the dissociation of the sulfonic group, and the second dissociation is due to
dissociation of the protonated amino group (pKa2). Thus in aqueous solutions, HEPES
molecule possesses both negatively charged sulfonic group (SO3-) and a positively charged
amino groups (NH3+) and becomes a zwitterionic molecule [14]. Due to donor acceptor
sites, HEPES provides a number of possibilities for formation of hydrogen bonds with the
solvent. Fig 4.4 (a) shows the distribution of hydrogen bonds as a function of distance. The
average number of H-bonds for HEPES molecule ⟨NHB ⟩ with water molecules is 11.11
which is compared with the reported value of 11.94 [17].
We have verified the stability of HEPES structure by computing the RMSD (root mean
square deviation) as shown in Figure 4.4 (b).Using GROMACS tool g_rms, each structure
from trajectory is compared to a reference structure for all time frames. RMSD is calculated
using following formula:
𝑅𝑀𝑆𝐷 = √∑ (𝑥𝑖−𝑥𝑟𝑒𝑓)2 𝑛
𝑡=1
𝑁 (4.4)
where 𝑥𝑖 is the coordinate of the molecules at time 𝑡, 𝑥𝑟𝑒𝑓 is the reference structure
coordinate and 𝑁 is the total number of atoms in the molecule.
Initial structure as described in section 4.2 for HEPES is the reference structure and we
monitor the displacement of molecules from the centre of mass position with respect to the
reference structure. For a 10 nanosecond simulation, the HEPES molecules shows
structural stability in water with fluctuations around 0.1 nm (Figure 4.4b). We did not
observe any distortion in the geometry during this time
Chapter 5
Simulation of DMPC in presence of
buffer molecules
5.1 Introduction
Several Good’s buffers which fulfills the selection criteria based on pKa, solubility, low
membrane permeability and ease of preparation are commonly used in laboratories. In this
study we investigate the effect of three different buffer molecules on the DMPC lipid
bilayer, namely HydroxyEthyl Piperazine Ethane Sulfonic acid (HEPES), Morpholino
Ethane Sulfonic acid (MES), Piperazine Ethane Sulfonic acid (PIPES). We have discussed
the interactions with lipid bilayers by calculating number of hydrogen bonds, radial
distribution functions and density distributions.
5.2 Simulation Method
The equilibrated DMPC bilayer consisting of 128 lipid molecules with box dimensions of
64.0 × 64.0 × 70.0 Å is obtained from the previous simulations in Chapter 3. The geometry
of the simulation box is such that the bilayer surface is in the x,y-plane and the bilayer
normal is along the z-axis. Buffer molecules are first placed on top of bilayer with 1.5 nm
distance from the head group. Water molecules are then added to the system and the
required concentration of buffer is obtained by increasing the number of buffer molecules
and decreasing the number of water molecules. The system is further equilibrated in the
NPT ensemble for 5ns.
We have chosen a temperature of 310 K to ensure the system temperature is well above the
bilayer melting transition temperature of 297 K. The temperature is maintained at 310 K
using a Nosé-Hoover thermostat and the pressure is maintained at 1 bar using the
Parrinello-Rahman barostat with semi isotropic pressure coupling. Both the temperature
and pressure of the solvent and lipid are controlled independently. The particle mesh Ewald
summation was used to account for the long-range electrostatic interactions. During the
simulations all bonds were constrained using the LINKS algorithm. We derived the partial
charges and optimised the structure for MES and PIPES buffer molecules in the similar
fashion as outlined for the HEPES molecule in Chapter 4.
5.3 Results and Discussion
5.3.1 Mass density
Density is computed by dividing the simulation box into number of slices along the z-
direction. Mass of the reference molecule in each individual slice is computed over all
frames which is then divided by the volume of each slice to obtain the local density in each
slice. The plot of the mass densities for the three simulation systems under study are shown
in the Figure 5.3. The density of buffer molecules indicates that buffer molecules are
uniformly distributed in the aqueous region and the non-zero value next to the bilayer head
groups indicate that there is a weak interaction of these molecules with the bilayer. In the
case of HEPES we observe that the buffer density penetrates into the bilayer to a greater
extent when the buffer concentration is increased and a weak maxima is observed in the
vicinity of the head groups. Similar trends are observed with MES and PIPES. However in
all cases, the density drops towards the centre of the bilayer indicating that the buffer
molecules predominantly interact with the zwitterionic head group region of the DMPC
bilayer. An important result is that the buffer molecules shows a weak electrostatic
attraction towards the oppositely charged head group molecules in the bilayer.
5.3.2 Hydrogen bonds
Calculation of hydrogen bonds involves identifying donor and acceptors as follows; A
hydrogen atom attached to a relatively electronegative atom will play the role of hydrogen
bond donor while an electronegative atom such as fluorine, oxygen or nitrogen will act as
the hydrogen bond acceptor, irrespective of whether it is bonded to hydrogen or not. In the
Figure 5.3: density distribution of the buffer molecules at different concentrations.
Average density of buffer molecules have been amplified by multiplying a factor of 8
and 10.Maximum density for buffer molecules lies near the head group region showing
a weak attraction towards the lipid head groups.
donor molecule, the electronegative atom attracts the electron cloud from the hydrogen
nucleus by decentralising the electron cloud, giving rise to a partial positive charge on the
hydrogen atom and a partial negative charge on the electronegative atom.
In our study we calculated the hydrogen bonds based on the following criteria; the distance
between the water oxygen (OW) and the DMPC oxygen is less than or equal to 3.25Å and
the hydrogen bond angle 𝜃, which is the angle between the DMPC oxygen and H-OW
bonds of water is less than or equal to 350 as proposed by Raghavan et.al. [18].
In this study several hydrogen bonding forms have been explored; between buffer
molecules and the lipids, between water and the lipids as well as between water and buffer
molecules. The results are summarized in Table 5.3.2 which shows that all the buffer
molecules form hydrogen bonds with the DMPC lipids. Although the presence of buffer
molecules for the concentrations examined in this study has a weak influence on the DMPC
bilayer some differences can be observed. In the case of HEPES the number of water-
DMPC hydrogen bonds shows a small decrease when the number of HEPES molecules is
increased to 10. However the water-DMPC hydrogen bonds for MES and PIPES do not
show any changes with the buffer concentration. Similar number of hydrogen bonds are
obtained on comparing the values for pure lipids hydrogen bond with water from the study
[16].
Table 5.3.2 (a)
5.3.3. Area per lipid
One of the important quantities in describing the behaviour of lipid bilayers is the average
area per lipid. We calculated the average area per lipid molecule by multiplying the time
average XY dimensions of the simulation box and dividing the result by the number of
lipid molecules present in one leaflet of the bilayer.
Table 5.3.3 presents the area per lipid and bilayer thickness under different buffer and
concentration. For reference DMPC system the calculated area per lipid is 62.59 Å2 , which
is close to the experimental value of 61.2 Å2 at 300 K and 1 bar, and is in good agreement
with the values obtained in previous simulations [13]. From the results we can conclude
that the buffer molecules do not influence the area per head group of the bilayers.
5.3.4 Radial distribution function
Radial distribution function (RDF) is a useful tool to describe the structure of a system. It
gives the value of local density of a particle in a shell at a distance r from the reference
molecule. We have plotted RDF for different concentrations of buffer molecules in order
to obtain better insight into probability distribution of water molecules around the lipid
bilayers through its coordination number. To calculate RDF from simulations, the
neighbours around each atom or molecule are sorted into bins. Finally the number of
neighbours in each bin is averaged over the entire simulation time.
We define the coordination number as the number of neighbours in its first hydration shell
and is obtained by integrating the RDFs curve up to its first minimum and is presented is
table 5.3.4. A slight decrease in the coordination number at higher concentrations of buffer
molecule is observed and this is consistent with the decrease in the HBs observed earlier
for the case of the HEPES molecules.
System
Number
of buffer
molecule
Coordination number
for
Lipid methyl groups
and water oxygen
Coordination number
for Lipid non
esterified oxygen and
water oxygen
DMPC + water
(reference) 0 7.5765 @ 4.65 2.2945 @ 3.25
DMPC + water +
HEPES 2 7.5555 @ 4.65 2.2936 @ 3.25
DMPC + water +
HEPES 10 7.4685 @ 4.65 2.2768 @ 3.25
DMPC + water +
MES 2 7.5420 @ 4.65 2.2846 @ 3.25
DMPC + water +
MES 8 7.5231 @ 4.65 2.2794 @3.25
DMPC + water +
PIPES 2 7.5700 @ 4.65 2.2878 @ 3.25
DMPC + water +
PIPES 8 7.4972 @ 4.65 2.2889 @ 3.25
Table 5.3.4: coordination number at different buffer concentrations
Chapter 6
Umbrella sampling
6.1 Introduction
Calculation of free energy differences is one of the most important thermodynamic
parameter which helps us in the thermodynamically most favourable states. It also helps
us to estimate reaction rates or free energy barriers for a given system. In a finite time
simulation it is generally impossible to sample all the possible configurations for a given
ensemble because of different energy barriers on the free energy landscape. Hence there
is a need for biased sampling where we can force the system at a specific reaction
coordinate in order to sample enough configurations which are necessary to get free energy
landscape at that reaction coordinate. In our study we have estimated the free energy
landscape for insertion of HEPES molecule by first keeping it in aqueous phase (state a)
and then bringing it inside the middle of the bilayer (state b). In the following discussion
we have presented a short description of umbrella sampling methods adopted from the
study [19].
In a canonical ensemble the free (Helmholtz) energy of a system is computed as:
𝐴 = −1
𝛽 ln(𝑄𝑁𝑉𝑇) (6.1)
Where
𝑄𝑁𝑉𝑇 =1
ℎ3𝑁𝑁!∬ exp [−𝛽𝐻(𝑥, 𝑝𝑥)] 𝑑𝑥 𝑑𝑝𝑥 (6.2)
Here 𝐻(𝑥, 𝑝𝑥), is the Hamiltonian of the system. 𝑥 and 𝑝𝑥 are 3N-dimentional vectors
containing the atomic coordinates and momenta of the particles in the system. ℎ is the
Planck constant. The probability to find the system in a particular microscopic
configuration 𝐻(𝑥, 𝑝𝑥) is defined as
𝑃(𝑥, 𝑝𝑥) =exp [−𝛽𝐻(𝑥, 𝑝𝑥)]
∬ exp [−𝛽𝐻(𝑥′, 𝑝′𝑥)] 𝑑𝑥′ 𝑑𝑝′𝑥
(6.3)
we are interested in a free energy difference between two states as function of reaction co-
ordinate which possible to obtain from biased simulations such as Umbrella sampling.
In Umbrella sampling a bias potential, an additional energy term is applied to the system
to ensure efficient sampling along the whole reaction coordinate. We are using harmonic
potential which allows the forces to vary according to the nature of interactions of HEPES
and DMPC lipid i.e. forces will build up until certain critical interactions are broken. The
functional form of harmonic biasing potential can be written as:
𝑤𝑖(𝑧) = (𝐾/2)(𝑧 − 𝑧𝑖)2 (6.4)
If 𝑈(𝑹, 𝑧) be the potential energy of the system as a function of position and reaction
coordinate then the biased potential energy of the system becomes:
𝑈𝑏(𝑹, 𝑧) = 𝑈𝑢(𝑹, 𝑧) + 𝑤𝑖(𝑧) (6.5)
Hence the unbiased probability distribution along z coordinate according to equation 6.3
will become
𝑃𝑢(𝑧𝑖) =∫ 𝛿(𝑧−𝑧𝑖)exp [−𝛽𝑈(𝑹,𝑧)]𝑑𝑧𝑑𝑹
∫ exp [−𝛽𝑈(𝑹,𝑧)]𝑑𝑧𝑑𝑹 (6.6)
Similarly, the biased probability distribution from equation 6.5 will become
𝑃𝑏(𝑧𝑖) =∫ 𝛿(𝑧 − 𝑧𝑖) exp [−𝛽𝑈(𝑹, 𝑧) + 𝑤𝑖(𝑧) ]𝑑𝑧𝑑𝑹
∫ exp [−𝛽𝑈(𝑹, 𝑧) + 𝑤𝑖(𝑧)]𝑑𝑧𝑑𝑹 (6.7)
Which leads to,
𝑃𝑢(𝑧𝑖) = 𝑃𝑏(𝑧𝑖) exp[𝛽𝑤𝑖(𝑧)] < exp[−𝛽𝑤𝑖(𝑧)] > (6.8)
Now the free energy as a function of reaction coordinate z can be defined as:
𝐴(𝑧𝑖) = −1
𝛽ln ∫ 𝛿(𝑧 − 𝑧𝑖) exp[−𝛽𝑈(𝑹, 𝑧)] 𝑑𝑧𝑑𝑹 (6.9)
From equation 6.6 and 6.7, we get
𝐴(𝑧𝑖) = − (1
𝛽) 𝑃𝑏(𝑧𝑖) − 𝑤𝑖(𝑧) + 𝐹𝑖 (6.10)
this can be obtain from MD simulations.
Here 𝐹𝑖 = − (1
𝛽) ln < exp[−𝛽𝑤𝑖(𝑧)] > (6.11)
6.2 Steps in Umbrella techniques
Generate a series of configuration along reaction coordinate using constant velocity
steered molecular dynamic simulation (cv-SMD)
Extract frames from trajectory generated above by dividing the reaction coordinate
into windows with desired COM spacing
Run umbrella sampling on in individual window by restraining the molecule within
window corresponding to desire COM distance
Estimate 𝑃𝑏(𝑧𝑖) for each simulation
Combine results from all simulations using Weighted Histogram Analysis Method
(WHAM)
6.3 Results and discussion
HEPES molecule is kept at a distance of 3.5 nm from the centre of mass distance
of DMPC lipid bilayer and the values of 𝑧𝑖 ranged from 3.5 to 0 nm with ∆𝑧𝑖 = 0.2
nm
However depending upon the overlap between windows we have to save
configurations more often, or sufficient to save configurations less often. The idea
is to get sufficient overlap between windows in the umbrella histograms to get
continuous energy profile.
During constant velocity Steered molecular dynamic simulation (cv-SMD) HEPES
molecule was moved with a pull rate of 0.01 nm per ps using a dummy atom that
is attached to the centre of mass of the HEPES via a virtual spring with a spring
constant k, of 1000 kJ mol-1nm-2
The dummy atom was moved at a constant velocity in the direction perpendicular
to the membrane plane (z- axis) with restrictions on x and y co-ordinates.
We are monitoring free energy change of HEPES molecule between two
thermodynamic states: one above membrane (state a) and one in the middle of
membrane (state b) with z-axis as a reaction coordinate.
In each window we simulated the system for 10 ns. The work done to pull the
nanotube across the lipid bilayer using the cv-SMD simulations was used to
calculate the potential of mean force .The PMF curves was generated after
combining all the results from each window using the weighted histogram analysis
method (WHAM).
At room temperature a molecule with N number of atoms will have 3N degrees of freedom.
For HEPES molecule with restrains along X and Y coordinates, it will have one
translational, three rotational (nonlinear molecule) and 95 vibrational (3N-4) degrees of
freedom. Rotational and translation degree of freedom contributes 0.5 RT of total energy
per molecule and RT of total energy per molecule for vibrational degree of freedom which
is occurring at temperature more than 5000C. Hence at room temperature HEPES molecule
has 2.0 RT of energy per molecule in order to access rotational and translational degrees
of freedom. In our special case even if we consider only one translational mode (along z-
direction) and ignore vibrational and rotational mode; HEPES molecule will have 0.308
Figure 6.3.3: a) free energy profile for insertion of HEPES from aqueous phase to lipid phase
b) average and standard deviation generated from the WHAM procedure [3]
∆𝐺𝑎→𝑏 = 15.74 𝑘𝑐𝑎𝑙𝑚𝑜𝑙−1
Aqueous phase
(HEPES+water) Lipid bilayers
Figure 6.3.3 Figure 6.3.3
𝑘𝑐𝑎𝑙 𝑚𝑜𝑙−1 of translational energy which is not sufficient to cross an energy barrier of
15.74 𝑘𝑐𝑎𝑙 𝑚𝑜𝑙−1 at temperature of 310 K. Hence we can confidently state that at
temperature of 310K it is not possible for HEPES molecule to insert inside the DMPC lipid
bilayer.
During the course of biased simulations, HEPES molecule is penetrating in the lipid bilayer
by creating a hydrophobic defect and exposing the hydrophobic membrane core to water.
HEPES insertion is accompanied by the breaking of Hydrogen bonds between lipid head
groups and water and between the lipid molecules themselves. When HEPES molecule was
placed in the middle of bilayer (state b), there is strong repulsion between hydrophobic
core and charged atom on HEPES molecule which give rise to highest energy in the PMF
curve.
Values on the PMF curve gets less and less negative as we move HEPES molecule from
state a to state b with its lowest value of 15.74 𝑘𝑐𝑎𝑙𝑚𝑜𝑙−1 at 2.5 nm from COM distance
of lipid. Finally a conclusion can be drawn that in order to penetrate HEPES molecule in
the middle of bilayer an energy barrier of 15.74 𝑘𝑐𝑎𝑙𝑚𝑜𝑙−1 has to be crossed and from the
above discussion, it is not feasible for HEPES molecule to be in state b.
Chapter 7
Conclusions and suggestions for future
work
7.1 Conclusions
Molecular dynamic simulations of DMPC lipid bilayers and buffer molecules are carried
out using GROMACS simulation package. Simulation results for a DMPC and water
system are verified with the experimentally reported values and found to be in good
agreement. Partial charges on buffer molecules are derived from ab-initio calculations at
the Hartree-Fock level of theory to account for the columbic interactions. Simulations of
DMPC lipid bilayers with buffers molecules shows a weak interactions of buffer molecules
toward lipid head groups. Similar results are observed for density distribution of buffer
molecules at different concentrations with maximum density near the lipid head groups.
We observed hydrogen bond formation between buffer molecule and lipid head groups
however area per lipid and bilayer thickness remains unaffected during simulation time.
Finally free energy profile of HEPES molecule along reaction coordinate (z-axis) are
obtained using umbrella sampling techniques. Results from the plots suggests that at
temperature of 310 K, energy possess by HEPES molecule is not sufficient to cross the
energy barrier of 15.74 𝑘𝑐𝑎𝑙𝑚𝑜𝑙−1. Thus it will remain in the aqueous phase with a
maximum HEPES density near the lipid head groups.
7.2 Future work
In future it is useful to incorporate salt mixtures along with buffer molecules to investigate
the effect on bilayer properties. Different lipids having net positive, negative and neutral
charge can be studied in presence of various buffer molecules to figure out extent of
coulomb interactions and its role in lipid bilayers properties such as bending rigidity,
bilayer swelling and phase transition.
References
1. Available from http: // www. rsc.org/ Education/ Teachers/ Resources/ cfb/
cells.htm;2015
2. Available from: http://free-stock-illustration. com/ phospholipids +structure
+properties ;2015
3. Shankar Kumar, D.B., Robert H. Swendsen, Peter A. K and John M. Rosenberg,
The Weighted Histogram Analysis Method for Free-Energy Calculations on
Biomolecules. I. The Method. Computational Chemistry, 1992. 13(8): p. 1011-
1021.
4. Brand, E.G., Molecular dynamic simulation of fluid lipid membrane, in KTH
Engineering Science. 2011, Royal Institute of Technology,Stockholm,Sweden. p.
103.
5. Available from: http://chemistry.elmhurst.edu/ ;2015
6. Fennell, E.D. and W. Hakan, The Colloidal Domain: Where Physics, Chemistry,
Biology, and Technology Meet. Second Edition ISBN: 978-0-471-24247-5 p. 672
7. Bouvrais, H., L. Duelund, and J.H. Ipsen, Buffers affect the bending rigidity of
model lipid membranes. Langmuir, 2014. 30(1): p. 13-6.
8. Daan Frenkel and Berend Smit, Understanding Molecular Simulation; From
Algorithms to Applications Second Edition. ISBN: 978-0-12-267351-1. 2002.
9. Erik Lindahl, D.v.d.S., Berk Hess. Available from: http://www.gromacs.org/.
10. Lyubartsev, P.A.; Available from: http:// people .su.se /~jjm/ Stockholm_Lipids
/Downloads.html.
11. Berk Hess, H.B., Herman J. C. Berendsen,Johannes G. E. M. Fraaije, LINCS: A
Linear Constraint Solver for Molecular Simulations. Computational Chemistry,
1997. 18: p. 1463-1472.
12. Pohle, W., et al., Lipid hydration: headgroup CH moieties are involved in water
binding. Biopolymers, 2004. 74(1‐2): p. 27-31.
13. Norbert Kučerkaa, M.-P.N., John Katsarasa, Fluid phase lipid areas and bilayer
thicknesses of commonly used phosphatidylcholines as a function of temperature.
Biochimica et Biophysica Acta (BBA) - Biomembranes, 2011. 1808(11): p. 2761-
2771.
14. Śledź, P., et al., An experimental charge density of HEPES. Acta Crystallographica
Section B: Structural Science, 2010. 66(4): p. 482-492.
15. Wang, J., et al., Development and testing of a general amber force field. J Comput
Chem, 2004. 25(9): p. 1157-74.
16. Carlos F. Lopez, S.O.N., and Michael L. Klein, Hydrogen Bonding Structure and
Dynamics of Water at the Dimyristoylphosphatidylcholine Lipid Bilayer Surface
from a Molecular Dynamics Simulation. Phys. Chem. B, 2004. 108: p. 6603-6610.
17. Taha, M., I. Khoiroh, and M.-J. Lee, Phase behavior and molecular dynamics
simulation studies of new aqueous two-phase separation systems induced by
HEPES buffer. The Journal of Physical Chemistry B, 2013. 117(2): p. 563-582.
18. Marta Pasenkiewicz-Gierula, Y.T., Hiroo Miyagawa, Kunihiro Kitamura, and
Akihiro Kusumi, Hydrogen Bonding of Water to Phosphatidylcholine in the
Membrane As Studied by a Molecular Dynamics Simulation: Location, Geometry,
and Lipid-Lipid Bridging via Hydrogen-Bonded Water. Phys. Chem, 1996. 101: p.
3677-3691.
19. Kastner, J., Umbrella sampling. Wiley Interdisciplinary Reviews: Computational
Molecular Science, 2011. 1(6): p. 932-942.
Appendix A
Input file for Gaussian charge calculation
%chk=charge.chk
#p hf/6-31g* geom=connectivity iop(6/33=2,6/42=17,6/41=10) pop=mk
Title Card Required
0 1
C 1.83718600 1.72023200 0.68732700
C 0.32581100 1.52051500 0.88957200
N -0.25971800 0.65354300 -0.19548300
C 0.53301800 0.77993200 -1.44947200
C 1.97236600 0.27769800 -1.24965500
N 2.40278800 0.49700200 0.13479200
H 2.03708400 2.60878700 0.05842300
H -0.21466600 2.47138700 0.87887100
H 0.01239100 0.22607100 -2.23353600
H 2.03745700 -0.79316100 -1.46305900
C -0.49095400 -0.78509600 0.22339000
C -1.80299900 -0.91701500 0.99534100
C 3.83994300 0.35727500 0.33257600
C 4.38040200 -1.00731800 -0.11400900
S -3.20120400 -0.27672900 -0.01544300
O -3.12646000 -1.05536300 -1.26985700
O -4.40923800 -0.38955600 0.80732800
O -2.74098800 1.17587300 -0.21443400
O 3.61329500 -2.10716000 0.34521500
H 3.55475100 -2.05139700 1.31179300
H 2.29584700 1.92050800 1.66083900
H 0.12292800 1.02696900 1.84121200
H 0.51205900 1.83886700 -1.72306600
H 2.61819000 0.80400200 -1.97842500
H 4.37570400 -1.08729400 -1.20526100
H 5.43281400 -1.07656400 0.20495000
H 4.03573800 0.48971400 1.40575100
H 4.42121100 1.14163100 -0.19449700
H -0.57276400 -1.36753700 -0.69702300
H 0.38303600 -1.12175200 0.78531400
H -1.99379400 -1.97337000 1.20163600
H -1.80041800 -0.37304500 1.94507200
H -1.30129200 1.02232600 -0.36349900
Appendix B
C.I.F. file for HEPES
##############################################################################
### ###
### Electronic paper (Acta Crystallographica Section E) ###
### ###
##############################################################################
# #
# This CIF contains the data in a paper accepted for publication in Acta #
# Crystallographica Section E. It conforms to the requirements of Notes #
# for Authors for Section E, and has been peer reviewed under the auspices #
# of the IUCr Commission on Journals. #
# #
# Full details of the Crystallographic Information File format #
# are given in the paper "The Crystallographic Information File (CIF): #
# a New Standard Archive File for Crystallography" by S. R. Hall, F. H. #
# Allen and I. D. Brown [Acta Cryst. (1991), A47, 655-685]. #
# #
# The current version of the core CIF dictionary is obtainable from #
# ftp://ftp.iucr.org/pub/cif_core.dic. The current version number is 2.4. #
# #
# Software is freely available for graphical display of the structure(s) in #
# this CIF. For information consult the CIF home page http://www.iucr.org/ #
# cif/home.html #
# #
# This file may be used for bona fide research purposes within the #
# scientific community so long as proper attribution is given to the journal #
# article from which it was obtained. #
# #
##############################################################################
data_I
_audit_creation_method
'HKL-3000SM automatic completion and interactive editing'
_audit_conform_dict_name cif_core.dic
_audit_conform_dict_version 2.3
_audit_block_code sm
_chemical_name_systematic
;
2-[4-(2-Hydroxyethyl)piperazin-1-ium-1-yl]ethanesulfonate
;
_chemical_name_common HEPES
_chemical_formula_moiety 'C8 H18 N2 O4 S1'
_chemical_formula_sum 'C8 H18 N2 O4 S1'
_chemical_formula_iupac 'C8 H18 N2 O4 S1' _chemical_formula_weight 238.31
_chemical_melting_point ?
_symmetry_cell_setting orthorhombic
;
_geom_special_details
; loop_
_geom_bond_atom_site_label_1
_geom_bond_atom_site_label_2
_geom_bond_site_symmetry_2
_geom_bond_distance
_geom_bond_publ_flag
S1 O1 . 1.4525(3) ? S1
O3 . 1.4532(2) ?
S1 O2 . 1.4771(2) ?
S1 C1 . 1.7874(3) ?
N2 C4 . 1.4719(3) ?
N2 C5 . 1.4724(3) ?
N2 C7 . 1.4736(3) ?
N1 C6 . 1.4971(3) ?
N1 C3 . 1.4984(3) ?
N1 C2 . 1.5008(3) ?
N1 H1N . 0.827(8) ?
O4 C8 . 1.4226(4) ?
O4 H1O4 . 0.848(10) ?
C1 C2 . 1.5239(4) ?
C1 H1A . 0.939(9) ?
C1 H1B . 0.950(8) ?
C5 C6 . 1.5162(3) ?
C5 H5A . 0.995(8) ?
C5 H5B . 0.963(8) ?
C3 C4 . 1.5190(3) ?
C3 H3B . 0.951(8) ?
C3 H3A . 0.949(8) ?
C6 H6A . 0.898(9) ?
C6 H6B . 0.987(8) ?
C4 H4B . 0.981(8) ?
C4 H4A . 0.988(8) ?
C2 H2A . 1.016(9) ? C2
H2B . 0.948(8) ?
C8 C7 . 1.5250(4) ?
C8 H8B . 0.946(9) ?
C8 H8A . 0.935(8) ?
C7 H7B . 0.988(8) ? C7
H7A . 1.037(7) ?
loop_
_geom_angle_atom_site_label_1
_geom_angle_atom_site_label_2
_geom_angle_atom_site_label_3
_geom_angle_site_symmetry_1
_geom_angle_site_symmetry_3
_geom_angle _geom_angle_publ_flag
O1 S1 O3 . . 114.856(17) ?
O1 S1 O2 . . 111.907(17) ?
O3 S1 O2 . . 111.966(15) ?
O1 S1 C1 . . 106.317(13) ?
O3 S1 C1 . . 105.650(15) ?
O2 S1 C1 . . 105.296(12) ?
C4 N2 C5 . . 108.376(18) ?
C4 N2 C7 . . 112.22(2) ?
C5 N2 C7 . . 108.719(19) ?
C6 N1 C3 . . 109.504(18) ?
C6 N1 C2 . . 113.10(2) ?
C3 N1 C2 . . 110.809(19) ?
C6 N1 H1N . . 109.3(5) ?
C3 N1 H1N . . 107.8(5) ?
C2 N1 H1N . . 106.1(5) ?
C8 O4 H1O4 . . 107.0(6) ?
C2 C1 S1 . . 110.620(17) ?
C2 C1 H1A . . 113.1(6) ?
S1 C1 H1A . . 106.9(6) ?
C2 C1 H1B . . 113.9(5) ? S1
C1 H1B . . 106.2(5) ?
H1A C1 H1B . . 105.5(8) ?
N2 C5 C6 . . 111.782(19) ?
N2 C5 H5A . . 110.8(4) ?
C6 C5 H5A . . 108.7(4) ?
N2 C5 H5B . . 109.5(5) ?
C6 C5 H5B . . 107.3(5) ?
H5A C5 H5B . . 108.7(7) ?
N1 C3 C4 . . 110.055(19) ?
N1 C3 H3B . . 104.6(5) ?
C4 C3 H3B . . 113.0(5) ?
N1 C3 H3A . . 107.7(4) ?
C4 C3 H3A . . 111.1(5) ?
H3B C3 H3A . . 110.1(7) ?
N1 C6 C5 . . 110.17(2) ?
N1 C6 H6A . . 107.9(6) ?
C5 C6 H6A . . 109.1(6) ?
N1 C6 H6B . . 105.6(4) ?
C5 C6 H6B . . 113.7(4) ?
H6A C6 H6B . . 110.1(7) ?
N2 C4 C3 . . 111.07(2) ?
N2 C4 H4B . . 107.2(5) ?
C3 C4 H4B . . 109.3(5) ?
N2 C4 H4A . . 111.4(4) ?
C3 C4 H4A . . 108.3(4) ?
H4B C4 H4A . . 109.5(6) ?
N1 C2 C1 . . 111.129(19) ?
N1 C2 H2A . . 107.6(5) ?
C1 C2 H2A . . 109.6(5) ? N1
C2 H2B . . 107.6(5) ?
C1 C2 H2B . . 112.4(5) ?
H2A C2 H2B . . 108.4(7) ?
O4 C8 C7 . . 114.27(2) ?
O4 C8 H8B . . 106.2(5) ?
C7 C8 H8B . . 111.5(5) ?
O4 C8 H8A . . 110.3(5) ?
C7 C8 H8A . . 108.4(5) ?
H8B C8 H8A . . 105.8(7) ?
N2 C7 C8 . . 114.71(2) ?
N2 C7 H7B . . 107.7(5) ?
C8 C7 H7B . . 110.3(5) ?
N2 C7 H7A . . 110.5(4) ?
C8 C7 H7A . . 110.7(4) ?
H7B C7 H7A . . 102.1(5) ? loop_
_geom_torsion_atom_site_label_1
_geom_torsion_atom_site_label_2
_geom_torsion_atom_site_label_3
_geom_torsion_atom_site_label_4
_geom_torsion_site_symmetry_1
_geom_torsion_site_symmetry_2
_geom_torsion_site_symmetry_3
_geom_torsion_site_symmetry_4
_geom_torsion
_geom_torsion_publ_flag
O1 S1 C1 C2 . . . . -59.26(2) ?
O3 S1 C1 C2 . . . . 178.27(2) ?
O2 S1 C1 C2 . . . . 59.63(2) ?
C4 N2 C5 C6 . . . . 59.21(3) ?
C7 N2 C5 C6 . . . . -178.55(2) ?
C6 N1 C3 C4 . . . . -56.75(3) ?
C2 N1 C3 C4 . . . . 177.80(2) ?
C3 N1 C6 C5 . . . . 55.97(3) ?
C2 N1 C6 C5 . . . . -179.911(19) ?
N2 C5 C6 N1 . . . . -58.33(3) ?
C5 N2 C4 C3 . . . . -59.66(2) ?
C7 N2 C4 C3 . . . . -179.726(19) ?
N1 C3 C4 N2 . . . . 59.63(3) ?
C6 N1 C2 C1 . . . . 62.57(3) ?
C3 N1 C2 C1 . . . . -174.03(2) ?
S1 C1 C2 N1 . . . . 159.105(18) ?
C4 N2 C7 C8 . . . . -68.69(3) ?
C5 N2 C7 C8 . . . . 171.44(2) ?
O4 C8 C7 N2 . . . . 76.07(3) ? loop_
;
University of Virginia
Department of Molecular Physiology & Biological Physics
1340 Jefferson Park Avenue
Charlottesville, VA 22908
USA
;
_publ_contact_author_email [email protected]
_publ_contact_author_fax +1-434-9821616
_publ_contact_author_phone +1-434-2430033
_publ_section_title
;
2-[4-(2-Hydroxyethyl)piperazin-1-ium-1-yl]ethanesulfonate at 100 K
; loop_
_publ_author_name
_publ_author_address
'Pawel Sledz'
;
University of Virginia
Department of Molecular Physiology & Biological Physics
1340 Jefferson Park Avenue
Charlottesville, VA 22908
USA
;
'Thomas Minor'
;
University of Virginia
Department of Molecular Physiology & Biological Physics
1340 Jefferson Park Avenue
Charlottesville, VA 22908
USA
;
'Maksymilian Chruszcz'
;
University of Virginia
Department of Molecular Physiology & Biological Physics
1340 Jefferson Park Avenue
Charlottesville, VA 22908,USA
Appendix C
.mdp file for pure DMPC in water simulation
title = Production run for DMPC in water
; Run parameters
integrator = md ; leap-frog integrator
nsteps = 5000 ; 2 * 500000 = 1000 ps
dt = 0.002
; Output control
; 2 fs
nstxout = 25000 ; save coordinates every 50.0 ps
nstvout = 25000 ; save velocities every 1.0 ps
nstenergy = 25000 ; save energies every 1.0 ps
nstlog = 25000 ; update log file every 1.0 ps
; Bond parameters continuation = yes ;
Restarting after NVT constraint_algorithm = lincs ;
holonomic constraints
constraints = all-bonds ; all bonds (even heavy atom-H bonds)
constrained
; Neighborsearching
cutoff-scheme = Verlet
ns_type = grid ; search neighboring grid cells
nstlist = 10 ; 20 fs, largely irrelevant with Verlet scheme
rcoulomb = 1.0 ; short-range electrostatic cutoff (in nm)
coulomb-modifier = Potential-shift-Verlet
vdwtype = Cut-off
rvdw = 1.0 ; short-range van der Waals cutoff (in nm)
vdw-modifier = Potential-shift-Verlet
; Electrostatics
coulombtype = PME ; Particle Mesh Ewald for long-range electrostatics
pme_order = 4 ; cubic interpolation
fourierspacing = 0.12 ; grid spacing for FFT
optimize-fft = yes table-extension = 1 ; Temperature coupling is on
tcoupl = Nose-Hoover ; modified Berendsen thermostat tc-grps
= DMPC MOL_SOL ; two coupling groups - more accurate tau_t = 0.1 0.1
; time constant, in ps ref_t = 310 310 ; reference temperature,
one for each group, in K
; Pressure coupling is on
pcoupl = Parrinello-Rahman ; Pressure coupling on in NPT
pcoupltype = semiisotropic ; uniform scaling of box vectors
tau_p = 10.0 10.0 ; time constant, in ps
ref_p = 1.013 1.013 ; reference pressure, in bar
compressibility = 4.5e-5 4.5e-5 ; isothermal compressibility
of water, bar^-1
; Periodic boundary conditions
pbc = xyz
; Dispersion correction
; 3-D PBC
DispCorr = EnerPres ;
Velocity generation
; account for cut-off vdW scheme
gen_vel = no ; Velocity generation is off
; COM motion removal
; These options remove motion of the bilayer relative to the
solvent/hepes nstcomm = 1
comm-mode = Linear comm-grps = DMPC MOL_SOL