Transition metal nitrido (M≡N) complexes are key intermediates in N2 fixation; they are also potentially useful reagents for the nitrogenation of various organic substrates1,2,3. Although a variety of transition metal nitrido complexes are known, few have oxidizing ability that are comparable to metal-oxo species, such as FeIV(O)P+• in cytochrome P450 enzymes4,5. Pioneering work by Meyer and Huynh6 has shown that [OsVI(terpy)(N)Cl2]+ (terpy=2,2′:6′,2″-terpyridine) and related complexes are highly electrophilic/oxidizing; they react with a variety of organic substrates resulting in the formation of novel osmium complexes in lower oxidation states. However, these complexes do not undergo C–H bond activation, especially for substrates with unactivated C–H bonds, such as alkanes. Previous studies have demonstrated that the ruthenium(VI) nitrido complexes bearing salen-type ligands are highly electrophilic7; in particular, the complex [Ru(N)(salchda)(MeOH)]+ (salchda=N,N′-bis(salicylidene)-o-cyclohexyldiamine dianion) is the only well-defined nitrido complex that is able to activate the C–H bonds of alkanes in the presence of pyridine8. A number of azido complexes, including Ru2(D(3,5-Cl2)PhF)4N3 (D(3,5-Cl2)PhF=N,N’-bis(3,5-dichlorophenyl) formamidinate)9,10, (iPrBPDI)CoN3 (iPrBPDI=2,6-(2,6-iPr2-C6H3=CPh)2C5H3N)11, [(3PDI2)Co2(μ-N3)(PMe3)2][OTf]3 (PDI=2,6-pyridyldiimine)12, Ni(Et3P)2(N3)213 and (C5Me5)2U[N(SiMe3)2](N3)14 can also undergo inter- or intramolecular C–H bond activation of alkanes and arenes via in situ generation of putative nitrido intermediates by thermolysis or photolysis.

Apart from the above systems, the use of solar energy to generate highly reactive nitrido complex in the excited state for the nitrogenation of organic substrates is an appealing approach. A number of d2 nitrido complexes, such as those of ReV and OsVI, have long-lived emissive excited states15,16,17,18,19,20,21; the emissions of these complexes were shown to originate mainly from metal-centered ligand field 3[(dxy)1(dπ*)1] excited states. Although some of these complexes are strong one-electron oxidants in their excited states, nitrogen atom transfer reactions of these complexes, especially towards inert organic substrates, have not been demonstrated.

Recently, we reported the synthesis of an osmium(VI) nitrido complex [OsVI(N)(L)(CN)3] (OsN, HL=2-(2-hydroxyphenyl)benzoxazole) via the oxidation of an osmium(III) guanidine precursor [Os(L){N(H)C(NH2)2}(CN)3] (OsG)22,23,24. In this work, we have synthesized a nitro derivative of OsN [OsVI(N)(NO2-L)(CN)3] (NO2-OsN, NO2-HL = 2-(2-hydroxy-4-nitrophenyl)benzoxazole via a similar procedure. The photophysical and photochemical properties of the two complexes have been investigated. OsN is very weakly emissive in both the solid state and fluid solution. In contrast, NO2-OsN is highly luminescent in both solid state and fluid solutions. More importantly, to the best of our knowledge, under visible-light excitation NO2-OsN becomes the most oxidizing/electrophilic nitrido species reported. It readily undergoes aliphatic C–H bond activation of hydrocarbons and ring-nitrogenation of arenes.


Synthesis and characterization of NO2-OsN

The synthesis of NO2-OsN is summarized in Fig. 1.

Fig. 1
figure 1

Synthetic route for NO2-OsN. The synthesis of NO2-OsG is similar to the previous reported method for OsG and iodosobenzene (PhIO) is used as the oxidant

NO2-OsN was isolated as light yellow PPh4+ salt in 35% yield. Consistent with its (dxy)2 ground state electronic configuration, this compound is diamagnetic (μeff ~0 μB), as evidenced by the sharp resonances in the normal range in the 1H nuclear magnetic resonance (NMR) spectrum (Supplementary Fig. 1). The electrospray ionization/mass spectrometry (ESI/MS) of NO2-OsN in MeOH (−ve mode) shows the parent anion [M] at m/z 539, which is shifted to m/z 540 in the 15N-labeled complex NO2-Os15N (Supplementary Fig. 2). In the infrared (IR) spectrum, the v(Os≡N) stretch is found at 1074 cm−1, which is shifted to 1046 cm−1 upon 15N labeling.

The molecular structure of NO2-OsN has been determined by X-ray crystallography (Fig. 2a, Supplementary Table 1 and Supplementary Data 1). Similar to OsN, the three cyano ligands are in meridional configuration and the nitride is trans to the phenoxy oxygen. The Os-N (nitrido) bond lengths of both complexes are similar (1.655(3) Å for NO2-OsN; 1.653(2) Å for OsN) and are within the range for Os≡N25.

Fig. 2
figure 2

Crystal characterization. The ORTEP (Oak Ridge Thermal Ellipsoid Plot) drawing of the anionic structures of NO2-OsN (a), 1 (b), 2 (c), 3 (d), 4 (e), 5 (f), 7b (g) and 8 (h)

Photophysical properties of OsN and NO2-OsN

The two Os(VI) nitrido complexes show intense ligand-centered ππ* transitions of the bidentate O^N ligand (L/NO2-L) at 230–310 nm with molar extinction coefficients (ε) of the order of 104 dm3 mol−1 cm−1 (Fig. 3a). For OsN, there is a moderately intense broad absorption band at 357 nm with molar absorptivity (ɛ) ~1.2 × 104 dm3 mol−1 cm−1 and a shoulder at 378 nm tailing down to about 500 nm. In NO2-OsN, the corresponding absorption band is more intense (~3.2 × 104 dm3 mol−1 cm−1) and is slightly blue-shifted with λmax at 365 nm. The lowest-energy absorption band in the two complexes is tentatively assigned to O^N ligand to Os≡N charge transfer (LML′CT) transitions, probably mixed with metal-centered dd transitions [(dxy)2→(dxy)l(dπ*)1].

Fig. 3
figure 3

Spectroscopic characterizations for OsN and NO2-OsN. a Ultraviolet/visible (UV/Vis) spectra of OsN and NO2-OsN in CH2Cl2 solution. b Emission spectra of OsN and NO2-OsN in CH2Cl2 solution and in solid state at 298 K (λex = 355 nm). c Normal Raman (λex = 785 nm) and resonance Raman spectra (λex = 355 nm) of NO2-OsN in acetonitrile solution

The LML′CT assignment is further supported by resonance Raman (RR) spectroscopic study of NO2-OsN (Fig. 3c), which shows enhancements of Raman signals corresponding to the Os≡N stretching mode (assigned based on the normal Raman spectra of the unlabeled and 15N-labeled complexes) and C=C, C=N, NO2 stretches of the bidentate N^O ligand upon 355 nm excitation. This is indicative of the involvement of both the bidentate N^O ligand and Os≡N in the electronic transition of the lowest-energy absorption band and is consistent with LML′CT [π(N^O)→*(Os≡N)] character. This is further supported by the results of the density functional theory (DFT)/time-dependent DFT (TDDFT) calculations.

DFT/TDDFT calculations have been performed on the osmium nitrido complexes. The frontier molecular orbital (MO) diagrams of OsN and NO2-OsN are shown in Supplementary Figs. 34 and Fig. 4, respectively, and the Cartesian coordinates for optimized geometries have been summarized in Supplementary Tables 23. The highest occupied molecular orbital (HOMO) of both complexes are predominantly localized on the bidentate O^N ligand. The closely lying lowest unoccupied molecular orbital (LUMO) and LUMO+1 are comprised of the antibonding orbitals of Os(dyz)≡N3−(py) (π*yz) and Os(dxz)≡N3−(px)(π*xz), respectively. A brief summary of the 10 lowest vertical transitions is shown in Supplementary Table 4; the corresponding simulated ultraviolet (UV) spectra (Supplementary Fig. 5) computed by TDDFT calculations are in good agreement with the experimental absorption spectra of these complexes. The S1/S2 states for the two complexes are predominantly derived from the HOMO→LUMO/LUMO+1 transitions and therefore can be considered as LML′CT states. For S3/S4 states, they are derived from HOMO−1 [dxy(Os)]→LUMO/LUMO+1, which can be considered as metal-centered ligand field dd states. By introducing the strong electron-withdrawing −NO2 group, the energy level of the S1–S4 states are increased. Such trend is consistent with the absorption data. Since both the geometry optimizations and TDDFT calculations were performed in the gas phase, we have also simulated the absorption of OsN using the linear response polarizable continuum model with dichloromethane matrix to examine the effect of the solvent. As shown in Supplementary Fig. 6, the simulated spectra did not show obvious improvement.

Fig. 4
figure 4

Density functional theory (DFT)/time-dependent DFT (TDDFT) calculations for NO2-OsN. Frontier molecular orbitals (MOs) of NO2-OsN at the optimized S0 geometries

Despite close resemblance of these two complexes, they exhibit very different emission properties (Fig. 3b). In the solid state, OsN exhibits a weak orange emission at 611 nm (Φ < 0.1%, τ = 0.14 μs), while NO2-OsN exhibits a much stronger and longer-lived emission at 591 nm (Φ = 11.7%, τ = 1.90 μs). With sub-microsecond lifetimes, these emissions are attributed to phosphorescence derived from LML′CT excited state. The blue-shifted emission observed in NO2-OsN is in agreement with its LML′CT character, due to the stabilization of the π orbitals of NO2-L by the strong electron-withdrawing and π-conjugating NO2 group. In CH2Cl2 solution, OsN shows a very weak emission at 620 nm (Φ< 0.001%), while NO2-OsN also displays a much strong emission at 594 nm (Φ = 3.0%, τ = 0.48 μs). The enhanced phosphorescence properties of NO2-OsN over that of OsN is possibly due to the strong electron-withdrawing effect of the –NO2 group that could effectively stabilize the dπ(Os) orbitals and raise the energy of the ligand field excited state. In 77 K EtOH-MeOH (4:1, v/v) glassy medium, the emissions of OsN and NO2-OsN remain structureless with maxima at 594 nm (τ = 1.38 μs) and 577 nm (τ = 5.90 μs), respectively (Supplementary Fig. 7 and Table 5), which are blue-shifted relative to those in CH2Cl2 solution. This is due to the rigidochromic effect in the low-temperature glassy medium, typically observed in phosphorescence of a charge transfer state.

Nanosecond transient absorption spectroscopy was carried out to provide insights into their emissive excited states. As shown in Supplementary Fig. 8, OsN exhibits no absorption features after 355 nm nanosecond laser excitation, while NO2-OsN shows two absorption features at ca. 300–340 nm and 400–550 nm, with strong ground state bleaching at 340–400 nm in the transient absorption difference spectra. The observation of transient absorption feature in the visible region for NO2-OsN is suggestive of the radical character involving the conjugated ligands in its emissive excited state, which is supportive of the LML′CT excited state origin.

Cyclic voltammetry of OsN and NO2-OsN

The redox properties of these two complexes were studied by cyclic voltammetry (CV). The CV of OsN shows an irreversible oxidation wave at Epa = 1.44 V and an irreversible reduction wave at Epa = −1.17 V vs. Saturated Calomel Electrode (SCE), which are tentatively assigned as the metal-centered OsVII/VI and OsVI/V process, respectively (Supplementary Fig. 9). Similar irreversible oxidation and reduction waves are also found for NO2-OsN at Epa = 1.88 V and −0.99 V, respectively. From the estimated E00 emission (OsN 2.05 eV, NO2-OsN 2.15 eV) and electrochemical data (Epc: OsN −0.93 V, NO2-OsN −0.75 V vs. Normal Hydrogen Electrode (NHE)), the excited state redox potentials are estimated to be 1.13 and 1.40 V for OsN and NO2-OsN, respectively (Supplementary Note 1)15. In order to support these assignments, further calculations have been conducted regarding the redox properties of the OsN and NO2-OsN. As shown in Supplementary Table 6, the DFT-calculated redox potentials match quite well with the experimentally determined values. The spin density calculations (Supplementary Fig. 10) on the redox species reveal that the reduction of the complexes is Os≡N based and leads to a weakened triple bond (1.65 Å → 1.75 Å), whereas one-electron oxidation largely retains the Os≡N bond with the generation of ligand-centered radical.

Photostabilty of NO2-OsN and OsN

Highly electrophilic nitrido complexes readily undergo coupling of the nitrido ligands to generate N27,8. However, both NO2-OsN and OsN are stable upon irradiation with blue light (λ > 460 nm) for 24 h at room temperature in CH2Cl2 solution, as monitored by their absorption and luminescence spectra. This indicates that the excited states of these complexes are stable with respect to nitrido coupling or other decomposition reactions.

C-H bond activation by the excited state of NO2-OsN (NO2-OsN*)

In accordance with the LML′CT character of its emission, NO2-OsN* should possess [Os=N] nitridyl character26,27, which would make it highly electrophilic.

NO2-OsN* is found to be a powerful electrophile/oxidant; it reacts readily with hydrocarbons with a wide range of C–H bond dissociation energies (BDE). The hydrocarbons investigated include xanthene (XAN, BDE = 75.5 kcal mol−1), 1,10-dihydroanthracene (DHA, 78.0 kcal mol−1), ethylbenzene (EB, 85.4 kcal mol−1), cyclooctane (c-OCT, 93.6 kcal mol−1) and cyclohexane (c-HEX, 95.4 kcal mol−1)28,29,30,31,32. Upon irradiation of a solution of NO2-OsN (5 × 10−5 M) in CH2Cl2 solution containing excess hydrocarbon (5 × 10−2 M) at 23 °C with blue light-emitting diode (LED) light (λ > 460 nm), the color of the solution gradually changed from light yellow to brown. The progress of the photochemical reaction was monitored by ultraviolet/visible (UV/Vis) spectrophotometry (vide infra). The rate of the photoreaction decreases with increasing BDE of the substrates, i.e., XAN>DHA>EB»c-OCT>c-HEX. No spectral changes were observed in the absence of light. In contrast, OsN remains unreactive under similar conditions, in accordance with its much shorter lifetime and lower emission quantum yield in solution.

Silica chromatography of the product solutions afforded two osmium products in each case, an osmium(IV) iminato and an osmium(III) ammine complex, as illustrated in Fig. 5.

Fig. 5
figure 5

Reaction of NO2-OsN with various hydrocarbons. Upon visible-light irradiation of NO2-OsN with hydrocarbons, the osmium(III) ammine complex 1 and osmium(IV) iminato complexes 2–6 are formed

Molecular structures

The molecular structure of the osmium(III) ammine complex [PPh4]1 was determined by X-ray crystallography (Fig. 2b and Supplementary Table 1). The distorted octahedral arrangement of the parent nitrido complex is retained in the ammine product; the three cyano ligands are in mer-configuration. The Os-N(NH3) (Os1-N5) bond length is 2.110(3) Å, typical of a Os-N single bond.

The molecular structures of the osmium(IV) iminato complexes 2, 3, 4 and 5 have also been determined by X-ray crystallography. As shown in Fig. 2c–f, the distorted octahedral arrangement of the ligands around the Os center in the parent NO2-OsN is also retained in these complexes. These complexes all feature a newly formed anionic iminato ligand; the Os-Niminato (Os-N5) bond distances are similar (1.758(11)–1.824(7) Å) and indicative of double bond character. The Os1-N5-C10 bond angles are also similar and close to linear, with an average value of ~174°. The C5-N10 iminato bonds are in a narrow range of 1.246(12)–1.278(4) Å, typical of a C=N double bond.

1 has a room temperature magnetic moment of μeff = 1.95 μB (Guoy method), consistent with the low-spin d5 configuration of osmium(III). Complexes 2–5 are diamagnetic, as evidenced by the sharp resonances in the normal range in the 1H NMR spectrum (Supplementary Figs. 1112), consistent with the low-spin d4 electronic configuration of the Os(IV) complexes. 15 were also characterized by IR spectroscopy, UV/Vis spectroscopy, ESI/MS and electrochemistry (Supplementary Figs. 1318).

ESI/MS of photochemical reactions

The progress of the photochemical reactions was followed by ESI/MS. The ESI/MS of NO2-OsN in CH2Cl2 (−ve mode) shows a predominant parent peak at m/z 539. The ESI/MS for the photochemical reaction mixture of NO2-OsN with DHA (Fig. 6) shows the appearance of a peak at m/z 719, which is assigned to the amido species [NO2-Os-(NH-DHA(H))] (see Fig. 9a). This peak is gradually shifted to m/z 717, which is consistent with the iminato species 2, [NO2-Os-(N = DHA(2H))]. These results suggest that the initially formed amido species undergoes oxidative dehydrogenation to give an iminato complex. After 12 h, the peak at m/z 717 becomes predominant, while the peak at m/z 539 is further decreased and the isotopic distribution shows that it is a mixture of parent (m/z 539) and the ammine complex 1 (m/z 542). Similar observations were also found for xanthene, ethylbenzene and cyclooctane (Supplementary Figs. 1920).

Fig. 6
figure 6

Electrospray ionization/mass spectrometry (ESI/MS) collected at various irradiation time intervals. a NO2-OsN (0.3 mM) and DHA (0.3 M) in CH2Cl2 is irradiated by visible light for 1 h, b for 3 h, and c for 12 h. Insets in (a, c) show the isotopic distribution patterns of the peaks centered at m/z 719 and 717

UV/Vis absorption and emission spectroscopy of photochemical reactions

The photochemical reactions of NO2-OsN with excess XAN, DHA and EB were also monitored by UV/Vis spectroscopy (Fig. 7). In the case of DHA, the absorbance at 374 nm due to NO2-OsN decreases with time, while the absorbance from around 410–600 nm increases with time, consistent with the formation of NO2-Os=(DHA(−2H)) and NO2-OsNH3 with λmax at 444 nm and 459, 551 nm, respectively. Similar UV/Vis spectral changes were observed for the photoreaction of NO2-OsN with XAN or EB (Supplementary Fig. 21).

Fig. 7
figure 7

Spectroscopic traces of NO2-OsN with various substrates. a Ultraviolet/visible (UV/Vis) spectral changes for the reaction of NO2-OsN with excess DHA in CH2Cl2 upon irradiation by blue light-emitting diode (LED). b UV/Vis spectral changes for the visible-light irradiation of NO2-OsN and cyclooctane in CH2Cl2 under Ar. c Emission intensity changes of NO2-OsN and cyclooctane in similar conditions

The emission spectrum of NO2-OsN is greatly interfered by the emission of the aromatic substrates. On the other hand, the photochemical reaction of NO2-OsN with cyclooctane in CH2Cl2 could be followed by both UV/Vis absorption and emission spectroscopy. As shown in Fig. 7b, c, there is a much larger change in emission intensity than in absorbance of the reaction mixture.

Kinetic isotope effects

The kinetic isotope effects (KIE) for the photochemical reaction of NO2-OsN with hydrocarbons were determined by ESI/MS. KIE was found to be ~4.1 from competition experiments using an equimolar mixture of cyclohexane (c-C6H12) and d12-cyclohexane (c-C6D12) as substrate (Fig. 8). The KIE was estimated from the ratios of the most intense peaks for the two osmium(IV) iminato products, assuming that the spraying and ionization efficiencies of the two ions are similar. Similarly, the KIE for ethylbenzene was found to be ~7.7 using an equimolar mixture of ethylbenzene (C6H5CH2CH3) and d10-ethylbenzene (C6D5CD2CD3) as substrate. These large KIE values indicate that C–H bond cleavage occurs in the rate-determining step.

Fig. 8
figure 8

Kinetic isotope effect (KIE) determination. a Electrospray ionization/ mass spectrometry (ESI/MS) showing the KIE effects of cyclohexane. b ESI/MS showing the KIE effects of ethylbenzene (red and blue codes are for the product of NO2-OsN with deuterated and normal substrates, respectively)

Photochemical reaction mechanism

Based on all the experimental results, a mechanism for C–H bond activation by NO2-OsN* is proposed, using DHA as an example (Fig. 9a). NO2-OsN* first abstracts a H-atom from DHA; this is followed by a N-rebound process to give an OsIV amido species. These processes are reminiscent of C–H bond activation by metal-oxo species33,34,35. The OsIV amido species undergoes further H-atom abstractions by NO2-OsN* to generate the OsIV iminato product 3; this is accompanied by the formation of NO2-OsNH3 (1). For substrates with weak C–H bonds, such as XAN and DHA, the amido species should be formed more rapidly than its subsequent dehydrogenation, and hence both the amido and the iminato species can be observed by ESI/MS. On the other hand, for ethylbenzene, cyclooctane and cyclohexane, which have stronger C–H bonds, the amido species should be formed much more slowly, hence only the iminato species can be observed.

Fig. 9
figure 9

Proposed reaction mechanisms. a The proposed reaction mechanism for NO2-OsN* with DHA. b The proposed mechanism for the reaction of NO2-OsN* with anthracene

Photochemical reaction of NO2-OsN with arenes

NO2-OsN* also readily reacts with anthracene (ANTH). ESI/MS of the product solution upon irradiation for 10 h shows two prodominant peaks at m/z 717 or 731, which are assigned to the osmium(IV) amido species [OsIV(NO2-L)(CN)3(NH-ANTH(H))] (7a) and the osmium(IV) p-benzoquinone iminato species [OsIV(NO2-L)(CN)3(N=ANTH(2H)=O)] (7b), respectively (Fig. 10).

Fig. 10
figure 10

The reaction pathways of NO2-OsN* with arenes. Photochemical reaction of NO2-OsN with anthracene affords 7a and 7b, while its reaction with benzene affords 8

Both (PPh4)[OsIV(NO2-L)(CN)3(NH-ANTH(H))] ([PPh4]7a) and (PPh4)[OsIV(NO2-L)(N=ANTH(2H)=O)(CN)3] ([PPh4]7b) could be isolated in moderate yields. They are characterized by 1H NMR, IR, ESI/MS, CV and elemental analysis (Supplementary Figs. 2225).

The molecular structure of (PPh4)[OsIV(NO2-L)(CN)3(N=ANTH(2H)=O)] ([PPh4]7b) has been determined by X-ray crystallography (Fig. 2g). The osmium center is 6-coordinated by three CN ligands, a bidentate O^N ligand and a newly formed iminato ligand in a distorted octahedron. The Os-N5 bond length is 1.793(2) Å. The C=N and C=O bond lengths in the newly formed iminato ligand are 1.284(4) and 1.221(4) Å, respectively.

In order to confirm the origin of O atom in resulting complexes, the photochemical reaction of NO2-OsN with anthracene was carried out in the presence of 97% H218O. ESI/MS of the reaction mixture shows that the peak at m/z 731 increases by two mass units to m/z 733 in the presence of H218O, while the peak at m/z 717 remains unchanged (Supplementary Fig. 26). Moreover, no exchange was found between [OsIV(NO2-L)(CN)3(N=Anth(2H)=16O)] with H218O in CH3CN for over 48 h. These results indicate that O atom in 7b originates from trace H2O in the reaction system.

In the photochemical reaction of NO2-OsN with anthracene, competition experiments using an equimolar mixture of anthracene and d10-anthracene as substrates were also conducted. A KIE value of around 1.3 (Supplementary Fig. 27) was obtained by ESI/MS; such a small value suggests that the aromatic C–H bond activation does not undergo a HAT/N-rebound process as in aliphatic C–H bond activation. A proposed mechanism is shown in Fig. 9b. NO2-OsN* first undergoes electrophilic attack at the arene to generate immediate I, which then undergoes proton shift to give the amido complex [OsIV(NO2-L)(CN)3(NH-ANTH(H))] (7a). 7a then undergoes nucleophilic attack by a water molecule followed by deprotonation to generate intermediate II, which is then oxidized by NO2-OsN* to generate the final p-benzoquinone iminato product [OsIV(NO2-L)(CN)3(N=ANTH(2H)=O)] (7b).

The excited state of NO2-OsN is also able to nitrogenate benzene, although the photoreaction is around 10 times slower than that with anthracene. ESI/MS (−ve mode) of a solution of NO2-OsN and excess benzene (after irradiation for 2 weeks) shows a predominant product peak at m/z 631, which is assigned to the species [OsIV(NO2-L)(CN)3(NC6H4O)] (8). In contrast to the anthracene reaction, the intermediate osmium amido species, [OsIV(NO2-L)(CN)3(NH-Ph)], was not observed; presumably the formation of this species is much slower than its subsequent oxidation. The complex [OsIV(NO2-L)(CN)3(NC6H4O] (8) could be isolated as PPh4+ salt with about 13% yield. It is characterized by 1H NMR, IR, CV and elemental analysis (Supplementary Figs. 2829). The X-ray crystal structure of [PPh4]8 shows Os-N5 bond distance of 1.758(11) Å (Fig. 2h). The C=N and C=O bond lengths in the newly formed ligand are 1.306(18) and 1.231(19) Å, respectively.


We have designed a highly luminescent osmium(VI) nitrido complex (NO2-OsN) with long-lived excited state. Experimental results and DFT calculations indicate that the emissive excited state of this complex exhibits LML′CT [π(N^O)→dπ*(Os≡N)] character, which is different from reported luminescent osmium nitrido complexes with predominant dd transition character. In accordance with the LML′CT character of its emission, NO2-OsN* possess [Os=N] nitridyl character, which to our knowledge is the most oxidizing/electrophilic nitrido species reported to date. NO2-OsN* readily undergoes C–H bond activation with alkanes and nitrogenation of arenes, including benzene. In the reaction with alkanes and alkylaromatics, the proposed mechanism involves initial H-atom abstraction from the organic substrate by NO2-OsN*, followed by a N-rebound process; which is reminiscent of C–H bond activation by metal-oxo species. On the other hand, reaction with arenes occur by direct electrophilic attack of NO2-OsN* at the aromatic ring. Our results should represent a significant advance in the photochemistry of metal nitrido complexes and in the design of reagents for the nitrogenation of organic substrates using visible light.


Synthesis of (PPh4)[OsVI(N)(NO2-L)(CN)3] (NO2-OsN)

The procedure is similar to that for OsN with minor modifications22,24. PhIO (220 mg, 1 mmol) was added to a solution of NO2-OsG (100 mg, 0.1 mmol) in CH3CN (40 mL), and the mixture was stirred at room temperature for 10 h under Ar. The green solution was evaporated to dryness; the residue was dissolved in a minimum amount of CH2Cl2 and then loaded onto a silica gel column. The column was eluted with CH2Cl2/acetone (v/v, 10:1) to give a yellow band; the solvent was removed under reduced pressure, and the yellow residue was recrystallized from CH2Cl2/Et2O. Single crystals suitable for X-ray crystallography were obtained by slow diffusion of diethyl ether into a MeCN solution of the compound. Yield: 31 mg, 35%. IR (KBr disc, cm−1): v(C≡N) 2157 and 2154; v(N=O) 1322; v(Os≡N) 1074; v(Os≡15N) 1046. 1H NMR (400 MHz, CDCl3): δ 8.91 (s, 1H, Ar−H), 7.97−7.90 (m, 6H, Ar−H), 7.80−7.77 (m, 8H, Ar−H), 7.73 (d, J = 8.0Hz, 1H, Ar−H), 7.67−7.62 (m, 8H, Ar−H), 7.55 (d, J = 12.0Hz, 2H, Ar−H), 6.56 (d, J = 9.3Hz, 1H, Ar-H). ESI-MS (−ve mode) in MeOH: m/z 539 (M); m/z 540 for 15N-labeled NO2Os15N. Anal. Calcd for C40H27N6O4POs: C, 54.79; H, 3.10; N, 9.58. Found: C, 54.70; H, 3.20; N, 9.60%. UV/Vis (CH2Cl2): λmax [nm] (ε [mol−1 dm3 cm−1]): 234sh (63660), 269sh (29270), 276 (33230), 291 (32520), 364 (32400).

Synthesis of (PPh4)[OsIII(NO2-L)(CN)3(NH3)] ([PPh4]1) and (PPh4)[OsIV(NO2-L)(CN)3(N=XAN(−2H))] ([PPh4]2)

Ten pyrex tubes (15 × 2 cm) each containing NO2-OsN (5 mg, 5.7 μmol) and xanthene (300 mg, 1.6 mmol) in 15 mL CH2Cl2 were prepared. Each tube was sealed by a rubber septum, degassed with Ar for 30 min and then irradiated with blue LED light for 6 h, whereby the light yellow solution turned red. The solutions were combined and the solvent was removed under reduced pressure. The unreacted xanthene was recovered by extraction with diethyl ether. The solid residue was then dissolved in a minimum amount of CH2Cl2 and loaded onto a silica gel column. The first yellow band (unreacted NO2-OsN) was eluted by CH2Cl2/acetone (v:v, 10:1). The second green band, which was a mixture of NO2-Os-(N=XAN(−2H)) and NO2-Os-(NH=XAN(−H)), was eluted by CH2Cl2/acetone (v:v, 4:1). The two complexes were eluted together due to their very similar structures, solubility and polarity. However, NO2-Os-(NH=XAN(H)) was slowly oxidized to NO2-Os-(N=XAN(2H)) during the process of recrystallization in air by slow diffusion of diethyl ether into a CH2Cl2 solution of the mixture. A third dark red band ([PPh4]1) was eluted by CH2Cl2/acetone/MeOH (v:v:v, 20:5:1).

Yield for [PPh4]1: 6 mg, 12%. Selected IR (KBr disc, cm−1): v(N-H) 3243; v(C≡N) 2109 and 2086; v(N=O) 1308. ESI-MS (−ve mode) in MeOH: m/z 542 ([M]), 525 [M - NH3]. Anal. Calcd for C40H30N6O4POs: C, 54.60; H, 3.44; N, 9.55%. Found: C, 54.50; H, 3.50; N, 9.47%. UV/Vis (MeOH): λmax [nm] (ε [mol−1 dm3 cm−1]): 269 (22120), 276 (22200), 294 (20230), 328 (14070), 377 (16600), 411 (11830), 459 (5120), 557 (1710). μeff = 1.95 μB.

Yield for [PPh4]2: 18 mg, 30%. Selected IR (KBr disc, cm−1): v(C≡N) 2131 and 2122; v(N=O) 1311; v(C=N) 1612. 1H NMR (400 MHz, CDCl3): δ 9.04 (s, 1H, Ar-H), 7.96 (d, J = 8.5Hz, 2H, Ar-H), 7.93–7.84 (m, 5H, Ar-H), 7.83–7.74 (m, 9H, Ar-H), 7.72–7.63 (m, 7.9Hz, 8H), 7.60 (d, J = 8.3Hz, 1H, Ar-H), 7.47 (t, J = 7.6Hz, 2H, Ar-H), 7.33 (d, J = 7.9Hz, 3H, Ar-H), 7.02 (dd, J = 15.2, 7.7Hz, 1H, Ar-H), 6.81–6.68 (m, 3H, Ar-H). ESI-MS (−ve mode) in MeOH: m/z 719 (M). Anal. Calcd for C53H35N6O5POs: C, 60.22; H, 3.34; N, 7.95. Found: C, 60.30; H, 3.40; N, 7.82%. UV/Vis (CH2Cl2): λmax [nm] (ε [mol−1 dm3 cm−1]): 267 (29290), 276 (27830), 287sh (22400), 335 (27740), 384 (24400), 403 (24070), 458 (10880).

Synthesis of (PPh4)[OsIV(N=DHA(−2H))(NO2-L)(CN)3] ([PPh4]3)

The procedure is similar to that for 2 except that 9,10-dihydroanthracene (DHA) was used instead of xanthene (XAN). The reactants in CH2Cl2 solution were irradiated with blue light for 24 h and complex 3 was isolated as PPh4+ salt by silica gel column chromatography and recrystallization by slow diffusion of diethyl ether into a CH2Cl2 solution of [PPh4]3. Yield for [PPh4]3: 19 mg, 32%. Selected IR (KBr disc, cm−1): v(C≡N) 2136 and 2127; v(C=N) 1638; v(N=O) 1313. 1H NMR (400 MHz, CDCl3): δ 9.04 (s, 1H, Ar-H), 8.14 (d, J = 7.5Hz, 2H, Ar-H), 7.98–7.88 (m, 5H, Ar-H), 7.86–7.78 (m, 8H, Ar-H), 7.75–7.66 (m, 8H, Ar-H), 7.67–7.56 (m, 4H, Ar-H), 7.55–7.48 (m, 3H, Ar-H), 6.93 (t, J = 8.3 Hz, 1H), 6.82 (t, J = 8.5 Hz, 3H, Ar-H), 6.37 (s, 2H, -CH2-). ESI-MS (−ve mode) in MeOH: m/z 717 (M). Anal. Calcd for C54H37N6O4POs: C, 61.47; H, 3.53; N, 7.97%. Found: C, 61.40; H, 3.48; N, 8.12%. UV/Vis (CH2Cl2): λmax [nm] (ε [mol−1 dm3 cm−1]): 261 (38700), 276 (29850), 285 (23260), 337 (28430), 376sh (22630), 444sh (9660).

Synthesis of (PPh4)[OsIV(N=EB(−2H))(NO2-L)(CN)3] ([PPh4]4)

The product was synthesized by a similar procedure as that for [PPh4]2 except that ethylbenzene (EB) was used instead of xanthene (XAN). After irradiation of the reactants in CH2Cl2 for 24 h, compound 4 was isolated as PPh4+ salt by silica gel column chromatography and recrystallized by slow evaporation of diethyl ether into a CH2Cl2 solution of [PPh4]4. Yield for [PPh4]4: 20 mg, 35%. Selected IR (KBr disc, cm−1): v(C≡N) 2140 and 2126; v(C=N) 1635; v(N=O) 1312. 1H NMR (400 MHz,CDCl3): δ 9.00 (s, 1H, Ar-H), 7.95–7.86 (m, 5H, Ar-H), 7.84–7.75 (m, 8H, Ar-H), 7.73–7.63 (m, 9H, Ar-H), 7.59 (d, J = 8.0 Hz, 1H, Ar-H), 7.45 (d, J = 8.3 Hz, 1H, Ar-H), 7.45 (d, J = 8.3 Hz, 1H, Ar-H), 7.24 (s, 1H, Ar-H), 6.97 (dd, J = 17.8, 8.4 Hz, 2H), 6.73 (d, J = 9.1 Hz, 1H, Ar-H), 5.18 (s, 3H, -CH3). ESI-MS (−ve mode) in MeOH: m/z 643 (M). Anal. Calcd for C48H35N6O4POs: C, 58.77; H, 3.60; N, 8.57. Found: C, 58.62; H, 3.50; N, 8.61%. UV/Vis (CH2Cl2): λmax [nm] (ε [mol−1 dm3 cm−1]): 261sh (24830), 269 (25790), 276 (23840), 288sh (18510), 329 (26560), 374sh (14480), 433sh (8160).

Synthesis of (PPh4)[OsIV(NO2-L)(CN)3(N=c-OCT(−2H))] ([PPh4]5)

The product was synthesized using a similar procedure for [PPh4]2 except that cyclooctane (c-OCT) was used instead of xanthene (XAN). After irradiation for about 72 h, compound 5 was isolated as PPh4+ salt by silica gel column purification and further purified from slow evaporation of diethyl ether into a CH2Cl2 solution of [PPh4]5. Yield for [PPh4]5: 15 mg, 27%. Selected IR (KBr disc, cm−1): v(C≡N) 2181 and 2120; v(C=N) 1630; v(N=O) 1311; 1H NMR (400 MHz, CDCl3): δ 8.92 (s, 1H, Ar-H), 7.91–7.85 (m, 4H, Ar-H), 7.81 (dt, J = 10.8, 5.4 Hz, 1H, Ar-H), 7.78–7.70 (m, 7H, Ar-H), 7.69–7.63 (m, 2H, Ar-H), 7.64–7.54 (m, 8H, Ar-H), 7.48 (p, J = 7.0 Hz, 2H, Ar-H), 6.81 (d, J = 9.3 Hz, 1H, Ar-H), 4.62 (t, J = 5.7 Hz, 4H, CH2), 1.73–1.57 (m, 10H). ESI-MS (−ve mode) in MeOH: m/z 649 (M); Anal. Calcd for C48H41N6O4POs: C, 58.41; H, 4.19; N, 8.51%. Found: C, 58.32; H, 4.25; N, 8.37%. UV/Vis (CH2Cl2): λmax [nm] (ε [mol−1 dm3 cm−1]): 258 (19060), 268 (17640), 276 (16790), 289 (15670), 326 (17520), 370sh (12390), 412sh (9950).

Synthesis of (PPh4)[OsIV(NO2-L)(CN)3(NH-ANTH(−H))] ([PPh4]7a) and (PPh4)[OsIV(NO2-L)(CN)3(N=ANTH (−2H) = O)] ([PPh4]7b)

Ten pyrex tubes (15 cm × 2 cm) each containing NO2-OsN (5 mg, 5.7 μmol) and anthracene (ANTH, 100 mg, 0.56 mmol) in CH2Cl2 (15 mL) were prepared. Each tube was sealed by a rubber septum and degassed with Ar for 30 min. Then, the tubes are irradiated by blue LED light for 2 days, whereby the light yellow solutions turned brown. The solutions in the tubes were combined and the solvent was removed under reduced pressure. The residue was washed with diethyl ether (100 mL) to remove the unreacted anthracene. The solid was then dissolved in a minimum amount of CH2Cl2 and then loaded onto a silica gel column. The first light yellow band, (PPh4)[OsIV(NO2-L)(N=ANTH (2H)=O)(CN)3] ([PPh4]7b), was eluted by CH2Cl2/Acetone (9:1) and the second band (PPh4)[OsIV(NO2-L)(NH-ANTH(H))(CN)3] ([PPh4]7a) was eluted by CH2Cl2/Acetone (4:1).

Yield for [PPh4]7a: (7 mg, 12%). Selected IR (KBr disc, cm−1): v(N-H) 3248; v(C≡N) 2145 and 2128; v(N=O) 1314. 1H NMR (400 MHz,CDCl3): δ 9.00 (d, J = 2.8 Hz, 1H); 8.13 (d, J = 7.8 Hz, 2H); 7.97–7.84 (m, 6H); 7.83–7.74 (m, 8H); 7.69–7.63 (m, 8H); 7.62–7.52 (m, 3H); 7.49 (d, J = 7.7 Hz, 1H); 7.29 (dd, J = 13.0, 5.2 Hz, 2H); 6.90 (t, J = 7.8 Hz, 1H); 6.84–6.74 (m, 3H); ESI-MS (−ve mode) in MeOH: m/z 717 (M); Anal. Calcd for C54H37N6O4OsP: C, 61.47; H, 3.53; N, 7.97. Found: C, 61.40; H, 3.62; N, 7.90%. UV/Vis (CH2Cl2): λmax [nm] (ε [mol−1 dm3 cm−1]): 232 (91670), 261 (59390), 276sh (47080), 337 (44270), 374sh (35790), 447sh (15430).

Yield for [PPh4]7b: (9 mg, 15%). Selected IR (KBr disc, cm−1): v(C≡N) 2149 and 2129; v(C=O) 1704 and 1649; v(C=N) 1612 and 1596; v(N=O) 1312. 1H NMR (400 MHz,CDCl3): δ 9.03 (d, J = 2.9 Hz, 1H); 8.59–8.53 (m, 2H); 8.37 (d, J = 8.0 Hz, 2H); 8.04 (dd, J = 9.4, 2.9 Hz, 1H); 7.98–7.92 (m, 2H); 7.90–7.84 (m, 4H); 7.76 (td, J = 7.8, 3.6 Hz, 9H); 7.67–7.56 (m, 9H); 7.52 (d, J = 8.2 Hz, 1H); 7.33 (t, J = 7.9 Hz, 1H); 7.02–6.89 (m, 4H). ESI-MS (−ve mode) in MeOH: m/z 731 (M); Anal. Calcd for C54H35N6O5OsP: C, 60.67; H, 3.30; N, 7.86. Found: C, 60.55; H, 3.35; N, 7.79%. UV/Vis (CH2Cl2): λmax [nm] (ε [mol−1 dm3 cm−1]): 236 (74870), 244 (65420), 270 (34320), 277 (35700), 286 (31110), 336 (29430), 439 (30840)

Synthesis of (PPh4)[OsIV(NO2-L)(CN)3(N=Ph=O(2H))] ([PPh4]8)

The synthetic route for [PPh4]8 is similar to that of [PPh4]7a except that benzene (2 mL) was used instead of anthracene, and the duration of the irradiation was 2 weeks. Yield for [PPh4]8: (7.7 mg, 14%). Selected IR (KBr disc, cm−1): v(C≡N) 2149 and 2140; v(C=O) 1623; v(C=N) 1615; v(N=O) 1307. 1H NMR (400 MHz, CDCl3): δ 9.08 (d, J = 2.8 Hz, 1H); 8.40 (d, J = 9.8 Hz, 2H); 8.20–8.13 (m, 1H); 7.98–7.90 (m, 4H); 7.86–7.72 (m, 10H); 7.71–7.56 (m, 10H); 7.07 (d, J = 9.3 Hz, 1H); 6.92 (t, J = 7.4 Hz, 2H). ESI-MS (−ve mode) in MeOH: m/z 631 (M); Anal. Calcd for C46H31N6O5POs: C, 57.02; H, 3.22; N, 8.67. Found: C, 57.10; H, 3.17; N, 8.70%. UV/Vis (CH2Cl2): λmax [nm] (ε [mol−1 dm3 cm−1]): 233 (76260), 239 (60300), 270 (39090), 277 (41510), 295 (38530), 337 (36260), 349 (35200), 427 (42520), 450 (34000).