FIELD OF THE INVENTION
This invention relates to Fe2(dobdc), a novel material that has a metal-organic framework with a high density of coordinatively-unsaturated FeII centers lining the pore surface. This material can be used for the separation of O2 from N2 and in a number of additional separation applications based on selective, reversible electron transfer reactions. In addition, it can be used for many other processes, including paraffin/olefin separations, nitric oxide/nitrous oxide separation, carbon monoxide removal, acetylene storage, and as an oxidation catalyst.
BACKGROUND OF THE INVENTION
With over 100 million tons produced annually, O2 is one of the most widely used commodity chemicals in the world.1 Its potential utility in processes associated with the reduction of carbon dioxide emissions from fossil fuel-burning power plants, however, means that the demand for pure O2 could grow enormously. For example, when implementing pre-combustion CO2 capture, pure O2 is used for the gasification of coal, which produces the feedstock for the water-gas shift reaction used to produce CO2 and H2.2 In addition, oxyfuel combustion has received considerable attention for its potential utility as an alternative to post-combustion CO2 capture. Here, pure O2 is diluted to 0.21 bar with CO2 and fed into a power plant for fuel combustion. Since N2 is absent from the resulting flue gas, the requirement for post-combustion separation of CO2 from N2 is eliminated.3
The separation of O2 from air is currently carried out on a large scale using an energy-intensive cryogenic distillation process.4 Zeolites are also used for O21N2 separation,5 both industrially and in portable medical devices. However, this process is inherently inefficient as the materials used adsorb N2 over O2 with poor selectivity. By employing materials that selectively adsorb O2 and can operate near ambient temperatures, lower energy and capital costs could be realized. Metal-organic frameworks (“MOFs”), which have already received considerable attention for applications in gas storage6 and separation,7 represent a promising new class of potential O2 separation materials.
The energy cost associated with the separation of hydrocarbons, as currently carried out at enormous scale via cryogenic distillation, could potentially be lowered through development of selective solid adsorbents that operate at higher temperatures and lower pressures. As a consequence of the similar sizes and volatilities of the hydrocarbons, separations, for example, of olefin/paraffin mixtures, such as ethylene/ethane and propylene/propane, must currently be performed at low temperatures and high pressures, and are among the most energy-intensive separations carried out at large scale in the chemical industry. Because these hydrocarbon gaseous mixtures are produced by cracking long-chain hydrocarbons at elevated temperatures, a substantial energy penalty arises from cooling the gases to the low temperatures required for distillation. Thus, tremendous energy savings could be realized if materials enabling the efficient separation of hydrocarbons at higher temperatures, than currently used in distillation, and atmospheric pressure were achieved.
Current competing approaches for separating hydrocarbons include membrane designs, organic solvent-based sorbents, as well as porous solid adsorbents featuring selective chemical interactions with the carbon-carbon double bond in olefins. In this latter category, MOFs, which offer high surface areas, adjustable pore dimensions, and chemical tenability, have received considerable attention as adsorbents in gas storage and separation applications, with particular emphasis on the dense storage of methane and hydrogen, and on the efficient removal of carbon dioxide from flue gas and natural gas deposits. More recently, MOFs represent a promising new class of potential hydrocarbon separation materials.
In addition to the separation of binary olefin/paraffin mixtures, there is tremendous current interest in separating ethane, ethylene, and acetylene from methane for the purification of natural gas. Indeed, a number of porous materials are able to selectively separate methane from mixtures including C2 hydrocarbons (ethane, ethylene, and acetylene). These materials, however, are unable to simultaneously purify the ethane, ethylene, and acetylene being removed from the gas stream. A separation process that utilizes the same adsorptive material for the separation and purification of all four components of a C1/C2 mixture could potentially lead to substantial efficiency and energy savings over current processes.
Ethylene produced in a naphtha cracker contains an impurity of approximately 1% acetylene. However, there are strict limitations to the amount of acetylene that can be tolerated in the feed to an ethylene polymerization reactor. The current technology for this purpose uses absorption with liquid DMF, but the use of solid adsorbents could potentially provide an energy-efficient alternative.
In addition, early efforts in developing metal-organic framework catalysts have largely focused on new synthetic methods for incorporating catalytic functionalities onto the pore surface, as well as proof-of-concept studies, such as the heterogenization of well-known homogeneous catalysts or simple acid/base activation of substrates. While these examples demonstrate the viability of metal-organic frameworks as heterogeneous catalysts, they provide little improvement over existing systems and do not take full advantage of properties unique to metal-organic frameworks, including the ability to design specific and spatially separated active sites. In particular, framework incorporation of reactive transition metal intermediates, such as metal-ligand multiple bonds or low-coordinate metal centers, is a promising area that has yet to be explored. In principle, redox catalysis involving the formation of metal species in unusual coordination environments, geometries, and/or oxidation states that are entirely unfeasible in homogeneous systems could proceed easily in the context of metal-organic frameworks wherein each metal center is held fixed and isolated.
SUMMARY OF THE INVENTION
Metal-organic frameworks have received considerable attention for a variety of gas separation applications. However, the use of Fe2(dobdc), a metal-organic framework featuring redox-active metal centers for gas separations based on selective, reversible (partial) electron transfer reactions represents a novel advance in the field. This material may be used for numerous separation and storage applications including, but not limited to, paraffin/olefin separations, oxygen/nitrogen separation, carbon monoxide removal, acetylene storage, and nitric oxide/nitrous oxide separations. This material displays incredible separation properties at temperatures that are much more favorable to those currently used in industrial applications.
One embodiment is a material including Fe2(2,5-dioxido-1,4-benzenedicarboxylate). A method of making Fe2(dobdc) (dobdc=2,5-dioxido-1,4-benzenedicarboxylate) may include reacting FeCl2 with H4dobdc (dobdc=2,5-dioxido-1,4-benzenedicarboxylate) in a reaction mixture to produce Fe2(dobdc). The reaction mixture may also include dimethylformamide (DMF) and methanol.
Fe2(dobdc) may use to separate a variety of mixtures. A embodiment of a method of separating a mixture stream including O2 and N2 may include contacting a mixture stream comprising O2 and N2 with a material comprising Fe2(dobdc) to obtain a stream richer in O2 as compared to the mixture stream, and obtain a stream richer in N2 as compared to the mixture stream.
An embodiment of a method of separating a mixture including a first chemical and a second chemical may include contacting a mixture stream including the first chemical and the second chemical with a material comprising Fe2(dobdc), obtaining a stream richer in the first chemical as compared to the mixture stream, and obtaining a stream richer in the second chemical as compared to the mixture stream.
For example, the first chemical may be a paraffin and the second chemical may be an olefin. The first chemical may be ethane and the second chemical may be ethene. The first chemical may be propane and the second chemical may be propene. The first chemical may be nitric oxide and the second chemical may be nitrous oxide.
An embodiment of a method of storing acetylene may include contacting acetylene with Fe2(dobdc).
A method of oxidizing a material may include contacting the material with Fe2(dobdc).
BRIEF DESCRIPTION OF THE DRAWINGS
FIG. 1 is a graphical representation of a portion of the crystal structure of desolvated Fe2(dobdc) as viewed approximately along the [001] direction.
FIG. 2 is a diffuse reflectance UV-visible-NIR spectra of methanol solvated, desolvated Fe2(dobdc), and H4dobdc.
FIG. 3 is a graph showing excess O2 and N2 adsorption isotherms collected for Fe2(dobdc) at various temperatures.
FIG. 4 is graph showing the uptake and release of O2 in Fe2(dobdc) over 13 cycles at 211 K.
FIG. 5 is a graph that shows calculated N2 and O2 breakthrough curves during adsorption of simulated air by Fe2(dobdc).
FIG. 6 is a Mössbauer spectra measured between 94 and 252 K for Fe2(dobdc) in the presence of O2.
FIG. 7 is an infrared spectra obtained for Fe2(dobdc) with and without O2 and at various temperatures.
FIG. 8 is a series of graphical representations of a first coordination spheres for the iron centers within Fe2(dobdc) and its O2 and N2 dosed variants, dosed at various temperatures.
FIG. 9 is a graph showing the separation of a mixture of ethane and ethane.
FIG. 10 is a graph showing the separation of a mixture of propane and propene.
FIG. 11 is a graph comparing the powder X-ray diffraction patterns of as-synthesized Fe2(dobdc), Zn2(dobdc), and Mg2(dobdc).
FIG. 12 is a Rietveld refinement of the experimental neutron diffraction pattern of desolvated Fe2(dobdc).
FIG. 13 is a graph showing N2 adsorption in Fe2(dobdc) at 77 K.
FIG. 14 is a TGA of Fe2(dobdc) under N2.
FIG. 15 a graph showing dual-site Langmuir-Freundlich fits for Oxygen and Nitrogen adsorption in Fe2(dobdc).
FIG. 16 is a graph showing isosteric heats of adsorption of O2 and N2.
FIG. 17 is a graph of O2/N2 selectivity as a function of pressure at various temperatures.
FIG. 18 is a schematic drawing of VSA apparatus.
FIG. 19 is a series of graphs showing a calculated N2 adsorption breakthrough curves and calculated O2 desorption breakthrough curves during adsorption/desorption of simulated air by Fe2(dobdc) at various temperatures.
FIG. 20 is graph showing temperature dependence of quadrupole splitting for Fe2(dobdc), Fe2(O2)2(dobdc), and Fe2(O2)(dobdc).
FIG. 21 is a graph showing temperature dependence of the logarithm of the Mössbauer spectral absorption area of Fe2(dobdc).
FIG. 22 is a graph showing temperature dependence of the isomer shifts Fe2(dobdc), Fe2(O2)2(dobdc), and Fe2(O2)(dobdc).
FIG. 23 is a graph showing relative absorption areas of Fe2(dobdc), Fe2(O2)2(dobdc), and Fe2(O2)(dobdc) as a function of temperature.
FIG. 24 shows graphs of the effects of progressive dosage of O2 at low temperature and of outgassing at low temperature on the IR spectra of activated Fe2(dobdc).
FIG. 25 is an ATR spectra of activated Fe2(dobdc) and a partially oxidized sample.
FIG. 26 is series of Raman spectra of activated Fe2(dobdc), a partially oxidized sample, and an activated sample subject to 40 mbar of oxygen.
FIG. 27 is Rietveld refinement of the experimental neutron diffraction pattern of Fe2(dobdc) exposed to O2 at 100K.
FIG. 28 is Rietveld refinement of the experimental neutron diffraction pattern of Fe2(dobdc) exposed to O2 at 298K.
FIG. 29 shows, at the top, a graphical representation of a structure of Fe2(O2)2(dobdc)-202 as viewed down the (001) direction. At the bottom are an H4(dobdc) ligand and the first coordination spheres for the iron centers in the solid state structures obtained upon dosing Fe2(dobdc) with acetylene, ethylene, ethane, propylene, and propane.
FIG. 30 is a series of graphs, the top row of which are gas adsorption isotherms for methane, ethane, ethylene, and acetylene (a) and for propane and propylene (b) in Fe2(dobdc) at 318 K, and the bottom row of which are experimental breakthrough curves for the adsorption of equimolar ethane/ethylene (c) and propane/propylene (d) mixtures flowing through Fe2(dobdc).
FIG. 31 is a series of graphs showing calculations of the adsorption selectivity for ethane/ethylene (upper left), propane/propylene (upper right), acetylene/ethylene (lower left) and acetylene/methane, ethylene/methane, ethane/methane (lower right) in Fe2(dobdc) at 318 K.
FIG. 32 is a series of curves showing mol % (left) and concentration (right) of propane and propylene during adsorption (upper) and desorption (lower) of a simulated breakthrough experiment.
FIG. 29 is a series of curves showing mol % (left) and concentration (right) of ethane and ethylene during adsorption (upper) and desorption (lower) of a simulated breakthrough experiment.
FIG. 34 is a series of graphs showing production capacities of 99% pure propane (left) and 99.5% pure propylene (right) as a function of the total pressure at the inlet to the adsorber for Fe2(dobdc), Mg2(dobdc), NaX zeolite, Cu3(btc)2, Cr3(btc)2, ITQ-12, and Fe-MIL-100.
FIG. 35 is a series of graphs showing production capacities of 99% pure ethane (left) and 99.5% pure ethylene (right) as a function of the total pressure at the inlet to the adsorber for Fe2(dobdc), Mg2(dobdc), and NaX zeolite.
FIG. 36 shows, at left, a graph of calculated methane, ethane, ethylene, and acetylene breakthrough curves for various gases in Fe2(dobdc), and, at right, a schematic representation of the separation of a mixture of methane, ethane, ethylene, and acetylene using Fe2(dobdc) in an adsorption process.
FIG. 37 shows transient breakthrough of acetylene/ethylene mixture in an adsorber bed packed with Fe2(dobdc).
FIG. 38 is a graphical representation of a portion of the structure of Fe2(dobdc) showing carbon monoxide (CO) coordinated to the open Fe2+ site.
FIG. 39 is an infrared spectrum of Fe2(dobdc) under successively increasing doses of CO.
FIG. 40 is graph of low-pressure adsorption of CO, CH4, N2, and H2 in Fe2(dobdc) at 298 K.
FIG. 41 shows the excess adsorption isotherms of CO, CH4, N2, and H2 collected for Fe2(dobdc) at 318 K, and shows (inset) the isosteric heat of CO adsorption in Fe2(dobdc) as a function of loading.
FIG. 42 show the infrared spectrum of CO adsorbed on Fe2(dobdc) at room temperature.
FIG. 43 is a graphical representation of crystal structures of Fe2(dobdc) with adsorbed N2, CO, or D2.
FIG. 44 is an 1H NMR of products of the reaction of Fe2(dobdc) with excess 1,4-cyclohexadiene in CD3CN.
FIG. 45 is a table showing dual-site Langmuir-Freundlich parameters for O2 isotherms in Fe2(dobdc) at different temperatures.
FIG. 46 is a table shownig dual-site Langmuir-Freundlich parameters for N2 isotherms in Fe2(dobdc) at different temperatures.
FIG. 47 is a table showing Mössbauer Spectral Parameters for Fe2(dobdc) Obtained Before and After Oxygenation.
FIG. 48 is a table showing unit cell lengths and volumes.
FIG. 49 is a diagram showing the oxidation of propylene to acetone using O2 as the oxidant.
FIG. 50 shows representative oxidation reactions.
DETAILED DESCRIPTION OF THE INVENTION
Described is a method of separating a target component from a chemical mixture using Fe2(dobdc). FIG. 1 is a portion of the crystal structure of desolvated Fe2(dobdc) as viewed approximately along the [001] direction (H atoms have been omitted for clarity.) This material has a metal-organic framework with a high density of coordinatively-unsaturated FeII centers lining the pore surface. This material can be used for the separation of O2 from N2 and in a number of additional separation applications based on selective, reversible electron transfer reactions. In addition to being used as an O2 separation material, it can be used for many other processes, including paraffin/olefin separations, nitric oxide/nitrous oxide separation, carbon monoxide removal, acetylene storage, and as an oxidation catalyst.
The high surface areas and open metal coordination sites possible within metal-organic frameworks make them particularly attractive for the development of an adsorption-based process for the separation of O2 from air. While coordinatively-unsaturated metal centers have been generated in such materials via chelation by post-synthetically modified bridging ligands,8 or via insertion into open ligand sites,9 they are most often created by evacuation of frameworks that have metal-bound solvent molecules. This strategy has been employed to expose M2+ cation sites in some of the most widely-studied frameworks, such as M2(dobdc) (M=Mg, Mn, Co, Ni, Zn; dobdc4−=2,5-dioxido-1,4-benzenedicarboxylate)10 and M3(BTC)2 (M=Cu, Cr, Mo; BTC3−=1,3,5-benzenetricarboxylate).11
To achieve a high selectivity for the coordination of O2 over N2, one can take advantage of the greater electron affinity of the former molecule. Indeed, coordinatively-unsaturated CrII centers in Cr3(BTC)2 give rise to an exceptionally strong preference for adsorbing O2 relative to N2 via charge transfer. Although the interaction with O2 proved too strong to achieve full reversibility with this material, the result demonstrates the potential power of frameworks with redox-active metal centers for the separation of O2 and N2. In view of its widespread deployment as an O2 carrier in biology,12 FeII was chosen.
The air-free reaction between FeCl2 and H4dobdc (dobdc4−=2,5-dioxido-1,4-benzenedicarboxylate) in a mixture of DMF and methanol affords Fe2(dobdc).4DMF, a metal-organic framework adopting the MOF-74 (or CPO-27) structure type. The desolvated form of this material displays a BET surface area of 1350-1360 m2/g and features a hexagonal array of one-dimensional 11 Å wide channels lined with coordinatively-unsaturated FeII centers. With a compact tetra-anionic bridging ligand, the structure features a unprecedented high surface density of 2.9 FeII coordination sites available per 100 11 Å2 on its surface, with spacings of just 6.84(1) and 8.98(2) Å between iron atoms along and around a channel, respectively. Thus, it appears to provide a near optimal platform for the high-capacity adsorption of small olefins, such as ethylene and propylene. Furthermore, the Mg2+ or Co2+ analogues of this structure type have recently been shown to disply selective adsorption for olefins over paraffins. The higher the surface area and softer metal character of Fe2(dobdc) as compared to the recently reported materials should lend both higher selectivity and capacity to the iron(II) framework.
Gas adsorption isotherms at 298 K indicate that Fe2(dobdc) binds O2 preferentially over N2, with an irreversible capacity of 9.3 wt %, corresponding to the adsorption of one O2 molecule per two iron centers. Remarkably, at 211 K, O2 uptake is fully reversible and the capacity increases to 18.2 wt %, corresponding to the adsorption of one O2 molecule per iron center. Mössbauer and infrared spectra are consistent with partial charge transfer from iron(II) to O2 at low temperature and complete charge transfer to form iron(III) and O22− at room temperature. The results of Rietveld analyses of powder neutron diffraction data (4 K) confirm this interpretation, revealing O2 bound to iron in a symmetric side-on mode with dO-O=1.25(1) Å at low temperature and in a slipped side-on mode with dI-O=1.6(1) Å when oxidized at room temperature. Application of ideal adsorbed solution theory in simulating breakthrough curves show Fe2(dobdc) to be a promising material for the separation of O2 from air at temperatures well above those currently employed in industrial settings.
Herein, we report the synthesis and O2 binding properties of Fe2(dobdc), a metal-organic framework with a high density of coordinatively-unsaturated FeII centers lining the pore surface.
This invention will be better understood with reference to the following experimental examples, which are intended to illustrate specific embodiments within the overall scope of the invention.
Experimental Section
General. Unless otherwise noted, all procedures were performed under an N2 atmosphere using standard glovebox or Schlenk techniques. Anhydrous, air-free N,N-dimethylformamide (DMF) and methanol were purchased from commercial vendors and further deoxygenated by purging with N2 for at least 1 h prior to being transferred to an inert atmosphere glovebox. All other reagents were obtained from commercial vendors at reagent grade purity or higher and used without further purification.
Synthesis of Fe2(dobdc). Anhydrous ferrous chloride (1.1 g, 9.0 mmol), 1,4-dihydroxyterephthalic acid (0.71 g, 3.6 mmol), DMF (300 mL) and methanol (36 mL) were added to a 500-mL Schlenk flask. The reaction mixture was heated at 393 K and stirred for 18 h to afford a red-orange precipitate. The solid was collected by filtration and washed with 100 mL of DMF to yield 2.0 g (91%) of Fe2(dobdc).4DMF. Anal. Calcd. for C20H30Fe2N4O10: C, 40.16; H, 5.06; N, 9.37. Found: C, 40.26; H, 5.08; N, 9.24. A sample of this compound (1.9 g, 3.3 mmol) was soaked in 100 mL of DMF at 393 K for 24 h after which the solvent was decanted, and the solid was then soaked in 100 mL of methanol at 343 K for 24 h. The methanol exchange was repeated three times, and the solid was collected by filtration to yield 1.25 g (87%) of Fe2(dobdc).4MeOH as a yellow-ochre powder. Anal. Calcd. for Fe2Cl2H18O10: C, 33.21; H, 4.18. Found: C, 33.42; H, 4.09. A sample of this compound was fully desolvated by heating under dynamic vacuum (<10 μbar) at 433 K for 24 h to yield Fe2(dobdc) as a light green powder. Anal. Calcd. for Fe2C8H2O6: C, 31.42; H, 0.66. Found: C, 31.55; H, 0.50.
Low-Pressure Gas Adsorption Measurements. For all gas adsorption measurements 200-225 mg of Fe2(dobdc).4MeOH was transferred to a pre-weighed glass sample tube under an atmosphere of nitrogen and capped with a Transeal. Samples were then transferred to Micromeritics ASAP 2020 gas adsorption analyzer and heated at a rate of 0.1 K/min from room temperature to a final temperature of 433 K. Samples were considered activated when the outgas rate at 433 K was less than 2 Oar/min. Evacuated tubes containing degassed samples were then transferred to a balance and weighed to determine the mass of sample, typically 150-175 mg. The tube was transferred to the analysis port of the instrument where the outgas rate was again determined to be less than 2 Oar/min at 433 K. Nitrogen gas adsorption isotherms at 77 K were measured in liquid nitrogen, while O2 measurements between 200 and 273 K were measured using liquid nitrogen/solvent slurry baths. All measurements above 273 K were performed using a recirculating dewar connected to an isothermal bath.
Transmission Infrared and Diffuse Reflectance UV-vis-NIR Spectroscopy. Prior to O2 dosing, Fe2(dobdc).4MeOH samples were activated under dynamic vacuum (residual pressure<0.1 μbar) at 433 K for 18 h. Infrared spectra were collected on thin deposits of sample supported on a silicon wafer in an airtight quartz cell that allows for collection of spectra under controlled atmospheres. The film was prepared from a suspension of Fe2(dobdc) in methanol. Transmission FTIR spectra were collected at 2-cm−1 resolution on a Bruker IFS 66 FTIR spectrometer equipped with a DTGS detector. Diffuse Reflectance UV-vis-NIR spectra were recorded on a Cary 5000 spectrophotometer equipped with reflectance sphere. Spectra of the desolvated framework were recorded on a thick self-supported wafer of the sample. Attenuated total reflection (ATR) spectra were recorded on a Bruker single reflection ALPHA-Platinum ATR spectrometer with a diamond crystal accessory.
Neutron Diffraction Data Collection and Refinement. Neutron powder diffraction (NPD) experiments were carried out on 0.9698 g and 0.6200 g of Fe2(dobdc) and Fe2(O2)(dobdc) respectively using the high-resolution neutron diffractometer, BT1, at the National Institute of Standards and Technology Center for Neutron Research (NIST). Both samples were placed in a He purged glove box, loaded into a vanadium can equipped with a gas loading valve, and sealed using an indium O-ring. Neutron diffraction data were collected using a Ge(311) monochromator with an in-pile 60′ collimator corresponding to a wavelength of 2.0782 Å. The samples were loaded into a top-loading closed cycle refrigerator and then data were collected at 4 K. After data collection of the bare material, O2 loading was then carried out. The sample was warmed to 125 K and then exposed to a predetermined amount of gas (2.0 O2 per Fe2+). Upon reaching an equilibrium pressure at the loading temperature, the sample was then slowly cooled to ensure complete adsorption of the O2. Data was then collected at 4 K.
NPD measurements of N2-loaded Fe2(dobdc) were performed on the Echidna instrument14 located at the Opal research reactor and operated by the Bragg Institute within the Australian Nuclear Science and Technology Organisation (ANSTO). A desolvated sample weighing 1.079 g was transferred to a vanadium cell in an Ar-filled glovebox. The cell was equipped with heaters for the gas line and valve to allow condensable gases to be loaded in the sample when mounted in the closed cycle refrigerator. The high-resolution diffractometer was configured with a Ge(331) monochromator using a take-off angle of 140° with no collimation at the monochromator and fixed tertiary 5′ collimation, resulting in a wavelength of 2.4406 Å. Diffraction data were collected at ˜9 K for the evacuated framework and with sequential loadings of 0.5, 1.0 and 2.0 N2:Fe, where the cryostat and sample were heated above 80 K to facilitate adsorption of the 99.999% pure N2 gas.
All NPD data were analyzed using the Rietveld method as implemented in EXPGUI/GSAS. The activated Fe2(dobdc) model was refined with all structural and peak profile parameters free to vary, resulting in a structure very similar to that determined using single crystal X-ray diffraction. Fourier difference methods were then employed to locate the adsorbed molecules in the data collected from the samples subsequently loaded with O2 or N2. The atoms in the adsorbed molecules were modeled individually. For the N2 adsorbed sample the two N atoms were constrained to maintain the fractional occupancy and isotropic displacement parameter within each diatomic molecule. For analysis of Fe2(dobdc) loaded with 2.0 O2/Fe, only fractional occupancies were constrained to maintain the same values, while all other parameters were allowed to vary. Further, for data collection of the irreversibly oxidized sample, Fe2(O2)(dobdc), the modeled O atoms were constrained to maintain the same fractional occupancies and isotropic displacement parameters. Once a stable structural model was obtained the isotropic displacement parameters of the adsorbed O2 molecule were allowed to vary independently of one another and then the displacement parameter for O(1b) were allowed to refine anisotropically.
Mössbauer Spectroscopy. The Mössbauer spectra of Fe2(dobdc), Fe2(O2)2(dobdc), and Fe2(O2)(dobdc) were measured at various temperatures between 94 and 298 K with a constant acceleration spectrometer which utilized a rhodium matrix cobalt-57 source, and was calibrated at 295 K with α-iron foil. The absorber contained 45(1) mg/cm2 of powder mixed with boron nitride. The Fe2(dobdc) absorber was prepared in an N2-filled glovebox, cooled to 77 K with liquid nitrogen, and inserted into a pre-cooled cryostat under dry helium. The sample of Fe2(O2)2(dobdc) was prepared in situ by dosing the evacuated cryostat to 300 mbar O2 at 94 K and allowing 3 h for equilibration. The sample of Fe2(O2)(dobdc) was prepared in situ by warming the oxidized sample above 250 K in the cryostat. The spectra of Fe2(dobdc) were measured at 298, 94, and 45 K in the absence of O2, after which the sample was warmed to 94 K and dosed with O2. Additional spectra were measured between 94 and 298 K and then subsequently measured again at 94 and 298 K. All spectra were fit with symmetric Lorenzian quadrupole doublets; the resulting spectral parameters, listed in the order of measurement, are given in FIG. 47. FIG. 47 shows Mössbauer Spectral Parameters for Fe2(dobdc) Obtained before and after oxygenation. The temperature dependence of the observed isomer shifts and relative absorption areas are plotted in FIGS. 22 and 23, respectively; further spectral details are provided in the Supporting Information. FIG. 22 is a temperature dependence of the isomer shifts Fe2(dobdc), Fe2(O2)2(dobdc), and Fe2(O2)(dobdc); and FIG. 23 is a relative absorption areas of Fe2(dobdc), Fe2(O2)2(dobdc), and Fe2(O2)(dobdc) as a function of temperature; The relative statistical errors associated with the isomer shifts, quadrupole splittings, line widths, percent areas, and absolute areas between 94 and 298 K are also given in FIG. 47.
Other Physical Measurements. Thermogravimetric analysis was carried out at a ramp rate of 1° C./min in a nitrogen flow with a TA instruments TGA 5000. Powder X-ray diffraction patterns were collected on air-free samples sealed in quartz capillaries on a Bruker Advance D8 powder X-ray diffractometer equipped with a capillary stage.
Results and Discussion
Synthesis of Fe2(dobdc). The reaction of anhydrous FeCl2 with H4dobdc in a mixture of DMF and methanol affords a solvated form of Fe2(dobdc) as a red-orange microcrystalline powder. FIG. 11 is a comparison between the powder X-ray diffraction patterns of as-synthesized Fe2(dobdc), Zn2(dobdc), and Mg2(dobdc). Powder x-ray diffraction data (see FIG. 11) show the compound to adopt the MOF-74 or CPO-27 structure type displayed in FIG. 1, as previously reported for M2(dobdc) (M=Mg, Mn, Co, Ni, Zn).10 The compound rapidly changes color to dark brown upon exposure to air, presumably due to at least partial oxidation of the FeII centers by O2. Based upon color, it is likely that the brown phase previously reported as Fe2(dobdc) is actually some oxidized form of the compound.10h Note that, perhaps owing to their air-sensitive nature, only a very few metal-organic frameworks based upon iron(II) have yet been isolated.15
The new framework was completely desolvated by soaking it in methanol to exchange coordinated DMF, followed by heating under dynamic vacuum at 433 K for 48 h. The resulting solid was light green in color. FIG. 12 is a Rietveld refinement of the experimental neutron diffraction pattern of desolvated Fe2(dobdc). The calculated pattern is in good agreement with the experimental data (crosses) as evidenced by the difference pattern. Rietveld analysis of the powder neutron diffraction data collected for Fe2(dobdc) indicate retention of the framework structure with no residual bound solvent (see FIG. 12). Thus, desolvation converts the FeII centers of the framework from an octahedral coordination geometry with one bound solvent molecule to a square pyramidal geometry with an open coordination site.
FIG. 13 is N2 adsorption in Fe2(dobdc) at 77 K. Low-pressure N2 adsorption data obtained for Fe2(dobdc) at 77 K reveal a type I adsorption isotherm characteristic of a microporous solid. The data indicate a BET surface area of 1360 m2/g (1535 m2/g Langmuir) (see FIG. 13). This value is significantly higher than the 920 m2/g Langmuir surface area reported for the material prepared in the presence of air and is in close agreement with the BET surface areas of 1218 m2/g and 1341 m2/g reported for Ni2(dobdc) and Co2(dobdc), respectively, indicating full evacuation of solvent molecules from the pores of the material.16 FIG. 14 is a TGA of Fe2(dobdc) under N2.
UV-vis-NIR Spectroscopy. FIG. 2 is a diffuse reflectance UV-visible-NIR spectra of methanol solvated, desolvated Fe2(dobdc), and H4dobdc. FIG. 2 shows the electronic absorption spectra for Fe2(dobdc).4MeOH, Fe2(dobdc), and H4dobdc. The spectrum for the yellow-ochre compound Fe2(dobdc).4MeOH exhibits a low energy doublet with peaks at 11600 cm−1 and 7600 cm−1. High-spin Fen centers in an octahedral symmetry are expected to show a spin-allowed transition, 5Eg←5T2g, in the near infrared region,17 and in many compounds this band is split into a doublet due to a lower symmetry ligand field, which lifts the two-fold orbital degeneracy of the 5Eg term. At higher energy, a broad component centered at 16000 cm−1 and a strong band with a maximum around 21000 cm−1 appear in the spectrum. The structure and position of these absorptions suggest they arise from mixing of d-d and charge transfer (LMCT and MLCT) transitions.18 Heating the solvated material at 433 K in vacuo results in removal of coordinated methanol with the formation of five-coordinative Fen centers. The corresponding change in symmetry at the metal site to approximately C4ν strongly affects the electronic transitions, which is evident from the spectrum of the desolvated material. In particular, the band at 21000 cm−1 slightly shifts to lower energy, mixing with the component at 16000 cm− and with the d-d transition, resulting in a strong absorption extending through 13000 cm−1. The very strong absorption maximum at 4400 cm−1 is associated with a d-d transition, with enhanced intensity owing to loss of an approximate inversion center in the ligand field upon conversion from pseudooctahedral to square pyramidal coordination.
O2 and N2 Adsorption. Gas adsorption isotherms indicate that Fe2(dobdc) preferrentially binds O2 over N2 at all temperatures measured (201, 211, 215, 226, and 298 K). FIG. 3 is a graph showing excess O2 adsorption isotherms collected for Fe2(dobdc) at 211, 226, and 298 K, and N2 adsorption at 298 K. Filled and open circles represent adsorption and desorption, respectively. As shown in FIG. 3, the O2 adsorption isotherm measured at 298 K is extremely steep, climbing to near 9.3 wt % at a pressure of just 0.01 bar. As the pressure is increased to 1.0 bar, uptake increases slightly to 10.4 wt %. The steep initial rise in the isotherm is consistent with strong binding of O2 to some of the FeII centers, while the subsequent gradual increase in adsorption is likely due to O2 physisorbed to the framework surface. Importantly, the amount of strongly bound O2 corresponds to 0.5 molecules per iron center. Adsorption of N2 under these conditions is noticeably lower, gradually rising to just 1.3 wt % at 1.0 bar. The selectivity factor of this material, calculated as the mass of O2 adsorbed at 0.21 bar divided by the mass of N2 adsorbed at 0.79 bar, is 7.5. Although this selectivity factor is among the highest reported for metal-organic frameworks,19 room temperature O2 adsorption was found to be irreversible. Attempts to identify conditions to release coordinated O2 by heating at temperatures of up to 473 K under dynamic vacuum ultimately lead to decomposition of the framework.
Upon dosing Fe2(dobdc) with O2 at lower temperatures, it was noted that the black color characteristic of the oxidized framework could be returned to light green by applying vacuum to the sample, suggesting reversible O2 adsorption. Additional O2 adsorption experiments confirmed this result. As shown in FIG. 3, at 226 K the framework adsorbs 14.1 wt % O2 at 0.21 bar, or 0.82 O2 molecules per iron site. Although adsorption at this temperature is largely reversible, O2 uptake decreases to 11.9 wt % after four adsorption/desorption cycles. Lowering the adsorption temperature to 211 K results in an increased O2 uptake of 18.2 wt %, corresponding to 1.0 molecules of O2 per iron center. The amount of O2 adsorbed at this temperature was found to decrease only slightly to 17.5 wt % after eight adsorption/desorption experiments. However, by cycling at a rapid rate, allowing just 2 min for adsorption and 25 min for desorption (instead of the 4-5 h typically required for collecting a full isotherm), resulted in no noticeable loss in adsorption capacity after 13 cycles (see FIG. 4, which is a graph showing the uptake and release of O2 in Fe2(dobdc) over 13 cycles at 211 K. Adsorption occurred within 2 min upon application of 0.21 bar of O2 and desorption was carried out by placing the sample under dynamic vacuum for 25 min).
To predict how Fe2(dobdc) would perform as an O2/N2 separation material, ideal adsorbed solution theory (ILAST) was employed at temperatures for which O2 adsorption is reversible. The O2 and N2 isotherms measured at 201, 211, 215, and 226 K were modeled with dual-site Langmuir-Freundlich fits. FIG. 15 is dual-site Langmuir-Freundlich fits for Oxygen (upper) and Nitrogen (lower) adsorption in Fe2(dobdc). The continuous solid lines are the dual-site Langmuir-Freundlich fits using the parameters specified in FIG. 45 (O2) and FIG. 46 (N2). FIG. 45 shows dual-site Langmuir-Freundlich parameters for O2 isotherms in Fe2(dobdc) at different temperatures. FIG. 46 shows dual-site Langmuir-Freundlich parameters for N2 isotherms in Fe2(dobdc) at different temperatures.
FIG. 16 is isosteric heats of adsorption of O2 and N2, determined from the dual-Langmuir-Freundlich fits in FIG. 45, FIG. 46 and application of equation (2). Isosteric heats of adsorption calculated from these fits are plotted in FIG. 16 and indicate higher enthalpies for O2 adsorption than N2 adsorption over the entire pressure range measured. The higher propensity of O2 to accept charge from FeII results in a larger initial isosteric heat of −41 kJ/mol, as compared to that of N2 (−35 kJ/mol). Accordingly, Fe2(dobdc) displays a high O2/N2 selectivity at 201, 211, 215, and 226 K. FIG. 17 shows O2/N2 selectivity as a function of pressure at 201 K, 211 K, 214 K, and 226 K. The selectivity ranges from 4.4 to over 11 and reaches a maximum of 11.4 at 201 K and about 0.4 bar.
The high O2/N2 selectivity, in conjunction with the rapid and reversible cycling times, suggest that Fe2(dobdc) warrants further consideration as an adsorbent for O2/N2 separations via a modified vacuum-swing adsorption (VSA) process. FIG. 18 is a schematic drawing of VSA apparatus. Here, dry air is flowed over a packed bed of Fe2(dobdc) at temperatures near 210 K, which could potentially offer significant cost and energy savings over current separation technologies that are performed at much lower temperatures. Breakthrough experiments were simulated at 211 and 226 K to evaluate the performance of Fe2(dobdc) for the separation of O2 from N2 at concentrations similar to those present in air (see FIG. 5). FIG. 5 is a graph that shows calculated N2 (diamonds) and O2 (squares) breakthrough curves during adsorption of simulated air (O2:N2=0.21:0.79) by Fe2(dobdc) at 211 K. The methodology adopted for the breakthrough simulations has been described.20 The x-axis in FIG. 5 is a dimensionless time, τ, obtained by dividing the actual time, t, by the contact time between the gas and metal-organic framework crystallites, alu. For a given adsorbent, under selected operating conditions, the breakthrough characteristics are uniquely defined by r, allowing the results presented here to be equally applicable to laboratory scale equipment as well as to industrial scale adsorbers. It is apparent from the simulated curves that N2 quickly saturates the sample, as evidenced by the low breakthrough time. The mole % of N2 in the outlet stream as a function of dimensionless time is presented in FIG. 19, which is a calculated N2 breakthrough curve during adsorption of simulated air (O2:N2=0.21:0.79) by Fe2(dobdc) at 211 K (lower left) and 226 K (upper left). Calculated O2 breakthrough curve during the desorption step of the vacuum-swing adsorption process at 211 K (lower right) and 226 K (upper right). In contrast to currently employed VSA processes, in which N2 is selectively adsorbed on the packed bed while O2 is collected, Fe2(dobdc) would selectively adsorb O2.21 Accordingly, shortly after N2 breakthrough, the gas stream is pure nitrogen while O2 is retained by the framework. Upon O2 breakthrough, the VSA process is advanced to the second step, in which vacuum is applied to the sample bed. Although the gas at the outlet is initially a mixture of N2 and O2 the concentration of O2 quickly increases to near 100 mole % (see FIG. 19). This results in a large supply of pure O2. After a majority of the O2 is removed from the adsorber, a low-pressure flow of pure N2 would be flowed over the material to fully regenerate the bed for subsequent cycling.
Mössbauer Spectra. The different O2 adsorption behavior at low versus room temperature suggests the existence of two different modes by which O2 binds to the open iron sites in Fe2(dobdc). Mössbauer spectroscopy was employed to probe the electronic structure at the metal center. At all temperatures, the spectra of Fe2(dobdc) in the absence of O2 feature a simple doublet. At 298 K this doublet exhibits an isomer shift of 1.094(3) mm/s and a quadrupole splitting of 2.02(1) mm/s. These values are consistent with high-spin iron(II) in a square pyramidal coordination environment, as established below for the structure of the compound. Upon exposure to O2, a small amount (ca. 5-15%, depending upon temperature) of high-spin iron(II) is still observed, presumably because a small portion of the iron(II) sites remain unoxygenated.
FIG. 6 is a Mössbauer spectra measured between 94 and 252 K for Fe2(dobdc) in the presence of O2. As shown in FIG. 6, the spectrum obtained in the presence of O2 at 94 K indicates that almost all of the iron in the sample has a substantially reduced isomer shift that is approximately halfway between those expected for high-spin iron(II) and high-spin iron(III). This suggests a partial transfer of electron density from each of the FeII centers in the framework to form a weak bond with an O2 species that is somewhere between the neutral molecule and superoxide. Thus, exposure of Fe2(dobdc) to O2 at low temperatures is consistent with the formation of Fe2(O2)2(dobdc), featuring one weakly held O2 molecule per iron atom. This is fully consistent with the observation of a reversible adsorption of 18.2 wt % O2 at 211 K. At this point it is not possible to determine from the Mössbauer spectral results whether the electron transfer is static or dynamic, with an electron transfer time that is faster than the ca. 10−7 s time scale of the iron-57 Mössbauer spectral experiment.
Upon warming to 222 K and above, further changes arise in the Mössbauer spectra, which are clearly indicative of the formation of high-spin iron(III). The temperature at which this change in oxidation state occurs is consistent with the temperature at which we first observe the onset of and irreversible uptake of O2 uptake in gas adsorption experiments (ca. 220 K). The change in oxidation state together with the irreversible uptake of 9 wt % O2 suggest the formation of a compound of formula Fe2(O2)(dobdc), in which half of the FeIII centers strongly bind a peroxide anion. Note that, consistent with the presence of at least two different coordination environments, one with O22− bound and one without, fitting the spectra requires the use of at least two doublets for the iron(III) components.
The temperature dependence of the quadrupole splitting of main spectral components observed for the framework in the presence of O2, corresponding to the FeII centers in Fe2(dobdc), the FeII/III centers in Fe2(O2)2(dobdc), and the FeIII centers in Fe2(O2)(dobdc), is shown in FIG. 20. As expected and in agreement with the Ingalls model,22 the quadrupole splitting of the square pyramidal high-spin FeII center in Fe2(dobdc) decreases the most with increasing temperature, a decrease that results from changes in the electronic population of the 3dxy, 3xz, and Myz orbitals, whose degeneracy has been removed by the low-symmetry component of the crystal field. Furthermore, there is a smaller decrease in the splitting upon warming of the other two components. FIG. 21 is a temperature dependence of the logarithm of the Mössbauer spectral absorption area of Fe2(dobdc). The temperature dependence of the logarithm of the Mössbauer spectral absorption area of Fe2(dobdc) (see FIG. 21), is well fit with the Debye model for a solid23 and yields a Debye temperature, ΘD, of 225(7) K, a value that is reasonable for the compound. Overall, the Mössbauer data point to a situation where, as a sample of Fe2(dobdc) is warmed under O2, an activation barrier is overcome for the transfer of electrons from two different iron centers to form a bound peroxide anion at every other iron site.
Infrared Spectra. The presence of various Fe—O2 adducts as a function of temperature should also be apparent by infrared spectroscopy. FIG. 7 shows an infrared spectra obtained for Fe2(dobdc) in the absence of O2 at room temperature, and upon dosing with 30 mbar of O2 at room temperature, and at a low temperature near 100 K. Difference spectra between the bare and O2 dosed materials at low and room temperature are shown. Spectra collected in transmission mode on thin films of Fe2(dobdc) (see FIG. 7), reveal a number of framework vibrations below 1300 cm−1. The reactivity of Fe2(dobdc) towards O2 was followed at both room temperature and near 100 K. The series of spectra obtained at near 100 K with varying O2 loadings are shown in FIG. 24.
Part (a) of FIG. 24 shows IR spectra of activated Fe2(dobdc); effect of progressive dosage of O2 at low temperature. Maximum coverage 30 mbar. Part (b) of FIG. 24 shows the effect of outgassing at low temperature. It is evident that under these conditions the interaction with oxygen is fully reversible. Bands associated to the superoxo species are clearly visible at 1129, 541 and 511 cm−1, while bands originally at 1250, 1198 and at 580 cm−1, shift to 1266, 1186 and 595 cm−1 respectively. Animation of vibrational modes of Ni2(dobdc) homologue on optimized structure computed with CRYSTAL code, reveal that all of them are related with the C-0 bonds of the linker, being the bands at 1250 at 580 cm−1 strongly correlated. [1]
Oxygenation of Fe2(dobdc) at low temperature gives rise to the spectrum indicated in FIG. 7, and the most relevant changes are evident in the difference spectrum shown in magenta. New bands are seen at 1129, 541, and 511 cm−1, while significant shifts are seen in the frameworks bands originally at 1250, 1198, and 580 cm−1 (causing negative components in the difference spectrum). The component at 1129 cm−1 is assigned to ν(0-0) of a partially-reduced (near superoxo) O2 species coordinated to FeII/III sites. The first overtone for this stretching mode is also clearly visible at 2238 cm−1. The band at 541 cm−1 is associated with the Fe—O2 vibration of the of this species, whereas the band at 511 cm−1 is attributed to an Fe—Olinker mode of the framework, reflecting the O2 adsorption induced modification in Fe.Olinker bonds.24 The interaction with O2 at low temperature is completely reversible by applying vacuum to the sample cell.
Oxygenation of Fe2(dobdc) at room temperature gives rise to the spectrum indicated in FIG. 7, which can be explained in terms of the formation of a peroxo species coordinated to FeIII centers.25 The main features in this case are a peak at 790 cm−1, due to a ν(O—O) vibrational mode, and a pair of peaks at 697 and 670 cm−1, arising from the peroxo ring modes of the Fe-(η2-O2) unit. The peaks at 550 cm−1 and 507 cm−1 are further assigned to the νasym and νsym modes of the iron-oxygen bond of the peroxo species.
Similar features are more clearly visible in the ATR spectrum of an oxidized sample (see FIG. 25). FIG. 25 is an ATR spectra of activated Fe2(dobdc) and of a partially oxidized sample. The spectra were collected inside a N2 filled glove box. Bands due to peroxo species are clearly visible at 796, 697 and 669 cm−1, confirming the data obtained in transmission mode on the sample carefully reacted at room temperature (see FIG. 7).
Small changes are also visible in the Raman spectrum of the sample upon O2 interaction (see FIG. 26). FIG. 26 is a Raman spectra collected with 512 nm laser at 5% of power on sample in a cell cooled by liquid nitrogen. Spectra of activated Fe2(dobdc); partially oxidized sample; effect of 40 mbar of oxygen on activated sample. Raman spectra have been collected on the sample cooled with a liquid nitrogen flux in order to reduce the laser damaging effects. In this case a band at 630 cm−1 is the most evident feature of the formation of a peroxo species. Smaller bands at 674 and 729 are also visible [2,3].
Overall, the vibrational spectra are fully consistent with the model already developed from interpretation of the O2 adsorption data and Mössbauer spectra.
Structures via Neutron Powder Diffraction. Powder neutron diffraction data provide direct structural details of the means by which O2 and N2 interact with Fe2(dobdc) (see FIG. 8). FIG. 8 shows a first coordination spheres for the iron centers within Fe2(dobdc) and its O2 and N2 dosed variants, as determined from Rietveld analysis of neutron powder diffraction data. The structures depicted are for samples under vacuum (upper left), dosed with N2 at 100 K (upper right), dosed with O2 at 100 K (lower left), and dosed with O2 at 298 K (lower right). All diffraction data were collected below 10 K. Values in parentheses give the estimated standard deviation in the final digit of the number. Initial data collected on an evacuated sample of Fe2(dobdc) confirm the presence of accessible FeII sites with a square pyramidal coordination environment. Here, each iron center is coordinated by 0 donor atoms from two aryloxide units (located at the front right and back left basal positions) and three carboxylate groups (at the remaining positions) from surrounding dobdc4− ligands. Note that the arrangement of framework O donor atoms is the same in each depiction shown in FIG. 8.
FIG. 27 is Rietveld refinement of the experimental neutron diffraction pattern of Fe2(dobdc) exposed to O2 at 100K. The calculated pattern is in good agreement with the experimental data (crosses) as evidenced by the difference pattern. A Rietveld refinement was performed against data collected for a sample of Fe2(dobdc) that was cooled to 100 K, dosed with two equiv of O2 per iron, and then cooled to 4 K (see FIG. 27). Three different O2 adsorption sites are evident in the resulting model. The highest occupancy site, with a refined occupancy of 0.917(8) O2 molecules per iron, is located at the open iron coordination position. Significantly, the O2 molecule binds in a symmetric side-on coordination mode, with Fe—O distances of 2.09(2) and 2.10(1) Å. The O—O separation of 1.25(1) Å lies between the internuclear distances observed for free O2 (1.2071(1) Å)26 and typical of an O2− superoxide unit (1.28 Å).4 This again is consistent with only partial reduction of O2 under these conditions. Although symmetric side-on coordination of superoxide and peroxide to other transition metals has been reported27 this represents, to the best of our knowledge, the first crystallographic evidence of non-bridging side-on binding of any dioxygen species to iron in a non-enzyme system.28 The second and third O2 adsorption sites, with occupancies of 0.857(9) and 0.194(8), respectively, occur in the pores of the framework at distances of greater than 3 Å from the iron center and organic linker (see FIG. 28), indicating weak dispersive type interactions between the adsorbate and the framework walls.
FIG. 28 is Rietveld refinement of the experimental neutron diffraction pattern of Fe2(dobdc) exposed to O2 at 298K. The calculated pattern is in good agreement with the experimental data (crosses) as evidenced by the difference pattern.
FIG. 29 shows a structure of Fe2(O2)2(dobdc)-2O2 as viewed down the (001) direction. (H atoms have been omitted for clarity.) There is an ethylene molecule bound to the open coordination site at each iron(II) center. At the bottom are an H4(dobdc) ligand and the first coordination spheres for the iron centers in the solid state structures obtained upon dosing Fe2(dobdc) with acetylene, ethylene, ethane, propylene, and propane. Note that for propane in Fe2(dobdc) the adsorbed hydrocarbon molecule has orientational disorder with respect to the open metal center. Of several refined models, the single-molecule with large displacement parameters is the most reasonable.
Rietveld refinement performed against data collected on a sample of Fe2(dobdc) that had been dosed with an excess of O2 at room temperature, evacuated, and subsequently cooled to 4 K was also performed (see FIG. 29). The data were best fit by a model in which O2 is coordinated to iron in an asymmetric side-on mode and at a refined occupancy of 0.46(2). The model indicates substantial elongation of the O—O distance to 1.6(1) Å, consistent with a two-electron reduction of O2 to peroxide. With an Fe—O2 centroid distance of 2.26(1) Å, the peroxide unit also appears to have slipped substantially towards one of the bridging ligands. This type of coordination of peroxide has been observed previously in naphthalene dioxygenase28a and has also been proposed based upon spectroscopic evidence for a number of non-heme iron complexes.29
Neutron powder diffraction data were further collected on a sample of Fe2(dobdc) dosed with 0.5, 1.0, and 2.0 equiv of N2 dosed at 80 K. Upon dosing with approximately 0.5 equiv of N2, a binding site at the metal center is apparent with an occupancy of 0.641(5). Nitrogen coordinates end on with an Fe—N—N angle of 179(1)° and an Fe—N distance of 2.30(1) Å. The N—N distance of 1.133(15) Å is slightly longer than the N—N distance of free nitrogen (1.0977(1) Å).30 Additional N2 uptake reveals a second site that runs more parallel to the pore walls, with N . . . O contacts between 3.4 and 3.6 Å. The close N2-framework interactions are the origins of the relatively high enthalpy for adsorption. The metal-specific interactions, however, are clearly much weaker than for O2, which results in interaction of both atoms with the metal, electron transfer, and a significant compression of the unit cell upon adsorption (see FIG. 48). FIG. 48 shows a table of unit cell lengths and volumes.
The differences in how O2 binds to iron within Fe2(dobdc) at low versus high temperatures suggests that the framework undergoes electron transfer processes similar to those reported for nonheme iron-containing enzymes.31 In these systems, O2 typically progresses through a number of electron transfer steps starting with superoxo and peroxo. In the case of Fe2(dobdc) at low temperature, each iron shares one of its electrons with a single O2 molecule, resulting in oxidation of all of the metal centers to an intermediate iron(II/III) oxidation state. This charge transfer is reversible at low temperatures and accounts for the high gas uptake demonstrated in the gas adsorption experiments. However, at elevated temperatures two electrons are transferred to the adsorbing O2 molecule, the first presumably being shared in a manner analogous to what occurs at low temperature, and the second subsequently arriving from an adjacent iron center by promotion over an activation barrier via the available thermal energy. In this scenario, all of the metal centers within the framework are converted to iron(III), half of which are coordinated irreversibly to a peroxide anion, while the other half remain five-coordinate.
The foregoing results demonstrate the ability of Fe2(dobdc) to selectively bind O2 over N2 via electron transfer interactions. Breakthrough curves calculated using single-component gas adsorption isotherms and ideal adsorbed solution theory indicate that the material should be capable of the high-capacity separation of O2 from air at temperatures as high as 226 K. This is substantially higher than the cryogenic temperatures currently used to separate O2 from air on a large scale. At still greater temperatures, a thermal activation barrier to the formation of iron(III)-peroxide species is overcome and desorption of O2 is no longer possible. Efforts are underway to synthesize related metal-organic frameworks with an increased activation barrier for the formation of peroxide, thereby generating a high-capacity O2 separation material that can operate closer to ambient temperatures.
In addition, the efficacy of the new redox-active framework in performing a variety of other gas separations where charge transfer might also lead to selectivity. Additional example separations include, but are not limited to, paraffin/olefin separations, carbon monoxide removal, acetylene storage, and nitric oxide/nitrous oxide separations.
FIG. 9 is a graph showing the separation of a mixture of ethane and ethane. A 50/50 mixture of ethane and ethene is flowed through Fe2(dobdc) at 318 K. The framework adsorbs ethene first, supplying greater than 99.5% purity ethane. After ethene “breaks through” gas feed is turned off to supply greater than 99% purity ethene.
FIG. 10 is a graph showing the separation of a mixture of propane and propene. A 50/50 Mixture of propane and propene is flowed through Fe2(dobdc) at 318 K. The framework adsorbs propene first, supplying greater than 99.5% purity propane. After propene “breaks through” gas feed is turned off to supply greater than 99% purity propene.
To investigate the ability of Fe2(dobdc) to adsorb light hydrocarbons, pure component equilibrium adsorption isotherms for methane, ethane, ethylene, acetylene, propane and propylene were measured at 318, 333, and 353 K. FIG. 30 shows the data obtained at 318 K, with the remaining date presented in FIG. 11. FIGS. 30 (a) and (b) show gas adsorption isotherms for methane, ethane, ethylene, and acetylene (a) and for propane and propylene (b) in Fe2(dobdc) at 318 K. Filled and open circles represent adsorption and desorption data, respectively. The adsorption capacities at 1 bar correspond to 0.77, 5.00, 6.02, 6.89, 5.67, and 6.66 mmol/g, respectively. FIGS. 26 (c) and (d) are experimental breakthrough curves for the adsorption of equimolar ethane/ethylene (c) and propane/propylene (d) mixtures flowing through a 1.5 mL bed of Fe2(dobdc) at 318 K with a total gas flow of 2 mL/minute at atmospheric pressure. After breakthrough of the olefin and return to an equimolar mixture composition, a nitrogen purge was applied, leading to desorption of the olefin. Note that in an actual separation scenario, desorption would instead be carried out by applying a vacuum and/or raising the temperature. As evidenced by the initial steep rise in the isotherms, Fe2(dobdc) displays a strong affinity for the unsaturated hydrocarbons acetylene, ethylene, and propylene. Additionally, the uptake of these gases at 1 bar approaches the stoichiometric quantity expected if one gas molecule is adsorbed per iron (II) center. The propane and ethane adsorption capacities under these conditions, though lower than those of their unsaturated counterparts, are both significantly higher than observed for methane, which has lower polarizability and a smaller kinetic diameter. Importantly, all of the isotherms are completely reversible and exhibit no hysteresis. Further, equilibrium adsorption experiments at 318K (FIG. 12) indicate no loss in olefin uptake capacity after 15 ethylene adsorption/desorption cycles. Additionally, no loss in propylene uptake was observed after 40 adsorption/desorption cycles as verified by thermogravimetric analysis (FIG. 12).
Powder neutron diffraction experiments were carried out to determine the nature of the interactions of these adsorbate molecules within Fe2(dobdc). In a typical experiment, Fe2(dobdc) was dosed with deuterated gas at 100 K and cooled to 4 K for data collection. Rietveld refinements were performed agains these data to provide the structural models presented in FIG. 28. Analogous to the results obtained investigating the coordination of dioxygen to the iron centers of this material, only one adsorption site is apparent. This site corresponds to the open coordination site of the exposed Fe2+ cations, upon dosing sub-stoichiometric equivalents of gas per framework iron. The unsaturated hydrocarbons, acetylene, ethylene, and propylene, display the anticipated side-on binding modes, with Fe—C distances lying in the range 2.42(2) to 2.60(2) Å. These distances are substantially longer than the separations of 2.020(5) to 2.60(2) Å observed for the diamagnetic complex [Fe(C2H4)4]2, one of the very few iron(II)-olefin species to be structurally characterized previously. The difference suggests that the metal centers within Fe2(dobdc) maintain a high-spin electron configuration when binding these gases, consistent with weaker interactions that can be reversed with little energy penalty. The interactions of both ethane and propane with the metal cations in Fe2(dobdc) are weaker, as evidenced by the elongated Fe—C distance of approximately 3 Å. This is in good agreement with the Mg—C distance reported for methane adsorption in Mg2(dobdc), a system in which the metal-adsorbate interactions are also a result of ion-induced dipole interactions between coordinatively-unsaturated metal cations and hydrocarbon deuterium atoms.
The strength of the hydrocarbon binding with Fe2(dobdc) was determined quantitatively through analysis of the gas adsorption data. The data for acetylene, ethylene, ethane, propane, and propylene, expressed in terms of absolute loadings, were fitted with the dual-Langmuir-Freundlich isotherm model, whereas methane adsorption data were fitted with a single-site Langmuir model. Isosteric heats of adsorption were calculated form the fits to compare the binding enthalpies of these gases under various loadings (see FIG. 13). Heats of adsorption for acetylene (−47 kJ/mol), ethylene (−45 kJ/mol), and propylene (−44 kJ/mol) show a significant reduction as the loading approaches the value corresponding to one gas molecule per iron(II) center, again consistent with the exposed metal cations presenting the strongest adsorption sites in the material. Propane (−33 kJ/mol), ethane (−25 kJ/mol), and methane (−20 kJ/mol) adsorption enthalpies are all considerably lower in magnitude, with the trend reflecting the decreasing polarizabilities of these molecules from propane to ethane to methane.
Adsorption selectivities were calculated using ideal adsorbed solution theory (IAST) using the fitted isotherms of the experimental isotherm data for relevant gas mixtures in Fe2(dobdc) and a number of other porous material for which analogous gas uptake properties have been reported (see FIG. 31). FIG. 31 shows calculations of the adsorption selectivity, Sads, using Ideal Adsorbed Solution Theory for ethane/ethylene (upper left), propane/propylene (upper right), acetylene/ethylene (lower left) and acetylene/methane, ethylene/methane, ethane/methane (lower right) in Fe2(dobdc) at 318 K. For the equimolar mixture of ethylene and ethane at 318 K, the adsorption selectivities obtained for Fe2(dobdc) are significantly greater than those calculated for either zeolite NaX or the isostructural metal-organic framework Mg2(dobdc), which display seletvities of 9-14 and 4-7, respectively. The latter result is consistent with the softer character of Fe2+ relative to Mg2+, leading to a stronger interaction with the π electron cloud of the olefin. Similarly, in comparing the performance of Fe2(dobdc) with other porous materials for the separation of a propane/propylene mixture (selectivity=13-15), it is rivaled in selectivity only by zeolite ITQ-12 which displays adsorption selectivity of 15 while the other materials display selectivities from 3-9. Note, however, that the selectivities of ITQ-12 for this mixture were calculated from data collected at 303 K, and it is expected that selectivity of this material will be lower at higher temperatures. Adsorption selectivities were also calculated using LAST for Fe2(dobdc) in an equimolar four-component mixture of methane, ethane, ethylene, and acetylene at 318 K, as relating to the purification of natural gas. For an adsorption-based process operating at 1 bar, the calculated acetylene/methane, ethylene/methane, and ethane/methane selectivities are 700, 300, and 20, respectively. These values are much higher than those recently reported (13.8, 11.1, and 16.6, respectively) for a zinc-based metal-organic framework, also based on an analogous calculation procedure.
To evaluate performance of Fe2(dobdc) in an actual adsorption-based separation process, breakthrough experiments were performed in which an equimolar ethylene/ethane or propylene/propane mixture was flowed over a packed bed of the solid with a total flow of 2 mL per minute at 318 K (see FIG. 32 and FIG. 33). FIG. 32 is curves showing mol % (left) and concentration (right) of propane and propylene during adsorption (upper) and desorption (lower) of a simulated breakthrough experiment. FIG. 29 is curves showing mol % (left) and concentration (right) of ethane and ethylene during adsorption (upper) and desorption (lower) of a simulated breakthrough experiment. In a typical experiment, the gas mixture was flowed through 300 to 400 mg of metal-organic framework crystallites packed into 1.5 mL glass column, and the outlet gas stream was monitored by a gas chromatograph equipped with a flame ionization detector. As expected from the calculated selectivites, in each case, the alkane was first to elute through the bed, while the solid adsorbent retained the olefin. For the C3 hydrocarbons, the outlet gas contained undetectable levels of propylene, resulting in a propane feed that appeared to be 100% pure, within the detection limit of the instrument (˜100 ppm). Upon saturation of the metal centers within the adsorbent, propylene “broke through” and the outlet gas stream then quickly reached equimolar concentrations. By stopping the gas feed and flowing a purge of nitrogen through the bed, the small amount of weakly bound propane remaining in the pores of the framework could be quickly removed, while the iron-bound propylene then desorbed more slowly. Greater than 99% pure propylene was realized during the desorption step of the breakthrough experiment. In a similar manner, breakthrough experiments showed that Fe2(dobdc) can separate an equimolar mixture of ethylene and ethane into the pure component gases of 99% and 99.5% purity.
Although breakthrough experiments are quite valuable for evaluating the gas separation capabilities of a material, in practice they can be difficult and time consuming. In order to compare Fe2(dobdc) with other reported adsorbents for ethylene/ethane and propylene/propane separations, we sought to demonstrate that the breakthrough characteristics could instead be simulated with reasonable accuracy. Assuming that (i) intra-crystalline diffusion is negligible through an isothermal adsorption bed in thermodynamic equilibrium; (ii) plug flow proceeds through the bed; and (iii) the binary mixture adsorption equilibrium in the packed bed of crystallites can be calculated using LAST, we were able to solve a set of partial differential equiations and calculate breakthrough curves for both ethylene/ethane and propylene/propane mixtures. The resulting transient gas composition profiles (see FIG. 16 and FIG. 17) are in excellent agreement with the experimental results shown in FIG. 32 and FIG. 33.
Given this validation, analogous simulations were employed to make quantitative comparisons with other materials. From the simulated breakthrough curves, the time interval during which the exit gas compositions have a purity of 99% propane can be determined, together with the amount of 99% pure propane produced in this time interval. The production capacities, expressed as the amount of propane produced per liter of adsorbent are shown in FIG. 34 over a range of pressures for the zeolites ITQ-12 at 303 K and NaX at 318 K, and for the metal-organic frameworks Cu3(btc)2 (btc3−=1,3,5-benzenetricarboxylate) at 318 K, Cr3(btc)2 at 298 K, and Fe-MIL-100 at 303 K. FIG. 34 (left) is production capacity of 99% pure propane, expressed as mol propane produced per L adsorbent material, as a function of the total pressure at the inlet to the adsorber. The separation characteristics of Fe2(dobdc) at 318 K are compared to that of Mg2(dobdc) (318 K), NaX zeolite (318 K), Cu3(btc)2 (318 K), Cr3(btc)2 (298 K), ITQ-12 (303 K), and Fe-MIL-100 (303 K). (Right) is the production capacity of 99.5% pure propylene, expressed as mol propane produced per L adsorbent material, as a function of the total pressure at the inlet to the adsorber. These results indicate that the propane production capacity of Fe2(dobdc) at 318 K, which ranges up to 5.8 mol/L at a total pressure of 1.0 bar, is at least 20% higher than that of any of these other materials. A similar method was used to calculate the amount of polymer-grade (99.5%+) propylene that can be produced by these materials, again leading to a higher capacity for Fe2(dobdc) than for any other material. The compound Mg2(dobdc) exhibits a lower productivity than Fe2(dobdc), a result of the lower adsorption selectivity of this material. Although zeolite ITQ-12 displayed a comparable selectivity to Fe2(dobdc), its capacity limitation, which stems from its low pore volume of 0.134 cm3/g, results in a propylene productivity that is just 47% of that of the metal-organic framework.
For the separation of ethylene/ethane mixtures, the breakthrough simulations indicate an even greater advantage of Fe2(dobdc) over other adsorbents, with production capacities that are roughly double those of Mg2(dobdc) and zeolite NaX (see FIG. 35). FIG. 35 is production capacities of 99% pure ethane (left), and 99.5% pure ethylene (right), expressed as mol produced per L adsorbent material, as a function of the total pressure at the inlet to the adsorber. The separation characteristics of Fe2(dobdc) at 318 K are compared to that of Mg2(dobdc) (318 K), and NaX zeolite at temperatures of 298 K, and 323 K.
In order to establish the feasibility of using Fe2(dobdc) for the task of selectively separating methane from mixtures including C2 hydrocarbons (ethane, ethylene, and acetylene), breakthrough calculations were carried out for the mixture. The graph on the left of FIG. 36 shows calculated methane, ethane, ethylene, and acetylene breakthrough curves for an equimolar mixture of the gases at 1 bar flowing through a fixed bed of Fe2(dobdc) at 318 K. FIG. 36 presents simulated data on the gas phase molar concentrations exiting an adsorber packed with Fe2(dobdc) and subjected to a feed gas consisting of an equimolar mixture of methane, ethane, ethylene, and acetylene at a total pressure of 1 bar and a temperature of 318 K. Note that the breakthrough times reflect the relative adsorption selectivities (acetylene>ethylene>ethane>methane) for the material, and that the curves indicate a clean, sharp breakthrough transition for each successive gas.
Based on these results, the diagram at the right in FIG. 36 demonstrates how it might be possible to procure pure methane, ethane, ethylene, and acetylene using three packed beds of Fe2(dobdc). The diagram on the right in FIG. 36 shows a schematic representation of the separation of a mixture of methane, ethane, ethylene, and acetylene using just three packed beds of Fe2(dobdc) in a vacuum swing adsorption or temperature swing adsorption process. In this process, a gas mixture is fed into the first bed and methane, the fraction with the lowest adsorptivity, breaks through first. Pure methane can be collected until the second gas, ethane, breaks through. When the third component of the gas stream, ethylene is present in the eluent, the gas flow is diverted to a second bed, from which additional pure methane is collected during the adsorption step, and from which a mixture of ethane and ethylene is subsequently desorbed. This ethane/ethylene mixture is then separated into its pure components using a third adsorbent bed. By halting the feed into the first bed just prior to breakthrough of acetylene, pure acetylene can be obtained via desorption.
The use of Fe2(dobdc) for removal of acetylene from mixtures with ethylene was investigated. FIG. 37 is transient breakthrough of acetylene/ethylene mixture in an adsorber bed packed with Fe2(dobdc). The inlet gas is maintained at partial presses p1=100 kPa, p2=1 kPa, at a temperature of 318 K. Simulated breakthrough characteristics for a feed mixture containing 1 bar of ethylene and 0.01 bar of acetylene at 318 K indicate that final acetylene concentrations on the order of 10 ppm could be realized (see FIG. 37).
Fe2(dobdc) can also be used for carbon monoxide separation. Fe2(dobdc) for the selective adsorption of carbon monoxide from H2, N2, and CH4 was investigated. FIG. 41 shows the Excess adsorption isotherms of CO, CH4, N2, and H2 collected for Fe2(dobdc) at 318 K. Isosteric heat of CO adsorption in Fe2(dobdc) as a function of loading. (inset). Single-component equilibrium adsorption isotherms collected on a sample of Fe2(dobdc) at 318 K (FIG. 41) indicate significantly higher uptake of CO than N2, H2, or CH4 over the entire pressure range measured. The CO isotherm displays a steep rise at low pressure and saturates over 12 wt % at 1 bar, while the other gases measured remain below 1.3 wt % at this pressure. Accordingly, the isosteric heat of CO adsorption (41 kJ/mol) as calculated from fits to isotherms collected at multiple temperatures is significantly higher than N2, H2, and CH4 (35, 10.1, 20 kJ/mol, respectively). The high adsorption enthalpy of carbon monoxide to the Fe2+ centers in Fe2(dobdc) as compared to N2, CH4, and H2 indicate that this material may be used for the adsorptive separation of these gases.
FIG. 38 is a portion of the structure of Fe2(dobdc) showing carbon monoxide (CO) coordinated to the open Fe2+ site. FIG. 39 is an infrared spectrum of Fe2(dobdc) under successively increasing doses of CO. FIG. 40 is low-pressure adsorption of CO, CH4, N2, and H2 in Fe2(dobdc) at 298 K.
Infrared spectroscopy was used to investigate the nature of the interaction between the iron cations in Fe2(dobdc) and adsorbed carbon monoxide. FIG. 42 show the Infrared spectrum of CO adsorbed on Fe2(dobdc) at room temperature. Although infrared spectra for metal-organic frameworks of this structure type have a large number of vibrations at lower frequency, the pertinent region for metal carbonyl stretches is unobscured. Indeed, upon dosing an activated framework sample with CO at room temperature a clear band is evident at 2160 cm−1. With higher CO loading this band intensifies and shifts slightly to 2159 cm−1. At high coverage a number of additional bands appear at 2110, 2125, and 2190 cm−1. The CO band at 2159 cm−1 is assigned to the iron-bound carbonyl species, near the shift that has been previously reported for CO bound to the metal cation centers in Mg2(dobdc) and Ni2(dobdc). While the IR bands seen for these three materials are all blue-shifted relative to the IR stretch of gas phase CO (2143 cm−1), the shift seen for Fe2(dobdc) is red-shifted considerably compared to the Mg and Ni materials. This is likely attributed to the back-bonding from the Fe2+ to the 2π* antibonding orbital of CO weakening the C-0 bond as compared to CO bound to Mg2(dobdc) and Ni2(dobdc).
Powder neutron diffraction experiments were also carried out to crystallographically characterize (Fe—CO)2(dobdc). Desolvated Fe2(dobdc) was dosed with 0.75, and subsequently 1.5, equivalents of CO (per Fe2+) at 300 K and cooled to 4 K for data collection. FIG. 43 show Crystal structures of Fe2(dobdc) with adsorbed N2, CO, or D2. Carbon, iron, oxygen, nitrogen, and deuterium atoms are shown. At sub-stoichiometic CO loadings only one adsorption site is apparent, with an occupancy of 0.84(1). Consistent with infrared spectroscopy and gas adsorption experiments the strongest binding site is the unsaturated iron cation center. Carbon monoxide binds to the iron center end on at a Fe—C distance of 2.22(2) Å. The C-0 distance for this complex of 1.11(2) is slightly shorter than that of free CO (1.127) consistent with the corresponding blue shift seen via IR. CO forms a nearly linear adduct with a Fe—C—O angle of 172.6(1)°. At the higher CO loading of 1.5 per Fe2+ the first binding site saturates at an occupancy of 0.96(2) and a second site is apparent in which CO is parallel to the pore wall at a distance of 3.3-3.6 Å and an occupancy of 0.44(2).
Finally, given its clear ability to activate O2, Fe2(dobdc) can be employed as a catalyst for the oxidation of hydrocarbons. For example, Fe2(dobdc) reacts rapidly in air to produce either Fe2(O2)2(dobdc) (low temperature) or Fe2(O2)(dobdc) (room temperature) both of which contain reactive oxygen, either as superoxide in the former or peroxide in the latter. The large pore volume, high surface areas, accessible metal centers, and thermally stable nature of both of these resulting materials make them very promising oxidation catalysts. Although work with a number of systems, including the oxidation of methane to methanol and the oxidation of ethane/ethane and propane/propene. A representative reaction is shown in FIG. 49.
Fe2(dobdc) catalyzes the oxidation of propylene to acetone with air as the oxidant. Although the yield of the reaction under current conditions is low the selectivity is approximately 100%. Examples of other reactions that may be chaptalized are shown below in FIG. 50.
Liquid-phase Hydrocarbon Oxidation Using Fe2 (dobdc). In molecular Fe-oxo chemistry, N-oxides, peroxides, and hypervalent iodine-based O-atom transfer reagents are often used as sacrificial oxidants to generate the reactive Fe species from initial FeII complexes. Fe2(dobdc) was examined for liquid-phase C—H activation studies involving O-atom transfer reagents. While only limited reactivity was observed using pyridine-N-oxide and iodosylbenzene, upon addition of a solution of 2-(tert-butylsulfonyl)iodosylbenzene (tBuSO2PhIO) (5 equiv.) and excess 1,4-cyclohexadiene (1,4-CHD) (24 equiv.) in CD3CN to the acetonitrile-solvated framework production of benzene (70% conversion based on iodosylarene) was observed (FIG. 1). A control experiment in which no metal-organic framework was added led to less than 3% benzene conversion. In addition, preliminary reactivity studies show that the framework is also capable of facilitating the room temperature conversion of toluene to benzyl alcohol/benzaldehyde and cyclohexane to cyclohexanol/cyclohexanone, albeit in low yields (<10% and <3%, respectively) with modest alcohol:ketone selectivities (3.5:1 and 4:1, respectively). Despite low yields and selectivities, these preliminary experiments provide indirect evidence that the oxidized iron framework is a strong oxidant, capable of functionalizing even the C—H bonds of cyclohexane (BDE=99.3 kcal/mol).
Gas-phase Oxidation of Fe2(dobdc). Using a fully desolvated framework and a gaseous oxidizing agent without C—H bonds would circumvent any possible side-reactions such as H-atom abstraction. For this reason, we examined the gas phase oxidation of Fe2(dobdc) with oxidants such as N2O or O2. The reactivity of Fe2(dobdc) sample oxidized with a gas phase oxidant was probed using 1,4-CHD. After addition of neat, excess 1,4-CHD, the framework gradually changed color from dark red brown to light yellow (similar in color to the methanol-solvated framework). Benzene was formed in 40% yield, demonstrating that the framework is capable of C—H activation.
Catalytic Oxidation of 1,4-Cyclohexadiene by Fe2(dobdc). Fe2(dobdc) was added to a stirring solution of excess 1,4-cyclohexadiene and 2-(tert-butylsulfonyl)iodosylbenzene in CD3CN. 1,2,4,5-tetramethylbenzene was added as an internal standard. The reaction mixture was stirred overnight at room temperature, filtered, and washed with 1 mL of CD3CN. Reduction of the iodosylarene to 2-(tert-butylsulfonyl)iodobenzene (quantitative) and formation of benzene (70% yield, assuming 1 equiv of iodosylarene consumed leads to 1 equiv of benzene produced) was detected by 1H NMR. A 1H NMR of 1,4-cyclohexadiene was taken to quantify the amount of benzene in the starting material (1.3%). An identical control reaction run without Fe2(dobdc) was also performed, leading to ˜3% conversion by 1H NMR. FIG. 44 shows the 1H NMR of products of the reaction of Fe2(dobdc) with excess 1,4-cyclohexadiene in CD3CN.
This application discloses several numerical ranges in the text and figures. The numerical ranges disclosed inherently support any range or value within the disclosed numerical ranges even though a precise range limitation is not stated verbatim in the specification because this invention can be practiced throughout the disclosed numerical ranges.
The above description is presented to enable a person skilled in the art to make and use the invention, and is provided in the context of a particular application and its requirements. Various modifications to the preferred embodiments will be readily apparent to those skilled in the art, and the generic principles defined herein may be applied to other embodiments and applications without departing from the spirit and scope of the invention. Thus, this invention is not intended to be limited to the embodiments shown, but is to be accorded the widest scope consistent with the principles and features disclosed herein. Finally, the entire disclosure of the patents and publications referred in this application are hereby incorporated herein by reference.
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Patent Application
20130053585
