Interaction of (-)-epigallocatechin gallate with silver nanoparticles
Goutam Kumar Chandra1, Debi Ranjan Tripathy2, Swagata Dasgupta2 and Anushree Roy1*
1Department of Physics, Indian Institute of Technology Kharagpur, 721302, India
2Department of Chemistry, Indian Institute of Technology Kharagpur, 721302, India
Interactions between silver nanoparticles and (-)-epigallocatechin gallate (EGCG) have
been investigated. Prior to the addition of EGCG molecules the silver particles are
stabilized by borate ions. Studies on the surface plasmon resonance band of silver
particles suggest that the EGCG molecules remove the borate ions from the surface of the
metal particles due to the chelating property of the ions. The complex formation by
EGCG and borate ions has been confirmed by NMR studies and pH titration. A possible
scheme of interaction between the two has been proposed.
Key words: Silver colloid, EGCG, UV-Vis, NMR
PACS codes: 87.64.k, 87.14.ej, 82.70.Dd, 68.43.Mn
Electronic mail: firstname.lastname@example.org
Polyphenols are natural substances, present in beverages obtained from plants,
fruits and vegetables, such as red wine and tea. The dominant and most important
catechin in green tea is (-)-Epigallocatechin gallate (EGCG), a potent antioxidant, which
has been reported to show anti-cancer activity and is presently under investigation in
clinical studies [1-3]. Silver ions (Ag+) and silver-based compounds are also known to
exhibit strong antimicrobial effects [4, 5]. The active ingredients in silver-based drugs are
“oligodynamic” silver ions . In medical literature, an interesting case-history reveals
the oncolytic role of Ag+ . This case history also reports the role of EGCG in anti-
cancer dietary therapy. However, Ag+ can have only limited usefulness as an
antimicrobial agent due to the interfering effects of their salts . Such adverse effects of
Ag+ can be avoided by using the corresponding metal nanoparticles. Use of silver (Ag)
nanoparticles is an efficient and reliable tool for improving the biocompatibility of Ag in
different biological processes. It is common knowledge that the biological activities of
several polyphenols are affected by transition metal ions [9-11]. With increased use of Ag
nanoparticles as drug carriers it would be interesting to investigate its interaction with
Silver colloids are prepared by using sodium borohydride (NaBH4) as a reducing
agent. Silver nitrate (AgNO3), sodium borohydride (NaBH4) of analytical reagent grade
(SRL, India), were used to prepare the silver sol. A colloidal silver solution was prepared
in deionized water following the method described by Creighton et al . In this
chemical route, AgNO3 is reduced by an excess amount of NaBH4. 2.2 mM AgNO3 was
added dropwise to 1 mM NaBH4 at 4oC. Vigorous stirring for 20 minutes was necessary
to stabilize the colloidal solution. Later, it was left at room temperature for approximately
1 hour till the solution became transparent yellow. EGCG was obtained from Sigma-
UV-Visible (UV-Vis) spectra were recorded using a spectrophotometer, Model
Lambda-45 (Make Perkin-Elmer). For optical absorption measurements the samples were
kept in a microcuvette with an optical pathlength of 1 cm. 1H NMR spectra were recorded
on a Bruker 400 MHz spectrometer at 22.5 ºC.
3. Results and Discussion
3.1 Formation of borate esters of EGCG
The pH of the Ag sol is measured to be 8.43, which remains constant during the
time course of the experiment. Just after addition of 0.5 mM of EGCG, the pH of
colloidal solution decreases to 7.72. As time progresses the pH of the solution gradually
decreases further. After 8 hrs the pH of the solution reaches a value ~ 7.30 and remains
constant with time as shown in Fig. 1. The acid dissociation constants of EGCG
molecules (inset of Fig. 1)  indicate that in a basic medium deprotonation of the
aromatic OH groups of the molecule occurs. The decrease in pH of the colloidal solution
after addition of EGCG, thus, indicates the release of H+ due to such an ad-molecule in
the sol. We believe that the pH of the solution decreases further due the formation of
borate esters of EGCG .
The complexation of EGCG with borate ion has been demonstrated by NMR
spectroscopic measurements. The 1H NMR spectrum of the gallate and pyrogallol moiety
of EGCG in D2O in water suppression mode are (δ6.883(s)2H) and (δ6.474(s)2H)
(shown in Fig. 2(a)). In presence of NaOH the 1H NMR spectrum of gallate and
pyrogallol moiety of EGCG in D2O in water suppression mode are (δ6.869(s)2H) and
(δ6.469(s)2H) (shown in Fig. 2(b)). However, in presence of NaBH4 the 1H NMR
spectrum of gallate and pyrogallol moiety of EGCG in D2O in water suppression mode
are (δ6.878(s) and δ6.748(s) 2H) and (δ6.467(S) and δ6.345(s) 2H) (shown in Fig. 2(c)).
Due to the formation of a chelate involving the ortho phenolic group with borate, there is
a split in the NMR spectrum along with broadening [15-16]. We have seen that two
protons show more shielding which is only possible if boron is tetra coordinated and with
a negative charge. Since the two aromatic protons of ring A are deuterated they do not
appear here. The possible path of the reaction of EGCG and borate ions is proposed in
3.2 Stability of metal colloids with EGCG in solution
Furthermore, studies on the surface plasmon resonance (SPR) band of the Ag
particle provide direct evidence of the interaction between Ag colloids and EGCG. The
SPR band of Ag colloids (shown in Fig. 3) appears at 397 nm. The measurements were
carried out immediately after direct addition of EGCG molecules (0.5 mM in the sol) in
the metal sol and subsequently at half hour intervals over a duration of 3 hrs. The broken
lines in Fig. 3 demonstrate the change in spectral profile of the plasmon band of Ag
colloids at different time intervals on addition of EGCG (for clarity, we have shown only
a few characteristic spectra taken just after mixing (0 hr), after 1 hr, 2 hrs and 3 hrs). We
observe (i) an increase in intensity of the absorption maximum and (ii) a red shift (by 8
nm) of the absorption maximum of plasmon band on addition of EGCG in the beginning,
which remains constant at a later time.
The nanosized particles possess a very large surface-to-volume ratio, and
consequently their properties are mostly governed by the surface states. It is well known
that the SPR band of Ag colloids in solution is strongly influenced by any chemical
modification of the surface, depending on whether the ad-molecule is nucleophilic and
therefore donates electron density into the particle surface (blue-shift of the SPR band),
or is electrophilic and withdraws electron density from the particle surface (red-shift of
the SPR band). In the present case, the Ag particles in the sol are stabilized by the anions
(borate ions). Thus the red-shift of the SPR band of the Ag colloids (shown in Fig. 3) by
addition of EGCG indicates a decrease of electron density (anions) from the colloidal
surface that indicates a desorption or removal of anions (borate ions) from the surface of
the metal particles.
As the Ag colloids in our experiments are suspended in an aqueous solution and
excess NaBH4 was used in the chemical synthesis, the following experiments were
performed to obtain a clearer view on the metal-molecule interaction. The absorption
band of an aqueous solution of EGCG appears at 275 nm (solid line in Fig. 4(a))
whereas, a double peak absorption band of 0.5 mM of EGCG in 1 mM NaBH4 (same
concentration as added during synthesis of Ag sol) solution appears at 279 nm and 316
nm (shown by dotted line in Fig. 4(a)). This feature of the absorption band of EGCG in
NaBH4 solution, most likely arises from the deprotonated EGCG molecule and the
corresponding borate esters of EGCG. The absorption spectra obtained on successive
addition of 0.5 mM aqueous solution of EGCG and NaBH4 solution of EGCG to Ag
colloids is given in Fig. 4(b) and Fig. 4(c), respectively. On addition of an aqueous
solution of EGCG to Ag colloids, the characteristic absorption band at 275 nm of EGCG
remains unchanged and another weak shoulder originating from the EGCG-borate
complex appears at a higher wavelength (indicated by an arrow in Fig. 4(b)). Initially we
observe an increase in intensity and a red shift of the plasmon band of the metal colloid
by ~ 8 nm. Subsequently, there is a further red shift of the plasmon band (as shown in
Fig. 4(b)) for the higher concentration of the added molecule. However, on addition of
NaBH4 solution of EGCG in Ag sol, along with the appearance of the characteristic
double peak structure of deprotonated EGCG and borate ester in the spectra, there is an
increase in intensity and red-shift by ~ 4 nm of the absorption maximum of plasmon band
of silver colloids (Fig. 4(c)). The relative shift of the plasmon band in above two cases
has been compared in Fig. 5. The smaller shift in plasmon band in Fig. 4(c) than what
was observed in Fig. 4(b) (shown by filled and open circles, respectively, in Fig. 5), can
be explained by the fact that in case of the aqueous solution of EGCG in Ag colloids, the
ad-molecules are free to strip off the borate ions present at the surface of the Ag colloids
and can form a complex. However, for EGCG dissolved in NaBH4 solution the molecules
are deprotonated and form a complex with borate ions (prior to addition to the colloidal
solution of Ag). Thus, the probability of the EGCG molecules to interact with the borate
ions present on the surface of the Ag colloids is lower in comparison to the previous case
where the interaction of EGCG occurs directly with the sol. The above results, once
again, indicate that EGCG molecules interact with the borate ions on the surface of Ag
3.3 Change in surface charge of Ag colloids in presence of EGCG
Next we estimate the change in surface charge and surface potential of Ag
colloidal particles due to the interaction with the EGCG molecules. The shift in the
wavelength of absorption maximum of the plasmon band before (λ0) and after (λ)
desorption of the anions from the particle surface is given by the equation ,
where [Ag] is the net silver concentration in the colloid (distributed in all particles of the
colloidal solution) and [anion] is the concentration of anions removed from the particle
surface. The spectral shift (λ-λ0) in Fig. 3 is 61 meV. Hence, we estimate the fractional
change in charge density upon desorption of anions from the surface of the Ag particles to
= 0.04, which is equivalent to ~ 0.5×10-4 M concentration of borate ions
(anion) in solution for [Ag]=1.2 ×10-3 M (used during sample preparation).
To estimate the change in surface potential of the Ag particles due to desorption
of anions from the surface by EGCG, we have studied the change in maximum
wavelength of the SPR band of Ag colloids with different concentrations of EGCG in the
solution (shown in Fig. 6). From the shift in the plasmon band and using the expression in
Eq. 1, we estimate the fractional change in charge density of metal particles with increase
in concentration of EGCG in solution. The change in surface potential arising from the
change in charge ∆q on the surface of particle of radius R as estimated using the
expression ∆V = ∆q/4πεR  is shown in inset of Fig. 6. It is clear that as we increase
the concentration of EGCG there is an initial increase in ∆V. At around 0.2 to 0.3 mM
concentration of EGCG, ∆V reaches a maximum value and then decreases with further
increase in the concentration of the ad-molecule. A possible explanation to the observed
change in surface potential of the Ag colloid on addition of EGCG is given. With
2 / 1
increase in concentration, as more EGCG molecules are available in the solution, higher
amounts of borate ions are removed from the surface of Ag colloids and thus, the surface
potential of the colloids increases as shown in Fig. 6. However, with further increase in
concentration of EGCG, the excess ad-molecules (after removing the negative ions layers
from the colloidal surface) or the complex start to interact directly with the surface of the
colloids (by neutralizing the particles) which decreases the surface potential of the
Spectroscopic measurements thus indicate that the added EGCG molecules are
capable of stripping off borate ions from the surface of the Ag colloidal particles in the
sol with the formation of borate esters. This study has far reaching implications in terms
of the usage of metal nanoparticles as drug carriers. Changes in chemical composition
and surface charge for such drug-nanoparticle combinations require further investigation
to be able to use them effectively and beneficially.
A. Roy and S. Dasgupta thank DRDO, India for financial assistance. D. R. Tripathy is
thankful to CSIR, India for a Junior Research Fellowship.
 S. Valcic, B. N. Timmermann, D. S. Alberts, G. A. Wächter, M. Krutzsch, J. Wymer,
J. M. Guillén, Anti-Cancer Drugs 7(4), 461 (1996).
 H. L. Gensler, B. N. Timmermann, S. Valcic, G. A. Wächter, R. Dorr, K. Dvorakova,
D. S. Alberts, Nutr. Cancer 26(3), 325 (1996).
 M. Barthelman, W. B. Bair III, K. K. Stickland, W. Chen, B. N. Timmermann, S.
Valcic, Z. Dong, G. T. Bowden, Carcinogenesis 19, 2201 (1998).
 F. Furno, K. S. Morley, B. Wong, B. L. Sharp, P. L. Arnold, S. M. Howdle et al., J
Antimicrob Chemother 54, 1019 (2004).
 S. Abuskhuna, J. Briody, M. McCann, M. Devereux, K. Kavanagh, J. B. Fontecha et
al., Polyhedron 23, 1249 (2004).
 Von Nageli C., Naturforsch Ges, Denkschriften der Schweiz. 33, 1 (1893).
 J. S. Kim, E. Kuk, K. N. Yu, J. H. Kim, S. J. Park, H. J. Lee, S. H. Kim, Y. K. Park,
Y. H. Park, C. Y. Hwang, Y. K. Kim, Y. S. Lee, D. H. Jeong, M. H. Cho, Nanomedicine
3, 95 (2007).
 S. A. Jovanovic, M. G. Simic, S. Steenken, Y. Hara, J. Chem. Soc., Perkin Trans. 2,
 A. Furukawa, S. Oikawa, M. Murata, Y. Hiraku, S. Kawanishi, Biochem.
Pharmacol. 66, 1769 (2003).
 S. Azam, N. Hadi, N. U. Khan, S. M. Hadi, Toxicol. Vitro 18, 55 (2004).
 J.A. Creighton, C.G. Blatchford, M. Grant Albrecht, J. Chem. Soc. Faraday Trans.
75, 790 (1979).
 M. Kumamoto, T. Sonda, K. Nagayama, M. Tabata, Biosci. Biotechnol. Biochem.
65(1), 126 (2001).
 J. Böesken, N. Vermaas, J. Phys. Chem. 35(5), 1477 (1931).
 J. Knoeck, J. K. Taylor, Analytical Chemistry 41(13), 1730 (1969).
 R. Pizer, P. J. Ricatto, Inorg. Chem. 33, 4985 (1994).
 A. Henglein, Chem. Mater. 10, 444 (1998).
 P. C. Hiemenz, in Principles of Colloid and Surface Chemistry edited Marcel
Dekker, Inc. New York (1986), p.746.
Figure 1. Change in pH of Ag colloids on addition of EGCG in the sol. Inset presnts the
structure of the EGCG molecule and the pKa value of two protons are shown.
Figure2. (a) 1H NMR spectrum of EGCG in D2O in water suppression mode. (b) 1H
NMR spectrum of EGCG and NaOH in D2O in water suppression mode, (c) 1H NMR
spectrum of EGCG and NaBH4 in D2O in water suppression mode.
Figure 3. Time dependent study of the plasmon band of Ag colloids on addition of
EGCG in the sol.
Figure 4. (a) The solid and dash lines represent the absorption spectra of EGCG in
aqueous solution and EGCG in NaBH4 solution respectively. (b) Titration of Ag colloids
with 0.5 mM EGCG in aqueous solution. (c) Titration of Ag colloids with 0.5 mM EGCG
in NaBH4 solution. The red arrows indicate the order of the spectra taken with increase
in volume ratio of EGCG.
Figure 5. Comparison between the relative shift of the plasmon band in case of aqueous
solution of EGCG (filled circles) and NaBH4 solution of EGCG (open circles) in Ag
Figure 6. Concentration dependent study of the plasmon band of Ag colloids on addition
of different concentration of EGCG in the Ag sol. Inset of the figure shows the change in
surface potential of the Ag colloids (∆V) with different concentration (C-EGCG) of
Scheme 1. Complex formation of EGCG with NaBH4.
0.02.5 5.07.5 24.0
pH of the solution
NaBH4 + H2O
Absorbance (Arb. units)
Absorbance (Arb. units)
200 300 400 500 600
Relative shift of plasmon band (nm)
Concentration of EGCG (mM)
Bare Ag colloids
0.02 mM EGCG
0.05 mM EGCG
0.1 mM EGCG
0.2 mM EGCG
0.3 mM EGCG
0.5 mM EGCG
0.6 mM EGCG
0.7 mM EGCG
Absorbance (Arb. units)
∆ ∆V (mV)