摘要:

Mendeleev Communications Electronic Version, Issue 4, 1998 (pp. 129–168) Mechanism of the inhibiting action of electrolytes on the micellar effect in alkaline hydrolysis of p-nitrophenyl ethyl chloromethylphosphonate Lucia Ya. Zakharova,* Ludmila A. Kudryavtseva and Alexander I. Konovalov A. E. Arbuzov Institute of Organic and Physical Chemistry, Kazan Scientific Centre of the Russian Academy of Sciences, 420088 Kazan, Russian Federation.Fax: +7 8432 75 2253; e-mail: vos@glass.ksu.ras.ru The influence of KCl, KBr and sodium salicylate (NaSal) on the micellar effect of cetylpyridinium bromide in the alkaline hydrolysis of p-nitrophenyl ethyl chloromethylphosphonate has been studied and the effects of electrolytes on the rate constant and surface potential compared; based on the data obtained, it can be concluded that the reaction inhibition is determined both by a change in the structure and properties of the micellar aggregates and by a decrease in the concentration of the nucleophile in the micelles due to a decrease in the surface potential.Alkaline hydrolysis reactions of organophosphorus compounds are accelerated by micelles of cationic surfactants and retarded by micelles of anionic surfactants.1 The concentration (or separation in the case of inhibition) of reagents in the micellar pseudo-phase is the main reason for micellar catalysis.1 A substrate is completely or partially (depending on the structure) solubilized by micelles, and the concentration of the hydroxide ion in the micellar pseudo-phase is determined by the surface potential.Additives which change the potential, such as electrolytes,2 alcohols3 and other co-surfactants,4 exert an effect on micellar catalysis. In addition, the structure and properties of a micellar system change under the action of electrolytes, which is due to a decrease in the surface potential of the micelles. As the electrolyte concentration increases to a certain value Ccr, the micellar transition sphere–cylinder is observed.5 Although the pseudo-phase model of micellar catalysis does not take into account the geometry of the aggregates, it can be assumed that the micellar transition sphere–cylinder also exerts an effect on the reaction rates in micelles.In this work, we address the problems involved in investigating the factors which determine the nature of the effect of electrolytes on micellar catalysis.The potential of the micellar surface, which affects both the concentration of nucleophile and the structure of micelles, is considered to be the main factor. We therefore studied the effect of cetylpyridinium bromide (CPB) micelles on the rate of alkaline hydrolysis of p-nitrophenyl ethyl chloromethylphosphonate 1 (see Scheme 1) over a wide concentration range of salts KCl, KBr and NaSal.This concentration range covers the regions of both spherical and cylindrical micelles. Compound 1 was obtained according to the literature procedure.6 A sample of CPB was precipitated twice from ethanol using diethyl ether. The reaction kinetics were studied by spectrophotometry on a Specord UV-Vis instrument by monitoring the change in the optical density of solutions at 400 nm (formation of the p-nitrophenolate anion).The observed rate constants were calculated using the least-squares method. A ca. 20-fold acceleration of the reaction studied was observed in CPB micelles in the absence of electrolytes. Inorganic anions with different hydrophilicities (Br– and Cl–) and an organic anion Sal–, whose behaviour in micellar solutions differs strongly from that of other hydrophobic counterions,7 were used in the experiment.In the series of Cl–, Br– and Sal– counterions studied, only the salicylate anion exhibits nucleophilic activity with respect to the substrate, although this is, however, several orders of magnitude lower than for the hydroxide ion.Therefore, we subsequently neglect the contribution of the reaction of Sal– with compound 1 to the observed rate constant. The primary salt effect in the reaction of alkaline hydrolysis of 1 in the absence of surfactants was observed only for the salicylate ion: the observed rate constant decreases ca. 5-fold (from 0.02 to 0.004 s–1) as the concentration of NaSal increases from 0.05 to 0.5 M.In the presence of KCl and KBr, the rate of alkaline hydrolysis of 1 in the absence of micelles remains unchanged over a wide range of salt concentrations (0–2 M). The addition of electrolytes to the micellar solution decreases the catalytic effect of micelles to the extent of complete suppression of micellar catalysis in the region of high salt concentration (~1 M).The experimental data were analysed in semilogarithmic coordinates similarly to ref. 8 (see Figure 1). As can be seen from the plot, the kobs vs. log CS dependence for each counterion contains two linear regions with different O NO2 + OH– P O ClH2C EtO O– + –O P O ClH2C EtO NO2 Scheme 1 1 2 3 0.10 0.05 –4 –3 –2 –1 log CS kobs /s–1 Figure 1 The dependence of the observed rate constant for the hydrolysis of 1 in CPB micelles on the logarithm of the concentration of KCl (1), KBr (2) and NaSal (3) (25 °C, 0.001 M CPB, 0.005 M NaOH). akaq = 0.02 s–1.bThe values of km, corresponding to the plateau of kobs vs. Csurf plot. Table 1 The values of KS and km for the reaction of basic hydrolysis of 1 in micellar solutions of CPB in the presence of KBr (25 °C, 0.001 M CPB, 0.005 M NaOH).CKBr /M Kb/M–1 km/s–1 km/kaq a 0.002 350 0.36 18 0.003 380 0.26 13 0.005 410 0.22 11 0.01 550 0.13 6.5 0.02 890 0.054 2.7 0.05 1022 0.052 2.6 0.1 1262 0.047 2.4 0.2 1312 0.036 1.8 0.3 — 0.028b 1.4Mendeleev Communications Electronic Version, Issue 4, 1998 (pp. 129-168) slopes. According to ref. 8, the values of salt concentrations at the inflection points of Ccr were interpreted as the concentrations of counterions corresponding to the sphere–cylinder transition of the CPB micelles.For Cl–, Br– and Sal–, Ccr are equal to 0.1, 0.02 and 0.0015 M, respectively. The replacement of the cation (K+ by Na+) has no effect on the rate constant. Thus, the activity series for the counterions studied as a function of the extent of their action on the rate of alkaline hydrolysis of 1 is the following: Cl– < Br–< Sal–, and this coincides with the lyotropic series obtained previously.9 It is noteworthy that the Ccr values for chloride and bromide ions found in this work for CPB coincided with the analogous values for cetyltrimethylammonium bromide micelles obtained previously.8 Despite the fact that ion-molecular reactions of nucleophilic substitution in the presence of electrolytes has been studied previously, the mechanism of this phenomenon remains unclear.The question of the effect of the shape of the aggregates on the reactivity of compounds has not yet been answered. To compare the mechanism of the inhibition effect of electrolytes in spherical and cylindrical micelles, we studied a series of kobs–log Csurf dependences at different concentrations of KBr covering the regions of both spherical and cylindrical micelles (see Figure 2).The data obtained were analysed in terms of the pseudo-phase model of micellar catalysis by equation (1):10 where kaq and km/s–1 are the rate constants in aqueous and micellar phases, respectively; Kb/M–1 is the reduced binding constant of the substrate; and Csurf is the concentration of the surfactant minus CMC.The results of mathematical processing are presented in Table 1. As the concentration of the salts increases, the binding constant of the substrate increases due to the salting-out effect of inorganic ions with respect to the hydrophobic compound. It is also known that the site of localization and binding constant of the solubilizate can change depending on the shape of the micellar particles.11 The calculated values of km were analysed in the semilogarithmic coordinates (see Figure 3).The character of the dependence obtained is similar to that of the plot presented in Figure 1. The values of the Br– concentration in the inflection point are Ccr = 0.02M, which coincides with Ccr in Figure 1.It is noteworthy that the slopes of the linear dependence before the inflection point (equation of line before the point Ccr :km = –0.29log CS – 0.45) and after it (equation of line after the point Ccr :km = –0.039log CS – 0.008) differ strongly. This indicates that the inhibition of the micellar effect by the electrolytes in these regions occurs to different extents and, probably, via different mechanisms.The data on the change in the catalysis value km/kaq presented in Table 1 agree with this assumption. In the region of existence of spherical micelles, the efficiency of micellar catalysis in the presence of KBr decreases by ~7 times but only twice in the region of cylindrical micelles. To elucidate the mechanism of action of electrolytes on the micellar effect, we calculated the change in the potential of the micellar surface (y) as the salt concentration increases.It is shown4 that a Nernst correlation exists between the surface potential and CMC, equation (2). Using our data from measuring the surface tension of micellar solutions of CPB in the presence of salts, and the semi-empirical expression presented in ref. 12, we calculated CMC values at different concentrations of KBr and KCl and then y values from equation (2) (see Figure 3). Analysing the data presented in Figures 1 and 3, we may draw the following conclusions concerning the mechanism of inhibiting action of electrolytes in micellar catalysis. The value of the inhibition action is independent of the nature of the counterion. For all electrolytes studied, we observed a decrease in kobs to the value equal to the rate constant in water.The surface potential of micelles upon complete suppression of the micellar effect (kobs = kaq) is not zero. This is related to the fact that the inhibiting action of electrolytes is caused by the simultaneous decrease in the surface potential of the micelles and displacement of reactive counterions from the Stern layer by unreactive counterions. When hydroxide ions are completely displaced from the micellar surface by unreactive anions, the micellar effect is completely suppressed, although the potential in the Stern layer differs from zero.The km–log CS and kobs–log CS plots consist of two linear regions, whereas the y–log CS dependence is linear over the whole range of electrolyte concentrations (Figure 3) and can be expressed by the equation y = –41.6log CS + 53.2 (n = 11, r = 0.999).A similar linear dependence was obtained when the data from ref. 13 were plotted. It is of special interest that the Ccr values for Br– and Cl– correspond to the same values of the surface potential (124 and 123 mV, respectively) (see Figure 3).This indicates that there is a critical value of the surface potential at which the mechanism of electrolyte action changes sharply. This ycr value is most likely the characteristic one for CPB micelles and results in micellar transitions. The presence of a break in the kobs–log Cs dependence implies that in spherical and cylindrical micelles the factor of 1 2 3 4 5 6 7 8 9 10 0.10 0.05 0.001 0.002 0.003 kobs /s–1 Csurf/M Figure 2 The dependence of the observed rate constant for the hydrolysis of 1 on CPB concentration: (1) 0, (2) 0.002, (3) 0.003, (4) 0.005, (5) 0.01, (6) 0.02, (7) 0.05, (8) 0.1, (9) 0.2, (10) 0.3 M KBr. kobs = kaq + kmKbCsurf 1 + KbCsurf (1) km/s–1 log CS 0.4 0.3 0.2 0.1 –3 –2 –1 y/mV 100 50 –2.0 –1.5 –1.0 log CS Figure 3 The dependence of the rate constant in the micellar phase on the logarithm of the concentration of KBr (insertion: the dependence of the surface potential on the logarithm of the concentration of KBr: (1) calculated from equation (2), (2) data from ref. 13, (3) on the logarithm of KCl concentration). 1 2 3 d|y|/dlog CMC = 59.16 mV (2)Mendeleev Communications Electronic Version, Issue 4, 1998 (pp. 129–168) concentration with a decrease in the surface potential is suppressed to different extents or this indicates the existence of additional mechanisms of inhibition action, which are not associated with the concentration effect. Perhaps the effect of the micellar microenvironment, which does not depend directly on the surface potential, becomes determining in cylindrical micelles and changes insignificantly when salts are added.In fact, published data exist on the change in the degree of counterion binding,11 the site of localization of reagents and the solubilizing capability of micelles14 for the sphere–cylinder transition. In addition, a denser packing of surfactant molecules in cylindrical micelles as compared to spherical micelles can lead to a change in the microenvironment of the substrate, its orientation and mobility and, as a consequence, its reactivity. An alternative explanation for the existence of the break is the assumption that two main inhibiting factors act before the Ccr point: a decrease in the surface potential and displacement of reactive counterions, while after Ccr, only the first factor acts, which results in weakening of the inhibition effect.References 1 K. Martinek, A. K. Yatsimirsky, A. V. Levashov and I. V. Beresin, Micellization, Solubilization and Microemulsions, ed. K. L. Mittal, Plenum Press, New York–London, 1977, p. 489. 2 D. Grand, J. Phys. Chem., 1990, 94, 7585. 3 J. Kibblewhite, C. J. Drummond. F. Grieser and T. W. Healy, J. Phys. Chem., 1987, 91, 4658. 4 R.A. Hobson, F. Grieser and T. W. Healy, J. Phys. Chem., 1994, 98, 274. 5 S.Ikeda, Surfactants in Solution, ed. K. L. Mittal, Plenum Press, New York–London, 1984, p. 825. 6 V. E. Bel’skii, L. A. Kudryavtseva, O. M. Il’ina and B. E. Ivanov, Zh. Obshch. Khim., 1970, 49, 2470 [J. Gen. Chem. USSR (Engl. Transl.), 1970, 49, 2180]. 7 M. A. Cassidi and G. G. Warr, J. Phys. Chem., 1996, 100, 3237. 8 L. Ya. Zakharova, S. B. Fedorov, L. A. Kudryavtseva, V. E. Bel’skii and B. E. Ivanov, Izv. Akad. Nauk, Ser. Khim., 1993, 1396 (Russ. Chem. Bull., 1993, 42, 1329). 9 W. Jencks, Catalysis in Chemistry and Enzymology, McGraw-Hill, New York, 1969. 10 F. M. Menger and C. E. Portnoy, J. Am. Chem. Soc., 1967, 89, 4698. 11 B. Herzog, K. Huber and A. R. Renie, J. Colloid Interface Sci., 1994, 164, 370. 12 K. Shinoda, T. Nakagawa, B. Tamamushi and T. Isemura, Colloidal Surfactants, Academic Press, New York–London, 1963. 13 N. O. Mchedalov-Petrosyan, L. P. Loginova and V. N. Kleshchevnikova, Zh. Fiz. Khim., 1993, 67, 1649 (in Russian). 14 S. Ikeda, Colloid Polym. Sci., 1991, 269, 49. Received: Moscow, 17th December 1997 Cambridge, 27th February 1998; Com. 8/00197J

ISSN:0959-9436     

出版商:RSC    

年代:1998

数据来源: RSC

摘要:

Mendeleev Communications Electronic Version, Issue 4, 1998 (pp. 129–168) Oximes, amidoximes and hydroxamic acids as nitric oxide donors Leonid N. Koikov,*a Natalia V. Alexeeva,a Elena A. Lisitza,a Emmanuil S. Krichevsky,a Nikita B. Grigoryev,a Alexandr V. Danilov,a Irina S. Severina,b Natalia V. Pyatakovab and Vladimir G. Granika a Centre for Medicinal Chemistry, All-Russian Chemical-Pharmaceutical Institute, 119815 Moscow, Russian Federation.Fax: +7 095 246 6633 b Institute of Biomedical Chemistry, 119832 Moscow, Russian Federation. Fax: +7 095 245 0857 Quaternized pyridine aldoximes (2- and 4-PAM), some hydroxamic acids and amidoximes produce NO under mild oxidation and activate soluble guanylate cyclase. Recently we have reported that some oximes of 2-arylmethylene- and 2-arylmethylquinuclidin-3-one gave NO and the parent ketones under mild oxidation.The most active NO donors containing a 2-HO-phenyl group proximal to the oxime fragment activated soluble guanylate cyclase; 4-HO-isomers, 2-MeO- and 4-MeO-derivatives as well as the oxime of quinuclidin-3-one were much less active.1–2 The aim of this work is an investigation of the factors affecting the ability of the oxime group to serve as NO precursor, with special attention given to the influence of its conjugation with heteroatoms (O, N) and aromatic rings.For this purpose three series of compounds: oximes RCH=NOH 1 and 2, hydroxamic acids RC(=O)NOH 3 and amidoximes RC(NH2)=NOH 4 were chosen. Methyl derivatives 1a, 3a, 4a were used as the reference compounds and aromatic substituents in the above series were designed for an elucidation of the possible role of H-bonding (R: b, Ph; c, 2-HO; d, 2-MeO; e, 4-HO; f, 4-MeO-phenyl; h, 2-Py, i, 4-Py; j, 2,6-Py) through interaction at the enzyme site at physiological pH values.Quaternized pyridine aldoximes 2h,i served as strongly electron-deficient nuclei lacking H-bond acceptor properties.The required compounds were obtained according to the published procedures from hydroxylamine and the corresponding aldehydes for syn-aldoximes3 [1a: bp 113–114 °C (lit.,4 112– 114 °C); 1b: mp 29–31 °C (lit.,5 35 °C); 1c: mp 58–59 °C (lit.,6 56–57 °C); 1d: mp 90–92 °C (lit.,5 92 °C); 1e: mp 62–65 °C (lit.,7 68–70 °C); 1f: mp 52–54 °C (lit.,3 61–62 °C)], or the corresponding esters for hydroxamic acids [3d: mp 132–134 °C (acetone–diethyl ether, lit.,8 129–131 °C); 3e: mp 179 °C (H2O, lit.,9 168 °C); 3f: mp 159–160 °C (acetone–hexane, lit.,9 162 °C); 3h·0.5H2O: mp 136 °C (H2O, lit.,10 120 °C, anhydrous); 3i: mp 175 °C (H2O, lit.,10 161 °C); pyridine-2,6-dihydroxamic acid 3j·0.5H2O: mp 185 °C (H2O, lit.,10 217 °C, anhydrous)] or the corresponding nitriles for amidoximes [4h: mp 113–114 °C (H2O, lit.,11 115 °C); 4i: mp 205 °C (H2O, lit.,11 199 °C); pyridine-2,6-diamidoxime 4j: mp 235–237 °C (H2O, lit.,12 214 °C)].Commercial preparations of 1h (Merck), 1i (Lancaster), 2a (Aldrich) and 3b,c (Reakhim, Russia) were used. Quaternization of 1h,i with MeI was carried out in MeOH at room temperature. Amidoximes 4a,b,g and acetamidine hydrochloride were a gift from Dr S.M. Vinogradova. According to 1H NMR spectroscopy the purity of all samples was more than 98% and compounds 1e,f contained ca. 5% of anti-isomers. The results of oxidation of the above compounds with K3[Fe(CN)6] are given in Table 1. NO was trapped and determined as [Fe(CN)5NO]2– (nitroprusside) anion by pulsed differential polarography according to the previously described protocol.1–2 Under these conditions oximes 1 do not generate NO, which is in sharp contrast with our earlier finding that (E)-2-[(2'-hydroxyphenyl)methylene]- and 2-[(2'-hydroxyphenyl) methyl]quinuclidin-3-one gave NO in 17% and 10% yields, respectively.A possible explanation for this difference may lie in the fact that the rigid structure of the quinuclidine derivatives allows for intramolecular interaction of the 2'-OH group and the oxime fragment, which is impossible for syn-oxime 1c.Even so, the absence of any difference within the series 1, comprising both the strong acceptor pyridine and strong donor hydroxyphenyl rings, as well as the nonconjugated methyl group, is rather surprising. Probably, the competition between the donor–acceptor properties of R and the acidities of oxime and phenolic OH groups, responsible for the proportion of oxime anions, accounts for the phenomenon. The difference is more pronounced for hydroxamic acids 3, which are completely ionized at the pH employed13–15 (Table 2).Among them the most active NO donor proved to be acetohydroxamic acid 3a. The pyridine ring essentially inhibited the activity 3h–j, though 3j shows some residual activity.The absence of any visible trend in the aromatic sub-series 3b–f allows us to suggest the operation of several opposing factors. In any case, the involvement of a formal oxime group in conjugation with the oxygen lone pair (hydroxamic acids exists as 3 and not 11) in 3a–f leads to a marked increase in activity compared to the corresponding oximes 1a–f, 3a being half as active as NH2OH·HCl.The simple amidoximes 4a,b essentially mimic the behaviour of the corresponding hydroxamic acids 3a,b. At the same time, the activity of non-conjugated phenylacetic derivative 4g, is only half of that of benzamidoxime 4b instead of the expected value between 4a and 4b. In contrast to hydroxamic acids, the substitution of a benzene ring for pyridine leads to a sudden leap in amidoxime activity. The values for compounds 4h,i are close to the value for 4a.The activity of more conjugated 4i is 1.5 times higher than that of 4h and pyridine-2,6-diamidoxime 4j is twice as active as its 2-substituted prototype 4h. The pathways leading to NO generation from oximes, amidoximes and hydroxamic acids are to be investigated separately but the observed facts may be rationalized as N H R OH N Me I N H OH R NH O OH R N NH2 OH N 1 2 3 4 h R = 2-Py i R = 4-Py j R = Scheme 1 aNa2[Fe(CN)5NO] 100%, NH2OH·HCl 55.8%.b2,6-Disubstituted pyridyl. Table 1 Yield of NO (%) from oximes, amidoximes and hydroxamic acids: oxidation (c = 2×10–4 M, 4% EtOH–H2O) by K3[Fe(CN)6] at pH 12.a R Compound 1 2 3 4 Me a 0.0 — 22.9 25.0 Ph b 0.5 — 9.0 10.0 2-HOC6H4 c 0.0 — 14.0 — 2-MeOC6H4 d 0.0 — 5.1 — 4-HOC6H4 e 0.0 — 6.5 — 4-MeOC6H4 f 0.0 — 16.4 — 4-HOC6H4CH2 g — — — 5.5 2-Py h 0.0 6.4 0.0 20.6 4-Py i 7.4 62.2 0.8 29.5 2,6-Pyb j — — 3.1 40.0Mendeleev Communications Electronic Version, Issue 4, 1998 (pp. 129-168) follows. At pH 12 all the oximes (except 1a) and hydroxamic acids studied are ionized > 90% (Table 2) and the first step in the oxidation is undoubtedly the loss of an electron from their anion (Scheme 2).Within the series of oximes 1a–i, 2h–j only acceptor pyridine rings provide the favourable combination of an increase in content of 5 and in radical 6 (presented in two resonance structures 6a and 6b) the stabilisation responsible for the subsequent NO generation.The absence of a correlation between 1h,i, 2h,i acidity and the yield of NO shows the importance of the stabilisation. The latter is higher for 4-Py than for the 2-Py substituent, 1-methyl-4-pyridinealdoxime 2i being the most active of all the compounds tested. Nor can the adverse contribution of ortho-effects in 1h, 2h, especially steric shielding by N–Me in 2h, be excluded.A control experiment demonstrated that 4h,i are stable at pH 12, i.e. NO formation is not caused by hydroxylamine release due to hydrolysis or other processes. The behaviour of hydroxamic acids is essentially the same (Scheme 3). Both predominant oxo-form 3 and minor iminoform 11 give the better conjugated (compared to 9) imino-anion 10, converting into tautomeric radicals 12,13, of which the latter is involved in reactions similar to that of 6.TLC examination of the reaction mixtures originating from 3b,c,f reveals only the presence of the corresponding carboxylic acids. No detectable amounts of the products of ring hydroxylation or radical dimerisation have been found. Amidoximes are not so straightforward. Though their acidity is low and their basicity is close to pyridine (pKa: 4a 5.95, 4b 5.10, Py 5.1018), they form salts in water not only with acids but also with alkalis.19 So, in this case both the anion of 4 can be oxidized into 18 and the neutral amidoximes can give cation radical 17 followed by deprotonation to 18 (Scheme 4).The reactive 18 can behave similarly to the above mentioned key-radicals 6 and 13 (Schemes 2 and 3), forming NO via N,O-intermediate 19, but this nevertheless seems not to be the principal route, if at all.Despite the fact that 4b gives benzamide and some benzoic acid as the end-products (TLC), the first detectable reaction product is PhCN (GC-MS). According to the literature the latter is formed from 4b and strong oxidizers, while under conditions similar to ours a low yield of 5-amino-4,5-dihydro- 3,5-diphenyl-1,2,4-oxadiazole was obtained.20 On mixing of 0.11 mmol of 4b, 0.3 mmol of K3[Fe(CN)6] and 0.9 mmol of KOH in 0.5 ml of water at 80 °C the initially clear solution almost immediately becomes opaque (emulsion of hydrophobic PhCN) and a strong smell of bitter almond can be observed.After 2–3 min the solution becomes clear again and contains no 4b.A parallel experiment without K3[Fe(CN)6] showed that after 5 min only about half of 4b was hydrolyzed to benzamide. We have no exact kinetic data but the consumption of 4b in the presence of K3[Fe(CN)6] is much faster than the alkaline hydrolysis leading to benzamide and hydroxylamine, i.e. elimination of PhCN from some radical intermediate (probably 18 ® 20 ® 21) but not simple hydrolysis is the main source of NO from amidoximes. The radical 21 or its anion have been reported as NO precursors under these conditions.21 General considerations do not allow us to exclude oxidation of the amidoxime NH2 group instead of NOH as the first step, but the much more basic and more electron-rich MeC(=NH)NH2 does not give NO under the conditions used, which supports the suggested scheme.The two-fold drop in activity upon substitution of Me for Ph in 3a/3b and 4a/4b can be attributed to a decrease in reactivity of the radicals stabilized by the aromatic ring. Further manifestation of this effect aggravated by a reduction in the electron density on anion 10, might be responsible for the low activity of pyridyl hydroxamic acids 3h–j. Since the nature of R has very little influence on the acidity of the =NOH group in amidoximes,18 the acceptor properties of pyridyl substituents are not as important in steps 4 ® 17 ® 18, but they certainly play a role in the subsequent stages, which may account for the lack of a completely parallel route in the series 3 and 4.Preliminary tests22 show that about a two-fold activation of soluble guanylate cyclase from human platelets is achieved by 3a,c and 4h at a concentration 10–6 mol dm–3. 3e (4-OH isomer of 3c) is less active (×2.5 at 10–5 mol dm–3) and OMe-derivatives of OH-acids 3d,f are not active at all. 3b, 4a,b give a ca. 1.5-fold activation at 10–4–10–5 mol dm–3, while R CH N OH OH– R CH N O – e– R CH N O R CH N O OH or H2O R CH NO OH R CH NO O – e– RCHO + NO Scheme 2 1,2 5 6a 6b 7 8 OH– R C NHOH O OH– R C NHO O R C NOH OH 3 11 9 R C NOH O 10 OH– – e– R C NOH O 12 R C NO OH 13a R C NO OH 13b OH or H2O R C NO OH OH 14 R C NO OH O 15 R C NO OH O 16 RCOOH + NO Scheme 3 aFor Me2C=NOH.% of anion = 100/[1 + 10(pKa – pH)]. Table 2 Ionization of oximes and hydroxamic acids in water at pH 12 and room temperature. Compound 1 2 3 pKa % of anion pKa % of anion pKa % of anion a 12.4a 28.47 — — 9.4613 99.71 b 10.685 95.43 — — 8.7515 99.94 c 9.316 99.80 — — 7.4313 99.997 d 10.885 92.95 — — — — f 10.925 92.32 — — 9.014 99.90 h 10.1417 98.64 8.017 99.99 8.714 99.95 i 9.9917 99.03 8.5717 99.96 7.814 99.994 R C N NH2 – e– Scheme 4 OH R C N NH2 OH OH– R C N NH2 O R C N NH2 O 4 17 18a 18b OH or H2O R C NO NH2 OH 19 R C N NH OH 20 NHOH + R CN .. . 21 OH– NO RCONH2 + RCOOH . . . – e– – NOMendeleev Communications Electronic Version, Issue 4, 1998 (pp. 129–168) pyridine aldoximes 1h, 2i,h give a ‘bell-shaped’ curve with a maximum at ca. 10–5 mol dm–3 (Table 3). In general, enzyme activation data for the hydroxamic acids do not contradict their behaviour under chemical oxidation (Table 1), but the influence of an aromatic substitution pattern in 3b–f is strikingly similar to that observed for oximes of 2-arylmethylenequinuclidin- 3-ones1,2 (see above).Consequently, at a physiological pH compatible with the existence of intramolecular hydrogen bonds 22, the 2-OH-phenyl group provides either superior stabilisation of the intermediates (or the released NO) or higher complementarity to the active site, i.e.we can see the pronounced ortho-effect in 3c. The data for pyridine aldoximes also suggest the involvement of some ortho-interaction or site complementarity, since 2-pyridyl-substituted oximes 1h, 2h activate soluble guanylate cyclase better than 4-substituted 2i and, at the lower concentrations, better than hydroxylamine (Table 3).Since the preparation of soluble guanylate cyclase used is not free from non-specific oxidative enzymes also capable of producing NO, we cannot tell whether these ortho-effects are connected with the complementarity to soluble guanylate cyclase itself, to non-specific oxidative enzymes (P-450 etc.) or to an increase in the lifetime of NO released by non-specific enzymes, which allows NO to reach the soluble guanylate cyclase more efficiently and to cause its activation.Such stabilisation of NO by N-hydroxyguanidine (23, R = H), its derivatives and L-N-hydroxyarginine (L-NOHA) 24 is well documented.23,24 It should be noted that anions of oximes do not interact with NO.25 Thus, although oxidation of =N–OH-containing substrates (or their tautomers 3) at pH 12 cannot be considered as truly biomimetic, this very simple method allows us to carry out a fast preliminary screening of potential NO precursors. As a result, we were able to reveal the unknown NO generating potential of the well-known oximes, amidoximes and hydroxamic acids (there is only one brief mention of NO formation from N-hydroxybenzenesulfonamide: Piloty acid, the rate of which correlates with the rate of hydroxysulfonamide hydrolysis26) and some correlation between the chemical oxidation and soluble guanylate cyclase activation for these hydroxylamine derivatives.Though the better NO yields and values of soluble guanylate cyclase activation achieved in vitro are comparable to that of hydroxylamine itself, the use of the three classes of readily available new NO donors as templates for design of NO releasing ‘pro-drugs’ with desired in vivo properties looks rather promising.One more argument in favour of such a suggestion lies in the similarity of the observed chemistry and NO biosynthesis by nitric oxide synthase from L-arginine 23 via L-NOHA 24 followed by formation of NO and L-citrulline 2527,28 (oxidation of simpler N-hydroxyguanidines is quite complicated29).In conclusion, we cannot avoid mentioning that hydroxylamine, hydroxamic acids and especially quaternary pyridine aldoximes 2h (2-PAM) and 2i (4-PAM) were the first efficient antidotes against nerve gas poisoning.8,10,14,15,17 The commonly accepted ‘nucleophilic’ mechanism of acetylcholine esterase reactivation could not explain all the phenomena observed in vivo, which may account for the potential NO contribution.The last hypothesis is far beyond the scope of this work and must be investigated separately. This work was supported by the Russian Foundation for Basic Research (grant no. 96-04-48325). References 1 L. N. Koikov, N. V. Alexeeva, N. B. Grigoryev, V. I. Levina, K. F. Turchin, T. Ya. Filipenko, I.S. Severina, I. K. Ryaposova and V. G. Granik, Mendeleev Commun., 1996, 94. 2 L. N. Koikov, N. V. Alexeeva, N. B. Grigoryev, V. I. Levina, K. F. Turchin, T. Ya. Filipenko, M. D. Mashkovsky, M. E. Kaminka, V. B. Nikitin, G. N. Engalycheva, M. A. Kalinkina, I. S. Severina, I. K. Ryaposova and V. G. Granik, Khim.-Farm. Zh., 1997, 5, 28 (Chem. Abstr., 1997, 127, 272489). 3 E. Beckmann, Ber., 1890, 23, 1680. 4 H. Wieland, Ber., 1907, 40, 1677. 5 O. L. Brady and R. G. Goldstein, J. Chem. Soc., 1926, 1918. 6 Merck Index, 1996, 12, 8479. 7 M. Sekiya, N. Yanaihara and T. Masui, Chem. Pharm. Bull., 1961, 9, 945. 8 M. A. Stolberg, W. A. Mosher and T. Wagner-Jauregg, J. Am. Chem. Soc., 1957, 79, 2615. 9 J. Hase, K. Kobayashi, N. Kawaguchi and K. Sakamoto, Chem. Pharm. Bull., 1971, 19, 363. 10 B. E. Hackley Jr., R. Plapinger, M. Stolberg and T. Wagner-Jauregg, J. Am. Chem. Soc., 1955, 77, 3651. 11 R. Delaby, P. Reynaud and T. Tupin, Bull. Soc. Chim. France, 1957, 714. 12 G. A. Pearse Jr. and J. Wisowaty Jr., J. Heterocycl. Chem., 1973, 10, 647. 13 Y. K. Agrawal, V. P. Khare and A. S. Kapoor, J. Electroanalyt. Chem., 1974, 54, 433. 14 T. Wagner-Jauregg, Arzneimittel-Forshung, 1956, 6, 194. 15 A.L. Green, G. L. Sainsbury, B. Saville and M. Stansfield, J. Chem. Soc., 1958, 1583. 16 I. Hayashi, K. Ogihara and K. Shimitzu, Bull. Chem. Soc. Jpn., 1983, 56, 2432. 17 S. F. Mason, J. Chem. Soc., 1960, 22. 18 J. Barrans, Ann. Fac. Sci. Univ. Toulouse Sci. Math. Sci. Phys., 1964, 25, 7 (Chem. Abstr., 1964, 60, 12004). 19 F. Tiemann and P. Krieger, Ber., 1884, 17, 1685. 20 J. Stieglitz, Ber., 1889, 17, 3148. 21 V. I. Levina, A. V. Danilov and N. B. Grigoryev, Khim.-Farm. Zh., 1998, 53 (in Russian). 22 I. S. Severina, I. K. Ryaposova, L. B. Volodarsky, D. C. Mozhuchin, A. Ya. Tichonov, G. Ya. Schwartz, V. G. Granik, D. A. Grigoryev and N. B. Grigoryev, Biochem. Molec. Biology Intern., 1995, 36, 913. 23 A. Zembovicz, T. A. Swierkosz, G.J. Southan, M. Hecker and J. R. Vane, Brit. J. Pharmacol., 1992, 107, 1001. 24 J. G. Southan, S. S. Gross, H. Hecker, A. I. Marlett, H. G. Parkers, E. E. Anggrad and J. R. Vane, Portland Press Proc. (Biology of Nitric Oxide 4), 1994, 8, 255. 25 G. A. Russel, R. K. Norris and A. R. Metcalfe, J. Am. Chem. Soc., 1972, 94, 4959. 26 A. Gzzesiok, H. Weber, R. Z. Pino and M. Feelish, Portland Press Proc. (Biology of Nitric Oxide 4), 1994, 8, 238. 27 J. F. Kerwin, J. R. Lancester and P. L. Feldman, J. Med. Chem., 1995, 38, 4343. Table 3 Activation of soluble guanylate cyclase (2 series) relative to control = 1. Compound Concentrations tested/mol dm–3 10–6 10–5 10–4 10–3 Series 1 1h 1.3 2.0 1.6 — 2h 1.4 2.1 1.1 — 2i 1.1 1.6 1.5 — NH2OH·HCl 1.1 1.3 2.1 — Series 2 4a — 1.4 1.3 1.3 3b — 1.4 1.7 1.5 4b — 1.4 1.3 1.2 NH2OH·HCl — 2.5 2.2 3.6 NH O O H OH NH RHN NH2 N RHN NH2 OH O RHN NH2 + NO 22 O O 23 24 25 COOH NH2 R = LScheme 5Mendeleev Communications Electronic Version, Issue 4, 1998 (pp. 129-168) 28 V. G. Granik, S. Yu. Ryabova and N. B. Grigoriev, Usp. Khim. 1997, 792 (Russ. Chem. Rev., 1997, 66, 717). 29 J. M. Fukuto, G. C. Wallage, R. Hszieh and G. Chaudhuri, Biochem. Pharmacol., 1992, 43, 607. Received: Moscow, 28th October 1997 Cambridge, 15th December 1997; Com. 7/07978H

ISSN:0959-9436     

出版商:RSC    

年代:1998

数据来源: RSC