# Thermodynamic Study of Tl6SBr4 Compound and Some Regularities in Thermodynamic Properties of Thallium Chalcohalides

Authors: Dunya Mahammad Babanly; Qorkhmaz Mansur Huseynov; Ziya Saxaveddin Aliev; Dilgam Babir Tagiyev; Mahammad Baba Babanly
Journal: Advances in Materials Science and Engineering
 (2017)

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## Abstract

The solid-phase diagram of the Tl-TlBr-S system was clarified and the fundamental thermodynamic properties of Tl6SBr4 compound were studied on the basis of electromotive force (EMF) measurements of concentration cells relative to a thallium electrode. The EMF results were used to calculate the relative partial thermodynamic functions of thallium in alloys and the standard integral thermodynamic functions (-ΔfG0, -ΔfH0, and S0298) of Tl6SBr4 compound. All data regarding thermodynamic properties of thallium chalcogen-halides are generalized and comparatively analyzed. Consequently, certain regularities between thermodynamic functions of thallium chalcogen-halides and their binary constituents as well as degree of ionization (DI) of chemical bonding were revealed.


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## Body

## 1. Introduction

Chalcohalides ofp-elements are of considerable interest as promising functional materials of modern electronic engineering. Multitude of them exhibit semiconductor, thermoelectric, photoelectric, topological insulator, radiation detector, and magnetic properties [1–3]. Tl6S(Se)I4 ternary compounds are known as effective X-ray and γ-ray detectors, outperforming the current state-of-the-art material for room temperature operation, CdZnTe (CZT) [4, 5]. Given the promising performance of thallium-based chalcogenides and chalcogen-halides, these compounds continue to attract attention despite toxicity of thallium derivatives.Knowledge of phase equilibria and thermodynamic properties of phases is of key importance in designing techniques and optimizing conditions for the fabrication, crystal growth of multicomponent inorganic materials.The investigation of phase equilibria in Tl-X-Hal (X-S, Se, Te; Hal-Cl, Br, I) systems was started from the beginning of the 80th years of the last century. A special attention was paid to quasibinary systems Tl2X-TlHal because of possibility of formation of ternary compounds [6–11]. Existence of 11 ternary compounds was established in the Tl2X-TlHal systems: 6 ternary compounds of type Tl5X2Hal (all selenium and tellurium systems) and 4 ternary compounds of type Tl6XHal4 (all sulphurous systems and Tl-Se-I system). Tl2TeHal6 compounds were detected in the systems Tl-Te-Hal [12, 13].Tl6SHal4 (Hal-Cl, Br, I), Tl6SeI4, and Tl2TeBr6 compounds crystallize in a tetragonal structure, with space groupP4/mnc[6, 7, 14, 15]; Tl5Se2Br(I) and Tl5Te2Hal compounds have a tetragonal structure, with space groupI4/mcm[8, 11, 16–19]. Tl2TeCl6 compound crystallizes in a cubic system, Sp.gr.Fm-3mand Tl2TeCl6 in a monoclinic system, Sp. gr.P21/c [13, 15].Physicochemical investigation of Tl-X-Hal (X-S, Se, Te; Hal-Cl, Br, I) systems was implemented in detail at a wide or full concentration range. A number of polythermal and isothermal sections as well as projections of liquidus surfaces were constructed. The primary crystallization and homogeneity areas of phases were fixed and the fundamental thermodynamic functions of ternary compounds and solid solutions were determined [20–23].In this contribution, we present the thermodynamic study of Tl6SBr4 compound, summarize all data on thermodynamic properties of thallium chalcohalides, and carry out a comparative review between the latter. At the end of the paper, we present some regularities detected in the thermodynamic properties of thallium chalcohalides.


## 2. Experimental Details

### 2.1. Synthesis and Analysis

For planning experiments, we have used the solid-phase diagram of the Tl-TlBr-S system [24] which allowed us to determine the relevant compositions of samples for thermodynamic studies and to select conditions for their synthesis and thermal treatment (Figure 1). We have composed electrochemical cell of the type (1)-Tlsol.∣liquid  electrolyte,Tl+∣TlBr–Tl2S–Tl2S3sol.+in which the left electrode was pure metallic thallium and the right electrodes were samples from the mentioned region. A saturated glycerin solution of KBr with the addition of 0.1 mass% TlBr was used as an electrolyte.Figure 1
Solid-phase equilibrium diagram of the system Tl-TlBr-S at 300 K [24]. The compositions of the studied samples are given by hollow circles in the proper three-phase regions.Initial compounds Tl2S and TlBr were synthesized to prepare the right electrodes of the electrochemical cell of the type (1). Tl2S was synthesized by alloying of stoichiometric amounts of high-purity elemental components (Tl, 99.999 mass%, Alfa Aesar; S, 99.999 mass%, Alfa Aesar) in an evacuated silica ampoules at temperatures 30–50 K above the melting point. Tl2S, melting congruently at 728 K [17], readily crystallizes while slowly cooling the sample.TlBr was prepared by an indirect method reported in [18]. At first, metallic thallium was dissolved in the dilute sulphuric acid (7–10 mol%) at 350 K to get the Tl2SO4 solution. Then diluted HBr was added to a hot 2% Tl2SO4 solution until complete precipitation of TlBr. Yellowish green TlBr was separated from the mother liquor and washed with icy distilled water. The product was dried over KOH in a desiccator at 380–400 K and stored in the dark to prevent its decomposition.The synthesized compounds were identified by differential thermal analysis DTA (NETZSCH 404 F1 Pegasus system) and X-ray powder diffraction XRD (Bruker D8 ADVANCE diffractometer, CuKα1 radiation) methods.Alloys of the subsystem TlBr–Tl2S–Tl2S3 were prepared by blending and interacting TlBr and Tl2S compounds and elemental sulphur in various ratios in evacuated quartz vessels. They were subjected to a long-term stepped homogenizing annealing under the conditions described in [24]. The total mass of samples was 1 g and, after determining the solidus temperature, samples were additionally held at 20–30 K below the solidus for 500 h.


### 2.2. EMF Measurements

To measure the EMF of the chains type (1), electrodes, electrolyte, and electrochemical cell were prepared. The left electrode was made by attaching metallic thallium to a molybdenum current collector. Taking into account oxidization of thallium even at room temperature, before assembling electrochemical cell, the left electrodes were kept in glycerin, since metallic thallium does not directly interact with it [19].The right electrodes (see (1)) were prepared by pressing powdered equilibrium alloys of the system under study into current collectors in the form of cylindrical tablets with a weight of ~0.5 g and placed in a tubular furnace; the temperature was stabilized at 350 K for 40–50 h. The wires were sealed in glass jackets to protect them from contact with the electrolyte. EMF was measured by the compensation method in the temperature range of 300–390 K with the accuracy of ±0.1 mV, using the high-resistance universal B7-34A digital voltmeter. In each experiment the first EMF reading was performed approximately 30 h after the start of the experiment and at least 2-3 h after reaching the desired temperature, which ensures the achievement of equilibrium. The EMF measurements were carried out 2–7 days or more in consideration of homogenization of the electrode alloys, after the cell had been assembled. Equilibrium values were considered the EMF readings that varied by no more than 0.5 mV irrespective of the direction of temperature change at repeated measurements at a given temperature. In order to eliminate the contribution of the thermopower, all contacts and leads were kept at the same temperature.Techniques of assembling the electrochemical cell and EMF measurements are described in detail in [25, 26].


## 2.1. Synthesis and Analysis

For planning experiments, we have used the solid-phase diagram of the Tl-TlBr-S system [24] which allowed us to determine the relevant compositions of samples for thermodynamic studies and to select conditions for their synthesis and thermal treatment (Figure 1). We have composed electrochemical cell of the type (1)-Tlsol.∣liquid  electrolyte,Tl+∣TlBr–Tl2S–Tl2S3sol.+in which the left electrode was pure metallic thallium and the right electrodes were samples from the mentioned region. A saturated glycerin solution of KBr with the addition of 0.1 mass% TlBr was used as an electrolyte.Figure 1
Solid-phase equilibrium diagram of the system Tl-TlBr-S at 300 K [24]. The compositions of the studied samples are given by hollow circles in the proper three-phase regions.Initial compounds Tl2S and TlBr were synthesized to prepare the right electrodes of the electrochemical cell of the type (1). Tl2S was synthesized by alloying of stoichiometric amounts of high-purity elemental components (Tl, 99.999 mass%, Alfa Aesar; S, 99.999 mass%, Alfa Aesar) in an evacuated silica ampoules at temperatures 30–50 K above the melting point. Tl2S, melting congruently at 728 K [17], readily crystallizes while slowly cooling the sample.TlBr was prepared by an indirect method reported in [18]. At first, metallic thallium was dissolved in the dilute sulphuric acid (7–10 mol%) at 350 K to get the Tl2SO4 solution. Then diluted HBr was added to a hot 2% Tl2SO4 solution until complete precipitation of TlBr. Yellowish green TlBr was separated from the mother liquor and washed with icy distilled water. The product was dried over KOH in a desiccator at 380–400 K and stored in the dark to prevent its decomposition.The synthesized compounds were identified by differential thermal analysis DTA (NETZSCH 404 F1 Pegasus system) and X-ray powder diffraction XRD (Bruker D8 ADVANCE diffractometer, CuKα1 radiation) methods.Alloys of the subsystem TlBr–Tl2S–Tl2S3 were prepared by blending and interacting TlBr and Tl2S compounds and elemental sulphur in various ratios in evacuated quartz vessels. They were subjected to a long-term stepped homogenizing annealing under the conditions described in [24]. The total mass of samples was 1 g and, after determining the solidus temperature, samples were additionally held at 20–30 K below the solidus for 500 h.


## 2.2. EMF Measurements

To measure the EMF of the chains type (1), electrodes, electrolyte, and electrochemical cell were prepared. The left electrode was made by attaching metallic thallium to a molybdenum current collector. Taking into account oxidization of thallium even at room temperature, before assembling electrochemical cell, the left electrodes were kept in glycerin, since metallic thallium does not directly interact with it [19].The right electrodes (see (1)) were prepared by pressing powdered equilibrium alloys of the system under study into current collectors in the form of cylindrical tablets with a weight of ~0.5 g and placed in a tubular furnace; the temperature was stabilized at 350 K for 40–50 h. The wires were sealed in glass jackets to protect them from contact with the electrolyte. EMF was measured by the compensation method in the temperature range of 300–390 K with the accuracy of ±0.1 mV, using the high-resistance universal B7-34A digital voltmeter. In each experiment the first EMF reading was performed approximately 30 h after the start of the experiment and at least 2-3 h after reaching the desired temperature, which ensures the achievement of equilibrium. The EMF measurements were carried out 2–7 days or more in consideration of homogenization of the electrode alloys, after the cell had been assembled. Equilibrium values were considered the EMF readings that varied by no more than 0.5 mV irrespective of the direction of temperature change at repeated measurements at a given temperature. In order to eliminate the contribution of the thermopower, all contacts and leads were kept at the same temperature.Techniques of assembling the electrochemical cell and EMF measurements are described in detail in [25, 26].


## 3. Results and Discussion

### 3.1. Thermodynamic Study of the Ternary Compound Tl6SBr4

The solid-phase equilibrium diagram of the Tl-TlBr-S subsystem that had been constructed in [24] is given in Figure 1. As can be seen from Figure 1, there are 4 three-phase regions in the TlBr–Tl2S–Tl2S3 subsystem: TlBr–TlS–Tl2S3 (I), TlBr–TlS–Tl6SBr4 (II), Tl6SBr4–Tl4S3–TlS (III), and Tl2S–Tl6SBr4–Tl4S3 (IV). The EMF values measured in heterogeneous phase regions I–IV were processed by the least squares method [25, 26] and presented as the following linear equations: (2)E=a+bT±tSE2n+Sb2T-T¯21/2,where n is the number of pairs of E and T values; SE and Sb are the error variances of the EMF readings and b coefficient, respectively; T¯ is the average of the absolute temperature; t is Student’s test. At the confidence level of 95% and n≥20, Student’s test is t≤2 [25, 26]. The composed equation of the mode (2) is presented in Table 1. The experimental data of Ti and Ei and steps of calculation for the phase region II (Table 1), which is of special interest in terms of calculation of thermodynamic functions of the Tl6SBr4 compound, are presented in Table 2. The values of T¯, a, b, SE2, and Sb2 quantities in (2) were calculated based on Table 2.Table 1
Temperature dependences of EMF of the concentration chains type(1) in some phase regions of the subsystem TlBr–Tl2S–Tl2S3.
Number
Phase region in Figure1
E
,
m
V
=
a
+
b
T
±
t
⋅
S
E
(
T
)
1
TlBr–TlS–Tl2S3
552
,
6
-
0
,
120
T
±
2
1
,
8
24
+
8
⋅
1
0
-
5
T
-
342
,
4
2
1
/
2
K
K
i
m
2
TlBr–TlS–Tl6SBr4
486
,
1
-
0
,
038
T
±
2
0
,
9
24
+
5
⋅
1
0
-
5
T
-
342
,
4
2
1
/
2
k
k
m
3
T
l
6
S
B
r
4–Tl4S3–TlS
465
,
8
-
0
,
016
T
±
2
1
,
5
24
+
7
⋅
1
0
-
5
T
-
342
,
4
2
1
/
2
k
k
m
4
T
l
2
S–Tl6SBr4–Tl4S3
383
,
4
+
0
,
086
T
±
2
1
,
1
24
+
6
⋅
1
0
-
5
T
-
342
,
4
2
1
/
2
k
k
mTable 2
The calculation steps of the EMF measurements for the TlBr–TlS–Tl6SBr4 phase region.
T
i, K
E
i, mV
T
i
-
T
-
E
i
T
i
-
T
-
T
i
-
T
-
2
E
E
i
-
E
300,5
476,2
-
41
,
90
-
19952
,
78
1755,61
474,57
1,63
301,2
476,1
-
41
,
20
-
19615
,
32
1697,44
474,54
1,56
305,1
473,5
-
37
,
30
-
17661
,
55
1391,29
474,39
-
0
,
89
311,2
474,9
-
31
,
20
-
14816
,
88
973,44
474,16
0
,
74
313
473,2
-
29
,
40
-
13912,08
864,36
474,09
-
0
,
89
317,7
473,4
-
24
,
70
-
11692
,
98
610,09
473,91
-
0
,
51
319,3
473,2
-
23
,
10
-
10930
,
92
533,61
473,85
-
0
,
65
324,1
472,8
-
18
,
30
-
8652
,
24
334,89
473,66
-
0
,
86
328,7
474,1
-
13
,
70
-
6495
,
17
187,69
473,48
0
,
62
331,2
472,2
-
11
,
20
-
5288
,
64
125,44
473,39
-
1
,
19
335,4
472,1
-
7
,
00
-
3304
,
70
49,00
473,23
-
1
,
13
341,5
473,9
-
0
,
90
-
426
,
51
0,81
472,99
0
,
91
345,4
472,1
3,00
1416,30
9,00
472,84
-
0
,
74
349,3
473,1
6,90
3264,39
47,61
472,69
0
,
41
351,6
472,1
9
,
20
4343,32
84,64
472,61
-
0
,
51
356,1
472,8
13
,
70
6477,36
187,69
472,43
0
,
37
360,4
471,1
18
,
00
8479,80
324,00
472,27
-
1
,
17
364,2
471,2
21
,
80
10272,16
475,24
472,12
-
0
,
92
366,3
473,1
23
,
90
11307,09
571,21
472,04
1,06
369,3
472,9
26
,
90
12721,01
723,61
471,93
0,97
374,2
473,2
31
,
80
15047,76
1011,24
471,74
1,46
380,8
472,3
38
,
40
18136,32
1474,56
471,48
0,82
382,9
470,9
40
,
50
19071,45
1640,25
471,40
-
0
,
50
388,2
470,6
45
,
80
21553,48
2097,64
471,20
-
0
,
60Our results of measuring the EMF of the cells type(1) in the TlBr–Tl2S–Tl2S3 composition region were fully consistent with the solid-phase equilibrium diagram of the Tl-TlBr-S subsystem [24] (Figure 1). The EMF values at the given temperature, within I–IV three-phase regions, virtually coincide independently of the gross compositions of the right electrodes and vary discontinuously in transition from one of the regions to another. The EMF values at 300 K temperature for the phase areas showing in Table 1 are given in Figure 1.It should also be noted that numerical values of EMF and equations of their temperature dependence in the phase regions I, III, and IV (Table1) practically coincide with corresponding data [27] for the binary compounds TlS, Tl4S3, and Tl2S, respectively. This testifies reversibility of the electrochemical cells type (1) and therefore indirectly points to the absence of appreciable regions of solid solutions based on the aforementioned sulfides in the TlBr–Tl2S–Tl2S3 subsystem.The EMF values measured in the phase region II (Table1) can be assigned to the compound Tl6SBr4 and can be used in thermodynamic calculations. The calculation of the relative partial molar functions of thallium from the equation of the temperature dependence of the EMF in this phase region gave the quantities(3)ΔG-Tl=-45,80±0,07kJ·mol-1;ΔH-Tl=-46,90±0,48kJ·mol-1;ΔS-Tl=-3,71±1,39J·mol-1·K-1which are thermodynamic functions of the potential-forming reaction(4)Tl+4TlBr+TlS=Tl6SBr4according to Figure 1.Based on (4), we determined ΔZ0, the standard thermodynamic functions of formation (ΔG0, ΔH0) of Tl6SBr4:(5)ΔZ0Tl6SBr4=ΔZTl¯+4ΔZ0TlBr+ΔZ0TlS,where ΔZ0 is the standard Gibbs free energy ΔfG0298 and standard enthalpy of formation ΔfH0298 for the corresponding compound. The standard entropy of Tl6SBr4 was calculated as(6)SoTl6SBr4=ΔSTl¯+S0Tl+4S0TlBr+S0TlS.For calculations besides our ownΔZ¯Tl data, we used the standard integral thermodynamic functions of TlS [27] and TlBr [28] and the standard entropy of thallium [28]:TlS:ΔfG0=-51,6±0,42 kJ·mol−1; ΔfH0=-52,72±2,01 kJ·mol−1; S0298=-3,6±5,8 J·K−1·mol−1.TlBr:ΔfG0=-167,4±0,6 kJ·mol−1; ΔfH0=-172,7±0,7 kJ·mol−1; S0298=122,6±0,2 J·K−1·mol−1.Tl:S0298=64,2±0,2 J·mol−1·K−1.The errors were found by the error accumulation method.Calculated integral thermodynamic functions of Tl6SBr4 compound are given in Table 3. This table also summarizes the thermodynamic functions of other thallium chalcohalides.Table 3
Standard integral thermodynamic functions of ternary compounds in the Tl-X-Hal (X-S, Se, Te; Hal – I, Br, Cl) systems (T=298K).
Compound
-
Δ
f
G
0
(
298
K
)
-
Δ
f
H
0
(
298
K
)
S
0
298   J⋅K−1⋅mol−1
kJ⋅mol−1
Tl6SCl4
833
,
5
±
3
,
7
928
,
1
±
14
,
0
599
±
9
Tl6SBr4
76
8
,
2
±
2
,
9
791
,
3
±
5
,
2
644
±
9
Tl6SI4
601
,
7
±
2
,
5
595
,
1
±
4
,
0
672
±
10
Tl6SeI4
613
,
1
±
1
,
5
609
,
7
±
2
,
6
671
±
5
Tl5Se2Cl
392
,
8
±
1
,
1
421
,
6
±
5
,
1
433
,
9
±
7
,
2
Tl5Se2Br
374
,
3
±
1
,
0
384
,
3
±
2
,
7
447
,
6
±
6
,
4
Tl5Se2I
341
,
7
±
0
,
8
345
,
3
±
2
,
5
449
±
8
Tl5Te2Cl
355
,
9
±
1
,
1
377
,
1
±
5
,
0
4
7
4
,
1
±
6
,
8
Tl5Te2Br
340
,
6
±
1
,
6
344
,
5
±
2
,
7
483
,
4
±
6
,
2
Tl5Te2I
300
,
4
±
1
,
3
301
,
1
±
2
,
3
475
,
8
±
6
,
6


### 3.2. Comparative Review of Thermodynamic Properties of Thallium Chalcohalides

Using obtained values of the standard integral thermodynamic functions of formation and standard entropies of thallium chalcohalides, other fundamental characteristics, standard thermodynamic functions of atomization of these compounds, were calculated. As is known, the atomization thermodynamic functions are quantities that characterize the change of relevant thermodynamic functions during decomposition of a compound to monatomic gas mixture. The atomization energy of ternary compounds was calculated using(7)ΔatHcomp=∑ΔatHelem.-ΔfHcomp,where ΔfH(comp) is the enthalpy of formation of a compound and ∑ΔatHelem. is the sum of atomization enthalpies of elements in a compound. The atomization entropy of ternary compounds was calculated on the following equation: (8)ΔatS0comp=∑S0at.gas.-S0comp.Here S0(comp) is the absolute standard entropy and ∑S0(at.gas.) is the sum of the absolute entropies of elemental constituents of the considered compound in a monoatomic gas state.The Gibbs free energy of atomization of ternary compounds were calculated from Gibbs-Helmholtz equation using the data obtained from (7) and (8):(9)ΔatGcomp=ΔatH0comp-TΔatS0comp.Results are given in Table4.Table 4
Standard thermodynamic functions of atomization of thallium chalcogen-halides.
Compound
Δ
a
t
G
0  (298 K)
Δ
a
t
H
0  (298 K)
Δ
a
t
S
0  (298 K)  J⋅K−1 mol−1
kJ⋅mol−1
Tl5Se2Cl
1564
1858
988
Tl5Se2Br
1531
1816
958
Tl5Se2I
1488
1775
962
Tl5Te2Cl
1480
1766
960
Tl5Te2Br
1442
1728
961
Tl5Te2I
1389
1669
939
Tl6SCl4
2142
2534
1314
Tl6SBr4
1987
2377
1308
Tl6SI4
1784
2172
1303
Tl6SeI4
1754
2145
1313The standard thermodynamic functions of atomization, formation, and formation from appropriate binary compounds (Tl2X and TlHal) of thallium chalcogen-halides are summarized in Table 5, for comparative analysis.Table 5
Comparison of thermodynamic functions of atomization, formation from elemental components, and formation from binary compounds of thallium chalcogen-halides.
Compound
Δ
a
t
G
0
-
Δ
f
G
0
-
Δ
f
G
0 (b.c)
Δ
a
t
H
0
-
Δ
f
H
0
-
Δ
f
H
0 (b.c)
kJ⋅mol−1
Tl5Se2Cl
1564
392,8
17,0
1858
421,6
28,1
Tl5Se2Br
1531
374,3
16,1
1816
384,3
26,4
Tl5Se2I
1488
334,0
17,9
1775
324,0
15,1
Tl5Te2Cl
1480
355,9
12,5
1766
377,1
7,8
Tl5Te2Br
1442
340,1
14,3
1728
343,9
10,2
Tl5Te2I
1389
296,5
12,8
1669
286,8
12,1
Tl6SCl4
2142
833,5
2,8
2534
928,1
3,6
Tl6SBr4
1987
787,2
6,6
2377
791,3
8,2
Tl6SI4
1784
601,7
9,7
2172
595,1
9,0
Tl6SeI4
1754
613,1
16,6
2145
609,7
22,3As can be seen from Table5, the relationship between the standard thermodynamic functions of atomization, formation, and formation from appropriate binary compounds (Tl2X and TlHal) for all ternary compounds is as follows:(10)ΔatZ0≥ΔfZ0≥ΔfZ0b.c.,where Z is Gibbs free energy (G) or enthalpy (H).The atomization Gibbs free energies and enthalpies of all ternary compounds are very large positive quantities. The standard thermodynamic functions of formation of ternary compounds are 3–5 times smaller by absolute value than the proper atomization functions. This is associated with the fact thatΔatH0 is the minimal energy required to split up the crystal lattice into separate atoms. However, ΔatG0 is the driving force of the reverse process, combination of monatomic gases to form a crystal lattice.The standard thermodynamic functions of formation of ternary compounds are much smaller than the Gibbs free energies and enthalpies of formation from binary constituents. The reason of such a sharp distinction can be explained by the fact that formation of a ternary compound from its binary constituents is not accompanied by a considerable energetic change in the system. Moreover, during the latter process the oxidation state numbers of elements, consequently the type of chemical bonding do not alter significantly. However, during formation of ternary compound from elemental components, quantities change significantly and therefore total energy of the system decreases sharply.The high numerical values of the atomization entropy of all ternary chalcogen-halides can be explained by the dramatically increase in disorder during the decomposition of their crystal lattice (Table5).


### 3.3. Some Regularities in Thermodynamic Properties of Thallium Chalcogen-Halides

The comparative analysis of different thermodynamic functions of thallium chalcohalides with degree of ionization of the chemical bonding in those compounds as well as with the proper thermodynamic functions of binary compounds have shown the availability of some regularities.The conformity between the standard Gibbs free energies and enthalpies of formation of ternary (Tl6XHal4 and Tl5X2Hal) compounds and the sum of the proper functions of binary (TlHal and Tl2X) compounds is demonstrated in Figure 2. As shown in Figure 2, the absolute values of ΔfG0 and ΔfH0 functions of all ternary compounds are higher (~3–7%) than the sum of the proper functions of binary compounds.Figure 2
The correlation betweenΔfG0 and ΔfH0 functions of thallium chalcohalides and the sum of the proper functions of binary compounds.The correlations betweenΔfG2980 and ΔfH2980 functions of ternary and binary TlHal compounds are represented in Figure 3. As can be seen, these dependencies are linear for all compounds of the type Tl6XHal4; however the linear dependencies for Tl5Se2Hal and Tl5Te2Hal compounds with the same halogen atoms differ from each other.Figure 3
The correlation betweenΔfG0 and ΔfH0 functions of ternary and binary TlHal compounds.This is due to the fact that, TlHal compounds play a decisive role in the thermodynamic functions of the ternary compounds Tl6XHal4. Reversely, the main contribution in the thermodynamic functions of Tl5X2Hal compounds belongs to thallium chalcogenides Tl2X (X-Se, Te). Since the thermodynamic functions of formation of Tl2Se and Tl2Te compounds are considerably distinctive from each other, the values of relevant functions for Tl5Se2Hal and Tl5Te2Hal ternary compounds also differ by magnitude (Figure 3).The dependence graphs of the standard thermodynamic functions (Gibbs free energy and enthalpy) of formation and atomization of the ternary compounds Tl6XHal4 and Tl5X2Hal upon the ionization degree (ID) of chemical bonding are demonstrated in Figure 4.Figure 4
The dependence of the standard thermodynamic Gibbs free energy and enthalpies of formation (a, b) and atomization (c) of the ternary compounds on the degree of ionization (ID) of chemical bonding.
(a)
(b)
(c)The ID of a chemical bond in thallium chalcohalides was calculated by classical method [29]. For this aim, the chemical bond in CsF compound with the highest value of ID was considered pure ionic type and the difference of the relative electronegativities of elements (ΔREN) in this compound was found to be ΔREN = 3,2. Taking into account the equalities ΔREN = 0 and ID = 0% for nonpolar covalent bonds, the following equation was obtained.(11)ID%=31,25·ΔREN.Calculation of theΔREN for thallium chalcohalides is demonstrated by an example of Tl6SBr4 compound.All thallium atoms in Tl6SBr4 compound are in Tl1+ state. The values of relative electronegativities (REN) of Tl, S, and Br that were used in calculations are, respectively, 1,4; 2,6; and 2,9 [29].Since there are different anions (chalcogen and halogen) in the compound, firstly the average REN for the [SBr4] anion group and later ΔREN for Tl6SBr4 compound were calculated:REN [SBr4] = (2,6+2,9·4)/5=2,84;ΔREN Tl6SBr4 = 2,84 − 1,4 = 1,44.The averaged ID of the chemical bonds in thallium chalcogen-halides were calculated using (11): ID (%) = 31,25·ΔREN=31,25·1,44 = 45%. The calculated ΔREN and ID values for all thallium chalcohalides are summarized in Table 6.Table 6
Δ
R
E
N and ID values for thallium chalcohalides.
Compound
Δ
R
E
N
ID, %
Tl6SCl4
1,6
50
Tl6SBr4
1,44
45
Tl6SI4
1,2
37,5
Tl6SeI4
1,04
33,5
Tl5Se2Cl
1,23
38,5
Tl5Se2Br
1,17
36
Tl5Se2I
1,07
33
Tl5Te2Cl
1,03
32
TI5Te2Br
0,97
30
Tl5Te2I
0,87
27Both thermodynamic properties of ternary compounds have a positive linear tendency with ID of bonding. Since the lattice energy of substance rises with an increase in the ID of chemical bond, the extension of the above-mentioned thermodynamic functions is natural (Figure4).Unlike the energetical by nature thermodynamic functions (ΔG0, ΔH0) the atomization entropy of the ternary compounds Tl6XHal4 and Tl5X2Hal has virtually the same values within a certain error: Sat=120±3 K·mol−1·K−1 (Figure 5).Figure 5
The correlation between the atomization entropy of ternary compounds and the ionization degree (ID) of chemical bonding.It can be explained by the fact that the entropy of atomization is an indicator of the rise of irregularity during decomposition of crystal lattice into monatomic gas mixture. The same numerical value of atomization entropies of all considered ternary compounds is the result of the transformation of the system from regular crystallic state with the lowest value of entropy into the irregular atomic gas mixture during the atomization process. The difference between the entropy of a substance (with the same formula) in a crystal state and the entropy of a monoatomic gas mixture is nearly two orders smaller than the value of the atomization entropy and therefore does not affect the magnitude of the latter.


## 3.1. Thermodynamic Study of the Ternary Compound Tl6SBr4

The solid-phase equilibrium diagram of the Tl-TlBr-S subsystem that had been constructed in [24] is given in Figure 1. As can be seen from Figure 1, there are 4 three-phase regions in the TlBr–Tl2S–Tl2S3 subsystem: TlBr–TlS–Tl2S3 (I), TlBr–TlS–Tl6SBr4 (II), Tl6SBr4–Tl4S3–TlS (III), and Tl2S–Tl6SBr4–Tl4S3 (IV). The EMF values measured in heterogeneous phase regions I–IV were processed by the least squares method [25, 26] and presented as the following linear equations: (2)E=a+bT±tSE2n+Sb2T-T¯21/2,where n is the number of pairs of E and T values; SE and Sb are the error variances of the EMF readings and b coefficient, respectively; T¯ is the average of the absolute temperature; t is Student’s test. At the confidence level of 95% and n≥20, Student’s test is t≤2 [25, 26]. The composed equation of the mode (2) is presented in Table 1. The experimental data of Ti and Ei and steps of calculation for the phase region II (Table 1), which is of special interest in terms of calculation of thermodynamic functions of the Tl6SBr4 compound, are presented in Table 2. The values of T¯, a, b, SE2, and Sb2 quantities in (2) were calculated based on Table 2.Table 1
Temperature dependences of EMF of the concentration chains type(1) in some phase regions of the subsystem TlBr–Tl2S–Tl2S3.
Number
Phase region in Figure1
E
,
m
V
=
a
+
b
T
±
t
⋅
S
E
(
T
)
1
TlBr–TlS–Tl2S3
552
,
6
-
0
,
120
T
±
2
1
,
8
24
+
8
⋅
1
0
-
5
T
-
342
,
4
2
1
/
2
K
K
i
m
2
TlBr–TlS–Tl6SBr4
486
,
1
-
0
,
038
T
±
2
0
,
9
24
+
5
⋅
1
0
-
5
T
-
342
,
4
2
1
/
2
k
k
m
3
T
l
6
S
B
r
4–Tl4S3–TlS
465
,
8
-
0
,
016
T
±
2
1
,
5
24
+
7
⋅
1
0
-
5
T
-
342
,
4
2
1
/
2
k
k
m
4
T
l
2
S–Tl6SBr4–Tl4S3
383
,
4
+
0
,
086
T
±
2
1
,
1
24
+
6
⋅
1
0
-
5
T
-
342
,
4
2
1
/
2
k
k
mTable 2
The calculation steps of the EMF measurements for the TlBr–TlS–Tl6SBr4 phase region.
T
i, K
E
i, mV
T
i
-
T
-
E
i
T
i
-
T
-
T
i
-
T
-
2
E
E
i
-
E
300,5
476,2
-
41
,
90
-
19952
,
78
1755,61
474,57
1,63
301,2
476,1
-
41
,
20
-
19615
,
32
1697,44
474,54
1,56
305,1
473,5
-
37
,
30
-
17661
,
55
1391,29
474,39
-
0
,
89
311,2
474,9
-
31
,
20
-
14816
,
88
973,44
474,16
0
,
74
313
473,2
-
29
,
40
-
13912,08
864,36
474,09
-
0
,
89
317,7
473,4
-
24
,
70
-
11692
,
98
610,09
473,91
-
0
,
51
319,3
473,2
-
23
,
10
-
10930
,
92
533,61
473,85
-
0
,
65
324,1
472,8
-
18
,
30
-
8652
,
24
334,89
473,66
-
0
,
86
328,7
474,1
-
13
,
70
-
6495
,
17
187,69
473,48
0
,
62
331,2
472,2
-
11
,
20
-
5288
,
64
125,44
473,39
-
1
,
19
335,4
472,1
-
7
,
00
-
3304
,
70
49,00
473,23
-
1
,
13
341,5
473,9
-
0
,
90
-
426
,
51
0,81
472,99
0
,
91
345,4
472,1
3,00
1416,30
9,00
472,84
-
0
,
74
349,3
473,1
6,90
3264,39
47,61
472,69
0
,
41
351,6
472,1
9
,
20
4343,32
84,64
472,61
-
0
,
51
356,1
472,8
13
,
70
6477,36
187,69
472,43
0
,
37
360,4
471,1
18
,
00
8479,80
324,00
472,27
-
1
,
17
364,2
471,2
21
,
80
10272,16
475,24
472,12
-
0
,
92
366,3
473,1
23
,
90
11307,09
571,21
472,04
1,06
369,3
472,9
26
,
90
12721,01
723,61
471,93
0,97
374,2
473,2
31
,
80
15047,76
1011,24
471,74
1,46
380,8
472,3
38
,
40
18136,32
1474,56
471,48
0,82
382,9
470,9
40
,
50
19071,45
1640,25
471,40
-
0
,
50
388,2
470,6
45
,
80
21553,48
2097,64
471,20
-
0
,
60Our results of measuring the EMF of the cells type(1) in the TlBr–Tl2S–Tl2S3 composition region were fully consistent with the solid-phase equilibrium diagram of the Tl-TlBr-S subsystem [24] (Figure 1). The EMF values at the given temperature, within I–IV three-phase regions, virtually coincide independently of the gross compositions of the right electrodes and vary discontinuously in transition from one of the regions to another. The EMF values at 300 K temperature for the phase areas showing in Table 1 are given in Figure 1.It should also be noted that numerical values of EMF and equations of their temperature dependence in the phase regions I, III, and IV (Table1) practically coincide with corresponding data [27] for the binary compounds TlS, Tl4S3, and Tl2S, respectively. This testifies reversibility of the electrochemical cells type (1) and therefore indirectly points to the absence of appreciable regions of solid solutions based on the aforementioned sulfides in the TlBr–Tl2S–Tl2S3 subsystem.The EMF values measured in the phase region II (Table1) can be assigned to the compound Tl6SBr4 and can be used in thermodynamic calculations. The calculation of the relative partial molar functions of thallium from the equation of the temperature dependence of the EMF in this phase region gave the quantities(3)ΔG-Tl=-45,80±0,07kJ·mol-1;ΔH-Tl=-46,90±0,48kJ·mol-1;ΔS-Tl=-3,71±1,39J·mol-1·K-1which are thermodynamic functions of the potential-forming reaction(4)Tl+4TlBr+TlS=Tl6SBr4according to Figure 1.Based on (4), we determined ΔZ0, the standard thermodynamic functions of formation (ΔG0, ΔH0) of Tl6SBr4:(5)ΔZ0Tl6SBr4=ΔZTl¯+4ΔZ0TlBr+ΔZ0TlS,where ΔZ0 is the standard Gibbs free energy ΔfG0298 and standard enthalpy of formation ΔfH0298 for the corresponding compound. The standard entropy of Tl6SBr4 was calculated as(6)SoTl6SBr4=ΔSTl¯+S0Tl+4S0TlBr+S0TlS.For calculations besides our ownΔZ¯Tl data, we used the standard integral thermodynamic functions of TlS [27] and TlBr [28] and the standard entropy of thallium [28]:TlS:ΔfG0=-51,6±0,42 kJ·mol−1; ΔfH0=-52,72±2,01 kJ·mol−1; S0298=-3,6±5,8 J·K−1·mol−1.TlBr:ΔfG0=-167,4±0,6 kJ·mol−1; ΔfH0=-172,7±0,7 kJ·mol−1; S0298=122,6±0,2 J·K−1·mol−1.Tl:S0298=64,2±0,2 J·mol−1·K−1.The errors were found by the error accumulation method.Calculated integral thermodynamic functions of Tl6SBr4 compound are given in Table 3. This table also summarizes the thermodynamic functions of other thallium chalcohalides.Table 3
Standard integral thermodynamic functions of ternary compounds in the Tl-X-Hal (X-S, Se, Te; Hal – I, Br, Cl) systems (T=298K).
Compound
-
Δ
f
G
0
(
298
K
)
-
Δ
f
H
0
(
298
K
)
S
0
298   J⋅K−1⋅mol−1
kJ⋅mol−1
Tl6SCl4
833
,
5
±
3
,
7
928
,
1
±
14
,
0
599
±
9
Tl6SBr4
76
8
,
2
±
2
,
9
791
,
3
±
5
,
2
644
±
9
Tl6SI4
601
,
7
±
2
,
5
595
,
1
±
4
,
0
672
±
10
Tl6SeI4
613
,
1
±
1
,
5
609
,
7
±
2
,
6
671
±
5
Tl5Se2Cl
392
,
8
±
1
,
1
421
,
6
±
5
,
1
433
,
9
±
7
,
2
Tl5Se2Br
374
,
3
±
1
,
0
384
,
3
±
2
,
7
447
,
6
±
6
,
4
Tl5Se2I
341
,
7
±
0
,
8
345
,
3
±
2
,
5
449
±
8
Tl5Te2Cl
355
,
9
±
1
,
1
377
,
1
±
5
,
0
4
7
4
,
1
±
6
,
8
Tl5Te2Br
340
,
6
±
1
,
6
344
,
5
±
2
,
7
483
,
4
±
6
,
2
Tl5Te2I
300
,
4
±
1
,
3
301
,
1
±
2
,
3
475
,
8
±
6
,
6


## 3.2. Comparative Review of Thermodynamic Properties of Thallium Chalcohalides

Using obtained values of the standard integral thermodynamic functions of formation and standard entropies of thallium chalcohalides, other fundamental characteristics, standard thermodynamic functions of atomization of these compounds, were calculated. As is known, the atomization thermodynamic functions are quantities that characterize the change of relevant thermodynamic functions during decomposition of a compound to monatomic gas mixture. The atomization energy of ternary compounds was calculated using(7)ΔatHcomp=∑ΔatHelem.-ΔfHcomp,where ΔfH(comp) is the enthalpy of formation of a compound and ∑ΔatHelem. is the sum of atomization enthalpies of elements in a compound. The atomization entropy of ternary compounds was calculated on the following equation: (8)ΔatS0comp=∑S0at.gas.-S0comp.Here S0(comp) is the absolute standard entropy and ∑S0(at.gas.) is the sum of the absolute entropies of elemental constituents of the considered compound in a monoatomic gas state.The Gibbs free energy of atomization of ternary compounds were calculated from Gibbs-Helmholtz equation using the data obtained from (7) and (8):(9)ΔatGcomp=ΔatH0comp-TΔatS0comp.Results are given in Table4.Table 4
Standard thermodynamic functions of atomization of thallium chalcogen-halides.
Compound
Δ
a
t
G
0  (298 K)
Δ
a
t
H
0  (298 K)
Δ
a
t
S
0  (298 K)  J⋅K−1 mol−1
kJ⋅mol−1
Tl5Se2Cl
1564
1858
988
Tl5Se2Br
1531
1816
958
Tl5Se2I
1488
1775
962
Tl5Te2Cl
1480
1766
960
Tl5Te2Br
1442
1728
961
Tl5Te2I
1389
1669
939
Tl6SCl4
2142
2534
1314
Tl6SBr4
1987
2377
1308
Tl6SI4
1784
2172
1303
Tl6SeI4
1754
2145
1313The standard thermodynamic functions of atomization, formation, and formation from appropriate binary compounds (Tl2X and TlHal) of thallium chalcogen-halides are summarized in Table 5, for comparative analysis.Table 5
Comparison of thermodynamic functions of atomization, formation from elemental components, and formation from binary compounds of thallium chalcogen-halides.
Compound
Δ
a
t
G
0
-
Δ
f
G
0
-
Δ
f
G
0 (b.c)
Δ
a
t
H
0
-
Δ
f
H
0
-
Δ
f
H
0 (b.c)
kJ⋅mol−1
Tl5Se2Cl
1564
392,8
17,0
1858
421,6
28,1
Tl5Se2Br
1531
374,3
16,1
1816
384,3
26,4
Tl5Se2I
1488
334,0
17,9
1775
324,0
15,1
Tl5Te2Cl
1480
355,9
12,5
1766
377,1
7,8
Tl5Te2Br
1442
340,1
14,3
1728
343,9
10,2
Tl5Te2I
1389
296,5
12,8
1669
286,8
12,1
Tl6SCl4
2142
833,5
2,8
2534
928,1
3,6
Tl6SBr4
1987
787,2
6,6
2377
791,3
8,2
Tl6SI4
1784
601,7
9,7
2172
595,1
9,0
Tl6SeI4
1754
613,1
16,6
2145
609,7
22,3As can be seen from Table5, the relationship between the standard thermodynamic functions of atomization, formation, and formation from appropriate binary compounds (Tl2X and TlHal) for all ternary compounds is as follows:(10)ΔatZ0≥ΔfZ0≥ΔfZ0b.c.,where Z is Gibbs free energy (G) or enthalpy (H).The atomization Gibbs free energies and enthalpies of all ternary compounds are very large positive quantities. The standard thermodynamic functions of formation of ternary compounds are 3–5 times smaller by absolute value than the proper atomization functions. This is associated with the fact thatΔatH0 is the minimal energy required to split up the crystal lattice into separate atoms. However, ΔatG0 is the driving force of the reverse process, combination of monatomic gases to form a crystal lattice.The standard thermodynamic functions of formation of ternary compounds are much smaller than the Gibbs free energies and enthalpies of formation from binary constituents. The reason of such a sharp distinction can be explained by the fact that formation of a ternary compound from its binary constituents is not accompanied by a considerable energetic change in the system. Moreover, during the latter process the oxidation state numbers of elements, consequently the type of chemical bonding do not alter significantly. However, during formation of ternary compound from elemental components, quantities change significantly and therefore total energy of the system decreases sharply.The high numerical values of the atomization entropy of all ternary chalcogen-halides can be explained by the dramatically increase in disorder during the decomposition of their crystal lattice (Table5).


## 3.3. Some Regularities in Thermodynamic Properties of Thallium Chalcogen-Halides

The comparative analysis of different thermodynamic functions of thallium chalcohalides with degree of ionization of the chemical bonding in those compounds as well as with the proper thermodynamic functions of binary compounds have shown the availability of some regularities.The conformity between the standard Gibbs free energies and enthalpies of formation of ternary (Tl6XHal4 and Tl5X2Hal) compounds and the sum of the proper functions of binary (TlHal and Tl2X) compounds is demonstrated in Figure 2. As shown in Figure 2, the absolute values of ΔfG0 and ΔfH0 functions of all ternary compounds are higher (~3–7%) than the sum of the proper functions of binary compounds.Figure 2
The correlation betweenΔfG0 and ΔfH0 functions of thallium chalcohalides and the sum of the proper functions of binary compounds.The correlations betweenΔfG2980 and ΔfH2980 functions of ternary and binary TlHal compounds are represented in Figure 3. As can be seen, these dependencies are linear for all compounds of the type Tl6XHal4; however the linear dependencies for Tl5Se2Hal and Tl5Te2Hal compounds with the same halogen atoms differ from each other.Figure 3
The correlation betweenΔfG0 and ΔfH0 functions of ternary and binary TlHal compounds.This is due to the fact that, TlHal compounds play a decisive role in the thermodynamic functions of the ternary compounds Tl6XHal4. Reversely, the main contribution in the thermodynamic functions of Tl5X2Hal compounds belongs to thallium chalcogenides Tl2X (X-Se, Te). Since the thermodynamic functions of formation of Tl2Se and Tl2Te compounds are considerably distinctive from each other, the values of relevant functions for Tl5Se2Hal and Tl5Te2Hal ternary compounds also differ by magnitude (Figure 3).The dependence graphs of the standard thermodynamic functions (Gibbs free energy and enthalpy) of formation and atomization of the ternary compounds Tl6XHal4 and Tl5X2Hal upon the ionization degree (ID) of chemical bonding are demonstrated in Figure 4.Figure 4
The dependence of the standard thermodynamic Gibbs free energy and enthalpies of formation (a, b) and atomization (c) of the ternary compounds on the degree of ionization (ID) of chemical bonding.
(a)
(b)
(c)The ID of a chemical bond in thallium chalcohalides was calculated by classical method [29]. For this aim, the chemical bond in CsF compound with the highest value of ID was considered pure ionic type and the difference of the relative electronegativities of elements (ΔREN) in this compound was found to be ΔREN = 3,2. Taking into account the equalities ΔREN = 0 and ID = 0% for nonpolar covalent bonds, the following equation was obtained.(11)ID%=31,25·ΔREN.Calculation of theΔREN for thallium chalcohalides is demonstrated by an example of Tl6SBr4 compound.All thallium atoms in Tl6SBr4 compound are in Tl1+ state. The values of relative electronegativities (REN) of Tl, S, and Br that were used in calculations are, respectively, 1,4; 2,6; and 2,9 [29].Since there are different anions (chalcogen and halogen) in the compound, firstly the average REN for the [SBr4] anion group and later ΔREN for Tl6SBr4 compound were calculated:REN [SBr4] = (2,6+2,9·4)/5=2,84;ΔREN Tl6SBr4 = 2,84 − 1,4 = 1,44.The averaged ID of the chemical bonds in thallium chalcogen-halides were calculated using (11): ID (%) = 31,25·ΔREN=31,25·1,44 = 45%. The calculated ΔREN and ID values for all thallium chalcohalides are summarized in Table 6.Table 6
Δ
R
E
N and ID values for thallium chalcohalides.
Compound
Δ
R
E
N
ID, %
Tl6SCl4
1,6
50
Tl6SBr4
1,44
45
Tl6SI4
1,2
37,5
Tl6SeI4
1,04
33,5
Tl5Se2Cl
1,23
38,5
Tl5Se2Br
1,17
36
Tl5Se2I
1,07
33
Tl5Te2Cl
1,03
32
TI5Te2Br
0,97
30
Tl5Te2I
0,87
27Both thermodynamic properties of ternary compounds have a positive linear tendency with ID of bonding. Since the lattice energy of substance rises with an increase in the ID of chemical bond, the extension of the above-mentioned thermodynamic functions is natural (Figure4).Unlike the energetical by nature thermodynamic functions (ΔG0, ΔH0) the atomization entropy of the ternary compounds Tl6XHal4 and Tl5X2Hal has virtually the same values within a certain error: Sat=120±3 K·mol−1·K−1 (Figure 5).Figure 5
The correlation between the atomization entropy of ternary compounds and the ionization degree (ID) of chemical bonding.It can be explained by the fact that the entropy of atomization is an indicator of the rise of irregularity during decomposition of crystal lattice into monatomic gas mixture. The same numerical value of atomization entropies of all considered ternary compounds is the result of the transformation of the system from regular crystallic state with the lowest value of entropy into the irregular atomic gas mixture during the atomization process. The difference between the entropy of a substance (with the same formula) in a crystal state and the entropy of a monoatomic gas mixture is nearly two orders smaller than the value of the atomization entropy and therefore does not affect the magnitude of the latter.


## 4. Conclusion

By using electromotive force (EMF) measurements a regulated complex of thermodynamic properties for the Tl6SBr4 compound was obtained. The data regarding the thermodynamic properties of thallium chalcogen-halides were systematized and comparatively analyzed. Some correlations between thermodynamic functions of thallium chalcogen-halides and their binary constituents as well as ionization degree of chemical bonding were revealed.



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*Source: 5370289-2017-08-22.xml*