PMCCPMCCPMCC

Search tips
Search criteria 

Advanced

 
Logo of sensorsMDPI Open Access JournalsMDPI Open Access JournalsThis articleThis JournalInstructions for authorssubscribe
 
Sensors (Basel). 2017 November; 17(11): 2628.
Published online 2017 November 15. doi:  10.3390/s17112628
PMCID: PMC5713075

Interaction between Diethyldithiocarbamate and Cu(II) on Gold in Non-Cyanide Wastewater

Abstract

A surface-enhanced Raman scattering (SERS) detection method for environmental copper ions (Cu2+) was developed according to the vibrational spectral change of diethyldithiocarbamate (DDTC) on gold nanoparticles (AuNPs). The ultraviolet-visible (UV-Vis) absorption spectra indicated that DDTC formed a complex with Cu2+, showing a prominent peak at ~450 nm. We found Raman spectral changes in DDTC from ~1490 cm−1 to ~1504 cm−1 on AuNPs at a high concentration of Cu2+ above 1 μM. The other ions of Zn2+, Pb2+, Ni2+, NH4+, Mn2+, Mg2+, K+, Hg2+, Fe2+, Fe3+, Cr3+, Co2+, Cd2+, and Ca2+ did not produce such spectral changes, even after they reacted with DDTC. The electroplating industrial wastewater samples were tested under the interference of highly concentrated ions of Fe3+, Ni2+, and Zn2+. The Raman spectroscopy-based quantification of Cu2+ ions was able to be achieved for the wastewater after treatment with alkaline chlorination, whereas the cyanide-containing water did not show any spectral changes, due to the complexation of the cyanide with the Cu2+ ions. A micromolar range detection limit of Cu2+ ions could be achieved by analyzing the Raman spectra of DDTC in the cyanide-removed water.

Keywords: surface-enhanced Raman spectroscopy, plasmonic gold nanoparticles, diethyldithiocarbamate, industrial electroplating wastewater, cyanide removal

1. Introduction

The resonant plasmonic enhancement of the local electric field on noble metal substrates could provide a highly sensitive platform for achieving single-molecule label-free detection [1]. SERS has been applied for detecting traces of organic compounds adsorbed on metal substrates [2]. A localized surface plasmon band of AuNPs can be utilized as a platform for studying chemical and biological reactions [3]. Plasmonic nanoparticles have been introduced to study heavy metal pollutants [4,5,6]. Detailed molecular interactions between organic compounds and metal atoms can be estimated with a combination of quantum-mechanical density functional theory (DFT) calculations [7,8].

Developments in sensing, identifying, and detecting heavy metal ions in aqueous solutions could contribute to the advanced treatment of wastewater [9]. The treatment of heavy metal ions in wastewater has been a significant challenge for environmental scientists [10]. However, because of the high toxicity of cyanide (CN) species, electroplating wastewater can be categorized into two kinds of wastewater: cyanide and non-cyanide [11]. Chlorination in highly alkaline conditions can be an efficient method for the reduction of cyanide ions in wastewater [12,13,14,15].

Diethyldithiocarbamate (DDTC) has been known to bind with metal complexes [16,17,18]. Among the various metal ions, Cu2+ has been found to interact strongly with DDTC [19,20,21,22]. Plasmonic nanoparticle-mediated SERS has been employed to detect hazardous species, such as heavy metal ions, in environmental samples [23]. The SERS spectrum of the DDTC-Cu2+ complex has recently been reported in a combination of quantum mechanical calculations [24].

The development of new, convenient methods for the spectroscopic characterization of contaminants in water effluent is still of significant importance in environmental fields [25,26]. Despite various methods for detecting ionic species [27] in aqueous solutions, there has been no report of a Raman spectroscopy-based analytical approach to DDTC-correlated copper ion quantification in real industrial wastewater samples. In this work, we found that SERS could be applied for detecting Cu2+ ions with the micromolar sensitivity in non-cyanide wastewater samples. In the case of cyanide presence in wastewater, samples need to be treated with alkaline chlorination before Cu2+ detection. The potential application of this research is to develop a quick and easy spectroscopic tool to estimate the toxic amounts of harmful chemicals in wastewater. Our work may also be used to detect the presence of cyanide ions in wastewater samples before and after alkaline chlorination.

2. Materials and Methods

2.1. Materials and Preparation of AuNPs and DDTC-Metal Complex

Sodium diethyldithiocarbamate trihydrate ((C2H5)2NCSSNa·3H2O) and the metal ionic substances were purchased from Sigma Aldrich (St. Louis, MO, USA). AuNPs were prepared by the previous method [28]. Our quantification methods for Cu2+ ions were based on our recent investigation [29].

We prepared AuNPs using a citrate reduction method. First, a triple-distilled water solution of hydrogen tetrachloroaurate trihydrate was mixed, stirred, and heated to the boiling point of water. Subsequently, sodium citrate was quickly added to this mixture and continuously stirred while the mixture was boiling. Finally, the level of the reaction solution was always kept at the beginning levels for 1 h by adding triple-distilled water slowly and continuously. The AuNPs were obtained at about 20 nm in diameter according to the measurements by Otsuka ELZ-2 and high-resolution transmission electron microscope (TEM) (JEOL JEM-3100).

To prepare the UV-Vis experiment with the DDTC-Cu2+ complex, all of DDTC (0.89 mM in triple-distilled water, 500.0 µL) and Cu2+ (1.0 mM in triple-distilled water, 50.0 µL) were put into a 2.0 mL Eppendorf tube as a first step. This mixture solution (pH = 7.0) was stirred and kept stable for 30 min at room temperature. In the second step, 450.0 µL of triple-distilled water was added into this mixture to obtain 1000.0 µL solution of DDTC-Cu2+ complex with 50.0 µM final concentration of Cu2+. After that, UV-Vis spectra of 1000.0 µL of DDTC-Cu2+ complex was recorded. Samples with other metal ions were prepared by substituting Cu2+.

For the SERS experiment of DDTC-Cu2+ complex on AuNPs, in the first step, all of the DDTC (8.9 mM in triple-distilled water, 50.0 µL) and Cu2+ (10.0 mM in triple-distilled water, 5.0 µL) was put into a 2.0 mL Eppendorf tube. This mixture solution (pH = 7.0) was stirred and kept stable for 30 min at room temperature. In the second step, 445.0 µL of AuNP solution was added into this mixture to obtain a 500.0 µL solution of the DDTC-Cu2+ complex on AuNPs with a 100.0 µM final concentration of Cu2+. Then, SERS spectra of 500.0 µL of the DDTC-Cu2+ complex on AuNPs was recorded. Samples with other metal ions were prepared by substituting Cu2+.

2.2. Instrumentations and DFT Calculations

UV-Vis absorption spectral changes of the DDTC-metal complexes before and after applying to the AuNP colloidal solution were obtained with a 3220 PC spectrophotometer (Mecasys, Daejeon, Korea). Atomic percentages in wastewater was obtained using a NEXION 350 D ICP-MS spectrometer (Perkin-Elmer, Boston, MA, USA). DFT calculations [30] and potential energy distribution were performed using the previous literatures [31]. The Au6 cluster is one of the simplest models of gold atoms. It includes calculations to predict the energetic stabilities and intramolecular interactions of the adsorbates on Au surfaces. This model includes six gold atoms that can connect with each other to generate the triangular geometry needed to form gold clusters.

All Raman data were obtained by using a Raman microscope system RM 1000 spectrometer (Renishaw, Gloucestershire, UK) with a 632.8 nm HeNe excitation laser and a CCD camera. The SERS spectra were recorded by using spectroscopic glass tubes after the preparation of the Cu2+ detection samples. The integration time for SERS measurement was set up at 10 s per spectrum with a range of 200–3200 cm−1. Prior to performing SERS, the spectral positions were calibrated based on Si peak at 520 cm−1.

2.3. Preparation of Wastewater Samples and Removal of the Cyanide Species Using Alkaline Chlorination

The real water samples were obtained from the wastewater treatment center (Pusan, Korea). The cyanide reactions could be derived from the previous literature [32]. Samples “S1” and “S2” were obtained before and after the process of removing the cyanide species, respectively.

3. Results and Discussion

3.1. Adsorption of DDTC-Cu2+ on AuNPs

Scheme 1 is a diagram of our detection of Cu2+ ions with a complex of DDTC and subsequent adsorption on AuNPs. As shown in Scheme 1a, our method would be able to detect Cu2+ ions not only using the UV-Vis method, but, more importantly, also based on the SERS tool, which could demonstrate a much higher selectivity and sensitivity capacity than the UV-Vis method.

In general, our method could be promisingly applied to wastewater samples in both the presence of CN and the absence of CN. Under wastewater conditions without CN, the results indicate the ability for DDTC-Cu2+ complex detection via both the colorimetric indicator and the SERS tool (as shown in Scheme 1b with the S2 sample). Moreover, in the case of the presence of CN (the S1 sample), our approach may also be useful as a quick and simple method to identify the cyanide species in electroplating industrial water, since the copper cyanide complex cannot bind efficiently with DDTC, based on the results of UV-Vis and SERS in comparison with the S2 sample.

Figure 1a shows a photo of DDTC-metal complexes. The Cu2+ ion exhibited a yellow color, which was supported by the UV-Vis absorption spectra of DDTC-metal complexes, as shown in Figure 1b. The inset in Figure 1b shows the UV-Vis absorption spectra, as well as a photo of DDTC-Cu2+ corresponding to various concentrations of the Cu2+ ion. The absorption bands of DDTC-Cu2+ exhibited prominent bands at ~450 nm, which is in different from other tested ions as previous reported [21]. The band at 520 nm is the spectrum of the pristine AuNPs just after synthesis, without any DDTC complexes. In Figure 1c, upon adsorption on AuNP surfaces, the plasmonic bands of initial AuNPs at 520 nm became considerably redshifted to ~700 nm, indicating the aggregation of AuNPs due to the strong binding of sulfur atoms in DDTC on Au. Although we found that the aggregation-induced color and UV-Vis spectral changes after adsorption upon AuNPs in Figure 1d did not depend on the metal ionic species, presumably due to the strong binding of the sulfur atoms in DDTC on Au, the strong binding of the Cu2+ ions with DDTC as shown in Figure 1a,b may change the minute adsorption characteristics on AuNPs. Despite the extensive aggregation of AuNPs, regardless of the complex types of DDTC with different ions as indicated in Figure 1d, SERS may exhibit minute spectral changes depending on the binding modes. As listed in Table 1, our DFT calculations predicted that the ν(N=C) mode at 1490–1520 cm−1 for DDTC could be sensitively changed on Au atoms, depending on the binding modes and the presence of Cu(II) ions. To find any different interfacial interactions, we performed Raman spectroscopy.

Figure 1
(a) Photo of DDTC and DDTC-metal complexes for NH4+, K+, Ca2+, Mg2+, Cd2+, Pb2+, Hg2+, Zn2+, Co2+, Cr3+, Ni2+, Fe2+, Fe3+, Cu2+, and Mn2+ ions. (b) UV-Vis absorption spectra of DDTC-metal complexes. The inset shows the absorption bands at ~450 nm and ...
Table 1
Spectral data and vibrational assignments for DDTC and DDTC-Cu2+ on Au.

3.2. Raman Spectra of DDTC-Cu2+ on AuNPs

Figure 2a exhibits normal Raman (NR) for the solid state of DDTC, and the SERS spectra of DTTC, DDTC-Zn2+, and DDTC-Cu2+ on AuNPs. Our spectra appear consistent with that in the previous report [24]. Notably, the vibrational band at ~1490 cm−1 was prominently blueshifted to ~1504 cm−1, as marked in red arrows in the case of DDTC-Cu2+. Such spectral changes were not observed for the SERS spectra of DDTC-metal complexes on AuNPs, as illustrated in Figure 2b. The difference may be due to the exceptionally high binding energy of the Cu2+ ion to DDTC. To explain the spectral changes, the quantum mechanical DFT calculations were introduced to better assign the Raman peaks of DDTC with a complex of the metal ion in a free and adsorbed state on Au6 cluster atoms. An appropriate vibrational assignment is summarized in Table 1.

Figure 2
(a) Normal Raman (NR) for the solid state of DDTC and SERS spectra of DDTC, DDTC-Zn2+, and DDTC-Cu2+ on AuNPs. In the case of the DDTC-Cu2+ complex, the vibrational band at ~1490 cm−1 was prominently blueshifted to ~1504 cm−1, as marked ...

3.3. DFT Calculations of DDTC-Cu2+ on AuNPs

The DFT calculated spectra of DDTC and DDTC-Cu2+ on the Au6 cluster under the polarizable continuum model (PCM), appeared to match well with the SERS spectrum of the experimental Raman spectrum of DDTC. The bands at ~1423 and ~1490 cm−1 can be both ascribed to the vibrational modes of C=N stretching and CH2 bending modes. Of these, the stretching vibration of C=N is supposed to be more Raman-active dominant. These two bands, which are sensitive to the C=N stretching modes, can be expected to change considerably on AuNPs if the copper ion replaces the sulfur atom, leading to change in the relative Raman signals based on the present theoretical calculation. Although not shown here, the bond length of C=N of DDTC appeared to decrease from 1.39 to 1.34 Å after binding to Cu2+, resulting in increased vibrational frequencies.

3.4. Quantification of the Cu2+ Ion on the Basis of Raman Spectra

According to a previous report [33], the C=N stretching vibrational frequency should increase when the Schiff base is bound to Lewis acids such as H+ and BF3. Considering that the Cu2+ ion, as an electron pair receptor, could play the role of a Lewis acid, its binding to the nitrogen atom could increase the C=N stretching vibrational frequencies. A recent SERS study also indicated that the DDTC-based thiram and ziram may coordinate with a gold film as either a monodentate or a bidentate mode on Au [34].

Figure 3a shows the concentration-dependent SERS spectra of DDTC on AuNPs. The peak intensities at ~1504 cm−1 steadily increased, depending on the concentration of the Cu2+ ion, as magnified in Figure 3b. The calibration curve of the Raman peak intensities versus [Cu2+] is shown in Figure 3c.

Figure 3
(a) Cu2+ concentration-dependent SERS spectra of DDTC on AuNPs in distilled water. (b) A magnified view of the spectral region from 1380 to 1600 cm−1. (c) Three independent measurements of Raman intensities of vibrational bands at ~1504 cm−1 ...

3.5. Raman Spectroscopic Quantification of Cu2+ Ions in Electroplating Wastewater Samples

Considering that alkaline chlorination can remove hazardous cyanide species from wastewater samples [12,13,14,15], we applied our method to detecting the presence of cyanide ions in real wastewater samples before and after alkaline chlorination. Table 2 shows the atomic percentages of various metal ionic species in electroplating wastewater samples. Figure 4 shows our spectroscopic results from the electroplating wastewater samples: standard solution of [CN] = 100 ppm, “S1” (cyanide-containing), and “S2” (after alkaline chlorination). Under our experimental conditions, UV-Vis absorption and SERS spectra of DDTC on AuNPs, depending on the concentration of Cu2+ for sample “S2” after alkaline chlorination, looked similar to those in the distilled water, whereas the cyanide-containing samples of the standard and “S1” did not exhibit such behaviors. The complex formation of the Cu2+ ion with the CN species may hamper the binding of Cu2+ and DDTC. In Figure 4b, the absorption band was weakened for the cyanide-containing wastewater samples. This interpretation could also be supported by the relatively weak CN intensity at ~2114 cm−1 [29] of the wastewater after the alkaline chlorination treatment of sample “S2”, as shown in Figure 4c.

Figure 4
(a) Initial photo of the industrial wastewater samples: [CN] = 100 ppm, “S1” (cyanide-containing), and “S2” (after alkaline chlorination). Photo of wastewater samples after dilution and treatment with DDTC. (b) UV-Vis absorption ...
Table 2
Atomic percentages of various metal ionic species in electroplating wastewater samples.

Figure 5 shows the concentration-dependent SERS spectra of DDTC on AuNPs in electroplating the wastewater sample “S2”. The peak intensities at ~1504 cm−1 steadily increased, depending on the concentration of the Cu2+ ion, similar to the case of the distilled water. The detection limit of the current SERS method was found to be around ten times lower than that of the colorimetric test under our experimental conditions. The lowest concentration of our SERS detection of Cu2+ in wastewater samples was around 1 ppm, which is lower than the Environmental Protection Agency permission level (1.3 ppm = ~20 μM) for drinkable water [29]. Figure 6 illustrates the alkaline chlorination process of the influent sample “S1” to remove the cyanide species in electroplating the industrial wastewater to produce non-cyanide wastewater “S2”. The following equations can be applied to treat the cyanide wastewater by alkaline chlorination.

8CN + 2Cu2+ → 2Cu(CN)3 + (CN)2 (Stoichiometry cyanide reaction with Cu2+)

Cl2 + 2NaOH → NaOCl + NaCl + H2O (alkaline chlorination)

NaOCl + CN → OCN + NaCl (Destruction of CN)

2OCN + 3OCl + 2OH → N2 + 3Cl + 2CO32− + H2O (Destruction of OCN and OCl)
Figure 5
(a) UV-Vis absorption spectra of the DDTC-Cu2+ complex in wastewater with bands at ~450 nm, depending on the concentrations of the Cu2+ ion. The inset shows a photo of the DDTC-Cu2+ complex with [Cu2+] from 0 to 50 ppm in wastewater. (b) Cu2+ concentration-dependent ...
Figure 6
An alkaline chlorination process of the influent sample “S1” to remove the cyanide species in electroplating industrial wastewater to produce the non-cyanide wastewater in sample “S2”.

Alkaline chlorination can be divided into two steps. (1) A highly alkaline condition (pH > 10) will suppress the generation of gaseous HCN to maintain the free cyanide ions in wastewater (workers should be cautious about exposure to the gas in the atmosphere). A chlorine gas injection at least seven times higher than that of cyanide will yield cyanate (OCN), avoiding the formation of the metal cyanide complexes and the other chlorine adducts, including cyanogen chloride (CNCl). (2) The cyanide adducts, such as OCN, can be destroyed by lowering the pH to 8.5 to decompose them to CO2 and N2.

4. Conclusions

Our study showed that a facile detection method for Cu2+ ions in the DDTC-metal complexes could be achieved by monitoring specific marker bands in the SERS spectra. The SERS bands at ~1504 cm−1 increased after the introduction of DDTC-Cu2+ complexes on AuNPs. This could be interpreted as the conformation of the complex that would have different orientations on Au as supported by DFT calculations. The other ions of Ni2+, Fe2+, Co2+, Mn2+, Zn2+, Pb2+, Mg2+, Cd2+, Ca2+, Hg2+, NH4+, Cr3+, Fe3+, and K+ did not exhibit such spectral behaviors. The UV-Vis absorption and a colorimetric method were also introduced to check the [Cu2+]-induced spectroscopic changes. Our method can be successfully applied to real electroplating wastewater samples. After removal of the CN species via alkaline chlorination, the DDTC spectral features could be correlated with the concentration of Cu2+.

Scheme 1
Schematic diagram of detection of Cu2+ ions with (a) a complex of DDTC and subsequent adsorption on AuNPs and (b) in electroplating wastewater after alkaline chlorination under the interference from the other ionic species.

Acknowledgments

This work was supported by the Korea Environment Industry & Technology Institute (KEITI) through the Technologies for the Water Supply & Sewerage Policy of Public Technology Program Based Environmental Policy Project funded by Korea Ministry of Environment (MOE) (No. 2016000700005). The authors would like to thank Moon-Kyung Kim and Taekyung Kim for helping the experiments.

Author Contributions

Author Contributions

S.-W.J. and N.H.L. conceptualized the study. T.D.N. conducted DFT calculations. K.-D.Z. provided the insight of the ionic detection for environmental water samples. N.H.L. designed and conducted the experiments. S.-W.J. analyzed the data. All authors read and reviewed the manuscript.

Conflicts of Interest

Conflicts of Interest

The authors declare no conflict of interest.

References

1. Chang T.W., Wang X., Mahigir A., Veronis G., Liu G.L., Gartia M.R. Marangoni convection assisted single molecule detection with nanojet surface enhanced Raman spectroscopy. ACS Sens. 2017;25:1133–1138. doi: 10.1021/acssensors.7b00427. [PubMed] [Cross Ref]
2. Ouyang L., Jiang Z., Wang N., Zhu L., Tang H. Rapid surface enhanced Raman scattering (SERS) detection of sibutramine hydrochloride in pharmaceutical capsules with a β-cyclodextrin-Ag/polyvivnyl alcohol hydrogel substrate. Sensors. 2017;17:1601 doi: 10.3390/s17071601. [PMC free article] [PubMed] [Cross Ref]
3. Kosman J., Jatschka J., Csaki A., Fritzsche W., Juskowiak B., Stranik O. A New Strategy for silver deposition on Au nanoparticles with the use of peroxidase-mimicking DNAzyme monitored via a localized surface plasmon resonance technique. Sensors. 2017;17:849 doi: 10.3390/s17040849. [PMC free article] [PubMed] [Cross Ref]
4. Koudelkova Z., Syrovy T., Ambrozova P., Moravec Z., Kubac L., Hynek D., Richtera L., Adam V. Determination of zinc, cadmium, lead, copper and silver using a carbon paste electrode and a screen printed electrode modified with chromium(III) oxide. Sensors. 2017;17:1832 doi: 10.3390/s17081832. [PMC free article] [PubMed] [Cross Ref]
5. Biyani M., Biyani R., Tsuchihashi T., Takamura Y., Ushijima H., Tamiya E., Biyani M. DEP-On-Go for simultaneous sensing of multiple heavy metals pollutants in environmental samples. Sensors. 2017;17:849 doi: 10.3390/s17010045. [PMC free article] [PubMed] [Cross Ref]
6. Futra D., Heng L.Y., Surif S., Ahmad A., Ling T.L. Microencapsulated Aliivibrio fischeri in alginate microspheres for monitoring heavy metal toxicity in environmental waters. Sensors. 2014;14:23248–23268. doi: 10.3390/s141223248. [PMC free article] [PubMed] [Cross Ref]
7. Costa A.C., Jr., Ramos J.M., Tellez Soto C.A., Martin A.A., Raniero L., Ondar G.F., Versiane O., Moraes L.S. Fourier Transform Infrared and Raman spectra, DFT: B3LYP/6–311G(d,p)calculations and structural properties of bis(diethyldithiocarbamate)copper(II) Spectrochim. Acta A. 2013;105:259–266. doi: 10.1016/j.saa.2012.11.053. [PubMed] [Cross Ref]
8. Ricci M., Lofrumento C., Becucci M., Castellucci E.M. The Raman and SERS spectra of indigo and indigo-Ag2 complex: DFT calculation and comparison with experiment. Spectrochim. Acta A. 2017;188:141–148. doi: 10.1016/j.saa.2017.06.036. [PubMed] [Cross Ref]
9. Leng Y., Qian S., Wang Y., Lu C., Ji X., Lu Z., Lin H. Single-indicator-based multidimensional sensing: Detection and identification of heavy metal ions and understanding the foundations from experiment to simulation. Sci. Rep. 2016;6:25354 doi: 10.1038/srep25354. [PMC free article] [PubMed] [Cross Ref]
10. Awasthi A.K., Zeng X., Li J. Integrated bioleaching of copper metal from waste printed circuit board—A comprehensive review of approaches and challenges. Environ. Sci. Pollut. Res. Int. 2016;23:21141–21156. doi: 10.1007/s11356-016-7529-9. [PubMed] [Cross Ref]
11. Akcil A., Erust C., Gahan C.S., Ozgun M., Sahin M., Tuncuk A. Precious metal recovery from waste printed circuit boards using cyanide and non-cyanide lixiviants—A review. Waste Manag. 2015;45:258–271. doi: 10.1016/j.wasman.2015.01.017. [PubMed] [Cross Ref]
12. Lidia S., Francesco Z.G., Santosh N.K., Anna M.P. Copper electrodeposition and oxidation of complex cyanide from wastewater in an electrochemical reactor with a Ti/Pt anode. Ind. Eng. Chem. Res. 2000;39:2132–2139.
13. Dutra A.J., Rocha G.P., Pombo F.R. Copper recovery and cyanide oxidation by electrowinning from a spent copper-cyanide electroplating electrolyte. J. Hazard. Mater. 2008;152:648–655. doi: 10.1016/j.jhazmat.2007.07.030. [PubMed] [Cross Ref]
14. Lunn G., Sansone E.B. Destruction of cyanogen bromide and inorganic cyanides. Anal. Biochem. 1985;147:245–250. doi: 10.1016/0003-2697(85)90034-X. [PubMed] [Cross Ref]
15. Wild S.R., Rudd T., Neller A. Fate and effects of cyanide during wastewater treatment processes. Sci. Total Environ. 1994;156:93–107. doi: 10.1016/0048-9697(94)90346-8. [Cross Ref]
16. Mehta V.N., Anil Kumar M., Kailasa S.K. Colorimetric detection of copper in water samples Using dopamine dithiocarbamate-functionalized Au nanoparticles. Ind. Eng. Chem. Res. 2013;52:4414–4420. doi: 10.1021/ie302651f. [Cross Ref]
17. Cvek B., Milacic V., Taraba J., Ping D.Q. Ni(II), Cu(II), and Zn(II) diethyldithiocarbamate complexes show various activities against the proteasome in breast cancer cells. J. Med. Chem. 2008;51:6256–6258. doi: 10.1021/jm8007807. [PMC free article] [PubMed] [Cross Ref]
18. Sedlacek J., Martins L.M.D.R.S., Danek P., Pombeiro A.J.L., Cvek B. Diethyldithiocarbamate complexes with metals used as food supplements show different effects in cancer cells. J. Appl. Biomed. 2014;2:301–308. doi: 10.1016/j.jab.2014.04.002. [Cross Ref]
19. Han J., Liu L., Yue X., Chang J., Shi W., Hu Y. A binuclear complex constituted by diethyldithiocarbamate and copper(I) functions as a proteasome activity inhibitor in pancreatic cancer cultures and xenografts. Toxicol. Appl. Pharmacol. 2013;273:477–483. doi: 10.1016/j.taap.2013.09.009. [PubMed] [Cross Ref]
20. Noll C.A., Betz L.D. Determination of copper ion by modified sodium diethyldithiocarbamate procedure. Anal. Chem. 1952;24:1894–1895. doi: 10.1021/ac60072a008. [Cross Ref]
21. Uddin M.N., Salam M.A., Hossain M.A. Spectrophotometric measurement of Cu(DDTC)2 for the simultaneous determination of zinc and copper. Chemosphere. 2013;90:366–373. doi: 10.1016/j.chemosphere.2012.07.029. [PubMed] [Cross Ref]
22. Wang T., Fu Y., Huang T., Liu Y., Wu M., Yuan Y., Li S., Li C. Copper ion attenuated the antiproliferative activity of di-2-pyridylhydrazone dithiocarbamate derivative; However, there was a lack of correlation between ROS generation and antiproliferative activity. Molecules. 2016;21:1088 doi: 10.3390/molecules21081088. [PubMed] [Cross Ref]
23. Wei H., Abtahiabc S.M.H., Vikesland P.J. Plasmonic colorimetric and SERS sensors for environmental analysis. Environ. Sci. Nano. 2015;2:120–135. doi: 10.1039/C4EN00211C. [Cross Ref]
24. Tellez S.C.A., Costa A.C., Jr., Ramos J.M., Vieira L.S., Rost N.C.V., Versiane O., Rangel J.L., Mondragon M.A., Raniero L., Martin A.A. Surface enhanced Raman scattering, electronic spectrum, natural bond orbital, and mulliken charge distribution in the normal modes of diethyldithiocarbamate copper(II) complex, [Cu(DDTC)2] Spectrochim. Acta A Mol. Biomol. Spectrosc. 2013;116:546–555. doi: 10.1016/j.saa.2013.07.083. [PubMed] [Cross Ref]
25. Park M., Anumol T., Daniels K.D., Wu S., Ziska A.D., Snyder S.A. Predicting trace organic compound attenuation by ozone oxidation: Development of indicator and surrogate models. Water Res. 2017;119:21–32. doi: 10.1016/j.watres.2017.04.024. [PubMed] [Cross Ref]
26. Yan S., Yao B., Lian L., Lu X., Snyder S.A., Li R., Song W. Development of fluorescence surrogates to predict the photochemical transformation of pharmaceuticals in wastewater effluents. Environ. Sci. Technol. 2017;51:2738–2747. doi: 10.1021/acs.est.6b05251. [PubMed] [Cross Ref]
27. Aulsebrook M.L., Biswas S., Leaver F.M., Grace M.R., Graham B., Barrios A.M., Tuck K.L. A luminogenic lanthanide-based probe for the highly selective detection of nanomolar sulfide levels in aqueous samples. Chem. Commun. 2017;53:4911–4914. doi: 10.1039/C7CC01764B. [PubMed] [Cross Ref]
28. Lee P.C., Meisel D. Adsorption and surface-enhanced Raman of dyes on silver and gold sols. J. Phys. Chem. 1982;86:3391–3395. doi: 10.1021/j100214a025. [Cross Ref]
29. Ly N.H., Seo C., Joo S.W. Detection of copper(II) ions using glycine on hydrazine-adsorbed gold nanoparticles via Raman spectroscopy. Sensors. 2016;16:1785 doi: 10.3390/s16111785. [PMC free article] [PubMed] [Cross Ref]
30. Nguyen D.B., Nguyen T.D., Kim S., Joo S.W. Vibrational fingerprints of N6-methyladenine and N6,N6-dimethyladenine in Raman spectra. Vib. Spectrosc. 2017;90:7–13. doi: 10.1016/j.vibspec.2017.01.007. [Cross Ref]
31. Jamroz M.H. Vibrational energy distribution analysis (VEDA): Scopes and limitations. Spectrochim. Acta A Mol. Biomol. Spectrosc. 2013;114:220–230. doi: 10.1016/j.saa.2013.05.096. [PubMed] [Cross Ref]
32. Duke F.R., Courtney W.G. Complexes in oxidation–reduction reactions. The copper(II)–cyanide reaction. J. Phys. Chem. 1952;56:19–21. doi: 10.1021/j150493a005. [Cross Ref]
33. López-Garriga J.J., Babcock G.T., Harrison J.F. Factors influencing the C=N stretching frequency in neutral and protonated Schiffs bases. J. Am. Chem. Soc. 1986;108:7241–7251. doi: 10.1021/ja00283a019. [Cross Ref]
34. Sánchez-Cortés S., Domingo C., García-Ramos J.V., Aznárez J.A. Surface-enhanced vibrational study (SEIR and SERS) of dithiocarbamate pesticides on gold films. Langmuir. 2001;17:1157–1162. doi: 10.1021/la001269z. [Cross Ref]

Articles from Sensors (Basel, Switzerland) are provided here courtesy of Multidisciplinary Digital Publishing Institute (MDPI)