## Abstract

Relationships between the various physical and chemical properties of isostructural compounds take place according to the Periodic Table that is a fundamental basis of Chemistry. The systematization of this approach, data vs. the Periodic Table, will contribute to further development of the solid state chemistry theory. The lanthanides and the actinides make up the *f* block of the Periodic Table. The lanthanides are the elements produced as the 4*f* sublevel is filled with electrons and the actinides are formed while filling the 5*f* sublevel. In this paper, we analyze some classes of compounds formed by the lanthanides with other elements of the Periodic Table, which can count into the thousands of binary compounds. The special place of lanthanides in the Periodic System of Elements made it possible to establish strict nonlinear relationships between the standard entropy and the lanthanide atomic number of the compounds *Ln*_{2}*X*_{3} (*X* = O, S, Se, Te), *Ln*N, *Ln*B_{4}, and *Ln*F_{3} in the solid state. This relationship, based on tetrad-effect, can be applied to other physical and chemical properties of the isostructural compounds. The thermodynamic properties of actinides have been studied much less than lanthanides, but the similarity of physicochemical properties makes it possible for us to estimate, with sufficient accuracy, unexplored properties using fundamental laws. One of these laws is the tetrad-effect concept that is an effective tool to predict missing thermodynamic values for lanthanide and actinide compounds and to rationally plan experiments.

## Introduction

Before to share our ideas we would like to cite the words of well-known American scientist Gschneidner [1]. “Systematics is a powerful tool for understanding the physical and chemical nature of materials. In addition, systematics allows one to predict properties and behaviors with a reasonable confidence level in the absence of experimental data”.

Previous review articles evidenced the relation of thermodynamic data with Periodic Law [2], [3], [4], [5] and established a strict relationship between the enthalpy of formation, melting point and the atomic numbers of components in the semiconductor A^{III}B^{V} phases, with diamond-like structure of sphalerite and wurtzite types. The proposed model was used for the critical assessment of the thermodynamic properties of isostructural compounds. The relationship between the reduced enthalpy *Z*_{i}=Z_{A}+Z_{B}) has been used for a critical assessment of the thermodynamic properties of A^{III}B^{V} phases.

The Similarity Method was used for the critical analysis of specific heat ^{III}B^{V} isostructural phases. A critical analysis of heat capacities ^{III}B^{V} and A^{II}B^{VI}. More than 3000 experimental data have been analyzed. One part of the material, concerning the A^{III}B^{V} phases was presented in [2], [3]. Another part, related to the fourth group and A^{II}B^{VI} compounds, will be published later.

It was found that the dependence of the heat capacities *Z*_{i}), such as BN (hex) Z_{i}=12 and glassy pure carbon Z=6; BP and AlN (Z_{i}=20); AlP (Z_{i}=28) and pure Si (Z=14); BAs and GaN (Z_{i}=38); AlAs and ZnS (Z_{i}=46); AlSb, GaAs, InP, CdS (Z_{i}=64) and pure Ge (Z=32); GaSb, InAs, and CdSe (Z_{i}=82); InSb, CdTe (Z_{i}=100) and pure gray Sn (Z=50); have the same heat capacity experimental values in the solid state within the experimental uncertainty.

Another approach of heat capacity analysis with the use of a hybrid model was earlier presented by Pässler [6] for the fourth group A^{III}B^{V} and A^{II}B^{VI} compounds from absolute zero up to room temperature. In this publication there is a full set of 96 bibliographic references up to 2010.

It is also necessary to cite the Ref. [7] that deals with heat capacity of GaB^{V} and InB^{V} (B^{V}=P, As, Sb) above 298 K. The slight differences in the dependence of ^{III}B^{V}, A^{II}B^{VI} phases and pure elements may be due to both impurities and isotopic composition effects [8], [9], [10]. The “tetrad-effect” phenomenon was also used for the analysis, correction and prediction of thermodynamic data for the lanthanide (*Ln*) compounds. It is connected to the 4*f*-electrons of the lanthanide elements (*Ln*: La–Lu; their atomic numbers are 57–71).

The most sensitive to the tetrad-effect thermodynamic functions of lanthanide compounds are standard entropies and entropies of formation, because they are the most susceptible to the influence of the 4*f*-electrons of the lanthanides. We analyzed some classes of lanthanides with other elements of the Periodic Table, which account for only a sampling of the thousands of similar binary compounds possible. As an example, we use the tetrad-effect concept for the analysis and prediction of the standard entropies of *Ln*_{2}*X*_{3} (*X*=O, S, Se, Te), solid phases, but this approach can also be applicable to other classes of the *Ln* compounds as *Ln*N, *Ln*B_{2}, *Ln*B_{4}, *Ln*B_{6}, *Ln*F_{3} and other compounds. The tetrad-effect concept gives us the ability to develop a solid state chemistry theory for lanthanide alloys.

We have demonstrated that the concept of the tetrad effect and symmetric function: *a*_{0}+*a*_{1}*x*+*a*_{2}*x*^{2}+*a*_{4}*x*^{4} (a_{i} are the fitting parameters and *x*=|*N*–N_{Gd}|, where *N* and N_{Gd}, the lanthanide and gadolinium atomic numbers respectively, can be used successfully to analyze and predict the standard entropies of solid lanthanide compounds at 298 K.

The tetrad-effect concept can be also applied to the actinides.

## Tetrad-effect

For the first time, the term “tetrad-effect” was proposed by Peppard et al*.* in 1969 [11]. They found that the plot of log *K* (*K* is the ratio of the lanthanide concentration in the organic phase to that in the aqueous phase) vs. *Z* (the atomic number of the lanthanide) consists of four separate curves, each encompassing four points (La–Ce–Pr–Nd, Pm–Sm–Eu–Gd, Gd–Tb–Dy–Ho and Er–Tm–Yb–Lu). So, four tetrads are formed, with Gd being an element common to the second and third tetrads.

The theoretical explanation of the tetrad-effect was given by Nugent [12] who showed that this effect originates from the interelectronic interaction energy of the *n* electrons in 4fn configuration and is connected to the *E*1 and *E*3 Racah’s parameters dependence on the quantum numbers L and S for the ground electronic state of each *Ln*^{3+} ion. The coefficient of *E*1 is responsible for the 1/2-filled shell effect and the coefficient of *E*3 is responsible for the 1/4 and 3/4-filled shell effects. The quantum numbers *S* and *L* for the ground electronic state of *Ln*^{3+} ions are presented in Fig. 1 [13].

In accordance with [14], the magnetic properties of the rare earth metals can be understood in terms of what we will call the standard model; herewith the magnetic 4f electrons in the metal have the same angular-momentum quantum numbers as in the free ion. They interact, however, with the surrounding electric field of the crystal, and with each other through an indirect exchange mediated by the conduction electrons.

So, the tetrad-effect of pure lanthanides results from an interaction of the spin angle moments and orbital quantum numbers. Spin entropy increases the degree of magnetic order and reduces magnetic entropy of the spin system. Under the same conditions, the standard entropies of pure lanthanides depend mainly on the spin and orbital magnetic components. See Fig. 1.

Later Lefevre et al*.* [15] synthesized the phases in the *R*_{2}Co_{2}I series (*R*=La, Y, Pr, Nd, Tb–Ho) and studied their structural and magnetic properties. Ferromagnetic ordering was observed for all compounds. For *R*_{2}Co_{2}I (*R*=La, Y) band-type ferromagnetism was concluded. For *R*_{2}Co_{2}I (*R*=Pr, Nd, Tb–Ho) the values of T_{C} suggest that a polarization of the 5d electrons enhances the 4f-4f exchange interaction as is well known e.g. in the case of the behaviors of GdI_{2} [16]. A deviation from the de Gennes rule [17] for the light rare earth metal compounds was ascribed to a polarization of the 5d electrons. A similar deviation had been observed for the *R*_{2}T_{2}X series [18] and also explained in terms of a polarization of the 5d electrons by the 4f moments.

If we take in consideration the standard entropies of pure lanthanides at 298 K (Fig. 2), we can observe the convex tetrad-effect for two *Ln* branches. The right branch (heavy lanthanides) is sufficiently well-formed, while a similar regularity of the left branch (light lanthanides) is broken.

In our opinion the behavior of thermodynamic functions must be close (according to the tetrad-effect) to the symmetric function relative to gadolinium. We used this rule in the thermodynamic analysis of the lanthanide tellurides [5]. Therefore, having a reasonably accurate description of the standard entropies in the right branch (heavy lanthanides), we can reconstruct the description of the left branch (light lanthanides) using the equation:

where N* _{Ln}* is the atomic number of the

*Ln*element, N

_{Gd}is the atomic number of Gd (N

_{Gd}=64) and

*σ*is the standard error.

The whole description of standard entropies was made for the hexagonal unit cell of *Ln* pure lanthanides. Additional references related to the tetrad-effect concept can be taken from [5], [19], [20], [21]. If we compare the standard entropies of pure lanthanides and those of their chalcogenides (sulfides, selenides and tellurides), we can see a similarity of these entropies vs. *N*-N_{Gd}. It is obvious that this similarity between the chalcogenides is due to the influence of lanthanides, a principal part of these compounds.

The description of the lanthanide chalcogenides was created without taking into account the differences in structures. The influence of structural factors can be considered insignificant (within the error of entropy determination).

The standard thermodynamic parameters of the pure lanthanide and binary lanthanide compounds with other elements of the Periodic Table in the solid state also follow the tetrad-effect concept [4], [5]. In this case the structural factor is decisive.

If the tetrad-effect is observed to be the structural parameters of the isostructural compounds (such as a unit cell volume or the shortest distance between the *Ln* and second element atoms), (see Figs. 3, 4), this phenomenon should also be extended to the other physicochemical properties of solids [5].

If the tetrad-effect of the physical and chemical properties is not observed in the isostructural lanthanide compounds, this indicates an experimental inaccuracy in the determination of these properties. The reduction of the lanthanide atomic fraction in the compound leads to a leveling of this rule.

The available information on the thermodynamic properties of lanthanide compounds is usually limited due to great experimental difficulties caused by the high reactivity of lanthanides (especially light lanthanides) and their instability in the air. Typically, lanthanide alloys decompose into *Ln*_{2}O_{3} and free nanoparticles of the second component when coming into contact with atmospheric air.

In our recent paper [5], we demonstrated how we can apply the tetrad-effect to correct the available standard entropies of pure lanthanides. The standard entropies of heavy lanthanides were obtained with a smaller experimental error than for light rare earth metals. If we apply the tetrad-effect concept, we can correct the entropies of light rare earth metals using the symmetric function.

## Standard entropies at 298 *K* of the chalcogenide *Ln*_{2}*X*_{3} compounds (*X*=S, Se, Te)

The available information on the structures and standard entropies at 298 K of the solid *Ln*_{2}S_{3}, *Ln*_{2}Se_{3}*Ln*_{2}Te_{3} compounds [4], [18], [19], [20], [21], [22], [23], [24] is presented in Tables 1–3
.

Ln | Lattice system | Space group | Ln_{0.4}S_{0.6}, J mol^{−1} K^{−1}) | ||
---|---|---|---|---|---|

[21], [22], [23], [24], [25] | [19] | Calc. (this work) | |||

La | ortho [19], [20] cubic [21] | Pnma [19], [20]Id [21] | 32.443 | 32.995 | 32.92 |

Ce | ortho [19], [20] cubic [21] | Pnma [19], [20]Id [21] | 35.486 | 36.066 | 36.15 |

Pr | ortho [19], [20] cubic [22] | Pnma [20]Id [22] | 37.880 | 38.158 | 37.72 |

Nd | ortho [19] cubic [21] | Pnma [19], [20]d [21] | 37.215 | 37.070 | 38.15 |

Pm | cubic [24] | d [24] | 38.945 | 37.489 | 37.84 |

Sm | ortho [19] cubic [23] | Pnma [19], [20]Id [24] | 35.752 | 35.899 | 37.11 |

Eu | cubic [24] ortho [20] | Pnma [20]Id [25] | 36.301 | – | 36.19 |

Gd | cubic [19], [21] ortho [20] | Pnma [20], [21]Pnma [20] | 33.341 | 36.066 | 35.22 |

Tb | cubic [22] ortho [20] | Pnma [20], [23]Pnma [20] | 38.130 | – | 36.19 |

Dy | cubic [23] ortho [20] | Pnma [20], [23]Pnma [20] | 38.845 | – | 37.11 |

Ho | ortho [20] | Pnma [20] | – | – | 37.84 |

Er | monocl [20] | P2_{1}/m [20] | – | – | 38.15 |

Tm | monocl [20] hex [20] | P2_{1}/m [20]Rc [29] | – | – | 37.72 |

Yb | hex [19], [20], [25] | Rc [19], [20], [25] | 37.864 | – | 36.15 |

Lu | hex [20], [25] | Rc [20], [25] | 32.825 | – | 32.92 |

Ln | Lattice system | Space group | Ln_{0.4}Se_{0.6}, J mol^{−1} K^{−1}) | ||
---|---|---|---|---|---|

[20] | [19] | Calc. (this work) | |||

La | cubic [19] | Id [22] | 40.44 | 40.083 | 40.41 |

Ce | cubic [19] | Id [22] | – | 44.35 | 43.91 |

Pr | cubic [19] | Ia | – | 46.024 | 45.35 |

Nd | cubic [19] | Ia | 44.82 | 44.852 | 45.49 |

Pm | cubic [19] | Ia | – | 45.354 | 44.95 |

Sm | ortho [19] | Pnma [20] | 44.24 | 43.765 | 44.23 |

Eu | – | – | – | – | 43.65 |

Gd | cubic [19] ortho [20] | IaPnma [20] | – | 43.932 | 43.44 |

Tb | ortho [20] | Pnma [20] | – | – | 43.65 |

Dy | ortho [20] | Pnma [20] | – | – | 44.23 |

Ho | ortho [20] | Fddd [20] | – | – | 44.95 |

Er | ortho [20] | Fddd [20] | – | – | 45.49 |

Tm | ortho [20] | Fddd [20] | – | – | 45.35 |

Yb | ortho [20] | Fddd [20] | – | – | 43.91 |

Lu | ortho [20] | Fddd [20] | – | – | 40.41 |

Ln | Lattice system | Space group | Ln_{0.4}Te_{0.6}, J mol^{−1} K^{−1}) | |
---|---|---|---|---|

[20] | Calc. (this work) | |||

La | cubic [19] | Id [22] | 46.325 | 46.61 |

Ce | cubic [19] | Id [22] | 50.208 | 49.80 |

Pr | cubic [19] | Ia | 51.882 | 51.11 |

Nd | cubic [19] ortho [20] | IaPnma [20] | 49.790 | 51.22 |

Pm | cubic [22] | Ia | 51.212 | 50.72 |

Sm | ortho [19], [20] | Pnma [20] | 49.622 | 50.05 |

Eu | – | 49.52 | ||

Gd | ortho [20] | Pnma [20] | 49.790 | 49.32 |

Tb | ortho [20] | Fddd [20] | – | 49.52 |

Dy | ortho [19], [20] | Fddd [20] | – | 50.05 |

Ho | ortho [20] | Fddd [20] | – | 50.72 |

Er | ortho [20] | Fddd [20] | – | 51.22 |

Tm | ortho [20] | Fddd [20] | – | 51.11 |

Yb | ortho [20] | Fddd [20] | – | 49.80 |

Lu | ortho [20] | Fddd [20] | – | 46.61 |

As can be seen, the structural data for most of the *Ln*_{2}S_{3} are contradictive, making it impossible to determine the real structures at 298 K. However, despite the difference in reported structures, the entropy data of *Ln*_{2}S_{3} at 298 K are often close to each other. So, the attempt to describe all of the entropy data for *Ln*_{2}S_{3} without identifying them as definite structures seems to be reasonable in this case. The following equation was obtained:

where *x*=|N* _{Ln}*–N

_{Gd}|;

*a*

_{0},

*a*

_{1}, and

*a*

_{4}are fitting parameters. The calculated entropy values for the Ln

_{0.4}S

_{0.6}at 298

*K*are listed in Table 1 and presented in Fig. 5.

The information on the structures of the solid *Ln*_{2}Se_{3} compounds and their standard entropies at 298 K [18], [19], [20], [21] is presented in Table 2. The entropy data for *Ln*_{2}Se_{3} were described by the equation:

The available data on the structures of the solid *Ln*_{2}Te_{3} compounds and their standard entropies at 298 K are presented in Table 3. The entropies of the *Ln*_{2}Te_{3} were described by the equation:

The results of the calculation using eq. (4) are given in Table 3 and plotted in Fig. 5.

## Standard entropies of formation of the *Ln*_{2}X_{3} chalcogenide compounds (X=S, Se, Te)

Since standard entropy values are available for compounds of rare-earth elements with other elements of the Periodic Table (at a given temperature), we can estimate the standard entropy of formation of these binary compounds with the formula:

where *x* is the atomic fraction of A component. The formation entropy of the sesquichalcogenides of lanthanides (*Ln*_{0.4}Te_{0.6}, *Ln*_{0.4}Se_{0.6}, *Ln*_{0.4}S_{0.6}) vs. the atomic number of lanthanides was calculated and presented in Fig. 6. The standard entropies of the pure lanthanides and chalcogenide were taken from [18], [19]. The graphs of the formation entropies are W-shaped in the case of lanthanide sesquichalcogenides.

Also the formation entropy graph of the *Ln*In_{3} intermetallic compounds has an inclined S-shape [3] Fig. 7. The use of the tetrad-effect concept helps with the standardization of thermodynamic data, both for pure lanthanides, and their compounds with other elements, and the development of the solid state chemistry theory.

## Standard entropies at 298 K of the solid *Ln*_{2}O_{3} compounds

We used the data reported in the review [18] and in the electronic database [19] as a source of information on the structures and standard entropies of the *Ln*_{2}O_{3} at 298 K (see Table 4). As can be seen from Table 4, the standard entropy values of *Ln*_{2}O_{3} change in accordance with the M-type of the tetrad-effect. There are local maxima at the points corresponding to Nd, Ho, and local minima at the points corresponding to La, Lu and Eu (Gd).

Ln | Lattice system | Space group | Ln_{0.4}O_{0.6}, J mol^{−1} K^{−1}) | |||
---|---|---|---|---|---|---|

[19] | [20] | Calc. (this work) | ||||

Ln_{0.4}O_{0.6} (cubic) | Ln_{0.4}O_{0.6} (hex) | |||||

La | hex [19], [20] | Pm1 [22]Ia | 25.464 | 25.464 | 21.78 | 25.54 |

Ce | hex [19], [20] | Pm1 [22]Ia | 29.62 | 29.623 | 26.58 | 29.37 |

Pr | hex [19], [20] | Pm1 [22]Ia | 30.54 | 31.129 | 29.19 | 31.15 |

Nd | hex [19], [20] | Pm1 [22]Ia | 31.74 | 31.715 | 30.33 | 31.61 |

Pm | cubic [19] monocl [20] | Pm1 [22]Ia | 31.6 | 31.464 | 30.60 | 31.34 |

Sm | monocle [19], [20] | Pm1 [22]Ia | 30.12 | 30.208 | 30.47 | 30.82 |

Eu | cubic [19], [20] | Ia | 27.28 | 29.288 | 30.25 | 30.38 |

Gd | cubic [19] | Ia | 30.12 | 30.125 | 30.16 | 30.21 |

Tb | cubic [19], [20] | Ia | 31.84 | 31.38 | 30.25 | 30.38 |

Dy | cubic [19], [20] | Ia | 29.96 | 29.957 | 30.47 | 30.82 |

Ho | cubic [19], [20] | Ia | 31.276 | 31.631 | 30.60 | 31.34 |

Er | cubic [19], [20] | Ia | 30.626 | 30.878 | 30.33 | 31.61 |

Tm | cubic [19], [20] | Ia | 27.94 | 27.95 | 29.19 | 31.15 |

Yb | cubic [19], [20] | Ia | 26.62 | 26.61 | 26.58 | 29.37 |

Lu | cubic [19], [20] | Ia | 21.992 | 21.991 | 21.78 | 25.54 |

The shape of an M is symmetrical relative to its centre, so we used the symmetrical function (with Gd is the central point) to describe the standard entropies of *Ln*_{2}O_{3}:

where *x*=|N* _{Ln}*–N

_{Gd}| and

*a*

_{0},

*a*

_{1},

*a*

_{2},

*a*

_{4}are fitting parameters.

According to Table 4, the entropy values of the *Ln*_{2}O_{3} with a hexagonal structure (*Ln*=La, Ce, Pr, Nd) exceed those with a cubic structure (*Ln*=Lu, Yb, Tm, Er), although these lanthanides have a symmetrical disposition relative to Gd. This indicates that the function *S*(*x*) is closely related with *Ln*_{2}O_{3} structure, so different functions *S*(*x*) must be used to describe the entropies of the hexagonal and cubic *Ln*_{2}O_{3}. Using the least squares method, the following equations were obtained:

The calculated entropy values of the hexagonal and cubic *Ln*_{0.4}O_{0.6} are listed in Table 4 and are presented in Fig. 8. Some of these values refer to metastable structures and their knowledge is important for the thermodynamic modeling of the phase equilibria.

The difference between the hexagonal and cubic forms of the *Ln*_{0.4}O_{0.6} compounds gives the entropies of transformation (Δ^{Str}).

Supplementary information on the tetrad-effect is available in [25], [26], [27], [28]. It is easy to calculate the standard entropies and entropies of formation for the isostructural *Ln*N, *Ln*B_{2}, *Ln*B_{4}, *Ln*B_{6}, *Ln*F_{3} [18], [19], [20], [21], [22], [27], [28], [29], [30], [31], [32], [33], [34] and other compounds, using a similar procedure.

## Standard entropies at 298 K of the *Ln*N, *Ln*B_{4} and *Ln*F_{3} solid compounds

All *Ln*N solid compounds have a cubic structure (space group *Fm**m*) [18], [19], [20]. The data [19] for the standard entropies of *Ln*N at 298 K are described by the equation:

This description, shown in Fig. 9 (line 1), demonstrates the validity of the tetrad-effect for the standard entropies of lanthanide nitrides. The *Ln*B_{4} solid compounds all have a tetragonal structure (space group *P*4/*mbm*) [18]. The data [28] for the standard entropies of *Ln*B_{4} (*Ln*=Gd–Tm, Lu) at 298 K are described by the equation:

This description, presented in Fig. 9 (line 2), shows that the standard entropies of heavy lanthanide borides (*Ln*B_{4}) at 298 K change in accordance with the tetrad-effect (right branch). So, it is easy to reconstruct the left branch for the light lanthanide tetraborides.

The solid *Ln*F_{3} compounds have two possible structures: hexagonal (space group *P**c*1) for *Ln*=La–Eu and orthorhombic (space group *Pnma*) for *Ln*=Sm–Lu [20]. Both crystalline forms of the *Ln*F_{3} were found for La, Sm, Eu, Gd, Ho, Tm, Lu [29], [30], [31], [32], [33], [34], [35]. The experimental data [29], [30], [31], [32], [33], [34], [35] for the standard entropies at 298 K of hexagonal *Ln*F_{3} (*Ln*=La–Nd) and orthorhombic *Ln*F_{3} (*Ln*=Gd, Dy, Er, Lu) were described by the equations:

The data [29], [30], [31], [32], [33], [34], [35] and results of the calculation using eqs. (11), (12) and Fig. 10 confirm the validity of the tetrad-effect for the standard entropies of lanthanide fluorides. The difference of the *Ln*F_{3} into another.

## Actinides, 5f elements

The thermodynamic properties of actinides have been studied much less than lanthanides, but the similarity of physicochemical properties makes it possible for us to estimate, with sufficient accuracy, unexplored properties using fundamental laws.

So, the “tetrad-effect” phenomenon can be also used for the analysis, correction and prediction of thermodynamic data for the actinides (*An*) compounds. It is connected to the 5*f*-electrons of the actinide elements (Ac–Lr; their atomic numbers are 227–266).

The Table 5 presents the crystal structure, half-life, standard entropies and densities of the solid pure actinides at 298 K.

An | N | Space group [20] | Half-life [36] | d g/cm^{3} [36] | d g/cm^{3} [37] | d g/cm^{3} calc. | |||
---|---|---|---|---|---|---|---|---|---|

Ac-227 | 89 | Fmm | 21.77 year | 10.07 | 10.7 | 10.02 | 56.48±6 | 61.9±0.8 | 59.57 |

Th-232 | 90 | Fmm | 1.40·10^{10} year | 11.72 | 11.78 | 14.76 | 53.39±0.5 | 51.8±0.5 | 53.75 |

Pa-231 | 91 | I4/mmm | 3.25·10^{4} year | 15.37 | 15.37 | 17.82 | 51.88±4.2 | 51.6±0.8 | 50.29 |

U-238 | 92 | Fmm | 4.47·10^{9} year | 19.05 | 19.05 | 19.19 | 50.21±0.2 | 50.2±0.2 | 49.2 |

Np-237 | 93 | Imm | 2.14·10^{6} year | 20.45 | 20.25 | 18.87 | 50.46±1.1 | 50.45±0.4 | 50.48 |

Pu-244 | 94 | Fmm | 2.41·10^{4} year | 19.86 | 19.84 | 16.87 | 56.02±0.84 | 54.46±0.8 | 54.11 |

Am-243 | 95 | Fmm | 7370 year | 13.67 | 11.7 | 13.19 | 54.64±2.7 | 55.4±2 | 60.12 |

Cm-244 | 96 | Fmm | 17.6 year | 13.51 | 7.0 | 7.81 | 72.0±3 | 70.8±3 | 68.48 |

Bk-247 | 97 | P6_{3}mmc | 1380 year | – | – | 13.19 | – | – | 60.12 |

Cf-251 | 98 | P6_{3}mmc | 898 year | – | – | 16.87 | – | – | 54.11 |

Es-252 | 99 | Fmm | 472 year | – | – | 18.87 | – | – | 50.48 |

Fm-257 | 100 | – | 100 day | – | – | 19.19 | – | – | 49.2 |

Md-258 | 101 | – | 51 day | – | – | 17.82 | – | – | 50.29 |

No-259 | 102 | – | 58 min | – | – | 14.76 | – | – | 53.75 |

Lr-266 | 103 | – | 11 h | – | – | 10.02 | – | – | 59.57 |

The standard entropies of the actinides [19] and [20] can be described (see Fig. 11) by an equation

The density of the actinides [36] and [37] can be described (see Fig. 12) by an equation

## Conclusion

A new relationship of thermodynamic data with Periodic Law was established.

The tetrad-effect concept is an effective tool in predicting the missing thermodynamic values for lanthanide compounds.

The combination of the tetrad-effect concept with the symmetric function

*a*_{0}+*a*_{1}*x*+*a*_{2}*x*^{2}+*a*_{4}*x*^{4}permits the analysis of the available experimental data for the standard entropies of the solid lanthanide compounds at 298 K and the prediction of the missing ones.The standard entropies of transformation between different crystalline structures of lanthanide compounds can be evaluated.

Using the standard entropies of the lanthanide compounds and the initial pure elements gives the possibility to calculate the standard entropies of formation of the lanthanide compounds. These entropies, combined with the experimental Gibbs energies of formation, yield the standard enthalpies of formation of the lanthanide compounds.

For the first time more then 80 standard entropies at 298 K of

*Ln*_{2}S_{3},*Ln*_{2}Se_{3},*Ln*_{2}Te_{3},*Ln*B_{4}, and*Ln*F_{3}solid compounds were evaluated for different crystalline forms.The standardization of thermodynamic data for both pure lanthanides and their compounds with other elements serves for the development of the solid state chemistry theory.

The tetrad-effect concept can be also applied to the actinides.

## Highlight

The physicochemical properties of pure lanthanides, as well as actinides and their compounds with other elements of the periodic system, are subject to a certain law.

This law can be called a “tetrad-effect” and it works best for the isostructural phases.

The tetrad-effect concept is an effective tool for predicting missing thermodynamic values for lanthanide and actinide compounds.

## Article note

A collection of invited papers based on presentations at the The 16^{th} International IUPAC Conference on High Temperature Chemistry (HTMC-XVI), held in Ekaterinburg, Russia, July 2–6, 2018.

## Acknowledgements

We would like to thank Prof. Lorie Wood from the University of Colorado (USA) for the language help. This work was financially supported by the Russian Foundation for Basic Research (project no. 17-08-01723).

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**Published Online:**2019-03-28

**Published in Print:**2019-06-26

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