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resonance peak. In addition, the use of the NaBH4 reducing agent allowed for the rapid formation of AgNPs (~5 min) at room temperature, and no significant change of the plasmonic band was observed as a function of time shown in Supplementary Figure S1. As such, the synthesis of the Ag/GO composite was carried out under the same reaction conditions. Comparing to the absorption peak of bPoalryemeArsg2N02P0,s1,2t,h2e44A1 g/GO composite had a relatively broad absorption band between 330 nm and5 o5f0102 nm. This result was expected because of possibly localized agglomeration of randomly deposited AgNPs onto the GO surface whereas the agglomeration is not typically observed in small and monodispersed metal NPs in water [41]. In addition, the particle size of AgNPs (11.7 ± 7.1 nm) of the composite was unexpectedly increased up to 2.5 times compared to that of the bare AgNPs, leading 3. Results and Discussion 3.1. Structure and Morphology of Synthesized Nanoparticles and Nanofiber Membranes to the change of the plasmonic bandwidth and position. Figure 1 shows the optical property of synthesized GO, Ag nanoparticle (AgNP), and Ag/GO The synthesized GO possessed two different absorption peaks at 237 nm for π-π* transition composite. The absorption spectra of the AgNP colloidal solution indicated the conventional peak mode of aromatic C-C bond and at 300 nm for n-π* transition mode of C=O bond, respectively [40,42]. at ~390 nm associated with the formation of small and spherical AgNPs [38,40]. The particle size of Unlike the GO, such characteristic peaks were not observed for the Ag/GO composite in an AgNPs was estimated to 4.7 ± 2.5 nm (Figure 1), which was well-matched with its plasmonic resonance absorption spectrum, possibly due to their chemical structure change during the synthesis process peak. In addition, the use of the NaBH reducing agent allowed for the rapid formation of AgNPs (e.g., GO to rGO) [43]. Nevertheless, the particle size was still relatively smaller, and the composite 4 (~5 min) at room temperature, and no significant change of the plasmonic band was observed as a showed a better dispersion under our experimental conditions than those of the thermal-driven function of time shown in Supplementary Figure S1. As such, the synthesis of the Ag/GO composite method (Supplementary Figure S2). It was anticipated that the relatively high dispersion was carried out under the same reaction conditions. Comparing to the absorption peak of bare AgNPs, characteristics of the prepared Ag/GO composites were contributed from the use of NaBH4. In other the Ag/GO composite had a relatively broad absorption band between 330 nm and 500 nm. This result words, NaBH4 tends to have excellent reducing power for -C=O groups, but relatively low for -COOH was expected because of possibly localized agglomeration of randomly deposited AgNPs onto the GO and -OH species [43]. To understand the tendency of the reducing behavior of NaBH4, the prepared surface whereas the agglomeration is not typically observed in small and monodispersed metal NPs in NPs were examined via FT-IR (Supplementary Figure S3). The Ag/GO exhibited several strong water [41]. In addition, the par−t1icle size of AgNP−1s (11.7 ± 7.1 nm) −o1f the composite was unexpectedly vibrational peaks at ~ 3300 cm (-OH), 1620 cm (-C=C), 1050 cm (-C-O-C), but the relatively weak increasedupto2.5timescomparedtothatoft−h1ebareAgNPs,leadingtothechangeoftheplasmonic intensityof-C=Ovibrationalpeakat1710cm .Therefore,theremaining-OHand/or-COOHgroup bandwidth and position. in the Ag/GO composite could enable their desire dispersity in an organic solvent. Figure 1. UV-vis spectra of synthesized nanoparticles and their presentative STEM images. Figure 1. UV-vis spectra of synthesized nanoparticles and their presentative STEM images. FTihgeusryen2thsehsoizweds tGhOe dpiogsisteaslspedhotwtooadnidffeSrEenMt aibmsoagrpetsionf pbeaarke-sPaAt N23,7GnOm-PfoArNπ,-πa*ntdraAnsgi/tGioOn -mPAodNe noaf naorofimbeartimc Cem–Cbrbaonnesd. aTnhde actol3o0r0onfmGOforand-π*Atgr/aGnOsitimonodmifoiede noafnCo=fiOberbsonchda,nrgeespdefcrtoivmelyw[h4i0te,42to]. uUnilfiokremthlye GdaOr,ksugcrahychaacraocstsertihseticmpeemakbsrawner.eTnhoet onbostearbvleddfeofrecthtsewAegr/eGOnoctoombpseorsvitedininanboatbhsodripgtitoanl pspheocttorsuman,dpoSsEsMiblyimdaugeetso, wthheicrhchiemmpilcieasl stthrautctuhreehcyhdanrogpehdiluicringattuhresoyfntPhAesNiscporuolcdesasll(oew.g.,foGrOthtoe sruGcOce)s[s4f3u]l. iNnceovreprotrhaetlieosns,othfethpearstyicnlethseisziezewdansasntiollfilrlelrastivinetloy sthmealnlearn,oafnibdertshevciaomelpeoctsriotespsihnonwinegd. Ha obwetetevrerd,istphersaiovneraugnededriaomuretexrpoerfiminednitvaildcuoanldnitainoonfsibtehransttrhaonsdesoafntdheitshedrmistarli-bdurtiivoen smheotwhoed (Supplementary Figure S2). It was anticipated that the relatively high dispersion characteristics of the prepared Ag/GO composites were contributed from the use of NaBH4. In other words, NaBH4 tends to have excellent reducing power for –C=O groups, but relatively low for –COOH and –OH species [43]. To understand the tendency of the reducing behavior of NaBH4, the prepared NPs were examined via FT-IR (Supplementary Figure S3). The Ag/GO exhibited several strong vibrational peaks at ~3300 cm−1 (–OH), 1620 cm−1 (–C=C), 1050 cm−1 (–C–O–C), but the relatively weak intensity of –C=O vibrational peak at 1710 cm−1. Therefore, the remaining –OH and/or –COOH group in the Ag/GO composite could enable their desire dispersity in an organic solvent. Figure 2 shows the digital photo and SEM images of bare-PAN, GO-PAN, and Ag/GO-PAN nanofiber membranes. The color of GO and Ag/GO modified nanofibers changed from white to uniformly dark gray across the membrane. The notable defects were not observed in both digital photos and SEM images, which implies that the hydrophilic nature of PAN could allow for the successfulPDF Image | Polyacrylonitrile Nanofiber Membrane Water Purification
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