Applications of Surface Science 19 (19X4) I-13 North-Holland. Amsterdam CHEMICAL MODIFICATION PROPERTIES OF NICKEL * Received 17 October 1983: accepted OF CHEMISORPTIVE for publication AND CATALYTIC 1X June 1984 Several reactions representing important categories of catalytic systems have been studied on chemically modified single crystal surfaces. These reactions are methanation of CO and CO:. hydrogenolysis of ethane. hydrogenation of ethylene. and q&propane ring-opening and hydrogenolysis. Poisoning of the above reactions by ordered. suhmonolayer coverages of sulfur shou large nonlinear effects for sulfur coverages versus reactivity attenuation. These data together with related chemisorption results are reviewed with emphasis on the author’s own work. These studies suggest that the dominant effect in poisoning by sulfur is an electronic one and extends over distances larger than the atomic radius. Related studies have addressed the role of potasstum promoters in nickel catalysts for methanation. Potassium decreases the rate of methane formation and increases the rate of higher hydrocarbons relative to the clean nickel surface. Similar results have been reported for supported nickel catalysts suggesttng that support effects play a small role in catalytic promotion by potassium. 1. Introduction It has long been recognized that the addition of impurities to metal catalysts can provide large effects on both activity, selectivity, and resistance to poisoning of the pure metal [l]. For example, the catalytic properties of metals can be altered greatly by the addition of a second transition or group IB metal or by adding promoters such as potassium or sulfur. On the other hand catalytic processing is often plagued by loss of activity due to the inadvertent contamination of catalysts by undesirable impurities. In either case the catalytic properties are dramatically altered by the modification of the chemistry by the surface impurity. Although these effects are well recognized in the catalytic industry, the details of how these chemical alterations come about are not at all understood. Difficulties are encountered in interpreting much of the existing literature addressing this question because of the uncertainty in the location of the impurity (support or metal particle). the impurity concentration at the metal surface, and the chemical nature of the impurity. In general these * This work was performed at Sandia National Laboratories and supported ment of Energy under contract number DE-AD04-76DP00789. 037%5963/84/$03.00 0 Elsevier Science Publishers (North-Holland Physics Publishing Division) B.V. by the US Drpart- difficulties can be circumvented if model catalytic systems such as metal single crystals can be used in conjunction with surface analytic iechniques. This combination of kinetics at elevated pressures coupled with surface spectroacopies has been used extensively to study methanation of CO [2] and CO1 [3] as well as alkane hydrogenolysis reactions [4,5]. The appropriateness of these idealized systems as models for supported catalysts has now been well-documented for several reactions [2-41 and will not be discussed here. We wish in this discussion to survey our recent studies in probing the fundamental mechanism by which impurities, either electropositive or electronegative relative to nickel, change the chemisorptive or catalytic properties of single crystal surfaces of this material. This will include a comparison of the results obtained on these model systems with similar data derived by others on supported metal systems. 2. Experimental These studies used the specialized apparatus [2.5] shown in fig. 1. The custom-built catalytic reactor, contiguous to the surface analysis system, employs a retraction belows that supports the metal crystal and allows translation in situ from the reactor to the surface analysis chamber. A liquid-nitrogen cooled manipulator in conjunction with a line-of-sight mass spectrometry was used for the thermal desorption experiments described. The base pressure in MASS SPECTROMETER ELECTRON I GAS CATALYTIC GUN CHROMATOGRAPH REACTOR 3 IRGY I ION Fig. 1. operation An ultrahigh at atmospheric vacuum apparatus pressure ANALYSIS AND SURFACE PREPARATION CHAMBER PUMP for in a catalytic studying reactor. single crystal catalysis before and after the analysis chamber and the reactor is lo- “’ Torr. The single crystals of nickel (- 1.0 cm’ surface area) are mounted on tungsten leads and heated resistively. The samples were cleaned by oxidation at 1400 K in lop6 Torr 0, followed by reduction at 800 K in 5 Torr H,. A typical Auger spectrum of a clean nickel surface is given in refs. [2] and [5]. 3. Discussion 3. I. Electronegative modifiers 3. I. I. Modification of chemisorptioe properties The effect of preadsorbed electronegative adsorption-desorption using thermal behavior programmed atoms Cl, S, and P on the of CO and H, on Ni(lOO) has been studied [6] desorption (TPD), low energy electron diffraction (LEED), and Auger spectroscopy (AES). It has been found that the presence of the electronegative atoms causes a reduction of the adsorption rate, the adsorption bond strength and the capacity of the Ni(lOO) surface for CO and H, adsorption. The poisoning effect becomes stronger with increasing electronegativity of the preadsorbed atoms. The observed effect of preadsorbed submonolayers of Cl, S, and P on CO TPD curves is shown in figs. 2a-2c. The additives Cl. S, and P were dosed the surface was from Cl,, H,S, and PH,, respectively. When appropriate, flashed to a sufficient temperature to eliminate any residual surface hydrogen. Coverages were based on a combination of Auger, LEED, and TPD measurements. The CO curves represent sorbed adlayer coverages CO coverage. presence As can be seen the CO of the preadsorbed pronounced the total CO desorption after a CO exposure adlayer. sufficient uptake The effects decreases markedly of P, however, than for Cl, or S. Fig. 3 shows the observed total CO uptake on the corresponding Cl no CO desorption was detected for different pread- to reach the stationary in the are much less dependence of the precoverage of impurity. In the case of at coverages > 0.4 monolayers, ML, whereas even for saturated S and P precoverages, some low temperature desorption peaks were detected. Adlayers of Cl, S and P cause a reduction of hydrogen uptake and a shift of the TPD peak maxima to a lower temperature. As shown in figs. 4a-4c, at higher foreign atom precoverages a lower temperature state becomes more pronounced. The extent of the effect increases in the sequence P, S, Cl. As shown in fig. 5, the reduction of H, coverage is most rapid in the presence of Cl atoms such that at chlorine coverages higher than 0.2 a negligibly small amount of desorbing hydrogen is detected. Since the Cl, S and P atomic and covalent radii are similar (0.99, 1.04 and 1.10 A, respectively [20]) it was concluded that the electronegativity factor plays a major role in explaining the difference in their poisoning effect. L? I+: Goodnw~ 4 / C‘henmol nmh/rutrot~ ofproprrtrr~ o/ .%‘I A similar study [7] to that discussed above has been carried out presence of C and N. These impurities have the same electronegativities and Cl, 2.5 and 3.0. respectively. The comparison N and those for S and electronegativity effects Cl are entirely consistent dominate poisoning of with occupying close atomic size. the same between the results with the interpretation chemisorption adsorption sites. in the as S for C and that for adatoma In the case of APco El,, =o =o.os =0.17 =o.z&? loo 200 300 ‘ma 500 TEMPERATURE SM) (K) S APCC APcc 200 TEMPERATURE Fig. 2. Effect deaorption of varying from (K) (a) chlorine, Ni( 10). CO exposure 300 400 500 600 TEMPERATURE (K) (h) sulfur, of 6 L. and (c) phosphorus precovemgr c,n CO thermal D. W. Goodmm / Chemrcul modifcutwn ofpropertresof 5 Nr adatoms with the same electronegativity but with different atomic radii (S and C, Cl and N), the effect becomes less pronounced with decreasing atomic radius. eT co 0 0.1 0.2 0.3 ADlll-fIVE Fig 3. Dependence 0.4 0.5 COVERAGE 0.6 0.7 (ML) of total CO adsorption on additive 1 100 precoverage A 200 zo.17 300 400 TEMPERATURE(K) 500 AA P *pIi, ep=o 25 fi I lO\ 200 Fig. 4. Effect desorption 400 300 TEMPERATURE (K) of varying 200 500 (a) chlorine, from Ni(lOO). H, exposure 1 I 500 400 300 TEMPERATURE IKI (b) sulfur. and (c) phosphorus of 10 L. 1 precoverage on H, thermal D. W. Coodmun / Chemrwl modi’icutml 6 3.1.2. Modification Kinetic function reaction similar of cata(vtic actiuig studies [3,6,8,9] of sulfur coverage over Ni(lOO), to results of properr~es O/ NI have been carried over Ni(lOO) the sulfided surface for the clean surface out and for Ni(lll). For (fig. 6) shows at considerably n several reactions as a the methanation behavior remarkably reduced hydrogen partial Cl .S AP 0 Fig. 5. Dependence 0.1 0.2 0.3 0.4 ADDITIVE COVERAGE (ML) of H, adsorption on additive I 0.5 precoverage Id NCH4 10 IO 1 /T -1O3 (K-l) Fig. 6. An Arrhenius plot of the rate of methanation over a sulfided Ni(lOO) catalyst at 120 Torr and a Hz/CO ratio equal to four. 0,‘s are expressed as fractional monolayers. NC,, is the turnover frequency or the number of methane molecules produced per nickel atom site per4second. D. W. Goodman / Chenucd ofpropertresof Ni modification 7 pressure. For clean Ni(lOO) [2] a departure from Arrhenius linearity is observed at 700 K. Associated with the negative deviation of this plot is a rise in the surface carbon level. This rise in carbon level continues until the carbon level reaches 0.5 ML, the saturation level. This deviation, or rollover, of the Arrhenius plot has been interpreted as reflecting or critical hydrogen coverage of 4% the reaction linearity increase This from a saturation adsorbed behavior indicates surface the chemisorption the kinetics that atomic of the rate of surface sulfur sulfur conditions at 600 K, some 100 K lower reaction in surface carbon level is associated with steady-state surface. Both rate at identical the departure coverage. carbon results and the hydrogen sulfur hydrogenation. discussed above the TPD studies departs effective which These results results for Hz on a sulfur show that surface similarly temperature. this deviation is very coverage of atomically For a sulfur from Here too, an from linearity. in reducing the in an attenuation are consistent poisoned the poisoning is very nonlinear. Fig. 7 shows this nonlinear relationship coverage and the methanation rate at 600 K. A precipitous with Ni(lOO) effect of between the drop is seen for the catalytic activity at the lower sulfur coverages. The poisoning effect quickly maximizes and no further reduction in reaction rate is found at sulfur levels exceeding 0.2 monolayers. An identical reduction of methanation activity for supported Ni/AI,O, has been observed by Rostrup-Nielsen and Pedersen for sulfur poisoning [lo]. These authors also observed a nonlinear effect of sulfur on the reaction rate and, as here, a constant activation energy with sulfur coverage. The initial change in the reaction rate poisoning in fig. 7 suggests that ten or more equivalent nickel sites are deactivated by one sulfur atom. There are two possible causes for this effect: (a) a long-range electronic I I 0.2 0.3 0.4 Additive Coverage (ML) Fig. 7. Methanation rate as a function of phosphorus and sulfur coverage Pressure = 120 Torr, Hz/CO = 4. Reaction temperature = 600 K. on a Ni(100) catalyst. effect (ligand effect) or (b) an ensemble effect, the requirement that a certain number of surface atoms are necessary for a reaction to occur. Experimentally these two possibilities can be distinguished. If long-range electronic effects are most important. then the reation rate should be expected to be a function of the relative electronegativity of the poison. If indeed a t.en nickel atom ensemble is required for methanation then changing the electronic character of the poison should have little effect on the reaction rate. Substituting phosphorus for sulfur in a similar set of experiments [9] results in a marked change in the magnitude of poisoning at low coverages as indicated in fig. 7. Phosphorus. presumably because of its less electronegative character, poisons only the four nearest neighbor metal atom sites. These results support the conclusion that long-range electronic effects are playing a major role in the sulfur deactivation Similar catalytic ethylene of a nickel methanation catalyst. nonlinear poisoning of nickel by sulfur reaction including ethane hydrogenation [ll]. and suggest that the dominant and extends over distances 3.2. Electropositive has been seen for other [ll] and cyclopropane hydrogenolysis CO1 methanation [3]. These studies influence of sulfur poisoning larger than the atomic radius is an electronic of sulfur. [Xl. also one modifier5 Alkali atoms on a transition metal ionic state, donating a large fraction surface are known to exist in a partially of their valence electron to the metal, resulting transition This been in a work function decrease. metal surface atoms has explaining adsorbed activity the role of alkali molecules in ammonia electronegative adatoms additional electron density on the shown to be a major factor in in altering the chemisorption bonding of such as N, [ 121 or CO [13]. and in promoting catalytic synthesis [14]. We have discussed above the role of impurities in poisoning nickel toward methanation activity. These results have been ascribed, to a large extent, to an electronic effect. In the context of this interpretation it is expected that an electropositive additive such as potassium might have the opposite effect, i.e. to increase nickel’s methanation although activity. certain steps A recent study in the reaction [15] has shown mechanism that this is not are strongly the case accelerated by the presence of potassium. Kinetic measurements of methanation over a Ni(100) catalyst containing well-controlled submonolayer quantities of potassium adatoms show a decrease in the steady-state rate under a variety of reaction conditions (fig. 8). The presence of potassium did not alter the apparent activation energy associated with the kinetics. The potassium did, however, change the steady-state carbide coverage which increased from 10% of a monolayer for clean Ni(lOO) to 30% of a monolayer Adsorbed for a potassium coverage of 10% of a monolayer. potassium caused a marked increase in the steady-state rate and selectivity of Ni(lOO) for higher hydrocarbon studied, the overall rate of higher hydrocarbon potassium-dosed surface; so that potassium with respect to this reaction, Fischer-Tropsch synthesis. At all temperatures production was faster on the may be considered synthesis. In a manner identical to that used for the clean of carbide formation via CO disproportionation 01 I 0 8. Relative Ni(lOO) surface [16], the rate (2 CO + C.,,, + CO,) was 171 0.05 0.10 POTASSL&l Fig. a true promoter methanation 0.15 COVERAGE rate as a 0.20 (ML) function of potassium coverage at various reaction conditions. r = 1 .02 0 .04 .08 .06 .l POTASSIUM COVERAGE (ML) Fig. 9. function The relative of potassium initial rate coverage. of reactive carbon formation PC.,, = 24 Tom, T = 500 K. from CO disproportionation as a measured for the potassium-covered surfaced carbide (as determined by Auger spectroscopy) the carbon-free tion. The surface. increase potassium coverage reduction Potassium of the markedly initial is shown of the activation in energy increases rate of fig. 9. Of from by observing the growth in with time in CO. starting from carbide the rate of CO dissociabuildup at particular 23 kcal mol- 500 K with significance is the ’ for the clean Ni(100) surface to 10 kcal mol-’ The model, for a 10% surface coverage of potassium. effects of potassium upon the kinetics of CO hydrogenation on this single-crystal Ni(lOO) catalyst are to: (I) decrease the rate of methane formation, and (2) increase the rate of higher hydrocarbon production. These same effects have been reported for high-surface area-supported nickel catalysts. This agreement between bulk. indicates that the major mechanism catalyst’s activity and selectivity it is rather a consequence been drawn in the case found iron-free that atoms of the support Potassium adatoms then disproportionation reaction carbon coverages. is not related of direct K-Ni of iron catalysts the potassium areas single crystal nickel and supported nickel by which potassium additives alter the to the support material, but that interactions. A similar conclusion has for ammonia synthesis where it was reside upon patches of iron and not upon [17]. cause a very large increase in the rate of the CO and a decrease in its activation energy for low At low carbon coverages and the conditions of our measure- ments the surface should be covered with adsorbed CO so that CO adsorption does not limit the disproportionation rate. Similarly, oxygen removal via CO, formation is relatively rapid so that CO disproportionation must be rate-limited instead by the dissociation of adsorbed CO into atoms. The observation of a potassium-induced disproportionation is then consistent with the adsorption observed Ni(lOO) [13]. These been explained tive potassium adsorbed increase increase carbon and oxygen in the rate of CO in the heat of CO in the thermal desorption studies from alkali-covered effects are also observed on other metals, and they have in terms donates of an electronic extra electron ligand effect. whereby density to the nickel which in turn donate electron density to the adsorbed CO increases the extent of backbonding in the metalLC0 complex, increased metalLC0 bond strength and a decrease in GO bond the electroposisurface atoms. molecule. resulting This in an strength. This model satisfactorily explains the decrease in the activation energy for carbide build-up (rate-limited by CO dissociation) brought about by potassium. This is entirely analogous to the explanation for dissociative N2 adsorption on potassium-promoted iron [18]. In spite of this increase in the rate of CO dissociation or carbide buildup, the overall rate of methanation decreases and the activation energy is unchanged in the presence of potassium. This indicates that other step in the methanation sequence, either hydrogen adsorption or hydrogenation but not CO dissociation, is rate-limiting for methane production under these condi- tions. It should be noted that an increasing carbide level has been associated with a decreasing methanation rate on clean Ni(lOO) [19]. The most noticeable influence of potassium addition upon surface coverages is to increase markedly the coverage of molecular CO since potassium increases its heat of adsorption. On clean Ni(lOO), it was shown [16] that increasing the carbide level increases the rate of carbide removal by hydrogenation with Hz (in the absence of CO where the hydrogen addition step is clearly rate-limited). The decrease in methanation activity brought about by potassium must therefore be related to a poisoning of either the hydrogen adsorption or hydrogen addition steps by a combination of adsorbed potassium and the consequently higher CO coverages. Potassium was shown to decrease the rate of hydrogen adsorption on iron, and CO is known to decelerate hydrogen adsorption on Ni(100). Surface carbide is also known to decrease the hydrogen adsorption rate on Ni(100). The effects of potassium and addition step are not known. The influence of adsorbed carbons is likely is consistent that carbon adsorbed CO potassium upon upon the rate of the the synthesis with results on supported catalysts. chain growth is rate-limiting. Thus hydrogen of higher hydro- For these reactions, the observed effect it of potassium to increase the steady-state carbide coverage can be related to the increase in supply of reactants for chain growth. That is. the more carbon present on the surface, the greater the chances C-C bond formation. This satisfactorily activity for higher hydrocarbon production sium. It is also consistent with the observation for reaction explains increases events leading to the observation that the upon dosing with potas- on clean Ni(lOO) that conditions 0 / K=O.lOML iw;; = 0 20 TIME 40 60 80 (MINUTES) Fig. 10. Methane production from a C02/H, (b) a sulfided Ni(lOO) catalyst, (c) a potassium covered Ni(lOO) covered Ni(lOO) catalyst. reaction mixture over (a) a clean Ni(lOO) catalyst. covered Ni(100) catalyst, and (d) a potassium + sulfur leading toward to higher equilibrium higher hydrocarbons. Intrinsic electronic to interpreting effects should moderate Recent experiments [3]. Referring carbide catalytic is the inference or compensate have shown coverages poisoning for the effects promotion in terms of an electropositive of an electronegative of sulfur decreases 01 impurity impurity. methanation the rate of methane of potassium in the presence the effects of sulfur. of sulfur and conclusions and promoters integrating kinetic can be quite useful modify have been used to examine tive and reactive properties atoms distributions this to be true in the case of CO, to fig. 10, the adsorption Catalytic studies analytical techniques poisons the product and that adsorption formation significantly. The adsorption shows that the potassium can neutralize 3. Summary shifts surface measurements with modern surface in detailing the mechanisms by which chemistry. Model single crystal catalysts the effects of surface impurities on the chemisorpof nickel. The effect of preadsorbed electronegative Cl. N, S. C. and P on the adsorption-desorption on a Ni(lOO) surface have been addressed. behavior of CO and H1 It is found that the presence of these impurities causes a reduction of the adsorption rate. the adsorption strength and the capacity of the surface for CO and Hz. The poisoning effect becomes stronger with increasing electronegativity of the preadsorbed atoms. Reactivity studies on the methanation reaction over a sulfided Ni( 100) catalyst indicate that poisoning by sulfur at low coverages is long-range in that one sulfur atom deactivates ten or more nickel atom sites. Ancillary studies with phosphorus demonstrate a correlation between the electronegativity of the poison and its ability to attenuate methanation activity. Potassium addition to a Ni(100) catalyst results in a marked increase in the ability of the surface to dissociate CO together with a significant decrease in the associated activation energy. The overall methane formation rate falls with a corresponding increase in the higher hydrocarbon production. These results suggest that the promotion mechanism of potassium does not require metal-support interaction or a support material. The results outlined here are but a few that have been obtained in the surface science area, addressing the effects of surface impurities on surface chemistry. These kinds of studies, particularly when coupled through kinetics with similar ones on supported catalysts. can be invaluable in defining the fundamental mechanisms by which surface modifiers change the course of catalytic reactions. The insights so developed will be helpful in the design of new generations of more efficient practical catalysts. Acknowledgement We would like to acknowledge the partial support Department of Energy, Office of Basic Energy Sciences, Sciences. of this work by the Division of Chemical References [I] Metal-Support and Metal-Additive Effects m Catalysis. Eds. B. Imelik. C. Naccache. G. Coudurier, H. Praliaud. P. Meriaudeau, P. Gallerot. G.A. Martin and J.<‘. Vrdrine (Elsevier. Amsterdam. 1982) p, 315. [2] D.W. Goodman. R.D. Kelley. T.E. Madey and J.T. Yates. Jr.. J. Catalyuc 63 (19X0) 226. [3] D.E. Peeblrs. D.W. Goodman and J.M. White. J. Phys. Chem. X7 (19X3) 437X. [4] D.W. Goodman, Act. Chem. Res. 17 (1984) 194. [5] D.W. Goodman, J.T. Yates. Jr. and T.E. Made?. Surface Sci. 93 (1980) L135. [6] M. Kiskinova and D.W. Goodman, Surface Sci. 108 (19X1) 64. [7] M. Kiskinova and D.W. Goodman, Surface Sci. 109 (19X1) L555. [X] D.W. Goodman. J. Vacuum Sci. Technol. 2 (1984) X73. [9] D.W. Goodman, in: Proc. AIChE Meeting. 1984. [lo] J.R. Rostrup-Nielsen and K. Pedersen. J. Catalysis 50 (1975)395. 1111 D.W. Goodman. in preparation. [I21 S. Anderson and U. Jostell, Surface Sci. 46 (1974) 625. [13] M. Kiskinova, Surface Sci. 11 (1981) 584. [I41 G. Ertl, Catalysis in Rev.-Sci. Eng. 21 (19X0) 201. [15] C.T. Campbell and D.W. Goodman. Surface SCI. 123 (19X2) 413. [16] D.W. Goodman. R.D. Kelley. T.E. Madey and J.M. White. J. Catalysis 64 (1980) 479. [17] G. Ertl. to be published. [1X] G. Ertl. S.B. Lee and M. Weis. Surface SCI. 114 (19X2) 527. [19] R.D. Kelley and D.W. Goodman, Surface Sci. 123 (1982) L743. [20] C. Kittel. Introduction to Solid State Physics (Wiley. New York. 1971).
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