2,6-Bis(1,4,7,10-tetraazacyclododecan-1-ylmethyl)pyridine and Its Benzene Analog as Nonmetallic Cleaving Agents of RNA Phosphodiester Linkages

Abstract

2,6-Bis(1,4,7,10-tetraazacyclododecan-1-ylmethyl)pyridine (11a) and 1,3-bis(1,4,7,10-tetraazacyclododecan-1-ylmethyl)benzene (11b) have been shown to accelerate at 50 mmol·L⁻¹ concentration both the cleavage and mutual isomerization of uridylyl-3′,5′-uridine and uridylyl-2′,5′-uridine by up to two orders of magnitude. The catalytically active ionic forms are the tri- (in the case of 11b) tetra- and pentacations. The pyridine nitrogen is not critical for efficient catalysis, since the activity of 11b is even slightly higher than that of 11a. On the other hand, protonation of the pyridine nitrogen still makes 11a approximately four times more efficient as a catalyst, but only for the cleavage reaction. Interestingly, the respective reactions of adenylyl-3′,5′-adenosine were not accelerated, suggesting that the catalysis is base moiety selective.

1. Introduction

Artificial ribonucleases, i.e., small molecular compounds that catalyze the cleavage of RNA phosphodiester linkages under neutral conditions, have been the subject of continuous interest since the early 1990s [1,2,3,4]. The most active catalysts reported so far are complexes of transition metals and lanthanides, exhibiting half-lives of the order of 10 h for the cleavage of dinucleoside-3′,5′-monophosphates at 1.0 mmol·L⁻¹ concentration of the complex at neutral pH and 25 °C [5,6]. Conjugation to an oligonucleotide or peptide nucleic acid (PNA) confers such agents sequence selectivity, turning them into real enzyme mimics [7]. Hybridization between the guiding oligonucleotide and the target sequence increases the local concentration and, hence, activity of the catalytic moiety. This interaction, when sufficiently strong, may render catalysis by the artificial ribonuclease essentially concentration-independent. For example, a PNA-conjugate of Cu²⁺: 2,9-dimethylphenanthroline cleaves a bulge in the target RNA opposite to the Cu²⁺ complex with a half-life as low as 30 min at 4 μmol·L⁻¹ concentration of both the artificial RNase and the substrate, at pH 7.4 and 37 °C [8]. While metal ion based artificial RNases are undoubtedly useful for in vitro tailoring of large RNA molecules, a sufficient supply of metal ions under the metal-deficient intracellular conditions may become a rate-limiting factor. Purely organic cleaving agents (Figure 1) do not suffer from the same limitation, but the desired cleaving activity may be more difficult to achieve.

Several of the most active non-metallic cleaving agents known are derivatives of guanidine. Tris[2-(benzimidazol-2-yl)ethyl]amine (1) at 1 mmol·L⁻¹ concentration cleaves RNA at pH 6.0, the half-life for the fission of a single RNA phosphodiester linkage being 60 h at 37 °C [9]. The cleaving agent tends to aggregate under these conditions, and the efficiency of 1 in its non-aggregated form is somewhat lower [10]. Diguanidinocalix[4]arenes (2 and 3) cleave dinucleoside-3′,5′-monophosphates at a comparable rate in 80% aq. DMSO at pH 10.4 [11]. The half-lives range from 3 to 300 h at 50 °C, depending on the identity of the base moieties. Melamine constructs anchored via Zn²⁺:cyclen moieties to uracil bases (4) accelerate the cleavage of UpU by two orders of magnitude at neutral pH (t_½ = 12 h at 90 °C) [12,13]. The other markedly efficient non-metallic agents include quaternized 1,4-diazabicyclo[2,2,2]octane conjugates of histidine (5). They exhibit at 0.5 mmol·L⁻¹ concentration half-lives of approximately 40 h for the cleavage of a single phosphodiester bond within a 10-mer oligoribonucleotide at pH 7.0 and 37 °C [14]. Among polyamines, the tetracation of 1,4,16,19-tetraoxa-7,10,13,22,25,28-hexaazacyclotriacontane (6) is catalytically exceptionally active (at [6] = 5 mmol·L⁻¹, t_½ = 200 h at 50 °C) [15]. In addition, several non-metallic agents cleave selectively some particular phosphodiester bond within large RNA molecules, although the catalytic activity towards short oligonucleotides is low. The trans-activation response (TAR) element of HIV RNA, for example, is cleaved by guanidinium based structures 7 [16], 8 [17] and 9 [18] and neomycin B (10) [19]. Multifunctional constructs that contain amino, amido and imidazolyl groups [20,21,22,23,24] or incorporate a 1,4-diazabicyclo[2.2.2]octane dimer attached to a hydrophobic tail [25,26] have, in turn, been shown to cleave tRNA molecules at specific sites, usually at 5′-CpA-3′ sites within single-stranded regions. We now report on 2,6-bis(1,4,7,10-tetraazacyclododecan-1-ylmethyl)pyridine (11a) and 1,3-bis(1,4,7,10-tetraazacyclododecan-1-ylmethyl)benzene (11b) as non-metallic cleaving agents. Both 11a and 11b feature two cyclen rings connected by a relatively rigid m-xylylene-type linker for a high density of amino groups. Somewhat unexpectedly, 11a,b seem to exhibit a selectivity for uracil bases, normally associated with Zn²⁺ chelates of cyclen. The cleaving activity of uncomplexed 11a,b, however, is considerably lower than what is typically observed with related Zn²⁺ complexes.

Figure 1. Representative examples of nonmetallic cleaving agents described in the literature.

Figure 1. Representative examples of nonmetallic cleaving agents described in the literature.

2. Results

2.1. Synthesis of Cleaving Agents 11a and 11b

2,6-Bis(1,4,7,10-tetraazacyclododecan-1-ylmethyl)pyridine (11a) and 1,3-bis(1,4,7,10-tetraazacyclododecan-1-ylmethyl)benzene (11b) were obtained by the reaction of 1,4,7-tris(tert-butoxycarbonyl)-1,4,7,10-tetraazacyclododecane with 2,6-bis(bromomethyl)pyridine and 1,3-bis(bromomethyl)benzene, respectively, in MeCN in the presence of K₂CO₃, followed by removal of the tert-butoxycarbonyl protections with TFA in a mixture of MeOH and CH₂Cl₂ [27].

2.2. Determination of the pK_a Values of the Cleaving Agents

The pK_a values of 11a and 11b have been previously determined by potentiometric titration at 25 °C (I = 0.1 mol·L⁻¹) [28]. Both of the compounds undergo five consecutive protonations on increasing the acid concentration to 0.1 mol·L⁻¹. The pK_a values obtained with 11a are 11.08, 10.14, 8.97, 7.84 and 2.30. Interestingly, replacement of the pyridine nitrogen atom with methine group has only a minor effect on the protolytic equilibria, the pK_a values of 11b being 11.25, 10.02, 8.90, 7.97 and 2.07. To obtain the values at 90 °C, i.e., under the conditions of kinetic experiments, ¹H NMR spectrometric titrations in D₂O were carried out. The compound (11a or 11b) was dissolved in phosphoric acid (0.10 mol·L⁻¹) and 1.0 mol·L⁻¹ sodium deuteroxide in D₂O was gradually added. A downfield shift of the ³¹P signal of the buffer and an upfield shift of the methylene signals of 11a and 11b were observed (Figure 2). The pK_a values were then calculated on the basis of the pK_a values of phosphoric acid at 90 °C [29]. The values obtained with 11a were 11.34 ± 0.22, 11.18 ± 0.11, 8.26 ± 0.07, 6.67 ± 0.14 and 2.60 ± 0.14. As the third pK_a value of phosphoric acid was extrapolated based on values obtained at much lower temperatures, the two most alkaline pK_a values of 11a are subject to some uncertainty. This uncertainty did not affect our results, however, since only the pK_a values of the tri- (SH₃³⁺), tetra- (SH₄⁴⁺) and pentaprotonated (SH₅⁵⁺) species, 8.26, 6.67 and 2.60, respectively were needed to analyze the kinetic data. For the same reason, titration of 11b was not extended beyond pH 11.0. The pK_a values of the tri- (SH₃³⁺) and tetraprotonated (SH₄⁴⁺) species of 11b were 8.4 ± 0.2 and 7.5 ± 0.6, respectively, pK_a of the pentaprotonated species being too low to be determined by this method. It is worth noting that the pK_a values were obtained in a 0.1 mol·L⁻¹ phosphate buffer, while the kinetic measurements were carried out in 1.0 mol·L⁻¹ NaClO₄. Owing to this difference in background electrolyte, the pK_a values under the conditions of kinetic measurements may slightly deviate from those determined by NMR titration. Most likely, none of the cyclen nitrogens is exceptionally basic, but the proton distribution is statistic.

Figure 2. Chemical shift of the methylene protons of 11a (■) and 11b (□) as a function of pH; T = 90 °C; [phosphoric acid] = 0.10 mol·L⁻¹. The lines have been added to illustrate the trends of chemical shift versus pH.

Figure 2. Chemical shift of the methylene protons of 11a (■) and 11b (□) as a function of pH; T = 90 °C; [phosphoric acid] = 0.10 mol·L⁻¹. The lines have been added to illustrate the trends of chemical shift versus pH.

2.3. Kinetic Measurements

The cleavage of uridylyl-3′,5′-uridine (3′,5′-UpU) to uridine 2′,3′-cyclic phosphate and uridine, and its concurrent isomerization to 2′,5′-UpU was studied in excess of cleaving agent (11a or 11b) under acidic conditions where 11a and 11b exist in tri-, tetra- or pentacationic forms. The measurements were carried out at different concentrations of 11a or 11b in the range from 10 to 70 mmol·L⁻¹. At each concentration, the proportions of ionic forms were altered by titration with 3.5, 3.8, 4.5 or 5.0 equivalents (eq.) of perchloric acid. Under the most acidic conditions studied, concentration of free hydronium ion became significant and was taken into account when calculating the pH of the reaction solutions. For the same reason, the buffer ratios were not entirely constant over all the buffer concentrations employed. These deviations, however, were deemed small enough to not significantly affect the results of the kinetic measurements. Sodium perchlorate (1.0 mol·L⁻¹) was used as a background electrolyte. The starting concentration of UpU was 0.50 mmol·L⁻¹.

The pseudo first-order rate constants obtained for the cleavage and isomerization reactions as functions of [11a] and [11b] are presented in Figure 3. As seen, both reactions exhibit a first-order dependence on the catalyst concentration with both 11a and 11b and regardless of the distribution among the various ionic forms (Equation (1)).

$$k_{\text{obs}}=k_{\text{cat}}{\left[\text{catalyst}\right]}_{\text{total}}+k_{\text{uncat}}$$

(1)

where k_cat and k_uncat refer to the second-order rate constant for the catalyzed reaction and the first-order rate constant for the uncatalyzed (background) reaction, respectively. In most cases, the catalyzed reaction was overwhelmingly faster than the uncatalyzed one, precluding reliable determination of the latter term.

Figure 3. Observed pseudo first-order rate constants for (A) cleavage and (B) isomerization of UpU as a function of [11a] and (C) cleavage and (D) isomerization of UpU as a function of [11b]; T = 90 °C, I(NaClO₄) = 1.0 mol·L⁻¹. The catalyst (11a or 11b) was titrated alternatively with 3.5 (○), 3.8 (●), 4.5 (□) or 5.0 (■) eq. of perchloric acid.

Figure 3. Observed pseudo first-order rate constants for (A) cleavage and (B) isomerization of UpU as a function of [11a] and (C) cleavage and (D) isomerization of UpU as a function of [11b]; T = 90 °C, I(NaClO₄) = 1.0 mol·L⁻¹. The catalyst (11a or 11b) was titrated alternatively with 3.5 (○), 3.8 (●), 4.5 (□) or 5.0 (■) eq. of perchloric acid.

The catalytic activity of 11a is increased with the increasing extent of protonation. Curiously, with 11b this dependence is much weaker. In solutions where the catalyst has been titrated with 3.5 eq. of perchloric acid, [SH₄⁴⁺] = [SH₃³⁺] and, hence, the pH is 6.7 and 7.5 for 11a and 11b respectively. Under these conditions, the first-order rate constants for the cleavage of UpU in the absence of any cleaving agents are approximately 3 × 10⁻⁷ and 2 × 10⁻⁶ s⁻¹, respectively [30]. Uncatalyzed isomerization is pH-independent with a first-order rate constant of 10⁻⁶ s⁻¹, the conversion to both directions taking place as readily. Accordingly, accelerations of more than two orders of magnitude are achieved with both 11a and 11b at 50 mmol·L⁻¹ concentration. Catalysis by 11a was also studied with adenylyl-3′,5′-adenosine (3′,5′-ApA) as the substrate. Virtually no rate acceleration could be observed, suggesting that the reasonably high cleaving activity of 11a depends on the presence of uracil base. It is also worth noting that monomeric 1,4,7,10-tetraazacyclododecane (cyclen) did not catalyze the cleavage or isomerization of 3′,5′-UpU.

Figure 4 shows the pH-rate profiles for the 11a- and 11b-catalyzed cleavage and isomerization of UpU. For reference, speciation curves for the various ionic forms of the catalysts have been included as well. Again, the pH-dependence of the catalytic activity of 11a and the relative pH-independence of the catalytic activity of 11b is evident. In the pH range of the kinetic experiments, protolytic equilibria of the catalysts are adequately described in terms [SH₃]³⁺, [SH₄]⁴⁺ and (in the case of 11a) [SH₅]⁵⁺. The observed second-order rate constants for 11a and 11b may, hence, be expressed by Equations (2) and (3), respectively.

$$k_{\text{cat}}\left(\mathbf{11}\mathit{a}\right)=\frac{k_5{\left[{\text{H}}^{+}\right]}^2+k_4{K}_{\text{a}5}\left[{\text{H}}^{+}\right]+k_3{K}_{\text{a}4}{K}_{\text{a}5}}{{\left[{\text{H}}^{+}\right]}^2+K_{\text{a}5}\left[{\text{H}}^{+}\right]+K_{\text{a}4}{K}_{\text{a}5}}$$

(2)

$$k_{\text{cat}}\left(\mathbf{11}b\right)=\frac{k_4\left[{\text{H}}^{+}\right]+k_3{K}_{\text{a}4}}{\left[{\text{H}}^{+}\right]+K_{\text{a}4}}$$

(3)

where k₃, k₄ and k₅ are the second-order rate constants for the reactions catalyzed by the tri-, tetra- and pentaprotonated species, respectively. K_a4 and K_a5 are the acid dissociation constants for the tetra- and pentaprotonated species, respectively. The acid dissociation constants were obtained by NMR spectrometric titrations as described above and the rate constants by non-linear least-squares fitting of the observed second-order rate constants (k_cat) to Equations (2) and (3). The values are summarized in Table 1.

Figure 4. pH-rate profiles for the (A) 11a- and (B) 11b-catalyzed cleavage (■) and isomerization (□) of UpU; T = 90 °C, I(NaClO₄) = 1.0 mol·L⁻¹.

Figure 4. pH-rate profiles for the (A) 11a- and (B) 11b-catalyzed cleavage (■) and isomerization (□) of UpU; T = 90 °C, I(NaClO₄) = 1.0 mol·L⁻¹.

Table 1. Second-order rate constants for the cleavage and isomerization of UpU, catalyzed by the tri-, tetra- and pentacationic forms of 11a and 11b; T = 90 °C, I(NaClO₄) = 1.0 mol·L⁻¹.

Rate Constant	11a		11b
	Cleavage	Isomerization	Cleavage	Isomerization
k5/10−3 L·mol−1·s−1	26.1 ± 0.2	6.2 ± 0.2	N/A a	N/A a
k4/10−3 L·mol−1·s−1	7.37 ± 0.06	4.7 ± 0.1	17.5 ± 0.4	15 ± 3
k3/10−3 L·mol−1·s−1	N/A b	0.5 ± 0.2	11.1 ± 0.8	4 ± 6

^a The concentration of the pentacationic form of 11b is negligible under the experimental conditions; ^b Fitting to Equation (2) gave a negative value.

Table 1. Second-order rate constants for the cleavage and isomerization of UpU, catalyzed by the tri-, tetra- and pentacationic forms of 11a and 11b; T = 90 °C, I(NaClO₄) = 1.0 mol·L⁻¹.

Rate Constant	11a		11b
	Cleavage	Isomerization	Cleavage	Isomerization
k5/10−3 L·mol−1·s−1	26.1 ± 0.2	6.2 ± 0.2	N/A a	N/A a
k4/10−3 L·mol−1·s−1	7.37 ± 0.06	4.7 ± 0.1	17.5 ± 0.4	15 ± 3
k3/10−3 L·mol−1·s−1	N/A b	0.5 ± 0.2	11.1 ± 0.8	4 ± 6

^a The concentration of the pentacationic form of 11b is negligible under the experimental conditions; ^b Fitting to Equation (2) gave a negative value.

Comparison of the second order rate constants of the cleavage reaction catalyzed by 11a suggests that SH₅⁵⁺ is approximately 4 times as active as SH₄⁴⁺ and the latter is, in turn, at least one order of magnitude more active than SH₃³⁺. In fact, whether the tricationic form of 11a contributes at all to the catalysis is questionable. Unlike cleavage, isomerization is catalyzed approximately equally by the penta- and tetracationic forms of 11a. Even the tricationic species appears to exhibit some activity, although the reliability of this result is debatable. The benzene analog 11b does not undergo a fifth protonation under conditions of the kinetic runs. Catalysis of cleavage and isomerization by SH₄⁴⁺ predominates over a wide pH range and is approximately three times as efficient with 11b as with 11a. In the case of 11b, catalytic activity of SH₃³⁺ is also evident although lower than that of SH₄⁴⁺.

3. Discussion

3.1. Base-Selectivity of 11a

The uracil-selectivity of 11a parallels the behavior previously observed with the dinuclear Zn²⁺ complex of a structural analog, 1,3-bis(1,5,9-triazacyclododecan-3-yloxymethyl)benzene. In that case, one of the Zn²⁺(azacrown) moieties anchors the cleaving agent to a uracil base, the other moiety cleaving the neighboring phosphodiester linkage. Accordingly, 3′,5′-ApU and 3′,5′-UpA are cleaved much faster than 3′,5′-ApA or other dinucleoside monophosphates that do not contain uracil bases. 3′,5′-UpU is not cleaved, suggesting that both Zn²⁺(azacrown) moieties are engaged in uracil binding, but the catalytic activity is restored by addition of a third azacrown ligand [31,32,33]. A key difference between the present results and those obtained in the presence of Zn²⁺ is, however, seen in the respective pH-rate profiles. In the latter case, efficient catalysis was only observed under neutral and mildly alkaline conditions (where coordination of Zn²⁺ to deprotonated N3 atom of uracil prevails) whereas in the present case, catalysis by 11a and 11b was most pronounced under acidic conditions. In fact, under such conditions, Zn²⁺ would not even be appreciably coordinated by cyclen [12].

Compared to their metal chelates, binding of uncomplexed azacrowns to nucleobases is much weaker and has been studied much less extensively. One could, however, envision a binding mode unique to uracil (and thymine) bases. The two oxo substituents may both accept a hydrogen bond from a single dicationic cyclen molecule. In adenine, orientation of the two potential hydrogen bond acceptors (N1 and N7) is not conducive for such binding. In the case of tetracationic 11a (or 11b) and UpU, one of the cyclen moieties would bind electrostatically to the anionic phosphodiester linkage and the other one via hydrogen bonding to one of the uracil bases (Figure 5). While the former interaction is undoubtedly stronger, the inefficiency of cyclen itself as a catalyst indicates that the latter is also vital in achieving a sufficient local concentration. Similar behavior has also been reported with other bifunctional cleaving agents, notably the calixarene derivatives 2 and 3 that cleave 3′,5′-GpU, 3′,5′-GpG and 3′,5′-UpU from one to two orders of magnitude faster than the other dinucleoside monophosphates [11]. Attempts to quantify the affinity of cyclen to uridine and adenosine by NMR titrations were unsuccessful-significant binding was only observed under conditions where the uracil base is deprotonated (data presented in Figure S1 in the supporting information). Apparently interactions between 11a (or 11b) and dinucleoside monophosphates are too complex to be studied by this simplified model system.

Figure 5. MOPAC (PM6)-minimized structure for tetracationic 11b (green) hydrogen bonded (dashed lines) to the monoanionic, pentacoordinate intermediate (orange) of UpU cleavage and hydrolysis.

Figure 5. MOPAC (PM6)-minimized structure for tetracationic 11b (green) hydrogen bonded (dashed lines) to the monoanionic, pentacoordinate intermediate (orange) of UpU cleavage and hydrolysis.

3.2. Mechanism of the Catalysis by 11a and 11b

In striking contrast to the Zn²⁺(azacrown)-based catalysts, 11a and 11b catalyze isomerization almost as efficiently as cleavage. To the best of our knowledge, the present study is the first report on catalysis of isomerization of RNA phosphodiester linkages by a non-metallic small molecular entity. The tetracationic forms of 11a and 11b facilitate both cleavage and isomerization to approximately the same extent, making stabilization of the common phosphorane intermediate an attractive mechanistic alternative. This together with the observed base-selectivity suggests that 11a and 11b interact with 3′,5′-UpU by simultaneous binding of the doubly protonated cyclen ligands to the uracil base and the internucleosidic phosphodiester linkage. Evidently, binding is enforced upon formation of the phosphorane intermediate by attack of the 2′-OH. Protonation of the pyridine nitrogen makes 11a a somewhat better catalyst, but only in the case of cleavage. The additional acceleration could be tentatively attributed to assistance of the departure of the 5′-oxygen by hydrogen bonding from the protonated pyridine nitrogen.

4. Experimental Section

4.1. General Methods

NMR spectra were recorded on a Bruker Avance 400, 500, or 600 NMR spectrometer and the mass spectra on a Bruker Daltonics Micro-TOF-Q high resolution mass spectrometer. The ¹H NMR chemical shifts were referenced to internal TMS. The reagents, including 1,4,7-tris(tert-butoxycarbonyl)-1,4,7,10-tetraazacyclododecane, were commercial products that were used as received.

4.2. 2,6-Bis(1,4,7,10-tetraazacyclododecan-1-ylmethyl)pyridine (11a)

Compound 11a was prepared as described previously by Xiang et al [27]. Accordingly, 2,6-bis(bromomethyl)pyridine was treated with 1,4,7-tris(tert-butoxycarbonyl)-1,4,7,10-tetraazacyclododecane in MeCN in the presence of K₂CO₃ and the tert-butoxycarbonyl protections were removed with TFA in 1:4 (v/v) mixture of MeOH and CH₂Cl₂. The product was converted to free base with strong anion-exchange resin (Dowex 1X2, mesh 200, OH⁻-form) in water. The ¹H NMR spectrum of the material thus obtained was identical to that previously reported for 11a. ¹H NMR (D₂O, 500 MHz): δ 7.72 (t, J = 7.8 Hz, 1H), 7.35 (d, J = 7.8 Hz, 2H), 3.64 (s, 4H), 2.50–2.68 (m, 32H). ¹³C NMR (D₂O, 125.8 MHz): δ 158.4, 138.3, 122.9, 59.6, 50.9, 45.0, 44.2, 43.2. HRMS (ESI⁺): m/z calcd 448.3876 obsd 448.3860 [M + H]⁺.

4.3. 1,3-Bis(1,4,7,10-tetraazacyclododecan-1-ylmethyl)benzene (11b)

Compound 11b was prepared as described above for 11a except that 1,3-bis(bromomethyl)benzene was used instead of 2,6-bis(bromomethyl)pyridine as the starting material. The ¹H NMR spectrum of the product was identical to that previously reported for 11b. ¹H NMR (D₂O, 500 MHz): δ 7.32 (t, J = 8.0 Hz, 1H), 7.23 (s, 1H), 7.16 (d, J = 8.0 Hz, 2H), 3.58 (s, 4H), 2.55–2.78 (m, 32H). ¹³C NMR (D₂O, 125.8 MHz): δ 138.4, 130.7, 129.0, 128.6, 57.5, 50.6, 44.8, 43.3, 43.2. m/z calcd 447.3918 obsd 447.3913 [M + H]⁺.

4.4. Determination of the pK_a Values

The pK_a values of 11a and 11b were determined by NMR spectrometric titrations at 90 °C in D₂O buffered with 0.10 mol·L⁻¹ phosphoric acid. Accordingly, compound 11a or 11b was dissolved in phosphoric acid (0.10 mol·L⁻¹) and 1.0 mol·L⁻¹ sodium deuteroxide in D₂O was gradually added. The pK_a values were determined as inflection points of the plots of the ¹H chemical shifts of the methylene protons as a function of pH. The pH axis, in turn, was calibrated on the basis of the observed ³¹P chemical shift and known pK_a values of phosphoric acid at 90 °C [29].

4.5. Kinetic Measurements

The reactions were carried out in sealed tubes immersed in a thermostated water bath (90.0 ± 0.1 °C). The pH of the reaction solutions were adjusted by titrating 11a or 11b (10–70 mmol·L⁻¹) with 3.5, 3.8, 4.5 or 5.0 eq. of perchloric acid. In other words, 11a and 11b served as both cleaving agents and buffers. Sodium perchlorate (1.0 mol·L⁻¹) was used as a background electrolyte. The initial concentration of 3′,5′-UpU and 3′,5′-ApA was 500 μmol·L⁻¹. 4-Nitrophenol (1.0 mmol·L⁻¹) was used as an internal standard. To rule out the possibility of nucleophilic catalysis by the phenolic internal standard, some of the kinetic runs were also carried out in the absence of this standard, with identical results.

The composition of the samples withdrawn at appropriate time intervals was analyzed by HPLC on a Hypersil-Keystone Aquasil C18 column (4 × 150 mm, 5 μm) using a mixture of MeCN and a 50 mmol·L⁻¹ TRIS buffer (pH 8.1) containing 50 mmol·L⁻¹ ammonium chloride as an eluent. The cleaving agents 11a and 11b were present in at least 20-fold excess in all samples and they eluted as broad peaks. To reduce the concentration of 11a and 11b to a level where these peaks would not overlap with those of the other components, the samples were diluted with water (1:10) before injection. For the first 8 min, isocratic elution with 100% buffer was applied, followed by a linear gradient from 0% to 15% of MeCN over 11 min. A constant flow rate of 1.0 mL·min⁻¹ and a detection wavelength of 260 nm were employed. The observed retention times (t_R, min) for 3′,5′-UpU, its reaction products and the internal standard were: 4.7 min (uridine), 10.8 min (4-nitrophenol), 14.7 min (2′,5′-UpU) and 15.7 (3′,5′-UpU). The products were characterized by spiking with authentic samples.

The molar absorptivities of the 2′- and 3′-isomers of UpU were assumed to be identical. Calculation of the rate constants for the cleavage and isomerization reactions was based on the signals of 3′,5′-UpU, 2′,5′-UpU and uridine. The signals of uridine monophosphates were not used as their integration was not entirely reproducible. The conversion of uridine monophosphates to uridine was, under the conditions employed, so slow that it did not appreciably affect the time-dependent concentration of uridine. In other words, uridine could be assumed to form exclusively by cleavage of UpU. Cleavage and isomerization of UpU obeyed the first-order rate law throughout the kinetic runs (a representative time profile is presented in Figure S2 in the supporting information), as could be expected given the large excess of the cleaving agents 11a and 11b. Pseudo-first-order rate constants for the cleavage and isomerization reactions were calculated by numerical fitting of the experimental data to the differential rate equations, (data summarized in Tables S1–S4 in the supporting information).

5. Conclusions

The bis-cyclen cleaving agents 11a and 11b catalyze the cleavage and isomerization of UpU under neutral and acidic conditions, in all likelihood by lowering the negative charge on the phosphodiester linkage through interaction with a doubly protonated cyclen moiety. Additional binding of the other cyclen moiety to one of the uracil bases is also needed for efficient catalysis. Compared to the other non-metallic cleaving agents published so far, the catalytic activity of 11a and 11b appears to be somewhat lower than that of the most active ones (1 and 5). Quantitative comparison is difficult, since the experimental data for various catalysts refer to very different conditions. The highest cleaving activities have been observed with 1 and 5 by using oligonucleotide targets [9,14]. With dinucleoside monophosphates, the most efficient cleaving agents are the calixarene derivatives 2 and 3, but in that case the data was obtained in 80% aqueous DMSO [11].