Skip to main content

Composition tunable cobalt–nickel and cobalt–iron alloy nanoparticles below 10 nm synthesized using acetonated cobalt carbonyl


A general organometallic route has been developed to synthesize Co x Ni1−x and Co x Fe1−x alloy nanoparticles with a fully tunable composition and a size of 4–10 nm with high yield. In contrast to previously reported synthesis methods using dicobalt octacarbonyl (Co2(CO)8), here the cobalt–cobalt bond in the carbonyl complex is first broken with anhydrous acetone. The acetonated compound, in the presence of iron carbonyl or nickel acetylacetonate, is necessary to obtain small composition tunable alloys. This new route and insights will provide guidelines for the wet-chemical synthesis of yet unmade bimetallic alloy nanoparticles.


Two-component alloy nanoparticles based on Fe, Co, and Ni are of great interest in the catalysis of, for example, the Fischer–Tropsch synthesis or the decomposition of cellulose (Cabet et al. 1998; Zhao et al. 2011; Jia and Schuth 2011). More than the single metals, bimetallic mixtures make it possible to tune carbon deposition and carbide formation rates, which are crucial for catalytic activity and lifetime (Cnossen et al. 1994; Pinheiro and Gadelle 2001) or the adsorbate bond dissociation energies as a function of the metal d-band center as described by the Newns–Anderson model (Nilsson et al. 2008). With bimetallic nanoparticles, catalytic performance is often also enhanced by their superior sintering resistance (Alloyeau et al. 2010; Cao and Veser 2010). Furthermore, an advantage over, for example, Pt, Pd, or Rh is that 3d transition metals are abundant and low priced, and can be used to replace expensive noble metals in catalytic processes (Nørskov et al. 2011; Haynes and Lide 2012).

Ideally, bimetallic catalytic nanoparticles should be prepared with a tunable composition and as small as possible, <10 nm, to maximize their surface-to-volume ratio. Although the preparation of bimetallic nanoparticles has been widely researched (Hyeon 2003; Wang and Li 2011), no general approach has been reported to synthesize Co–Ni or Co–Fe particles <10 nm with a tunable composition. Larger Co x Fe1−x particles in the 10–20 nm range have been prepared by thermal decomposition of organometallic compounds in high-boiling organic solvents, for instance using iron pentacarbonyl (Fe(CO)5) and Co(η3-C8H13)(η4-C8H12) or Co(N(SiMe3)2)2 (Desvaux et al. 2005), or iron(III) and cobalt(II) acetylacetonate (Chaubey et al. 2007). Smaller particles of 5–8 nm were synthesized using bimetallic carbonyl clusters that contain both iron and cobalt, but with a fixed elemental composition of FeCo3 (Robinson et al. 2009). CoNi particles of 30-nm size with a fixed elemental composition were prepared in triethylene glycol with polyvinylpyrrolidone (Hu et al. 2008), and smaller particles were made through a bio-based approach in apoferritine cavities or supported in polymer films (Abes et al. 2003; Gálvez et al. 2010). Monodisperse 8-nm nanoparticles from cobalt and nickel acetate hydrates were also reported but only with a ratio of Co40Ni60 (Murray et al. 2001). Besides wet-chemical techniques, physical evaporation methods have been used to prepare Co–Fe nanoparticles, but this too did not lead to particles <10 nm with a tunable composition (Reetz et al. 1995; Li et al. 2001; Wang et al. 2003).

Here, we report a novel organometallic method to synthesize colloidal nanoparticles of Co–Ni and Co–Fe with a fully tunable composition and a size of 4–10 nm. Our method relies on a straightforward and inexpensive pre-treatment of dicobalt octacarbonyl in dry acetone before it is thermally decomposed together with iron carbonyl or nickel acetylacetonate. First, the importance of the acetonation step will be demonstrated. Second, the tunability of nanoparticle alloy composition will be examined. Finally, it will be shown how the crystal structure of Co–Ni and Co–Fe nanoparticles can be controlled through the choice and concentration of surfactant molecules present during synthesis.

Experimental section


Nickel(II) acetylacetonate (Ni(acac)2; 95 %), cobalt(III) acetylacetonate (Co(acac)3; 99.99 %), trioctylphosphine oxide (TOPO; 99 %), dioctyl ether (99 %), 1,2-dichlorobenzene (anhydrous, 99 %), 2-propanol (anhydrous, 99 %), and cyclohexane (anhydrous, 99.5 %) were purchased from Aldrich. Dicobalt octacarbonyl (Co2(CO)8; hexane stabilized, 95 %), iron pentacarbonyl (Fe(CO)5; 99.5 %), oleic acid (OA; 97 %), acetone (anhydrous, 99.8 %), and toluene (anhydrous, 99.99 %) were obtained from Acros. Benzene (≥99.5 %) was obtained from Fluka. All chemicals were used as received.

Co x Ni1−x nanoparticle synthesis

Co x Ni1−x particles were made by combining literature recipes for the preparation of pure Co or pure Ni nanoparticles and by adding an acetonation step (Murray et al. 2001; Bao et al. 2009). Pure Co nanoparticles were prepared using a Co:OA:TOPO molar ratio of 12.15:2.38:1 (Bao et al. 2009), whereas pure Ni nanoparticles were prepared using a molar ratio nickel(II) acetate tetrahydrate (Ni(CH3COO)2·4H2O) to OA to tributylphosphine to tributylamine of 4:2:1:8 (Murray et al. 2001). Based on this, the following interpolating formulas were used to calculate reactant amounts for a standard synthesis: [OA] = 0.196[Co] + 0.516[Ni] and [TOPO] = 0.0824[Co] + 0.217[Ni], where [i] is the molar concentration of i. First, Co2(CO)8 and Ni(acac)2 were left to dissolve for 30 min in 3 mL of anhydrous acetone in a nitrogen atmosphere glove box, under occasional stirring of the flask by hand. Next, OA and TOPO were simultaneously added to 12 mL dioctyl ether in an adapted round-bottom synthesis flask (see Fig. S1 in Online Resource 1) inside the glove box, and the solution was subsequently heated to 280 °C in a nitrogen Schlenk line outside the glove box. The metal precursor solution was then injected from airtight vials in the hot ligand-containing solvent. Mixtures were refluxed for 30 min, allowed to cool to room temperature, and transferred back to the glove box before further analysis. No amines were used, because we observed that amines destabilize ε-Co nanoparticles (they act as a hard Lewis base forming a strong Co–NH2R bond; see Fig. S2 in Online Resource 1). Synthesis series A1–A4 were made in which the Co-to-Ni metal and/or the metal-to-ligand ((Co + Ni)/(OA + TOPO)) ratios were systematically varied. Essentially, series A1 and A2 keep the amounts of surfactants constant and series A3 and A4 keep the amounts of organometallic precursors constant. Exact amounts of metal precursors and ligands used for all Co x Ni1−x syntheses are given in Table S1 in Online Resource 1. It was verified with duplo syntheses for all syntheses in the manuscript that the results are reproducible.

Co x Fe1−x nanoparticle synthesis

The same procedure as for the Co x Ni1−x nanoparticles was used, but with Ni(acac)2 replaced by Fe(CO)5 and with the following formulas to calculate the amounts of OA and TOPO: [OA] = 0.196[Co] + 0.75[Fe] and [TOPO] = 0.0823[Co] + 0[Fe]. This was based on literature Fe:OA ratios of 1:1 and 1:3 (Murray et al. 2001; Farrell et al. 2003), and the absence of TOPO in reported Fe nanoparticle syntheses (Farrell et al. 2003). Synthesis series A5–A7 aimed to study the Co x Fe1−x composition dependency on the organometallic precursors and organic ligands concentrations. Exact amounts of the chemicals used can be found in Table S2 in Online Resource 1.

Alternating gradient magnetometer (AGM) measurements

A volume of 4 μL of dioctyl ether nanoparticle dispersion was added to airtight glass vials inside the glove box. Magnetization curves were measured using a MicroMag 2900 AGM (Princeton Measurements Corporation). Volume-averaged magnetic dipole moments and magnetic size polydispersities were determined from the curves according to Chantrell et al. (1978). Saturation magnetization values were calculated by dividing the average dipole moment by the average particle volume from transmission electron microscopy.

Transmission electron microscopy (TEM) and energy dispersive X-ray spectroscopy (EDX)

Carbon-coated Formvar Cu-grids (Agar Scientific) were dipped in nanoparticle dispersions and imaged on a Tecnai 12 (FEI) operating at 120 kV, equipped with a SIS CCD camera Megaview II. ITEM software (Olympus) was used to measure size distributions based on at least 200 particles. A Tecnai 20 (FEI) microscope operated at 200 kV, equipped with a field emission gun, Gatan 694 camera, and EDAX spectrometer was used for EDX analysis. For this purpose, raw nanoparticle dispersions were submitted to three washing cycles using 2-propanol to destabilize and cyclohexane to redisperse the particles. At least five different micron-sized spots and up to 20 individual nanoparticles were analyzed in each batch to determine particle composition and to test its uniformity over the batch.

Ultraviolet–visible (UV/Vis) spectroscopy

The UV/Vis spectra in Fig. 1 and in Fig. S3c (in Online Resource 1) were acquired on a Perkin-Elmer 950 spectrometer, making use of quartz airtight cuvettes. Samples were loaded in the glove box. A Varian Cary 50 Conc spectrometer was used to acquire the remaining spectra in Online Resource 1. Samples measured on this machine were exposed to air while measuring. UV/Vis spectra of the raw syntheses can indicate the presence of 3d transition metal containing molecular species. They display (weak) absorption features in the UV/Vis regime because of discrete dd transitions. In contrast, nanoparticles containing hundreds to thousands of atoms are expected to form continuous d-bands like the bulk systems (Lau et al. 2008) that are typically 5-eV broad (Khanna et al. 1979). When the 3d-bands are partly filled, as in the case of Fe, Co, and Ni, this allows a myriad of optical transitions and continuous absorption in the UV/Vis regime (Johnson and Christy 1974). Hence, continuous absorption, without the presence of specific absorption peaks, is expected throughout the whole UV/Vis regime.

Fig. 1

UV/Vis absorption spectra of Co2(CO)8 in a dioctyl ether, before and after addition of 100-μL dry acetone, resulting in Co–Co bond breaking, and b in anhydrous acetone, before and after exposure to air

X-ray powder diffraction (XRD)

XRD diffraction patterns were acquired on a Bruker D8 Advance and a Bruker D2 Phaser diffractometer. Cobalt Kα1,2 X-ray tubes (λ = 1.790 Å) operating at 30 kV were used, with currents of 45 and 10 mA, respectively. Typically, data points were acquired between 40° < 2θ < 100° every 0.2° with 13 s step−1. XRD samples were prepared inside a glove box and enclosed in an airtight and X-ray transparent box to probe the non-oxidized as prepared metal nanoparticles.


First, UV/Vis spectroscopy will be used to demonstrate that Co2(CO)8 reacts with acetone. Next, it will be shown that the acetonation step has a strong effect on the cobalt alloy nanoparticle preparation. The tunability of Co x Ni1−x and Co x Fe1−x particle composition will then be addressed, before revealing the particle magnetic properties. Finally, it is shown how the crystal structure of the nanoparticles is affected by the choice and concentration of the organic ligand molecules present during synthesis. The results will be further interpreted in more general terms in the "Discussion" section.

Acetonation of cobalt carbonyl

Our alloy nanoparticle synthesis approach relies on the pre-treatment of Co2(CO)8 with dry acetone before it is thermally decomposed. In experiments using an analytical balance, mass loss was recorded on Co2(CO)8 dissolution in acetone, corresponding to 3.1 CO molecules per Co2(CO)8. The UV/Vis spectrum of Co2(CO)8 in dioctyl ether is shown in Fig. 1a before and after addition of 100 μL of dry acetone. The initial spectrum is identical to that of Co2(CO)8 in 2-methylpentane (Abrahamson et al. 1977); the peak at 350 nm is assigned to σ → σ* transitions of Co–Co derived molecular orbitals. On addition of 100 μL of dry acetone to the 2.5-mL dioctyl ether solution, a rapid decrease of the 350-nm peak intensity occurs, indicating that Co–Co bonds are broken. Figure 1b zooms in on the part of the spectrum >350 nm, for Co2(CO)8 dissolved directly in dry acetone. A stable species exhibiting two absorption features at 472 and 517 nm is observed, which is assigned to 4T1g → 4T1g(P) transitions in high-spin octahedrally coordinated Co2+ 3d 7 species (Bayliss and McRae 1954; Lever 1984). This is the species from which we start the nanoparticle alloy synthesis. It is different from the species formed when the solution is exposed to air or oxygen, which would exhibit features at 512 and 574 nm because of charge transfer transitions due to O2 adsorption on the octahedrally coordinated Co2+ cations (Semenov et al. 2002). No relevant solvent effects were observed for any of the other metal precursors used in this study (see Fig. S3 in Online Resource 1).

Beneficial effect of cobalt carbonyl acetonation on nanoparticle alloy synthesis

To dissolve the organometallic precursors prior to injection into hot dioctyl ether with OA and TOPO, the best solvent was acetone. Other precursor solvents like dioctyl ether or dichlorobenzene did not result in well-defined nanoparticles. TEM pictures of raw Co x Ni1−x synthesis products are shown in Fig. 2. With dioctyl ether as the precursor solvent, the product consisted of polydisperse nanoparticles and irregularly shaped nickel crystals (determined by EDX) up to hundreds of nanometers in diameter (Fig. 2a). With dichlorobenzene as the precursor solvent, nanoflakes were obtained (Fig. 2b), and a UV/Vis transition was found around 670 nm, indicating the presence of residual molecular transition metal species (Fig. S4 in Online Resource 1). With acetone as the precursor solvent, spherical Co x Ni1−x (Fig. 2c) and Co x Fe1−x (Fig. 2d) nanoparticles were obtained and no organometallic remnants of the precursors were detected by UV/Vis; the success of acetone is ascribed to the disproportionation of Co2(CO)8, presented in the previous section.

Fig. 2

TEM pictures of the Co–Ni synthesis products when anhydrous a dioctyl ether, b dichlorobenzene, or c acetone were used to dissolve the Co2(CO)8 and Ni(acac)2 before thermal decomposition in dioctyl ether. With acetone only 4–10 nm nanoparticles were obtained. d The a priori acetonation of Co2(CO)8 also yields small Co–Fe nanoparticles

Tunability of nanoparticle alloy composition

Tunability of Co x Ni1−x nanoparticle alloy composition was realized across the entire range from pure cobalt to pure nickel. This was done by systematic variation of the concentrations of the organometallic precursors and organic ligands. Figure 3 presents the average sizes and compositions as determined by TEM–EDX (additional data are provided in Table S1 and Fig. S5–6 in Online Resource 1). Figure 3a quantifies how the size and polydispersity of the nickel-rich particles decreases when the Co/Ni precursor ratio was varied at constant surfactant concentrations (series A1 and A2). Figure 3b shows the metal-to-metal ratio measured with EDX versus the metal-to-metal ratio used during nanoparticle synthesis. Cobalt-rich nanoparticles (X Co,prec > 65 %) contained more cobalt than expected from the reactant ratio, whereas nanoparticles with less cobalt contained even less than expected from the reactant ratio. Figure 3c, d shows the results for constant amounts of Co and Ni precursors and variable amounts of surfactants, all resulting in diameters from 4 to 10 nm (series A3 and A4). Figure 3d shows that for a Co/(Co + Ni) precursor ratio of 67 %, the same ratio ends up in the nanoalloys for all ligand ratios OA/(OA + TOPO) ≤ 70 %. On increasing the amount of OA further in series A3, the nanoparticles became increasingly nickel-rich, making more Co x Ni1−x compositions accessible. The corresponding UV/Vis spectra, at ligand ratios OA/(OA + TOPO) > 70 %, showed that the formation of these nickel-rich particles occurs at the expense of the formation of molecular species, likely cobalt-oleate (see Fig. S6c in Online Resource 1).

Fig. 3

a TEM Co x Ni1−x particle sizes and b EDX compositions versus the precursor Co/(Co + Ni) ratio in series A1 (black circles) and A2 (red squares). c, d Show similar curves for series A3 (green circles) and A4 (blue squares). Through series A3, the accessible particle composition could be extended to all cobalt–nickel ratios. The dotted lines in b and d are guides-to-the-eye corresponding to total metal precursor incorporation into the nanoparticles. (Color figure online)

Spherical Co x Fe1−x nanoparticles between 4 and 8.5 nm could be prepared in much the same way as the Co x Ni1−x particles (see Fig. 4a and Fig. S7–9 in Online Resource 1). The relative amounts of cobalt and iron precursors were found in approximately the same ratio inside the nanoparticles as shown in Fig. 4b, although the particles were slightly more cobalt-rich than expected. Figure. 4c, d shows that nanoparticles prepared with a Co/(Co + Fe) precursor ratio of 50 % (series A7) varied between 4 and 6 nm and that they all had an EDX-determined Co/(Co + Fe) ratio between 50 and 60 %. Changing the OA/(OA + TOPO) ratio did thus not significantly change the metal composition. Furthermore, no sharp UV/Vis absorption features were detected for the raw Co x Fe1−x syntheses, indicating almost complete precursor incorporation in the nanoparticles.

Fig. 4

a TEM Co x Fe1−x particle sizes and b EDX compositions versus the precursor Co/(Co + Fe) ratio in series A5 (black circles) and A6 (red squares). c, d Show similar curves for series A7 (blue squares). All cobalt–iron compositions for small Co x Fe1−x particles were accessible in series A6. The dotted lines in b and d are guides-to-the-eye corresponding to total metal precursor incorporation into the nanoparticles. (Color figure online)

Magnetization of the particles

The Co x Ni1−x and Co x Fe1−x nanoparticle dispersions behave as magnetic fluids, as shown in Fig. 5. The magnetic properties allow for size selective precipitation, and monodisperse Co x Ni1−x and Co x Fe1−x batches can be obtained as such (see, for example, Table S3 in Online Resource 1). Magnetization curves of multiple nanoparticle dispersions, containing ca. 1 v/v% particles in dioctyl ether, were acquired using an alternating gradient magnetometer. The average magnetic dipole moments, polydispersity in the magnetic diameter, and saturation magnetization values of 4 raw syntheses are listed in Table 1.

Fig. 5

Pictures of Co x Ni1−x (left) and Co x Fe1−x (right) dispersions in dioctyl ether when held against a 1.3 T magnet. Typical, normalized magnetization curves of Co x Ni1−x (black, x = 0.66) and Co x Fe1−x (red, x = 0.53) dispersions reveal a higher magnetic dipole moment for the Co x Ni1−x nanoparticles. (Color figure online)

Table 1 Magnetic properties of Co x Ni1−x and Co x Fe1−x alloy nanoparticles

Nanocrystalline structural phase analyses

Figure 6 shows powder X-ray diffractograms of the raw Co x Ni1−x synthesis products of series A1 and A2 acquired in an inert environment to prevent the nanoparticles from oxidizing. Note that the phases are assigned in combination with TEM–EDX-determined compositions on individual nanoparticles as described in the "Experimental section". These analyses showed that the elemental composition from one particle to another was uniform within ten atomic percent. In Fig. 6a, a transition in series A1 was observed from nickel hexagonal close-packed (hcp) patterns for almost pure Ni aggregates, to ε-Co patterns (Murray et al. 2001) for the Co0.96Ni0.04 nanoparticles. The transitions in the XRD patterns indicate a gradually changing average nanoparticle crystal structure and since no sharp peaks were observed, the presence of larger crystals next to the nanoparticles can be excluded. In combination with the EDX results, the Co x Ni1−x particles showing fcc peaks are assigned to a fcc CoNi phase.

Fig. 6

Powder X-ray diffractograms of raw Co x Ni1−x nanoparticles, acquired in a nitrogen gas atmosphere, as made in synthesis series a A1 and b A2. The crystal phase assignments are based on the combination with the EDX results

Figure 6b displays a gradual change in nanoparticle crystal structure for series A2, going from fcc Ni, through hcp Ni and fcc CoNi to fcc Co. Pure nickel aggregated nanomaterials exhibited an fcc crystal structure, in contrast to almost Ni pure aggregates in series A1. For the pure cobalt nanoparticles, fcc Co was now observed in contrast to the less dense ε-Co structure for the Co0.96Ni0.04 nanoparticles in series A1. For both synthesis series A3 and A4, mainly fcc CoNi diffractograms were observed as shown in Fig. S7 (in Online Resource 1). Adding more OA (series A3), or changing the relative OA:TOPO ratios with fixed OA + TOPO amounts (series A4), did not result in crystal structure changes. Figure S9 (in Online Resource 1) shows the XRD patterns of the Co x Fe1−x nanoparticles. All materials exhibit a fcc crystal structure, but the noise in the patterns reveals that the particles were amorphous, while the crystallinity increased for Co/(Co + Fe) ratios ≥ 90 %. The Co x Fe1−x nanoparticle phase behavior was found to be much less complex, and less dependent on the ligands used, than that for the Co x Ni1−x nanoparticles.


In the following, the presented results are systematically dealt with before ending with two general discussions. The requirements for preparing transition bimetal particles are examined in terms of the strengths of the interactions between metal atoms and organic ligands. Finally, it is addressed why these nanoparticles are suitable model systems in the search for non-noble metal based catalysts.

Acetonation step

Hieber and Sedlmeier (1954) showed that dicobalt octacarbonyl can undergo a disproportionation reaction with Lewis bases. Typically, pyridine is found to be a base for the disproportionation of metal-carbonyls through the coordination of the nitrogen lone pair electrons. Spectrochemical series show that acetone acts as an intermediately strong Lewis base (Hieber and Sedlmeier 1954; Richmond et al. 1984). In analogy of mechanistic disproportionation studies (Hieber and Sedlmeier 1954; Sisak and Markó 1987), we propose that dicobalt octacarbonyl undergoes the following disproportionation reaction in acetone:

$$ 3Co_{2} \left( {CO} \right)_{8} + 12\left( {CH_{3} } \right)_{2} CO \to 2\left[ {Co^{2 + } \left( {\left( {CH_{3} } \right)_{2} CO} \right)_{6} } \right]\left[ {Co^{ - } \left( {CO} \right)_{4} } \right]_{2} + 8CO $$

On Co2(CO)8 dissolution in acetone, a mass loss occurred that corresponds to 3.1 CO molecules per Co2(CO)8. This is in fair agreement with the expected value of 2.7 on the basis of the proposed reaction equation. It is also supported by UV/Vis spectroscopy as shown in Fig. 1. After Co2(CO)8 acetonation, absorption due to octahedrally coordinated Co2+ was observed, whereas the tetracarbonyl cobaltate anions are thought to be tetrahedrally coordinated (Bühl et al. 2006) and non-absorbing in the UV/Vis regime (Semenov et al. 2002).

Scheme to synthesize cobalt alloy nanoparticles

The cobalt carbonyl acetonation product reacted with Fe(CO)5 and nickel(II) acetylacetonate to 4–10 nm spherical Co x Ni1−x and Co x Fe1−x nanoparticles with a high yield, while the use of intact Co2(CO)8 did not. This was shown in Fig. 2. On this basis, successful preparation of Co x Ni1−x and Co x Fe1−x nanoparticles is proposed to occur according to Scheme 1.

Scheme 1

Synthesis scheme of the Co x Ni1−x and Co x Fe1−x alloy nanoparticles

Although we observe that synthesis using the proposed [Co2+((CH3)2CO)6][Co(CO)4]2 complex results in better alloy nanoparticles than when Co2(CO)8 is used, it remains to be revealed what the origin of this effect is. Molecular mechanistic studies of the formation of monometallic Co nanoparticles (Lagunas et al. 2006; Samia et al. 2006; de Silva et al. 2007) showed that Co2(CO)8 decomposition leads rapidly to larger Co4(CO)12 clusters and ligand-substituted analogs. On the basis of UV/Vis, we concluded that the Co–Co bonds are broken because of the acetone, which likely prevents the instantaneous formation of Co4(CO)12 intermediates. We propose that the lack of larger cobalt clusters facilitates the mixing of Co and Ni or Co and Fe atoms in alloy nanoparticles. Also, the presence of an overall neutral complex of ligated cations and carbonylate anions might favor the stabilization of mono-cobalt building blocks, for example, by a facilitated de-protonation of the oleic acid molecules in solution to form bonding oleate complexes. Such intermediates would have slower and similar reaction rates as the Fe(CO)5 or Ni(acac)2 precursors.

The failure to obtain uniform well-mixed Fe x Ni1−x nanoparticles underpins the importance of the proposed disproportionated cobalt complex in the synthesis. The studies of Hieber and others has shown that base-induced disproportionation reactions exist for vanadium (Richmond et al. 1984), manganese (Hieber et al. 1961), iron (Hieber and Kahlen 1958), and nickel (Hieber et al. 1932) carbonyls and further studies might exploit this for the synthesis of other families of alloy nanoparticles.

Structure, composition, and possibility of oxidation of the cobalt alloy nanoparticles

The TEM–EDX results for the Co x Ni1−x and Co x Fe1−x nanoparticles, as shown in Figs. 3 and 4, revealed that the obtained particles contain both metals and that the bulk-determined composition is the same in individual nanoparticles. The powder X-ray diffractograms in Fig. 6 featured only one crystallographic phase per synthesis. In combination with the TEM–EDX results, this indicates that small alloy nanoparticles with one (poly)crystalline phase per synthesis were obtained. Furthermore, because this is not a seeded growth synthesis, core–shell structures are not likely. To determine the atomic distribution within one bimetallic nanoparticle, more advanced characterization methods such as scanning transmission electron microscopy combined with electron energy loss spectroscopy would be needed (van Schooneveld et al. 2010; den Breejen et al. 2011). Nonetheless, series A1 and A2 hinted at important information on the surface composition of the nanoparticles. Small Co x Ni1−x alloy particles were only obtained when increasingly more cobalt was added. This increased the total metal-to-ligand ratio. In a monometallic synthesis, particles normally grow larger when increasing the metal-to-ligand ratio. Here, the opposite behavior is observed and it can be explained by ligand-induced metal segregation (Menning and Chen 2009). For cobalt–nickel alloys, the surface would consist of nickel atoms in vacuum (Menning and Chen 2009). However, for oxygen atoms, it has been predicted that the adsorbate–metal interactions drive cobalt atoms to the particle surface (Menning and Chen 2009). It is also known that cobalt has a higher affinity for oleic acid than nickel. We suggest that the particles were large in order to shield the nickel atoms behind the relatively little amount of cobalt atoms that were forming the surface with the oxygen-containing ligand functional groups. In this view, the particles became smaller on addition of more cobalt, because more cobalt could sit at the particle interface. For bimetallic nanoparticles, these results show that next to the metal-to-ligand ratio, the metal–ligand affinity plays an important role in controlling their size and shape. In this view, single-crystal phase alloy nanoparticles were prepared where the first outer layer consisted of cobalt atoms in case of the Co x Ni1−x nanoparticles.

Finally, it is noted that the examined particles are unlikely to be oxidized. They were prepared in a nitrogen atmosphere Schlenk line and stored in a nitrogen atmosphere glove box. The XRD and AGM measurements were done under exclusion from air. No oxidation-related peaks were observed in XRD, and the nanoparticle magnetic properties are indicative of the highly magnetic metals as compared with the somewhat less magnetic metal oxides. The inferior magnetic properties of the Co x Fe1−x with respect to the Co x Ni1−x particles might, however, be due to a slight degree of iron oxidation, undetectable by XRD. In case of oxidation, iron is likely oxidized first in Co x Fe1−x , while the oxidation of cobalt is expected to occur first in Co x Ni1−x nanoparticles as a result of their respective oxidation potentials (Haynes and Lide 2012).

Magnetic properties of the alloy nanoparticles

The saturation magnetization values for pure Fe, Co, and Ni solids at room temperature are 1,711, 1,424, and 485 kA m−1, respectively (Chikazumi 1964). In bulk alloys of iron, cobalt, and nickel, saturation magnetizations are found to be intermediate between their components (Crangle and Hallam 1963). For the bimetallic nanoparticles prepared here, the saturation magnetization values were of the same order of magnitude, indicating a good magnetic quality. They are at least as magnetic as magnetite or maghemite nanoparticles of the same size, because the latter are usually less magnetic than expected from the magnetization of about 450 kA m−1 for bulk magnetite or maghemite (Chikazumi 1964). The saturation magnetization values and average magnetic dipole moments of the Co x Fe1−x particles were, however, lower than those of the Co x Ni1−x particles. Possibly, a minor degree of iron oxidation resulted in loss of magnetization. Alternatively, it could be due to the lower degree of Co x Fe1−x crystallinity, since crystalline defects are known to have a detrimental effect on the magnetic properties of nanoparticles (Luigjes et al. 2011). Overall, it is important to note that the effective magnetic properties for alloy nanoparticles cannot be solely predicted on the basis of the bulk magnetic properties, but effects such as crystallinity and the ease and degree of metal oxidation should be taken into account. Here, an example is reported where Co x Ni1−x particles display superior magnetic properties to their Co x Fe1−x analogs, while the opposite is expected based on bulk properties alone.

Ligand tunability of the crystal structure

Figure 7 summarizes the phase behavior of the Co x Ni1−x and Co x Fe1−x alloys obtained at the synthesis temperature of 280 °C and indicates the stable phases of the bulk alloys for comparison (Baker 1992). The figure combines the determined crystalline phases in the nanoparticles (based on EDX and XRD as shown in Fig. 6) with the respective synthesis parameters. It must be noted that Fig. 7 is based on the here presented 40 syntheses and that the exact elemental fractions at which the transitions occur, or the discreteness with which the boundaries are drawn, are subject to an error of a few percent because of the limited amount of data points. However, while the crystalline phase behavior of bulk alloys is typically described as a function of temperature only, we summarized in Fig. 7 that the phase behavior of the Co x Ni1−x and Co x Fe1−x nanocrystalline alloys is a function of the type of ligands used, their mutual ratios, and their concentration ratios with respect to the metals. These are essential state variables, and additional ones compared with bulk systems, when describing the alloy nanoparticle phase behavior. It is striking, for example, that both ε-Co and fcc Co nanoparticles, having a less dense respectively a denser structure than hcp Co, can be obtained in the Co x Ni1−x synthesis series by varying the reactant concentrations. Figure 7 shows the first detailed description of the Co x Ni1−x and Co x Fe1−x phase behavior as a function of oleic acid and trioctylphosphine oxide ligands. To fully control bimetallic particle formation at the nanometer scale in general, it is recommended to study their syntheses in the systematic way as shown here.

Fig. 7

Summary of the phase behavior of Co x Ni1−x and Co x Fe1−x nanoparticles when synthesized at 280 °C following the described wet-chemical synthesis route. The phase behavior of bulk metal alloys (Baker 1992) is shown for comparison

General energetic considerations of preparing alloy nanoparticles

The previous discussion raises the question what the general requirements are with respect to the strength of the metal–metal, ligand–ligand, and metal–ligand interactions. In designing an alloy nanoparticle synthesis method, one can first consider metal–metal interactions. The bulk alloy phase diagrams indicated that Co/Ni and Co/Fe are miscible over a large range of elemental ratios at the synthesis temperature of 280 °C (Baker 1992). Furthermore, the enthalpies of formation were favorable. For Co x Fe1−x bulk systems, experimental and calculated enthalpies of formation for ordered or interstitial alloys were reported to be respectively −10 to −1 kJ mol−1 and −22 to −1 kJ mol−1 for all x (de Boer et al. 1989). For Co x Ni1−x bulk systems, these were found to be respectively 0 and −13 to +3 kJ mol−1 for all x (de Boer et al. 1989).

Secondly, the metal–ligand interactions should be considered. In the synthesis of nanoparticles, extensive use is made of a few ligands that include phosphines (R3P), phosphites (R3PO), acids (RCOOH), alcohols (ROH), amines (RNH2), and thiols (RSH) (Donega 2011). An assumption in this study was that particle stability would be favored if the average dissociation energies for M x –M y  ~ M x –M x  ~ M y –M y  ≥ M x/y –La, and M x/y –Lb. Although solvation and surface energy arguments are neglected here, the idea of the requirement is that metal atoms would be prone to leaching from the nanoparticle surface by strongly binding ligands. Literature values of dissociation energies of cationic species Fe+–Fe and Co+–Fe are ca. 260 kJ mol−1 (Haynes and Lide 2012), between M+–S with M = Fe, Co, Ni they are 250–260 kJ mol−1 (Marks 1990), and between M+–NH2 they are 232–235 kJ mol−1 for Ni, 247–260 kJ mol−1 for Co and 280 kJ mol−1 for Fe (Marks 1990; Haynes and Lide 2012). Based on this, it was decided not to use thiols or amines in the synthesis of Co x Ni1−x and Co x Fe1−x nanoparticles. Although amines are usually applied in nickel nanoparticle synthesis, we verified by ligand-exchange tests on pure ε-Co nanoparticles, prepared by the Puntes method (Puntes et al. 2001), that these aggregated and even dissolved on post-synthesis addition of dodecylamine and 1-dodecanethiol, respectively (see Fig. S2 in Online Resource 1). Kitaev (2008) also noted the (partial) dissolution of cobalt nanoparticles on thiol addition. Instead, OA and TOPO molecules that both act as soft Lewis bases on the hard Lewis acid transition metals were chosen for their mild binding energies with cobalt and iron.

The third consideration concerns the dilemma between bond strength and amount of ligands used in the bimetal nanoparticle synthesis. Ligands, here OA and TOPO, which are just right to form cobalt and iron nanoparticles cannot prevent nickel from aggregating when used in equally low concentrations. On the other hand, ligands, such as the amines that bind strongly with nickel, dissolve the cobalt and iron into molecular complexes. The preparation of composition tunable transition metal nanoparticles, from metals with seemingly incompatible ligand affinity, can be realized by the use of one of the ligands at higher concentrations, at the expense of product yield. For example, the low binding strength of OA and TOPO initially prevented the formation of Co x Ni1−x particles with low cobalt content in series A1 and A2, but by adding more ligands, such particles were obtained in series A3, albeit together with cobalt molecular complexes and thus incomplete conversion.

Model systems for non-noble metal based catalysis

Solution prepared nanoparticles are capped with ligands to prevent them from aggregation. These ligands might seriously lower their activity in a catalytic reaction that occurs at the particle surface. In this respect, it is more useful to prepare nanoparticles on a support material through classic preparation routes used in heterogeneous catalysis. The advantage of using colloidal nanoparticles is, however, that the size and composition of all particles is readily controlled, as, for example, shown in this study. These particles, when coated with different ligands and consisting of different metal atoms, are then suitable model systems to study the interactions of alloys with the chemical intermediates of catalyzed reactions. Especially, the Newns–Anderson model predicts the adsorbate bond dissociation energies and adsorbate-induced metal segregation in bimetallic systems, as a function of the metal d-band center, providing a predictive framework for active non-noble metal catalysts (Nilsson et al. 2008; Menning and Chen 2009; Nørskov et al. 2011).


A generally applicable organometallic synthesis route, based on the reaction of Co2(CO)8 with acetone, is reported for the synthesis of 4–10 nm Co x Ni1−x and Co x Fe1−x nanoparticles with tunable elemental compositions. Based on the results of seven series of syntheses where the metal precursor concentrations and ligand type and concentrations were varied, insights intrinsic to the size, composition, and phase behavior of stable bimetallic alloy nanoparticles has been obtained. These basic insights will provide guidelines for the wet-chemical synthesis of yet unmade bimetallic alloy nanoparticles. We further envisage that the well-defined Co x Ni1−x and Co x Fe1−x nanoparticles are suitable prototypes to test the Newns–Anderson model as used in catalysis.


  1. Abes JI, Cohen RE, Ross CA (2003) Block-copolymer-templated synthesis of iron, iron–cobalt, and cobalt–nickel alloy nanoparticles. Mater Sci Eng C 23:641–650. doi:10.1016/j.msec.2003.08.001

    Article  Google Scholar 

  2. Abrahamson HB, Frazier CC, Ginley DS, Gray HB, Lilienthal J, Tyler DR, Wrighton MS (1977) Electronic spectra of dinuclear cobalt carbonyl complexes. Inorg Chem 16:1554–1556. doi:10.1021/ic50172a062

    Article  CAS  Google Scholar 

  3. Alloyeau D, Prevot G, Le Bouar Y, Oikawa T, Langlois C, Loiseau A, Ricolleau C (2010) Ostwald ripening in nanoalloys: when thermodynamics drives a size-dependent particle composition. Phys Rev Lett 105:255901. doi:10.1103/PhysRevLett.105.255901

    Article  CAS  Google Scholar 

  4. Baker H (1992) ASM handbook: alloy phase diagrams, Vol. 3. ASM International, Materials Park, Ohio

    Google Scholar 

  5. Bao Y, An W, Turner CH, Krishnan KM (2009) The critical role of surfactants in the growth of cobalt nanoparticles. Langmuir 26:478–483. doi:10.1021/la902120e

    Article  Google Scholar 

  6. Bayliss NS, McRae EG (1954) Solvent effects in the spectra of acetone, crotonaldehyde, nitromethane and nitrobenzene. J Phys Chem 58:1006–1011. doi:10.1021/j150521a018

    Article  CAS  Google Scholar 

  7. Bühl M, Grigoleit S, Kabrede H, Mauschick FT (2006) Simulation of 59Co NMR chemical shifts in aqueous solution. Chem–Eur J 12:477–488. doi:10.1002/chem.200500285

    Google Scholar 

  8. Cabet C, Roger AC, Kiennemann A, Läkamp S, Pourroy G (1998) Synthesis of new Fe–Co based metal/oxide composite materials: application to the Fischer–Tropsch synthesis. J Catal 173:64–73. doi:10.1006/jcat.1997.1885

    Article  CAS  Google Scholar 

  9. Cao A, Veser G (2010) Exceptional high-temperature stability through distillation-like self-stabilization in bimetallic nanoparticles. Nat Mater 9:75–81. doi:10.1038/nmat2584

    Article  CAS  Google Scholar 

  10. Chantrell R, Popplewell J, Charles S (1978) Measurements of particle size distribution parameters in ferrofluids. IEEE Trans Magn 14:975–977. doi:10.1109/TMAG.1978.1059918

    Article  Google Scholar 

  11. Chaubey GS, Barcena C, Poudyal N, Rong C, Gao J, Sun S, Liu JP (2007) Synthesis and stabilization of FeCo nanoparticles. J Am Chem Soc 129:7214–7215. doi:10.1021/ja0708969

    Article  CAS  Google Scholar 

  12. Chikazumi S (1964) Physics of magnetism. Wiley, New York

    Google Scholar 

  13. Cnossen RG, Lee S, Sacco A Jr (1994) Carbon deposition over transition metal alloys—I. Generation of 〈NiCo〉 〈FeNi〉 and 〈CoFe〉 phase diagrams. Carbon 32:1143–1150. doi:10.1016/0008-6223(94)90224-0

    Article  CAS  Google Scholar 

  14. Crangle J, Hallam GC (1963) The magnetization of face-centred cubic and body-centred cubic iron + nickel alloys. Proc R Soc Lond A Math Phys Sci 272:119–132. doi:10.1098/rspa.1963.0045

    Article  CAS  Google Scholar 

  15. de Boer FR, Boom R, Mattens WCM, Miedema AR, Niessen AK (1989) Cohesion in metals. Transition metal alloys, Vol 1. Cohesion and structure. Elsevier, Amsterdam

    Google Scholar 

  16. de Silva RM, Palshin V, Fronczek FR, Hormes J, Kumar CSSR (2007) Investigation of the influence of organometallic precursors on the formation of cobalt nanoparticles. J Phys Chem C 111:10320–10328. doi:10.1021/jp070499k

    Article  Google Scholar 

  17. den Breejen JP, Frey AM, Yang J, Holmen A, van Schooneveld MM, de Groot FMF, Stephan O, Bitter JH, de Jong KP (2011) A highly active and selective manganese oxide promoted cobalt-on-silica Fischer–Tropsch catalyst. Top Catal 54:768–777. doi:10.1007/s11244-011-9703-0

    Article  Google Scholar 

  18. Desvaux C, Amiens C, Fejes P, Renaud P, Respaud M, Lecante P, Snoeck E, Chaudret B (2005) Multimillimetre-large superlattices of air-stable iron–cobalt nanoparticles. Nat Mater 4:750–753. doi:10.1038/nmat1480

    Article  CAS  Google Scholar 

  19. Donega CdM (2011) Synthesis and properties of colloidal heteronanocrystals. Chem Soc Rev 40:1512–1546. doi:10.1039/C0CS00055H

    Article  CAS  Google Scholar 

  20. Farrell D, Majetich SA, Wilcoxon JP (2003) Preparation and characterization of monodisperse Fe nanoparticles. J Phys Chem B 107:11022–11030. doi:10.1021/jp0351831

    Article  CAS  Google Scholar 

  21. Gálvez N, Valero E, Ceolin M, Trasobares S, López-Haro M, Calvino JJ, Domínguez-Vera JM (2010) A bioinspired approach to the synthesis of bimetallic CoNi nanoparticles. Inorg Chem 49:1705–1711. doi:10.1021/ic902128g

    Article  Google Scholar 

  22. Haynes WM, Lide DR (2012) CRC handbook of chemistry and physics (internet edition). CRC, Boca Raton, FL

    Google Scholar 

  23. Hieber W, Kahlen N (1958) Reaktionen des Eisenpentacarbonyls mit verschiedenartigen N-Basen, II. Entstehung vorwiegend zweikerniger Carbonylferrate. Chem Ber 91:2234–2238. doi:10.1002/cber.19580911032

    Article  CAS  Google Scholar 

  24. Hieber W, Sedlmeier J (1954) Über Metallcarbonyle, LXII. Mitteil.): Über die Reaktion des Kobalt-tetracarbonyls mit verschiedenartigen Basen II). Chem Ber 87:25–34. doi:10.1002/cber.19540870105

    Article  Google Scholar 

  25. Hieber W, Mühlbauer F, Ehmann EA (1932) Derivate des Kobalt- und Nickelcarbonyls (XVI. Mitteil. über Metallcarbonyle). Ber Dtsch Chem Ges A&B 65:1090–1101. doi:10.1002/cber.19320650709

    Article  Google Scholar 

  26. Hieber W, Beck W, Zeitler G (1961) Neuere Anschauungen über Reaktionsweisen der Metallcarbonyle, insbesondere des Mangancarbonyls. Angew Chem 73:364–368. doi:10.1002/ange.19610731104

    Article  CAS  Google Scholar 

  27. Hu M-J, Lu Y, Zhang S, Guo S-R, Lin B, Zhang M, Yu S-H (2008) High yield synthesis of bracelet-like hydrophilic Ni–Co magnetic alloy flux-closure nanorings. J Am Chem Soc 130:11606–11607. doi:10.1021/ja804467g

    Article  CAS  Google Scholar 

  28. Hyeon T (2003) Chemical synthesis of magnetic nanoparticles. Chem Commun 8:927–934. doi:10.1039/B207789B

    Article  Google Scholar 

  29. Jia C-J, Schuth F (2011) Colloidal metal nanoparticles as a component of designed catalyst. Phys Chem Chem Phys 13:2457–2487. doi:10.1039/C0CP02680H

    Article  CAS  Google Scholar 

  30. Johnson PB, Christy RW (1974) Optical constants of transition metals: Ti, V, Cr, Mn, Fe, Co, Ni, and Pd. Phys Rev B Solid State 9:5056. doi:10.1103/PhysRevB.9.5056

    Article  CAS  Google Scholar 

  31. Khanna SN, Cyrot-L F, Desjonquères MC (1979) Density of electronic states in amorphous and liquid cobalt. J Phys F Met Phys 9:79–84. doi:10.1088/0305-4608/9/1/011

    Article  CAS  Google Scholar 

  32. Kitaev V (2008) Comment on effect of polar solvents on the optical properties of water-dispersible thiol-capped cobalt nanoparticles. Langmuir 24:7623–7624. doi:10.1021/la800641s

    Article  CAS  Google Scholar 

  33. Lagunas A, Jimeno C, Font D, Solà L, Pericàs MA (2006) Mechanistic studies on the conversion of dicobalt octacarbonyl into colloidal cobalt nanoparticles. Langmuir 22:3823–3829. doi:10.1021/la053016h

    Article  CAS  Google Scholar 

  34. Lau JT, Rittmann J, Zamudio-Bayer V, Vogel M, Hirsch K, Klar P, Lofink F, ller T, v Issendorff B (2008) Size dependence of L 2,3 branching ratio and 2p core-hole screening in X-ray absorption of metal clusters. Phys Rev Lett 101:153401. doi:10.1103/PhysRevLett.101.153401

    Article  CAS  Google Scholar 

  35. Lever ABP (1984) Inorganic electronic spectroscopy, Vol 33. Studies in physical and theoretical chemistry. Elsevier, Amsterdam

    Google Scholar 

  36. Li XG, Takahashi S, Watanabe K, Kikuchi Y, Koishi M (2001) Hybridization and characteristics of Fe and Fe–Co nanoparticles with polymer particles. Nano Lett 1:475–480. doi:10.1021/nl010007u

    Article  CAS  Google Scholar 

  37. Luigjes B, Woudenberg SMC, de Groot R, Meeldijk JD, Torres Galvis HM, de Jong KP, Philipse AP, Erné BH (2011) Diverging geometric and magnetic size distributions of iron oxide nanocrystals. J Phys Chem C 115:14598–14605. doi:10.1021/jp203373f

    Article  CAS  Google Scholar 

  38. Marks TJ (1990) Bonding energetics in organometallic compounds: ACS symposium series. ACS, Washingthon, DC

    Book  Google Scholar 

  39. Menning CA, Chen JG (2009) General trend for adsorbate-induced segregation of subsurface metal atoms in bimetallic surfaces. J Chem Phys 130:174709. doi:10.1063/1.3125926

    Article  Google Scholar 

  40. Murray CB, Sun S, Doyle H, Betley T (2001) Monodisperse 3d transition-metal (Co, Ni, Fe) nanoparticles and their assembly into nanoparticle superlattices. MRS Bull 26:985–991. doi:10.1557/mrs2001.254

    Article  CAS  Google Scholar 

  41. Nilsson A, Pettersson LGM, Nørskov JK (2008) Chemical bonding at surfaces and interfaces. Elsevier, Amsterdam

    Google Scholar 

  42. Nørskov JK, Abild-Pedersen F, Studt F, Bligaard T (2011) Density functional theory in surface chemistry and catalysis. Proc Natl Acad Sci USA 108:937–943. doi:10.1073/pnas.1006652108

    Article  Google Scholar 

  43. Pinheiro JP, Gadelle P (2001) Chemical state of a supported iron–cobalt catalyst during CO disproportionation: I. Thermodynamic study. J Phys Chem Solids 62:1015–1021. doi:10.1016/S0022-3697(00)00265-1

    Article  CAS  Google Scholar 

  44. Puntes VF, Krishnan KM, Alivisatos AP (2001) Colloidal nanocrystal shape and size control: the case of cobalt. Science 291:2115–2117. doi:10.1126/science.1058495

    Article  CAS  Google Scholar 

  45. Reetz MT, Helbig W, Quaiser SA (1995) Electrochemical preparation of nanostructural bimetallic clusters. Chem Mater 7:2227–2228. doi:10.1021/cm00060a004

    Article  CAS  Google Scholar 

  46. Richmond TG, Shi QZ, Trogler WC, Basolo F (1984) Kinetics and mechanism of Lewis-base-induced disproportionation of vanadium hexacarbonyl and its phosphine-substituted derivatives. J Am Chem Soc 106:76–80. doi:10.1021/ja00313a017

    Article  CAS  Google Scholar 

  47. Robinson I, Zacchini S, Tung LD, Maenosono S, Thanh NTK (2009) Synthesis and characterization of magnetic nanoalloys from bimetallic carbonyl clusters. Chem Mater 21:3021–3026. doi:10.1021/cm9008442

    Article  CAS  Google Scholar 

  48. Samia ACS, Schlueter JA, Jiang JS, Bader SD, Qin C-J, Lin X-M (2006) Effect of ligand–metal interactions on the growth of transition-metal and alloy nanoparticles. Chem Mater 18:5203–5212. doi:10.1021/cm0610579

    Article  CAS  Google Scholar 

  49. Semenov VV, Cherepennikova NF, Lopatin MA, Khorshev SY, Fominykh ZY, Kirillov AI, Sedel’nikova VN, Domrachev GA (2002) Formation of gels and films from hexamine- and hexamidecobalt(II) carbonylcobalt complexes. Russ J Gen Chem 72:657–666. doi:10.1023/a:1019588828253

    Article  CAS  Google Scholar 

  50. Sisak A, Markó L (1987) Mechanistic studies on the disproportionation of dicobald octacarbonyl with hard Lewis bases. J Organomet Chem 330:201–206. doi:10.1016/0022-328X(87)80288-7

    Article  CAS  Google Scholar 

  51. van Schooneveld MM, Gloter A, Stephan O, Zagonel LF, Koole R, Meijerink A, Mulder WJM, de Groot FMF (2010) Imaging and quantifying the morphology of an organic–inorganic nanoparticle at the sub-nanometre level. Nat Nanotechnol 5:538–544. doi:10.1038/nnano.2010.105

    Article  Google Scholar 

  52. Wang D, Li Y (2011) Bimetallic nanocrystals: liquid-phase synthesis and catalytic applications. Adv Mater 23:1044–1060. doi:10.1002/adma.201003695

    Article  CAS  Google Scholar 

  53. Wang ZH, Choi CJ, Kim JC, Kim BK, Zhang ZD (2003) Characterization of Fe–Co alloyed nanoparticles synthesized by chemical vapor condensation. Mater Lett 57:3560–3564

    Article  CAS  Google Scholar 

  54. Zhao M, Church TL, Harris AT (2011) SBA-15 supported Ni–Co bimetallic catalysts for enhanced hydrogen production during cellulose decomposition. Appl Catal B 101:522–530. doi:10.1016/j.apcatb.2010.10.024

    Article  CAS  Google Scholar 

Download references


MMvS and JvR thank the Netherlands Organization for Scientific Research (NWO-CW and NWO-FOM) for financial support. We thank C. de Mello Donegá and B. M. Weckhuysen for discussions.

Open Access

This article is distributed under the terms of the Creative Commons Attribution License which permits any use, distribution, and reproduction in any medium, provided the original author(s) and the source are credited.

Author information



Corresponding authors

Correspondence to Matti M. van Schooneveld or Frank M. F. de Groot.

Electronic supplementary material

Below is the link to the electronic supplementary material.

Supplementary Material 1 (1490 kb)

Rights and permissions

Open Access This article is distributed under the terms of the Creative Commons Attribution 2.0 International License (, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Reprints and Permissions

About this article

Cite this article

van Schooneveld, M.M., Campos-Cuerva, C., Pet, J. et al. Composition tunable cobalt–nickel and cobalt–iron alloy nanoparticles below 10 nm synthesized using acetonated cobalt carbonyl. J Nanopart Res 14, 991 (2012).

Download citation


  • Synthesis
  • Nanoparticles
  • Cobalt alloy
  • Carbonyl disproportionation
  • Acetone