# A BTT-Based Colorimetric Dual Sensor for Hg(II) and Selected Anions with Molecular Logic Operations

Authors: Veikko Uahengo; Ping Cai; Likius S. Daniel
Journal: Advances in Chemistry
 (2016)

---

## Abstract

A benzotrithiophenes (BTT) based colorimetric sensor (2) was synthesized via a simple one-step reaction process, and its recognition properties towards several biologically important anions and cations were investigated by naked eye observation and spectroscopic methods of UV-vis and 1H NMR analysis in DMSO. The molar addition of anions such as F−, AcO−, and H
2
P
O
4
- induced a marked red shift of the charge transfer band (Δ
λ
=
94 nm, from 440 nm to 534 nm) concomitant with a clearly visible “naked eye” detectable colorimetric activities (from orange to pink). However, the molar addition of H
2
P
O
4
- did not induce significant spectral changes, compared to F− and AcO−. Furthermore, the molar addition of Hg2+ to2 resulted in hypochromic shift at 440 nm and the eventual disappearance of a low energy band at 534 nm, concomitant with the colorimetric activities (from orange to yellow). Moreover, both spectral and color changes induced by the addition of anions (F− and AcO−) were all reversible by the molar addition of metal cations of 3
d
5
–
10. The reversibility properties triggered the logic operation studies, and, subsequently, the complementary IMP/INH logic functions based on color and spectral switching (ON/OFF) were confirmed. Conclusively,2 can thus be utilized as a colorimetric molecular switch modulated by AcO−/M
I
I.


---

## Body

## 1. Introduction

Thiophene-basedπ-conjugated polymers and their derivatives have been attracting attention in organic electronic devices such as organic light emitting diodes (OLED), organic field effect transistors (OFET), organic photovoltaics (OPV), and electrochromics [1–10]. These functionalities are due to the disk-shaped planar conformation with rigid π-electron framework, which facilitate strong intermolecular interactions that are suitable for developing organic semiconductor materials. Benzotrithiophenes (BTT) are very unique due to their rare structure ofC
3h symmetry with three identical thiophene groups resulting in a possible 3-dimensional star-shaped structure. In fact, the star-shaped conformation has attracted much attention in recent times, especially in the field of organic semiconductors, due to its planarity, delocalized π-electron system, and highly organized 2-dimensional network, and it reportedly possesses high thermal stability [11–23].However, despite their excellent fluorescent and polymerization properties, thiophene-based compounds have rarely been used in the development of chemosensors [24–31]. In theory, thiophene-based compounds can be very ideal for excellent sensor in designing, based on their structural engineering or/and manipulation, especially their disc-shape planar structure, presenting an ideal platform for smooth electronic communications. For instance, BTT with its π-electron framework is potentially likely to make an excellent chemosensor, especially when it is coupled with a powerful electron withdrawing group (EWG) such as the nitro group (–NO2), fittingly resulting in a moiety with strong electronic coupling, from the receptor to the reporting unit. Hydrazone-based sensors for acetate and fluoride ions have been widely reported in literature, with the –NH protons acidity enhanced by the presence of powerful electron withdrawing groups, like NO2 and CF3 [32–37]. By using the principles of coupling a BTT, a strong electron donating group (EDG) itself, to another strong EWG with relatively low LUMO level such as dinitrophenylhydrazine, is highly likely to produce a chemosensor with remarkable dynamic electronic communication. Moreover, the presence of soft (donor) atoms such as sulphur in the ring raises the prospect of dual sensing, for both cations and anions, which stems from the presence of both the anion receptors (–NH) and the cationphilic (e.g., Hg2+ and Zn2+) thiophene group in the structure. In literature, it has been well documented that dual sensing systems are highly likely to display molecular logic operation properties.In recent years, developments in supramolecular chemistry fields have shown that chemosensors can act as useful tools in information processing and computation at molecular level. In these systems, the chemically coded information is normally converted into optical changes as the output through electronic communications, generally between the receptor and the reporter units of the structure. Even though literature has reported a number of different molecular logic gates such as AND, OR, INIHIBIT, NOR, IMPLICATION, XOR, YES, NOT, NAND, and XNOR [29], combinatorial logic gates having complementary IMP/INH logic functions remain rare and elusive. The reported systems are generally devised by the modulation of either the emission properties or colorimetric changes and restored by different combinations of specific ionic species [38–44].As a tributary of supramolecular chemistry, chemosensors are designed for a specific function based on complementary topological geometries and chemical properties of the target species. The significance of sensing of biologically important anions such as acetate, fluoride, and dihydrogen phosphate [29, 32–37] has been reported and highlighted in literature, and the same can be said for cations such as mercury, copper, and zinc [45–49]. However, ideal sensors with satisfactory performances, especially with combinatorial logic functions, still remain to be desired. Here we report on a two-way sensor based on a BTT-dinitrophenylhydrazone receptor (2) in Scheme 1, a dual colorimetric sensor selective to both cations (Hg2+) and anions (AcO−, F−, and partially H
2
P
O
4
-). In addition, the sensor has displayed a reversible colorimetric system based on two inputs F−/Zn2+ complementary IMPLICATION/INHIBITION (IMP/INH) logic functions.Scheme 1
Synthetic route and the structure of2.


## 2. Experimental

### 2.1. Instruments

1H NMR spectra were acquired on a Varian Mercury VX-300 MHz spectrometer. UV-vis spectra were recorded using a Tu-1901 UV-vis spectrophotometer (1 cm quartz cell) at 25°C. C, H, and N elemental analyses were acquired on a Perkin-Elmer 240C analytical instrument.


### 2.2. Materials

Commercially available chemicals were used without further purification and were all of analytical grades. All tetrabutylammonium (TBA+) salts (F−, Cl−, Br−, I−, AcO−, and H
2
P
O
4
-), hydrated metal nitrate salts (Hg2+, Zn2+, Cu2+, etc.), 1,3,5-trichlorobenzene, and all other chemicals were purchased from Sigma-Aldrich. All UV-vis titrations were performed in 1.0 × 10−5 M solution of2 in DMSO except the Job plot (1.0 × 10−4 M) or unless mentioned otherwise.


### 2.3. Synthesis and Characterization of2

The sensor (2), (E)-1-(benzo[1,2-b:3,4-b′:5,6-b′′]trithiophen-2-ylmethylene)-2-(2,4-dinitrophenyl) hydrazone, was synthesized as follows. Compound1[15, 50] (0.0176 g, 0.26 mmol) and 2,4-dinitrophenylhydrazine (0.053 g, 0.26 mmol) were dissolved in ethanol and 5 mL of H2PO4 was added. The solution mixture was refluxed while stirred magnetically for 8 h and a yellow precipitate formed. After cooling to room temperature, the yellow precipitate was washed repeatedly with small quantity of hot and then cold ethanol to yield a pure yellow solid (2). Yield was 85%. 1H NMR (300 MHz, DMSO-d) δ 11.60 (s, H
N
H), 8.86 (s, 1
H
b
e
n), 8.39 (s, 1
H
b
e
n), 8.36 (s, 1
H
C
H), 7.98 (d, 1
H
b
e
n), 7.61 (d, 2
H
t
h
i
o), 7.41 (d, 2
H
t
h
i
o), 7.39 (s, 1
H
t
h
i
o). Elemental Analysis for C19H10N4O4S3: Calculated C, 50.21%, H, 2.22%, N, 14.08%. Found C, 52.41%, H, 2.41%, N, 13.63%.


## 2.1. Instruments

1H NMR spectra were acquired on a Varian Mercury VX-300 MHz spectrometer. UV-vis spectra were recorded using a Tu-1901 UV-vis spectrophotometer (1 cm quartz cell) at 25°C. C, H, and N elemental analyses were acquired on a Perkin-Elmer 240C analytical instrument.


## 2.2. Materials

Commercially available chemicals were used without further purification and were all of analytical grades. All tetrabutylammonium (TBA+) salts (F−, Cl−, Br−, I−, AcO−, and H
2
P
O
4
-), hydrated metal nitrate salts (Hg2+, Zn2+, Cu2+, etc.), 1,3,5-trichlorobenzene, and all other chemicals were purchased from Sigma-Aldrich. All UV-vis titrations were performed in 1.0 × 10−5 M solution of2 in DMSO except the Job plot (1.0 × 10−4 M) or unless mentioned otherwise.


## 2.3. Synthesis and Characterization of2

The sensor (2), (E)-1-(benzo[1,2-b:3,4-b′:5,6-b′′]trithiophen-2-ylmethylene)-2-(2,4-dinitrophenyl) hydrazone, was synthesized as follows. Compound1[15, 50] (0.0176 g, 0.26 mmol) and 2,4-dinitrophenylhydrazine (0.053 g, 0.26 mmol) were dissolved in ethanol and 5 mL of H2PO4 was added. The solution mixture was refluxed while stirred magnetically for 8 h and a yellow precipitate formed. After cooling to room temperature, the yellow precipitate was washed repeatedly with small quantity of hot and then cold ethanol to yield a pure yellow solid (2). Yield was 85%. 1H NMR (300 MHz, DMSO-d) δ 11.60 (s, H
N
H), 8.86 (s, 1
H
b
e
n), 8.39 (s, 1
H
b
e
n), 8.36 (s, 1
H
C
H), 7.98 (d, 1
H
b
e
n), 7.61 (d, 2
H
t
h
i
o), 7.41 (d, 2
H
t
h
i
o), 7.39 (s, 1
H
t
h
i
o). Elemental Analysis for C19H10N4O4S3: Calculated C, 50.21%, H, 2.22%, N, 14.08%. Found C, 52.41%, H, 2.41%, N, 13.63%.


## 3. Results and Discussion

### 3.1. UV-Vis Titration of2 with Anions

The sensor (2) is characterized by two absorption bands in the visible region in DMSO, the high and low energy bands at 440 nm and 534 nm, respectively, ascribed to the existence of charge transfer (CT) of the electron withdrawing 2,4-dinitrophenylhydrazone moiety and the electron donating BTT unit, respectively. The molar addition of anions (AcO− and F−) to2 resulted in the intensity decrease of the band at 440 nm, while intensity increase was experienced at 534 nm as shown in Figures 1(a) and 1(b). In addition to the spectral changes, the color of2 changed from orange to purple (inset). An isosbestic point at 469 nm was indicating the existence of two distinctive species at equilibrium during the titration process. It is well known that the interaction of anions (AcO−, F−, and H
2
P
O
4
-) with hydrazone moiety is through hydrogen bonding with the NH proton in the sensor, the action ascribed to geometrical complementarity, and the chemical properties of the species [32–37]. The addition of other anions (Cl−, Br−, I−, and H
2
P
O
4
-) did not induce much significant or noticeable changes (Figure 2(c)). The glimpse on the interaction modes is suggested by the titration curves as shown in Figures 2(a) and 2(b). However, Job’s plot displays a more complex binding mode (Figure 3).Figure 1
Changes in UV-vis absorption spectra of2(1 × 10−5 M) upon the addition of 1 equiv. (a) AcO− and (b) F−, all in DMSO at 25°C.
(a)
(b)Figure 2
Titration profile on the band at 440 nm and 534 nm in (a) AcO−, (b) F−, and (c) UV-vis absorption spectra of Cl−, Br−, I−, and H
2
P
O
4
-, respectively, all in DMSO at 25°C.
(a)
(b)
(c)Figure 3
Job’s plot for (a) AcO− and (b) F−, both in DMSO at 1 × 10−4 M.
(a)
(b)


### 3.2. UV-Vis Titrations of2 with Cations

Interestingly, the addition of molar equivalents of Hg2+ to2 resulted in the color changes from yellow to light yellow (almost colorless), which was concomitant with the disappearance of the spectra band at 534 nm, while the increase in intensity was observed at 440 nm (Figure 4). The interaction is suspected to be of coordination nature involving two immediate cationphilic neighboring atoms (sulphur and nitrogen) and the mercury ion. The complementary size of Hg2+ is suspected to have played a major role in the selection preference. Conclusively, the coordination of Hg2+ to2 interferes with the intermolecular charge transfer (ICT) between the electron rich –NH and the electron deficient –NO2 at 534 nm, thereby disrupting charge transfer activities across the structural sphere, resulting in the disappearance of the peak at 534 nm. Other cations such as Cu2+ and Zn2+ showed similar effects; however, none of them were able to vanquish the band (534 nm) completely, even when huge quantities were used. However, it appears that the reversibility properties (logic operations) which are modulated by inputs (cations and anions) are stronger than the coordination interactions to some extent, as discussed in the next section.Figure 4
Changes in UV-vis absorption spectra of2(1 × 10−5 M) upon the addition of (a) 0.3 equiv. Hg2+ and (b) 4 equiv. Zn2+, all in DMSO at 25°C.
(a)
(b)


### 3.3. Reversibility and Logic Operations Studies

More details on interactions were obtained from the reversibility studies, which led to the conclusion that the reversible colorimetric activities of2 upon the addition of anions and cations resemble two inputs with complementary “IMP/INH” logic functions. The addition of anions to2 which resulted in spectral and naked eye colorimetric changes was reversed to their initial state, both spectra and color, when molar amount of cations (Zn2+) was added (Figure 5(a)). The reversible yellow-orange-yellow-orange cycles were repeated several times (4 times) by alternating addition of 2 equiv. F− and about 1.2 equiv. of Zn2+ with consistent and continuous cycles shown in Figure 5(b). The total amount of equiv. added during the four cycles was almost 1(2) : 17F− : 7Zn2+, which has little effect on the absorption intensities of2, even though the fourth cycle saw the molar amounts slightly increased, compared to the first three. Similar results to Zn2+ were obtained upon molar additions of Cu2+ in more or less equivalent ratios.Figure 5
Reversible cycles and reproducible colorimetric switch of2 (1 × 10−5 M, in DMSO) modulated by the addition of F− and Zn2+ (≃2 : 1), respectively. (a) Spectral display of the first cycle. (b) Repeating cycles.
(a)
(b)The logic operations of2 are based on the reversibility and reproducibility of colorimetric-spectral switch upon mixing right combinations of F− and Zn2+. The addition of F− to2 induces spectral and color changes (o
u
t
p
u
t
534
n
m), while a further addition of Zn2+ to this solution reverses or reproduces the changes (o
u
t
p
u
t
440
n
m), both color and spectra, to restore the original position (2). This can be viewed as two different systems; first the output at 534 nm is controlled by two inputs, input-F and input-Zn, the system resembling a molecular INH logic gate, represented by the truth table (Figure 6(a)). On the other hand, the output at 440 nm is controlled by the same inputs but different order represents IMP logic gate. According to the Boolean logic systems, the two systems resemble a two-input complementary IMP/INH logic functions (Figure 6(b)). In the 21st century, these systems of reversible-reproducible functions are of great interest in molecular level information processing. While molecular logic devices are already in use in some fields, applications in computational operations remain to be desired.Figure 6
Schematic representation of (a) truth table and (b) a combinatorial IMP/INH logic circuit.
(a)
(b)The interpretation of the logic operation functions is highlighted based on reversibility studies (Figure7(a)). The addition of appropriate combinations of F− and Zn2+ as inputs yields the outputs which are equivalent with complimentary IMP/INH logic functions [29, 44]. The process is triggered through the molar addition of input-1 (F−, AcO−) at 534 nm and reversed by the molar addition of input-2 (3d5–10). The spectral red shift which changes to 534 nm upon the addition of input-1 is complementary to INH logic gate, while the reversed activities at 440 nm are complementary to IMP logic gate. More additions of inputs have no significant effect on the absorption of the solution, as evidenced by the number of cycles performed (Figure 5(b)). Moreover, colorimetric activities are concentration-dependent, where colors intensify upon the increase of concentration (Figure 7(b)).Figure 7
(a) UV-vis spectra of2 (1 × 10−5 M) in DMSO with different combinations of F− and Z
n
I
I and molecular logic functions “IMP” (440 nm) and “INH” (534 nm). (b) Reversible colorimetric activities of2 with F− and Z
n
I
I.
(a)
(b)


### 3.4. In Depth Study on the Interaction of2 with Hg2+ and Zn2+

The addition of cations (H
g
I
I and Z
n
I
I) to2 displayed different spectral behaviors compared to anions, which prompted further investigation in order to have a clear understanding on the interaction behaviors of the species involved. The addition of H
g
I
I or Z
n
I
I to2 resulted in the “naked eye” detectable color change, from orange to yellowish (almost colorless), concomitant with spectral changes, at 440 nm and 534 nm (Figure 4). Individually, the addition of 0.3 equiv. H
g
I
I to2 resulted in the complete disappearance of the absorption band at 534 nm, initially assigned to the benzotrithiophene moiety and the intensity increase of the band at 440 nm. Contrastingly, similar behaviors were observed upon the addition of Z
n
I
I to2; however, the absorption band at 534 nm could not disappear completely even when excess amount of Z
n
I
I was added.Consequently, more titrations were carried out in order to understand the similarities and differences of2 towards H
g
I
I and Z
n
I
I. Firstly, the addition of H
g
I
I to2 resulted in the complete disappearance of the band at 534 nm after only 0.3 equiv., while enhancement was experienced at 440 nm. To this, AcO− molar equiv. was added, which saw the reappearance of the enhanced band at 534 nm simultaneously with the gradual disappearance of the band at 440 nm (Figure 8(a)). Conversely, reversing the mixing order by adding AcO− to2first, followed by H
g
I
I, resulted in all changes to be restored back to the initial free sensor (2); however, further addition of H
g
I
I caused the disappearance of the 534 nm band (Figure 8(b)). Deducing from this, it can safely be concluded that the association constant of H
g
I
I is higher with anions (AcO−) than with2. Secondly, comparative titration studies were carried out using Z
n
I
I instead of H
g
I
I. It was confirmed that Z
n
I
I can only reverse and restore the original status of2; however, further addition after the restoration did not result in any significant spectral changes, even when excess amount was added (Figures 8(c) and 8(d)). The overall summation drawn from this system was that2 showed strong interactions with H
g
I
I compared to Z
n
I
I irrespective of the presence of anions. On the other hand, Z
n
I
I can only slightly interact with2 in the absence of the anions (Figure 4(b)), while weak or no interaction was observed in the presence of anions (Figure 8(c)). Therefore, Z
n
I
I in this case is only suited for logic operation functions as an input for the reverse and restoration of2. Therefore, this means2 not only serves as an anion (AcO−, F−, etc.) sensor, with logic operation functions, but also is simultaneously a cation (H
g
I
I) sensor, suspected to interact via coordination with nitrogen and sulphur atoms in the structure.Figure 8
UV-vis titrations for2 (1 × 10−5 M) in DMSO, displaying reversible effects upon the additions of (a) H
g
I
I then AcO−, (b) AcO− then Hg2+, (c) AcO− then Z
n
I
I, and (d) Z
n
I
I then AcO−.
(a)
(b)
(c)
(d)The colorimetric activities are heavily dependent on the concentration of sensor. For instance, at 100μmol·L−1, the addition of F− to2 resulted in the change of color from orange to deep violet, while similar addition of F− to2 at 10 μmol·L−1 saw the change in color from light orange to pink (Figure 9(b)). Furthermore, the molar addition of Hg2+ to2 at 100 μmol·L−1 resulted in an intense yellow color (from orange), while light yellow color was observed at 10 μmol·L−1 (Figure 9(a)).Figure 9
Colorimetric activities observed upon the additions of Hg2+ or F− to2 at different concentrations: (a) 10 μmol·L−1 and (b) 100 μmol·L−1.
(a)
(b)


### 3.5. DFT Studies of2 with Anions

Applying theoretical approaches based on evidences from the spectroscopic data, molecular modeling calculations (DFT) atB
3
L
Y
P
/
6
-
31
G
∗ level in DMSO were performed to simulate or predict the possible geometrical conformation of2 and the complexed mode2-F. Accordingly, upon optimizing the structures evident correlations in structural differences between2 and the2-F adduct were observed as shown in Figure 10. For instance, the presence of F− saw the whole structure slightly elongate from 14.247 to 14.449 Å (N1 to S14, two furthest points) which resulted in 4.68° structural distortion as revealed by the peripheral structure angle (N1C15S14) increase, from 131.02 to 135.70° (Figure 11). The initially planar NO2 group to the benzene ring experienced distortion upon the introduction of F−. Overwhelmingly, there is more evidence suggesting that the interaction between2 and F− is within the conclave region of –NH; for example, the distance between closest NO2 (N14) and the –NH (N8) increased significantly from 2.533 to 2.721 Å, due to hydrogen bonding interaction between –NH and F− resulting in NH–F as indicated (Figure 11). In addition, Mulliken’s atomic charges at the nitrogen atom of–NH changed from −0.540 to −0.568 with the formation of the complex2-F. The increase of the negative charge environment confirms the intercharge transfer (ICT) between2 and F−, which lowers down the energy levels of the frontier orbitals through the stabilization of π
∗ excited state of2 by charge delocalization. The HOMO-LUMO gaps of the complexes of2have decreased (Figure 10) and this signifies the decrease in the molecular energy and thus stability. Lowering of the HOMO-LUMO gap is responsible for absorption to be redshifted to longer wavelength and thus the pink coloration is observed.Figure 10
HOMO and LUMO diagrams of2in the presence and absence of F− in DMSO.Figure 11
Optimized structure showing the positions of atoms.


## 3.1. UV-Vis Titration of2 with Anions

The sensor (2) is characterized by two absorption bands in the visible region in DMSO, the high and low energy bands at 440 nm and 534 nm, respectively, ascribed to the existence of charge transfer (CT) of the electron withdrawing 2,4-dinitrophenylhydrazone moiety and the electron donating BTT unit, respectively. The molar addition of anions (AcO− and F−) to2 resulted in the intensity decrease of the band at 440 nm, while intensity increase was experienced at 534 nm as shown in Figures 1(a) and 1(b). In addition to the spectral changes, the color of2 changed from orange to purple (inset). An isosbestic point at 469 nm was indicating the existence of two distinctive species at equilibrium during the titration process. It is well known that the interaction of anions (AcO−, F−, and H
2
P
O
4
-) with hydrazone moiety is through hydrogen bonding with the NH proton in the sensor, the action ascribed to geometrical complementarity, and the chemical properties of the species [32–37]. The addition of other anions (Cl−, Br−, I−, and H
2
P
O
4
-) did not induce much significant or noticeable changes (Figure 2(c)). The glimpse on the interaction modes is suggested by the titration curves as shown in Figures 2(a) and 2(b). However, Job’s plot displays a more complex binding mode (Figure 3).Figure 1
Changes in UV-vis absorption spectra of2(1 × 10−5 M) upon the addition of 1 equiv. (a) AcO− and (b) F−, all in DMSO at 25°C.
(a)
(b)Figure 2
Titration profile on the band at 440 nm and 534 nm in (a) AcO−, (b) F−, and (c) UV-vis absorption spectra of Cl−, Br−, I−, and H
2
P
O
4
-, respectively, all in DMSO at 25°C.
(a)
(b)
(c)Figure 3
Job’s plot for (a) AcO− and (b) F−, both in DMSO at 1 × 10−4 M.
(a)
(b)


## 3.2. UV-Vis Titrations of2 with Cations

Interestingly, the addition of molar equivalents of Hg2+ to2 resulted in the color changes from yellow to light yellow (almost colorless), which was concomitant with the disappearance of the spectra band at 534 nm, while the increase in intensity was observed at 440 nm (Figure 4). The interaction is suspected to be of coordination nature involving two immediate cationphilic neighboring atoms (sulphur and nitrogen) and the mercury ion. The complementary size of Hg2+ is suspected to have played a major role in the selection preference. Conclusively, the coordination of Hg2+ to2 interferes with the intermolecular charge transfer (ICT) between the electron rich –NH and the electron deficient –NO2 at 534 nm, thereby disrupting charge transfer activities across the structural sphere, resulting in the disappearance of the peak at 534 nm. Other cations such as Cu2+ and Zn2+ showed similar effects; however, none of them were able to vanquish the band (534 nm) completely, even when huge quantities were used. However, it appears that the reversibility properties (logic operations) which are modulated by inputs (cations and anions) are stronger than the coordination interactions to some extent, as discussed in the next section.Figure 4
Changes in UV-vis absorption spectra of2(1 × 10−5 M) upon the addition of (a) 0.3 equiv. Hg2+ and (b) 4 equiv. Zn2+, all in DMSO at 25°C.
(a)
(b)


## 3.3. Reversibility and Logic Operations Studies

More details on interactions were obtained from the reversibility studies, which led to the conclusion that the reversible colorimetric activities of2 upon the addition of anions and cations resemble two inputs with complementary “IMP/INH” logic functions. The addition of anions to2 which resulted in spectral and naked eye colorimetric changes was reversed to their initial state, both spectra and color, when molar amount of cations (Zn2+) was added (Figure 5(a)). The reversible yellow-orange-yellow-orange cycles were repeated several times (4 times) by alternating addition of 2 equiv. F− and about 1.2 equiv. of Zn2+ with consistent and continuous cycles shown in Figure 5(b). The total amount of equiv. added during the four cycles was almost 1(2) : 17F− : 7Zn2+, which has little effect on the absorption intensities of2, even though the fourth cycle saw the molar amounts slightly increased, compared to the first three. Similar results to Zn2+ were obtained upon molar additions of Cu2+ in more or less equivalent ratios.Figure 5
Reversible cycles and reproducible colorimetric switch of2 (1 × 10−5 M, in DMSO) modulated by the addition of F− and Zn2+ (≃2 : 1), respectively. (a) Spectral display of the first cycle. (b) Repeating cycles.
(a)
(b)The logic operations of2 are based on the reversibility and reproducibility of colorimetric-spectral switch upon mixing right combinations of F− and Zn2+. The addition of F− to2 induces spectral and color changes (o
u
t
p
u
t
534
n
m), while a further addition of Zn2+ to this solution reverses or reproduces the changes (o
u
t
p
u
t
440
n
m), both color and spectra, to restore the original position (2). This can be viewed as two different systems; first the output at 534 nm is controlled by two inputs, input-F and input-Zn, the system resembling a molecular INH logic gate, represented by the truth table (Figure 6(a)). On the other hand, the output at 440 nm is controlled by the same inputs but different order represents IMP logic gate. According to the Boolean logic systems, the two systems resemble a two-input complementary IMP/INH logic functions (Figure 6(b)). In the 21st century, these systems of reversible-reproducible functions are of great interest in molecular level information processing. While molecular logic devices are already in use in some fields, applications in computational operations remain to be desired.Figure 6
Schematic representation of (a) truth table and (b) a combinatorial IMP/INH logic circuit.
(a)
(b)The interpretation of the logic operation functions is highlighted based on reversibility studies (Figure7(a)). The addition of appropriate combinations of F− and Zn2+ as inputs yields the outputs which are equivalent with complimentary IMP/INH logic functions [29, 44]. The process is triggered through the molar addition of input-1 (F−, AcO−) at 534 nm and reversed by the molar addition of input-2 (3d5–10). The spectral red shift which changes to 534 nm upon the addition of input-1 is complementary to INH logic gate, while the reversed activities at 440 nm are complementary to IMP logic gate. More additions of inputs have no significant effect on the absorption of the solution, as evidenced by the number of cycles performed (Figure 5(b)). Moreover, colorimetric activities are concentration-dependent, where colors intensify upon the increase of concentration (Figure 7(b)).Figure 7
(a) UV-vis spectra of2 (1 × 10−5 M) in DMSO with different combinations of F− and Z
n
I
I and molecular logic functions “IMP” (440 nm) and “INH” (534 nm). (b) Reversible colorimetric activities of2 with F− and Z
n
I
I.
(a)
(b)


## 3.4. In Depth Study on the Interaction of2 with Hg2+ and Zn2+

The addition of cations (H
g
I
I and Z
n
I
I) to2 displayed different spectral behaviors compared to anions, which prompted further investigation in order to have a clear understanding on the interaction behaviors of the species involved. The addition of H
g
I
I or Z
n
I
I to2 resulted in the “naked eye” detectable color change, from orange to yellowish (almost colorless), concomitant with spectral changes, at 440 nm and 534 nm (Figure 4). Individually, the addition of 0.3 equiv. H
g
I
I to2 resulted in the complete disappearance of the absorption band at 534 nm, initially assigned to the benzotrithiophene moiety and the intensity increase of the band at 440 nm. Contrastingly, similar behaviors were observed upon the addition of Z
n
I
I to2; however, the absorption band at 534 nm could not disappear completely even when excess amount of Z
n
I
I was added.Consequently, more titrations were carried out in order to understand the similarities and differences of2 towards H
g
I
I and Z
n
I
I. Firstly, the addition of H
g
I
I to2 resulted in the complete disappearance of the band at 534 nm after only 0.3 equiv., while enhancement was experienced at 440 nm. To this, AcO− molar equiv. was added, which saw the reappearance of the enhanced band at 534 nm simultaneously with the gradual disappearance of the band at 440 nm (Figure 8(a)). Conversely, reversing the mixing order by adding AcO− to2first, followed by H
g
I
I, resulted in all changes to be restored back to the initial free sensor (2); however, further addition of H
g
I
I caused the disappearance of the 534 nm band (Figure 8(b)). Deducing from this, it can safely be concluded that the association constant of H
g
I
I is higher with anions (AcO−) than with2. Secondly, comparative titration studies were carried out using Z
n
I
I instead of H
g
I
I. It was confirmed that Z
n
I
I can only reverse and restore the original status of2; however, further addition after the restoration did not result in any significant spectral changes, even when excess amount was added (Figures 8(c) and 8(d)). The overall summation drawn from this system was that2 showed strong interactions with H
g
I
I compared to Z
n
I
I irrespective of the presence of anions. On the other hand, Z
n
I
I can only slightly interact with2 in the absence of the anions (Figure 4(b)), while weak or no interaction was observed in the presence of anions (Figure 8(c)). Therefore, Z
n
I
I in this case is only suited for logic operation functions as an input for the reverse and restoration of2. Therefore, this means2 not only serves as an anion (AcO−, F−, etc.) sensor, with logic operation functions, but also is simultaneously a cation (H
g
I
I) sensor, suspected to interact via coordination with nitrogen and sulphur atoms in the structure.Figure 8
UV-vis titrations for2 (1 × 10−5 M) in DMSO, displaying reversible effects upon the additions of (a) H
g
I
I then AcO−, (b) AcO− then Hg2+, (c) AcO− then Z
n
I
I, and (d) Z
n
I
I then AcO−.
(a)
(b)
(c)
(d)The colorimetric activities are heavily dependent on the concentration of sensor. For instance, at 100μmol·L−1, the addition of F− to2 resulted in the change of color from orange to deep violet, while similar addition of F− to2 at 10 μmol·L−1 saw the change in color from light orange to pink (Figure 9(b)). Furthermore, the molar addition of Hg2+ to2 at 100 μmol·L−1 resulted in an intense yellow color (from orange), while light yellow color was observed at 10 μmol·L−1 (Figure 9(a)).Figure 9
Colorimetric activities observed upon the additions of Hg2+ or F− to2 at different concentrations: (a) 10 μmol·L−1 and (b) 100 μmol·L−1.
(a)
(b)


## 3.5. DFT Studies of2 with Anions

Applying theoretical approaches based on evidences from the spectroscopic data, molecular modeling calculations (DFT) atB
3
L
Y
P
/
6
-
31
G
∗ level in DMSO were performed to simulate or predict the possible geometrical conformation of2 and the complexed mode2-F. Accordingly, upon optimizing the structures evident correlations in structural differences between2 and the2-F adduct were observed as shown in Figure 10. For instance, the presence of F− saw the whole structure slightly elongate from 14.247 to 14.449 Å (N1 to S14, two furthest points) which resulted in 4.68° structural distortion as revealed by the peripheral structure angle (N1C15S14) increase, from 131.02 to 135.70° (Figure 11). The initially planar NO2 group to the benzene ring experienced distortion upon the introduction of F−. Overwhelmingly, there is more evidence suggesting that the interaction between2 and F− is within the conclave region of –NH; for example, the distance between closest NO2 (N14) and the –NH (N8) increased significantly from 2.533 to 2.721 Å, due to hydrogen bonding interaction between –NH and F− resulting in NH–F as indicated (Figure 11). In addition, Mulliken’s atomic charges at the nitrogen atom of–NH changed from −0.540 to −0.568 with the formation of the complex2-F. The increase of the negative charge environment confirms the intercharge transfer (ICT) between2 and F−, which lowers down the energy levels of the frontier orbitals through the stabilization of π
∗ excited state of2 by charge delocalization. The HOMO-LUMO gaps of the complexes of2have decreased (Figure 10) and this signifies the decrease in the molecular energy and thus stability. Lowering of the HOMO-LUMO gap is responsible for absorption to be redshifted to longer wavelength and thus the pink coloration is observed.Figure 10
HOMO and LUMO diagrams of2in the presence and absence of F− in DMSO.Figure 11
Optimized structure showing the positions of atoms.


## 4. Conclusion

In summary, we have succeeded in synthesizing a dual colorimetric sensor for both anions and cation based on a simple one-step reaction, with high selectivity and sensitivity responses. The spectroscopic and visual observations made were all correlating with theoretical studies undertaken. This module has very excellent properties which can be developed and translated further into industrial based applications for sensing or even more for molecular logic functions, such as keypad locks.



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*Source: 6438187-2016-06-21.xml*