Critical Evaluation and Thermodynamic Optimization of the Cu-Zn, Cu-Se and Zn-Se Binary Systems

: In our study, a complete review of the literature, critical evaluation and thermodynamic assessment of the Cu-Zn, Cu-Se and Zn-Se binary systems were carried out. The modiﬁed quasi-chemical model (MQM) was applied to describe the Gibbs energy of the liquid phase. The Gibbs energies of all intermetallic compounds and terminal solid solutions were described using the compound energy formalism (CEF) model. The re-optimization of the Cu-Zn binary system was carried out by considering the ordered bcc_B2 crystal structure of the β ’ phase. Moreover, the β and δ phases in the Cu-Zn binary system with the same bcc_A2 crystal structure were modeled as one single phase in the present work. A self-consistent thermodynamic database was constructed for the Cu-Zn, Cu-Se and Zn-Se binary systems, work that formed part of a comprehensive thermodynamic database development project researching zinc-based biodegradable materials.


Introduction
Zinc-based alloys are a new kind of biodegradable material proposed by researchers.Zinc plays a vital role in the human body and is actively involved in constructing many mechanisms and functions, such as cell proliferation and bone metabolism [1].Zincbased alloys deserve to be regarded as a new exciting research field because of their moderate corrosion rate [2].A review of zinc-based alloys has been conducted, focusing on the exploration of their cytotoxicity, biocompatibility, processing, corrosion rate and mechanical properties [3][4][5][6][7].Recently, some new kinds of zinc-based alloys, such as porous zinc scaffolds, have been developed [8,9].A new generation of Zn-Cu binary alloys have been investigated as biodegradable cardiovascular implant materials, which show good antibacterial properties against Staphylococcus aureus, with Cu concentrations greater than 2 wt.% according to in vitro experimental results [10].Xiao et al. [11] provided a detailed description of Zn-Ag alloys as biodegradable materials and reviewed a series of advances in related research fields.Su et al. [12] concluded that zinc-based ceramic biomaterials are being developed as synergistic nanocomposite platforms that can combine cancer targeting, bio-imaging and responsive drug delivery with other potential applications.Jones et al. [13] evaluated the prospects of zinc-based applications in wound closure devices (e.g., absorbable sutures, staples, surgical staples, etc.).Yuan et al. [14] provided an outlook on the prospects of designing bio-functionalized coatings on the surface of zinc-based brain transfer materials.Since the degradation behavior of alloys in vivo affects their mechanical integrity and even their biocompatibility, and affects bioactivity directly through degradation products, Li et al. [15] conducted a study on the choice of extraction media and its effects on the cytotoxicity of zinc and its alloys.However, the main problem with zinc-based is their lack of mechanical strength compared to iron-based and magnesium-based alloys, which limits the application of zincbased alloys as implantable materials.Up to now, several series of zinc-based alloys, such as Zn-Mg-based, Zn-Cu-based, and Zn-Mn-based alloys, have been developed.Unfortunately, most zinc-based alloys were not afforded the mechanical properties matched to the human body and ideal biocompatibility.To enhance the mechanical properties of zinc-based alloys, many alloying elements, such as Ag, Ca, Sr, Se, Li, Y etc., were considered in order to improve the strength and toughness of Zn alloys [16][17][18][19].
Copper is a common additive element in Zn-based alloys, with a moderate solid solubility in the zinc matrix.The mechanical properties of Zn alloys can be improved by solution strengthening.Tang et al. [10] reported that adding Cu to zinc-based alloys could improve their tensile strength in research on cardiovascular scaffolds.In addition, the fracture elongation of Zn-based alloys can be improved by increasing their Cu content, which significantly meets the requirements for stent implantation.For example, Bednarczyk et al. [20] reported that the prepared Zn-0.5Cu alloy exhibited superplastic characteristics, and the elongation reached 510% using the ECAP treatment at room temperature.Niu et al. [21] reported that the grains of alloys could be refined clearly with the Cu additive.
Selenium, as one of the essential trace elements in the human body, participates in human metabolism, enhances human immunity, improves physical quality and delays the body aging.The proposed daily intake of selenium for the human body is 60-70 µg/d [22,23].A lack of selenium will cause a decline in human immunity, increasing the incidence of tumors, cardiovascular diseases, liver diseases, and so on.Among its characteristics, the antioxidant properties of selenium protein play an important role in maintaining the cardiovascular system and skeletal muscles, which can effectively protect the cardiovascular system and repair muscle [24,25].Selenium also has a protective effect on oxidative stress and anti-defense systems in the kidney, according to some experimental animal model test results [26][27][28].Therefore, selenium can be regarded as a potential candidate additive element for the development of Zn-based medical materials.However, only a few studies have reported on the application of selenium in medical alloys as so far.Persaud-Sharma et al. [29] studied the application of Se to Mg-Zn-based alloys in cardiovascular stents.They pointed out that the elastic modulus of the alloy can be adapted to the cardiovascular system due to the addition of Se.
Although the secondary phase and solution strengthening are important for improving the properties of Zn-based alloys, information on the thermodynamic modeling phase equilibria of Zn-Cu-Se system has rarely been investigated.To design new Zn-Cu-Se alloys and investigate the relationship between their microstructure and mechanical properties, knowledge of the accurate phase equilibria in the Zn-Cu-Se systems is required.However, obtaining such results only through experiments is often complicated and expensive.Therefore, the best economic approach is to systematically obtain the thermodynamic properties of multi-component systems by the calculation of phase diagrams (CALPHAD) [30].Our goal was to construct a thermodynamic database for calculating the phase equilibria of Zn-based multicomponent systems using the CALPHAD method.The modified quasi-chemical model (MQM) for the liquid phase was used, which can better describe the short-range ordered behavior in the liquid solution compared to the Bragg-Williams model (BMW) and associated model (AM) [31].For the solid solutions, the compound energy formalism (CEF) was used to describe the Gibbs free energy functions, according to the sub-lattice structure [32].
In the present work, a complete literature review, critical evaluation and thermodynamic assessment of the Cu-Zn, Cu-Se, and Zn-Se binary systems were carried out using the CALPHAD approach [30].This is a part work of our group's wider development project of a thermodynamic database for zinc-based multicomponent system, which could benefit the development of zinc-based biodegradable materials.

Critical Review of the Experimental Literature Data 2.1. Cu-Zn Binary System
There are many thermodynamic investigations on solid and liquid alloys of the Cu-Zn binary system.However, the experimental data is significantly scattered.The data on the phase equilibria and thermodynamic properties of Cu-Zn binary systems available in the literature were critically evaluated and re-optimized in the present work.
There are already several thermodynamic descriptions of the Cu-Zn binary system in the literature [44][45][46][47][48][49][50].Spencer [44] published the first one in 1986.Later, Kowalski and Spencer [45] carried out a better thermodynamic evaluation, fitting well with the experimentally assessed phase diagram except for the Zn-rich corner [43].This thermodynamic description was accepted in the COST507 (COST531) database [51].To facilitate the description of ternary Al-Cu-Zn systems, Liang and Chang [46] simplified the description of the γ (Cu 5 Zn 8 ) phase from a four-sub-lattice to a single sub-lattice model.Based on the COST507 database [52], David et al. [47] modified the thermodynamic description, adopting their own electromotive force (EMF) measurements of Zn-rich alloys.Gierlotka and Chen [48] provided two sets of thermodynamic descriptions by considering or disregarding the β (bcc_A2)/β (bcc_B2) disorder-order transition.However, the ordered β (bcc_B2) phase and disordered β (bcc_A2) phase were treated as two separated phases.They also introduced the concept of temperature dependence for the enthalpy during the mixing of the liquid phase based only on the derived experimental enthalpy data, which was not reasonable.To combine it with the γ (Cu 5 Zn 8 ) phase in Al-Cu system, Wang et al. [49] changed the model of the γ (Cu 5 Zn 8 ) phase to be (Zn) 4 (Cu, Zn) 1 (Cu, Zn) 8 based on the COST507 database [51], which was modeled as (Al) 4 (Al, Cu) 1 (Cu) 8 .The model of (Al) 4 (Al, Cu) 1 (Cu) 8 for the γ (Cu 5 Zn 8 ) phase in the Al-Cu system was only used to constrain the composition range of the γ (Cu 5 Zn 8 ) phase and did not consider any information on the crystal structure.Similar to Wang et al. [49], Liang et al. [50] re-optimized the Cu-Zn system to build a comprehensive thermodynamic description of the ternary Al-Cu-Zn system.In their paper, the four-sub-lattice model for the γ(Cu 5 Zn 8 ) phase was simplified to be (Cu) 4 (Cu, Zn) 6 (Cu, Zn) 16 , without considering its realistic crystal structure.In addition, the δ phase was modeled as a separate phase by Liang et al. [50], which was modeled as the same phase, BCC_A2, in the previous assessment [44][45][46]48,49].
In summary, after carefully evaluating all the previous thermodynamic descriptions, we found that none of the thermodynamic descriptions of the Cu-Zn binary system could be directly extrapolated to multi-component systems because of the inconsistent models, which prevents the construction of databases of multicomponent systems for the purpose of high-throughput computational material design.
The crystal structure of the cubic γ phase in the Cu 5 Zn 8 prototype structure is a highly complex one, which stabilizes over a relatively wide composition range.The unit cell contains 52 atoms occupying four sets of sites denoted by 8c, 8c, 12e and 24g (Wyckoff notation).The distribution of the Cu and Zn atoms over all the sites was investigated by Bradley et al. [52] using the XRD technique in 1931, Heidenstam et al. [53] using neutron diffraction in 1968 and Gourdon et al. [54] using neutron and XRD diffraction in 2007.Mixing Cu and Zn on all four sub-lattices, eliminated by Heidenstam et al. [53], fostered a rather poor agreement with the diffraction data.Thus, the evidence for the atomic distribution of Cu and Zn is not conclusive.The mixing of Cu and Zn at site 8c has been accepted by Kowalski and Spencer [45].Based on the experimental results of Gourdon et al. [54], Cu and Zn atoms prefer to substitute at the M3 (12e) and M4 (24g) sites.In this paper, the model (Cu) 2 (Zn) 2 (Cu, Zn) 3 (Cu, Zn) 6 was used to describe the γ (Cu 5 Zn 8 ) phase based on the crystal structure and atomic distribution information.
The crystal structure of the δ (bcc_A2) phase was first investigated by Schubert and Wall [55], who reported it as cubic structure.Later, Lenz and Schubert [56] corrected this description, adding that the δ (bcc_A2) phase is hexagonal.Degtyareva [57] confirmed that the formation of the hexagonal structure of the δ (bcc_A2) phase is the structural distortion of the body-centered cubic lattice.Thus, the δ phase and the β phase should be modeled the same as the phase bcc_A2.
All the original experimental works on the thermodynamic properties of Cu-Zn binary systems were examined carefully and collected in Table 1.All the directly measured data were used in the present work for the thermodynamic optimization instead of the derived data.A typical case of derived data is that regarding integral enthalpy, obtained from experiments on the temperature dependence of the experimental vapor pressure, or EMF data.These direct data are compiled in Table 1.
The enthalpies of the mixing of liquid Cu-Zn alloys, ∆H liquid m , at 1127 • C [58] and 1100 • C [59] were directly measured by the calorimetry method.The results obtained by Parameswaran [58] when x Zn > 0.5 showed a large deviation.Samson-Himmelstjema [60] calculated the liquid properties at 1000 • C based on their measured enthalpy values of the solid phases at 20 • C.There were significant discrepancies between the different results.
The chemical potentials of Zn in the solid phase in the Cu-Zn system have been intensively studied by the referenced studies [76][77][78][79][80][81].The experimental data on the chemical potentials of Zn in the solid fcc_A1 phase were in agreement with each other at lower Zn concentrations (less than 0.1 at.% Zn), which increasingly diminished with increasing Zn concentrations.The results on the chemical potentials of Zn in the β (bcc_A2) phase determined by Ölander [76] contradicted the values obtained by Seith and Krauss [77] and Hargreaves [78], which showed considerable differences.The available results for γ (Cu 5 Zn 8 ) and hcp_A3 phases were only obtained by Ölander [76].

Cu-Se Binary System
The Cu-rich part of the Cu-Se phase diagram was reviewed by Hansen and Anderko [41] based on previous experimental data.Later, Heyding [82], Bernardini et al. [83], Murray and Heyding [84], Babitsyna et al. [85], Glazov and Kim [86] and Glazov et al. [87] re-investigated the phase diagram of the Cu-Se system in restricted composition ranges.Glazov et al. [88] assessed the phase equilibria of the Cu-Se system accordingly.The liquid phase exhibited two miscibility gaps in the Cu-rich region above 1100 • C [85] and in the Se-rich region above 523 • C [84], respectively.The boundary for the high-temperature miscibility gap at the copper-rich region was determined by [86], which suggested a high critical temperature.The highest temperature area of the liquidus line, in the vicinity of Cu 2 Se, was determined by Glazov et al. [87] (32.5-35.6 at.% Se) using the high-precision differential thermal analysis (DTA) method.The liquid miscibility gap in the Se-rich region is characterized by a high Se vapor pressure.Thus, there is only one data point (98. 2 at.% Se, 963 • C) on the Se-rich side [89].The fcc_A1 terminal solid solution of Cu exhibited negligible solubility of Se, and the rhombohedral terminal solid solution of Se exhibited negligible solubility of Cu.Seven stable phases were reported in the Cu-Se system: β-Cu 2−x Se, α-Cu 2 Se, Cu 3 Se 2 , α-CuSe, β-CuSe, γ-CuSe and CuSe 2 .The lower temperature phase of α-Cu 2 Se was reported to be stable below 123 • C, with a relatively narrow homogeneity range [84].All the compounds in the Cu-Se system, except the β-Cu 2−x Se phase, were stoichiometric, with a negligible homogeneity range.The high-temperature β-Cu 2−x Se was stable between 123 ± 15 • C and 1130 • C, at stoichiometry (x = 0), with a broad homogeneity range extending on the Se side to form a defect compound.The homogeneity range of β-Cu 2−x Se at room temperature was reviewed by Chakrabarti and Laughlin [90].The reported range was approximately between 35.4 and 36.0 at.% Se, corresponding to 0.18 ≤ x ≤ 0.22 in the β-Cu 2−x Se phase.The homogeneity range increased further at higher temperatures.Muhsin [91] measured the homogeneity range of β-Cu 2−x Se at 627 • C, ∆x = 0.012, which was less than the previous measurement value, ∆x = 0.106 at 652 • C, reported by Bernardini [83].
Gattow and Schneidener [92], Askerova et al. [93] and Rau and Rabenau [94] measured the enthalpies of the formation of the compounds α-Cu 2 Se, β-Cu 2−x Se, α-CuSe, Cu 3 Se 2 and CuSe 2 at 298.15 K by the calorimetry method, the EMF method and vapor pressure method.Mills et al. [95] evaluated the data based on the previous experimental results.For β-Cu 2−x Se, the enthalpies of formation were estimated in by [94].Their results were a little scattered, whereas the data evaluated by Mills et al. [95] were reasonable to some extent.The standard entropies of the compounds CuSe 2 , CuSe, Cu 3 Se 2 and Cu 2 Se at 298.15K were reported by Askerova et al. [93], Rau and Rabenau [94] and Mills [95] as well.
Stølen et al. [96] measured the heat capacity of α-CuSe, β-CuSe and γ-CuSe by the adiabatic shield calorimetry method from T = 5 K to 653 K. Heat capacity data for α-Cu 2 Se and β-Cu 2 Se were reported by Kubaschewski and Nolting [97] and Blachnik and Gunia [98].The heat capacity value at 300 K reported by Blachnik and Gunia [98] was too large, and we have doubts about its validity.The heat of the fusion of Cu 2 Se was measured by Murray and Heyding [84] and Glazov and Mendelevich [99].The heat of the γ-CuSe peritectic decomposition and the transformation heat for α-CuSe/β-CuSe were determined by Stølen et al. [96].
For the liquid phase, the activities of Cu and Se at 1100 • C were determined by Blachnik and Bolte [100].Askerova and Yazawa [101] calculated the activities of Cu and Se at 1200 • C and 1150 • C by the Gibbs-Duhem integration.These were difficult to illustrate in the figure because of their very small value.The original experimental results of the thermodynamic properties of the different Cu-Se compounds are presented in Table 2.
Du et al. [102] optimized the Cu-Se system using the associate model for the liquid phase.The calculated heat capacities of Cu 2 Se were not in strong agreement with the experimental data [97,98].Moreover, the β-Cu 2−x Se phase was stable from a high temperature to room temperature.However, in [102], it was only stable above 378 K. Thus, the Cu-Se binary system was re-optimized in the present work.[84,[93][94][95][96][97][98][99][100] on the thermodynamic properties of the Cu-Se system at 298.15 K.

Phases
Experimental Method

Zn-Se Binary System
The Zn-Se system was reviewed by Sharma and Chang [101] and Brebrick and Liu [103].Only one intermediate phase, ZnSe, was reported in the Zn-Se binary system, which is congruently formed.There are three different polymorphs: α-ZnSe, with the zinc blende (sphalerite) structure, which is stable to the melting point; β-ZnSe, with the sodium chloride structure being is stable only at high pressures; and the third form of ZnSe, with the wurtzite structure that is metastable at all temperatures and pressures.However, Okada et al. [104] indicated that α-ZnSe transformed to the wurtzite-type structure at 1411 • C, according to their DTA results.
The melting point of ZnSe was measured at 1515 ± 20 • C by Fischer [105], at 1526 ± 10 • C by Sysoev et al. [106] and at 1522 ± 2 • C by Okada et al. [104].Sharma and Chang [107] assessed the temperature to be 1526 • C. In the present work, the melting point of ZnSe was taken to be 1522 • C. Since the values of Fischer [105] and Sysoev et al. [106] were obtained under high pressure inert gas conditions, the T m may be affected by the deviation from the congruent composition due to the dissociative evaporation of ZnSe.
The liquidus data of the whole Zn-Se binary system have been less rigorously studied.It was determined by [108][109][110][111] only over the range of 0-9 at.%Se, and 68-90 at.%Se and 99-100 at.%Se by [112,113].The liquid miscibility gap and the monotectic reaction in the Zn-ZnSe region were predicted by Sharma and Chang [101] and compared to the similar liquid miscibility gap in the Zn-Te system [114].In the present study, both the experimental results and calculated results by Sharma and Chang [101] were considered.
The mutual solid solubilities of Zn and Se have not been measured, which are most likely negligible.The crystal structures of the solid phases in the Zn-Se system are listed in Table 3.The standard enthalpies and entropies of the formation of α-ZnSe at 298.15 K were reported by Korneeva et al. [115], Wösten et al. [116], Sedgwick [117], Terpilowski et al. [118], Flögel [119], Hassan et al. [120], Kirk et al. [121], Bardi et al. [122], Nasar et al. [123], Brebrick and Liu [103] and Schönherr et al. [124].The original experimental data are all summarized in Table 3.The average standard enthalpies and entropies of formation were calculated giving equal weight to these results, excepting those in [115], which are marked by a star symbol.Chen et al. [125] optimized the Zn-Se system using the associate solution model for the liquid phase.In this study, the Zn-Se system was re-optimized using the MQM model for the liquid phase.The ZnSe phase was treated as a stoichiometric phase in the present work.[115][116][117][118][119][120][121][122][123][124][125] on the standard entropy of the α-ZnSe phase at 298.15 K.

Thermodynamic Modeling
The optimizations of the Cu-Zn, Cu-Se and Zn-Se binary systems were carried out with the Factsage thermodynamic software [126].The thermodynamic parameters of the pure elements were extracted from the SGTE database [127].All phases and their thermodynamic models involved in these binary systems are listed in Table 4.

Liquid Phase
The thermodynamic properties of the liquid phase were modeled with the MQM model developed by Pelton et al. [128,129].The associated notation and detailed description of the MQM model are given in [128,129].The same notations are used in the present work, and a brief description of MQM model is given as follows: Taking the Cu-Zn binary system, for example, the quasi-chemical pair exchange reaction can be considered: where the Cu-Zn pair represents a first-nearest-neighbor pair of atoms.The Gibbs energy change of the formation of one mole of the Cu-Zn pairs with Cu-Cu and the Zn-Zn pairs is ∆g CuZn 2 . Let n Cu and n Zn be the number of moles of Cu and Zn, according to Reaction (1).n CuCu , n ZnZn , and n CuZn be the number of moles of the Cu-Cu, Zn-Zn and Cu-Zn pairs.Z Cu and Z Zn are the coordination numbers of Cu and Zn.Then, the Gibbs energy of the solution is given by: where G 0 Cu and G 0 Zn are the molar Gibbs energies of the pure components Cu and Zn, and ∆S con f ig is the configurational entropy of the mixing, given by randomly distributing the Cu-Cu, Zn-Zn and Cu-Zn pairs in the one-dimensional Ising approximation.The expression for ∆S con f ig is as follows: where X CuCu , X ZnZn and X CuZn are the mole fractions of the Cu-Cu, Zn-Zn and Cu-Zn pairs, respectively.Y Cu and Y Zn are the coordination-equivalent fractions of Cu and Zn, which can be expressed as: Moreover, the following elemental balance equations can be written as follows: It may be noted that there is no exact expression for the configurational entropy in three dimensions.Although Equation ( 3) is only an approximate expression in three dimensions, it is exact one dimensionally (when Z = 2) [128].As explained in [128], one is forced by the approximate nature of Equation ( 3) to use non-exact values for the coordination numbers in order to yield a good fit between the experimental data and the calculated ones.The mathematical approximation of the one-dimensional Ising model of Equation ( 3) can be partially compensated by selecting values of Z Cu and Z Zn which are smaller than the experimental values [130].As is known, the MQM model is sensitive to the ratio of the coordination numbers, but less sensitive to their absolute values.From a practical standpoint, for developing large thermodynamic databases, the values of Z Cu and Z Zn of the order of 6 have been deemed necessary for solutions with a small or medium degree of ordering (i.e., alloy solutions).
The item ∆g CuZn is the model parameter for reproducing the excess Gibbs energy of the Cu-Zn liquid phase, which can be expressed as follows: where g 0 CuZn , g s0 CuZn and g 0t CuZn are the adjustable model parameters, which can be functioned according to the temperature dependence.The s and t are exponential powers, which can be set to 0, 1, 2, and so on.The equilibrium state of the system is obtained by minimizing the total Gibbs energy at a constant elemental composition, temperature and pressure.The equilibrium pair distribution is calculated by setting: This gives the "equilibrium constant" for the "quasi-chemical pair reaction" of Equation (10): Moreover, the model permits Z Cu and Z Zn to vary, with the composition as follows [128]:

Solution Phases
In the present work, the solid phases hcp_Zn, hex_A8, bcc_A2 and fcc_A1 were modeled with the single sub-lattice as (Zn, Cu, Se).The configuration entropy of the Bragg-Williams-type and a sub-regular solution approximations was used for the excess Gibbs energy and the configurational entropy of the Bragg-Williams type.Hillert et al. [32] introduced the CEF model to describe the solid phase Gibbs energy with the sub-lattice, and an ideal mixing on each sub-lattice was assumed.The intermetallic compounds of the binary systems were modeled by using sub-lattice models based on the crystal structure and solid solutions.The definition of the Gibbs energy depended on the appropriate choice of lattice stoichiometry and the mixture of substances in any given lattice.
Taking the β-Cu 2−x Se phase as an example, and the Gibbs energy expression of β-Cu 2−x Se phase, based on the CEF model, which is obtained by mixing the Cu and Se elements on two sub-lattices with a stoichiometric ratio of 2:1 as (Cu, Se) 2 (Cu, Se), the Gibbs energy can be expressed as follows: The y I Cu , y I Se , y Π Cu and y Π Se here represent the positional fractions of Cu and Se on the first and second sub-lattices, respectively.y 0 Cu:Se , y 0 Cu:Cu , y 0 Se:Se , and y 0 Se:Cu are the Gibbs energy of terminal members, respectively.n L i:i:j represents the interaction energy between Cu and Se on the second sub-lattice when the first sub-lattice is taken up by Cu or Se, and n L i:j:i represents the interaction energy between Cu and Se on the first sub-lattice when the second sub-lattice is taken up by Cu or Se.
The sub-lattice formalism applied to the bcc_A2 and bcc_B2 phases was introduced by Dupin and Ansara [131], and the same notations were used in the present work.The Gibbs energy functions of the bcc_A2 and bcc_B2 phases were modeled as one single bcc phase with the combined sub-lattice structures as one single sub-lattice (Cu, Zn) for the disorder part (bcc_A2), and two sub-lattices (Cu, Zn)(Cu, Zn) for the ordered part (bcc_B2).The molar Gibbs energy of the whole bcc phase with these disordered (bcc_A2) and ordered (bcc_B2) parts can be expressed as follows: where G disorder bcc_A2 is the Gibbs energy contribution of the bcc phase from the disordered part (bcc_A2), modeled with a signgle sublattice (Cu, Zn).The Gibbs energy expression of bcc_A2 can be written as follows: The items 0 G bcc_A2 Cu and 0 G bcc_A2 Zn are the Gibbs energy of the pure Cu and Zn with a bcc_A2 crystal structure.n L disorder i,j refers to the interaction parameters of the disordered part of the bcc phase (bcc_A2).
In the equation below, G order bcc_B2 is the Gibbs energy contribution of the bcc phase from the ordered part (bcc_B2), modeled with two sublattices (Cu, Zn)(Cu, Zn).The Gibbs energy of bcc_B2 can be expressed as follows: where 0 L bcc_B2 i,j is the Gibbs energy of the hypothetical compound ij: CuZn, CuCu, ZnCu and ZnZn.Items n L I i,j:i and n L Π i:i,j are the interaction parameters of the ordered part of bcc_B2.Due to the crystallographic symmetry of the bcc_B2 phase, the following relations are introduced: Moreover, relations exist in the parameters between the ordered and disordered solutions, which were used in the present work and were described in detail in [131].

Stoichiometric Intermetallic Compounds
In the present work, the seven intermetallic compounds α-Cu 2 Se, Cu 3 Se 2 , α-CuSe, β-CuSe, γ-CuSe, CuSe 2 and ZnSe were treated as stoichiometric compounds.The Gibbs energy per mole of the formula unit Cu x Se y is expressed as follows: where ∆G Cu x Se y f is the Gibbs energy of the formation per mole of the formula unit Cu x Se y .Because of the sufficiency of the heat capacity data for the compound CuSe [40], the ∆C p of CuSe is given by the formula: where the parameters a, b, c, d, e and f were evaluated in the present work.
The molar Gibbs energies of the pure elements and stoichiometric phases can be described by: where ∆ 298.15KH 0 f is the molar enthalpy of the given substance generated by the pure element (∆ 298.15KH 0 f of the stable element was determined as 0 J•mol at T = 298.15K and the pressure of 101.3kPa, as the reference state), ∆ 298.15KH 0 f is the molar entropy at T = 298.15K and C p is the molar heat capacity.The heat capacity of alloys in the Zn-Se and Cu-Se binary Metals 2022, 12, 1401 13 of 32 systems, which were evaluated by the Neumann-Kopp rule [132], were not reported in the experiment.

Cu-Zn Binary System
The present calculated phase diagram of the Cu-Zn system, compared with the original experimental data from Bauer and Hansen [36], Ruer and Kremers [37] and Parameswaran and Healy [58], is shown in Figure 1.Based on previous experimental results [36], Ruer and Kremers [37] re-investigated the Cu-Zn system using the thermal analysis method.The liquidus data provided by Parameswaran and Healy [58] using the calorimetry method showed a slight difference with [37], especially in the Zn-rich region.Miodownik [43] critically reviewed the experimental phase diagram of the Cu-Zn binary system, omitting the EMF results provided by David et al. [47].Figure 1 represents the calculated phase diagram in this work together with the results of [43].The calculated liquidus curve, located between the illustrations of [37] and [58], fit well with the invariant reaction temperatures of the assessed phase diagram [43], as shown in Figure 1.In addition, the limited thermodynamic information for the boundaries of these phases, fcc_A1, β (bcc_B2), γ (Cu 5 Zn 8 ) and hcp_A3, at the temperature below about 400 • C, illustrated by Hansen and Anderko [41], represented an uncertainty.This is because the present broad-scale optimization work resulted in minor differences from the previously calculated results [45,50].
by Spencer [44] and Liang et al. [50], is shown in Figure 2. The thermodynamic description by Spencer [44] agreed well with the experimentally assessed phase diagram [43], excepting the Zn-rich corner.In the present study, the liquid solution was modeled by the MQM model, and the seven solid solutions were modeled by the CEF model.All the parameters of the thermodynamic models obtained in this work are listed in Tables 5 and 6.A complete comparison of the present work with the previous thermodynamic descriptions [45,47,48,50] and the experimentally assessed basis [43] is provided for the invariant reactions in Table 7.Compared with the experimental data [43], the present calculated phase diagram and invariant reactions show an improvement in the liquidus curve and Zn-rich corner compared with the work of [45], while maintaining the same level of agreement in the rest of the phase diagram.Moreover, Liang et al. [50] determined the γ (Cu5Zn8) phase to be (Cu)4(Cu, Zn)6(Cu, Zn)16, without considering information about the detailed crystal structure.In addition, the δ phase should not be modeled as a separate phase, which has the same bcc_A2 crystal structure as the bcc solution phase.Gierlotka and Chen [48] provided two sets of thermodynamic descriptions by considering or disregarding the β (bcc_A2)/β′ (bcc_B2) disorder-order transition.However, the ordered β′ (bcc_B2) phase and disordered β (bcc_A2) phase were modeled as two separated phases.The ordered β′ phase should be modeled as the ordered part (bcc_B2) of the bcc phase, as discussed above.Therefore, the phases of δ, β and β′, were treated as one single bcc phase.Then, they were modeled with the two parts of the Gibbs energy functions, with (Cu, Zn) for the disordered bcc_A2 part and (Cu, Zn)(Cu, Zn) for the ordered bcc_B2 part.As shown in Figure 1, the present optimized results of the bcc phase are in strong agreement with the available experimental data.Moreover, thanks to the more reliable experimental data in the composition region of 90-98 at.% Zn reported David et al. [47], the modeling of liquidus in the Zn-rich region was improved in the present work.Compared with the original experimental data [36,37,47,58] and previously optimized results [45,47,50], the presently calculated results show a reasonable agreement with the experimental results and other calculated results.The present calculated phase diagram, compared with the previous optimized results by Spencer [44] and Liang et al. [50], is shown in Figure 2. The thermodynamic description by Spencer [44] agreed well with the experimentally assessed phase diagram [43], excepting the Zn-rich corner.In the present study, the liquid solution was modeled by the MQM model, and the seven solid solutions were modeled by the CEF model.All the parameters of the thermodynamic models obtained in this work are listed in Tables 5 and 6.A complete comparison of the present work with the previous thermodynamic descriptions [45,47,48,50] and the experimentally assessed basis [43] is provided for the invariant reactions in Table 7.Compared with the experimental data [43], the present calculated phase diagram and invariant reactions show an improvement in the liquidus curve and Zn-rich corner compared with the work of [45], while maintaining the same level of agreement in the rest of the phase diagram.Moreover, Liang et al. [50] determined the γ (Cu 5 Zn 8 ) phase to be (Cu) 4 (Cu, Zn) 6 (Cu, Zn) 16 , without considering information about the detailed crystal structure.In addition, the δ phase should not be modeled as a separate phase, which has the same bcc_A2 crystal structure as the bcc solution phase.Gierlotka and Chen [48] provided two sets of thermodynamic descriptions by considering or disregarding the β (bcc_A2)/β (bcc_B2) disorder-order transition.However, the ordered β (bcc_B2) phase and disordered β (bcc_A2) phase were modeled as two separated phases.The ordered β phase should be modeled as the ordered part (bcc_B2) of the bcc phase, as discussed above.Therefore, the phases of δ, β and β , were treated as one single bcc phase.Then, they were modeled with the two parts of the Gibbs energy functions, with (Cu, Zn) for the disordered bcc_A2 part and (Cu, Zn)(Cu, Zn) for the ordered bcc_B2 part.As shown in Figure 1, the present optimized results of the bcc phase are in strong agreement with the available experimental data.Moreover, thanks to the more reliable experimental data in the composition region of 90-98 at.% Zn reported David et al. [47], the modeling of liquidus in the Zn-rich region was improved in the present work.Compared with the original experimental data [36,37,47,58] and previously optimized results [45,47,50], the presently calculated results show a reasonable agreement with the experimental results and other calculated results.
This work ZnSe phase, format (Zn)(Se) : This work Figure 3 shows the calculated enthalpy of the mixing of the liquid phase at 900 and 1100 • C, together with the experimental data [58][59][60][61]63,68,70] and previously optimized results [45,48,50].It should be noted that, among all the experimental data, only three sets [58][59][60] were directly measured by the calorimetry method.The other reported values of the enthalpy of the mixing data were derived from the measured vapor pressure and EMF results, which were converted into the chemical potential.Gierlotka and Chen [48] optimized the liquid phase based on the derived data of the enthalpy of the mixing, which presented as relatively high, as shown in Figure 3.The calculated enthalpy in the present work was in strong agreement with the experimental data by Samson-Himmelstjema [60].In addition, the direct experimental data [58,59] are scattered.This may be due to the vapor pressures of the zinc being too high to affect the accuracy of the experimental results.The calculated results in the present work showed reasonable agreement with the experimental data in the Zn-poor region.
Table 7.The calculated invariant reactions in the Cu-Zn system compared with the experimental data from ref. [44] and calculated data from refs.[45,47,48,50].

Reaction
Reaction Type Temperature ( presented as relatively high, as shown in Figure 3.The calculated enthalpy in the present work was in strong agreement with the experimental data by Samson-Himmelstjema [60].
In addition, the direct experimental data [58,59] are scattered.This may be due to the vapor pressures of the zinc being too high to affect the accuracy of the experimental results.
The calculated results in the present work showed reasonable agreement with the experimental data in the Zn-poor region.Figure 5 shows the calculated enthalpies of the formation of the solid phases at 25 °C and 300 °C, compared with the experimental data [60,[71][72][73][74][75].The present calculated results agree well with the experimental data.The formation enthalpy of the ordered β′ (Bcc_B2) phase shows a strong temperature dependence.The presently calculated chemical potential of Zn for the solid phases at 500 °C and 727 °C agrees with the experimental Figure 5 shows the calculated enthalpies of the formation of the solid phases at 25 • C and 300 • C, compared with the experimental data [60,[71][72][73][74][75].The present calculated results agree well with the experimental data.The formation enthalpy of the ordered β (Bcc_B2) phase shows a strong temperature dependence.The presently calculated chemical potential of Zn for the solid phases at 500 • C and 727 • C agrees with the experimental data [76][77][78][79][80][81], as shown in Figure 6.The experimental data for the fcc_A1 phase was scattered.The presently calculated chemical potential of Zn in the β (bcc_A2) and γ (Cu5Zn8) phases at 500 • C are in excellent accordance with the experimental data of Ölander [76].

Cu-Se Binary System
The optimized parameters of the stable phases in the Cu-Se binary system are listed in Tables 5 and 6.The phase equilibria and thermodynamic properties of this system were

Cu-Se Binary System
The optimized parameters of the stable phases in the Cu-Se binary system are listed in Tables 5 and 6.The phase equilibria and thermodynamic properties of this system were

Cu-Se Binary System
The optimized parameters of the stable phases in the Cu-Se binary system are listed in Tables 5 and 6.The phase equilibria and thermodynamic properties of this system were calculated using the optimized parameters, performed using the Factsage software.
The calculated phase diagram, compared with the experimental data [82][83][84][85][86][87] and the optimized results by Du et al. [102], is shown in Figure 7.The present calculated phase diagram agrees well with the available data.The calculated homogeneity range of β-Cu 2−x Se at 627 • C, ∆x = 0.028, is consistent with the results by Muhsin [91].The presently calculated boundaries for the liquid miscibility gap at the Cu-end and the Se-end are in agreement with the experimental results [87,89].The calculated invariant reactions, together with the experimental results and optimized results by Du et al. [100], are all listed in Table 8.As demonstrated in Table 8, the Cu-Se binary system was well reproduced in the present work.Cu2−xSe at 627 °C, Δx = 0.028, is consistent with the results by Muhsin [91].The presently calculated boundaries for the liquid miscibility gap at the Cu-end and the Se-end are in agreement with the experimental results [87,89].The calculated invariant reactions, together with the experimental results and optimized results by Du et al. [100], are all listed in Table 8.As demonstrated in Table 8, the Cu-Se binary system was well reproduced in the present work.Table 8.The calculated invariant reactions in the Cu-Se system compared with the experimental data from ref. [88] and calculated data from ref. [100].

Reaction Reaction Type Temperature (°C)
Composition (Zn at.%) Refs.  Figure 8 shows the standard enthalpy of formation in the Cu-Se system at 25 • C compared with the experimental data [92][93][94][95].The presently optimized results are closer to the experimental data than that of Du et al. [100].The standard entropy of formation at 25 • C, compared with the experimental data [92][93][94][95] and previously optimized results by Du et al. [100], is shown in Figure 9. Compared with the calculated results by Du et al. [100], the results of the present work show better agreement with the experimental data.As shown in Figures 10 and 11, the calculated enthalpy and entropy of mixing at 1127 • C, compared with the calculated results by Du et al. [100], indicate that our calculated results using the MQM model [128,129] are considerably more acceptable.
Table 8.The calculated invariant reactions in the Cu-Se system compared with the experimental data from ref. [88] and calculated data from ref. [100].

Reaction
Reaction Type Temperature ( the experimental data than that of Du et al. [100].The standard entropy of formation at 25 °C, compared with the experimental data [92][93][94][95] and previously optimized results by Du et al. [100], is shown in Figure 9. Compared with the calculated results by Du et al. [100], the results of the present work show better agreement with the experimental data.As shown in Figures 10 and 11, the calculated enthalpy and entropy of mixing at 1127 °C, compared with the calculated results by Du et al. [100], indicate that our calculated results using the MQM model [128,129] are considerably more acceptable.Figure 12 presents the calculated heat capacities of Cu2Se in the Cu-Se system with the experimental data measured by Kubaschewski and Nolting [97] and Blachnik and Gunia [98], and the calculated results by Du et al. [100].The present calculated results are in strong agreement with the experimental data in the present work.Figure 13 shows the calculated heat capacities of CuSe in the Cu-Se system compared with the experimental data measured by [96] and the calculated results by Du et al. [100].The present calculated results show very strong agreement with the experimental data.The calculated activities of Cu and Se at 1100 °C are shown in Figure 14, compared with the experimental data determined by Blachnik and Bolte [102] and the calculated by Du et al. [100].Figure 12 presents the calculated heat capacities of Cu 2 Se in the Cu-Se system with the experimental data measured by Kubaschewski and Nolting [97] and Blachnik and Gunia [98], and the calculated results by Du et al. [100].The present calculated results are in strong agreement with the experimental data in the present work.Figure 13 shows the calculated heat capacities of CuSe in the Cu-Se system compared with the experimental data measured by [96] and the calculated results by Du et al. [100].The present calculated results show very strong agreement with the experimental data.The calculated activities of Cu and Se at 1100 • C are shown in Figure 14, compared with the experimental data determined by Blachnik and Bolte [102] and the calculated by Du et al. [100].
Figure 12 presents the calculated heat capacities of Cu2Se in the Cu-Se system with the experimental data measured by Kubaschewski and Nolting [97] and Blachnik and Gunia [98], and the calculated results by Du et al. [100].The present calculated results are in strong agreement with the experimental data in the present work.Figure 13 shows the calculated heat capacities of CuSe in the Cu-Se system compared with the experimental data measured by [96] and the calculated results by Du et al. [100].The present calculated results show very strong agreement with the experimental data.The calculated activities of Cu and Se at 1100 °C are shown in Figure 14, compared with the experimental data determined by Blachnik and Bolte [102] and the calculated by Du et al. [100].

Zn-Se Binary System
In the present work, the MQM model was used for liquid phase to optimize the Zn-Se binary system.The calculated phase diagram, compared with the experimental data [108,109,111,113] and optimized data [125], is shown in Figure 15, and it is in strong agreement with those data.Moreover, the melting point of ZnTe was optimized to be 1522 °C

Zn-Se Binary System
In the present work, the MQM model was used for liquid phase to optimize the Zn-Se binary system.The calculated phase diagram, compared with the experimental data [108,109,111,113] and optimized data [125], is shown in Figure 15, and it is in strong agreement with those data.Moreover, the melting point of ZnTe was optimized to be 1522 • C in the present work, thus reproducing the results reported by Okada et al. [104].The calculated invariant reactions, together with the assessment results by Sharma and Chang [101] and optimized results by Chen et al. [125], are all listed in Table 9.It is worth noting that the calculated temperature and compositions of the monotectic reaction (Liquid#1 ↔ Liquid#2 + ZnSe) by Chen et al. [125] were inconsistent with the results of Sharma and Chang [101] and our results.Table 9.The calculated invariant reactions in Zn-Se system compared with experimental data from ref. [100] and calculated data from ref. [123].The calculated standard enthalpy and entropy of the formation of ZnSe at 25 • C in this work were compared with the averaged values of experimental results [103, [116][117][118][119][120][121][122][123][124] and the optimized results by Chen et al. [125], and these are listed in Table 3.The present calculated result was slightly lower than that of Chen et al. [125], which was in closer agreement with experimental values.Figure 16 shows the calculated standard enthalpy of the formation of ZnSe at 25 • C, compared with the experimental results [106,118,123,133] and previously optimized results by Chen et al. [125].The present calculated enthalpy showed better consistency with the experimental data [118,123,133].The present calculated standard entropy of the formation of ZnSe at 25 • C, compared with the experimental results [118,123] and previously optimized results by Chen et al. [125], is shown in Figure 17.The present calculated result is slightly different from the experimental results, within the acceptable range.The calculated enthalpy and entropy of mixing for the liquid phase of the Zn-Se system at 1727 °C, compared with the calculated results by Chen et al. [125], are shown in Figures 18 and 19, respectively.The V-shaped enthalpy and M-shaped entropy curves indicate that the liquid phase had a maximum short-range order (SRO) at 50 at.% Se.Moreover, the calculated entropy results in this work are more consistent with the ideal state of the entropy of mixing than those calculated by Chen et al. [125].The calculated enthalpy and entropy of mixing for the liquid phase of the Zn-Se system at 1727 • C, compared with the calculated results by Chen et al. [125], are shown in Figures 18 and 19, respectively.The V-shaped enthalpy and M-shaped entropy curves indicate that the liquid phase had a maximum short-range order (SRO) at 50 at.% Se.Moreover, the calculated entropy results in this work are more consistent with the ideal state of the entropy of mixing than those calculated by Chen et al. [125].The calculated enthalpy and entropy of mixing for the liquid phase of the Zn-Se system at 1727 °C, compared with the calculated results by Chen et al. [125], are shown in Figures 18 and 19, respectively.The V-shaped enthalpy and M-shaped entropy curves indicate that the liquid phase had a maximum short-range order (SRO) at 50 at.% Se.Moreover, the calculated entropy results in this work are more consistent with the ideal state of the entropy of mixing than those calculated by Chen et al. [125].

Conclusions
Critical evaluations and thermodynamic reassessments of the Cu-Zn, Cu-Se and Zn-Se binary systems were conducted in the present work.The MQM method was applied to describe the Gibbs energy of the liquid phase.The Gibbs energies of all the intermetallic compounds and terminal solid solutions were described by the CEF method.
The critical literature assessment and thermodynamic re-optimization of the Cu-Zn binary system were carried out considering the ordered bcc_B2 crystal structure of the β' phase.The β and δ phases with the same bcc_A2 crystal structure were treated as one single phase.The γ(Cu5Zn8) phase was modeled as four sub-lattices based on the information about the crystal structure and atomic distribution.
In the Zn-Se system, two miscibility gaps of the liquid were identified in the Zn-rich and Se-rich regions.Only one intermediate phase, ZnSe, which is congruently formed, was treated as a stoichiometric compound in the present thermodynamic modeling.The Gibbs free energies of each phase were formulated in this work, which allowed the liquids, enthalpies of mixing, entropies of mixing, activities, enthalpies of formation and entropies of formation to be well represented.
A self-consistent thermodynamic database was constructed for the Cu-Zn, Cu-Se and Zn-Se binary systems, which formed part of the wider thermodynamic database research project conducted by our group on Mg/Zn-based multi-component systems [134][135][136][137][138][139].Additionally, it provided reliable data supporting the search for ideal Zn-based biodegradable materials.Moreover, some of the experiments could be argued to verify the phase diagram (the miscibility gap) of the Se-rich part of the Cu-Se system and the Zn-Se system, although such experiments are difficult to perform due to the high volatility of Zn and Se.

Conclusions
Critical evaluations and thermodynamic reassessments of the Cu-Zn, Cu-Se and Zn-Se binary systems were conducted in the present work.The MQM method was applied to describe the Gibbs energy of the liquid phase.The Gibbs energies of all the intermetallic compounds and terminal solid solutions were described by the CEF method.
The critical literature assessment and thermodynamic re-optimization of the Cu-Zn binary system were carried out considering the ordered bcc_B2 crystal structure of the β' phase.The β and δ phases with the same bcc_A2 crystal structure were treated as one single phase.The γ(Cu 5 Zn 8 ) phase was modeled as four sub-lattices based on the information about the crystal structure and atomic distribution.
In the Cu-Se system, two miscibility gaps of the liquid were identified on each side of the compound Cu 2 Se.The intermetallic compounds, Cu 3 Se 2 , α-CuSe, β-CuSe, γ-CuSe, CuSe 2 and α-Cu 2 Se, were treated as stoichiometric compounds.The compound β-Cu 2−x Se, which has a homogeneity range, was treated using a two-sub-lattice model, (Cu, Va) 2 Se.
In the Zn-Se system, two miscibility gaps of the liquid were identified in the Zn-rich and Se-rich regions.Only one intermediate phase, ZnSe, which is congruently formed, was treated as a stoichiometric compound in the present thermodynamic modeling.The Gibbs free energies of each phase were formulated in this work, which allowed the liquids, enthalpies of mixing, entropies of mixing, activities, enthalpies of formation and entropies of formation to be well represented.
A self-consistent thermodynamic database was constructed for the Cu-Zn, Cu-Se and Zn-Se binary systems, which formed part of the wider thermodynamic database research project conducted by our group on Mg/Zn-based multi-component systems [134][135][136][137][138][139].Additionally, it provided reliable data supporting the search for ideal Zn-based biodegradable materials.Moreover, some of the experiments could be argued to verify the phase diagram (the miscibility gap) of the Se-rich part of the Cu-Se system and the Zn-Se system, although such experiments are difficult to perform due to the high volatility of Zn and Se.

Figure 2 .Table 6 .
Figure 2. The calculated phase diagram of the Cu-Zn system compared with the previously optimized data from refs.[45,50].

Figure 3 .
Figure 3.The calculated enthalpy of the mixing of the liquid phase at 900 and 1100 °C in the Cu-Zn system compared with the experimental data from refs.[58-61,63,68,70] and previously optimized calculations data from refs.[45,48,50].

Figure 3 .
Figure 3.The calculated enthalpy of the mixing of the liquid phase at 900 and 1100 • C in the Cu-Zn system compared with the experimental data from refs.[58-61,63,68,70] and previously optimized calculations data from refs.[45,48,50].The present calculated values of the relative chemical potential of Zn in the liquid phase at 627, 927, 1100 and 1200 • C reproduced the experimental results [61-70] very closely, as shown in Figure 4.The relative chemical potential of Zn in the liquid was calculated at different temperatures to compare the different experimental results, which varied only a little in the wide temperature range from 627 • C to 1200 • C.

Figure 4 .
Figure 4.The calculated chemical potential of Zn for the liquid phase at 627, 927, 1100 and 1200 °C in the Cu-Zn system compared with the experimental data [61-70].

Figure 4 .
Figure 4.The calculated chemical potential of Zn for the liquid phase at 627, 927, 1100 and 1200 • C in the Cu-Zn system compared with the experimental data [61-70].

Metals 2022 , 32 Figure 5 .
Figure 5.The calculated standard enthalpies of formation at 25 and 300 °C in the Cu-Zn system compared with the experimental data from refs.[60,71-75].

Figure 6 .
Figure 6.The calculated chemical potential of Zn for the solid phases at 500 and 727 °C in the Cu-Zn system compared with the experimental data from refs.[76-81].

Figure 5 . 32 Figure 5 .
Figure 5.The calculated standard enthalpies of formation at 25 and 300 • C in the Cu-Zn system compared with the experimental data from refs.[60,71-75].

Figure 6 .
Figure 6.The calculated chemical potential of Zn for the solid phases at 500 and 727 °C in the Cu-Zn system compared with the experimental data from refs.[76-81].

Figure 6 .
Figure 6.The calculated chemical potential of Zn for the solid phases at 500 and 727 • C in the Cu-Zn system compared with the experimental data from refs.[76-81].

Figure 7 .
Figure 7.The calculated phase diagram of the Cu-Se system compared with the experimental data from refs.[82-87] and previously optimized results by Du et al. [102].

Figure 7 .
Figure 7.The calculated phase diagram of the Cu-Se system compared with the experimental data from refs.[82-87] and previously optimized results by Du et al. [102].

Figure 8 .
Figure 8.The calculated standard enthalpy of formation at 25 °C in the Cu-Se system compared with the experimental data from refs.[92-95] and previously optimized results by Du et al. [100].

Figure 8 .
Figure 8.The calculated standard enthalpy of formation at 25 • C in the Cu-Se system compared with the experimental data from refs.[92-95] and previously optimized results by Du et al. [100].Metals 2022, 12, x FOR PEER REVIEW 21 of 32

Figure 9 .
Figure 9.The calculated standard entropy of formation at 25 °C in the Cu-Se system compared with the experimental data from refs.[93-95] and previously optimized results by Du et al. [100].

Figure 9 .
Figure 9.The calculated standard entropy of formation at 25 • C in the Cu-Se system compared with the experimental data from refs.[93-95] and previously optimized results by Du et al. [100].

Figure 9 .
Figure 9.The calculated standard entropy of formation at 25 °C in the Cu-Se system compared with the experimental data from refs.[93-95] and previously optimized results by Du et al. [100].

Figure 10 .
Figure 10.The calculated enthalpy of mixing for the liquid phase at 1127 °C in the Cu-Se system compared with previously optimized results by Du et al. [100].

Figure 10 .
Figure 10.The calculated enthalpy of mixing for the liquid phase at 1127 • C in the Cu-Se system compared with previously optimized results by Du et al. [100].Metals 2022, 12, x FOR PEER REVIEW 22 of 32

Figure 11 .
Figure 11.The calculated entropy of mixing for the liquid phase at 1127 °C in the Cu-Se system compared with the previously optimized results by Du et al. [100].

Figure 11 .
Figure 11.The calculated entropy of mixing for the liquid phase at 1127 • C in the Cu-Se system compared with the previously optimized results by Du et al. [100].

Figure 12 . 32 Figure 12 .
Figure 12.The calculated heat capacities of Cu 2 Se in the Cu-Se system compared with the experimental data from refs.[97,98] and previously optimized results by Du et al. [100].

Figure 13 .
Figure 13.The calculated heat capacities of CuSe in the Cu-Se system compared with the experimental data from ref. [96] and previously optimized results by Du et al. [100].

Figure 13 .
Figure 13.The calculated heat capacities of CuSe in the Cu-Se system compared with the experimental data from ref. [96] and previously optimized results by Du et al. [100].

Figure 13 .
Figure13.The calculated heat capacities of CuSe in the Cu-Se system compared with the experimental data from ref.[96] and previously optimized results by Du et al.[100].

Figure 14 .
Figure 14.The calculated activities of Cu and Se at 1100 °C in the Cu-Se system compared with the experimental data from refs.[102] and previously optimized results by Du et al. [100].

Figure 14 .
Figure 14.The calculated activities of Cu and Se at 1100 • C in the Cu-Se system compared with the experimental data from ref. [102] and previously optimized results by Du et al. [100].

Metals 2022 , 32 Figure 15 .
Figure 15.The calculated phase diagram of the Zn-Se system compared with the experimental data from refs.[108,109,111,113] and previously optimized results by Chen et al.[125].

Figure 15 .
Figure 15.The calculated phase diagram of the Zn-Se system compared with the experimental data from refs.[108,109,111,113] and previously optimized results by Chen et al.[125].

Metals 2022 , 32 Figure 15 .
Figure 15.The calculated phase diagram of the Zn-Se system compared with the experimental data from refs.[108,109,111,113] and previously optimized results by Chen et al.[125].

Figure 16 .
Figure 16.The calculated standard enthalpy of formation at 25 °C in the Zn-Se system compared with the experimental data from refs.[106,118,123,133] and previously optimized results by Chen et al.[125].

Figure 16 .
Figure 16.The calculated standard enthalpy of formation at 25 • C in the Zn-Se system compared with the experimental data from refs.[106,118,123,133] and previously optimized results by Chen et al.[125].

Figure 17 .
Figure 17.The calculated standard entropy of formation at 25 °C in the Zn-Se system compared with the experimental data from refs.[118,123] and previously optimized results by Chen et al.[125].

Figure 18 .
Figure18.The calculated enthalpy of mixing at 1727 °C in the Zn-Se system compared with previously optimized results by Chen et al.[125].

Figure 17 .
Figure 17.The calculated standard entropy of formation at 25 • C in the Zn-Se system compared with the experimental data from refs.[118,123] and previously optimized results by Chen et al.[125].

Metals 2022 , 32 Figure 17 .
Figure 17.The calculated standard entropy of formation at 25 °C in the Zn-Se system compared with the experimental data from refs.[118,123] and previously optimized results by Chen et al.[125].

Figure 18 .
Figure18.The calculated enthalpy of mixing at 1727 °C in the Zn-Se system compared with previously optimized results by Chen et al.[125].

Figure 18 .
Figure 18.The calculated enthalpy of mixing at 1727 • C in the Zn-Se system compared with previously optimized results by Chen et al. [125].

Figure 19 .
Figure 19.The calculated entropy of mixing at 1727 °C in the Zn-Se system compared with previously optimized results by Chen et al. [125].

Figure 19 .
Figure 19.The calculated entropy of mixing at 1727 • C in the Zn-Se system compared with previously optimized results by Chen et al. [125].

Table 1 .
Summary of original experimental resultson the thermodynamic properties of the Cu-Zn binary system.

Table 2 .
Summary of the original experimental work

Table 3 .
Summary of the original experimental work [103,

Table 4 .
Structural parameters of the phases and thermodynamic models used in the present work.
ZnCuZn are the values of Z Cu when all the nearest neighbors of a Cu atom are Cu atoms, and when all nearest neighbors of a Cu atom are Zn atoms, respectively.Z Zn ZnZn and Z Zn CuZn are defined similarly.The composition of the maximum short-range ordering (SRO) is determined by the ratio of the coordination numbers Z Cu CuZn /Z Zn CuZn .The values of the coordination numbers chosen in the present study are listed in Table5.