Preparation of the Water-Soluble Pyrene-Containing Fluorescent Polymer by One-Pot Method

A new water-soluble pyrene-containing fluorescent polymer, 1-{31-S-[poly(acryloyl ethylene diamine hydrochloride)-21-methyl propionic acid]}propionyloxy hexyloxy pyrene (P3) with defined structure, was designed and synthesized using the click reaction between thiol and a carbon-carbon double bond. The intermediate products P1 (S-1-dodecyl-S1-[poly(N-Boc-acryloyl ethylene diamine)-21-methyl propionic acid]trithiocarbonate) and AHP (1-(acryloyloxy hexyloxy)pyrene) were prepared via reversible addition fragmentation chain transfer (RAFT) polymerization and Williamson synthesis, respectively. Conjugating AHP with P1, P2 (1-{31-S-[poly(N-butoxycarbonyl-acryloyl ethylene diamine)-2”-methyl propionic acid]} propionyloxy hexyloxy pyrene) was synthesized, adopting both the reduction reaction of a trithioester bond of P1 to thiol and the click reaction between thiol and the carbon-carbon double bond of AHP simultaneously. P3 was obtained by the deprotection of the resulting Boc-protected polymer (P2) with aqueous HCl. The experiment results showed that P2 exhibited a bright blue-violet emission band at approximately 387–429 nm. After deprotection, P3 displayed good solubility in water and not only exhibited a blue-violet fluorescence emission band at approximately 387–429 nm in aqueous solution but also had the similar photoluminescent spectra to those of AHP and P2 in dichloromethane. The fluorescence quantum yields of P2 in dilute tetrahydrofuran and P3 in a dilute aqueous solution were 0.44 and 0.39, respectively. This experiment provided a novel insight into the study of water-soluble fluorescent polymers.


Introduction
Water-soluble fluorescent polymers have drawn much attention in recent years given their successful utility in distinguishing different proteins [1] and isozymes [2], as an effective and sensitive probe for further bio-applications differentiating tumorous and malignant cells [3,4], ranging from cytotoxicity studies to pharmacodiagnosis.Water is usually regarded as an ideal solvent in terms of its environmental impact and low cost.Water solubility is a prerequisite of those fluorescent polymers for applications in biological environments [5,6], since as long as the fluorescent polymers enjoy water solubility they can be uniformly dispersed in the aqueous medium of the system under characterization.The water-soluble fluorescent polymers in the field of applied biotechnology research exhibited unique advantages.To tackle this issue, several designed strategies to prepare water-soluble fluorescent polymers, mainly including copolymerization and chemical modification, have been well established and applied to the development of various excellent fluorescent polymers.Co-polymerization is a family of methods that fluorochrome copolymerizes directly with a water-soluble monomer.It has been demonstrated to be a simple, effective strategy to obtain a water-soluble copolymer, but it generally enjoys several limitations due to low molecular weight, poor water-solubility and low fluorescence intensity.Chemical modification method that was also the designed strategy in this contribution, which was chemically bonded to the fluorescent dye on the polymer chain or born hydrophilic groups to fluorescent polymers.Water-soluble poly(acrylic acid) has been covalently labeled with a fluorescent hydrophobic chromophore, naphthalene (Np), randomly attached onto the polymer backbone with an amount of 3 mol % [7,8].Curtis W. Frank and co-workers [9,10] reported that pyrene end-labeled poly(ethy1ene glycol) (PEG) was synthesized by direct esterification between PEG and l-pyrenebutyric acid (PBA).As an important and widespread tool in biomedical research and disease diagnosis [4,11], water-soluble fluorescent polymers with suitable molecular weight may be used for fluorescent detection of protein and image in the cells [12].
In order to obtain the polymer with controlled and narrow distribution of molecular weight, living radical polymerization is a conventional polymerization method.Reversible addition-fragmentation chain transfer (RAFT) polymerization is one of the most popular living radical polymerization methods for the production of well-defined polymers.After polymerization, the RAFT agent end-groups can easily be converted into thiol, opening manifold opportunities for thiol modification reactions [13].The functional groups are effectively introduced into the polymer terminal groups by these reactions, such as thiol-ene [13], thiol-epoxy reaction [14], and so on.Such reaction of thiol and epoxy, alkenes, and alkynes is one kind of click-chemistry reactions.
The past decade has seen the emergence of "click chemistry"; the term "click chemistry" defines a series of chemical reactions respecting several criteria announced in 2001 by Sharpless and co-workers [15].Click chemistry is addressing a set of powerful, highly-reliable, and selective reactions for the rapid synthesis of useful new compounds and combinatorial libraries [16].Click chemistry possesses many significant advantages, such as a certain modularity [17], excellent selectivity, high purity, high efficiency, a wide scope of applications, only inoffensive byproducts, stereospecific, mild reaction conditions, and simple product isolation, etc. [15,[18][19][20].Since S-H bonds are relatively weak, thiol groups are subject to rapid oxidation during purification and storage and, thereby, result in the low conversion in the following click reaction.To circumvent this limitation, the synthesis of thiol groups and click reaction were simultaneously performed in one system (one-pot method).Highly efficient reactions of thiols with the reactive carbon-carbon double bond [20] (thiol-ene click-chemistry reaction) is one of the most mature click-chemistry reactions, in which thiol can rapidly react with the terminal C=C double bond to form a C-S bond under mild conditions, which has been applied in diverse preparation areas, such as functional polymer nanoparticles [21] and beads [22], amphipathic well-defined polymers [23], desired dendritic macromolecules [24], nanocapsules [25], substrate surface modification [20], polymer functionalization [26], and so forth.
The pyrene moiety is one of the most useful fluorophores due to its striking efficiency among excimer formation and subsequent changes in its emission properties [27].Pyrene can emit blue fluorescence with a high fluorescence quantum yield (0.65, acetonitrile) and a long fluorescence lifetime (440 ns, a cyclohexane solution, 290 ns, ethanol) [28] responsible to the unique polycyclic aromatic hydrocarbon-conjugated structure.Therefore, pyrene is an important signaling unit, which is widely used for various analytes [29][30][31].However, pyrene, or other conventional fluorescent molecules with alternating single and double bond conjugated structures, are faced with the thorny aggregation problem leading to emission spectrum red-shift and fluorescence quenching.There were several projects to avoid this phenomenon by introducing large steric groups at reactive sites of pyrene to avoid the accumulation of the conjugated plane [32,33].However, most of the works were studies of the responses and characteristics when pyrene-containing polymers dissolved in organic solvent.For example, the fluorescence quantum yield and infrared absorption spectrum of pyrene derivatives in Robert M. Edkins 1 experiment showed the dependency of the solvent [34].This article will discuss how the pyrenyl functional end group is introduced into a water-soluble polymer, which is applied to the light emitting properties of pyrene in aqueous solution.
In this study, S-1-dodecyl-S 1 -[poly(N-Boc-acryloyl ethylene diamine)-2 1 -methyl propionic acid]trithiocarbonate (P1) was prepared via RAFT polymerization using N-Boc-acryloyl ethylene diamine as a monomer.Boc-protected fluorescent polymer (P2) with regular structure was synthesized using the click reaction of thiol (the reduction reaction production of trithioester bond of P1) and the carbon-carbon double bond of AHP.Water-soluble pyrene-containing fluorescent polymer (P3) was obtained by the deprotection of the resulting Boc-protected polymer (P2).P3 was characterized and measured by Fourier transform infrared spectrophotometry, nuclear magnetic resonance spectrometry, UV-Visible (UV-VIS) spectrophotometry, and fluorescence spectrophotometry, respectively, and the fluorescence quantum yield of P3 in aqueous solution was obtained.The fluorescent polymer P3 had good water solubility and also showed good optical performance.

Instruments and Measurements
Fourier transform infrared (FTIR) spectra were recorded on a Varian 640-IR FTIR spectrophotometer (Varian, Salt Lake City, UT, USA) using KBr pellets.Nuclear magnetic resonance spectroscopy (NMR) was performed on a Bruker AVANCE III 600 MHz digital NMR spectrometer (Bruker, Zurich, Switzerland) using CDCl 3 and D 2 O as solvent at room temperature.Chemical shifts were measured using tetramethylsilane (TMS) as an internal standard.The number average molecular weight (M n ), weight average molecular weight (M w ), and polydispersity index (PDI, M w /M n ) of polymers were determined by a Waters 515 gel permeation chromatograph (GPC) (Waters, Milford, MA, USA).Two chromatographic columns (Agilent Technologies, PLgel 5 µm 500 Å, PLgel 5 µm Mixed-C) were used in series.THF was used as eluent at a flow rate of 1.0 mL/min at 30 ˝C.Universal calibration was done using seven standard polystyrene samples (1600, 3790, 6000, 11,500, 44,700, 105,800, and 903,000).High-resolution atmospheric pressure-chemical ionization Fourier-transform ion cyclotron resonance mass-spectroscopy (HR-APCI-FT-ICR-MS) was performed on a Bruker Daltonik apex-Ultra 7.0 T Fourier-transform ion cyclotron resonance mass spectrometer (Bruker, Bremen, Germany) equipped with an atmospheric pressure chemical ionization source operating in the nebulizer-assisted electrospray mode.The sample was dissolved in methanol (high-performance liquid chromatography grade) solvent.The sample molecule was ionized with H + ions.UV-VIS spectra were recorded on a UV-2550 spectrophotometer (Shimadzu, Kyoto, Japan).Photoluminescent (PL) spectra were recorded on a RF-5301PC fluorescence spectrophotometer (Shimadzu, Kyoto, Japan).

Synthesis of N-Butoxycarbonyl-Ethylene Diamine (N-Boc-EDA)
N-Boc-EDA was synthesized according to published literature [35].Ethylenediamine (30 mL, 448 mmol) and THF (150 mL) were placed into a 500 mL round-bottom flask with moderate stirring at ´5 to 0 ˝C.Then, the THF (100 mL) solution of Boc 2 O (20 mL, 87.06 mmol) was added dropwise into the cold mixture.After the addition, the reaction was continued for 24 h at room temperature, and a white suspension was obtained.The white suspension was filtered and the filtrate was rotary evaporated to give a pale yellow oily liquid.Then the liquid was washed extensively with saturated NaCl aqueous solution and filtered.The filtrate was extracted with ethyl acetate three times, and the combined organic layer was dried over anhydrous Na 2 SO 4 overnight and filtered.Solvents were removed by rotary evaporation to give N-Boc-EDA as a pale yellow oily liquid 0.11 g (yield 73%). 1 H NMR (600 MHz, D 2 O) δ (ppm): 3.02 (t, J = 6.0 Hz, 2H), 2.58 (t, J = 6.0 Hz, 2H), 1.34 (s, 9H).

Synthesis of S-1-Dodecyl
S-1-dodecyl-S 1 -(α,α 1 -dimethyl-α"-acetic acid)trithocarbonate (RAFT agent) was synthesized according to published literature [36].P1 was synthesized according to procedures in the literature [37].The reaction mechanism of P1 was shown in Scheme 1. N-Boc-AEDA (6.000 g, 28.08 mmol) and solvent THF (30 mL) were mixed in a 100 mL eggplant-shaped flask with magnetic stirring and dissolved completely.RAFT agent (0.600 g, 1.64 mmol) and AIBN (0.048 g, 0.29 mmol) were added.The mixture was refluxed for 5 h under a nitrogen atmosphere.THF was removed by rotary evaporation to give a pale yellow solid.It was washed with water several times, dried in a vacuum oven to afford P1 as a yellow solid (6.402 g, yield 97%).
Polymers 2015, 7, page-page 4 at −5 to 0 °C.Then, the THF (100 mL) solution of Boc2O (20 mL, 87.06 mmol) was added dropwise into the cold mixture.After the addition, the reaction was continued for 24 h at room temperature, and a white suspension was obtained.The white suspension was filtered and the filtrate was rotary evaporated to give a pale yellow oily liquid.Then the liquid was washed extensively with saturated NaCl aqueous solution and filtered.The filtrate was extracted with ethyl acetate three times, and the combined organic layer was dried over anhydrous Na2SO4 overnight and filtered.Solvents were removed by rotary evaporation to give N-Boc-EDA as a pale yellow oily liquid 0.11 g (yield 73%). 1 H NMR (600 MHz, D2O) δ (ppm): 3.02 (t, J = 6.0 Hz, 2H), 2.58 (t, J = 6.0 Hz, 2H), 1.34 (s, 9H).

Synthesis of 1-(Acryloyloxy Hexyloxy)pyrene (AHP)
The reaction mechanism of AHP was shown in Scheme 1. HP (0.65 g, 3 mmol), BHA (0.70 g, 3 mmol), potassium carbonate (1.38 g, 10 mmol), a small amount of catalyst 18-crown-6, and solvent acetone (20 mL) were added to a 50 mL single-neck round-bottom flask equipped with a spherical condenser.The mixture was heated at reflux and magnetically stirred throughout, overnight.Potassium carbonate was removed by suction filtration, and acetone was removed by rotary evaporation to give a white powder displaying blue-green under an ultraviolet lamp.The white powder was chromatographically purified on silica gel eluting with dichloromethane: petroleum ether (1:1, V:V) as eluent to collect the third ribbon (showing a blue fluorescence).The eluent was evaporated to dryness and the residue was dried until constant weight in a vacuum oven to give AHP as a white solid (0.374 g, 33%).Figure 1   Scheme 1.The reaction routes of BHA, AHP, P1-P3.

Synthesis of 6-Bromohexyl Acrylate (BHA)
The reaction mechanism of BHA was shown in Scheme 1. BHA was synthesized according to procedures in the literature [37].

Synthesis of 1-(Acryloyloxy Hexyloxy)pyrene (AHP)
The reaction mechanism of AHP was shown in Scheme 1. HP (0.65 g, 3 mmol), BHA (0.70 g, 3 mmol), potassium carbonate (1.38 g, 10 mmol), a small amount of catalyst 18-crown-6, and solvent acetone (20 mL) were added to a 50 mL single-neck round-bottom flask equipped with a spherical condenser.The mixture was heated at reflux and magnetically stirred throughout, overnight.Potassium carbonate was removed by suction filtration, and acetone was removed by rotary evaporation to give a white powder displaying blue-green under an ultraviolet lamp.The white powder was chromatographically purified on silica gel eluting with dichloromethane: petroleum ether (1:1, V:V) as eluent to collect the third ribbon (showing a blue fluorescence).The eluent was evaporated to dryness and the residue was dried until constant weight in a vacuum oven to give AHP as a white solid (0.374 g, 33%).Figure 1

Synthesis of 1-{3′-S-[poly(N-Butoxycarbonyl-Acryloyl Ethylene Diamine)-2″-Methyl Propionic acid]}propionyloxy Hexyloxy Pyrene (P2) and 1-{3′-S-[poly(Acryloyl Ethylene Diamine Hydrochloride)-2′-Methyl Propionic acid]}propionyloxy Hexyloxy Pyrene (P3)
The reaction mechanism of P2 and P3 was shown in Scheme 1. P1 (200.0 mg, 0.077mmol), NaBH4 (3.8 mg, 0.1 mmol), AHP (34.0 mg, 0.09 mmol), TEA (10 μL, 0.072 mmol), and solvent THF (2 mL) were added to a 5 mL eggplant-shaped flask.Then, the system was degassed for at least three cycles by pulling a vacuum and filling with nitrogen gas under magnetic stirring in an ice bath.The mixture was stirred at room temperature in a nitrogen atmosphere for 48 h.After removal of the solvent, a pale yellow solid was obtained and chromatographically purified on silica gel eluting with dichloromethane to remove the first two ribbons which were the excess AHP and the reaction byproducts.Then methanol was used as eluent to give P2 as a wheat-colored solid (0.202g, 96%).P2 (100 mg) was dissolved in 10 mL of THF, and then HCl gas was passed through the solution for the purpose of deprotection of the resulting Boc-protected polymer (P2) until an amount of precipitate formed.The formed precipitate was filtered and washed with THF, and dried in a vacuum oven to afford the desired water-soluble fluorescent polymer P3 as a pale brown solid (71.5 mg, 95%).

Synthesis of 1-{3′-S-[poly(N-Butoxycarbonyl-Acryloyl Ethylene Diamine)-2″-Methyl Propionic acid]}propionyloxy Hexyloxy Pyrene (P2) and 1-{3′-S-[poly(Acryloyl Ethylene Diamine Hydrochloride)-2′-Methyl Propionic acid]}propionyloxy Hexyloxy Pyrene (P3)
The reaction mechanism of P2 and P3 was shown in Scheme 1. P1 (200.0 mg, 0.077mmol), NaBH4 (3.8 mg, 0.1 mmol), AHP (34.0 mg, 0.09 mmol), TEA (10 μL, 0.072 mmol), and solvent THF (2 mL) were added to a 5 mL eggplant-shaped flask.Then, the system was degassed for at least three cycles by pulling a vacuum and filling with nitrogen gas under magnetic stirring in an ice bath.The mixture was stirred at room temperature in a nitrogen atmosphere for 48 h.After removal of the solvent, a pale yellow solid was obtained and chromatographically purified on silica gel eluting with dichloromethane to remove the first two ribbons which were the excess AHP and the reaction byproducts.Then methanol was used as eluent to give P2 as a wheat-colored solid (0.202g, 96%).P2 (100 mg) was dissolved in 10 mL of THF, and then HCl gas was passed through the solution for the purpose of deprotection of the resulting Boc-protected polymer (P2) until an amount of precipitate formed.The formed precipitate was filtered and washed with THF, and dried in a vacuum oven to afford the desired water-soluble fluorescent polymer P3 as a pale brown solid (71.5 mg, 95%).

Synthesis of 1-{3 1 -S-[poly(N-Butoxycarbonyl-Acryloyl Ethylene Diamine)-2"-Methyl Propionic acid]}propionyloxy Hexyloxy Pyrene (P2) and 1-{3 1 -S-[poly(Acryloyl Ethylene Diamine Hydrochloride)-2 1 -Methyl Propionic acid]}propionyloxy Hexyloxy Pyrene (P3)
The reaction mechanism of P2 and P3 was shown in Scheme 1. P1 (200.0 mg, 0.077 mmol), NaBH 4 (3.8 mg, 0.1 mmol), AHP (34.0 mg, 0.09 mmol), TEA (10 µL, 0.072 mmol), and solvent THF (2 mL) were added to a 5 mL eggplant-shaped flask.Then, the system was degassed for at least three cycles by pulling a vacuum and filling with nitrogen gas under magnetic stirring in an ice bath.The mixture was stirred at room temperature in a nitrogen atmosphere for 48 h.After removal of the solvent, a pale yellow solid was obtained and chromatographically purified on silica gel eluting with dichloromethane to remove the first two ribbons which were the excess AHP and the reaction byproducts.Then methanol was used as eluent to give P2 as a wheat-colored solid (0.202g, 96%).P2 (100 mg) was dissolved in 10 mL of THF, and then HCl gas was passed through the solution for the purpose of deprotection of the resulting Boc-protected polymer (P2) until an amount of precipitate formed.The formed precipitate was filtered and washed with THF, and dried in a vacuum oven to afford the desired water-soluble fluorescent polymer P3 as a pale brown solid (71.5 mg, 95%).

The reaction Mechanism of the One-Pot Reaction
Scheme 1 outlines the basic reaction mechanism.Thiol is obtained by a reduction reaction of the trithioester of P1.The weak sulfur-hydrogen bond of thiols are readily oxidized to disulfide bonds during storage or purification, resulting in difficulty of subsequent click-chemistry reactions.The one-pot method used in this paper can solve the problem easily.In the same system, both the reduction reaction of the trithioester bond of P1 to thiol, the click reaction of thiol, and the carbon-carbon double bond of AHP occurred simultaneously.As a result, a Boc-protected amino group fluorescent polymer (P2) was synthesized, then water-soluble pyrene-containing fluorescent polymer (P3) with a defined structure was obtained by the deprotection of the resulting Boc-protected polymer (P2) with aqueous HCl.

FTIR Analysis of AHP, P2, and P3
Figure 4 was the FTIR spectra of AHP, P2, and P3.As seen from the AHP spectrum, the characteristic stretching vibration absorption peak of the ester carbonyl group C=O bond was shown at cm ´1.The absorption peak was shown at 1596 cm ´1 resulting from that stretching vibration of the C=C bond in acrylic ester (-OCO-C=C).Absorption peaks at approximately 2939 and 2862 cm ´1 were assigned to the asymmetric and symmetric stretching vibration and asymmetric stretching vibration of methylene group C-H bond, respectively.The peak at 1408 cm ´1 responded to the C-H bond shear vibration of the vinyl end group (=CH 2 ).At around 1192 cm ´1 the absorption peak was the asymmetric stretching vibration of the C-O-C bond.Two absorption peaks were shown at 1620 and 1510 cm ´1 resulting from that stretching vibration of the aromatic ring skeleton of pyrene.There were no blockbuster absorption peaks of acid at 3300-2500 cm ´1 in this spectrum.Comparing the spectra of P2 and P3, the biggest difference was the absorption peak from 4000 to 2500 cm ´1.The absorption peaks shown at 3500-3300 cm ´1 and 3330-3150 cm ´1 were the stretching vibrations of the N-H bond in the primary amine and primary amine salt in the P3 spectrum, respectively, which was due to the removal of the Boc group and formed a -NH 2 and -NH 2 ¨HCl structure with HCl gas in repeating units.At around 1366 and 1390 cm ´1 absorption peaks were the vibration of the C-H bond of t-butyl in the P2 spectrum, and the former intensity was about twice as strong as the latter.The two peaks significantly reduced after removal of the Boc protection in the P3 spectrum, at around 1693 cm ´1 the ester carbonyl group C=O bond stretching vibration peak disappeared, remaining only at 1653 cm ´1, the solid amide C=O bond stretching absorption peak, which indicated that the number and morphology of the C=O bond was changed.These results clearly manifested the formation of AHP, P2, and P3.

The reaction Mechanism of the One-Pot Reaction
Scheme 1 outlines the basic reaction mechanism.Thiol is obtained by a reduction reaction of the trithioester of P1.The weak sulfur-hydrogen bond of thiols are readily oxidized to disulfide bonds during storage or purification, resulting in difficulty of subsequent click-chemistry reactions.The one-pot method used in this paper can solve the problem easily.In the same system, both the reduction reaction of the trithioester bond of P1 to thiol, the click reaction of thiol, and the carbon-carbon double bond of AHP occurred simultaneously.As a result, a Boc-protected amino group fluorescent polymer (P2) was synthesized, then water-soluble pyrene-containing fluorescent polymer (P3) with a defined structure was obtained by the deprotection of the resulting Boc-protected polymer (P2) with aqueous HCl.

FTIR Analysis of AHP, P2, and P3
Figure 4 was the FTIR spectra of AHP, P2, and P3.As seen from the AHP spectrum, the characteristic stretching vibration absorption peak of the ester carbonyl group C=O bond was shown at 1713 cm −1 .The absorption peak was shown at 1596 cm −1 resulting from that stretching vibration of the C=C bond in acrylic ester (-OCO-C=C).Absorption peaks at approximately 2939 and 2862 cm −1 were assigned to the asymmetric and symmetric stretching vibration and asymmetric stretching vibration of methylene group C-H bond, respectively.The peak at 1408 cm −1 responded to the C-H bond shear vibration of the vinyl end group (=CH2).At around 1192 cm −1 the absorption peak was the asymmetric stretching vibration of the C-O-C bond.Two absorption peaks were shown at 1620 and 1510 cm −1 resulting from that stretching vibration of the aromatic ring skeleton of pyrene.There were no blockbuster absorption peaks of acid at 3300-2500 cm −1 in this spectrum.Comparing the spectra of P2 and P3, the biggest difference was the absorption peak from 4000 to 2500 cm −1 .The absorption peaks shown at 3500-3300 cm −1 and 3330-3150 cm −1 were the stretching vibrations of the N-H bond in the primary amine and primary amine salt in the P3 spectrum, respectively, which was due to the removal of the Boc group and formed a -NH2 and -NH2•HCl structure with HCl gas in repeating units.At around 1366 and 1390 cm −1 absorption peaks were the vibration of the C-H bond of t-butyl in the P2 spectrum, and the former intensity was about twice as strong as the latter.The two peaks significantly reduced after removal of the Boc protection in the P3 spectrum, at around 1693 cm −1 the ester carbonyl group C=O bond stretching vibration peak disappeared, remaining only at 1653 cm −1 , the solid amide C=O bond stretching absorption peak, which indicated that the number and morphology of the C=O bond was changed.These results clearly manifested the formation of AHP, P2, and P3.

NMR Analysis of P3
P3 is soluble in water.It is characterized by NMR, UV-VIS, and PL spectroscopy.Figure 5 showed the 1 H NMR spectrum of P3. 1 H NMR (600 MHz, D 2 O, δ) showed a chemical shift peak from 7.60 to 8.40 ppm; these signals were assigned to the aromatic protons in pyrene units.There were two chemical shift peaks from 1.32 to 1.82 ppm and 1.94 to 2.37 ppm, which was attributed to protons of CH 2 and CH groups in the polymer main chain.Two chemical shift peaks from 2.97 to 3.20 ppm and 3.21 to 3.60 ppm corresponding to protons of CH 2 -NHCO and CH 2 -NH 2 . HCl in the polymer side chain were observed.There were two chemical shift peaks from 3.95 to 4.12 ppm and 3.75 to 3.80 ppm, which were assigned to protons of COO-CH 2 and C 6 H 4 O-CH 2 .The 1 H NMR spectrum also confirmed the presence of the pyrene unit in the P3 structure.This proved that the pyrene unit was really attached to the P1 chain and P2 was synthesized after the click reaction of thiol reduced from P1 and the carbon-carbon double bond of AHP.

NMR Analysis of P3
P3 is soluble in water.It is characterized by NMR, UV-VIS, and PL spectroscopy.Figure 5 showed the 1 H NMR spectrum of P3. 1 H NMR (600 MHz, D2O, δ) showed a chemical shift peak from 7.60 to 8.40 ppm; these signals were assigned to the aromatic protons in pyrene units.There were two chemical shift peaks from 1.32 to 1.82 ppm and 1.94 to 2.37 ppm, which was attributed to protons of CH2 and CH groups in the polymer main chain.Two chemical shift peaks from 2.97 to 3.20 ppm and 3.21 to 3.60 ppm corresponding to protons of CH2-NHCO and CH2-NH2 .HCl in the polymer side chain were observed.There were two chemical shift peaks from 3.95 to 4.12 ppm and 3.75 to 3.80 ppm, which were assigned to protons of COO-CH2 and C6H4O-CH2.The 1 H NMR spectrum also confirmed the presence of the pyrene unit in the P3 structure.This proved that the pyrene unit was really attached to the P1 chain and P2 was synthesized after the click reaction of thiol reduced from P1 and the carbon-carbon double bond of AHP.

UV-VIS and PL Analysis
Figure 7 is the UV-VIS spectra of AHP, P1, and P2 in CH2Cl2.As it can be seen from the P1 spectrum, there was only one characteristic absorption peak at 310 nm resulting from C=S double bond [35,37]; in sharp contrast, it had disappeared in the UV-VIS spectrum of P2.The numbers and positions of the UV-VIS absorption peak of P2 were consistent with those of AHP. Figure 8 is the PL spectra of AHP, P1, and P2 in CH2Cl2.The fluorescence emission peak of P1 using its maximum absorption wavelength of 310 nm in the UV-VIS spectrum as the excitation wavelength was not observed.345 nm was chosen as the excitation wavelength of AHP and P2 according to the reference literature [34,38].AHP and P2 showed the fluorescence spectra of the same shape and three typical fluorescence emission peaks at 387, 407, and 429 nm, respectively.Since unreacted AHP had been removed during the processing of P2 purified by silica gel column chromatography, these data indicated that P2 fluorescence emission was not due to residual AHP, but from pyrene units in P2.Figures 7 and 8 revealed that the pyrene-containing unit AHP was really introduced to the P1 chain and P2 was successfully prepared after one-pot reaction.

UV-VIS and PL Analysis
Figure 7 is the UV-VIS spectra of AHP, P1, and P2 in CH 2 Cl 2 .As it can be seen from the P1 spectrum, there was only one characteristic absorption peak at 310 nm resulting from C=S double bond [35,37]; in sharp contrast, it had disappeared in the UV-VIS spectrum of P2.The numbers and positions of the UV-VIS absorption peak of P2 were consistent with those of AHP.

UV-VIS and PL Analysis
Figure 7 is the UV-VIS spectra of AHP, P1, and P2 in CH2Cl2.As it can be seen from the P1 spectrum, there was only one characteristic absorption peak at 310 nm resulting from C=S double bond [35,37]; in sharp contrast, it had disappeared in the UV-VIS spectrum of P2.The numbers and positions of the UV-VIS absorption peak of P2 were consistent with those of AHP. Figure 8 is the PL spectra of AHP, P1, and P2 in CH2Cl2.The fluorescence emission peak of P1 using its maximum absorption wavelength of 310 nm in the UV-VIS spectrum as the excitation wavelength was not observed.345 nm was chosen as the excitation wavelength of AHP and P2 according to the reference literature [34,38].AHP and P2 showed the fluorescence spectra of the same shape and three typical fluorescence emission peaks at 387, 407, and 429 nm, respectively.Since unreacted AHP had been removed during the processing of P2 purified by silica gel column chromatography, these data indicated that P2 fluorescence emission was not due to residual AHP, but from pyrene units in P2.Figures 7 and 8 revealed that the pyrene-containing unit AHP was really introduced to the P1 chain and P2 was successfully prepared after one-pot reaction.Figure 8 is the PL spectra of AHP, P1, and P2 in CH 2 Cl 2 .The fluorescence emission peak of P1 using its maximum absorption wavelength of 310 nm in the UV-VIS spectrum as the excitation wavelength was not observed.345 nm was chosen as the excitation wavelength of AHP and P2 according to the reference literature [34,38].AHP and P2 showed the fluorescence spectra of the same shape and three typical fluorescence emission peaks at 387, 407, and 429 nm, respectively.Since unreacted AHP had been removed during the processing of P2 purified by silica gel column chromatography, these data indicated that P2 fluorescence emission was not due to residual AHP, but from pyrene units in P2.Figures 7 and 8 revealed that the pyrene-containing unit AHP was really introduced to the P1 chain and P2 was successfully prepared after one-pot reaction.P2 was soluble in common organic solvents, such as dichloromethane, trichloromethane, and THF, and exhibited a bright blue-violet fluorescence emission band in solution.P3 was soluble in water and exhibited a bright blue-violet fluorescence emission band in water, too.Figures 9 and 10 were UV-VIS and PL spectra of AHP in H2O, P2 in dichloromethane, and P3 in H2O, respectively.Since AHP was insoluble in water, there were no UV-VIS absorption peaks and fluorescence emission peaks of AHP in the aqueous solution.P3 had good water solubility, and showed the UV-VIS characteristic absorption bands of pyrene, and were consistent with those of P2 in dichloromethane solution.There were three fluorescence emission peaks at 387, 407, and 429 nm of P3 in aqueous solution, respectively, which were consistent with those of P2 in dichloromethane solution.Therefore, UV-VIS and PL measurement results showed that: P2 was prepared by the one-pot method of thiol reduced from P1 and the carbon-carbon double bond of AHP; water-soluble fluorescent polymer P3 was obtained by the deprotection of the resulting Boc-protected polymer (P2); and it was also confirmed that UV-VIS absorption and fluorescence emission of P2 and P3 come from their own structure, rather than the residual AHP.The fluorescence quantum yields of P2 (Φu = 0.44) in dilute THF and P3 (Φu = 0.39) in dilute aqueous solution were measured using DPA as a reference substance (Φs=0.90)[39] according to the formula:  P2 was soluble in common organic solvents, such as dichloromethane, trichloromethane, and THF, and exhibited a bright blue-violet fluorescence emission band in solution.P3 was soluble in water and exhibited a bright blue-violet fluorescence emission band in water, too.Figures 9 and 10 were UV-VIS and PL spectra of AHP in H 2 O, P2 in dichloromethane, and P3 in H 2 O, respectively.Since AHP was insoluble in water, there were no UV-VIS absorption peaks and fluorescence emission peaks of AHP in the aqueous solution.P3 had good water solubility, and showed the UV-VIS characteristic absorption bands of pyrene, and were consistent with those of P2 in dichloromethane solution.There were three fluorescence emission peaks at 387, 407, and 429 nm of P3 in aqueous solution, respectively, which were consistent with those of P2 in dichloromethane solution.Therefore, UV-VIS and PL measurement results showed that: P2 was prepared by the one-pot method of thiol reduced from P1 and the carbon-carbon double bond of AHP; water-soluble fluorescent polymer P3 was obtained by the deprotection of the resulting Boc-protected polymer (P2); and it was also confirmed that UV-VIS absorption and fluorescence emission of P2 and P3 come from their own structure, rather than the residual AHP.The fluorescence quantum yields of P2 (Φ u = 0.44) in dilute THF and P3 (Φ u = 0.39) in dilute aqueous solution were measured using DPA as a reference substance (Φ s =0.90) [39] according to the formula: Φ u " Φ s pn 2 u F u {n 2 s F s qpA s {A u q (1) Polymers 2015, 7, page-page P2 was soluble in common organic solvents, such as dichloromethane, trichloromethane, and THF, and exhibited a bright blue-violet fluorescence emission band in solution.P3 was soluble in water and exhibited a bright blue-violet fluorescence emission band in water, too.Figures 9 and 10 were UV-VIS and PL spectra of AHP in H2O, P2 in dichloromethane, and P3 in H2O, respectively.Since AHP was insoluble in water, there were no UV-VIS absorption peaks and fluorescence emission peaks of AHP in the aqueous solution.P3 had good water solubility, and showed the UV-VIS characteristic absorption bands of pyrene, and were consistent with those of P2 in dichloromethane solution.There were three fluorescence emission peaks at 387, 407, and 429 nm of P3 in aqueous solution, respectively, which were consistent with those of P2 in dichloromethane solution.Therefore, UV-VIS and PL measurement results showed that: P2 was prepared by the one-pot method of thiol reduced from P1 and the carbon-carbon double bond of AHP; water-soluble fluorescent polymer P3 was obtained by the deprotection of the resulting Boc-protected polymer (P2); and it was also confirmed that UV-VIS absorption and fluorescence emission of P2 and P3 come from their own structure, rather than the residual AHP.The fluorescence quantum yields of P2 (Φu = 0.44) in dilute THF and P3 (Φu = 0.39) in dilute aqueous solution were measured using DPA as a reference substance (Φs=0.90)[39] according to the formula:

Figure 6
Figure6are the GPC chromatograms for the standard sample (polystyrene), P1, and P2 which were shown as a blue line, red line, and green line, respectively.The Mn of the standard sample was labeled as 3.79 × 10 3 g•mol −1 .The Mn of P1 and P2 were given by the software as 2.60 × 10 3 g•mol −1 and 2.50 × 10 3 g•mol −1 , respectively.PDI of P1 is 1.39.The theoretical molecular weight of P2 is Mn(P2) = M(AHP) + Mn(P1) − M(CS2C12H25) = 372 + 2600 − 245 = 2727 g•mol −1 .The analytical datum from the GPC experiment was similar with the theoretical result, which proved that AHP bonded with the P1 chain as shown in Scheme 1.

Figure 6
Figure 6 are the GPC chromatograms for the standard sample (polystyrene), P1, and P2 which were shown as a blue line, red line, and green line, respectively.The M n of the standard sample was labeled as 3.79 ˆ10 3 g¨mol ´1.The M n of P1 and P2 were given by the software as 2.60 ˆ10 3 g¨mol ´1 and 2.50 ˆ10 3 g¨mol ´1, respectively.PDI of P1 is 1.39.The theoretical molecular weight of P2 is M n (P2) = M(AHP) + M n (P1) ´M(CS 2 C 12 H 25 ) = 372 + 2600 ´245 = 2727 g¨mol ´1.The analytical datum from the GPC experiment was similar with the theoretical result, which proved that AHP bonded with the P1 chain as shown in Scheme 1.