Recognition of AMP, ADP and ATP through Cooperative Binding by Cu(II) and Zn(II) Complexes Containing Urea and/or Phenylboronic-Acid Moieties.

We report a series of Cu(II) and Zn(II) complexes with different ligands containing a dipicolyl unit functionalized with urea groups that may contain or not a phenylboronic acid function. These complexes were designed for the recognition of phosphorylated anions through coordination to the metal ion reinforced by hydrogen bonds involving the anion and NH groups of urea. The complexes were isolated and several adducts with pyrophosphate were characterized using Xray diffraction measurements. Coordination of one of the urea nitrogen atoms to the metal ion promoted the hydrolysis of the ligands containing 1,3-diphenylurea units, while ligands bearing 1-ethyl-3-phenylurea groups did not hydrolyze significantly at room temperature. Spectrophotometric titrations, combined with ¹H and 31P NMR studies, were used in investigating the binding of phosphate, pyrophosphate (PPi), and nucleoside 5'-polyphosphates (AMP, ADP, ATP, CMP, and UMP). The association constants determined in aqueous solution (pH 7.0, 0.1 M MOPS) point to a stronger association with PPi, ADP, and ATP as compared with the anions containing a single phosphate unit. The [CuL⁴]2+ complex shows important selectivity for pyrophosphate (PPi) over ADP and ATP.

1. Introduction

Phosphorylated metabolites are involved in biologically relevant processes [1], such as transport of chemical energy [2] (n class="Chemical">adenosine triphosphate, ATP, and pyrophosphate (PPi), signal transduction and transmission [3,4,5], activation of platelets [6], and protein kinases [7] (adenosine monophosphate, AMP, and adenosine diphosphate (ADP), or DNA replication catalyzed by DNA polymerase, a process in which PPi plays an important role [8,9,10]. Thus, the design and synthesis of artificial receptors that bind phosphorylated anions is an important scientific goal with potential application in sensing, optical imaging and in vitro clinical diagnosis [11,12,13,14,15,16,17,18,19]. For instance, pyrophosphate (PPi) is one of the hydrolysis products of ATP and is released in DNA/RNA polymerase reactions [20,21]. Abnormal levels of this anion have been related to a number of diseases, including arthritis and cancer [22].

The interaction of pan class="Chemical">Cu(II) and pan class="Chemical">Zn(II) ions with nucleoside 5′-polypan class="Chemical">phosphates (AMP, ADP, ATP, CMP, and UMP) were studied in detail by Sigel et al. in the early 90’s. [23,24,25,26,27] The formation of macrochelates was clearly defined for adenine nucleotides, thanks to the coordination of both the phosphate chains and the nitrogen N-7 of the purine residue. [28,29] Since then, different types of molecular receptors have been used for the recognition of phosphorylated anions in aqueous media [1]: (1) Linear or macrocyclic positively charged receptors, generally polyammonium systems [30,31,32,33] or receptors containing guanidinium or imidazolium groups [34,35]; (2) Metal complexes, generally coordinatively unsaturated Cu2+ or Zn2+ complexes, with acyclic (i.e., dipicolyl or terpyridyl derivatives [36,37,38,39,40,41,42] or Schiff base ligands [43]) or macrocyclic ligands [44,45,46]; (3) Ditopic receptors that combine a metal coordinating unit and hydrogen-bond donors to reinforce anion binding [47,48].

In a previous work, we investigated the ability of the pan class="Chemical">Cu2+ and pan class="Chemical">Zn2+ complexes derived from L to bind anions through cooperative binding, involving (i) coordination of the anion to the pan class="Chemical">metal ions, and (ii) hydrogen-bonding interactions involving the coordinated anion and the NH groups of the urea moiety as hydrogen-bond donors [49]. More recently we have shown that the [CuL2]2+ complex binds sulphate through such cooperative binding [50]. Thus, we envisaged that the [CuL2]2+ complex and related derivatives could be useful for the recognition of phosphorylated anions. Herein, we report a series of ligands containing a bis(pyridin-2-ylmethyl)amine unit for coordination to Cu2+ and Zn2+, and a urea moiety that is expected to reinforce anion binding through hydrogen-bonding interactions. The flexibility of the receptor was modulated by including a benzyl (L and L) or ethyl (L and L) spacer connecting the urea and bis(pyridin-2-ylmethyl)amine units. When considering the ability of phenylboronic acids to bind cis-diol groups [51,52,53], we also prepared ligands L, L, and L in an attempt to reinforce the binding to AMP, ADP, and ATP. We report a series of X-ray structures and 1H and 31P NMR studies that provide insight into the nature of the interactions established between the Zn2+ and Cu2+ complexes and different anions. Spectrophotometric titrations were used to determine the stoichiometries and association constants characterizing anion binding.

2. Results

2.1. Synthesis and Characterization of the Ligands and Metal Complexes

The preparation of L and the corresponding pan class="Chemical">Cu2+ and pan class="Chemical">Zn2+ complexes using sulphate and nitrate as counterions were described in a previous work [49]. The syntheses of L and L started from (3-aminophenyl)boronic acid (1), which was protected using ethane-1,2-diol to give compound 3 in quantitative yield (Scheme 1). Compound 3 was subsequently reacted with 1-(chloromethyl)-2-isocyanatobenzene or 1-chloro-2-isocyanatoethane to yield compounds 5 and 7, respectively. Alkylation of bis(pyridin-2-ylmethyl)amine with 5 (or 7) provided compound 6 (or 8), which were purified using MPLC on neutral Al2O3. This afforded directly ligands L and L, thanks to the deprotection of the phenylboronic acid group during the chromatographic separation. The alkylation of bis(pyridin-2-ylmethyl)amine with 5 and 7 were found to proceed in rather low yields (Scheme 1).

Scheme 1

Synthesis of ligands L, L and L: (i) Ethane-1,2-diol, Δ, 100% (3), 85% (4); (ii) Compound 3, 1-(Chloromethyl)-2-isocyanatobenzene, Et2O, r.t., 16 h, 91%; (iii) Bis(pyridin-2-ylmethyl)amine, CH3CN, DIPEA, 70 °C, 5 d; (iv) MPLC, neutral Al2O3, CH2Cl2:MeOH, 40% (two steps); (v) Compound 3, 1-Chloro-2-isocyanatoethane, Et2O, r.t., 16 h, 89%; (vi) Bis(pyridin-2-ylmethyl)amine, CH3CN, DIPEA, 70 °C, 5 d; (vii) MPLC, neutral Al2O3, CH2Cl2:MeOH, 24% (two steps); (viii) Compound 4, N-bromosuccinimide (NBS), dibenzoylperoxide, CCl4, Δ, 16 h, 54%; (ix) Bis(pyridin-2-ylmethyl)amine, CH3CN, DIPEA, Δ, 16 h; (x) MPLC, neutral Al2O3, CH2Cl2:MeOH, 42% (two steps).

The synthesis of L started from pan class="Chemical">m-tolylboronic acid (2), which was converted to the bromomethyl derivative 9 following the literature procedure [53]. Alkylation of pan class="Chemical">bis(pyridin-2-ylmethyl)amine with compound 9 in pan class="Chemical">acetonitrile using N,N-Diisopropylethylamine (DIPEA) as a base and subsequent purification gave L.

The synthesis of ligand pan class="Chemical">L4 was initiated by protecting compound 11 with pan class="Chemical">di-tert-butyl dicarbonate and subsequent reaction of 12 with pan class="Chemical">bis(pyridin-2-ylmethyl)amine in acetonitrile using DIPEA as a base (Scheme 2). Deprotection of compound 13 with trifluoroacetic acid (TFA) was followed by reaction of 14 with 1-isocyanato-4-nitrobenzene affording ligand L4.

Scheme 2

Synthesis of ligand L: (xi) di-tert-butyl dicarbonate, dioxane, 0 °C, 48 h, 80% (12); (xii) Bis(pyridin-2-ylmethyl)amine, CH3CN, DIPEA, 70 °C, 3 d, 39%; (xiii) trifluoroacetic acid (TFA:CH2Cl2 (1:1), r.t., 16 h, 96%; (xiv) 1-isocyanato-4-nitrobenzene, CHCl3, r.t., 2 h, 85%.

The reaction of 1 equivalent of ligand (Ln; (n = 1, 3, 4 or 5)) with 1 equiv of hydrated M(n class="Chemical">ClO4)2 salts (M = Cu or Zn) in THF (L), acetonitrile (L and L), or methanol (L) at room temperature, provided the desired complexes as the perchlorate salts (except for [ZnL5](ClO4)2 that was prepared in situ for 1H-NMR measurements). In the case of L, the [CuL4(SO4)] complex was also prepared by a similar procedure in methanol. The complexes were isolated in 82–97% yields, with the exception of those derived from L, which were obtained in lower yields (49% and 59% for [ZnL3](ClO4)2 and [CuL3](ClO4)2, respectively).

As expected, the IR spectra (KBr discs) feature bands due to ν(N-H) and ν(C=O) modes associated to the presence of the pan class="Chemical">urea group in L, L, and L derivatives, while ν(O-H) and ν(O-B-O) modes are also observed when the boronic moiety is present (L, L, and L). In all cases, the bands corresponding to the ν(Ph/Py) mode are present, and the coordination of the pan class="Chemical">metal ions induces significant shifts with respect to the corresponding free ligands (see Materials and Methods Section). It is noticeable that the bands corresponding to the νas(Cl-O) (stretching) and δas(O-Cl-O) (bending) modes of the perchlorate groups appear without splitting for all complexes at ca. 1100 and 625 cm−1, respectively, as befit uncoordinated anions [54,55]. In the case of [CuL4(SO4)], the bands corresponding to the νa(S-O) and νa(O-S-O) modes are splitted, as expected for a coordinated sulphate anion with low symmetry. This is in agreement with UV-vis diffuse reflectance spectroscopy, which provided different positions for the d-d absorption band observed for [CuL4(SO4)] and [CuL4](ClO4)2 (706 and 633 nm, respectively).

Conductivity measurements were carried out in 10−3 M n class="Chemical">methanol solutions at 25 °C. The molar conductivity of the perchlorate salts (154.9–171.3 cm2 Ω−1 mol−1) are in the range reported for 2:1 electrolytes [56], indicating that these complexes are completely dissociated in methanol solution. In the case of [CuL4(SO4)], the low solubility of this charge-neutral complex prevented us from determining its molar conductivity value, confirming that the sulphate anion is directly bonded to the Cu2+ ion.

2.2. X-ray Crystal Structures

The solid state structures of different complexes of L were investigated by using X-ray diffraction measurements. Table 1 presents the bond distances of the n class="Chemical">metal coordination environments, while views of the structures are shown in Figure 1 and Figure 2. The complexes differ in the nature of the metal ion (Zn2+ or Cu2+) and the anion (sulphate or pyrophosphate). The Cu2+ ions in [CuL4(SO4)] and [CuL4(H2PPi)] complexes present octahedral coordination with a strong Jahn-Teller distortion [57]. The ligand adopts an ‘open wing butterfly’ conformation that is similar to those observed for the Cu2+ complexes of L2 [49]. The equatorial plane of the coordination polyhedron in [CuL4(SO4)] is defined by the donor atoms of the dipicolylamine unit [N(4), N(5) and N(6)] and an oxygen atom of the anion [O(4)] (mean deviation from planarity: 0.04 Å), with the metal ion being placed 0.01 Å below this plane in [CuL4(SO4)] and 0.12 Å above it in [CuL4(H2PPi)]. The apical positions in [CuL4(SO4)] are occupied by one of the nitrogen atoms of the urea subunit [N(3)] and an oxygen atom of a sulphate anion of an adjacent complex molecule [O(5b)] (Figure 1). Thus, the presence of μ2–η1:η1-sulphate anions bridging two neighboring complex molecules leads to the formation of a coordination polymer (Figure S1, Supplementary Materials). In [CuL4(H2PPi)], the apical positions are delineated by one of the nitrogen atoms of the urea subunit [N(3)] and an oxygen atom of the H2PPi2− anion [O(8)], which coordinates in a κ2-H2PPi2− mode forming a six-membered chelate ring.

Table 1

Bond distances (Å) of the metal coordination environments.

	[CuL4(SO4)]	[CuL4(H2PPi)]	[{CuL4}2(μ-PPi)]	[{ZnL4}2(μ-PPi)]
M(1)-N(3)	2.728(3)	2.670(1)	-	-
M(1)-N(4)	2.044(3)	2.039(1)	2.100(2)	2.340(6)
M(1)-N(5)	2.005(3)	1.994(1)	1.990(2)	2.045(7)
M(1)-N(6)	2.000(2)	1.991(1)	1.989(2)	2.041(6)
M(1)-O(4)	1.960(2)	1.930(1)	1.938(1)	2.021(5)
M(1)-O(5)	2.247(2)	-		-
M(1)-O(8)	-	2.263(1)	2.172(2)	1.949(5)

Figure 1

(a) X-ray crystal structure of [CuL4(SO4)] with labelling scheme; (b) X-ray crystal structure of [CuL4(H2PPi)] with labelling scheme. The Oak Ridge Thermal-Ellipsoid Plot Program (ORTEP) plots are at the 30% probability level. Symmetry transformations used to generate equivalent atoms for [CuL4(SO4)]: #2 −x + 1, y − 1/2,−z + 3/2.

Figure 2

(a) X-ray crystal structure of [{ZnL4}2(μ-PPi)] with labelling scheme; (b) X-ray crystal structure of [{CuL4}2(μ-PPi)] with labelling scheme. The ORTEP plots are at the 30% probability level.

The cis angles of the coordination polyhedron (81.0°–98.8° in [pan class="Chemical">CuL4(SO4)] and 82.4°–98.4° in [pan class="Chemical">CuL4(H2PPi)]) are relatively close to the one expected for a regular pan class="Disease">octahedral coordination (90°), whereas the corresponding trans angles (162.7°–178.0° for [CuL4(SO4)] and 164.4–173.8 for [CuL4(H2PPi)]) deviate up to 18° from the ideal one (180°) (Figure S2, Supplementary Materials).

The pan class="Chemical">sulphate anion in [pan class="Chemical">CuL4(SO4)] interacts with the pan class="Chemical">metal ion via a coordinate bond and with the urea moiety through a moderate hydrogen-bonding interaction, the latter involving one of the NH groups of the urea unit as hydrogen-bond donor and an oxygen atom of the anion as hydrogen-bond acceptor [N(2)⋯O(6) 2.768(3) Å; N(2)-H(2N)⋯O(6), 1.97(3) Å; N(2)-H(2N)⋯O(6) 161(3)°]. The value of the S(1)-O(6)-H(2N) angle (116.8°) is close to the ideal one (122° ± 10°) [58]. The interaction of the anion with another complex molecule causes sulphate to move away from the N(3)-H(3N) fragment, which interacts with an oxygen atom of another sulphate anion via an intermolecular hydrogen-bonding interaction.

We have also obtained single crystals suitable for X-ray diffraction measurements of n class="Chemical">[{ZnL4}2(μ-PPi)] and [{CuL4}2(μ-PPi)] (Figure 2), in which the fully deprotonated pyrophosphate anion acts as a bridging μ2κ4-PPi4− ligand forming two six-membered chelate rings [59,60]. This bridging mode of the anion has been previously reported by Hong and coworkers in the solid state for dinuclear Zn2+ complexes derived from di(2-picolyl)amine [61,62]. The ligand in [{CuL4}2(μ-PPi)] adopts an ′open wing butterfly′ conformation (Figure 2), which results in a square pyramidal geometry around the Cu2+ ion. The basal plane is defined by the three donor atoms of the dipicolylamine unit [N(4), N(5), and N(6) for Cu(1) and N(10), N(11) and N(12) for Cu(2)] and an oxygen atom of pyrophosphate [O(4) or O(9)] [mean deviation from planarity: 0.03 Å for Cu(1) and 0.05 Å for Cu(2)], while the apical position is occupied by another oxygen atom of the anion [O(8) or O(5)]. The metal ion is placed 0.29 Å [Cu(1)] or 0.28 Å [Cu(2)] above the basal plane. The cis angles of this plane (82.8°–95.7°) and those involving the oxygen atom occupying the apical position, the metal centre and the donor atoms of the equatorial plane (93.3°–102.5°), as well as the trans angles (157.4°–166.8°), are relatively close to the ideal ones (90 and 180°, respectively). The index of trigonality τ, which amounts to 0.12 for Cu(1) and 0.16 for Cu(2) (τ = 0 for an ideal square pyramidal geometry and τ = 1 for a regular trigonal bipyramidal environment) [63] is in agreement with the square pyramidal polyhedron.

The ligand L in pan class="Chemical">[{ZnL4}2(μ-PPi)] adopts a ′bent propeller′ conformation and wraps around the pan class="Chemical">metal ions providing trigonal bipyramidal coordination environments. The equatorial plane of the bipyramid is defined by the pan class="Chemical">nitrogen atoms of the pyridine units [N(5) and N(6) for Zn(1) and N(11) and N(12) for Zn(2)] and an oxygen atom of the pyrophosphate anion [O(8) for Zn(1) and O(5) for Zn(2)]. The apical positions are occupied by the amine nitrogen atom and one of the oxygen atoms of the anion [N(4) and O(4) for Zn(1) and N(10) and O(9) for Zn(2)]. The Zn2+ ion is placed 0.24 Å [Zn(1)] or 0.25 Å [Zn(2)] above the equatorial plane. The angles involving the donor atoms of this plane (113.9°–124.7°), as well as the trans angle (170.4°–170.6°) are close to the ones expected for a regular trigonal bipyramid (120° and 180°, respectively). The index of trigonality τ amounts to 0.76 for both metals [63], which is in agreement with the indicated geometry.

The pan class="Chemical">PPi4− anions in both pan class="Chemical">[{ZnL4}2(μ-PPi)] and [pan class="Chemical">{CuL4}2(μ-PPi)] show a cooperative binding in which the anion interacts simultaneously with the metal ion via coordinate bonds, and with the urea moiety through Y-shape hydrogen-bonding interactions. The N-H(N)-O angles and distances (Table 2) show that these interactions are rather symmetrical and can be regarded as moderate, although the N⋯O distances point to a slightly weaker interaction in the Zn2+ complex. In all cases, the P-O-H(N) angles (109°–122°) are close to the ideal value for a tetrahedral anion (122° ± 12°) [58].

Table 2

Intramolecular hydrogen-bonding interactions observed in the solid state structures of [CuL4(SO4)], [{CuL4}2(μ-PPi)] and [{ZnL4}2(μ-PPi)].

		d(D-H)/Å	d(H⋯A)/Å	d(D⋯A)/Å	D-H⋯A/°
[CuL4(SO4)]	N(2)-H(2N)⋯O(6)	0.82(3)	1.97(3)	2.768(3)	161(3)
[{CuL4}2(μ-PPi)]	N(2)-H(2N)⋯O(10)	0.79(2)	2.04(3)	2.830(3)	175(2)
	N(3)-H(3N)⋯O(8)	0.74(3)	2.08(3)	2.797(2)	161(3)
	N(8)-H(8N)⋯O(6)	0.79(2)	1.98(3)	2.765(2)	173(2)
	N(9)-H(9N)⋯O(5)	0.82(3)	1.94(3)	2.751(2)	169(2)
[{ZnL4}2(μ-PPi)]	N(2)-H(2N)⋯O(10)	0.73(9)	2.12(9)	2.850(9)	172(10)
	N(3)-H(3N)⋯O(8)	0.76(9)	2.13(9)	2.880(9)	168(10)
	N(8)-H(8N)⋯O(6)	0.82(9)	2.05(9)	2.870(8)	178(9)
	N(9)-H(9N)⋯O(5)	0.75(9)	2.15(9)	2.876(9)	163(10)

2.3. Stability of the Complexes Toward Hydrolysis

The pan class="Chemical">1H-NMR spectra of the pan class="Chemical">Zn2+ complexes of both L and L recorded in wet pan class="Chemical">dmso-d6 were observed to change over time, which caused an increase of the number and complexity of the signals (Figures S3 and S4, Supplementary Materials). This suggests that both [ZnL1]2+ and [ZnL2]2+ complexes hydrolyse in aqueous solution to form the [ZnL6]2+ complex (Scheme 3), 2-aminophenylboronic acid or 3-nitroaniline, and carbon dioxide. The presence of a 3-nitroaniline molecule in the molecular structure of [CuL2(μ-SO4)]2 reported recently also points in this direction [50]. In the case of [ZnL2](ClO4)2, new resonances appear in the 1H-NMR spectrum from 7.35 to 6.60 ppm, none of which correspond to the complex or the free ligand. The presence of a signal at 6.94 ppm due to 3-nitroaniline confirmed the hydrolysis of the complex. The relative intensity of the signals attributable to the [ZnL2]2+ species and 3-nitroaniline indicate that 6% of the complex has hydrolysed after four hours at room temperature, while after 48, 96, and 168 h this percentage increases to 28%, 43%, and 49%, respectively. A similar situation was observed for [ZnL1]2+, which hydrolysed to a slightly lower extent after 4 h (~5%). 1H DOSY experiments performed for [ZnL2]2+ 168 h after dissolution of the complex allowed discriminating the three species that are present in solution on the basis of their different diffusion coefficients (Figure 3). Taking the diffusion coefficient of dmso-d5 as a reference (D = 6.81 × 10−10 m2·s−1) [64], these studies provided diffusion coefficients D at 25 °C of 1.34 × 10−10 m2·s−1, 1.85 × 10−10 m2·s−1, and 3.64 × 10−10 m2·s−1 for [ZnL2]2+, [ZnL6]2+, and 3-nitroaniline, respectively.

Scheme 3

Ligands and phosphorylated anions discussed in the present work.

Figure 3

DOSY 1H-NMR spectrum (500 MHz, 298 K) recorded for [ZnL2]2+ 168 h after dissolution of the complex in dmso-d6.

The hydrolysis of the pan class="Chemical">urea unit in [pan class="Gene">CuL2]2+ was monitored in aqueous solution by following the absorption band of pan class="Chemical">3-nitroaniline (λmax = 357 nm, ε = 1486 M−1·cm−1) over time and employing the method of initial rates (Figure S5, Supplementary Materials). The observed pseudo-first-order rate constants (kobs) and half-life times (t1/2) were determined by fitting the data obtained at 390 nm using two temperatures (25 and 50 °C, I = 0.1 M NaClO4) and two pH values (5.5 and 7.0). In line with previous studies [65], our results did not reveal significant pH dependence of the kobs values in this pH range, which were determined to be 4.5 ± 0.1 × 10−5·s−1 at 25 °C and 7.30 ± 0.04 × 10−4 s−1 at 50 °C. The corresponding half-life times are 258 min at 25 °C and 19 min at 50 °C. Thus, the [CuL2]2+ complex experiences significant hydrolysis in aqueous media at room temperature. Analogous studies performed for the [CuL4]2+ complex provided rate constants of 3.12 ± 0.01 × 10−9·s−1 and 1.265 ± 0.002 × 10−7·s−1 at 25 and 50 °C, respectively, which correspond to half-life times of ~89 (25 °C) and ~2 (50 °C) months. Thus, the replacement of the 1-(3-nitrophenyl)-3-phenylurea unit of L2 by a 1-ethyl-3-(3-nitrophenyl)urea group increases the stability toward hydrolysis of the corresponding Cu2+ complex by 3–4 orders of magnitude.

Most of the studies regarding the decomposition of pan class="Chemical">ureas fopan class="Chemical">cused on its hydrolysis to pan class="Chemical">ammonium and carbamate ions [66,67] (the latter is unstable and its decomposition gives rise to the formation of ammonium ions, carbon dioxide, and water [68]) by urease [69]. Kinetic experiments performed in water at pH 7 and 38 °C showed that the value of kobs for this reaction decreases as the substitution on the urea moiety increases (from 5913 s−1 for urea to 0.075 s−1 for N-methylurea [70,71]). The value reported for the uncatalyzed hydrolysis of tetramethylurea (6.0×10−11 s−1) points to a very slow reaction in the absence of urease [72]. Thus, we conclude that the relatively high rate constants determined for the hydrolysis of the urea groups in [ZnL1]2+, [ZnL2]2+, and [CuL2]2+ are related to the coordination of a nitrogen atom of the urea unit to the metal ion.

2.4. Binding to Phosphorylated Anions

The binding of phosphorylated anions n class="Chemical">phosphate, AMP, CMP, UMP, PPi, ADP, and ATP to [CuL3](ClO4)2, [CuL4](ClO4)2, and [CuL5](ClO4)2 was investigated by using spectrophotometric titrations in aqueous solutions (pH = 7.0, MOPS buffer). The absorption spectra of the complexes show a d-d absorption band with a maximum at 615 ([CuL3]2+), 654 ([CuL4]2+), and 643 nm ([CuL5]2+), typical of dxz, dyz → dx transitions in a tetragonal ligand field [73]. This is consistent with the Jahn-Teller distorted octahedral environment, where two coordination positions are likely occupied by water molecules, and supported by the molar conductivity values of these complexes in methanol solution. Addition of phosphate, AMP, CMP, or UMP causes slight changes in the d-d absorption band of the complexes, in particular, a slight bathochromic shift of the absorption maximum and small changes in the molar extinction coefficients (Figure 4, see also Figures S6–S8, Supplementary Materials). This indicates that the complexes retain the distorted octahedral coordination upon anion binding. A completely different situation is however observed upon addition of PPi, ADP, and ATP, as these anions provoke both an important bathochromic shift of the d-d absorption band and the appearance of a shoulder in the low energy side. This is characteristic of Cu2+ complexes having trigonal bipyramidal coordination geometries, which in the case of [CuL2]2+ complexes, was related to the de-coordination of the weakly bonded urea nitrogen atom [49]. This is in line with the X-ray structure of [{ZnL4}2(μ-PPi)] shown in Figure 2, in which the anion coordinates to the metal ion in a bidentate fashion and establishes hydrogen-bonding interactions with the urea group.

Figure 4

Family of UV/vis spectra taken during the course of the titration of [CuL4]2+ (5 × 10−3 M in H2O, pH 7.0, MOPS 0.1 M, 25 °C) with standard solutions (0.5 M) of: (a) NaH2PO4; (b) Na2AMP; (c) Na2ADP; and, (d) Na2ATP. Insets: titration profiles at selected wavelengths vs equivalents of anion and species distribution diagram.

The titration profiles obtained with n class="Chemical">AMP, CMP, and UMP were satisfactory analyzed using a 1:1 binding model, providing the association constants listed in Table 3. In the case of PPi, ADP and ATP satisfactory fittings required an equilibrium model, including both 2:1 and 1:1 species ([CuLn]2+: Anion, n = 3, 4 or 5). The high resolution mass spectra recorded by electrospray ionization (ESI+) for solutions of [CuL4]2+ in the presence of one equivalent of PPi, ADP, or ATP show peaks due to the 2:1 and 1:1 entities (Table S1 and Figure S9, Supplementary Materials), which supports the model used for the determination of association constants. A similar situation was observed for phosphate, which also forms 2:1 and 1:1 complexes. The association constants obtained from the analysis of the titration curves are reported in Table 3. The anions containing a single phosphate unit (phosphate, AMP, CMP, and UMP) provide similar Log K11 values, which show that the nature of the nucleobase does not affect significantly the association constants. Thus, most likely the nucleobase is not participating significantly in the recognition process as observed for CMP and UMP in previous studies [28]. In the case of AMP, similar values of the stability constants were obtained for the corresponding adducts, so the formation of a macrochelate ring involving both the phosphate and the nitrogen N-7 of the adenosine moiety does not seem to take place. This could be related to the arrangement of the ligands around the Cu2+ ion in the complexes, which may block the effective approach of the nitrogen N-7 of adenosine to the inner sphere of the Cu2+ ion, thus inhibiting its coordination [29].

Table 3

Association constants (log K values) and pA values obtained from spectrophotometric titrations in aqueous solutions (pH 7, MOPS buffer). 1

		Phosphate	AMP	CMP	UMP	PPi	ADP	ATP
[CuL3]2+	Log K11	4.20(1)	4.35(1)	3.59(1)	4.02(1)	4.82(4)	4.02(1)	4.28(1)
	Log K21	-	-	-	-	4.14(5)	2.42(4)	3.00(4)
	pA	5.16	5.31	4.56	4.98	7.77	5.44	6.15
[CuL4]2+	Log K11	3.44(1)	3.80(1)	3.31(1)	2	2	6.83(9)	6.26(5)
	Log K21	1.72(7)	-	-			4.8(1)	4.32(6)
	pA	4.56	4.76	4.29			10.44	9.39
[CuL5]2+	Log K11	3.45(3)	3.31(3)	3.51(1)	3.00(1)	6.1(3)	4.89(2)	4.61(1)
	Log K21	3.67(7)	-	-	-	-	3.81(2)	3.41(3)
	pA	5.94	4.29	4.48	4.00	11.01	7.52	6.85

1 pA values defined as pA= −log[Anion]free, with [Anion] = 0.001 M and [(CuLn)2+] = 0.01 M (pH 7.0). 2 Precipitation during the titration prevented the determination of association constants.

The comparison of association constants obtained with different equilibrium models may be misleading. Thus, we used pA values defined as pA = −log[Anion]free using an anion concentration of 0.001 M and a concentration of [n class="Chemical">CuLn]2+ complex of 0.01 M (pH 7.0). The definition of pA is similar to that of pM often used to assess the relative stabilities of metal complexes in aqueous media [74]. The pA values obtained for all of the monophosphate anions are rather similar (Figure 5, see also Table 3), with no particular selectivity for any of them being observed. When considering the spectral changes that were displayed during the titrations, this suggests monodentate coordination of the phosphate anion to the metal center in the 1:1 complexes. The values obtained for the anions containing two or three phosphate units are clearly higher, particularly in the case of [CuL4]2+ and [CuL5]2+. This can be attributed, at least in part, to a bidentate coordination of the anion to the metal center, which for [CuL3]2+ and [CuL4]2+ triggers the de-coordination of the urea nitrogen atom. However, the nature of the receptor results in rather different stabilities. The pA values obtained for [CuL3]2+ and [CuL5]2+ show a similar trend, with the highest stability being observed for PPi. However, [CuL5]2+ shows higher pA values than [CuL3]2+, perhaps because of the more open structure of [CuL5]2+ related to the absence of the urea group. The high selectivity of [CuL5]2+ for PPi over ADP and ATP suggests that the cis-diol groups of the nucleotides are not forming esters with the phenylboronic acid moiety of the ligand.

Figure 5

pA values (pA= −log[Anion]free, with [Anion] = 0.001 M and [(CuLn)2+] = 0.01 M and pH 7.0) calculated for the association of [CuLn]2+ complexes (n = 3, 4 or 5) with phosphorylated anions with the equilibrium constants listed in Table 3.

Unfortunately, the addition of PPi to aqueous solutions of [n class="Chemical">CuL4]2+ caused the precipitation of the 2:1 aduct, which is subsequently redissolved upon addition of an excess of the anion. This prevented us from determining the corresponding association constants. Nevertheless, the pA values characterizing the association of [CuL4]2+ with ADP and ATP are clearly higher than those that were obtained for [CuL5]2+ and [CuL3]2+. We attribute this to the electron withdrawing effect of the –NO2 group of L4, which results in: (1) A weaker coordination of the urea group to the metal ions, so that it can be more easily displaced by anion coordination; and (2) A cooperative binding through coordination of the anion to the metal center and hydrogen-bonding interactions involving the urea NH donors and oxygen atoms of the anion (as evidenced in the X-ray structures shown in Figure 2). These interactions are likely weaker in the case of [CuL3]2+, and might be additionally hindered by the presence of the boronic group in position 2 with respect to the urea unit.

In the case of [pan class="Chemical">CuL3]2+ and [pan class="Chemical">ZnL3]2+ complexes, the high resolution mass spectra recorded in pan class="Chemical">dmso in the presence of one equivalent of AMP, ADP, and ATP show peaks due to 1:1 entities (Figure S10, Supplementary Materials). The position and isotopic profiles of the peaks indicate that the phenylboronic moiety has reacted with the cis-diol units present in the sugar ring of nucleotides in all cases. Similar measurements performed in aqueous solution did not evidence the formation of phenylboronic esters in the recognition of the nucleotides in this medium, suggesting that this cooperative interaction is not present in aqueous solution.

2.5. NMR Studies

The interaction of the [n class="Chemical">ZnL4]2+ complex with phosphorylated anions was investigated by using 1H-NMR spectroscopy in dmso-d6 solution, which was selected as solvent in view of the low solubility of the complex in aqueous media. The 1H-NMR signals of the urea protons were particularly informative with respect to the interaction of the anion with the complex (Figure 6). These signals are observed at 9.40 and 6.52 ppm in the spectrum of the [ZnL4]2+ complex, dissolved as the perchlorate salt. The addition of phosphate or AMP does not provoke significant changes in the chemical shifts of the urea protons. However, the signal at 9.40 ppm experiences important shifts to lower fields upon addition of one equivalent of PPi or ADP, shifting to 10.40 and 10.33 ppm, respectively. In parallel, the signal at 6.52 ppm undergoes smaller downfield shifts to 6.89 and 6.81 ppm, respectively. These spectral changes reflect the establishment of hydrogen-bonding interactions involving the urea fragment and the anion [75]. Interestingly, the addition of ATP provokes smaller shifts of the signals of urea protons to 9.53 and 6.88 ppm, which is in line with the lower pA value determined for the association of ATP and [CuL4]2+. A similar behavior is also observed for the [ZnL3]2+ complex, which contains a phenylboronic function (Figure S11, Supplementary Materials).

Figure 6

1H-NMR spectra (300 MHz, 298 K) recorded for the [ZnL4]2+ complex in the presence of different anions as their sodium salts in dmso-d6.

The corresponding pan class="Chemical">31P NMR spectrum of the pan class="Chemical">ATP adduct (Figure 7) shows three signals at −9.55, −20.92 and −9.05 ppm due to the Pα, Pβ, and Pγ nuclei, respectively. The corresponding chemical shifts measured for the uncoordinated pan class="Chemical">ATP anion are −10.90, −22.42, and −9.26 ppm. The small chemical shift induced by coordination in the signal of Pγ and the relatively large chemical shifts experienced by Pα and Pβ indicates that only the two inner phosphate groups of ATP play a significant role in the coordination to the metal ion. In the case of ADP coordination to the metal ion induces important upfield shifts of the signals of both Pα and Pβ, from −7.29 to −9.13 ppm (Pα) and from −5.56 to −7.46 ppm (Pβ). Taken together, these results indicate that both ADP and ATP coordinate to the metal ion through the phosphate units containing Pα and Pβ, likely in a similar way as observed in the solid state for [{ZnL4}2(μ-PPi)] and [{CuL4}2(μ-PPi)] (Figure 2). It is also worth noting that the spectrum recorded in the presence of ATP of PPi shows a small signal at 0 ppm due to the presence of phosphoric acid, indicating that the complex catalyzes the hydrolysis of the PPi anion and the triphosphate unit of ATP. In the case of [ZnL3]2+, similar 31P chemical shifts are observed, but the higher relative intensity of the signal at 0 ppm for polyphosphorylated anions indicates a higher extent of the hydrolysis process (Figure S12, Supplementary Materials).

Figure 7

31P NMR spectra (500 MHz, 298 K) recorded for [ZnL4]2+ complex in the presence of AMP, ADP, ATP and phosphate as their sodium salts in dmso-d6. The 31P NMR spectra of free metabolites are shown as colored traces.

The pan class="Chemical">31P NMR spectra recorded in the presence of pan class="Chemical">phosphate shows two very broad signals, which evidences the presence of different species in solution involved in dynamic processes. In the case of pan class="Chemical">AMP, the 31P NMR spectra show at least three signals for both [ZnL3]2+ and [ZnL4]2+ complexes, none of which coincides with that of free AMP, again suggesting the presence of several species in solution.

To check whether the structures in solution of [n class="Chemical">ZnL4(H2PPi)] and [{ZnL4}2(μ-PPi)] complexes correspond to those observed in solid state, the geometries of both monomeric and dimeric species were modeled by means of DFT calculations (TPSSh/SVP) in dmso solution (Figure S13, Supplementary Materials). In both cases, the possibility that the pyrophosphate anion was totally deprotonated or doubly protonated was considered, and the corresponding 31P NMR spectra of the four minimum energy geometries were calculated at the TPSSh/TZVP level (Table 4). The minimum energy geometry obtained for the [{ZnL4}2(μ-PPi)] species is in agreement with the one previously described in the solid state, where identical conformations of the ligands backbone (‘bent propeller’), coordination polyhedron around the Zn(II) metal ion (trigonal bipyramid), and intramolecular hydrogen-bonding interactions are present. In the case of the [ZnL4(H2PPi)] species, the obtained geometry differs considerably from that observed for the [CuL4(H2PPi)] complex in the solid state. The coordination polyhedron around the Zn2+ metal ion can be now best described as a square pyramid, with the ligand in an ‘open wing butterfly‘ conformation. Despite this, it is noticeable to remark that in both geometries the pyrophosphate anion is coordinated to the Zn(II) metal ions forming six-membered chelate rings in κ2-H2PPi2− or μ2κ4-PPi4− modes for [ZnL4(μ-PPi)] and [{ZnL4}2(μ-PPi)], respectively. Hydrogen bond interactions between the oxoanion and the urea moieties are observed in both cases.

Table 4

31P measured chemical shifts (dmso-d6) and calculated chemical shifts using the GIAO method at the TPSSh/TZVP level (see Computational Details) for [ZnL4(H2PPi)] and [{ZnL4}2(μ-PPi)] species (fully deprotonated and doubly protonated forms of the pyrophosphate anion were considered).

Species	δ (Experimental)	δ (Calculated)Deprotonated Form	δ (Calculated)Doubly Protonated Form
[{ZnL4}2(μ-PPi)]	−5.00	−5.90	−10.37
[ZnL4(H2PPi)]	−7.75	−72.15	−6.74

The comparison of the calpan class="Chemical">culated chemical shifts with the experimental values recorded in the presence of 0.5 or 1 equivalents of pan class="Chemical">pyrophosphate anion are in agreement with those calculated for a fully deprotonated form in the case of the [{ZnL4}2(μ-PPi)] dimeric complex, and with a doubly protonated form for the [ZnL4(H2PPi)] monomeric complex. The good agreement between experimental and calculated data suggests that both complexes adopt the calculated minimum energy geometries in solution.

3. Materials and Methods

3.1. General Methods

Elemental analyses were carried out on a ThermoQuest Flash EA 1112 elemental analyzer. ESI-TOF low resolution mass spectra (MS) were recorded from n class="Chemical">MeOH/MeCN/CHCl3, MeOH/MeCN, MeCN/CHCl3, or MeCN solutions, while the high resolution MS were recorded from MeCN/H2O or MeCN/dmso solutions, in both cases using a LC-Q-q-TOF Applied Biosystems QSTAR Elite spectrometer in the positive mode. IR spectra were recorded using a Bruker Vector 22 spectrophotometer equipped with a Golden Gate attenuated total reflectance (ATR) accessory (Specac). 1H, 13C and 31P NMR spectra were recorded at 25 °C on Bruker Avance 300 and Bruker Avance 500 spectrometers, and spectral assignments were based in part on 2D COSY, HSQC, and HMBC experiments. UV/vis spectra were recorded with a Perkin-Elmer Lambda 900 spectrophotometer. The spectra obtained from solutions were recorded with quartz cells (path length: 1 cm) and the cell holder was thermostatted at 25.0 °C, through circulating water. Anion binding studies were performed by monitoring the spectral changes of 10−3 M solutions of [CuL3](ClO4)2 or [CuL5](ClO4)2 complexes in H2O at pH 7.0 upon addition of a 0.1 M solution of the corresponding sodium salt containing a 10−3 M concentration of the corresponding complex at pH 7.0. For the [CuL4](ClO4)2 complex, the concentrations of the titration solutions and the solutions of the sodium salts were 5 × 10−3 M and 0.5 M, respectively. The pH was buffered with MOPS in all cases. Binding constants were obtained by using a simultaneous fit of the UV/vis absorption spectral changes at 7–12 selected wavelengths in the range 500–1200 nm. A minimum of 26 absorbance data points at each of these wavelengths was used, and all spectrophotometric titration curves were fitted with the HYPERQUAD 2008 (HypSpec) program [76].

Reagents

pan class="Chemical">(3-Aminophenyl)boronic acid (1), pan class="Chemical">3-tolylboronic acid (2), pan class="Chemical">2-bromoethanamine hydrobromide (11), ethane-1,2-diol, di-tert-butyl dicarbonate, bis(pyridin-2-ylmethyl)amine, 1-isocyanato-4-nitrobenzene, and 1-chloro-2-isocyanatoethane were obtained from commercial sources and used as received. Solvents were of reagent grade and used without further purification.

Although we have experienced no diffipan class="Chemical">culties with the pan class="Chemical">perchlorate salts, these should be regarded as potentially explosive and handled with care [77].

3.2. Synthesis

pan class="Chemical">3-(1,3,2-Dioxaborolan-2-yl)aniline (3). A solution of pan class="Chemical">(3-aminophenyl)boronic acid (1) (2.536 g, 16.04 mmol) and pan class="Chemical">ethane-1,2-diol (1.169 mL, 20.85 mmol) in acetonitrile (50 mL) was heated to reflux with stirring for 6 h. The solvent was removed by rotary evaporation and the resulting oil was dried under vacuum, after which it became a pale brown solid (3) that was used without further purification (2.605 g, 100%). δH (solvent CDCl3, 500 MHz, 298 K): 7.23–7.17 (m, 2H), 7.14 (m, 1H), 6.80 (ddd, 1H, 3J = 7.7 Hz, 4J = 2.6 Hz, 4J = 1.4 Hz), 4.35 (s, 4H), 3.49 (s, 2H). δC (solvent CDCl3, 125.8 MHz, 298 K): 145.8, 128.9, 125.2, 121.3, 118.4, 66.1. MS-ESI+, m/z (%BPI): [3 + H]+, 164.1 (47%). Elem. Anal. Calcd for C8H10BNO2: C, 59.0; H, 6.2; N, 8.6%. Found: C, 58.6; H, 6.3; N, 8.5%. IR: 3444, 3361, 3215 ν(N-H), 2981, 2910 ν(C-H), 1625, 1579, 1484, 1443 ν(C=C), 1338 ν(C-BO2), 1210 ν(O-B-O) cm−1.

pan class="Chemical">2-(3-Tolyl)-1,3,2-dioxaborolane (4). This compound was prepared by adapting the experimental procedure found in the literature [53]. A solution of n>n class="Chemical">3-tolylboronic acid (2) (1.829 g, 13.05 mmol) and ethane-1,2-diol (0.951 mL, 16.96 mmol) in pan class="Chemical">toluene (50 mL) was heated to reflux with stirring for 16 h using a Dean-Stark apparatus for water removal. The resulting solution was filtered while hot and the filtrate concentrated to dryness. The residue was purified by column chromatography on SiO2 with CH2Cl2 as the eluent to give pure product 4 as a pale yellow oil (1.691 g, 80%). δH (solvent CDCl3, 500 MHz, 298 K): 7.67 (s, 1H), 7.65 (m, 1H), 7.32–7.31 (m, 2H), 4.37 (s, 4H), 2.39 (s, 3H). δC (solvent CDCl3, 125.8 MHz, 298 K): 137.3, 135.6, 132.4, 131.9, 127.9, 66.1, 21.4. MS-ESI+, m/z (%BPI): [4 + H]+, 163.1 (38%). Elem. Anal. Calcd for C9H11BO2: C, 66.7; H, 6.8%. Found: C, 66.6; H, 6.8%. IR: 3023, 2974, 2908 ν(C-H), 1607, 1583, 1481 ν(C=C), 1335 ν(C-BO2), 1206 ν(O-B-O) cm−1.

pan class="Chemical">1-(3-(1,3,2-Dioxaborolan-2-yl)phenyl)-3-(2-(chloromethyl)phenyl)urea (5). A solution of compound 3 (1.400 g, 8.590 mmol) and pan class="Chemical">1-(chloromethyl)-2-isocyanatobenzene (1.184 mL, 8.590 mmol) in pan class="Chemical">diethyl ether (40 mL) was stirred at room temperature for 16 h. The precipitate formed was isolated by filtration and washed with diethyl ether (3 × 5 mL) to give 2.594 g of the desired compound (91%) as a white solid. δH (solvent dmso-d6, 500 MHz, 298 K): 9.38 (s), 9.20 (s), 8.25 (s), 8.21 (s), 7.88 (m), 7.69–7.64 (m), 7.61 (m), 7.43 (m), 7.34–7.31 (m), 7.27–7.19 (m), 7.06 (m), 4.85 (s), 4.35 (s), 4.32 (s), 3.39 (s). δC (solvent dmso-d6, 125.8 MHz, 298 K): 152.7, 139.4, 137.5, 130.6, 129.2, 128.5, 127.9, 127.6, 124.0, 123.1, 122.4, 121.1, 65.9, 65.7, 62.8, 43.5. MS-ESI+, m/z (%BPI): [5 + H]+, 331.1 (7%); [5 − PG + H]+, 305.1 (23%); [5 − Cl]+, 295.1 (9%); [5 − PG − Cl]+, 269.1 (85%). Elem. Anal. Calcd for C16H16BClN2O3: C, 58.1; H, 4.9; N, 8.5%. Found: C, 58.4; H, 4.9; N, 8.3%. IR: 3285 ν(N-H), 2979, 2912 ν(C-H), 1637 ν(C=O), 1606, 1586, 1489, 1477 ν(C=C), 1560 δ(N-H), 1335 ν(C-BO2), 1214 ν(O-B-O), 672 ν(C-Cl) cm−1.

pan class="Chemical">1-(3-(1,3,2-Dioxaborolan-2-yl)phenyl)-3-(2-chloroethyl)urea (7). A solution of compound 3 (1.400 g, 8.590 mmol) and pan class="Chemical">1-chloro-2-isocyanatoethane (0.755 mL, 8.590 mmol) in pan class="Chemical">diethyl ether (40 mL) was stirred at room temperature for 16 h. The precipitate formed was isolated by filtration and washed with diethyl ether (3 × 5 mL) to give 2.052 g of the desired compound (89%) as a white solid. δH (solvent dmso-d6, 500 MHz, 298 K): 8.70 (s, 1H), 7.76 (m, 1H), 7.55−7.52 (m, 1H), 7.27–7.25 (m, 2H), 6.39 (t, 1H, 3J = 5.7 Hz), 4.31 (s, 4H), 3.66 (t, 2H, 3J = 6.2 Hz), 3.42 (c, 2H, 3J = 6.0 Hz). δC (solvent dmso-d6, 125.8 MHz, 298 K): 155.1, 155.0, 139.9, 139.4, 128.4, 127.7, 127.4, 127.2, 123.8, 123.7, 120.9, 119.8, 65.6, 62.8, 44.5, 44.4, 41.2. MS-ESI+, m/z (%BPI): [7 + H]+, 269.1 (48%); [7 − PG + H]+, 243.1 (100%). Elem. Anal. Calcd for C11H14BClN2O3: C, 49.2; H, 5.3; N, 10.4%. Found: C, 49.3; H, 5.2; N, 10.4%. IR: 3329 ν(N-H), 2978, 2914 ν(C-H), 1629 ν(C=O), 1605, 1486, 1476 ν(C=C), 1564 δ(N-H), 1333 ν(C-BO2), 1214 ν(O-B-O), 614 ν(C-Cl) cm-1.

n class="Chemical">2-(3-(Bromomethyl)phenyl)-1,3,2-dioxaborolane (9). This compound was prepared by adapting the experimental procedure found in the literature [53]. A mixture of compound 4 (1.570 g, 9.693 mmol), NBS (1.830 g, 10.18 mmol) and PDB (0.056 g, 0.173 mmol) in CCl4 (40 mL) was heated to reflux with stirring for 16 h. The reaction mixture was allowed to cool to room temperature, the precipitated succinimide was removed by filtration and the filtrate was concentrated under reduced pressure. The residue was purified by column chromatography on SiO2 with CH2Cl2 as the eluent to give pure product 9 as a pale yellow oil (1.039 g, 45%). δH (solvent CDCl3, 500 MHz, 298 K): 7.84 (m, 1H), 7.74 (m, 1H), 7.51 (m, 1H), 7.37 (t, 1H, 3J = 7.5 Hz), 4.51 (s, 2H), 4.39 (m, 4H). δC (solvent CDCl3, 125.8 MHz, 298 K): 136.3, 135.5, 134.9, 132.3, 128.5, 66.2, 33.6. MS-ESI+, m/z (%BPI): [9 − Br]+, 161.1 (100%). Elem. Anal. Calcd for C9H10BBrO2: C, 44.9; H, 4.2%. Found: C, 45.0; H, 4.3%. IR: 2976, 2908 ν(C-H), 1605, 1583 ν(C=C), 1338 ν(C-BO2), 1216 ν(O-B-O), 602 ν(C-Br) cm−1.

pan class="Chemical">tert-Butyl-(2-bromoethyl)carbamate (12). This compound was prepared according to the literature procedure [78]. A suspension of compound 11 (2.500 g, 12.08 mmol) in 40 mL of n>n class="Chemical">dioxane was stirred at 0 °C for 30 min, and subsequently a solution of di-tert-butyl dicarbonate (2.663 g, 12.08 mmol) and pan class="Chemical">triethylamine (1.701 mL, 12.08 mmol) in 15 mL of dioxane was added slowly. The mixture was stirred at 0 °C for two hours, and at room temperature for two days. The solid formed was filtered and the filtrate concentrated to dryness. The resulting oil was dissolved in chloroform (50 mL) and washed with water (3 × 15 mL). The organic layer was dried over anhydrous sodium sulfate and the solvent removed by rotary evaporation. The residue was dried under vacuum for several hours to give 2.152 g (80%) of 12 as a pale yellow oil. δH (solvent CDCl3, 500 MHz, 298 K): 5.02 (s, 1H), 3.50 (m, 2H), 3.42 (m, 2H), 1.42 (s, 9H). δC (solvent CDCl3, 125.8 MHz, 298 K): 155.7, 79.9, 42.5, 32.8, 28.4. MS-ESI+, m/z (%BPI): [12 + Na]+, 246.0 (1%); [12 − Boc + H]+, 124.0 (68%). Elem. Anal. Calcd for C7H14BrNO2: C, 37.5; H, 6.3; N, 6.3%. Found: C, 37.1; H, 5.7; N, 6.8%. IR: 3336 ν(N-H), 2977, 2932 ν(C-H), 1689 ν(C=O), 1507 ν(N-H), 1162 νa(N-C) cm−1.

pan class="Chemical">tert-Butyl-(2-(bis(pyridin-2-ylmethyl)amino)ethyl)carbamate (13). A solution of compound 12 (2.030 g, 9.060 mmol), pan class="Chemical">bis(pyridin-2-ylmethyl)amine (1.528 mL, 8.237 mmol), pan class="Chemical">N,N-diisopropylethylamine (2.898 mL, 16.47 mmol) and a catalytic amount of KI in acetonitrile (100 mL) was heated to reflux with stirring for three days. The resulting solution was filtered while hot and the filtrate concentrated to dryness. The residue was extracted with chloroform (5 × 50 mL) and water (25 mL), the organic layers combined and dried over anhydrous sodium sulfate, and the solvent evaporated under reduced pressure. The resulting oil was purified on a CombiFlash RF-200, using a 48 g-neutral alumina column and CH2Cl2 as eluent to obtain pure product 13 as an orange oil which was dried under vacuum for several hours (1.092 g, 39%). δH (solvent CDCl3, 500 MHz, 298 K): 8.51 (m, 2H), 7.60 (m, 2H), 7.38 (d, 2H, 3J = 7.8 Hz), 7.12 (m, 2H), 5.80 (s, 1H), 3.83 (s, 4H), 3.20 (m, 2H), 2.67 (m, 2H), 1.41 (s, 9H). δC (solvent CDCl3, 125.8 MHz, 298 K): 159.3, 156.3, 149.2, 136.6, 123.2, 122.2, 78.8, 60.3, 53.7, 38.6, 28.6. MS-ESI+, m/z (%BPI): [13 + Na]+, 365.2 (100%); [13 + H]+, 343.2 (19%). Elem. Anal. Calcd for C19H26N4O2: C, 66.6; H, 7.7; N, 16.4%. Found: C, 66.3; H, 7.7; N: 15.6%. IR: 3315 ν(N-H), 3051–2821 ν(C-H), 1699 ν(C=O), 1590, 1569 ν(Py), 1520 ν(N-H), 1167 νa(N-C), 757 ν(C-H) cm−1.

N′,N′-Bis(pyridin-2-ylmethyl)ethane-1,2-dipan class="Chemical">amine (14). A solution of compound 13 (1.075 g, 3.139 mmol) and n>n class="Chemical">trifluoroacetic acid (10 mL, 129.3 mmol) in chloroform (10 mL) was stirred at room temperature for 16 h. The solvent was evaporated under reduced pressure and the residue was dissolved in chloroform (30 mL). The acid excess was neutralized with an aqueous solution of NaOH (1 M) and the organic layer washed with distilled water (2 × 15 mL). The organic phase was dried over anhydrous sodium sulfate and the solvent removed by rotary evaporation to give the pure product 14 as an orange oil that was dried under vacuum for several hours (0.727 g, 96%). δH (solvent CDCl3, 500 MHz, 298 K): 8.50 (m, 2H), 7.62 (m, 2H), 7.45 (d, 2H, 3J = 7.8 Hz), 7.12 (m, 2H), 3.82 (s, 4H), 2.77 (t, 2H, 3J = 6.1 Hz), 2.65 (t, 2H, 3J = 6.0 Hz), 2.06 (s, 2H). δC (solvent CDCl3, 125.8 MHz, 298 K): 159.7, 149.2, 136.5, 123.1, 122.1, 60.8, 57.4, 39.7. MS-ESI+, m/z (%BPI): [14 + H]+, 243.2 (100%). Elem. Anal. Calcd for C14H18N4: C, 69.4; H, 7.5; N, 23.1%. Found: C, 69.1; H, 6.9; N, 22.8%. IR: 3360 ν(N-H), 3054–2823 ν(C-H), 1589, 1568, 1473, 1432 ν(Py), 756 ν(C-H) cm−1.

pan class="Chemical">(3-(3-(2-((Bis(pyridin-2-ylmethyl)amino)methyl)phenyl)ureido)phenyl)boronic acid (L). A solution of compound 5 (1.150 g, 3.479 mmol), pan class="Chemical">bis(pyridin-2-ylmethyl)amine (0.587 mL, 3.163 mmol), pan class="Chemical">N,N-diisopropylethylamine (1.113 mL, 6.325 mmol) and a catalytic amount of KI in acetonitrile (50 mL) was heated to reflux with stirring for three days. The resulting solution was filtered while hot and the filtrate concentrated to dryness. The residue was extracted with chloroform (5 × 50 mL) and water (25 mL), the organic extracts combined and dried over anhydrous sodium sulfate, and the solvent evaporated under reduced pressure. The resulting oil was purified on a CombiFlash RF-200, using a 48 g-neutral alumina column and CHCl3/MeOH as eluent (from 0 to 3%; the desired product eluted from 2 to 3%) to obtain pure product L as a pale brown solid (0.607 g, 40%). δH (solvent dmso-d6, 500 MHz, 298 K): 10.30 (s, 1H, H14), 8.96 (s, 1H, H16), 8.50 (ddd, 2H, H1, 3J = 4.8 Hz, 4J = 1.7 Hz, 4J = 0.8 Hz), 8.03 (m, H12), 8.01 (s, H22), 7.77 (m, 1H, H23), 7.76–7.73 (m, H20), 7.71 (td, H3, 3J = 7.7 Hz, 4J = 1.8 Hz), 7.46 (m, 1H, H18), 7.40 (m, 2H, H4), 7.30 (t, 1H, H19, 3J = 7.7 Hz), 7.27–7.20 (m, 5H, H2, H9 and H11), 6.93 (td, 1H, H10, 3J = 7.4 Hz, 4J = 1.2 Hz), 3.80 (s, 4H, H6), 3.72 (s, 2H, H7). (See Figure S14 in Supplementary Materials for labelling scheme of the ligand). δC (solvent dmso-d6, 125.8 MHz, 298 K): 157.7 C5, 152.6 C15, 149.0 C1, 139.4 C13, 139.2 C17, 136.9 C3, 129.9 C9, 127.9 C19, 127.9 C18, 127.8 C11, 125.6 C8, 124.2 C23, 123.6 C4, 122.5 C2, 121.5 C10, 120.2 C20, 119.4 C12, 58.5 C6, 56.4 C7. MS-ESI+, m/z (%BPI): [L + H]+, 468.2 (100%). Elem. Anal. Calcd for C26H26BN5O3: C, 64.3; H, 5.8; N, 14.4%. Found: C, 64.5; H, 5.1; N: 14.6%. IR: 3290 ν(N-H/O-H), 3050–2830 ν(C-H), 1695 ν(C=O), 1593, 1571, 1477 ν(Ph/Py), 1538 ν(N-H), 1207 ν(O-B-O), 749 ν(C-H) cm−1.

pan class="Chemical">(3-(3-(2-(Bis(pyridin-2-ylmethyl)amino)ethyl)ureido)phenyl)boronic acid (L). A solution of compound 7 (0.350 g, 1.303 mmol), pan class="Chemical">bis(pyridin-2-ylmethyl)amine (0.220 mL, 1.185 mmol) and pan class="Chemical">N,N-diisopropylethylamine (0.417 mL, 2.370 mmol) in acetonitrile (30 mL) was heated to reflux with stirring for four days. The resulting solution was filtered while hot and the filtrate concentrated to dryness. The residue was extracted with chloroform (5 × 20 mL) and water (10 mL). During this process a brown solid insoluble in both phases was formed. This solid was filtered off, the organic extracts were combined, dried over anhydrous sodium sulfate and the solvent evaporated under reduced pressure. The resulting oil was purified on a CombiFlash RF-200, using an 8 g-neutral alumina column and CH2Cl2/MeOH as eluent (from 0 to 5%; the desired product eluted from 3 to 5%) to obtain pure product L as a pale yellow solid (0.113 g, 24%). δH (solvent dmso-d6, 500 MHz, 298 K): 8.55 (s, 1H, H11), 8.48 (m, 2H, H1), 7.96 (s, 2H, H17), 7.72 (td, 2H, H3, 3J = 7.7 Hz, 4J = 1.7 Hz), 7.60–7.56 (m, 4H, H4, H15 and H18), 7.33 (m, 1H, H13), 7.23 (m, 2H, H2), 7.18 (t, 1H, H14, 3J = 7.6 Hz), 6.15 (m, 1H, H9), 3.81 (s, 4H, H6), 3.25 (c, 2H, H8, 3J = 5.9 Hz), 2.59 (t, 2H, H7, 3J = 6.0 Hz). (See Figure S14 in Supplementary Materials for labelling scheme of the ligand). δC (solvent dmso-d6, 125.8 MHz, 298 K): 159.0 C5, 155.3 C10, 148.8 C1, 139.7 C12, 136.5 C3, 134.7 C16, 127.7 C14, 127.0 C13, 123.8 C15, 122.8 C4, 122.2 C2, 119.8 C18, 59.6 C6, 53.8 C7, 37.0 C8. MS-ESI+, m/z (%BPI): [L + H]+, 406.2 (100%). Elem. Anal. Calcd for C21H24BN5O3: C, 62.2; H, 6.0; N, 17.3%. Found: C, 61.9; H, 6.1; N: 17.7%. IR: 3303 ν(N-H/O-H), 3054–2849 ν(C-H), 1659 ν(C=O), 1593, 1477 ν(Ph/Py), 1551 ν(N-H), 1338 ν(C-BO2), 757 ν(C-H) cm−1.

pan class="Chemical">1-(2-(Bis(pyridin-2-ylmethyl)amino)ethyl)-3-(4-nitrophenyl)urea (L). A solution of compound 14 (0.713 g, 2.942 mmol) and pan class="Chemical">1-isocyanato-4-nitrobenzene (0.498 g, 2.942 mmol) in pan class="Chemical">chloroform (40 mL) was stirred at room temperature for two hours. The solvent was evaporated under reduced pressure and the residue was purified on a CombiFlash RF-200, using a 12 g-silica gel column and CHCl3/MeOH as eluent (from 0 to 4% of methanol; the desired compound eluted at 4%) to give L as a yellow oil that became a solid after remaining under vacuum for several days (1.014 g, 85%). δH (solvent CDCl3, 500 MHz, 298 K): 8.95 (s, 1H, H11), 8.46 (m, 2H, H1), 8.00 (m, 2H, H14), 7.56–7.51 (m, 4H, H3 and H13), 7.26 (d, H4, 3J = 7.8 Hz), 7.09 (m, 2H, H2), 6.99 (s, 1H, H9), 3.73 (s, 4H, H6), 3.26 (c, 2H, H8, 3J = 5.1 Hz), 2.61 (t, 2H, H7, 3J = 5.9 Hz). (See Figure S14 in Supplementary Materials for labelling scheme of the ligand). δC (solvent CDCl3, 125.8 MHz, 298 K): 158.1 C5, 155.3 C10, 149.1 C1, 146.7 C12, 141.3 C15, 136.9 C3, 125.1 C14, 123.9 C4, 122.5 C2, 117.2 C13, 60.0 C6, 53.0 C7, 37.3 C8. MS-ESI+, m/z (%BPI): [L + H]+, 407.2 (100%). Elem. Anal. Calcd for C21H22N6O3: C, 62.1; H, 5.5; N, 20.7. Found: C, 62.4; H, 5.3; N, 20.0%. IR: 3317 ν(N-H), 3078–2804 ν(C-H), 1643 ν(C=O), 1614, 1591, 1475, 1433 ν(Ph/Py), 1553 νa(NO2), 1328 νs(NO2), 749 ν(C-H) cm−1.

(pan class="Chemical">3-((Bis(pyridin-2-ylmethyl)amino)methyl)phenyl)boronic acid (L). A solution of compound 9 (0.310 g, 1.287 mmol), pan class="Chemical">bis(pyridin-2-ylmethyl)amine (0.217 mL, 1.170 mmol), pan class="Chemical">N,N-diisopropylethylamine (0.412 mL, 2.340 mmol) and a catalytic amount of KI in acetonitrile (50 mL) was heated to reflux with stirring for 16 h. The resulting solution was filtered while hot and the filtrate concentrated to dryness. The residue was extracted with chloroform (5 × 25 mL) and water (15 mL), the organic layers combined and dried over anhidrous sodium sulfate, and the solvent evaporated under reduced pressure. The resulting oil was purified on a CombiFlash RF-200, using a 48 g-neutral alumina column and CH2Cl2/MeOH as eluent (from 0 to 5%; the desired product eluted from 4% to 5%) to obtain pure product L as a pale yellow solid (0.165 g, 42%). δH (solvent dmso-d6, 500 MHz, 298 K): 8.48 (ddd, 2H, H1, 3J = 4.8 Hz, 4J = 1.8 Hz, 4J = 0.8 Hz), 8.04 (s, 2H, H13), 7.80 (m, H14), 7.77 (td, H3, 3J = 7.7 Hz, 4J = 1.8 Hz), 7.67 (m, 1H, H11), 7.59 (m, 2H, H4), 7.47 (m, 1H, H9), 7.31 (t, 1H, H10, 3J = 7.5 Hz), 7.24 (m, 2H, H2), 3.70 (s, 4H, H6), 3.62 (s, 2H, H7). (See Figure S14 in Supplementary Materials for labelling scheme of the ligand). δC (solvent dmso-d6, 125.8 MHz, 298 K): 159.2 C5, 148.8 C1, 137.5 C8, 136.6 C3, 134.6 C14, 134.1 C12, 132.9 C11, 130.4 C9, 127.4 C10, 122.5 C4, 122.2 C2, 59.1 C6, 57.9 C7. MS-ESI+, m/z (%BPI): [L + Na]+, 356.2 (67%); [L + H]+, 334.2 (100%). Elem. Anal. Calcd for C19H20BN3O2: C, 68.5; H, 6.1; N, 12.6%. Found: C, 68.2; H, 6.0; N: 11.0%. IR: 3049–2850 ν(C-H), 1593, 1571, 1475 ν(Ph/Py), 1362 ν(C-BO2), 758 ν(C-H) cm−1.

General procedure for the preparation of [ML A solution of hydrated pan class="Chemical">Cu(ClO4)2 or pan class="Chemical">Zn(ClO4)2 (0.103 mmol) in THF (2 mL) was added to a solution of L (0.050 g, 0.103 mmol) in the same solvent (5 mL). The mixture was stirred at room temperature for an hour and the solvent was removed under reduced pressure. The solid was treated with diethyl ether (5 mL), filtrated and dried under vacuum.

[pan class="Chemical">CuL ([pan class="Gene">CuL1](pan class="Chemical">ClO4)2). Dark green solid. Yield: 0.077 g, 96%. MS-ESI+, m/z (%BPI): [CuL1(ClO4)]+, 629.1 (3%); [Cu(L1-H)]+, 529.1 (41%). Elem. Anal. Calcd for C26H26BCl2CuN5O11·H2O: C, 41.8; H, 3.8; N, 9.4%. Found: C, 42.1; H, 3.8; N, 9.1%. ΛM (MeOH, 10−3 M, 25 °C): 154.9 cm2·Ω−1·mol−1 (2:1 electrolyte). IR: 3358 ν(N-H/O-H), 1651 ν(C=O), 1614 ν(Ph/Py), 1549 ν(N-H), 1345 ν(C-BO2), 1053 νa(Cl-O), 619 νa(O-Cl-O) cm−1. UV/vis diffuse reflectance spectroscopy: 633 nm.

[pan class="Chemical">ZnL (pan class="Chemical">[ZnL1](ClO4)2). Light brown solid. Yield: 0.073 g, 97%. MS-ESI+, m/z (%pan class="Gene">BPI): [ZnL1(ClO4)]+, 630.1 (4%); [Zn(L1-H)]+, 530.1 (100%); [ZnL1]2+, 265.6 (71%). Elem. Anal. Calcd for C26H26BCl2N5O11Zn: C, 42.7; H, 3.6; N, 9.6%. Found: C, 42.6; H, 3.7; N: 9.3%. ΛM (MeOH, 10−3 M, 25 °C): 164.0 cm2·Ω−1·mol−1 (2:1 electrolyte). IR: 3354 ν(N-H/O-H), 1612 ν(Ph/Py), 1559 ν(N-H), 1343 ν(C-BO2), 1055 νa(Cl-O), 620 νa(O-Cl-O) cm−1. δH (solvent dmso-d6, 500 MHz, 298 K): 8.60 (m, 2H), 8.42 (s, 1H), 8.15 (s, 1H), 8.01 (s), 7.97 (m), 7.60–7.55 (m, 5H), 7.49–7.35 (m, 6H), 7.22 (m, 1H), 4.22 (d, 2H, H6A, 2J = 16.0 Hz), 3.82 (s, 2H), 3.67 (d, 2H, H6B, 2J = 16.0 Hz). δC (solvent dmso-d6, 125.8 MHz, 298 K): 154.4, 153.6, 147.6, 140.5, 138.6, 138.5, 134.8, 133.3, 129.4, 128.3, 127.9, 127.8, 127.5, 125.7, 124.9, 124.7, 124.4, 120.4, 55.4, 51.7.

General procedure for the preparation of [ML A solution of hydrated pan class="Chemical">Cu(ClO4)2 or pan class="Chemical">Zn(ClO4)2 (0.123 mmol) in acetonitrile (2 mL) was added to a solution of L3 (0.050 g, 0.123 mmol) in the same solvent (5 mL). The mixture was stirred at room temperature for 16 h and the solvent was removed under reduced pressure. The solid was treated with diethyl ether (5 mL), filtered, and dried under vacuum.

[pan class="Chemical">CuL (pan class="Chemical">[CuL3](ClO4)2). Dark green solid. Yield: 0.052 g, 59%. MS-ESI+, m/z (%pan class="Gene">BPI): [CuL3(ClO4)]+, 567.1 (16%); [Cu(L3-H)]+, 467.1 (8%); [CuL3]2+, 234.1 (100%). Elem. Anal. Calcd for C21H24BCl2CuN5O11·2H2O: C, 35.8; H, 4.0; N, 10.0%. Found: C, 35.7; H, 3.6; N, 10.1%. ΛM (MeOH, 10−3 M, 25 °C): 170.2 cm2·Ω−1·mol−1 (2:1 electrolyte). IR: 3364 ν(N-H/O-H), 1613 ν(Ph/Py), 1556 ν(N-H), 1341 ν(C-BO2), 1052 νa(Cl-O), 619 νa(O-Cl-O) cm−1. UV/vis diffuse reflectance spectroscopy: 585 nm.

[pan class="Chemical">ZnL (pan class="Chemical">[ZnL3](ClO4)2). Light brown solid. Yield: 0.041 g, 49%. MS-ESI+, m/z (%pan class="Gene">BPI): [Zn(L3-H)(OMe)]+, 482.1 (2%); [ZnL3(OMe)]2+, 241.6 (100%). Elem. Anal. Calcd for C21H24BCl2N5O11Zn·H2O: C, 36.7; H, 3.8; N, 10.2%. Found: C, 36.5; H, 4.0; N: 9.8%. ΛM (MeOH, 10−3 M, 25 °C): 167.2 cm2·Ω−1·mol−1 (2:1 electrolyte). IR: 3363 ν(N-H/O-H), 1612 ν(Ph/Py), 1565 ν(N-H), 1341 ν(C-BO2), 1054 νa(Cl-O), 619 νa(O-Cl-O) cm−1. δH (solvent dmso-d6, 300 MHz, 298 K): 8.60 (m), 8.52 (s), 8.08 (m), 7.95 (s), 7.62–7.49 (m, 6H), 7.37 (m, 1H), 7.20 (m, 1H), 6.24 (s, 1H), 4.37 (d, H6A, 2J = 16.0 Hz), 4.05 (d, H6B, 2J = 16.0 Hz), 3.60 (m), 2.83 (m). δC (solvent dmso-d6, 75.5 MHz, 298 K): 155.7, 154.6, 147.6, 140.6, 139.2, 134.8, 127.8, 127.5, 124.7, 124.5, 124.3, 120.3, 57.2, 54.9, 34.7.

General procedure for the preparation of [ML A solution of hydrated pan class="Chemical">Cu(ClO4)2, pan class="Chemical">Zn(ClO4)2 or Cu(SO4) (0.123 mmol) in methanol (2 mL) was added to a solution of L (0.050 g, 0.123 mmol) in the same solvent (5 mL). The mixture was stirred at room temperature for 16 h, and the precipitate formed was isolated by filtration, washed with methanol (2 mL) and diethyl ether (2 mL), and dried under vacuum. For the Zn2+ complex no precipitate was obtained, so the solvent was evaporated under reduced pressure and chloroform (5 mL) was added. The precipitate formed was stirred at room temperature for 16 h, filtered, washed with 5 mL of chloroform and 5 mL of diethyl ether, and dried under vacuum.

[pan class="Chemical">CuL (pan class="Chemical">[CuL4](ClO4)2). Light blue solid. Yield: 0.075 g, 86%. MS-ESI+, m/z (%pan class="Gene">BPI): [CuL4(ClO4)]+, 568.0 (83%); [Cu(L4-H)]+, 468.1 (22%); [CuL4]2+, 234.6 (100%). Elem. Anal. Calcd for C21H22Cl2CuN6O11·2H2O: C, 35.8; H, 3.7; N, 11.9%. Found: C, 35.9; H, 3.4; N, 11.5%. ΛM (MeOH, 10−3 M, 25 °C): 144.5 cm2·Ω−1·mol−1. IR: 3584, 3410, 3342 ν(N-H), 3089–2780 ν(C-H), 1697 ν(C=O), 1613, 1597 ν(Ph/Py), 1550 ν(N-H), 1504 νa(NO2), 1334 νs(NO2), 1093, 1061 νa(Cl-O), 620 νa(O-Cl-O) cm−1. UV/vis diffuse reflectance spectroscopy: 633 nm.

[pan class="Chemical">CuL ([pan class="Chemical">CuL4(SO4)]). Light blue solid. Yield: 0.047 g, 64%. MS-ESI+, m/z (%pan class="Gene">BPI): [Cu(L4+H)(SO4)]+, 566.1 (20%); [Cu(L4-H)]+, 468.1 (3%); [CuL4]2+, 234.6 (52%). Elem. Anal. Calcd for C21H22CuN6O7S·1.5H2O: C, 42.5; H, 4.3; N, 14.2%. Found: C, 42.7; H, 3.9; N, 13.9%. ΛM (MeOH, 10−3 M, 25 °C): the low solubility of this complex in methanol has prevented us from determining the conductivity value for this compound. IR: 3254 ν(N-H), 3117–2943 ν(C-H), 1692 ν(C=O), 1612, 1595 ν(Ph/Py), 1562 ν(N-H), 1502 νa(NO2), 1324 νs(NO2), 1106, 1049, 1029 νa(S-O), 600, 584 νa(O-S-O) cm−1. UV/vis diffuse reflectance spectroscopy: 706 nm. Slow evaporation of a solution of the complex in a dimethylformamide/water mixture provided dark blue single crystals suitable for X-ray diffraction analysis.

[pan class="Chemical">ZnL (pan class="Chemical">[ZnL4](ClO4)2). Light yellow solid. Yield 0.092 g, 95%. MS-ESI+, m/z (%pan class="Gene">BPI): [ZnL4(ClO4)]+, 569.1 (74%); [Zn(L4-H)]+, 469.1 (100%); [ZnL4]2+, 235.1 (83%). Elem. Anal. Calcd for C21H22Cl2N6O11Zn·CHCl3: C, 33.4; H, 2.9; N, 10.6%. Found: C, 33.8; H, 3.1; N: 10.7%. ΛM (MeOH, 10−3 M, 25 °C): 161.9 cm2·Ω−1·mol−1 (2:1 electrolyte). IR: 3372 ν(N-H), 1647 ν(C=O), 1614 ν(Ph/Py), 1556 ν(N-H), 1506 νa(NO2), 1329 νs(NO2), 1094, 1051 νa(Cl-O), 619 νa(O-Cl-O) cm−1. δH (solvent dmso-d6, 300 MHz, 298 K): 9.39 (s, 1H, H11), 8.61 (m, 2H), 8.16–8.06 (m, 4H), 7.63–7.57 (m, 6H), 6.52 (m, 1H, H9), 4.38 (d, 2H, H6A, 2J = 16.0 Hz), 4.06 (d, 2H, H6B, 2J = 16.0 Hz), 3.45 (m), 2.82 (m, 2H). δC (solvent dmso-d6, 75.5 MHz, 298 K): 154.6, 154.5, 147.5, 146.9, 140.6, 125.1, 124.7, 124.4, 117.0, 56.8, 54.0, 34.5.

Procedure for the preparation of [pan class="Chemical">CuL A solution of hydrated pan class="Chemical">Cu(ClO4)2 (0.150 mmol) in acetonitrile (2 mL) was added to a solution of L5 (0.050 g, 0.150 mmol) in acetonitrile (5 mL). The mixture was stirred at room temperature for 16 h and the solvent was removed under reduced pressure. The solid was treated with diethyl ether (5 mL), filtrated and dried under vacuum.

[pan class="Chemical">CuL (pan class="Chemical">[CuL5](ClO4)2). Dark blue solid. Yield: 0.075 g, 82%. MS-ESI+, m/z (%pan class="Gene">BPI): [CuL5(ClO4)]+, 495.1 (70%); [Cu(L5-H)]+, 395.1 (100%). Elem. Anal. Calcd for C19H20BCl2CuN3O10·H2O: C, 37.2; H, 3.6; N, 6.9%. Found: C, 37.4; H, 3.8; N, 7.1%. ΛM (MeOH, 10−3 M, 25 °C): 171.3 cm2·Ω−1·mol−1 (2:1 electrolyte). IR: 3441 ν(O-H), 1613, 1576, 1487 ν(Ph/Py), 1346 ν(C-BO2), 1048 νa(Cl-O), 619 νa(O-Cl-O) cm−1. UV/vis diffuse reflectance spectroscopy: 603 nm.

3.3. X-ray Diffraction Studies

Crystals of [pan class="Chemical">CuL4(SO4)] were obtained by evaporation of a solution of the isolated complex, as described above. Crystals of [pan class="Chemical">CuL4(H2PPi)] were grown by slow evaporation of an pan class="Chemical">acetonitrile–methanol (1:1) mixture containing stoichiometric amounts of [CuL4](ClO4)2 and sodium pyrophosphate. Finally, [{CuL4}2(μ-PPi)] and [{ZnL4}2(μ-PPi)] were crystallized by slow evaporation of solutions of [CuL4](ClO4)2 (acetonitrile-methanol mixture) or [ZnL4](ClO4)2 (deuterium oxide) in the presence of 0.5 equiv. of sodium pyrophosphate.

Three-dimensional X-ray data were collected on Bruker X8 APEXII pan class="Disease">CCD (pan class="Chemical">[{ZnL4}2(µ-PPi)], [pan class="Chemical">{CuL4}2(µ-PPi)] and [CuL4(H2PPi)]) or BRUKER-NONIUS X8 APEX CCD ([CuL4(SO4)]) diffractometers. The data of [{CuL4}2(µ-PPi)], [CuL4(H2PPi)]) and [CuL4(SO4)] were corrected for Lorentz and polarization effects and for absorption by semiempirical methods based on symmetry-equivalent reflections [79]. The crystal selected for [{ZnL4}2(µ-PPi)] was a twin, so that the correction for absorption was made with TWINABS [80]. Two domains were found and two corrected hkl files were generated, one for solving the structure (HKLF 4) and another for the final refinement (HKLF 5). Complex scattering factors were taken from the program SHELX-2017 running under the WinGX program system as implemented on a Pentium® computer [81,82]. The structures were solved by using the charge-flipping method with Superflip [83] (for complex [{ZnL4}2(µ-PPi)] or Patterson methods with DIRDIF2008 [84] (for [{CuL4}2(µ-PPi)], [CuL4(H2PPi)] and [CuL4(SO4)]). All of the structures were refined by full-matrix least-squares on F2 (SHELXL-2017) [85]. Hydrogen atoms were included in calculated positions and refined in riding mode for all of the compounds with the following exceptions: hydrogen atoms of urea NH moieties were refined freely in the final stages of refinement and hydrogen atoms of water molecules (one molecule per unit cell in [CuL4(H2PPi)] and six molecules per unit cell in crystals of [{ZnL4}2(µ-PPi)]) were located in a difference electron-density map and the H⋯H and O-H distances restrained.

In the final steps of refinement of the crystal structure of n class="Chemical">[{ZnL4}2(µ-PPi)], the data were cleaned up with SQUEEZE [86] to avoid the problems generated by disordered methanol and acetonitrile molecules in two voids with volumes of 255 and 115 Å3 and electron counts of 82 and 35, respectively, which agree with the presence of two acetonitrile and one methanol molecule, respectively.

Finally, refinement converged with anisotropic displacement parameters for all non-pan class="Chemical">hydrogen atoms for all four structures. Crystal data and details on data collection and refinement are summarized in Table 5.

Table 5

Crystal data and refinement details.

	[CuL4(SO4)]	[CuL4(H2PPi)]	[{CuL4}2(μ-PPi)]	[{ZnL4}2(μ-PPi)]
formula	C21H22CuN6O7S	C23H29CuN7O11P2	C42H44Cu2N12O13P2	C42H56N12O19P2Zn
MW	566.04	705.01	1113.91	1225.66
crystal system	orthorhombic	triclinic	triclinic	monoclinic
space group	Pbca	P −1	P −1	P 21/n
T/K	100(2)	100(2)	100(2)	100(2)
a/Å	19.636(3)	7.606(2)	13.5195(9)	10.2371(6)
b/Å	8.913(1)	11.984(3)	13.6036(9)	17.6978(10)
c/Å	25.692(3)	17.360(4)	14.5281(10)	28.5263(16)
α/deg	90	106.18(1)	76.346(4)	90
β/deg	90	95.12(1)	79.212(5)	95.104(3)
γ/deg	90	105.26(1)	76.738(4)	90
V/Å3	4496.30(10)	1443.5(6)	2502.0(3)	5147.7(5)
F(000)	2328	726	1144	2536
Z	8	2	2	4
λ, Å (Mo Kα)	0.71073	0.71073	0.71073	0.71073
Dcalc/g·cm−3	1.672	1.622	1.479	1.581
μ/mm−1	1.123	0.939	0.987	1.081
θ range/deg	2.969–25.149	1.855–30.706	1.457–26.389	1.356–26.391
Rint	0.0943	0.0424	0.0391	0.1223 c
reflns obsd	4016	8880	10203	13103
GOF on F2	1.051	1.013	1.023	1.011
R1 a	0.038	0.0300	0.0320	0.0768
wR2 (all data) b	0.0980	0.0746	0.0765	0.1789
Largest diff. peak and hole/e Å−3	0.464 and −0.533	0.532 and −0.366	0.397 and −0.434	0.959 and −1.946

a R1 = Σ||Fo| − |Fc||/Σ|Fo|. b wR2 (all data) = {Σ[w(||Fo|2 − |Fc|2)2]/Σ[w(Fo4)]}1/2. c Rint is based on agreement between observed single and composite intensities and those calculated from refined unique intensities and twin fractions for all 64,393 observations.

3.4. Computational Details

All of the calpan class="Chemical">culations presented in this work were performed employing the Gaussian 09 package (Revision B.01) [87]. Full geometry optimizations of [n>n class="Chemical">ZnL4(H2PPi)] and [{ZnL4}2(μ-PPi)] complexes were carried out in pan class="Chemical">dmso solution employing DFT within the hybrid meta-GGA approximation with the TPSSh exchange-correlation functional [88]. Input geometries were generated from the crystallographic data of [CuL4(H2PPi)] and [{ZnL4}2(μ-PPi)] by replacing the Cu(II) metal ion in the first one. For geometry optimization purposes we used the standard Ahlrichs’ valence double-ξ basis set including polarization functions (SVP) [89]. No symmetry constraints have been imposed during the optimizations. The stationary points found on the potential energy surfaces as a result of geometry optimizations were tested to represent energy minima rather than saddle points via frequency analysis. The default values for the integration grid (75 radial shells and 302 angular points) and the SCF energy convergence criteria (10−8 a.u.) were used in all the calculations. The 31P NMR shielding tensors were calculated using the GIAO [90] method at the TPSSh/TZVP [91] level. The isotropic shielding constants (σ) were converted to chemical shifts with respect to 85% aqueous H3PO4 by using the following expression [92,93]:δ

The shielding tensors of PH3 were calpan class="Chemical">culated at the same computational level.

Throughout this work solvent effects (pan class="Chemical">dmso) were included by using the polarizable continuum model (PCM), in which the solute cavity is built as an envelope of spheres centered on atoms or atomic groups with appropriate radii. In partipan class="Chemical">cular, we used the integral equation formalism (IEFPCM) variant as implemented in Gaussian 09 [94].

4. Conclusions

We have presented a series of pan class="Chemical">Cu2+ and pan class="Chemical">Zn2+ complexes containing pan class="Chemical">dipicolylamine units for metal ion coordination and urea groups. In the absence of phosphorylated anions, the urea group coordinates to the metal ion through one of the nitrogen atoms. Addition of monophosphate anions does not provoke the decoordination of the urea group, while the addition of PPi, ADP, or ATP causes decoordination of the urea group and a change of the coordination environment from distorted octahedral to trigonal bipyramidal. The coordination of the PPi and ADP anions to the metal ion appears to be reinforced by the presence of hydrogen bonds with the urea unit, as also observed in the solid state, while these interactions seem to be weaker in the case of ATP. The [CuL4]2+ and [CuL5]2+ complexes show important selectivities towards PPi, ADP, and ATP over anions containing a single phosphate group. The results indicate that the cooperative binding is established for the complexes derived from L4 during the anion recognition and that it is necessary to consider the N-type coordination mode of the urea moiety to prevent the receptor hydrolysis when designing urea based receptors with different delocalized withdrawing groups in their backbones.