Xinming Gua,
Zhipeng Wangb,
Honghua Wangb,
Guangyuan Zhoub and
Yanmin Zhou*a
aDepartment of Oral Implantology, Hospital of Stomatology, Jilin University, Changchun 130021, China. E-mail: zhouym@jlu.edu.cn
bDivision of Energy Materials (DNL22), Dalian Institute of Chemical Physics of the Chinese Academy of Sciences, Dalian 116023, China
First published on 29th January 2021
A series of wholly aromatic polyketones bearing benzimidazolone moieties (PK-BI) were synthesized via N–C coupling polycondensation. Calcium carbonate coupled with potassium carbonate was used for the first time to achieve a high molecular weight, with Tg of the polymer as high as 299 °C. The polymer structure was confirmed by solid state 13C NMR and FT-IR. The thermal stability of wholly aromatic polyketones with a benzimidazolone unit in the main chain was significantly improved, being higher than those of PEEKs and other amorphous PAEKs, proved by thermogravimetric analysis (TGA) and derivative thermogravimetric (DTG) analysis. The degradation activation energy (Ek) values estimated by Flynn–Wall–Ozawa (FWO) and Kissinger methods were 260.33 kJ mol−1 and 282.57 kJ mol−1, respectively, which are higher than those of PEEKs.
The difficulty in synthesis of the wholly aromatic polyketones presumably led to the paucity of reports. The reason was suspected to be its rigid skeleton caused by an aromatic ring moiety and a carbonyl moiety aligning on the same plane, which accelerated the aggregation of oligomers and precipitated in the reaction solvents even at high temperature, resulting in the suppression of the molecular weight.
While some aliphatic polyketones3 had been synthesized, wholly aromatic polyketones,4–12 a new series of high-performance polymers, were reported by Yonezawa's group (see Scheme 1). There were some aliphatic substitutes such as methoxyl and trifluoromethyl side groups in these polymers synthesized by either C–C coupling polycondensation or electrophilic polycondensation considering the solubility of polymer. The glass transition temperatures (Tgs) were usually lower than 220 °C. The methoxyl side groups in the polymer decreased the thermal stability of the polymer obviously compared with the aromatic backbone. Kricheldorf reported polyketones with the imidazolone unit and their poly ether ketone copolymers, but the research failed to get the wholly aromatic polyketone with benzimidazolone unit due to the low reactivity of 4,4′-diflorobenzophenone with silylated benzimidazolone in solid state melting polycondensation.13 Allan reported a developed N–C coupling polycondensation in TMS to synthesize the polysulfone with benzimidazolone unit.14 The polymer was easily soluble in chloroform and NMP.
Pyrolysis analysis was of importance in designing, processing and application of polymers. Systematic investigations about polymer characterization and mechanisms provided an efficient method to improve the structure design and achieve higher thermal durability. Features of the aromatic polymer were depicted as follows: thermal stability increased with the relative number of the aromatic groups per repeat unit of the polymer chain. The pyrolysis tended to begin with the breakage of the weakest bond in the bridging groups between aromatic rings. The introduction of the heteroatoms such as nitrogen, phosphorus and silicon by homo- or copolymerization of the monomers tended to be stable, and raised the temperature of thermal pyrolysis.
The decomposition kinetics of aliphatic polyketones based on styrene and carbon monoxide was detailed investigated by Jia's group.15 The Ek values estimated via Flynn–Wall–Ozawa method and Kissinger method were found to be in the range from 270.72 to 297.55 kJ mol−1. The degradation kinetics of wholly aromatic polyketone was not systematically studied yet due to the difficulty to obtain the polymer.
Here, for the first time, we reported the synthesis and the thermal degradation of a new member of heat-resistant wholly aromatic polyketone with benzimidazolone unit, PK-BI. We presumed that the big size & rigid benzimidazolone unit and nitrogen, as heteroatom, will both efficiently enhance the thermal durability compared to PEEK.
FT-IR spectrum was recorded on a Bio-Rad FTS-135 spectrophotometer. Solid state 13C NMR (100 MHz) spectrum was recorded on a Varian 400 instrument. Differential scanning calorimetry (DSC) was performed on a Mettler Toledo instrument DSC1 with a heating/cooling rate of 10 K min−1 in N2 (flow rate of 200 ml min−1). Tg was determined as the temperature at the midpoint of the thermal transition from the second heating curve. Thermogravimetric analysis (TGA) was performed on a Mettler Toledo instrument TGA/DSC1 at different heating rate from 5 K min−1 to 25 K min−1 under N2 or compressed air atmosphere (flow rate of 20 ml min−1) if the condition was not mentioned specially. T−5% was reported as the temperature at which 5% weight loss was observed.
(1) |
When the reaction rate constant was expressed by the Arrhenius equation and taking β as the heating rate, the reaction rate could be defined as eqn (2),
(2) |
(3) |
After integrating eqn (3) and taking logarithms, we obtained
(4) |
This function was based on the Doyle's approximation, when 20 ≤ x ≤ 60, lgp(x) may be closely approximated by eqn (5),
(5) |
Then, eqn (4) became
(6) |
Therefore, the apparent activation energy (Ek) could be obtained from the plot of lgβ against 1/T for a fixed degree of conversion.
f(α) = (1 − α)n | (7) |
(8) |
If the temperature raised at a constant rate β, then by differentiation of eqn (8) and defining that the maximum rate happened at the peak temperature (Tp), eqn (8) became
(9) |
Kissinger pointed out the product n(1 − α)n−1 was very nearly equal to unity. By substituting this value in eqn (9) and taking the logarithm on the both sides, we got
(10) |
It was possible for the determination of the degradation activation energy, Ek, by eqn (10). The plot of ln(β/Tp2) vs. 1/Tp would be a straight line, the slope of which permitted the calculation of Ek.
Entry | Solvent | Base | Temperature/°C | Time/h | Tg/°C |
---|---|---|---|---|---|
1 | DMI | K2CO3 | 129/188 | 2/8 | 238 |
2 | DMI | K2CO3/CaCO3 | 129/188 | 2/8 | 244 |
3 | CHP | K2CO3 | 136/208 | 2/8 | 243 |
4 | CHP | K2CO3/CaCO3 | 135/208 | 2/8 | 251 |
5 | TMS | K2CO3 | 135/200 | 2/8 | 229 |
6 | TMS | K2CO3/CaCO3 | 135/200 | 2/6 | 234 |
7 | TMS | K2CO3/CaCO3 | 135/200 | 2/8 | 239 |
8 | TMS | K2CO3/CaCO3 | 135/200 | 2/10 | 242 |
9 | DPS | K2CO3 | 135/200 | 2/8 | 273 |
10 | DPS | K2CO3/CaCO3 | 135/190 | 2/8 | 265 |
11 | DPS | K2CO3/CaCO3 | 135/195 | 2/8 | 275 |
12 | DPS | K2CO3/CaCO3 | 135/200 | 2/8 | 299 |
13 | DPS | K2CO3/CaCO3 | 135/200 | 2/12 | 299 |
The effect of carbonate salts on the polymerization system was deeply investigated. The effect of calcium carbonate on the reaction could not be ignored. It was due to formation of insoluble inorganic product, calcium difluoride, with the aid of carbonate calcium. The polycondensation of monomers gave not only polymer PK-BI, but also the small molecules, such as water, carbon dioxide and potassium fluoride. With the presence of calcium carbonate, the fluoride ion would form the calcium fluoride and turn to precipitate, which lead to the accumulation of the reaction. It was revealed with the same result that a higher Tg was detected by the present of calcium salt than those without calcium salt among the four solvent DMI, CHP, TMS and DPS chosen in our experiment. We preferred DPS to other solvents including DMI, CHP and TMS in considering of the solubility of the polymer since the boiling point of DPS is high enough to ensure a high reactive temperature up to 200 °C. The precipitated calcium fluoride could be removed by washing with acetic acid, which effectively improved the efficiency of polymerization.
The effects of time and temperature on the polymerization reaction were also obvious. With the increase of reaction time and temperature, the Tg of the polymer increased obviously. However, for DPS solvent system, entry 13, no increase for Tg was observed compared to entry 12. This may be because the Tg increase was not obvious as the molecular weight of the polymer increased to a certain range, that is, when the molecular weight of the polymer reached a critical molecular weight, Tg tended to be a constant.
The structure of PK-BI prepared in DPS was characterized by the FT-IR (Fig. 1) and quantitative solid state 13C NMR (Fig. 2) spectra. The FT-IR spectra of the polymer and the monomers thereof were shown in Fig. 1. The FT-IR spectrum of PK-BI indicated that 3059 cm−1 was attributed to the C–H stretching vibration of the aromatic rings. The CO stretching vibration of the urea part occurred at 1724 cm−1 owing to the presence of the ring strain, and that of the diphenylmethanone unit occurred at 1657 cm−1, 1386 cm−1 and 1165 cm−1 were attributed to the asymmetric and symmetric stretching vibration of the N–C–N group respectively.
Solid state 13C NMR was an effective method to characterize the structure of chemicals which were insoluble in common solvents. In Fig. 2, the signals of 190.68 ppm and 150.39 ppm were assigned to the C9 of diphenylmethanone unit and C1 of benzimidazolone moiety respectively. They were the critical peaks in the polymer. The solid state 13C NMR spectrum combined with the FT-IR spectrum confirmed that the structure was in accordance with that we designed.
Thermal property was evaluated by differential scanning calorimetry (DSC) and the second heating curve was shown in Fig. 3. There was only one glass transition at 299 °C. No melting transition was found during the test temperature range. It was in accordance with the theoretical results of the Allan S. Hay's research. The barrier to rotation of the C–O–C bond in the poly(aryl ether) resin was only 2.17 kcal mol−1, whereas the barrier to rotation of the C–N–C bond was calculated to be 41.79 kcal mol−1. The reason was that the conjugating o-phenylene pendent in the main polymer chain inhabited the ordered packing of the polymer. The derivative of imidazolidone unit was superior in respect to its distorting abilities, which suppressed the aggregation of the resulting polymer and maintained its solubility at the reaction temperature in DPS during the polymerization. It was necessary to note that the polymer prepared in TMS in the same condition gave a Tg of 239 °C, which was 60 °C lower than that of the polymer prepared above. This was because that the solubility of PK-BI in TMS was so poor that the oligomer would precipitate when the toluene was distilled off. The lower molecular weight of the polymer would dramatically debase the thermal and mechanical properties of the polymer. The reaction indicated that DPS was a favorable solvent in preparing polymer PK-BI.
Samples | β/K min−1 | T−5%/°C | Tonset/°C | Tp/°C |
---|---|---|---|---|
PK-BI | 5 | 566 | 554 | 575 |
PK-BI | 10 | 578 | 569 | 591 |
PK-BI | 15 | 588 | 580 | 603 |
PK-BI | 20 | 594 | 587 | 610 |
PK-BI | 25 | 600 | 593 | 617 |
PEEK | 10 | 546 | 547 | 569 |
PK-BI was studied by the two methods above to unveil the kinetic of the pyrogenation. The Ozawa method was reliable and suitable for the analysis of polymers without knowing the reaction mechanism.19 Different heating rate of PK-BI was tested. The results of heating rate at 5 K min−1, 10 K min−1, 15 K min−1, 20 K min−1 and 25 K min−1 were charted in Fig. 4. Since the weight loss percentage of PK-BI was higher than 65%, the activation energy was calculated from weight loss 5% to 30%.
The temperature at which the polymer weight loss happened at a certain heating rate was listed in Table 3. The apparent activation energy was calculated by the slope of lgβ − 1/T at different heating rates of 10, 15 and 20 K min−1 according to eqn (6). The average of the apparent activation energy was 260.33 kJ mol−1 which was much higher than that of PEEK calculated by the same method (231.8 kJ mol−1).
Weight loss | T/°C | R2 | Ek/kJ mol−1 | ||||
---|---|---|---|---|---|---|---|
5 K min−1 | 10 K min−1 | 15 K min−1 | 20 K min−1 | 25 K min−1 | |||
5% | 566 | 578 | 588 | 594 | 600 | 0.9949 | 250.74 |
10% | 578 | 590 | 600 | 606 | 612 | 0.9949 | 257.79 |
15% | 588 | 600 | 610 | 618 | 634 | 0.9984 | 237.20 |
20% | 599 | 610 | 621 | 628 | 644 | 0.9991 | 273.46 |
25% | 614 | 621 | 638 | 645 | 651 | 0.9991 | 283.97 |
30% | 660 | 638 | 690 | 696 | 703 | 0.9730 | 258.83 |
The Kissinger method was described as eqn (10). Thermal analysis of DTG showed the dynamic process when the polymer was heated. The rate of weight loss vs. temperature was determined. The activation energy (see Table 4) calculated by the Kissinger method from the thermogravimetric data of DTG was 282.57 kJ mol−1, which was higher than that calculated from FWO method.
β (K min−1) | Tp (K) | 1000/T (K−1) | Ek (kJ mol−1) | |
---|---|---|---|---|
FWO | Kissinger | |||
10 | 864 | 1.157 | 260.33 | 282.57 |
15 | 876 | 1.141 | ||
20 | 883 | 1.132 |
The difference between the FWO and Kissinger methods was 22.24 kJ mol−1, owing to the high char yield even at the final temperature. Most of the residues which remained by the complex mechanism were nonvolatile.
The TGA and DTG curves of PK-BI in N2 or compressed air at a heating rate of 10 K min−1 were depicted in Fig. 5, and those of PEEK in N2 atmosphere were given for control. In N2, the T−5% and Tp of PK-BI were 32 °C and 25 °C higher than those of PEEK respectively. The reason was that the present of heteroatom instead of ether linkage in PK-BI had higher bond energy than that of PEEK. The char yield values of PK-BI and PEEK in N2 at 900 °C were 62.0% and 52.6%. The residues of PK-BI contained more nonvolatile chemicals. The decomposition results of PK-BI in N2 and compressed air atmosphere were similar with each other when the temperature was below 550 °C. When the temperature increased, one peak was found in the DTG curve in N2 and the number for compressed air was two. The reason was that the oxygen in air reacted with the splitting aromatic free radicals. Oxygenation of aromatic rings took place and the volatile chemicals accounted for the large amount of weight loss. In compressed air, the rate of weight loss at 590 °C was twice of that in N2. The second peak was found at 644 °C. Much more volatile chemicals after oxygenation made the further weight loss. 68.6% of weight loss was found from 600 °C to 690 °C. The weight of nonvolatile degradation chemicals was 6.3% at 900 °C.
Fig. 5 TGA and DTG curves of PK-BI and PEEK at a heating rate of 10 K min−1: (a) PEEK in N2; (b) PK-BI in N2; (c) PK-BI in compressed air. |
PK-BI | PEEK [2] | ||
---|---|---|---|
Temp. (°C) | Chemicals detected | Temp. (°C) | Chemicals detected |
500 | CO2 | 450 | 4-Phenoxyphenol |
Toluene | 1,4-Diphenoxybenzene | ||
850 | CO2 | 600 | CO + CO2 |
Benzene | Diphenyl ether | ||
Aniline | 750 | Phenol | |
Fluorene | Benzene | ||
Diphenylamine | Dibenzofuran | ||
Phenazine | Hydroquinone | ||
9-Phenyl-9H-fluorene | 4-Dibenzofuranol | ||
1-Phenyl-1H-benzo[d]imidazol-2(3H)-one | 4-Hydroxybenzophenone | ||
1,3-Diphenyl-1H-benzo[d]imidazol-2(3H)-one | p-Benzoquinone | ||
1200 | CO2 | Benzophenone | |
Benzene | Biphenyl | ||
Aniline | Naphthalene | ||
Phenazine | Fluorene | ||
Fluorene | 1100 | 4-Hydroxybenzophenone | |
Phenazine | 1,4-Diphenoxybenzene | ||
1-Phenyl-1H-benzo[d]imidazol-2(3H)-one | 4-Phenylphenol | ||
1,3-Diphenyl-1H-benzo[d]imida-zol-2(3H)-one |
The results indicated that the organic decomposition chemicals were mainly the segments containing heteroatom aromatic organics and the aromatic ring such as aniline, fluorine and 9-phenyl-9H-fluorene. The volatile products at 500 °C were mainly carbon dioxide and toluene, indicating that the none conjugated ketonic carbonyl group was the weak bond when heated. With the test temperature ascending, 1-phenylbenzimidazolone accounting for large amounts of volatile products was detected which provided an indirect hint that the formation of C–N linkage in the reaction. The Py-GC/MS result was similar with that of PEEK8,20 except the heteroatom introduced by the benzimidazolone unit.
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