# A Study of the Initial Stages of Co Deposition on a Silver Electrode in Ammonia Medium Using an Electrochemical Quartz Crystal Microbalance

Authors: A. Montes-Rojas; A. L. Donjuan-Medrano
Journal: ISRN Electrochemistry
 (2013)

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## Abstract

The early stages of Co deposition on a silver electrode in ammonia medium were studied using cyclic voltammetry and chronoamperometry coupled with quartz crystal microbalance (EQCM) in ammonia solution. The results obtained by means of EQCM showed that during the initial stages of cobalt deposition a monolayer is formed on the substrate both in the underpotential and overpotential region, and this monolayer is formed at −600 mV and −980 mV. Once the cobalt deposition process starts, the growth is very fast making the investigation of the initial stages rather difficult. During this process, cobalt atoms transfer their two electrons through free species and not through cobalt hydroxide species adsorbed on the electrode as CoOH+ or Co(OH)2. In addition, it has been found that at potentials more positive than −600 mV, ammonia adsorption takes place on the substrate surface, and theses species are replaced when the cobalt atoms arrive at potentials more negative than −600 mV.


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## Body

## 1. Introduction

Cobalt is an element that involves a great interest due to its physical and chemical properties and technological applications. Some of its uses are as a catalyst in different reactions of technological interest or as a pigment for strong dark blue color. Also, this element is used in permanent magnet production as well as for preparation of super alloys of great hardness and resistant to high temperatures [1].One of the properties of this element, when combined with another metal, is the giant magnetoresistance (GMR) whose study has drawn the attention of diverse research teams [2–12]. The importance of this effect lies in that applications of these systems include domains such as informatics, for preparation of reading devices, or technology, for magnetic sensor production. On the basis of these studies it has been possible to show [3] that GMR occurs in materials formed by one magnetic element (Ni, Fe, or Co) and another nonmagnetic material (Au, Ag, Pd, Cu, etc.). Until now, the commercial preparation of these materials has been preferably performed by metal evaporation techniques [4–6], in which to avoid undesirable contaminations the whole system must be subject to high-vacuum conditions that generate high production costs.Because of this, electrodeposition of these materials using a mixed bath is explored with the aim of making their elaboration cheaper. Unlike the techniques of metallic evaporation, electrochemical methods allow us to work in conditions that are similar to those of the environment as well as to reduce the risks of contamination under inert and easily controllable conditions. Additionally, thanks to these methods, the film growth process can be known, and the quantity of deposited material can be controlled by the charge passing through the electrode using electrochemical techniques coupled with quartz microbalance.Notwithstanding this, some authors [7] have claimed that the magnetic properties sought depend on the method of preparation.One of the systems that have been studied to find out its magnetic properties is the system formed by cobalt and silver. In the literature, there are several works on the preparation of this system by physical methods [8, 9]; however, only few [7, 10–12] have used electrochemical methods to prepare it in a three-dimensional (granular) morphology. One of the most outstanding results, according to the authors [7], is that magnetic properties do not have the same intensity as when obtained by physical methods due to the fact that cobalt inclusions into the silver matrix do not have the same size or homogeneous distribution. These authors state that for a better control of GMR properties of the material, the first stages of its formation have to be known very well.Since in the preparation of this type of materials using electrochemical technique the growth of one metal takes place on a metal substrate of different nature, and the underpotential deposition process may be considered [13, 14]. According to the bibliography, there are no reports on results that support this idea; however, values obtained from extraction works (electron extraction from the substrate S, ϕS, and from the metal Me, ϕMe) of the cobalt and silver [15–18] (Table 1) satisfy the condition (1), and consequently the occurrence of UPD phenomenon should not be rejected. 						(1)ϕS>ϕMe.Table 1
Extraction works values for cobalt and silver at eV.
Metal
eV15
eV16
eV17
eV18
Ag
4.78
4.71
4.58
4.71
Co
4.70
4.25
4.18
4.16In addition to this hypothesis, it could be predicted that if this phenomenon occurs, cobalt atoms would be adsorbed on the substrate surface as completely discharged species, because the difference of electronegativities between the substrate (χAg=1.86) and adsorbate (χCo=1.80) meets the condition reported by Schultze and Koppitz [19], that is to say:
(2)|χAg-χCo|<0.5.It is important to emphasize that this hypothesis is supported by the results obtained with a similar system formed by cobalt on a gold substrate, even though this latter does not meet the condition of (1) using data of Trasatti [15]; however, Mendoza-Huizar et al. in 2002 [20], Flis-Kabulska in 2006 [21], and more recently Montes-Rojas et al. [22] have undertaken to prove the formation of said system.It is important to consider that different authors [23–25] have claimed that cobalt electrodeposition is thought to occur via the formation of CoOH+ and Co(OH)2 species. The hydroxide species formation depends on the pH of the deposition bath. On the one hand, for solution pH lower than 4.1, the authors proposed that Co2+ and OH- react producing CoOH+ “unstable complex.” It is followed by the reduction of this complex and its reaction with adsorbed hydrogen to form metallic Co. On the other hand, for solution pH between 4 and 4.5, the authors proposed that Co2+ and OH- react producing cobalt hydroxide (Co(OH)2). This compound is reduced to produce metallic Co. More recently, Pradhan et al. [24] and Matsushima et al. [25] have detected increased proportion of cobalt hydroxide species CoOH+ and Co(OH)2 that are adsorbed on a platinum substrate before giving rise to cobalt deposit formation when using solution of pH 4.1. However, these results have not been checked with solutions with higher pH.One of the tools used in this type of works is quartz crystal microbalance coupled with electrochemical techniques (Electrochemical Quartz Crystal Microbalance, EQCM), because this technique allows detecting very small mass variations produced during the UPD process [26–28] or in the first stages of the growth of one metal, thanks to the piezoelectric effect of a thin quartz sheet covered on both sides by a thin metal film used as electrode.This technique is very important for this kind of works according to Sauerbrey expression:(3)Δf=-(fo2Nρq)Δm,
where the resonance frequency (fο) of a acoustic wave spreading in the sheet changes (Δf) as a result of the mass variation on it (Δm) produced during an electrochemical experiment. Variables in parentheses are constants characteristic of the material (ρq is quartz density 2.648 g cm−3, N is the constant of quartz frequency 1.67 × 105 Hz cm−1, and fo is the resonance frequency in the fundamental mode) that may be grouped in a single constant called sensitivity factor Cf:
(4)Cf=fo2Nρq.It is noteworthy that in order to be able to use Sauerbrey expression, mass gain process on the electrode should fulfill certain considerations.(a)
Deposits should be homogeneously distributed on the surface of the electrode.(b)
Deposit films should be tightly linked to crystal, and it should be as rigid as the quartz.(c)
Changes of frequency upon film deposition should be below 2% of resonance frequency.The results shown in this work were obtained by studying the first stages of cobalt deposit formation on a silver substrate using quartz crystal microbalance coupled with electrochemical techniques.


## 2. Experimental

### 2.1. Solutions

The supporting electrolyte used in this work was prepared with (NH4)2SO4 in 1 M concentration. Cobalt solutions were prepared by dissolving Co(NO3)2 salts in tridistilled water, so that the metal ion concentration in the supporting electrolyte solution was 10-3M. All solutions were adjusted to pH 9.3 using reagent grade NaOH to diminish interferences of hydrogen evolution and to have the predominant species [Co(NH3)6]2+ [29]. In addition, prior to the realization of experiments the solution was purged with high-purity nitrogen to remove dissolved oxygen, and the same gas was used to maintain inert atmosphere during experiments.


### 2.2. Electrodes

Working electrodes (Seiko) of 0.9653 cm2 geometric area were gold films supported on polished quartz discs with titanium underlayer to improve gold adherence to quartz, vibrating in the fundamental mode at 9 MHz. These electrodes were modified potentiostatically at −960 mV with a thin layer of silver using a solution of cyanides [30]. The counter electrode was a platinum wire with a greater area than the working electrode. Potentials were measured against and are quoted versus the Ag|AgCl|NaCl 3 M reference electrode. In addition, the sensitive factor in the Sauerbrey equation (4) was determined by chronoamperometric thallium deposition [29], and its value was very close to the theoretical value (1.714±0.012×108Hzg-1cm2). Finally, all experiments were performed at room temperature.


### 2.3. Apparatus

Electrogravimetric experiments were carried out using a PAR potentiostat-galvanostat model 273A coupled with a QCM EG and G-Seiko microbalance model QCA922.


## 2.1. Solutions

The supporting electrolyte used in this work was prepared with (NH4)2SO4 in 1 M concentration. Cobalt solutions were prepared by dissolving Co(NO3)2 salts in tridistilled water, so that the metal ion concentration in the supporting electrolyte solution was 10-3M. All solutions were adjusted to pH 9.3 using reagent grade NaOH to diminish interferences of hydrogen evolution and to have the predominant species [Co(NH3)6]2+ [29]. In addition, prior to the realization of experiments the solution was purged with high-purity nitrogen to remove dissolved oxygen, and the same gas was used to maintain inert atmosphere during experiments.


## 2.2. Electrodes

Working electrodes (Seiko) of 0.9653 cm2 geometric area were gold films supported on polished quartz discs with titanium underlayer to improve gold adherence to quartz, vibrating in the fundamental mode at 9 MHz. These electrodes were modified potentiostatically at −960 mV with a thin layer of silver using a solution of cyanides [30]. The counter electrode was a platinum wire with a greater area than the working electrode. Potentials were measured against and are quoted versus the Ag|AgCl|NaCl 3 M reference electrode. In addition, the sensitive factor in the Sauerbrey equation (4) was determined by chronoamperometric thallium deposition [29], and its value was very close to the theoretical value (1.714±0.012×108Hzg-1cm2). Finally, all experiments were performed at room temperature.


## 2.3. Apparatus

Electrogravimetric experiments were carried out using a PAR potentiostat-galvanostat model 273A coupled with a QCM EG and G-Seiko microbalance model QCA922.


## 3. Results and Discussion

### 3.1. Voltammetric Characterization of a Silver Substrate

Figure1 shows a cyclic voltammogram (j-E) obtained at an electrode of quartz crystal modified with Ag film in electrolytic solution. This voltammogram has some characteristics that indicate the absence of faradaic processes since the very small current observed between −100 mV and −1000 mV corresponds to charging of the electrical double layer, and this feature is a criterion for the cleanliness of the surface of our substrates. Only when the potential is scanned at values more negative than −950 mV a cathodic current associated with hydrogen evolution is observed.Figure 1
Voltammogram of Ag/[(NH4)2SO4] 1 M system at pH 9.3 obtained at a scan rate of 5 mV s−1.


### 3.2. Voltammetric Characterization of UPD and OPD Zones

With the purpose to identify the processes that take place in the UPD and OPD region of the Co/Ag system, a large potential region was scanned using metal solution. In Figure2 a comparison is shown of the experimental voltammograms obtained at the silver electrode in both solutions, without (a) and with (b) Co(II) ions in solution.Figure 2
A comparison of two cyclic voltammetric curves obtained in the Ag/xM Co(II)+1 M (NH4)2SO4 (pH 9.3) system at two different Co(II) concentrations, (a) x= 0 and (b) x= 1 mM. The scan potential rate was of 5 mV s−1, and the potential interval was −100 mV and −990 mV. In the inset an amplification of the region comprising the peak of the alleged underpotential deposition is shown.The potential region, in Figure2(b), was scanned between –100 mV and –1000 mV. The potential scan started at −100 mV up to −1000 mV, and then it was reversed to the initial value. During the direct scan it can be noted that the cathodic current only increases when the potential is more negative than −980 mV, and this tendency still continues upon scan reversal. This current is associated with the process of cobalt deposit formation on the silver substrate because the potential region explored is more negative than the equilibrium potential (Eeq=-741mV) [20] which is known as overpotential region (OPD). In addition, in this same potential region the current measured must have a fraction associated with hydrogen evolution reaction.In the reverse potential scan, one crossover of the cathodic and anodic branches at −740 mV is observed which is typical of the metal deposition process on a foreign substrate. According to different authors [20, 31, 32], in this crossover region it is possible to study nucleation processes, and the parameters of the nucleation-growth mechanism can be obtained. At potentials more positive than −740 mV one anodic peak appeared at −548 mV due to dissolution of the cobalt previously deposited during the direct potential scan, because if the negative scan limit is shortened, the intensity of this peak decreases. Finally, between −400 mV and −100 mV the current found is very small probably due to the fact that the substrate returned to its state before the experiments.It is important to say that according to different authors [25] two current peaks were observed during cobalt dissolution from the electrode into the solution associated with dissolution of hydrogen rich cobalt phases that were previously formed during the cathodic sweep. In order to understand the nature of our peak, the curve j-E was prepared from Δf-E response and compared with the j-E curve obtained directly from the experiments, Figure 3.Figure 3
Comparison ofj-E curves obtained from Δf-E response (a) and directly from the experiment (b). The potential region scanned was −100 mV and −1000 mV, and the scan potential rate was 5 mV s−1.As may be seen the two curves are very well superimposed at potentials more positive than −850 mV, when the scan is performed towards more negative potentials. However, at potentials more negative than −850 mV the curves are quite different. This difference remains even when the potential scan is reversed until the passage of the current to anodic quadrant. It is important to mention that the two curves are completely superimposed in the dissolution peak located at −548 mV. This behavior is undoubtedly due to the fact that hydrogen formation reaction concurrent with cobalt reduction is greatly produced at potentials more negative than −850 mV, but the formation of this species does not intervene in cobalt deposit dissolution, since the two curves are almost completely superimposed at peak −548 mV. This proves that hydrogen-enriched cobalt phase is not formed, and that the deposit formed in these experiments is exclusively made up by Co species coming from soluble Co(II) species.A more careful examination of the cathodic scan of curves in Figure2 shows that there is a shoulder at −483 mV (−4.9 μA cm−2, peak A in the inset) probably associated with cobalt UPD process on the substrate given that this potential falls in the positive region with regard to Eeq. It is important to say that from the comparison between curves (a) and (b) it is clear that the peak A is indeed related to the system Co/Ag and not to the electrolyte.In order to determine the type of control limiting the peak at −483 mV, different experiments were carried out at variable scan rates, and a logarithmic curve of absolute current values associated with peak A as a function of scan rate was prepared as shown in Figure4.Figure 4
Logarithmic curve of absolute current peak (j) as a function of scan rate (v) for peak A.As can be seen, the absolute current value (|j|) of peak A increased with the scan rate increase (v), and the relationship found between both is linear with a slope of 0.5, which implies that this process is controlled by mass transport [33]. It is important to mention that this behaviour was reported by Mendoza-Huizar et al. [20] with Co/Au UPD process in the presence of chlorides due to three different contributions: an adsorption process and 2D and 3D nucleation. However, in our case it seems that NH3 species plays the most important role in the deposition mechanism.Additionally, Figure5 shows the behaviour of the cathodic peak potential (Epc) of peak A as a function of the scan rate within the range of 5–100 mV s−1. We can see that Epc shifts towards more negative potentials with an increasing scan rate as a result of the system’s irreversible behaviour [22].Figure 5
Current density curve of peak (j) as a function of the scan rate (v) for process A; the data were obtained from experiments in the conditions as in Figure 2.


### 3.3. Electromicrogravimetric Characterization of UPD and OPD Regions

Figure6 shows a typical frequency change curve (Δf) as a function of the potential scan obtained concurrently with cyclic voltammogram. This response was obtained by scanning the potential between −100 mV and −1000 mV.Figure 6
Frequency change (Δf) curves as a function of the potential for Ag/[Co2+] 1 mM, [(NH4)2SO4] 1 M system, and pH 9.3 when scanning the potential until −1050 mV (—) and −965 mV (---) at 5 mV s−1.According to this curve, during the negative scan from −100 mV to −400 mV, there is no detectable change in frequency (see inset), so the current detected in the voltammogram (Figure2) corresponds to the double-layer charging. However, a smooth variation in the frequency change is observed at potentials more negative than −400 mV but more positive than −980 mV. We think that this behavior of the change of frequency in this potential region is associated with the process of formation of the Co deposit on the substrate. It is noteworthy that at this potential (−980 mV) the change of frequency is around −10 Hz (mass increases) which makes us think that this value may be related to the mass of an incomplete monolayer. On continuing the negative scan at potentials more negative than −980 mV, a rapid decrease in frequency can be observed associated with the formation of massive deposit of Co on the monolayer. This process still continues when the scan reversal is produced at −1000 mV since the frequency keeps decreasing. Following scan reversal, the frequency remains constant between −800 mV and −600 mV until increasing (mass decreases) very rapidly in the region ca. −600 to −500 mV corresponding to anodic dissolution of Co deposit. Finally, the dissolution of Co traces on the substrate takes place partially since the frequency increases (mass decreases) slowly at potentials more positive than −500 mV until reaching almost the original value of Δf in the double-layer region.It should be emphasized that deposition processes of cobalt take place between −500 mV and −980 mV; however, the peak A is not located in this potential region, consequently it seems that this peak is associated with another process.Additional curves Δf-t were obtained at different negative potential steps (E2) which are shown in Figure 7.Responses of frequency change (Δf) as a function of time for (a) peak A region (see Figure 2) and (b) for potentials more negative than peak A potential. Bath solution was made up of [Co2+] 1 mM, [(NH4)2SO4] 1 M, and pH 9.3.
(a)
(b)
(c)These curves Δf-t show two behaviors in accordance with potential regions.(a)
E2 is more positive than −500 mV. These curves show no variations of Δf which implies that there is no variation of mass on the substrate. According to these results, peak A is not necessarily associated with the cobalt deposition process, because it is not accompanied by an important change of frequency (mass). Based on these results, it is possible to establish that the interaction between Co and Ag is not as important as to give rise to the UPD process, and thereby they can be excluded safely.(b)
E2 is more negative than −500 mV. The Δf changes slowly until Δf attains a plateau that depends on the cathodic limit potential (see Figures 7(a) and 7(b)), and this plateau is only observed when the cathodic potential is more negative than −900 mV but more positive than −980 mV (see Figure 7(c)). This behavior of Δf implies that the Co submonolayer formed may give rise to even more compact structure as has been mentioned for Pb/Au [34], for which reason Δfmax values obtained by voltammetry and chronoamperometry do not match. In addition, we assume that this plateau is associated with the total formation of a Co monolayer on the Ag substrate since the Δf  value is approximately 22 Hz (see Figure 8).Figure 8
Monitored (—) and average (---) evolution of frequency change over time when potential pulses of −980 mV for cobalt deposition and −150 mV for oxidation are imposed for 30 and 10 seconds, respectively.So the potential region in which the Co monolayer is formed on the substrate is limited by potentials more negative than −500 mV but more positive than −980 mV. According to these results, the first stages of cobalt deposit formation on the silver substrate seem not to follow an underpotential process, but rather the behavior of the Co/Au(111) system, reported by Kleinert et al. [35], who established that the initial stages of Co deposition take place by gradually decreasing the potential from −0.45 V to −0.8 V to overcome the high overpotential but avoid fast growth.


### 3.4. Effect of Ammonia and Sulfate Ion Adsorption on Silver Substrate

It has been mentioned in the literature [36, 37] that the process of sulfate or ammonia ion adsorption on a substrate may take place in the underpotential region. With the aim of obtaining more information, the adsorption of these species was studied using only the solution of supporting electrolyte.Concomitantly with the voltammogram of Figure1, the response of frequency was obtained in the absence of metal ion in solution, Figure 9.Figure 9
Frequency response as a function of potential scan for Ag/[(NH4)2SO4] 1 M system with (a) and without (b) pH adjustment obtained at a rate of 5 mV s−1.According to this curve (Figure9(a)), if the potential scan is made toward potentials more negative than −750 mV, an important decrease in frequency (increase of mass) is observed, which can be interpreted by the fact that supporting electrolyte (NH3, NH4+, and SO4-2 species) has a contribution in mass gain on the resonator, even without the presence of metal ion in the solution. However, if the same type of experiments is performed without adjusting the pH (pH = 6.5) of the solution, that is, if there are only NH4+ and SO4-2 ions, the response in frequency changes remarkably as can be seen in Figure 9(b).In this experiment, frequency variation of the unadjusted solution (in the absence of NH3, curve b) passes the quadrant of positive values (mass decrease), implying the loss of mass on the silver electrode probably due to the desorption of sulfate anions. According to this, frequency evolution toward negative values, in the curve a, is due to the adsorption of ammonia molecules on the silver substrate. This is possible because of the zero charge potential (Eq=0) of the silver substrate [38] −1000 mV, so the adsorption of a species with a pair of free electrons, such as NH3 molecule, may take place on a positively charged surface, even though the potential is in the quadrant of negative values.Now, in order to better define the contribution of ammonia in cobalt deposition, Δf curves obtained in the absence and presence of metal ion were superimposed as a function of potential, Figure 10.Figure 10
Fraction of the cyclic response of frequency change versus potential obtained at a rate of 5 mV s−1 using the following solutions: [(NH4)2SO4] 1 M (NH3 curve) and [Co2+] 1 mM + [(NH4)2SO4] 1 M (NH3−Co curve) adjusted at pH 9.3.According to these curves, in the presence of metal ion (NH3−Co curve) Δf attributed to ammonia adsorption on silver substrate is observed to be practically suppressed, and instead, there is a very small variation of the order of ten Hz which increases as the potential approaches −980 mV. This may be interpreted by the fact that ammonia adsorption on the silver substrate only takes place in the absence of metal ion at potentials more negative than −750 mV. Another possibility implies that the process of ammonia adsorption takes place in a particular potential region, whereas in another region the adsorption of cobalt atoms occurs.It has also been mentioned in the literature [23–25] that the process of cobalt deposit formation passes through formation of solid species precipitated on the electrode such as Co(OH)2; however, frequency variations detected in this work do not allow supporting this hypothesis. In addition, as will be seen further on, the intervention of NH3 species is more probable.


### 3.5. Determination of the Equivalent Molar Mass

These latter assumptions can be checked if apparent molar masses of the species adsorbed in different potential regions are determined, for which purpose curves from Figure6 were used.According to (5) resulting from the combination of Sauerbrey expression and second Faraday’s law, MM/z can be determined as
(5)Δf=(CfMMzF)ΔQ,
where MM/z is the equivalent molar mass of deposited species, and ΔQ is the charge density obtained using chronoamperometry, whereas the remaining terms keep their usual meaning.So, frequency change curve was traced as a function of charge density, Figure11, and from its slope MM/z was obtained by multiplying it with Faraday constant and sensitivity constant, as indicated by expression (5).Figure 11
(A) Chronoamperogram (a) and profile of Δf variation (b) over time, obtained by applying a potential pulse of −980 mV and using a solution formed by [Co2+] 1 mM, [(NH4)2SO4] 1 M, and Ag substrate as working electrode. (B) Frequency change diagram as a function of the charge, obtained from curves (a) and (b).Equivalent molar mass (MM/z) obtained was graphed for a wide potential range, Figure 12.Figure 12
Equivalent molar mass curve as a function of the potential applied.This figure shows that the equivalent molar mass (MM/z) adopts values dependent upon the potential region studied. Thus, between −300 mV and −600 mV, for instance, the equivalent molar mass varies between 12 and 20 g mol−1; whereas between −600 mV and approximately −950 mV, MM/z varies between 25 and 32 g mol−1. Finally, at the potential more negative than −950 mV, the MM/z values are close to 10 g mol−1.This behavior of MM/z confirms the assumptions from the above paragraphs, since in the potential region studied adsorption processes involving different species take place. For example, at potentials more positive than −600 mV, ammonia is the adsorbed species, because its equivalent molar mass is comprised between 12 and 20 g mol−1 (MM/z(NH3) = 17 g mol−1); whereas at potentials between −600 and −950 mV, the adsorbed species must be cobalt because its equivalent molar mass is comprised between 25 and 32 g mol−1 if two electrons are transferred (MM/z(Co) = 29.4 g mol−1). It is noteworthy that according to the information generated by this curve, there is no possibility of a partial charge transfer by cobalt atoms to the substrate, because the equivalent molar mass, in such case, should be superior to 30 g mol−1. Additionally, it is important to mention that equivalent molar masses above 30 g mol−1 indicative of intermediary cobalt hydroxide species, such as CoOH+ (MM/z = 37.965 g mol−1) or Co(OH)2 (MM/z = 46.465 g mol−1), were not obtained either, as mentioned by some authors for cobalt deposition in aqueous phase.All this information is summed up in Figure13 that outlines different stages of potential formation of cobalt deposit on the silver substrate.Schematic representation of cobalt underpotenial deposition process on a silver substrate, which takes into account ammonia adsorption: (a) adsorption of ammonia molecules at potentials more positive than −600 mV; (b) and (c) processes of Co underpotenial deposit formation between −600 and −920 mV; (d) process of total silver substrate covering by cobalt at potentials ranging between −920 and −980 mV.
(a)
(b)
(c)
(d)According to this diagram, before the cobalt deposition process starts, (Figure13(a)) ammonia is adsorbed on the silver substrate at potentials more positive than −600 mV. When the cobalt deposition process initiates, at potentials more negative than −600 mV, NH3 molecules are displaced from the silver substrate by metallic Co atoms (Figures 13(b) and 13(c)). Finally, silver substrate is completely covered by Co monolayer at potentials between −920 and −980 mV (Figure 13(d)).


## 3.1. Voltammetric Characterization of a Silver Substrate

Figure1 shows a cyclic voltammogram (j-E) obtained at an electrode of quartz crystal modified with Ag film in electrolytic solution. This voltammogram has some characteristics that indicate the absence of faradaic processes since the very small current observed between −100 mV and −1000 mV corresponds to charging of the electrical double layer, and this feature is a criterion for the cleanliness of the surface of our substrates. Only when the potential is scanned at values more negative than −950 mV a cathodic current associated with hydrogen evolution is observed.Figure 1
Voltammogram of Ag/[(NH4)2SO4] 1 M system at pH 9.3 obtained at a scan rate of 5 mV s−1.


## 3.2. Voltammetric Characterization of UPD and OPD Zones

With the purpose to identify the processes that take place in the UPD and OPD region of the Co/Ag system, a large potential region was scanned using metal solution. In Figure2 a comparison is shown of the experimental voltammograms obtained at the silver electrode in both solutions, without (a) and with (b) Co(II) ions in solution.Figure 2
A comparison of two cyclic voltammetric curves obtained in the Ag/xM Co(II)+1 M (NH4)2SO4 (pH 9.3) system at two different Co(II) concentrations, (a) x= 0 and (b) x= 1 mM. The scan potential rate was of 5 mV s−1, and the potential interval was −100 mV and −990 mV. In the inset an amplification of the region comprising the peak of the alleged underpotential deposition is shown.The potential region, in Figure2(b), was scanned between –100 mV and –1000 mV. The potential scan started at −100 mV up to −1000 mV, and then it was reversed to the initial value. During the direct scan it can be noted that the cathodic current only increases when the potential is more negative than −980 mV, and this tendency still continues upon scan reversal. This current is associated with the process of cobalt deposit formation on the silver substrate because the potential region explored is more negative than the equilibrium potential (Eeq=-741mV) [20] which is known as overpotential region (OPD). In addition, in this same potential region the current measured must have a fraction associated with hydrogen evolution reaction.In the reverse potential scan, one crossover of the cathodic and anodic branches at −740 mV is observed which is typical of the metal deposition process on a foreign substrate. According to different authors [20, 31, 32], in this crossover region it is possible to study nucleation processes, and the parameters of the nucleation-growth mechanism can be obtained. At potentials more positive than −740 mV one anodic peak appeared at −548 mV due to dissolution of the cobalt previously deposited during the direct potential scan, because if the negative scan limit is shortened, the intensity of this peak decreases. Finally, between −400 mV and −100 mV the current found is very small probably due to the fact that the substrate returned to its state before the experiments.It is important to say that according to different authors [25] two current peaks were observed during cobalt dissolution from the electrode into the solution associated with dissolution of hydrogen rich cobalt phases that were previously formed during the cathodic sweep. In order to understand the nature of our peak, the curve j-E was prepared from Δf-E response and compared with the j-E curve obtained directly from the experiments, Figure 3.Figure 3
Comparison ofj-E curves obtained from Δf-E response (a) and directly from the experiment (b). The potential region scanned was −100 mV and −1000 mV, and the scan potential rate was 5 mV s−1.As may be seen the two curves are very well superimposed at potentials more positive than −850 mV, when the scan is performed towards more negative potentials. However, at potentials more negative than −850 mV the curves are quite different. This difference remains even when the potential scan is reversed until the passage of the current to anodic quadrant. It is important to mention that the two curves are completely superimposed in the dissolution peak located at −548 mV. This behavior is undoubtedly due to the fact that hydrogen formation reaction concurrent with cobalt reduction is greatly produced at potentials more negative than −850 mV, but the formation of this species does not intervene in cobalt deposit dissolution, since the two curves are almost completely superimposed at peak −548 mV. This proves that hydrogen-enriched cobalt phase is not formed, and that the deposit formed in these experiments is exclusively made up by Co species coming from soluble Co(II) species.A more careful examination of the cathodic scan of curves in Figure2 shows that there is a shoulder at −483 mV (−4.9 μA cm−2, peak A in the inset) probably associated with cobalt UPD process on the substrate given that this potential falls in the positive region with regard to Eeq. It is important to say that from the comparison between curves (a) and (b) it is clear that the peak A is indeed related to the system Co/Ag and not to the electrolyte.In order to determine the type of control limiting the peak at −483 mV, different experiments were carried out at variable scan rates, and a logarithmic curve of absolute current values associated with peak A as a function of scan rate was prepared as shown in Figure4.Figure 4
Logarithmic curve of absolute current peak (j) as a function of scan rate (v) for peak A.As can be seen, the absolute current value (|j|) of peak A increased with the scan rate increase (v), and the relationship found between both is linear with a slope of 0.5, which implies that this process is controlled by mass transport [33]. It is important to mention that this behaviour was reported by Mendoza-Huizar et al. [20] with Co/Au UPD process in the presence of chlorides due to three different contributions: an adsorption process and 2D and 3D nucleation. However, in our case it seems that NH3 species plays the most important role in the deposition mechanism.Additionally, Figure5 shows the behaviour of the cathodic peak potential (Epc) of peak A as a function of the scan rate within the range of 5–100 mV s−1. We can see that Epc shifts towards more negative potentials with an increasing scan rate as a result of the system’s irreversible behaviour [22].Figure 5
Current density curve of peak (j) as a function of the scan rate (v) for process A; the data were obtained from experiments in the conditions as in Figure 2.


## 3.3. Electromicrogravimetric Characterization of UPD and OPD Regions

Figure6 shows a typical frequency change curve (Δf) as a function of the potential scan obtained concurrently with cyclic voltammogram. This response was obtained by scanning the potential between −100 mV and −1000 mV.Figure 6
Frequency change (Δf) curves as a function of the potential for Ag/[Co2+] 1 mM, [(NH4)2SO4] 1 M system, and pH 9.3 when scanning the potential until −1050 mV (—) and −965 mV (---) at 5 mV s−1.According to this curve, during the negative scan from −100 mV to −400 mV, there is no detectable change in frequency (see inset), so the current detected in the voltammogram (Figure2) corresponds to the double-layer charging. However, a smooth variation in the frequency change is observed at potentials more negative than −400 mV but more positive than −980 mV. We think that this behavior of the change of frequency in this potential region is associated with the process of formation of the Co deposit on the substrate. It is noteworthy that at this potential (−980 mV) the change of frequency is around −10 Hz (mass increases) which makes us think that this value may be related to the mass of an incomplete monolayer. On continuing the negative scan at potentials more negative than −980 mV, a rapid decrease in frequency can be observed associated with the formation of massive deposit of Co on the monolayer. This process still continues when the scan reversal is produced at −1000 mV since the frequency keeps decreasing. Following scan reversal, the frequency remains constant between −800 mV and −600 mV until increasing (mass decreases) very rapidly in the region ca. −600 to −500 mV corresponding to anodic dissolution of Co deposit. Finally, the dissolution of Co traces on the substrate takes place partially since the frequency increases (mass decreases) slowly at potentials more positive than −500 mV until reaching almost the original value of Δf in the double-layer region.It should be emphasized that deposition processes of cobalt take place between −500 mV and −980 mV; however, the peak A is not located in this potential region, consequently it seems that this peak is associated with another process.Additional curves Δf-t were obtained at different negative potential steps (E2) which are shown in Figure 7.Responses of frequency change (Δf) as a function of time for (a) peak A region (see Figure 2) and (b) for potentials more negative than peak A potential. Bath solution was made up of [Co2+] 1 mM, [(NH4)2SO4] 1 M, and pH 9.3.
(a)
(b)
(c)These curves Δf-t show two behaviors in accordance with potential regions.(a)
E2 is more positive than −500 mV. These curves show no variations of Δf which implies that there is no variation of mass on the substrate. According to these results, peak A is not necessarily associated with the cobalt deposition process, because it is not accompanied by an important change of frequency (mass). Based on these results, it is possible to establish that the interaction between Co and Ag is not as important as to give rise to the UPD process, and thereby they can be excluded safely.(b)
E2 is more negative than −500 mV. The Δf changes slowly until Δf attains a plateau that depends on the cathodic limit potential (see Figures 7(a) and 7(b)), and this plateau is only observed when the cathodic potential is more negative than −900 mV but more positive than −980 mV (see Figure 7(c)). This behavior of Δf implies that the Co submonolayer formed may give rise to even more compact structure as has been mentioned for Pb/Au [34], for which reason Δfmax values obtained by voltammetry and chronoamperometry do not match. In addition, we assume that this plateau is associated with the total formation of a Co monolayer on the Ag substrate since the Δf  value is approximately 22 Hz (see Figure 8).Figure 8
Monitored (—) and average (---) evolution of frequency change over time when potential pulses of −980 mV for cobalt deposition and −150 mV for oxidation are imposed for 30 and 10 seconds, respectively.So the potential region in which the Co monolayer is formed on the substrate is limited by potentials more negative than −500 mV but more positive than −980 mV. According to these results, the first stages of cobalt deposit formation on the silver substrate seem not to follow an underpotential process, but rather the behavior of the Co/Au(111) system, reported by Kleinert et al. [35], who established that the initial stages of Co deposition take place by gradually decreasing the potential from −0.45 V to −0.8 V to overcome the high overpotential but avoid fast growth.


## 3.4. Effect of Ammonia and Sulfate Ion Adsorption on Silver Substrate

It has been mentioned in the literature [36, 37] that the process of sulfate or ammonia ion adsorption on a substrate may take place in the underpotential region. With the aim of obtaining more information, the adsorption of these species was studied using only the solution of supporting electrolyte.Concomitantly with the voltammogram of Figure1, the response of frequency was obtained in the absence of metal ion in solution, Figure 9.Figure 9
Frequency response as a function of potential scan for Ag/[(NH4)2SO4] 1 M system with (a) and without (b) pH adjustment obtained at a rate of 5 mV s−1.According to this curve (Figure9(a)), if the potential scan is made toward potentials more negative than −750 mV, an important decrease in frequency (increase of mass) is observed, which can be interpreted by the fact that supporting electrolyte (NH3, NH4+, and SO4-2 species) has a contribution in mass gain on the resonator, even without the presence of metal ion in the solution. However, if the same type of experiments is performed without adjusting the pH (pH = 6.5) of the solution, that is, if there are only NH4+ and SO4-2 ions, the response in frequency changes remarkably as can be seen in Figure 9(b).In this experiment, frequency variation of the unadjusted solution (in the absence of NH3, curve b) passes the quadrant of positive values (mass decrease), implying the loss of mass on the silver electrode probably due to the desorption of sulfate anions. According to this, frequency evolution toward negative values, in the curve a, is due to the adsorption of ammonia molecules on the silver substrate. This is possible because of the zero charge potential (Eq=0) of the silver substrate [38] −1000 mV, so the adsorption of a species with a pair of free electrons, such as NH3 molecule, may take place on a positively charged surface, even though the potential is in the quadrant of negative values.Now, in order to better define the contribution of ammonia in cobalt deposition, Δf curves obtained in the absence and presence of metal ion were superimposed as a function of potential, Figure 10.Figure 10
Fraction of the cyclic response of frequency change versus potential obtained at a rate of 5 mV s−1 using the following solutions: [(NH4)2SO4] 1 M (NH3 curve) and [Co2+] 1 mM + [(NH4)2SO4] 1 M (NH3−Co curve) adjusted at pH 9.3.According to these curves, in the presence of metal ion (NH3−Co curve) Δf attributed to ammonia adsorption on silver substrate is observed to be practically suppressed, and instead, there is a very small variation of the order of ten Hz which increases as the potential approaches −980 mV. This may be interpreted by the fact that ammonia adsorption on the silver substrate only takes place in the absence of metal ion at potentials more negative than −750 mV. Another possibility implies that the process of ammonia adsorption takes place in a particular potential region, whereas in another region the adsorption of cobalt atoms occurs.It has also been mentioned in the literature [23–25] that the process of cobalt deposit formation passes through formation of solid species precipitated on the electrode such as Co(OH)2; however, frequency variations detected in this work do not allow supporting this hypothesis. In addition, as will be seen further on, the intervention of NH3 species is more probable.


## 3.5. Determination of the Equivalent Molar Mass

These latter assumptions can be checked if apparent molar masses of the species adsorbed in different potential regions are determined, for which purpose curves from Figure6 were used.According to (5) resulting from the combination of Sauerbrey expression and second Faraday’s law, MM/z can be determined as
(5)Δf=(CfMMzF)ΔQ,
where MM/z is the equivalent molar mass of deposited species, and ΔQ is the charge density obtained using chronoamperometry, whereas the remaining terms keep their usual meaning.So, frequency change curve was traced as a function of charge density, Figure11, and from its slope MM/z was obtained by multiplying it with Faraday constant and sensitivity constant, as indicated by expression (5).Figure 11
(A) Chronoamperogram (a) and profile of Δf variation (b) over time, obtained by applying a potential pulse of −980 mV and using a solution formed by [Co2+] 1 mM, [(NH4)2SO4] 1 M, and Ag substrate as working electrode. (B) Frequency change diagram as a function of the charge, obtained from curves (a) and (b).Equivalent molar mass (MM/z) obtained was graphed for a wide potential range, Figure 12.Figure 12
Equivalent molar mass curve as a function of the potential applied.This figure shows that the equivalent molar mass (MM/z) adopts values dependent upon the potential region studied. Thus, between −300 mV and −600 mV, for instance, the equivalent molar mass varies between 12 and 20 g mol−1; whereas between −600 mV and approximately −950 mV, MM/z varies between 25 and 32 g mol−1. Finally, at the potential more negative than −950 mV, the MM/z values are close to 10 g mol−1.This behavior of MM/z confirms the assumptions from the above paragraphs, since in the potential region studied adsorption processes involving different species take place. For example, at potentials more positive than −600 mV, ammonia is the adsorbed species, because its equivalent molar mass is comprised between 12 and 20 g mol−1 (MM/z(NH3) = 17 g mol−1); whereas at potentials between −600 and −950 mV, the adsorbed species must be cobalt because its equivalent molar mass is comprised between 25 and 32 g mol−1 if two electrons are transferred (MM/z(Co) = 29.4 g mol−1). It is noteworthy that according to the information generated by this curve, there is no possibility of a partial charge transfer by cobalt atoms to the substrate, because the equivalent molar mass, in such case, should be superior to 30 g mol−1. Additionally, it is important to mention that equivalent molar masses above 30 g mol−1 indicative of intermediary cobalt hydroxide species, such as CoOH+ (MM/z = 37.965 g mol−1) or Co(OH)2 (MM/z = 46.465 g mol−1), were not obtained either, as mentioned by some authors for cobalt deposition in aqueous phase.All this information is summed up in Figure13 that outlines different stages of potential formation of cobalt deposit on the silver substrate.Schematic representation of cobalt underpotenial deposition process on a silver substrate, which takes into account ammonia adsorption: (a) adsorption of ammonia molecules at potentials more positive than −600 mV; (b) and (c) processes of Co underpotenial deposit formation between −600 and −920 mV; (d) process of total silver substrate covering by cobalt at potentials ranging between −920 and −980 mV.
(a)
(b)
(c)
(d)According to this diagram, before the cobalt deposition process starts, (Figure13(a)) ammonia is adsorbed on the silver substrate at potentials more positive than −600 mV. When the cobalt deposition process initiates, at potentials more negative than −600 mV, NH3 molecules are displaced from the silver substrate by metallic Co atoms (Figures 13(b) and 13(c)). Finally, silver substrate is completely covered by Co monolayer at potentials between −920 and −980 mV (Figure 13(d)).


## 4. Conclusions

The initial stages of cobalt deposition process on a silver substrate were studied using cyclic voltammetry and chronoamperometry coupled with quartz microbalance in ammonia solution. The results obtained showed that during the Co deposit formation process on a silver substrate, no process of underpotential deposition is observed, even though the cobalt forms a monolayer on the substrate which starts from −600 mV to −980 mV. During this process, the cobalt transfers its two electrons towards the electrode from soluble, and not solid species such as Co(OH)2. Furthermore, it was found that at potentials more positive than −600 mV, ammonia adsorption takes place on the substrate’s surface, and the above species leave its surface as this is occupied by cobalt.



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*Source: 624163-2013-01-31.xml*