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Unexpected Like-Charge Self-Assembly of a Biguanide-
based Antimicrobial Polyelectrolyte
Afroditi Maria Zaki, Alessandro Troisi and Paola Carbone*
School of Chemical Engineering and Analytical Science, University of Manchester, Oxford Road,
Manchester M13 9PL, UK.
Department of Chemistry and Centre for Scientific Computing, University of Warwick, Coventry CV4
7AL, UK.
AUTHOR INFORMATION
Corresponding Author: [email protected]
Abstract: Polyelectrolyte chains dissolved in good solvent are expected to collapse in compact
configurations in the presence of multivalent ions. Here, we show that a weakly charged, hydrophilic
polyelectrolyte containing biguanide groups self-assembles in water also in the presence of monovalent
counterions, even at low salt concentrations. The polymer assembles in a compact, ordered, hairpin-like
shape that, with increasing the ionic strength of the solution, can collapse further in three- or five-folded
structures. Neither water nor ions mediate the self-assembly which, instead, is driven by the like-charge
pairing of the biguanide units. The thermodynamics of the self-assembly show that the self-association
is enthalpically driven, isodesmic (at least at low aggregation number), and is favored by increasing salt
concentration. This unique self-assembly behavior may be linked to the well-known polymer’s
antimicrobial properties and could help in rationalizing its biological activity.
TOC GRAPHICS
Keywords: PHMB, Like-charge ion pairing, polyelectrolytes, folding, antibacterial
Polyelectrolytes (PEs) are macromolecules containing electrolyte groups that dissociate in aqueous
solutions and, releasing ions, make the polymer chain charged. Examples of such polymers include
synthetic and biological molecules (DNA or peptides) and their behavior is dominated by inter- and
intra-chain electrostatic interactions. Polyelectrolytes can assume a large variety of conformations as a
function of the solvent polarity, chain charge density and rigidity, salt concentration, temperature and
valency of the counterions.1-3 This rich conformational phase diagram is the result of the balance
between short range (Van der Waals) and long range (Coulomb) interactions between the polymer and
the counterions. Specifically, salt-induced polymer condensation is the transition from an extended
structure of the chain to a compact, ordered one that occurs upon addition of multivalent ions into the
solution. This effect is well known for DNA strands which despite being highly negatively charged,
show aggregation in the presence of multivalent ions,4, 5 but it is also common to other polyelectrolytes.6,
7 The degree of order of the compact structure depends on the degree of rigidity of the chain with toroid
or folded conformations shown by polymer with rigid or semi-flexible backbone.8 Counterion
condensation around the charged groups of the polymer backbone is often invoked to justify like-charge
aggregation and the majority of the theoretical derivations focus on the assembly of rigid highly charged
polyelectrolyte chains seen as proxy for DNA strands.9 While the inter- and intra-chain attraction
induced by multivalent ions is well documented experimentally,6, 10, 11 computationally12-14 and
theoretically,15, 16 more controversial is the effect that monovalent ions have on the chain association.9, 17-
21 Different mechanisms including depletion attractions, polymer entanglements or entropic effect of the
ions have been proposed to explain those experiments and simulations showing like-charge pairing in
presence of monovalent ions.9 In all cases, only in PEs characterized by high charge density (i.e. with a
Manning parameter ξ = λB)/b, where λB is the Bjerrum length, in water, at room temperature λB 0.7 nm,
and b is the distance between neighbouring charged monomers larger than 1)22 ion condensation, and
therefore like-charge attraction, is possible and with monovalent ions Tom et al.13 recently suggested
that ξ must exceed the value of 8 when the total charge of the monomer is 1.
In this paper we show, by means of atomistic molecular dynamics simulations, that the salt-induced
condensation can also occur in polyelectrolyte chains with low charge density (ξ 0.53) and in the
absence of multivalent ions if the monomer interactions allow for strong like-charge association. It is
important to notice here that amphiphilic polyelectrolytes (APEs)23 containing both hydrophilic and
hydrophobic blocks, constitute a different category of polymers as their self-assembly is driven by
unfavorable polymer-solvent interactions.
The polymer investigated here is polyhexamethylene biguanide (PHMB), a biguanide derivative
where each biguanide group along the chain is separated by six methyl groups (Figure 1). Such polymer
is known to possess antimicrobial activity against a wide variety of bacteria and is present in a large
group of formulated commercial products,24, 25 but the mechanism of its biocidal action is not known. In
what follows, we show that polymer chains containing biguanide groups self-assemble in ordered
compact structures even at low concentration of monovalent ions and -among other ordered
conformations- they predominantly form hairpin-like structures similar to that typical of biological
polyelectrolytes. Our simulation results are in agreement with recent dynamic light scattering
experiments showing that PHMB indeed aggregates in solution26, but propose a different self-assembly
mechanism than that of micelle formation. This aggregation behavior could be linked to the
antimicrobial activity that PHMB shows against a surprisingly wide variety of species27 and could
support a proposed recently alternative mechanism to its bactericidal properties that involves a direct
condensation with the bacterial chromosome28 rather than the most common and so far accepted
hypothesis that the polymer interacts only with the bacterial cell membrane.29
Figure 1. Chemical structure of one of the possible tautomers of a PHMB dimer.
Single chain structure and energetics. In all the simulations, the polyelectrolyte chains display a
counterintuitive behavior, as they self-assemble into ordered folded structures with the positively
charged groups facing each other. The collapse of the chains, described by the change in their radius of
gyration (Rg), occurs within a few nanoseconds after the beginning of the simulations (Figure 2). Within
few nanoseconds, the –initially extended– pentamer chain folds in a “hairpin-like” structure typical of
RNA30 or globular proteins31 and its Rg decreases from approximately 1.5 nm to 0.9 nm. The dodecamer,
can reach a similar configuration with a drop of its Rg from 2.7-3 nm to 2 nm (in agreement with the
only previous computational work reported in the literature32), but at high concentration of salt it can
further collapse reducing the Rg to around 1.0-1.6 nm with the chain forming a “three-folded” or even a
“five-folded” structure.
(a)
(b)
(c)
(d)
(a) (b)
(c) (d)
Figure 2. Top: Time evolution of the radius of gyration (Rg) of the pentamer (up) and the dodecamer
(down), at Cs = 225 mM (similar results are obtained at other salt concentrations see Figure S3). Bottom:
Selected folded and unfolded configurations of the chains.
The intra-chain (and we will see later inter-chain as well) association observed in the PHMB chain
can be related to the remarkable like-charge pairing properties demonstrated for free guanidinium ions
in previous experimental and computational studies.33-37 According to these studies, the association of
the like-charged cations stems from hydrophobic attraction which overcomes the electrostatic repulsion.
In particular, it was shown that hydrogen bonds are formed between the oxygen atoms of the water
molecules and the nitrogen atoms of the ions but not between the water and the carbon atoms (despite
their relative high charge) and therefore the cations (which have a planar symmetry) behave as
hydrophobic surfaces.35 In order to examine whether this is the case also in the present polymeric
system, the distribution of the hydrogen bonds (HBs) formed between water and the polymer chain was
investigated. To identify a HB, we used a geometrical criterion similar to that employed by Karimi et
al.38 which includes the distance between the water oxygen atom (acceptor) and a hydrogen of the
biguanide group (dH···O) and the value of the donor-hydrogen-acceptor planar angle (N−H∙∙∙O). This
calculation has been repeated for both the biguanide groups (Bgd+) in the unfolded chain and those
paired in a folded one to see whether the HBs’ arrangement is visibly affected by the intra-chain
association (Figure 3). The densely populated cluster of data points at short dH···O distance (smaller than
0.2 nm) and angles (ϕ) larger than 150˚ satisfies the typical requirements of HB formation,38 verifying
the presence of a HB network around the Bgd+ group of the polyelectrolyte and is in agreement with
similar geometrical values that have been found for the HBs formed by the guanidinium ions in aqueous
solution.35 The points in the plot that correspond to smaller angles and larger distances represent the
water molecules that are in the vicinity of the biguanide groups, but are not hydrogen-bonded to them.
The two plots of Figure 3a show that the structure of the hydrogen-bonded water molecules is not
affected by the folding of the chain since the two scattered plots are almost identical. Indeed, our
simulations show that neither water molecules nor ions are present between the paired cationic groups
and that the hydrogen-bonded water molecules are organized in the same plane of the biguanide groups
and therefore their arrangement is not affected by the folding. Figure 3b reports the distribution of the
cosine of the angle (ϕ) formed by the vectors connecting the centers of mass of two paired biguanide
groups with either the oxygen of the water molecules or a Cl- counterion. In the calculations only water
molecules and counterions closer than the distance corresponding to the second minimum of their RDFs
(0.52 nm for the water molecules and 0.56 nm for the Cl -, see Figure S4) to the center of mass of at least
one biguanide group (Bgd+CoM) are included. Figure 3c shows the dihedral angle distribution for the N-
C-N-C and the N-C-N-H backbone dihedrals of the biguanide, as well as the distribution of the C-N-
H···O dihedral angles for all the water molecules that form HBs with the Bgds+.
(a) (b) (c)
Figure 3. (a) the N-H∙∙∙O angles against the H∙∙∙O distance for all the water oxygen atoms. Calculations
performed on a folded (top) and an unfolded (bottom) dodecamer chain at Cs = 150 mM; (b)
distributions of the cosine of the angle (ϕ) calculated between the centers of mass of the paired
biguanides dBgd+
CoM and the oxygen atoms of the water molecules (solid black line) and the Cl- ions (red
dashed line), where dBgd+
CoM−Owater < 0.52 nm and dBgd+
CoM-Cl- < 0.56 nm, at Cs = 150 mM; (c) probability
distribution of the N-C-N-C and the N-C-N-H dihedral angles of the Bgd+ and the C-N-H···O dihedral
angles for all the hydrogen-bonded water molecules.
The plots show that the biguanide group is planar and that the highest probability of finding a water
molecule in its proximity is in the equatorial region (ϕ between 90˚ and 70˚) of the biguanide plane.
Calculating the number of HBs in both the folded and unfolded state for the pentamer and the
dodecamer chains (Table 1), we find that, on average, around 4.5 water molecules are hydrogen-bonded
to each biguanide group irrespectively to whether the chain is folded and to the salt concentration. This
indicates that not all the six hydrogen atoms of the Bgd+ form separate hydrogen bonds with the water.
Indeed as Figure 3b and 3c show, the counterions condense on the same plane occupied by the water
molecules and therefore compete with them to form a HB with the Bgd+ hydrogen atoms available (in
agreement with what has been observed for the guanidinium solutions35). It is important to note here that
the fact that the number of HB does not change upon folding implies that PHMB is soluble in water and
that the self-assembly is not driven by poor solubility (i.e. water is a good solvent at this temperature as
shown experimentally26).
The folding of the polyelectrolyte chain and the pairing of the biguanide groups is driven by the
“hydrophobicity” of the carbon surface of the biguanide groups, as the hydrophilic (i.e. carrying positive
partial charges) carbon atoms do not form hydrogen bonds with the water and therefore assume a
hydrophobic behavior (water cannot wet the molecule surface). Figure 4 shows how when the transition
from the extended to the folded state takes place (for example at 20 and 50 ns, see for the structural
changes at these times in Figure 2), as expected the polymer-polymer electrostatic energy component
increases of approximately 60 kJ·mol-1, but at the same time the Lennard-Jones (LJ) polymer-polymer
energy component decreases of around 180 kJ·mol-1. The plots of Figure 4 refer to the pentamer and the
dodecamer in a specific salt concentration (225 mM), but similar results are obtained for any other ion
concentration.
Table 1. Number of hydrogen bonds per Bgd+ calculated for the pentamer and the dodecamer
considering dHO 0.2 nm and ϕ 150˚ (see text). Values have been averaged over 3 ns and include
different folded structures.
Cs [mM] folded structure unfolded structurePentamer
0 4.9 0.5 5.2 0.575 4.6 0.4 5.0 0.4150 4.7 0.4 5.2 0.5225 4.2 0.4 4.9 0.5300 4.7 0.5 4.7 0.4
Dodecamer
0 4.5 0.6 4.0 0.775 4.6 0.6 4.2 0.7
150 4.0 0.6 4.2 0.7225 3.6 0.6 4.4 0.7300 4.1 0.6 4.8 0.7
A better understanding of the amount of energy gained per biguanide group during the folding can be
estimated using the simulations performed on the pentamer where, due to the short chain length, the
polymer folds only in hairpin-like structures. In this case, the chain contains only five biguanide groups
and only two like-charge pairings can be formed. Monitoring the short-range polymer-polymer LJ and
Coulomb interactions it is possible to observe the respective variations when the chain folds. The
folding reduces the LJ interactions by around 50-60 kJ·mol-1 and increases the electrostatic interactions
by around 12-19 kJ·mol-1. Since in the pentamer only two pairs can be formed and in the dodecamer six
are allowed, we can estimate that the gain in the LJ energy and the increase in the Coulomb one when
two biguanide groups pair are approximately −25 kJ·mol-1 and 10 kJ·mol-1, respectively.
Figure 4. Time evolution of the Lennard-Jones (upper panel) and the Coulomb (lower panel) energy
components for the polymer-polymer interaction calculated for the PHMB pentamer (left) and the
PHMB dodecamer (right) at Cs = 225 mM. In grey the instantaneous values saved every 20 ps, in red
(LJ) and cyan (Coulomb) the running averages with an average length of 150 data points.
Free energy of association. The effect of the ion concentration on the chain folding mechanism can be
quantified calculating the free energy of association (ΔG) of two separate dimers. The free energy
profile presented in Figure 5 shows that the ion concentration slightly increases the free energy barrier
for dissociation (see Table 2). This result agrees with the fact that at high ionic strength the chain can
fold in very compact shape and folding seems to be irreversible (in the time scale of our simulations). 39
Again when the oligomers are associated no water molecules or ions could be found in between the pair.
Table 2. Free energy of association, enthalpy (internal energy) and entropy (multiplied by the
temperature, 293 K) calculated for 1+1 PHMB dimers and for 2+1 PHMB dimers at different salt
concentrations.
Cs [mM] ΔG [kJˑmol-1] ΔH [kJˑmol-1] −¿TΔS [kJˑmol-1]Two dimers (1+1)
0 −¿4.9 0.5 −¿35.3 25.5 30.4150 −¿7.0 1.2 −¿36.3 25.4 29.3300 −¿8.2 1.1 −¿39.9 25.9 31.7
Three dimers (2+1)0 −¿5.0 0.9 −¿36.6 11.1 31.6
150 −¿5.9 0.9 −¿33.3 11.3 27.4300 −¿7.8 0.9 −¿36.3 11.3 28.5
Looking at the various interactions that contribute to the chains’ association (Figure S5), we notice
again that upon association the polymer-polymer Coulomb potential increases of an amount (+20
kJ·mol-1 ca.) that is almost independent of the ion concentration. Similar increase is shown by the LJ
potential calculated between the polymer and the water molecules. The polymer-polymer LJ potential
(−50 kJ·mol-1) together with the Coulomb one calculated between the polymer and counterions (−30
kJ·mol-1) are the interactions responsible for the drop in free energy when the chains associate. In
particular the latter contribution is higher for high ion concentrations. This indicates that an increase in
the ionic strength of the solution increases the number of counterions around the polymer and, screening
the polymer charge groups, favors chain association. This can be also observed from the calculation of
the chloride-carbon RDF that shows that ion condensation occurs at high ionic strength and that the
number of counterions condensing around the biguanide groups is higher in the folding state than in the
unfolded one (Figure S6 and S7). This latter observation shows also that, probably due to the
localization of the polymer charges, folding favors ion condensation.
Figure 5 also indicates that the chain association, at least at low aggregation number, is an isodesmic
process40 where the ΔG values, within their errors, show the same increment regardless of the number of
PHMB oligomers that associate. Calculating the enthalpy (ΔH) (assumed to be equal to the total internal
energy) and the entropy (ΔS) of association from the PMF profile, we see that the self-assembly
mechanism is enthalpically driven and that with increasing the ion concentration, while the (positive)
entropic contribution to the free energy does not change, the enthalpy increases. This is another feature
that differentiates the physics of association in these polyelectrolytes from multivalent-salt induced
condensation where upon association (and ion concentration) the entropy of water and ions increases.2, 41
0.5nm
2nm
0.25nm
2nm
Figure 5. Free energy of association (PMF) calculated for 1+1 PHMB dimers (top) and for 2+1 PHMB
dimers (bottom), at different ion concentrations.
Multiple chains association. Polyelectrolyte aggregates in 1:1 salt solutions have been reported
experimentally. In these studies, however, the ratio of assembled to non-assembled chains is very small
and the aggregates disappear in the presence of excess salt.42 The simulations performed on multiple-
chain systems here reveal simultaneous intra- and inter-chain association, which, contrary to what seen
in experiments with other PEs, is enhanced by high ionic strength, as this behavior is the most
predominant in the systems with Cs = 300 mM, with three out of four chains forming a cluster, in the
time scale of the simulation (Figure S8).
In summary, we have found that the very widely used and commercially available biocide PHMB is
the first example of loosely charged polyelectrolyte that self assembles in a good solvent in the presence
of monovalent ions. The self-assembly leads to ordered structures where the charged biguanide groups
almost face each other and which resemble the intermediate conformations shown by proteins in the
early stages of fibrils formation.31 The self-assembly is enthalpically driven and the underlying
mechanism appears to be isodesmic, indicating that large aggregates could be formed. The resulting
clusters become more stable at high salt concentrations and are soluble in water at least as much as the
unfolded chains (they present the same number of HBs and both Coulomb and Lennard-Jones polymer-
water energy components remain negative) and therefore phase separation should not occur upon
folding. This unique behavior is due to the experimentally known like-charge association of the
guanidinium in water solution and could provide a mechanistic explanation for the antibacterial activity
shown by PHMB against an unusual wide variety of bacteria. Indeed recent experimental data28 shows
that unlike other antimicrobial polycations that kill bacteria by disrupting their membrane after binding
to it, PHMB crosses the microbial (as well as mammalian) cellular membrane and condenses with the
bacterial chromosome. Since our simulations show that PHMB forms in water a compact, regular, stable
and water/ion impermeable nano-object we can hypothesize that its mechanism of interaction with the
lipid membrane is similar to that observed for positively charged nanoparticles or cell penetrating
peptides.43-45 Further simulations and experiments are needed to confirm this hypothesis. It is also worth
noting that it is not guaranteed that all the biguanide-based polymers show this peculiar behavior, as it is
possible that an optimal distance between the charged biguanide groups along the chain is needed to
allow for self-assembly. These results open up the possibility of using PHMB also for applications other
than antimicrobial solutions, such as structural materials or for nanopattering of surfaces.
Supporting Information
Computational details on the model employed for the polyelectrolyte and the simulations performed
as well as additional supporting figures.
Notes
The authors declare no competing financial interest.
Acknowledgements
The authors thank Professor Steve Yeates for providing the initial experimental data and Professor
Andrew Masters for useful discussion on the fundamental nature of the polyelectrolytes. We thank the
Computational Shared Facility (CSF) of the University of Manchester as well as the N8 HPC Centre of
Excellence, coordinated by the Universities of Leeds and Manchester for the computing time. This work
has been sponsored by the Leverhulme grant number RPG-2013-246.
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