Construction of luminescent coordination polymers based on 5-(1-(carboxymethyl)-pyrazol-3-yl)isophthalic ligand for sensing Cu2+ and acetone

Journal Pre-proofs Construction of luminescent coordination polymers based on 5-(1-(carboxymethyl)-pyrazol-3-yl)isophthalic ligand for sensing Cu2+ and acetone Yanhui Zhao, Zheyu Zhang, Tieping Cao, Li Wang, Yong Fan, Teng Wan, Jia Jia PII: DOI: Reference:

S0277-5387(19)30759-4 https://doi.org/10.1016/j.poly.2019.114314 POLY 114314

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Polyhedron

Received Date: Revised Date: Accepted Date:

22 August 2019 4 December 2019 14 December 2019

Please cite this article as: Y. Zhao, Z. Zhang, T. Cao, L. Wang, Y. Fan, T. Wan, J. Jia, Construction of luminescent coordination polymers based on 5-(1-(carboxymethyl)-pyrazol-3-yl)isophthalic ligand for sensing Cu2+ and acetone, Polyhedron (2019), doi: https://doi.org/10.1016/j.poly.2019.114314

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Construction of luminescent coordination polymers based on 5(1-(carboxymethyl)-pyrazol-3-yl)isophthalic ligand for sensing Cu2+ and acetone Yanhui Zhao[a], Zheyu Zhang[a], Tieping Cao[a], Li Wang[b], Yong Fan[b], Teng Wan[a] and Jia Jia*[a] a College

of Chemistry, Baicheng Normal University, Baicheng 137000, Jilin, P. R. China.

E-mail: [email protected] b College

of Chemistry, Jilin University, Changchun 130012, Jilin, P. R. China.

Abstract Two new coordination polymers (CPs), namely, [Zn3(L)2(phen)3(H2O)2·2H2O]n (phen=1,10-phenanthroline) (1) and [Pb(HL)]n (2) were constructed from the coordination reaction of 5-(1-(carboxymethyl)-pyrazol-3-yl)isophthalic acid (H3L) ligand and Zn(II) or Pb(II) ions under hydrothermal conditions. It was found that 1 and 2 exhibited an infinite one-dimensional (1D) chain and three-dimensional (3D) framework with left-handed and right-handed helical chains based on single crystal X-ray diffraction analysis, respectively. Both of them had good luminescent property at room temperature. Meanwhile, 1 possessed highly luminescent sensing properties for environmentally relevant Cu2+ ions with a quenching coefficient Ksv of 1.509×104 M−1, and the fluorescence quenching efficiency of acetone reached 90%, which indicated that 1 could be taken as a potential candidate for developing multifunctional luminescent sensors. Our work thus paves a way for developing CPs as an appealing platform to construct crystalline materials for environmental applications.

Keywords: Coordination polymers; Fluorescent sensing; Cu2+ ions; Acetone

1. Introduction In recent years, more and more attention has been paid to the study of luminescent coordination polymers (CPs), because they are widely used in fluorescence sensing, nonlinear optics, photo catalysis, displays and biomedical imaging [1]. In particular, the exploration of luminescent CPs as chemical sensors is in an increasing trend. Owning to their crystallinity, porosity, large specific surface area and adjustable structure, the luminescent CPs sensors have multiple advantages such as high sensitivity, good selectivity, short response time, stability and reusability [2]. So far, it has been reported that some CPs exhibit excellent luminescence sensing for metal ions [3], anions [4], small molecules [5], vapors and explosives [6]. In luminescent sensing of an analyte, it is most intuitive and convenient to detect the luminescence changes of CPs (including the enhancement or quenching of fluorescence intensity and changeable emission color that can be easily observed by naked eyes). For instance, Li and coworkers synthesized a porous luminescent Zn(II)CP, that could be exploited as a good fluorescent chemical sensor for toxic heavy metal ions at ppb level (3.3 ppb Hg2+, 19.7 ppb Pb2+) with 84 % quenching efficiency upon addition of 19.6 μM Hg2+ [7]. Mandal et al. successfully prepared a stable luminescent Zn(II)-CP, which had discriminative detection of trace amounts of nitro aromatic explosives with different numbers of –NO2 groups in solution or in vapor phase through fluorescence quenching effect [8]. Additionally, porosity and functional groups within the framework, such as Lewis basic sites in the ligands, further promote preconcentrate, improve the detection sensitivity and the binding of preferred analytes for selective detection. For example, Qian et al. constructed a luminescent Eu( Ⅲ )-CP

containing Lewis basic pyridyl sites for sensing Cu2+. Such uncoordinated Lewis basic sites provided a platform for the interactions between pyridyl nitrogen atoms and Cu2+ ions, leading to luminescence quenching effect [9]. Similar examples for specific host–guest recognition are rare compared with the open Lewis acidic metal sites [10-13]. Overall, the luminescent CPs-based sensors can be used in many aspects of environmental monitoring, which is of great practical significance. However, the rational design and construction of luminescent CPs is challenging to some extent. It was found that many factors had an important influence on their luminescent properties, including structural characteristics, coordination environment of metal ions, nature of the pores, the interactions with guest molecules through hydrogen bonding and  stacking interactions [1]. Therefore, the rational selection of organic ligands is of great significance for constructing luminescent sensing CPs. Of numerous ligands, the aromatic carboxylate ligands containing azole rings might be the good candidates [14]. For instance, Cao et al. adopted triazine-carboxylate ligand to construct an anionic fluorescent Zn(II)-CP, which could be used as highly efficient sensor to detect Fe3+ ions [10] ； Zhu and coworkers synthesized a Eu(Ⅲ)-CP by using pyrazole-carboxylate ligand applied as an excellent luminescent probe sensing Fe3+ and Cr2O72− ions [15]. In our previous work, we had been conducting the construction and application of luminescent CPs from azole-carboxylate ligands (Scheme 1), which presented the following advantages: (1) the large π-conjugated skeleton of benzene and azole rings enhanced luminescence; (2) the multi-carboxylate groups would not only provide multiple coordination sites to construct various architectures but also join the metal

ions together to afford polynuclear metal organic clusters, thus largely stabilizing CP structure even showing excellent stability in aqueous solution; (3) the uncoordinated nitrogen atoms from azole rings and uncoordinated carboxylate oxygen atoms could easily form interactions with analytes. Using H3TZI and H3TZBT ligands (Scheme 1) to coordinate with lanthanide(III), zinc(II) and lead(II) ions, a series of luminescent CPs had been prepared and studied in detail, which showed highly luminescent sensing properties for lanthanide(III) ions and acetone [16-18].

Scheme 1. Structural diagram of ligands. As part of our continuing work in the context, we have more recently carried out the coordination reaction of 5-(1-(carboxymethyl)-pyrazol-3-yl)isophthalic acid (H3L) ligand (Scheme 1) containing Lewis basic pyrazole sites with Zn (II) or Pb(II) under hydrothermal condition to successfully synthesize luminescent CPs [Zn3(L)2 (phen)3(H2O)2·2H2O]n (phen=1,10-phenanthroline) (1) and [Pb(HL)]n (2). 1 displays an infinite 1D chain, while 2 presents a complex 3D framework. Both of them show strong luminescence emission in solid state condition. Notably, 1 exhibits good luminescent sensing property to detect Cu2+ and acetone. The quenching coefficient (Ksv) of Cu2+ is 1.509×104 M−1, and the fluorescence quenching efficiency of acetone reaches 90%, which is higher than that in our previous work [the quenching efficiency is 55% and 87% for {[Zn2(μ5-tzbt)(μ-trz)]·3.5H2O}n (H3tzbt = 1-(triazol-1-yl)-2,4,6benzene

tricarboxylic

acid,

trz

=

1,2,4-triazolate)

and

{[Zn2(μ5-tzbt)(μ-

OH)(phen)]·4H2O}n (phen = 1,10-phenanthroline), respectively] [16]. Herein, we would like to report our found.

2. Experimental Section

2.1. Materials and Methods All chemicals used in this work were of reagent grade. They were commercially available and used as purchased without further purification. The IR spectra (KBr pellets) were recorded in the range 400−4000 cm−1 on a Nicolet Impact 410 spectrometer. Elemental analyses(C, H and N) were performed on an Elementar Vario EL cube CHNOS Elemental Analyzer. Thermogravimetric analyses (TGA) were carried out with a PerkinElmer TGA7 instrument, with a heating rate of 10 °C·min−1 under air atmosphere. Powder Xray diffraction (XRD) measurements were performed with a D/MAX2550 diffractometer with Cu-Kα radiation (λ = 1.5418 Å) in the 2θ range of 4−40°. Photoluminescence spectra were obtained by an Edinburgh Instruments FLS 920 spectrophotometer. X-ray photoelectron spectroscopy (XPS) was recorded under a ultra-high vacuum (< 10−7 Pa) at a pass energy of 55 eV on a PerkinElmer PHI 5000C ESCA system using a Al Kα (1486 eV) anode. Elemental analyses for Zn and Cu were obtained using a PLASMA-SPEC(I) inductively coupled plasma (ICP) atomic emission spectrometer.

2.2. Synthesis of the compounds 2.2.1. Synthesis of [Zn3(L)2(phen)3(H2O)2·2H2O]n (1) A mixture of H3L ligand (0.029 g, 0.1 mmol), Zn(OAc)2·2H2O (0.011 g, 0.05 mmol), 1,10-Phenanthroline (0.010 g, 0.05 mmol) and distilled water (5.0 mL) was put into a beaker, and then NaOH (0.1M, 2 mL) was slowly dropped to adjust the pH value. After stirring for 30 min, the mixture was transferred to a 15 mL Teflon-lined autoclave, heated at 120 °C in the oven for 72 h. Colorless block crystals were filtered after cooling to room temperature and dried in air (57.0% yield based on Zn). Elemental analysis (%) found: C, 55.45; H, 3.10; N, 10.31. Calcd for C62H42N10O14Zn3: C, 55.28; H, 3.14; N, 10.40%. IR (KBr, cm−1): 3421(s), 1616(s), 1372(s), 1143(w), 1090(m), 1052(w), 1000(w), 923(w), 847(s), 778(w), 725(s). 2.2.2. Synthesis of [Pb(HL)]n (2) The synthesis method was the same as that of compound 1, except that phen auxiliary ligand was not added to the reactants and the metal salt was replaced with Pb(NO3)2. The amount of H3L ligand and Pb(NO3)2 was 0.058 g (0.2 mmol) and 0.033 g (0.1 mmol), respectively. Finally colorless block crystals were obtained (38.0% yield based on Pb). Elemental analysis (%) found: C, 31.68; H, 1.67; N, 5.61. Calcd for C13H8N2O6Pb: C, 31.52; H, 1.63;

N, 5.65%. IR (KBr, cm−1): 3117(s), 1844(w), 1692(s), 1547(s), 1387(s), 1311(w), 1212(w), 1159(w), 1098(w), 1052(w), 1000 (w), 923 (w), 794(w), 748(w), 671(w). 2.3.

X-ray crystallography (See ESI 1.1 and Table S1 and S2)

2.4. The metal ions sensing experiment The powders of 1 (5mg) were immersed in aqueous solution of different metal ions (0.01 mol/L, 5mL). The stable suspensions were obtained by ultrasonic treatment of 30 min, aging for 24 h. Upon the excitation wavelength of λex = 300 nm, the fluorescence quenching experiment was carried out. 2.5. The solvent sensing experiment (See ESI 1.2)

3. Results and Discussion 3.1. Crystal structures 3.1.1. Structural description of [Zn3(L)2(phen)3(H2O)2·2H2O]n (1) Compound 1 belongs to monoclinic system, C 2/c space group, in which the asymmetric unit is composed of one and a half crystallographically independent Zn(II) ions and phen ligands, one fully deprotonated L3-, one coordinated water and one lattice water molecule. The coordination environment of Zn(II) is depicted in Fig.1a, where Zn1 is four-coordinated by

two nitrogen atoms and two oxygen atoms coming from phen ligand and two different L3- ligands, respectively. Unlike Zn1, Zn2 is five-coordinated by two N atoms and three O atoms, in which N atoms are from phen ligand, O atoms from the coordinated water molecule and two different L3- ligands. The Zn–O distances vary from 1.957(2) to 2.090(2) Å, whilst the range of Zn–N bond lengths is 2.074(3) to 2.164(3) Å.

Fig.1. (a) Coordination environment of Zn(II) ions. (b) 2D layered structure of 1 viewing along baxis; (c) topological view showing the equivalent 2D framework of 1.

L3- ligand exhibits only one coordination mode in 1 (Scheme 2a), and three carboxylate groups of L3- all show monodentate (η1μ1χ1) coordination mode to coordinate with three Zn(II) ions, forming one-dimensional (1D) chain along c axis (Fig. 1b). Because of the special position of Zn1, the 1D chain is neither a common ladder lattice chain nor a zigzag chain. The terminal coordination of phen ligand hinders the expansion of spatial dimension. Such 1D chains are extended through  stacking interactions to produce a 2D layered network (Fig. 1b). The inversion-

related planes of aromatic rings in phen ligands are completely parallel, in which the distance of centroid is 3.653 Å and dihedral angle is 0. From the perspective of topology, the 2D structure of 1 could be simplified to 44 square grid, existing open windows viewed along b-axis (Fig. 1c).

Scheme 2 Coordination modes of H3L ligand in 1 (a) and 2 (b), respectively.

3.1.2. Structural description of [Pb(HL)]n (2) Compound 2 crystallizes in the monoclinic system with P21/c space group. The asymmetric unit contains a Pb (II) ion and a HL2− ligand. As shown in Fig. 2a, Pb1 is seven-coordinated by seven oxygen atoms from the five different HL2− ligands to form a hemi-directed [PbO7] geometry (Fig. 2b). The Pb–O distances range from 2.456(3) to 2.755(3) Å.

HL2− ligand also exhibits one coordination mode in 2 (Scheme 2b). Different from 1, three carboxylate groups of HL2− have three different coordination modes including monodentate (η1μ1χ1), bridging chelating (η2μ1χ2) and bridging tetradentate (η2μ3χ4). PbO7 polyhedron are connected via carboxylate groups becoming edge-sharing metal chains. These infinite inorganic metal chains are linked by HL2− ligands to construct a 2D structure

(Fig. 2b), which further connected together to build up a 3D framework (Fig. 2d). Interestingly, 2 contains left-handed and right-handed spiral chains grown along crystallographic 21 screw axis, with a pitch of 11.466 Å, which is formed by bridging HL2− ligands and Pb (II) ions. (Fig. 2c).

Fig.2. (a) Coordination environment of Pb(II) ion; (b) 2D layered structure of 2; (c) Left - handed and right - handed helical chains in 2; (d) 3D structure of 2.

3.2. Characterization The PXRD spectra of 1 and 2 are in accord with the simulated ones, indicating that these compounds are pure phase (Fig. S1). The different orientation of the crystal plane should be the main reason for differences in intensity [19-22]. Their thermal stabilities are tested by TGA. The first weight-loss stage of 1 is from 30 to 183 °C (Fig. S2), owing to the loss of lattice water and coordinated water molecules, with a weight loss rate of 4.8% (calcd. 5.2%). With the increase of temperature, it remains relatively stable in the range of

183–315 °C, and the skeleton starts to collapse until 320 °C. Compound 2 is stable until 360 °C. When heating to 477 °C, the organic ligands are decomposed and the skeletal structure is destroyed. The final product is PbO (obs:44.8%, calcd. 45.2%). The relevant references well show that the combination of TGA and XRD can be used to characterize the decomposition and conversion of the compounds or the thermal stability of the products obtained by oxidation or reduction reaction [23-26]. 3.3. Luminescence and sensing properties At room temperature, the solid state fluorescence emission and excitation spectra of 1 and 2 are provided in Fig. 3 and Fig. S3, respectively. Under the same experimental conditions, the emission spectrum of free H3L ligand is recorded as compared, which has a strong emission at 367nm (λex=300 nm), assigned to π→π* transitions. The maximum emission peak of 1 is at 372 nm, which can be attributed to the ligand-based luminescence, since it is similar to that of H3L ligand [7]. In addition, the luminescence intensity of 1 is significantly improved owing to the immobilization of ligands in the compound after coordination, which is beneficial to energy transfer among organic ligands, and reduces the intraligand HOMO-LUMO energy gap [27]. The broad emission of 2 is at 470 nm with red-shift, which is different from the metal centered transition of s and p orbitals containing s2-metal clusters [28]. Herein, the emission band of 2 may be ascribed to ligand-to-metal charge transfer from delocalized π bonds of H3L ligand to p orbitals of Pb2+ center [29].

Fig. 3. Fluorescence emission spectra of 1, 2 and the H3L ligand.

Considering the certain regularity of fluorescence quenching of 1, we study its potential sensing abilities for both metal ions and volatile organic solvent molecules (VOSMs). To determine the potential sensing property of metal ions, the luminescent emissions of 1 dispersed in M(NO3)n (10-2 M) aqueous solutions (M = K+, Na+, Ag+, Pb2+, Ni2+, Co2+, Cd2+, Cu2+, Mg2+, Ca2+, Al3+) were measured at first. Cu2+ shows excellent quenching effect on 1 (Fig. 4), because the unsaturated state of electrons in the outer layer of Cu2+ which makes it become a better electron receptor [30]. Fluorescence emission spectra of 1 in different metal solutions are shown in Fig. S4. These results show 1 can well recognize Cu2+ ions.

Fig.4. Fluorescence intensities of 1 in M(NO3)n (10-2 M) aqueous solutions (M = K+, Na+, Ag+, Pb2+, Ni2+, Co2+, Cd2+, Cu2+, Mg2+, Ca2+, Al3+).

In order to study the changes of luminescence intensities influenced by different Cu2+ concentration, a series of Cu(NO3)2 aqueous solutions were prepared (10-5 - 10-4 M). As seen in Fig. 5, the intensities of Cu2+@1 decrease gradually with Cu2+ concentration increasing, and the quenching level (I0/I) has a good linear relationship with Cu2+ concentration by Stern–Volmer (SV) equation [31]: I0/I = 1 + KSV[M], where I0 and I are intensities of 1 without Cu2+ and adding Cu2+ ions respectively, [M] is Cu2+ concentration and KSV (the slope) is Stern-Volmer quenching constant. The KSV value is 1.509 × 104 M-1, and other comparable CP-based sensors for Cu2+ are listed in Table S3. This result indicates that 1 can conveniently detect a spot of Cu2+ ions [32].

Fig.5. (a) Fluorescence intensities of 1 at different Cu2+ concentrations; (b) Linear relationship of 1 in different concentrations of Cu2+ solutions.

We study anti-interference sensing ability of 1 through competitive experiments, and further prove that 1 is a good luminescent sensor to detect copper ions. The detailed experimental results were as follows: 0.08 mL Cu(NO3)2 (10-2 M) were slowly dripped into suspensions which contained powder sample of 1 (5 mg) and 10-2 M other metal ions (4 mL), respectively. The luminescence spectra of the above suspensions are depicted in Fig. S6. It is

worth noting that after adding Cu2+ ions, the influence of other metal ions on fluorescence intensity of 1 shows a great quenching effect, which indicates that the detection of Cu2+ will not be hindered by other metal ions. To understand the quenching mechanism, the PXRD measurements are carried out. PXRD spectrum of Cu2+@1 is in agreement with 1 (Fig. S5), which illustrates the framework of 1 after soaking in Cu2+ solution has not been destroyed. So this luminescence quenching effect will not be ascribed to the decomposition of the framework. When Cu2+ ions interact with the potential Lewis sites of CPs, due to its unsaturated electron configuration (3d9), the πrich system in the compound can easily contribute its electrons to electron deficient receptors and release excitation energy through non-radiative pathways. Thus, the efficiency of energy transformation π*→π is changed [33,34]. In addition, the characteristic peak of Cu2+ ions can be seen from X-ray photoelectron spectroscopy (XPS) (Fig. S7), indicating that Cu2+ ions diffuse into the pores of 1 or are adsorbed on the surface. Owing to the radii and coordination modes of Cu2+ and Zn2+ ions are similar, we speculate metal ion exchange maybe occur, so ICP analysis is also carried out. The results show some of the Zn2+ ions in 1 are replaced by Cu2+, and the ratio of Cu2+:Zn2+ is 1:2.32 (Table S4). In summary, the results show that electrostatic interactions and the photo-induced electron transfer mechanism, as well as metal ion exchange play an important role in detecting Cu2+ ions in aqueous solution [35,36]. Additionally, the N1s peak at 399.4 eV from uncoordinated pyrazole of H3L ligand in 1 is shifted to 399.9 eV after soaking in 10-2 M Cu(NO3)2 solution (Fig. S8), indicating the existence of weak interaction formed by Cu2+ ions and nitrogen atoms.

Next, to investigate the potential sensing ability of small solvent molecules, fluorescence intensities of 1 in different solvent emulsions are monitored. As shown in Fig. 6, the solvent molecules have effect on the photoluminescence (PL) intensities of 1 in different extent, and it is found that acetone exhibits the most obvious quenching effect (PL spectra in Fig. S9). The main reason for this phenomenon is that the interactions between different solvent molecules and the skeleton structure of 1 are distinct [37].

Fig.6. Luminescence intensities of 1 in different solvents (λex = 300 nm).

We selected ethanol as the dispersion medium in the following sensing experiments, because the fluorescence emission spectrum of 1 in ethanol was the strongest. The sensing sensitivities of 1 were measured in ethanol dispersion by adding acetone step by step (Fig. 7a). With the increase of acetone content, the fluorescence intensity decreased gradually, which was almost proportional to acetone concentration (Fig. S10). Effect of acetone volume ratio on fluorescence intensity of 1 can be fitted by the first order exponential decay (Fig. 7b), suggesting that the fluorescence quenching by acetone is diffusion controlled [38]. When acetone content is 2.00 %, the

quenching efficiency reaches 90 % for 1, which is calculated by (1-I/I0) ×100% (I0 is the initial intensity and I are intensities after adding acetone). The quenching efficiency of 1 and other reported acetone sensors based on luminescent CPs are comparable (Table S5). Moreover, the PXRD spectra of 1 immersed in acetone and ethanol are in line with the simulated one, illustrating stability of the crystal structure (Fig. S11). Therefore, 1 can be exploited as a promising luminescent probe for the detection of acetone. Such fluorescence quenching effect caused by solvent molecules is mainly attributed to the physical interaction between solvent and solute. This quenching mechanism may be owing to the energy competition between the excited CP particles and acetone molecules adsorbed on the surface and in pores of 1. The energy absorbed by organic ligands in 1 is transferred to acetone molecules, thus reducing the luminescence intensity [38].

Fig.7. (a) Fluorescence titration of 1 dispersed in ethanol (1 mg/mL) by adding acetone gradually (λex = 300 nm); (b) Luminescence intensities of 1-ethanol emulsion by gradually adding acetone.

4. Conclusions

In summary, using 5-(1-(carboxymethyl)-pyrazol-3-yl)iso-phthalic ligand (H3L), two new coordination polymers (CPs) have been successfully synthesized under hydrothermal conditions. Both 1 and 2 exhibit intensively fluorescence emissions at room temperature. Additionally, 1 is a good CP-based luminescent sensor for the detection of acetone and Cu2+ ions through the quenching effect. The present research demonstrates that luminescent CPs can be rationally designed and explored as potential sensors to detect a small amount of specific analytes in environmental area. It is anticipated that with continued efforts in the design, synthesis and optimization of new materials, luminescent CPs-based sensors are on their way to practical applications. Other CP-based fluorescence sensors constructed from H3L ligand and its derivatives will be carried out and an attempt will be made to detect gases in the future.

Appendix A. Supplementary data CCDC 1887317 and 1887316 contains the supplementary crystallographic data for compounds 1 and 2, respectively. These data can be obtained free of charge via http://www.ccdc.cam.ac.uk/conts/retrieving.html,

or

from

the

Cambridge

Crystallographic Data Centre, 12 Union Road, Cambridge CB2 1EZ, UK; fax: (+44) 1223-336-033; or e-mail: [email protected].

Acknowledgments We gratefully acknowledge the financial support through the National Natural Science Foundation of China (no. 21573003).

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Author Contribution Statement Yanhui Zhao: Data curation and Writing- Original draft preparation Zheyu Zhang: Software and Validation Tieping Cao: Funding acquisition Li Wang: Conceptualization Yong Fan: Resources Teng Wan: Formal analysis Jia Jia*: Supervision, Writing- Reviewing and Editing

Declaration of Interest Statement We declare that we have no financial and personal relationships with other people or organizations that can inappropriately influence our work, there is no professional or other personal interest of any nature or kind in any product, service and/or company that could be construed as influencing the position presented in, or the review of, the manuscript entitled, “Construction of luminescent coordination polymers based on 5-(1-(carboxymethyl)-pyrazol-3-yl)isophthalic ligand for sensing Cu2+ and acetone”.

Highlights

1. Two new coordination polymers have been successfully synthesized. 2. 1 possessed highly luminescent sensing property for Cu2+ ions (Ksv =1.509×104 M−1). 3. The fluorescence quenching efficiency of 1 for acetone reached 90%.

Graphical abstract

Graphical abstract Two new luminescent coordination polymers with 5-(1-(carboxymethyl)-pyrazol-3yl)isophthalic ligand and Zn(II) / Pb(II) have been prepared under hydrothermal conditions. Notably, 1 possessed highly luminescent sensing properties for Cu2+ ions (Ksv =1.509×104 M−1) and acetone.