Research Letters in Inorganic Chemistry
Volume 2008 (2008), Article ID 216058, 5 pages
doi:10.1155/2008/216058
Research Letter

Mechanistic Aspects of Osmium(VIII) Catalyzed Oxidation of L-Tryptophan by Diperiodatocuprate(III) in Aqueous Alkaline Medium: A Kinetic Model

Nagaraj P. Shetti, Ragunatharaddi R. Hosamani, and Sharanappa T. Nandibewoor

P.G. Department of Studies in Chemistry, Karnatak University, Dharwad 580 003, India

Received 24 November 2008; Accepted 11 December 2008

Academic Editor: Wolgang Linert

Copyright © 2008 Nagaraj P. Shetti et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

In presence of osmium(VIII), the reaction between L-tryptophan and diperiodatocuprate(III) DPC in alkaline medium exhibits 1:4 stochiometry (L-tryptophan:DPC). The reaction shows first-order dependence on [DPC] and [osmium(VIII)], less than unit order in both [L-tryptophan] and [alkali], and negative fractional order in [periodate]. The active species of catalyst and oxidant have been identified. The main products were identified by spectral studies and spot test. The probable mechanism was proposed and discussed.

1. Introduction

In the recent past [1], some relatively stable copper(III) complexes have been prepared, namely, the periodate, guanidine, and tellurate complexes. The Cu3+/Cu2+ reduction potential is  –1.18 V in alkaline solution [2]. The copper(III) periodate complex (DPC) exhibits different multiple equilibria involving different copper(III) species in aqueous alkaline medium. It is interesting to know which of the copper(III) species is the active oxidant.

L-tryptophan (L-trp) is an essential aminoacid and it is needed to maintain optimum health. Osmium(VIII) acts as an efficient catalyst in many redox reactions [3, 4] involving different complexities due to the formation of different intermediate complexes, free radicals, and multiple oxidation states of osmium.

The uncatalyzed reaction of oxidation of L-tryptophan by DPC has been studied [5]. We have observed that the microamounts of osmium(VIII) catalyze the oxidation of L-trp by DPC in alkaline medium. In order to understand the active species of oxidant and catalyst and to propose the appropriate mechanism, the title reaction is investigated in detail, in view of various mechanistic possibilities.

2. Experimental

All chemicals used were of reagent grade and millipore water was used throughout the work. A solution of L-trp (s.d. fine) was prepared by dissolving an appropriate amount of recrystallized sample in millipore water. A stock solution of osmium(VIII) was prepared and standardized by the method reported earlier [6]. The copper(III) periodate complex was prepared [7] and standardized by standard procedure [8].

2.1. Kinetic Measurements

All kinetics measurements were carried out as in earlier work [6].

3. Results and Discussion

The results indicated 1:4 stoichiometry as given in Scheme 1.

216058.sch.001
Scheme 1: 1:4 stochiometry of osmium(VIII) catalyzed oxidation of L-trp by DPC reaction.

The main product, indole-3-acetic acid, was separated by TLC, using the mixture of methyl acetate, isopropanol, and 25% ammonium hydroxide in the ratio of 45:35:20. IR, NMR spectra and its melting points were compared with the literature and were in good agreement. The LC-MS analysis of isolated product indicated the presence of indole-3-acetic acid as molecular ion peak, m/z 175.

In the presence of catalyst, the reaction is understood to occur via parallel paths with contributions from the uncatalyzed and catalyzed paths. The total rate constant ( 𝑘 𝑇 ) is equal to the sum of the rate constants of the catalyzed ( 𝑘 𝐶 ) and uncatalyzed ( 𝑘 𝑈 ) reactions. Hence, 𝑘 𝐶 = 𝑘 𝑇 − 𝑘 𝑈 . The reaction orders have been determined from the slopes of log 𝑘 𝑐 versus log (concentration) plots by varying the concentration of L-trp, Os(VIII), OH−, and I O 4 − , in turn, while keeping the other concentrations constant. The order in both [DPC]  and [Os(VIII)]    was found to be unity. The order in [L-trp]  and [OH−]  was found to be less than unity, and in [periodate]  to be negative and less than unity. It is well known that [9] Os(VIII) exists as (OsO4(OH)2]2+ in aqueous alkaline medium. It was found that the increase in ionic strength increased the rate of reaction and decrease in dielectric constant of the medium increased the rate of reaction. Initially added products did not have any significant effect on the rate of reaction. Test for free radicals indicated the participation of free radical in the reaction [6]. These experimentally determined orders and results could be well accommodated in Scheme 2.

216058.sch.002
Scheme 2: The osmium(VIII) catalyzed oxidation of L-trp by DPC.

Based on the experimental results, monoperiodatocuprate MPC was considered to be the active species of DPC complex. The fractional order with respect to L-trp concentration indicates the formation of a complex between L-trp and osmium(VIII) species. Spectroscopic evidence for the complex formation between catalyst and substrate was obtained from UV-vis spectra of Os(VIII), L-trp, and a mixture of both. A bathochromic shift of about 6 nm from 255 nm to 261 nm in the spectra of Os(VIII) was observed. The Michaelis-Menten plot also proved the complex formation between catalyst and reductant. Such a complex between a substrate and a catalyst has been observed in other studies [6].

Scheme 2 leads to the following rate law: R a t e [ D P C ] = 𝑘 𝐶 = 𝑘 𝑇 − 𝑘 𝑈 = 𝑘 𝐾 1 𝐾 2 𝐾 3 [ L - t r p ] [ O H − ] [ O s ( V I I I ) ] ℛ , ( 1 ) where ℛ denotes [ H 3 I O 6 3 − ] + 𝐾 1 [ O H − ] [ H 3 I O 6 3 − ] + 𝐾 1 𝐾 2 [ O H − ] + 𝐾 1 𝐾 2 𝐾 3 [ O H − ] [ L - t r p ] which explains all the observed kinetic orders of different species. The rate law (1) can be rearranged into the following form which is suitable for verification: [ O s ( V I I I ) ] 𝑘 𝑐 = [ H 3 I O 6 3 − ] 𝑘 𝐾 1 𝐾 2 𝐾 3 [ L - t r p ] [ O H − ] + [ H 3 I O 6 3 − ] 𝑘 𝐾 2 𝐾 3 + 1 [ L - t r p ] 𝑘 𝐾 3 + 1 [ L - t r p ] 𝑘 . ( 2 ) According to (2), others being constant, the plots of [Os(VIII)]/ 𝑘 𝐶 versus 1/[L-trp], [Os(VIII)]/ 𝑘 𝐶 versus 1/[OH−], and [Os(VIII)]/ 𝑘 𝐶 versus [H3 I O 6 2 − ] were linear as in Figure 1. From the intercepts and slopes of such plots, the reaction constants K1, K2, K3, and k were calculated as ( 1 5 . 6 ± 0 . 4 ) dm3 mol−1, ( 3 . 3 ± 0 . 1 0 )  ×  10−4 mol dm−3, ( 0 . 7 1 ± 0 . 0 2 )  ×  104 dm3 mol−1, ( 3 . 2 ± 0 . 0 4 )  ×  103 dm3 mol−1s−1, respectively. The values of K1 and K2 obtained were in good agreement with previously reported values [10]. These constants were used to calculate the rate constants over different experimental conditions; when compared with the experimental 𝑘 𝐶 values, they were found to be in reasonable agreement with each other, which fortifies Scheme 2.

fig1
Figure 1: Verification of rate law (1) of Os(VIII) catalyzed oxidation of L-tryptophan by DPC at 298 K (conditions as in Table 1). (a) [Os(VIII)]/ 𝑘 𝑐 versus 1/[L-trp]; (b) [Os(VIII)]/ 𝑘 𝑐 versus 1/[OH−]; (c) [Os(VIII)]/ 𝑘 𝑐 versus [H2 I O 6 3 − ].

Similarly K1, K2, K3, and k were calculated at four different temperatures (288, 293, 298, and 303 K) and used to compute the activation parameters and thermodynamic quantities. The values of Ea, Δ 𝐻 # , Δ 𝑆 # , and Δ 𝐺 # and l o g 𝐴 were obtained and found to be 42.0  ±  2 kJ mol−1, 44.0  ±  2 kJ mol−1 - 3 0 . 0 ± 1 . 5  J K−1 mol−1, 53.0  ±  3 kJ mol−1, and 1 1 . 0 ± 0 . 5 , respectively. (Ea, Δ 𝑆 # , Δ 𝐻 # , and l o g 𝐴 were 51.7  ±  3 kJ mol−1, −114  ±  6 J K−1 mol−1, 48.2  ±  2 kJ mol−1, and 10.5, resp., for the uncatalyzed reaction [5].) The catalyst Os(VIII) alters the reaction path by lowering the energy of activation (i.e., it provides an alternative pathway with lower activation parameters for the reaction).

The thermodynamic quantities, Δ 𝐻 (kJ mol−1), Δ 𝑆 (J K−1 mol−1), and Δ 𝐺 (kJ mol−1) using K1 were calculated to be –47, 182, and −6.4, respectively. Similarly the values using K2 were calculated to be 97.7, 262.8, and 18.6, respectively and the values using K3 to be –144.0, −412.0, and −22.0, respectively.

The effect of ionic strength and dielectric constant of the medium on the rate explains qualitatively the reaction between two negatively charged ions, as seen in Scheme 1. The moderate Δ 𝐻 # and Δ 𝑆 # values are favorable for electron transfer reaction. The negative value of Δ 𝑆 # suggests that the intermediate complex is more ordered than the reactants [11]. The observed modest enthalpy of activation and a higher-rate constant for the slow step indicate that the oxidation presumably occurs via an innersphere mechanism. This conclusion is supported by earlier observations [12].

4. Conclusion

Among various species of Cu(III) in alkaline medium, monoperiodatocuprate(III) is considered to be the active species for the title reaction. The active species of osmium(VIII) is understood to be as [OsO4(OH)2]2−. The activation parameters evaluated for the catalyzed and uncatalyzed reactions explain the catalytic effect on the reaction. The Os(VIII) catalyst alters the reaction path by lowering the energy of activation.

tab1
Table 1: Effects of [DPC], [L-trp], [OH−], [ I O 4 − ],  and [Os(VIII)]  on the osmium(VIII) catalyzed oxidation of L-trp by DPC in alkaline medium at 298 K, I  =  0.20 mol dm−3.

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