Supporting information
Crystallographic Information File (CIF) https://doi.org/10.1107/S2053229615024122/fn3211sup1.cif | |
Structure factor file (CIF format) https://doi.org/10.1107/S2053229615024122/fn3211Isup2.hkl |
CCDC reference: 1442717
Our recent work has focused on the preparation of VIV oxyfluorides due to their interest as frustrated magnets. We have found that the successful synthesis of two-dimensionally connected vanadium(IV) oxyfluoride structures, for example, kagome lattices, requires the use of ionic liquids as solvents (Aidoudi et al., 2011a,b, 2014; Clark et al., 2015). On the other hand, there have been several previous reports of solvothermally synthesized vanadium compounds incorporating selenium, which are generally two- and three-dimensional in nature, and can attribute this high-dimensional structural property to the incorporation of selenium-based anionic linkers (Nguyen et al., 2011; Glor et al., 2011). Reduced dimensionally-extended vanadium compounds can also be prepared by these routes, for example, VO(SeO2OH)2 (Kim et al., 2010) and (4,4'-bipyridine)V2Se2O8 (Dai et al., 2003). During solvothermal synthesis experiments aimed at producing two- and three-dimensional vanadium(IV) selenites with triangular lattices, a new V4+ layer structure, V2O2F4(H2O)2.H2O, (I), was discovered. This is apparently the first example of a fully reduced V4+ layered compound synthesized by solvothermal (rather than ionothermal) techniques. The structure is comprised of VOF4(H2O) corner- and edge-sharing octahedral building units. V2O2F4(H2O)2.H2O or VOF2(H2O).1/2H2O, (I), is related structurally to previously synthesized vanadium oxyfluoride compounds, VOF3 (Supel et al., 2007).
Vanadium trifluoride (VF3, Alfa, 98%; 0.002 mol, 0.215 g) and ethylene glycol (Fisher 99%+; 0.0032 mol, 0.2 ml) were added to a 40% solution of HF (0.5 ml, Alfa). Diethylamine [guanidine carbonate salt (0.001 mol, 0.09 g) was used in a different experiment in place of diethylamine and produced similar results] (Sigma, 99.5%; 0.001 mol, 0.5 ml) and selenious acid (Aldrich 99.999%; 0.001 mol, 0.129 g) were added to the resultant mixture before being sealed in a Teflon-lined stainless steel autoclave. This was heated at 393 K for 4 d, then allowed to cool to ambient temperature. The final product was filtered, washed in water and allowed to dry overnight at 333 K. The crystals obtained were blue blocks, indicating V4+, of typical dimension 0.06 × 0.04 × 0.03 mm. These were separated from the bulk product, a brown powder, under an optical microscope. The crystals recovered were too scarce to be analysed using powder X-ray diffraction or to be sent for elemental analysis.
Crystal data, data collection and structure refinement details are summarized in Table 1. H atoms were located from Fourier maps and refined isotropically.
The VOF4(H2O) building unit of (I) (Fig. 1) exhibits a single vanadium site in a distorted octahedral environment (Fig. 2) and a single uncoordinated water molecule. The short V═O bond length along with the longer trans V—F and cis V—OH2 bond lengths are comparable to those seen in the cis-building unit of [C6H4N22][VOF4(H2O)]2.H2O, (II) (Aldous et al., 2007). Selected bond lengths for (I) and (II) are shown for comparison in Table 2. The octahedral units are linked via fluoride ligands to produce a new two-dimensional corner and edge-sharing layer compound of V4+ (Fig. 3a). Bond-valence-sum analysis (Brese & O'Keeffe, 1991) confirms the oxidation state of the vanadium centre as V4+, oxidized in situ from V3+ (Table 3). The layer in (I) resembles that of the VOF3 structure, (III) (Supel et al., 2007), with both forming a layer comprised of corner- and edge-sharing octahedral units bridged via fluoride ligands (Fig. 3b). Aside from the different vanadium oxidation states, there are a number of significant differences between these two structures. The presence of uncoordinated water molecules in (I) results in longer inter-layer V···V distances, due to the hydrogen bonding from atom O3 to the layer [O3···H2 = 1.86 (4) Å and H2—O2 = 0.86 (4) Å], compared to those in (III) (Table 4). The elongated trans-fluoride ligand, F1, in (I) is involved in the edge-sharing V—F bonds, while in (III), the equivalent ligand is involved in the corner-sharing V—F bond. This results in a significant difference in the intra-layer V···V distances (Table 4). The layers of (I) can be seen to stack in a `staggered" manner (Fig. 4a.), while the layers in (III) stack in an `eclispsed' manner (Fig. 4b) when both are viewed along [010]. There are many previous examples of layered V4+-containing compounds that have synthesized solvothermally (Nguyen et al., 1995; Massa et al., 2002); however, these compounds owe their two-dimensional structural properties to phosphate and sulfate linkers. More recently, there have been examples of V4+-containing layers, synthesized via ionothermal methods (Aidoudi et al., 2011a,b, 2014). These compounds exhibit two-dimensional layers comprised fully of V4+ corner-sharing octahedral units. This appears to make compound (I) the first example of a purely V4+ layered compound produced via solvothermal techniques. From the presented synthesis route, compound (I) appears as a minor phase, together with a majority unidentified phase(s). Several further attempts to prepare (I) as the majority phase were unsuccessful. The synthetic method will need to be refined in order to produce (I) as the bulk phase, but this could lead to a simpler more cost-effective route, compared to ionothermal techniques, to obtain layered V4+ compounds for physical property investigation.
Our recent work has focused on the preparation of VIV oxyfluorides due to their interest as frustrated magnets. We have found that the successful synthesis of two-dimensionally connected vanadium(IV) oxyfluoride structures, for example, kagome lattices, requires the use of ionic liquids as solvents (Aidoudi et al., 2011a,b, 2014; Clark et al., 2015). On the other hand, there have been several previous reports of solvothermally synthesized vanadium compounds incorporating selenium, which are generally two- and three-dimensional in nature, and can attribute this high-dimensional structural property to the incorporation of selenium-based anionic linkers (Nguyen et al., 2011; Glor et al., 2011). Reduced dimensionally-extended vanadium compounds can also be prepared by these routes, for example, VO(SeO2OH)2 (Kim et al., 2010) and (4,4'-bipyridine)V2Se2O8 (Dai et al., 2003). During solvothermal synthesis experiments aimed at producing two- and three-dimensional vanadium(IV) selenites with triangular lattices, a new V4+ layer structure, V2O2F4(H2O)2.H2O, (I), was discovered. This is apparently the first example of a fully reduced V4+ layered compound synthesized by solvothermal (rather than ionothermal) techniques. The structure is comprised of VOF4(H2O) corner- and edge-sharing octahedral building units. V2O2F4(H2O)2.H2O or VOF2(H2O).1/2H2O, (I), is related structurally to previously synthesized vanadium oxyfluoride compounds, VOF3 (Supel et al., 2007).
The VOF4(H2O) building unit of (I) (Fig. 1) exhibits a single vanadium site in a distorted octahedral environment (Fig. 2) and a single uncoordinated water molecule. The short V═O bond length along with the longer trans V—F and cis V—OH2 bond lengths are comparable to those seen in the cis-building unit of [C6H4N22][VOF4(H2O)]2.H2O, (II) (Aldous et al., 2007). Selected bond lengths for (I) and (II) are shown for comparison in Table 2. The octahedral units are linked via fluoride ligands to produce a new two-dimensional corner and edge-sharing layer compound of V4+ (Fig. 3a). Bond-valence-sum analysis (Brese & O'Keeffe, 1991) confirms the oxidation state of the vanadium centre as V4+, oxidized in situ from V3+ (Table 3). The layer in (I) resembles that of the VOF3 structure, (III) (Supel et al., 2007), with both forming a layer comprised of corner- and edge-sharing octahedral units bridged via fluoride ligands (Fig. 3b). Aside from the different vanadium oxidation states, there are a number of significant differences between these two structures. The presence of uncoordinated water molecules in (I) results in longer inter-layer V···V distances, due to the hydrogen bonding from atom O3 to the layer [O3···H2 = 1.86 (4) Å and H2—O2 = 0.86 (4) Å], compared to those in (III) (Table 4). The elongated trans-fluoride ligand, F1, in (I) is involved in the edge-sharing V—F bonds, while in (III), the equivalent ligand is involved in the corner-sharing V—F bond. This results in a significant difference in the intra-layer V···V distances (Table 4). The layers of (I) can be seen to stack in a `staggered" manner (Fig. 4a.), while the layers in (III) stack in an `eclispsed' manner (Fig. 4b) when both are viewed along [010]. There are many previous examples of layered V4+-containing compounds that have synthesized solvothermally (Nguyen et al., 1995; Massa et al., 2002); however, these compounds owe their two-dimensional structural properties to phosphate and sulfate linkers. More recently, there have been examples of V4+-containing layers, synthesized via ionothermal methods (Aidoudi et al., 2011a,b, 2014). These compounds exhibit two-dimensional layers comprised fully of V4+ corner-sharing octahedral units. This appears to make compound (I) the first example of a purely V4+ layered compound produced via solvothermal techniques. From the presented synthesis route, compound (I) appears as a minor phase, together with a majority unidentified phase(s). Several further attempts to prepare (I) as the majority phase were unsuccessful. The synthetic method will need to be refined in order to produce (I) as the bulk phase, but this could lead to a simpler more cost-effective route, compared to ionothermal techniques, to obtain layered V4+ compounds for physical property investigation.
Vanadium trifluoride (VF3, Alfa, 98%; 0.002 mol, 0.215 g) and ethylene glycol (Fisher 99%+; 0.0032 mol, 0.2 ml) were added to a 40% solution of HF (0.5 ml, Alfa). Diethylamine [guanidine carbonate salt (0.001 mol, 0.09 g) was used in a different experiment in place of diethylamine and produced similar results] (Sigma, 99.5%; 0.001 mol, 0.5 ml) and selenious acid (Aldrich 99.999%; 0.001 mol, 0.129 g) were added to the resultant mixture before being sealed in a Teflon-lined stainless steel autoclave. This was heated at 393 K for 4 d, then allowed to cool to ambient temperature. The final product was filtered, washed in water and allowed to dry overnight at 333 K. The crystals obtained were blue blocks, indicating V4+, of typical dimension 0.06 × 0.04 × 0.03 mm. These were separated from the bulk product, a brown powder, under an optical microscope. The crystals recovered were too scarce to be analysed using powder X-ray diffraction or to be sent for elemental analysis.
Crystal data, data collection and structure refinement details are summarized in Table 1. H atoms were located from Fourier maps and refined isotropically.
Data collection: CrystalClear (Rigaku, 2004); cell refinement: CrystalClear (Rigaku, 2004); data reduction: CrystalClear (Rigaku, 2004); program(s) used to solve structure: SHELXS97 (Sheldrick, 2008); program(s) used to refine structure: SHELXL97 (Sheldrick, 2008); molecular graphics: DIAMOND (Brandenburg, 2009); software used to prepare material for publication: WinGX (Farrugia, 2012) and PLATON (Spek, 2009).
V2O2F4(H2O)2·H2O | F(000) = 512 |
Mr = 263.93 | Dx = 2.638 Mg m−3 |
Monoclinic, C2/c | Mo Kα radiation, λ = 0.71073 Å |
Hall symbol: -C2yc | Cell parameters from 1673 reflections |
a = 14.453 (8) Å | θ = 3.5–28.9° |
b = 4.8879 (19) Å | µ = 2.87 mm−1 |
c = 9.663 (5) Å | T = 173 K |
β = 103.24 (2)° | Block, blue |
V = 664.5 (6) Å3 | 0.06 × 0.04 × 0.03 mm |
Z = 4 |
Rigaku SCXmini diffractometer | 585 reflections with I > 2σ(I) |
Radiation source: fine-focus sealed tube | Rint = 0.115 |
Graphite monochromator | θmax = 27.3°, θmin = 2.9° |
dtprofit.ref scans | h = −18→18 |
Absorption correction: multi-scan (REQAB; Rigaku, 1998) | k = −6→6 |
Tmin = 0.742, Tmax = 1.000 | l = −12→12 |
3138 measured reflections | 1080 standard reflections every 1 reflections |
750 independent reflections |
Refinement on F2 | Primary atom site location: structure-invariant direct methods |
Least-squares matrix: full | Secondary atom site location: difference Fourier map |
R[F2 > 2σ(F2)] = 0.035 | Hydrogen site location: inferred from neighbouring sites |
wR(F2) = 0.071 | All H-atom parameters refined |
S = 1.01 | w = 1/[σ2(Fo2) + (0.0095P)2] where P = (Fo2 + 2Fc2)/3 |
750 reflections | (Δ/σ)max = 0.030 |
63 parameters | Δρmax = 0.56 e Å−3 |
0 restraints | Δρmin = −0.67 e Å−3 |
V2O2F4(H2O)2·H2O | V = 664.5 (6) Å3 |
Mr = 263.93 | Z = 4 |
Monoclinic, C2/c | Mo Kα radiation |
a = 14.453 (8) Å | µ = 2.87 mm−1 |
b = 4.8879 (19) Å | T = 173 K |
c = 9.663 (5) Å | 0.06 × 0.04 × 0.03 mm |
β = 103.24 (2)° |
Rigaku SCXmini diffractometer | 750 independent reflections |
Absorption correction: multi-scan (REQAB; Rigaku, 1998) | 585 reflections with I > 2σ(I) |
Tmin = 0.742, Tmax = 1.000 | Rint = 0.115 |
3138 measured reflections | 1080 standard reflections every 1 reflections |
R[F2 > 2σ(F2)] = 0.035 | 0 restraints |
wR(F2) = 0.071 | All H-atom parameters refined |
S = 1.01 | Δρmax = 0.56 e Å−3 |
750 reflections | Δρmin = −0.67 e Å−3 |
63 parameters |
Geometry. All s.u.'s (except the s.u. in the dihedral angle between two l.s. planes) are estimated using the full covariance matrix. The cell s.u.'s are taken into account individually in the estimation of s.u.'s in distances, angles and torsion angles; correlations between s.u.'s in cell parameters are only used when they are defined by crystal symmetry. An approximate (isotropic) treatment of cell s.u.'s is used for estimating s.u.'s involving l.s. planes. |
Refinement. Refinement of F2 against ALL reflections. The weighted R-factor wR and goodness of fit S are based on F2, conventional R-factors R are based on F, with F set to zero for negative F2. The threshold expression of F2 > 2σ(F2) is used only for calculating R-factors(gt) etc. and is not relevant to the choice of reflections for refinement. R-factors based on F2 are statistically about twice as large as those based on F, and R- factors based on ALL data will be even larger. |
x | y | z | Uiso*/Ueq | ||
V1 | 0.18501 (4) | 0.19656 (10) | 0.61917 (6) | 0.00822 (18) | |
F1 | 0.19765 (13) | 0.4512 (4) | 0.4665 (2) | 0.0113 (4) | |
F2 | 0.21071 (14) | −0.1169 (4) | 0.7467 (2) | 0.0125 (4) | |
O1 | 0.10702 (19) | −0.0680 (5) | 0.4776 (3) | 0.0133 (6) | |
O2 | 0.09784 (17) | 0.3392 (4) | 0.6657 (3) | 0.0136 (5) | |
O3 | 0.0000 | 0.1972 (8) | 0.2500 | 0.0137 (8) | |
H1 | 0.127 (3) | −0.201 (9) | 0.467 (5) | 0.027 (14)* | |
H2 | 0.070 (3) | −0.001 (10) | 0.403 (5) | 0.036 (14)* | |
H3 | 0.033 (3) | 0.292 (8) | 0.230 (6) | 0.037 (16)* |
U11 | U22 | U33 | U12 | U13 | U23 | |
V1 | 0.0096 (3) | 0.0066 (3) | 0.0085 (3) | 0.0004 (2) | 0.0022 (2) | 0.0001 (2) |
F1 | 0.0159 (11) | 0.0086 (9) | 0.0100 (10) | 0.0018 (7) | 0.0042 (9) | 0.0012 (8) |
F2 | 0.0149 (10) | 0.0092 (9) | 0.0119 (12) | 0.0009 (7) | 0.0004 (9) | 0.0039 (8) |
O1 | 0.0166 (14) | 0.0084 (13) | 0.0132 (15) | 0.0010 (11) | 0.0001 (11) | −0.0019 (12) |
O2 | 0.0137 (11) | 0.0114 (12) | 0.0157 (15) | 0.0022 (9) | 0.0035 (11) | −0.0009 (10) |
O3 | 0.0150 (18) | 0.0108 (17) | 0.015 (2) | 0.000 | 0.0032 (16) | 0.000 |
V1—O2 | 1.592 (2) | V1—O1 | 2.027 (3) |
V1—F2 | 1.948 (2) | V1—F1ii | 2.174 (2) |
V1—F1 | 1.971 (2) | F1—V1ii | 2.174 (2) |
V1—F2i | 1.972 (2) | F2—V1iii | 1.972 (2) |
O2—V1—F2 | 102.39 (11) | F2i—V1—O1 | 164.14 (10) |
O2—V1—F1 | 98.60 (11) | O2—V1—F1ii | 171.78 (11) |
F2—V1—F1 | 159.00 (9) | F2—V1—F1ii | 85.83 (8) |
O2—V1—F2i | 98.46 (11) | F1—V1—F1ii | 73.18 (8) |
F2—V1—F2i | 86.65 (5) | F2i—V1—F1ii | 81.86 (9) |
F1—V1—F2i | 90.68 (9) | O1—V1—F1ii | 83.84 (10) |
O2—V1—O1 | 96.67 (13) | V1—F1—V1ii | 106.82 (8) |
F2—V1—O1 | 85.48 (11) | V1—F2—V1iii | 141.81 (11) |
F1—V1—O1 | 91.75 (11) |
Symmetry codes: (i) −x+1/2, y+1/2, −z+3/2; (ii) −x+1/2, −y+1/2, −z+1; (iii) −x+1/2, y−1/2, −z+3/2. |
Experimental details
Crystal data | |
Chemical formula | V2O2F4(H2O)2·H2O |
Mr | 263.93 |
Crystal system, space group | Monoclinic, C2/c |
Temperature (K) | 173 |
a, b, c (Å) | 14.453 (8), 4.8879 (19), 9.663 (5) |
β (°) | 103.24 (2) |
V (Å3) | 664.5 (6) |
Z | 4 |
Radiation type | Mo Kα |
µ (mm−1) | 2.87 |
Crystal size (mm) | 0.06 × 0.04 × 0.03 |
Data collection | |
Diffractometer | Rigaku SCXmini |
Absorption correction | Multi-scan (REQAB; Rigaku, 1998) |
Tmin, Tmax | 0.742, 1.000 |
No. of measured, independent and observed [I > 2σ(I)] reflections | 3138, 750, 585 |
Rint | 0.115 |
(sin θ/λ)max (Å−1) | 0.646 |
Refinement | |
R[F2 > 2σ(F2)], wR(F2), S | 0.035, 0.071, 1.01 |
No. of reflections | 750 |
No. of parameters | 63 |
H-atom treatment | All H-atom parameters refined |
Δρmax, Δρmin (e Å−3) | 0.56, −0.67 |
Computer programs: CrystalClear (Rigaku, 2004), SHELXS97 (Sheldrick, 2008), SHELXL97 (Sheldrick, 2008), DIAMOND (Brandenburg, 2009), WinGX (Farrugia, 2012) and PLATON (Spek, 2009).
Compound | Bond | Bond length |
(I) | V1═O2 | 1.592 (2) |
V1—F1 | 2.174 (2) | |
V1—O1 | 2.027 (3) | |
cis-(II) | V2═O3 | 1.641 (3) |
V2—F5 | 2.084 (3) | |
V2—O4 | 2.035 (3) | |
trans-(II) | V1═O1 | 1.606 (3) |
V1—F3 | 1.960 (2) | |
V1—O2 | 2.305 (3) | |
(III) | V1═O1 | 1.551 (2) |
V1—F1 | 1.972 (2) | |
V1—F3 | 2.294 (2) |
Atom | Σ s(ij) | Atom | Σ s(ij) |
V1 | 3.942 | F2 | 0.477b |
O2 | 1.676a | O1 | 0.517a |
F2 | 0.514b | F1 | 0.276b |
F1 | 0.482b |
Note: s(ij) values calculated for B = 0.37. References: (a) Brown & Altermatt (1985); (b) Brese & O'Keeffe (1991). |
Compound | V—V inter-layer | V—V edge-shared | V—V corner-shared |
(I) | 5.650 (8) | 3.330 (2) | 3.704 (5) |
(III) | 5.070 (6) | 3.131 (4) | 3.871 (3) |