# Synthesis of Nitrogen Doped Carbon and Its Enhanced Electrochemical Activity towards Ascorbic Acid Electrooxidation

Authors: Sankararao Mutyala; Mathiyarasu Jayaraman
Journal: International Journal of Electrochemistry
 (2014)

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## Abstract

Nitrogen doped carbon, synthesized by a novel way of carbonizing polyaniline in an inert atmosphere at a constant temperature of800°C, exhibits several unique features. The carbon: nitrogen ratio is found to increase with the treatment duration up to 120 minutes and a mass reduction of 60 wt% is observed with an interesting observation of the retention of the bulk polymer morphology, surprisingly, even after the carbonization process. The electrochemical activity evaluated with potassium hexacyanoferrate and hexamine ruthenium redox systems at a regular time interval helps to tune the catalytic activity. This type of nitrogen doped carbon prepared from polyaniline base exhibits excellent electrocatalytic activity as illustrated by the oxidation of ascorbic acid in neutral medium.


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## Body

## 1. Introduction

Carbon is one of the prospective candidates in the field of electroanalysis mainly because of its broad potential window, very little background current, rich surface chemistry, chemical stability, and most importantly abundance [1]. A range of active carbon materials demonstrates requisite characteristics of a good catalyst support; however, they generally exhibit poor inherent catalytic activity for many technologically relevant reactions [2].Previously, several methods have been used to alter the carbon support in an effort to improve its electrochemical reactivity. In addition to optimization of morphological properties, chemical modification of the carbon surface has been explored in order to enhance or tune the electrochemical activity of the carbon materials. Introduction of heteroatom such as oxygen, nitrogen, boron, sulfur, and halogen into the carbon matrix plays an important role in improving the catalytic performance [3]. For example, boron doping in carbon materials significantly improves the electrical conductivity and it is influenced by the boron doping level [4]. Sulfur doped amorphous carbon has been used as anode material for lithium ion batteries [5]. The added sulfur favorably increases the charge capacity and improves the electrochemical properties of the anode. However, the incorporated sulfur heteroatoms produce some side effects when they exist in unfavourable states.Among the heteroatom’s investigated, nitrogen doped carbon (NDC) has received significant attention as competitive oxygen reduction electrocatalysts. It is because nitrogen atom can donate the lone pair of electron to the carbon substrates more easily, which undergoes delocalization within the carbon material. Therefore, the adsorption properties as well as the electron transfer rate of the carbon during electrocatalytic processes may be enhanced significantly by N-doping [6, 7].In general, NDC has been prepared either by high temperature pyrolysis of precursor containing nitrogen and carbon [8–10] or by postannealing of various carbons in the presence of ammonia [11]. A number of N-doped mesoporous carbons have been directly synthesized, using various N-containing hydrocarbons (e.g., acetonitrile [12], polypyrrole [13, 14], or polyacrylonitrile [15, 16]) as carbon precursors and mesostructured silica as hard templates. N-doped mesoporous carbon spheres have also been successfully fabricated by using melamine formaldehyde as the precursor [17]. NDC materials have been synthesized using polyaniline-carbon composites that revealed electrocatalytic activity enhancement in oxygen reduction reaction [18]. Earlier attempts were reported [19, 20] in converting the polyaniline into nitrogen containing carbon. However, to our knowledge, there are no reports on the investigation of tuning the electrochemical activity of NDC materials. Thus, the extent of the electrocatalytic activity of these NDC and their application for other electrochemical reactions remain unknown.In this work, we report a novel synthetic strategy for NDC that entails the carbonization of nitrogen containing polymeric material in a controlled environment to produce the nitrogen containing carbon materials. Typically, polyaniline was synthesized via a chemical oxidative polymerization and subjected to heat treatment in an inert atmosphere under a linear time intervals to modulate the composition. By this effort, the electrochemical activities of these NDCs could be optimized and improved to accomplish desired electrochemical activity.


## 2. Experimental Methods

### 2.1. Preparation of Polyaniline

Polyaniline (PANI) was synthesized based on the classical chemical oxidative polymerization of aniline. In a typical synthesis, 2.59 mg of aniline hydrochloride and 5.71 g of ammonium peroxydisulfate were dissolved in 50 mL water in separate volumetric flasks. Both solutions were kept for an hour at room temperature, then mixed in a beaker, briefly stirred, and left to undergo polymerization. After 24 hours, PANI precipitate was subsequently collected on a Whatman filter paper and washed with three 100 mL portion of 0.2 M hydrochloric acid and acetone. In this washing process, 0.2 M HCl removed all residual monomers followed by a final washing with acetone to remove low-molecular oligomers. This also prevented the formation of agglomerates of PANI during drying, to facilitate fine powder formation. The green polyaniline powder was dried in vacuum at 65°C and subjected to carbonization process.


### 2.2. Synthesis of NDC

PANI was carbonized in an inert atmosphere at 800°C systematically for various time intervals. Typically, 1.5 g of PANI in a silica boat was introduced in a tubular furnace. To produce inert atmosphere, high purity argon gas flow was maintained throughout the heat treatment process. The heat treated PANI; that is, NDCs obtained at different time intervals 30, 60, 90, and 120 minutes were labelled as NDC-1, NDC-2, NDC-3, and NDC-4.


### 2.3. Electrode Preparation

In order to characterize these NDCs, they were made as carbon past electrodes, by mixing 6 mg of the respective NDC powder with 20μL of paraffin oil and this ratio was maintained uniformly for the entire studies. The resulting paste was packed into the cavity electrodes (outer diameter 3 mm and inner diameter 1.6 mm) and a brass rod was used for electrical contact. The electrode surface was made smooth and cleaned carefully with deionised water before the electrochemical measurements.


### 2.4. Characterization

Surface morphology of the carbonized PANI was analyzed using scanning electron microscopy (SEM) [VEGA3 TESCAN]. Raman spectra were recorded using high resolution dispersive Renishaw make Laser Raman spectrophotometer employing helium-neon excitation laser of maximum power density 2.0 watts (633 nm). Fourier transform-infrared (FTIR) vibration spectrum was taken by a Nexus 670 model FTIR spectrometer (make: Thermo Electron Corporation, USA). The wavelength region selected for taking the FTIR spectrum was 400–4000 cm−1. For taking the spectra of these synthesized materials, first it was mixed with high quality potassium bromide (KBr) followed by making it as pellets and introducing it in the IR path and measurements are executed in transmission mode. The elemental composition (CHN) analysis was recorded using Elementar vario EL III, German. Thermal stability was characterized by thermogravimetric analysis (TGA) with model SDT Q600 V8.3 Build 101.


### 2.5. Electrochemical Measurements

Electrochemical measurements were performed using a potentiostat, Autolab model PGSTAT-30, in a conventional three-electrode configuration, with nitrogen containing carbon paste as the working electrode and a platinum and Ag/AgCl electrode as counter and reference electrodes, respectively. Cyclic voltammetry was carried out in a solution containing 0.01 M of potassium ferricyanide + potassium ferrocyanide in 0.1 M potassium nitrate solution at room temperature (25±1°C). Impedance measurements were performed in a similar electrochemical cell using Ivium Technologies, Compactstat Electrochemical analyzer in 0.01 M potassium ferricyanide + potassium ferrocyanide in 0.1 M potassium nitrate solution by applying an alternating voltage of 5 mV in a frequency range from 0.01 Hz to 100 kHz using THALES 4.13 software. All the solutions were prepared in fresh Millipore water of resistivity 18.2 MΩ·cm.


## 2.1. Preparation of Polyaniline

Polyaniline (PANI) was synthesized based on the classical chemical oxidative polymerization of aniline. In a typical synthesis, 2.59 mg of aniline hydrochloride and 5.71 g of ammonium peroxydisulfate were dissolved in 50 mL water in separate volumetric flasks. Both solutions were kept for an hour at room temperature, then mixed in a beaker, briefly stirred, and left to undergo polymerization. After 24 hours, PANI precipitate was subsequently collected on a Whatman filter paper and washed with three 100 mL portion of 0.2 M hydrochloric acid and acetone. In this washing process, 0.2 M HCl removed all residual monomers followed by a final washing with acetone to remove low-molecular oligomers. This also prevented the formation of agglomerates of PANI during drying, to facilitate fine powder formation. The green polyaniline powder was dried in vacuum at 65°C and subjected to carbonization process.


## 2.2. Synthesis of NDC

PANI was carbonized in an inert atmosphere at 800°C systematically for various time intervals. Typically, 1.5 g of PANI in a silica boat was introduced in a tubular furnace. To produce inert atmosphere, high purity argon gas flow was maintained throughout the heat treatment process. The heat treated PANI; that is, NDCs obtained at different time intervals 30, 60, 90, and 120 minutes were labelled as NDC-1, NDC-2, NDC-3, and NDC-4.


## 2.3. Electrode Preparation

In order to characterize these NDCs, they were made as carbon past electrodes, by mixing 6 mg of the respective NDC powder with 20μL of paraffin oil and this ratio was maintained uniformly for the entire studies. The resulting paste was packed into the cavity electrodes (outer diameter 3 mm and inner diameter 1.6 mm) and a brass rod was used for electrical contact. The electrode surface was made smooth and cleaned carefully with deionised water before the electrochemical measurements.


## 2.4. Characterization

Surface morphology of the carbonized PANI was analyzed using scanning electron microscopy (SEM) [VEGA3 TESCAN]. Raman spectra were recorded using high resolution dispersive Renishaw make Laser Raman spectrophotometer employing helium-neon excitation laser of maximum power density 2.0 watts (633 nm). Fourier transform-infrared (FTIR) vibration spectrum was taken by a Nexus 670 model FTIR spectrometer (make: Thermo Electron Corporation, USA). The wavelength region selected for taking the FTIR spectrum was 400–4000 cm−1. For taking the spectra of these synthesized materials, first it was mixed with high quality potassium bromide (KBr) followed by making it as pellets and introducing it in the IR path and measurements are executed in transmission mode. The elemental composition (CHN) analysis was recorded using Elementar vario EL III, German. Thermal stability was characterized by thermogravimetric analysis (TGA) with model SDT Q600 V8.3 Build 101.


## 2.5. Electrochemical Measurements

Electrochemical measurements were performed using a potentiostat, Autolab model PGSTAT-30, in a conventional three-electrode configuration, with nitrogen containing carbon paste as the working electrode and a platinum and Ag/AgCl electrode as counter and reference electrodes, respectively. Cyclic voltammetry was carried out in a solution containing 0.01 M of potassium ferricyanide + potassium ferrocyanide in 0.1 M potassium nitrate solution at room temperature (25±1°C). Impedance measurements were performed in a similar electrochemical cell using Ivium Technologies, Compactstat Electrochemical analyzer in 0.01 M potassium ferricyanide + potassium ferrocyanide in 0.1 M potassium nitrate solution by applying an alternating voltage of 5 mV in a frequency range from 0.01 Hz to 100 kHz using THALES 4.13 software. All the solutions were prepared in fresh Millipore water of resistivity 18.2 MΩ·cm.


## 3. Result and Discussion

### 3.1. Elemental Analysis

Table1 shows the elemental analysis of PANI and pyrolyzed PANI that reflects the varying amount of carbon and nitrogen depending on the treatment duration at 800°C. As expected, the carbon content increases to a value of 70% on heat treatment in NDC-2 and NDC-3 samples. However, any further increase in treatment duration results in a decrease in carbon content perhaps due to the expected decomposition of the carbon structure. This can be further confirmed by observing the nitrogen content, where it decreases from a value of 11% to 6.5%. Decomposition is clearly reflected in the C/N ratio that interestingly increases to a moderate value of 10.5. During the carbonization of PANI, it is possible that phenazine-like cross-linked units [21] are formed by the cross-linking of PANI chains accounting for the 71% of carbon and 12% nitrogen (leading to a C/N ratio of ~6.0), as is proved by the spectral analysis reported below. Prolonged heat treatment, nevertheless, leads to the decomposition of the phenazine like carbon structure facilitating a decrease in carbon and nitrogen content as observed and these expected processes are proposed in Figure 1. Depending on the experimental conditions, the samples can always contain some oxygen, chlorine, and sulphur [22] and during the heat treatment their content decreases.Table 1
CHN analysis of polyaniline and NDC materials.
Sample description
C (wt%)
H (wt%)
N (wt%)
S (wt%)
Others (wt%)
C/N Ratio
PANI
57.0
4.5
11.0
3.2
24.0
5.2
NDC-1
65.7
0.6
11.6
0.1
22.0
5.7
NDC-2
70.8
0.6
11.7
0.1
16.8
6.1
NDC-3
70.9
0.6
10.4
0.1
18.0
6.8
NDC-4
68.3
0.6
6.5
0.1
24.5
10.5Figure 1
Schematic illustration of changes in the polyaniline structure during heat treatment at 800°C in an inert atmosphere.


### 3.2. FITR Analysis

Figure2 shows a comparison of FTIR spectra of these materials in the range of 400–4000 cm−1. The characteristic band of PANI appears at 1565 cm−1 corresponding to the benzenoid and quinoid rings and the band at 1482 cm−1 is attributed to the C=C aromatic ring stretching vibration. The 1296 cm−1 band is assigned to C–N vibrational stretching of a secondary aromatic amine, whereas the peak at about 1115 cm−1 corresponds to aromatic C–H in-plane bending mode. The C–H out-of-plane deformations of the 1,4-disubstituted rings are located in the region of 804 cm−1. The band at 503 cm−1 is related to the out-of-plane C–H wagging vibrations. In general, the region 2500–4000 cm−1 of the spectra strongly reflects the hydrogen bonding. This can be attributed to H-bond formation between the –N–H and =N–H groups in adjacent polymer chains while the band at 3627 cm−1 is assigned to the overtone band of nitrogen atoms in PANI.Figure 2
FTIR spectra of PANI and heat treated PANI such as NDC-1, NDC-2, NDC-3, and NDC-4 exposed to systematic time intervals 30, 60, 90, and 120 minutes, respectively, in an inert atmosphere at 800°C.After carbonization, however, most of the peaks disappear along with the emergence of many new peaks indicating structural changes as shown in the schematics (Figure1). After 30 minutes of carbonization (NDC-1), a decrease in intensity of the band at 3307 cm−1 is observed, ascribed to amine stretching (N–H) vibration. It is due to the reduction in the number of hydrogen connected to the nitrogen atoms in PANI [23]. Further, the two main peaks at 1573 cm−1 and 1232 cm−1 have been broadened and shifted, perhaps due to the cross-linking of the polymeric rings reflecting the formation of phenazine type rings. As the treatment time increases, a new band appears at 2996 cm−1 corresponding to the C–H aromatic stretching vibration. The broader region observed in the case NDC-2 reveals a loss of residual water in the sample. The absorption band about 1743 cm−1 in NDC-3 clearly indicates the presence of C=O group. This is reasoned as the structural changes followed by the formation of oxime-like moiety. The appearance of peaks at 2209 cm−1 and 2212 cm−1 in NDC-1 and NDC-3 may be attributed to cumulated stretching vibration of the N=C=O or the nitrile group. The peak at 806 cm−1 in NDC-3 reflects the N–H out-of-plane wagging and twisting vibration. The band at 1213 cm−1 in NDC-4 corresponds to sp2/sp3 C–C vibrations. The peak at 949 cm−1 observed in NDC-2 supports the presence of oxime-like structures in the sample. It is interesting to note that the C–N asymmetric stretching vibration at 1296 cm−1 (PANI) is shifted to 1288 (NDC-2); 1260 cm−1 (NDC-3) is due to the change in bond length between nitrogen and carbon atom. After carbonization process, the peaks at 1573, 1501, 1550, and 1568 cm−1 in NDC-1, NDC-2, NDC-3, and NDC-4 indicate the aromatic C=C vibrational stretching with sp2 configuration rather than olefinic one. In the case of NDC-4, the characteristic peak at 2459 cm−1 corresponds to multiple bonds resulting in overtone bands of respective nitrogen containing carbonaceous materials. These observations clearly indicate that nitrogen (heteroatom) incorporation is successful in carbonaceous materials as shown in Figure 2.


### 3.3. Raman Spectroscopy Analysis

Raman spectroscopy is a widely used method for analyzing different carbonaceous materials particularly to distinguish various types of bonds between carbon atoms. Accordingly, Figure3 shows the Raman spectrum of PANI and NDC materials. From the spectra, it is observed that the simple PANI spectrum is transformed to a pattern represented by two peaks at 1582 and 1348 cm−1, corresponding to the “so-called” graphitic (G) and disordered (D) band parts, respectively. In the case of NDC (heat treated PANI), the position of the two main bands results from PANI by two steps: (i) loss of protonating acid in the first step, which is followed by the (ii) formation of phenazine–like cross-linked units during the carbonization process which is supported by the elemental and FTIR analysis. During the heat treatment of PANI, the above-mentioned bands appear at dissimilar intensities followed by a refinement of the D and G bands in a systematic time interval. On careful examination of relative integrated intensity ratio (ID/IG), it is found to decrease corresponding to the number and/or size of graphitic micro domains, and therefore an increase in the number of fourfold coordinated carbon atoms (sp3/sp2) is ascertained. The peak position and peak intensity slightly change from one material to another perhaps due to the structural disorder in the matrix. The ID/IG ratio of synthesized PANI, NDC-1, NDC-2, NDC-3, and NDC-4 was calculated using Raman intensity and the values are found to be 0.9, 0.92, 0.96, 0.98, and 0.99, respectively. The increases in ID/IG ratio after heat treatment clearly confirm the graphitization of polyaniline leading to successful carbonization process.Figure 3
Laser Raman spectra of PANI and heat treated PANI such as NDC-1, NDC-2, NDC-3, and NDC-4 exposed to systematic time intervals 30, 60, 90, and 120 minutes, respectively, in an inert atmosphere at 800°C. Excitation wavelength is 633 nm.


### 3.4. Surface Morphology Analysis

The surface morphology of the carbonized PANI is examined using scanning electron microscopy (SEM). Accordingly, Figure4 shows typical morphological features of both PANI and NDC. When it is viewed from an angle perpendicular to the surface at a low magnification, it appears to contain white spots all across the surface. This clearly indicates the surface roughness of the matrix associated with a granularity of the conductive materials. The SEM images (Figure 4) further indicate that the synthesized PANI morphology is conserved even after the carbonization process, as observed by many researchers [24–29]. Thus, the retention of morphology is observed with a small shrinkage in size of the particle in NDC-2. Further close observation reveals small defects at the edges of the particles.Figure 4
Scanning electron microscopy (SEM) micrographs of PANI and heat treated PANI such as NDC-1, NDC-2, NDC-3, and NDC-4 exposed to systematic time intervals 30, 60, 90, and 120 minutes, respectively, in an inert atmosphere at 800°C.


### 3.5. Thermal Stability Analysis

TGA analysis is performed to investigate the thermal stability of the materials and Figure5 shows the TGA curves of both PANI and NDC. All materials exhibit considerable amount of mass reduction below 100°C, perhaps due to the loss of absorbed water molecules or trapped hydrogen chloride. However, above 200°C, major mass reduction takes place illustrating the superior thermal stability of NDC compared to that of PANI base. This is due to faster degradation of the small chains of PANI base. In the case of NDC, significant weight loss occurs between 450 and 850°C owing to the oxidative decomposition of polymer chains followed by incorporation of the nitrogen atom [30]. The stability of the NDC increases with the heat treatment duration and thus NDC-4 shows maximum thermal stability. These results confirm that the weight loss of the carbonized material increases with temperature. Above 800°C all these materials, interestingly, result in complete degradation (i.e., nearly zero mass) which indicates the formation of metal-free NDC by this process. In contrast, most of the processes pertain to carbonaceous material preparation; incorporation of metal impurities is implicit [31].Figure 5
Thermogravimetric analysis (TGA) of PANI and heat treated PANI such as NDC-1, NDC-2, NDC-3, and NDC-4 exposed to systematic time intervals 30, 60, 90, and 120 minutes, respectively, in an inert atmosphere at 800°C.


### 3.6. Cyclic Voltammetric Studies

Electrochemical activity of NDC (carbonized polyaniline) has been examined using cyclic voltammetry with the help of standard redox systems such as potassium hexacyanoferrate [Fe(CN)6]3−/4−. The response observed in terms of difference in cathodic and anodic peak potential (ΔEp=Ep,a–Ep,c) and the performance is discussed in terms of ΔEp values (for an ideal system it should be 59/n mV at 25°C, where n is the number of electrons involved in the redox reaction). The [Fe(CN)6]3−/4− is an outer sphere redox system that depends strongly on the surface heterogeneity of the carbon matrix. The other outer sphere redox system hexaammineruthenium (III) [Ru(NH3)6]3+/2+ that has very minimal surface dependence on particular surface sites or functional groups is also employed as the redox system for activity assessment.Figure6 shows the cyclic voltammogram behaviour of polyaniline and various NDC electrodes in 0.01 M potassium ferricyanide and hexaammineruthenium (III) in 0.1 M potassium nitrate solution. In general, all cyclic voltammograms exhibit similar current-potential profiles in these redox systems except PANI in Figures 6(a) and 6(f) and NDC-1 in Figures 6(b) and 6(g); these are suggesting that the surface conditions of the modified electrode are almost similar. Interestingly, PANI modified paste electrode shows a capacitive loop and the poor conductivity of PANI is explained due to the presence of leucoemeraldine or pernigraniline form. In the case of NDC-1, the electrode surface just reflects an insulating behaviour of the material and it is understandable that 30 minutes of treatment is not sufficient to fully convert PANI into a conductive carbonised form. Other NDCs show a good redox activity and the peak-potential separation for those electrodes is given in Table 2.Table 2
Peak-to-peak separation obtained from cyclic voltammograms of respective redox systems.
Electrode
ΔEp, mV
[Fe(CN)6]3−/4−
[Ru(NH3)6]3+/2+
NDC-1
—
—
NDC-2
150
141
NDC-3
140
120
NDC-4
130
100
Polyaniline
—
—Figure 6
Cyclic voltammograms of different NDC materials: ((a)–(e)) represent the PANI, NDC-1, NDC-2, NDC-3, and NDC-4 in 0.01 M potassium ferricyanide + 0.1 M potassium nitrate solution and ((f)–(j)) represent the PANI, NDC-1, NDC-2, NDC-3, and NDC-4 in 0.01 M of hexaammineruthenium (III) + 0.1 M potassium nitrate solution. Scan rate is 20 mVs−1.Except NDC-1, all other NDCs exhibit clear redox behaviour with better peak-to-peak separation(ΔEp) values. For other NDCs, the peak-to-peak separation is observed in between 100 and 150 mV and cathodic/anodic peak current ratios (Ia/Ic) are close to one. It is reported that the introduction of nitrogen heteroatom in the carbon structure improves the electroactivity of the materials since the nitrogen containing lone pair of electrons undergoes delocalization within the carbon material [31–34]. This lone pair of electrons is responsible for the enhanced electrochemical activity of the NDCs. The surface in-homogeneity of the NDCs in terms of microstructural characteristics/surface functionalization is evidenced by the slight increase in the ΔEp values (10–20 mV) of [Fe(CN)6]3−/4− redox system.Table2 results are indicative of the electrocatalytic activity for the [Fe(CN)6]3−/4−/[Ru(NH3)6]3+/2+ redox reaction, as clearly evidenced by significant peak-potential separation and high peak current (ipa,ipc) for these electrodes. These results indicate that the NDC-4 carbon shows better electrocatalytic activity for the [Fe(CN)6]3−/4−/[Ru(NH3)6]3+/2+ redox reaction compared to other NDC carbon paste electrodes. The peak current densities for the NDC-3 and NDC-4 are higher than that of other electrodes, which might be owing to the high surface roughness and hence a higher effective surface area.


### 3.7. Electrochemical Impedance Spectroscopy (EIS) Studies

Electrochemical impedance spectroscopy is performed to investigate the activity of the PANI and NDC using freely diffusing and negatively charged redox species. The corresponding Nyquist complex plane impedance plots of the electrodes are shown in Figure7. The preparation procedure, carbonization process, and the heat treatment temperatures had a profound influence on the impedance spectra. The impedance spectrum of PANI exhibits only diffusion processes and all other NDC materials show a charge transfer process followed by diffusion. Further, all NDCs exhibit similar impedance behaviour except NDC-1, where the close observation does not show a perfect Nyquist behaviour (semicircle) that can be attributed to the incomplete nitrogen doping and high residual particles. In a comparison, the NDCs exhibit a depressed semicircle in the high frequency region followed by a straight line with a slope of nearly 45° in the low frequency region, which is typical of a porous film coated on metals in the asymmetric metal/film/electrolyte configuration [35]. The depressed semicircle in the high frequency region could be ascribed to the charge (electron and proton) exchange at the carbon electrode/electrolyte interface. A straight line at low frequencies can be explained using a Warburg diffusion element due to the semi-infinite diffusion of ions at the carbon electrode/electrolyte interface [36]. Thus, an equivalent circuit model is employed in this study to represent the impedance behaviour of the porous electrode at the open circuit potential and it is portrayed in Figure 8.Figure 7
Electrochemical impedance spectroscopy of Polyaniline and different NDC materials, measurements have been performed at the formal potential of the [Fe (CN)6]3−/4− redox couple (5 mM, +200 mV versus Ag/AgCl 3 M KCl) in the frequency range of 5 Hz (final) to 40 kHz (initial) with an amplitude of 5 mV.Figure 8
A schematic representation of the equivalent circuit used for fitting the data in this study.In this circuit,Rs represents the solution resistance; R1 and R2 are the charge transfer resistance Rct. Q1 and Q2 are the double layer capacitance expressed as Cdl. The fitted results according to the equivalent circuit are also shown in Figure 8. The good fit implies that the equivalent circuit models can reasonably explain the electrochemical processes at the interface of the carbon supports/electrolytes at open circuit potential. Kinetic parameters calculated from the Nyquist plot are listed in Table 3. A comparison of the EIS Nyquist plots shows that the size of the semicircle drastically decreases with varying nitrogen content in the NDC electrode closer to the conventional glassy carbon electrode, and this can be ascribed to the doping of nitrogen atoms. For the PANI electrode, the impedance does not accord with the trend observed as it behaves like a highly resistive matrix. The distorted semicircle behaviour of NDC-1 in the high frequency region is due to the porous nature of the matrix which can be attributed to incomplete carbonization. A comparison of the charge transfer resistance among various NDCs with that on conventional glassy carbon electrode (GCE) reveals the ease of charge (electron) transfer across the interface of the NDC paste electrode/electrolyte. In particular, the NDC-4, prepared with a heat treatment at 800°C for 120 minutes, shows lowest nitrogen content with the smallest Rct (highest value of exchange current i0) suggesting that the electrochemical activity of the sample is superior compared to that of other electrodes.Table 3
Charge transfer resistance (Rct), double layer capacitance (Cdl), and exchange current (i0) for various NDC electrodes in 0.01 M [Fe(CN)6]3−/4− + 0.1 M KNO3 solution at the open circuit potential. The kinetic parameters have been calculated using the Randles equivalent circuit shown in Figure 8.
Electrode
R
ct (Ω)
C
dl (μF)
i
0 (mA cm−2)
Polyaniline
—
—
—
NDC-1
508
23
2.34 × 10−3
NDC-2
450
240
2.64 × 10−3
NDC-3
317
537
3.70 × 10−3
NDC-4
310
519
3.83 × 10−3
GCE
200
0.07
1.83 × 10−3


### 3.8. Electrochemical Oxidation of Ascorbic Acid

During this investigation, it is observed that the NDC prepared from the PANI base exhibits excellent electrochemical activity. The activity enhancement is reasoned as the nitrogen atom doped in the carbon network containing the lone pair of electron that undergoes delocalization which is responsible for the improved conductivity. In an effort to portray the catalytic activity, the best performed material, that is, NDC-4, has been utilized as the electrode material for ascorbic acid oxidation. Ascorbic acid is an important molecule in biological systems and extensive research has been in progress to develop voltammetric methods for its estimation [37–39]. However, because of its high overpotential, poor reproducibility, low selectivity, and poor sensitivity on the conventional electrodes, it is difficult to determine ascorbic acid by direct oxidation in a neutral medium.Figure9 shows a comparison of the cyclic voltammogram of 10 mM ascorbic acid using Vulcan carbon (without N doping) and NDC paste electrodes as working electrodes. Ascorbic acid shows a sluggish response in the form of an oxidative wave at 0.30 V on pure carbon electrode, while the nitrogen doped electrode leads to a significant negative shift of oxidation potential (Ep=0.22V) along with a concomitant enhancement in the peak current density confirming better reversibility. Both these (i.e., greatly enhanced peak current, almost double, and the negative shift in the anodic overpotential of 0.22 V) indicate strong electrocatalytic activity of the NDC electrode with respect to ascorbic acid electrooxidation. A large decrease in the overpotential of the ascorbic acid could be considered as a kinetic effect facilitating a substantial increase in the electron transfer rate of ascorbic acid oxidation, which could in turn be attributed to the delocalization of lone pair of electrons of the heteroatom.Figure 9
Cyclic voltammogram of 10 mM ascorbic acid by using (a) Vulcan carbon paste electrodes and (b) NDC paste electrodes. Scan rate is 20 mVS−1.


## 3.1. Elemental Analysis

Table1 shows the elemental analysis of PANI and pyrolyzed PANI that reflects the varying amount of carbon and nitrogen depending on the treatment duration at 800°C. As expected, the carbon content increases to a value of 70% on heat treatment in NDC-2 and NDC-3 samples. However, any further increase in treatment duration results in a decrease in carbon content perhaps due to the expected decomposition of the carbon structure. This can be further confirmed by observing the nitrogen content, where it decreases from a value of 11% to 6.5%. Decomposition is clearly reflected in the C/N ratio that interestingly increases to a moderate value of 10.5. During the carbonization of PANI, it is possible that phenazine-like cross-linked units [21] are formed by the cross-linking of PANI chains accounting for the 71% of carbon and 12% nitrogen (leading to a C/N ratio of ~6.0), as is proved by the spectral analysis reported below. Prolonged heat treatment, nevertheless, leads to the decomposition of the phenazine like carbon structure facilitating a decrease in carbon and nitrogen content as observed and these expected processes are proposed in Figure 1. Depending on the experimental conditions, the samples can always contain some oxygen, chlorine, and sulphur [22] and during the heat treatment their content decreases.Table 1
CHN analysis of polyaniline and NDC materials.
Sample description
C (wt%)
H (wt%)
N (wt%)
S (wt%)
Others (wt%)
C/N Ratio
PANI
57.0
4.5
11.0
3.2
24.0
5.2
NDC-1
65.7
0.6
11.6
0.1
22.0
5.7
NDC-2
70.8
0.6
11.7
0.1
16.8
6.1
NDC-3
70.9
0.6
10.4
0.1
18.0
6.8
NDC-4
68.3
0.6
6.5
0.1
24.5
10.5Figure 1
Schematic illustration of changes in the polyaniline structure during heat treatment at 800°C in an inert atmosphere.


## 3.2. FITR Analysis

Figure2 shows a comparison of FTIR spectra of these materials in the range of 400–4000 cm−1. The characteristic band of PANI appears at 1565 cm−1 corresponding to the benzenoid and quinoid rings and the band at 1482 cm−1 is attributed to the C=C aromatic ring stretching vibration. The 1296 cm−1 band is assigned to C–N vibrational stretching of a secondary aromatic amine, whereas the peak at about 1115 cm−1 corresponds to aromatic C–H in-plane bending mode. The C–H out-of-plane deformations of the 1,4-disubstituted rings are located in the region of 804 cm−1. The band at 503 cm−1 is related to the out-of-plane C–H wagging vibrations. In general, the region 2500–4000 cm−1 of the spectra strongly reflects the hydrogen bonding. This can be attributed to H-bond formation between the –N–H and =N–H groups in adjacent polymer chains while the band at 3627 cm−1 is assigned to the overtone band of nitrogen atoms in PANI.Figure 2
FTIR spectra of PANI and heat treated PANI such as NDC-1, NDC-2, NDC-3, and NDC-4 exposed to systematic time intervals 30, 60, 90, and 120 minutes, respectively, in an inert atmosphere at 800°C.After carbonization, however, most of the peaks disappear along with the emergence of many new peaks indicating structural changes as shown in the schematics (Figure1). After 30 minutes of carbonization (NDC-1), a decrease in intensity of the band at 3307 cm−1 is observed, ascribed to amine stretching (N–H) vibration. It is due to the reduction in the number of hydrogen connected to the nitrogen atoms in PANI [23]. Further, the two main peaks at 1573 cm−1 and 1232 cm−1 have been broadened and shifted, perhaps due to the cross-linking of the polymeric rings reflecting the formation of phenazine type rings. As the treatment time increases, a new band appears at 2996 cm−1 corresponding to the C–H aromatic stretching vibration. The broader region observed in the case NDC-2 reveals a loss of residual water in the sample. The absorption band about 1743 cm−1 in NDC-3 clearly indicates the presence of C=O group. This is reasoned as the structural changes followed by the formation of oxime-like moiety. The appearance of peaks at 2209 cm−1 and 2212 cm−1 in NDC-1 and NDC-3 may be attributed to cumulated stretching vibration of the N=C=O or the nitrile group. The peak at 806 cm−1 in NDC-3 reflects the N–H out-of-plane wagging and twisting vibration. The band at 1213 cm−1 in NDC-4 corresponds to sp2/sp3 C–C vibrations. The peak at 949 cm−1 observed in NDC-2 supports the presence of oxime-like structures in the sample. It is interesting to note that the C–N asymmetric stretching vibration at 1296 cm−1 (PANI) is shifted to 1288 (NDC-2); 1260 cm−1 (NDC-3) is due to the change in bond length between nitrogen and carbon atom. After carbonization process, the peaks at 1573, 1501, 1550, and 1568 cm−1 in NDC-1, NDC-2, NDC-3, and NDC-4 indicate the aromatic C=C vibrational stretching with sp2 configuration rather than olefinic one. In the case of NDC-4, the characteristic peak at 2459 cm−1 corresponds to multiple bonds resulting in overtone bands of respective nitrogen containing carbonaceous materials. These observations clearly indicate that nitrogen (heteroatom) incorporation is successful in carbonaceous materials as shown in Figure 2.


## 3.3. Raman Spectroscopy Analysis

Raman spectroscopy is a widely used method for analyzing different carbonaceous materials particularly to distinguish various types of bonds between carbon atoms. Accordingly, Figure3 shows the Raman spectrum of PANI and NDC materials. From the spectra, it is observed that the simple PANI spectrum is transformed to a pattern represented by two peaks at 1582 and 1348 cm−1, corresponding to the “so-called” graphitic (G) and disordered (D) band parts, respectively. In the case of NDC (heat treated PANI), the position of the two main bands results from PANI by two steps: (i) loss of protonating acid in the first step, which is followed by the (ii) formation of phenazine–like cross-linked units during the carbonization process which is supported by the elemental and FTIR analysis. During the heat treatment of PANI, the above-mentioned bands appear at dissimilar intensities followed by a refinement of the D and G bands in a systematic time interval. On careful examination of relative integrated intensity ratio (ID/IG), it is found to decrease corresponding to the number and/or size of graphitic micro domains, and therefore an increase in the number of fourfold coordinated carbon atoms (sp3/sp2) is ascertained. The peak position and peak intensity slightly change from one material to another perhaps due to the structural disorder in the matrix. The ID/IG ratio of synthesized PANI, NDC-1, NDC-2, NDC-3, and NDC-4 was calculated using Raman intensity and the values are found to be 0.9, 0.92, 0.96, 0.98, and 0.99, respectively. The increases in ID/IG ratio after heat treatment clearly confirm the graphitization of polyaniline leading to successful carbonization process.Figure 3
Laser Raman spectra of PANI and heat treated PANI such as NDC-1, NDC-2, NDC-3, and NDC-4 exposed to systematic time intervals 30, 60, 90, and 120 minutes, respectively, in an inert atmosphere at 800°C. Excitation wavelength is 633 nm.


## 3.4. Surface Morphology Analysis

The surface morphology of the carbonized PANI is examined using scanning electron microscopy (SEM). Accordingly, Figure4 shows typical morphological features of both PANI and NDC. When it is viewed from an angle perpendicular to the surface at a low magnification, it appears to contain white spots all across the surface. This clearly indicates the surface roughness of the matrix associated with a granularity of the conductive materials. The SEM images (Figure 4) further indicate that the synthesized PANI morphology is conserved even after the carbonization process, as observed by many researchers [24–29]. Thus, the retention of morphology is observed with a small shrinkage in size of the particle in NDC-2. Further close observation reveals small defects at the edges of the particles.Figure 4
Scanning electron microscopy (SEM) micrographs of PANI and heat treated PANI such as NDC-1, NDC-2, NDC-3, and NDC-4 exposed to systematic time intervals 30, 60, 90, and 120 minutes, respectively, in an inert atmosphere at 800°C.


## 3.5. Thermal Stability Analysis

TGA analysis is performed to investigate the thermal stability of the materials and Figure5 shows the TGA curves of both PANI and NDC. All materials exhibit considerable amount of mass reduction below 100°C, perhaps due to the loss of absorbed water molecules or trapped hydrogen chloride. However, above 200°C, major mass reduction takes place illustrating the superior thermal stability of NDC compared to that of PANI base. This is due to faster degradation of the small chains of PANI base. In the case of NDC, significant weight loss occurs between 450 and 850°C owing to the oxidative decomposition of polymer chains followed by incorporation of the nitrogen atom [30]. The stability of the NDC increases with the heat treatment duration and thus NDC-4 shows maximum thermal stability. These results confirm that the weight loss of the carbonized material increases with temperature. Above 800°C all these materials, interestingly, result in complete degradation (i.e., nearly zero mass) which indicates the formation of metal-free NDC by this process. In contrast, most of the processes pertain to carbonaceous material preparation; incorporation of metal impurities is implicit [31].Figure 5
Thermogravimetric analysis (TGA) of PANI and heat treated PANI such as NDC-1, NDC-2, NDC-3, and NDC-4 exposed to systematic time intervals 30, 60, 90, and 120 minutes, respectively, in an inert atmosphere at 800°C.


## 3.6. Cyclic Voltammetric Studies

Electrochemical activity of NDC (carbonized polyaniline) has been examined using cyclic voltammetry with the help of standard redox systems such as potassium hexacyanoferrate [Fe(CN)6]3−/4−. The response observed in terms of difference in cathodic and anodic peak potential (ΔEp=Ep,a–Ep,c) and the performance is discussed in terms of ΔEp values (for an ideal system it should be 59/n mV at 25°C, where n is the number of electrons involved in the redox reaction). The [Fe(CN)6]3−/4− is an outer sphere redox system that depends strongly on the surface heterogeneity of the carbon matrix. The other outer sphere redox system hexaammineruthenium (III) [Ru(NH3)6]3+/2+ that has very minimal surface dependence on particular surface sites or functional groups is also employed as the redox system for activity assessment.Figure6 shows the cyclic voltammogram behaviour of polyaniline and various NDC electrodes in 0.01 M potassium ferricyanide and hexaammineruthenium (III) in 0.1 M potassium nitrate solution. In general, all cyclic voltammograms exhibit similar current-potential profiles in these redox systems except PANI in Figures 6(a) and 6(f) and NDC-1 in Figures 6(b) and 6(g); these are suggesting that the surface conditions of the modified electrode are almost similar. Interestingly, PANI modified paste electrode shows a capacitive loop and the poor conductivity of PANI is explained due to the presence of leucoemeraldine or pernigraniline form. In the case of NDC-1, the electrode surface just reflects an insulating behaviour of the material and it is understandable that 30 minutes of treatment is not sufficient to fully convert PANI into a conductive carbonised form. Other NDCs show a good redox activity and the peak-potential separation for those electrodes is given in Table 2.Table 2
Peak-to-peak separation obtained from cyclic voltammograms of respective redox systems.
Electrode
ΔEp, mV
[Fe(CN)6]3−/4−
[Ru(NH3)6]3+/2+
NDC-1
—
—
NDC-2
150
141
NDC-3
140
120
NDC-4
130
100
Polyaniline
—
—Figure 6
Cyclic voltammograms of different NDC materials: ((a)–(e)) represent the PANI, NDC-1, NDC-2, NDC-3, and NDC-4 in 0.01 M potassium ferricyanide + 0.1 M potassium nitrate solution and ((f)–(j)) represent the PANI, NDC-1, NDC-2, NDC-3, and NDC-4 in 0.01 M of hexaammineruthenium (III) + 0.1 M potassium nitrate solution. Scan rate is 20 mVs−1.Except NDC-1, all other NDCs exhibit clear redox behaviour with better peak-to-peak separation(ΔEp) values. For other NDCs, the peak-to-peak separation is observed in between 100 and 150 mV and cathodic/anodic peak current ratios (Ia/Ic) are close to one. It is reported that the introduction of nitrogen heteroatom in the carbon structure improves the electroactivity of the materials since the nitrogen containing lone pair of electrons undergoes delocalization within the carbon material [31–34]. This lone pair of electrons is responsible for the enhanced electrochemical activity of the NDCs. The surface in-homogeneity of the NDCs in terms of microstructural characteristics/surface functionalization is evidenced by the slight increase in the ΔEp values (10–20 mV) of [Fe(CN)6]3−/4− redox system.Table2 results are indicative of the electrocatalytic activity for the [Fe(CN)6]3−/4−/[Ru(NH3)6]3+/2+ redox reaction, as clearly evidenced by significant peak-potential separation and high peak current (ipa,ipc) for these electrodes. These results indicate that the NDC-4 carbon shows better electrocatalytic activity for the [Fe(CN)6]3−/4−/[Ru(NH3)6]3+/2+ redox reaction compared to other NDC carbon paste electrodes. The peak current densities for the NDC-3 and NDC-4 are higher than that of other electrodes, which might be owing to the high surface roughness and hence a higher effective surface area.


## 3.7. Electrochemical Impedance Spectroscopy (EIS) Studies

Electrochemical impedance spectroscopy is performed to investigate the activity of the PANI and NDC using freely diffusing and negatively charged redox species. The corresponding Nyquist complex plane impedance plots of the electrodes are shown in Figure7. The preparation procedure, carbonization process, and the heat treatment temperatures had a profound influence on the impedance spectra. The impedance spectrum of PANI exhibits only diffusion processes and all other NDC materials show a charge transfer process followed by diffusion. Further, all NDCs exhibit similar impedance behaviour except NDC-1, where the close observation does not show a perfect Nyquist behaviour (semicircle) that can be attributed to the incomplete nitrogen doping and high residual particles. In a comparison, the NDCs exhibit a depressed semicircle in the high frequency region followed by a straight line with a slope of nearly 45° in the low frequency region, which is typical of a porous film coated on metals in the asymmetric metal/film/electrolyte configuration [35]. The depressed semicircle in the high frequency region could be ascribed to the charge (electron and proton) exchange at the carbon electrode/electrolyte interface. A straight line at low frequencies can be explained using a Warburg diffusion element due to the semi-infinite diffusion of ions at the carbon electrode/electrolyte interface [36]. Thus, an equivalent circuit model is employed in this study to represent the impedance behaviour of the porous electrode at the open circuit potential and it is portrayed in Figure 8.Figure 7
Electrochemical impedance spectroscopy of Polyaniline and different NDC materials, measurements have been performed at the formal potential of the [Fe (CN)6]3−/4− redox couple (5 mM, +200 mV versus Ag/AgCl 3 M KCl) in the frequency range of 5 Hz (final) to 40 kHz (initial) with an amplitude of 5 mV.Figure 8
A schematic representation of the equivalent circuit used for fitting the data in this study.In this circuit,Rs represents the solution resistance; R1 and R2 are the charge transfer resistance Rct. Q1 and Q2 are the double layer capacitance expressed as Cdl. The fitted results according to the equivalent circuit are also shown in Figure 8. The good fit implies that the equivalent circuit models can reasonably explain the electrochemical processes at the interface of the carbon supports/electrolytes at open circuit potential. Kinetic parameters calculated from the Nyquist plot are listed in Table 3. A comparison of the EIS Nyquist plots shows that the size of the semicircle drastically decreases with varying nitrogen content in the NDC electrode closer to the conventional glassy carbon electrode, and this can be ascribed to the doping of nitrogen atoms. For the PANI electrode, the impedance does not accord with the trend observed as it behaves like a highly resistive matrix. The distorted semicircle behaviour of NDC-1 in the high frequency region is due to the porous nature of the matrix which can be attributed to incomplete carbonization. A comparison of the charge transfer resistance among various NDCs with that on conventional glassy carbon electrode (GCE) reveals the ease of charge (electron) transfer across the interface of the NDC paste electrode/electrolyte. In particular, the NDC-4, prepared with a heat treatment at 800°C for 120 minutes, shows lowest nitrogen content with the smallest Rct (highest value of exchange current i0) suggesting that the electrochemical activity of the sample is superior compared to that of other electrodes.Table 3
Charge transfer resistance (Rct), double layer capacitance (Cdl), and exchange current (i0) for various NDC electrodes in 0.01 M [Fe(CN)6]3−/4− + 0.1 M KNO3 solution at the open circuit potential. The kinetic parameters have been calculated using the Randles equivalent circuit shown in Figure 8.
Electrode
R
ct (Ω)
C
dl (μF)
i
0 (mA cm−2)
Polyaniline
—
—
—
NDC-1
508
23
2.34 × 10−3
NDC-2
450
240
2.64 × 10−3
NDC-3
317
537
3.70 × 10−3
NDC-4
310
519
3.83 × 10−3
GCE
200
0.07
1.83 × 10−3


## 3.8. Electrochemical Oxidation of Ascorbic Acid

During this investigation, it is observed that the NDC prepared from the PANI base exhibits excellent electrochemical activity. The activity enhancement is reasoned as the nitrogen atom doped in the carbon network containing the lone pair of electron that undergoes delocalization which is responsible for the improved conductivity. In an effort to portray the catalytic activity, the best performed material, that is, NDC-4, has been utilized as the electrode material for ascorbic acid oxidation. Ascorbic acid is an important molecule in biological systems and extensive research has been in progress to develop voltammetric methods for its estimation [37–39]. However, because of its high overpotential, poor reproducibility, low selectivity, and poor sensitivity on the conventional electrodes, it is difficult to determine ascorbic acid by direct oxidation in a neutral medium.Figure9 shows a comparison of the cyclic voltammogram of 10 mM ascorbic acid using Vulcan carbon (without N doping) and NDC paste electrodes as working electrodes. Ascorbic acid shows a sluggish response in the form of an oxidative wave at 0.30 V on pure carbon electrode, while the nitrogen doped electrode leads to a significant negative shift of oxidation potential (Ep=0.22V) along with a concomitant enhancement in the peak current density confirming better reversibility. Both these (i.e., greatly enhanced peak current, almost double, and the negative shift in the anodic overpotential of 0.22 V) indicate strong electrocatalytic activity of the NDC electrode with respect to ascorbic acid electrooxidation. A large decrease in the overpotential of the ascorbic acid could be considered as a kinetic effect facilitating a substantial increase in the electron transfer rate of ascorbic acid oxidation, which could in turn be attributed to the delocalization of lone pair of electrons of the heteroatom.Figure 9
Cyclic voltammogram of 10 mM ascorbic acid by using (a) Vulcan carbon paste electrodes and (b) NDC paste electrodes. Scan rate is 20 mVS−1.


## 4. Conclusions

Nitrogen doped carbon has been prepared from polyaniline base that exhibits unique electrocatalytic activity for ascorbic acid oxidation. The C/N ratio in this is found to increase with treatment duration as evidenced by elemental analysis. SEM analysis has confirmed that the surface morphology is preserved even after the carbonization process of PANI. The conditions assuring that the conversion of PANI molecular structure to the corresponding nitrogen-enriched carbon, while preserving a good yield, have been sought. The molecular structure and its changes, that is, polyaniline and carbonized PANI, are represented by disordered carbon-like material having different types of bonds between carbon and nitrogen atoms, as illustrated by phenazine-like cross-linked units, quinoid units, and so forth. Electrochemical characterization shows improved electrochemical activity for NDC compared to that on polyaniline or just heat treated (30 minutes) NDC. In a typical redox reaction, theΔEp value has been observed as 100 mV for the carbon material heat treated for 120 minutes. The impedance behaviour in the form of Nyquist plot shows a semicircle followed by a 45° straight line behaviour (Warburg impedance) characteristic of diffusion followed by the charge transfer of the electroactive species at the electrode-electrolyte interface. Thus, the carbonized PANI, that is, nitrogen containing carbon, constitutes a novel material promising for several potential applications like biosensors and fuel cell electrocatalysts. This is especially true during the presence of nitrogen atoms in carbonized material having lone pair of electrons that undergoes delocalization. Further, the catalytic activity of the synthesized material has been demonstrated using ascorbic acid electrooxidation. Thus, the present nitrogen incorporated carbon opens new ways to tune chemical and electrochemical reactivity using in a legion of applications.



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*Source: 246746-2014-06-26.xml*