English

• 0.   Introduction

  Organic light emitting diodes (OLEDs) are known as "Dream Display" owing to their several advantages, such as low energy consumption, spontaneous lumine-scence, which is expected to be the next generation panel display and solid-state lighting technique^[1-2]. Iridium complexes are widely used in OLEDs because of their high luminescent quantum efficiency^[3]. In order to meet the requirement of practicability, in addition to the luminescent efficiency, the long-term stability of devices greatly attracts the attention of researchers. In addition, exploring multidentate complexes with strong stability is the main topic of research today. For example, Chi et al.^[4] developed a collection of bis-tridentate Ir(Ⅲ) metal complexes. In terms of these complexes, 100% of internal quantum efficiency was achieved, the entire visible region was covered, and the stability of the organic electrolu-minescent device was greatly increased. They also developed a class of facial tridentate phosphor neutral iridium complexes^[5-7], and the bis-cyclometallated phosphorus ligands were not luminescent because of broken conjugate and the dominant emissive groups were diimine ligands, which was rare in iridium complexes. At the same time, the intramolecular π-π accumulation in these complexes was also found, but the model complex Ir(tpit)(bpy)Cl was less studied and the solid state lighting as well as electroluminescence performance hadn′t been reported. Our research group improved this kind of complexes with dipyridine ligands containing ester groups, the luminescence in solid state could be enhanced by 17 times compared with that in the solution state, which was caused by strong aggregation-induced luminescence enhancement effect^[8]. In addition, it was found that this kind of complexes can be used as silver ion probes with the detection limit up to 0.13 μmol·L^{-1 [9]}, indicating a good application prospect for these complexes. The stability of the iridium complexes was able to be enhanced by intramolecular π-π stacking. The most reported complexes with intramolecular π-π stacking were ionic, like which Chen et al.^[10] synthesized an ionic iridium complex containing intramolecular π-π accumulation. However, neutral complexes with intramolecular π-π stacking were rarely reported^[11-14]. For example, Congrave et al.^[15] synthesized some neutral complexes with phenylpyridine (ppy)-based cyclometalating ligands. The intramolecular π-π interaction weakens the elongation of excited state for metal-ligand, thus reduces the ability of external substances to enter the metal coordination center. The lifetime of electrochemical cells containing these iridium complexes could last up to 585 minutes, 4 times longer than that of materials without π-π interaction.

  4, 5-diazo-9, 9-spirobifluorene (sb) is widely used in the transition metal complexes^[16-19], which is a kind of rigid diimine ligand^[20-21] and fluorene groups are linked to dipyridine using carbon atoms with small conjugation, reducing the molecular aggregation and luminescent quenching in light-emitting iridium complexes^[22-25]. For example, 22.6 and 26.2 lm·W^-1 of luminous electrochemical cell power efficiency for complexes [Ir(ppy)₂sb]PF₆ and [Ir(dFppy)₂sb]PF₆ were achieved^[22], which were the highest efficiencies reported at the time. Since the ligand is electrically neutral, the iridium complexes prepared by it are ionic. Based on the above background, we synthesized neutral iridium complexes by introducing ligand sb (4, 5-diazo-9, 9-spirodifluorene) in tridentate phosphor. By comp-aring complex Ir(tpit)(sb)Cl (tpitH₂=triphenyl phos-phite) with model complex Ir(tpit)(bpy)Cl (bpy=2, 2′-bipyridine) reported in the literature, the impact of diimine ligand on the performance of iridium complexes was studied.

  1.   Experimental

  1.1   Materials and characterization

  All reagents without special instructions are commercially analyzed pure products, which can be used directly after purchase. NMR were recorded on a BRUKER Avance Ⅲ 400 spectrometer. X-ray crys-tallography diffraction data was tested by a Bruker SMART AEX Ⅱ diffractometer. HRMS were deter-mined by AB Triple TOF 5600^plus spectrometer. UV spectra were recorded on a TU-1901 spectrophoto-meter. Luminescence lifetime and quantum efficiency were measured by the Edinburgh (FLS-920) time-dependent single-photon counting fluorometer. Fluore-scence spectra was obtained at room temperature using a PerkinElmer LS-55 spectrophotometer. Cyclic voltammetry was recorded in dichloromethane on a Chenhua CHI60A electrochemical workstation with the tetra-n-butyl amine hexafluorophosphate (0.1 mol·L^-1) as the supporting electrolyte, ferrocene as the external standard, glassy carbon electrode as the working electrode, platinum plate as the counter electrode, and saturated silver/silver chloride as the reference electrode. OLEDs were prepared by evap-oration and film thickness was monitored by Inficon thickness measuring instrument with a resolution of 0.001 nm·s^-1. Electroluminescence spectra, CIE coor-dinates, J-V characteristic curves, brightness and other parameters were measured by Photo Research PR 670 photometer combining with Keithley 2400 dc power driver.

  1.2   Syntheses of iridium complexes

  Ir(tht)₃Cl₃ (tht=tetrahydrothiophene)^[5], 4, 5-diazo-9, 9-spirodifluorene (sb)^[17] and reference Ir complex Ir(tpit)(bpy)Cl (tpitH₂=triphenyl phosphite, bpy=2, 2′-bipyridine)^[6] were synthesized according to the literatures.

  Synthesis of Ir(tpit)(sb)Cl: sb (0.29 g, 0.92 mmol), Ir(tht)₃Cl₃ (0.52 g, 0.92 mmol), triphenyl phosphate (0.29 g, 0.92 mmol), sodium acetate (0.38 g, 4.6 mmol) and decalin (20 mL) were added in a 100 mL round-bottomed flask, and then the solution was heated for 12 h under nitrogen atmosphere. After the reaction was completed, the reaction mixture was cooled to room temperature, and then poured into the silica gel column. The decalin was eluted with petroleum ether, followed by elution with dichloro-methane/ethyl acetate (3:1, V/V) to obtain the yellow solid of the complex Ir(tpit)(sb)Cl, with a yield of 53% (0.42 g). The crystals for single crystal diffraction were prepared by recrystallization with dichloromethane and n-hexane mixed solution. ¹H NMR (400 MHz, CDCl₃): δ 8.30 (d, J=8 Hz, 2H), 7.94 (d, J=8.1 Hz, 1H), 7.87 (d, J=7.7 Hz, 1H), 7.67 (d, J=5.9 Hz, 2H), 7.55 (t, J=8 Hz, 1H), 7.45 (t, J=8 Hz, 1H), 7.26~7.17 (m, 4H), 7.14~7.02 (m, 7H), 6.96~6.85 (m, 8H). ³¹P NMR (162 MHz, CDCl₃): δ 113.35 (s, 1P). HRMS ((+)-ESI): m/z=819.139 0, Calcd. 819.138 9 for [C₄₁H₂₇IrN₂O₃P]([M-Cl]⁺). Elemental analysis Calcd. For C₄₁H₂₇IrN₂O₃PCl(%): C 57.64, H 3.19, N 3.28. Found(%): C 57.62, H 3.20, N 3.27.

  1.3   Structure determination

  In order to study the structure of the complex, the single-crystal structure was also tested from dichloromethane solution at room temperature. A light yellow crystal of compound Ir(tpit)(sb)Cl with approxi-mate dimension of 0.25 mm×0.23 mm×0.20 mm was selected, followed by mounted on a glass fiber. By using a Bruker SMART AEX Ⅱ diffractometer equipped with a graphite-monochromator with Mo Kα radiation (λ=0.071 073 nm), the intensity data were collected with ω scan mode at 150(2) K. Intensity data were obtained by empirical absorption. In the range of 2.243 < θ < 24.997 (-11 ≤ h ≤ 15, -19 ≤ k ≤ 19, -22 ≤ l ≤ 22), a total of 20 330 reflections were collected, of which 7 185 were independent (R_int=0.048 2) and 6 018 were observed with I > 2σ(I). Based on the multi-scan technique, the intensity data were corrected for empirical absorption as well as for polarization and Lorentz effects^[26]. The structure was solved by direct method, and was optimized by full-matrix least-squares methods on F² with SHELX-97^[27]. By using fixed isotropic thermal parameters and riding model position parameters, the hydrogen atoms were located theoretically and refined. SQUEEZE was used in structural refinement to eliminate disordered solvent. By using anisotropic displacement parameters, all non-H atoms were refined. The refinement parameters and the crystal data of complex are shown in Table 1.

  Table 1

  

  Table 1.  Crystal data, data collection and structure refinement parameters for complex Ir(tpit)(sb)Cl

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  Formula	C42H30Cl3IrN2O3P		θ range for data collection/(°)	2.243~24.997
  Formula weight	939.07		F(000)	1 684
  Crystal system	Orthorhombic		h, k, l	-11~15, -19~19, -22~22
  Space group	Pbca		Reflection measured	20 330
  a/nm	1.334 2(3)		Unique reflection	7 185
  b/nm	1.651 9(4)		Rint	0.048 2
  c/nm	1.874 6(5)		Parameter refined	443
  V/nm3	4.131 8(18)		R (F), wR (F2)* (all reflections)	0.064 9, 0.069 7
  Z	4		GOF (F2)	0.92
  Dc/(g·cm-3)	1.375		Largest diff. peak and hole/(e·nm-3)	756 and -521
  μ(Mo Kα)/cm-1	6.2
  * w=1/[σ2(Fo2)+(0.057 5P)2+31.626 1P], P=(Fo2+2Fc2)/3.

  CCDC: 1812631.

  2.   Results and discussion

  2.1   Synthesis and characterization

  The synthesis route of iridium complex Ir(tpit)(sb)Cl is shown in Scheme 1. The reaction was completed with one-pot method. The coordinated water in raw material IrCl₃·3H₂O was replaced by tetrahydrothio-phene leading to the increase of oil solubility, enabling the reaction to be carried out in the organic solvent. The coordination reaction was propitious due to the boiling point of decalin is as high as 187 ℃ and it didn′t contain active hydrogen disturbing coordination reaction. As an alkali, sodium acetate was able to promote the dehydrogenation process of bicyclic metallization. In combination with the above conditions, the yield of the target iridium complex was achieved to 53% by one-pot reaction. The number of hydrogen in the NMR spectrum of the product was consistent with the theoretical value. Only a single peak signal at δ 113.5 appeared in the phosphorus spectrum, indicating that only one phosphorus ligand participated in the coordination. The charge/mass ratio of the main peak of the HRMS was 819.139 0, which was consistent with the molecular weight (819.138 9) of the target product with dechlorination. All three points above show that the correct target product was obtained.

  Scheme 1

  

  Scheme 1.  Synthetic route of iridium complexes

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  It should be mentioned that the crystal was only used for the single-crystal structure testing, and dichloromethane-free compounds purified by chromatography on the silica gel column were used for the rest characterization.

  The structure of single-crystal is shown in Fig. 1. The figure shows a distorted octahedral configuration with the iridium atomic coordination center. The iridium atom coordinates with the phosphite ligand, a sb ligand and a chlorine atom. The phosphorus atom in the phosphite ester ligand and two benzene rings participate in the coordination in a facial configura-tion. Because of the molecular limitations of these two cyclometalated benzene rings, phosphorus atoms tilt toward them. The dipyridine in ligand sb is orthogonal to the two cyclometallated benzene rings, and the spirofluorene in ligand sb is orthogonal to dipyridine. Therefore, π-π accumulation of uncoordinated benzene rings in phosphite ester with dipyridine is impeded, which is different from the structure of the reference complex Ir(tpit)(bpy)Cl. It is obvious that Ir(tpit)(bpy)Cl contains intramolecular π-π accumula-tion, leading to significantly decrease of rotary vibration for uncoordinated benzene rings^{[6, 8]}. The chlorine in the para-position of phosphorus atom neutralizes the surplus positive charge of iridium atoms and lead to electric neutrality of iridium complex. The bond length of Ir-C is 0.204 7 and 0.205 5 nm, the bond length of Ir-N is 0.219 5 and 0.221 3 nm, the bond length of Ir-P is 0.213 4 nm, and the bond length of Ir-Cl is 0.244 6 nm. All these bond lengths are within the bond length range of similar complexes reported in the literature^{[6, 8-9]}.

  Figure 1

  

  Figure 1.  Perspective view of complex Ir(tpit)(sb)Cl with selected displacement ellipsoids drawn at 10% probability level

  H atoms and solvent molecules are omitted for clarity; Selected bond lengths (nm) and angles: Ir1-C30 0.204 7(8), Ir1-C29 0.205 5(8), Ir1-P1 0.213 4(2), Ir1-N1 0.219 5(6), Ir1-N2 0.221 3(6), Ir1-Cl1 0.244 6(3), C30-Ir1-C29 97.0(3)°, C30-Ir1-P1 80.5(3)°, C29-Ir1-P1 80.7(3)°, C30-Ir1-N1 172.2(3)°, C29-Ir1-N1 90.7(3)°, P1-Ir1-N1 101.85(18)°, C30-Ir1-N2 91.7(3)°, C29-Ir1-N2 171.0(3)°, P1-Ir1-N2 98.31(18)°, N1-Ir1-N2 80.7(2)°, C30-Ir1-Cl1 93.8(3)°, C29-Ir1-Cl1 94.2(3)°, P1-Ir1-Cl1 171.77(9)°, N1-Ir1-Cl1 84.58(17)°, N2-Ir1-Cl1 87.72(18)°

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  To evaluate the thermophysical properties of complexes, the thermogravimetry analysis (TGA) studies were performed (Fig. 2). All these complexes exhibited very good thermal stability. The 5% weight loss temperature (T_d) of complexes Ir(tpit)(bpy)Cl and Ir(tpit)(sb)Cl are 348 and 274 ℃, respectively. The higher T_d of Ir(tpit)(bpy)Cl may be attributed to the existence of intramolecular π-π accumulation. The good thermal stability is very advantageous for the preparation of evaporation OLED devices.

  Figure 2

  

  Figure 2.  Thermal gravimetric curves of as-prepared iridium(Ⅲ) complexes

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  2.2   UV-Vis absorption and photoluminescence properties

  The UV-Vis spectra of the iridium complexes in CH₂Cl₂ (10 μmol·L^-1) and the photoluminescence spectra in PMMA (1%) are shown in Fig. 3(a). It can be seen from the figure that the UV-Vis spectra are able to divided into two regions. The first region is the strong bands below 370 nm (ε > 4×10⁴ L·mol^-1·cm^-1), which is caused by the ligand-centered (LC) π-π^* transition. The second area at a lower energy region of more than 370 nm absorption bands (ε > 1.0×10⁴ L·mol^-1·cm^-1) can be attributed to metal-to-ligand charge transfer (MLCT) transitions. Compared with Ir(tpit)(bpy)Cl, the absorption band of Ir(tpit)(sb)Cl in the first area near 330 nm contains one more absorption peak obviously, which can be attributed to the π-π^* transition absorptions of fluorene groups in sb ligands.

  Figure 3

  

  Figure 3.  UV-Vis absorption, photoluminescence spectra (a, in CH₂Cl₂) and emission decay curves (b, in PMMA) of irdium(Ⅲ) complexes

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  As can be seen from the emission spectra of complexes (Fig. 3(a)), the maximum wavelengths of complexes Ir(tpit)(sb)Cl and Ir(tpit)(bpy)Cl are 512 and 520 nm, respectively, in the green region, and the two peaks show the same shape. The blue shift of emission wavelength for Ir(tpit)(sb)Cl is mainly due to the fact that the LUMO levels of such complexes mainly distribute in pyridine ligands^[6], and spiro-fluorene groups are electron-donating groups so that LUMO energy levels of materials are raised, which can broaden the energy gap and lead to blue shift of wavelengths. In order to reduce luminescence quen-ching of phosphorescent materials induced by oxygen, complexes were doped in PMMA film with 1% mass concentration. The luminescent life (Fig. 2(b) and Table 2) of Ir(tpit)(sb)Cl (1.12 μs) was shorter than that of Ir(tpit)(bpy)Cl (1.60 μs). And its quantum efficiency was 30%, which was far lower than that of Ir(tpit)(bpy)Cl (94%). Based on the above information, the calculated radiation decay rates of Ir(tpit)(sb)Cl and Ir(tpit)(bpy)Cl are 2.7×10⁵ and 5.9×10⁵ s^-1, respectively, and the non-radiation decay rates are 6.3×10⁵ and 3.8×10⁴ s^-1, respectively. It can be found that the radioactive decay rate of Ir(tpit)(bpy)Cl is more than twice as much as that of Ir(tpit)(sb)Cl, while the non-radioactive decay rate of Ir(tpit)(bpy)Cl lowers more than one order of magnitude, indicating that π-π stacking plays a major role in reducing the non-radioactive transition rate.

  Table 2

  

  Table 2.  Photophysical properties for the iridium complexes

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  Complex	λmaxa/nm	ηa/%	τa/μs	EHOMOb/eV	ELUMOc/eV	Eg, opt/eV
  Ir(tpit)(bpy)Cl	520	94	1.60	-5.72	-3.41	2.31
  Ir(tpit)(sb)Cl	512	30	1.12	-5.73	-3.39	2.34
  a Photoluminescence spectra, lifetime and quantum yields were recorded in PMMA at a mass concentration of 1%; b EHOMO=-4.8-E1/2, ox, oxidation potentials E1/2, ox/mV=(Epa+Epc)/2, where Epa and Epc are the anodic and cathodic peak potentials referenced to the Fc+/Fc couple in CH2Cl2; c LUMO levels ELUMO=EHOMO+Eg, opt, where Eg, opt was estimated from the absorption edge.

  2.3   Electrochemical properties

  The electrochemical properties of iridium complexes were tested by cyclic voltammetry (Fig. 4). The oxidation potential of Ir(tpit)(bpy)Cl was 915 mV (vs Fc⁺/Fc). The oxidation potential of Ir(tpit)(sb)Cl was 928 mV, higher than that of Ir(tpit)(bpy)Cl. Thus, the frontier orbital energy levels of complexes were calculated (Table 2). The HOMO energy levels of Ir(tpit)(bpy)Cl and Ir(tpit)(sb)Cl were -5.72 and -5.73 eV, respectively, indicating that instead of ppy, sb ligand can stabilize the HOMO level of complex. According to the ultraviolet absorption edge, the energy gaps of Ir(tpit)(bpy)Cl and Ir(tpit)(sb)Cl were 2.31 and 2.34 eV, respectively, showing an increasing trend, which is consistent with blue shift of luminescence wavelength. The LUMO levels of Ir(tpit)(bpy)Cl and Ir(tpit)(sb)Cl were -3.41 and -3.39 eV, respectively. The higher LUMO level of Ir(tpit)(sb)Cl is caused by the spirofluorene groups which can increase the LUMO level of the complex, proving the blue shift of the luminescence wavelength.

  Figure 4

  

  Figure 4.  Cyclic voltammetry curves of as-prepared iridium complexes in CH₂Cl₂

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  2.4   Electrophosphorescent properties

  The electroluminescent devices doped with these iridium complexes were prepared by evaporation method to evaluate their practical application value. The device structure is ITO/TAPC (10 nm)/TCTA (35 nm)/mCP: complex (20 nm)/TmPyPB (50 nm)/Liq (1 nm)/Al (120 nm). Schematic diagram of device structure and energy levels of compounds are shown in Fig. 5. Di-(4-(N, N-ditolyl-amino)-phenyl) cyclohexane (TAPC) acts as hole injection and hole transport material, and N, N, N-tris(4-(9-carbazolyl)phenyl)amine (TCTA) and 1, 3, 5-tri((3-pyridyl)-phen-3-yl)benzene (TmPyPB) are electron blocking material and electron transport material, respectively. 8-Hydroxyquinolinola (Liq) and aluminum (Al) are used as electron injection transport material and cathode, respectively. The emitting layer is a blend of 1, 3-bis(N-carbazolyl)benzene (mCP) as the host material and Ir complexes as the dopant with 5%(w/w) of Ir(tpit)(bpy)Cl and 8%(w/w) of (Ir(tpit)(sb)Cl, respectively.

  Figure 5

  

  Figure 5.  Structural drawing of the materials (a) and energy level diagrams of OLEDs (b)

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  The electroluminescent characteristics and asso-ciated data of devices are shown in Fig. 6 and Table 3. As shown in Fig. 6(a), the maximum wavelengths of Ir(tpit)(bpy)Cl (device A) and Ir(tpit)(sb)Cl (device B) were at 532 and 520 nm, respectively. Compared with the spectra of complexes in PMMA, these spectra showed red shift by 12 nm and 8 nm, which is caused by the aggregation effect induced by increase of the concentration of complexes. The space steric hind-rance of spirobifluorene can reduce intermolecular aggregation, leading to smaller red shift of Ir(tpit)(sb)Cl. There was no additional peak of the host material in the spectrum, indicating that the energy of it is transmitted to the guests effectively. The turn on voltage of device A was about 3.6 V (Fig. 6(b)), the luminance increases with the voltage and a maximum luminance of 9 641 cd·m^-2 at 11 V was achieved. In addition, the efficiencies of devices A and B are revealed in Fig. 6(c, d). A maximum current efficiency of 60 cd·A^-1 and external quantum efficiency of 18.2% were successfully achieved for device A together with CIE of (0.34, 0.57). Device B required a higher turn on voltage of 4.5 V with the maximum brightness of 3 531 cd·m^-2, a maximum current efficiency of 14 cd·A^-1 and external quantum efficiency of 4.6% along with the CIE coordinate of (0.30, 0.55). And the external quantum efficiencies of devices are consistent with that of photoluminescence. The efficiency of device B was about 25% of that of device A, which is mainly caused by the low photoluminescence quantum efficiency resulting from the flexible groups in Ir(tpit)(sb)Cl and lack of intramolecular π-π accumulation.

  Figure 6

  

  Figure 6.  Electroluminescent characteristics and associated data of devices A and B: (a) EL spectra of all devices; (b) Current density-voltage-luminance (J-V-L) characteristics; (c) Luminance efficiencies vs luminance curves; (d) External quantum efficiency vs luminance curves

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  Table 3

  

  Table 3.  Summary of device luminescence and efficiency data

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  Device (Dopant)	λEL, max/nm	Turn-on votage/V	Brightness/(cd·m-2)	Current efficiency/(cd·A-1)	EQE/%	CIE coordinates (x, y)
  A(Ir(tpit)(bpy)Cl)	532	3.6	9 641	60	18.2	0.34, 0.57
  B(Ir(tpit)(sb)Cl)	520	4.5	3 531	14	4.6	0.30, 0.55

  3.   Conclusions

  In this paper, a new iridium complex Ir(tpit)(sb)Cl (tpitH₂=triphenyl phosphite) was synthesized by steric ligand 4, 5-diaza-9, 9-spirobifluorene(sb), and it was compared with the similar complex Ir(tpit)(bpy)Cl (bpy=2, 2′-bipyridine). Crystal structure analysis shows that the spirofluorene groups destroyed the intramole-cular π-π accumulation of the complex, leading to blue shift of spectra and decrease of luminescent efficiencies. As for the electroluminescent devices, the maximum current efficiency and external quantum efficiency of complex Ir(tpit)(bpy)Cl were 60 cd·A^-1 and 18.2%, respectively, while the complex Ir(tpit)(sb)Cl achieved lower efficiencies (maximum current efficiency of 14 cd·A^-1 and maximum external quantum efficiency of 4.6%). It means that the intramolecular π-π accumulation plays an important role in reducing the luminescence quenching of the flexible groups. Based on this phenomenon, it is expected to design luminescent materials of iridium complexes with high luminescence performance and aggregation-induced luminescent activity.

  
  Acknowledgements: The authors acknowledge financial support from the National Natural Science Foundation of China (Grant No.21572001).
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  Scheme 1  Synthetic route of iridium complexes

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  Figure 1  Perspective view of complex Ir(tpit)(sb)Cl with selected displacement ellipsoids drawn at 10% probability level

  H atoms and solvent molecules are omitted for clarity; Selected bond lengths (nm) and angles: Ir1-C30 0.204 7(8), Ir1-C29 0.205 5(8), Ir1-P1 0.213 4(2), Ir1-N1 0.219 5(6), Ir1-N2 0.221 3(6), Ir1-Cl1 0.244 6(3), C30-Ir1-C29 97.0(3)°, C30-Ir1-P1 80.5(3)°, C29-Ir1-P1 80.7(3)°, C30-Ir1-N1 172.2(3)°, C29-Ir1-N1 90.7(3)°, P1-Ir1-N1 101.85(18)°, C30-Ir1-N2 91.7(3)°, C29-Ir1-N2 171.0(3)°, P1-Ir1-N2 98.31(18)°, N1-Ir1-N2 80.7(2)°, C30-Ir1-Cl1 93.8(3)°, C29-Ir1-Cl1 94.2(3)°, P1-Ir1-Cl1 171.77(9)°, N1-Ir1-Cl1 84.58(17)°, N2-Ir1-Cl1 87.72(18)°

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  Figure 2  Thermal gravimetric curves of as-prepared iridium(Ⅲ) complexes

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  Figure 3  UV-Vis absorption, photoluminescence spectra (a, in CH₂Cl₂) and emission decay curves (b, in PMMA) of irdium(Ⅲ) complexes

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  Figure 4  Cyclic voltammetry curves of as-prepared iridium complexes in CH₂Cl₂

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  Figure 5  Structural drawing of the materials (a) and energy level diagrams of OLEDs (b)

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  Figure 6  Electroluminescent characteristics and associated data of devices A and B: (a) EL spectra of all devices; (b) Current density-voltage-luminance (J-V-L) characteristics; (c) Luminance efficiencies vs luminance curves; (d) External quantum efficiency vs luminance curves

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  Table 1.  Crystal data, data collection and structure refinement parameters for complex Ir(tpit)(sb)Cl

  Formula	C42H30Cl3IrN2O3P		θ range for data collection/(°)	2.243~24.997
  Formula weight	939.07		F(000)	1 684
  Crystal system	Orthorhombic		h, k, l	-11~15, -19~19, -22~22
  Space group	Pbca		Reflection measured	20 330
  a/nm	1.334 2(3)		Unique reflection	7 185
  b/nm	1.651 9(4)		Rint	0.048 2
  c/nm	1.874 6(5)		Parameter refined	443
  V/nm3	4.131 8(18)		R (F), wR (F2)* (all reflections)	0.064 9, 0.069 7
  Z	4		GOF (F2)	0.92
  Dc/(g·cm-3)	1.375		Largest diff. peak and hole/(e·nm-3)	756 and -521
  μ(Mo Kα)/cm-1	6.2
  * w=1/[σ2(Fo2)+(0.057 5P)2+31.626 1P], P=(Fo2+2Fc2)/3.

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  Table 2.  Photophysical properties for the iridium complexes

  Complex	λmaxa/nm	ηa/%	τa/μs	EHOMOb/eV	ELUMOc/eV	Eg, opt/eV
  Ir(tpit)(bpy)Cl	520	94	1.60	-5.72	-3.41	2.31
  Ir(tpit)(sb)Cl	512	30	1.12	-5.73	-3.39	2.34
  a Photoluminescence spectra, lifetime and quantum yields were recorded in PMMA at a mass concentration of 1%; b EHOMO=-4.8-E1/2, ox, oxidation potentials E1/2, ox/mV=(Epa+Epc)/2, where Epa and Epc are the anodic and cathodic peak potentials referenced to the Fc+/Fc couple in CH2Cl2; c LUMO levels ELUMO=EHOMO+Eg, opt, where Eg, opt was estimated from the absorption edge.

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  Table 3.  Summary of device luminescence and efficiency data

  Device (Dopant)	λEL, max/nm	Turn-on votage/V	Brightness/(cd·m-2)	Current efficiency/(cd·A-1)	EQE/%	CIE coordinates (x, y)
  A(Ir(tpit)(bpy)Cl)	532	3.6	9 641	60	18.2	0.34, 0.57
  B(Ir(tpit)(sb)Cl)	520	4.5	3 531	14	4.6	0.30, 0.55

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