# Flower-Like Mn-Doped CeO2 Microstructures: Synthesis, Characterizations, and Catalytic Properties

Authors: Ling Liu; Jingjing Shi; Xiaojun Zhang; Jianzhou Liu
Journal: Journal of Chemistry
 (2015)

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## Abstract

Mn-doped CeO2 flower-like microstructures have been synthesized by a facile method, involving the precipitation of metallic alkoxide precursor in a polyol process from the reaction of CeCl3·7H2O with ethylene glycol in the presence of urea followed by calcination. By introducing manganese ions, the composition can be freely manipulated. To investigate whether there was a hybrid synergic effect in CH4 combustion reaction, further detailed characteristics of Mn-doped CeO2 with various manganese contents were revealed by XRD, Raman, FT-IR, SEM, EDS, XPS, OSC, H2-TPR, and N2 adsorption-desorption measurements. The doping manganese is demonstrated to increase the storage of oxygen vacancy for CH4 and enhance the redox capability, which can efficiently convert CH4 to CO2 and H2O under oxygen-rich condition. The excellent catalytic performance of MCO-3 sample, which was obtained with the starting Mn/Ce ratios of 0.2 in the initial reactant compositions, is associated with the larger surface area and richer surface active oxygen species.


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## Body

## 1. Introduction

Metal oxide is an important catalyst support in many catalytic reactions and serves especially as a substitute for the transitional noble catalyst in the activation of hydrocarbon. Recently, as an important functional metal oxide, CeO2 has attracted increasing interest with respect to its tremendous applications in environmental catalysis due to its oxygen vacancy defects and high oxygen storage capacity associated with the facile Ce4+/Ce3+ redox cycle [1–4]. However, owing to the poor thermal stability, pure CeO2 does not perform well in real catalysis. The addition of other metals (M = Cu, Co, Ni, etc.) into CeO2 fluorite lattice has been proven to exhibit higher oxygen storage capacity and better catalytic property than pure CeO2 [5–7]. In principle, the high activity of MOx-CeO2 is correlated with the synergistic effect between MOx and CeO2, which facilitates the electron exchanges between Mn+/Mn+1 and Ce3+/Ce4+, with both components being significantly more readily reduced or oxidized than the corresponding independent ones. Consequently, controllable synthesis of doped CeO2 catalysts, which possess facile redox process and high concentration of oxygen vacancies, will be beneficial to the enhancement of catalytic activity.In general, the activity of a catalyst is associated with various structural factors, such as chemical composition, surface modifications, specific surface area, surface oxygen vacancies, and preferential exposure of reactive facets [8–12]. As for a mixed oxide catalyst, the high activity and stability in the catalytic reaction are significantly affected by the dispersion of active component. The synthetic method is the critical factor to control the dispersion of active component. Therefore, the recent reports highlighted some new routes for the synthesis of doped CeO2 catalysts, which produced high catalytic performance. For example, hollow and solid MnOx-CeO2 nanospheres have been synthesized with a supercritical antisolvent process and used for the selective catalytic reduction of NO with NH3 [13]. CeO2 doped with transition metal ions (Co2+ and Ni2+), and Co/Ni binary-doped CeO2 mesoporous hollow nanospheres were prepared by a one-step solvothermal method and showed strikingly higher catalytic activity, owing to the intrinsic surface defects of the samples [14]. Cu-doped CeO2 spheres were prepared by a simple hydrothermal method and the excellent catalytic performance of Cu-doped (10 at.%) CeO2 spheres is associated with the porous spherical structure, high redox capability, and high oxygen vacancy [15]. Mesoporous CuO-CeO2 catalysts were prepared by a surfactant-assisted coprecipitation method and the precursors exerted a great influence on the properties of CuO-CeO2 catalysts. However, to our knowledge, little attention has been paid to the synthesis of doped CeO2 catalysts by a polyol-based precursor route [16].Herein, we report the synthesis of Mn-doped CeO2 flower-like microstructures via thermal decomposition of metallic alkoxide precursors, which were synthesized in ethylene glycol-mediated process. Preliminary CH4 catalytic oxidation experiments indicated that the Mn-doped CeO2 samples showed strikingly higher catalytic activity than pure CeO2, owing to the rich surface active oxygen species and large surface area.


## 2. Materials and Methods

### 2.1.  Synthesis

All chemicals and solvents were of analytical grade and used as received without further purification or modification. Mn-doped CeO2 catalysts were synthesized by a facile polyol-based precursor and annealing method. The prepared catalysts were Mn-doped CeO2 powder with the Mn/Ce molar ratios of 0.1, 0.15, 0.2, and 0.3. As to the synthesis of Mn-doped CeO2 (marked as MCO-1, Mn:Ce = 0.1), typically, 0.04 g of Mn(CH3COO)2·4H2O, 0.6 g of CeCl3·7H2O, 0.5 g of CO(NH2)2, and 2 g of poly(vinylpyrrolidone) (PVP; K-30) were dissolved into 50 mL of EG in a 150 mL round flask to form a clear solution. The resulting solution was then heated to 180°C under reflux and constant stirring. The clear solution became opaque after 20 min and the reaction was stopped after refluxing for 1 h. Upon finishing the reaction, the sample was allowed to cool naturally, after which the final product was collected by centrifugation and washed with absolute ethanol several times and then dried in air at 80°C. Thermal decomposition of the precursors was achieved in muffle furnace at a heating rate of 6°C/min up to 450°C maintained for 2 h in static air.Mn-doped CeO2 catalysts with different Mn contents (Mn:Ce = 0.15, 0.2, and 0.3, which were marked as MCO-2, MCO-3, and MCO-4, resp.) were prepared under identical conditions, in order to investigate the role of composition in the catalytic activities. For comparison, pure CeO2 was also prepared.


### 2.2. Characterization

Phase purity was examined by X-ray diffraction (XRD) on a Bruker D8-Advance powder X-ray diffractometer with Cu Kα radiation (λ=0.15418 nm). The morphologies and structures of the products obtained were determined by an FEI Quanta 250 emission scanning electron microscope (SEM) equipped with an energy dispersive X-ray spectrometer (EDS). Fourier transform infrared (FT-IR) spectra were recorded for samples using KBr pellet technique in the range of 400–4000 cm−1 (Bruker VERTEX 80v). Raman spectra were obtained using a Bruker Senterra Raman spectrometer with a laser wavelength of 785 nm. Surface analysis was carried out with X-ray photoelectron spectroscopy (XPS, Thermo ESCALAB 250Xi) with a standard Al Kα source. All binding energies were referenced to the C1s peak (284.8 eV) arising from surface hydrocarbons (or adventitious hydrocarbons). Measurement of specific surface area and analysis of porosity for the products were performed through measuring N2 adsorption-desorption isotherms at 77 K with a Quantachrome NOVA-3000 system. Specific surface area and pore size were calculated by the BET (Brunauer-Emmett-Teller) method and the BJH (Barrett-Joyner-Halenda) method, respectively.The oxygen storage capacity (OSC) experiments were performed on a PCA-1200 instrument by pulse technique. The samples were pretreated at 550°C in flowing H2 for 45 min and then in flowing Ar for 20 min and subsequently cooled to 200°C in Ar atmosphere. The reduced samples were oxidized at 300°C with pulse of O2 periodically at an interval of 3 min until a constant value being obtained for the peak intensity. The O2-OSC values were determined by the amount of O2 consumed during the O2 pulse.The temperature-programmed reduction measurements under a H2 environment (H2-TPR) were performed with a PCA-1200 instrument. Typically, the catalyst sample (30 mg) was pretreated under an O2 stream at 300°C for 30 min. After the sample cooled to room temperature, a flow of H2/Ar was introduced into the samples at a flow rate of 30 mL/min, and the temperature was increased to 900°C at a rate of 10°C/min.


### 2.3. Catalytic Tests

The activity measurements were carried out in a continuous flow fixed-bed microreactor at atmospheric pressure. In the experiments, 200 mg of catalyst was loaded into a stainless steel reactor with a gas mixture typically containing 1% CH4, 21% O2, and 78% N2 at the flow rate of 23.4 mL/min and the space velocity of 4000 h−1 in the temperature range from 250 to 500°C. A portion of the product stream was extracted periodically from the reactor with an automatic sampling valve and analyzed using a gas chromatograph with a thermal conductivity detector.


## 2.1.  Synthesis

All chemicals and solvents were of analytical grade and used as received without further purification or modification. Mn-doped CeO2 catalysts were synthesized by a facile polyol-based precursor and annealing method. The prepared catalysts were Mn-doped CeO2 powder with the Mn/Ce molar ratios of 0.1, 0.15, 0.2, and 0.3. As to the synthesis of Mn-doped CeO2 (marked as MCO-1, Mn:Ce = 0.1), typically, 0.04 g of Mn(CH3COO)2·4H2O, 0.6 g of CeCl3·7H2O, 0.5 g of CO(NH2)2, and 2 g of poly(vinylpyrrolidone) (PVP; K-30) were dissolved into 50 mL of EG in a 150 mL round flask to form a clear solution. The resulting solution was then heated to 180°C under reflux and constant stirring. The clear solution became opaque after 20 min and the reaction was stopped after refluxing for 1 h. Upon finishing the reaction, the sample was allowed to cool naturally, after which the final product was collected by centrifugation and washed with absolute ethanol several times and then dried in air at 80°C. Thermal decomposition of the precursors was achieved in muffle furnace at a heating rate of 6°C/min up to 450°C maintained for 2 h in static air.Mn-doped CeO2 catalysts with different Mn contents (Mn:Ce = 0.15, 0.2, and 0.3, which were marked as MCO-2, MCO-3, and MCO-4, resp.) were prepared under identical conditions, in order to investigate the role of composition in the catalytic activities. For comparison, pure CeO2 was also prepared.


## 2.2. Characterization

Phase purity was examined by X-ray diffraction (XRD) on a Bruker D8-Advance powder X-ray diffractometer with Cu Kα radiation (λ=0.15418 nm). The morphologies and structures of the products obtained were determined by an FEI Quanta 250 emission scanning electron microscope (SEM) equipped with an energy dispersive X-ray spectrometer (EDS). Fourier transform infrared (FT-IR) spectra were recorded for samples using KBr pellet technique in the range of 400–4000 cm−1 (Bruker VERTEX 80v). Raman spectra were obtained using a Bruker Senterra Raman spectrometer with a laser wavelength of 785 nm. Surface analysis was carried out with X-ray photoelectron spectroscopy (XPS, Thermo ESCALAB 250Xi) with a standard Al Kα source. All binding energies were referenced to the C1s peak (284.8 eV) arising from surface hydrocarbons (or adventitious hydrocarbons). Measurement of specific surface area and analysis of porosity for the products were performed through measuring N2 adsorption-desorption isotherms at 77 K with a Quantachrome NOVA-3000 system. Specific surface area and pore size were calculated by the BET (Brunauer-Emmett-Teller) method and the BJH (Barrett-Joyner-Halenda) method, respectively.The oxygen storage capacity (OSC) experiments were performed on a PCA-1200 instrument by pulse technique. The samples were pretreated at 550°C in flowing H2 for 45 min and then in flowing Ar for 20 min and subsequently cooled to 200°C in Ar atmosphere. The reduced samples were oxidized at 300°C with pulse of O2 periodically at an interval of 3 min until a constant value being obtained for the peak intensity. The O2-OSC values were determined by the amount of O2 consumed during the O2 pulse.The temperature-programmed reduction measurements under a H2 environment (H2-TPR) were performed with a PCA-1200 instrument. Typically, the catalyst sample (30 mg) was pretreated under an O2 stream at 300°C for 30 min. After the sample cooled to room temperature, a flow of H2/Ar was introduced into the samples at a flow rate of 30 mL/min, and the temperature was increased to 900°C at a rate of 10°C/min.


## 2.3. Catalytic Tests

The activity measurements were carried out in a continuous flow fixed-bed microreactor at atmospheric pressure. In the experiments, 200 mg of catalyst was loaded into a stainless steel reactor with a gas mixture typically containing 1% CH4, 21% O2, and 78% N2 at the flow rate of 23.4 mL/min and the space velocity of 4000 h−1 in the temperature range from 250 to 500°C. A portion of the product stream was extracted periodically from the reactor with an automatic sampling valve and analyzed using a gas chromatograph with a thermal conductivity detector.


## 3. Results and Discussion

### 3.1. Characteristics of Mn-Doped CeO2 Flower-Like Microstructures with Various Manganese Contents

To investigate whether there was a hybrid synergic effect in CH4 combustion reaction, we acquired detailed information on the structure and local atomic composition of the Mn-doped ceria with various Mn contents. Fundamental characteristics of the samples were revealed by FT-IR, XRD, SEM, EDS, XPS, Raman, BET, OSC, and H2-TPR.A polyol-based precursor route was developed to synthesize the Mn-doped CeO2 samples with various Mn contents. Figure 1 displays the typical FT-IR spectrum of the MCO-1 precursor. The vibrational bands of νa(CH2) and νs(CH2) at 2888 and 2844 cm−1 as well as the strong peak of ν(C–O) band at 1102 cm−1 derived from the ethylene glycol unit were observed, and the stretching vibrations of carboxylate group in acetate ions, νa(COO−) and νs(COO−), at 1465 and 1382 cm−1 were also detected. A broader band occurring at 3395 cm−1 can be attributed to the stretching vibration of OH groups linked by hydrogen bonds, and the band at 899 cm−1 can be viewed as ν(C–C). Thus, we conclude that the precursor compound appears to be an alkoxide, which is similar to those previously reported metallic alkoxide precursors in ethylene glycol-mediated process [17–22].Figure 1
Typical FT-IR spectrum of the as-obtained MCO-1 precursor.XRD was employed to ascertain the change in bulk crystal structure for CeO2 support. Figure 2 shows the XRD patterns of the Mn-doped CeO2 samples with various Mn contents prepared by heat treatment of those precursors. The 2θ values were located at 28.5°, 33.1°, 47.4°, 56.2°, 59.0°, and 69.4° for the pure CeO2. It is clear that the diffraction peaks of all the samples correspond to the (111), (200), (220), and (311) planes that can be indexed to the cubic fluorite structure of CeO2 crystals (JCPDS Card number 34-0394). The peak positions showed no critical change upon doping with guest metals; and no peaks were observed corresponding to doped metal and other individual oxides. The peaks of MnOx are not detected in the Mn-doped CeO2 samples even when the amount of initial Mn content in the raw material reached up to 30 mol%, which indicates the existence of well dispersion of MnOx species on the surface of CeO2 and/or the incorporation of Mn into the CeO2 lattice. However, the decrease of peak intensity and the slight increase of the peak width with the introduction of the dopant indicate that the grain sizes decrease after the metal ions are doped into the ceria. Moreover, as shown in Table 1, the lattice parameters obtained from the calculation of the (111) peak of Mn-doped CeO2 are smaller than that of pure CeO2, which can prove that Mn atoms probably replace some of Ce sites and enter into the CeO2 lattice [23]. Because the ionic radius of Mnn+ (Mn4+ = 0.53 Å, Mn3+ = 0.645 Å, and Mn2+ = 0.83 Å) is smaller than that of Ce4+ (1.01 Å), when Mnn+ embedded in CeO2 lattice and takes the place of Ce4+, the contraction and distortion of the ceria lattice occur, leading to the decrease of the cell parameter [24–26].Table 1
Lattice parameters and the proportions of O′′ and Mn3+ of pure CeO2 and Mn-doped CeO2 samples calculated from XRD and XPS, respectively.
Samples
Lattice parameter (Å)
O′′/(O′′ + O′) (%)
Mn3+/(Mn2+ + Mn3+) (%)
Pure CeO2
5.4113
39.5
—
MCO-1
5.4059
44.7
44.9
MCO-2
5.3983
45.4
45.1
MCO-3
5.3938
50.6
56.1
MCO-4
5.4015
45.9
56.8Figure 2
XRD patterns of Mn-doped CeO2 samples with different Mn contents.Raman scattering is an effective tool for the investigation of the effects of doping on nanomaterials, as the incorporation of dopants leads to shifts of the lattice Raman vibrational peak positions. Figure3 displays the Raman spectra of pure CeO2 as well as Mn-doped CeO2 samples with different Mn contents. For the pure CeO2, a strong peak at 463 cm−1 can be assigned to the F2g Raman active mode of the cubic fluorite structure of CeO2, which is due to the symmetric breathing mode of the oxygen atoms around cerium ions. The band at around 279 cm−1 can be related to the oxygen vacancies in CeO2 lattice attributed to the presence of defective structure [13, 27]. Compared to the pure CeO2, the peak intensity decreased greatly and became broader and red-shifted for the Mn-doped CeO2. The red-shift could be attributed to the changes in lattice parameter with crystallite size, as it was previously reported that a decrease of the particle size of CeO2 from 5 μm to 6.1 nm resulted in a shift to lower energy and was well explained by phonon confinement model [14, 28–30]. Additionally, the downshift is plausibly related to the presence of the Mn dopant, which would give rise to an increase in optical absorption [13, 31]. Another reason of shifting and broadening may be the increase in oxygen vacancies, which is related to structural defects derived from partially incorporation of manganese into CeO2 lattice, in agreement with the decrease of lattice parameter [32]. In the Mn-doped ceria samples, the extra oxygen vacancies were generated by the incorporation of Mn ion into the ceria fluorite lattice to compensate for the valence mismatch between the Mnn+ and Ce4+ ions. One piece of supporting evidence for the possible increase of defect density is that the as-prepared pure CeO2 sample shows a light yellow color, while the Mn-doped samples present various shades of taupe colors [14, 33].Figure 3
Raman spectra of pure CeO2 and Mn-doped CeO2 samples with different Mn contents. Peak positions (F2g) are shown on the right.The detailed morphologies and microstructures of the as-obtained Mn-doped CeO2 with different Mn contents were characterized by SEM. As shown in Figure 4, the samples are composed of a great deal of flower-like architectures with a diameter of 2-3 μm, and the entire microstructure of the architecture was built from petals which connected with each other forming the flower-like microstructure by self-assembly. The results implied that doping Mn in CeO2 did not change the total flower-like morphology. To determine the elemental compositions of the flower-like microstructures, EDS analysis has been carried out. The EDS spectrum and elemental mapping of the MCO-1 sample were depicted in Figure 5. Specifically, it appears that the pattern peaks of Mn, Ce, and O are clearly evident in the spectra collected, revealed the existence of the elements, and are accompanied with strong Au signals originated from gold plating on the sample before SEM examination. The elemental mapping results illustrate that the sample is mixed-metal oxide rather than a mixture of pure Mn and Ce phases. Moreover, the actual Mn/Ce ratios of the as-synthesized samples calculated from EDS are listed in Table 2. As can be seen, the actual Mn/Ce ratios in the products increased with the Mn/Ce ratios in the starting materials. The actual Mn/Ce ratios for the samples with the starting Mn/Ce ratios of 0.1, 0.15, 0.2, and 0.3 in the initial reactant compositions are 0.062, 0.070, 0.078, and 0.087, respectively. In the series of synthetic processes, the initial Mn/Ce molar ratio in the starting materials did not totally coincide with that of these solid precipitation, and it is more likely to follow a curved relation for the powder synthesized in EG, which coincided with our previously reported results [18]. The EDS results indicate that the doped Mn contents are smaller than the initial reactant compositions; in other words, only a portion of the added Mn ions incorporate into the ceria lattice. This may be due to the large disparity of the ionic radii, which might make the insertion into the ceria lattice more difficult [34].Table 2
Actual Mn/Ce ratios of as-synthesized Mn-doped CeO2 samples based on the EDS results.
Samples
MCO-1
MCO-2
MCO-3
MCO-4
Starting Mn/Ce ratio
0.1
0.15
0.2
0.3
Actual Mn/Ce ratio
0.062
0.070
0.078
0.087Figure 4
SEM images of the Mn-doped CeO2 samples with different Mn contents: (a) MCO-1, (b) MCO-2, (c) MCO-3, and (d) MCO-4 and (e) pure CeO2.
(a)
(b)
(c)
(d)
(e)Figure 5
Typical EDS spectrum (a) and elemental mapping (b) of the as-synthesized MCO-1 sample.
(a)
(b)XPS was performed in order to further illuminate the surface composition and the chemical state of the elements existing in Mn-doped CeO2 samples with various Mn contents. The XPS results suggest that the surface Mn/(Mn + Ce) ratios were rather low, even when the amount of initial Mn content in the raw material reached up to 30 mol% (surface Mn/(Mn + Ce) ≈ 0.072), which coincided with the EDS results. As displayed in Figure 6(a), the two sets of spin-orbital multiplets, corresponding to the Ce 3d3/2 and Ce 3d5/2 contributions, are labeled as u and v [15, 35–37]. For 3d5/2 of Ce(IV), the Ce 3d94f2Ln−2 and Ce 3d94f1Ln−1 states form the peaks v and v′′, and the Ce 3d94f1Ln state corresponds to the peak v′′′. For 3d5/2 of Ce(III), the Ce 3d94f2Ln−1 and Ce 3d94f1Ln states produce the peaks v° and v′. For Ce 3d3/2 labeled as u, the same assignment can be carried out. The result suggests that there is a certain amount of Ce3+ in all the Mn-doped CeO2 samples.Figure 6
XPS region spectra of (a) Ce 3d, (b) O 1s, and (c) Mn 2p for pure CeO2 (i) and Mn-doped CeO2 samples with different Mn contents: (ii) MCO-1, (iii) MCO-2, (iv) MCO-3, and (v) MCO-4.
(a)
(b)
(c)The O 1s XPS spectra for the Mn-doped ceria samples early show the existence of two states of surface oxygen atoms (Figure6(b)). The main peak O′ at ca. 529.4 eV is characteristic of lattice oxygen atoms; an apparent shoulder peak O′′ at ca. 531.3 eV has been assigned to oxide defects or absorbed oxygen ions with low coordination [13, 15, 16]. The strong peaks of the catalysts at 531.3 eV suggest that they are expected to have better oxygen storage capacity, which would be promising for their higher catalytic oxidation activity. As shown in Table 1, the ratio of O′′ of the MCO-3 sample obviously increased (50.6%), indicating that the content of surface oxygen vacancy is increased by doping suitable amounts of Mn. However, the surface oxygen vacancy contents would be decreased with further increase in the Mn contents, which may be due to the formation of bulk MnOx on the surface.The Mn 2p XPS spectra of Mn-doped CeO2 samples are displayed in Figure 6(c). The peaks are weak because of the low metal concentration of the surface elements; however, the compositions can still be identified in the spectra. The double peaks with binding energies of ca. 641.6 and 653.3 eV correspond to the characteristic of Mn 2p3/2 and Mn 2p1/2 signals, respectively [38, 39]. After refined fitting, the spectrum could be deconvolved into four peaks. The peaks at 641.3 and 653.3 eV can be assigned to the presence of Mn(II), while the other two peaks at 643.6 and 656.5 eV are characteristic of the Mn(III). This result suggests the coexistence of Mn2+/Mn3+ ion couple in the Mn-doped CeO2 samples. The relative concentrations of Mn3+ are summarized in Table 1. It is obvious that the proportion of Mn3+ increases with the increase of Mn doping concentration.As discussed above, the MCO-3 sample contains more amount of Mn3+ species and oxide defects (O′′), which are expected to exhibit different reduction properties and catalytic oxidation activities subsequently. These results provide an evidence of existence of redox equilibrium of Mn3+  +  Ce3+  ↔  Mn2+  +  Ce4+, which has been claimed to be the source of a synergistic interaction between manganese and ceria species in the Mn-doped CeO2 catalysts.The textural properties of the as-synthesized Mn-doped CeO2 samples were further investigated by measuring adsorption-desorption isotherms of N2 at 77 K, as shown in Figure 7. The hysteresis features of these samples should be classified as type H3 loop, suggesting the presence of aggregates of plate-like particles which give rise to slit-shaped pores [10, 40]. The texture data of the series of the samples are summarized in Table 3. Herein, the specific surface areas using the BET method for these samples are 56.0, 75.7, 91.0, and 74.2 m2/g, respectively. It was found that the MCO-3 sample exhibited higher BET surface area and smaller BJH pore size than those of the other Mn-doped CeO2 samples. Thus, such high surface areas will undoubtedly benefit surface adsorption during catalytic reactions.Table 3
BET surface areas, average pore sizes, and total pore volumes of Mn-doped CeO2 with various Mn contents.
Samples
BET surface area (m2/g)
Average pore size (nm)
Total pore volume (cm3/g)
MCO-1
56.0
13.04
0.100
MCO-2
75.7
8.12
0.085
MCO-3
91.0
7.90
0.109
MCO-4
74.2
16.64
0.167Figure 7
The N2 adsorption-desorption isotherms of Mn-doped CeO2 catalysts with various Mn contents: (a) MCO-1, (b) MCO-2, (c) MCO-3, and (d) MCO-4.
(a)
(b)
(c)
(d)In redox catalysis, the role of ceria is usually to act as an oxygen transferring component. The oxygen storage capacity (OSC) and the reducibility are important characteristics to determine its catalytic properties. The OSC results for all samples are displayed in Table4. Obviously, all the three Mn-doped CeO2 samples have much higher OSC than the pure CeO2. MCO-3 sample exhibited an OSC of 166.2 μmol O2/g, which is much higher than that of the other Mn-doped CeO2. These results are consistent with the Raman and XPS results evidencing structure defects. Previous studies have reported that the presence of defects in the structure and the exposure of more reactive crystallite planes at the surface should facilitate the formation of oxygen vacancies and enhance the OSC [41–43]. Therefore, the higher oxygen consumption is related to the defect density and the exposure of crystallite planes which is associated with the lower energy of formation of oxygen vacancies.Table 4
Oxygen storage capacity (OSC) of pure CeO2 and Mn-doped CeO2 with various Mn contents.
Samples
Pure CeO2
MCO-1
MCO-2
MCO-3
MCO-4
OSC (μmol O2/g)
89.5
111.5
133.0
166.2
155.4H2-TPR was performed to explore the oxygen reactivity and reducibility of the pure ceria and Mn-doped ceria. Generally, the reducibility of oxide is associated with the formation of oxygen vacancies: the more susceptibly reducible an oxide is, the easier it can generate oxygen vacancies [11]. The H2 consumption profiles as a function of temperature for all of the samples are shown in Figure 8. The reduction behavior of pure CeO2 was divided into two steps: the α peak at lower temperature (350–550°C) is due to the reduction of surface oxygen of CeO2, and the β peak at higher temperature (ca. 820°C) is due to the reduction (Ce4+ → Ce3+) of bulk CeO2 [12–16, 25–28]. The β peak of bulk CeO2 reduction was commonly observed at around 820°C, with no significant change being observed for any samples. However, the α peak of surface reduction was changed significantly upon Mn doping, and new peak (γ) has appeared below 300°C due to the reduction of doped Mn element (Mn3+→ Mn2+) [13]. Owing to the doping with Mn element, the α peaks are shifted to lower temperature, and the peak areas increase. In the MCO-3 and MCO-4 samples, the α peaks are around 376°C, which are lower than those of MCO-1 (415°C) and MCO-2 (406°C) samples. Additionally, the γ peak of MCO-4 sample is at 261°C, while the γ peak shifts to the lower temperature (238°C). Therefore, it is obvious that the MCO-3 sample shows high redox properties at the lowest temperature among Mn-doped CeO2 samples with various manganese contents. From these observations, it is evident that when Mn ions are doped into the ceria, the surface oxygen concentration has been improved as more oxygen vacancies are produced. This is good in agreement with the results of the Raman, XPS, and OSC analyses. Therefore, a higher concentration of these surface defects can be expected for Mn-doped ceria. It is generally known that ceria can trap and release oxygen via the transformation between Ce3+ and Ce4+. When Mn dopant was incorporated, the Mn-doped CeO2 samples can easily trap and release oxygen via the interaction between Mn3+/Mn2+ and Ce4+/Ce3+, and simultaneously the surface oxygen can participate in the CH4 catalytic oxidation. Consequently, the MCO-3 sample may exhibit an excellent catalytic performance at the lowest temperature as a result of the highest redox properties, which will also be verified by the catalytic activity evaluation in the following text.Figure 8
H2-TPR profiles of pure CeO2 and Mn-doped CeO2 catalysts with different Mn contents.


### 3.2. Catalytic Performance of Mn-Doped CeO2 Flower-Like Microstructures with Various Manganese Contents

Catalytic oxidation of CH4 to CO2 and H2O under oxygen-rich condition plays an important role in energy supply using natural gas and here is used as a probe reaction to evaluate the catalytic performance of the Mn-doped CeO2 samples. Figure 9(a) shows the CH4 conversions at various temperatures over Mn-doped CeO2 with various Mn contents. It is obvious that Mn-doped CeO2 samples display enhanced catalytic activity for CH4 oxidation, which is more active than that of pure CeO2. It is worth noting that the MCO-3 sample has higher activity than the catalysts with higher or lower Mn content. The reaction temperatures at CH4 conversions of T10 and T50 are summarized in Table 5. The value of T10 and T50 in the MCO-3 sample is 339 and 405°C, respectively, which is much lower than that of the other Mn-doped CeO2 samples; and T90 was observed at 457°C for the MCO-3 sample. The results show that adding Mn in CeO2 can obviously promote the catalytic activity of the Mn-doped CeO2, which could be interpreted in terms of the facile reduction property induced by adding Mn in CeO2. Kinetic studies have shown that the reaction mechanism of CH4 oxidation over metal oxide nanocrystals is the Mars-van Krevelen redox model. The reoxidation of the reduced metal oxide sites by the gaseous oxygen is the rate-limiting step [12, 44]. High bulk oxygen mobility and formation of highly active oxygen species activated by the oxygen vacancies are widely recognized as the main factors influencing the catalytic activity of binary oxides for CH4 catalytic oxidation activity [12]. In our work, the improvement in catalytic activity can be attributed to the incorporation of extraneous atoms into CeO2 fluorite lattice. The interaction between Mn2+/Mn3+ and Ce3+/Ce4+ couples takes place at boundaries of ceria, which leads to the valence changes of manganese species [13, 45, 46]. After a small amount of Mn ions is introduced into the CeO2 lattice, the replacement of Mnn+ for Ce4+ results in a slight lattice contraction in the ceria lattice due to the smaller size of Mn ion and, more importantly, the generation of oxygen vacancies for charge compensation. Thus free oxygen molecules in reactant gas would be captured by these oxygen vacancies in the CeO2 lattice to form active oxygen species, leading to more adsorbed reactant molecules being oxidized to CO2 in turn. From the characterization and calculation results, the MCO-3 sample has a higher surface area, providing easily accessible pores for gas diffusion, which also favors the efficient oxidation of CH4. Moreover, higher oxygen mobility and richer surface active oxygen species are achieved in the MCO-3 sample. These are beneficial to the oxidation-reduction reaction. These are the reasons why the MCO-3 sample shows a better catalytic performance.Table 5
The reaction temperatures at CH4 conversions of 10% (T10) and 50% (T50).
Samples
Pure CeO2
MCO-1
MCO-2
MCO-3
MCO-4
T
10 (°C)
418
387
370
339
360
T
50 (°C)
—
457
446
405
432Figure 9
(a) Plots of CH4 conversion versus temperature over pure CeO2 and Mn-doped CeO2 with various manganese contents; (b) catalytic stability test of Mn-doped CeO2 with various manganese contents.
(a)
(b)Catalytic stabilities for CH4 oxidation were further investigated over these Mn-doped CeO2 samples at 450°C for 82 h. As shown in Figure 9(b), the CH4 conversion over the MCO-3 sample is 80% during the first run and then tended to decrease, but it is still kept above 60% after 82 h on stream. The reason for deactivation could be attributed to the coke formation and/or the textural changes at high temperatures which could decrease the active sites. More work is underway to determine the underlying catalytic mechanism and the reason for deactivation of the doped ceria microstructures, and the result will be reported elsewhere. However, it can be seen from the CH4 conversion versus time on stream curves that the other three Mn-doped CeO2 samples demonstrate robust long-term stabilities with less than 5% changes relative in the absolute CH4 conversions after 82 h on stream.


## 3.1. Characteristics of Mn-Doped CeO2 Flower-Like Microstructures with Various Manganese Contents

To investigate whether there was a hybrid synergic effect in CH4 combustion reaction, we acquired detailed information on the structure and local atomic composition of the Mn-doped ceria with various Mn contents. Fundamental characteristics of the samples were revealed by FT-IR, XRD, SEM, EDS, XPS, Raman, BET, OSC, and H2-TPR.A polyol-based precursor route was developed to synthesize the Mn-doped CeO2 samples with various Mn contents. Figure 1 displays the typical FT-IR spectrum of the MCO-1 precursor. The vibrational bands of νa(CH2) and νs(CH2) at 2888 and 2844 cm−1 as well as the strong peak of ν(C–O) band at 1102 cm−1 derived from the ethylene glycol unit were observed, and the stretching vibrations of carboxylate group in acetate ions, νa(COO−) and νs(COO−), at 1465 and 1382 cm−1 were also detected. A broader band occurring at 3395 cm−1 can be attributed to the stretching vibration of OH groups linked by hydrogen bonds, and the band at 899 cm−1 can be viewed as ν(C–C). Thus, we conclude that the precursor compound appears to be an alkoxide, which is similar to those previously reported metallic alkoxide precursors in ethylene glycol-mediated process [17–22].Figure 1
Typical FT-IR spectrum of the as-obtained MCO-1 precursor.XRD was employed to ascertain the change in bulk crystal structure for CeO2 support. Figure 2 shows the XRD patterns of the Mn-doped CeO2 samples with various Mn contents prepared by heat treatment of those precursors. The 2θ values were located at 28.5°, 33.1°, 47.4°, 56.2°, 59.0°, and 69.4° for the pure CeO2. It is clear that the diffraction peaks of all the samples correspond to the (111), (200), (220), and (311) planes that can be indexed to the cubic fluorite structure of CeO2 crystals (JCPDS Card number 34-0394). The peak positions showed no critical change upon doping with guest metals; and no peaks were observed corresponding to doped metal and other individual oxides. The peaks of MnOx are not detected in the Mn-doped CeO2 samples even when the amount of initial Mn content in the raw material reached up to 30 mol%, which indicates the existence of well dispersion of MnOx species on the surface of CeO2 and/or the incorporation of Mn into the CeO2 lattice. However, the decrease of peak intensity and the slight increase of the peak width with the introduction of the dopant indicate that the grain sizes decrease after the metal ions are doped into the ceria. Moreover, as shown in Table 1, the lattice parameters obtained from the calculation of the (111) peak of Mn-doped CeO2 are smaller than that of pure CeO2, which can prove that Mn atoms probably replace some of Ce sites and enter into the CeO2 lattice [23]. Because the ionic radius of Mnn+ (Mn4+ = 0.53 Å, Mn3+ = 0.645 Å, and Mn2+ = 0.83 Å) is smaller than that of Ce4+ (1.01 Å), when Mnn+ embedded in CeO2 lattice and takes the place of Ce4+, the contraction and distortion of the ceria lattice occur, leading to the decrease of the cell parameter [24–26].Table 1
Lattice parameters and the proportions of O′′ and Mn3+ of pure CeO2 and Mn-doped CeO2 samples calculated from XRD and XPS, respectively.
Samples
Lattice parameter (Å)
O′′/(O′′ + O′) (%)
Mn3+/(Mn2+ + Mn3+) (%)
Pure CeO2
5.4113
39.5
—
MCO-1
5.4059
44.7
44.9
MCO-2
5.3983
45.4
45.1
MCO-3
5.3938
50.6
56.1
MCO-4
5.4015
45.9
56.8Figure 2
XRD patterns of Mn-doped CeO2 samples with different Mn contents.Raman scattering is an effective tool for the investigation of the effects of doping on nanomaterials, as the incorporation of dopants leads to shifts of the lattice Raman vibrational peak positions. Figure3 displays the Raman spectra of pure CeO2 as well as Mn-doped CeO2 samples with different Mn contents. For the pure CeO2, a strong peak at 463 cm−1 can be assigned to the F2g Raman active mode of the cubic fluorite structure of CeO2, which is due to the symmetric breathing mode of the oxygen atoms around cerium ions. The band at around 279 cm−1 can be related to the oxygen vacancies in CeO2 lattice attributed to the presence of defective structure [13, 27]. Compared to the pure CeO2, the peak intensity decreased greatly and became broader and red-shifted for the Mn-doped CeO2. The red-shift could be attributed to the changes in lattice parameter with crystallite size, as it was previously reported that a decrease of the particle size of CeO2 from 5 μm to 6.1 nm resulted in a shift to lower energy and was well explained by phonon confinement model [14, 28–30]. Additionally, the downshift is plausibly related to the presence of the Mn dopant, which would give rise to an increase in optical absorption [13, 31]. Another reason of shifting and broadening may be the increase in oxygen vacancies, which is related to structural defects derived from partially incorporation of manganese into CeO2 lattice, in agreement with the decrease of lattice parameter [32]. In the Mn-doped ceria samples, the extra oxygen vacancies were generated by the incorporation of Mn ion into the ceria fluorite lattice to compensate for the valence mismatch between the Mnn+ and Ce4+ ions. One piece of supporting evidence for the possible increase of defect density is that the as-prepared pure CeO2 sample shows a light yellow color, while the Mn-doped samples present various shades of taupe colors [14, 33].Figure 3
Raman spectra of pure CeO2 and Mn-doped CeO2 samples with different Mn contents. Peak positions (F2g) are shown on the right.The detailed morphologies and microstructures of the as-obtained Mn-doped CeO2 with different Mn contents were characterized by SEM. As shown in Figure 4, the samples are composed of a great deal of flower-like architectures with a diameter of 2-3 μm, and the entire microstructure of the architecture was built from petals which connected with each other forming the flower-like microstructure by self-assembly. The results implied that doping Mn in CeO2 did not change the total flower-like morphology. To determine the elemental compositions of the flower-like microstructures, EDS analysis has been carried out. The EDS spectrum and elemental mapping of the MCO-1 sample were depicted in Figure 5. Specifically, it appears that the pattern peaks of Mn, Ce, and O are clearly evident in the spectra collected, revealed the existence of the elements, and are accompanied with strong Au signals originated from gold plating on the sample before SEM examination. The elemental mapping results illustrate that the sample is mixed-metal oxide rather than a mixture of pure Mn and Ce phases. Moreover, the actual Mn/Ce ratios of the as-synthesized samples calculated from EDS are listed in Table 2. As can be seen, the actual Mn/Ce ratios in the products increased with the Mn/Ce ratios in the starting materials. The actual Mn/Ce ratios for the samples with the starting Mn/Ce ratios of 0.1, 0.15, 0.2, and 0.3 in the initial reactant compositions are 0.062, 0.070, 0.078, and 0.087, respectively. In the series of synthetic processes, the initial Mn/Ce molar ratio in the starting materials did not totally coincide with that of these solid precipitation, and it is more likely to follow a curved relation for the powder synthesized in EG, which coincided with our previously reported results [18]. The EDS results indicate that the doped Mn contents are smaller than the initial reactant compositions; in other words, only a portion of the added Mn ions incorporate into the ceria lattice. This may be due to the large disparity of the ionic radii, which might make the insertion into the ceria lattice more difficult [34].Table 2
Actual Mn/Ce ratios of as-synthesized Mn-doped CeO2 samples based on the EDS results.
Samples
MCO-1
MCO-2
MCO-3
MCO-4
Starting Mn/Ce ratio
0.1
0.15
0.2
0.3
Actual Mn/Ce ratio
0.062
0.070
0.078
0.087Figure 4
SEM images of the Mn-doped CeO2 samples with different Mn contents: (a) MCO-1, (b) MCO-2, (c) MCO-3, and (d) MCO-4 and (e) pure CeO2.
(a)
(b)
(c)
(d)
(e)Figure 5
Typical EDS spectrum (a) and elemental mapping (b) of the as-synthesized MCO-1 sample.
(a)
(b)XPS was performed in order to further illuminate the surface composition and the chemical state of the elements existing in Mn-doped CeO2 samples with various Mn contents. The XPS results suggest that the surface Mn/(Mn + Ce) ratios were rather low, even when the amount of initial Mn content in the raw material reached up to 30 mol% (surface Mn/(Mn + Ce) ≈ 0.072), which coincided with the EDS results. As displayed in Figure 6(a), the two sets of spin-orbital multiplets, corresponding to the Ce 3d3/2 and Ce 3d5/2 contributions, are labeled as u and v [15, 35–37]. For 3d5/2 of Ce(IV), the Ce 3d94f2Ln−2 and Ce 3d94f1Ln−1 states form the peaks v and v′′, and the Ce 3d94f1Ln state corresponds to the peak v′′′. For 3d5/2 of Ce(III), the Ce 3d94f2Ln−1 and Ce 3d94f1Ln states produce the peaks v° and v′. For Ce 3d3/2 labeled as u, the same assignment can be carried out. The result suggests that there is a certain amount of Ce3+ in all the Mn-doped CeO2 samples.Figure 6
XPS region spectra of (a) Ce 3d, (b) O 1s, and (c) Mn 2p for pure CeO2 (i) and Mn-doped CeO2 samples with different Mn contents: (ii) MCO-1, (iii) MCO-2, (iv) MCO-3, and (v) MCO-4.
(a)
(b)
(c)The O 1s XPS spectra for the Mn-doped ceria samples early show the existence of two states of surface oxygen atoms (Figure6(b)). The main peak O′ at ca. 529.4 eV is characteristic of lattice oxygen atoms; an apparent shoulder peak O′′ at ca. 531.3 eV has been assigned to oxide defects or absorbed oxygen ions with low coordination [13, 15, 16]. The strong peaks of the catalysts at 531.3 eV suggest that they are expected to have better oxygen storage capacity, which would be promising for their higher catalytic oxidation activity. As shown in Table 1, the ratio of O′′ of the MCO-3 sample obviously increased (50.6%), indicating that the content of surface oxygen vacancy is increased by doping suitable amounts of Mn. However, the surface oxygen vacancy contents would be decreased with further increase in the Mn contents, which may be due to the formation of bulk MnOx on the surface.The Mn 2p XPS spectra of Mn-doped CeO2 samples are displayed in Figure 6(c). The peaks are weak because of the low metal concentration of the surface elements; however, the compositions can still be identified in the spectra. The double peaks with binding energies of ca. 641.6 and 653.3 eV correspond to the characteristic of Mn 2p3/2 and Mn 2p1/2 signals, respectively [38, 39]. After refined fitting, the spectrum could be deconvolved into four peaks. The peaks at 641.3 and 653.3 eV can be assigned to the presence of Mn(II), while the other two peaks at 643.6 and 656.5 eV are characteristic of the Mn(III). This result suggests the coexistence of Mn2+/Mn3+ ion couple in the Mn-doped CeO2 samples. The relative concentrations of Mn3+ are summarized in Table 1. It is obvious that the proportion of Mn3+ increases with the increase of Mn doping concentration.As discussed above, the MCO-3 sample contains more amount of Mn3+ species and oxide defects (O′′), which are expected to exhibit different reduction properties and catalytic oxidation activities subsequently. These results provide an evidence of existence of redox equilibrium of Mn3+  +  Ce3+  ↔  Mn2+  +  Ce4+, which has been claimed to be the source of a synergistic interaction between manganese and ceria species in the Mn-doped CeO2 catalysts.The textural properties of the as-synthesized Mn-doped CeO2 samples were further investigated by measuring adsorption-desorption isotherms of N2 at 77 K, as shown in Figure 7. The hysteresis features of these samples should be classified as type H3 loop, suggesting the presence of aggregates of plate-like particles which give rise to slit-shaped pores [10, 40]. The texture data of the series of the samples are summarized in Table 3. Herein, the specific surface areas using the BET method for these samples are 56.0, 75.7, 91.0, and 74.2 m2/g, respectively. It was found that the MCO-3 sample exhibited higher BET surface area and smaller BJH pore size than those of the other Mn-doped CeO2 samples. Thus, such high surface areas will undoubtedly benefit surface adsorption during catalytic reactions.Table 3
BET surface areas, average pore sizes, and total pore volumes of Mn-doped CeO2 with various Mn contents.
Samples
BET surface area (m2/g)
Average pore size (nm)
Total pore volume (cm3/g)
MCO-1
56.0
13.04
0.100
MCO-2
75.7
8.12
0.085
MCO-3
91.0
7.90
0.109
MCO-4
74.2
16.64
0.167Figure 7
The N2 adsorption-desorption isotherms of Mn-doped CeO2 catalysts with various Mn contents: (a) MCO-1, (b) MCO-2, (c) MCO-3, and (d) MCO-4.
(a)
(b)
(c)
(d)In redox catalysis, the role of ceria is usually to act as an oxygen transferring component. The oxygen storage capacity (OSC) and the reducibility are important characteristics to determine its catalytic properties. The OSC results for all samples are displayed in Table4. Obviously, all the three Mn-doped CeO2 samples have much higher OSC than the pure CeO2. MCO-3 sample exhibited an OSC of 166.2 μmol O2/g, which is much higher than that of the other Mn-doped CeO2. These results are consistent with the Raman and XPS results evidencing structure defects. Previous studies have reported that the presence of defects in the structure and the exposure of more reactive crystallite planes at the surface should facilitate the formation of oxygen vacancies and enhance the OSC [41–43]. Therefore, the higher oxygen consumption is related to the defect density and the exposure of crystallite planes which is associated with the lower energy of formation of oxygen vacancies.Table 4
Oxygen storage capacity (OSC) of pure CeO2 and Mn-doped CeO2 with various Mn contents.
Samples
Pure CeO2
MCO-1
MCO-2
MCO-3
MCO-4
OSC (μmol O2/g)
89.5
111.5
133.0
166.2
155.4H2-TPR was performed to explore the oxygen reactivity and reducibility of the pure ceria and Mn-doped ceria. Generally, the reducibility of oxide is associated with the formation of oxygen vacancies: the more susceptibly reducible an oxide is, the easier it can generate oxygen vacancies [11]. The H2 consumption profiles as a function of temperature for all of the samples are shown in Figure 8. The reduction behavior of pure CeO2 was divided into two steps: the α peak at lower temperature (350–550°C) is due to the reduction of surface oxygen of CeO2, and the β peak at higher temperature (ca. 820°C) is due to the reduction (Ce4+ → Ce3+) of bulk CeO2 [12–16, 25–28]. The β peak of bulk CeO2 reduction was commonly observed at around 820°C, with no significant change being observed for any samples. However, the α peak of surface reduction was changed significantly upon Mn doping, and new peak (γ) has appeared below 300°C due to the reduction of doped Mn element (Mn3+→ Mn2+) [13]. Owing to the doping with Mn element, the α peaks are shifted to lower temperature, and the peak areas increase. In the MCO-3 and MCO-4 samples, the α peaks are around 376°C, which are lower than those of MCO-1 (415°C) and MCO-2 (406°C) samples. Additionally, the γ peak of MCO-4 sample is at 261°C, while the γ peak shifts to the lower temperature (238°C). Therefore, it is obvious that the MCO-3 sample shows high redox properties at the lowest temperature among Mn-doped CeO2 samples with various manganese contents. From these observations, it is evident that when Mn ions are doped into the ceria, the surface oxygen concentration has been improved as more oxygen vacancies are produced. This is good in agreement with the results of the Raman, XPS, and OSC analyses. Therefore, a higher concentration of these surface defects can be expected for Mn-doped ceria. It is generally known that ceria can trap and release oxygen via the transformation between Ce3+ and Ce4+. When Mn dopant was incorporated, the Mn-doped CeO2 samples can easily trap and release oxygen via the interaction between Mn3+/Mn2+ and Ce4+/Ce3+, and simultaneously the surface oxygen can participate in the CH4 catalytic oxidation. Consequently, the MCO-3 sample may exhibit an excellent catalytic performance at the lowest temperature as a result of the highest redox properties, which will also be verified by the catalytic activity evaluation in the following text.Figure 8
H2-TPR profiles of pure CeO2 and Mn-doped CeO2 catalysts with different Mn contents.


## 3.2. Catalytic Performance of Mn-Doped CeO2 Flower-Like Microstructures with Various Manganese Contents

Catalytic oxidation of CH4 to CO2 and H2O under oxygen-rich condition plays an important role in energy supply using natural gas and here is used as a probe reaction to evaluate the catalytic performance of the Mn-doped CeO2 samples. Figure 9(a) shows the CH4 conversions at various temperatures over Mn-doped CeO2 with various Mn contents. It is obvious that Mn-doped CeO2 samples display enhanced catalytic activity for CH4 oxidation, which is more active than that of pure CeO2. It is worth noting that the MCO-3 sample has higher activity than the catalysts with higher or lower Mn content. The reaction temperatures at CH4 conversions of T10 and T50 are summarized in Table 5. The value of T10 and T50 in the MCO-3 sample is 339 and 405°C, respectively, which is much lower than that of the other Mn-doped CeO2 samples; and T90 was observed at 457°C for the MCO-3 sample. The results show that adding Mn in CeO2 can obviously promote the catalytic activity of the Mn-doped CeO2, which could be interpreted in terms of the facile reduction property induced by adding Mn in CeO2. Kinetic studies have shown that the reaction mechanism of CH4 oxidation over metal oxide nanocrystals is the Mars-van Krevelen redox model. The reoxidation of the reduced metal oxide sites by the gaseous oxygen is the rate-limiting step [12, 44]. High bulk oxygen mobility and formation of highly active oxygen species activated by the oxygen vacancies are widely recognized as the main factors influencing the catalytic activity of binary oxides for CH4 catalytic oxidation activity [12]. In our work, the improvement in catalytic activity can be attributed to the incorporation of extraneous atoms into CeO2 fluorite lattice. The interaction between Mn2+/Mn3+ and Ce3+/Ce4+ couples takes place at boundaries of ceria, which leads to the valence changes of manganese species [13, 45, 46]. After a small amount of Mn ions is introduced into the CeO2 lattice, the replacement of Mnn+ for Ce4+ results in a slight lattice contraction in the ceria lattice due to the smaller size of Mn ion and, more importantly, the generation of oxygen vacancies for charge compensation. Thus free oxygen molecules in reactant gas would be captured by these oxygen vacancies in the CeO2 lattice to form active oxygen species, leading to more adsorbed reactant molecules being oxidized to CO2 in turn. From the characterization and calculation results, the MCO-3 sample has a higher surface area, providing easily accessible pores for gas diffusion, which also favors the efficient oxidation of CH4. Moreover, higher oxygen mobility and richer surface active oxygen species are achieved in the MCO-3 sample. These are beneficial to the oxidation-reduction reaction. These are the reasons why the MCO-3 sample shows a better catalytic performance.Table 5
The reaction temperatures at CH4 conversions of 10% (T10) and 50% (T50).
Samples
Pure CeO2
MCO-1
MCO-2
MCO-3
MCO-4
T
10 (°C)
418
387
370
339
360
T
50 (°C)
—
457
446
405
432Figure 9
(a) Plots of CH4 conversion versus temperature over pure CeO2 and Mn-doped CeO2 with various manganese contents; (b) catalytic stability test of Mn-doped CeO2 with various manganese contents.
(a)
(b)Catalytic stabilities for CH4 oxidation were further investigated over these Mn-doped CeO2 samples at 450°C for 82 h. As shown in Figure 9(b), the CH4 conversion over the MCO-3 sample is 80% during the first run and then tended to decrease, but it is still kept above 60% after 82 h on stream. The reason for deactivation could be attributed to the coke formation and/or the textural changes at high temperatures which could decrease the active sites. More work is underway to determine the underlying catalytic mechanism and the reason for deactivation of the doped ceria microstructures, and the result will be reported elsewhere. However, it can be seen from the CH4 conversion versus time on stream curves that the other three Mn-doped CeO2 samples demonstrate robust long-term stabilities with less than 5% changes relative in the absolute CH4 conversions after 82 h on stream.


## 4. Conclusions

In summary, Mn-doped CeO2 flower-like microstructures have been successfully synthesized via a polyol-based precursor process at 180°C and subsequent direct thermal decomposition at 450°C. The resultant samples were used as catalysts in CH4 combustion under oxygen-rich condition. Catalytic results suggest that the Mn-doped CeO2 show relatively higher activity. The fundamental characteristics of the Mn-doped CeO2 samples with different Mn contents were revealed to investigate whether there was a hybrid synergic effect in CH4 combustion reaction. SEM results reveal that the doping Mn ions in CeO2 did not change the total flower-like morphology. BET, XPS, OSC, and H2-TPR results suggest that the higher surface area, more Mn3+, richer surface active oxygen species, and higher bulk oxygen mobility are responsible for the better performance of the MCO-3 sample. The as-obtained doped CeO2 should be a promising material for environmental application and is expected to be useful in many other application fields. It is also believed that this synthetic method may provide a powerful synthetic technology for the future application of binary/ternary metal oxide nano/microstructures.



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*Source: 254750-2015-12-08.xml*