Applied Surface Science 55 (1992) 297-301 North-Holland
s u r f a c e s c h ~ n c e
Surface segregation induced by chemisorption at the alloy/solution interface
V. L~z~rescu 2, O. Radoviei b and M. Vass a a Institute o f Physical Chemistry, Spl. Independent.el 202, Bncharest 77 208, Romania
G¢,neral Chemistry Department, Polytechnic Institote o f Bucharest, Spl. Independent, ei 313, Bncharest, Romania
Received 24 June t991; accepted for publication 25 November 1991
Au-Ag vacuum-deposited alloy films with a small content of gold (5-10 at%) were found to exhibit unusual potentiodynamic behaviuur in alkaline media. The changes observed in the I - E profiles during the first 10-12 potential scans preceding the attainment of the stationary, shape were assigned to a phenomenon of surface segregation of silver induced by the chemisorption of oxygen atoms, resulting in a HO- discharge step.
I. Introduction
The chemical compositions of alloy surface and alloy bulk are frequently different as a result of either the thermodynamic equilibrium condi- tions or non-equilibrium phenomena. Usually, the surface becomes enriched in the component with the lower heat of sublimation after an annealing treatment, respectively the lower rate of sputter- ing after an ion bombardment, or in that one forming the stronger bonds with the adsorbate after a gas-phase chemisorption process.
As the phase diagramme reveals, silver and gold form continuous series of solid solutions over the entire compositional range [1]. Since the sublimation heat of gold exceeds that of silver by more than 100 k J / g [2], a pronounced surface enrichment in silver is expected to occur for their thermally equilibrated alloys, according to the regular solution model developed by van Santen and Boersma [3] for disordered monophasic bi- nary alloys,
However, the experimental data do not sup- port these predictions. Whatever the investigated alloy sample was, epitaxially grown films [4], bulk ingots [5] or foils [6], no appreciable surface seg- regation has been observed. Even the results re-
ported by Overbury and Somorjai [7], apparently discordant, turned out to be in good agreement with these conclusions [6].
In clear-cut contrast with all these findings stands the observation of significant (although much less than the theoretical predictions) sur- face segregation of silver for alumina-supported alloy catalysts reported by Toreis and Verykios [8]. Their results could be explained, in our opin- ion, provided that the specific conditions of the catalyst preparation are taken into account. Un- like the alloys discussed before, all of them ob- tained in high vacuum or inert atmosphere, the catalysts were exposed to oxygen during their preparation [8]. Therefore, it seems plausible to suppose that the surface excess of silver is, in this case, only a consequence of the preferential in- teraction of oxygen with one of the alloy compo- nents.
This assumption found an unexpected support in the results of cyclic voltammetry investigations on the behaviour of A u - A g alloys in alkaline solutions that revealed a definite phenomenon of surface segregation of silver induced by oxygen ehemisorption at the alloy/solution interface.
Studying the effects of the oxygen interaction with A u - A g alloys at the solid/gas and the
0169-4332/92/$05.00 © 1992 - Elsevier Science Publishers B.V. All rights reserved
V. Ldzdrescu a aL / Segregation indaced by chemisorption at the alloy/sohaion interface
solid/solution interfaces [9] it has been found that during repeated potential scans, the alloys with low percentages of gold (5-10 at%) exhib- ited an unusual potentiodynamie behaviour point- ing out important changes in their surface com- position. It is the aim of this paper to report on this interesting phenomenon.
2. Experimental
The measurements were carried out on poly- crystalline alloy films vacuum-deposited on opti- cally polished glass substrates. Every precaution had been taken in order to get a homogeneous material. Yhe two components were simultane- ously evaporated from closely positioned but sep- arate sources containing the pure metals, at indi- vidual constant evaporation rates. A heated sub- strate as weii as a subsequent annealing for 30 min have been used to enhance the atom mobility after the condensation. The heating temperature (350°C) was chosen to be equal to the highest of the Tammann temperatures of the two compo- nents (Au), where surface diffusion is known [10,11] to become appreciable. The residual gas pressure did not exceed 10 -8 Torr during the evaporation and the annealing steps.
The thickness of the deposit was greater than 3000 .~ in order to avoid both the influence of the substrate [12] and the effect of thickness fluctua- tions. The latter ones, usually less than 100 ,~ under such circumstances [13] could not bring about changes in the electrochemical behaviour of the film, observed to be identical with that of the massive metal starting with 1200 ,~ [!4-16].
The exgeriments were performed at room tem- perature in 1M KOH solution in doubly distilled water, in a three-compartment cell of conven- tional design. Two platinum wires embedded in the glass surface ensured the electrical connec- tion to the measuring circuit. The working elec- trode potential measured relative to a saturated calomel electrode (SCE) was controlled by a PAR-EG&G potentiostat (Model 173) fed by a PAR-EG & G Universal Programmer (Model 179). The cyclic voltammograms taken with a constant
scan rate of 10 mV s-~ were recorded with a Hewlett-Packard recorder.
3. Results and discussion
As seen in figs. I and 2, the I - E profiles exhibited under these circumstances by the alloys containing 5 to 10 at% Au-Ag underwent contin- uous changes during the repe~ ted potential scans. The second anodic peak (B), greatly enhanced in the course of the first 5-6 scans was noticed to be slowly diminished in the following ones. Ade- quately, the corresponding cathodic peaks suf- fered similar changes. Such a peculiar behaviour has never been observed for either simple silver films [17] or alloys with a higher content of gold [9].
That the detailed shape of the voltammogram is very sensitive to trace impurities as well as to surface structure [18-20], providing, as it has been claimed [18], a genuine "finger-print" for a clean and definite surface is well-known. Thereby, there is no doubt that the first voltammogram recorded for each alloy separately gives direct information on every change happened in the surface composition and structure. As a matter of fact, a conclusive image of the alloying effects operating in this case has been recently reported [91.
On the other hand, the complete miscibility of the components [1], the moderate exothermic en- thalpy of formation [21] indicating that these al- loys equilibrate fairly readily and the clear evi- dence on the absence of the surface segregation phenomenon [4-6] when they are thermally equi- librated under vacuum conditions are good rea- sons to suppose that a film of uniform composi- tion was obtained. Besides, unlike most of the modern techniques developed for the met- al/vacuum interfaces, which furnish only local information, the voltammograms give integrated information fl'om the whole investigated surface [221.
Consequently, neither the alloying effects, nor the alloy non-homogeneity could be responsible for the changes in the I - E curves reported here. Therefore, the origin of the continuous modifica-
V. L~z~rescu et aL / Segregation induced by chemisorption at the alloy ~solution interface
tion of the voltammogram under consideration should lie in the nature of the electrode processes involved.
A careful examination of some of the charac- teristic features of the anodic oxidation processes taking place on Ag electrodes in alkaline solu- tions [23,24] led to the conclusion that the well- known ability of silver to incorporate oxygen from the gas phase has a correspondent in one of its
first steps. It has been shown that after a minor dissolution process (A), a non-stoichiometric sub- surface oxide is formed by diffusion into the silver lattice of the chemisorbed oxygen, resulting in a H O - discharge step (B). Development of a thick layer of stoichiometric AgzO (C) followed by the formation of a mixed Ag(i)Ag(IIl)O 2 (D) ends the anodic oxidatioa of silver in alkaline media, as generally agreed [25-27].
l/mA Io.i mA D
• . ~ ~ , ~ ~ f 0.i~0.~ o .~ E/~v~ sc~
(0l
l/mA [ 0.1 mA B
A
' " ' o
I (c}
Fig. 1. Cyclic voltammograms of 5 at% Au-Ag alloy in IM KOH solution recorded during the repeated potential scans: (a) Ist; (b) 6th; (c) 10th.
300 V. Ldz~rescu et al. / Segregation induced by chemisorption at the alloy/sohttion interface
Thus, it is the electrode process (B) involved in the subsurface oxide layer growth that is mostly influenced in the above-mentioned experiments. This process was shown to be strongly dependent on the more or less porous structure of the vac- uum-evaporated film structure [17] suggesting the oxygen diffusion into the bulk as the rate-de- termining step. Therefore, its variations brought about by the repeated potential scans as well as the fluctuations of its cathodic correspondent re-
flect changes in the alloy surface and subsurface layer structure. Tile considerable increases ob- served during the first 5-6 runs and the subse- quent decreases noticed in the course of the last ones regarding the peak B height and width sug- gest that we witness a metal distension phe- nomenon soon followed by its opposite.
Since it is known [28,29] that the presence of oxygen on the surface causes an increase in the self-diffusion coefficient of the silver atoms by a
I/rnA [ 0.2 mA C D
- 0.2 0 A ~ . ~
(aJ
I/mA T J. 0.2 mA BC
~__...--~ • ~ .2~...c.~ . . . . ~ [~" O. 0.4 0.6 E/VvsSCE (hi
I 0.1 mA D
Fig. 2. Cyclic voltammugrams of 10 at% Au-Ag al!oy in IM KOH solution recorded during the repeated potential scans: (a) lst; (b) 5th; (e) 12th.
v. LSzdresctt et aL / Segregation induced by chemisorption at the alloy ~sob((ion #(terrace
f ac to r o f 100, it may be s u p p o s e d tha t o n e o f the c o n s e q u e n c e s w o u l d be the " p u s h i n g d o w n " 1o the b o t t o m layers of the gold a t o m s f o u n d in small p e r c e n t a g e s , This p rocess resul ts firstly in subsu r f ace layers with a m o r e p o r o u s s t r uc tu r e which t u r n e d in to m o r e c o m p a c t ones , finally.
T h e s t a t i ona ry s h a p e o f the cyclic v o l t a m m o - g r a m s r e c o r d e d for bo th 5 a n d 10 a t % A u - A g alloys r e sembl ing closely t h a t o f the c o m p a c t e l e c t rode ins tead o f t ha t c o r r e s p o n d i n g to the silver film o b t a i n e d in the s ame cond i t i ons [17] is conclus ive p r o o f in this respect . T h e fact t ha t such a b e h a v i o u r has no t b e e n obse rved lor p u r e si lver f i lms gives f u r t h e r suppor t to these a s sump- tions.
Th i s is, in o u r view, c l e a r ev idence o f a phe- n o m e n o n of su r f ace s e g r e g a t i o n i n d u c e d by c h e m i s o r p t i o n a t the a l l o y / s o l u t i o n in te r face . As f a r as we know, it is the first r e p o t o f this k ind, a d d i n g a va luab le a r g u m e n t in f avour o f the idea t ha t a close s imilar i ty exists indee¢! b e t w e e n the p h e n o m e n a t ak ing p lace a t the so l i c : /gas a n d the s o l i d / s o l u t i o n in te r faces .
]References
[I] M. Hansen, Constitution of Binary Alloys (McGraw-Hill. New York, 1958).
[2] C.J. Smithells, Metals Reference Book II (Bulterworths, London, 1962).
[3] R,A. van Santen and M.A.M. Boersma, J. Catal. 34 (1974) 13.
[4] S.C. Fain, Jr, and J.M. McDavid, Phys, Rev. B 9 (1974) 5089,
[5] R. Bouwman, L.H. Toneman, M.A.M. Boersma and R.A. van Santen. Surf. Sci. 59 (1076) 72.
16] M. Yabumoto, K. Watanabe and T. Yamashina, Surf. Sci. 77 (1978) 615.
[7] S.H. Overbury and G.A. Somorjai, Surf, Sci. 55 (1976) 209.
[8] N. Toreis and X.E. Vc, rykios, J. Catal. 108 (1987) 161. [9] V..L~z~rescu and M. Vass, Rev. Roum. Chim. 36 (1991),
in press. [10] S.L Gregg, The Surface Chemistry of Solids (Chapman &
Hall, London, 1961). [11] R, Bouwman and W.M,H. Sachtler. Surf. Sci. 24 (1971)
350. [12] D. Henning and K.G. Wed, Z, Phys. Chem. (NF) 98
(1975) 149. [13] F. Holland, Vacuum Deposition of Thin Films (Chapman
& Hall, London, 1961). [14] I. Vartires. Stud. Cercet. Chim. 18 (1970) 683. [15] O. Radovici and M.E. Macovschi. Rev. Room. Chim. 16
(197t) 16. [16] M.E. Macovschi, Stud. Cereet. Chim, 20 (1972)849. [17] V. I~zarescu, O. Radovici and M. Vass, Rev. Roum.
Chim. 32 (1987) 895. [18] R. Parsons, Surf. Sci. 101 (1980)316. [19] B.E. Conway, H. Angerstein-Kozlowska and F.C, Ho, J.
Vac. Sci. Technol. 14 (1977) 351. [20] B.E. Conway. Prog. Surf. Sei. 16 (1984) 1. [21] R.L. Moss and L. Whally, Adv. Catal. 22 (1972) 115. [22] J. Clavilier and J.P. Chauvineau, J. Electroanal. Chem.
100 (1979) 461. [23] V. l~z-~rescu. O. Radovici and M. Vass, Electrochem.
Acta 30 (1985) 1407. [24] V. Lfiz~rescu, O. Radovici and M. Vass, Rev. Roum.
Chim. "31 (1986) 461. [25] P. Stonehart. Electroehim. Acta 13 (1968) 1789. [2,5] B.V. Tilak, R.S. Perkins, H. Angerstein-Kozlowska and
B.E. Conway. Electrochim. Acta 17 (1972) 1447. [27] B.G. Pound, D.D. Macdonald and J.V¢. Tomlinson, Elec-
trochim. Acta ~ (1980) 563. [28] G.E. Rhead, Acta Met. 13 (1965) 233. [29] S.K. Sharma and J. Spitz, Thin Solid Films 56 (1979) LI7.