Advanced Search
RSS LinkedIn Twitter

Journal Archive

Platinum Metals Rev., 2013, 57, (3), 161


Preparation of Dispersed Spherical Platinum Particles with Controlled Size and Internal Structure

Versatile and cost-effective route to platinum powders for large scale electronic applications

  • Brendan P. Farrell, Igor V. Sevonkaev and Dan V. Goia*
  • Center for Advanced Materials Processing, Clarkson University,
  • Potsdam, New York 13699, USA
  • *Email:

Article Synopsis

Uniform dispersed spherical platinum particles were precipitated by reducing Pt(IV) hexaammine ([Pt(NH3)6]4+) complex ions with l-ascorbic acid in the presence of polymeric dispersants. By varying the nature and the amount of dispersing agent the average diameter of the Pt spheres could be adjusted between 200 nm and 800 nm. Electron microscopy and X-ray diffraction (XRD) evaluations revealed that the final Pt particles were the result of an irreversible aggregation of small (~6 nm) nanoparticles. The size of the constituent crystallites was controllably increased through a subsequent heat treatment process without affecting the shape or the dispersion of the Pt spheres. The method described represents a versatile and cost-effective route for producing Pt powders at the sub-micrometre or micrometre scale with controlled crystallinity for thick film electronic applications.


The optical (1), catalytic (2) and adsorptive (3, 4) properties of dispersed matter depend not only on their chemical composition but also on the size, shape and structure of individual particles (57). In most applications, particle uniformity is also essential for optimal performance (5, 811). For example, highly uniform Pt particles with different sizes and structures are the preferred choice in electronic (10), catalytic (8, 12, 13) and biomedical (11) applications. The most widely used route to prepare such Pt powders is the liquid phase reduction of Pt salts (14, 15). The primary reasons for the popularity of this approach are the simplicity of the experimental setups and the versatility provided by the variety of solvents, dispersants, complexing agents and reductants used. The selection of the latter is particularly important as it offers the possibility of controlling the reaction kinetics and, implicitly, the properties of precipitated particles (16). Sodium citrate (17, 18), hydrazine (19) and ascorbic acid (2026) are often used for this purpose.

While the solution reduction route typically yields uniform and well dispersed single Pt crystals (14, 27), their size is usually very small (less than 10 nm). This is the reason why for applications requiring large Pt crystals (> 1 μm), as is the case of the manufacture of electrodes (28), the Czochralski (29, 30), zone melting (31), or Clavilier (32) methods are preferred (33) despite their poor control of particle size, uniformity, and dispersion. Chemical precipitation methods can also generate sub-micrometre and micrometre size Pt particles under carefully controlled experimental conditions. As a rule, however, they are highly polycrystalline (i.e. formed by aggregation of small nanosize crystallites) (7, 34) and are seldom suitable for electronic applications. The main reason is the overlap of ‘intraparticle’ sintering of constituent crystallites with the ‘interparticle’ mass transport during densification, which leads to electrode defects. Gases resulting from the decomposition of organics trapped in the grain boundaries further compromise the quality of the sintered metallic structures and their adhesion to the substrate. In order to extend the range of their applications, the crystallinity of the precipitated particles needs to be increased.

In this study we show that precipitated polycrystalline Pt spheres can be subjected to a heat treatment process that increases their crystallinity and eliminates the undesired residual organics without causing irreversible particle aggregation. The resulting powders possess all attributes (uniformity, dispersion, purity, and structure) necessary for obtaining the thin and dense Pt sintered structures sought in most electronic applications.


Materials and Reagents

Hexachloroplatinic acid (H2PtCl6) solution containing 25.6 wt% Pt, ammonium hydroxide (NH4OH) 14.8 N, hydrochloric acid 12.1 N, gum arabic and l-ascorbic acid (C6H8O6) reagent grade were all used as received.

Particles Precipitation and Heat Treatment

All precipitation experiments were carried out in a 1 l jacketed glass reactor connected to a constant temperature bath. In the first step, dispersed hexamine Pt complex particles were prepared by delivering over 20 min 24.4 g of concentrated NH4OH into a stirred H2PtCl6 solution. The latter was prepared in the reaction vessel by adding 30.5 g of concentrated H2PtCl6 (equivalent to 7.8 g Pt metal) into 275 cm3 of deionised water in which various dispersants (see Table I) were previously dissolved for at least 1 hour. Once the addition of ammonia solution was finished, 27.5 g of l-ascorbic acid crystals were rapidly added to the vigorously stirred Pt complex and the temperature was increased to 68°C. After maintaining the dispersion at this temperature for 30 min, the polymeric dispersant was hydrolysed to allow the settling and separation of Pt particles. For this purpose, the temperature and pH of the dispersion were adjusted to 83 ± 2°C and 0.6 ± 0.1 (using concentrated hydrochloric acid solution), respectively, and the stirring was continued for a further 90 min. After settling, the particles were washed several times with deionised water and rinsed with acetone before they were dried at 60°C in vacuum for 6 h.

Table I

Precipitation Conditions and Properties of Precipitated Platinum Spheres

SampleDispersing agentAmount of dispersant, wt% based on PtParticle size, nmSurface area, m2 g−1Weight loss, wt%Crystallite size, nm
S1 Gum arabic 10 550 ± 70 0.4 2.3 6.0 ± 0.5
S2 Gum arabic 20 220 ± 50 1.12 3.4 6.0 ± 0.5
S3 Sodium alginate 3 820 ± 100 0.3 2.9 6.0 ± 0.5

Table I gives the nature and the amount of polymeric dispersant used along with the key data for the Pt particles obtained, while Figure 1 illustrates schematically the precipitation process. The subsequent heat treatment step consisted of keeping the dried and screened powders for variable lengths of time in an inert atmosphere at temperatures of up to 500°C.

Fig. 1.

Schematics of the precipitation process for preparing the spherical platinum particles used in this study. FR (1 and 2) stand for ‘flow rate’ and indicate pumps used to deliver the reagents in a controlled manner.

CPA = hexachloroplatinic acid; L-AA = l-ascorbic acid; DA = dispersing agent

Schematics of the precipitation process for preparing the spherical platinum particles used in this study. FR (1 and 2) stand for ‘flow rate’ and indicate pumps used to deliver the reagents in a controlled manner.  CPA = hexachloroplatinic acid; L-AA = l -ascorbic acid; DA = dispersing agent


Particle Characterisation

The size and morphology of the metallic particles were assessed by field emission scanning electron microscopy (FESEM) using a JEOL JSM-7400F instrument. ImageJ software (35) was used to determine their size distribution based on the acquired electron micrographs. At least 200 randomly selected particles were measured for this purpose. The crystalline structure of the particles was evaluated by powder XRD with a Bruker AXS D8 FOCUS diffractometer. For the XRD pattern acquisition, the step width and period were 0.01° and 3 s respectively, while the source, sample and detector slits were 2 mm, 0.6 mm and 1 mm. The diffraction patterns obtained were used to calculate the size of the constituent crystallites based on Scherrer's equation (36). (Although this approach to determining the subunit size is not very accurate in absolute terms, it was decided that the significant crystallite size increase (up to an order of magnitude) during heat treatment makes XRD an adequate tool to monitor the change in powder crystallinity). Thermal gravimetric analysis (TGA) measurements (Perkin Elmer Pyris 1 TGA) were used to estimate the amount of organic matter incorporated into the Pt powders.

Results and Discussions

Precipitation of Platinum Spheres

During the slow addition of ammonium hydroxide (Figure 1, Step 2), a yellow precipitate of ammonium hexachloroplatinate was formed, followed by immediate conversion to the bright orange Pt(IV) hexaamine complex. The two consecutive reactions are reflected by Equations (i) and (ii):

H2PtCl6 + 2NH4OH → [NH4]2+[PtCl6]2− + 2H2O (i)

[NH4]2+[PtCl6]2− + 6NH3 → [Pt(NH3)6]4+ + 2NH4+ + 6Cl (ii)

The immediate colour change to green upon the rapid addition of ascorbic acid crystals (Step 4) indicated the reduction of Pt(IV) to Pt(II) and the formation of [Pt(NH3)4][PtCl4] (‘Magnus’ green salt’) a process formally captured by Equation (iii) (36):

2[Pt(NH3)6]4+ + 8Cl + 2C6H8O6 → [Pt(NH3)4][PtCl4] + 2C6H6O6 + 4NH4Cl + 4NH3 (iii)

The green precipitate consists of alternately stacked square planar [PtCl4]2− cations and [Pt(NH3)4]2+ anions, its formal structure usually being given in a simplified manner as PtCl2(NH3)2. At a higher temperature (68°C), the excess ascorbic acid slowly but quantitatively reduces the Pt2+ species to Pt0 as suggested by the gradual change of the dispersion colour from green to grey-black. This process is formally captured by Equation (iv):

PtCl2(NH3)2 + C6H8O6 → Pt0 + C6H6O6 + 2NH4Cl (iv)

The electron microscopy evaluations of the isolated solids revealed that well dispersed and quite uniform spherical Pt particles were obtained in all experiments (Figure 2). The median size of the particles was influenced by both the nature and the amount of dispersing agent used. The average size of the particles decreased from ~550 nm to ~220 nm when the level of gum arabic was increased from 10 wt% to 20 wt% (Figures 2(a) and 2(b)). This outcome is expected as an increased amount of dispersant favours the formation of a larger number of aggregation centres and reduces the number of constituent nanocrystals captured by each aggregate (38). In the case of sodium alginate, when an even lower amount of polymer was used due to a high viscosity of the starting solution, the average particle size increased to ~800 nm (Figure 2(c)).

Fig. 2.

Field emission electron micrographs of platinum spherical particles obtained in the presence of: (a) 10% gum arabic; (b) 20% gum arabic; and (c) 3% sodium alginate

Field emission electron micrographs of platinum spherical particles obtained in the presence of: (a) 10% gum arabic; (b) 20% gum arabic; and (c) 3% sodium alginate


The X-ray diffractograms of the three samples were essentially indistinguishable. For illustration, the pattern obtained for the particles obtained in the presence of 10% gum arabic is given in Figure 3(a). The unusually broad peaks for such large particles provided the first indication that the metal spheres may be assemblies of much smaller Pt entities. Indeed, the calculations based on Scherrer's equation (36) gave a value of ~6 nm for the size of the Pt crystallites. Additional inspection of the particles at high magnification (Figure 3(b)) confirmed both the aggregated nature of the Pt spheres and the calculated size of the constituent crystallites.

Fig. 3.

(a) XRD pattern and (b) high magnification FESEM images of platinum particles in Sample S1

(a) XRD pattern and (b) high magnification FESEM images of platinum particles in Sample S1


Considering the extensive internal grain boundary formed during the aggregation of a very large number of such small entities, it is expected that a significant amount of polymeric dispersant is trapped inside the large spheres. TGA analysis was used to determine not only the total residual amount of organic matter incorporated in the final dry powder but also the dynamics of its decomposition as a function of temperature. The decomposition pattern shown in Figure 4 for gum arabic was typical for both dispersants but the total weight loss recorded at 450°C varied with the type and amount of polymer used. In the case of gum arabic, it increased from ~2.3% to ~3.4% when the polymer amount was doubled from 10% to 20% (Table I, Samples S1 and S2). The increase in the residual organic matter in the latter case is likely the result of a larger external surface area associated with spheres of smaller diameter. Although the particle diameter was comparable to that recorded in Sample S1, in the case of sodium alginate the weight loss was larger (~2.9 %). Since the internal grain boundary and external surface area in both cases should be roughly similar (comparable size of both crystallites and spheres), the reason for the difference was likely the higher molecular weight of sodium alginate.

Fig. 4.

TGA data for the platinum spheres in Sample S1

TGA data for the platinum spheres in Sample S1


Heat Treatment of Platinum Nanoparticles

It is well known that the sintering temperature of nanoparticles is significantly lower than that of much larger entities of the respective materials (39, 40). Since the large precipitated particles contain nanosubunits, finding a temperature where their sintering is confined inside each sphere without intersphere mass transport (and thus powder sintering) taking place could be a viable way to increase particle crystallinity without irreversible particle aggregation. Also, as the sintering temperature of Pt is well above the decomposition point of most organic polymers, another advantage of such treatment would be a significant reduction of the amount of dispersant trapped in the internal grain boundary. In order to find a temperature at which the ‘intraparticle’ and ‘interparticle’ sintering are separated, four aliquots of Sample S1 were kept for 1 hour in an inert atmosphere at 200°C, 300°C, 400°C and 500°C, respectively. XRD analysis revealed a significant increase in the crystallinity of the Pt particles with temperature, as judged both by the width of the diffraction peaks (Figure 5(a)) and the increase in the calculated crystallite size (Figure 5(b) and Table II).

Fig. 5.

(a) XRD pattern and (b) calculated crystallite size of platinum spheres as precipitated and treated at different temperatures for 1 hour

(a) XRD pattern and (b) calculated crystallite size of platinum spheres as precipitated and treated at different temperatures for 1 hour


Table II

The Variation of Platinum Crystallite Size with Temperature

Temperature, °C100200300400500
Crystallite size (111), nm 6.0 ± 0.7 8.0 ± 0.8 9.5 ± 0.9 12.0 ± 1.2 24.0 ± 2.5

As indicated by the TGA data in Figure 6, the increase in crystallinity was also associated with a significant reduction in the amount of residual organic matter (from ~2.3% to ~0.2%).

Fig. 6.

TGA plots for precipitated and heat treated platinum powders

TGA plots for precipitated and heat treated platinum powders


Compared to the image of the original precipitated particles shown in Figure 3(b), the scanning electron microscopy (SEM) of the heat treated powders (Figures 7(a) and 7(b)) showed a much smoother surface, a clear indication of a significant reduction in the internal grain boundary. It is noteworthy that the exposure to elevated temperature for a relatively long time also causes the merging/sintering to a certain extent of the surface crystallites resulting in the loss of their original morphology. The analysis of multiple micrographs also showed that no interparticle ‘bridging’ took place at temperatures of 400°C or below. In contrast, at 500°C severe interparticle fusion was observed (Figure 7(c)).

Fig. 7.

(a) and (b) FESEM of platinum spheres kept at 400°C at two magnifications; (c) FESEM of platinum spheres heat treated at 500°C for 1 hour

(a) and (b) FESEM of platinum spheres kept at 400°C at two magnifications; (c) FESEM of platinum spheres heat treated at 500°C for 1 hour


These findings suggest two sintering regimes of spherical composite particles taking place at different size scales. At temperatures below 400°C, ‘intraparticle’ coarsening occurs as a result of the growth of constituent subunits and the reduction of internal grain boundaries. At 500°C, interparticle mass transport becomes significant and results not only in the growth of the constituent Pt crystallites, but also severe aggregation of the large Pt spheres. Since the latter cannot be redispersed to form electronic inks capable of depositing smooth and continuous thin Pt films, the optimum temperature at which powders suitable for electronic applications (crystalline and non-aggregated) can be prepared is ~400°C.


This study describes a precipitation method for obtaining concentrated dispersions of uniform polycrystalline Pt spheres. By tailoring the reaction conditions it is possible to control the final particle size in the 200 nm to 800 nm range. A heat treatment process capable of increasing the crystallinity of the precipitated spheres and decreasing the content of residual dispersant is also reported. The combination of the two processes makes possible the preparation of reasonably crystalline, uniform and well dispersed Pt spheres, which are suitable for thick film electronic applications. The use of widely available Pt salt, common reagents, and the simple experimental setup makes the reported preparation route suitable for the manufacturing of spherical Pt powders on a large scale.


This research was supported in part by a grant from DuPont Electronics Materials, Research Triangle Park, North Carolina, USA.



  1.  A. Henglein, B. G. Ershov and M. Malow, J. Phys. Chem., 1995, 99, (38), 14129 LINK
  2.  A. Roucoux, J. Schulz and H. Patin, Chem. Rev., 2002, 102, (10), 3757 LINK
  3.  R. R. Adžić and N. M. Marković, Electrochim. Acta, 1985, 30, (11), 1473 LINK
  4.  A. Eichler, F. Mittendorfer and J. Hafner, Phys. Rev. B, 2000, 62, (7), 4744 LINK
  5.  E. Matijević and D. Goia, Croat. Chem. Acta, 2007, 80, (3–4), 485 LINK
  6.  I. V. Sevonkaev, ‘Size and Shape of Uniform Particles Precipitated in Homogeneous Solutions’, PhD Thesis, Clarkson University, USA, 2009 LINK
  7.  I. V. Sevonkaev and V. Privman, World J. Eng., 2009, 6, P909
  8.  Q.-S. Chen, Z.-Y. Zhou, F. J. Vidal-Iglesias, J. Solla-Gullón, J. M. Feliu and S.-G. Sun, J. Am. Chem. Soc., 2011, 133, (33), 12930 LINK
  9.  I. Halaciuga, S. LaPlante and D. V. Goia, J. Mater. Res., 2009, 24, (10), 3237 LINK
  10.  R. K. Roy, J. I. Njagi, B. Farrell, I. Halaciuga, M. Lopez and D. V. Goia, J. Colloid Interface Sci., 2012, 369, (1), 91 LINK
  11.  Y. (J.). Yamashita, Y. Hosono and K. Itsumi, Jpn. J. Appl. Phys., Part 1, 2006, 45, (5B), 4684 LINK
  12.  H. A. Gasteiger, S. S. Kocha, B. Sompalli and F. T. Wagner, Appl. Catal. B: Environ., 2005, 56, (1–2), 9 LINK
  13.  D. van der Vliet, C. Wang, M. Debe, R. Atanasoski, N. M. Markovic and V. R. Stamenkovic, Electrochim. Acta, 2011, 56, (24), 8695 LINK
  14.  T.-H. Tran and T.-D. Nguyen, Colloids Surf. B: Biointerfaces, 2011, 88, (1), 1 LINK
  15.  Y. Yamauchi and K. Kuroda, Chem. Asian J., 2008, 3, (4), 664 LINK
  16.  I. Halaciuga, S. LaPlante and D. V. Goia, J. Colloid Interface Sci., 2011, 354, (2), 620 LINK
  17.  A. S. Hussein, P. Murugaraj, C. Rix and D. Mainwaring, ‘Mechanism of Formation and Stabilization of Platinum Nanoparticles in Aqueous Solvents’, Smart Materials II, Melbourne, Australia, 16th–17th December, 2002, “Proceedings of SPIE”, eds. A. R. Wilson and V. V. Varadan, 2002, Volume 4934, pp. 70–77 LINK
  18.  N. Varghese and C. N. R. Rao, J. Colloid Interface Sci., 2012, 365, (1), 117 LINK
  19.  D.-H. Chen, J.-J. Yeh and T.-C. Huang, J. Colloid Interface Sci., 1999, 215, (1), 159 LINK
  20.  H. Borsook and G. Keighley, PNAS, 1933, 19, (9), 875 LINK
  21.  D. R. Nieto, F. Santese, R. Toth, P. Posocco, S. Pricl and M. Fermeglia, ACS Appl. Mater. Interfaces, 2012, 4, (6), 2855 LINK
  22.  H. Ataee-Esfahani, L. Wang, Y. Nemoto and Y. Yamauchi, Chem. Mater., 2010, 22, (23), 6310 LINK
  23.  L. Wang and Y. Yamauchi, J. Am. Chem. Soc., 2010, 132, (39), 13636 LINK
  24.  L. Wang, Y. Nemoto and Y. Yamauchi, J. Am. Chem. Soc., 2011, 133, (25), 9674 LINK
  25.  L. Wang and Y. Yamauchi, Chem. Asian J., 2010, 5, (12), 2493 LINK
  26.  Y. Song, Y. Yang, C. J. Medforth, E. Pereira, A. K. Singh, H. Xu, Y. Jiang, C. J. Brinker, F. van Swol and J. A. Shelnutt, J. Am. Chem. Soc., 2004, 126, (2), 635 LINK
  27.  J. Yin, J. Wang, Y. Zhang, H. Li, Y. Song, C. Jin, T. Lu and T. Zhang, Chem. Commun., 2011, 47, (43), 11966 LINK
  28.  V. Komanicky and W. R. Fawcett, Electrochim. Acta, 2004, 49, (8), 1185 LINK
  29.  R. Komatsu and S. Uda, Mater. Res. Bull., 1998, 33, (3), 433 LINK
  30.  O. Weinstein and W. Miller, J. Cryst. Growth, 2010, 312, (7), 989 LINK
  31.  J. Billingham, P. S. Bell and M. H. Lewis, J. Cryst. Growth, 1972, 13–14, 693 LINK
  32.  J. Clavilier, R. Faure, G. Guinet and R. Durand, J. Electroanal. Chem. Interfacial Electrochem., 1979, 107, (1), 205 LINK
  33.  H. J. Scheel, J. Cryst. Growth, 2000, 211, (1–4), 1 LINK
  34.  D. T. Robb, I. Halaciuga, V. Privman and D. V. Goia, J. Chem. Phys., 2008, 129, (18), 184705 LINK
  35.   ImageJ, Image Processing and Analysis in Java, W. S. Rasband, US National Institutes of Health, Bethesda, Maryland, USA, 1997–2001: (Accessed on 12th April 2013)
  36.  R. Zsigmondy and P. Scherrer, “Kolloidchemie: Ein Lehrbuch”, 3rd Edn., Leipzig, Germany, 1920
  37.  N. N. Greenwood and A. Earnshaw, “Chemistry of the Elements”, 2nd Edn., Butterworth-Heinemann, Burlington, Massachusetts, USA, 1997
  38.  J. Park and V. Privman, Recent Res. Dev. Stat. Phys., 2000, 1, 1 LINK
  39.  J.-T. Wu and S. L.-C. Hsu, J. Nanopart. Res., 2011, 13, (9), 3877 LINK
  40.  Y. Jianfeng, Z. Guisheng, H. Anming and Y. N. Zhou, J. Mater. Chem., 2011, 21, (40), 15981 LINK

Further Reading

M. K. Carpenter and I. C. Halalay, GM Global Technology, Inc, ‘Platinum Particles with Varying Morphology’, US Patent 7,381,240; 2008

K.-A. Starz, D. V. Goia, J. Köhler and V. Bänisch, OMG AG & Co, KG, ‘Noble Metal Nanoparticles, a Process for Preparing These and Their Use’, European Appl. 1,175,948; 2002

H. Tsuji, Yokohama Town Service Co, Ltd, ‘Method for Producing Platinum Colloid, and Platinum Colloid Produced by the Same’, US Patent 6,455,594; 2002

K. Miyashita, R. Ogawa and M. Kezuka, ‘Metallic Colloid Particles and Process for Producing Same’, US Appl. 2005/0,186,129

The Authors

Brendan Farrell is a Research and Development Project Leader with Metalor Technologies, USA. He completed his PhD in Physical Chemistry at Clarkson University, Potsdam, New York, USA, under the direction of Professor Dan V. Goia.

Igor Sevonkaev has a PhD in Physics and currently holds a Research Associate position in the Department of Chemistry & Biomolecular Science at Clarkson University, Potsdam. He is primarily involved in industrial projects focused on design and preparation of materials for fuel cell and photovoltaic applications. His expertise is in the development of metallic (gold, silver, platinum, palladium and iridium) and non-metallic (lead(II) sulfide and magnesium fluoride) particles of various sizes and shapes for practical applications.

Dan V. Goia is a Professor in the Department of Chemistry & Biomolecular Science/Center for Advanced Materials Processing (CAMP) at Clarkson University, Potsdam. Prior to joining Clarkson in 2001 he was the Research and Development Director in the Electronic Materials Division of Degussa Corporation. His research focuses on the synthesis, characterisation, and modification of fine metallic particles.

Read more from this issue »