Progress of the research
on the thermostability of heteropoly compounds
Wu Qingyin, Cao
Lei, Feng Wenqi
( Department of Chemistry, Zhejiang University, Hangzhou 310027, China)
Received Jan. 12, 2004; Support from the National Natural Science Foundation of
China (20271045) and SRTP Foundation of Zhejiang University for this work is greatly
appreciated.
Abstract In this
paper, the factors influencing the thermostability of heteropoly compounds were reviewed,
such as external cation including organic cation, alkaline-earth metals cation, alkali
metals cation, transition metals cation and rare-earth metals cation as well as internal
heteroatoms including transition metal and nonmetal atoms.
Keywords Heteropoly compounds, Thermostability, DTA
1. INTRODUCTION
Heteropoly compounds (HPC) are widely used in industrial catalysis and solid chemistry
[1,2]. The study of thermostability of heteropoly acid (HPA)
can provide important information about the design of catalyst and basal data of solid
high-proton conductivity of HPA. It can also provide study evidence about the application
of HPA in corrosion resistant. The thermostability of HPA is controlled by factors such as
central heteroatom, component atom, ionic charge, electronegativity and counter cation. We usually judge the thermostability by the exothermic peak temperature
of the DTA curve.
The overall thermostability rule of representative HPA is
as follows: H3PW12O40£¾H4SiW12O40£¾H4GeW12O40£¾H3PMo12O40¡ÝH5PMo10V2O40¡ÝH7PMo8V4O40£¾H4SiMo12O40£¾H4GeMo12O40. And
heteropoly salts of Keggin and Wells-Dawsonare also characterized by thermal analysis [3].
Generally, the thermostability of some reduced HPA is
higher than that of oxidized HPA. And the thermostability of HPA salts is generally higher
than that of homologus HPA.
2. FACTORS AFFECTING THE
THERMOSTABILITY
2.1.The external cation
2.1.1 The organic cation
Table 1 shows the thermoanalytical data of
HPC containing organic cation [4]. The TG-DTA curve of A3PMo12O40
and A4SiMo12O40 (A= organic cation) shows that the weight
loss of ammonium salt and tetramethyl ammonium salt occurs in two steps: (I) the loss of
hydration water at 72oC and
38oC and (II)the mass loss. It
indicates that there is clearly difference between the TG curve and DTA curve of A3PMo12O40
containing four organic cations because ammonium salt has only one exothermic peak on DTA
curve and tetramethyl ammonium salt has two exothermic peaks.
Table 1 Thermoanalysis data of HPC containing organic cation
Sample |
The first exothermic peak temperature (oC) |
The second exothermic peak temperature (oC) |
(NH4)3PMo12O40 |
496 |
|
[(CH3)4N]3PMo12O40 |
448 |
464 |
[(C2H5)4N]3PMo12O40 |
352 |
380 |
[(C4H9)4N]3PMo12O40 |
308 |
372 |
(NH4)4SiMo12O40 |
486 |
|
[(C2H5)4N]3SiMo12O40 |
291 |
406 |
[(C4H9)4N]3SiMo12O40 |
256 |
372 |
The TG
curve shows that the weight loss of tetraethyl ammonium salt and tetrabutyl ammonium salt
occurs in one step, which indicate that there is no hydration water in molecule. Similar
to tetramethyl ammonium salt, their weight loss has two continuous steps. So there are two
continuous exothermic peaks on the corresponding DTA curve.
Ma Ronghua studied the
thermostability of peroxonibium heteropoly acid salts containing tungsten. In their study,
the weight loss of tetraheptyl ammonium salt such as a-[(C7H15)4N]3H2[SiW11(NbO2)·O39]·H2O
has five steps in thermal decomposition and weight loss of a-[(C7H15)4N]4[PW11(NbO2)·O39]·H2O has four steps [5]. The fact that
when organic cation becomes bigger the peaks position will move forward and the binding
ability of HPA salts with water will be weaken, which is due to that the bigger organic
cation can be oxidized easier.
2.1.2 The alkaline-earth metals cation
Table 2 is thermoanalysis data of molybdophosphates and molybdosilicates. It can be seen
that the DTA and the DSC curves are coincided with each other when comparing the relative
thermostability of HPA salts. We can know from the thermograms of molybdophosphates and
molybdosilicates of alkaline-earth metals that exothermic peaks on the DTA curve move
forward little by little. Along with that the main quantum number of counterions increases
the temperature of exothermic peaks is due to drop and HPA salts become instable. The
water loss temperature of molybdosilicates and molybdophosphates indicates that the
binding ability of molybdosilicates with water is greater than that of molybdophosphates,
which is the same with the corresponding HPA.
Table 2 Thermoanalysis data of
alkaline-earth metals
Sample |
Exothermic peak temperature of DTA (oC) |
Exothermic peak temperature of DSC (oC) |
Mg1.5PMo12O40 |
436 |
467 |
Ca1.5PMo12O40 |
418 |
452 |
Sr1.5PMo12O40 |
406 |
444 |
Ba1.5PMo12O40 |
392 |
|
Mg2SiMo12O40 |
360 |
|
Sr2SiMo12O40 |
340 |
|
Ba2SiMo12O40 |
290 |
|
Thermostability of alkaline-earth metals salts is greater than
their homologus acids and exothermic peak temperature rises as cations radius enlarges,
which matches the thermal decomposition temperature of the carbonate and can be explained
by the ionic polarization.
2.1.3 The alkali metals cation
K3PMo12O40 and Cs3PMo12O40
both have a little hydration water from their thermogram. There is no exothermic peak on
the DTA curve during the whole heating-up course (20-700oC). So it is believed that they have not decomposed. There
is a strong exothermic peak reflecting melting of K3PMo12O40
at 644oC and Cs3PMo12O40
at 696oC.
Thermostability of alkali metals salts is lower than their homologus
acids. As the organic cations enlarge the corresponding exothermic peak positions move
forward and binding ability of HPA salts with water is weaken because bigger HPA can be
oxidized easier.
Exothermic peak of alkali metals will be a little lower when periodic
number increases.
2.1.4 The metal cation of the same subgroup B
It is well known that the HPA salts containing Ag and Cu have special performance. Two
representative HPAs (H4SiMo6W6O40 and H5SiMo11VO40)
and their salts containing Cu and Ag have been synthesized and the thermostability and
catalysis property of those samples have been studied systematically [6]. It is indicated that the thermostability of HPA
salts is greater than that of their homologus acids.
Table 3 DTA data of HPA and HPA salts
Sample |
Decomposition temperature (oC) |
Sample |
Decomposition temperature (oC) |
H4SiMo6W6O40 |
450 |
H5SiMo11VO40 |
380 |
CuSiMo6W6O40 |
480 |
CuSiMo11VO40 |
393 |
AgSiMo6W6O40 |
503 |
AgSiMo11VO40 |
515 |
2.1.5 The transition metals cation
Table 4 shows the thermography data of HPA containing transition metals [7]. Those compounds have similar DTA curves and similar thermal
properties.
Table 4 Thermoanalysis data of heteropoly
compounds containing transition metal
Sample |
Exothermic peak temperature £¨oC£© |
Cu1.5AlCoW11 |
468 |
Co1.5AlCoW11 |
472 |
Ni1.5AlCoW11 |
476 |
Zn1.5AlCoW11 |
485 |
FeAlCoW11 |
544 |
CrAlCoW11 |
534 |
The
thermostability of all of transition metal salts is greater than their homologus acids and
increases with the cation charge increasing. The thermostability of bivalent transition
metal salts also changes with cation electronegativity. The lower the electronegativity
is, the greater the thermostability is.
2.1.6 The rare-earth metals cation
Rare-earth metals have empty 5d orbit, so they can become the position to transferring
electron for catalysis. When led-in the counter position the rare-earth metal can change
obviously the catalytic feature of HPA. Table 5 shows the exothermic peaks data of HPA
salts containing rare-earth metals on the DTA curve [8]. The thermostability of HPA is
related to not only composition and structure, but also the radius of counter cations. The
thermostability of the same series HPA salts will become greater as the atomic number of
rare-earth counter cations increases.
According to the
experiment result from table 5, the thermostability order is: LnHGeW12O40£¾H4GeW12O40,
LnHSiW12O40£¾H4SiW12O40, and LnHSiW12O40£¾LnHGeW12O40.
The
thermostability order of HPA salts containing rare-earth metals is the same with that of
HPA, which indicates that it is the heteropoly anion affecting the thermostability of
LnHSiW12O40 and LnHGeW12O40.
Table 5 Exothermic peak temperature of
rare-earth metal on DTA curve
Sample |
Ln |
Ce |
Nd |
Sm |
Eu |
Gd |
H* |
LnHGeW12O40 |
530 |
540 |
543.3 |
546.3 |
485 |
567.1 |
471 |
LnHSiW12O40 |
556.5 |
559.8 |
561 |
563.7 |
529.9 |
567.8 |
512 |
(H* is the one replacing of Ln)
2.2 The
internal heteroatom
2.2.1 The internal transition metals heteroatom
People studied the thermostability of HPA containing different internal ligand atoms
by experiments including TG-DTA, XPS, IR and solubility experiment.
Table 6 shows the DTA data of HPA containing transition metals[9,10].
Table 6 Exothermic peak temperature of
ZMW11 on DTA curve
Z |
Fe3+ |
Co2+ |
Ni2+ |
Zn2+ |
Al3+ |
Ga3+ |
CrW11 |
441 |
393 |
400 |
|
420 |
|
MnW11 |
|
|
376 |
382 |
|
390 |
FeW11 |
|
|
|
|
470 |
|
CoW11 |
|
|
|
|
436 |
|
CuW11 |
425 |
385 |
390 |
386 |
400 |
418 |
ZnW11 |
|
410 |
421 |
400 |
|
|
We can obtain the rule from
the data of table 6 and 7:
(I): The thermostability of the same
series of rare-earth ternary HPA salts is similar.
(II): The thermostability of the same
series of ZMW11 is different with the difference of Z. The thermostability of
MW11 containing Fe3+£¬Al3+ and Ga3+ is greater than that containing
Co2+£¬Ni2+
and Zn2+. So the thermostability of MW11 becomes greater with
increasing of electron change of Z.
(III): The thermostability of both MW11 and Ln(MW11)2 is
greater than that of corresponding Keggin structural MW12O40.
Table 7 Exothermic peak temperature of
Ln(MW11)2 on DTA curve
Ln |
La |
Ce |
Pr |
Nd |
Sm |
Eu |
Gd |
Dy |
CrW11 |
425 |
¡¡ |
¡¡ |
430 |
423 |
¡¡ |
¡¡ |
¡¡ |
MnW11 |
405 |
¡¡ |
¡¡ |
404 |
¡¡ |
404 |
405 |
406 |
FeW11 |
¡¡ |
¡¡ |
¡¡ |
484 |
485 |
482 |
486 |
490 |
CoW11 |
¡¡ |
¡¡ |
451 |
|
452 |
452 |
451 |
¡¡ |
CuW11 |
407 |
407 |
409 |
406 |
412 |
408 |
406 |
406 |
ZnW11 |
425 |
438 |
¡¡ |
435 |
432 |
422 |
413 |
¡¡ |
2.2.2 The internal nonmetals heteroatom
The thermal decomposition of the heteropolytungstates [PW11M(H2O)O39]n-
(M=Mn, Co, Ni, Cu, Fe) has been studied by Cavaleiro, and the decomposition products
identified by powder X-ray diffraction, FTIR and NMR spectroscopy [11].
Seven new-type pentabasic heteropoly complexes with the general
molecular formula K10H5[Ln(PMo5W4V2O39)2]·nH2O
(Ln = La, Ce, Pr, Nd, Eu, Gd, Dy) synthesized by Zhou and the thermal stability studied by
water solubility test, TG-DTA, XRD and IR at various temperature [12,13].
According to Table 8, the main factor influencing thermostability of
Ln(XM11)2 and Ln(X2M17)2 is the
thermostability of ligands XM11 and X2M17, the
subsequence is the same with that of the corresponding XW12O40 and X2M18O62[14,15].
Table 8 Thermoanalysis data of different internal nonmetal atoms
Heteropoly component compounds |
Temperature of thermal
decomposition(oC ) |
Heteropoly component compounds |
Temperature of thermal decomposition(oC) |
Ln(BW11)2 |
410-440 |
Ln(PW9Mo2)2 |
546 |
Ln(GeW11)2 |
560-572 |
Ln(AsW11)2 |
563-585 |
Ln(PW11)2 |
605-616 |
Ln(As2Mo17)2 |
278-300 |
Ln(PMo11)2 |
450-500 |
Ln(As2W17)2 |
480-500 |
Ln(SiW9Mo2)2 |
300-350 |
Ln(P2Mo17)2 |
318 |
Ln(SiW10V)2 |
430 |
Ln(P2Mo16V)2 |
278-299 |
Table 9 is the
thermoanalysis data of HPAs containing silicon and phosphorus [16,17]. The thermostability of HPA containing V is lower than
those that of containing Mo and W. Pope believes that small bond angle of bridging oxygen
goes against the formation of HPA and stable d-pp bond, so the thermostability of corresponding HPA is low.
Table 9 Thermoanalysis data of some
heteropoly acids
Heteropoly acids |
Exothermic peak temperature (oC ) |
Heteropoly acids |
Exothermic peak temperature (oC) |
H4SiW12O40 |
533 |
H3PW12O40 |
586 |
H4SiW9Mo3O40 |
486 |
H3PMo12O40 |
430 |
H4SiW6Mo6O40 |
450 |
H4PMo11VO40 |
380 |
H4SiW3Mo9O40 |
410 |
H6PMo9V3O40 |
335 |
H4SiMo12O40 |
360 |
H8PMo7V5O40 |
280 |
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