Flash Photolysis Studies of Reactive Organometallic Intermediates

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7 Flash Photolysis Studies of Reactive Organometallic Intermediates Relevant to Homogeneous Catalysis Peter C. Ford and Simon T. Belt Department of Chemistry, University of California, Santa Barbara, C A 93106

The application of flash photolysis with time-resolved optical and infrared detection techniques to the study of reactive organometallic intermediates is described. Examples of these studies are given for several systems. These include tricoordinate rhodium(I) phosphine complexes proposed to be key intermediates in the homogeneous catalytic activation of dihydrogen and the photocatalytic activation of C-H bonds, the coordinatively unsaturated metal carbonyl cluster Ru (CO) , plus manganese(I) intermediates relevant to the carbonylation of metal-carbon bonds via migratory insertion. 3

11

T H E N A T U R E A N D D Y N A M I C S of key reactive intermediates must be characterized for a thorough understanding of homogeneous catalysis mechanisms. Such species are generally formed only in (very) low steady-state concentrations. Thus they are difficult to observe by direct methods during a catalytic cycle, and their presence usually can only be inferred from such methods as kinetics studies and stereochemical results. However, by using the flash photolysis technique, it is possible to generate relatively high nonequilibrium concentrations of organometallic intermediates that can be interrogated kinetically and spectroscopically (see e.g., refs. 1-19). In this context, one might anticipate using flash photolysis to probe a wide variety of other reactive species including electronic excited states (ES), coordinatively unsaturated complexes formed by ligand dissociation or reductive elimination, redox partners of E S electron-transfer reactions, radical products of homolytic bond cleavages, and unstable isomers produced by 0065-2393/92/0230-0105$06.00/0 © 1992 American Chemical Society

In Homogeneous Transition Metal Catalyzed Reactions; Moser, W., et al.; Advances in Chemistry; American Chemical Society: Washington, DC, 1992.


106

H O M O G E N E O U S TRANSITION M E T A L C A T A L Y Z E D REACTIONS

E S isomerizations. Under favorable circumstances the characterizations are aided by comparison with data from low-temperature matrix experiments. Under these conditions, intermediates, which would have high reactivity at ambient temperature, may be trapped indefinitely and studied by using a full range of spectroscopic methods (20). This chapter describes several studies in which flash lamp and laser flash photolysis with time-resolved optical and IR detection were used to probe the structure and dynamics of reactive organometallic intermediates of the type routinely proposed in thermal catalytic cycles. This overview will focus on three systems: 1. intermediates in catalysis and photocatalysis by rhodium(I) phosphine complexes, 2. coordinatively unsaturated carbonyltriruthenium clusters, and 3. intermediates relevant to the mechanism of migratory C O insertion into metal-alkyl bonds. In all three examples, the intermediates studied were coordinatively unsaturated species generated by the photodissociation of carbon monoxide.

Rhodium(I) Phosphine Intermediates In a study carried out several years ago by our group (21), flash lamp photolysis with optical detection revealed that irradiation of RhCl(CO)(PPh ) in benzene solution results in C O labilization to give the 14-electron tricoordinate complex RhCl(PPh ) (A). This intermediate is often proposed as the active species involved in the catalytic hydrogénation of alkenes by Wilkinson's complex RhCl(PPh ) (22). The reaction dynamics of this intermediate are summarized in Scheme I. Consistent with the previous proposals, A displayed a reactivity (k = 1 x 10 M s" ) toward H more than 4 orders of magnitude greater than that of the 16-electron trisphosphine complex RhCl(PPh ) . 3

3

2

3

3

5

x

3

2

1

1

2

3

RhCl(PPh ) 3

2

+ H 400 nm), is proposed to occur via formation of a high-energy isomer of R u ( C O ) . At short wavelengths, substitution by donor ligands (eq 7) is the dominant pathway. Substitution has been proposed to occur via formation of the coordinatively unsaturated triruthenium cluster R u ( C O ) , the type 3

3

3

12

12

12

irr

3

12

3

n


110


RhCI(CO)L

2


= 30-300 ps (dep. on L)

C-H Activation Products C H "+ CO — * C H CHO 6

9 6

! Ç-C H 6

RhCI(CO)L2

e

12

— - Q-C H e

s

10

• H

2

Scheme II. C-H activation hy Rh(I) photocatalysts. of intermediate proposed for photoassisted hydrogénation of alkenes by clusters. Λν(λ>400 nm)

Ru (CO) 3

+ 3L

12

> 3Ru(CO) L

(6)

4

Μ λ < 4 0 0 nm)

Ru (CO) 3

> Ru (CO)nL + C O

+ L

12

(7)

3

In accord with these observations, short-wavelength flash lamp photol ysis (\ > 315 nm, using optical detection techniques) of R u ( C O ) in tetrahydrofiiran (THF) solution demonstrated the formation of an interme diate proposed to be R u ( C O ) ( T H F ) , which reacts with donor ligands via rate-limiting dissociation of T H F . When the reaction was carried out in cyclohexane, the R u ( C O ) S adduct proved too short-lived to allow direct observation (S is solvent). The substitution products R u ( C O ) L were formed within the duration of the 3 0 - μ 5 flash. irr

3

3

3

12

n

u

3

n

We extended these studies of the kinetic behavior of the transients characteristic of the photosubstitution pathways by using X e C l excimer laser as the 20-ns excitation source with an IR diode laser as the probe source and a H g - C d - T e fast IR detector system (55). This system allows the de termination of time-resolved infrared (TRIR) spectra. Laser flash photolysis (308 nm) of R u ( C O ) in isooctane under A r results in formation of a transient IR spectrum (200 ns). Figure 1 shows depletion of the carbonyl stretching ( v ) bands at 2061, 2031, 2017, and 2011 cm" 3

12

co


1

FORD & B E L T

Reactive Organometallic Intermediates


7.


111

112


characteristic of this cluster and the appearance of several new bands assigned to an isomer of R u ( C O ) (C). This intermediate was previously reported as one short-wavelength photolysis product in low-temperature hydrocarbon glasses (56). In T H F or in mixed cyclohexane-THF solutions, the relatively stable solvent complex R u ( C O ) T H F (D) was observed and identified on the basis of its v band at 2049 c m " [cf. R u ( C O ) · 2 M e T H F at 2049 c m in hydrocarbon glasses (56)]. In the absence of added C O , C decays via second-order kinetics to regenerate R u ( C O ) i . The second-order rate constant (k = 2.4 Χ 10 M ~ s" , determined from the first-order rate plots at various excess C O concen trations) for reaction with C O proved to be within an order of magnitude of the diffusion-controlled limit (1.3 Χ 10 M " s" ) in isooctane (55) and 3 orders of magnitude larger than those found for the intermediates C r ( C O ) or M n ( C O ) in alkane solutions (I, 5, 7, 10). Thus, we conclude that there must be negligible stabilization of C either by the isooctane solvent or from the bridging C O reported (56) to be a feature of its structure. In alkane solutions containing T H F , trapping by C O to give R u ( C O ) and by the donor ligand T H F to form D are competitive. However, D itself is labile and reacts with C O to re-form the starting cluster. T h e reactivity of this transient as a function of [ T H F ] and [CO] proved to be consistent with a limiting dissociative substitution mechanism. These observations are sum marized in Scheme III. 3

u

3


c

3

n

1

o

3

1

u

2

9

2

l

1

10

1

1

5

2

9

3

Unsaturated Mononuclear Carbonylmanganese

12

Compounds

Carbon-carbon bond formation is a key step in catalytic C O activation in homogeneously catalyzed processes such as hydroformylations of alkenes, carbonylations of alcohols, homologations of carboxylic acids, and reductive C O polymerization (57). One fundamental organometallic reaction com monly invoked in proposed schemes for such catalytic cycles is the reversible migratory insertion of C O into an alkyl-metal bond (58), for which eq 8 serves as a prototype.

CH

O.

/CH

3

3

+ CO (8)

C Ο Our third example of using flash photolysis techniques to probe the structures and dynamics of reactive organometallic intermediates involves a study of coordinatively unsaturated mononuclear Mn(I) carbonyls. This study In Homogeneous Transition Metal Catalyzed Reactions; Moser, W., et al.; Advances in Chemistry; American Chemical Society: Washington, DC, 1992.

7.

FORD & BELT

Ru (CO) 3

113


i l £ 2

12

^

Ru (CO) 3

n

c


+co

Ru (CO) 3

Ru (CO)i2 3

n

Ru (CO) (THF) 3

n

D Scheme III. Reactions of the coordinatively unsaturated cluster Ru3(CO)n. was initiated with the aim of obtaining a deeper understanding of such C - C bond formation mechanisms. Investigations focusing on eq 8 (59-62) concluded that this reaction proceeds via methyl migration (as opposed to C O insertion) with rate-limiting formation of an unsaturated acyl intermediate, ( C H C O ) M n ( C O ) (E). Donor solvents and other nucleophiles have marked effects on the reaction dynamics (63-65). Despite the extensive kinetic and stereochemical studies carried out to elucidate the overall reaction mechanism, there has been no direct observation of the 16-e" acyl intermediate E . In this context, our preliminary studies have shown that laser flash photolysis of ( C H C O ) M n ( C O ) causes C O photodissociation. A transient forms and undergoes solvent-dependent rearrangement to the alkyl complex competitive with trapping by C O to regenerate the starting complex (66). Preliminary data suggest that the reactive intermediate formed in hydro carbon solutions may be the η bound acyl species F , consistent with the oretical predictions (67, 68). In T H F this intermediate is the η acyl species G with a solvent molecule in the cis coordination site. Such results offer one possible reason for the marked solvent effects on migratory insertion rates. 3

3

4

5

2

1

F

G


114


The

behavior of the acyl complex has also led us to investigate with

time-resolved optical and infrared techniques the transient intermediates resulting from the flash photolysis of C H M n ( C O ) 3

(H).

5

O u r goal was to

provide a model for the pertinent spectroscopic and kinetic data relevant to unsaturated Mn(I) intermediates (69). Laser flash photolysis (X

= 308 nm)

irr

of H in cyclohexane or isooctane solutions results in the 100-μ5 TRIR spec trum shown in Figure 2.


The depletion of Η is evident with the negative absorbance changes (A

Abs

) values noted for v

modes at 2014 and 1991 cm" . Accompanying 1

c o

these changes, a transient species is formed that has three v 1986, 1974, and 1940 cm" in the TRIR spectrum and a X 1

m a x

c o

bands at

at 410 nm in

the optical spectrum. These properties are close to those attributed to cisC H M n ( C O ) · C H , which is formed by C O photodissociation from H in a 3

4

4

methane matrix (70). These spectroscopic observations are consistent with the photolabilization of C O followed by solvation to give d s - C H M n ( C O ) S 3

4

(I). hv CH Mn(CO) 3

5

+ S

> cts-CH Mn(CO) S + C O 3

(9)

4

0.04

-0.06

I 2040

ι

1 ι 2020

\ ι 2000

ι 1980

1

1 1960

Wavenumbers / cm "

1

1 1940

1

1 1920

1

Figure 2. Time-resolved IR spectrum obtained 100 μ$ after laser flash pho tolysis of CH Mn(CO)s in isooctane under Ar. The negative bands correspond to the depletion of CH Mn(CO) ; the positive bands correspond to cisCH Mn(CO) S. 3

3

5

3

4


7.

FORD & B E L T

115


We have not observed transients resulting from either trans-CO labilization or homolytic metal-alkyl bond cleavage. However, prolonged irra diation leads to the appearance of visible and IR absorbances that indicate the production of M n ( C O ) . 2

10

The decay kinetics of I are consistent with the reaction with C O . Under argon the decay of I follows second-order kinetics. In contrast, under C O both the rates of decay of I and the re-formation of C H M n ( C O ) are ac celerated and follow pseudo-first-order kinetics (Figure 3). The second-order rate constant for the reaction of c i s - C H M n ( C O ) S with C O (2.1 ± 0.1 x 10 M " s" ) shows excellent agreement between the IR and optical detection methods. It lies in the same range as other weakly bound solvent-carbonylmetal intermediates, such as C r ( C O ) S , measured by flash photolysis techniques (I, 6, JO).


3

3

6

1

5

4

1

5

Significantly, when T H F is used as the solvent, the reaction of I with C O (as studied by optical detection) is 4 orders of magnitude slower (k = 1.4 Χ 10 M " s' ). This change is consistent with the increased donor strength of T H F . Thus, the combined spectroscopic and kinetic data show that photolysis of C H M n ( C O ) in hydrocarbon or T H F solutions results in 2

2

1

1

3

5

ο

Ε c ο

400

800

1200

1600

Time, /is Figure 3. Kinetic traces showing the decay of cis-CH Mn(CO) S (S is cyclo hexane) at 1976 cm and the reformation of CH Mn(CO) at 2014 cm following laser flash photolysis of CH Mn(CO) in cyclohexane under 0.1 atm of CO. IR spectral changes are shown in transmittance mode. 3

1

3

3

5

4

1

5


116


the formation of m - C H M n ( C O ) S (S is solvent), which reacts with C O at rates comparable to those found for analogous solvent complexes of d carbonylmetals. Although c i s - C H M n ( C O ) S is the first transient species observable in these experiments, competition experiments suggest that the primary photoproduct C H M n ( C O ) shows a remarkable selectivity toward reaction with C O over alkane solvation. In cyclohexane the yield of I from the photolysis of H is a factor of 5 higher under argon than under C O , with otherwise identical conditions. This feature, which has been observed by both TRIR and optical detection methods, is unprecedented for simple earbonylmetals of this type. It suggests that C H M n ( C O ) is sufficiently long-lived to be trapped selectively by C O relative to the solvent alkane (Scheme IV). 3

4

6

3


3

4

4

3

4

In contrast, we observed no [CO] dependence on transient yields following irradiation of H in T H F or of C r ( C O ) in cyclohexane. Thus, C H M n ( C O ) must be trapped much more effectively by the stronger donor, T H F . In the case of C r ( C O ) , our observations are in accord with the extremely rapid solvation of the singlet state C r ( C O ) fragment as measured by other workers (12-17). Apparently the lifetime of this species is too short to allow for selectivity between C O (10~ M) and solvent. One possible explanation for the apparent selectivity of the C H M n ( C O ) fragment would be that this species is formed in a triplet ground state having either a trigonal bipyramidal C geometry with an axial C H ligand or a 6

3

4

6

5

2

3

3 t

CH MniCO> 3

5

4

3

•

CH Mn(CO) 3

4

CH Mn(CO)< 3

Scheme IV. Competitive trapping of the unsaturated intermediate CH Mn(CO) (E). 3


4

7.

FORD & B E L T


117

square pyramidal geometry with a basal C H ligand (71). Either geometric or electronic constraints may give this species sufficient lifetime to dem onstrate selectivity in coordinating a sixth ligand. 3


Acknowledgments Key contributors to the experimental studies summarized here are David A. Wink, Cris Tina Spillett, John DiBenedetto, and David W. Ryba (all of U C S B ) and T. L . Netzel and D . Pourreau (of Amoco Technology Company). This research was sponsored by a grant (DE-FG03-85ER13317) from the Division of Chemical Sciences, Office of Basic Energy Sciences, U . S . D e partment of Energy. The instrumentation used was constructed from com ponents purchased with funds from the National Science Foundation (CHE-87-22561 and C H E - 8 ^ 1 1 3 0 2 0 ) , the U C S B Faculty Research C o m mittee, and the U C S B Quantum Institute, and from components donated by the Newport Corporation and the Amoco Technology Company. S. T. Belt acknowledges support from a N A T O Fellowship awarded through the Science Engineering Research Council (United Kingdom).

References 1. Kelly, J. M.; Bent, D. V.; Herman, H.; Schulte-Frohlinde, H.; Koerner von Gustorf, E. J. Organomet. Chem. 1974, 69, 259-269. 2. Kelly, J. M.; Bonneau, R. J. Am. Chem. Soc. 1980,102,1220-1221. 3. Perutz, R. N.; Scaiano, J. C. J. Chem. Soc., Chem. Commun. 1984, 457-458. 4. Creaven, B. S.; Dixon, A. J.; Kelly, J. M.; Long, C.; Poliakoff, M. Organo metallics 1987, 6, 2600-2605. 5. Kobayashi, T.; Ohtani, H.; Noda, H.; Teratani, S.; Yamazaki, H.; Yasufuku, K. Organometallics 1986, 5, 110-113. 6. Poliakoff, M.; Weitz, E. Adv. Organomet. Chem. 1986, 25, 277-316. 7. Church, S. P.; Herman, H.; Grevels, F.-W.; Schaffner, K. Inorg. Chem. 1985, 24, 418-422. 8. Dixon, A. J.; Healy, Μ. Α.; Hodges, P. M.; Moore, B. D.; Poliakoff, M.; Simpson, M. B.; Turner, J. J.; West, M. A. J. Chem. Soc., Faraday Trans. 2 1986, 82, 2083-2092. 9. Dobson, G. R.; Hodges, P. M.; Healy, Μ. Α.; Poliakoff, M.; Turner, J. J.; Firth, S.; Asali, K. J. J. Am. Chem. Soc. 1987, 109, 4218-4224. 10. Church, S. P.; Herman, H.; Grevels, F.-W.; Schaffner, K. J. Chem. Soc., Chem. Commun. 1984, 785-786. 11. Weiller, Β. H.; Wasserman, E. P.; Bergman, R. G.; Moore, C. B.; Pimentel, G. C. J. Am. Chem. Soc. 1989, 111, 8288-8289. 12. Simon, J. D.; Peters, K. S. Chem. Phys. Lett. 1983, 98, 53-56. 13. Simon, J. D.; Xie, X. J. Phys. Chem. 1986, 90, 6751-6753. 14. Rothberg, L. J.; Cooper, N. J.; Peters, K. S.; Vaida, V. J. Am. Chem. Soc. 1982, 104, 3536-3537. 15. Joly, A. G.; Nelson, K. A. J. Phys. Chem. 1989, 93, 2876-2878. 16. Wang, L.; Zhu, X.; Spears, K. G. J. Phys. Chem. 1989, 93, 2-4. 17. Yu, S.-C.; Xu, X.; Lingle, R.; Hopkins, J. B. J. Am. Chem. Soc. 1990, 112, 3668-3669.



118


18. Moore, J. N.; Hansen, P. Α.; Hochstrasser, R. M. Chem. Phys. Lett. 1987, 138, 110-114. 19. Moore, J. N.; Hansen, P. Α.; Hochstrasser, R. M. J. Am. Chem. Soc. 1989, 111, 4563-4566. 20. Perutz, R. N. Annu. Rep. Prog. Chem., Sect. C 1985, 157. 21. Wink, D. Α.; Ford, P. C. J. Am. Chem. Soc. 1987,109,436-442. 22. Halpern, J. Inorg. Chim. Acta 1981, 50, 11-19. 23. (a) Kunin, A. J.; Eisenberg, R. S. J. Am. Chem. Soc. 1986, 108, 535-536; (b) Kunin, A. J.; Eisenberg, R. S. Organometallics 1988, 7, 2124-2129. 24. Sakakura, T.; Sodeyama, T.; Tokunaga, Y.; Tanaka, M. Chem. Lett. 1987, 2211-2214. 25. Sakakura, T.; Tanaka, M. J. Chem. Soc., Chem. Commun. 1987, 758-759. 26. Sakakura, T.; Sodeyama, T.; Tokunaga, Y.; Tanaka, M. Chem. Lett. 1988, 263-264. 27. Sakakura, T.; Susaki, K.; Tokunaga, Y.; Wada, K.; Tanaka, M. Chem. Lett. 1988, 155-158. 28. Sakakura, T.; Tanaka, M. Nouv. J. Chim. 1989, 13, 737-745. 29. Normura, K.; Saito, Y. J. Chem. Soc., Chem. Commun. 1988, 161. 30. (a) Maguire, J. Α.; Boese, W. T.; Goldman, A. S. J. Am. Chem. Soc. 1989, 111, 7088; (b) Maguire, J. Α.; Boese, W. T.; Goldman, M. E.; Goldman, A. S. Coord. Chem. Rev. 1990, 97, 179-192. 31. Janowicz, A. H.; Bergman, R. G. J. Am. Chem. Soc. 1982, 104, 352. 32. Bergman, R. G. Science (Washington, D.C.) 1984, 223, 902, and references therein. 33. Hoyama, J. K.; Graham, W. A. G. J. Am. Chem. Soc. 1982, 104, 3723-3725. 34. Ghosh, C. K.; Graham, W. A. G. J. Am. Chem. Soc. 1987, 109, 4726-4727. 35. (a) Crabtree, R. H. Chem. Rev. 1985, 85, 245; (b) Crabtree, R. H. J. Am. Chem. Soc. 1987, 109, 5047. 36. Jones, W. D.; Feher, F. J. Acc. Chem. Res. 1989, 22, 91. 37. Belt, S. T.; Haddleton, D. M.; Perutz, R. N.; Smith, Β. P. H.; Dixon, A. J. J. Chem. Soc., Chem. Commun. 1987, 1347-1349. 38. Belt, S. T.; Grevels, F.-W.; Klotzbucher, W. E.; McCamley, Α.; Perutz, R. N. J. Am. Chem. Soc. 1989, 111, 8373-8382. 39. Belt, S. T.; Duckett, S. B.; Haddleton, D. M.; Perutz, R. N. Organometallics 1989, 8, 748-759. 40. Ford, P. C.; Friedman, A. In Photocatalysis: Fundamentals and Application Serpone, N., Ed.; Wiley: New York, 1989; Chapter 16, pp 541-564. 41. Spillett, C. T.; Ford, P. C. J. Am. Chem. Soc. 1989, 111, 1932-1933. 42. Spillett, C. T. Ph.D. Dissertation, University of California—Santa Barbara, 1989. 43. Ford, P. C.; Netzel, T. L.; Spillett, C. T.; Pourreau, D. B. Pure Appl. Chem. 1990, 62, 1091-1094. 44. Netzel, T. L., Amoco Technology Company, personal communication, 1989. 45. Desrosiers, M. F.; Wink, D. Α.; Trautman, R.; Friedman, Α. Ε.; Ford, P. C. J. Am. Chem. Soc 1986, 108, 1917-1927. 46. Ford, P. C. J. Organomet. Chem. 1990, 383, 339-356. 47. Johnson, B. F. G.; Lewis, J.; Twigg, M. V. J. Organomet. Chem. 1974, 67, C75-C76. 48. Johnson, B. F. G.; Lewis, J.; Twigg, M. V. J. Chem. Soc., Dalton Trans. 1975, 1876-1879. 49. Grevels, F.-W.; Reuvers, J. G. Α.; Takats, J. Angew. Chem., Int. Ed. Engl. 1981, 20, 452-460. 50. Grevels, F.-W.; Reuvers, J. G. Α.; Takats, J. J. Am. Chem. Soc. 1981, 103, 4069-4073.



7.

FORD & B E L T


119

51. Bamford, C. H.; Mahmud, M.V.J. Chem. Soc., Chem. Commun. 1972, 762-763. 52. Austin, R. G.; Paonessa, R. S.; Giordano, P. J.; Wrighton, M. S. In Inorganic and Organometallic Photochemistry; Wrighton, M. S., Ed.; Advances in Chem istry 168; American Chemical Society: Washington, DC, 1978; pp 189-214. 53. Graff, J. L.; Sanner, R. D.; Wrighton, M. S. Organometallics 1982, 1, 837-842. 54. Doi, Y.; Tamura, S.; Koshizuki, K. J. Mol. Catal. 1983, 19, 213-222. 55. DiBenedetto, J. Α.; Ryba, D. W.; Ford, P. C. Inorg. Chem. 1989, 28, 3503-3507. 56. Bentsen, J. G.; Wrighton, M. W. J. Am. Chem.Soc.1987, 109, 4530-4544. 57. Henríci-Olivé, G.; Olivé, S. Catalyzed Hydrogenation of Carbon Monoxide Springer-Verlag: Berlin, 1984. 58. Collman, J. P.; Hegedus, J. P.; Norton, J. R.; Finke, R. G. Principles and Applications of Organotransition Metal Chemistry; University Science Book Mill Valley, CA, 1987; Chapter 6, pp 355-400. 59. Wojcicki, A. Adv. Organomet. Chem. 1973, 11, 87. 60. Calderazzo, F. Angew. Chem., Int. Ed. Engl. 1977, 16, 299. 61. Flood, T. C. Top. Stereochem. 1980, 12, 37. 62. Flood, T. C.; Jensen, J. E.; Statler, J. A. J. Am. Chem. Soc. 1981, 103, 4410. 63. Butler, I.; Basolo, F.; Pearson, R. G. Inorg. Chem. 1967, 6, 2074. 64. Cawse, J. N.; Fiato, R. Α.; Pruett, R. J. Organomet. Chem. 1979, 172, 405. 65. Webb, S.; Giandomenico, C.; Halpern, J. J. Am. Chem. Soc. 1986, 108, 345. 66. Belt, S. T.; Ford, P. C.; Ryba, D. W. Abstracts of Papers, 199th National Meeting of the American Chemical Society, Boston, MA; American Chemical Society: Washington, DC, 1990; INOR 460. 67. Ziegler, T.; Versluis, L.; Tschinke, V. J. Am. Chem. Soc. 1986, 108, 612. 68. Axe, F. U.; Marynick, D. S. J. Am. Chem. Soc. 1988, 110, 3728-3734. 69. Belt, S. T.; Ryba, D. W.; Ford, P. C. Inorg. Chem. 1990, 29, 3633-3634. 70. Horton-Mastin, A.; Poliakoff, M.; Turner, J. J. Organometallics 1986, 5, 405-408. 71. Daniel, C. Coord. Chem. Rev. 1990, 97, 141-154. RECEIVED for review October 19, 1990. ACCEPTED revised manuscript May 8, 1991.


Flash Photolysis Studies of Reactive Organometallic Intermediates

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