Prem Jyoti Singh Rana,
Pallavi Singh and
Prasenjit Kar*
Department of Chemistry, Indian Institute of Technology, Roorkee, 247667, India. E-mail: kar.prasen@gmail.com; prkarfcy@iitr.ac.in
First published on 13th July 2016
The present study comprises a deeper comprehension on the applicability of environmentally benign water soluble fluorescent Carbon Nanoparticles (CNs) synthesised from jamun (Syzygium cumini). We have synthesised two types of CNs i.e., surface non-passivated and surface passivated. The morphological investigation of either type of CN shows a narrow particle size distribution with an average size of 40 nm and 42 nm respectively. These CNs show potential candidacy as cell imaging agents due to cell viability up to a high concentration of 30 μg mL−1 as revealed by cytotoxicity analysis. Furthermore, we employed hemoglobin as a target to explore the biosensing ability of CNs based on a turn ON–OFF mechanism. Moreover, we have made a reversible fluorescent turn ON–OFF–ON switch taking the CNs–Hb composite system in conjugation with a large excess H2O2. This unbelievable fluorescence enhancement of the CNs–Hb composite system on exposure to excessive H2O2 is due to a decrement in particle size that conversely increases the surface area to volume (S/V) ratio which in turn intensifies the PL spectra. Using the above intriguing changes, a nanoparticle based implication logic operation (IMP) was created with Hb and H2O2 as inputs.
Scheme 1 Synthesis of CNs from anthocyanin pigments of Syzygium cumini through a hydrothermal process. |
The Raman spectra of the CNs-A display two broad peaks at around 1386 cm−1 and 1605 cm−1, which are attributed to the D band (sp3-hybridized) and G band (sp2-hybridized) respectively. The D band is associated with vibrations of carbon atoms in the termination plane and related to sp3 defects while the G band corresponds to the vibration of sp2-hybridized carbon atoms. The ratio of the intensity of the disordered D band and crystalline G band ID/IG was 1.22, indicative of the nanocrystalline nature of CNs (Fig. 1b). This was further confirmed by TEM analysis. Elemental analysis revealed the composition of the CNs to be C 53.60 wt%, H 4.31 wt% and N 0.0 wt%, for CNs-A and C 56.22 wt%, H 4.77 wt% and N 2.18 wt% for CNs-B.
The UV-vis absorption spectra display a broad absorption band in the range of 200–600 nm for both the CNs-A and CNs-B. The CNs-A show relatively more prominent absorption bands located at 250 nm for the π–π* transition with a lower intensity absorption shoulder (compared to the π–π* transition) at around 288 nm for n–π* transition. The former π–π* transition is strongly coupled with surface electronic states. Compared to CNs-A, CNs-B involving surface passivation show a less featured absorption band at around 253 nm for the π–π* transition with an absorption shoulder located at 325 nm for the n–π* transition shown in Fig. 1c. It may be assumed that it was the surface amino-groups that passivate the traps on the surface of CNs-B and lead to a broad transition in the region of 290–350 nm with the shoulder at 325 nm (Fig. 1c). Moreover, the n–π* transition associated with surface passivated CNs exhibits a bathochromic shift by 37 nm relative to CNs-A. Unlike the n–π* transition, the π–π* transition is steady for both CNs-A and B. The absorption spectra of both the CNs-A and B portray high energy tailing in the visible region which was ascribed to Mie scattering caused by nanoparticles.24
Moreover, Fig. 1d and e shows the photoluminescence behavior of CNs-A and CNs-B respectively. The shift in emission peak positions with different excitation wavelengths arose not only from different sizes of CNs but also from different emissive sites on CNs.25 CNs-A exhibit excitation-wavelength-dependent photoluminescence (PL) properties with emission peaks ranging from 300 nm to 650 nm on excitation from 275 nm to 445 nm. The strongest fluorescence emission band located at 426 nm, was observed under 335 nm excitation. In CNs-A, there was a clear bathochromic shift with the increase of excitation wavelength, which explains multiple transition modes with different probabilities (Fig. 1d). However, CNs-B exhibit excitation-wavelength-independent photoluminescence properties with emission peaks ranging from 300 nm to 650 nm centered at 500 nm on excitation from 275 nm to 445 nm. The related fluorescence spectrum shows the presence of a single transition mode. Moreover, the emission peak of CNs-B was red shifted by a 74 nm contrast to the strongest intensity peak in CNs-A centered at 426 nm. On the basis of the above interpretation it is evident that the photoluminescence behavior is not centered on the core shell but is also due to surface functionality.
Fig. 1f shows the fluorescence decay of CNs-A and CNs-B in aqueous solution on excitation at 375 nm using the Time Correlated Single Photon Counting (TCSPC) technique. This shows tri-exponential and bi-exponential behavior with an average lifetime τ(average) of 10.23 ns and 20.53 ns for CNs-A and CNs-B respectively (Table 1). This measured lifetime is related to the radiative and non-radiative electron–hole recombination processes. The radiative rate, kr, is correlated to the fluorescence quantum yield, ϕ, as kr = ϕ/τ(average). The fluorescence radiative rate constant was calculated by taking an average lifetime of 10.23 ns and 20.53 ns for CNs-A and CNs-B respectively. It was found to be in the order of 105 s−1 and 106 s−1 for CNs-A and CNs-B respectively. It is noteworthy that kr for CNs-B is 10 times more than that of CNs-A which suggests that the radiative recombination in CNs-B was faster than that of CNs-A. Moreover, kr of this order suggests that emission in these CNs originates from an optically allowed transition. Whilst the non-radiative rate constant of CNs was calculated by using ϕ = kr/(kr + knr), which was found to be in the order of 107 s−1 for either type of CN, it is also very fast. These observed recombination processes having a PL lifetime in the nanosecond range result from the strong coupling between the extended π electron system of the core with that of surface functionalities.
Sample | Excitation (nm) | τ1 (ns) | τ2 (ns) | τ3 (ns) | Average τ (ns) | CHISQ |
---|---|---|---|---|---|---|
CNs-A | 375 | 0.43(14.84%) | 2.75(57.78%) | 13.60(27.38%) | 10.23 | 1.26 |
CNs-B | 375 | 6.46(50.72%) | 24.37(49.29%) | — | 20.53 | 1.26 |
The morphology of the CNs was characterized using transmission electron microscopy (TEM) which shows the high degree of monodispersity with a narrow size distribution range having an average size of 40 and 42 nm for CNs-A and B respectively (Fig. 2a and c). The presence of lattice fringes in High Resolution Transmission Electron Microscopy (HRTEM) shows the crystalline nature of CNs with lattice spacing of 0.35 and 0.27 nm for CNs-A and B respectively (Fig. 2a (inset) and d). Selected Area Electron Diffraction (SAED) shows a concentric ring pattern along with a bright spot which is again significant proof for the crystallinity of CNs-A (Fig. 2b). Results obtained from the TEM study are consistent with the Raman analysis.
Fig. 3 (a) CLSM images showing fluorescence signals of C3H10T1/2 cells imaged by CNs-A and B under excitation 493 nm. (b) Cytotoxicity tests for CNs-A and B. |
A literature survey figures out that CNs are efficient nanosensors owing to their narrow range of selectivity.26–30 Herein, the Fe3+ ion imparts a drastic change in PL quenching as compared to other metal salts (Fig. 4a and b). This is attributed to non-radiative electron transfer that involves partial transfer of an electron from the excited state of CNs to the d orbital of the Fe3+ ion.31 Although similar responses were obtained for both CNs A and B, CNs-B show a comparatively higher sensitivity toward the Fe3+ ion due to amine induced modulation of the chemical and electronic transition.32,33 Successive addition of the Fe3+ ion leads to a gradual decrease in PL intensity at 435 nm revealing that the intensity of the CNs-A was sensitive to Fe3+ ion concentration (Fig. SI1†) (a similar study was performed with CNs-B and the Stern–Volmer plot for quenching in CNs A and B is provided in Fig. SI2 and Table SI1†).
Fig. 4 (a) Fluorescence response of CNs-A in the presence of different cations. (b) Performance of CNs-A comparing fluorescence intensities in the presence of different metal ions. |
To rule out the possibility of the presence of any fluorescence quenching caused by the globin moiety, a parallel experiment using bovine albumin serum protein has been carried out to ensure the cause of quenching. It has no emission in the range of 250–650 nm (Fig. 5e). The overall fluorescence from the CNs-protein composite system is due to the CN moiety itself, and there is no other fluorescence contribution from the protein part. Therefore the aforementioned analysis concluded that, in particular, the heme moiety in haemoglobin accounts for the quenching phenomenon.
This overwhelming effect Fe3+ over other metal salts laid the foundation of further study that covers the biosensing application of CNs using haemoglobin. The absorption spectrum of hemoglobin shows two peaks, one of which is weak and less prominent at 270 nm whereas another is strong and centred at 405 nm (Fig. 5a).
Moreover, Zhang et al. demonstrate the IFE of Cr(VI) using a hydrophilic ionic chemosensor.27c In addition to this Huang et al.35 and Barati et al.36 showed the IFE of Hemoglobin on the fluorescence quenching of CNs. The high molar extinction coefficient of Hemoglobin and the efficient overlap of its absorption spectrum with the absorption and emission spectrum of CNs make it a suitable absorber for the IFE. Furthermore for a detailed explanation whether the absorption wavelength and/or emission light were/was absorbed by the hemoglobin in the system based on the IFE, we have performed two sets of experiments. The first set of experiments proves that the fluorescence decrease was excitation wavelength-dependent. The maximum fluorescence decrease occurs at 405 nm (irrespective to Hb concentration), which was treated as the absorption maximum of the hemoglobin peak associated with a higher molar extinction coefficient Fig. 6a. Besides this, there was also a fluorescence decrease at 275 nm which was related to the absorption maximum of another hemoglobin peak having a lower molar extinction coefficient. Furthermore the second set of experiment shows the extent of fluorescence quenching at different emission wavelengths with excitation at 335 nm. Herein, the maximum decrease in fluorescence occurs at a wavelength of 400 nm which was near to the absorption maximum of hemoglobin. Consequently, Hb absorbs emission light at 380 nm, 400 nm and 420 nm more intensively than longer wavelengths Fig. 6b. This investigation shows that hemoglobin absorbs the emission light of CNs. These two experiments finally suggested that the fluorescence of CNs mainly decreased by the IFE of Hb rather than other processes. Further proof for the IFE comes from the lifetime measurement before and after the addition of hemoglobin discussed in the upcoming section. Here successive addition of Hb increases the absorbance of Hb, which would shield absorption and excitation light from the fluorophore. Thus there was less light available for the fluorophore and, as a result, the absorption and emission intensity of CNs decreased.
Further successive addition of haemoglobin in CNs results in considerable quenching of fluorescence intensity along with a gradual bathochromic shift thus CNs can used as fluorescent probes for haemoglobin detection (Fig. 5b).35,36 Variation of fluorescence intensity of CNs is proportional to Hb concentration, which is well explained by considering the Stern–Volmer relationship:
F0/F = 1 + kqτ0[Q] = 1 + ksv[Q] | (1) |
In order to gain deeper insight into the quenching phenomenon, we have further elaborated our discussion using ksv. It is important to recognize that the obtained linear Stern–Volmer plot does not prove whether the quenching is dynamic or static since both can give a linear Stern–Volmer plot.37 These two main quenching processes can be differentiated by temperature variation, viscosity or a time related single photon counting measurement (TCSPC). Therefore we have recorded the fluorescence life time decay curve of the CNs-A and CNs-A–Hb system (Fig. 5f) using a TCSPC experiment in order to observe the change in fluorescence lifetime of the fluorophore before and after addition of the quencher. Whilst static quenching involves a constant lifetime decay of the fluorophore both in the presence and absence of the quencher, dynamic quenching involves the change in fluorescence lifetime of the fluorophore after addition of the quencher.37
We obtained well fitted triexponential decay components in the absence and presence of Hb which give an average lifetime of 10.22 and 10.09 ns (Table 2). A constant value of the average fluorescence lifetime before and after the addition of the quencher clearly reveals the presence of static quenching in the CNs–Hb system. The unaltered lifetime obtained after addition of Hb involves the formation of a non-emissive ground state complex. This non emissive complex does not decrease the decay time of uncomplexed CNs. The entire fluorescence is only because of remaining uncomplexed CNs.37 Moreover the constant lifetime before and after the addition of the quencher indicates no complex formation in the excited state or energy transfer between Hb and CNs. On the basis of this fact it is concluded that the quenching is due the IFE rather than other processes.
Samples | Excitation (nm) | τ1 (ns) | τ2 (ns) | τ3 (ns) | Average τ (ns) |
---|---|---|---|---|---|
CNs-A | 375 | 3.97(39.86%) | 0.70(13.3%) | 12.13(46.82%) | 10.22 |
CNs-A + Hb | 375 | 3.77(39.73%) | 11.89(47.84%) | 0.61(12.43) | 10.09 |
CNs A + H2O2 | 375 | 4.00(39.57%) | 0.66(12.48%) | 11.81(47.94%) | 9.99 |
CNs-A + Hb + H2O2 | 375 | 4.00(39.66%) | 0.65(13.31%) | 12.02(47.03%) | 10.14 |
Another piece of evidence for the formation of the ground state complex between CNs and Hb comes from the absorption spectrum of the CNs, Hb and CNs–Hb composite system.36 The non-superimposition of the absorption spectrum of the CNs–Hb composite and the sum of the individual absorption spectrum of CNs and Hb within the experimental error confirm the formation of the ground state complex. The enhancement of the effective size of the ground state complex (CNs–Hb composite) is observable by a bathochromic shift of the absorption spectra of the composite as compared to the sum of the individual absorption spectrum of the CNs and Hb system (Fig. SI4†).
As from the above discussion it is clear that hemoglobin itself has an extremely high potential for fluorescence quenching of CNs.20,21 Now the forthcoming section involves building of a reversible turn ON–OFF–ON switch based on the interaction of excessive H2O2 with the preceding CNs–Hb composite system. A literature survey conceded that further application of H2O2 leads to more pronounced fluorescence intensity quenching based on hydroxyl radical (˙OH) formation which was accomplished by the Fenton reaction (Scheme 3).38–42 This ˙OH has a very high reduction potential of 2.74 V that makes it a very efficient oxidising agent. This effectively oxidises the surface emissive group of CNs, which leads to the quenching in fluorescence intensity of CNs.
Scheme 2 Mechanism of the turn ON–OFF–ON system in CNs under different input conditions of Hb and H2O2. |
To the best of our knowledge, it is the first report which shows an enormous fluorescence enhancement on excessive addition of H2O2 to the CNs–Hb composite (Fig. 8a). We have made four systems to understand the interaction of excessive H2O2 and the CNs–Hb composite. The first system has CNs-A alone, the second system has CNs-A + Hb, the third system has CNs-A + H2O2 and the fourth system has CNs-A + Hb + H2O2. The photoluminescence spectra involving the interaction of H2O2 with CNs show high fluorescence enhancement as compared to CNs alone. The TEM study affirmed a noticeable reduction in particle size from 40 nm to 4 nm on addition of a large excess of H2O2 (Fig. SI7†). This decrement in particle size conversely increases the surface area to volume ratio which is strong evidence for enhanced photoluminescence in the CNs-A–H2O2 system.
There is also an increment in photoluminescence intensity of the CNs–Hb system on addition of H2O2 (Fig. 8a). However, the peak intensity is less as compared to the CNs A–H2O2 system. It is proposed that there are two process working simultaneously in the CNs A–Hb–H2O2 system, viz. elevation in the surface area to volume ratio of CNs on addition of a large excess of H2O2 that accounts for the credit point of the PL enhancement in Fig. 8a. Secondly, generation of ˙OH by the Fenton reaction occurring in the reaction medium, regarded as the debit point for the PL enhancement. It is a well known fact that H2O2 causes degradation of haemoglobin thereby releasing the Fe2+ ion from the complexed CNs A–Hb composite. This released Fe2+ (derived according to Scheme 3) and H2O2 act as scavengers for ˙OH and convert it into −OH and HO2˙ respectively (Scheme 3 proposed mechanism in a large excess of H2O2).38 In this way the majority of the ˙OH radical is consumed readily before imparting its effect on the emissive group present on the surface of CNs. However the remaining few unconsumed ˙OH radicals present in the medium impart their role on CNs. Therefore the quenching effect of the ˙OH radical was overshadowed through its overconsumption by H2O2. Hence besides having ˙OH radicals in the system, we obtained enhanced fluorescence (Fig. 8a). A constant lifetime after addition of excessive H2O2 in either system i.e., CNs A and the CNs A–Hb composite system are direct evidence for the absence of any type of energy transfer or electron transfer process. The entire phenomenon of fluorescence turn ON–OFF–ON is solely governed by tuning in the particle size of CNs (Table 2).
From the above discussion it is apparent that the overall PL enhancement of the CNs A–Hb–H2O2 system under the influence of H2O2 is due to mitigation in the particle size (Scheme 2). We have also performed similar experiments with a phosphate buffer of pH 7.4 to normalize the system in a biological medium. Analogous results were obtained regarding the quenching trend (Fig. 7a) and PL enhancement on adding an excess of peroxide (Fig. SI5†). Variation in PL intensity of CNs with hemoglobin concentration maintains linearity up to a very high concentration of 10 μM with ksv, the correlation coefficients are shown in Table SI3.† A similar study for CNs-B under control pH 7.4 is shown in Fig. SI6 and Table SI3.†
Fig. 7 (a) Typical PL quenching of CNs-A in different concentrations of Hb 0–10 μM (a–k). (b) Linear relationship between I0/I and Hb concentration in the range of 0–10 (μM) under controlled pH 7.4. |
This reversible fluorescence ON–OFF–ON switch influences the construction of a logic operation for nanoparticles as shown in Fig. 8a. IMPLICATION logic gate is obtained using Hb and H2O2 as inputs. The system is considered to be in the ON state when it is above the threshold value and designated as 1. It remains OFF when below the threshold value and denoted as 0. Emission intensity at 421 nm was assigned as output 1 (Fig. 8a). In the case of output 1 a fluorescence of 7.5 × 104 has been taken as a threshold value. In the presence of Hb the fluorescence intensity of the solution is below the threshold value (0). In all other circumstances it remained in the ON state (1). This logic operation resembles the IMPLICATION (Fig. 8b) logic gate and is represented in Fig. 8c as a combinatorial logic scheme.
In summary, we have demonstrated an easy one step hydrothermal approach towards water soluble photoluminescent CNs from Indian jamun (Syzygium cumini) as a carbon source. The toxicity studies exhibit that the CNs display zero to very low toxicity to a biological environment. Furthermore, we employed hemoglobin as a targeting moiety to explore the biosensing ability of CNs based on the turn ON–OFF mechanism. Moreover, we have made a reversible fluorescent turn ON–OFF–ON switch taking the CNs–Hb composite system in conjugation with a large excess of H2O2.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/c6ra14308c |
This journal is © The Royal Society of Chemistry 2016 |