# Multiphoton Excitation and Energy Transfer Pathways in Mn²⁺–Sulfonyl Calixarene Complexes

Constance Lecourt, Gilles Ledoux, Yan Suffren, Erwann Jeanneau, Dominique Luneau, Cédric Desroches

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Constance Lecourt, Gilles Ledoux, Yan Suffren, Erwann Jeanneau, Dominique Luneau, et al. Multi-photon Excitation and Energy Transfer Pathways in Mn²⁺–Sulfonyl Calixarene Complexes. Dalton Transactions, 2025, 10.1039/D5DT02234G. hal-05349781

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# Multiphoton excitation and energy transfer pathways in Mn²⁺-sulfonyl calixarene complexes

Constance Lecourt, ID a Gilles Ledoux, ID b Yan Suffren, ID c Erwann Jeanneau, a Dominique Luneau ID a and Cedric Desroches ID *a

The complexes based on Mn²⁺ ions and sulfonylcalixarene macrocycles can exhibit, when excited by blue light (360 to 400 nm), a broad luminescence band around 600 nm, resulting from the d-d transition ⁴T₁(t₂g⁴eg¹) → ⁶A₁(t₂g³eg²) of the Mn²⁺ ions. A new original synthetic route to access the phenylethynyl-sulfonylcalix[4]arene macrocycle (paThiaSO₂) and its corresponding complexes with Mn²⁺ ions has been followed and the first experience *via* excitation with lower-energy multiphoton absorption have been realized. The results obtained demonstrate the possible two-photon sensitization of Mn²⁺ ions through the sulfonylcalixarene macrocycle.

Received 18th September 2025.

Accepted 3rd November 2025

DOI: 10.1039/d5dt02234g

rsc.li/dalton

## 1. Introduction

The optical properties of 3d metal coordination complexes are becoming increasingly attractive due to the abundance and low cost of these metals compared to 4d and 5d metals.¹ A large number of studies are being conducted to move away from precious metals in fields such as light-emitting diodes,² photocatalysts,³ light sensors in dye-sensitized solar cells,⁴ or phototherapy.⁵ In recent years, there has been a growing interest in research on 3d metal coordination compounds in the field of optics. Manganese has the ability to exhibit a wide range of oxidation states. Among them, +I, +II, and +IV can display luminescence properties: for the +I state (d⁶) *via* Metal-to-Ligand Charge Transfer (MLCT),⁶ for the +II (d⁵) state *via* metal-centered transitions (MC),⁷ and for the +IV state (d³) *via* ligand-to-metal charge transfer (LMCT).⁸

Since the beginning of the 20th century, mineral compounds based on Mn²⁺ have been used as luminescent materials. Mn(II)-doped oxides,⁹ nitrides,⁹ phosphates,¹⁰ borosilicate glasse,¹¹,¹² and sulfides¹³ are considered promising candidates for the development of inexpensive and non-toxic luminescent mineral materials, used as green or red phosphors. However, it is only in recent decades that Mn(II)-based complexes with ligands such as halogenure/phosphine oxides,¹⁴ halogenure/crown ethers,¹⁵ and the sulfonylcalixarene macrocycle¹⁶,¹⁷ have shown luminescent properties in

both solid and solution states. In previous work, we found that under solvothermal conditions, *p-tert*-butylsulfonylcalix[4]arene mixed with a Mn²⁺ salt and fluoride forms tetranuclear metal complexes [Mn₄(ThiaSO₂)₂F]⁻, which upon excitation at 360 nm at room temperature exhibit a strong orange eye-perceived luminescence at a wavelength of about 580 nm. This emission results from the transition between the ⁴T₁(⁴G) excited state and the ⁶A₁(⁶S) ground state of the Mn²⁺ ions present in the cluster (Fig. 1). For several years, we have continued our investigations by modifying this luminescent system to better exploit the symbiosis between the sulfonylcalixarene

<figure><img src="image_3.png" /><figcaption>**Fig. 1** Representation of tetranuclear metal anionic complexes [Mn₄(ThiaSO₂)₂F]⁻, ThiaSO₂ = *p*-tert-butylsulfonylcalix[4]arene.</figcaption></figure>

<figure><img src="image_4.png" /></figure>

<footnote>aUniversite Claude Bernard Lyon 1, CNRS, LMI UMR 5615, Villeurbanne, F-69100, France. E-mail: cedric.desroches@univ-lyon1.fr</footnote>

<footnote>bUniv. Lyon, Université Claude Bernard Lyon 1, CNRS, Institut Lumiere Matiere, F-69622 Villeurbanne, France</footnote>

<footnote>cUniv Rennes, INSA Rennes, CNRS, ISCR "Institut des Sciences Chimiques de Rennes", Rennes F-35000, France</footnote>
ligand and Mn²⁺ ions. It has been shown that the macrocycle conformation,¹⁷,¹⁸ increasing electron delocalization along the phenolic units, as well as modulation of the counter anion¹⁹ significantly alter the optical properties of this family of complexes in the solid-state, such as emission wavelength and oxygen sensitivity. Calix[4]arene macrocycles and their derivatives have demonstrated that the unique combination of four donor-π-acceptor (D-π-A) dipoles endows these systems with remarkable second-order Non-Linear Optical (NLO) properties.²⁰⁻²³ In the cone conformation, the four phenolic units are oriented in the same direction, resulting in a hypochromic shift of the Charge Transfer (CT) band, along with a significant increase in the second-order molecular hyperpolarizability (β). It has also been shown that the D-π-A units within calix[4]arenes do not behave entirely independently, and that the geometry of the cone, whether perfectly symmetric or pinched, affects the total dipole moment and consequently the β values. Other NLO-related properties of this family have also been reported in the literature, in particular their optical limiting capabilities, which are primarily attributed to two-photon absorption mechanisms. In this context, the thiacalix[4]arene family has emerged as particularly promising for optical limiting applications.²⁴ Molecular engineering efforts have led to the identification of (phenylethynyl)thiacalix[4]arenes and their derivatives as excellent candidates for such applications, based on the principle that increased electronic delocalization enhances nonlinear optical properties. Building on these findings, we investigated the ability of sulfonylcalix[4]arenes to sensitize Mn²⁺ ions via a two-photon absorption process. Beyond demonstrating that this family represents the first class of ligands capable of sensitizing Mn²⁺ ions through such a mechanism, this study also opens up new perspectives in the field. Furthermore, this work describes a synthetic route to access the phenylethynylsulfonylcalix[4]arene macrocycle (paThiaSO₂) and its corresponding complexes with Mn²⁺ ions.

## 2. Results and discussion

### 2.1. Synthesis

The use of the thiacalixarene macrocycle as a ligand can be achieved in two ways: (i) the first approach involves using the macrocycle as a platform capable of carrying different types of ligands, which can be grafted onto either the upper or lower part of the macrocycle. (ii) The second approach relies on the chelating ability provided by the phenolic functions located near the oxidized or non-oxidized sulfur atoms. In the case of the molecular system [Mn₄(ThiaSO₂)₂F]⁻, the phenolic functions must be preserved. In this context, increasing delocalization along the phenolic units can be achieved either by directly synthesizing the macrocycle with a pre-modified phenol, such as phenylthiacalixarene,¹⁸ or by subsequently modifying the lipophilic part of the thiacalixarene.²⁵,²⁶ The target ligand, (phenylethynyl)sulfonylcalix[4]arene, cannot be synthesized via the cyclocondensation of four 4-(phenylethynyl)phenol

groups due to the harsh conditions required for this synthesis (alkaline medium, high temperature, and H₂S atmosphere). Therefore, a synthetic route starting from *p*-tert-butylthiacalixarene had to be developed. The reaction scheme followed to obtain (phenylethynyl)sulfonylcalix[4]arene is described in Fig. 2. This synthetic route enables the preparation of a sulfonylcalixarene modified on its lipophilic moiety while preserving its phenolic groups. For paThiaSO₂, the multi-step synthesis (Fig. 2) starting from *p*-tert-butylthiacalixarene (ThiaS) encountered two major obstacles. The first was the protection of the phenolic groups (Fig. 3, step c), to neutralize the complexing power of the macrocycle towards the palladium and copper salts used in the Sonogashira coupling between phenylacetylene and tetra-bromo-thiacalixarene. The second obstacle was the oxidation of sulfur atoms to sulfonyl groups. Acetylation of the phenolic groups proved to be the most reasonable choice for both the protection and deprotection steps of phenolic alcohols. The oxidation step could only be performed out before the deprotection of the acetyl groups and under mild and controlled oxidation conditions to prevent the oxidation of the already formed ethynyl function. It is noteworthy that the formation of sulfonyl groups completely deactivates the macrocycle for the Sonogashira coupling, thus necessitating the coupling prior to oxidation.

The polynuclear complexes K[Mn₄(ThiaSO₂)₂F] (1),¹⁷ and NBu₄[Mn₄(ThiaSO₂)₂F] (2) were synthesized by a solvothermal method at 170 °C by mixing 1 equivalent of the macrocycle with 5 equivalents of Mn²⁺ in a methanol/water mixture [10 : 1], in the presence of 6 equivalents of a fluorinated salt (either KF or NBu₄F) acting both as a base and as a µ4-bridging ligand. The products for these two syntheses were recovered as pale yellow single crystals and exhibited strong orange eye-perceived luminescence upon a 400 nm laser pointer beam. The same solvothermal procedure, but this time with the macrocycle paThiaSO₂, yielded a non-luminescent powder and the characterization did not allow to conclude on the possible formation of a major complex. Irradiation of the same reaction mixture under microwave (900 W, 30 s) produced a non-crystalline powder (3) exhibiting luminescence at room temperature (Fig. 3). Mass spectrometric analysis of this powder, freshly dissolved in dimethylformamide (DMF), shows the presence of the anion [Mn₄(paThiaSO₂)₂F]⁻, indicating that the complex K [Mn₄(paThiaSO₂)₂F] (3) has indeed been formed. Several attempts were made to recrystallize this powder without success in crystallizing the desired compound. Finally, the [Mn₄(paThiaSO₂)₂F]⁻ complex was isolated as a single crystal by replacing the K⁺ counter-anion with tetrabutylammonium (NBu₄⁺). The compound NBu₄[Mn₄(paThiaSO₂)₂F] (4) is obtained either by solvothermal reaction, mixing paThiaSO₂ and MnCl₂·4H₂O in the presence of NBu₄F in a mixture of DMF and methanol in a closed reactor at 110 °C, or by recrystallization of the complex (3) in a methanol/DMF mixture in the presence of NBu₄F at 110 °C. According to the HSAB theory, it seems that increasing the affinity between [Mn₄(paThiaSO₂)₂F]⁻ and the counteranion, namely NBu₄⁺, stabilizes the intimate ion pair NBu₄[Mn₄(paThiaSO₂)₂F] in
<figure><img src="image_5.png" /></figure>

<figure><img src="image_6.png" /><figcaption>**Fig. 2** The reaction scheme for the preparation of paThiaSO₂. (a) Phenol/AlCl₃, toluene, 72%. (b) N-Bromosuccinimide, acetone, 71%. (c) NaOAc, O(Ac)₂, 70 °C, 88%. (d) Phenylacetylene, PdCl₂(PPh₃)₂, Cul, Et₃N, THF, 85%. (e) NaOH, THF/MeOH, 82%. (f) NaBO₃·4H₂O, CH₃COOH/H₂O₂, CHCl₃, 72%.</figcaption></figure>

<figure><img src="image_7.png" /><figcaption>**Fig. 3** Reaction scheme for the preparation of the complexes [Mn₂(paThiaSO₂)(DMF)₄(CH₃CN)₂] (5) and NBu₄[Mn₄(paThiaSO₂)₂F] (4).</figcaption></figure>

solution and thus promotes its crystallization. In addition, vapor-phase acetonitrile diffusion into a solution of (3) dissolved in DMF allowed crystallization of the neutral dinuclear

complex [Mn₂(paThiaSO₂)(DMF)₄(CH₃CN)₂] (5). This dinuclear complex is more easily formed by reacting paThiaSO₂ with MnCl₂·4H₂O in the presence of triethylamine in DMF and then
<figure><img src="image_8.png" /></figure>

crystallizing by acetonitrile diffusion. Previous studies have shown that the complex [Mn₄(ThiaSO₂)₂F]⁻ is unstable in solution to light and to highly coordinating solvents such as DMF or DMSO, resulting in the formation of an analogous dinuclear complex [Mn₂(ThiaSO₂)(DMF)₄(H₂O)₂].¹⁹

## 2.2. Crystal structure

The structure of complex (1) has been discussed in previous articles.¹⁷ Compounds (2) and (4), like compound (1), consist of squares of four manganese(ii) ions sandwiched between two ThiaSO₂ macrocycles, as shown in Fig. 4. In the center of the square formed by the four manganese(ii) ions, the presence of µ₄⁻F⁻ confers a negative charge to the cluster. The electroneutrality of the complex is achieved by the presence of the cation K⁺ for (1) and (3), or NBu₄⁺ for (2) and (4). The originality of this type of aggregate lies in the peculiar coordination of the Mn²⁺ ions, which are located in the center of a capped trigonal biprism with C₂ᵥ symmetry. We also note a relatively unusual square plane coordination of the fluoride anion µ⁴. Among these three different complexes, the interatomic distances between the Mn²⁺ ions and the oxygen atoms of the coordination sphere do not show any major variations. In complexes (1), (2) and (4), a center of symmetry is located on the fluorine atom. Thus, the two macrocycles sandwiching the manganese ions are perfectly identical. However, for (1), the macrocycles adopt a cone conformation, whereas for (2) and (4), the conformation is a pinched cone. Between (2) and (4), it is (2) that has the most pinched cone conformation (Fig. S1).

In compound (1), the cation K⁺ is coordinated by sulfonyl and methanol groups. In compound (2), the shortest inter-action distance between the [Mn₄(paThiaSO₂)₂F]⁻ anion and NBu₄⁺ is 4.553 Å. This interaction occurs between the oxygen of a phenoxy group and the nitrogen atom of the NBu₄⁺ cation

(Fig. S1). These alternating anions and cations form chains along the *a*- and *b*-axes (Fig. 5). The *ab*-planes formed by these chains are stacked along the *c*-axis with only weak van der Waals-type interactions. In compound (4), the shortest inter-action distance between the [Mn₄(paThiaSO₂)₂F]⁻ anion and NBu₄⁺ is 4.027 Å. This interaction takes place between an oxygen of a sulfonyl group and the nitrogen atom of the NBu₄⁺ cation (Fig. S2). The ion pairs {[Mn₄(paThiaSO₂)₂F]⁻; NBu₄⁺} are assembled in the *ab*-plane by ionic interactions between the oxygen of the sulfonyl groups of the macrocycle and the nitrogen atoms of the NBu₄⁺ cation. The *ab*-planes are stacked by introducing a phenylethynyl moiety into the cavity of a macrocycle belonging to another layer (Fig. S3). Two macro-cycles are interlocked one inside the other by the π-interaction between two phenylethynyl moieties (shortest distance 3.469 Å). The torsion angles for the four different phenylethy-nylphenolic units are 50.8°, 3.7°, 64.8° and 36.1°.

The dinuclear complex (5) consists of a paThiaSO₂ macro-cycle adopting a 1,2-alternate conformation and coordinating two Mn²⁺ ions. The coordination sphere of each Mn²⁺ ion is completed by two DMF molecules and one acetonitrile molecule. The coordination of the two Mn(ii) ions is perfectly equivalent due to the presence of an inversion center at the center of the complex. The [MnO₅N₁] coordination sphere exhibits a distorted octahedral geometry. The interatomic distances are 2.115(2) Å and 2.109(2) Å for Mn–Oₚhenol, 2.240(2) Å for Mn–Oₚulfonyl, 2.249(3) Å for Mn–Nₐcetonitrile, and 2.150(3) Å and 2.198 (3) Å for the Mn–OₐDMF bond lengths. The torsion angles for the two different phenylethynylphenol units are 31.8° and 15.60°.

## 2.3. Photophysical characterization

**Absorption in DMF solution.** Fig. 6 shows the absorption spectra at room temperature in DMF solution of K

<figure><img src="image_9.png" /><figcaption>**Fig. 4** X-ray structures of compounds (2) (a), (4) (b) and (5) (c). For compounds (2) and (4), the ThiaSO₂ and paThiaSO₂ macrocycles adopt a cone conformation and Mn(ii) ion assumes a capped biprism trigonal geometry. For compound (5), the paThiaSO₂ macrocycle adopts a 1,2-alternate conformation and Mn(ii) ions assume a distorted octahedral geometry. Atoms are depicted as follows: Mn (purple), O (red), S (yellow), C (grey), F (light green) and N (blue). Hydrogen atoms are omitted for clarity.</figcaption></figure>
<figure><img src="image_10.png" /><figcaption>Fig. 5 (a) Packing of compound (2), projection along the c-axis. (b) Packing of compound (4), projection along the a-axis. The complexes [Mn₄(ThiaSO₂)₂F] and [Mn₄(paThiaSO₂)₂F] are represented in red, and the NBu₄⁺ cation in blue.</figcaption></figure>

<figure><img src="image_11.png" /><figcaption>Fig. 6 Absorption spectra in DMF solution of compounds (1), (2), (3), (4) and (5) at room temperature, c = 4.07 × 10⁵ M for (1), c = 4.2 × 10⁵ M for (2), c = 2.4 × 10⁵ M for (3), c = 2.38 × 10⁵ M for (4) and c = 2.98 × 10⁴ M for (5). The left ordinate scale corresponds to compounds (1) to (4), and the right ordinate scale corresponds to compound (5).</figcaption></figure>

[Mn₄(ThiaSO₂)₂F] (1), (NBu₄)[Mn₄(ThiaSO₂)₂F] (2), K[Mn₄(paThiaSO₂)₂F] (3), (NBu₄)[Mn₄(PaThiaSO₂)₂F] (4) and [Mn₂(paThiaSO₂)(DMF)₄(CH₃CN)₂] (5) between 300 and 450 nm. The absorption spectrum of (1) is identical to that of (2). The observed absorption bands are mainly the signature of the ThiaSO₂ ligand. It can easily be hypothesized that at this concentration the complexes (1) and (2) are present as free ion pairs, and thus the cation, K⁺ for (1) and NBu₄⁺ for (2), has no influence on the absorption. The band can be attributed to π-π* transitions of the ThiaSO₂ ligand. The molar extinction coefficient of the intense absorption band at 350 nm is within experimental accuracy identical for the two compounds with a value of εmax = 72 000 M⁻¹ cm⁻¹. The absorption spectra of compounds (3) and (4) show four absorption maxima at 305 nm (ε = 125 135 M⁻¹ cm⁻¹), 321 nm (ε = 112 140 M⁻¹ cm⁻¹), 356 nm (ε = 46 780 M⁻¹ cm⁻¹), and 373 nm (ε = 47 360 M⁻¹ cm⁻¹).

The profiles of the first three bands (εmax at 305, 321, and 356 nm) correspond to those already described in the literature for the calixarene macrocycle family or for phenylethanethylene monomers.²² The band εmax at 373 nm is attributed to the ThiaSO₂ macrocycle backbone. It is shifted by 23 nm compared to the complexes (1) and (2) and its molar extinction coefficient decreases. For compound (5), the spectral profile is identical to that of compounds (3) and (4). However, a red shift of 10 nm is observed for the absorption maxima of compound (5). The molar absorption coefficients are about ten times lower than those observed for compounds (3) and (4).

### Solid-state excitation and emission spectra

*One-photon excitation.* The Stokes excitation and emission spectra in the solid-state at room temperature for compounds (1), (2), (3), and (4) are shown in Fig. 7. The one-photon excitation spectral profiles for compounds (1) and (3) are similar, with maxima at 400 nm and 422 nm, respectively. The excitation spectral profiles of compounds (2) and (4) are also similar. They exhibit multiple maxima at 326 nm, 370 nm and 412 nm for compound (2) and at 339 nm, 366 nm and 414 nm for compound (4). All compounds exhibit an intense symmetric emission band centered at 600 nm (1), 615 nm (2), 645 nm (3) and 660 nm (4). In all cases, this orange-red emission band originates from the ⁴T₁ → ⁶A₁ transition of Mn (II) in a high-spin d⁵ configuration. The functionalization of sulfonylcalixarene with phenylethynyl units induces a bathochromic shift of 50 nm in the absorption bands, shifting the excitation threshold from 450 nm for compounds (1) and (2) to about 500 nm for compounds (3) and (4). A similar shift is observed in the emission maxima, indicating a change in photophysical properties. The spectroscopic variations reflect a sensitivity to the nature of the cation present, with a clear distinction between the complexes formed with potassium ion (K⁺) and those with tetrabutylammonium (NBu₄⁺). This differentiation is supported by measurements carried out under aerobic and anaerobic conditions, highlighting the influence of the environment on the electronic behavior of the studied systems.
<figure><img src="image_12.png" /><figcaption>Fig. 7 Solid-state excitation (blue line) and emission (black line) spectra of compounds (1), (2), (3), and (4), at room temperature and under air.</figcaption></figure>

Fig. 8 exhibits the emission spectra under Stokes excitation in air and under vacuum for compounds (2) and (4), with tetra-butylammonium as the counteranion. In contrast to compound (1), complexes (2) and (4) show luminescence that is highly sensitive to the presence or absence of oxygen, being 49 times and 2.5 times higher, respectively, in the absence of O₂. At room temperature, the lifetimes of (2) are 1.84 ms in vacuum and 0.68 ms in air, while those of (4) are 0.68 ms (vacuum) and 0.23 ms (air), respectively. These emission lifetimes are shorter than the lifetime measured in air for compound (1), which is 1.63 ms. Fig. S4 shows the evolution over time of the luminescence intensity of the compounds (2) and (4), starting from air and then exposed to a vacuum. Compound (4) responds significantly faster than compound (2), reaching its maximum emission intensity after a few seconds. However, the emission intensity of the compound (2) shows a remarkable increase under vacuum. This difference is probably due to a slower oxygen desorption rate in the structure of (2). Several effects may be responsible for these results: (i) the energy levels of the triplet states of the luminescent anionic complex, as well as the spin-orbit coupling, may be influenced by the iono-covalent character of the cation-anion

<figure><img src="image_13.png" /><figcaption>Fig. 8 Solid-state emission spectra of compounds (2) (a) and (4) (b) upon excitation at 330 nm at room temperature, under air (red line) and vacuum (blue line) conditions.</figcaption></figure>
interaction; (ii) a change in the rigidity and lattice vibrations
may also play a role. Such modifications promote the diffusion
of molecular oxygen and enhance the coupling between the
electronic levels of the luminescent entity and those of oxygen.
In the case of these complexes, the origin of the phenomenon
could be a combination of both effects, with a predominant
role attributed to oxygen diffusion processes. The structures
containing the NBu₄⁺ cation show significantly weaker inter-
actions between the anion and the cation, as well as lower den-
sities (1.393 g cm⁻³ for compound (2), 1.392 g cm⁻³ for com-
pound (4), compared to 1.51 g cm⁻³ for compound (1)).
Among complexes (1), (2), and (4), complex (2) has the largest
distance between the nitrogen atom of Bu₄N⁺ and the oxygen
of a sulfonyl group with dN'-OS = 4.87 Å (for (4), dN'-OS =
4.027 Å, and for (1), dK'-OS = 2.7 Å).

The excitation and emission measurements for the dinuc-
lear compound (5) as a function of temperature, in the pres-
ence and absence of O₂, are shown in Fig. S5 and S6. The
solid-state emission spectrum of (5) exhibits a broad band cen-
tered at around 725 nm under a photo-excitation at 325 nm at

ambient pressure. To avoid oxygen (O₂)-induced quenching,
the luminescence was measured in a vacuum cavity and the
maximum emission band increased by 20%. The solid-state
emission has also been measured at variable temperature
(77-300 K) under excitation at 325 nm in an inert atmosphere
(N₂) (Fig. S6). The luminescence increased by 96% (Fig. S5),
and the emission maximum shifted by 20 nm from 723 nm to
743 nm from 300 K to 77 K. The emission of complex (5) is
very weak and, unlike compounds (1) to (4), is not visible to
the naked eye. It is sensitive to oxygen quenching and to temp-
erature. In contrast to the previously reported analogous
dinuclear complexes, the replacement of *tert*-butyl functions,
such as in the complex [Mn₂(ThiaSO₂)(DMF)₄(H₂O)₂]¹⁹ by
phenyl or phenylethynyl groups, such as in the complexes
[Mn₂(ppThiaSO₂)(DMF)₆] (ppThiaSO₂ = *p*-phenylsulfonylcalix
[4]arene)¹⁸ and [Mn₂(paThiaSO₂)(DMF)₄(CH₃CN)₂] (5), respect-
ively, had significant effects on the photophysical properties of
the complex. The emission of the latter two complexes is
weaker and red-shifted compared to the former. These effects
are consistent with the observation that the absorption

<figure><img src="image_14.png" /><figcaption>Fig. 9 Solid-state excitation and emission spectra of compounds (1), (2), (3) and (4) at room temperature and under air. In red are the two-photon excitation spectra and in green the resulting emission spectra (anti-Stokes) of compounds (1) to (4). The emission was measured with a 600 nm low-pass filter, which explains the cutoff in the spectra. In black are the emission spectra under one-photon excitation (Stokes).</figcaption></figure>

<figure><img src="image_15.png" /></figure>
decreases from ThiaSO₂ to ppThiaSO₂ and paThiaSO₂ macrocycles, which act as antennas.

**Two-photon excitation.** The anti-Stokes excitation and emission spectra, in the solid-state at room temperature, for compounds (1) to (4) are shown in Fig. 9. All the anti-Stokes excitation emission spectra show an emission band corresponding to that obtained under Stokes excitation. This shows that all the presented complexes can be excited by two-photon absorption. This confirms that sulfonylcalixarene is a remarkable antenna for sensitizing Mn²⁺ ions through both one- and two-photon excitation. Among the four compounds, compounds (1) and (3) exhibit the largest two-photon excitation band around 720 nm. The anti-Stokes excitation spectrum of compound (2) shows a weak two-photon excitation band, while compound (4) shows none. As in the case of one-photon absorption, the replacement of the K⁺ counterion by NBu₄⁺ induces the most significant change in the photophysical properties of this molecular system.

The room temperature emission lifetime measurements (Stokes and anti-Stokes) of compounds (1) to (4) in air are shown in Fig. S7. Compound (1) exhibits a nearly monoexponential luminescence decay with a calculated lifetime of τ = 1.74 ms. This lifetime is in agreement with previously reported values for the same compound.¹⁶ Compound (2) shows a biexponential luminescence decay with τ₁ = 0.0153 ms (85%) and τ₂ = 0.85 ms (15%). The first decay is attributed here to luminescence quenching caused by the presence of oxygen. The lifetimes for compounds (3) and (4) show multiexponential decay curves, with average lifetimes of τ = 0.091 ms and τ = 0.076 ms, respectively.

The luminescence results confirm that the molecular system [Mn₄(ThiaSO₂)₂F]⁻ has the ability to be excited by either one-photon or two-photons. However, the functionalization of the system with phenylethynyl chains only resulted in a shift in the Stokes wavelengths of both excitation and emission for the system, without improving the nonlinear absorption. The increased electron delocalization along the phenolic moieties seems to destabilize the electronic delocalization of the thiacalixarene crown, thereby reducing the two-photon absorption capacity of this molecular system. Optical measurements also revealed the important role of the interactions between the cation and the luminescent anion, especially with respect to energy transfer to molecular oxygen.

### 3. Conclusion

Thiacalixarene complexes have been studied since the late 1990s when this macrocycle was first synthesized. The structure of this macrocycle, with its chelating functions formed by phenolic groups located near oxidized or non-oxidized sulfur atoms, immediately showed strong potential for the development of metal complexes. In addition to its role as a highly structuring ligand for the formation of polynuclear complexes, thiacalixarene exhibits interesting electronic properties that allow it to efficiently sensitize Mn²⁺ ions. Tetranuclear complexes based on Mn²⁺ ions and sulfonylcalixarene macrocycles

exhibit, when excited with blue light (360 to 400 nm), a broad luminescence band around 600 nm, resulting from the d-d transition T₁(t₂g⁴eg¹) → ⁶A₁(t₂g³eg²) of the Mn²⁺ ions. To broaden the applications of these luminescent complexes, their ability to be excited by lower energy multiphoton absorption was investigated. Previous nonlinear optics studies had highlighted the interesting properties of this macrocycle when functionalized with phenylethynyl groups. Various complexes based on *p*-tert-butylsulfonyl[4]arene and *p*-phenylethynylsulfonylcalix[4]arene macrocycle derivatives have been synthesized and characterized. The results obtained demonstrate the possibility of two-photon sensitization of Mn²⁺ ions through the sulfonylcalixarene macrocycle. However, increasing electronic delocalization along the phenolic units negatively affects the anti-Stokes excitations properties of these molecular systems. Depending on the nature of the counteranion (NBu₄⁺ or K⁺), the luminescence of the Mn²⁺ ions can be quenched more or less intense. The most probable mechanism is an energy transfer from the excited complex to O₂, thereby exciting O₂ from its ground state ³Σ⁻g⁻ to its excited state ¹Σ⁺g⁺.²⁷,²⁸ The quenching is more effective when the interaction between the tetrabutylammonium and the sulfonyl groups is weaker and when the open structure facilitates the diffusion of O₂ within the crystalline network. This work contributes to a better understanding of the sulfonylcalixarene/Mn²⁺ luminescent systems. It also provides a way to functionalize the upper rim of the macrocycle to increase electron delocalization along the phenolic units while preserving the complexing nature of the phenolic functions. Further studies are underway to explore and better understand the sensitivity of this type of system to oxygen.

### 4. Experimental

All chemicals and solvents were used as received (solvents and chemicals: Aldrich); *p*-tert-butylthiacalix[4]arene (*p*-tert-ThiaS),²⁹ thiacalix[4]arene (ThiaS), *p*-tert-butylsulfonylcalix[4]arene (ThiaSO₂),³⁰ *p*-bromo-thiacalix[4]arene (ThiaSBr)³¹ and K [Mn₄(ThiaSO₂)₂F] (1)¹⁷ were synthesized using the protocols from the literature.

#### 4.1 Synthesis of *p*-bromo-acetoxythiacalix[4]arene (ThiaSBrOAc)

Under inert atmosphere, ThiaSBr (4.9 g, 6 mmol) is suspended in acetic anhydride (50 ml), and anhydrous sodium acetate (10 g) is added. The solution is refluxed for 24 hours and then hydrolyzed for 1 hour after returning to room temperature. The powder is filtered under vacuum and rinsed with methanol. After drying, the *p*-bromo-acetoxythiacalix[4]arene is used without purification for the next step. Yield = 88%. RMN ¹H (Fig. S8, CDCl₃, 300 MHz, 293 K): δ (ppm) = 7.9 (d, 4H, *J* = 4.64 Hz, H₁,₃-Ar), 7.69 (d, 2H, *J* = 2.35 Hz, H₁,₃-Ar), 7.19 (d, 2H, *J* = 2.29 Hz, H₁,₃-Ar), 2.55 (s, 3H, ArO-COCH₃), 2.41 (s, 6H, ArO-CO-CH₃), 1.71 (s, 3H, ArO-CO-CH₃). MS (ESI): *m/z* = 1002.6 [M + Na]⁺. IR: ν (cm⁻¹) = 3058, 2362, 2332, 2284, 2172, 2106, 1906,

<figure><img src="image_16.png" /></figure>
1768, 1546, 1414, 1366, 1170, 1112, 1078, 1042, 1010, 900, 876, 834, 792, 762, 690, 632. Melting point: 354 °C.

## 4.2 Synthesis of *p*-phenylacetylene-acetoxythiacalix[4]arene (*paThiaSOAc*)

Under inert atmosphere, ThiaSBrOAc (0.74 g, 0.75 mmol) is dissolved in anhydrous THF (15 ml), followed by the addition of triethylamine Et₃N (0.45 ml). To this solution PdCl₂(PPh₃)₂ (0.052 g, 0.074 mmol), CuI (0.002 g, 0.007 mmol), and phenylacetylene (0.45 ml, 4.1 mmol) are added successively. The solution turns dark orange. The reaction mixture is heated to 40 °C for 48 hours. The solution is then evaporated to dryness. The product obtained is dissolved in 50 ml of dichloromethane and washed with 2 × 25 ml of HCl (1 M). The organic phase is dried with Na₂SO₄ and concentrated. The addition of methanol allows the precipitation of a white powder of paThiaSOAc. After filtration and drying, paThiaSOAc is obtained with a yield of 85%. RMN ¹H (Fig. S9, CDCl₃, 300 MHz, 293 K): δ (ppm) = 7.66 (s, 8H, H₁,₃-Ar), 7.5 (dd, 8H, *J* = 2.95, 6.66 Hz, H₁₀,₁₄-Ar), 7.36 (m, 12H, H₁₁-₁₃-Ar), 1.83 (s, 12H, ArO-COH₃). MS (ESI): *m/z* = 1087.1 [M + Na]⁺. IR: *ν* (cm⁻¹) = 3062, 2360, 2328, 1770, 1600, 1572, 1492, 1434, 1368, 1172, 1080, 1010, 894, 818, 802, 757, 688, 626. Melting point: 310 °C.

## 4.3 Synthesis of *p*-phenylacetylenethiacalix[4]arene (*paThiaS*)

paThiaSOAc (0.5 g, 0.47 mmol) is suspended in 20 mL of THF and 6 mL of a concentrated sodium hydroxide solution (8 M, THF (4 ml)/methanol (2 ml)) is added. The solution is heated under reflux for 4 hours until the powder is completely dissolved. The solution is evaporated to dryness and the product is redissolved in 20 mL chloroform, then washed with 2 × 10 mL HCl (1 M). The organic phase is dried over MgSO₄ and then evaporated to dryness. The product is taken up in ether and precipitated with stirring. After filtration and drying, paThiaS is obtained with a yield of 82%. RMN ¹H (Fig. S10, CDCl₃, 300 MHz, 293 K): δ (ppm) = 9.29 (d, 4H, *J* = 3.09 Hz, Ar-OH), 7.83 (s, 8H, H-Ar), 7.5 (m, 8H, H-Ar), 7.32 (m, 12H, H-Ar). RMN ¹³C (CDCl₃, 100 MHz, 293 K): δ (ppm) = 157.8 (Ar, C5), 142.2 (Ar, C1,3), 131.6 (Ar, C10,14), 128.5 et 128.4 (Ar, C₁₁-₁₃), 122.8 (Ar, C9), 120.6 (Ar, C4,6), 117.4 (Ar, C2), 89.8 (C≡C, C7), 87.1 (C≡C, C8). MS (ESI): *m/z* = 895.1 [M - H]⁻. IR: *ν* (cm⁻¹) = 3316, 3054, 2258, 2336, 1770, 1598, 1578, 1550, 1492, 1446, 1386, 1342, 1314, 1260, 1236, 1176, 1156, 1074, 1026, 892, 814, 752, 688. Melting point: 215 °C.

## 4.4 Synthesis of *p*-phenylacetylenesulfonylcalix[4]arene (*paThiaSO₂*)

In a 10 ml flask, 0.2 g of paThiaS (0.22 mmol) is dissolved in 0.4 mL of chloroform. To this solution, 3 mL of acetic acid, 1 mL of hydrogen peroxide (30%) and 0.38 g of sodium perborate tetrahydrate NaBO₃·4H₂O (2.5 mmol) are added. The solution was stirred for 16 hours at room temperature. Then, 10 mL of HCl (1 M) and 10 mL of chloroform are added to the reaction medium for extraction. The organic phase is extracted, washed with 10 mL HCl (1 M) and dried over MgSO₄. The resulting solution is evaporated to dryness. The product is

taken up in ether and precipitated with stirring. After filtration and drying, paThiaSO₂ is obtained with a yield of 72%. RMN ¹H (Fig. S11, DMSO-d₆, 300 MHz, 293 K): δ (ppm) = 8.14 (s, 8H, H₁,₃-Ar), 7.51 (m, 8H, H₁₀,₁₄-Ar), 7.35 (m, 12H, H₁₁-₁₃-Ar). RMN ¹³C (DMSO-d₆, 100 MHz, 293 K): δ (ppm) = 137.3 (Ar, C5), 132.4 (Ar, C1,3), 131.2 (Ar, C10,14), 129.87 (Ar, C4,6), 128.3 (Ar, C₁₁-₁₃), 121.9 (Ar, C9), 89.5 (C≡C, C7), 86.6 (C≡C, C8). MS (ESI): *m/z* = 1023.1 [M - H]⁻. IR: *ν* (cm⁻¹) = 3456, 2958, 2924, 2853, 2363, 1591, 1494, 1468, 1411, 1384, 1267, 1197, 1166, 1136, 1080, 1037, 932, 910, 799, 756, 715, 690, 616. Melting point: 230 °C.

## 4.5 Synthesis of NBU₄[Mn₄(ThiaSO₂)₂F] (2)

In a Teflon autoclave of 20 mL were added ThiaSO₂ (0.05 g, 0.06 mmol), MnCl₂·4H₂O (0.05 g, 0.3 mmol), and tetra-*n*-butylammonium fluoride hydrate (TBAF) (0.1 g, 0.38 mmol anhydrous basis). The reactants were dissolved in a solvent mixture of MeOH/H₂O (10/0.5 in mL). After heating for two days in an oven at 170 °C, long needle-like crystals of compound (2) were isolated, washed several times with methanol, and dried (yield = 74%). Elemental analysis (mass%): C₉₆H₁₂₄F₁N₁Mn₄O₂₄S₈ (2171.26 g mol⁻¹): calc Mn 10.12, S 11.81; found Mn 10.05, S 11.72. IR *ν* (cm⁻¹) = 3443, 2959, 2870, 1604, 1517, 1462, 1364, 1331, 1265, 1220, 1196, 1136, 1087, 907, 836, 796, 748, 651, 627.

## 4.6 Synthesis of K[Mn₄(paThiaSO₂)₂F] (3)

paThiaSO₂ (0.01 g, 9.76 µmol), MnCl₂·4H₂O (0.01 g, 0.05 mmol) and KF (0.02 g, 0.34 mmol) are suspended in 5 mL of methanol. The mixture is heated under a microwave (900 W) for 3 × 30 s. A white powder, which shows an intense red eye-perceived emission under a 400 nm laser pointer, is obtained by centrifugation and rinsed 3 times with 3 mL of methanol. After drying, the light yellow powder of (3) is obtained in 32% yield. MS (ESI): *m/z* = 2278.8 [M]⁻. IR *ν* (cm⁻¹) = 3443, 1583, 1492, 1470, 1387, 1338, 1268, 1191, 1128, 1079, 925, 827, 785, 743, 695, 617.

## 4.7 Synthesis of NBU₄[Mn₄(paThiaSO₂)₂F] (4)

**Method 1:** In a Teflon autoclave of 10 mL were added paThiaSO₂ (0.05 g, 9.76 µmol), MnCl₂·4H₂O (0.01 g, 0.05 mmol) and TBAF (0.02 g, 0.34 mmol). The reactants were dissolved in a solvent mixture of DMF/MeOH (0.3/0.5 in mL). After heating for 24 h in an oven at 110 °C and slow cooling (0.1° min⁻¹), needle-like crystals of compound (4) were isolated (yield 43%). **Method 2:** In a Teflon autoclave of 10 mL were added 0.03 g of (3) and 0.02 g TBAF (0.34 mmol). The reactants were dissolved in a solvent mixture of DMF/MeOH (0.3/0.5 in mL) After heating for 24 h in an oven at 110 °C and slow cooling (0.1° min⁻¹), needle-like crystals of compound (4) were isolated, washed several times with methanol, and dried (yields 34%). Elemental analysis (mass %): C₁₂₈H₉₂F₁N₁Mn₄O₂₄S₈ (2523.36 g mol⁻¹): calc Mn 8.71, S 10.16; found Mn 8.73, S 10.11. MS (ESI): *m/z* = 2278.8 [M]⁻. IR *ν* (cm⁻¹) = 3451, 1590, 1494, 1462, 1384, 1250, 1184, 1136, 1078, 984, 928, 830, 792, 751, 690, 653, 624.
## 4.8 Synthesis of [Mn₂(paThiaSO₂)(DMF)₄(ACN)₂] (5)

Method 1: 0.01 g (4.1 µmol) of complex (3) is dissolved in 0.2 ml of DMF. After slow diffusion of acetonitrile vapor, compound (5) is recovered in the form of yellow single crystals (yields 27%). Method 2: paThiaSO₂ (0.02 g, 0.0196 mmol) and MnCl₂·4H₂O (0.01 g, 0.05 mmol) are dissolved in 0.5 ml of DMF. Triethyl amine (20 µl, 0.14 mmol) are added to the solution. After slow diffusion of acetonitrile vapor, compound (5) is recovered in the form of yellow single crystals (yields 43%). Elemental analysis (mass%): C₇₂H₆₂N₆Mn₂O₁₂S₄ (1441.43 g mol⁻¹): calc Mn 7.62, S 8.9; found Mn 7.64, S 8.11. IR ν (cm⁻¹) = 3437, 2960, 2923, 2853, 2370, 2345, 1591, 1494, 1384, 1322, 1269, 1189, 1158, 1119, 1070, 832, 799, 755, 717.

## 4.9 Characterizations

Suitable crystals of compounds (2), (4) and (5) were selected and mounted on a Rigaku-OD Synergy-S single-crystal diffractometer equipped with an Hypix-100 detector. Intensities were collected at 100 K with copper radiation (λ = 1.54184 Å) by means of the CrysalisPro software.³² Reflection indexing, unit-cell parameters refinement, Lorentz-polarization correction, peak integration and background determination were carried out with the CrysalisPro software.³² An analytical absorption correction was applied using the modeled faces of the crystal.³³ The resulting set of *hkl* was used for structure solution and refinement. The structures were solved with the ShelXT³⁴ structure solution program using the intrinsic phasing solution method and by using Olex2³⁵ as the graphical interface. The model was refined with version 2018/3 of ShelXL³⁶ using least-squares minimization.

CCDC 2034491 for (2), 2425373 for (4) and 2430432 for (5) contain the supplementary crystallographic data for this paper.

Solid-state excitation and emission spectra were recorded with a commercial fluorimeter (Horiba Jobin Yvon FL3 22, Fluorolog-3) equipped with a Xe lamp 450 W, and a UV Vis near-IR photomultiplier (Hamamatsu R928, sensitivity 190–860 nm). The excitation/emission spectra were realized on powder samples pasted directly onto copper plates using conductive silver glue. Appropriate filters were utilized to remove the laser light, the Rayleigh scattered light, and associated harmonics from the emission spectra. The emission spectra were corrected for the instrumental response function. For the measurements realized at variable temperatures (77 K–300 K), the samples were introduced in an OptistatCF liquid nitrogen-cooled cryostat from Oxford Instruments. Luminescence decays (τ > 10 µs) were also measured at room temperature using this apparatus with a xenon flash lamp (phosphorescence mode). Lifetimes were averaged of 2 or 3 independent determinations. The air pressure-dependent solid-state luminescence spectra were realized in a cryostat equipped with a primary pump.

Stokes emission and excitation spectra (black and blue curves respectively) are made on a home made spectrofluorimeter. A xenon laser-driven light source (EQ99 from Energetiq)

is coupled into a Jobin Yvon Gemini double monochromator and used to illuminate the sample over a 2 × 2 mm spot. The emission is then collected by an optical fiber feeding a monochromator (ANDOR KYMERA328i) equipped with an EMCCD camera (ANDOR NEWTON) and a set of order removinf filters. The whole setup has been calibrated by use of a calibrated power meter for the light source (918D from Newport) and by a calibrated lamp (Avantes Avalight-DH-CAL) for the detection.

Anti-Stokes emission and excitation spectra (green and red curves respectively) are performed using an OPO laser (NT-230-50-SH from Ekspla) as the light source and the same detection system as described for Stokes measurement but with the addition of a low pass filter at 600 nm to remove the laser diffusion.

Lifetime were performed using the OPO laser as the excitation source but this time the light is collected by another optical fibre and send to a Jobin Yvon TRIAX330 monochromator coupled with a Peltier cooled R2949 Hamamatsu photomultiplier. The emitted photons are sorted according to their arrival after the laser pulse thanks to an MCS6A multichannel scaler from FastcomTec. The light diffused by the laser is filtered by the monochromator and additional short or high pass filters depending on the conditions of excitation and emission.

**Nuclear magnetic resonance.** Proton ¹H NMR spectra were recorded on a Bruker AVS 300 (300 MHz) spectrometer. (CD₃)₂SO was used as the intern deuterated reference δH (ppm) 2.50.

**Mass spectrometer.** Mass spectra were recorded on a MicrOTOFD II-Bruker spectrometer with an ElectroSpray Ionization method (ESI), allowing a mass detection between 50 and 20 000 m/z.

## Conflicts of interest

There are no conflicts to declare.

## Data availability

Supporting data are included in the supplementary information (SI). Supplementary information: synthesis details, photophysical data, and X-ray crystallography details. See DOI: https://doi.org/10.1039/d5dt02234g.

CCDC 2034491 (2), 2425373 (4) and 2430432 (5) contain the supplementary crystallographic data for this paper.³⁷a-c

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37 (a) CCDC 2034491: Experimental Crystal Structure Determination, 2025, DOI: 10.5517/ccdc.csd.cc2691rb;

(b) CCDC 2425373: Experimental Crystal Structure Determination, 2025, DOI: 10.5517/ccdc.csd.cc2mdsvp;

(c) CCDC 2430432: Experimental Crystal Structure Determination, 2025, DOI: 10.5517/ccdc.csd.cc2ml21c.