Stephen D. Evans*, Simon R. Johnson, Yaling L. Cheng and Tiehan Shen
Department of Physics and Astronomy, University of Leeds, Leeds, UK LS2 9JT, s.d.evans@leeds.ac.uk
First published on UnassignedUnassigned22nd December 1999
Small aromatic organothiol derivatives, with the structure HS–C6H4–X, have been used to stabilise gold nanoparticles. The nature of the functional group, X, is important for controlling the relative strength of the particle–particle and particle–solvent interactions and hence in determining the physical properties of these systems (e.g. solubility). Particles were stabilised with different ligands for which X=OH, –COOH, –NH2, and –CH3 and thin films of the particles were formed, by solution evaporation, on microelectrode patterned surfaces. The electronic behaviour indicates that conduction can be understood in terms of an activated electron tunnelling model. Finally, preliminary studies were carried out on the effect of exposure to different chemical vapours on the electronic transport properties.
The principal advantage offered by organic materials is the promise for better chemical specificity (and lower power consumption). Early work in this area focused on the development of the highly conjugated phthalocyanine derivatives that showed high sensitivity (ppb) to small amounts of electron donating and accepting species.4 However, poor reproducibility of film formation, water sensitivity and slow response times have led to only limited application of these materials. The advent of conducting polymers (e.g. polypyrroles, polythiophenes) has in contrast led to the development of a number of commercial devices (Aromascan, Bloodhound, Neotronics, Alpha-MOS) based on olfactory mimics.5 These devices rely on processing of information obtained from a number of sensor elements, each of a slightly different chemical composition, which give differing responses to a given analyte. These systems appear to hold much promise but do suffer reproducibility problems due to the effects of water vapour and lack specificity.
In this paper we explore the feasibility of using organo-functionalised metallic nanoparticles for vapour sensing. Such hybrid systems combine organic and inorganic materials and offer a novel approach to vapour sensing. Our interest in these systems arises because of recent developments in the synthesis of surfactant stabilised metallic nanoparticles.6 Our synthetic route for the preparation of the nanoparticles is a modification of that reported by Brust et al. and subsequently Leff et al., and is based on the reduction of AuCl4− to Aun in the presence of an alkylthiol derivative.6,7 The role of the thiol is purportedly to provide a thermodynamic control over the size of nanoparticles, achieved by controlling the ratio of thiol to AuCl4− present at the start of the reduction.
The particle clusters produced are typically between 1.5 and 3 nm in diameter and contain between 103 and 832 Au atoms in the core and 33 to 132 alkylthiols in the ligand shell, respectively. The strong nature of the thiol–Au interaction allows one to modify the ω-functional group of alkylthiols or in our case the para-position of the phenyl ring (Fig. 1). Studies carried out to date have focused on using alkyl derivatives with –CH3 functional groups; this relatively inert moiety reduces particle–particle interaction and leads to the production of stabilised particles which do not aggregate (or agglomerate) and which are soluble in organic solvents. We have recently shown that one is not restricted to using such essentially passive stabilising layers, but that one can introduce different chemical groups, for example azobenzene units, which when taken in conjunction with the properties of the gold nanoparticles will provide materials with interesting new properties.8
Fig. 1 Schematic representation of two surfactant stabilised nanoparticles each of radius r, separated by a dielectric of relative permittivity εr and thickness δ (twice the ligand length). Four different functional ligands were used to stabilise the particles (I–IV). |
(1) |
The important points to be noted regarding eqn. (1) are:
i) Since β is typically of the order of 1 Å−1 the first term demonstrates that the conductivity is extremely sensitive to the separation of the metallic cores, giving nearly an order of magnitude decrease per Å increase in separation.
ii) The activation energy, Ec, is essentially the Coulomb energy associated with charging two neutral particles and is thus inversely proportional to the relative permittivity of the dielectric media separating the cores and the radius of the cores (with a small correction for the core–core separation).
It is apparent from eqn. (1) that any process that changes either the core–core separation or the permittivity of the medium between the cores will be readily detectable by following changes in the conductivity. In the study presented here we show that this effect can be utilised, using ligand-stabilised nanoparticles, for chemical vapour sensing. The stabilising ligands used here were chosen for two reasons: firstly, they are short and hence should give reasonable conductivities, and secondly, we have control over the nature of the functional group (Fig. 1).
Sample type IV was synthesised using a route described previously.11
Compounds I (HS–C6H4–OH), III (HS–C6H4–NH2), and IV (HS–C6H4–CH3) were obtained from Aldrich and compound II (HS–C6H4–COOH) from Toronto Research Chemicals.
The initial solutions from which the nanoparticles were formed contained gold∶sulfur ratios of 0.55∶1, 0.74∶1, 0.73∶1 and 0.85∶1 for samples I–IV respectively. The nanoparticles formed were soluble in a variety of solvents dependent on the nature of the functional group.
The composition of the nanoparticles was established using the Scienta ESCA 300 instrument at Daresbury Laboratories, Warrington, UK. A monochromated Al Kα X-ray source, at a power level of 2.8 kW, was used and C 1s, O 1s, Au 4f and S 2p levels were recorded, at an electron take-off angle of 90°. The base pressure in the sample chamber was <10−9 mbar. The analyser slit width and pass energy were 1.9 mm and 150 eV respectively and the system was calibrated with respect to the Ag 3d peak from a standard sample.
Fig. 2 Experimental set-up for measuring the electrical response of films upon exposure to analytes in a carrier gas. The flow meters were used to control the flow rate in each of the arms. |
Zero grade nitrogen (BOC) was used as a ‘carrier' gas and the flow was divided and sent through two arms of the apparatus. The flow rate in each arm was independently set, between 0.1–1.2 L min−1, using adjustable flow meters (RS supplies). In one arm the N2 was bubbled through the solvent under investigation. This arm contained a solenoid valve, which could be opened or closed to allow control of analyte flow to the sample compartment. All measurements were carried out at room temperature (22 ± 0.1°C) and the samples were allowed to equilibrate under an atmosphere of dry nitrogen for 900 s before any readings were taken. The d.c. sample response was obtained by measuring the current, at a fixed voltage, during an exposure–recovery cycle. The current measurement and control over the solenoid valves were performed using a computer-interfaced electrometer and an IEEE card.
The typical protocol followed for determining the response to the analytes was as follows: current readings were collected for 900 s, with ‘dry' nitrogen flowing (0.6 L min−1) through the sample chamber, to serve as a baseline. This was followed by a 600 s exposure to analyte, at a controlled flow rate. Following the cessation of analyte flow (by closing the solenoid valve) current readings were then taken for a further 900 s to monitor the recovery of the sample. During this time ‘dry' nitrogen was passed through the compartment.
Fig. 3 X-ray photoelectron spectra of the sulfur 2p region for samples I–IV. |
Abbreviated name | Functional group | Particle sizea/nm | σ/Ω−1 cm−1 | Activation energy (Ec)/kJ mol−1 |
---|---|---|---|---|
aMetal core diameter determined using transmission electron microscopy (TEM). | ||||
I | OH | 3.2 | 7.8 × 10−7 | 5.5 |
II | COOH | 2.9 | 2.5 × 10−6 | 6.7 |
III | NH2 | 6.0 | 7.8 × 10−2 | 2.6 |
IV | CH3 | 3.6 | 6.1 × 10−4 | 8.3 |
The current–voltage (I–V) characteristics were obtained for all films at room temperature and as a function of temperature between 100 and 250 K. All films displayed ohmic behaviour and the room temperature conductivities (Table 1) were found to vary between ∼10−6 and 10−2 Ω−1 cm−1. These values are between 7 and 11 orders of magnitude lower than the conductivity of bulk gold, 4 × 105 Ω−1 cm−1, and indicate that the stabilising ligands, surrounding the metallic cores, serve to insulate the cores. This is in contrast to the studies by Musick et al. who reported significant fusion of particles leading to the formation of percolating pathways and resulting in conductivities of the order of 103 Ω−1 cm−1.18 However, our results are in agreement with the work of Terrill et al. who, using long chain alkanethiols to stabilise their particles, found conductivities decreased from 10−5 to 10−9 Ω−1 cm−1 upon increasing the alkyl chain length of the stabilising ligand from eight to sixteen carbon units, C8 (HS(CH2)7CH3) and C16 (HS(CH2)15CH3), on 4 nm diameter particles.19 For sample IV, which is most comparable in size (3.6 nm) to Terrill's particles we expect the smaller thickness of our ligand (∼6 Å) to lead to a core separation of ∼12 Å compared to a core separation of ∼18 Å in their case. Using these values in eqn. (1) we would expect our sample IV to display a conductivity ∼2 orders of magnitude higher than theirs. From experiment we only find our systems to have a conductivity ca. one order of magnitude larger. This could arise for several reasons: a) our average core size is smaller, and b) it is possible that in the alkane systems one might have interpenetration between the alkane chains on neighbouring particles, thus leading to a reduced core–core separation.
Samples I and II gave similar conductivity values ∼10−6 Ω−1 cm−1 while the larger particles (III) gave rise to a much greater conductivity ∼10−2 Ω−1 cm−1 and particles of IV displayed conductivities between these extremes. This trend of increasing conductivity with increasing particle size is qualitatively as one would expect from eqn. (1), however the data are not sufficient to allow quantitative interpretation and ignore differences in the permittivity of the stabilising ligands.
Fig. 4 shows the variation of the conductivity as a function of temperature. All systems I–IV displayed a linear behaviour when plotted as ln σ vs. 1/T indicating that the classic model of activated tunnelling proposed by Neugebauer and Webb is applicable to these systems.
Fig. 4 Conductivity versus reciprocal temperature (Kelvin). Lines are fits to the data, the goodness of fit was better than 0.99 in all cases. |
The activation energies, Ec, obtained from the slopes in Fig. 4 are given in Table 1. For samples I, II and IV, which have similar particle sizes, the values of Ec range between 5.5 and 8.3 kJ mol−1. This is similar to the value of 9.5 kJ mol−1 reported by Terrill et al. for C8 stabilised particles. Sample III has an activation energy approximately a factor of two less than the other samples, this is as expected since Ec has a 1/r dependence.
Fig. 5 Response of samples I–IV upon exposure to methanol in N2 (91 ppth). |
Sample | τinitial/s | τrecovery/s |
---|---|---|
τ is the time taken to (rise or) decay to e−2 of its initial value. | ||
I | 73 | 29 |
II | 61 | 219 |
III | 20 | 110 |
IV | 27 | 31 |
Samples II and III displayed good repeatability; Fig. 6 shows the response to repeated exposure–recovery cycles for sample II.
Fig. 6 Response of sample II, in repeated exposure–recovery cycle, to methanol in N2 (91 ppth). |
Ellipsometric studies were carried out on two of these systems (II and IV) and the optical response monitored as a function of partial pressure of the analyte. Unfortunately these studies are problematic since the optical thickness is dependent on both the relative permittivity as well as the actual thickness, either of which may change during the experiment. Fig. 7 shows changes in the film thickness, calculated on the assumption that the relative permittivity of the films remains constant.20 It shows that the film thickness decreases for sample IV (CH3) and increases for sample II (COOH). Such changes are consistent with the changes observed in the conductivity, i.e. indicating that decreases in conductivity are associated with film swelling (increased particle separation) while increasing conductivity is associated with decreases in particle separation (or, alternatively with an increase in the relative permittivity of the film).
Fig. 7 Ellipsometric response of samples II and IV upon exposure to methanol, as a function of partial pressure (p/po). The changes in film thickness were estimated by assuming that the relative permittivity of the film (n = 2.63, k = 1.55) remained constant during exposure. |
Other polar analytes such as ethanol and propan-1-ol showed qualitatively similar behaviour to methanol.
Fig. 8 The magnitude of the response (I/Io), for particles I–IV, upon exposure to a range of analytes. |
Footnote |
† Originally prepared for a presentation at Materials Chemistry Discussion No. 2, 13–15 September 1999, University of Nottingham, UK. |
This journal is © The Royal Society of Chemistry 2000 |