xu2013
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www.rsc.org/materials
0959-9428(2010)20:1;1-A
ISSN2050-7488
Materials for energy and sustainability
Journal of
Materials Chemistry A
www.rsc.org/MaterialsA Volume1 | Number 1 | January 2013 | Pages 0000–0000
Journal of
Materials Chemistry A
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This article can be cited before page numbers have been issued, to do this please use: J. Xu, L. Zhang, R. Shi and Y. Zhu, J.
Mater. Chem. A, 2013, DOI: 10.1039/C3TA13188B.
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1
Chemical exfoliation of graphitic carbon nitride for efficient heterogeneous2
photocatalysis34
Jing Xu,† Liwu Zhang, † Rui Shi, Yongfa Zhu* 5
Department of Chemistry, Tsinghua University, Beijing, 100084, PR China67
ABSTRACT. Single atomic layer nanosheet materials show great application potential in8
many fields due to their enhanced intrinsic properties from their counterparts and newly born9
properties. Herein, g-C3 N4 nanosheets with single atomic layer structure is prepared by a10
simple chemical exfoliation method. The as-prepared nanosheets show single atomic11
thickness of 0.4 nm and lateral size of micrometers. The structure and photocatalytic12
properties of the as-prepared single layer g-C3 N4 are then studied. Compared with the bulk g-13
C3 N4, single layer g-C3 N4 nanosheets show great superiority in photogenerated charge carriers14
transfer and separation. Accordingly, the photocatalytic H2 production and pollutant15
decomposition activities, and photocurrent generation of single layer g-C3 N4 nanosheets are16
much higher than that of the bulk g-C3 N4, indicating the great application potential of single17
layer g-C3 N4 nanosheets in photocatalysis and photosynthesis.18
19202122232425262728
2930313233
Keywords: Carbon nitride; Single atomic layer; Nanosheet; Photocatalysis3435363738
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1. INTRODUCTION34
Single atomic layer nanosheets have attracted extensive attention due to their unique5
structural and physiochemical properties.1 Since the discovery of the two-dimensional atomic6
crystal graphene,2 which represents many intriguing properties different from bulk graphite7
and potentials in diverse applications, great efforts have been performed to synthesize8
nanosheets with single atomic layer structure.3-7 By exfoliating layered materials into9
nanosheets, exotic electronic properties and high specific surface areas accompanying with10
greatly enhanced host capabilities have been obtained and show great potential in application11
in electronics, energy storage, solar energy conversion, etc.8, 9 12
Graphite-like carbon nitride (g-C3 N4), a metal-free polymer semiconductor, has attracted13
plenty of attention due to its potential application in solar energy conversion, photosynthesis,14electrocatalysis, bioimaging and biomedical application.10-21 The g-C3 N4 has been shown to be15
able to produce H2 by water splitting and decompose organic pollutants under visible light16
irradiation by pioneering works of Wang and coworkers.22 More potential applications of g-17
C3 N4 are emerging as researches carry on in structure engineering and activity improving. 12,1823-31 19
Motivated by graphene, researchers have tried to prepare the nanosheet form of g-C 3 N4 to20
fully explore the potential of g-C3 N4. Compared with graphite, the layer of g-C3 N4 is21
composed by C-N bonds instead of C-C bonds, while weak van der Waals force exists22 between the layers. Encourage by the exfoliation of graphite into graphene layers by the23
widely used Hummers method,32 Liu and coworkers employed the Hummers method to24
exfoliate bulk g-C3 N4.33 However, instead of nanosheets, particles with several hundred25
nanometers thickness were obtained and the planar atomic structure of g-C3 N4 has been26
destroyed, indicating that the Hummers method may destroy the intrinsic structure of g-C 3 N4.27
The failure is attributed to the not strong enough hydrogen bonding between the layers of28
strands of polymeric melon units with NH/NH2 groups proposed by Lostsch et al.,34 which is29
different from the planar pure covalent bonding cohesion within the graphite. Liu and30coworkers thus developed a direct thermal oxidation “etching” process of bulk g-C3 N4 to get31
g-C3 N4 nanosheets with a thickness of around 2 nm, implying a multilayer of g-C 3 N4 (6-732
layers).33 Ultrathin g-C3 N4 nanosheets were also prepared by ultrasound exfoliation or liquid33
exfoliation routes from bulk g-C3 N4.11, 35 The resulted nanosheets possess thickness of >2 nm.34
Instead of the “top-down” fabrication of g-C3 N4 nanosheets, Wang and Coworkers found that35
a “bottom-up” method by modifying polycondensation of g-C3 N4 precursors could result in36
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thin C3 N4 nanosheets with thickness of around 3.6 nm.36 Although different methods have1
successfully been developed to get g-C3 N4 nanosheets, the as-prepared g-C3 N4 nanosheets are2
still thicker than 2nm and composed of more than 6 C-N layers. It is still a great challenge to3
prepare real graphene-like g-C3 N4 material with single atomic layer.4
Herein, we have for the first time obtained the single atomic layer g-C3 N4 nanosheets5
(Monolayer-C3 N4) by a simple chemical exfoliation method. Since g-C3 N4 is not strong6
enough against the strong oxidation effect exerted by KMnO4 oxidant used in the Hummers7
method for graphite exfoliation, KMnO4 is no more used in the chemical exfoliation method.8
The obtained Monolayer-C3 N4 is then characterized and performances in photosynthesis and9
photocatalysis under visible light irradiation are investigated.10
2.
EXPERIMENTAL SECTION11
Synthesis of single atomic layer g-C3N4 nanosheets. g-C3 N4 was prepared by heating12dicyandiamide (Tianjin Fuchen Chemical Reagents factory, China) in a muffle furnace for 4 h13
to 550 °C and keep at this temperature for another 4 h in air. g-C3 N4 monolayer nanosheets14
were synthesized via the chemical exfoliation method. The as-prepared g-C3 N4 (1 g) was15
mixed with 10mL of H2SO4 (98 wt %) in a 50mL flask and stirred for 8 h at room temperature.16
Then the mixture was slowly poured into 100 mL of deionized water and sonicated for17
exfoliation. The temperature of the suspension increased rapidly, and the color changed from18
yellow to light yellow. The obtained suspension was then subjected to 10 min of centrifugation19
at 3,000 r.p.m. to remove any unexfoliated g-C3 N4. The obtained light yellow suspension was20centrifuged, washed thoroughly with deionized water to remove the residual acid, and finally21
drying at 80 °C in air overnight. In order to eliminate the structural defects, the obtained22
powders (0.3 g) were put into a flask with 150 mL of methanol and refluxed on a mantle heater23
at 65 °C for 6 h. After centrifuged and dried at 80 °C, the obtained products were g-C3 N4 24
nanosheets.25
Characterization of the Samples. The samples were characterized by powder X-ray26
diffraction (XRD) on a Bruker D8-advance X-ray diffractometer at 40 kV and 40 mA for27
monochromatized Cu Kα (λ = 1.5406 Å) radiation. The Brunauer-Emmett-Teller (BET)28
specific surface area and pore volume of the samples were characterized by nitrogen29
adsorption at 77 K with Micromeritics 3020 instrument. Transmission electron microscopy30
(TEM) images were obtained by Hitachi HT-7700 electron microscope operated at an31
accelerating voltage of 100 kV. Atomic Force Microscope (AFM) images were acquired in32
phase mode in air using a Digital Instrument Shimadzu SPM-9600 (The samples were33
prepared by drop-casting corresponding dilute dispersions onto freshly cleaved mica surface).34
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Fourier transformed infrared (FTIR) spectra were recorded on a Bruker VERTEX 7001
spectrometer between 4000 and 600 cm-1. Diffuse reflection spectra (DRS) were obtained on a2
Hitachi U-3010 UV-vis spectrophotometer. Photoluminescence spectra (PL) of the samples3
were obtained at room temperature excited by incident light of 318 nm using a fluorescence4
spectrometer (JASCO FP-6500). Elemental analysis results were collected from an EA 30005analyzer. 6
Photocatalytic tests and Photoelectrochemical Performance. The photocatalytic7
activities for H2 production were evaluated under visible light irradiation (λ > 420 nm). Visible8
irradiation was provided by a 500 W xenon lamp with a 420 nm cutoff filter and the average9
visible light intensity was 40.0 mW cm-2. 20 mg of the photocatalyst powder was dispersed in10
an aqueous solution (20 mL) containing triethanolamine (10 vol. %) as a sacrificial electron11
donor. 3 wt. % Pt was loaded on the surface of the photocatalyst sample by the in situ12
photodeposition method using H2PtCl6. The suspension solution was then purged with N2 for13at least 30 min to remove air and then sealed with a rubber septum. The temperature of the14
reaction solution was maintained at room temperature by a flow of cooling water during the15
photocatalytic reaction. The amount of evolved hydrogen was analyzed by a Shimadzu GC-16
2014 gas chromatography equipped with a thermal conductive (TCD) detector and a 5 Å17
molecular sieve column, using N2 as the carrier gas. 18
The photocatalytic activities were further evaluated by the degradation of phenol and19
methylene blue (MB) under visible light irradiation. In each run, 50 mL of MB solution20
(2.0×10−5 M) or phenol solution (2.0 mg L-1) containing 25 mg of as-synthesized photocatalyst21
were placed in a glass beaker. Before irradiation, the suspensions were magnetically stirred in22
the dark for 2 h to ensure equilibrium between the photocatalyst and the model molecules. At23
certain time intervals, 2 mL of the suspensions were taken and centrifuged to remove the24
particles. The concentration of phenol was analyzed using a HPLC with a UV absorbance25
detector operated at 270 nm coupled to a Venusil XBP-C18 column. The concentration of the26
MB was analyzed by recording the absorption intensity at 663 nm using a Hitachi U-3010 UV-27
vis spectrophotometer.28
The photoelectrochemical properties were performed on a CHI 660B electrochemical29
system (Shanghai, China) using a standard three-electrode cell with a working electrode, a30
platinum wire counter electrode, and a standard calomel electrode (SCE) reference electrode.31
0.1 M Na2SO4 was used electrolyte. The working electrodes were prepared as follows: 2 mg of32
as-prepared photocatalyst was suspended in 1 mL of water to produce slurry, which was then33
dip-coated on a 20 mm × 40 mm indium-tin oxide (ITO) glass electrode. Electrodes were34
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exposed in air for 1 day to eliminate water and subsequently heated at 200 °C for 1 day. All1
investigated working electrodes were of similar thickness. The electrochemical impedance2
spectroscopy (EIS) was carried out at the open circuit potential. A sinusoidal ac perturbation of3
5 mV was applied to the electrode over the frequency range 0.05-105 Hz.4
53. RESULTS AND DISCUSSION6
7
Figure 1. Illustration of synthetic strategy. (a) Intercalation of H2SO4 (98 wt %) in the interplanar space of g-8
C3 N4. (b) Intercalated g-C3 N4 was exfoliated into single layer due to the rapid heating effect of H2SO4 (98 wt %)9
mixing with water.10
20 22 24 26 28 30 32 34
Bulk C3N
4
H2SO4 intercalated
I n t e n s i t y / a . u .
2Theta / degree
11
Figure 2. XRD patterns of the bulk g-C3 N4 before and after H2SO4 intercalation.12
The synthetic strategy is illustrated in Figure 1. First, the bulk g-C3 N4 was mixed with13
H2SO4 (98 wt %) and stirred for 8 hours at room temperature to allow the intercalation of14
H2SO4 in the interlayer space of g-C3 N4. The intercalation mechanism is generally similar15
with the widely reported H2SO4 intercalated graphite.37 The intercalation of H2SO4 into bulk16
g-C3 N4 is confirmed by X-ray diffraction (XRD) (Figure 2). It is found that the (002)17
diffraction at around 27.4 o relating to the characteristic interlayer stacking structure is shifted18
to 25.0 o, indicating that the interlayer distance is expanded from 0.325 nm to 0.356 nm. Then19
the mixture was slowly poured into deionized water and sonicated, due to the sonication and20
rapid heating effect when concentrated H2SO4 is mixed with water, the intercalated bulk g-21
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C3 N4 was exfoliated into single layer. The obtained dispersion was then subjected to1
centrifugation to remove any unexfoliated and aggregated g-C3 N4. The exfoliation is found to2
significantly depend on the concentration of sulfuric acid. H2SO4 with lower concentrations3
(75 wt% and 50 wt%) were also studied, however the results show that lower concentration4
H2SO4 failed to exfoliate bulk g-C3 N4 into single layer (Figure S1 and S2 in Supporting5Information). Compared with the reported thermal oxidation “etching” process33, ultrasound6
exfoliation11 or “bottom-up” method36 for the fabrication of g-C3 N4 nanosheets, the chemical7
exfoliation method allows intercalation of H2SO4 in the interlayer space of g-C3 N4, thus8
higher possibility to obtain single layer nanosheet after exfoliation. Moreover, the chemical9
exfoliation is also more cost-efficient than the reported methods mentioned above.10
11
12
13
14
15
16
17
18
19
20
21
22
Figure 3. Typical AFM images (a) and TEM images (b) of the as-prepared Monolayer-C3 N4 nanosheets. The23
tables and curves in the right panel show the height and width information of different nanosheets from the AFM24
images.25
26
Figure 3a shows the typical atomic force microscope (AFM) image of the exfoliated g-27
C3 N4 nanosheets. The lateral size of these sheets is ranging from tens of nanometers to several28
micrometers. The thickness analysis of the nanosheets by AFM reveal an average thickness of29
about 0.4 nm, which is very close to the theoretical thickness of monolayer g-C3 N4 (about30
0.325 nm). Statistical studies of the thickness of single layer g-C3 N4 nanosheets by measuring31
different samples confirm this observation (Figure S3 in the supporting information). Some32
multilayered g-C3 N4 nanosheets with thickness from 1 nm to 4 nm are also observed in the33
AFM studies, which comprise ca. 40% of the sample, indicating the current chemical34
aa
b
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exfoliation can produce g-C3 N4 nanosheets with 60% single layer C3 N4. TEM image (Figure1
3b) illustrates the very transparent feature of the nanosheets, indicating the ultrathin thickness2
of the nanosheets. The darker part in the TEM image can be attributed to the overlap of3
several g-C3 N4 nanosheets or a multilayer nanosheet. The bulk g-C3 N4 before exfoliation4
shows a thickness of more than 10 nm (Figure S4 and S5), indicating the effectiveness of the5current chemical exfoliation method. The EDX studies (Figure S6) confirmed the elemental6
composition of the nanosheets, which are shown to be composed of C and N elements, while7
the Cu detected can be attributed to the copper substrate for TEM investigation. Notably,8
oxygen is not detected in the element analysis of the nanosheets, implying the g-C3 N4 is not9
oxidized by concentrated H2SO4 employed for exfoliation.10
11
12
1314
15
16
17
18
19
20
21
22
23
24
25
Figure 4. a). XRD patterns, b). FTIR spectra, c). Enlarged FTIR spectra of the bulk g-C3 N4 26
and Monolayer-C3 N4.27
28
The structure, composition and chemical states of the Monolayer-C3 N4 is further29
investigated by XRD, X-ray photoelectron spectroscopy (XPS), Fourier transform infrared30
(FTIR) etc. In the XRD patterns (Figure 4a), the (002) diffraction at around 27.4 o relates to31
the characteristic interlayer stacking structure, while the (100) diffraction at 13.0 o indicates32
the interplanar structural packing. It has been reported in some other monolayer structures that33
due to the formation of agglomerates and crumples of the monolayer nanosheets by van der34
Waals force during preparing sample for XRD measurment, the XRD pattern of the35
10 20 30 40 50 60 70
Bulk g-C3N
4
I n t e n s i t y / a . u .
2 Theta / degree
Monolayer-C3N
4
a)
4000 3000 2000 1000
Monolayer-C3N
4
Bulk g-C3N
4
I n t e n s i t y / a . u .
Wavenumber / cm-1
C-N triazine
b)
1800 1600 1400 1200 1000 800
12531320
14051572
Monolayer-C3N
4
Bulk g-C3N
4
I n t e n s i t y /
a . u .
Wavenumber / cm-1
1632 807
c)
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monolayer nanosheets could resemble that of bulk form.38-40 However, it is observed that the1
intensity of (002) diffraction related to the interlayer stacking is significantly weakened after2
exfoliation as expected. The multilayer components in the sample also contribute to the3
observed (002) diffraction.4
The strong FTIR absorption bands of Monolayer-C3 N4 in Figure 4b and 4c further revealed5a typical molecular structure of graphitic carbon nitride. The absorption band near 1572 and6
1632 cm-1 are attributed to C=N stretching, while the three bands at 1253, 1320 and 1425 cm-1 7
correspond to aromatic C-N stretching. The peak at 807 cm -1 belongs to triazine ring mode,8
which correspond to condensed CN heterocycles. The broad band at 3000 – 3500 cm-1 9
corresponds to uncondensed terminal amino groups (-NH2 or =NH groups). The FTIR results10
are in fairly good accordance with the reports of g-C3 N4 material prepared by11
polycondensation and polymerization reactions.25,26 The Raman spectra are also invesitigated12
to confirm the molecular structure of g-C3 N4 (Figure S7 in supporting information). In the13Raman spectra for both bulk and monolayer g-C3 N4, there are two characteristic bands related14
to the disordered D (around 1300 cm-1) and graphitic G (around 1500 cm-1) bands, indicating15
the formation of graphitic structure. The Raman bands at 600 – 800 cm-1 can be attributed to16
the in-plane rotation of sixfold rings in a graphitic carbon nitride layer.41 17
18
19
20
21
22
23
24
25
Figure 5 .
a) C1s XPS spectra; b) N1s XPS spectra of the bulk g-C3 N4 and Manolayer-C3 N4 nanosheets.2627
The chemical states of the Monolayer-C3 N4 and the bulk g-C3 N4 were studied by XPS28
(Figure 5). The C1s spectra show two peaks locating at about 284.6 eV and 288.0 eV. The29
288.0 eV peak is further deconvoluted into two Gaussian-Lorenzian peaks. The main30
contribution peak at 287.9 eV is attibuted to the sp2 hybridized carbon bonded to N inside the31
triazine rings, while the peak at 288.6 is assigned to the sp2 hybridized carbon in the triazine32
296 292 288 284
a)
I n t e n s i t y / a . u .
Binding energy/eV
284.6
C 1s
288.0
Monolayer-C3N
4
bulk g-C3N
4
408 404 400 396
b)
I n t e n s i t y / a . u .
Binding energy/eV
398.6
N 1s
Monolayer-C3N
4
bulk g-C3N
4
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ring bonded to the –NH2 group. 35 The peak at 284.6 eV is typically ascribed to sp2 C=C1
bonds. The peak of 398.6 eV in the N1s spectra can also be deconvoluted into two Gaussian-2
Lorenzian peaks. The dominant peak at 398.7 eV corresponds to the sp2-bonded N involved in3
the triazine rings (C-N=C), while the peak at 399.7 eV is attributed to the bridging N atomes4
in N-(C)3 or N bonded with hydrogen.35
56
7
8
9
10
11
12
1314
Figure 6. a). DRS spectra and b). PL spectra of the bulk g-C3 N4 and Monolayer-C3 N4.15
16
The optical properties have been investigated by UV-Vis diffuse reflectance spectra (DRS)17
and photoluminenscence (PL) measurements (Figure 6a and 6b). It is found that the18
absorption edge of Monolayer-C3 N4 shows a remarkable blue shift from 470 to 425 nm,19
corresponding to an increase in the band gap from 2.64 eV to 2.92 eV compared with that of20
bulk g-C3 N4. This blue shift performance can be presumably ascribed to the decrease of21conjugation length and the strong quantum confinement effect due to the single layer structure22
of g-C3 N4 nanosheets. The PL spectra demonstrate that under photoexcitation at 318 nm, the23
emission peak of the bulk g-C3 N4 locates at around 464 nm, while the position of the emission24
peak is blue shifted to to 438nm in the case of Monolayer-C3 N4. The blue shift of the25
emission peak by 26 nm is in well agreement with the larger bandgap by 0.28 eV of26
Monolayer-C3 N4 nanosheets.27
The photocatalytic H2 production from water in the presence of the bulk g-C3 N4 or28
Monolayer-C3 N4 were studied under visible-light irradiation (λ > 420 nm), as shown in Figure297a. 3 wt.% Pt was loaded on the surface of the photocatalyst samples by the in situ30
photodeposition method from H2PtCl6 solution. It is found that Monolayer-C3 N4 shows a31
significant improvement over the reference bulk g-C3 N4. The rate of H2 evolution on32
Monolayer-C3 N4 reaches 230 µmolg-1h-1, which is about 2.6 times the rate of the bulk g-C 3 N4 33
(90 µmolg-1h-1).34
35
350 400 450 500 550 600
Monolayer-C3N
4
b)
I n t e n s i t y / a . u .
Wavelength / nm
Bulk g-C
3N
4
200 300 400 500 600 700 800
Monolayer-C3N
4
a)
Bulk g-C3N
4
A b s .
Wavelength / nm
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1
2
3
4
56
7
Figure 7. a) Photocatalytic H2 production on bulk-C3 N4 and monolayer-C3 N4. b) Photocatalytic decomposition of8
phenol under visible light irradiation (λ > 420 nm). c) Stability measurement.9
10
The superiority of Monolayer-C3 N4 for photocatalysis application is further confirmed by11
the photodegradation of phenol under visible light irradiation. A first-order linear relationship12
was revealed by the plots of ln(C /C 0) versus irradiation time (Figure 7b). The determined13reaction-rate constants, k , were 0.0633 and 0.2589 h-1, respectively, for bulk g-C3 N4 and14
Monolayer-C3 N4. The photocatalytic decomposition rate over the monolayer nanosheet was15
more than four times as fast as the bulk g-C3 N4. The Monolayer-C3 N4 also shows a more than16
threefold enhancement in the photocatalytic degradation of methylene blue under visible light17
irradiation, as shown in Figure S8 in supporting information. The stability of the Monolayer-18
C3 N4 as a photocatalyst is also evaluated under visible light irradiation (Figure 7c). It is found19
that the photocatalytic activity only very slightly decreased after five successive cycles of20
photocatalysis degradation tests, indicating the Monolayer-C3 N4 is fairly stable under the21studied conditions.22
It is well known that the photocatalytic activity is greatly related to surface area, charge23
transporting, light absorption and so on. The properties and photocatalytic activity of the24
single atomic layer g-C3 N4 is different with multilayer g-C3 N4 mainly in three aspects: i) The25
electron and hole mobility in the monolayer is significantly greater than that in the multilayer,26
which has been proved in the study of graphene. ii) The surface area of monolayer is bigger27
than that of multilayer, which is also very important for a photocatalyst. iii) The light28
absorption is different due to the quantum size effect, the absorption edge is expected to be29more blue-shifted in the case of monolayer, which could affect the photocatalytic activity by30
shifting the position of conduction and valence bands of g-C3 N4. Since the Monolayer-C3 N4 31
was obtained from bulk g-C3 N4 by chemical exfoliation, the crystallinity should be similar in32
both materials, which is also confirmed by the XRD patterns. Therefore, the greatly enhanced33
photocatalytic activity of Monolayer-C3 N4 than the bulk g-C3 N4 in both H2 production and34
phenol degradation can be attributed to several reasons: First, the increased surface area, the35
0
50
100
150
200
250
300
Monolayer-C3N
4
H 2
e v
o l v e d / u m o l g - 1 h - 1
Sample
Bulk g-C3N
4
a)
0 1 2 3 4-1.2
-0.9
-0.6
-0.3
0.0
Blank
Bulk g-C3N4
Monolayer-C3N4
l n ( C / C
o )
Time / h
b)
0.30
0.45
0.60
0.75
0.90
1.05
c)
C / C
0
Time
1st 3rd 5th2nd 4th
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0 30 60 90 120
0
4
8
12
16
20
C u r r e n t / µ A
Time/s
bulk g-C3N
4
of f
Light on
Monolayer-C3N
4
a)
0 200 400 600
0
1k
2k (iv)
(iii)(ii)
b)
- Z " /
o h m
Z'/ohm
(i)
measured surface area of Monolayer-C3 N4 is 205.8 m2/g, which is almost 50 times larger than1
that of bulk-C3 N4 (4.3 m2/g), suggesting more active sites in the Monolayer-C3 N4 for2
photocatalytic reaction. Secondly, the improved photogenerated charge carriers transportation3
and separation due to the monolayer nanosheet structure. The monolayer nanosheet structure4
can significantly reduce the distance for the charge carriers to transfer from the place5generated to the solid-liquid interface due to the ultrathin structure. Finally, the negatively6
shifted conduction band due to the quantum size effect can increase the activity of7
photogenerated electrons.8
The improved charge carrier separation in Monolayer-C3 N4 is investigated by the9
photocurrent and electrochemical impedance spectroscopy (EIS) measurements (Figure 9).10
The potential of the electrodes against a Pt counter electrode was set at 0.0 V vs saturated11
calomel electrode (SCE). As shown in Figure 9a, a fast and uniform photocurrent response12
was observed for each switch-on and switch-off event in both bulk g-C3 N4 and Monolayer-13C3 N4 electrodes. This photoresponsive phenomenon was entirely reversible. The photocurrent14
of the Monolayer-C3 N4 is about four times as high as that of the bulk g-C3 N4 electrode, which15
indicates that the separation efficiency of photoinduced electrons and holes is significantly16
improved in the Monolayer-C3 N4 nanosheet.17
18
19
20
21
22
23
24
25
26
Figure 8. a) Photocurrent response under chopped illumination. b) The EIS response of bulk g-C 3 N4 ((i) dark,27
(ii) under visible light irradiation) and Monolayer-C3 N4 electrodes ((iii) dark, (iv) under visible light irradiation).28
29The effect of monolayer nanosheet structure on the kinetics of interfacial charge transfer30
was confirmed by EIS. Figure 8b shows the EIS Nyquist plots of the bulk g-C3 N4 and31
Monolayer-C3 N4 electrodes in dark or under visible light irradiation. The Nyquist plot was32
also fitted to the equivalent Randle circuit (Figure 8b, inset), where Rs is the electrolyte33
solution resistance, CPE is the constant phase element for the electrode and electrolyte34
interface, and Rct is the interfacial charge transfer resistance across the electrode/electrolyte. A35
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12
lower value of Rct suggests more efficient charge transfer across the electrode/electrolyte1
interface, reducing the possibility of charge recombination and thus enhancing the2
photocurrent response.42 The fitted Rct values for the bulk g-C3 N4 and Monolayer-C3 N4 under3
visible light irradiation are 2570.7 and 980.2 Ω, respectively, indicating that the Monolayer-4
C3 N4 possesses more efficient charge transfer than that of the bulk g-C3 N4. One possible5reason for the more efficient charge transport in nanosheets than the bulk g-C3 N4 could be the6
electron-phonon interaction in the material. The lattice photons are different in the low7
dimension material, which could affect the conductivity of the material. The efficient charge8
mobility has been observed in low dimension materials, one typical example is graphene,9
which shows very high electron mobility.2 However, the exact mechanism is still not very10
clear.11
12
4.
CONCLUSION13
In summary, we have successfully obtained single atomic layer g-C3 N4 nanosheets by a14
simple chemical exfoliation of the bulk g-C3 N4. Although there are still 40% of multilayer15
nanosheets existing in the product, it is for the first time single layer g-C3 N4 nanosheets are16
produced. Compared with the bulk g-C3 N4, single layer g-C3 N4 nanosheets show much larger17
surface area and great superiority in photogenerated charge carriers transport. Accordingly, the18
photocatalytic activity and photocurrent of single layer g-C3 N4 nanosheets are significantly19
enhanced. A threefold enhancement in photocatalytic H2 production is observed in the single20
layer nanosheet as photocatalyst. Experiments trying to seperate the single layer nanosheets21
from the multilayer ones are undergway. The single layer g-C3 N4 shows great potential in the22
application both in environment purification and solar energy conversion.23
24
ASSOCIATED CONTENT25
Supporting Information.26
This material is available free of charge via the Internet.27
AUTHOR INFORMATION28
Corresponding Author29
E-mail: [email protected]
E-mail: [email protected]
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13
Present address of Liwu Zhang: Cavendish Laboratory, University of Cambridge, JJ1
Thomson Ave, Cambridge, CB3 0HE, UK2
Author Contributions3
† These authors have contributed equally to this work.4
5
ACKNOWLEDGMENT6
The project was supported by the National Basic Research Program of China (973)7
(2013CB632403), National High Technology Research and Development Program of China8
(863) (2012AA062701), Special Project on Innovative Method from the Ministry of Science9
and Technology of China (No.2009IM030500), and Atmospheric Environment Monitoring &10Pollution Control Program of Jiangsu Province (AEMPC201103). 11
12
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By a simple chemical exfoliation method, for the first time the single atomic layer g-C3 N4
nanosheets are prepared.
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