Anthracene-Based Lanthanide Metal-Organic Frameworks : Synthesis , Structure , Photoluminescence , and Radioluminescence Properties

Four anthracene-based lanthanide metal-organic framework structures (MOFs) were synthesized from the combination of the lanthanide ions, Eu3+, Tb3+, Er3+, and Tm3+, with 9,10-anthracenedicarboxylic acid (H2ADC) in dimethylformamide (DMF) under hydrothermal conditions. The 3-D networks crystalize in the triclinic system with P-1 space group with the following compositions: (i) {{[Ln2(ADC)3(DMF)4·DMF]}n, Ln = Eu (1) and Tb (2)} and (ii) {{[Ln2(ADC)3(DMF)2(OH2)2·2DMF·H2O]}n, Ln = Er (3) and Tm (4)}. The metal centers exist in various coordination environments; nine coordinate in (i), while seven and eight coordinate in (ii). The deprotonated ligand, ADC, assumes multiple coordination modes, with its carboxylate functional groups severely twisted away from the plane of the anthracene moiety. The structures show ligand-based photoluminescence, which appears to be significantly quenched when compared with that of the parent H2ADC solid powder. Structure 2 is the least quenched and showed an average photoluminescence lifetime from bi-exponential decay of 0.3 ns. On exposure to ionizing radiation, the structures show radioluminescence spectral features that are consistent with the isolation of the ligand units in its 3-D network. The spectral features vary among the 3-D networks and appear to suggest that the latter undergo significant changes in their molecular and/or electronic structure in the presence of the ionizing radiation.


Introduction
Metal-organic framework (MOF) structures that display linker-based luminescence characteristics have been receiving an increasing amount of attention in recent years.Their 2-D and 3-D networks offer the opportunity to fine-tune the luminescence characteristics of the organic linker molecules by isolating them in well-defined environments [1][2][3][4][5][6].Of interest to us is the potential of MOFs as radioluminescent (scintillating) materials for the detection of ionization radiation, including neutrons, protons, and gamma rays.Advancement in the science of detecting ionizing radiation is of great significance in radiography, biological safety, medical devices, biochemical analysis, particle physics, astrophysics, and nuclear materials identification and monitoring.Anthracene, with its highly luminescent chromophore, has the highest light output (rated at 100%) among organic scintillators 72 h in a convection oven.The vial was cooled to room temperature and the colorless crystals were filtered and repeatedly washed with fresh DMF and vacuum filtered.(

Characterization
Single crystal X-ray analysis (SCXA) was conducted on a Bruker APEX-II CCD diffractometer.A suitable crystal was isolated from the sample and mounted onto the instrument using Paratone Oil.Measurements were made at ω scans of 1 • per frame for 40 s using Mo Kα radiation (fine-focus sealed tube, 45 kV, 30 mA).The structures were solved with the Superflip structure solution program, using the Charge Flipping solution method [28] and using Olex2 as the graphical interface [29].The models were refined with version 2013-4 of ShelXL using least squares minimization [30].The total number of runs and images was based on the strategy calculation from the program APEX2 [31].Cell parameters were retrieved and refined using SAINT software [32].Data reduction was performed using the SAINT software, which corrects for Lorentz polarization.All non-hydrogen atoms were refined anisotropically.Hydrogen positions were calculated geometrically and refined using the riding model.Powdered X-ray diffraction (PXRD) patterns were recorded on a Panalytical Empyrean Series 2 X-ray diffractometer.The X-ray source was a Cu Kα (λ = 1.5418Å) with anode at a voltage of 45 kV and current of 40 mA.Diffraction patterns were recorded between the 2θ angles of 4 • -40 • with a step size of 0.026 • .Simulated PXRD patterns were obtained from SCXA data using Mercury 3.1 software from Cambridge Crystal Structure Database (CCDC).Infrared measurements were recorded on a Bruker Alpha-P FTIR spectrophotometer (intensive pattern: m-medium, s-strong, w-weak).The sample was introduced into the spectrophotometer using KBr as a zero-background powder and measurements were acquired between 350 and 4000 cm −1 .Thermogravimetric analysis was conducted on a TA Instrument Q50 thermal analyzer.Approximately 4 mg of sample was heated at a rate of 5 • C/min from ambient temperature to 900 • C under airflow.Elemental analysis was performed by Atlantic Microlab, Norcross, GA, USA.

Photoluminescence and Radioluminescence
Room temperature solid-state photoluminescence measurement was conducted on Photon Technology International fluorometer equipped with a 75 Watts Xenon Arc Lamp, excitation and emission monochromators, and a photomultiplier detector.A powdered sample of each structure was smeared between quartz slides, and excitation and emission spectra were recorded.Fluorescence lifetimes of the same samples were measured using an Edinburgh Instruments time-correlated single photon counting (TCSPC) system.In this measurement, an excitation pulse diode laser (LDH-P-C-375, 372 nm) was used as excitation light sources.The detection system consisted of a high-speed microchannel plate photomultiplier tube (MCP-PMT, Hamamatsu R3809U-50) and TCSPC electronics.The decays curves were fitted by the polyexponential functions after deconvolution with the instrument response function (IRF).
Radioluminescence measurements were conducted using an ion beam induced luminescence (IBIL) method in the Ion Beam Laboratory, Sandia Laboratories, New Mexico, using published procedures [11,12].The experimental setup and conditions involved a 2.5 MeV proton beam, a current density 12,000 nA/cm 2 with the sample under 4.3 × 10 −6 Torr vacuum pressure and ambient temperature.The beam was focused onto the sample with a spot size estimated to be 120 µm × 175 µm.Data was collected using a fiber optics coupled CCD spectrophotometer.

Structure description of 1 and 2:
The PXRD patterns of 1 (Eu) and 2 (Tb), along with the simulated profile of 2, show peaks in identical 2θ positions for both (Electronic Supplementary Information (ESI) Figure S1).The MOFs also show identical PXRD profiles as the simulated pattern of 1, which confirms that each sample crystallizes as a pure phase.Crystal structure data for single SCXA are presented in Table 1.Both PXRD and SCXA analyses show that 1 and 2 are isostructural, so detailed analysis is given for 1 only.The crystal structure of 1 refines in a triclinic P-1 space group as a 3-D coordination polymeric network, with minimum voids and no measurable porosity.
Metal coordination: Structure 1 consists of two crystallographically identical Eu atoms per unit cell.There are five ADC units and two DMF molecules surrounding each Eu1 atom (Figure 1a).The Eu1 atom has nine coordinates, all with Eu1-O bonds.Seven Eu-O bonds are with the oxygen atoms from the five ADC ligands and two Eu1-O bonds are with oxygen atoms of two DMF molecules, generating an irregular EuO 9 coordination polyhedron.A list of select bond lengths and angles for 1 and 2 is presented in Table S1.The Eu-O bond lengths range from 2.363(1) Å for Eu-O3 to 2.572(2) Å for Eu-O1 and are similar to those observed in related coordination polymers [33,34].The two Eu atoms are bridged by the oxygen atoms of two ADC ligands, with O1 atoms coordinating to Eu1 and creating an intradinuclear Eu•••Eu distance of 4.036 Å.

Ligand coordination:
The ADC unit coordinates in three modes, namely, µ 2 :η 3 (bis-bridging-chelating), µ 2 :η 2 (bis-bridging), and η 2 (bis-chelating).The bridging ligands link four metal atoms, whereas the bis-chelating ligands involve the linking of two.Various interconnected polymeric chains can be identified in the structure.Along the (100) direction, -(ADC-Eu 2 ) n -chains are present, with the ADC units coordinating Eu atoms in bis-bidentate chelating mode, and with two adjacent Eu1 atoms bridged by oxygen atoms of the ligands carboxylate functional group (Figure 1b).Along the (010) direction, -(ADC-Eu 2 ) n -chains are also present, with the ADC units coordinating Eu atoms in bis-bidentate bridging/chelating mode through the ligands' carboxylate groups.Each Eu atom is coordinated by three carboxylate oxygen atoms, and each carboxylate oxygen atom coordinates two Eu atoms.The -(ADC-Eu 2 ) n -chains are also present along the c direction with the ADC units in bis-bidentate bridging mode; each carboxylate group coordinates two Eu atoms (Figure 1c).The nearest Eu•••Eu distance along the length of an ADC unit is 11.4 Å.Interestingly, the carboxylate groups are significantly twisted outside the plane of the anthracene moiety and measure 63.6 • (C6-C2-C1-O2) for the bis-chelating, 85.8 • (C11-C10-C9-O3) for the bis-bridging, and 68.7 • for the bis-bridging/chelating ligands.The twisting of the carboxylate groups, as compared to a coplanar configuration, is consistent with reported DFT calculations on the parent H 2 ADC molecule, which showed its potential energy to be at a minimum with a 60 • rotation of the COOH group [35].The interconnectivity of the chains through the Eu1 atoms creates a 3-D arrangement, with channels along the b axis and the coordinated DMF solvent inside.Though non-continuous solvent accessible voids constitute 11% of the structure, nitrogen adsorption analysis at 77 K on the activated sample of 1 shows no appreciable porosity.

Ligand coordination:
The ADC unit coordinates in three modes, namely, µ2:η3 (bis-bridging-chelating), µ2:η2 (bis-bridging), and η2 (bis-chelating).The bridging ligands link four metal atoms, whereas the bis-chelating ligands involve the linking of two.Various interconnected polymeric chains can be identified in the structure.Along the [100] direction, -(ADC-Eu2)n-chains are present, with the ADC units coordinating Eu atoms in bis-bidentate chelating mode, and with two adjacent Eu1 atoms bridged by oxygen atoms of the ligands carboxylate functional group (Figure 1b).Along the [010] direction, (ADC-Eu2-)n chains are also present, with the ADC units coordinating Eu atoms in bis-bidentate bridging/chelating mode through the ligands' carboxylate groups.Each Eu atom is coordinated by three carboxylate oxygen atoms, and each carboxylate oxygen atom coordinates two Eu atoms.The -(ADC-Eu2)n-chains are also present along the c direction with the ADC units in bis-bidentate bridging mode; each carboxylate group coordinates two Eu atoms (Figure 1c).The nearest Eu•••Eu distance along the length of an ADC unit is 11.4 Å.Interestingly, the carboxylate groups are significantly twisted outside the plane of the anthracene moiety and measure 63.6° (C6-C2-C1-O2) for the bis-chelating, 85.8° (C11-C10-C9-O3) for the bis-bridging, and 68.7° for the bis-bridging/chelating ligands.The twisting of the carboxylate groups, as compared to a coplanar configuration, is consistent with reported DFT calculations on the parent H2ADC molecule, which showed its potential energy to be at a minimum with a 60° rotation of the COOH group [35].The interconnectivity of the chains through the Eu1 atoms creates a 3-D arrangement, with channels along the b axis and the coordinated DMF solvent inside.Though non-continuous solvent accessible voids constitute 11% of the structure, nitrogen adsorption analysis at 77 K on the activated sample of 1 shows no appreciable porosity.

Structure description of 3 and 4:
The PXRD patterns of 3 (Er) and 4 (Tm), along with the simulated profile of 4, show peaks in identical 2θ positions (ESI Figure S2).The structures show PXRD profiles that are identical to the simulated pattern of 4, which confirms that they both crystallize as pure phases.Both PXRD and SCXA (Table 1) show that 3 and 4 are isostructural, so detailed analysis is given for 4 only.The structure is a 3-D network consisting of two crystallographically inequivalent Tm atoms, six ADC ligands, two coordinated, and two lattice, DMF molecules, and two coordinated, and one lattice, water molecules.
Metal Coordination: The coordination environment for each of the two crystallographically inequivalent Tm atoms is shown in Figure 2. The Tm1 atom has eight coordinates.Six are Tm1-OCARB

Structure description of 3 and 4:
The PXRD patterns of 3 (Er) and 4 (Tm), along with the simulated profile of 4, show peaks in identical 2θ positions (ESI Figure S2).The structures show PXRD profiles that are identical to the simulated pattern of 4, which confirms that they both crystallize as pure phases.Both PXRD and SCXA (Table 1) show that 3 and 4 are isostructural, so detailed analysis is given for 4 only.The structure is a 3-D network consisting of two crystallographically inequivalent Tm atoms, six ADC ligands, two coordinated, and two lattice, DMF molecules, and two coordinated, and one lattice, water molecules.
Metal Coordination: The coordination environment for each of the two crystallographically inequivalent Tm atoms is shown in Ligand coordination: Three coordination modes can be identified for the ADC linker, namely, bridging (µ 2 :η 2 ), bis-chelating (η 2 ), and bis-monodentate (η 1 ).The bis-chelating ligands coordinate Tm1 and Tm2 atoms along both the b and c axes to create a 2-D "ladder-like" conformation, with the "ladder rungs" along the b axis (Figure 2b).The "ladder" structure is like that reported by Wang et al. in a related but different structure [13].Along the b axis, the bis-chelating and bis-monodentate coordinating ADC units are coordinated to Tm1•••Tm2 centers in an alternating arrangement.The bis-bridging ADC units, which are aligned along the a axis, intersect the 2-D ladder arrangement at the bimetallic Tm1•••Tm2 centers to complete the 3-D network (Figure 2b).As in the case of 1 and 2, the carboxylate groups are significantly twisted outside the plane of the anthracene moiety, with a twist angle of 62.2 • (C30-C27-C26-O7) for the bis-bridging ligand and 77.6 • (C3-C2-C1-O2) for the bis-chelating ligands.As discussed earlier, the twisting is dictated by the minimum energy conformation from the 60 • rotation of the carboxylate, as shown by DFT calculations [34].The uncoordinated oxygen atoms of the carboxylate groups on the bis-monodentate coordinating ADC units form strong hydrogen bonds with nearby coordinated water molecules, thus further stabilizing the ligand and providing restriction to its rotation (Figure 2c).The closest interchromophore distance is 12.5 Å.Narrow channels are present along the b direction.However, like 1, nitrogen adsorption analysis at 77 K on an activated sample of 4 shows no appreciable porosity.Ligand coordination: Three coordination modes can be identified for the ADC linker, namely, bridging (µ2:η2), bis-chelating (η2), and bis-monodentate (η1).The bis-chelating ligands coordinate Tm1 and Tm2 atoms along both the b and c axes to create a 2-D "ladder-like" conformation, with the "ladder rungs" along the b axis (Figure 2b).The "ladder" structure is like that reported by Wang et al. in a related but different structure [13].Along the b axis, the bis-chelating and bis-monodentate coordinating ADC units are coordinated to Tm1•••Tm2 centers in an alternating arrangement.The bis-bridging ADC units, which are aligned along the a axis, intersect the 2-D ladder arrangement at the bimetallic Tm1•••Tm2 centers to complete the 3-D network (Figure 2b).As in the case of 1 and 2, the carboxylate groups are significantly twisted outside the plane of the anthracene moiety, with a twist angle of 62.2° (C30-C27-C26-O7) for the bis-bridging ligand and 77.6° (C3-C2-C1-O2) for the bis-chelating ligands.As discussed earlier, the twisting is dictated by the minimum energy conformation from the 60° rotation of the carboxylate, as shown by DFT calculations [34].The uncoordinated oxygen atoms of the carboxylate groups on the bis-monodentate coordinating ADC units form strong hydrogen bonds with nearby coordinated water molecules, thus further stabilizing the ligand and providing restriction to its rotation (Figure 2c).The closest interchromophore distance is 12.5 Å.Narrow channels are present along the b direction.However, like 1, nitrogen adsorption analysis at 77 K on an activated sample of 4 shows no appreciable porosity.

FTIR Analysis:
The nature of the ADC units in the structures was further investigated by analysis of their Fourier transformed infrared spectra (FTIR) and a comparison with that of H2ADC (ESI Figure S3).The band at 3448 cm −1 in all samples indicates the presence of O-H from adsorbed water on the MOFs and on H2ADC.The 2925 cm −1 and 2967 cm −1 bands observed in H2ADC were assigned to weak intramolecular OH bonds between non-planar C=O and H on the aromatic ring at the 1, 4, 5, and 8 carbon positions.These bands were not observed in 1-4, and their absence is attributed to C=O coordination to the metal atom, thus limiting their interactions with aromatic H.The band observed at 1687 cm −1 in the spectrum of H2ADC is attributed to the HO-C=O, with localized charges on the ligand's carboxylic acid functional groups.This band was not observed in 1-4; instead, two individual bands were observed at 1601 cm −1 and 1551 cm −1 , which are attributed to variation in stretching vibrations of the C-O bonds in the three different ligand conformations.These observations indicate that the ligand is deprotonated (as ADC) within the MOF structures.The band at 1562 cm −1 in the MOF spectra is attributed to of metal-oxygen bonds [36].
Thermal Analysis: The thermal behavior of the structures was investigated by thermogravimetric analysis.The TGA curves of 1 and 2 show weight loss between 100 and 450 °C representing the loss of coordinated and uncoordinated DMF molecules (~30 wt %).Weight loss commencing around 440 °C (~40 wt %) is attributed to the loss of ADC units, and residue (~30 wt %) is attributed to lanthanide oxides.The TGA curves of 3 and 4 show small weight loss events up to 100 °C, attributed to the loss of H2O molecules (~10 wt %).Weight loss up to 400 °C (~15 wt %) is FTIR Analysis: The nature of the ADC units in the structures was further investigated by analysis of their Fourier transformed infrared spectra (FTIR) and a comparison with that of H 2 ADC (ESI Figure S3).The band at 3448 cm −1 in all samples indicates the presence of O-H from adsorbed water on the MOFs and on H 2 ADC.The 2925 cm −1 and 2967 cm −1 bands observed in H 2 ADC were assigned to weak intramolecular O•••H bonds between non-planar C=O and H on the aromatic ring at the 1, 4, 5, and 8 carbon positions.These bands were not observed in 1-4, and their absence is attributed to C=O coordination to the metal atom, thus limiting their interactions with aromatic H.The band observed at 1687 cm −1 in the spectrum of H 2 ADC is attributed to the HO-C=O, with localized charges on the ligand's carboxylic acid functional groups.This band was not observed in 1-4; instead, two individual bands were observed at 1601 cm −1 and 1551 cm −1 , which are attributed to variation in stretching vibrations of the C-O bonds in the three different ligand conformations.These observations indicate that the ligand is deprotonated (as ADC) within the MOF structures.The band at 1562 cm −1 in the MOF spectra is attributed to of metal-oxygen bonds [36].
Thermal Analysis: The thermal behavior of the structures was investigated by thermogravimetric analysis.The TGA curves of 1 and 2 show weight loss between 100 and 450 • C representing the loss of coordinated and uncoordinated DMF molecules (~30 wt %).Weight loss commencing around 440 • C (~40 wt %) is attributed to the loss of ADC units, and residue (~30 wt %) is attributed to lanthanide oxides.The TGA curves of 3 and 4 show small weight loss events up to 100 • C, attributed to the loss of H 2 O molecules (~10 wt %).Weight loss up to 400 • C (~15 wt %) is attributed to loss of DMF.Weight loss event commencing around 400 • C (~45 wt %) is attributed to the loss of ADC units, and residue (~30 %) is attributed to lanthanide oxides.

Photoluminescence
The photoluminescence behavior of each compound was investigated.The room temperature solid-state photoluminescence emission spectra of the structures along with that of solid H 2 ADC are presented in Figure 3.The spectrum of Na 2 ADC in dilute aqueous solution was also recorded for comparison (ESI Figure S5).The spectrum of Na 2 ADC in aqueous solution shows two defined vibronic peaks: one with λ max at 425 nm and a shoulder at 450 nm.This is similar to that reported for pure anthracene [37], except that a smaller left shoulder peak expected at ~400 nm was not defined.The MOF structures (except 3) show emission spectra with distinct vibronic peaks that are similar in profile to those observed for Na 2 ADC in aqueous solution, thus suggesting that the emission is linker-based.
The emission peaks from the structures are within the 400-600 nm region, with their wavelength maxima (λ max ) observed between that of the Na 2 ADC in dilute aqueous solution at 425 nm and that of the H 2 ADC powder at 500 nm.The emission maxima of the structures are therefore red-shifted compared to the ADC sodium salt solution and blue-shifted compared to the H 2 ADC powder.Further, a Stokes shift was observed among the structures as follows: 60 nm for 1 (380 nm ex-max to 440 nm em-max ), 65 nm for 2 (380 nm ex-max to 435 nm em-max ), 50 nm for 3 (389 nm ex-max to 430 nm em-max ) and 30 nm for 4 (400 nm ex-max to 430 nm em-max ), all of which are smaller than the 87 nm observed for H 2 ADC.Except for 4, the Stokes shift values are larger than the 41 nm observed in Zn-PCN-14, which contains the larger and rotatable anthracene liker, 5,5 -(anthracene-9,10-diyl)diisophthalinic acid (DPATC) [2].With the exception of Structure 3, the peaks are more defined than those observed in Zn-PCN-14.By comparison, the emission spectrum of H 2 ADC is broad with less defined peaks and a larger Stokes shift (Figure 4).The broad spectral features of H 2 ADC are likely ascribed to changes in the excited state geometry of the molecule due to the rotation of its -COOH groups to near coplanar conformation with the anthracene moiety.This can result in a lower energy excited state complex due to increased resonance, π overlap, and charge transfer interactions between the functional group and the ring system [34].However, the ADC units in Structures 1-4 are deprotonated and are rigidified by coordination to the metal atoms.Rotation of the carboxylate groups is expected to be restricted as a result.This ridification, coupled with the separation of individual ADC units in the structures, will therefore reduce the level of interligand interactions and, by extension, reduce the extent of non-radiative relaxation pathways that would otherwise exist in solid forms of both anthracene and H 2 ADC.
Within each structure, the cofacial alignment of ADC units in the (100) direction is interrupted by ADC units in the (010) direction.The closest cofacial distances are 14.5 Å in 1 and 12.5 Å in 4, which are beyond the distance within which significant interchromophore coupling interactions among the phenyl rings of ADC units would be present [38].The nearest distances between the planar face of one anthracene moiety and the hydrogen atoms on the edges of another, range between 3.689 (H12•••C3) and 5.242 Å (H12•••C7) for 1, and between 3.397 (H4•••C24) and 5.542 Å (H4•••C21) for 4.These edge-to-face distances are in the range within which C-H•••π interactions are possible between the-orbitals of the hydrogens and the π system of the anthracene moieties.Such interactions could contribute to the non-radiative decay pathways and to the observed Stokes shifts.The broad featureless emission spectrum of 3 could be the result of more severe structural changes that brought ADC units closer on exposure to UV excitation.The possibility of the inductive effects of the Er atoms on the linker that can cause perturbation of the electronic transitions occurring in the ligand to result in more diffuse spectrum is also worthy of consideration and warrants further investigation.
Of note is that no luminescence spectral features from the lanthanide ions were detected in the visible region (for Eu 3+ and Tb 3+ ) and were not measured in the near-infrared region (for Tm 3+ and Er 3+ ) which is beyond the range of our standard fluorimeter.It is speculated, however, that following direct excitation the photoemissions of the latter two metals ions would be weak or non-existent due to their low molar absorption coefficient (typically lower that 10 L mol −1 cm −1 ) [1][2][3][4].Time-resolved photoluminescence decay: Time-resolved photoluminescence measurements were also acquired to further investigate the local environment of the anthracene units in the 3-D networks.Structures 1 Eu (not shown), 3 (Er), and 4 (Tm) yielded photoluminescence decay curves of low intensity that almost overlap with the instrument response function (IRF) (ESI Figure S6), while the decay curve for 2 (Tb), like that of H2ADC, was quite distinct from the IRF (Figure 4).The decay curves were fitted with the biexponentional function, I α exp τ τ exp τ τ , Time-resolved photoluminescence decay: Time-resolved photoluminescence measurements were also acquired to further investigate the local environment of the anthracene units in the 3-D networks.Structures 1 Eu (not shown), 3 (Er), and 4 (Tm) yielded photoluminescence decay curves of low intensity that almost overlap with the instrument response function (IRF) (ESI Figure S6), while the decay curve for 2 (Tb), like that of H 2 ADC, was quite distinct from the IRF (Figure 4).The decay curves were fitted with the biexponentional function, I = α 1 exp − τ τ 1 + α 2 exp − τ τ 2 , which corresponds to two different photo emissive rates, where I is the intensity, τ is the time, τ 1 and τ 2 are their corresponding excited state decay lifetimes, and α is the pre-exponential factor.The faster a radiative lifetime a major component has, the more τ 1 is attributed to emission from monomeric-like ADC units, and the more τ 2 is attributed to ADC units involved in coupling interactions, as observed for anthracene dimers.For Structure 2 (Tb), lifetimes τ 1 = 0.2 ns and τ 2 = 0.5 ns and weighted average lifetime τ o = 0.3 ns are much shorter than the 4.9 ns, 16 ns, and 9.5 ns, respectively, we determined for H 2 ADC (ESI Table S2).These lifetimes are also shorter than the average lifetime value of τ o = 2.0 ns reported elsewhere for anthracene in monomeric isolated arrangements [39] and shorter than τ o = 5 ns reported for Zn-PCN-14 [2].which corresponds to two different photo emissive rates, where I is the intensity, τ is the time, τ1 and τ2 are their corresponding excited state decay lifetimes, and α is the pre-exponential factor.The faster a radiative lifetime a major component has, the more τ1 is attributed to emission from monomeric-like ADC units, and the more τ2 is attributed to ADC units involved in coupling interactions, as observed for anthracene dimers.For Structure 2 (Tb), lifetimes τ1 = 0.2 ns and τ2 = 0.5 ns and weighted average lifetime τo = 0.3 ns are much shorter than the 4.9 ns, 16 ns, and 9.5 ns, respectively, we determined for H2ADC (ESI Table S2).These lifetimes are also shorter than the average lifetime value of τo = 2.0 ns reported elsewhere for anthracene in monomeric isolated arrangements [39] and shorter than τo = 5 ns reported for Zn-PCN-14 [2].As discussed earlier, changes in the excited state geometry of bulk ligand molecules due to the rotation of its -COOH groups to near coplanar conformation with the anthracene moiety and reorganization towards end-to-face herringbone arrangement, which can facilitate excimer formation and strong interchromophore interactions, are quite likely.This could have contributed to the much longer lifetime (τ2) compared to the MOF structures [8,34].
The short lifetimes observed for Structures 1-4 in comparison to those of H2ADC and Zn-PCN-14 suggest that there is significant fluorescence quenching in the structures.Similar quenching of ligand fluorescence in complexes of lanthanides ions, including Tb 3+ and Eu 3+ have been previously observed [40] and is postulated to occur by the energy transfer between the ligand and the paramagnetic lanthanide ions via a cross-relaxation mechanism.

Radioluminescence
Radioluminescence (scintillation) is the emission of radiation after a material absorbs radiation with energy generally ≥10 eV that leads to π-electron ionization (Iπ) [7].The ionization is followed by ion recombination (the recombining of secondary electrons with their parent electrons) that populates available singlet (S) and triplet (T) states.This is followed by non-radiative thermal As discussed earlier, changes in the excited state geometry of bulk ligand molecules due to the rotation of its -COOH groups to near coplanar conformation with the anthracene moiety and reorganization towards end-to-face herringbone arrangement, which can facilitate excimer formation and strong interchromophore interactions, are quite likely.This could have contributed to the much longer lifetime (τ 2 ) compared to the MOF structures [8,34].
The short lifetimes observed for Structures 1-4 in comparison to those of H 2 ADC and Zn-PCN-14 suggest that there is significant fluorescence quenching in the structures.Similar quenching of ligand fluorescence in complexes of lanthanides ions, including Tb 3+ and Eu 3+ have been previously observed [40] and is postulated to occur by the energy transfer between the ligand and the paramagnetic lanthanide ions via a cross-relaxation mechanism.

Radioluminescence
Radioluminescence (scintillation) is the emission of radiation after a material absorbs radiation with energy generally ≥10 eV that leads to π-electron ionization (Iπ) [7].The ionization is followed by ion recombination (the recombining of secondary electrons with their parent electrons) that populates available singlet (S) and triplet (T) states.This is followed by non-radiative thermal deactivation to the lowest vibrational level of the first excited state S 1 before relaxation to lower electronic levels with an accompanying emission of radiation [41].In this work, proton ion beam-induced luminescence (IBIL) spectroscopy was used to assess the radioluminescence spectral profile of the structures and H 2 ADC, as this is known to simulate the production of recoil protons by elastic scattering of fast neutrons within an organic scintillator [2].
The IBIL emission spectral profiles for Structures 1-3 are compared with their respective photoluminescence spectra and to that of H 2 ADC (Figure 3).The IBIL spectrum of 4 was not measured since the crystal faces were not of sufficiently large dimensions to fit the ion beam without penetration during data collection.The similarities in the IBIL spectral profile of 1 and 2 to their respective photoluminescence spectrum and to that of a dilute solution of Na 2 ADC show that the IBIL is a product of the MOF crystal only and not of any H 2 ADC impurities from synthesis or a result of any damage caused by the beam.Interestingly, for 1, its IBIL spectrum shows two distinct vibronic peaks at 440 and 460 nm that almost overlap its photoluminescence spectrum (though a small red shift was observed).The overlap is consistent with the local environment of highly isolated ligand units in the structure remaining unaltered upon exposure to the proton beam [42].For structures 2 (with λ max-IBIL at 445 nm) and 3 (with λ max-IBIL at 475 nm), there significant red shifts in the IBIL spectrum of each when compared with their respective photoluminescence spectrum.This also translates into Stokes shift values (between the photoluminescence excitation λ max and the λ max-IBIL ) of 65 (445-380 nm) for 2 and 85 nm (490-375 mm) for 3, respectively.Interestingly also is that the IBIL emission peaks remained defined in 2, while they are broadened and featureless in 3.These Stokes shift values are within close proximity of 78 nm reported for Zn-PCN-14 (which contains the DPATC linker) [2], but are much less than the 115 nm (515-400 nm) that we observed for H 2 ADC (Figure 3).These Stokes shifts and peak broadening (in the case of 3) suggest that the relaxation pathways described above may not be strictly observed due to changes in the molecular and/or electronic structures of materials on exposure to ionizing radiation.Such changes could possibly be a distortion of the chromophore environment, resulting in a shortening of inter-ligand distances and an increase in inter-chromophore interactions.It is notable also that, because of the significant Stokes shift, there was a relatively small spectral overlap between excitation and emission, and this is favorable for the use of the material as a scintillator in that self-absorption can be minimized [2].

Conclusions
The combination of lanthanide ions Eu 3+ , Tb 3+ , Er 3+ and Tm 3+ with the H 2 ADC under hydrothermal conditions yielded four 3-D anthracene-based lanthanide MOFs in two different structure types; the Eu and Tb MOFs are isostructural, as are the Er and Tm MOFs.The deprotonated ligand, ADC, assumes multiple coordination modes in the structures and its carboxylate functional groups are severely twisted away from the plane of the anthracene moiety, which is consistent with its lowest energy conformation.The structures possess very narrow channels and show no appreciable porosity.The structures exhibit ligand-based photoluminescence that is significantly quenched.The Tb-containing MOF was least quenched and showed an average photoluminescence lifetime, τ o , of 0.3 ns.On exposure to ionizing radiation, the structures also show ligand-based radioluminescence.

Figure 1 .
Figure 1.(a) Coordination environment of Eu1 atoms in 1.(b) Interconnectivity of bis-chelating chains along the (100) direction.(c) Interconnectivity of bis-bridging and bis-chelating chains along the (010) direction (Coordinated solvent and hydrogen atoms are omitted for clarity).

Figure 2 .
Figure 2. (a) The coordination environment of Tm1 and Tm2 in 4. (b) Interconnectivity of two chains with the ADC units in bis-chelating and bis-monodentate coordination modes along the (010) direction.(c) Hydrogen bonding between ADC and coordinated water molecules.(Coordinated solvent molecules are omitted for clarity).

Figure 2 .
Figure 2. (a) The coordination environment of Tm1 and Tm2 in 4. (b) Interconnectivity of two chains with the ADC units in bis-chelating and bis-monodentate coordination modes along the (010) direction.(c) Hydrogen bonding between ADC and coordinated water molecules.(Coordinated solvent molecules are omitted for clarity).

Figure 3 .
Figure 3. Photoluminescence excitation (blue), emission (green), and IBIL (red) spectra of 1-4 and H 2 ADC.(Excitation wavelength was 380 nm for all emission spectra.Excitation spectra were monitored at emission wavelength of 435 nm for 1-4 and at 525 nm for H 2 ADC.IBIL spectrum was not recorded for 4).

Table 1 .
Crystal structure and refinement data for