Rapid-Response and Highly Sensitive Boronate Derivative-Based Fluorescence Probe for Detecting H2O2 in Living Cells.

Intracellular H2O2 monitoring is important and has driven researchers to pursue advancements for the rapid identification of H2O2, since H2O2 is short-lived in cell lines. An arylboronate derivative has been investigated as a chemospecific fluorescence recognition agent for H2O2. Triphenylimidazoleoxadiazolephenyl (TPIOP) boronate was contrived as a novel candidate for the rapid and sensitive recognition of H2O2. The probe was conjugated using the TPIOP functional group acting as an excellent fluorescent enhancer. The TPIOP group stimulated the polarization of C-B bond due to its extended π-conjugation, which included heteroatoms, and induced the production of rapid signal because of the highly polar C-B bond along with the corresponding boronate unit. While H2O2 reacts with TPIOP boronate, its nucleophilic addition to the boron generates a charged tetrahedral boronate complex, and then the C-B bond migrates toward one of the electrophilic peroxide oxygen atoms. The resulting boronate ester is then hydrolyzed by water into a phenol, which significantly enhances fluorescence through aggregation-induced emission. The TPIOP boronate probe responded to H2O2 rapidly, within 2 min, and exhibited high sensitivity with a limit of detection of 8 nM and a 1000-fold selectivity in the presence of other reactive oxygen species. Therefore, the developed TPIOP boronate chemodosimeter was successfully utilized to visualize and quantify intracellular H2O2 from human breast cancer (MCF-7) cells, as well as gaseous and aqueous H2O2 from environmental samples using Whatman paper strips coated with TPIOP boronate.

1. Introduction

Hydrogen peroxide (H2O2) is a small yet important reactive oxygen species (ROS), which is present in biological systems, and exerts wide physiological and pathological effects [1]. Abnormal levels of H2O2 in the human body can cause long-term damage to cells and organs and lead to significant neurodegeneration, oxidative stress, and cancer [2]. Thus, the far-ranging impingements of H2O2 homeostasis encouraged scientists to construct sensitive, rapid response, and selective and accurate sensors for detecting H2O2.

H2O2 presents a unique inherent conflict of reactivity over the other ROS, because most of the other ROS are operated by one electron transfer pathway. Moreover, H2O2 possesses amphiphilic reactivity; its labile O–O bond allows it to react as a two-electron electrophilic oxidant, whereas H2O2 can also be a good nucleophile due to the α-effect of the adjacent nonbonding orbitals on its oxygen atoms [3, 4]. Boronates present unique abilities for detecting amphiphilic substances and exhibit chemoselectivity for H2O2, while the aryl derivative bound to the boron atom converts to phenol when reacting with H2O2 [3, 4].

Although numerous aryl derivatives conjugated with boronate have been developed as H2O2 chemosensors, their slow response times cause difficulties for tracking H2O2 in situ [5-30]. Since H2O2 has a short half-life, the slow responses of H2O2 chemosensors caused researchers to question the accuracy of the measured concentrations of H2O2 from in situ cell lines and the environment. Therefore, designing a novel molecule which would facilitate the fast detection of H2O2 has been a challenge. Zhang et al. recently reported that the polarity of the C–B bond in boronate represented the key to achieving fast and sensitive recognition of H2O2 [5-7]. They determined that the extended conjugation of the π-electron system of tetraphenylethylene (TPE) combined with boronate compound could enhance the polarity of C–B bond, thus achieving rapid monitoring of H2O2 through aggregation-induced emission (AIE) [5-7]. This finding opened a new window toward designing a fluorogenic probe for H2O2 sensing through significantly increasing the C–B bond polarity. Incorporating heteroatoms into a fluorogenic probe using new structural design strategies for synthesizing intensive AIE luminogens caused large electron perturbations and increased the emission intensity of luminogens [31]. For example, imidazole rings present lone pairs of electron-rich nitrogen atoms, which can induce polarization by intramolecular charge transfer and have been widely exploited in the fields of biology and fluorescent sensors [32]. Many researches have recently been focusing on derivatives of phenylimidazole chemosensors based on their enhanced fluorescence properties. For example, Takagi et al. synthesized fused π-conjugated diphenylimidazole derivatives, which exhibited superior optical properties [33]. Based on these findings, we designed an imidazole containing boronate, which included a triphenyl group in the imidazole ring bridged with oxadiazolepheylboronate, and utilized it for H2O2 detection. The additional oxadiazole ring was introduced to enhance the electron affinity associated with the electron transporting properties of the highly photoluminescent compound [34].

The newly synthesized triphenylimidazoleoxadiazolephenyl (TPIOP) boronate chemosensor was tested as a fast-response and highly sensitive chemosensor. The high degree of π-conjugation created an excellent electrostatic potential on the carbon atom bound to the boron atom. The boronate group acted as a recognition unit, and the extended triphenylimidazoleoxadiazole moiety significantly amplified the inherent fluorescence of the chemosensor compared to that of the earlier chemodosimeter containing a simple phenyl unit. As expected, the TPIOP boronate probe responded rapidly to H2O2, within 2 min of coming into contact with H2O2. When the probe was triggered using H2O2, the weakly fluorescent TPIOP boronate converted into triphenylimidazoleoxadiazolephenol (TPIOP-OH), which exhibited much stronger fluorescence, and the enhanced emission intensity was caused by the mechanistic pathway of AIE. The limit of detection (LOD) of H2O2 for the TPIOP boronate probe was approximately 8 nM. Also, H2O2 can be visually detected by exposing Whatman paper coated with TPIOP boronate to UV radiation. This TPIOP boronate H2O2 chemodosimeter exhibited rapid response, high chemoselectivity, high sensitivity, and low cytotoxicity, which rendered it useful for detecting H2O2 in MCF-7 (human breast cancer) cell lines.

2. Materials and Methods

2.1. Chemicals and Reagents

4-Cyanobenzaldehyde, benzil, 4-bromobenzoic acid, bis(pinacolato)diboron, 1,1′-carbonyldiimidazole (CDI), [1,1′-bis(diphenylphosphino)ferrocene]dichloropalladium(II)dichloride (PdCl2 (dppf)), H2O2, potassium super-oxide (KO2), t-butyl hydroperoxide (TBHP), m-chloroperoxybenzoic acid (mCPBA), hypochlorous acid (HOCl), HEPES buffer solution, Whatman papers, Dulbecco's phosphate-buffered saline (DBS), Roswell Park Memorial Institute (RPMI) medium, fetal bovine serum (FBS), penicillin, streptomycin, and 3-(4,5-dimethylthiazol-2-yl)-2,5-diphenyltetrazolium bromide (MTT) were purchased from Sigma-Aldrich (St. Louis, MO, USA). Ammonium acetate, acetic acid, ethanol, hydroxylamine hydrochloride, sodium hydroxide, ethyl acetate, hexane, sodium bicarbonate, dimethylformamide (DMF), dimethyl sulfoxide (DMSO), 1,4-dioxane, and potassium acetate were purchased from Daejung Chemicals (Siheungsi, Kyunggido, Republic of Korea). Sodium nitrate (NaNO3 −), potassium perchlorate (KClO4 −), sodium sulfate (Na2SO4), sodium nitrite (NaNO2), and benzoyl peroxide (BPO) were obtained from AccuStandard (New Haven, CT, USA). The MCF-7 cells were purchased from the Korean Cell Line Bank (Seoul, Republic of Korea). All reagents were used as received without further purification.

2.2. Instrumentation

All UV-Vis absorption spectra were measured in the 300–800 nm range, using polystyrene cells of 1 mm path lengths on an S-3100 spectrophotometer (Sinco, Seoul, Republic of Korea). Fluorescence spectra were recorded using a LS-45 luminescence spectrometer (PerkinElmer, Waltham, MA, US). Both 1H and 13C nuclear magnetic resonance (NMR) spectra were recorded using a Bruker Avance 600 MHz spectrometer (Billerica, MA, US). The mass spectra were obtained in positive mode using a Synapt G2 high-resolution mass spectrometer (HR-MS) (Waters, Milford, MA, US). The pH of the solution was adjusted using a HI 2210 pH meter (Hanna Instruments, Woonsocket, RI, USA). Fluorescence images were acquired using a LSM 700 confocal laser scanning microscope (Carl Zeiss, Jena, Germany) equipped with a 63× oil immersion objective lens and a diode laser as light source. Cytotoxicity tests were performed using a Spectramax M2 microplate reader (Molecular Devices, Sunnyvale, CA, USA).

2.3. Synthesis of TPIOP Boronate

2.3.1. Preparation of 4-(4,5-Diphenyl-1H-imidazol-2-yl)benzonitrile

A solution of 4-cyanobenzaldehyde ((2) in Scheme 1) (1.80 g, 13.73 mM), benzil ((1) in Scheme 1) (2.90 g, 14.1 mM), and ammonium acetate (8.50 g, 110.39 mM) in acetic acid (50 mL) was refluxed for 24 h under N2 flow. After cooling, the solution was poured into ice-cooled water to precipitate the product. The yellow solid was collected and dried to form 4-(4,5-diphenyl-1H-imidazol-2-yl)benzonitrile ((3) in Scheme 1) (4.20 g) with 95% yield.

Scheme 1

Synthesis of TPIOP boronate.

1H NMR (400 MHz, DMSO) δ 13.01 (brs, 1H), 8.25 (d, J = 8.4 Hz, 2H), 7.94 (d, J = 8.4 Hz, 2H), 7.53 (d, J = 7.2 Hz, 4H), 7.45–7.29 (m, 6H). 13C NMR (100 MHz, DMSO) δ 141.2, 134.8, 133.2, 130.1, 130.0, 129.0, 128.8, 128.5, 126.0, 119.4, 110.6.

2.3.2. Preparation of N′-Hydroxy-4-(4,5-Diphenyl-1H-imidazol-2-yl)benzamidine

Hydroxylamine hydrochloride (NH2OH·HCl) (18.8 mmol, 1.31 g) and sodium hydroxide (18.8 mmol, 752 mg) were added to a solution of benzonitrile ((3) in Scheme 1) (17.1 mM, 5.50 g) in ethanol (5 mL), and then water (10 mL) was sequentially added to the solution for 20 min at 0°C. Then, the resulting mixture was allowed to reflux while stirring for 18 h. The pH of the solution was adjusted to 2 using 1 N HCl, and the aqueous phase was washed using ethyl acetate. Upon cooling (0°C) and neutralization with sodium bicarbonate, a precipitate formed, which was subsequently filtered, washed, and dried to obtain pure N′-hydroxy-4-(4,5-diphenyl-1H-imidazol-2-yl)benzamidine ((4) in Scheme 1) (5.30 g) with 87% yield.

1H NMR (400 MHz, DMSO) δ 12.73 (brs, 1H), 9.71 (s, 1H), 8.07 (d, J = 8.4 Hz, 2H), 7.77 (d, J = 8.4 Hz, 2H), 7.55 (d, J = 7.3 Hz, 4H), 7.46–7.20 (m, 6H), 5.84 (s, 2H). 13C NMR (100 MHz, DMSO) δ 151.2, 145.8, 133.4, 131.3, 128.9, 127.7, 127.5, 127.2, 126.1, 125.2, 125.0.

2.3.3. Preparation of 4-Carboxyphenyl Boronate (CPB)

Bis(pinacolato)diboron ((6) in Scheme 1) (5.47 mM, 1.40 g), PdCl2(dppf) (3 mol%, 0.49 mM, 109.00 mg), and potassium acetate (14.93 mM, 1.50 g) were added to a mixture of benzoic acid ((5) in Scheme 1) (4.98 mM, 1.00 g) in dry 1,4-dioxane (10 ml). Then, resulting mixture was degassed three times using N2 gas and was stirred at 80°C for 12 h. The reaction mixture was filtered through celite and concentrated in vacuo. The brown CPB solid (IUPAC name: 4-(4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2-yl)benzoic acid) (963.70 mg) was obtained with a good 78% yield.

1H NMR (400 MHz, DMSO) δ 13.04 (brs, 1H), 7.94 (d, J = 8.0 Hz, 2H), 7.77 (d, J = 8.0 Hz, 2H), 1.29 (s, 12H). 13C NMR (100 MHz, DMSO) δ 168.1, 135.3, 134.0, 132.4, 129.1, 85.0, 25.6.

2.3.4. Preparation of TPIOP Boronate

Carbonyl diimidazole (0.90 mM, 145.90 mg) in N2 was added to a solution of benzoic acid ((7) in Scheme 1) (0.75 mM, 186.10 mg) in dry DMF (3 ml), and the reaction mixture was stirred for 1 hr at ambient temperature. Then, N′-hydroxy-4-(4,5-diphenyl-1H-imidazol-2-yl)benzamidine ((4) in Scheme 1) (0.90 mM, 320 mg) was slowly added to the above mix, and the reaction mixture was heated at 110°C for ∼18 h. The reaction mixture was cooled to 25°C and poured into ice-cold water (25 mL) and extracted using methylene chloride. The combined organic phase was washed with brine, dried over anhydrous sodium sulfate, filtered, and concentrated in vacuo. The obtained residue was purified utilizing column chromatography using silica gel to generate pure TPIOP boronate (IUPAC name: 5-(4-(4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2-yl)phenyl)-3-(4-(4,5-diphenyl-1H-imidazol-2-yl)phenyl)-1,2,4-oxadiazole) ((8) in Scheme 1) (369.60 mg) as a brown solid substance with excellent 87% yield.

1H NMR (400 MHz, DMSO) δ 12.94 (brs, 1H), 8.92 (dd, J = 1.6, 4.4 Hz, 2H), 8.31 (d, J = 8.5 Hz, 2H), 8.20 (d, J = 8.5 Hz, 2H), 8.12 (dd, J = 1.6, 4.4 Hz, 2H), 7.56 (d, J = 7.2 Hz, 2H), 7.52 (d, J = 7.2 Hz, 2H), 7.47–7.23 (m, 6H), 1.22 (s, 12H) (Figure S1A).13C NMR (100 MHz, DMSO) δ 168.2, 163.5, 154.1, 151.4, 144.1, 133.2, 132.5, 131.1, 129.7, 127.5, 124.2, 123.7, 123.5, 81.3, 25.6 (Figure S2A). The m/z value was determined to be 567.46 (Figure S3A).

2.4. Spectroscopy Measurements

The TPIOP boronate solution was prepared using 10 mM HEPES buffer at pH 7.4 containing 2 vol% DMSO. The final concentrations of the TPIOP boronate solution used to carry out UV-Vis and fluorescence measurements were 20 and 2 μM in 10 mM HEPES buffer at pH 7.4 containing 2 vol% of DMSO, respectively. In addition, 15 mM solutions of ROS such as KO2, NO3 −, TBHP, mCPBA, HOCl, ClO4 −, SO4 2−, NO2 −, NO3 −, and BPO (benzoyl peroxide) were prepared using double distilled water.

2.5. Computational Methods

Quantum calculations using the density functional theory (DFT) were carried out for the abovementioned probe molecule. The generalized gradient approximation method involved the Becke three-parameter plus Lee-Yang-Parr (B3LYP) functional, while the basis set was the Pople 6-31 + G(d,p) one [33-35]. The intrinsic solvent model was considered using the c-pcm model, the dielectric constant being 78.39. All calculations were carried out using the Q-Chem 4.3 program. Graphical representation for the calculated results was obtained using the IQmol software [36, 37].

2.6. Paper Strip Test

For the paper strip-based detection of H2O2, Whatman paper (8 mm diameter) samples were first immersed into 1 μM TPIOP boronate solution for 5 min and subsequently dried in air. The dried papers were exposed to different concentrations of H2O2 for 2 min. Then, the papers were illuminated under a UV lamp (365 nm), and fluorescence images were obtained.

2.7. Cell Culture, Cytotoxicity Tests, and Confocal Microscopy Imaging

The MCF-7 cells were cultured in RPMI 1640 supplemented with 10% FBS, 100 μg/mL penicillin, and 100 μg/mL streptomycin. The cells were maintained in an incubator at 37°C in 5% CO2 environments. For the cytotoxicity tests, the cells were seeded in a 96-well plate containing culture media. After overnight culture, the cells were incubated using different concentrations of TPIOP boronate. To measure the viability of the cells, 0.5 mg/mL MTT medium was added to each of the cells for 4 h and the produced formazan was dissolved in 0.1 mL DMSO and analyzed using a Spectramax microwell plate reader. The cytotoxic effects of TPIOP boronate were calculated using the following equation:where OD(sample) and OD(control) are the optical densities of the sample and control, respectively.

For live cells imaging, cells were seeded in 35 mm glass-bottomed dishes containing culture media. After overnight culture, the MCF-7 cells were incubated with 10 μM TPIOP boronate for 30 min, washed with DBS, and incubated with 10 μM H2O2 for 30 min. Fluorescence images were acquired using an LSM 700 confocal laser scanning microscope (Carl Zeiss, Jena, Germany) equipped with a 63× oil immersion objective lens and a diode laser as light source [38].

3. Results and Discussion

3.1. Spectral Studies of TPIOP Boronate

The detailed synthesis of TPIOP boronate is represented in Scheme 1. The TPIOP boronate probe was characterized using 1H NMR, 13C NMR, and HR-MS techniques (Figures S1A, S2A, and S3A, respectively). We initially evaluated the photophysical properties of the TPIOP boronate probe, and its ability to track H2O2 was investigated using HEPES buffer solution (10 mM, pH 7.4 containing 2 vol% DMSO). The optical properties of TPIOP boronate were analyzed, and the results are represented own in Figure 1. The 2 μM solution of TPIOP boronate in 10 mM HEPES buffer solution (10 mM, pH 7.4 containing 2 vol% of DMSO) exhibited an excitation maximum centered at 346 nm. The TPIOP boronate probe presented weak fluorescence at 467 nm with a Stokes shift of 121 nm (Figure 1). After the probe was triggered using H2O2, a significant turn-on fluorescent enhancement was observed at 467 nm, and the fluorescence was also visually observed using an UV lamp, as shown in Figure 2(a).

Figure 1

Emission (λ max = 467 nm) and its corresponding excitation (λ max = 346 nm) spectra obtained for 2 μM TPIOP boronate in HEPES buffer solution (10 mM, pH 7.4, and 2 vol% DMSO).

Figure 2

(a) Fluorescence emission spectra of the probe TPIOP boronate (1) before and (2) after reacting with H2O2 to form TPIOP-OH. (b) Time-dependent fluorescence intensity at 467 nm in 2 μM TPIOP boronate using various concentrations (0 to 15 μM) of H2O2 at 10 mM HEPES buffer solution (pH 7.4 and 2 vol% DMSO).

The TPIOP boronate probe contained TPIOP and a boronic ester moiety in its structure. It is well known that the boronate group undergoes oxidation in the presence of H2O2, and the oxidation of boronate is caused by the enhanced nucleophilicity of H2O2 due to the α-effect, imparted by the adjacent nonbonding orbitals on its oxygen atoms and its weak O–O bonds. The nucleophilic addition of H2O2 to the boron atom results in a charged tetrahedral boronate complex, which subsequently undergoes a 1,2-insertion where the C–B bond migrates to one of the electrophilic peroxide oxygen atoms. The resulting borate ester is then hydrolyzed by water into phenol (Scheme 2) [6, 10, 11].

Scheme 2

Chemical structure of TPIOP boronate and its reaction product with H2O2 (TPIOP-OH) via the proposed mechanism pathway.

The conversion of TPIOP boronate into TPIOP-OH was supported by 1H NMR, 13C NMR, and HR-MS data (Figures S1B, S2B, and S3B, respectively). The 1H NMR of TPIOP boronate presented a methyl singlet peak at 1.07 ppm, which disappeared after TPIOP boronate reacted with H2O2. Then, a new peak appeared at 6.25 ppm, which was attributed to phenolic –OH proton (Figure S1B). The 13C NMR spectrum contained a methyl peak which appeared at 25.5 ppm and disappeared after the conversion of boronate into phenol (Figure S2B). After injecting H2O2 into the TPIOP boronate sample, a new m/z value was observed at 457.49 [M]+, which corresponded to the molecular weight of TPIOP-OH (Figure S3B). This demonstrated that while reacting with H2O2, TPIOP boronate was converted into TPIOP-OH (Scheme 2), and the yield was found to be 78%.

The conformational change from hydrophobic to hydrophilic form during the conversion of TPIOP boronate into TPIOP-OH led to aggregation. Intramolecular rotation associated with this conversion was restricted due to physical constraints, which blocked the nonradiative relaxation and commenced the radiative decay. Therefore, the intensity of the emission was enhanced based on an AIE mechanism.

A computational study was utilized to elucidate the characteristics of the C–B and B–O chemical bonds in TPIOP boronate. The polarities of the C–B and B–O bonds were relatively high given the electronegativities of the individual atoms (Figures S4 and S5), and the C–B bond was the most labile site for the H2O2 (Scheme 2). This was caused by extensively delocalized π-electrons throughout the TPIOP group. Moreover, the presence of heteroatoms increased the electron perturbation throughout TPIOP in half. Therefore, the electron density of the carbon atom bound to boron was high, which would lead to the high polarity of the C–B bond. This leads to the activation of the reaction centers during oxidation reaction of boronate in the TPIOP boronate probe, which allowed for the rapid identification of H2O2. To achieve rapid H2O2 detection using TPIOP boronate, we examined the time-dependent fluorescent kinetics, as shown in Figure 2(b). Upon adding H2O2 to TPIOP boronate, the fluorescence intensity at 467 nm increased rapidly with time and achieved its maximum within 2 mins, which intimated that TPIOP boronate was an effective fluorescent probe able to detect H2O2 very rapidly. This was due to the presence of active reaction centers (C and B) in TPIOP boronate, which were provided by the TPIOP moiety.

3.2. Sensitive Detection of H2O2 Using TPIOP Boronate

The initial detection ability of TPIOP boronate for H2O2 was analyzed using UV-Vis absorbance studies. We added solutions of H2O2 with concentrations ranging from 1 to 11 μM to 20 μM TPIOP boronate (pH 7.4, HEPES buffer solution, 2 vol% DMSO) during these experiments. The absorbance intensity at 270 nm increased linearly as the concentration of H2O2 increased from 1 to 11 μM (Figure S6A). A good linearity was obtained between the concentration of H2O2 and absorbance intensity at 270 nm (R 2 = 0.9896) (Figure S6B). Sensitive detection of H2O2 was further achieved through fluorescence spectroscopy. Figure 3 illustrates the increase in fluorescence intensity as the concentration of H2O2 increased from 0 to 13.5 μM. A linear calibration curve with the regression coefficient of 0.9986 was obtained when the fluorescence intensity at 467 nm was plotted against the concentration of H2O2 (inset, Figure 3). The LOD was estimated to be 8 nM (signal to noise ratio (S/N) = 3), which was significantly lower than the reported range (Table 1). This revealed that the TPIOP boronate probe was able to detect nanomolar level concentration of H2O2.

Figure 3

Fluorescence response of TPIOP boronate after reacting with different concentrations of H2O2 (0–13.5 μM) in 10 mM HEPES buffer solution (pH 7.4 and 2 vol% DMSO). Insets: plot of fluorescent intensity at 467 nm against the concentration of H2O2 concentration and fluorescent images obtained when 2 μM TPIOP boronate coated Whatman paper was exposed to different concentrations of H2O2 (0–6 μM).

Table 1

Comparison of LOD and response time values of present probe with those of boronate-based H2O2 sensors recently reported in the literature.

No.	System	Response time (min)	LOD (nM)	References
1	Boronic ester of TPE	∼10	520	[5]
2	Carbon dot featuring boronate recognition unit	30	750	[7]
3	N-4-(Benzyl boronic pinacol ester) pyridinium bromide moiety on TPE	30	180	[8]
4	TPE modified with boronic ester	10	950	[9]
5	Diboronate functionalized TPE	60	3200	[10]
6	Imine derivative of TPE	40	100	[11]
7	Modified hemicyanine dye	90	13	[12]
8	9H-1,3-dichloro-7-hydroxy-9,9-dimethylacridine-2-one	60	420	[13]
9	2-(3-(4-Hydroxystyryl)-5,5-dimethylcyclohex-2-enylidene) malononitrile	30	70	[14]
10	Mitochondria targeted benzothiazole probe	120	23	[15]
11	Phenanthroimidazole, benzonitrile, and phenyl boronate	10	148	[16]
12	4-Carboxy-3-fluorophenylboronic acid and 7-hydroxycoumarin-conjugated probe	60	760	[17]
13	1,3-Bis(bispyridin-2-ylimino)isoindolin-4-ol	40	9.1	[18]
14	Tetrahydroquinoxaline iminocoumarin derivative	10	60	[19]
15	Dioxetane-based probe	—	75000	[20]
16	2-Dicyanomethylene-3-cyano-4,5,5-trimethyl-2,5-dihydrofuran	60	61	[21]
17	Naphthalimide-coumarin-based ICT-activated FRET sensor	60	1350	[22]
18	Lysosome-targeted two-photon probe	—	1210	[23]
19	Cyanosilbene-boronate-based AIEE probe	—	455	[24]
20	Borylated boron dibenzopyrromethene dye	—	248	[25]
21	Mitochondria-targeted probe	4	40	[26]
22	p-Nitroaniline and 7-amino-4-methyl coumarin bearing probe	8	100	[27]
23	Dicyanomethylene-4-H-chromene	10	450	[28]
24	Dicyanomethylene-4-H-pyran	30	79	[29]
25	4-Hydroxynaphthalimide derivate	40	2000	[30]
26	TPIOP boronate probe in this study	2	8	This work

Considering the best performance of TPIOP boronate, we also extended the study to create solid state H2O2 sensors using paper strips. We determined that depending on its concentration; H2O2 renders Whatman paper emissive (inset, Figure 3). This demonstrated that the paper strips coated with TPIOP boronate could potentially act as environmental H2O2 detector.

3.3. DFT Calculations on Molecular Orbitals of TPIOP Boronate

To analyze the sensitivity of the abovementioned probe, the frontier molecular orbitals in TPIOP boronate were calculated and are represented in Figure 4. The splitting of the highest occupied molecular orbital (HOMO) and lowest unoccupied molecular orbital (LUMO) energy levels occurred at the opposite ends of the molecule: HOMO was located at the opposite end of the boronate group, whereas LUMO was located near the C–B bond. As can be seen from the LUMO of TPIOP boronate, π orbitals extended from the biphenyl moiety to the boron atom. It is well known that the mechanism for sensing H2O2 of TPIOP boronate involves the oxygen atom of H2O2 interacting with the C–B bond through a Lewis acidic reaction. The LUMO level of the probe in this reaction was lowered by HOO−, which facilitated the breaking of the C–B bond. When HOMO located near LUMO, the possibility of electron transitions would be high and the interaction with HOO– would be obstructed by the electron-rich area near the C–B bond. The electron transitions might be hindered by the splitting of the frontier orbitals, which is responsible for the high sensitivity of TPIOP boronate for H2O2. The HOMO/LUMO transition energy was quantitatively calculated employing time-dependent DFT using optimized conformations and DFT calculations (Figure 4). It can be seen that the energy gap increased from 3.022 to 3.188 eV after TPIOP boronate reacted with H2O2. These findings coincided with the experimental data obtained using UV spectroscopy (Figure S6A).

Figure 4

Optimized geometries of TPIOP boronate and TPIOP-OH and their HOMO-LUMO energy gaps.

3.4. Selectivity and Interference Study

Further investigations were carried out to determine the selectivity and inference ability of TPIOP boronate toward H2O2. In addition, the fluorescence response of TPIOP boronate toward H2O2 was assayed for various ROS. The fluorescence response of TPIOP boronate upon adding 15 μM H2O2 to it is illustrated in Figure 5. Under similar reaction conditions, adding 15 mM solutions (1000× more concentrated) of other ROS, such as KO2, NO3 −, TBHP, mCPBA, HOCl, ClO4 −, SO4 2−, and NO2 −, to TPIOP boronate did not induce significant changes in the fluorescence intensity compared to that of H2O2 (Figure 5(a)), and the detection of H2O2 was not hindered even in the presence of ROS solutions 1000× more concentrated than the H2O2 solution (Figure 5(b)). These findings were also confirmed by the fluorescence images in the insets of Figures 5(a) and 5(b) and indicated that TPIOP boronate can also be used to visually identify and discriminate the presence of H2O2 from wide ranges of ROS pools under UV radiation. The bar chart representation of the fluorescence response of TPIOP boronate in the presence of various ROS is shown in Figure 5(c). From the above studies, we concluded that TPIOP boronate was 1000 times more sensitive to H2O2 than to other ROS when other ROS were present. Also, it was clearly observed that the TPIOP boronate probe presented rapid and nanomolar level sensitivity toward H2O2.

Figure 5

Fluorescence emission spectra of TPIOP boronate after reacting with (a) 15 μM H2O2 and 15 mM of other ROS and (b) 15 μM H2O2 along with 15 mM of other ROS. (c) Bar chart of selectivity and interferences of TPIOP boronate. Experimental conditions: 2 μM of TPIOP boronate in 10 mM HEPES buffer solution (pH 7.4 and 2 vol% DMSO). (1) TPIOP probe, (2) H2O2, (3) KO2, (4) NO3 −, (5) TBHP, (6) mCPBA, (7) HOCl, (8) ClO4 −, (9) SO4 2−, (10) NO2 −, (11) ONOO−, and (12) BPO, respectively. Insets: corresponding fluorescence images.

These results obtained using the TPIOP boronate encouraged us to further investigate the possibility of using it for fluorescence imaging in living cells. Before considering the biological applications of TPIOP boronate, its sensitivity in terms of its fluorescent behavior was tested as a function of pH. The fluorescence emission intensity at 467 nm was monitored before and after adding 15 μM H2O2 to a 2 μM TPIOP boronate probe solution and was plotted against the pH (Figure S7A). The fluorescence images observed for TPIOP boronate at different pH levels and the fluorescence responses after adding H2O2 to it are illustrated in Figure S7B. It can be noticed that the emission intensity is usually high in basic media (pH 7–12), but it reached its maximum at pH 7-8. Hence, the probe solution was maintained at the physiological pH of 7.4 throughout all the experiments.

3.5. Cytotoxicity of TPIOP Boronate and Its H2O2 Detection in Live MCF-7 Cells

Since the TPIOP boronate probe exhibited excellent sensitivity (nM level) for the detection of H2O2, we hypothesized that it would be possible to detect H2O2 in cell lines using TPIOP boronate. Before using the TPIOP boronate probe for live cell imaging, its biocompatibility was tested using an MTT assay. The bioimaging applications of TPIOP boronate for detecting H2O2 were demonstrated using living MCF-7 cells. The cytotoxicity of the probe was low, as shown in Figure S8, which reveals that the MCF-7 cells were able to survive concentration of TPIOP boronate up to 100 μM. We chose a 10 μM solution of TPIOP boronate for staining the probe. Living MCF-7 cells stained with TPIOP boronate were used to detect H2O2, and live images were recorded using a Zeiss LSM 700 confocal microscope. Images of H2O2 in the MCF-7 cells were recorded after the TPIOP boronate probe (10 μM) and 10 μM H2O2 were incubated for 30 min at 37°C. The TPIOP boronate-stained MCF-7 cells generated weak blue emissions (Figure 6(a)), whereas the TPIOP boronate-stained MCF-7 cells incubated with H2O2 generated strong blue emissions (Figure 6(b)). The increase in the emission intensity of the probe after interacting with the live MCF-7 cells was due to H2O2 and is illustrated in Figure S9. These results demonstrated that the TPIOP boronate probe in our study would be amenable for live-cell H2O2 imaging.

Figure 6

Confocal fluorescence microscopy images of MCF-7 cells incubated with (a) 10 μM probe and (b) 10 μM H2O2 and probe. Scale bar = 10 μm (blue channel of (b)).

4. Conclusions

The findings of our current study indicated that a novel TPIOP boronate chemodosimeter containing highly polar C–B bond was designed, synthesized, characterized, and utilized for H2O2 detection. Increasing the polarity of the C–B bond can increase the reactivity of TPIOP boronate with H2O2. This was achieved by introducing a TPIOP moiety using CPB. Adding H2O2 to TPIOP boronate triggered the formation of TPIOP-OH, and then the fluorescence intensity was increased via the AIE mechanism. Therefore, the abovementioned TPIOP boronate probe could become a fluorescent tool for the rapid, selective, and sensitive monitoring of H2O2. The lowest LOD of 8 nM was achieved using TPIOP boronate at physiological pH level, which was below the range reported in the literature. In addition, paper strips coated with TPIOP boronate were used for on-site naked-eye H2O2 detecting experiments using UV radiation. Furthermore, TPIOP boronate exhibited low cytotoxicity and was utilized as fluorescent marker for detecting H2O2 in living cells [35].