Myeong Ho
Kim ‡
,
Gajendra
Gupta ‡
and
Jinkwon
Kim
*
Department of Chemistry, Nanotechnology Laboratory, Kongju National University, 182 -Shinkwan Kongju-Chungnam, 314-701, Republic of Korea. E-mail: jkim@kongju.ac.kr; Fax: +82 418528496; Tel: +82418568613
First published on 5th October 2012
Solution-based synthetic routes are attractive strategies for synthesizing GeTe materials, because they have the potential to impart morphology control on the crystallites and permit liquid-based processing of films and patterned structures. Two liquid phase reaction systems for GeTe nanoparticles (NPs) have been studied using GeCl2·dioxane and trioctylphosphine-tellurium (TOP-Te) in oleylamine (OLA) as solvent and reducing agent and using GeCl2·dioxane and (Et3Si)2Te in trioctylphosphine oxide (TOPO) without the use of any reducing agent. The morphology of the GeTe powders had a strong dependence on the Te source and reaction medium. The SEM image of NPs obtained by the reaction of GeCl2·dioxane and (Et3Si)2Te reveals that with an increase in reaction time (2, 10, 15 and 30 min), the size of the NPs increases and their shape becomes uniform. However, it is interesting to observe that after 30 min, the morphology of the nanoparticles was maintained even after longer reaction times i.e., the duration of heating had no pronounced influence on the size and morphology of the nanocrystals after a particular period of time. Reaction with TOP-Te leads to the formation of irregular GeTe nanocrystals through the so called Ostwald-ripening process. However, with (Et3Si)2Te as Te source, a ligand exchange reaction mechanism has been proposed leading to the formation of well-dispersed GeTe nanoparticles of uniform shape.
Solution-based synthetic routes represent an attractive alternative for depositing films and generating dimensionally controlled nanoscale materials, including for quantum-confined binary antimonide and telluride semiconductors. Formation of colloidal faceted GeTe particles and phase change memory materials with distinct properties are recently reported.10–13 However, there have been very few reports describing liquid-phase routes to chalcogenide phase change materials. Recently, R. E. Schaak and co-workers described an important addition to the small number of reports on solution routes to Ge-based phase change materials: a bench top liquid-phase synthesis of crystalline GeTe via reduction of GeI2 with tert-butylaminoborane (TBAB) in the presence of TOP-Te at 180 °C.14 The GeTe product consists of highly faceted microcrystals having cube-shape morphology with a narrow size distribution. More recently, Alivisatos et al. demonstrated size dependent polar ordering by the synthesis of GeTe nanocrystals over a wide range of sizes.15,16 The production of these nanocrystals of widely varying sizes is facilitated by the use of Ge(II) precursors with different reactivities. In all the recent progress, TOP-Te has been generally used for the synthesis of GeTe nanocrystals. On the other hand, alkylsilyl compounds of Te have been exploited as efficient precursors in the atomic layer deposition (ALD) process for Ge2Sb2Te5 (GST) thin film.17 Particularly, (Et3Si)2Te proved to be a better ALD precursor compared to alkyls and alkylamides of Te. Upon reaction with metal halides, the exchange reaction is facilitated by fast bonding of trialkylsilyl moieties and halides. Based on the above considerations, we have conducted two liquid phase syntheses of GeTe nano crystals; one method via reduction of GeCl2·dioxane with OLA in the presence of TOP-Te, another method via the substitution reaction of GeCl2·dioxane and (Et3Si)2Te in TOPO. Smaller GeTe products are obtained with (Et3Si)2Te as Te source as compared to its TOP-Te analogue. These two reactions show that the shape and size are strongly dependent on the Te precursor.
A clear yellow TOP-Te complex stock solution (0.75 M) was first prepared by dissolving 288 mg Te powder in 3 mL trioctylphosphine (TOP) at 200 °C. GeCl2·dioxane (0.75 mmol, 173.73 mg) was dissolved in 1 mL TOP via sonication. Oleylamine (15 mL) was placed in a three neck flask and dried under vacuum at 70 °C for 1 h. Then the reaction flask was flushed with nitrogen and the temperature was raised to 150 °C and the Ge precursor solution was injected. The solution color immediately changed from colorless to yellow, presumably due to the reduction of Ge2+ to Ge0. After 1 min, 1 mL of 0.75 M TOP-Te solution was injected into the Ge solution and stirred for the desired time and the reaction was allowed to cool down to room temperature. The resulting GeTe precipitate was purified by washing with 1:1 acetone/chloroform and dried under vacuum, yielding a gray powder.
(b) Synthesis of GeTe nanocrystals using substitution reaction (sample 2)
GeCl2·dioxane (0.75 mmol, 173.73 mg) was dissolved in 2 mL TOP via ultrasonication. TOPO (4 g) was placed in a three neck flask and dried under vacuum at 70 °C for 1 h. Then the reaction flask was flushed with nitrogen and the temperature was raised to 250 °C and the Ge precursor solution was injected. The Te precursor (Et3Si)2Te (0.75 mmol, 268.1 mg) was dissolved in 2 mL TOP via sonication, and was injected into the reaction mixture and stirred for the desired time and the reaction was allowed to cool down to room temperature. The resulting GeTe precipitate was purified by washing with 1:1 acetone/chloroform and dried under vacuum, yielding a gray powder.
Fig. 1 XRD patterns of rhombohedral GeTe crystals composed of (a) reference, (b) amorphous sample, (c) sample 1 and (d) sample 2. |
SEM images of sample 1 and sample 2 at different reaction times are displayed in Fig. 2 and Fig. 3, respectively. For sample 1, at the beginning of the reaction, the products are amorphous with a size of about 20 nm as displayed in Fig. 2a, but after 10 min, the amorphous powders start to agglomerate and transform into bigger crystalline particles of different sizes. After 30 min, the final size and shape of the crystals are formed without further significant change. In the case of sample 2, amorphous powders formed in the initial stage of the reaction turned crystalline without significant growth of particles, as shown in Fig. 3a and 3b. Further heating of the reaction mixture produced uniform GeTe crystals.
Fig. 2 SEM images of GeTe crystals (sample 1) produced from reaction of Ge2+ and TOP-Te in OLA at 150 °C and reaction times of (a) 2 min, (b) 10 min, (c) 30 min, (d) 60 min. |
Fig. 3 SEM images of GeTe crystals (sample 2) produced from reaction of Ge2+ and (Et3Si)2Te in TOPO at 250 °C and reaction times of (a) 2 min, (b) 10 min, (c) 30 min, (d) 60 min (inset: SEM image of a single GeTe crystal). |
On the basis of the above observations, plausible growth mechanisms of GeTe NPs can be suggested as illustrated in Scheme 1. In the reduction method, i.e., for sample 1, the growth process can be explained by two steps, an initial nucleating stage and a subsequent crystal growth process. The Ge atoms were formed by reduction of Ge2+ by oleylamine. At the same time, Te atoms were also formed in solution by thermal decomposition. These two species in solution immediately react to produce GeTe seed crystals. As the reaction time increases, the GeTe seed crystals start to agglomerate together to form much bigger crystals as shown in Fig. 2b. With further increase in reaction time, larger GeTe NPs grow at the expense of smaller ones through the so called Ostwald-ripening process when the temperature is maintained at 150 °C. This prolonged heating can supply enough energy to the system to overcome the energy barrier for ripening.18 During this process, smaller particles will dissolve to feed the growth of larger ones. Thus, only irregular nanocrystals are formed.
Scheme 1 Schematic illustration for the growth processes of GeTe nanocrystals. |
However, in the case of NPs formed from the reaction of Ge2+ and (Et3Si)2Te in TOPO, a ligand exchange reaction as shown in eqn (1) takes place to form GeTe seed powders. In this case, we assume that the rate of the substitution reaction might be slower than that in the case of sample 1. Furthermore, the seeds tend to grow bigger crystals by subsequent reaction of Ge2+ and Te2− ions instead of the agglomeration of seeds. SEM images show that the duration of heating had no pronounced influence on the size and morphology of the nanocrystals after a reaction period of 30 min. The completed reaction mixture shows none of the smaller particles. Thus, refluxing for 30 min and 1 h resulted in similar size and shape of the synthesized nanocrystals. A highly practical feature of our ligand exchange method is that the final nanocrystals’ size is highly reproducible. From this above two different growth behaviours, we assume that the Te source plays a very important role in determining the shape and size of the nanocrystals.
(1) |
Fig. 4 (a) TEM and (b) HRTEM images of the GeTe crystals produced from reaction of Ge2+ and (Et3Si)2Te in TOPO at 250 °C and a reaction time of 1 h. |
Fig. 5 Size distribution histograms for the GeTe crystallites obtained at 1 h using (a) TOP-Te and (b) (Et3Si)2Te. |
The thermal behaviour of samples containing GeTe particles was investigated using DSC as shown in Fig. 6. Fig. 6a shows the curve for sample 1 obtained at 1 h, whereas Fig. 6b displays the curve of sample 2 at 1 h. In Fig. 6a, an endotherm is observed at 724.1 °C which agrees well with the melting point of bulk GeTe (725 °C).19 Whereas, in Fig. 6b, an endotherm is observed at 721.8 °C.
Fig. 6 DSC traces for the GeTe crystals for (a) sample 1 and (b) sample 2 at 1 h reaction times. |
Inferences of the oxidation state of germanium and tellurium atoms in the nanomaterials were assigned through XPS. Fig. 7 shows the XPS data of sample 1 measured in the Ge 3d and Te 3d regions for GeTe crystals after etching to remove the oxide layer on the surface. A peak binding energy at 29.75 eV for GeTe crystals is attributed to Ge 3d. Peaks for Te 3d5/2 and Te 3d3/2 were observed at 573 eV and 583.45 eV. Peak values of Ge 3d and Te 3d of GeTe nanocrystals are in good agreement with values reported in the literature.19,20 The surface of GeTe crystals were oxidized upon exposure to air for a long time.21–23
Fig. 7 XPS spectra of the GeTe product (sample 1) in the Ge 3d and Te 3d regions. |
Footnotes |
† Electronic Supplementary Information (ESI) available: STEM image and EDS spectrum along with elemental mapping and XPS spectra of the GeTe product. See DOI: 10.1039/c2ra21790b |
‡ These authors contributed equally. |
This journal is © The Royal Society of Chemistry 2013 |