EXAFS Study on the Coordination Chemistry of the Solvated Copper(II) Ion in a Series of Oxygen Donor Solvents.

The structures of the solvated copper(II) ion in water and nine organic oxygen donor solvents with similar electron-pair donor ability, but with different space-demanding properties at coordination, have been studied by EXAFS. N,N'-Dimethylpropyleneurea and N,N,N',N'-tetramethylurea are sufficiently space demanding at coordination to make the axial positions not accessible, resulting in square-planar copper(II) solvate complexes with an intense green color. The mean Cu-O bond distances in these two solvate complexes are 1.939(3) and 1.935(3) Å, respectively. The best fits of the remaining solvates, which are light blue in different hues, are obtained with a Jahn-Teller distorted-octahedral model consisting of four strongly bound solvent molecules in the equatorial positions at 1.96(2) Å and two in the axial positions but with different Cu-Oax bond distances: ca. 2.15 and 2.32 Å. This is in agreement with observations in solid-state structures of compounds containing hexaaquacopper(II) complexes crystallizing in noncentrosymmetric space groups and all reported crystal structures containing a [Cu(H2O)5(O-ligand)] complex with Jahn-Teller distortion. Such a structure is in agreement with previous EPR and EXAFS studies proving the hydrated copper(II) ion to be a noncentrosymmetric complex in aqueous solution. The refinements of the EXAFS data of the solids [Cu(H2O)6](ClO4)2, [Cu(H2O)6](BrO3)2, [Cu(H2O)6]SiF6, Cu(NO3)2·2.5H2O, and CuSO4·5H2O gave Cu-O bond distances significantly different from those reported in the crystallographic studies but similar to the configuration and bond distances in the hydrated copper(II) ion in aqueous solution. This may depend on whether the orientation of the axial positions is random in one or three dimensions, giving a mean structure of the solid with symmetry higher than that of the individual complexes. This study presents the very first experimental data from the new X-ray absorption spectroscopy beamline Balder at the MAX IV synchrotron radiation facility in Lund, Sweden, as well as the utilized properties of the beamline.

Introduction

The most debated hydrated metal ion by fn class="Chemical">ar in recent years is copper(II). It was assumed for a long time that the hydrated copper(II) ion is six-coordinate with a tetragonally elongated octahedral configuration along a 4-fold axis, known as Jahn–Teller distortion,[1−3] in aqueous solution. It can be concluded that a majority of the solid compounds containing a hydrated copper(II) ion have this configuration[4,5] (Table S1). This has led many to believe that the same structure is also present in aqueous solution, even though a structure of a metal complex in the solid state cannot be related to its structure in solution.[6] Linear electric field EPR studies gave the first indications that the hydrated copper(II) ion in aqueous solution was not centrosymmetric, as required by a regular Jahn–Teller distorted octahedron.[7,8] A combined neutron scattering and molecular dynamics study proposed that the hydrated copper(II) ion is five-coordinate in aqueous solution.[9] This study was followed a by series of publications using EXAFS and XANES spectroscopy, X-ray and neutron scattering on liquids, and DFT and QM/MD simulations on different levels to study the coordination chemistry of the hydrated copper(II) ion in aqueous solution.[10−25] A majority of these studies propose a tetragonally elongated square-pyramidal configuration as the most likely or stable structure,[9,10,13,15,16,25] but several studies have proposed dynamic equilibria among four-, five-, and/or six-coordinated hydrate complexes,[14,19,20,22,23] as well as a six-coordinate Jahn–Teller distorted-octahedral configuration.[11,12,18,21] This shows that the discussion of the structure of the hydrated copper(II) ion aqueous solution is still a matter of debate.

The most extensive experimental studies have been performed by Frank and co-workers, who in a series of studies have applied n class="Chemical">XANES and high-k EXAFS spectroscopy on both aqueous solutions and frozen samples of the hydrated copper(II) ion.[13,22,25] They have applied three basic models: five-coordination in a tetragonally elongated square-pyramidal configuration and six-coordination in Jahn–Teller distorted-octahedral configurations with equal (centrosymmetric) and different Cu–O bond distances in the axial positions (noncentrosymmetric). The EXAFS data of an aqueous copper(II) solution were fitted equally well with square-pyramidal and noncentrosymmetric Jahn–Teller distorted-octahedral models, with Cu–O bond distances of 1.97 and 2.21 Å and of 1.97, 2.19, and 2.33 Å, respectively.[22] On the other hand, in the refinement of XANES data using the MXAN program, the best fit was obtained with a square-pyramidal model with Cu–O bond distances of 1.95 and 2.23 Å.[22] Studies on frozen samples of 1,3-propanediol and 1,5-pentanediol aqueous glasses revealed asymmetric six-coordination with Cu–Oeq, Cu–Oax1, and Cu–Oax2 bond distances of 4 × 1.94, 2.22, and 2.34 Å, respectively, from EXAFS data, while MXAN data revealed copper sites with two kinds of six-coordination, asymmetric Jahn–Teller distorted-octahedral (4 × 1.94, 1 × 2.14, and 2.28 Å) and capped-square-pyramidal configurations (5 × 1.94 and 2.22 Å), and five-coordinated sites in a square-pyramidal configuration (4 × 1.95 and 2.23 Å).[25] D’Angelo and co-workers have studied the solvated copper(II) ion methanol, dimethyl sulfoxide and acetontrile solution by combined XANES and EXAFS, showing that tetragonally elongated square-pyramidal coordination is preferred in these solvents.[26,27]

It is important to emphasize that techniques such as n class="Chemical">EXAFS and XANES spectroscopy cannot give an absolute answer about the structure, as several models may fit the experimental data equally or almost equally well and the starting model may affect the outcome of the refinement. It is therefore important to test as many reasonable structure models as possible. Calculations have shown that the energy barrier between centrosymmetric Jahn–Teller distorted [Cu(H2O)4(H2O)2]2+ and noncentrosymmetric [Cu(H2O)4(H2O)(H2O)]2+ is small, −82 meV (−7.95 kJ mol–1).[17] Independent QMCF/MD molecular dynamics calculations did observe this delicate energy balance, resulting in a mean equilibrium geometry with Cu–O bond distances of 4 × 2.03, 2.15, and 2.30 Å and 4 × 2.07 and 2 × 2.2 Å including and excluding the second hydration shell into the QM zone, respectively, and a B3LYP/MM simulation, 4 × 2.02 and 2 × 2.29 Å.[11,12]

In order to give another perspective on this debate, a survey and analysis of reported solid-state structures containing four-, five-, and n class="Chemical">six-coordinate copper(II) hydrates and other copper(II) complexes with oxygen donor ligands are presented in this study. Of these structures, a large majority have a Jahn–Teller distorted-octahedral geometry around copper(II). Of the 139 reported crystal structures containing a [Cu(H2O)6]2+ ion, 105 report a regular Jahn–Teller distorted configuration with pairwise equal Cu–O bond distances due to symmetry rules of the space groups. The mean Cu–Oeq and Cu–Oax bond distances in these structures are 1.981 and 2.332 Å, respectively (Table S1). Two structures containing a [Cu(H2O)6]2+ ion crystallize in a centrosymmetric space group, but the copper in the [Cu(H2O)6]2+ ion is not in the center of symmetry,[28,29] and another five structures crystallize in noncentrosymmetric space groups.[30−33] In these seven structures the axial Cu–O bond distances are significantly different with mean distances of 2.298 and 2.362 Å (Table S1). A limited number of the hexaaquacopper(II) complexes are reported to have regular or slightly irregular octahedral configurations: 7 and 21, respectively (Table S1).

To further check whether there are more examples showing a significant difference in the Cu–Oax bond distances, crystal structures containing complexes with the composition [Cu(H2O)5O′], where O′ is a monodentate oxygen donor ligand, with reported Jahn–Teller distortion were summarized, as such complexes cannot individually be centrosymmetric. Indeed, all of these structures display significantly different Cu–Oax bond distances (Table S2), and they all have similar Cu–O bond distances in the equatorial positions independent of whether the O′ ligand binds in an equatorial or an axial position. Four of these structures have water molecules in the axial positions, and the difference in Cu–Oax bond distance is 0.07–0.43 Å, and a similar pattern is seen in the compounds with the O′ ligand in the axial position (Table S2).

A possible reason as to why a majority of the structures with n class="Chemical">hexaaquacopper(II) ions crystallize in centrosymmetric space groups is that the direction of possibly different Cu–Oax bond distances is randomly distributed in the structure. The mean structure, from a crystallographic point of view, becomes centrosymmetric with identical Cu–Oax bond distances. This is certainly also the case for the 28 crystal structures reporting an apparent regular or a slightly distorted octahedral [Cu(H2O)6]2+ complex, but here the random orientation of the axial positions is distributed in three dimensions (Table S1). When the orientation of the axial positions is randomly distributed in the structure, the mean structure has a higher symmetry in comparison to the individual complexes, and the observed space group is thereby allowed to have higher symmetry in comparison to the individual complexes. By using a lattice-independent structure method such as EXAFS the distances to the absorbing atom are independent of orientation in space, giving the actual distance distribution. A previous EXAFS study has shown that the crystal structures of [Cu(H2O)6](BrO3)2 and [Cu(H2O)6]SiF6, and some other six-coordinate homoleptic copper(II) complexes displaying regular octahedral geometry, actually have a distorted geometry with two well-separated distances.[34] This “too high symmetry” effect has been also seen in e.g. the crystal structures of [Sc(H2O)8.0](CF3SO3)3 and [Lu(H2O)8.2](CF3SO3)3.[35,36] In these two cases, a phase transition to lower symmetry takes place on cooling and the true structure is observed in the low-temperature phases. EXAFS studies have shown that these complexes have the same structure independent of the temperature of the solid or in aqueous solution.[35,36]

The number of tetra- and pentaaquacopper(II) n class="Chemical">complexes with no other ligands within the sum of the van der Waals radii[37] reported in crystallographic studies is low. Only four structures, each with a tetra- or pentaaquacopper(II) ion, have been reported (Table S3). Due to the limited number of such reported structures, the literature search was extended to all four-and five-coordinate copper(II) complexes with oxygen donor ligands. The four-coordinate complexes have all a square-planar coordination geometry with a mean Cu–O bond distance of 1.928 Å (68 structures) (Table S3). Of the five-coordinate copper(II) complexes with oxygen donor ligands all except one display a tetragonally elongated square-pyramidal geometry, with the last one being a trigonal bipyramid (Table S3). The mean Cu–O bond distance in the square-pyramidal copper(II) complexes is 1.955 Å in the equatorial plane and 2.258 Å to the ligand in the axial position (37 structures) (Table S3).

To summarize the present knowledge about the structure of the hydrated n class="Chemical">copper(II) ion in aqueous solution, (1) there is strong evidence that it is noncentrosymmetric, as shown by linear electric field EPR[6,7] and X-ray absorption spectroscopy studies,[13,22,25] (2) different kinds of theoretical simulations have shown that [Cu(H2O)5]2+ and [Cu(H2O)5··H2O]2+ units are more stable in aqueous solution in comparison to a regular Jahn–Teller distorted [Cu(H2O)6]2+ ion,[9−16,21−23,25] and (3) solid-state structures containing [Cu(H2O)6]2+ ions crystallize in noncentrosymmetric space groups or in centrosymmetric space groups but the copper in [Cu(H2O)6]2+ is not in the center of symmetry and [Cu(H2O)5(O′)] complexes display a significant difference in the axial Cu–O bond distances as discussed above.

The aim of this study is to collect high-quality EXAFS data to high k values of solvated n class="Chemical">copper(II) ions in solution in series of oxygen donor solvents and to test which of the three different models, a tetragonally elongated square pyramid (5-coordination) and tetragonally elongated octahedra with the same or different axial Cu–O bond distances (6-coordination), fit the data best and to make comparisons to previously reported EXAFS and MXAN studies[13,22,25] on the hydrated copper(II) ion in aqueous solution. The studied solvents all have similar physicochemical properties (Table S4) and represent increasing spatial demand upon coordination in order to study whether lower coordination numbers are present for the solvents most space-demanding at coordination. For example, it has previously been reported that the copper(II) ion is four-coordinate in hexamethylphosphoric triamide, a space-demanding solvent at coordination.[38] Another aim is to confirm or disprove whether the Cu–O bond distances reported in the crystal structures of [Cu(H2O)6](ClO4)2, [Cu(H2O)6](BrO3)2, [Cu(H2O)6]SiF6, Cu(NO3)2·2.5H2O, and CuSO4·5H2O are in agreement with the Cu–O bond distances obtained by EXAFS. If the crystallographic investigations of the reported structures cannot be confirmed by EXAFS, it becomes evident that crystallographic studies of compounds crystallizing in e.g. centrosymmetric space groups may result in structural information with higher symmetry in comparison to the individual units, e.g. metal complexes, thereby leading to an incorrect description.

Experimental Section

Chemicals

Methanol (CH3OH; MeOH), n class="Chemical">N,N-dimethylformamide ((CH3)2NCHO; dmf), N,N-diethylformamide ((CH3CH2)2NCHO; def), N,N-dimethylacetamide ((CH3)2NC(CH3)O; dma), N,N-diethylacetamide ((CH3CH2)2NC(CH3)O; dea), N,N-dimethylpropionamide ((CH3)2NC(CH3CH2)O; dmp), N,N-diethylpropionamide ((CH3CH2)2NC(CH3CH2)O; dep), N,N,N′,N′-tetramethylurea ((CH3)2N)2CO; tmu), and N,N′-dimethylpropyleneurea ((CH2)3N(CH3)2CO; dmpu), all Sigma-Aldrich, were used as purchased except for dmpu, which was purified by distillation over calcium hydride (CaH2; Merck) under reduced pressure and stored over 3 Å molecular sieves in a dark bottle. Deionized water that was further purified by a Milli-Q Plus Ultrapure water system, giving water with 18.2 MΩ cm resistance was used in syntheses of the hydrated copper(II) salts and in the preparation of aqueous solutions.

Copper powder (n class="Disease">Aldrich, 99.9999% purity, lot #1297) was dissolved in concentrated nitric acid (Merck, analytical grade). After a part of the obtained solution was cooled in a refrigerator, solid copper(II) nitrate hemipentahydrate (Cu(NO3)2·2.5H2O) precipitated. After dilution of the remaining part of this solution with deionized water, a 5 mol dm–3 sodium hydroxide solution (prepared from sodium hydroxide (NaOH; Merck, analytical grade) was added to precipitate copper(II) hydroxide, which was rinsed several times with water. Anhydrous copper(II) trifluoromethanesulfonate (Cu(CF3SO3)2) was prepared by adding an excess of trifluoromethanesulfonic acid (CF3SO3H; Fluka) dropwise to an aqueous slurry of copper(II) hydroxide until a clear solution was obtained. The obtained solution was filtered, and water and excess acid were boiled off at approximately 450 K in an oven. The resulting anhydrous copper(II) trifluoromethanesulfonate was repeatedly ground using a mortar and pestle with oven drying at 450 K in between until a fine, dry, almost white powder was obtained. The dry salt was stored in the oven at 450 K to avoid uptake of water. Hexaaquacopper(II) perchlorate ([Cu(H2O)6](ClO4)2) was prepared by dissolving copper(II) hydroxide in dilute perchloric acid (HClO4), the volume was reduced, and precipitation took place after cooling in a refrigerator. Copper(II) sulfate pentahydrate (CuSO4·5H2O) was prepared in the same way as the perchlorate salt but using dilute sulfuric acid, prepared from concentrated sulfuric acid (Merck, analytical grade, 98%). The identities of the prepared solid compounds were confirmed by determinations of the unit cell parameters crystallographically.

Solutions and Crystals

The solutions for the EXAFS studies were prepn class="Chemical">ared by dissolving anhydrous copper(II) trifluoromethanesulfonate in the respective solvent to a concentration of 0.19 mol dm–3 (Table S5). All solutions, except the dmpu and tmu solutions, are light blue with somewhat different hues. The dmpu and tmu solutions are dark green. In another experiment a saturated copper(II) trifluoromethanesulfonate dmpu solution was stored in a refrigerator for several years. Only low-quality single-crystals of tetrakis(N,N′-dimethylpropyleneurea)copper(II) trifluoromethanesulfonate monosolvate ([Cu(dmpu)4](CF3SO3)2·dmpu; 1) were obtained. The reported crystal structure represents the best of these. Repeated attempts to prepare better crystals, using different common methods, failed.

Balder Beamline at the MAX IV Synchrotron Light Facility, Lund, Sweden

Copper K-edge X-ray absorption data were collected in transmisn class="Chemical">sion mode at the Balder beamline at the MAX IV synchrotron light facility, Lund University, Lund, Sweden. Balder is a new high-flux wiggler beamline for X-ray absorption and emission spectroscopy at the 3.0 GeV storage ring.[39] High data acquisition speed is crucial to be able to perform X-ray spectroscopy experiments over 2000 eV without significant radiation damage. The double-crystal fixed exit monochromator (DCM) (FMB Oxford) is equipped with a direct drive motor on the Bragg axis, allowing for scan speeds up to 0.5 s/1000 eV. In the current configuration of the data acquisition a full EXAFS scan can be performed within acquisition times down to 12 s. Spectra were acquired using a continuous scan scheme, where the Bragg axis as well as the vertical beam offset are moved simultaneously with constant velocity to fix the vertical position of the beam. The Bragg axis is equipped with a rotary encoder with a resulting resolution of 50 counts/μrad. Data acquisition was performed using an Em# electrometer device,[40] which is an MAX IV codevelopment together with ALBA of Spain. The acquisition is (hardware) triggered at predefined positions of the Bragg axis on the basis of a comparison of the encoder readout with a look-up table of trigger positions at FPGA (field programmable gate array) level utilizing the PandABox developed at Soleil in France, and Diamond in the United Kingdom.[41] The DCM is equipped with two sets of crystals, Si(111) and Si(311), of which the Si(111) crystal set was employed in this study. A vertically position sensitive ionization chamber is coupled in closed-loop operation to a piezo drive on the pitch axis of the second monochromator crystal for further stabilization of the beam position on the sample during a scan. Custom-developed ionization chambers were used for transmission measurements. The ion chambers are 30 cm long; the first one, I0, contained 1.5 bar of N2 (applied potential 2.0 kV) and the second one, I1, contained 0.2 bar of Ar and 1.8 bar of N2 (applied potential 2.5 kV).

Extended X-ray Absorption Fine Structure (EXAFS)

The copper K-edge X-ray absorption data in this study were collected in transmisn class="Chemical">sion mode. The liquid sample cells were made of a 3.0 mm Teflon spacer and Kapton foil windows held together with titanium frames. The solid samples were measured as pressed pellets with cellulose or polyethylene as the binding medium. The XAS spectra were measured in continuous energy scanning at a speed of 50 s/full EXAFS spectrum (kmax = 18 Å–1). The monochromatic flux at the sample was ∼1012 photons/s with a spot size of approximately 0.10 (horizontal) × 2.0 (vertical) mm. For each sample, 20 repeats were examined for possible radiation damage and afterward accumulated into an average spectrum. Radiation damage, if it happens, is in solid samples seen as sharp bends on the absorption coefficient curves and as color variation of the sample visible live by a macro camera. In general, only a single EXAFS scan was recorded on each sample position. Immediately before the start of each repeat, the sample was shifted by 0.20 mm horizontally into a fresh position to avoid radiation dose accumulation. It was seen that aqueous solutions and solid hydrates were the most prone to radiation damage, due to water radiolysis as reported before.[42] In such cases, when bubbles were seen rapidly forming or abnormal changes in the EXAFS spectrum were observed, the scanning speed was increased to 25 s/full EXAFS spectrum. The energy axis was calibrated with repeated spectra of a copper foil with the first inflection point assigned as 8980.3 eV.[43] The EXAFSPAK[44] program package was used for data treatment. The EXAFS oscillations were extracted using standard procedures for pre-edge subtraction, spline removal, and data normalization.[45] Model fitting, including both single and multiple backscattering pathways, was performed with theoretical phase and amplitude functions calculated ab initio by means of the computer code FEFF7.[46] The k3-weighted EXAFS oscillation was analyzed using a nonlinear least-squares fitting procedure.

Large-Angle X-ray Scattering (LAXS)

The scattering from the free surface of a saturated dmpu solution of n class="Chemical">copper(II) trifluoromethanesulfonate, (∼0.8 mol dm–3) was measured with a large-angle θ–θ goniometer, as previously described.[47,48] Intensity data were collected in the range 1 < θ < 65° using Mo Kα radiation (λ = 0.7107 Å), following the same procedure as described elsewhere.[49] The experimental intensities were corrected for absorption and polarization and normalized to a stoichiometric unit of volume corresponding to one copper atom. After subtraction of the structure-independent coherent and Compton scattering, the remaining structure-dependent intensity function i(s) was Fourier-transformed to obtain a modified radial distribution function (RDF), expressed in the form D(r) – 4πr2r0. Minor erroneous peaks below 1.2 Å in the RDFs were removed by a Fourier back-transform procedure to align the intensity function before fitting the model functions. The KURVLR program[50] was used for data treatment and the STEPLR program[51] for least-squares refinements of model parameters by comparing calculated intensity contributions for distinct interatomic interactions with the experimental reduced intensities for values of s > 3.7 Å–1 (s = (4π/λ) sin θ).

Single-Crystal X-ray Diffraction

Data collection were performed on a Bruker SMART platform equipped with a CCD n class="Chemical">area detector and a graphite monochromator using Mo Kα (λ = 0.7107 Å) radiation at ambient room temperature. A hemisphere of data with 1271 frames was collected using the ω scan method (0.3° frame width). The crystal to detector distance was 50 mm. The first 50 frames were remeasured at the end of the data collection to monitor crystal and instrument stability. The structure was solved by direct methods in the SHELX 2016/6 program package[52] and refined using full-matrix least squares on F.

Non-n class="Chemical">hydrogen atoms were treated anisotropically. Hydrogen atoms were calculated in ideal positions riding on their respective carbon atoms. Crystal and experimental data for 1 are summarized in Table .

Table 1

Crystallographic Data for 1

	C38H72CuF6N12O12S2
mol wt	1130.73
cryst syst	monoclinic
space group	P21/c
a/Å	12.629(6)
b/Å	21.740(10)
c/Å	10.050(5)
α/deg	90
β/deg	103.046(8)
γ/deg	90
V/Å3	2688(2)
T/K	298(2)
Z	2
ρcalcd/g cm–3	1.397
μ/mm–1	0.570
cryst size/mm	0.27 × 0.22 × 0.18
θ range/deg	1.66–25.68
index ranges	–15 ≤ h ≤ 15, −23 ≤ k ≤ 26, −11 ≤ l ≤ 12
no. of measd rflns	13755
no. of unique rflns (Rint)	5094 (0.0511)
refinement method	full-matrix least squares on F2
final R1, wR2 (I > 2σ(I))a	0.0727, 0.1960
final R1, wR2 (all data)a	0.1197, 0.2324
max diff peak/e Å–3	0.377
max diff hole/e Å–3	–0.273

R values are defined as R1 = ∑||Fo| – |Fc||/∑|Fo| and wR2 = [∑[w(Fo2 – Fc2)]/∑[w(Fo2)2]]0.5.

R values are n class="Chemical">defined as R1 = ∑||Fo| – |Fc||/∑|Fo| and wR2 = [∑[w(Fo2 – Fc2)]/∑[w(Fo2)2]]0.5.

UV–Vis Spectrophotometry

A PerkinElmer Lambda 2 double-beam spectrophotometer was used to record the UV–vis spectra of the copper(II) trifluoromethanesulfonate solutions studied by n class="Chemical">EXAFS. The recorded spectra after appropriate dilution are shown in Figure S1.

Results and Discussion

EXAFS Study of the Hydrated Copper(II) ion in Aqueous Solution and the Solid State

In this study EXAFS data on an aqueous solution of n class="Chemical">copper(II) trifluoromethanesulfonate and the solids [Cu(H2O)6](ClO4)2, Cu(NO3)2·2.5H2O, and CuSO4·5H2O have been collected at the Balder beamline. They are compared with data on a 0.50 mol dm–3 aqueous solution of copper(II) perchlorate and the solids [Cu(H2O)6](BrO3)2, and [Cu(H2O)6]SiF6, collected at beamline 4-1 (old station) at the Stanford Synchrotron Radiation Lightsource (SSRL), reported in ref (34). The EXAFS spectra of the aqueous solutions and the solids [Cu(H2O)6](ClO4)2, [Cu(H2O)6](BrO3)2, and [Cu(H2O)6]SiF6 almost superimpose each other, showing that they have identical or at least very similar structures (Figure ). Also solid Cu(NO3)2·2.5H2O almost superimposes with the aqueous copper(II) solutions, implying a structural similarity even though copper(II) binds nitrate oxygens in the equatorial and axial positions[53−55] (Figure ). The data collected at SSRL have been refitted with the three models used in this study. The results of the refinements of the EXAFS data of the aqueous solutions and these solids are summarized in Table . The best fit of the hydrated copper(II) ion in aqueous solution is obtained by a model with four Cu–Oeq bond distances in the equatorial plane at 1.956(3) Å and two separate Cu–Oax bond distances of 2.14(2) and 2.32(2) Å, which are in close agreement with an EXAFS study reported by Frank et al.[22] In the solids [Cu(H2O)6](ClO4)2 and [Cu(H2O)6]SiF6, the Cu–Oeq bond distances are within the limit of errors the same, 1.963(6) Å, the Cu–Oax bond distances are slightly longer than those in aqueous solution, 2.18(1), 2.34(1) Å and 2.21(2), 2.32(3) Å, respectively. In solid [Cu(H2O)6](BrO3)2 the Cu–Oeq and Cu–Oax bond distances are slightly longer, 1.967(5), 2.21(2) Å and 2.42(2) Å.

Figure 1

Raw EXAFS spectra of a 0.20 mol dm–3 aqueous copper(II) trifluoromethanesulfonate solution (black line), 0.50 mol dm–3 aqueous copper(II) perchlorate solution (reported in ref (34), purple line, offset 4), solid [Cu(H2O)6](ClO4)2 (red line, offset 4), solid Cu(NO3)2·2.5H2O (blue line, offset 6), solid [Cu(H2O)6](BrO4)2 (reported in ref (34), yellow line, offset 8), and [Cu(H2O)6]SiF6 (reported in ref (34), green line, offset 10).

Table 2

Summary of Refinements of EXAFS Data Using a Noncentrosymmetric Tetragonally Elongated Octahedral Geometry of the Hydrated Copper(II) ion in Water (aq) and the Solid State for [Cu(H2O)6](ClO4)2 (A), Cu(NO3)2·2.5H2O (B), CuSO4·5H2O (C), [Cu(H2O)6](BrO3)2 (D), and [Cu(H2O)6]SiF6 (E)a

	water	water*	A	B	C	D*	E*
d(Cu–Oeq)	1.957(3)	1.954(8)	1.963(3)	1.959(3)	1.959(3)	1.967(5)	1.962(6)
σ2(Cu–Oeq)	0.0055(3)	0.0069(8)	0.0060(3)	0.0052(3)	0.0051(3)	0.0052(7)	0.0050(8)
n(Cu–Oeq)	4	4	4	4	4	4	4
d(Cu–Oax1)	2.14(2)	2.15(5)	2.184(8)	2.176(6)	2.218(9)	2.21(2)	2.21(2)
σ2(Cu–Oax1)	0.007(2)	0.012(6)	0.0065(9)	0.0072(6)	0.0066(7)	0.010(2)	0.011(4)
n(Cu–Oax1)	1	1	1	1	1	1	1
d(Cu–Oax2)	2.32(2)	2.36(4)	2.343(8)	2.394(8)	2.376(9)	2.42(2)	2.32(3)
σ2(Cu–Oax2)	0.009(2)	0.014(6)	0.0076(8)	0.0084(8)	0.0074(9)	0.010(2)	0.012(3)
n(Cu–Oax2)	1	1	1	1	1	1	1
d(MS(CuO4))	3.914b	3.908b	3.926b	3.917b	3.918b	3.934b	3.924b
σ2(MS(CuO4))	0.012(3)	0.013(4)	0.010(3)	0.010(2)	0.032(3)	0.010(4)	0.010(4)
n(MS(CuO4))	3*4	3*4	3*4	3*4	3*4	3*4	3*4
d(Cu–S1)					3.58(2)
σ2(Cu–S1)					0.012(3)
n(Cu–S1)					1
d(Cu–S2)					3.74(7)
σ2(Cu–S2)					0.024(8)
n(Cu–S2)					1
S02	0.93(4)	1.03(4)	1.06(4)	0.95(3)	1.05(3)	0.72(5)	0.84(5)
E0	8989.7(5)	8988.7(6)	8989.6(5)	8989.6(3)	8989.9(5)	8989.5(5)	8989.9(5)
F	18.14	8.19	16.36	7.98	12.85	8.19	9.69

Definitions: distance, d/Å; Debye-Waller coefficient, σ2/Å2; number of distances, n; amplitude reduction factor, S02; threshold energy, E0/eV; weighted F factor, F. The asterisk denotes data collected at SSRL in 2001. Estimated errors within parentheses include the statistical errors from the refinements and estimated experimental errors. Parameters without following parentheses have been fixed.

The linear multiple scattering distance with in the CuO4 equatorial plane has been linked to the Cu–O bond distance.

Raw EXAFS spectra of a 0.20 mol dm–3 aqueous n class="Chemical">copper(II) trifluoromethanesulfonate solution (black line), 0.50 mol dm–3 aqueous copper(II) perchlorate solution (reported in ref (34), purple line, offset 4), solid [Cu(H2O)6](ClO4)2 (red line, offset 4), solid Cu(NO3)2·2.5H2O (blue line, offset 6), solid [Cu(H2O)6](BrO4)2 (reported in ref (34), yellow line, offset 8), and [Cu(H2O)6]SiF6 (reported in ref (34), green line, offset 10).

Definitions: distance, d/Å; Debye-Waller coefficient, σ2/Å2; number of distances, n; amplitude reduction factor, S02; threshold energy, E0/eV; weighted F factor, F. The asterisk denotes data collected at SSRL in 2001. Estimated errors within pn class="Chemical">arentheses include the statistical errors from the refinements and estimated experimental errors. Parameters without following parentheses have been fixed.

The linear multiple scattering distance with in the n class="Chemical">CuO4 equatorial plane has been linked to the Cu–O bond distance.

The mean Cu–Oeq and n class="Chemical">Cu–Oax bond distance in solid Cu(NO3)2·2.5H2O have been refined to 1.959(3), 2.176(6), and 2.39(1) Å, respectively (Table ). The fitting using models with copper binding four solvent molecules in the equatorial plane and two in an axial position at the same Cu–Oax bond distance (centrosymmetric Jahn–Teller distorted-octahedral geometry) or only one solvent molecule in the axial position of a tetragonally elongated square pyramid are slightly worse than the model with different bond distances in the axial positions. The structure parameters obtained in the refinements applying these models are given in Table and Table S6. The fit of raw EXAFS data and the Fourier transforms are shown in Figures and 3, respectively.

Figure 2

Fit of raw EXAFS data of (a) solid copper(II) sulfate pentahydrate (CuSO4·5H2O, offset 10), (b) solid hexaaquacopper(II) hexafluorosilicate ([Cu(H2O)6]SiF6, offset 8), (c) solid hexaaquacopper(II) bromate ([Cu(H2O)6](BrO3)2, offset 6), (d) solid hexaaquacopper(II) nitrate (Cu(NO3)2·2.5H2O, offset 4), (e) solid hexaaquacopper(II) perchlorate ([Cu(H2O)6](ClO4)2, offset 2), and (f) aqueous solution of copper(II) trifluoromethanesulfonate (no offset).

Figure 3

Fit of Fourier transforms of EXAFS data of (a) solid copper(II) sulfate pentahydrate (CuSO4·5H2O, offset 1.0), (b) solid hexaaquacopper(II) hexafluorosilicate ([Cu(H2O)6]SiF6, offset 0.8), (c) solid hexaaquacopper(II) bromate ([Cu(H2O)6](BrO3)2, offset 0.6), (d) solid hexaaquacopper(II) nitrate ([Cu(H2O)6](NO3)2, offset 0.4), (e) hexaaquacopper(II) perchlorate (Cu(NO3)2·2.5H2O, offset 0.2), and (f) aqueous solution of copper(II) trifluoromethanesulfonate (no offset).

Fit of raw EXAFS data of (a) solid n class="Chemical">copper(II) sulfate pentahydrate (CuSO4·5H2O, offset 10), (b) solid hexaaquacopper(II) hexafluorosilicate ([Cu(H2O)6]SiF6, offset 8), (c) solid hexaaquacopper(II) bromate ([Cu(H2O)6](BrO3)2, offset 6), (d) solid hexaaquacopper(II) nitrate (Cu(NO3)2·2.5H2O, offset 4), (e) solid hexaaquacopper(II) perchlorate ([Cu(H2O)6](ClO4)2, offset 2), and (f) aqueous solution of copper(II) trifluoromethanesulfonate (no offset).

Fit of Fourier transforms of EXAFS data of (a) solid n class="Chemical">copper(II) sulfate pentahydrate (CuSO4·5H2O, offset 1.0), (b) solid hexaaquacopper(II) hexafluorosilicate ([Cu(H2O)6]SiF6, offset 0.8), (c) solid hexaaquacopper(II) bromate ([Cu(H2O)6](BrO3)2, offset 0.6), (d) solid hexaaquacopper(II) nitrate ([Cu(H2O)6](NO3)2, offset 0.4), (e) hexaaquacopper(II) perchlorate (Cu(NO3)2·2.5H2O, offset 0.2), and (f) aqueous solution of copper(II) trifluoromethanesulfonate (no offset).

The three crystallographic studies on [Cu(n class="Chemical">H2O)6](ClO4)2 have reported very different Cu–O bond distance distributions, in spite of reporting the same space group, P21/c (No. 14) (Table S7).[56−58] Two of these report very similar unit cell parameters,[56,57] while the third study differs significantly[58] (Table S7). In the first reported structure,[56] the hydrated copper(II) ion is six-coordinate with the expected Cu–Oeq bond distances for a Jahn–Teller distorted complex. By a fit the present EXAFS data with the reported Cu–O bond distances fixed, the fit is reasonable but the axial distances are clearly wrong with a very large Debye–Waller coefficient, σ2 = 0.05 Å2, and a remaining wave in the residual (Figure S2a); the corresponding Fourier transform (FT) is shown in Figure S3a. The other two reported structures[57,58] propose pairwise Cu–O bond distances at 2.090, 2.164, and 2.280 Å and 1.969, 2.084, and 2.202 Å, respectively, which are in strong contradiction to most other reported hexaaquacopper(II) complexes (Table S1). The calculated EXAFS spectra based on the reported Cu–O bond distances are almost completely out of phase in comparison to the experimental EXAFS data (Figure S2b,c) and the corresponding FTs in Figure a.

The crystallographic studies of [Cu(n class="Chemical">H2O)6](BrO3)2 and [Cu(H2O)6]SiF6 report a regular octahedral structure of the hexaaquacopper(II) ion with Cu–O bond distances of 2.079 and 2.074 Å,[59,60] respectively, but they have been proven to have a nonregular octahedral geometry as reported before.[34] The calculated EXAFS functions on these structures are completely out of phase with the experimental data (Figure S2d,e) and the corresponding FTs in Figure S3b,c, showing that the reported structures from crystallography cannot be correct as discussed above and before.[34]

The crystal structure of Cu(NO3)2·2.5n class="Chemical">H2O has been reported in three papers.[53−55] Copper(II) binds two water molecules and two nitrate oxygens in the equatorial positions at Cu–O bond distances of 1.959 and 1.986 Å, respectively and additionally three nitrate oxygens at longer distances, one at 2.391 Å and two close to 2.66 Å[53] (Table S7b). The other two determinations report slightly different Cu–O bond distances, 2.476 and two close to 2.62 Å (Table S7b).[54,55] The fit of the EXAFS data gave a mean Cu–Oeq bond distance of 1.959 Å and three longer Cu–Oax/Cu···N distances to nitrate ions at 2.183(5), 2.398(5), and 2.734(8) Å. The Cu–Oeq bond distance obtained in this EXAFS study is slightly shorter (1.959(3) Å) than the mean distances in the reported crystallographic investigations (1.972 and 1.990 Å)[53,55] but is in agreement with the Cu–Oeq distances in aqueous solution and the other salts containing hydrated copper(II) ions (Table ). It is interesting to note that the Cu–O bond distance at 2.39(1) Å fits perfectly, and the longest Cu–O/N distances fit reasonably well with distances reported in the crystallographic study of Cu(NO3)2·2.5H2O. However, these distances cannot be refined without the presence of a relatively short Cu–Oax bond distance, refined to 2.176(6) Å, which is absent in the crystal structure. The best possible fit of the EXAFS data with the reported Cu–O bond distances in ref (53) is shown in Figure S2f and the corresponding FT in Figure S3d. In solid CuSO4·5H2O, which crystallizes in the centrosymmetric space group P1̅ (No. 2), copper binds four water molecules in the equatorial plane and two sulfate oxygens in the axial positions in room-temperature studies.[61−66] The mean Cu–Oeq bond distances in CuSO4·5H2O obtained by EXAFS in this study, 1.959(3) Å (Table ), is in very good agreement with those in the reported crystallographic studies. However, for the axial positions two different Cu–Oax bond distances are discerned, 2.22(1) and 2.38(1) Å (Table ). The long Cu–Oax,SO4 bond distance is in good agreement with that reported distances in the crystallographic studies,[61−66] while the short Cu–Oax,SO4 bond distance obtained in this EXAFS study is significantly shorter. The fit of the raw EXAFS data and the Fourier transforms of the studied solid copper(II) hydrates are shown in Figures and 3, respectively, and the refined structure parameters are given in Table . Also in this case it is proven that the crystallographically determined Cu–O bond distances are not in full agreement with the experimental EXAFS data as shown in Figure S2g and the corresponding FT data in Figure S3e.

These results show that the structure of the [Cu(n class="Chemical">H2O)6]2+ complex in solid [Cu(H2O)6(ClO4)2, [Cu(H2O)6](BrO3)2, and [Cu(H2O)6]SiF6, the [Cu(OH2)2(ONO2)2]·unit in Cu(NO3)2·2.5H2O, and the [Cu(H2O)4(OSO3)2] unit in CuSO4·5H2O reported from crystallographic studies cannot be confirmed by the lattice-independent EXAFS method. All of the analyzed solid-state structures were solved in centrosymmetric space groups, which required pairwise equal Cu–O bond distances or a regular octahedral geometry. It therefore seems likely that the Cu–Oax bonds in these compounds also may have different bond lengths, according to the EXAFS results, and that they are randomly oriented in the solid state in either one dimension, resulting in an apparent centrosymmetric Jahn–Teller distorted-octahedral configuration, or in three dimensions, resulting in regular or slightly distorted octahedra. As a consequence, it seems likely that most of the reported crystal structures containing a hexaaquacopper(II) ion crystallizing in a centrosymmetric space group actually have a similar bond distance distribution in the axial positions, as observed in aqueous solution and the five solids analyzed in this study. It is therefore important to complement crystallographic studies with a lattice-independent method such as EXAFS to secure that a high-symmetry model indeed is the correct one for complexes which may have a lower symmetry. Coordination geometries where such a check is vital are those for metal complexes with Jahn–Teller distorted-octahedral and capped-trigonal-prismatic configurations.

Structure of the Solvated Copper(II) Ion in Methanol and Six Amide Solvents Studied by EXAFS

The structure of the solvated copper(II) ion in n class="Chemical">methanol, dmf, def, dma, dea, dmp, and dep show the same pattern as in water with four solvent molecules in the equatorial positions at ca. 1.96 Å and two significantly different axial Cu–O bond distances. No homoleptic copper(II) methanol solvate has been reported in the solid state,[4] and only four copper(II) complexes with four bound methanol molecules have been reported.[67−70] The mean Cu–Oeq bond distance in the methanol-solvated copper(II) ion in solution has been refined to 1.975(4) Å, and the Cu–Oax bond distances have been refined to 2.202(8) and 2.34(1) Å. The mean Cu···C distance and the Cu–Oeq–C three-legged scattering path were refined to 3.03(2) and 3.18(4) Å, respectively, which corresponds to a Cu–O–C bond angle of 128(2)°, assuming a O–C bond distance of 1.39 Å, which is in full agreement with the bond angles in the reported solid solvates.[67−70] Zitolo and D’Angelo have reported an EXAFS and MXAN analysis of the methanol solvated copper(II) ion in solution. They tested two models, a tetragonally elongated square-pyramidal and a centrosymmetric Jahn–Teller distorted-octahedral configuration, showing that the tetragonally elongated square pyramid did fit best with a mean Cu–Oeq bond distance of 1.98 Å, a Cu–Oax distance of 2.27 Å, and a mean Cu–Oeq–C bond angle of 129.5°.[26] They reported also that the dimethyl sulfoxide and acetonitrile solvated copper(II) ions also have a tetragonally elongated square-pyramidal configuration in solution.[26,27]

Six structures of solid compounds containing a hexakis(n class="Chemical">dmf)copper(II) ion have been reported, three of which display a Jahn–Teller distorted-octahedral configuration,[71−73] while the other three have an irregular octahedral geometry.[74−76] The mean Cu–Oeq bond distance in the dmf-solvated copper(II) ion in dmf solution has been refined to 1.963(3) Å, and the Cu–O bond distances in the axial positions have been refined to 2.178(8) and 2.33(1) Å. The Cu···C distance and the Cu–O–C three-legged scattering path have been refined to 2.855(7) and 3.03(2) Å, respectively, which corresponds to a Cu–O–C bond angle of 124(1)°, assuming a O=C bond distance of 1.25 Å, which is in full agreement with the bond angles in the reported structures containing hexakis(dmf)copper(II) ions.[71−76]

No structures of any hexacoordinate n class="Chemical">copper(II) complex with the remaining amide solvents used in this study have been reported.[4] In the structure of tetrakis(dma)copper(II) perchlorate, four dma molecules are bound in the equatorial positions, and perchlorate oxygens are present in the axial positions at long distance but shorter than the van der Waals radii of copper and oxygen.[37,77] The results of the EXAFS studies of the def-, dma-, dea-, dmp-, and dep-solvated copper(II) ion in the respective solvents are fully in line with the results obtained in dmf. The fit of raw EXAFS data and Fourier transforms are shown in Figures and 5, respectively, and the refined structure parameters are given in Table . The Cu–Oeq bond distances in the dmf- and def-solvated copper(II) ions are slightly longer than in the dma, dea, dmp, and dep copper(II) solvates (Table ). The Cu–O–C angles in the dmf and def copper(II) solvates, 124(1)°, are significantly smaller than the dma, dea, dmp and dep angles, 130(1)° (Table ). This pattern is also seen in the solid structures of dmf- and dma-solvated copper(II) ions with mean Cu–O–C bond angles of 124.5 and 129.6°, respectively.[71−77] With an alkyl group binding to the amide carbon, the electron density on the oxygen becomes slightly smaller and the binding character slightly more electrostatic in comparison to formamides with a hydrogen binding to the amide carbon. The fits of raw EXAFS data and the Fourier transform of the methanol and amide solvent copper(II) solvates are shown in Figures and 5, respectively, and the refined structure parameters are given in Table .

Figure 4

Fit of raw EXAFS data of copper(II) trifluoromethanesulfonate in (a) N,N-dimethylpropylene urea (dmpu, offset +18), (b) N,N,N’N’-tetramethylurea (tmu, offset +16), (c) N,N-diethylpropionamide (dep, offset +14), (d) N,N-dimethylpropionamide (dmp, offset +12), (e) N,N-diethylacetamide (dea, offset +10), (f) N,N-dimethylacetamide (dma, offset +8), (g) N,N-diethylformamide (def, offset +6), (h) N,N-dimethylformamide (dmf, offset +4), (i) methanol (offset +2), and (j) aqueous solution acidified with trifluoromethanesulfonic acid.

Figure 5

Fit of Fourier transforms of EXAFS data of (a) N,N-dimethylpropylene urea (dmpu, offset +1.8), (b) N,N,N′,N′-tetramethylurea (tmu, offset +1.6), (c) N,N-diethylpropionamide (dep, offset +1.4), (d) N,N-dimethylpropionamide (dmp, offset +1.2), (e) N,N-diethylacetamide (dea, offset +1.0), (f) N,N-dimethylacetamide (dma, offset +0.8), (g) N,N-diethylformamide (def, offset +0.6), (h) N,N-dimethylformamide (dmf, offset + 0.4), (i) methanol (offset +0.2), and (j) aqueous solution acidified with trifluoromethanesulfonic acid.

Table 3

Summary of Refinements of EXAFS Data Using a Noncentrosymmetric Tetragonally Elongated Octahedral Geometry of the Solvated Copper(II) ion in Water (aq), Methanol (M), N,N-Dimethylformamide (dmf), N,N-Dimethylacetamide (dma), N,N-Dimethylpropionamide (dmp), N,N-Diethylformamide (def), N,N-Dimethylacetamide(dea), N,N-Dimethylpropionamide (dep), N,N′-Dimethylpropyleneurea (dmpu), and N,N,N′,N′-Tetramethylurea (tmu)a

	water	methanol	dmf	def	dma	dea	dmp	dep	dmpu	tmu
d(Cu–Oeq)	1.957(3)	1.975(3)	1.963(3)	1.967(3)	1.956(3)	1.956(3)	1.952(3)	1.951(3)	1.939(3)	1.935(3)
σ2(Cu–Oeq)	0.0055(3)	0.0064(3)	0.0061(3)	0.0058(3)	0.0060(3)	0.0061(3)	0.0062(3)	0.0058(3)	0.0057(3)	0.0060(3)
n(Cu–Oeq)	4	4	4	4	4	4	4	4	4	4
d(Cu–Oax1)	2.14(2)	2.202(8)	2.178(8)	2.186(3)	2.14(1)		2.17(1)	2.16(3)	2.11(4)
σ2(Cu–Oax1)	0.007(2)	0.0069(8)	0.0068(8)	0.007(1)	0.007(2)		0.007(2)	0.011(2)	0.014(4)
n(Cu–Oax1)	1	1	1	1	1		1	1	1
d(Cu–Oax2)	2.32(2)	2.34(1)	2.33(1)	2.34(1)	2.32(2)		2.34(2)	2.30(4)	2.27(4)
σ2(Cu–Oax2)	0.009(2)	0.007(2)	0.008(1)	0.007(2)	0.010(2)		0.014(3)	0.014(5)	0.013(5)
n(Cu–Oax2)	1	1	1	1	1		1	1	1
d(MS(CuO4))	3.914	3.951	3.926	3.935	3.912	3.913	3.904	3.902	3.878	3.870
σ2(MS(CuO4))	0.012(3)	0.011(3)	0.012(2)	0.012(2)	0.009(3)	0.009(2)	0.011(4)	0.009(4)	0.009(3)	0.014(5)
n(MS(CuO4))	3*4	3*4	3*4	3*4	3*4	3*4	3*4	3*4	3*4	3*4
d(Cu–C)		3.03(2)	2.855(7)	2.859(9)	2.93(1)	2.92(1)	2.94(1)	2.94(1)	2.85(1)	2.91(2)
σ2(Cu–C)		0.013(2)	0.009(4)	0.009(1)	0.011(1)	0.011(1)	0.012(1)	0.011(2)	0.014(2)	0.013(3)
n(Cu–C)		4	4	4	4	4	4	4	4	4
d(Cu–O–C)		3.18(4)	3.03(2)	3.03(3)	3.07(2)	3.06(2)	3.07(1)	3.08(1)	3.02(4)	3.09(1)
σ2(Cu–O–C)		0.026(5)	0.011(3)	0.013(2)	0.010(1)	0.011(2)	0.010(1)	0.009(1)	0.009(2)	0.011(1)
n(Cu–O–C)		8	8	8	8	8	8	8	8	8
∠Cu–O–C		127.9(5)	123.9(3)	123.9(3)	130.9(4)		130.3(4)	132.2(6)	131.8(6)
d(Cu–N)			3.99(1)	3.99(2)	4.00(2)	4.01(2)	4.01(2)	4.01(3)
σ2(Cu–N)			0.009(4)	0.010(2)	0.010(2)	0.010(2)	0.009(3)	0.010(3)
n(Cu–N)			4	4	4	4	4	4
d(Cu–N–C)			4.27(4)	4.29(4)	4.24(5)	4.25(4)	4.24(7)	4.22(6)
σ2(Cu–N–C)			0.006(4)	0.006(4)	0.012(5)	0.012(4)	0.015(9)	0.012(7)
n(Cu–N–C)			8	8	8	8	8	8
S02	0.93(4)	1.09(4)	1.10(4)	1.07(4)	1.09(4)	1.10(4)	1.10(4)	0.95(5)	0.92(3)	0.97(4)
E0	8989.7(5)	8990.0(5)	8989.8(5)	8991.1(5)	8989.9(5)	8988.9(5)	8989.5(5)	8989.5(5)	8988.2(5)	8987.3(5)
F	18.14	18.26	16.13	19.73	14.95	12.91	17.09	16.80	20.93	23.85

Definitions: distance; d/Å, Debye–Waller coefficient, σ2/Å2; number of distances, n; amplitude reduction factor, S02; threshold energy, E0/eV; weighted F factor, F. Estimated errors within parentheses includes the statistical errors from the refinements and estimated experimental errors. Parameters without following parentheses have been fixed.

The linear multiple scattering distance with in the CuO4 equatorial plane has been linked to the Cu–O bond distance.

Definitions: distance; d/Å, Debye–Waller coefficient, σ2/Å2; number of distances, n; amplitude reduction factor, S02; threshold energy, E0/eV; weighted F factor, F. Estimated errors within pn class="Chemical">arentheses includes the statistical errors from the refinements and estimated experimental errors. Parameters without following parentheses have been fixed.

The linear multiple scattering distance with in the n class="Chemical">CuO4 equatorial plane has been linked to the Cu–O bond distance.

Fit of raw EXAFS data of n class="Chemical">copper(II) trifluoromethanesulfonate in (a) N,N-dimethylpropylene urea (dmpu, offset +18), (b) N,N,N’N’-tetramethylurea (tmu, offset +16), (c) N,N-diethylpropionamide (dep, offset +14), (d) N,N-dimethylpropionamide (dmp, offset +12), (e) N,N-diethylacetamide (dea, offset +10), (f) N,N-dimethylacetamide (dma, offset +8), (g) N,N-diethylformamide (def, offset +6), (h) N,N-dimethylformamide (dmf, offset +4), (i) methanol (offset +2), and (j) aqueous solution acidified with trifluoromethanesulfonic acid.

Fit of Fourier transforms of EXAFS data of (a) n class="Chemical">N,N-dimethylpropylene urea (dmpu, offset +1.8), (b) N,N,N′,N′-tetramethylurea (tmu, offset +1.6), (c) N,N-diethylpropionamide (dep, offset +1.4), (d) N,N-dimethylpropionamide (dmp, offset +1.2), (e) N,N-diethylacetamide (dea, offset +1.0), (f) N,N-dimethylacetamide (dma, offset +0.8), (g) N,N-diethylformamide (def, offset +0.6), (h) N,N-dimethylformamide (dmf, offset + 0.4), (i) methanol (offset +0.2), and (j) aqueous solution acidified with trifluoromethanesulfonic acid.

Test of Different Models in the Refinements of EXAFS Data

The refined structure parameters of the solvated n class="Chemical">copper(II) ions using three models, a tetragonally elongated square pyramid and centrosymmetric and noncentrosymmetric tetragonally elongated octahedra, need to be compared. The solid compounds have all a well-defined composition, which suggests that a five-coordinate complex can be excluded. A comparison of the two Jahn–Teller distorted models shows that the mean Cu–Oax bond distance in the centrosymmetric model becomes fairly close to the average of the two Cu–Oax bond distances in the noncentrosymmetric model (Table and Table S6). Furthermore, the Debye–Waller coefficients, σ2, become unreasonably large, strongly indicating that the distance consists of at least two separated distances. Applying the noncentrosymmetric model with two well-separated Cu–Oax bond distances results in the refined Debye–Waller coefficients are within the expected values for bond distances of this kind, 0.005–0.009 Å–1. This strongly indicates that the Cu–Oax bond distances in the studied solid hydrates and solvates are different and are well separated with a difference of 0.15–0.20 Å (Tables and 3).

For the studied solutions the tetragonally elongated square-pyramidal model has to be included as well in this compn class="Chemical">arison. Applying the centrosymmetric octahedral model results in very large Debye–Waller coefficients for the Cu–Oax bond distances as found in the solid hydrate samples discussed above (Table S8a). When the square-pyramidal model is applied, the Cu–Oax bond distance becomes close to the value obtained by using the centrosymmetric octahedral model but the Debye–Waller coefficients becomes significantly smaller, 0.009–0.014 Å2 (Table S8b), but still of an order indicating a wide bond distance distribution for a single bond.

The pattern of bond distances and Debye–Waller coefficients and the fact that the EXAFS spectra of solid [n class="Chemical">Cu(H2O)6](ClO4)2, Cu(NO3)2·2.5H2O, [Cu(H2O)6](BrO3)2, and [Cu(H2O)6]SiF6 and the aqueous solutions of copper(II) superimpose (Figure ) strongly indicate the hydrated copper(II) ion and the solvated copper(II) ion in methanol and the six amide solvents bind six solvent molecules in a noncentrosymmetric tetragonally elongated octahedral geometry. This model is in full agreement with the observation using EPR that the hydrated copper(II) ion is noncentrosymmetric in aqueous solution[6,7] and is in full agreement with the EXAFS studies reported by Frank et al.[13,22,25] The survey of structure determinations of solid compounds containing a hexaaquacopper(II) ion or a pentaaqua(O-ligand)copper(II) complex described in the Introduction strongly indicates that individual copper(II) complexes in fact are six-coordinate and noncentrosymmetric. It is therefore very important to apply a non-lattice-dependent method such as EXAFS to determine the structures of such compounds.

Structure of the Solvated Copper(II) Ion in dmpu and tmu Studied by EXAFS

In the solvents which are space demanding upon coordination, n class="Chemical">dmpu and tmu, the axial positions are protected by the ligands in the equatorial positions (see below), resulting in square-planar complexes. It was not possible to locate any more solvent molecules within a reasonable bond distance. The Cu–O bond distances in the dmpu- and tmu-solvated copper(II) ions are significantly shorter, 1.939(3) and 1.935(3) Å, respectively, than the shortest Cu–Oeq bond distances in the hexasolvated copper(II) ions, 1.954(3) Å, for acetamide and propionamide (Table ) but are in agreement with four-coordinated copper(II) complexes with oxygen donor ligands (Table S3). The copper(II) trifluoromethanesulfonate solutions in dmpu and tmu have an intense dark green color due to a strong absorption band in the UV region and another at around 800 nm, both tailing into the visible region (Figure S1).

Structure of the dmpu-Solvated Copper(II) Ion in dmpu Solution Studied by LAXS

The radial distribution function of a LAXS study of a 0.8 mol dm–3 copper(II) n class="Chemical">trifluoromethanesulfonate solution shows a peak just below 2 Å assigned to the Cu–O bond distance and refined to 1.93(2) Å (Figure ). The LAXS model used includes interatomic interactions between the copper(II) ion and the solvating ligands and interactions within the solvent molecules and within the anions.

Figure 6

(Top) LAXS radial distribution curves for a 0.8 mol dm–3 copper(II) trifluoromethanesulfonate dmpu (top) separate model contributions (offset 14) of the tetrakis(dmpu)copper(II) complex (solid line), the trifluoromethanesulfonate ion (dashed line), and dmpu solvent (dotted line); (middle) experimental RDF with D(r) −4pr2ρ0 (solid line), sum of model contributions (dashed line), and difference (dotted line); (bottom) reduced LAXS intensity functions s.i(s) (thin line) and model s.icalc(s) (thick line).

(Top) LAXS radial distribution curves for a 0.8 mol dm–3 n class="Chemical">copper(II) trifluoromethanesulfonate dmpu (top) separate model contributions (offset 14) of the tetrakis(dmpu)copper(II) complex (solid line), the trifluoromethanesulfonate ion (dashed line), and dmpu solvent (dotted line); (middle) experimental RDF with D(r) −4pr2ρ0 (solid line), sum of model contributions (dashed line), and difference (dotted line); (bottom) reduced LAXS intensity functions s.i(s) (thin line) and model s.icalc(s) (thick line).

Crystal Structure of [Cu(dmpu)4](CF3SO3)2·dmpu (1)

The crystal structure of 1 consists of tetrakis(n class="Chemical">N,N’-dimethylpropyleneurea)copper(II) and trifluoromethanesulfonate ions, and with an additional noncoordinated N,N′-dimethylpropyleneurea molecule in the lattice. The almost planar dmpu molecules are stacked perpendicular to the equatorial plane with two crystallographically independent ligands having Cu–O bond distances of 1.900(3) and 1.902(3) Å, with Cu–O–C angles of 127.3(3) and 129.5(3)°, respectively, forming a regular square-planar coordination (Figure ). The low quality of the crystal made it necessary to add additional loose structural restraints to obtain sound results. For both of the ligand molecules, it was possible to refine two alternate positions, C14A/B and C24A/B, for the middle propylene carbon with partial occupancies at 73/27 and 53/47%, respectively, whereas the other ligand molecule showed the typical half-chair formation partial distribution refinement of its carbon, C14. The copper(II) methyl carbon distances Cu–C are approximately 3.7(1) Å, at roughly 45° from the flat CuO4 plane. Bond distances and angles in the trifluoromethanesulfonate ions are in agreement with those in previous studies, but due to disorder alternative positions were added.[4] The noncoordinated dmpu oxygen is 7.8 Å away from the copper(II) ion. Selected crystallographic data are given in Table , and selected bond distances and angles are given in Table . By a view perpendicular to the CuO4 plane of the tetrakis(N,N’-dimethylpropyleneurea)copper(II) ion it is clearly seen that the dmpu methyl groups effectively hinder access of ligands to the axial positions. Furthermore, the methyl groups near the axial position have no bonding properties to the copper(II) ion.

Figure 7

Structure of the tetrakis(dmpu)copper(II) unit in 1. Ellipsoids for all non-hydrogen atoms are set at 40% probability.

Table 4

Selected Bond Distances (Å) and Angles (deg) from the Crystal Structure Determination of Solid [Cu(dmpu)4](CF3SO3)2·dmpu

bond distance		bond angle
Cu–O1	1.900(3)	O1–Cu–O2	90.15(14)
Cu–O2	1.902(3)	O1–Cu–O2′	89.86(14)

Structure of the tetrakis(dmpu)copper(II) unit in 1. Ellipsoids for all non-n class="Chemical">hydrogen atoms are set at 40% probability.

Summary of the Coordination Chemistry of the Hydrated and Solvated Copper(II) Ions

Even though a large majority of the n class="Chemical">hexaaquacopper(II) complexes reported in the solid state are found to be centrosymmetric (Table S1), it has not been possible to confirm this with the lattice-independent EXAFS method in this study. It therefore seems very likely that the direction of the short and long axial Cu–O bond distances can be randomly distributed in solid compounds, resulting in a mean structure with higher symmetry in comparison to the symmetry of the individual complexes. This seems also to be the case for hexaaquacopper(II) ions reported to have a regular or somewhat irregular octahedral geometry, as some of these have been shown to have the expected Jahn–Teller distortion (vide supra). Of the complexes without a center of symmetry or with the center of symmetry not on copper in the [Cu(H2O)6]2+ complex, only a few display almost similar Cu–Oax distances, while the remaining structures display significant different Cu–Oax distances (Table S1). Furthermore, all reported [Cu(H2O)5(O-donor ligand)] complexes with Jahn–Teller distortion display significantly different Cu–Oax distances independent of whether the O-donor ligand is in equatorial or axial position (Table S2). The high k range EXAFS data collected in this study and by Frank et al.[22] allows a high resolution of distances. Using a model with two different axial Cu–Oax bond distances resulted in stable refinements independent of the system. This includes all solvents where copper(II) is six-coordinate, all studied solvents except tmu and dmpu, and the solids [Cu(H2O)6](ClO4)2, [Cu(H2O)6](BrO3)2, [Cu(H2O)6]SiF6, Cu(NO3)2·2.5H2O, and CuSO4·5H2O. The similar UV–vis spectra of the hydrated copper(II) ion in aqueous solution and the solvated copper(II) ion in methanol, dmf, def, dma, dea, dmp, and dep further support a similar configuration (Figure S1).

Conclusions

The structure of the solvated copper(II) ion in 10 n class="Chemical">oxygen donor solvents with similar bonding characteristics but with different space-demanding properties on coordination have been studied by EXAFS spectroscopy. In the solvents with large space-demanding properties on coordination, dmpu and tmu, copper(II) is shown to have a square-planar configuration with mean Cu–O bond distances of 1.93(2) Å. The best fits in the other solvents are obtained with a noncentrosymmetric tetragonally elongated octahedral model with different axial Cu–O bond distances with mean Cu–Oeq, Cu–Oax1, and Cu–Oax2 bond distances of ca. 1.96, 2.15, and 2.32 Å, respectively. This model is in full agreement with that proposed by Frank et al. for the hydrated copper(II) ion from EXAFS studies.[13,22,25] However, from the point-of-view of EXAFS data other configurations such as tetragonally elongated square pyramidal cannot be ruled out. EPR studies have shown that the hydrated copper(II) ion in aqueous solution is noncentrosymmetric.[7,8] A large number of number of theoretical simulations have concluded that [Cu(H2O)5]2+ and [Cu(H2O)5···H2O]2+ configurations are more stable in aqueous solution in comparison to the centrosymmetric Jahn–Teller distorted-octahedral configuration.[11,12,15,16,21,23] An in-depth survey of solid-state structures containing isolated hydrated copper(II) ions has shown that hexaaquacopper(II) complexes crystallizing in noncentrosymmetric space groups as well as in centrosymmetric space groups where the center of symmetry is not on the copper in the [Cu(H2O)6]2+ ion display significantly different Cu–O bond distances in the axial positions (Table S1). Furthermore, all of the [Cu(H2O)5(O-ligand)] complexes displaying Jahn–Teller distortion show the same splitting in the Cu–Oax bond distances independent of the position of the O-ligand (Table S2). EXAFS spectra of aqueous copper(II) solutions and the solids [Cu(H2O)6](ClO4)2, [Cu(H2O)6](BrO3)2, and [Cu(H2O)6]SiF6 are superimposable, strongly indicating that the hydrated copper(II) ions in these salts have the same or very similar configurations around copper as in aqueous solution. This is in spite of the fact that the crystallographic studies report centrosymmetric structures with a regular octahedral configuration for the last two complexes. This strongly indicates that copper(II) complexes reported to be centrosymmetric in the solid state are mean structures of noncentrosymmetric entities with random orientation of the copper(II) complex in the individual unit cells. A summary of the present information from different methods and publications is as follows.

The hydrated copper(II) ion in aqueous solution is n class="Chemical">six-coordinate with a noncentrosymmetric tetragonally elongated octahedral geometry, and the difference in the Cu–Oax bond distances is on the order of 0.2 Å,

The solvated copper(II) ion in the seven organic n class="Chemical">oxygen donor solvents without steric demands on coordination have the same configuration in solution as that of the hydrated copper(II) ion.

The solvated copper(II) ion has a four-coordinate squn class="Chemical">are-planar configuration in space-demanding solvents on coordination, as the axial positions become inaccessible.

It seems very likely that all six-coordinate n class="Chemical">copper(II) complexes reported to be centrosymmetric in the solid state have a noncentrosymmetric tetragonally elongated octahedral configuration with a random orientation of at least the axial ligands, but as crystallography gives the mean of all unit cells in the solid, the mean structure becomes centrosymmetric.