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Poly(o-anisidine) coatings on copper: synthesis, characterizationand evaluation of corrosion protection performance
Sonal Patila, S.R. Sainkarb, P.P. Patila,*
aDepartment of Physics, North Maharashtra University, P.O. Box 80, Jalgaon 425001, Maharashtra, IndiabNational Chemical Laboratory, Pune 411008, India
Received 7 March 2003; received in revised form 26 August 2003; accepted 6 October 2003
Abstract
The poly(o-anisidine) (POA) coatings were synthesized on copper (Cu) by electrochemical polymerization (ECP) of
o-anisidine (OA) and their corrosion protection performance in an aqueous solution of 3% NaCl was investigated by
potentiodynamic polarization technique. The ECP of OA was carried out under cyclic voltammetric conditions from an
aqueous solution of sodium oxalate to generate strongly adherent and smooth POA coatings on Cu substrates. These
coatings were characterized by cyclic voltammetry (CV), UV-vis absorption spectroscopy, Fourier transform infrared
(FTIR) spectroscopy, scanning electron microscopy (SEM) and X-ray diffraction (XRD) measurements. The optical
absorption spectroscopy study reveals the formation of the mixed phase of pernigraniline base (PB) and emeraldine salt
(ES) form of POA. The potentiodynamic polarization curves were used to evaluate the ability of the POA coatings to
protect the Cu surface. The potentiodynamic polarization curves show that the POA coating increases the corrosion
potential and drastically reduces the corrosion rate of copper. The corrosion rate of POA coated Cu is �100 times lower
than that observed for bare Cu.
# 2003 Elsevier B.V. All rights reserved.
Keywords: Corrosion-resistant coatings; Conducting polymer coatings; Poly(o-anisidine) coatings; Cyclic voltammetry; Copper
1. Introduction
Copper is widely used in microelectronics for
wiring, electromagnetic interference (EMI) shielding,
electrostatic dissipation, etc. Despite the fact that
copper is noble, it readily corrodes in a variety of
environments. Particularly, it is more susceptible to
the presence of chlorides, sulfur and applied fields [1].
It has been shown that the use of benzotriazole (BTA)
significantly improves the corrosion resistance of Cu
[2,3]. However, it is toxic and it does not provide the
corrosion protection at high potentials and elevated
temperatures. As a result, several attempts [4–8] have
been made to formulate new and environmently favor-
able polymeric coatings. Guenbour et al. [4] have
investigated the corrosion protection of Cu by poly-
aminophenol coatings synthesized by the ECP of
2-aminophenol from an alkaline hydroalcoholic
solution. Cieileo et al. [5] have shown that the oxime
compounds result in the formation of a polymeric
Cu(II) inhibitor complex which exhibits strong in-
hibition.
The use of conducting polymers as coating materi-
als for corrosion protection of metals/alloys has
Applied Surface Science 225 (2004) 204–216
* Corresponding author. Tel.: þ91-257-252187;
fax: þ91-257-252183.
E-mail address: [email protected] (P.P. Patil).
0169-4332/$ – see front matter # 2003 Elsevier B.V. All rights reserved.
doi:10.1016/j.apsusc.2003.10.050
become one of the most exciting new research fields
in most recent times [9–14]. A number of reports on
the use of conducting polymers for the corrosion
protection of metals have appeared in the literature
in the mid-1990s. In view of the ability of the con-
ducting polymer coatings to protect the metal surfaces,
there is a growing interest particularly during the
past 3–4 years to synthesize these coatings on iron,
aluminum and their alloys and to evaluate the corro-
sion protection offered by them [9–16]. However,
only few studies [17] have been carried out on the
corrosion protection of copper by conducting polymer
coatings inspite of its use in wide range of technolo-
gical applications. In most of these studies, the con-
ducting polymers were first synthesized chemically
and then deposited on the metal surface. Brusic et al.
[17] have deposited the films of polyaniline and its
derivatives on Cu by spin coating technique and
studied the corrosion protection properties as a func-
tion of the applied potential and temperature. It was
observed that these films could either provide signifi-
cant corrosion to Cu exposed to water or enhance the
corrosion rate. They found that the chemical nature of
the polymer backbone, oxidation state and the extent
and nature of polymer doping significantly affects the
corrosion protection properties.
In the studies reported in this paper, we have
synthesized the POA coatings on Cu substrates by
ECP of OA and examined the ability of these coatings
to serve as protective coatings against the corrosion of
Cu. The objectives of the present study are (i) to
synthesize strongly adherent POA coatings on Cu
substrates; (ii) to investigate suitability of aqueous
sodium oxalate medium for the ECP of OA on Cu
substrates; (iii) to identify the oxidation state of POA
synthesized from sodium oxalate medium on Cu
substrates and (iv) to examine the possibility of using
a substituted derivative, POA for corrosion protection
of Cu.
The choice of OA monomer is due to the following
reasons: (a) The incorporation of the substituents in
the polymer skeleton is a common technique to
synthesize polymers having improved properties.
The OA is a substituted derivative of aniline with
methoxy (–OCH3) group substituted at ortho-position.
This study therefore explores the possibility of utiliz-
ing the POA as alternative to polyanilines for corro-
sion protection of Cu. (b) The monomer OA is
commercially available at low cost. (c) The conversion
of monomer to polymer is straightforward. (d) More
recently, our group [18,19] has investigated the ECP
of OA on low carbon steel substrates from aqueous
solution of oxalic acid. (e) Hardly any attempt
has been made to synthesize the POA coatings on
Cu substrates. In this work, cyclic voltammetry (CV)
is used to synthesize the POA coatings on Cu sub-
strates. These coatings were characterized by CV,
FTIR spectroscopy, UV-Vis absorption spectroscopy,
SEM and XRD measurements. The extent of corrosion
protection offered by these coatings to Cu in aqueous
solution of 3% NaCl was examined by the potentio-
dynamic polarization measurements and CV.
2. Experimental
Analytical reagents (AR) grade chemicals were
used throughout the present study. The OA monomer
was double distilled prior to its use. The aqueous
solution of sodium oxalate (C2O4Na2) was used as
the supporting electrolyte. The concentrations of
sodium oxalate and OA were kept constant at 0.2
and 0.1 M, respectively.
The Cu (99.98% purity) substrates (size �1 cm�1:5 cm and 0.5 mm thick) were cut from a piece of Cu
plate. The substrates were polished with a series of
emery papers, followed by thorough rinsing in acetone
and double distilled water and dried in air. Prior to any
experiment, the substrates were treated as described
and freshly used with no further storage.
The POA coatings were synthesized by ECP of OA
on Cu substrates under cyclic voltammetric condi-
tions. The ECP was carried out in a single compart-
ment three electrode cell with Cu as working
electrode (1.5 cm2), platinum as counter electrode
and saturated calomel electrode (SCE) as refer-
ence electrode. The cyclic voltammetric conditions
were maintained using a SI 1280B solartron electro-
chemical measurement system (UK) controlled by
corrosion software (CorrWare, Electrochemistry/
Corrosion Software, Scribner Associates Inc. sup-
plied by Solartron, UK). The synthesis was carried
out by cycling continuously the electrode potential
between �500 and 1500 mV at a potential scan rate
of 20 mV/s. The number of cycles was varied from 5
to 25. After deposition the working electrode was
S. Patil et al. / Applied Surface Science 225 (2004) 204–216 205
removed from the electrolyte and rinsed with double
distilled water and dried in air.
The corrosion protection performance of these coat-
ings was evaluated at room temperature in aqueous
solution of 3% NaCl having pH 6.23 by using elec-
trochemical techniques. The electrochemical techni-
ques include CV and potentiodynamic polarization
experiments. For these measurements, a Teflon holder
was used to encased the POA coated Cu substrates so
as to leave an area of 0.4 cm2 exposed to the solution.
The ability of the POA coating to protect the Cu
against dissolution was studied by recording the cyclic
voltammograms in an aqueous solution of 0.2 M
sodium oxalate in the potential range between �500
and 1500 mV at a scan rate of 20 mV/s. Before
polarization the substrates were immersed into the
solution and the open circuit potential (OCP) was
monitored until a constant value was reached. The
polarization resistance measurements were performed
by sweeping the potential between �250 and 250 mV
from OCP at the scan rate of 2 mV/s. All the measure-
ments were repeated at least four times and good
reproducibility of the results was observed. The corro-
sion potential (Ecorr) and corrosion current density
(Icorr) were obtained from the slopes of linear polar-
ization curves. The corrosion rate (CR) was calculated
by using the following expression:
CR ðmm=yearÞ ¼ 3:268 � 103 IcorrEW
r
where Icorr is the corrosion current density (A/cm2),
EW the equivalent weight of copper (g) and r the
density of Cu (g/cm3).
The FTIR transmission spectra of POA coating
were recorded in horizontally attenuated total reflec-
tance (HATR) mode in the spectral range 4000–
400 cm�1 using a Perkin-Elmer spectrometer, 1600
Series II, USA. The optical absorption studies of these
coatings were carried out ex situ at room temperature
in the wavelength range 300–1100 nm using micro-
processor controlled double beam UV-Vis spectro-
photometer (Hitachi, Model U 2000). The structural
properties were investigated using XRD technique.
The X-ray diffractograms were recorded with a
Rigaku diffractometer (Miniflex Model, Rigaku,
Japan) having Cu Ka (l ¼ 1:542 A). SEM was
employed to characterize the surface morphology with
a Leica Cambridge 440 Microscope (UK).
3. Results and discussion
3.1. Electrochemical behavior of Cu in an aqueous
solution of sodium oxalate
The Cu electrodes were first polarized under cyclic
voltammetric conditions in 0.2 M sodium oxalate
solution in order to understand the different processes
that occur at the electrode surface. The first, second
and 10th scans of cyclic voltammogram of the Cu
electrode polarized in a 0.2 M sodium oxalate solution
are shown in Fig. 1. The first positive cycle (Fig. 1a)
shows an increase in the anodic current density from
��177 mV which indicates that dissolution of Cu
Fig. 1. Cyclic voltammogram scans (a) first, (b) second and (c)
10th recorded during the polarization of Cu electrode in 0.2 M
sodium oxalate solution. Scan rate: 20 mV/s.
206 S. Patil et al. / Applied Surface Science 225 (2004) 204–216
begins at this potential. On polarizing further in the
anodic direction, a broad anodic peak (A) at �190 mV
is observed, which is attributed to the more intense
dissolution of Cu. As can be seen, the anodic current
density again increases between �531 and 739 mV
and beyond 750 mV it remains almost constant. Dur-
ing the negative cycle, the high value of the anodic
current reveals that the dissolution initiated during
positive cycle continues until the electrode potential
reduced to low values in the region of 0 mV. Thus, in
the potential range �177 to 500 mV, the Cu electrode
is active and undergoes anodic dissolution which
produces Cu2þ ions in its vicinity. These ions interact
with the oxalate electrolyte to form insoluble copper
oxalate, which adheres to the electrode surface thereby
forming a copper oxalate interphase. This interphase is
perhaps produced according to the following two
reactions:
Cu ! Cu2þ þ 2e�
Cu2þ þ ðC2O4Þ2� þ H2O ! CuC2O4 H2O
On repetitive cycling, the anodic peak A is still
observed. In addition to this, a new peak at
��100 mV is seen, which is assigned to the formation
of copper oxide. It is clearly seen that the position of
peak A is shifted in anodic direction and the current
density corresponding to this peak decreases gradually
with the number of scans. These observations suggest
stabilization of the Cu electrode as a result of the
formation of CuC2O4H2O on the electrode surface.
Thus, the anodic peak A is attributed to passivation
of the Cu electrode surface in the sodium oxalate
medium via the formation of CuC2O4H2O interphase.
This interphase appears to be sufficiently protective to
decrease the rate of Cu dissolution.
In order to justify the formation of CuC2O4H2O
interphase, we have performed the XRD studies on the
Cu electrode polarized in 0.2 M sodium oxalate solu-
tion. The XRD results of bare and polarized Cu
electrode (after 10 scans) are shown in Fig. 2. The
XRD pattern of bare Cu electrode (Fig. 2a) shows the
presence of diffraction peaks at 2y values of 43.48,50.68, 74.28, 89.88 and 95.08 corresponding to the Cu
substrate. The XRD pattern of polarized Cu electrode
(Fig. 2b) exhibits significant changes with respect to
the bare Cu. Apart from the characteristic peaks of Cu,
the XRD pattern indicates the presence of diffraction
Fig. 2. XRD pattern of (a) bare Cu, (b) polarized Cu substrate and (c) POA coated Cu. The (*) and (~) indicate the diffraction peaks due to
CuC2O4H2O and Cu2O, respectively.
S. Patil et al. / Applied Surface Science 225 (2004) 204–216 207
peaks at 2y values of 24.88, 36.28, 37.08, 41.88, 45.48,49.08 and 54.88 corresponding to CuC2O4H2O phase.
In addition, it also shows the diffraction peaks at 2yvalues of 30.28, 41.88 and 74.28 corresponding to
Cu2O.
Thus, the CVand XRD results clearly reveal that the
polarization of the Cu electrode in an aqueous solution
of sodium oxalate leads to the formation of the inter-
phase which mainly comprised of polycrystalline
CuC2O4H2O.
The SEM micrograph of the copper electrode polar-
ized in a 0.2 M sodium oxalate solution is shown in
Fig. 3. It indicates relatively uniform coverage and
formation of needle shaped crystals at the surface of
copper electrode.
3.2. Electrochemical polymerization of OA on Cu
from an aqueous solution of sodium oxalate
The first, second and 10th scans of the cyclic
voltammogram recorded during the ECP of OA on
the Cu electrode from 0.2 M sodium oxalate solution
are shown in Fig. 4. The main features of the first scan
(Fig. 4a) are not affected by the presence of OA
monomer. The anodic peak A with an emergence of
shoulders at �460 and 676 mV is observed. As dis-
cussed earlier, the peak A corresponds to the dissolu-
tion of the Cu electrode. The visual observation of the
working electrode during the first positive cycle shows
that the color of the Cu surface slowly changes to dark
black from the potential �500 mV. This observation
implies that the deposition of the POA begins during
the first positive cycle. Therefore, the emergence of
the shoulders at �460 and 676 mVare attributed to the
oxidation of OA monomer and thus its actual poly-
merization. The deposition of a thin layer of polymer
coating during the first cycle may be responsible for
the protection of Cu against dissolution and hence
negligibly small anodic current densities are observed
at high potentials (>797 mV) and during the reverse
cycle.
During the next scan, the broad anodic peak (A0) is
observed and rest of the features are similar to that of
the first scan. The peak A0 is centered at �453 mVand
it is significantly different from that observed in the
first scan. As the deposition of the POA coating begins
during the first positive cycle, the peak A0 may be
attributed to the polymerization process rather than to
the dissolution of Cu. On repetitive cycling, the vol-
tammograms identical to that of second scan are
obtained. However, the current density corresponding
to the peak A0 decreases gradually with the number
of scans.
The observation of negligibly small anodic current
densities at all potentials in the 10th scan suggests
the formation of electroinactive POA coating.
Fig. 3. SEM micrograph of interphase formed during the polarization of Cu substrate in 0.2 M sodium oxalate solution.
208 S. Patil et al. / Applied Surface Science 225 (2004) 204–216
The visualization of the Cu electrode after 10th scan
reveals the formation of a dark black colored POA
coating. The coating is uniform, compact and strongly
adherent.
The FTIR spectrum of POA coating synthesized on
Cu under cyclic voltammetric conditions (5 cycles)
recorded in HATR mode is shown in Fig. 5. This
spectrum exhibits the following spectral features: (i)
a broad and weak band centered at �3324 cm�1 due to
the characteristic N–H stretching vibration suggests
the presence of –NH– groups in OA units [20,21]. (ii)
The band at �1600 cm�1 is an indicative of stretching
vibrations in quinoid (Q) rings [20,23].
(iii) The band �1510 cm�1 represents the stretching
vibrations of the benzoid (B) rings [20–23].
(iv) The presence of Q and B bands clearly show that the
POA coating is composed of amine and imine units. It is
known that the ideal form of PANI contains roughly
equal amounts of Q and B units. The relative intensity
(1600/1510) of these bands is greater than unity. There-
fore, it can be concluded that the formation of perni-
graniline base (PB) is predominant in the coating. (v)
The bands at 1265 and 1658 cm�1 are attributed to
the presence of carboxyl groups of sodium oxalate in
the POA coating [24]. (vi) The bands at 1120 and
1031 cm�1 are attributed to the 1–4 substitution on
the benzene ring. (vii) The band at �1386 cm�1 is due
to the stretching of N–N bands. The presence of this
band indicates the formation of POA coating via head to
head coupling. (viii) The band at �1174 cm�1 is con-
sidered as a measure of the degree of delocalization of
Fig. 4. Cyclic voltammogram scans (a) first, (b) second and (c)
10th recorded during the synthesis of POA coating on Cu substrate
under cyclic voltammetric conditions. Scan rate: 20 mV/s.
Fig. 5. FTIR spectrum of the POA coating synthesized on Cu
substrate under cyclic voltammetric conditions. Scan rate: 20 mV/s.
S. Patil et al. / Applied Surface Science 225 (2004) 204–216 209
electrons on POA and is referred to as the electronic-
like band. It is a characteristic peak of emeraldine salt
(ES) phase of POA [22–25]. The presence of this band
suggests the formation of ES phase of POA in the
coating along with the PB. (ix) The weak band at
�1454 cm�1 is assigned to the C–N stretching vibra-
tions in quinoid imine units. (x) The non-observance of
the bands around 900 and 800–700 cm�1 reveals that
1,2- and 1,3-substitutions do not occur to a significant
extent, although the deposition of POA takes place at a
relatively high potential [25]. Thus, the FTIR spectro-
scopic study reveals that the ECP of OA has occurred
and results into the deposition of POA coating on the
Cu electrode surface.
It is surprising to observe that the XRD pattern of
the POA coated Cu (Fig. 2c) exhibits the diffraction
peaks corresponding to Cu. It does not show the
diffraction peaks corresponding to copper oxalate
interphase. Also, as the POA coating has a highly
disordered structure, it does not indicate any diffrac-
tion peak. Thus, the XRD result reveals that the copper
oxalate intephase does not exit at the electrode surface
which supports the FTIR spectroscopic study.
The optical absorption spectrum of POA coating
(Fig. 6) shows a broad peak at about 560 nm and a
shoulder at about 720 nm. The peak at 560 nm is
attributed to the presence of PB phase of POA. The
PB is the fully oxidized form of POA and is insulating
in nature [26]. The shoulder at �720 nm is a signature
of the ES phase of POA, which is the only electrically
conducting phase of POA [26]. The simultaneous
appearance of 540 nm peak and a shoulder at
Fig. 6. Optical absorption spectrum of POA coating in DMSO solution.
210 S. Patil et al. / Applied Surface Science 225 (2004) 204–216
800 nm clearly reveals the formation of mixed phase
of PB and ES phase of POA. Thus, the optical absorp-
tion spectroscopy results are in well agreement with
the CV and FTIR spectroscopy results.
The SEM micrograph of the POA coating synthe-
sized on Cu is shown in Fig. 7. It clearly reveals that
the POA coating is relatively homogeneous, compact
and featureless. Moreover, it does not indicate the
presence of the copper oxalate crystals on the elec-
trode surface which is in agreement with the XRD
result. The quality of the coating is so excellent that no
crack or detachment of the coating is observed. The
formation of the homogeneous and crack-free coating
is attributed to the presence of the Cu2þ ions in the
vicinity of the electrode during the ECP of OA [27,28].
The XRD and SEM (cf. Figs. 2c and 7) results
clearly reveal that the copper oxalate interphase does
not exist at the electrode surface. Therefore, it may be
thought that the copper oxalate formed during the
early stages of the growth decomposes into soluble
species and diffuses into the electrolyte and the ECP
of OA occurs on the Cu substrate from where it was
decomposed. As a consequence, the Cu substrate
surface still remains in the passive state. It seems
that the decomposition of the interphase generates a
suitable surface for the deposition of the POA.
Very recently, a similar process has been reported
by our group [18,19] for the synthesis of POA coatings
on low carbon steel (LCS) substrates from the aqueous
solution of oxalic acid. It has been shown that the
formation of the passive iron oxalate interphase and its
subsequent decomposition is necessary for the ECP of
OA to occur on the LCS substrates. By analogy with
this, it may be argued that the copper oxalate inter-
phase formed during early stages decomposes and
facilitates the ECP of OA on Cu.
3.3. Measurement of porosity in POA coatings
The coating porosity is one of the important para-
meters, which strongly governs the anti-corrosive
behavior of the coatings. Therefore, measurement of
the coating porosity is essential in order to estimate the
overall corrosion resistance of the coated substrate.
In this work, the porosity in POA coatings on Cu
substrates was determined from potentiodynamic
polarization resistance measurements [29]. The poten-
tiodynamic polarization curves for bare Cu, copper
oxalate coated on Cu (polarized Cu substrate in 0.2 M
sodium oxalate in the potential range between �500
and 1500 mV at a scan rate of 20 mV/s) and POA
coated on Cu in aqueous solution of 3% NaCl are
shown in Fig. 8. The values of the corrosion potential
(Ecorr), corrosion current density (Icorr), Tafel con-
stants (ba and bc), polarization resistance (Rp) and
corrosion rate obtained from these curves are given in
Fig. 7. SEM of POA coating synthesized on Cu substrate under cyclic voltammetric conditions (10 cycles, scan rate: 20 mV/s).
S. Patil et al. / Applied Surface Science 225 (2004) 204–216 211
Table 1. The porosity in POA coating was calculated
using the relation [29]
P ¼ Rps
Rp
� �10ð�jDEcorrj=baÞ
where P is the total porosity, Rps the polarization
resistance of the bare Cu, Rp the measured polarization
resistance of coated Cu, DEcorr the difference between
corrosion potentials and ba the anodic Tafel slope for
bare Cu substrate. The porosity in POA coating (15
cycles) was found to be �0.23%.
In order to investigate the influence of the coating
thickness on the porosity and corrosion protection
properties of the POA coatings, we have synthesized
the coatings by 5, 10, 15 and 20 cycles from �500 to
1500 mV at a scan rate of 20 mV/s and the potentio-
dynamic polarization resistance measurements were
performed in an aqueous solution of 3% NaCl. As can
be seen from Table 1, the porosity in coatings does not
change significantly when the deposition time (i.e., the
number of cycles) is varied. This suggests that the
thickness of the POA coating may not significantly
influence the porosity in the coating. The lower values
of the porosity in POA coatings permit an improve-
ment of the corrosion resistance by hindering the
access of the electrolyte to the Cu substrates.
Fig. 8. Potentiodynamic polarization curves for (a) bare Cu, (b) copper oxalate coated on Cu and (c) POA coated on Cu in aqueous solution of
3% NaCl.
Table 1
Potentiodynamic polarization resistance measurement results
Sample Ecorr (mV) Icorr (mA/cm2) ba (mV/dec) bc (mV/dec) Rp (O/cm2) CR (mm/year) P (%)
Bare Cu �234 24.06 72.0 110.0 784.05 0.28 –
Cu oxalate coated on Cu �182 69.50 85.0 130.0 321.10 0.80 –
POA 5 cycles �174 00.52 54.0 340.0 38911.60 0.006 0.29
POA 10 cycles �177 0.56 48.0 160.0 28537.19 0.006 0.44
POA 15 cycles �183 0.26 50.0 180.0 65583.99 0.003 0.23
POA 25 cycles �187 0.41 54.0 210.0 45311.65 0.004 0.38
212 S. Patil et al. / Applied Surface Science 225 (2004) 204–216
3.4. Corrosion protection performance of the
POA coating
The potentiodynamic polarization curve (Fig. 8a)
for bare Cu is consistent with dissolution of Cu with
corrosion potential (Ecorr) close to ��234 mV and
high anodic current (>1 mA/cm2) is observed at poten-
tials higher than �125 mV. The broad anodic peak
observed at �125 mV is probably associated with the
formation of copper chloride complexes. It is reported
[30] that in chloride media (<1 M) the formation of
cuprous chloride species is dominant and the electro-
dissolution of Cu is represented by the two step
reaction:
Cu þ Cl� ¼ CuCl þ e�
CuCl þ Cl� ¼ CuCl2�
In order to support this, we have carried out the
XRD measurements on Cu after the potentiodynamic
polarization measurements and the corresponding
XRD pattern is shown in Fig. 9. Apart from the
characteristic diffraction peaks of Cu, the XRD pattern
indicates the presence of diffraction peaks at 2y values
of 23.48, 29.08 32.08 and 38.68 due to the CuCl2. The
CuCl2 is brown yellowish in color and hence the broad
anodic peak may be attributed to the formation of
CuCl2 during potentiodynamic polarization measure-
ments. The visual observation of the electrode surface
after the potentiodynamic polarization measurements
shows that the Cu surface is covered with a layer of
brown yellowish colored coating.
The SEM micrograph of the POA coating after the
potentiodynamic polarization measurements in an
aqueous solution of 3% NaCl is shown in Fig. 10.
It exhibits relatively uniform coverage and the overall
texture is ‘pumice-like’.
The potentiodynamic polarization curve for copper
oxalate coated Cu is shown in Fig. 8b. Although the
Ecorr is shifted in the positive direction until �183 mV,
the Icorr is higher than that observed for bare Cu. This
observation reveals that the copper oxalate coating
provides poor corrosion protection to Cu.
The potentiodynamic polarization curve for POA
coated Cu (15 cycles) is shown in Fig. 8c. It is clearly
observed that the corrosion current density (Icorr)
decreases from 25 mA/cm2 for bare Cu to 0.26 mA/
cm2 for POA coated Cu. The Ecorr increases from
�234 mV for bare Cu to �183 mV for POA coated
Cu. The positive shift of 51 mV in Ecorr indicates the
protection of the Cu surface by the POA coating. The
corrosion rate of Cu is significantly reduced as a result
of the reduction in the Icorr. The corrosion rate of Cu is
found to be �0.003 mm/year which is �100 times
lower than that observed for bare Cu. These results
reveal that the POA acts as a protective layer on Cu and
improves the overall corrosion performance.
It is found that the corrosion rate does not change
significantly (cf. Table 1) when the deposition time (i.e.,
the number of cycles) is varied. Thus, it seems that the
thickness of the coating does not significantly affect the
corrosion protection properties of the POA coatings.
The outstanding corrosion protection offered by
POA coating to Cu may be due to the fact that the
Fig. 9. XRD pattern of Cu recorded after the potentiodynamic polarization resistance measurement in aqueous solution of 3% NaCl. The (*)
indicates the diffraction peaks due to CuCl2.
S. Patil et al. / Applied Surface Science 225 (2004) 204–216 213
deposited polymer is strongly adherent and uniformly
covers the entire electrode surface as evident by the
SEM. Furthermore, the delocalized p-electrons in this
polymer facilitate its strong adsorption on the Cu
surface leading to the outstanding corrosion inhibi-
tion. In addition, the oxygen of the methoxy group
may facilitates the complexation to the Cu surface and
helps to enhance the adhesion of the POA coating to
the Cu surface [17].
In order to further reveal the corrosion protection
ability of the POA coating, we have studied the elec-
trochemical behavior of the POA coated Cu electrode
in a 0.2 M aqueous solution of sodium oxalate (in the
absence of monomer). The CVs recorded for bare and
POA coated Cu in the potential range between �500
and 1500 mV at a scan rate of 20 mV/s in a 0.2 M
aqueous solution of sodium oxalate are shown in
Fig. 11. The first scan of the CV recorded for bare
Cu (Fig. 11a) is similar to that shown in Fig. 1a. As
discussed earlier, it reveals the dissolution of Cu and
formation of copper oxalate interphase. The first scan
of the CV recorded for POA coated Cu (Fig. 11b) is
significantly different from that for bare Cu. The
absence of the anodic peak A and the observation of
negligibly small current densities at all potentials indi-
cates that the dissolution of the underlying Cu substrate
is inhibited due to the POA coating. To support this, we
have added a copper-sensitive indicator, Murexide, to
the electrolyte and monitored the color change at the
polymer/electrolyte interface. This indicator is violet in
the absence of Cu2þ but changes to orange on com-
plexation with Cu2þ. It was observed that the color of
the electrolyte remains violet even after recording 15
scans for POA coated Cu which indicates the absence
of substantial amount of Cu2þ ions in the vicinity of
polymer/electrolyte interface. Thus, the POA coating
appears to have outstanding protective ability to inhibit
the dissolution of the Cu.
Fig. 10. SEM of Cu recorded after the potentiodynamic polarization resistance measurement in aqueous solution of 3% NaCl.
Fig. 11. Cyclic voltammograms of (a) bare Cu and (b) POA coated
Cu recorded in 0.2 M sodium oxalate solution. Scan rate: 20 mV/s.
214 S. Patil et al. / Applied Surface Science 225 (2004) 204–216
It is pointed out that the POA coating is soluble in
DMSO solution, whereas the copper oxalate inter-
phase is insoluble. The copper oxalate interphase
remains as it is even after keeping it for 30 min in
DMSO solution. As discussed earlier, the copper
oxalate interphase formed during the early stages
of the growth decreases the rate of Cu dissolution.
However, it does not prevail at the electrode surface
and it seems that it undergoes the dissolution and
facilitates the ECP of OA. The further evidence in
support of this was obtained by comparing the corro-
sion behavior of the POA removed Cu substrates with
that of bare Cu. The POA coating was removed
carefully by dissolving it in DMSO and the potentio-
dynamic polarization measurements were performed
in the aqueous solution of 3% NaCl. The potentio-
dynamic polarization curves for the bare Cu and the
POA removed Cu are shown in Fig. 12. Interestingly,
the Ecorr and the corrosion rate for both the samples
are very similar. This suggests that the passive copper
oxalate interphase formed during the early stages of
the growth does not remain at the electrode surface
and the protection of the Cu is mainly due to the POA
coating.
We have also performed the potentiodynamic polar-
ization resistance measurements by using the POA
coated Cu substrates after storing them in air at 25 8Cfor 7 days and the corresponding polarization curve is
shown in Fig. 13b. The higher shift (�70 mV) in Ecorr
as compared with the freshly prepared and dried
coating reveals the increase in the corrosion resistance
offered by the POA coatings to Cu. This may be
attributed to the dehydration of the polymer during
the storage process. Thus, POA coating shows the high
chemical as well as physical stability because the
coating keeps its adherence to Cu substrate even after
the storage.
4. Conclusions
The ECP of OA in an aqueous solution of sodium
oxalate results into the deposition of uniform, compact
Fig. 12. Potentiodynamic polarization curves for (a) bare Cu, (b) POA removed Cu recorded in aqueous solution of 3% NaCl.
Fig. 13. Potentiodynamic polarization curves for POA coated Cu
(a) freshly prepared and (b) after storing in air for 7 days at 25 8C.
S. Patil et al. / Applied Surface Science 225 (2004) 204–216 215
and strongly adherent POA coatings on Cu substrates.
The formation of POA coatings occurs after the
passivation of the Cu substrate via formation of
CuC2O4H2O interphase. The XRD measurement
clearly reveals the formation of polycrystalline
CuC2O4H2O interphase. It is found that the copper
oxalate interphase formed during early stages of the
synthesis decomposes and facilitates the ECP of OA
on Cu. Our investigations clearly reveals that the
sodium oxalate is a suitable medium for the ECP of
OA on the Cu substrate and it favors the formation of
the mixed phase of PB and ES forms of POA.
The POA coatings exhibit significant corrosion pro-
tection properties in an aqueous solution of 3% NaCl.
The superior corrosion protection properties of the POA
may be due to its strong adhesion and uniform coverage.
The corrosion rate of POA coated Cu is found to be
�100 times lower than that observed for bare Cu. It is
observed that the coatings remain stable chemically as
well as physically even after storing them in air for 7
days. Thus, the results of the present investigation
clearly points out the remarkable capability of the
POA to protect Cu against corrosion and dissolution.
Acknowledgements
The work was supported by All India Council for
Technical Education (AICTE), New Delhi and the
Department of Atomic Energy (DAE), India.
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