Advances in Condensed Matter Physics

Volume 2013 (2013), Article ID 297504, 7 pages

http://dx.doi.org/10.1155/2013/297504

Research Article

Spectral Investigation of Crystalline (CuHPO₄, Cu₂P₄O12, and Cu₂P₈O₂₂) and Glassy Copper Phosphates

Christiane Günther,1,2 Dörte Stachel,¹ and Lydia D. Bogomolova³

¹Otto-Schott-Institute, Friedrich-Schiller-University Jena, Fraunhoferstraße 6, 07745 Jena, Germany

²Fraunhofer IKTS-Institute for Ceramic Technologies and Systems, Michael-Faraday-Straße 1, 07629 Hermsdorf, Germany

³Skobel’tsyn Research Institute of Nuclear Physics, Moscow State University, Vorob’evy Gory, Moscow 119992, Russia

Received 2 May 2013; Accepted 17 July 2013

Academic Editor: Victor V. Moshchalkov

Copyright © 2013 Christiane Günther et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

Emerald green crystals of the new composition CuHPO₄ were synthesized and compared to (copper metaphosphate) Cu₂P₄O₁₂ and (copper ultraphosphate) Cu₂P₈O₂₂. Various copper ultraphosphate and metaphosphate glasses of different compositions between pure P₂O₅ and Cu₂P₄O₁₂ were melted in crucibles or in evacuated and sealed silica ampoules at 1473 K or 1373 K for 2 hrs. The UV-VIS-spectra and the IR-spectra of all crystals and glasses were measured and compared. The absorption band of Cu²⁺ was resolved into more component Gaussian bands and differentiated between square-pyramidal and octahedrally coordinated copper. These structural changes are responsible for colour changes from green to turquoise. The infrared spectroscopic properties of the copper phosphate glasses differ between metaphosphate and ultraphosphate structures but show similarities between the crystals and the glasses of the same structure type. EPR studies of some of the glasses show different kinds of spectra, with increasing copper content.

1. Introduction

Orthophosphoric acid condenses to diphosphoric acid under heat treatment. The related salts are called diphosphates (pyrophosphates), which contain P₂O₇ groups, for example, copper hydroxydiphosphate Cu₃[P₂O₆OH]₂ [1] and copper pyrophosphate α-Cu₂P₂O₇ [2]. Further condensation in the presence of cations leads to polyphosphates (short chains) or metaphosphates. Two kinds of metaphosphates, the catena phosphates with 2-corner-linked PO₄ tetrahedra (infinite chains of Q² units) and the cyclophosphates (rings of Q² units), have to be distinguished. In comparison to that, ultraphosphates show linked together Q² and Q³ (2- and 3-corner-linked PO₄ tetrahedra) and build layer or chain structures.

Basically, it is differentiated between nonbonded (Q⁰) monophosphates, primary bonded (Q¹) diphosphates, secondary bonded (Q²) meta- and cyclophosphates, and tertiary bonded (Q³) framework phosphates (pure P₂O₅). Polyphosphates and ultraphosphates are mixed structures (Q¹ and Q², resp., Q² and Q³) of different bonded structural (PO₄) units [3–5].

The copper ion in the copper phosphates is regularly coordinated with four, five, or six oxygen atoms, but most structures consist of tetrahedral or octahedral CuO groups. About twenty different structures of copper phosphates have been discovered to date. The larger family is that of copper monophosphates, which shows a molar ratio of Cu/P = 1. The new structure of CuHPO₄ does belong to this group [3]. The copper polyphosphates with a molar ratio of Cu/P < 1 are much less numerous, for example, the metaphosphate Cu₂P₄O₁₂ and the ultraphosphate Cu₂P₈O₂₂ [4, 6–9].

Phosphate glasses are hygroscopic, but highly resistant against hydrofluoric acid. They can accommodate high concentrations of transition metal ions and remain amorphous. Therefore, invert glasses with more than 50 mol% CuO are possible [10].

Copper phosphate glasses show very interesting electrical and optical properties. So, they can be used as superionic conductors, heat absorbers, solid-state lasers, colour filters, nonlinear optics, or copper releasing degradable phosphate glass fibres, which have potential uses in wound healing or as plant fertilizers [11–14].

With additional water content, the glasses exhibit changes in structure and properties, like density and colour [15–17]. These changes are important for possible applications and need further investigations. According to Bae and Weinberg [10], it is known that by melting, in crucibles a part of the P₂O₅ evaporates during the melting and in spite of that, P₂O₅ can absorb a lot of water. Only pure metaphosphate glasses are relatively stable. So, in this work the metaphosphate glass used for the IR-spectroscopy and the ultraphosphate glasses were melted in silica ampoules, which were sealed under vacuum. Partially, definite amounts of water were added for the investigations. The metaphosphate glasses studied with UV-VIS-spectroscopy were melted in a crucible and cooled under different conditions.

2. Experimental

Phosphoric acid (85%) and copper oxide were mixed in a mortar. This first reaction took several hours. Afterwards, the mixture was tempered at 373 K for a week and further at 503 K for another two days. Cu₂P₄O₁₂ with minor rests of Cu₂P₂O₇ was obtained in the form of a light green to turquoise coloured solid. After one week tempering at 373 K, emerald-green needles of the composition CuHPO₄ grow, if phosphoric acid (65%) is used. By further tempering with residues of H₃PO₄, these needles decompose to Cu₂P₄O₁₂. If the green crystals are kept in the air for several hours, they absorb water, become blue, and decompose to the powder of CuHPO₄·H₂O. The storage in nonaqueous solvents or under vacuum also leads to decomposition, but this time into turquoise powder. So, the crystals are kept in ethanol. The single crystal X-ray analysis of the new CuHPO₄ crystals was published in Günther et al. [3]. The X-ray diffraction of these crystals was performed on a D5000 of Siemens and is given in Figure 1.

Figure 1: XRD pattern of CuHPo₄.

The copper phosphate glasses were prepared of the synthesized Cu₂P₄O₁₂, P₂O5, and partially definite amounts of water. The metaphosphate glasses 1 and 2 were melted in a crucible at 1473 K for 2 hrs and cooled under different conditions. The glasses 3 and 4 were melted in silica ampoules (sealed under vacuum) with slowly cooling. The metaphosphate glass was also melted at 1473 K and the ultraphosphate glasses at 1373 K for 2 h. All those glasses were broken into pieces; the pieces were embedded, cut to plates, and polished for the spectroscopic investigations.

The contents of Cu²⁺ and Cu¹⁺ of some glasses were determined via complexometric titration [18].

The microcrystal spectrometer (Fa. Genuine Jackman Parts, Research School of Chemistry, Australian National University) of the University Bonn (working group of Professor, Dr. R. Glaum) provided the UV-VIS-spectrum of CuHPO₄. A Shimadzu type UV-3101PC was utilized for the other UV-VIS-spectra.

The infrared spectra of the crystals were measured of powdered samples using the KBr pellet technique, with the help of an IFS 66 Spectrometer of Bruker. The spectra of the glasses were calculated from their reflectance spectra by Kramers-Kronig transformation.

The EPR spectra of some glasses were measured using a spectrometer RE-1306 (Russian model) of X band frequency at 298 K. A list of the investigated samples is given in Table 1.

Table 1: List of investigated samples.

Powders

1
CuHPO₄
Copper(II) hydrogen phosphate

2
Cu₂P₄O₁₂
Copper(II) metaphosphate

3
Cu₂P₈O₂₂
Copper(II) ultraphosphate

Glasses

1
50 mol% CuO
Meta, rapidly cooled,

melted in open crucible

2
50 mol% CuO
Meta, slowly cooled,

melted in open crucible

3
17 mol% CuO + 1 mol% H₂O
Ultra, slowly cooled,

melted in ampoule

4
50 mol% CuO
Meta, slowly cooled, melted in ampoule

3. Results and Discussion

3.1. UV-VIS Spectroscopy

The absorption spectra of the regular octahedrally coordinated Cu²⁺ ion show one broadband at 12500 cm⁻¹ due to the transition. The Jahn-Teller effect causes a tetragonal distortion of the structure, which leads to the splitting of the orbital energy levels. So, three energy transitions are possible , , and [18].

The absorption band of the octahedrally coordinated Cu²⁺ of the turquoise crystals of copper metaphosphate (Cu₂P₄O₁₂) is found in the range between 8000 cm⁻¹ and 13000 cm⁻¹ (Figure 2). In the same range lies the broad Cu²⁺ band of the octahedrally bonded copper ultraphosphate (Cu₂P₈O₂₂) [19]. This broad band can be resolved into three-component Gaussian absorption bands at 8900 cm⁻¹, 10200 cm⁻¹, and 12600 cm⁻¹, due to the three energy transitions. One strong band at 10200 cm⁻¹ and weaker ones at lower and higher wavenumbers are refined [15–17].

Figure 2: Absorbance spectra of CuHPo₄ and Cu₂P₄O₁₂.

The copper of the emerald green crystals of copper hydrogen phosphate (CuHPO₄) is square-pyramidal coordinated, and the absorption band is shifted to higher wavenumbers in the range between 9000 cm⁻¹ and 15000 cm⁻¹ (Figure 2).

In this coordination, two energy transitions are possible and [20]. So, this band was resolved into two-component Gaussian bands centred at 10528 cm⁻¹ and 13233 cm⁻¹, while the second one is slightly stronger (Figure 3).

Figure 3: Peak fitting of the absorbance spectrum of CuHPo₄ (Origin).

The metaphosphate glasses 1 and 2 show shifted maxima and a different form of the Cu²⁺ band in the range between 7000 cm⁻¹ and 16000 cm⁻¹ (Figure 4). Glass 1 was rapidly cooled to the temperature of cold water, and glass 2 was slowly cooled to room temperature (approx. 5 K/min). Thus different kinds of structures were generated. The absorption band of glass 1 is shifted to higher wavenumbers than the band of glass 2, and that of glass 3 is shifted to even lower wavenumbers. So, glass 1 contains the highest part of square-pyramidal coordinated Cu²⁺.

Figure 4: Absorbance spectra of the metaphosphate glasses 1 and 2 and the ultraphosphate glass 3.

The resolved bands for the octahedral and square-pyramidal coordinated Cu²⁺ of the crystals were used to create five-component Gaussian absorption bands for the broad Cu²⁺ band in the glasses. The extinction coefficients of the Cu²⁺ in the crystals were used to estimate the parts of the different coordinations in the glasses. So, it was discovered that in the metaphosphate glass 1 nearly the half of the copper is square-pyramidal coordinated, in glass 2 nearly one-third, and in the ultraphosphate glass at least a quarter. Therefore, the increase of the copper content leads to more square-pyramidal coordinated copper.

Also the colour in the glasses changed slightly. Glass 1 is green, and glasses 2 and 3 are more turquoise. It is assumed that if the glasses are greener, more copper is square-pyramidal connected. One point in this favour is the structure of the emerald green CuHPO₄ crystals. Also rapid cooling leads to more square-pyramidal coordinated Cu²⁺ than slowly cooling.

Furthermore, it can be assumed that the green glasses contain more Cu¹⁺ (up to 4 mol%) than the turquoise ones, because of the stronger tail of the UV absorption edge which extends into the visible spectrum region [21]. Thus, the amount of the square-pyramidal coordinated Cu²⁺ seems to be connected to the amount of Cu¹⁺. Also in all glasses with green colour, certain amounts of water (about 1 mol%) were identified, but the glasses with purposefully added water showed a turquoise colour. Hence, the green colour is connected to water, Cu¹⁺, and a change in the coordination to square-pyramidal coordinated Cu²⁺.

3.2. IR-Spectroscopy

The IR-spectrum of CuHPO₄ exhibits a broad OH band at 3130 cm⁻¹ (Figure 5, Table 2). In the spectrum of Cu₂P₄O₁₂, a weak OH band is also present. This can be due to adsorbed water at the surface or little amounts of additional water in the structure. The IR-spectrum of Cu₂P₈O₂₂ does not show an OH band. The OH bands of the glasses cannot be investigated because the glasses are very hygroscopic and adsorb different amounts of water depending on the humidity and the temperature of the environment. The metaphosphate glasses are more resistant than the ultraphosphate glasses, but nonetheless sensitive. Only a very small band in the range between 1400 cm⁻¹ and 1200 cm⁻¹ is registrated and no band in the range between 800 cm⁻¹ and 700 cm⁻¹ in the spectrum of CuHPO₄. Thus, no ν(P=O)–, asymmetric ν(PO₂)–, and symmetric ν(P–O)-vibrations can be found (Table 2). The structure of this molecule does not allow them, because no pure P=O-groups are present, and to each PO₄ tetrahedron, one hydrogen and one copper ions are bound. Only two bridging oxygens are left for each tetrahedron, from which one is connected to the phosphor atom and one is connected to the copper ion of a neighbouring tetrahedron. The short P–O distance between P1–O4 is related to the P–O–Cu bond (O4–Cu: 2,36 Å) and no real double bond [3, 15–17].

Table 2: Data of the infrared spectra of CuHPO₄, Cu₂P₄O₁₂, Cu₂P₈O₂₂, glass 3 (17 mol% CuO + 1 mol% H₂O (ultra)), and glass 4 (50 mol% CuO (meta)); data in cm⁻¹; s: strong; m: middle; w: weak, b: broad.

CuHPO₄
Cu₂P₄O₁₂
Cu₂P₈O₂₂
Glass 3
Glass 4

ν(OH)
3130 m, b
3410 w, b
—
—
—

ν(P=O), ν as(PO₂)
1214 w
1325 m

1295 m

1279 m
1360 w

1330 m

1300 m
1396 w

1364 s

1310 m

1274 w
1375 w

1326 w

1295 m

1251 s

1211 w

ν s(PO₂)
1113 m

1065 m
1130 w

1100 w
1190 w

1150 m

1140 w

1110 m
1167 w

1109 m
1166 w

1116 m

ν as(P–O)
1043 s

1005 s

914 m
1042 s

1013 m
1030 w

995 m

960 s

930 s
1046 m

1003 m

955 s

939 w
1062 s

992 m

944 m

919 w

ν s(P–O)
—
725 m, b
760 m

750 w

710 m

690 m

640 m
760 m, b

670 m, b
750 m, b

Deformation vibration
611 w

578 m

544 w

571 m
578 w

562 m

521 m

498 m

461 w
570 w

550 m

500 s

470 s

440 m

410 w
470 m, b
510 m, b

Figure 5: IR-spectra of the crystals of CuHPo₄, Cu₂P₄O₁₂, Cu₂P₈O₂₂, the ultraphosphate glass 3, and the metaphosphate glass 4.

The IR-spectra of the crystals of Cu₂P₄O₁₂ and Cu₂P₈O₂₂ show a lot of bands in all the ranges between 1400 cm⁻¹ and 400 cm⁻¹. Both structures contain (P=O)-groups and a multitude of different structure elements. The metaphosphate (Cu₂P₄O₁₂) crystal structure is built up of Q²-bonded rings and the ultraphosphate (Cu₂P₈O₂₂) crystal structure of Q²- and Q³-bonded layers of 10-membered rings. The additional Q³ bonds lead to even more bands in the spectrum of Cu₂P₈O₂₂.

The spectra of the glasses exhibit much broader bands than the crystals. The symmetric ν(P–O)-vibrations and the deformation vibrations in the range between 850 cm⁻¹ and 400 cm⁻¹ are very similar in all glasses and can be compared to that ones in Cu₂P₄O₁₂ and Cu₂P₈O₂₂ crystals. The most differences in the spectra of the glasses appear in the range between 1400 cm⁻¹ and 850 cm⁻¹ [21]. So, these band complexes were separated with the help of Gaussian fitting (Table 2). In this range, the spectrum of the ultraphosphate glass 3 exhibits a similar trend to the spectrum of the ultraphosphate crystals (Cu₂P₈O₂₂), although the metaphosphate glass 4 shows similarities to the metaphosphate crystals (Cu₂P₄O₁₂). Accordingly, the structures of the glasses can be compared to those of the crystals.

3.3. EPR

The EPR spectra could be categorized into four types. The metaphosphate glasses 1 and 2 showed type I spectra (Figure 6). The copper content in these two glasses is very high, and so the spectra show a very broad line with and peak-to-peak width  G for glass 1 (green) and and  G for glass 2 (turquoise). The number of Cu²⁺ ions contributed to the EPR spectra is about 25% of the total amount of the introduced copper. The rest of the copper might form copper clusters or crystalline units with antiferromagnetic interactions between the Cu²⁺ ions, which do not contribute to the EPR spectra. The metaphosphate glasses were melted under oxidising atmosphere (air), so the reduction from the Cu²⁺ of Cu₂P₄O₁₂ to Cu⁰ and Cu¹⁺ is very unlikely. Besides Cu⁰ would change the colour of the glasses to red [22]. The ultraphosphate glasses were melted under vacuum (in sealed ampoules), so the reduction of Cu²⁺ to Cu¹⁺ is principally possible. But the formation of Cu⁰ is unlikely, due to the colour of the glasses. Ulraphosphate glasses with a copper concentration in a middle range (between 10 and 30 mol% CuO) exhibit a very narrow single symmetric Lorentzian line of the type II spectra with and  G (Figure 7). The shape and width of this line indicate the exchange interactions among Cu²⁺ ions in a common spin system. Here, the number of Cu²⁺ ions contributed to the EPR spectra adds up to 20–30%. The highest number was obtained for a glass containing 10 mol% H₂O. Hence, additional water increases the number of Cu²⁺ ions which contribute to the spectra.

Figure 6: EPR spectrum type I (metaphosphate glasses, 50 mol% CuO).

Figure 7: EPR spectrum type II (10–30 mol% CuO). Black spectrum experimental, red spectrum calculated.

The structure of spectrum type III (Figure 8) lies between the types I and II. It shows a single line broadened because of spin-spin interactions in a united spin system with higher Cu²⁺ concentrations. This type occurs for copper ultraphosphate glasses with a higher copper content (>30 mol% CuO). The number of Cu²⁺ ions contributed to the EPR spectra increases to >45 %. The -factor is with slightly smaller than that for spectrum type II and bigger than that for type I and the peak-to-peak width  G is bigger than that for type II and smaller than that for type I. Subsequently the -factor decreases with increasing the copper content, and the peak-to-peak width decreases.

Figure 8: EPR spectrum type III (>30 and <50 mol% CuO).

Ultraphosphates with a small copper content (<10 mol% CuO) change the shape of their spectra in comparison to the other glasses (Figure 9). Spectrum type 4 is the superposition of two spectra. Both spectra belong to Cu²⁺, but probably in different coordination states, which could be different kinds of octahedrally distortion or another coordination like square pyramidal.

Figure 9: EPR spectrum type IV (<10 mol% CuO).

One of the spectra exhibits a four-component hyperfine structure (HFS) for parallel orientation and a structureless peak for perpendicular orientation. The second spectrum is Lorentzian single line similar to spectrum type II. The measured data vary for the -factor only slightly between and and for the peak-to-peak width between  G and  G. The ratio () of the integrated intensity of the structureless line to that of the HFS spectrum of the last HFS spectrum accounts to 71 : 1 for a turquoise glass without water and to 167 : 1 for a green glass with about 1 mol% water and a certain amount of Cu¹⁺.

The experimental spectra were fitted to simulated ones to determine the spectral parameters of Cu²⁺ [23, 24]. The simulated spectra were calculated computing spin Hamiltonian of an axial symmetry with electron spin and nuclear spin [25]

The best HFS fit parameters of all samples were  cm⁻¹,  cm⁻¹, , and .

The EPR investigations are much more accurate and higher resolving for small copper contents. Therefore, only for glasses with less than 10 mol% CuO, different Cu²⁺ coordinations could be detected.

4. Summary

The crystals of CuHPO₄, Cu₂P₄O₁₂, and Cu₂P₈O₂₂ were compared to copper phosphate glasses. Some of the glasses were prepared in crucibles and the others in evacuated and sealed silica ampoules. The glasses show similar optical properties to the crystals. The Cu²⁺ band in the UV-VIS-spectra was investigated for square-pyramidal and octahedrally coordinated structures. These structures were compared to the glasses, which show different parts of both coordinations. The colours of the glasses differ from green to turquoise, depending on the coordination, Cu¹⁺ concentration, water content, and cooling procedure of the glasses.

The IR-spectra of the crystals and the glasses can be compared with each other, in spite of the fact that the glasses show much broader bands. The metaphosphate structure is similar in the crystals and the glasses. The same can be observed for the ultraphosphate structure. The most interesting changes from the metaphosphate to the ultraphosphate structure can be found in the range between 1400 cm⁻¹ and 850 cm⁻¹, where the ultraphosphate crystals show much more bands than the metaphosphate crystals. The EPR spectra change with the decreasing copper content, and at least two different coordinated Cu²⁺ ions were found for glasses with less than 10 mol% CuO.

Acknowledgments

The authors thank Professor Dr. R. Glaum and V. Dittrich from the Institute of Inorganic Chemistry of the University Bonn, Germany, for permitting the use of their Microcrystal Spectrometer. The authors also thank C. Apfel from the Institute of Inorganic Chemistry of the Friedrich-Schiller-University Jena, Germany, for the X-ray diffraction. Further, the authors thank Dr. A. Kriltz, M. Ludwig, and H. Süß from the Institute of Physical Chemistry of the Friedrich-Schiller-University Jena, Germany, and Drs. M. Müller, S. Ebbinhaus, B. Hartmann and C. Hertig of the Otto-Schott-Institute from the Friedrich-Schiller-University Jena, Germany, for their kind help and work.

References

R. Baies, V. Caignaert, V. Pralong, and B. Raveau, “Copper hydroxydiphosphate with a one-dimensional arrangement of copper polyhedra: Cu₃[P₂O₆OH]₂,” Inorganic Chemistry, vol. 44, no. 7, pp. 2376–2380, 2005.

B. E. Robertson and V. Calvo, “The crystal structure and phase transformation of -Cu₂P₂O₇,” Acta Crystal-Lographica B, vol. 22, pp. 665–672, 1967.

C. Günther, H. Görls, and D. Stachel, “Copper(II) hydrogenphosphate, CuHPO₄,” Acta Crystallographica Section E, vol. 65, p. i85, 2009.

R. Baies, V. Caignaert, V. Pralong, and B. Raveau, “Copper hydroxydiphosphate with a one-dimensional arrangement of copper polyhedra: Cu₃[P₂O₆OH]₂,” Inorganic Chemistry, vol. 44, no. 7, pp. 2376–2380, 2005.

O. Cozar, N. Vedeanu, D. A. Magdas, and I. Ardelean, “EPR and Raman investigation of some fluoro-calcium phosphate glasses containing copper ions,” Journal of Optoelectronics and Advanced Materials, vol. 10, no. 4, pp. 871–875, 2008.

M. Laugt, J. C. Guitel, I. Tordjman, and G. Bassi, “La structure cristalline du tétramétaphosphate de cuivre, Cu₂P₄O₁₂,” Acta Crystallographica Section B, vol. 28, pp. 201–208, 1972.

A. Olbertz, D. Stachel, I. Svoboda, and H. Fuess, “Crystal structure of copper ultraphosphate, Cu₂P₈O₂₂,” Zeitschrift für Kristallographie, vol. 211, no. 8, pp. 551–552, 1996.

M. T. Averbuch-Pouchot and A. Dur, “Crystal chemistry of ultraphosphates,” Zeitschrift für Kristallographie, vol. 201, no. 1-2, pp. 69–92, 1992.

G. D. Khattak, E. E. Khawaja, L. E. Wenger et al., “Composition-dependent loss of phosphorus in the formation of transition-metal phosphate glasses,” Journal of Non-Crystalline Solids, vol. 194, no. 1-2, pp. 1–12, 1996.

B. S. Bae and M. C. Weinberg, “Oxidatio-reduction equilibrium in copper phosphate glass melted in air,” Journal of the American Ceramic Society, vol. 74, no. 12, pp. 3039–3045, 1991.

W. Vogel, Glaschemie, Springer, New York, NY, USA, 3rd edition, 1992.

E. Metwalli, M. Karabulut, D. L. Sidebottom, M. M. Morsi, and R. K. Brow, “Properties and structure of copper ultraphosphate glasses,” Journal of Non-Crystalline Solids, vol. 344, no. 3, pp. 128–134, 2004.

M. A. Azooz, H. A. Elbatal, K. Elbadry, M. Abd ElMoneim, and S. M. ElAshry, “Preparation and application of some phosphoborosilicate glasses containing micronutrients as plant fertilisers,” Glass Technology, vol. 47, no. 6, pp. 164–166, 2006.

A. Duran and F. J. Valle, “Analysis of the different states of oxidation of copper in glasses: redox equilibrium,” Glass Technology, vol. 26, no. 4, pp. 179–185, 1985.

K. Meyer, A. Barz, and D. Stachel, “Effects of atmospheric humidity on the infrared reflectivity of vitreous P₂O₅ and ultraphosphate glasses,” Journal of Non-Crystalline Solids, vol. 191, no. 1-2, pp. 71–78, 1995.

D. Stachel and A. Barz, “Structure investigations of ultraphosphate glasses with some water content,” Journal of Physics and Chemistry of Solids, vol. 68, no. 5-6, pp. 1021–1023, 2007.

D. Stachel, A.-K. Hoffmann, and S. Ruck, “Sructure formation by H₂O and O (=Cu and Co) in ultraphosphate glasses with low cation contents,” Glass Science and Technology, vol. 75, no. C2, pp. 469–472, 2002.

B.-S. Bae and M. C. Weinberg, “Optical absorption of copper phosphate glasses in the visible spectrum,” Journal of Non-Crystalline Solids, vol. 168, no. 3, pp. 223–231, 1994.

R. Glaum, M. Weil, and D. Ozalp, “Beiträge zum thermischen Verhalten und zur Kristallchemie von wasserfreien Phosphaten. XV. Darstellung, Kristallstruktur und Eigenschaften von Kupfer(II)-ultraphosphat CuP₄O₁₁ ( Cu₂P₈O₂₂),” Zeitschrift für Anorganische und Allgemeine Chemie, vol. 622, no. 11, pp. 1839–1846, 1996.

A. F. Holleman and E. Wiberg, Lehrbuch der Anorganischen Chemie, Walter de Gruyter & Co., Berlin, Germany, 101st edition, 1995.

K. Meyer, A. Barz, and D. Stachel, “Effects of atmospheric humidity on the infrared reflectivity of vitreous P₂O₅ and ultraphosphate glasses,” Journal of Non-Crystalline Solids, vol. 191, no. 1-2, pp. 71–78, 1995.

J. Sułowska and I. Wacławska, “Structural role of Cu in the soil active glasses,” Processing and Application of Ceramics, vol. 6, no. 2, pp. 77–82, 2012.

F. Gonella, F. Caccavale, L. D. Bogomolova, and V. A. Jachkin, “Application of electron paramagnetic resonance to the study of Cu²⁺ ions in Cu-Na ion-exchanged glasses,” Applied Physics A, vol. 68, no. 5, pp. 539–546, 1999.

V. N. Bagratashvili, L. D. Bogomolova, V. I. Gerasimova et al., “Doping of nanoporous glasses by supercritical fluid impregnation of β-diketonate Cu,” Journal of Non-Crystalline Solids, vol. 345-346, pp. 256–259, 2004.

H. Imagawa, “ESR studies of cupric ion in various oxide glasses,” Physica Status Solidi (B), vol. 30, no. 2, pp. 469–478, 1968.