Metal-organic framework from an anthracene derivative containing nanoscopic cages exhibiting high methane uptake

Article abstract of DOI:10.1021/ja0771639

A microporous metal-organic framework, PCN-14, based on an anthracene derivative, 5,5′-(9,10-anthracenediyl)di-isophthalate (H₄adip), was synthesized under solvothermal reaction conditions. X-ray single crystal analysis revealed that PCN-14 con

Full text of DOI:10.1021/ja0771639

Published on Web 12/29/2007
Metal-Organic Framework from an Anthracene Derivative
Containing Nanoscopic Cages Exhibiting High Methane
Uptake
Shengqian Ma,† Daofeng Sun,† Jason M. Simmons,‡,§ Christopher D. Collier,†
Daqiang Yuan,† and Hong-Cai Zhou*,†
Department of Chemistry and Biochemistry, Miami UniVersity, Oxford, Ohio, 45056,
NIST Center for Neutron Research, National Institute of Standards and Technology,
Gaithersburg, Maryland 20899-6102, and Department of Materials Science and Engineering,
UniVersity of PennsylVania, Philadelphia, PennsylVania 19104
Received September 18, 2007; E-mail: zhouh@muohio.edu
Abstract: A microporous metal-organic framework, PCN-14, based on an anthracene derivative, 5,5′-
(9,10-anthracenediyl)di-isophthalate (H4adip), was synthesized under solvothermal reaction conditions. X-ray
single crystal analysis revealed that PCN-14 consists of nanoscopic cages suitable for gas storage.
N2-adsorption studies of PCN-14 at 77 K reveal a Langmuir surface area of 2176 m2/g and a pore volume
of 0.87 cm3/g. Methane adsorption studies at 290 K and 35 bar show that PCN-14 exhibits an absolute
methane-adsorption capacity of 230 v/v, 28% higher than the DOE target (180 v/v) for methane storage.
1. Introduction
research in the past decade due to their interesting structures
and various potential applications.8 In particular, their excep-
tionally high surface areas,9 uniform but tunable pore sizes,10
and functionalizable pore walls11 make MOFs suitable for
methane storage and a number of other applications. Several
Ongoing efforts have been made in the search for alternative
fuels to supplement or replace widely used gasoline and diesel
fuels in vehicular applications. Among various alternative fuels,
methane stands out when its profusion and availability are
considered.1 However, the lack of an effective, economic, and
safe on-board storage system is one of the major technical
barriers preventing methane-driven automobiles from competing
with the traditional ones. To promote the vehicular application
of methane, the U.S. Department of Energy (DOE) has set the
target for methane storage at 180 v(STP)/v (standard temperature
and pressure equivalent volume of methane per volume of the
adsorbent material) under 35 bar, near ambient temperature, with
the energy density of adsorbed natural gas (ANG) being
comparable to that of compressed natural gas (CNG) used in
current practice.2
(7) (a) Eddaoudi, M.; Moler, D. B.; Li, H.; Chen, B.; Reineke, T. M.; O’Keeffe,
M.; Yaghi, O. M. Acc. Chem. Res. 2001, 34, 319. (b) Janiak, C. J. Chem.
Soc., Dalton Trans. 2003, 2781. (c) Rowsell, J. L. C.; Yaghi, O. M.
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Champness, N. R.; Hubberstey, P.; Schro¨der, M. Acc. Chem. Res. 2005,
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Nature 2000, 404, 982. (b) Rowsell, J. L. C.; Yaghi, O. M. Angew. Chem.,
Int. Ed. 2005, 44, 4670. (c) Matsuda, R.; Kitaura, R.; Kitagawa, S.; Kubota,
Y.; Belosludov, R. V.; Kobayashi, T. C.; Sakamoto, H.; Chiba, T.; Takata,
M.; Kawazoe, Y.; Mita, Y. Nature 2005, 436, 238. (d) Sun, D.; Ma, S.;
Ke, Y.; Petersen, T. M.; Zhou, H.-C. Chem. Commun. 2005, 2663. (e) Sun,
D.; Ke, Y.; Mattox, T. M.; Ooro, B. A.; Zhou. H.-C. Chem. Commun. 2005,
5447. (f) Sun, D.; Ma, S.; Ke, Y.; Collins, D. J.; Zhou, H.-C. J. Am. Chem.
Soc. 2006, 128, 3896. (g) Ma, S.; Zhou, H.-C. J. Am. Chem. Soc. 2006,
128, 11734. (h) Ma, S.; Sun, D.; Ambrogio, M. W.; Fillinger, J. A.; Parkin,
S.; Zhou, H.-C. J. Am. Chem. Soc. 2007, 129, 1858. (i) Sun, D.; Ke, Y.;
Mattox, T. M.; Parkin, S.; Zhou. H.-C. Inorg. Chem. 2006, 45, 7566. (j)
Sun, D.; Collins, D. J.; Ke, Y.; Zuo, J.-L.; Zhou. H.-C. Chem.-Eur. J.
2006, 12, 3768. (k) Ma, S.; Wang, X.-S.; Manis, E. S.; Collier, C. D.;
Zhou, H.-C. Inorg. Chem., 2007, 46, 3432. (l) Ma, S.; Sun, D.; Wang,
X.-S.; Zhou, H.-C. Angew. Chem., Int. Ed. 2007, 46, 2458. (m) Collins, D.
J.; Zhou, H.-C. J. Mater. Chem. 2007, 17, 3154. (n) Yu, C.; Ma, S.; Pechan,
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Several types of porous materials including single-walled
carbon nanotubes,3 zeolites,4 and activated carbon5 have been
extensively tested and evaluated as potential storage media for
methane. However, the DOE targets for methane storage re-
main illusive despite significant progress in activated carbon
materials.6
Emerging as a new type of porous materials, metal-organic
frameworks (MOFs)7 have become a burgeoning field of
(9) (a) Chae, H. K.; Siberio-Perez, D. Y.; Kim, J.; Go, Y. B.; Eddaoudi, M.;
Matzger, A. J.; O’Keeffe, M.; Yaghi, O. M. Nature 2004, 427, 523. (b)
Ferey, G.; Mellot-Draznieks, C.; Serre, C.; Millange, F.; Dutour, J.; Surble,
S.; Margiolaki, I. Science 2005, 309, 2040.
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Yaghi, O. M. Science 2002, 295, 469. (b) Chen, B.; Ma, S.; Zapata, F.;
Lobkovsky, E. B.; Yang, J. Inorg. Chem. 2006, 45, 5718. (c) Chen, B.;
Ma, S.; Zapata, F.; Fronczek, F. R.; Lobkovsky, E. B.; Zhou, H.-C. Inorg.
Chem. 2007, 46, 1233.
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2334. (b) Wang, X.-S.; Ma, S.; Sun, D.; Parkin, S.; Zhou, H.-C. J. Am.
Chem. Soc. 2006, 128, 16474. (c) Bradshaw, D.; Claridge, J. B.; Cussen,
E. J.; Prior, T. J.; Rosseinsky, M. J. Acc. Chem. Res. 2005, 38, 273.
† Miami University.
‡ National Institute of Standards and Technology.
§ University of Pennsylvania.
(1) U.S. Energy Policy Act of 1992 (EPAct).
(2) Burchell, T; Rogers, M. SAE Tech. Pap. Ser. 2000, 2000-01-2205.
(3) Muris, M.; Dupont-Pavlovsky, N.; Bienfait, M.; Zeppenfeld, P. Surf. Sci.
2001, 492, 67.
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9
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10.1021/ja0771639 CCC: $40.75 © 2008 American Chemical Society

Methane Storage in MOF
A R T I C L E S
Scheme 1. Carboxylate Linkers
for 30 min and 80 mL degassed THF was added. After the addition of
15 mL degassed 2 M Na2CO3 solution, the mixture was heated to reflux
under nitrogen atmosphere for 40 h. The resulting yellow mixture was
diluted with water and extracted with CH2Cl2 three times. The mixed
organic phase was dried with MgSO4, and the solvent was removed to
give a brown solid. The crude product was purified by column
chromatography on silica gel with CHCl3 as the eluent to give 1 as a
yellow solid (0.6 g, 53%). 1H NMR (CDCl3): δ ) 8.9 (s, 2 H), 8.5 (s,
4 H), 7.6 (d, 4 H), 7.4 (m, 4 H), 4.0 (s, 12 H).
Synthesis of H4adip, 5,5′-(9,10-Anthracenediyl)di-isophthalic
Acid, 2. Compound 1 (0.6 g, 0.001 mol) was suspended in 50 mL of
THF, to which 10 mL of a 2 M KOH aqueous solution was added.
The mixture was stirred at room temperature overnight. THF was
removed using a rotary evaporator, and diluted hydrochloric acid was
added to the remaining aqueous solution until it became acidic. The
solid was collected by filtration, washed with water several times, and
porous MOFs have been screened for methane storage but none
have reached the DOE target.10a,12 A recent computational study
indicated that aromatic rings in MOFs can improve the methane-
binding energy, enhancing both the uptake and the heat of
methane-adsorption.13
Recently, a theoretically proposed MOF (IRMOF-993) based
on 9,10-anthracene-dicarboxylate (adc) (Scheme 1) was pre-
dicted to have a methane adsorption capacity of 181 v(STP)/v,
surpassing the DOE target.13 However, experiments in our
laboratory using 9,10-anthracene-dicarboxylate have led to an
ultramicroporous MOF (PCN-13, PCN stands for Porous
Coordination Network) with very limited methane uptake (see
Supporting Information Figure S1). Instead, PCN-13 exhibits
selective adsorption of hydrogen and oxygen over nitrogen and
carbon monoxide because of the confined pore size (∼3.5 Å).14
To enlarge the pore size and to continue our theme of building
metal-organic frameworks containing nanoscopic coordination
cages for gas storage,8f,g,h we have adopted a new ligand, 5,5′-
(9,10-anthracenediyl)di-isophthalate (adip, Scheme 1). Under
solvothermal reaction conditions, the reaction between H4adip
and Cu(NO3)2 gave rise to a porous MOF designated PCN-14.
In this contribution, we describe the synthesis and characteriza-
tion of H4adip and PCN-14 and the methane-adsorption studies
of the MOF.
1
dried to give 2 (0.4 g, 80%). H NMR (CDCl3): δ ) 13.5 (br, 4 H),
8.7 (s, 2 H), 8.2 (s, 4 H), 7.5 (m, 8 H).
Synthesis of PCN-14, Cu2(H2O)2(adip)‚2DMF. A mixture of 2
(0.005 g, 1.4 × 10-5 mol), Cu(NO3)2‚2.5H2O (0.02 g, 8.2 × 10-6 mol),
and 2 drops of HBF4 in 1.5 mL DMF was sealed in a Pyrex tube under
vacuum and heated to 75 °C at a rate of 1 °C/min, kept at that
temperature for 1 day, and cooled to room temperature at a rate of 0.1
°C/min. The resulting green block crystals were washed with DMF
(yield: 75% based on 2) and has a formula of Cu2(H2O)2(adip)‚2DMF,
which was derived from crystallographic data, elemental analysis
(calcd: C, 49.94; H, 4.42; N, 3.24. Found: C, 51.03; H, 4.54; N,
3.15%.), and TGA (Figure S2, Supporting Information).
X-ray Crystallography. Single-crystal X-ray structure determination
of PCN-14 was performed on a specially configured diffractometer
based on the Bruker-Nonius X8 Proteum using focused Cu-KR
radiation (λ ) 1.54178 Å). Raw data for all structures were processed
using SAINT and absorption corrections were applied using SADABS.16
The structures were solved by direct method and refined by full-matrix
least-squares on F2 with anisotropic displacement parameters for non-H
atoms using SHELX-97.17 The hydrogen atoms on the carbon were
placed in calculated position with isotropic displacement parameters
set to 1.2 × Ueq of the attached atom. Solvent molecules in the structure
were highly disordered and were impossible to refine using conventional
discrete-atom models. To resolve these issues, the contribution of
solvent electron density was removed by the SQUEEZE routine in
PLATON.18
2. Experimental Section
General Information. Commercially available reagents were used
as received without further purification. Elemental analyses (C, H, and
N) were obtained by Canadian Microanalytical Service Ltd.15 TGA was
performed under N2 on a Perkin-Elmer TGA 7 and a Beckman Coulter
SA3100 surface area analyzer was used to measure gas adsorption.
NMR data were collected on a Bruker 300 MHz spectrometer. XRPD
patterns were obtained on a Scintag X1 powder diffractometer system
using CuKR radiation with a variable divergent slit, solid-state detector,
and a routine power of 1400 W (40 kV, 35 mA). Powder samples were
dispersed on low-background quartz XRD slides (Gem Depot, Inc.,
Pittsburgh, Pennsylvania) for analyses.
Low-Pressure Nitrogen Sorption Measurements. The low-pressure
nitrogen adsorption measurements were performed at 77 K and 0-760
Torr on a Beckman Coulter SA 3100 surface area and pore size
analyzer. An as-isolated sample of PCN-14 was immersed in methanol
for 24 h, and the extract was decanted. Fresh methanol was subsequently
added, and the crystals were allowed to stay for an additional 24 h to
remove the nonvolatile solvates (DMF and H2O). The sample was
collected by decanting and treated with dichloromethane similarly to
remove methanol solvates. After the removal of dichloromethane by
decanting, the sample was dried under a dynamic vacuum (<10-3 Torr)
at room temperature (25 °C) overnight. Before the measurement, the
sample was dried again by using the “outgas” function of the surface
area analyzer for 4 h at 120 °C. High purity nitrogen (99.999%) was
used for the measurement. The regulator and pipe were flushed with
nitrogen before connecting to the analyzer. The internal lines of the
instrument were flushed three times by utilizing the “flushing lines”
function of the program to ensure the purity of N2.
Synthesis of 5,5′-(9,10-Anthracenediyl)bis(1,3-benzenedimethoxy-
carbonyl), 1. Anthracene 9,10-diboronic acid (0.5 g, 0.002 mol),
dimethyl-5-bromo-isophtalate (1.7 g, 0.006 mol) and Pd(PPh3)4 (0.02
g) were mixed in a 500 mL flask. The flask was pumped under vacuum
(12) (a) Noro, S.-i.; Kitagawa, S.; Kondo, M.; Seki, K. Angew. Chem., Int. Ed.
2000, 39, 1433. (b) Kondo, M.; Shimamura, M.; Noro, S.-i.; Minakoshi,
S.; Asami, A.; Seki, K.; Kitagawa, S. Chem. Mater. 2000, 12, 1288. (c)
Kesanli, B.; Cui, Y.; Smith Milton, R.; Bittner Edward, W.; Bockrath
Bradley, C.; Lin, W. Angew. Chem., Int. Ed. 2005, 44, 72. (d) Bourrelly,
S.; Llewellyn, P. L.; Serre, C.; Millange, F.; Loiseau, T.; Ferey, G. J. Am.
Chem. Soc. 2005, 127, 13519.
(13) Dueren, T.; Sarkisov, L.; Yaghi, O. M.; Snurr, R. Q. Langmuir 2004, 20,
2683.
(14) Ma, S.; Wang, X.-S.; Collier, C. D.; Manis, E. S.; Zhou, H.-C. Inorg. Chem.
2007, 46, 8499.
(15) Note: Certain commercial suppliers are identified in this paper to foster
understanding. Such identification does not imply recommendation or
endorsement by the National Institute of Standards and Technology, nor
does it imply that the materials or equipment identified are necessarily the
best available for the purpose.
High-Pressure Methane Sorption Measurements. High-pressure
methane sorption isotherm measurements on PCN-14 were performed
(16) SAINT+, version 6.22; Bruker Analytical X-Ray Systems, Inc.: Madison,
WI, 2001.
(17) Sheldrick, G. M. SHELX-97; Bruker Analytical X-Ray Systems, Inc.:
Madison, WI, 1997.
(18) Spek, A. L. J. Appl. Crystallogr. 2003, 36, 7.
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A R T I C L E S
Ma et al.
Figure 1. (a) Squashed cuboctahedral cage; (b) nanoscopic cage with 18 vertices, 30 edges, and 20 faces. Color scheme: C, gray; Cu, turquoise; and O,
red.
using a home-built fully computer-controlled Sievert apparatus at NIST.
The methane used for the high pressure measurements is scientific/
research grade with the purity of 99.999%. The detailed specification
of the Sievert apparatus and the data analysis can be found in a recently
published work.19 Briefly, the Sievert system is equipped with four
high-precision gauges (0.1%) and a closed-cycle cryostat, enabling
methane-adsorption measurements over a wide pressure (0-50 bar)
and temperature (125-290 K) range. In all measurements, about 200
mg solvent-exchanged sample was used, which was activated under
vacuum (less than 10-4 Torr) in two stages: first heating at room
temperature overnight, and then at 120 °C for at least 4 h. Once
activated, the samples were transferred to He-glove box and never
exposed to air.
Excess Adsorption and Absolute Adsorption. Details of excess
adsorption and absolute adsorption have been described in a recently
published work19 as well as in some other published work.20 In brief,
the capacity of excess adsorption is the amount of adsorption gas
interacting with the frameworks, whereas the capacity of absolute
adsorption is the amount of gas both interacting with the frameworks
and staying in pores in the absence of gas-solid intermolecular forces.
For systems with known crystal structure, it is possible to directly
measure the absolute adsorption in addition to excess adsorption.
and the adip ligand. In the ligand, the four carboxylate groups
and the two phenyl rings of the isophthalate motifs are almost
in a plane, whereas the dihedral angle between the anthracene
ring and the phenyl rings is 70.4°. Every 12 adip ligands connect
6 paddlewheel SBUs to form a squashed cuboctahedral cage
(Figure 1a), if one connects the centers of the six paddlewheels
and the six anthracenyl groups (broken lines in Figure 1a). The
anthracenyl rings in the cage are in close contact (2.6 Å between
an H atom and the center of a phenyl ring from the adjacent
anthracenyl group). The cuboctahedral cage has eight triangular
windows and six square windows for gas molecules to access
the interior surface. The cuboctahedral cage can also be viewed
as four intersecting hexagons. The dimensions of the hexagons
are 9.23 Å along an edge and 18.45 between two opposite
corners. Extending each hexagon in the cuboctahedral cage into
two-dimensional honeycombs gives rise to a three-dimensional
4-connected net (Figure 2). The three-dimensional net can also
be viewed as a framework consisting of cuboctahedral nano-
scopic cages (Figure 3a). An alternative way of viewing the
cage is to connect the centers of all isophthalate phenyl rings,
forming a polygon with 18 vertices, 20 faces, and 30 edges.
This polygon can be viewed as being formed by inserting an
irregular hexagonal prism in between the two halves of a
cuboctahedron (Figure 1b). The cage has 1150 Å3 of void and
is approximately spherical providing efficient and accessible
interior surface for gas storage.
3. Results and Discussion
Structural Descriptions of PCN-14. Single-crystal X-ray
diffraction21 revealed that PCN-14 crystallizes in the space group
R-3c, different from those of previously reported [Cu2L(H2O)2]
MOFs (L ) biphenyl-3,3′5,5′-tetracarboxylate, terphenyl-
3,3′′,5,5′′-tetracarboxylate, or quaterphenyl-3,3′′′,5,5′′′-tetracar-
boxylate),22 which all crystallize in R-3m space group. PCN-
14 consists of a dicopper paddlewheel secondary building unit
PCN-14 is very porous (Figure 3b). The solvent accessible
volume for the desolvated PCN-14 is 63.5%, calculated using
the PLATON routine,18 comparable to those of other MOFs
based on isophthalate derivitives.22a
Low-Pressure Nitrogen Sorption. A PCN-14 sample was
fully activated by the procedure described above in the
experimental section. The integrity of the framework was
confirmed by powder X-ray diffraction (PXRD) before the
nitrogen sorption measurements (Figure S3, Supporting Infor-
mation). Nitrogen sorption isotherms of the fully activated PCN-
14 sample (Figure 4) reveals typical Type-I sorption behavior,
confirming the permanent porosity of the activated PCN-14.
Calculated from the nitrogen adsorption data, the estimated BET
(19) Zhou, W.; Wu, H.; Hartman, M. R.; Yildirim, T. J. Phys. Chem. C. 2007,
111, 16131.
(20) (a) Dincaˇ, M.; Dailly, A.; Liu, Y.; Brown, C. M.; Neumann, D. A.; Long,
J. R. J. Am. Chem. Soc. 2006, 128, 16876. (b) Furukawa, H.; Miller, M.
A.; Yaghi, O. M. J. Mater. Chem. 2007, 17, 3197.
(21) X-ray crystal data for PCN-14: C270H162Cu18O90, fw ) 5989.9, Rhombo-
hedral, R-3c, a ) 18.4530 (4) Å, b ) 18.4530 (4) Å, c ) 76.976(4) Å, V
) 22699.7(1) Å3, Z ) 2, T ) 90 K, Fcalcd ) 0.871 g/cm3, R1 ( I > 2σ(I))
) 0.0518, wR2 (all data) ) 0.1591, GOOF ) 1.071.
(22) (a) Chen, B. L.; Ockwig, N. W.; Millward, A. R.; Contreras, D. S.; Yaghi,
O. M. Angew. Chem., Int. Ed. 2005, 44, 4745. (b) Lin, X.; Jia, J. H.; Zhao,
X. B.; Thomas, K. M.; Blake, A. J.; Walker, G. S.; Champness, N. R.;
Hubberstey, P. Schro¨der, M. Angew. Chem., Int. Ed. 2006, 45, 7358.
9
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Methane Storage in MOF
A R T I C L E S
Figure 2. 3D framework of PCN-14 viewed from the (a) [2 1 1] and (b) [1 0 0] directions.
Figure 3. 3D framework of PCN-14 viewed as a (a) cuboctahedral net and (b) space filling model on the [1 0 3] plane.
absolute adsorption decrease with increasing temperatures. The
saturation of excess methane adsorption in PCN-14 at 125 K
can reach 434 v(STP)/v, which corresponds to an adsorbed
methane density of 310 mg/mL. The density is 73.4% of that
of liquid methane (422.6 mg/mL) at 113 K.24 At 290 K and 35
bar, the excess adsorption capacity of methane in PCN-14 is
220 v(STP)/v, corresponding to an absolute adsorption capacity
of 230 v(STP)/v. The excess methane adsorption value is 22%
higher than the DOE target of 180 v(STP)/v for methane.2 To
the best of our knowledge, PCN-14 exhibits the highest methane
uptake capacity among reported porous materials for methane
adsorption.12,13
Figure 4. Nitrogen gas adsorption isotherm at 77 K.
surface area of PCN-14 is 1753 m2/g,23 and the estimated pore
volume is 0.87 cm3/g. These values are slightly higher than those
of MOF-505 but lower than those of the two other MOFs using
isophthalate derivatives.22 Assuming monolayer coverage, PCN-
14 has an estimated Langmuir surface area of 2176 m2/g.
High-Pressure Methane Sorption. High-pressure methane
sorption measurements were performed at various temperatures
to investigate the methane uptake. The methane uptake capacities
were converted directly into v(STP)/v by using the crystal-
lographic density of PCN-14 (0.871 g/cm3). As shown in Figure
5, the methane saturation uptake of both excess adsorption and
Analysis of Heat of Adsorption. The strength of interactions
between the framework and methane can be reflected by
isosteric heats of adsorption Qst. The isosteric heats of adsorption
of methane were calculated using the Clausius-Clapeyron
equation,25
Qst ) -R*d(ln P)/d(1/T)
using isotherms taken at 270, 280, and 290 K. As shown in
(24) Lide, D. R. Handbook of Chemistry and Physics, 73rd ed.; CRC Press,
Inc.: Boca Raton, FL, 1992.
(25) Roquerol, F.; Rouquerol, J.; Sing, K. Adsorption by Powders and Solids:
Principles, Methodology, and Applications; Academic Press: London, 1999.
(23) Walton, K. S.; Snurr, R. Q. J. Am. Chem. Soc. 2007, 129, 8552.
9
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A R T I C L E S
Ma et al.
Figure 6. Isosteric heats of adsorption of methane.
that adding more aromatic rings to the ligand and incorporating
nanoscopic cages to the framework can lead to higher affinity
of methane.13
4. Conclusions
In summary, a microporous MOF, PCN-14, based on a
predesigned anthacene derivative, 5,5′-(9,10-anthracenediyl)-
di-isophthalate, was synthesized and structurally characterized.
It contains nanoscopic cages suitable for methane uptake. N2
adsorption measurements of PCN-14 at 77 K reveal an estimated
Langmuir surface area of 2176 m2/g and an estimated pore
volume of 0.87 cm3/g. High-pressure methane adsorption studies
show that PCN-14 exhibits an absolute methane-adsorption
capacity of 230 v/v (28% higher than the DOE target of 180
v/v at ambient temperatures) and heats of adsorption of methane
of around 30 kJ/mol, both record highs among those reported
for methane-storage materials.
Acknowledgment. This work was supported by the Depart-
ment of Energy (DE-FC36-07GO17033) and the National
Science Foundation (CHE-0449634). H.-C.Z. acknowledges Dr.
Sean Parkin (the University of Kentucky) for single-crystal data
collection and structure refinement of PCN-14, the Research
Corporation for a Cottrell Scholar Award, and Air Products for
a Faculty Excellence Award. J.M.S. also acknowledges support
from DOE (BES DE-FG02-98ER45701).
Figure 5. High-pressure methane sorption isotherms at various temperatures
(a) excess adsorption; (b) absolute adsorption.
Figure 6, the Qst at low loading is as high as 30 kJ/mol, revealing
strong interactions between methane and the framework. The
Qst first slowly decreases and then increases gradually with the
methane loading. This indicates that at high-concentration
methane loading, the methane-methane interaction in addition
to the methane-framework interaction becomes dominant as
discovered in other MOFs systems.8g,19 The high Qst of PCN-
14 is unprecedented in MOFs8g,12 and supports the predictions
Supporting Information Available: Crystallographic infor-
mation file (CIF) of PCN-14, a TGA plot, and XPRD patterns
are available free of charge via the Internet at http://pubs.acs.org.
JA0771639
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