# Synthesis of New Blue Fluorescent Polymerizable 1,8-Naphthalimides and Their Copolymers with Styrene as Sensors for Fe(III) Cations

Authors: Ivo Grabchev; Stanislava Yordanova; Stanimir Stoyanov; Ivan Petkov
Journal: Journal of Chemistry
 (2014)

---

## Abstract

The synthesis, characterization, and functional properties of two new polymerizable 1,8-naphthalimides (MDs) have been described. Their copolymers with styrene designed to act as a fluorescence PET chemosensor have been investigated. The study also reports the influence of different metal cations (Ag+, Mg2+, Cu2+, Sr2+, Co2+, Pb2+, and Fe3+) on the fluorescence intensity of both low and high molecular weight fluorophores.


---

## Body

## 1. Introduction

In the recent years the development of molecular recognition and sensing systems for different analytes has received considerable attention. Fluorescent chemosensors utilised for detection of metal cations and protons in the environment were based on different molecular structures [1, 2]. The fluorescent polymers are very attractive for this purpose. In this case the fluorescent sensor units can be covalently bonded to the polymer chain, thus showing very similar effect to their monomeric sensor units [3]. The functional characteristics of polymer chemosensors can be expressed either by conformational changes of macromolecules or by the collective transport properties.Recently, new polymerizable 1,8-naphthalimide molecules to sensitive protons or metal cations have been synthesized and their functional properties are investigated. Due to the presence of a polymerizable group they can react with some commercial monomers, allowing copolymers with a green or blue fluorescence to be obtained. It was demonstrated that the copolymers of these polymerizable sensors can be used as homogeneous and heterogeneous photoinduced electron transfer (PET) fluorescent sensors sensitive to metal cations [4–9]. In all cases 1,8-naphthalimides are enough thermo- and water resistible so the polymers can be used for ion determination in solution without contaminating it. The scientific tasks on development of polymeric systems for detection of environment pollutants will be focused on finding such polymeric systems which have specific chemical, physical, and mechanical properties as transparency, resistance to different environment factor and the harmful chemical substances, flexibility, and so forth.In this paper we present the synthesis and functional properties of two new polymerizable 1,8-naphthalimides (MDs) and their copolymer with styrene designed to act as fluorescence chemosensors. The influence of different metal cations on the fluorescence intensity of both low and high molecular weight sensors has been investigated and discussed.


## 2. Experimental Part

### 2.1. Materials and Methods

4-Amino-N-allyl-1,8-naphthalimide was synthesized according to the method described previously [10]. Commercial styrene (St) was used after purification by distillation under reduced pressure. Dibenzoyl peroxide (DBP) (Fluka), crystallized from chloroform to methanol was used as an initiator of the free radical polymerization. Chloroacetyl chloride, piperidine, and dimethylamine were used as obtained from MERCK.UV/vis spectrophotometric investigations were performed using “Thermo Spectronic Unicam UV 500” spectrophotometer. The fluorescence spectra were taken from a “Cary Eclipse” spectrophotometer. All spectra were recorded using 1 cm path length synthetic quartz glass cells. Fluorescence quantum yield was determined on the basis of the absorption and fluorescence spectra, using anthracene as reference (Φ
st
=
0.27 [11]). All absorption and fluorescence measurements were carried out at 1 × 10−5mol L−1 for MDs. The polymer concentrations in the solutions for all measurements were 5 g L−1.The effect of the metal cations on fluorescence intensity has been measured by adding a few microliters of stock aqueous solution (c = 10−2mol L−1) of the metal cations to a known volume of the solution (3 mL) in acetonitrile for monomeric sensors and in aqueous solution for polymeric sensor. This addition was limited to 0.08 mL, so that dilution remained insignificant [12]. For all absorbance and fluorescence measurements the polymer thin film was placed diagonally in the sample quartz cuvette to improve measurement reproducibility. The reproducibility of the results was 99%. MgCl2·6H2O, Pb (NO3)2, SrCl2, FeCl3·6H2O, AgNO3, CuSO4·5H2O, and Co (NO3)2·6H2O were investigated as sources of metal cations.IR analysis of compounds was carried out using the infrared Fourier transform spectrometer (IRAffinity-1 “Shimadzu”) with the diffuse-reflectance attachment (MIRacle Attenuated Total Reflectance Attachment). The NMR spectra were obtained from a Bruker DRX-250 spectrometer, operating at 250.13 and 62.90 MHz for1H and 13C, respectively, using a dual 5 mm probe head. Deuteriochloroform and tetramethylsilane were used as a solvent and an internal standard.Thin layer chromatographic (TLC) analysis of the monomeric dyes was followed on silica gel (Fluka F60 254 20
×
20; 0.2 mm) using the solvent system n-heptane/acetone (1 : 1) as an eluent.The molecular characteristics of the poly(St-co-MD) were determined on a GPC Water 244 apparatus. The solvent was THF at a flow rate of 1.0 mL min−1 at 45°C. Both a differential refractive index and an UV/vis absorption detector (λ
A
=
375 nm) were used. Polystyrene calibration was used for all molecular weight calculations.


### 2.2. General Procedure for Synthesis of Monomeric Dyes MD1 and MD2 (Scheme1)

Scheme 1
Synthesis of monomeric MD1 and MD2.4-Amino-N-allyl-1,8-naphthalimide (0.01 mol) was dissolved in 50 mL of acetic acid and at 50°C 2 mL chloroacetyl chloride was added dropwise. The mixture was stirred at this temperature and after 2 h the product was isolated by pouring it into water and filtrated. After that 0.01 mol of this product was dissolved in dioxane and 0.05 mol of amines was added and stirred at 80°C for 4 h. The final products have been isolated with high yields and purity.


#### 2.2.1. Characterization of MD1

Yield 89%.
FTIR (KBr) cm−1: 3248, 2935, 2818, 1692, 1651, 1614, 1538, 1380, 1235, 781.
1H-NMR (CHCl3) δ (ppm): 10.54 (1H, NH); 8.65–8.44 (dd, 3H, Ar); 8.33–8.29 (d, 1H, Ar); 7.82–7.76 (t, 1H, Ar); 6.08–5.92 (m, 1H, CH=); 5.36–5.17 (dd, 1H, CH=); 4.81–4.79 (d, CH
2–CH=); 3.49 (s, 2H, CO–CH2–); 2.66 (s, 6H, CH3).
13C-NMR (CHCl3) δ (ppm): 171.9, 165.1, 164.9, 140.6, 133.7, 133.0, 132.3, 129.9, 128.0, 125.2, 124, 8, 120.2, 117.6, 64.3, 48.3, 46.2, 39.6.
Analysis: C19H19N3O3 (337.22 g mol−1): Calc. (%): C-67.67, H 5.63, N 12.46.
Found (%): C-67.44, H 5.69, N 12.39.


#### 2.2.2. Characterization of MD2

Yield 92%.
FTIR (KBr) cm−1: 3223, 2946, 2838, 1693, 1656, 1620, 1532, 1379, 1237, 777.
1H-NMR (CHCl3) δ (ppm): s 10.44 (1H, NH); 8.66–8.58 (dd, 3H, Ar); 8.29–8.20 (d, 1H, Ar); 7.85–7.79 (t, 1H, Ar); 6.08–5.92 (m, 1H, CH–CH2); 5.36–5.20 (dd, 2H, CH
2=CH), 4.81–4.79 (d, 2H, CH2–CH); 3.92 (s, 4H, CH2–N–CH2); 3.42 (s, 2H, –CH2–CO); 3.01 (s, 4H, CH2–O–CH2).
13C-NMR (CHCl3) δ (ppm): 164.1, 163.2, 162.3, 150.3, 134.1, 130.5, 129.5, 128.3, 127.8, 124.2, 121.9, 120.0, 107.7, 103.3, 55.8, 45.2, 44.4, 39.4, 30.8.
Analysis: C21H21N3O4 (379.24 g mol−1): Calc. (%): C-66.50, H 5.54, N 11.08.
Found (%): C-66.84, H 5.48, N 11.19.


### 2.3. Copolymerization

Free radical copolymerization of styrene with MDs was carried out in bulk [13]. 9.80 g styrene, 0.20 g of monomer MD, and 0.05 g DBP were mixed in an ampoule flushed with pure dry nitrogen. The ampoule was sealed and heated at 80°C in a thermostat for 8 h. The side-chain copolymers thus obtained were several times precipitated with ethanol from the chloroform. The precipitated copolymers were repeatedly washed with ethanol, recovered by filtration, and dried in vacuum to constant weight. Transparent fluorescent copolymers of blue emission were obtained. All spectrophotometric measurements were carried out with precipitated coloured polymers. Thin polymeric film used for the fluorescent investigations was obtained from deposition of a 10% solution of the copolymer in chloroform on glass surface. The thickness of the copolymer film was 40 μm, determined by microscope technique.


## 2.1. Materials and Methods

4-Amino-N-allyl-1,8-naphthalimide was synthesized according to the method described previously [10]. Commercial styrene (St) was used after purification by distillation under reduced pressure. Dibenzoyl peroxide (DBP) (Fluka), crystallized from chloroform to methanol was used as an initiator of the free radical polymerization. Chloroacetyl chloride, piperidine, and dimethylamine were used as obtained from MERCK.UV/vis spectrophotometric investigations were performed using “Thermo Spectronic Unicam UV 500” spectrophotometer. The fluorescence spectra were taken from a “Cary Eclipse” spectrophotometer. All spectra were recorded using 1 cm path length synthetic quartz glass cells. Fluorescence quantum yield was determined on the basis of the absorption and fluorescence spectra, using anthracene as reference (Φ
st
=
0.27 [11]). All absorption and fluorescence measurements were carried out at 1 × 10−5mol L−1 for MDs. The polymer concentrations in the solutions for all measurements were 5 g L−1.The effect of the metal cations on fluorescence intensity has been measured by adding a few microliters of stock aqueous solution (c = 10−2mol L−1) of the metal cations to a known volume of the solution (3 mL) in acetonitrile for monomeric sensors and in aqueous solution for polymeric sensor. This addition was limited to 0.08 mL, so that dilution remained insignificant [12]. For all absorbance and fluorescence measurements the polymer thin film was placed diagonally in the sample quartz cuvette to improve measurement reproducibility. The reproducibility of the results was 99%. MgCl2·6H2O, Pb (NO3)2, SrCl2, FeCl3·6H2O, AgNO3, CuSO4·5H2O, and Co (NO3)2·6H2O were investigated as sources of metal cations.IR analysis of compounds was carried out using the infrared Fourier transform spectrometer (IRAffinity-1 “Shimadzu”) with the diffuse-reflectance attachment (MIRacle Attenuated Total Reflectance Attachment). The NMR spectra were obtained from a Bruker DRX-250 spectrometer, operating at 250.13 and 62.90 MHz for1H and 13C, respectively, using a dual 5 mm probe head. Deuteriochloroform and tetramethylsilane were used as a solvent and an internal standard.Thin layer chromatographic (TLC) analysis of the monomeric dyes was followed on silica gel (Fluka F60 254 20
×
20; 0.2 mm) using the solvent system n-heptane/acetone (1 : 1) as an eluent.The molecular characteristics of the poly(St-co-MD) were determined on a GPC Water 244 apparatus. The solvent was THF at a flow rate of 1.0 mL min−1 at 45°C. Both a differential refractive index and an UV/vis absorption detector (λ
A
=
375 nm) were used. Polystyrene calibration was used for all molecular weight calculations.


## 2.2. General Procedure for Synthesis of Monomeric Dyes MD1 and MD2 (Scheme1)

Scheme 1
Synthesis of monomeric MD1 and MD2.4-Amino-N-allyl-1,8-naphthalimide (0.01 mol) was dissolved in 50 mL of acetic acid and at 50°C 2 mL chloroacetyl chloride was added dropwise. The mixture was stirred at this temperature and after 2 h the product was isolated by pouring it into water and filtrated. After that 0.01 mol of this product was dissolved in dioxane and 0.05 mol of amines was added and stirred at 80°C for 4 h. The final products have been isolated with high yields and purity.


### 2.2.1. Characterization of MD1

Yield 89%.
FTIR (KBr) cm−1: 3248, 2935, 2818, 1692, 1651, 1614, 1538, 1380, 1235, 781.
1H-NMR (CHCl3) δ (ppm): 10.54 (1H, NH); 8.65–8.44 (dd, 3H, Ar); 8.33–8.29 (d, 1H, Ar); 7.82–7.76 (t, 1H, Ar); 6.08–5.92 (m, 1H, CH=); 5.36–5.17 (dd, 1H, CH=); 4.81–4.79 (d, CH
2–CH=); 3.49 (s, 2H, CO–CH2–); 2.66 (s, 6H, CH3).
13C-NMR (CHCl3) δ (ppm): 171.9, 165.1, 164.9, 140.6, 133.7, 133.0, 132.3, 129.9, 128.0, 125.2, 124, 8, 120.2, 117.6, 64.3, 48.3, 46.2, 39.6.
Analysis: C19H19N3O3 (337.22 g mol−1): Calc. (%): C-67.67, H 5.63, N 12.46.
Found (%): C-67.44, H 5.69, N 12.39.


### 2.2.2. Characterization of MD2

Yield 92%.
FTIR (KBr) cm−1: 3223, 2946, 2838, 1693, 1656, 1620, 1532, 1379, 1237, 777.
1H-NMR (CHCl3) δ (ppm): s 10.44 (1H, NH); 8.66–8.58 (dd, 3H, Ar); 8.29–8.20 (d, 1H, Ar); 7.85–7.79 (t, 1H, Ar); 6.08–5.92 (m, 1H, CH–CH2); 5.36–5.20 (dd, 2H, CH
2=CH), 4.81–4.79 (d, 2H, CH2–CH); 3.92 (s, 4H, CH2–N–CH2); 3.42 (s, 2H, –CH2–CO); 3.01 (s, 4H, CH2–O–CH2).
13C-NMR (CHCl3) δ (ppm): 164.1, 163.2, 162.3, 150.3, 134.1, 130.5, 129.5, 128.3, 127.8, 124.2, 121.9, 120.0, 107.7, 103.3, 55.8, 45.2, 44.4, 39.4, 30.8.
Analysis: C21H21N3O4 (379.24 g mol−1): Calc. (%): C-66.50, H 5.54, N 11.08.
Found (%): C-66.84, H 5.48, N 11.19.


## 2.2.1. Characterization of MD1

Yield 89%.
FTIR (KBr) cm−1: 3248, 2935, 2818, 1692, 1651, 1614, 1538, 1380, 1235, 781.
1H-NMR (CHCl3) δ (ppm): 10.54 (1H, NH); 8.65–8.44 (dd, 3H, Ar); 8.33–8.29 (d, 1H, Ar); 7.82–7.76 (t, 1H, Ar); 6.08–5.92 (m, 1H, CH=); 5.36–5.17 (dd, 1H, CH=); 4.81–4.79 (d, CH
2–CH=); 3.49 (s, 2H, CO–CH2–); 2.66 (s, 6H, CH3).
13C-NMR (CHCl3) δ (ppm): 171.9, 165.1, 164.9, 140.6, 133.7, 133.0, 132.3, 129.9, 128.0, 125.2, 124, 8, 120.2, 117.6, 64.3, 48.3, 46.2, 39.6.
Analysis: C19H19N3O3 (337.22 g mol−1): Calc. (%): C-67.67, H 5.63, N 12.46.
Found (%): C-67.44, H 5.69, N 12.39.


## 2.2.2. Characterization of MD2

Yield 92%.
FTIR (KBr) cm−1: 3223, 2946, 2838, 1693, 1656, 1620, 1532, 1379, 1237, 777.
1H-NMR (CHCl3) δ (ppm): s 10.44 (1H, NH); 8.66–8.58 (dd, 3H, Ar); 8.29–8.20 (d, 1H, Ar); 7.85–7.79 (t, 1H, Ar); 6.08–5.92 (m, 1H, CH–CH2); 5.36–5.20 (dd, 2H, CH
2=CH), 4.81–4.79 (d, 2H, CH2–CH); 3.92 (s, 4H, CH2–N–CH2); 3.42 (s, 2H, –CH2–CO); 3.01 (s, 4H, CH2–O–CH2).
13C-NMR (CHCl3) δ (ppm): 164.1, 163.2, 162.3, 150.3, 134.1, 130.5, 129.5, 128.3, 127.8, 124.2, 121.9, 120.0, 107.7, 103.3, 55.8, 45.2, 44.4, 39.4, 30.8.
Analysis: C21H21N3O4 (379.24 g mol−1): Calc. (%): C-66.50, H 5.54, N 11.08.
Found (%): C-66.84, H 5.48, N 11.19.


## 2.3. Copolymerization

Free radical copolymerization of styrene with MDs was carried out in bulk [13]. 9.80 g styrene, 0.20 g of monomer MD, and 0.05 g DBP were mixed in an ampoule flushed with pure dry nitrogen. The ampoule was sealed and heated at 80°C in a thermostat for 8 h. The side-chain copolymers thus obtained were several times precipitated with ethanol from the chloroform. The precipitated copolymers were repeatedly washed with ethanol, recovered by filtration, and dried in vacuum to constant weight. Transparent fluorescent copolymers of blue emission were obtained. All spectrophotometric measurements were carried out with precipitated coloured polymers. Thin polymeric film used for the fluorescent investigations was obtained from deposition of a 10% solution of the copolymer in chloroform on glass surface. The thickness of the copolymer film was 40 μm, determined by microscope technique.


## 3. Results and Discussions

### 3.1. Photophysical Characteristics of Monomeric and Polymeric Fluorophores

The photophysical properties of 1,8-naphthalimide are known to depend mainly on the polarization of its chromophore system. In this study the functional properties of MDs were investigated in organic solvents of different polarity. Tables1 and 2 summarize the basic photophysical characteristics of MDs—absorption (λ
A) and fluorescence (λ
F) maxima, Stokes shift (
ν
A
-
ν
F
), oscillator strength (f), quantum yield of fluorescence (Φ
F), and energetic yield of fluorescence (E
F).Table 1
Photophysical characteristics of the MD1 in organic solvents of different polarities (see text).
Solvent
λ
abs (nm)
λ
flu (nm)
ε (L mol−1 cm−1)
ν
A
-
ν
F (cm−1)
Φ
F
E
F
f
Dimethyl sulfoxide
375
458
11100
4833
0.03
0.03
0.12
Dimethylformamide
374
452
11900
4614
0.03
0.05
0.12
Acetonitrile
371
452
13000
4830
0.07
0.09
0.14
Methanol
366
463
11900
5724
0.03
0.03
0.15
Ethanol
370
458
12000
5193
0.04
0.04
0.14
Acetone
372
450
12700
4660
0.01
0.02
0.13
Dichloromethane
374
445
13100
4266
0.05
0.09
0.12
Tetrahydrofuran
373
442
11500
4185
0.10
0.18
0.10
Chloroform
374
440
11700
4215
0.08
0.16
0.11Table 2
Photophysical characteristics of the MD2 in organic solvents of different polarities (see text).
Solvent
λ
abs (nm)
λ
flu (nm)
ε (L mol−1 cm−1)
ν
A
-
ν
F (cm−1)
Φ
F
E
F
f
Dimethyl sulfoxide
375
451
11400
4494
0.04
0.02
0.11
Dimethylformamide
374
448
12500
4417
0.06
0.03
0.12
Acetonitrile
372
434
13200
3840
0.11
0.05
0.11
Methanol
366
458
12300
5488
0.04
0.03
0.15
Ethanol
370
450
11500
4805
0.05
0.03
0.12
Acetone
372
434
12400
3840
0.02
0.01
0.10
Dichloromethane
375
451
13400
4494
0.10
0.04
0.13
Tetrahydrofuran
373
434
11500
3768
0.20
0.09
0.09
Chloroform
375
445
12400
4195
0.19
0.06
0.11In all organic solvents under study, the monomeric 1,8-naphthalimides are colourless absorbing in the ultraviolet region at 366–375 nm and emit blue fluorescence at 434–463 nm. The results show that the substituents in C-4 position do not affect the maxima positions significantly.The Stokes shift is a parameter, which indicates the difference in the properties and structure of the fluorophore between the ground stateS
0 and the first excited state S
1 (1). Consider the following:
(1)
(
ν
A
-
ν
F
)
=
(
1
λ
A
-
1
λ
F
)
×
10
7
(
c
m
-
1
)
.The Stokes shift values clearly depend strongly on the solvent polarityd. It is seen that the values are higher when alcohols are used as solvents and they were very similar to those of other monomeric 1,8-naphthalimide dyes [14–16]. The Stokes shift of the MD1 has relatively high values when compared to MD2, which is probably due to the conformational changes or electron density redistribution upon excitation.The ability of the MD molecules to emit absorbed light energy is characterized quantitatively by the quantum yield of fluorescence ΦF. The quantum fluorescence yield of MDs in all organic solvents was calculated on the basis of the absorption and fluorescence spectra using
(2)
Φ
F
=
Φ
st
S
u
S
st
A
st
A
u
n
D
u
2
n
D
st
2
,
where Φst is the quantum yield of the reference, A
st and A
u represent the absorbance of the reference and the sample, respectively, S
st and S
u are the integrals of the emission of the reference and the sample, respectively, and n
D
st and n
D
u are the refractive index of the reference and the sample, respectively.As seen from the data in Tables1 and 2, the MDs quantum yield depends on the solvent polarity also. The quantum yield is considerably higher in nonpolar media. In polar organic solvents, the MDs exhibit much weaker emission. In all cases their fluorescence is not strong which can be explained by the conformation change.An important characteristic of MDs is the oscillator strength (f); it reveals the effective number of electrons whose transition from the ground state S
0 to the excited S
1 state gives the absorption area in the spectrum. Values of the oscillator strength can be calculated using
(3)
f
=
4.32
×
10
-
9
Δ
ν
1
/
2
ε
max
,
where the Δν
1/2 is the width of the absorption band (in cm−1) at 1/2 ε
max.The values obtained forf for MD1 are 0.10 (tetrahydrofuran) and 0.14 (acetonitrile). The higher values in acetonitrile correlate well with the hypsochromic effect of the MD1 in this solvent. The similar behavior has been observed also in the case of MD2.The spectral characteristics of poly(St-co-MD) in the solid state are of interest in order to evaluate this copolymer as a heterogeneous fluorescent sensor. The copolymer was transparent and colourless, emitting blue fluorescence. The absorption and fluorescence spectra of poly(St-co-MD) in the solid state as a thin polymer film (d
=
40 μm) are presented in Figure 1, from which it is evident that the excitation and fluorescence spectra have bands with a single maximum at 365 nm and 450 nm, respectively. The spectral characteristics of the former reveal that the chemical structure of the chromophoric system does not change its conformation in the solid state.Figure 1
Absorption and fluorescence spectra of poly(St-co-MD2) in solid state as a thin polymer film (d
=
40 μm).


### 3.2. Molecular Weight and Spectral Characteristics of Poly(St-co-MD)

The amount of MDs incorporated into the polymer macromolecules has been determined spectrophotometrically by using a standard curve [17]. The results show that 1.53 wt% for MD1 and 1.45 wt% for MD2 have bonded to the polymer chain. Considering that the value was obtained for repeatedly precipitated copolymer where low molecular weight fractions have been removed during precipitation, the results are rather satisfactory and imply that the MDs are suitable for production of a blue fluorescent copolymer of polystyrene. This fact also demonstrated that some amount from MDs has been bonded to the low molar weight fractions of the polymer chains.The molecular weight characteristics of the copolymers obtained are collected in Table3. The molecular weight and molecular weight distribution confirm the formation of high molecular weight polymers. The molecular weights were found to range between M
w
=
1.11 and 1.34 × 10−5 and M
n
=
0.68
-
0
.
75
×
10
-
5 for copolymers with polydispersity M
w
/
M
n 1.63 and 1.78, respectively. The double detection shows close values for the elution time in both chromatograms indicating the presence of copolymers which absorb at about 375 nm in tetrahydrofuran solution.Table 3
Molecular weight and spectral characteristics in tetrahydrofuran solution of the copolymers (see text).
M
w
×
10
-
5
M
n
×
10
-
5
M
w
/
M
n
λ
A (nm)
λ
F (nm)
(ν
E
-
ν
F) cm−1
Poly(St-co-MD1)
1.11
0.68
1.63
375
421
2914
Poly(St-co-MD2)
1.34
0.75
1.78
373
428
3446


## 3.1. Photophysical Characteristics of Monomeric and Polymeric Fluorophores

The photophysical properties of 1,8-naphthalimide are known to depend mainly on the polarization of its chromophore system. In this study the functional properties of MDs were investigated in organic solvents of different polarity. Tables1 and 2 summarize the basic photophysical characteristics of MDs—absorption (λ
A) and fluorescence (λ
F) maxima, Stokes shift (
ν
A
-
ν
F
), oscillator strength (f), quantum yield of fluorescence (Φ
F), and energetic yield of fluorescence (E
F).Table 1
Photophysical characteristics of the MD1 in organic solvents of different polarities (see text).
Solvent
λ
abs (nm)
λ
flu (nm)
ε (L mol−1 cm−1)
ν
A
-
ν
F (cm−1)
Φ
F
E
F
f
Dimethyl sulfoxide
375
458
11100
4833
0.03
0.03
0.12
Dimethylformamide
374
452
11900
4614
0.03
0.05
0.12
Acetonitrile
371
452
13000
4830
0.07
0.09
0.14
Methanol
366
463
11900
5724
0.03
0.03
0.15
Ethanol
370
458
12000
5193
0.04
0.04
0.14
Acetone
372
450
12700
4660
0.01
0.02
0.13
Dichloromethane
374
445
13100
4266
0.05
0.09
0.12
Tetrahydrofuran
373
442
11500
4185
0.10
0.18
0.10
Chloroform
374
440
11700
4215
0.08
0.16
0.11Table 2
Photophysical characteristics of the MD2 in organic solvents of different polarities (see text).
Solvent
λ
abs (nm)
λ
flu (nm)
ε (L mol−1 cm−1)
ν
A
-
ν
F (cm−1)
Φ
F
E
F
f
Dimethyl sulfoxide
375
451
11400
4494
0.04
0.02
0.11
Dimethylformamide
374
448
12500
4417
0.06
0.03
0.12
Acetonitrile
372
434
13200
3840
0.11
0.05
0.11
Methanol
366
458
12300
5488
0.04
0.03
0.15
Ethanol
370
450
11500
4805
0.05
0.03
0.12
Acetone
372
434
12400
3840
0.02
0.01
0.10
Dichloromethane
375
451
13400
4494
0.10
0.04
0.13
Tetrahydrofuran
373
434
11500
3768
0.20
0.09
0.09
Chloroform
375
445
12400
4195
0.19
0.06
0.11In all organic solvents under study, the monomeric 1,8-naphthalimides are colourless absorbing in the ultraviolet region at 366–375 nm and emit blue fluorescence at 434–463 nm. The results show that the substituents in C-4 position do not affect the maxima positions significantly.The Stokes shift is a parameter, which indicates the difference in the properties and structure of the fluorophore between the ground stateS
0 and the first excited state S
1 (1). Consider the following:
(1)
(
ν
A
-
ν
F
)
=
(
1
λ
A
-
1
λ
F
)
×
10
7
(
c
m
-
1
)
.The Stokes shift values clearly depend strongly on the solvent polarityd. It is seen that the values are higher when alcohols are used as solvents and they were very similar to those of other monomeric 1,8-naphthalimide dyes [14–16]. The Stokes shift of the MD1 has relatively high values when compared to MD2, which is probably due to the conformational changes or electron density redistribution upon excitation.The ability of the MD molecules to emit absorbed light energy is characterized quantitatively by the quantum yield of fluorescence ΦF. The quantum fluorescence yield of MDs in all organic solvents was calculated on the basis of the absorption and fluorescence spectra using
(2)
Φ
F
=
Φ
st
S
u
S
st
A
st
A
u
n
D
u
2
n
D
st
2
,
where Φst is the quantum yield of the reference, A
st and A
u represent the absorbance of the reference and the sample, respectively, S
st and S
u are the integrals of the emission of the reference and the sample, respectively, and n
D
st and n
D
u are the refractive index of the reference and the sample, respectively.As seen from the data in Tables1 and 2, the MDs quantum yield depends on the solvent polarity also. The quantum yield is considerably higher in nonpolar media. In polar organic solvents, the MDs exhibit much weaker emission. In all cases their fluorescence is not strong which can be explained by the conformation change.An important characteristic of MDs is the oscillator strength (f); it reveals the effective number of electrons whose transition from the ground state S
0 to the excited S
1 state gives the absorption area in the spectrum. Values of the oscillator strength can be calculated using
(3)
f
=
4.32
×
10
-
9
Δ
ν
1
/
2
ε
max
,
where the Δν
1/2 is the width of the absorption band (in cm−1) at 1/2 ε
max.The values obtained forf for MD1 are 0.10 (tetrahydrofuran) and 0.14 (acetonitrile). The higher values in acetonitrile correlate well with the hypsochromic effect of the MD1 in this solvent. The similar behavior has been observed also in the case of MD2.The spectral characteristics of poly(St-co-MD) in the solid state are of interest in order to evaluate this copolymer as a heterogeneous fluorescent sensor. The copolymer was transparent and colourless, emitting blue fluorescence. The absorption and fluorescence spectra of poly(St-co-MD) in the solid state as a thin polymer film (d
=
40 μm) are presented in Figure 1, from which it is evident that the excitation and fluorescence spectra have bands with a single maximum at 365 nm and 450 nm, respectively. The spectral characteristics of the former reveal that the chemical structure of the chromophoric system does not change its conformation in the solid state.Figure 1
Absorption and fluorescence spectra of poly(St-co-MD2) in solid state as a thin polymer film (d
=
40 μm).


## 3.2. Molecular Weight and Spectral Characteristics of Poly(St-co-MD)

The amount of MDs incorporated into the polymer macromolecules has been determined spectrophotometrically by using a standard curve [17]. The results show that 1.53 wt% for MD1 and 1.45 wt% for MD2 have bonded to the polymer chain. Considering that the value was obtained for repeatedly precipitated copolymer where low molecular weight fractions have been removed during precipitation, the results are rather satisfactory and imply that the MDs are suitable for production of a blue fluorescent copolymer of polystyrene. This fact also demonstrated that some amount from MDs has been bonded to the low molar weight fractions of the polymer chains.The molecular weight characteristics of the copolymers obtained are collected in Table3. The molecular weight and molecular weight distribution confirm the formation of high molecular weight polymers. The molecular weights were found to range between M
w
=
1.11 and 1.34 × 10−5 and M
n
=
0.68
-
0
.
75
×
10
-
5 for copolymers with polydispersity M
w
/
M
n 1.63 and 1.78, respectively. The double detection shows close values for the elution time in both chromatograms indicating the presence of copolymers which absorb at about 375 nm in tetrahydrofuran solution.Table 3
Molecular weight and spectral characteristics in tetrahydrofuran solution of the copolymers (see text).
M
w
×
10
-
5
M
n
×
10
-
5
M
w
/
M
n
λ
A (nm)
λ
F (nm)
(ν
E
-
ν
F) cm−1
Poly(St-co-MD1)
1.11
0.68
1.63
375
421
2914
Poly(St-co-MD2)
1.34
0.75
1.78
373
428
3446


## 4. Effect of the Metal Cations on the Fluorescence Intensity of the MDs

The photophysical properties of MDs in the presence of different metal cations (Ag+, Mg2+, Cu2+, Sr2+, Co2+, Pb2+, and Fe3+) have been investigated in the view of their its potential sensor application. The ability of both MDs to detect metal cations has been tested in acetonitrile solution by monitoring the changes in their absorption and fluorescence spectra in the presence of various metal cations. Acetonitrile was chosen as solvent for all spectral measurements as it guarantee good solubility of the metal salts, ligands, and the respective complexes. Its ability to mix well with water allows direct usage of aqueous solutions of the metal salts in this study.In the presence of the guest metal cations an enhancement or quenching of fluorescence intensity was observed. The enhancement (FE) and the quenching (FQ) of the fluorescence emission have been used as a qualitative parameter for the detection of metal cations. FE =I
/
I
0 was determined from the ratio of maximum fluorescence intensity I, after the addition of metal cation, and minimum fluorescence intensity I
0, before metal cation addition. The FQ = I
0
/
I has been determined from the ratio between the maximum fluorescence intensity (I
0, solution free of metal cations) and the fluorescence intensity in the presence of metal cations (
I
).Figures2 and 3 present the calculated FQ and FE results for MD1 and MD2.Figure 2
Effect of the metal cations at concentrationc
=
10
-
5 mol L−1 on the fluorescence of MD1 in acetonitrile solution.Figure 3
Fluorescence quenching factor of MD2 in the presence of different metal cations (c
=
2
×
10
-
5 mol L−1) in acetonitrile solution.The highest enhancement of the monomer fluorescence intensity is observed in the presence of Fe3+ cations for compound MD1 (FE = 16.42) as can be seen from Figure 2. In the presence of Pb2+cations MD1 increases the fluorescence intensity with the respective FE = 9.05. The influence of the other cations under study (Mg2+> Co2+> Sr2+> Ag+> Cu2+) on the fluorescence intensity is negligible.Figure3 shows the fluorescence quenching of MD2 upon the addition of cations. As seen the strongest effect is again observed for Fe3+. In this case the complexation with Fe3+cations destabilizes the planarity of the 1,8-naphthalimide molecule and as a result the fluorescence is quenched, while Pb2+, Mg2+, Co2+, Sr2+, Cu2+, and Ag+ cations do not affect the fluorescence intensity of the MD2. Probably MD2 does not form a stable complex with these cations.


## 5. Effect of the Metal Cations on the Fluorescence of Poly(St-co-MDs)

The presence of the guest metal cations (Cu2+, Sr2+, Co2+, Ni2+, and Fe3+) in poly(St-co-MD) solution in this work is signaled by the quenching of the fluorescence intensity. The changes of the fluorescence intensity of poly(St-co-MD1) in aqueous solution, induced by the metal cations, have been investigated and the respective fluorescence responses of a polymer chromophore are presented in Figure 4. As it can be seen the addition of metal cations leads to a decrease of the polymer fluorescence intensity, different for each metal cation. In the case of Cu2+, Sr2+, Co2+, and Ni2+, the effect of metal cations on the fluorescence intensity is insignificant and the respective alteration of the fluorescent intensity is only 1–5%. The highest effect was observed in the presence of Fe3+ cations. In this case the quenching of the fluorescence intensity is 96%. A similar effect has been observed and in the case of poly(St-co-MD2) also. It reveals the good potential of both polymers as effective heterogeneous sensors for detection of Fe3+ ions in aqueous solutions even in the presence of other metal ions. These results were in good accordance with our other studies using polymer sensors for detecting metal ions in aqueous media [5–7]. In the form of solid polymer film these heterogeneous sensors can be used repeatedly for detection in aqueous solutions after prior removal of the coordinated metal ions.Figure 4
Effect of the metal cations at concentrationc = 2 × 10−4mol L−1 on the fluorescence of poly(St-co-MD1) in aqueous solution.The typical change in the fluorescence intensity of the copolymer induced by Fe3+ cations has been presented in Figure 5. The decrease of fluorescence intensity occurs after the addition of Fe3+ cations up to 2 × 10−4M. It is seen that the initial addition of the Fe3+ cations (5 × 10−5M) to the polymer leads to a decrease of the fluorescent intensity and the respective quenching effect is 31% which indicates very good sensor sensitivity. Further addition of the Fe3+ cations into the polymer solution decreases the fluorescence intensity more as can be seen in Figure 5. At high metal concentrations the fluorescence quenching is not full, which is probably due to a competition between the metal cations and the respective counterions from the solution for coordination with the chromophore site.Figure 5
The influence of Fe3+ cations on the fluorescence intensity of the poly(St-co-MD1) at different concentrations of Fe3+ in aqueous solution.


## 6. Conclusion

In this paper we discuss the synthesis and some functional properties of two new blue fluorescent polymerizable 1,8-naphthalimides and their copolymers with styrene. The photophysical characteristics of both low and high molecular weight fluorophores have been investigated. The influence of various metal cations (Ag+, Mg2+, Cu2+, Sr2+, Co2+, Pb2+, and Fe3+) on the fluorescence intensity of the new 1,8-naphthalimides has been studied with regard to their potential application as fluorescent sensors for metal ions. It has been shown that the fluorescence intensity depends strongly on the nature of metal cations. The new monomer compounds can detect Pb2+ and Fe3+. It has been shown that the blue fluorescent polymer films possess properties allowing their use as sensors for Fe3+ cations. On the basis of the present investigation it can be assumed that the new monomers and fluorescent copolymers are suitable for the selective detection of Fe3+cations.



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*Source: 793721-2014-01-05.xml*