The X-ray diffraction (XRD) patterns of synthesized Tb3+ and Tb3+&Bi3+ co-doped LaF3 samples are shown in Fig. 1a and 1b with their respective dopant concentrations. The total number of peaks and their position are observed to match well with that of ICDD File no.: 32–0483, which indicate that all the samples formed are in hexagonal phase of LaF3 (space group P3c1). However, peak shifting towards higher 2θ values were observed with increase in concentration of Tb3+ (Fig. 1a) as compared to that of Bi3+( Fig. 1b) in LaF3. This may be due to the variation in ionic radius of Tb3+( 92.3 pm, VI coordination) which is lesser compared to La3+( 103.2 pm, VI coordination), whereas the ionic radius of Bi3+( 103 pm, VI coordination) is similar to that of La3+.[37] Thus, it shows the effective replacement of La3+ with dopants Tb3+ and Bi3+ in LaF3 unit cell. Furthermore, no variation in width of diffraction peaks were observed irrespective of dopants (Tb3+& Bi3+) concentration or their combination used in samples. This proves all the samples are formed with nearly similar crystallite size. By utilizing Scherrer formula, the calculated crystallite size from FWHM of (111) reflection is ~ 11 nm.[38]
Particle size distribution or hydrodynamic diameter of samples were measured using dynamic light scattering (DLS) technique. Figure 2 shows the particle size distribution of all samples. As shown in them, size distribution of particles is spread over 10–100 nm range with most of them are in 20–40 nm range. This resultant narrow particle size distribution is one of the advantages of synthesis technique utilized for sample preparation. Further, measured zeta potential value is ~ + 45 mV, which indicate that particles are well dispersed in deionised water (at pH = 7) due to electrostatic repulsion occurring between them.
Since, the hydrodynamic diameter is observed to be similar for all samples, particle size analysis using transmission electron microscope (TEM) were carried out on one of it. Figure 3 shows the TEM image of LaF3:1%Tb,1%Bi sample. The nanoparticles are formed in spherical shape with average particle size of ~ 20 nm. However, this particle size value is much larger than that of crystallite size calculated using XRD data. This discrepancy may be due the polycrystalline nature of nanoparticles as evident in Fig. 3, which is caused by self-assembling of subunits to shape the resultant nanoparticle.[39]
X-ray Photoelectron Spectroscopy (XPS) was performed to determine the elemental presence in the LaF3:1%Tb,1%Bi nanophosphor. A wide-scan spectrum covering a binding energy range of 0-1300 eV was acquired. After carbon correction, the survey spectrum exhibited peaks attributed to C 1s, O 1s, F 1s, La (3p, 3d, 4p, and 4d), Bi (3d and 4f), and Tb 3d as shown in Fig. 4. The presence of Bi and Tb peaks in the spectrum confirms the successful doping of these ions into the LaF3 host lattice.
Fourier Transform Infrared (FTIR) spectroscopy was used to identify the functional groups present on the surface of LaF3:1%Tb,1%Bi nanophosphor. As shown in Fig. 5, a broad band centered at 3415 cm⁻1indicates the O-H stretching vibration of adsorbed water, while the peak at 1630 cm⁻1 is attributed to the bending vibrations of its O-H groups.[40] The characteristic peak at 1452 cm⁻1 is assigned to the asymmetric and symmetric bending vibrations of the O-H group from methanol. Additionally, the peak at 1352 cm⁻1 arises from the bending vibrations of the C-H bonds in the methyl group of methanol.[41] The spectra also show absorption of atmospheric CO2, evident by a small peak at ~ 2350 cm⁻¹.[40] These findings suggest that the surface of the nanophosphor is contaminated with adsorbed water and methanol, likely introduced during the sample preparation process.
To assess the light absorption properties relevant to sunscreen applications, we investigated the UV-visible absorption spectra of LaF3:Tb,Bi nanophosphors (such as LaF3:1.5%Tb and LaF3:1.5%Tb,10%Bi), as shown in Fig. 6.The spectra revealed a broad peak around 250 nm, corresponding to the electronic transition (1S0 → 1P1) in Bi³⁺ ions.[42, 43] This peak suggests efficient absorption of UV radiation by the nanophosphors. The broadness of the peak might indicate the presence of localized defect states within the material.[44]
Next, we explored the luminescence properties using photoluminescence (PL) excitation spectroscopy. These spectra assess how effectively different wavelengths of light can excite the material and cause it to emit light. The spectra were recorded in the 200–400 nm range while monitoring the characteristic Tb³⁺ emission at 543 nm (due to the 5D4 → 7F5 transition) as shown in Fig. 7.[45] This allows to observe how different light wavelengths influenced the emission from the Tb³⁺ ions.
The PL excitation spectra confirmed excitation of both LaF3:Tb and LaF3:Tb,Bi nanophosphors across various wavelengths in the near-UV region. These excitations correspond to different energy level transitions within Tb³⁺ ions (f-d and f-f transitions). Notably, LaF3:Tb,Bi displayed an additional strong excitation band between 225–275 nm, which was absent in LaF3:Tb alone. This new band aligns with the previously observed Bi³⁺ absorption peak (around 250 nm) and is attributed to the 1S0 → 1P1 transition in Bi³⁺ ions. The presence of this Bi3+ absorption band in the Tb3+ excitation spectrum indicates that energy transfer between the dopant ions might be possible.
Since, the intense excitation peak in the case of LaF3:1%Tb was observed at ~ 350 nm which corresponds to 5F6 → 5G4 transition of Tb3+.[46] Thus, this excitation source was used for optimizing the concentration of Tb3+ in LaF3 host. Figure 8a shows the emission spectra of LaF3:x%Tb (x = 0.5, 1, 1.5 & 2) in visible spectral range upon 350 nm excitation. Mainly four distinct emission peaks corresponding to 5D4→7F6 (488 nm), 5D4→7F5 (543 nm), 5D4→7F4 (583 nm) and 5D4→7F3(620 nm) electronic transitions in Tb3+ ion were observed. [47–49]
Initially, with increase in concentration of Tb3+, the PL emission intensity also increases. This increase may be due to the increase in absorption cross section of Tb3+ ion at 350 nm. However, emission intensity decreases for higher concentration of Tb3+ (> 1.5 mol%). This may be occurred due to the concentration quenching effects.[30, 50]
Similarly, Bi3+ excitation peak centred at ~ 250 nm, was used for optimising its concentration in LaF3:1.5%Tb nanophosphor. Figure 8b shows the emission spectra of LaF3:1.5%Tb,y%Bi (y = 0, 5, 10, 15 & 20) in visible spectral range upon 250 nm excitation. The observed emission spectra are identical to those of Tb3+ singly doped in LaF3 nanophosphors (Fig. 8a). Hence, all the emission peaks are characteristics of electronic transitions in Tb3+ ion. Since, on Bi3+ excitation (i.e., at 250 nm), the emission intensity of Tb3+ increases without any variation in number or position of peaks observed in PL emission spectrum demonstrates applicability of Bi3+ as an efficient sensitizer for Tb3+ ion. Figure 8c shows photographs of LaF3:1.5%Tb,10%Bi nanophosphors dispersed in water under daylight and a 250 nm UV light source. This comparison allows one to correlate the observed emission spectrum with the human eye's perception of colour.
To explore the luminescence capabilities and assess their suitability as phosphor applications, it's crucial to ascertain the material's quantum efficiency. This efficiency is defined as the proportion of emitted photons to that of absorbed photons. The quantum efficiency of LaF3:1.5%Tb3+,x%Bi3+ nanophosphors were assessed by monitoring the excitation at 250 nm and emission within 400 to 800 nm wavelength range as shown in table 1.
The energy transfer from sensitizer to activator ion occurs mainly by two ways, termed as radiative and nonradiative energy transfer process. The radiative energy transfer involves, reabsorption of sensitizer emission by an activator ion. Thus, to evaluate its contribution in energy transfer, overlap between the emission spectrum of LaF3:1%Bi3+ (upon 250 nm excitation) and excitation spectrum of LaF3:1%Tb3+ (for 543 nm emission) plotted in Fig. 9. A very small overlap between them were observed, which demonstrates that dominant contribution of non-radiative energy transfer process.[51]
Further, to investigate the type of non-radiative energy transfer process, occurring between Bi3+ and Tb3+ co-doped in LaF3, luminescence decay analysis was carried out. Figure 10a shows luminescence decay curves obtained upon excitation at 250 nm (corresponding to 1S0\(\:\to\:\)1P1 transition of Bi3+) and monitoring emission at 550 nm (corresponding to 3P1\(\:\to\:\)1S0 transition of Bi3+). These decay curves are well fitted with double exponential function: [52]
$$\:I\left(t\right)={I}_{0}+\:{A}_{1}{e}^{-\frac{t}{{\tau\:}_{1}}}+{A}_{2}{e}^{-\frac{t}{{\tau\:}_{2}}}$$
here, I(t) and I0 represents the photoluminescence intensity at time t and at t = 0, \(\:{\tau\:}_{1}\) and \(\:{\tau\:}_{2}\) denote decay lifetimes, with \(\:{A}_{1}\) and \(\:{A}_{2}\) as constants. Utilizing this, we can determine the average lifetime (\(\:<\tau\:>)\) through [52, 53]
$$\:<\tau\:>=\frac{{A}_{1}{\tau\:}_{1}^{2}+{A}_{2}{\tau\:}_{2}^{2}}{{A}_{1}{\tau\:}_{1}+{A}_{2}{\tau\:}_{2}}$$
The decay times corresponding to different dopant concentrations are illustrated in inset of Fig. 10a. Notably, the analysis reveals a sequential decrease in < τ > of the excited Bi3+ state from 993 ns to 805 ns with increasing Tb3+ concentration in LaF3. This observation substantiates the existence of energy transfer from Bi3+ to Tb3+ via a non-radiative mechanism. Efficiency (\(\:{\eta\:}_{ET}\)) of this energy transfer can be determined using:[53]
$$\:{\eta\:}_{ET}=1-\frac{{\tau\:}_{sa}}{{\tau\:}_{s}}$$
here \(\:{\tau\:}_{s}\:\text{a}\text{n}\text{d}\:{\tau\:}_{sa}\:\)represents the lifetime of Bi3+ singly doped and codoped with Tb3+ in LaF3, respectively. A consistent increase in \(\:{\eta\:}_{ET}\) is observed with rising Tb3+ concentration as shown in Fig. 10b. However, Tb3+ concentration is constrained to 2 mol% due to the onset of concentration quenching beyond it, as evidenced in PL emission spectra (Fig. 8a).
Adhering to the Dexter and Reisfeld approximation for multipolar interaction type for energy transfer, we evaluate the relation[54, 55]
$$\:\frac{{\tau\:}_{sa}}{{\tau\:}_{s}}\alpha\:\:{C}^{n/3}$$
here, \(\:C\) denotes the total concentration (i.e. sum of Tb3+ an Bi3+ concentrations in LaF3), and \(\:n=\:\)6, 8 and 10 correspond to dipole-dipole, dipole-quadrupole and quadrupole-quadrupole interaction, respectively. Figure 11 presents the result following linear fitting of the above equation. The optimal fitting outcome for n = 8, suggests the energy transfer is predominantly a consequence of dipole-quadrupole interaction.
The schematic diagram depicting the involved energy transfer between Bi3+ and Tb3+ is shown in Fig. 12. The incident 250 nm photon excites electron of Bi3+ from ground state 1S0 to 1P1 level via electric dipole transition.[33, 56] Then it relaxes via multiphoton process to lower energy level 3P1.[31] In the absence of activator ion (Tb3+) emission peak centred at ~ 550 nm occurs due to radiative emission caused by electronic transition from 3P1 excited state to ground state 1S0 of Bi3+. However, in the presence of Tb3+ as a co-dopant in LaF3:Bi3+ nanophosphor, resonant type energy transfer from 3P1 (of Bi3+) to 5D4 (of Tb3+) occurs via electric multipolar interaction.[56]
Cytotoxicity evaluation of LaF3:1.5%Tb,10%Bi was carried out using MTT assay on HaCaT cells. Cells treated with nanoparticles of different concentration (0, 0.1, 0.2, 0.3, 0.4, and 0.5 mg/mL). The cell viability percentage on treatment with respective dispersion concentrations are as shown in Fig. 13. The relative cell viability was estimated by taking the ratio of observed cell viability percentage after treatment of cells with and without nanoparticles. These are > 80% till 0.4 mg/mL concentration, which indicates negligible toxicity effect on HaCaT cell. Thus, obtained result display potential applicability of synthesized nanophosphors as an ingredient in sunscreen lotion to protect skin from UV rays.