1. IntroductionThe Electroless plating method for the deposition of dense films over porous substrates has recently assumed increasing importance and wider applications in the fabrication of composite Pd and Pd—alloy membranes for hydrogen production, separation and purification [1]. Some of the several advantages the electroless plating method has over other methods include its uniformity and easiness of coating over any surface of any shape, no energy supplies required, low cost, simple equipment as shown in Figure 1 and it also avoids accumulation of the deposits around the substrate edges to ensure in uniformity of coating [1]. However, it also has its drawbacks such as its time consuming procedure as a result of the several treatment steps involved [2].
Hydrogen production and purification using the novel membrane reactor module is gaining considerable attention due to the process intensification concept potential of the membrane reactor to integrate hydrogen separation and reaction in a single unit [3]. This unique ability of the membrane reactor enables an improved performance to be achieved such as an increase in reactant conversion and product selectivity through the removal of one of the products in a dehydrogenation reaction or to perform a hydrogenation reaction by dousing hydrogen through the membrane [3] [4]. This concept can be used in steam methane reforming and other hydrocarbon reactions and it offers several benefits in terms of increasing product conversions and cost reduction [5]. Palladium membranes have infinite selectivity for hydrogen due to their ability to transport hydrogen which is as a result of the very high solubility of hydrogen in the bulk over very wide temperature ranges [2]. In palladium based membrane reactors, palladium membranes can be used in an equilibrium limited reaction to remove one of these products and increase the conversion or to selectively saturate hydrogen through the membrane although in both scenarios, palladium has a catalytic function [4]. Ultra pure hydrogen is in demand and widely used in petroleum and petrochemical industries such as in petroleum refining, production of ammonia and methanol [6] [7]. However, more recently, advances in polymer electrolyte membrane fuel cell (PEMFC) for both stationary and vehicular applications has led to a surge in demand for ultra pure hydrogen [8].
Palladium membranes are the membranes of choice for hydrogen because they permeate only hydrogen when dense [5]. In decades past, thick palladium films in standalone forms were used with a thickness ranging from 10 µm - 200 µm and low hydrogen permeance, high cost and lacking the mechanical and thermal strength to withstand harsh operating conditions such as high temperature [2].
As a result of the challenges caused by the standalone thin palladium films, the focus has now shifted to composites where a thin palladium layer is deposited on porous support. These composites have several advantages over thin films including high hydrogen permeance as a result of the very low resistance to hydrogen permeation, high mechanical strength and low cost [2]. Thin palladium films with different thickness are produced using various methods of membrane fabrication such as chemical vapor deposition, electroplating, magnetron sputtering and electrochemical deposition. However, electroless plating is widely regarded as the most efficient and convenient method for preparation of composite palladium membranes because of its uniformity of coating [2]. The mechanism of electroless plating for the fabrication of palladium-based composite membranes has been well investigated and the experience is that the method has a near perfect throwing power due to its applicability in both conducting and nonconducting surfaces and is applicable as long as the plating solution has access to the substrate surface [1]. The method enjoys an ever-growing popularity due to the several advantages it enjoys over other methods including uniform coating, low cost, strong adhesion of the metallic layer on the substrate, simple equipment and procedure [9]. Electroless plating also avoids a build-up of the solution on the substrate edges thus resulting in a uniform and dense coating [1]. In the preparation of composite membranes using the electroless plating method, a porous support such as stainless steel, Vycor glass and alumina is required onto which a dense metallic film is deposited [2]. Ceramic alumina supports are usually preferred due to their stability at high temperature and pressure and also their uniform pore distribution which enhances the fabrication of defect-free membranes [2]. The quality of deposits and cost implications of the electroless plating process depends on several process factors which include operating temperature, plating time, plating area, concentration of reducing agents, pH, stabilising agents, and additives [10] [11]. The broader applicability and overall efficiency of the electroless plating method depends on the optimisation of these factors to improve both the uniformity of coating and quality of the metallic film deposits [11]. In the conventional electroless plating process, the major problem is how to achieve uniform densification of the palladium layer and also prevent mass transfer from the film into the solution. However, optimisation of these process factors is one critical way of ameliorating the mass transfer problem in the conventional electroless plating [8] [9].
This overview critically discuss the effects of the process factors on plating rate and efficiency of the electroless plating of Palladium-based membranes on porous support and the areas requiring further investigation. The scope of this paper is relevant especially considering the growing significance of membrane technology in hydrogen processes including its production, separation and purification for PEM fuel cell systems and also in several processes such as chemical synthesis, hydrogenation, semiconductor and manufacturing in the petroleum and petrochemical industry [12] [13].
The need for a better understanding and optimisation of the electroless plating method is more so when juxtaposed with the critical challenge of how to prepare thin, dense, uniformly coated and defect free Pd-based composite membranes that are selective to hydrogen and have long term durability [14]. To my knowledge, so far there has not been a review of the effect of these process factors on the efficiency of the electroless plating process.
The steps in electroless plating depend on the type of support but generally involve cleaning of the substrate, surface modification (which is usually a 2 step process of sensitization and activation), deposition of the palladium layer, drying and annealing of the membrane to activate the palladium layer [10]. The cleaning step is meant to remove any organic contaminants and to chemically prepare the substrate for the sensitization and activation steps and involves washing the substrate in an ultrasonic bath at temperatures 60˚C - 70˚C with distilled water and ethanol/isopopanol followed by drying at temperatures between 120˚C - 130˚C [7] [10].
Sensitization and ActivationPrior to the deposition of the metal on the support, the sensitization and activation steps are carried out on the porous ceramic substrate so as to create catalytic sites on the non-metallic surfaces and to also stimulate the adsorption of the metal ions, enhance strong adhesion of the Pd nuclei on the substrate and eliminate induction period of the metal to ensure better uniformity of coating and improved membrane quality [9] [15]. A picture of the Alumina ceramic support is shown in Figure 2.
Several sensitization solutions have been used such as SnCl2, AgNO3, metallic Na in Naphthalene solution and AuCl3. However, the most commonly used is SnCl2 while PdCl2 is typically used as the activation solution to deposit Nano-sized Pd nuclei on the porous substrate [15] [16]. Although surface activation is a standard requirement in electroless plating, it has its downside such as its time consuming nature, tin impurities, metal loss, and difficulty in control of film thickness and involves several steps which make it prone and susceptible to errors [7] [16].
Palladium can coexist with Tin during the sensitization step and this could affect the activity of Palladium towards hydrazine reducer thus slowing the rate of reaction and leading to a decrease in the deposition rate of the Pd metal [1] [7]. On the upside, it creates catalytic sites and also reduces the time it takes for the commencement of the deposition of palladium seeds onto the porous support which is also known as the induction period [15]. The pre-treatment steps to
deposit Pd nuclei onto the substrate also reduce the induction period and improves the plating efficiency [15]. The several steps and components of the electroless plating set up are shown in Figure 3.
K. L. Yeung and coworkers (1999) [15] compared the deposition rate of a clean support with the rate in a sensitized and activated support and reported a reduction in the induction period of up to 20 minutes for the palladium activated support.
Similar findings were reported by T. N. Khoperia (2003) [17] who investigated the effect of sensitization in electroless plating of Ni-P alloy and reported a decrease in the induction period and uniform coating after sensitization which underscores the relevance of sensitization during surface modification in electroless plating. Without activation, the induction time for 1 hour plating could be as much as between 20 - 45 minutes [15]. A longer induction time could affect the plating rate and lead to low plating efficiency and uneven coating which amplifies the need to identify a plating bath composition that could lead to minimal induction period in order to achieve high plating efficiency and improved quality of the Palladium film [15] [17].
The sensitization and activation cycle has been reported to be typically as follows [15] [16] :
1) Substrate dipped for 2 minutes in the solution and rinsed for 30 seconds in distilled water.
2) Substrate dipped in the activation solution for 2 minutes and rinsed for 30 seconds in distilled water.
The above procedure is repeated 10 times to obtain an evenly seeded support [7] [16]. Several authors reported a cycle of 10 dips in both solutions at a dipping time of 5 minutes each for the sensitization and activation solutions followed by rinsing in distilled water for about 25 seconds [7] [16].
The electroless plating process is also time consuming and the time between dips also adds to the cumbersome nature of the electroless process and makes it prone to errors and impurities [7]. To solve these problems, Li Anwu and coworkers (1996) [7] used a modified method where the sensitization step was skipped which avoided the tin impurities, improved the rate of palladium deposition and the metal adhesion to the porous support. In their work, this group of workers modified the γ-AlOOH sol with PdCl2 solution and deposited same on the porous Alumina support which ensured that the Pd seeds will be deposited on the surface of the substrate directly without having to carry out the prolonged
activation process [7]. Furthermore, the skipping of the sensitization step ensured that no Sn (11) solution was used and hence no tin impurities are likely to be formed [7].
In a similar trend, Zhao and his group (1998) [18] reported another modified method where the γ-alumina support was activated by a palladium-modified AlOOH sol. This method produced a smooth surface free of pinholes and defects and effectively avoided the impurities associated with the sensitization step. However, it involved complex and lengthy procedures such as drying the gel-coatings for 48 hours, calcination at 600˚C and reduction of the substrate in hydrogen at 500˚ [18]. Modifying the support with a palladium modified AlOOH sol will ensure there are enough Palladium nuclei to create catalytic sites on the porous support [19].
Li Na XU et al. (2002) [20] also developed a modified method for electroless plating without the SnCl2 sensitization which effectively avoided the Sn (11) impurities. In their work Li Na Xu and his group activated the surface of silicon wafers with palladium nuclei by forming a covalently bonded self assembled monolayers (SAMs) of aminopropyltriethoxysilane (APTS) on the silicon surface and then activated the substrate with PdCl2 solution. Apart from skipping the sensitization step, this method also enhanced the adhesion of the deposited metal and also avoided the usual surface roughening problems [20]. Figure 4 shows the SEM images of the outer, inner and cross sectional area taken after sensitization and activation of the Al2O3 support in Alkali and Gobina’s work on Electroless plating of palladium on Al2O3 ceramic support. Figure 4(c) shows flowery pores and a uniform growth of the Pd nuclei which enhances the formation of the Pd layer after the plating process with strong adhesion to the substrate [15].
2. Review of Electroless Plating Process Factors2.1. Reducing AgentThe common reducing agents used for the electroless plating of palladium and palladium alloy membranes are hydrazine, hydrophosphite, borohydride, dimethylamine boron and formaldehyde [21]. However, hydrazine and hyphoposphite are the more commonly used while formaldehyde is more commonly used in electroless copper plating [21] [22]. Although, hydrazine results in a better plating efficiency and was the first reducing agent to be used in the first electroless plating bath developed by Rhoda in 1958 but being a class-11 carcinogen, it has its obvious drawbacks which makes hyphoposphite also highly considered [22]. Apart from the advantage of not being susceptible to bulk precipitation, hypophosphite also has the advantage of maintaining a constant plating rate for a longer plating time and this is necessary for uniformity of coating and high quality Palladium deposits [22].
In the electroless plating of palladium in a hydrazine based bath, the redox reaction can be represented as follows [15] :
2Pd ( NH 3 ) 4 2 + + 4e − → 2Pd 0 + 8NH 3 E 0 = 0.0 V
N 2 H 4 + 4OH − → N 2 + 4H 2 O + 4e − E 0 = 1 . 12V
2Pd ( NH 3 ) 4 2 + + N 2 H 4 + 4OH − → 2Pd 0 + 8NH 3 + N 2 + 4H 2 OE = 1 . 12V
The electrons released during the reaction are used in the decomposition of the palladium amine complex to palladium and ammonia gas with the deposition rate increasing with the number of available Palladium sites [15].
K. L. Yeung et al. (1999) (15) reported that the plating rate is dependant upon the concentration of palladium and the reducing agent. Yeung and his group [15] investigated the plating kinetics in electroless plating of thin supported Pd membranes and reported that the plating rate increased with increasing concentration of both the hydrazine reducer and palladium. However, excess concentration of the hydrazine reducer could lead to bulk precipitation of the Palladium metal [15] [22]. The plating rate reported by this group after I hour of plating and also the rate reported by Collins and Way (1993) [23] were between 1 and 3 µm/hr at 320 - 360 K with hydrazine and palladium precursor concentration of 10 mL/L (1 M) and 3 - 5.5 g/L respectively. Collins and Way (1993) [23] reported that the plating rate significantly reduced after 1 hour plating time as a result of bulk decomposition of hydrazine by palladium.
Hydrazine is known to decompose rapidly in the presence of palladium [15]. Yeung et al. [15] also reported that increasing the concentration of the hydrazine from 1.5 to 10 mM increases the plating efficiency from 0.16 to 0.65. They demonstrated that at different hydrazine concentrations of 1.5, 3.3 and 10 mM, Pd film thickness of ~0.5, ~0.9 and ~1.75 µm were achieved respectively. However, the plating efficiency began to decrease from 0.72 to 0.66 and 0.55 with the increase in the concentration of palladium from 5.1 to 10.2 to 20.2 mM respectively [15]. This indicates that excessive concentration of palladium could result in low plating efficiency and low quality of deposits hence it is necessary to establish the optimum hydrazine concentration to achieve stability of the plating bath [15]. In a similar investigation carried out by Y. S. Cheng (1999) [24] on Pd/Ag codeposition, high quality Palladium deposits were obtained at hydrazine concentration of up to 20 mM and Ag content of 25 at%.
B. K. R. Nair et al. (2007) [25] also reported an increase in the plating rate with increasing concentration of Palladium and hydrazine. The maximum plating rate reported by B. K. R. Nair is 1.4 µm/h which is in line with the findings of the Collins and Way group [23].
It has been reported that the concentration of hydrazine is the limiting factor in determining the plating rate and efficiency of the electroless plating method for palladium-based membranes [15]. Some investigations carried out [15] [23] have shown that bulk precipitation is likely to occur at concentrations above 10 mM as demonstrated by K. L. Yeung and coworkers (1999) [15].
Further investigations are necessary to provide a better understanding in terms of the effect of some of the operating conditions such as pH of plating bath, plating time and NH4OH on the effect of this bulk precipitation over a wide range of N2H4 concentrations [26]. To ameliorate the problem of bulk precipitation in hydrazine-based plating baths K. L. Yeung et al. (1999) [15] suggested adding hydrazine in two equal portions with the first portion added at the commencement of the plating while the second portion is added midway during the plating.
This group reported an increase of 0.13 in the plating efficiency when a solution containing 10.2 mM (Pd) and 10 mM (N2H4) is added in 2 equal portions as compared to the plating efficiency when all the solution was added at once [15]. Since this group of workers used 2 equal portions of the hydrazine solution, what is required now is further investigation by varying the portions of the hydrazine solution into 3 or more in order to establish a concentration profile of these portions that results in an improved or optimum plating efficiency. Also, Yeung et al. [15] didn’t establish the effect of other variables such as plating temperature, time and concentration of EDTA and NH4OH when hydrazine is added in portions. Moreover there is the propensity that addition of separate portions of the hydrazine could lead to separate layers and uneven coating which could affect the quality of the palladium film.
2.2. pH of the Plating BathA constant pH of the plating solution should be maintained throughout the electroless plating process due to its effect on various phenomena that are associated with the metal-solution interface [26]. These phenomena include adsorption, structure of ions in the solution and the ionic strength of the gsolution which affects the plating rate and efficiency [17] [26]. The pH also affects the anodic and the pH on the anodic reaction where the reaction precedes charge transfer in the hypophosphite plating bath as represented in the following reactions [26] :
H 2 PO 2 − → HPO 2 − + H
( HPO 2 ) − + OH − → ( HPO 2 OH ) − + 1e −
It should be noted that a higher pH could lead to high plating rates and “plate-out” thus causing rough coating while a low pH could lead to low plating rates thus causing dull and uneven coating [15]. In another related investigation, F. Hanna et al. (2003) [21] reported an increase in the deposition rate of copper at 30˚C and 50˚C for the tartarate and EDTA baths up to pH 12.5 for tartarate bath and 13.0 for the EDTA bath. Above these pH values, the rate of deposition of the Pd film decreases. F. Hanna et al. [21] attributed this decrease to the decomposition of the OH− ions through the hydrolysis of formaldehyde to methylene glycol and the subsequent formation of formate ions through the oxidation of methylene glycol. The reaction at pH 12 and below can be represented as follows [21] :
Cu 2 + + 2HCHO + 4OH − → Cu 0 + H 2 + 2H 2 O + 2HCOO −
While the reaction at pH 12.5 and above can be represented as follows:
HCHO + OH − → CH 2 ( OH ) O −
CH ( OH ) O − + OH − → CHOO − + H 2 O + e −
Alkaline baths were reported to have higher deposition rate but decrease stability while acidic baths were observed to exhibit better adhesion characteristics particularly to stainless steel supports [1]. From the investigations conducted on the effect of pH of the plating bath on plating rate and efficiency, it can be construed that there is paucity of knowledge on the effect of pH of the plating bath in relation to other factors such as plating time and temperature. Most of the work on pH in electroless plating were carried out on the effect of pH on plating rate and not much was done on the effect of pH on the morphology of the deposits.
2.3. Plating Bath TemperatureThe plating bath temperature should be maintained at desired levels using certified thermometers in order to obtain consistent, uniform and high quality deposition [1]. The effect of bath temperature is related to the decomposition of the reducing agent in the plating bath and the plating efficiency increases with increase in the plating temperature [27]. However, at an optimum temperature, the plating efficiency starts to decrease due to the increase in the rate of decomposition of the reducing agent [15] [27]. The temperature range for optimum plating stability was reported by several authors [15] [21] to be in the range of 50˚C - 80˚C but never to exceed 90˚C to avoid bath decomposition or solution ‘Plate out’ [15]. However, the effect of temperature is also dependant on the stabilising agent in the bath since stabilising agents such as EDTA control the plating efficiency against temperature changes [15].
The stabilising agents ensure that temperature changes do not lead to excessive decomposition rates of the reducing agent up to the optimum temperature [15]. The control of these temperature changes depends on the type of stabilising agent and the composition of the plating bath [15] [26]. In this regard, Hanna and coworkers [21] used formaldehyde plating bath in the electroless plating of copper and reported an increase in the plating efficiency with increasing temperature.
This group used both EDTA and Tartarate plating baths. In the EDTA plating bath, the temperature was stable up to 70˚C and the plating efficiency increased with temperature up to 70˚C, after which it begins to decrease. For the tartarate bath, above 50˚C, the plating efficiency begins to reduce due to the rapid decomposition of the tartarate complexing agent. This indicates that the EDTA-bath has a stronger complexing ability compared to the tartarate-bath [21]. For electroless copper plating, the optimum temperatures were reported to be 50˚C for the tartarate bath and 30˚C for the EDTA bath [21]. Shin-Kun Ryi et al. (2010) [13] discovered that bulk precipitation occurred at 35˚C thereby leading to instability of the plating solution which is as a result of the absence of the EDTA stabilising agent in the solution. The absence of the stabilising agent was the reason for the decomposition of the plating solution at a comparably lower temperature of 35˚C which indicates that higher concentration of the stabilising agent could reduce the risk of bulk precipitation at high temperature [13].
The effect of plating bath temperature on the membrane morphology was also investigated by several authors including Shin-Kun Ryi et al. (2010) [13] who used electroless plating to deposit a 7.5 µm palladium film onto porous hastlerooy in an EDTA free bath. Ryi’s group [13] investigated the effect of plating bath temperature at 20˚C, 30˚C and 35˚C on the surface morphology of the membrane and showed that grain size increases with temperature. Since larger grain sizes have better permeation then it follows that higher plating temperatures result in better membrane quality [13]. Ryi’s group [13] showed that the bulk grains at 35˚C were found to be smaller than the 20˚C and 30˚C baths but the surface grain size at 35˚C was larger than those of the lower temperature. This is in concurrence with the findings of R. K. B Nair (2007) and his group [25] who synthesized palladium membranes on hollow fibres and reported a smaller grain sizes for lower plating bath temperatures. This group reported that a 23˚C plating bath has a lower grain size—0.5 - 1 µm—compared to a 50˚C plating bath which has a grain size of 1 - 2 µm. This implies that a lower bath temperature leads to smaller grain sizes and since smaller grain sizes lead to better coating, then it follows that lower bath temperature will produce more hydrogen permeable membranes [25] [27]. The SEM images of the membranes after plating at 293, 303 and 308 K are shown in Figures 4(a)-(c) respectively and it can be from the images that the surface grain size became smaller and more uniform with decrease in the plating temperature while the bulk grains became smaller with increasing temperature [13].
2.4. Air ExposureAir purges were initially used in surface cleaning during electroless plating of Pd and Pd alloy membranes but the method is increasingly becoming relevant in improving plating efficiency and quality of deposits [28].
Generally, the main contribution of air exposure has been reported to be in increasing the surface area and morphological changes to improve plating efficiency [21] [28]. A steady stream of air bubble through the plating solution has been reported to be the most common stabilizer for electroless copper plating baths [12]. In their work, Hanna and coworkers (2003) [21] investigated the effect of aeration on electroless plating bath with and without additives and reported an increase in the decomposition time to about 20 times than the baths without aeration which they attributed to the reoxidation of cuprous ion during the redox reaction at higher pH values by the formaldehyde reducer [21].
A similar finding was also reported by F. Roa and D. Way (2005) [28] who investigated
the effect of air exposure on Pd/Cu composite membranes. Although the air aeration was performed after the plating of the membrane, nonetheless it provides a better understanding of the effect of air exposure in improving membrane quality. F. Roa and Way [28] reported that the air exposure at higher temperatures led to oxidation of the palladium film to produce PdO which created more surface area for enhanced film deposition. Most of the work done on the effect of air aeration is in palladium-copper membranes hence there is paucity of knowledge on the effect of air aeration at various temperatures in palladium and palladium-alloy. Further work on the effect of air aeration in electroless plating will be relevant in optimisation of the electroless plating process to improve the plating rate and efficiency.
2.5. Plating Bath TemperatureThe plating rate and efficiency increases with plating time depending on the composition of the plating bath [15] [29]. K. L. Yeung et al. (1999) [15] reported that at certain point during the deposition process, the plating rate ceases to respond to film deposition which implies that no further deposition takes place. One reason for this could be that all the palladium in the solution has been deposited [13]. M. Kitiwan and D. Atong (2010) [29] investigated the electroless plating of palladium on ceramic support and reported an increase in the rate of deposition with time. In their work, this group showed that the palladium deposition started after 10 minutes which indicates that there was an induction period before the commencement of the plating process. The 10 minutes induction period was high and rather unexplained because prior to the plating process, the ceramic support was activated with Pd nuclei which would have drastically reduced the induction period [15].
M. Volpe et al. (2006) [30] investigated the deposition of palladium on anodic alumina and reported stable plating below 30 minutes of deposition time. However, after 30 minutes there was damage to the membranes which was attributed to the plating time longer than 30 minutes and also the pH of the solution [30]. This group reported that after the stable pH of 8.4, the high alkalinity of the plating bath led to the unstable plating solution. Impliedly, if the pH has been higher than 8.4 and the plating time was less than 30 minutes, the plating rate would have been stable. This indicates that the effect of plating time on the quality of deposits also depends on the pH of the plating solution [15] [30]. The effect of plating time is also dependant on the concentration of the metal and the reducing agent as shown by K. L. Yeung et al. (1999) [15] who reported an increase in the plating efficiency with time for 2 different reducing agents: Hydrazine and hypophosphite reducers for plating periods of 1 and 4 hours. Palladium was shown to deposit continuously over the 4 hour plating time in the hypophosphite bath with increase in the plating efficiency but the plating efficiency decreases from 0.96 to 0.79 as the concentration of palladium increases from 2.8 to 11.3 mM. However, the plating efficiency decreased with increase in the palladium concentration for both the hydrazine and hypophosphite baths but the plating rate and the final amount deposited increased [15]. There is the need for a better understanding of the effect of plating time vis-à-vis the concentration of the reducer and stabilising agent. Furthermore, there is paucity of knowledge as to whether or not the plating time will enhance plating efficiency at low or high temperatures.
The effect of plating time on the deposits morphology has been reported by several authors including Y. S. Cheng et al. (1999) [24]. In their work on PdAg codeposition on Vycor glass support, this group reported that at the beginning of the plating i.e. t = 0, there was generally a uniform seeding of the support but after 10 minutes, there was a mixed coating of silver and a nonuniform coating begins to appear. At 20 minutes, there was a more rapid growth of some of the grains compared to the others and the film assumed a nonuniform grain size and between 20, 30 and 40 minutes plating time, there was simultaneous nucleation and growth but a dense film was achieved at the end of 60 minutes [24]. Also, this group of workers reported that as the plating time increases, so does the competition for nucleation sites but if the initial deposition rate of silver is high, then palladium could be prevented from deposition which could result in a pure silver membrane [15].
To ameliorate this problem, a higher concentration of hydrazine reducing agent is added [15]. Competition for nucleation sites between silver and palladium leads to inhibition of palladium deposition if the initial rate of deposition of silver is high and this result in uneven coating which could also be improved by the addition of a higher concentration of the hydrazine reducing agent to enhance palladium deposition [24].
Also in an effort to solve this problem, Gaofeng Zeng et al. (2014) [31] developed a method which adjusted the imbalance in the deposition rate of the metals and regulated the competition for nucleation sites between both metals. The Gaofeng group developed a silver controlled codeposition method for the preparation of PdAg membranes in separate Pd and Ag plating baths. Silver is continuously fed into the palladium plating bath to restrict the silver concentration. Although this method showed some nonuniform distribution of the metal, it still improved the stability of the plating bath by reducing the precipitation of the plating bath. In this method, thin Pd/Ag membranes of ~2.5 µm and uniform silver distribution of ~25% were achieved [31].
2.6. Stabilising AgentThe plating solution for electroless plating usually contains EDTA (ethyldiamine triacetate) which serves as a complexing agent and stabilises the plating bath by controlling the plating process against temperature changes [15]. However, EDTA also has its drawbacks as it affects the purity of the palladium layer due to the absorption of the EDTA complex in the metal deposits [13]. F. Braun et al. (2011) [32] in their work discovered that membranes prepared without EDTA showed cracks and a dendritic morphology but the morphology of membranes prepared with EDTA and low concentration of hydrazine were more homogeneous. The effect of EDTA at different concentrations of the reducer has not been fully investigated to provide a better understanding as to the optimum EDTA concentration (wt %) at which the impurities could be avoided to achieve full bath stability. The concentration of the NH4OH stabilizing agent is another factor that affects the plating rate. Yeung et al. (1999) [15] investigated the effect of NH4OH by using different concentrations of the stabilizing agent and reported that high concentrations of NH4OH above 7M led to a decrease in the plating rate. However, at low concentration of NH4OH, the plating rate increased but this increase was succeeded by decomposition of the plating bath [15]. Several investigations have shown that the plating efficiency increases with decreasing concentration of the NH4OH [13] [15]. K. L. Yeung et al. (1999) [15] reported an increase in the amount of palladium deposited with decreasing concentration of NH4OH.
2.7. AdditivesIn addition to the complexing agents such as EDTA and Potassium/Sodium tartarate, additives also stabilize the bath against the spontaneous decomposition of plating baths and the formation of unwanted particles which could inhibit the plating efficiency [21]. Some of the additives used in electroless plating are 2,2-bipyridyl, mercaptobenzothiazole, thiourea and cyanide and they have been used as stabilizers in electroless plating to enhance plating rate and efficiency [21]. F. Hanna et al. (2003) [21] investigated the effect of several additives namely Cytosine, Thiourea, 2-mercaptobenzothiazole (2MBT), benzotriazole (BT) and Pyridine in the electroless plating of copper on pure copper coupons using formaldehyde as the reducing agent and reported a marked increase in the plating rate upon the addition of additives. The group reported an increase in the plating rate from 5.4 to 10.5 mg/cm2 h when 2 mg/l of 2 MBT is added to the EDTA bath at pH 13.
These additives have a greater adsorption ability at low concentrations on active copper sites compared to the EDTA hence the increase in the plating rate [13] [21]. But the phenomenon is only at low concentrations because at concentrations above 2 mg/l of 2 MBT, the plating rate begins to reduce steadily [21]. All the organic compounds investigated by this group exhibited similar trend which was also reported by Yang, Z et al. (2011) [33] in their investigation on the addition of Polyethylene glycol (PEG), Polypropylene glycol (PPG) and ethylene oxide terminal blocks termed EPE. Pizzi, et al. (2008) [34] also discovered that the plating rate decreases with an increase in the concentration of the additive up to 2 mg/l. Pizzi and his group [34] used SiO2/Si substrate for the electroless copper plating using a formaldehyde reducer and EDTA complexing agent at an optimum plating bath temperature of 70˚C, plating time of 60 minutes and a pH of 12.5. The Pizzi group also reported that at lower concentration of 0.5 mg/l and below, the difference in the plating rate was not profound but it increased with additional concentration of the stabilizers up to 2 mg/l when the plating rate starts to decrease. It is noteworthy that most of the work done on additives is on the electroless plating of copper hence there is paucity of knowledge regarding the effect of additives on the electroless plating of palladium and its alloys.
2.8. Deposits MorphologyPalladium membranes suffer from hydrogen embrittlement and Pd/Ag membranes are resistant to hydrogen embrittlement due to their ability to avoid α – β phase transition [3]. It is necessary to investigate the morphology of the deposits in electroless plating of palladium and palladium alloy membranes so as to provide a better understanding of the process and how the electroless plating factors could be optimised to improve hydrogen permeation. A better understanding of the effect of the process factors on deposits morphology will also provide a better understanding of the quality of these deposits and by implication, the plating rate and efficiency which also affects the hydrogen permeation properties [15]. Process factors such as plating rate, time, temperature and reducing agent determine the growth of the palladium film and grain size [27].
It has been reported that smaller grains generally lead to better coating and denser films as a result of the larger boundaries associated with the larger grains which could impede the selectivity of the membrane [10]. Even smaller grains may have larger boundary gap which implies that both smaller and larger grain sizes could affect the selectivity of the membrane [10] [27].
From the several investigations conducted it is apparent that there is paucity of knowledge on the effect of grain sizes on quality of deposits hence further studies are required to ascertain the effect of grain size on the quality of the palladium films. Investigations have shown that lower temperatures and lower plating cycles result in smaller grain growth and better uniformity of coating [10]. Also low temperatures maintain a uniform grain growth for much longer periods than high temperatures [10] [27]. Lower plating cycles result in more uniformly coated membranes and reduce the risk of defects in the metallic layer [27].
M. L. Bosko et al. (2011) [10] investigated the effect of plating time on the morphology of Pd-Ag films deposited over porous stainless steel support using the electroless plating method using 2 separate plating periods i.e. 90 minutes and 40 minutes over a plating cycle of 3 and 9 rounds respectively. This group [10] reported that a higher number of plating cycles resulted in more defects in the metallic film and increased the detrimental effect of silver dendrites growth which Huey-Ing [35] and his group attributed to the different growth patterns of the Pd and Ag grains. Y. S. cheng et al. [24] investigated the preparation of Pd/Ag membranes on porous Vycor tube and reported that higher concentration of hydrazine promotes the deposition of palladium. Furthermore, they also posited that at higher hydrazine concentration—20 mM—pure palladium films were obtained even though the silver concentration was higher at 25 at%. However, increasing the amount of NH4OH can improve the deposition of Pd and enhance that of Ag but very low concentration of NH4OH can result in bulk precipitation [24]. From their findings, this group of workers [24] concluded that the optimum plating bath conditions for a Pd/Ag codeposition are: 1) A low concentration of NH4OH. 2) A modest hydrazine to palladium ratio and 3) A high plating temperature.
In Pd/Ag electroless codeposition, the effect of Ag content in the plating bath on the deposits morphology has been studied by several authors [28] Huey-Ing Chen and his group (2004) [35] reported that the plating bath for pure palladium without silver showed nodular palladium agglomerates but when the silver content was added up to 50%, the layer became dendritic with crystallites whose porosity reaches a maximum at 50% Ag content. The group demonstrated that the Ag content in the deposited film increased as the Ag content in the plating bath increased [35]. It was observed that there was more Ag in the deposited layer than in the plating bath which indicates that under the plating conditions Ag inhibits the deposition of palladium [27] [35]. Also, there was no Ag for the 2 and 3 hour plating times except at 10% Ag content which implies that the strength of inhibition of palladium deposition by Ag decreased as the Ag content in the plating bath is reduced [35].
The deposit morphology of the Pd/Ag membranes was also investigated by Huey-Ing Chen et al. [35] and after varying the silver content of the plating bath at 50%, 25%, 12.5%, and 6.2 at%, they reported Ag content (at%) of 100, 30, 12.5 and 5.5 respectively. Y. S Cheng et al. [24] also compared the microstructure of the pure palladium and codeposited Pd/Ag films from the same plating bath conditions and reported that silver is dominant and it inhibits palladium deposition if its initial plating rate is high and could even lead to a pure silver membrane. However, the inhibition of deposition by either silver or palladium over the other metal depends on the initial plating rate. A high initial rate of palladium could result in inhibition of Ag deposition and same also for a high initial rate of silver. It is necessary that the initial plating rates for palladium and silver are controlled so as to avoid the inhibition of deposition for any of the metals [24].
Y. S. Cheng and K. L. Yeung [24] prepared a Pd/Ag membrane with thickness from a plating bath containing 10 mM Pd/Ag solution, Hydrazine concentration at 10 mM and temperature 328 K and reported that the plating bath with high concentrations formed a continuous film with small and uniform grain sizes while that with lower silver concentrations showed a flowery structure and larger grain size. The uneven grain sizes can be attributed to the inhibition effect of silver in the plating bath. At higher initial concentration of silver, there was a “domino” effect exerted by silver which inhibits palladium deposition [24]. Cheng and his group reported a better performance in hydrogen permeation for the Pd/Ag membranes compared to the Pure Pd membrane. There is very little work on the effect of pH and other process factors on the morphology of palladium membranes prepared through the electroless plating method.