Advanced Search
RSS LinkedIn Twitter

Journal Archive

Platinum Metals Rev., 1986, 30, (3), 120

Some Aspects of Electrocatalysis

A Study of Titanium and Tantalum When Alloyed with the Platinum Group Metals

  • By B. J. Piersma
  • By Wilson Greatbatch
  • Houghton College, Houghton, New York State
SHARE THIS PAGE:

Article Synopsis

To increase our understanding of the electrochemical processes involved during cardiac stimulation by implanted pacemakers, alloys were prepared containing electrocatalytically active platinum group metals and either titanium or tantalum which irreversibly form very inactive oxides. Our work has shown that alloys with as little as 5 per cent platinum group metals exhibit electrochemical characteristics which are more similar to the platinum group metals than to the valve metals. Under some of the conditions certain of these alloys appear to be better electro-catalysts than the platinum group metals. Alloying titanium and tantalum with small amounts of platinum group metals also appears to prevent anodic dissolution of oxide-free titanium and tantalum.

We define electrocatalysis as the variation of rate of an electrochemical reaction with change in electrode material. An electrocatalyst is thus a heterogeneous catalyst at which charge transfer occurs. In our on-going research programme to understand more fully the electrochemical processes in cardiac stimulation by pacemakers, work with more than thirty metals and alloys considered as possible electrode materials has been undertaken. These studies lead quite naturally to comparisons and correlations of electrocatalytic activity. A significant problem in making correlations with different metals is that even if the overall reaction remains the same, the mechanism is often different on different materials. In one attempt to avoid this difficulty we prepared a series of alloys of titanium and platinum for study. Titanium readily and irreversibly forms an oxide which protects the metal from dissolution, but which also makes it catalytically inactive, at least for the electrochemical processes in which we were interested. Platinum is probably the best electrocatalyst of all metals. In addition to the titanium-platinum series, alloys of titanium and tantalum with iridium and ruthenium were prepared; compositions are given in Table I.

Table I

Alloy Compositions

Electrode materialSourceActual composition
PtJohnson Matthey0.03% maximum impurity
TiAlfa-Ventron0.04% maximum impurity
TaAlfa-Ventron0.003% maximum impurity
Ti-5% PtMaterials Research5.24% Pt
Ti-10% PtMaterials Research9.74% Pt
Ti-20% PtMaterials Research20.20% Pt
Ti-30% PtMaterials Research29.83% Pt
Ti-20% IrMaterials Research19.66% Ir
Ti-20% RuMaterials Research20.19% Ru
Ti-20% PtMaterials Research19.49% Pt
Ta-20% IrMaterials Research19.26% Ir
Ta-20% RuMaterials Research20.39% Ru

After the studies were carried out, a semi-quantitative analysis of the surface structures of the alloys was made with a Kevex X-ray unit of a Scanning Electron Microscope. Comparisons of the platinum-peak heights indicated the same composition for the exposed surfaces, the surfaces not exposed to solution, and the interiors of the alloys examined after fracturing. Comparison of a tantalum-iridium surface, which had undergone severe electrochemical dissolution, with an unexposed sample indicated that both had the same surface composition. We concluded that the surface compositions of the alloys were essentially the same as those of the bulk compositions.

Experimental Conditions

Wire and rod electrodes were sealed in silicone rubber tubing or teflon tubing, respectively, and all had an exposed geometric area of 0.16 cm2. They were mechanically cleaned with silicon carbide cloth, degreased with acetone and rinsed with triple distilled water. Materials which formed an oxygen (or oxide) layer that could not be electrochemically reduced, for example, were mechanically cleaned before every anodic measurement. The alloys were in the form of rods with a diameter of about 7 mm and their surface areas were fixed using molten polyethylene. Typically a 25 cm2 platinum gauze electrode was used as a counter electrode and a Ag/AgCl or a Leeds and Northrup miniature glass electrode was used as a reference, each being calibrated versus a reversible hydrogen electrode (R.H.E.) in the same solution. Details will appear elsewhere (1).

Electrochemical Characterisation Using Cyclic Voltammetry

A qualitative comparison of electrocatalytic activity is readily made from cyclic voltammetry curves, as shown in Figure 1 for results in 1 M sulphuric acid at 25°C and in Figures 2 and 3 for physiological saline solution (0.15 M NaCl) at 37°C.

Fig. 1

Cyclic voltammetry curves in helium-saturated 1M sulphuric acid at 25°C

(a) platinum wire, ν = 5V/s, −0.2 to 1.6V

(b) oxide-free titanium wire, ν = 1V/s, −0.5 to 1.6V

(c) titanium-5% platinum, ν = 1V/s, −0.6 to 1.2V

(d) titanium-20% iridium, ν = 10V/s, −0.6 to 1.2V

Cyclic voltammetry curves in helium-saturated 1M sulphuric acid at 25°C(a) platinum wire, ν  = 5V/s, −0.2 to 1.6V(b) oxide-free titanium wire, ν  = 1V/s, −0.5 to 1.6V(c) titanium-5% platinum, ν  = 1V/s, −0.6 to 1.2V(d) titanium-20% iridium, ν  = 10V/s, −0.6 to 1.2V

Fig. 2

Cyclic voltammetry curves in helium-saturated physiological saline solution at 37°C

(a) platinum wire, ν = 5V/s, −0.5 to 1.5V

(b) oxide-free titanium wire, ν = 1V/s, −0.5 to 1.7V

(c) titanium wire, ν = 5V/s, −0.5 to 1.5V, detail of 2nd to 5th sweep cycles

Cyclic voltammetry curves in helium-saturated physiological saline solution at 37°C(a) platinum wire, ν  = 5V/s, −0.5 to 1.5V(b) oxide-free titanium wire, ν  = 1V/s, −0.5 to 1.7V(c) titanium wire, ν  = 5V/s, −0.5 to 1.5V, detail of 2nd to 5th sweep cycles

Fig. 3

Cyclic voltammetry curves in helium-saturated physiological saline solution, 37°C, ν = 5V/s, −0.5 to 1.4V, i = 1 mA/cm

(a) titanium-5% platinum

(b) titanium-10% platinum

(c) titanium-20% platinum

(d) titanium-30% platinum

Cyclic voltammetry curves in helium-saturated physiological saline solution, 37°C, ν  = 5V/s, −0.5 to 1.4V, i = 1 mA/cm(a) titanium-5% platinum(b) titanium-10% platinum(c) titanium-20% platinum(d) titanium-30% platinum

A number of generalisations can be made from these studies:

  • The cyclic voltammetry features of platinum change significantly in going from sulphuric acid to sodium chloride solution, but this is not the case for the alloys.

  • The peaks for H-adsorption and H-oxidation which are pronounced on platinum in sulphuric acid and absent on titanium, are present on the alloys but not as pronounced. Suitable variation of sweep speed, ν, and limits makes these peaks somewhat more evident. Potentials for these peaks are given in Table II. The positions for the two peaks are essentially the same for titanium-20 per cent platinum, titanium-30 per cent platinum and for platinum.

  • Figures 1(b) and 2(b) for oxide-free titanium show a characteristic anodic dissolution peak on the first anodic sweep followed by a cathodic peak as the sweep is reversed. This was characteristic of oxide-free titanium and tantalum electrodes. The peak is not present after the first cycle into the anodic region, presumably prevented by oxide formation. None of the alloys, including titanium-5 per cent platinum, exhibits this anodic dissolution peak. Further, no anodic dissolution was observed for any of these platinum-titanium alloys when tested in aqueous solutions.

  • Details of the irreversible formation of oxide on titanium are seen in Figure 2(c). The first cycle into the anodic region shows significant change due to oxide formation. Successive cycles show little or no additional oxide formed when the sweep is limited to the same potential limit. When the anodic potential limit is increased by several hundred millivolts, significant change is again seen on the first cycle in the higher potential region. Tantalum behaves in an identical way.

  • The oxides formed anodically on the titanium and tantalum alloys appear to be cathodically reduced, exhibiting behaviour similar to that of the platinum group metals and significantly different from either titanium or tantalum metal.

  • Comparison of the titanium-platinum alloys in Figure 3 suggests the same electrochemical processes occur at each electrode, with a greater degree of reaction and hence greater electrocatalytic activity as the amount of platinum in the alloy increases.

  • The titanium-iridium alloy exhibits a significantly greater electrocatalytic activity in the oxygen region than any of the other alloys; compare, for example, Figures 1(b) and 1(c) with 1(d).

  • Titanium alloys appear to be better electrocatalysts than tantalum alloys. From steady-state measurements it was found that a tantalum-iridium alloy undergoes dissolution at potentials anodic to 1.1V (versus R.H.E.).

Table II

Potentials of Adsorbed Hydrogen Peaks (vs. R.H.E.) in 1 M H2SO4

Electrode materialH1 (adsorption), voltsH2 (oxidation), volts
Pt0.220.10
Ti-30% Pt0.240.11
Ti-20% Pt0.240.10
Ti-10% Pt0.150.05
Ti-5% Pt−0.02-0.16
Ti
Ta-0.62
Ta-20% Pt0.230.12
Ta-20% Ir0.190.09
Ta-20% Ru0.150.04

Titanium-iridium and titanium-ruthenium had no observable peaks

Hads peaks are more pronounced as the per cent of platinum in the alloy increases

Galvanostatic Transient Studies in Physiological Solution

Much of our research programme has involved detailed analyses of some 30 metals and alloys using constant current pulses similar to those employed by heart pacemakers. A summary of these results from the perspective of electrocatalysis has been presented elsewhere (1). Typical results for the titanium-platinum alloys in physiological saline solution at 37°C are seen in Figures 4 and 5 for cathodic and anodic pulsing, respectively. (Note that the cathodic pulses have been inverted.) The double layer capacitance was determined for the alloys from the initial slopes of the charging curves, and the values are given in Table III. One unexplained value is the relatively high double layer capacitance for the titanium-iridium alloy.

Fig. 4

(Right) Cathodic galvanostatic charging curves (1 to 9 mA pulses in 1 mA increments) in helium-saturated physiological saline solution, 37°C, 0.16 cm2 electrode areas. Voltage scale (vertical) is 0.5V/cm, time scale (horizontal) is 1 ms/cm. The pulses have been inverted

(a) titanium-5% platinum

(b) titanium-10% platinum

(c) titanium-20% platinum

(d) titanium-30% platinum

(Right) Cathodic galvanostatic charging curves (1 to 9 mA pulses in 1 mA increments) in helium-saturated physiological saline solution, 37°C, 0.16 cm2 electrode areas. Voltage scale (vertical) is 0.5V/cm, time scale (horizontal) is 1 ms/cm. The pulses have been inverted(a) titanium-5% platinum(b) titanium-10% platinum(c) titanium-20% platinum(d) titanium-30% platinum

Fig. 5

(Far right) Anodic galvanostatic charging curves, all other conditions identical to Figure 4

(Far right) Anodic galvanostatic charging curves, all other conditions identical to Figure 4

Table III

Electrochemical Parameters for Alloys

Electrode materialDouble layer capacitance, C, μ F/cmVo.c. (vs. R.H.E.)ba (2.3 RT/F) bc 
Pt200.8222/3
Ti100.0822
Ta12.5-0.1622
Ti-5% Pt100.1722
Ti-10% Pt120.8122
Ti-20% Pt191.1122
Ti-30% Pt180.9222
Ti-20% Ir410.8411
Ti-20% Ru220.8922
Ta-20% Pt160.7022
Ta-20% Ir100.9022
Ta-20% Ru9.50.7322

Vo.c. is the open circuit potential versus the reversible hydrogen electrode established both before and after pulsing in physiological saline solution at 37°C; ba and bc are anodic and cathodic Tafel slopes

The double layer contribution to the polarisation of the charging curves was subtracted, assuming a constant average value of the double layer capacitance over the potential regions analysed, and Tafel curves were generated from the charging curves. Reasonably good Tafel slope data were obtained and the values are reported in Table III. Identical values of Tafel slopes for the titanium-platinum alloys tend to suggest that the mechanisms for the electrochemical processes are the same and that electrocatalytic comparisons are meaningful.

A simple approach to electrocatalysis is to compare the maximum polarisation of the electrodes at a given current density and pulse length. Figure 6 correlates the maximum values for polarisation of the titanium-platinum alloys, at a current of 5 mA (current density of 31 mA/cm2) with electronic work functions, ϕ, calculated assuming a linear relationship between work function and the composition of the alloy. A definite volcano-type relationship is evident for both cathodic and anodic processes. The open circuit potentials, except for titanium and tantalum which are indicative of dissolution, are typical of potentials established on platinum group metals in solutions with very low oxygen concentrations, and hence electrodes free of oxide on the surface. The cathodic process is reduction of water to form adsorbed hydrogen atoms with eventual hydrogen evolution at higher currents or longer times of polarisation. The anodic process is oxidation of adsorbed chloride ions to chlorine atoms with eventual chlorine evolution.

Fig. 6

Polarisation maxima from galvanostatic charging curves at 5 mA current for titanium-platinum alloys correlated with electronic work function

(a) for cathodic pulses

(b) for anodic pulses

Polarisation maxima from galvanostatic charging curves at 5 mA current for titanium-platinum alloys correlated with electronic work function(a) for cathodic pulses(b) for anodic pulses

An alternative approach is to make correlations of electrocatalytic activity with log i, where i is the current density. From the Tafel equation, taking a potential difference V in place of the overpotential η (which is not precisely defined here), b/ΔV (where b is the Tafel slope) is proportional to log i. The correlation of b/ΔV with electronic work function is made in Figure 7 for cathodic and anodic processes in physiological saline solution at 37°C. We observe a volcano-type relationship with titanium-30 per cent platinum showing maximum electrocatalytic activity for both cathodic and anodic processes.

Fig. 7

Correlation of (b/ΔV) with electronic work function (ϕ ) for platinum, titanium and titanium-platinum alloys in physiological saline solution at 37°C

(a) cathodic pulses

(b) anodic pulses

Correlation of (b/ΔV) with electronic work function (ϕ ) for platinum, titanium and titanium-platinum alloys in physiological saline solution at 37°C(a) cathodic pulses(b) anodic pulses

Electrocatalysis in Ethylene Oxidation

The anodic oxidation of ethylene at platinum electrodes has been studied for more than 20 years as a model for electrocatalysis particularly relevant for fuel cell reactions (2). We have reexamined ethylene oxidation, partly because of some disagreement with our initial mechanism proposals (3, 4), but primarily to make an electrocatalytic study with the titanium-platinum alloys. The measurements were made in 1 N sulphuric acid at 80°C with ethylene at 1, 0.1 and 0.01 atmospheres partial pressures using steady-state potentiostatic techniques. Steady-state Tafel behaviour was observed for platinum and for each of the titanium-platinum alloys with slopes of 2RT/F. The linear Tafel region decreased as the amount of platinum in the alloy decreased, for example, titanium-20 per cent platinum showed linear Tafel behaviour between 0.4 and 0.8 V (versus R.H.E.), while titanium-10 per cent platinum gave linear behaviour between 0.6 and 0.8 V. A negative pressure dependence of the current, and hence a negative order of reaction with respect to ethylene, was observed for platinum and for each of the titanium-platinum alloys, provided the measurements were made at potentials below the limiting current regions. The potential at which a limiting current is observed decreases as the partial pressure of ethylene is decreased.

A typical response of anodic current with change of ethylene partial pressure is given in Figure 8 for titanium-30 per cent platinum. These results are consistent with the earlier suggestions that the anodic oxidation of water to form OH radicals (which then react with adsorbed ethylene molecules) is the rate limiting step (2, 5).

Fig. 8

Dependence of anodic current for ethylene oxidation on ethylene partial pressures for titanium-30% platinum in 1 N sulphuric acid at 80°C. Measurement made at a potential of 0.45 V versus R.H.E.

+ 1 atmosphere ethylene

Δ 0.1 atmosphere ethylene

○ 0.01 atmosphere ethylene

Dependence of anodic current for ethylene oxidation on ethylene partial pressures for titanium-30% platinum in 1 N sulphuric acid at 80°C. Measurement made at a potential of 0.45 V versus  R.H.E.+ 1 atmosphere ethyleneΔ 0.1 atmosphere ethylene○ 0.01 atmosphere ethylene

One method of comparing the electrocatalytic activity for ethylene oxidation is to compare the current densities at a given potential in the linear Tafel regions. Figure 9, which correlates the current densities versus electronic work function at a potential of 0.6 V, exhibits a surprisingly good volcano-type curve with a maximum for electrocatalytic activity occurring between titanium-20 per cent platinum and titanium-30 per cent platinum. These results strongly indicate that some titanium-platinum alloys, particularly those ones with compositions between 20 to 30 per cent platinum, may be better electrocatalysts for organic oxidation reactions than platinum alone.

Fig. 9

Correlation of current densities of ethylene oxidation at 0.6 V versus electronic work function for platinum and titanium-platinum alloys

Correlation of current densities of ethylene oxidation at 0.6 V versus  electronic work function for platinum and titanium-platinum alloys

Electrochemical Behaviour in a Room Temperature Molten Salt System

Room temperature (20°C) highly conducting melts of AlCl3 with 1,3-dialkylimidazolium chlorides were reported in 1982 (6). These melt systems appear to be of particular interest as electrolytes for high energy density batteries. We were able to examine the behaviour of the titanium and tantalum alloys in these melt systems and the preliminary results were published as a U.S. Air Force Technical Report from the Frank J. Seiler Research Laboratory (7). The stability of the alloys in AlCl3-methylethylimidazolium chloride melts was examined using cyclic voltammetry. The potential region in which the electrode is stable, that is where it does not undergo dissolution, and in which the melt is electrochemically unreactive, is termed the electrochemical window. These were determined for melts with an AlCl3-mole fraction of 0.40 which behaved as Lewis bases, and with an AlCl3 mole fraction of 0.60 which behaved as Lewis acids. The cyclic voltammograms, taken at a sweep rate of 50 mV/s, indicated that all of the titanium alloys were subject to dissolution in both basic and acidic melts. Aluminium deposition could be observed only from acidic melts and only for platinum and titanium-5 per cent platinum electrodes. In contrast the tantalum alloys demonstrated much greater stability in the melts, in fact tantalum-20 per cent ruthenium gave the widest electrochemical window in basic melts of all the electrode materials examined.

The results of these studies are summarised in Table IV. The electrocatalytic activity can be inferred in the sense that the wider the electrochemical window observed, the lower is the electrocatalytic activity of the electrode.

Table IV

Electrochemical Windows on Titanium and Tantalum Alloys in AlCl3-MeEtImCl Melts

Electrode materialElectrochemically stable region, volts
Basic melt (mole fraction AlCl3 = 0.4)Acidic melt (mole fraction AlCl3 = 0.6)
Pt0.90 to -0.152.00 to 0.70
Ti-5% Pt-0.2 to -0.71.30 to 0.00
Ti-10% Pt-0.2 to -0.451.1 to 0.6
Ti-20% Ptnonenone
Ti-30% Ptnonenone
Ti-20% Ir-0.15 to -0.301.2 to 0.7
Ti-20% Ru10.25 to -2.0none
Ta10.40 to -1.011.9 to 0.5
Ta-20% Pt-0.1 to -0.81.05 to 0.3
Ta-20% Ru1.25 to -1.72.3 to -0.1
Ta-20% Ir0.8 to -1.51.95 to -0.05

All potentials are referred to an aluminium wire in the acidic (0.6) melt

Conclusions

Studies with electrodes of titanium and tantalum alloyed with platinum group metals have led to a number of interesting observations. Under many conditions the electrochemical behaviour of the alloys is more like that of the platinum group component than that of either titanium or tantalum, even when the platinum component is smaller. For several reactions, namely: hydrogen evolution, chlorine evolution and ethylene oxidation, some of the titanium-platinum alloys appear to be better electrocatalysts than platinum, with a maximum in activity for the alloys containing between 20 and 30 per cent platinum. From some considerations, titanium-20 per cent iridium appeared to be the most active, and tantalum-20 per cent ruthenium the most stable and least active of the alloys studied.

BACK TO TOP

References

  1. 1
    B. J. Piersma,, B. Turdell and W. Greatbatch, in press
  2. 2
    H. Wroblowa,, B. J. Piersma and J. O’M. Bockris, J. Electroanal. Chem., 1963, 6, 401
  3. 3
    W. E. Triaca,, T. Rabockai and A. J. Arvia, J. Electrochem. Soc., 1979, 126, 218
  4. 4
    W. E. Triaca,, A. M. Castro Luna and A. J. Arvia, J. Electrochem. Soc., 1980, 127, 827
  5. 5
    J. O’M. Bockris,, H. Wroblowa,, E. Gileadi and B. J. Piersma, Trans. Faraday Soc., 1965, 61, 2531
  6. 6
    J. S. Wilkes,, J. A. Levisky,, R. A. Wilson and C. L. Hussey, Inorg Chem., 1982, 21, 1263
  7. 7
    B. J. Piersma and J. S. Wilkes, FJSRLTR-82-0004, 1982, “Electrochemical Survey of Selected Cations and Electrode Materials in Dialkylimidazolium Chloro-Aluminate Melts”

Read more from this issue »

BACK TO TOP

SHARE THIS PAGE: