# Synthesis of Highly Emissive CdSe Quantum Dots by Aqueous Precipitation Method

Authors: Bing Gao; Chao Shen; Shuanglong Yuan; Yunxia Yang; Guorong Chen
Journal: Journal of Nanomaterials
 (2013)

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## Abstract

CdSe quantum dots (QDs) with high quantum yield (QY) up to 76.57% are synthesized using the aqueous precipitation method. With the control ofSeSO32- concentration in Se precursor, the nucleation speed and concentration of CdSe QDs are increased. The mass of obtained Cd2+ and Se2+ in nanocrystal is measured by inductively coupled plasma atomic emission spectrometry (ICP-AES). XRD and HRTEM are used to identify the crystal phase and morphology of the products which are pure CdSe crystals in the cubic zinc blende phase and uniformly dispersed in the solution with the size between 2 nm and 2.3 nm. Results demonstrate that the emission wavelength of CdSe QDs is 500 nm~560 nm along with the increased temperature 50°C~90°C and prolonged time 5 min~25 min.


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## Body

## 1. Introduction

Because of excellent size-dependent optical characteristics and chemical treatability, semiconducting CdSe quantum dots (QDs) have been widely applied in biological identification (medical diagnosis), solar cells, optoelectronic devices, display instruments, nonlinear optical equipment, and magnetic materials [1–3]. In 1993, Murray et al. [4] firstly prepared CdSe QDs by using trioctylphosphine oxide (TOPO) and trioctylphosphine (TOP) as the solvent and obtained the very high fluorescence quantum yield (QY) up to 80% [5–7]. However, TOPO is highly toxic, explosive, and inflammable as well as expensive and difficult to control. Therefore, investigations on phosphine-free synthesis of CdSe QDs have attracted researchers’ much attention in recent years. For example, Zhao et al. [8] obtained CdSe QDs with the ten carbonate cadmium of shorter carbon chain using cadmium oxide and decanoic acid as Cd precursor and the Se powder dispersed and dissolved by eighteen ene and eighteen amine as Se precursor, but QY decreased to about 50%. To be further closer to the standard of green chemistry in preparation of CdSe QDs, the low-temperature aqueous phase method was developed, which, besides nontoxicity, has advantages of lower cost, simple synthesis process, and the improved stability of CdSe QDs [9–11]. But QY of products was reduced even lower, generally 30% or less [12, 13]. In this context, it is essential as well as challenging to increase QY of CdSe QDs synthesized by the aqueous phase method.In the present work, the effective aqueous precipitation method has been explored where the control ofSeSO32- concentration in Se precursor was especially emphasized in order to realize speed-up of the nucleation of the products and increase of the concentration of CdSe QDs. We have demonstrated QY of the synthesized CdSe QDs maximum to 76.57% and discussed the relevant mechanism.


## 2. Experimental

The Se precursor for the present work was prepared by mixing the selenium powder (0.005 mol) (A.R, Shanghai Meixing Chemical Co., Ltd.), sodium sulfite (0.01 mol) (A.R, Sinopharm Chemical Reagent Co., Ltd.), sodium hydroxide (0.01 mol) (A.R, Shanghai Aijian ready-made Reagent Co., Ltd.), and deionized water (50 mL) with N2 protection and magnetic stirring. The mixture was heated to boiling while the solution turned from red brown to the black precipitate. Then sodium hydroxide (0.01 mol) was added, and after returning for 4 hours, the reactants were cooled down to the room temperature followed by nitrogen protection for 30 min.The Cd precursor was prepared by mixing water, ethanol, and oleic acid (A.R, Jiangsu Yonghua Fine Chemicals Co., Ltd.) together in volume ratio of 10 : 30 : 8. Cadmium acetate 0.001 mol (A.R, Sinopharm Chemical Reagent Co., Ltd.) and sodium hydroxide (0.7 g) were added as precipitation agents to the mixed solvent (48 mL). The mixture was under the N2 protection until it became clear and transparent. The reaction temperature was 50°C, 70°C, and 90°C.The CdSe QDs were synthesized by adding 10 ml Se precursor solution to the 48 mL Cd precursor solution, under N2 protection and magnetic stirring. The reactions were carried out at 50°C, 70°C, and 90°C for 5 min, 10 min, 15 min, 20 min, and 25 min, respectively, as marked in Table 1. The samples were centrifuged with ethanol and dispersed in hexane.Table 1
Sample numbers and reaction temperature and time.
Temperature
Time
5 min
10 min
15 min
20 min
25 min
50°C
I1
I2
I3
I4
I5
70°C
II1
II2
II3
II4
II5
90°C
III1
III2
III3
III4
III5X-ray diffraction spectra (XRD, D/MAX 2550 VB/PC, Japan, RIGAKU) (λCu=0.15406 nm) were recorded to identify the crystal phase and size. The high resolution transmission electron microscopy (HRTEM) (JEM-201, American FEI company) was used to characterize the morphology and structure of the samples. The optical absorption spectra (a Lambda 950 UV-Visible Spectrophotometer, Perkin Elmer, Waltham, MA) and the photoluminescent (PL) spectra (model Fluorolog-3-P, France Jobin Yvon company, model Cary 500, American Varian company) were measured for calculation of QY according to the absorption coefficient and integrated emission area. The mass of obtained Cd2+ and Se2+ in nanocrystal is measured by inductively coupled plasma atomic emission spectrometry (ICP-AES) (model IRIS 1000). The flow diagram of the reaction is shown in Figure 1.Figure 1
The flow diagram of the whole reaction.


## 3. Results and Discussion

Figure2 presents the XRD spectra of samples I1, II1, and III1 for crystal phase identification, where the XRD profile of CdSe crystals in the cubic zinc blende phase (JCPDS file no. 19-0191) is included at the bottom as the reference. Three main diffraction peaks are clearly identical at around 25.18°, 42.31°, and 49.52°, coinciding with those of CdSe crystals having different crystal planes (111), (220), and (311), respectively. No diffraction peak of other crystal phase is discovered in Figure 2, indicating that the structure with pure CdSe crystals was obtained.Figure 2
XRD patterns of sample I1, II1, and III1 (50°C, 70°C, and 90°C).The average diameter of CdSe crystals in sample I1, II1, and III1 is calculated according to the broadening of XRD by the Scherrer formulaD=kλ/βcosθ, where λ=0.15406 nm, β is the full wavelength at half maximum (FWHM) of diffraction peak (in Radian), and k is a constant (0.89) [13]. The calculated results are given in Tables 2, 3, and 4, where the estimated average grain diameter of CdSe QD is about 1.84 nm, 2.04 nm, and 2.27 nm, respectively.Table 2
Calculated diameters of CdSe crystals in sample I1 (50°C).
2θ
25.30°
42.24°
49.23°
θ
12.65°
21.12
24.62
FWHM (°)
10.3
4.73
2.98
FWHM (rad)
0.18
0.08
0.05
Radius (nm)
0.78
1.80
2.95
Average radius (nm)
1.84 nmTable 3
Calculated diameters of CdSe crystals in sample II1 (70°C).
2θ
25.37°
42.04°
49.74°
θ
12.69°
21.02
24.87
FWHM (°)
3.51
4.11
5.10
FWHM (rad)
0.08
0.07
0.09
Radius (nm)
2.34
2.10
1.68
Average radius (nm)
2.04 nmTable 4
Calculated diameters of CdSe crystals in   sample III1 (90°C).
2θ
25.51°
42.56°
49.25°
θ
12.76°
21.28
24.63
FWHM (°)
11.53
3.72
2.56
FWHM (rad)
0.20
0.06
0.04
Radius (nm)
0.70
2.43
3.69
Average radius (nm)
2.27 nmHRTEM photos of samples I1, I3, I5; II1, II3, II5 and III1, III3, III5 are presented in Figures3(a)–3(i). With the reaction temperature increasing from 50°C and 70°C to 90°C, the size of CdSe QDs becomes larger from 2.1 nm and 2.13 nm to 2.3 nm, respectively, which are consistent with the results to XRD. It is seen that the precipitated CdSe QDs in the three samples are dispersed uniformly.HRTEM photos of samples I1, I3, I5, II1, II3, II5, III1, III3, and III5.
(a)
I1 (50°C)
(b)
I3 (50°C)
(c)
I5 (50°C)
(d)
II1 (70°C)
(e)
II3 (70°C)
(f)
II5 (70°C)
(g)
III1 (90°C)
(h)
III3 (90°C)
(i)
III5 (90°C)Furthermore, HRTEM photos of samples I1, II1, and III1 for lattice parameter analysis are provided in Figure4. It is seen from the figure that the interplanar spacing of CdSe QDs in samples with the different reaction time is close to each other (0.3165 nm, 0.3162 nm, and 0.3265 nm), and they are all close to the interplanar spacing (0.35145 nm) of the (111) CdSe crystal plane corresponding to the strongest diffraction peak at 2θ=25.321° in XRD. This result further demonstrates that the obtained products are CdSe crystal phase.HRTEM photos of samples I1, II1, and III1 for lattice parameter analysis.
(a)
I1 (50°C)
(b)
II1 (70°C)
(c)
III1 (90°C)Figure5 shows the absorption spectra of samples I1~I5, II1~II5, and III1~III5. An absorption peak appears at 450 nm, 475 nm, and 510 nm, respectively, suffering an obvious blue shift compared with that of the bulk CdSe (717 nm). Such a blue shift (or band-gap broadening) phenomenon occurs as a consequence of the quantum size effect, showing that the products are already in nanoscale. However, with the reaction temperature increasing, the quantum size effect reduces due to the growing size of products, leading to the red shift of the absorption peak or narrowing of the band-gap.Absorption spectra of samples under different reaction temperature and time (a) 50°C, (b) 70°C, and (c) 90°C.
(a)
50°C
(b)
70°C
(c)
90°CFigures6(a), 6(b), and 6(c) show the normalized emission spectra of samples under different reaction temperature and time. For all three groups, under the excitation of blue light (460 nm), a broad emission band is observed peaking in the green region and showing obvious red shift with the increasing reaction time. Taking the 50°C group (a) as an example, it is seen that the emission peak is, respectively, at 500 nm, 502 nm, 505 nm, 509 nm, and 513 nm, corresponding to the reaction time changing from 5 min to 25 min with an increase of 5 min each. The reaction temperature exerts the same effect on the emission spectra of samples under 70°C and 90°C, shown in Figures 6(b) and 6(c); that is, the red shift occurs from 500 nm to 533 nm (70°C) and 510 nm to 560 nm (90°C), respectively. Similar to analysis on the absorption spectra above, the regular red shift of the emission band is due to the increase of grain size and the decrease of the band gap. Because the luminescence essence of the semiconducting CdSe QDs is the transition probability of the electrons in the band gap, along with the increased crystal size of products due to the prolonged reaction time and the increasing reaction temperature, the band gap of the products becomes narrower, leading to the red shift of emission wavelength. Figure 6(d) shows the real colour of samples under different temperature in daylight, which are yellow and orange to red.The emission spectra of samples under different reaction temperature and time ((a), (b), and (c); 50°C, 70°C, and 90°C) (λex=460 nm) and the picture of real samples (d).
(a)
50°C
(b)
70°C
(c)
90°C
(d)
real samplesIt is known via previously reported work that QY of CdSe QDs can be calculated according to formula (1) with rhodamine B as reference object [8, 14]:
(1)YQ=YR×IQIR×ARAQ×NQ2NR2,
where YR is the standard QY (95%) of rhodamine B, IQ and IR represent the integral emission areas of CdSe QDs and rhodamine B under 460 nm excitation, respectively, AR and AQ are the absorption coefficients (around 0.05 or less than 0.05) of the rhodamine B and CdSe QDs at 460 nm [15, 16], and NQ and NR are refractive indices of the n-hexane (1.375) and ethanol (1.362) used as the solvent for the CdSe QDs and rhodamine B.The absorption coefficients of samples I1, II1, and III1 and rhodamine B at 460 nm are 0.0287, 0.0565, 0.0530, and 0.0139, corresponding to their integral emission areas of1.29×107, 1.76×107, 1.17×107, and 7.9×106, respectively, under the 460 nm excitation. According to these data, QY of samples I1, II1, and III1 are calculated via formula (1) as 76.57%, 53.07% and 37.61%.It is obvious that along with the increased crystal size of CdSe QDs in the samples, QY decreases from 76.57% (I1) to 37.61% (III1) most likely due to the reduced quantum confinement effect. However, in the present work, QY of sample I1 reaches the level of 76.57%, much higher than those (~30%) reported with the aqueous precipitation method [13]. The main reason is due to the nearly complete reaction of Se precursor which much enhances the luminescence of CdSe QDs.In our work, black powders were precipitated in preparation of the Se precursor. According to the principle of chemical reaction [17], the red selenium precipitation occurs when selenite solution meets the reducing agent in acid solution and turns to black after being heated. So it can be inferred that the black precipitate is the unreacted Se powder. The selenium precipitation reduces the concentration of Se2− in the solution and makes the stoichiometric ratio inaccurate, which consequently affects the reaction speed and final concentration of CdSe QDs in the solution.It is known that thiosulfateS2O32- tends to decompose into sulfur and sulfurous acid in the acid solution, while it is stable in alkaline solution or alkali metal thiosulfate solution [17]. Similarly, instability of SeSO32- in the present work could be overcome by the addition of OH− to the Se precursor, guaranteeing the nearly-complete reaction of Se source. Also, consider the following reaction equations [18]:
(2)Se+SO32-⟶SeSO32-(3)SeSO32-+OH-⟶HSe-+SO42-(4)HSe-+OH-⟶Se2-+H2O(5)Cd2++Se2-⟶CdSeOH
- encourages the production of Se2- from SeSO32- to form CdSe QDs with Cd2+. So we add NaOH to Se precursor, and thus, Se powder nearly disappears.The masses ofCd2+ and Se2+ obtained from sample I1 (in solution) are measured by inductively coupled plasma atomic emission spectrometry (ICP-AES) shown in Table 5. The masses of Cd and Se source are 112 mg and 79 mg, and the qualities of Cd2+ and Se2+ in ICP test are 4.68 mg and 0.56 mg. The calculated proportion of Cd2+ in CdSe nanocrystal is 95.82%, and the total proportion of Se2+ in nanocrystal and unreacted to CdSe nanocrystal is 99.29%.Table 5
Determined Cd2+ and Se2+ % from ICP-AES analysis for sample I1 (50°C, 5 min).
Cd source
Se source
Cd2+ (tested by ICP)
Se2+ (tested by ICP)
Cd2+ (in CdSe)
Se2+ (in CdSe and unreacted  to CdSe)
112 mg
79 mg
4.68 mg
0.56 mg
95.82%
99.29%On the other hand, by takingCd2++Se2-→CdSe↓ as an elementary reaction, to make 0.005 mol Se powder react completely, 0.01 mol OH- is required. In the case without NaOH, there is only 5×10-9 (0.05×10-7) mol OH- in the 50 mL water. The addition of NaOH provides enough OH-. According to the reaction rate equations of V=K[Cd2+][Se2-], the content of OH- is 2×106 times as much as that in water. The increase of Se2- concentration speeds up the nucleation process of CdSe QDs and increases the concentration of the products, which leads to the high QY of CdSe QDs.


## 4. Conclusion

In this paper, CdSe quantum dots (QDs) are produced using an aqueous precipitation method. XRD patterns demonstrate the structure of products with the purely precipitated CdSe crystals. TEM manifests that the size of the CdSe QDs is between 2 nm and 2.3 nm with good monodispersity. The addition of NaOH to Se precursor speeds up the nucleation and increases the concentration of CdSe QDs. The ICP-AES shows that the calculated proportion of Cd2+ in CdSe nanocrystal is 95.82%, and the total proportion of Se2+ in nanocrystal and unreacted to CdSe nanocrystal is 99.29%. Furthermore, the band gaps of QDs blue shift compared to the CdSe bulk material show that the products are already in nanoscale. The photoluminescence spectra show the broad emission band centering at 500 nm~560 nm, depending on the size of the CdSe QDs. QY of CdSe QDs increases steadily along with the decreased crystal size with the maximum up to 76.57%. The CdSe QDs prepared in this paper with the environmental friendly method can probably be applied in the fields of LED and biological identification because of the high QY.In this paper, CdSe quantum dots (QDs) with high quantum yield (QY) up to 76.57% are synthesized using the aqueous precipitation method. With the control ofSeSO32- concentration in Se precursor, the nucleation speed and concentration of CdSe QDs are increased, and the quantum yield of the CdSe QDs is increased. Although the CdSe QDs have been studied for many years, we use the basis chemical knowledge to improve the photoluminescent property of the CdSe QDs. We propose the power of the basic chemistry.



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