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Article

Crystallography of Representative MOFs Based on Pillared Cyanonickelate (PICNIC) Architecture

by
Winnie Wong-Ng
1,*,
Jeffrey T. Culp
2,3 and
Yu-Sheng Chen
4
1
Materials Measurement Science Division, National Institute of Standards and Technology, Gaithersburg, MD 20899, USA
2
National Energy Technology Laboratory, United States Department of Energy, P.O. Box 10940, Pittsburgh, PA 15236, USA
3
AECOM, South Park, PA 15219, USA
4
ChemMatCARS, University of Chicago, Argonne, IL 60439, USA
*
Author to whom correspondence should be addressed.
Crystals 2016, 6(9), 108; https://doi.org/10.3390/cryst6090108
Submission received: 2 July 2016 / Revised: 18 August 2016 / Accepted: 22 August 2016 / Published: 5 September 2016
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Abstract

:
The pillared layer motif is a commonly used route to porous coordination polymers or metal organic frameworks (MOFs). Materials based on the pillared cyano-bridged architecture, [Ni’(L)Ni(CN)4]n (L = pillar organic ligands), also known as PICNICs, have been shown to be especially diverse where pore size and pore functionality can be varied by the choice of pillar organic ligand. In addition, a number of PICNICs form soft porous structures that show reversible structure transitions during the adsorption and desorption of guests. The structural flexibility in these materials can be affected by relatively minor differences in ligand design, and the physical driving force for variations in host-guest behavior in these materials is still not known. One key to understanding this diversity is a detailed investigation of the crystal structures of both rigid and flexible PICNIC derivatives. This article gives a brief review of flexible MOFs. It also reports the crystal structures of five PICNICS from our laboratories including three 3-D porous frameworks (Ni-Bpene, NI-BpyMe, Ni-BpyNH2), one 2-D layer (Ni-Bpy), and one 1-D chain (Ni-Naph) compound. The sorption data of BpyMe for CO2, CH4 and N2 is described. The important role of NH3 (from the solvent of crystallization) as blocking ligands which prevent the polymerization of the 1-D chains and 2-D layers to become 3D porous frameworks in the Ni-Bpy and Ni-Naph compounds is also addressed.

Graphical Abstract

1. Introduction

The continual rise in anthropogenic CO2 concentration since the dawn of the Industrial Revolution and its effect on climate change underlie the urgent need for the implementation of carbon mitigation approaches to stabilize the CO2 concentration in the atmosphere, which would result in a more sustainable global development [1,2,3]. Given the existing availability and usage of fossil fuel resources worldwide, particularly coal, fossil fuel-based energy sources are expected to remain the predominant source of energy in the foreseeable future.
Over the past twenty years, a great number of possible solid sorbents have been reported throughout the literature. Porous materials which offer a wide range of compositions and structures suitable for adsorption and capture of CO2 [4] near atmospheric pressure and over various temperature ranges include zeolites [5,6], activated carbon [7], smectites [8], oxide materials such as calcium oxide [9], lithium zirconates [10], and hydrotalcites [11]. There are also a vast number of reported metal organic frameworks (MOFs) or coordination polymer compounds [12,13,14,15,16,17,18,19,20,21,22,23,24,25,26,27,28,29,30,31,32,33,34,35,36,37,38,39,40,41,42,43,44,45] which show diverse properties for reversible CO2 adsorption over a range of pressure and temperature.
MOFs consist of metal centers and/or metal clusters connected by organic linkers, forming 3-D porous structures with 1-D, 2-D, or 3-D channel systems. The field of MOF research has been rapidly expanding in the past decade. According to Zhou and Kitagawa [12], the surge of MOF research in recent years has been due to five factors: (1) advances in cluster chemistry; (2) maturation of organic synthesis (ligand design and post-synthetic modification on linkers); (3) improvements for evaluation of sorption and structural properties; (4) interdisciplinary growth of MOFs, and (5) their expanding potential in applications.
The goals of this article are to give a brief description of flexible MOFs, with emphasis on the flexible PICNICs, and to discuss the crystallography of flexible and rigid PICNICs based on our recent crystallographic investigations on five Ni(CN)4-based compounds. A gas sorption study of a selected compound is also included.

1.1. Flexible Metal Organic Frameworks (MOFs)

Studies of flexible coordination polymers have been pioneered by Professor Kitagawa’s group at Kyoto University [46,47,48,49]. Since 1990, they have synthesized a great number of porous coordination polymers, providing a variety of properties. In their 2005 papers [47,48], they named the inorganic porous coordination polymers that are structurally flexible and possess selective adsorption characteristics along with the potential to withstand greater external stress than the third-generation coordination polymers (or MOFs). The features of the third-generation MOFs include their unique ability to undergo structural changes (with cell changes) during adsorption and desorption of guests between a closed (minimal porosity) and an open (high porosity) structure. These materials undergo reversible structural changes in response to external stimuli such as a guest inclusion.
Flexible MOFs open up an exciting new research area for the investigation of structure-property relationships in materials science. The flexible behavior in these materials occurs through several different mechanisms [50]. One type of flexible MOF occurs in multi-interpenetrating frameworks, wherein one framework shifts with respect to the others, thereby closing or opening the pores [41,42,43]. Another type of flexible MOF has flexible frameworks from adaptable supports [44,45], such as guest-host interactions that lead to very large swelling or breathe under external stimuli including temperature, pressure, and gas or solvent adsorption. For example, µ-53(Al, Cr) is known for its large reversible breathing amplitude between the hydrated and anhydrous form. A vanadium-based MOF, VO-(biphenyl-4,4′-dicarboxylate), which adopts an expanded µ-47 structure type, was found to display a distinct breathing effect (existence of both narrow pore and large pore forms) and has a high CO2 adsorption capacity [51]. Other flexible MOF structures such as Zn2(bpdc)2(bpee)]·2DMF (where bpdc = 4,4′-biphenyl dicarboxylate and bpee = 1,2-bis(4-pyridyl)ethylene) [52], and ([(Ni2L4)(bpdc)]·14H2O) [53] can reversibly restore and collapse their pore structure by adsorption of gases at high pressure [52].
The reversible structural changes in flexible MOFs occurring as a response to external stimuli such as a guest inclusion have been identified by the appearance of a step (gate opening) and a hysteresis in the adsorption/desorption measurements. In addition, some of these MOFs have unusual uptake behavior and preferential adsorption of one gas over the others. This is termed “selectivity” or viewed as the ratio of uptake concentrations of two gases at a given temperature and pressure. For example, Nijem et al. [54], using IR, Raman spectroscopy and density functional theory (DFT) calculations, reported their finding of the preferential adsorption of CO2 over N2 in MOF Zn2(bpdc)2(bpee) as due to the interactions of CO2 (quadrupole moment, polarity and stretching of the C=O bond) with the linkers, resulting in pores opening. Tanaka et al. [55] found that kinetics plays an important role in the gate-opening process in a flexible porous coordination polymer, {[Cd(benzophenone-4,4′-dicarboxylate)(4,4′-bipyridyl)]}n. Kauffman et al. [56] confirmed selective adsorption of CO2 from light gas mixture from the structural transition in the structurally dynamic porous coordination polymer, catena-bis(dibenzoylmethanato)-4,4′-bipyridyl)Ni(II), referred to as “Ni-DBMBpy” [57].

1.2. Ni(CN)4-Based MOFs (PICNICs)

Many structural changes in flexible MOFs have been observed in pseudo-1-D or 2-D materials which lack an extended covalent bridge in the third dimension. The structure of the Ni(CN)4-based flexible MOFs comprises extended 3-D coordination polymers which have strong coordinate covalent bridges in all three dimensions. Cyano-bridged complexes have been shown to form polymeric structures with 3-D Hofmann-like microporous frameworks [58], formed by metal-metal or metal-ligand-metal bridge connections in one, two, or three dimensions.
Back in 2001, Niel et al. [59] reported the isostructural 3-D coordination networks of the family of compounds {FeII(pyrazine)[MII(CN)4]} (M = Ni, Pd and Pt). These compounds undergo cooperative spin transitions at high temperatures, and the host–guest interactions inside the pores have considerable effects on the spin crossover properties of these materials. Agusti et al. [60] observed the thermal and light-induced spin crossover phenomena in the 3-D MOF of {[FeII(azpy)[MII(CN)4]}·nH2O (azpy = 4,4′azopyridine; M = Ni,Pd and Pt).
In recent years, National Energy and Technology Laboratory (NETL) has been one of the leading laboratories in the area of science and engineering research of novel Ni(CN)4-based flexible MOFs [56,61,62,63,64,65]. The precursors of these flexible MOFs are typically a cyanometallate complex that acts as a ligand and a transition metal complex with available coordination sites. The schematics of the pillared layered nickel-cyanide-based MOF that consists of a flexible framework is shown in Figure 1. They are collectively called pillared cyanonickelates, or PICNICs. The PICNIC family of compounds was developed for systematic studies of how pore structure and functionality could affect CO2 capture and separations. These sorbents are based on 2-D planar structures made from a tetracyano-nickelate coordination compound, which is a square planar complex (Figure 2). The nitrogen-end of the cyanide ligand from NiA can also coordinate with another transition metal, in this case, Ni (NiB). NiB acts as a linear linker between the tetracyano-nickelate groups, creating a 2-D square grid network (xy-plane). NiB in general has a six-fold octahedral coordination and it is along the z-axis that the organic pillar ligand coordinates. The size of the pores of the materials can be modified by the lengths of the pillared ligands. Figure 3 shows the schematics of the pillar ligands with different lengths, where one can perceive the size of the pore as defined by the length of the ligands.
These PICNICs have the unique ability to undergo dramatic structural changes during adsorption and desorption of guests between closed to open structure [66,67,68,69,70,71,72,73,74,75,76,77]. In some of the pillared layer systems, the pillars create a sorbent which requires a guest to maintain the structure of the pore. When this gas is removed, the sorbent collapses into a low-porosity state (Figure 1). These guests could be solvent or gas molecules. Gases such as CO2, CH4, or N2 can cause opening or collapse of the pores during the adsorption and desorption process. Many PICNICs exhibit hysteretic adsorption-desorption behavior which is often associated with the ‘gate-opening’ effect (Figure 4). They also show dynamic host-guest behavior due to structural transitions which occur between the guest-free and guest-loaded states [78,79,80,81,82].
The thermodynamic requirements of the induced structural change in PICNICS means that there is an activation energy that must be overcome in order to provide the energy needed to “power” the structural change. That energy is partially supplied by the energy given up during the adsorption of the gas. Different gases have different adsorption energies which can lead to selective behavior. If one gas can supply enough energy to transition the structure and the other gas cannot, then one is adsorbed and the other is not. It is thought that if gate-opening occurs at significantly different pressures for two gas components, the pores may open selectively for the preferred gas.
Detailed information of the crystal structure of PICNICs is essential for interpreting sorption data, for in-depth understanding of sorption mechanism, for modeling applications and for developing new materials for porous materials applications. In the following, our recent structural work on five selected Ni(CN)4-based novel materials is highlighted.

1.3. Five Selected Ni(Cn)4-Based Structural Studies

Many approaches to the design of porous coordination polymers involve the use of rigid mono- or bidentate heteroaromatic N-atom donor ligands. Coordination of these ligands to the Ni ions in the Ni(CN)4 groups would result in a multidimensional network via a self-assembly process [83]. With the goal of synthesizing and determining the structure of representative Ni(L)Ni(CN)4 (L = pillar organic ligands) compounds, the five ligands that we report in this paper are shown in Figure 5 as well as listed below. Often we found that the expected structures and those that we determined are quite different due to either the presence of guest molecules in the pores of the structure or the formation of 2-D or 1-D structures instead of the expected 3-D ones.
Compound 1 which was studied in our laboratory has been reported earlier [84]:
1.
1,2-bis(4-pyridyl)ethylene, C12N2H10, [Bpene]
2.
3-methyl-4,4′-bipyridine, C11N2H10, [BpyMe]
3.
3-amino-4,4′-bipyridine, C10N3H9, [BpyNH2]
4.
4,4′-bipyridine, C10N2H8, [Bpy]
5.
2,6-naphthyridine, C8N2H6, [Naph]
These ligands were chosen based on their lengths and functionalities. Using ligands of different lengths offer a great tenability of structural frameworks. Functional groups on the ligands offer variable configurations as well as possible modulation of CO2 affinity. In this study, one of the ligands involves a 4,4′-bipyridine ring (nicknamed Bpy) as the bridging ligands while two others are Bpy-based ligands containing additional functional groups of methyl (–CH3) and amine (–NH2). The Bpene ligand consists of two pyridine rings sandwiching an ethylene group. The 2,6-naphthyridine ligand (Naph) is a relatively short ligand with two pyridine rings sharing a common edge.

2. Results and Discussion

As shown below in our experimental procedure, crystal growths in these samples all involve the use of a mixture of DMSO, H2O and NH3. Interestingly, though all crystals were grown from very similar reaction conditions, the structures of the materials ranged from 1-D, 2-D and 3-D coordination polymers depending on the organic bridging ligand used. In addition, one of the 3-D structures is flexible whereas two of the 3-D structures are non-flexible. These five compounds are excellent examples of the structural diversity that can arise from a relatively simple set of building blocks and minor variations in ligand structure. Table 1 gives the data collection and structure solution for the compounds we describe in the following. The structure for Ni-Bpene has been reported previously from our laboratories [84].

2.1. Three-Dimensional (3-D) Structures

2.1.1. Ni(1,2-bis(4-pyridyl)ethylene)[Ni(CN)4] (Ni-Bpene)

In the first example, for simplicity, we refer to the sorbent as Ni-Bpene, which stands for Ni(Bpene)[Ni(CN)4] [84]. The expected formula without solvent molecule is C16H10N6Ni2. Ni-Bpene was found to adopt the 3-D Hofmann-type structure [58]. The molecular structure of the asymmetric unit with partial labeling is shown in Figure 6, and the complete labeling is given in supplementary Figure S1. The framework is based on the 2-D infinite layer-like tetracyanonickelate [Ni(CN)4]2− planar complex [85]. Ni3 and Ni4 are each coordinated to four C atoms of the C≡N groups forming a square-planar geometry. The N ends of the C≡N ligand further coordinate to Ni1 and Ni2 which act as linear linkers between the tetracyanonickelate molecules. All C≡N groups are bridging, creating a 2-D square grid network (Figure 7). The Ni1 and Ni2 ions are octahedrally surrounded by six N atoms, four from the C≡N units and the other two from two Bpene ligands. The layers are pillared by the Bpene ligands, which occupy the axial positions of the [NiN6] octahedron. These Bpene ligands further bridge together the 2-D Ni[Ni(CN)4] sheets that form the 3-D pillard-layered structure is shown Figure 8. Ni1 and Ni2 are shown to have an octahedral environment while Ni3 and Ni4 adopt a square planar geometry. The Bpene pillar ligands and the Ni[Ni(CN)4] layers encase empty voids of parallelepiped shapes which are created by the absence of Bpene coordination to Ni3 and Ni4 of the square plane [Ni(CN)4] building units. These void spaces provide pockets for the encapsulation of guest molecules [58].
The chains that make up the 2-D Ni[Ni(CN)4] sheets are arranged in a zigzag manner (for example, deviations of bond angles from 180° were observed. The bond distances of Ni-N and Ni-C within the 2-D sheet are all within the expected range (Table S1). The Ni3 and Ni4 have a square planar arrangement, and the mean Ni-C (1.860 Å) and C≡N (1.153 Å) bond lengths agree with the values reported for other tetracyanonickelate salts [86]. The Ni-N distances (range from 2.0168(13) Å to 2.099 (2) Å) are substantially longer than the Ni-C distances (1.856(2) Å to 1.865(2) Å), which also conform to the literature values [87]. The six-coordination Ni are of high spin configuration because nitrogen is acting as a weak-field ligand. When the Ni atom only has four coordinates (such as that in Ni(CN)4) [88], the low-spin square-planar coordination of Ni2+ ions results in a contraction.
Unexpectedly, one also observes that free Bpene ligands that are not coordinated to any Ni atoms are also present in the cavities of the structure. Positional disorder was observed in the free ligands. Similar disorder was further observed with half of the coordinated Bpene ligand molecules in the unit cell. Apparently there is sufficient space in the unit cell so these ligands have freedom to take on more than one configuration. Also, in the Bpene ligand, the ethylene moiety (C=C double bond) that connects the two pyridyl rings can have two conformations (Figure S1). This disorder was further observed with the free ligands in the lattice as well. Solvent molecules used as solvent of crystallization, such as water and dimethylsulfoxide (DMSO), were also found inside the cavities as disordered molecules. The chemical formula with inclusion of solvent and additional ligand is C24H35N7Ni2SO3. The guest Bpene ligand and solvents can be removed by a combined extraction and evacuation process to provide a material activated for sorption of gases.

2.1.2. Ni(3-methyl-4,4′-bipyridine)[Ni(CN)4], (Ni-BpyMe)

Tables S2–S6 give the atomic coordinates, anisotropic displacement parameters, selected pertinent bond distances, atomic coordinates for the hydrogen atoms and selected bond angles for Ni-BpyMe, respectively. Figure 9 gives the basic motif of the Ni(BpyMe)[Ni(CN)4] molecules. A complete labeling of the crystallographic independent unit is given in supplementary Figure S2.
Similar to Ni-Bpene, the Ni-BpyMe crystal is monoclinic with space group P2/n, a = 13.3483(14) Å, b = 7.1002(7) Å, c = 13.5625(14) Å, and β = 114.834(2)°. The structure of Ni-BpyMe consists of a 3-D net built from extended 2-D [Ni(CN)4] groups. These layers are connected to each other via the BpyMe ligands at the six-fold coordinated Ni2 site. Ni1 has a four-fold coordination environment. The interesting feature of this structure is that instead of locating the –CH3 group in one position of the pyridine ring as expected, it appears in two positions. The structure represents an average of two configurations which gives rise to the pseudosymmetry. The methyl group is distributed equally among the two pyridine rings; therefore, the occupancy of the methyl group in each pyridine ring site is 50%. The packing diagram of Ni-BpyMe is shown in Figure 10. The disordered hydrogen atom with an occupancy of 0.5 has been assigned as H4 (Table S5)
The bond distances of Ni1-N in the six-fold coordination environment (an average of 2.083 Å) are longer than that of the four-fold coordinated Ni2-C (an average of 1.862 Å), as expected. The average CN distance was found to be 1.152 Å. Bond distances within the bipyridine rings are as expected (Table S4). The two pyridine rings are not coplanar and form a dihedral angle of 45° to avoid steric hindrance between the two rings due to the bulky methyl group.
Similar to Ni-Bpene, disordered solvent of crystallization, DMSO, was also found in the pores (channels) of the structure (Figure 10). In each cluster of DMSO, there are two disordered positions of S (S1a and S2b) and O atoms (O1a and O2b), but the two carbon positions are not disordered (C9 and C10). The two resolved DMSO molecules are S1aO1aC9C10 and S2bO2bC9C10 (hydrogens not included). It is likely that highly disordered water molecules are also in the channel. The chemical formula of the compound is therefore C19H21N6Ni2O2S2.
Unlike that in Ni-Bpene, there is no extra free ligand entrapped in the lattice. It is expected that after the removal of DMSO, the voids in the structure will be able to accommodate guest molecules such as CO2. It is possible that the presence of the –CH3 groups would play a role in interacting with the guest molecules.
The gas adsorption properties of a large number of PICNIC derivatives were recently reported [61]. These materials were prepared by a heterogeneous ligand intercalation reaction which gave only powder products and hence detailed structural characterization was lacking. The Ni-BpyMe crystal sample prepared using the current technique (after extraction of guest DMSO with methanol and evacuation) gives the same CO2 adsorption isotherm as the powder sample prepared previously showing that the material can be prepared by two completely different synthetic techniques. Figure 11a gives the adsorption curves for Ni-BpyMe for both the crystal (red powder and black single crystals) and powder samples at 30 °C. In contrast to Ni-Bpene (Figure 11b), Ni-BpyMe gives a typical Type I adsorption isotherm with no indication of a structure transition over the measured range of temperature and pressures. Additional gas adsorption curves for crystalline Ni-BpyMe with CH4, N2 and CO2 are shown in Figure 12 as a function of temperature. As is typically observed with porous materials, the trend of these curves indicate that the crystal has the highest adsorption capacity for CO2 due to the fact that CO2 molecules (having quadrupole moments) have relatively stronger interaction (although weak intermolecular forces) with the BpyMe molecules than that with the CH4, and N2 molecules, respectively. As the temperature increases from 20 °C to 40 °C, the adsorption amount decreases relatively. This behavior is consistent with a physisorption mechanism.

2.1.3. Ni(3-amino-4,4′-bipyridine)[Ni(CN)4], (Ni-BpyNH2)

Tables S7 to S11 give the atomic coordinates, anisotropic displacement parameters, selected pertinent bond distances, atomic coordinates for the hydrogen atoms and selected bond angles, respectively, for Ni-BpyMe. Figure 13 gives the basic motif of the Ni(BpyNH2)[Ni(CN)4] molecules. A complete labeling of the crystallographic independent unit is given in supplementary Figure S3. It was difficult to grow high-quality Ni-BpyNH2 crystals, as reflected partly on the final relatively high residual values.
The compound was found to be orthorhombic having a space group Cmca. The unit cell dimensions were determined to be a = 14.7000(5) Å, b = 22.6879(7) Å, c = 13.8028(4) Å, V = 4603.4(2) Å3, and Z = 8. The b-axis is much longer than that of a- and c- and that is where the long axis of the ligand BpyNH2 aligns.
Ni-BpyNH2 forms a 3-D network, with a 2-D Ni(CN)4 square net connecting to each other via the BpyNH2 ligands. Figure 14 gives the 3-D packing diagram of the structure, viewing along the a-axis. It is clear that the fundamental structure is similar to the Ni-Bpene and Ni-BpyMe structures where parallelepiped-shaped cavities were enclosed by the 2-D Ni(CN)4 net and the BpyNH2 ligands. The 2-D Ni(CN)4 net is connected to each other via the bonding of the pyridine “N” atom to Ni2. The Ni2 atom is of six-fold coordination to N with relatively long Ni2-N distances (average of 2.079 Å) as compared to the four-fold coordination Ni1-C distances (average of 1.860 Å). The Ni(CN)4 net is arranged in a wave-like fashion. Figure 15 gives the “projected view” of the net where the NH2 groups are pointing towards the center of the pores (hydrogen atoms not shown in the figure).
Similar to Ni-BpyMe, one of the features of the Ni-BPyNH2 system is that the amine functional group, –NH2, has been solved using a disordered model resulting from an average of four configurations, giving rise to the observed pseudosymmetry. The NH2 group is found in the m-position relative to the N atom of the pyridine ring. It has one-quarter site occupancy in each of the four m-positions. In other words, the NH2 group has 25% probability of being at one of the four possible m-positions. Furthermore, similar to the structure of Ni-BpyMe, the two pyridine rings in the ligands are not coplanar; they are essentially perpendicular to each other to avoid large steric hindrance. The two disordered hydrogen atoms with an occupancy of 0.75 have been assigned to H4 and H7 (Table S10).
Based on the structure of Ni-BpyMe, it is expected that the solvent molecules DMSO are also entrapped in the channel. DMSO molecules were indeed located in two independent sites. However, these solvent molecules are highly disordered in the pores. Similar to Ni-Bpene and Ni-BpyMe, it is expected that when the disordered solvent molecules are extracted, they can be replaced by guest molecules. The relatively high residual electron density in the vicinity of the disordered DMSO solvent molecule is partly due to the inadequate displacement model (anisotropic ellipsoids) describing the thermal motions. The overall structure of the Ni-BpyNH2 network indeed gives important information for future guest molecule exchange studies.
In this system, no extra BpyNH2 ligand molecules were found to be inside the cavities of the structure. The chemical formula of the compound is therefore C18Ni2S2O2N7H21. Efforts to obtain gas adsorption data on the crystalline Ni-BpyNH2 sample were hampered by the inability to obtain a sufficient quantity of pure material since the crystals had to be mechanically separated from a significant amount of polycrystalline impurity.

2.2. Two-Dimensional (2-D) Structure

Ni(4,4′-bipyridine)[Ni(CN)4], (Ni-Bpy)

Tables S12 to S16 give the atomic coordinates, anisotropic displacement parameters, selected pertinent bond distances, atomic coordinates for the hydrogen atoms and selected bond angles, respectively, for Ni-Bpy. Figure 16 gives the basic motif of the Ni(Bpy)[Ni(CN)4] molecules. A complete labeling of the crystallographic independent unit is given in supplementary Figure S4.
The structure of the compound Ni (4,4′-bipyridine)[Ni(CN)4], or Ni-Bpy, was determined to be a 2-D metal organic cyanide-bridged framework instead of having a 3-D network. The resulting chemical formula is [Ni(CN)4Ni(C10H8N2)(NH3)2], or Ni2C14N8H14, instead of the expected Ni2C14N6H8. The crystal was found to be orthorhombic Pnnm, a = 7.2641((9) Å, b = 9.9285(12) Å, c = 11.4008(14) Å. The structure can be considered as extended 2-D sheets, while interacting with the neighboring sheets via van der Waals’ forces (Figure 16). The structure is essentially composed of –Ni-4,4′-Bpy-Ni-4,4′Bpy-Ni chains linked by [Ni(CN)4]2– anions. The six-fold coordination environment of the NiII includes two NH3 groups (in place of two –C≡N groups), while the coordination environment around the four-fold NiI is completed by two terminal –C≡N groups and two other –C=N- in the chain. As a result of these unexpected coordinates, cross-link bridging is no longer possible, and a 3-D structure is excluded.
The salient feature of the structure is that it consists of zigzag –Ni-NC-Ni-CN-Ni– chains. Each chain is further connected to the neighboring chains via the Bpy ligand to form a layered structure. The two pyridine rings are coplanar with each other. However, there is an abscence of a 3-D bridging of the layer to other layers via coordination bonds at the Ni sites. In other words, Ni-Bpy has a sheet-like structure spreading in the bc direction. Figure 17 gives the view of one such layer. This is because the two remaining available NiII sites on the other chain have been occupied with two strong Lewis bases, namely, the NH3 groups; therefore, the N site of the relatively weaker Lewis base –C≡N was “forced” to remain as a terminal group. This situation is different from a typical Hoffman-type of compound where instead of having the terminal –C≡N groups, the –C≡N groups bridge to the other Ni site on different chains to form a 2-D net (Figure 17). These sheets are connected to each other via van der Waal’s forces and hydrogen bonds (van der Waal radii for H is 1.2 Å, N: 1.55 Å [89]) (Figure 18). From Table S16, two of the Hs in the NH3 groups form hydrogen bonds (2.323 Å) to the terminal C≡N groups of the neighboring Ni-C-N-Ni-N-C-Ni chains in the structure as shown on Figure 19.
NH3, regarded as a basic molecule because it possesses a lone pair of electrons in its 3a1 orbital, is a classic example of an electron-donor Lewis base molecule [90] (a Lewis base donates a lone pair of electrons to a Lewis acid to form a Lewis adduct). This lone pair at the nitrogen is available for donation to other species (accept a proton) during bonding [90,91]. Madey and Houston [92] found that when NH3 is adsorbed on metal Ni(111), it is molecularly adsorbed, and is bonded to the surface via the N atom (becomes part of the structure) with the H atoms oriented away from the surface. Netzer and Madley [93] further confirmed that traces of pre-adsorbed oxygen on a metal surface will induce a high degree of azimuthal order in adsorbed molecules.
As a summary, one of the reasons that the 2-D nickel cyanide net does not form in Ni-Bpy is because of the strong Lewis acid–base reactions between NH3 with Ni that prevent the polymerization of the chains to become a 2-D net. Comparing to a number of other Hoffman-type compounds with Ni-groups, to our knowledge, this is one of the first compounds that we found in the Ni(Bpy)[Ni(CN)4] family that has NH3 groups as terminating ligands. Water of crystallization was reported to coordinate to the transition metals Ni or Cu [94,95,96]. Since our solvent of crystallization is a mixture of DMSO/H2O/NH3, apparently NH3 is a stronger Lewis base than H2O for competing for the coordination site to Ni.
It is unclear at this point why the functionalized bipyridine ligands BpyMe and BpyNH2 both give 3-D structures whereas the non-functionalized Bpy ligand yields a 2-D structure. One possibility is that the –R group in Ni-Bpy-R gives rise to steric hindrance which prevents the coordination of the NH3 groups to Ni, allowing the polymerization process to yield the 3-D structure. There may also be some effect where the higher symmetry of the Bpy ligand allows the 2-D network to propagate more quickly forcing the precipitation of this network before the loss of ammonia is complete. In the reaction with the less symmetrical Bpy-R, the kinetics for the propagation of the 2-D Bpy-R bridged structure may be slowed enough that this phase remains in solution longer. This would provide enough time for the NH3 concentration to drop to a point where the 3-D network can form via displacement of the coordinated NH3 ligands with bridging ligands. This mechanism is further supported by the formation of even lower dimensional 1-D chain structures with the shortest ligand in the series 2,6-naphthyridine. With the Naph linker (discussed below), the chain propagation kinetics are fast enough to crystallize the 1-D structure while the four blocking NH3 ligands remain coordinated to the octahedral Ni site.

2.3. One-Dimensional (1-D) Structure

(Ni(2,6-naphhyridine)[Ni(CN)4]), (Ni-Naph)

Tables S17–S21 give the atomic coordinates, anisotropic displacement parameters, selected pertinent bond distances, atomic coordinates for the hydrogen atoms and selected bond angles, respectively, for Ni-Naph. Figure 20 gives the basic motif of the Ni(Naph)[Ni(CN)4] molecules with partial labeling. A complete labeling of the crystallographic independent unit is given in supplementary Figure S5.
In the Ni-Naph compound, the ligand Naph has a relatively short length which consists of only two six-membered rings sharing one common edge, indicating if a 3-D cage-like structure forms; the resulting volume for CO2 capture is expected to be smaller than that in the Bpene, BpyMe and BpyNH2 compounds. The structure of Ni-Naph was found to be triclinic (space group P-1), with a relatively small unit cell dimension: a = 7.0315(3)Å, b = 7.9219(3)Å, c = 8.6103(3) Å, α = 67.816(1)°, β = 72.828(1)°, and γ = 73.698(1)°.
The salient feature of the Ni-Naph compound is that instead of having a 3-D or 2-D structure, it consists of one-dimensional chains running parallel to the c-axis (Figure 21). The Naph ligand, while coordinating to Ni of the Ni(CN)4 groups to form chains, it prevents the formation of a 2-D tetracyanonickelate net. In the Ni-Naph structure, the one-dimensional chains alternate with discrete Ni(CN)4 groups. Four NH3 groups instead of the expected C≡N groups were found bonding to the six-fold coordinated Ni site. These NH3 groups are terminated groups instead of propagating to form a higher dimension structure. As a result, 1-D chains of Ni(Naph)(NH3)4 and discrete units of planar [Ni(CN)4] groups were found parallel to each other along c-axis. The chemical formula of this compound (Ni2C12N10H18), can be written in terms of chemical moiety as Ni(CN)4·Ni(NH3)4·C8N2H6.
In the 1-D Ni(Naph)(NH3)4 chains, the N1-Ni1-N1 and N3-Ni1-N3 angles are all 180°. The six-fold coordinated Ni-N distances (2.1429(8) Å, 2.1145(8) Å, and 2.1353(9) Å) are within the expected Ni-N distances. In the discrete Ni(CN)4 units, the Ni2-C6 and Ni2-C5 bond distances of 1.8627(10) Å and 1.8588(10) Å are shorter than those of the Ni-N distances, as expected. The C5-Ni2-C5 angles and the C6-Ni2-C6 angles are all 180°. The –C≡N distances (1.1565(14) Å and 1.1592(14) Å) are within the expected range.
Another 1-D square tetracyano complex was also reported earlier by Černák and Abboud [97]. They found a one-dimensional structure of catena-poly[Ni2(CN)4(C10H8N2)2]n, consisting of infinite zigzag chains running parallel to the c-axis of the structure. The chains are composed of paramagnetic [Ni(dipy)2]2+ cations linked by diamagnetic [Ni(CN)4]2– anions via bridging cyano groups. The bridging cyano group occupies a cis position in the cation and a trans position in the anion, resulting in a cis-trans-type square tetracyano complexes.
All these molecules are connected to each other via intermolecular covalent forces. This is another excellent example illustrating that the concentration of solvent mixture of crystallization has an important effect on the final product of crystal growth and their structures. Different strategies such as varying the outgas rate of NH3 will be pursued for obtaining the 3-D structure of Ni-Naph.

3. Experimental Section

Certain trade names and company products are mentioned in the text or identified in illustrations in order to adequately specify the experimental procedures and equipment used. In no case does such identification imply recommendation or endorsement by the National Institute of Standards and Technology.
The details of the powder syntheses of these MOF compounds using a different synthetic method are reported elsewhere [61].

3.1. Material Synthesis and Crystal Growth

A technique [84] that we have found to be versatile for crystallization of Ni(L)[Ni(CN)4] compounds is a modification of a procedure originally used by Černák et al. to prepare crystalline 1-D [Ni(CN)4] containing chain compounds [97]. The approach involves the use of NH3 as a blocking ligand since a sufficient concentration of NH3 will prevent the formation of Ni-CN-Ni and Ni-L-Ni bridges which are required for polymerization. If the reaction mixture is contained in an open flask, the NH3 will outgas from the solution. Once the concentration of NH3 drops below a threshold level, assembly of the Ni(L)[Ni(CN)4] material will commence. Using a H2O/DMSO mixture as the solvent and a reaction temperature of ≈90 °C provided the necessary combination of NH3 outgassing rate and oligomer solubility to produce the polymeric structures. A good crop of crystals can typically be obtained in 24 h to 72 h. The technique has been found to be adaptable to various organic bridging ligands (L) in our laboratory. The general synthetic strategy has been reported previously [84] and its adaptation to the synthesis of the materials in the current report is as follows. The reactants 3-methyl-4,4′-bipyridine; 3-amino-4,4′-bipyridine; nickel cyanide hydrate Ni[Ni(CN)4]n(H2O)3 were prepared as previously described [61]. The 2,6-naphthyridine was purchased from the Florida Center for Heterocyclic Compounds and used as received. Water was purified by an in-house reverse osmosis system. All other reagents were purchased from Sigma-Aldrich and used as received. Precise yields are not given since the crystals are stored in the mother liquor and only removed in random batches as needed for analysis and other characterizations. Estimated yields for all reactions are in the range of 50%–75%.
Ni-BpyMe. At room temperature, a 50 mL flask was charged with 0.5 mmol polymeric nickel cyanide hydrate Ni[Ni(CN)4]n(H2O)3 and made to dissolve through the sequential addition of 6 mL H2O, 6 mL of reagent concentrated ammonium hydroxide solution, and 9 mL DMSO with stirring. (Caution: do not mix concentrated ammonium hydroxide and DMSO directly as rapid outgassing of NH3 will occur.) A solution of 0.5 mmol BpyMe in 9 mL warm DMSO was then added to the resulting solution. A six-inch air-cooled condenser was added and the flask was transferred to an oil bath preheated to 70 °C. The temperature of the oil bath was ramped to 90 °C over a time span of approximately 30 min after which time the stirring was stopped and the reaction left at 90 °C undisturbed for two days. The dissolved NH3 bubbled out of the solution rapidly during the initial hour, then slowed significantly while a crystalline product formed over the next two days. After completion, the reaction mixture was cooled to room temperature and the resulting crystals were isolated by first decanting off any suspended fine particles suspension of impurities while being careful to leave the crystals wetted within the reaction mixture. The impurities were removed by filtration and the filtrate returned to the flask. The pipetting and filtration cycle was repeated until the powdered impurities were removed. The light violet crystals were kept stored in the cleaned reaction mixture in a capped vial at room temperature until the X-ray diffraction measurements were taken.
Ni-BpyNH2. By the same general procedure used for Ni-BpyMe, 0.60 mmol of BpyNH2 was reacted with 0.5 mmol Ni2(CN)4 hydrate in a mixture of 6 mL H2O, 6 mL concentrated aqueous NH3, and 18 mL DMSO. The product contains a significant amount of a green powder impurity that obstructed complete characterization of the crystalline product by gas adsorption. A TGA scan was taken on a few pure crystals harvested from the stir bar.
Ni-Bpy. The crystals were prepared using the same general procedure and reactant ratios as for Ni-BpyMe, with the exception that Bpy was used in place of BpyMe.
Ni-Naph. The crystals were prepared using the same general procedure and reactant ratios as for Ni-BpyMe, with the exception that 2,6-naphthyridine was used in place of BpyMe.

3.2. Synchrotron X-Ray Diffraction Experiment

As most crystals are twin or multiplets, the crystals that we used for data collection in general have very small dimensions (for example, the Bpene crystal has a dimension of 0.016 × 0.011 × 0.006 mm3 and it has a thin-plate morphology). The crystals were mounted on the tip of a glass fiber with paratone oil and cooled down to 100 K with an Oxford Cryojet. X-ray diffraction experiments were performed with a Bruker D8 diffractometer in the vertical mount with a APEX II CCD detector (Bruker Corporation, Madison, WI, USA) using double crystals technique with Si(111) monochromator at 30 keV (λ ranges from 0.41328 Å to 0.4428 Å for the current studies) at sector 15 (ChemMatCARS), Advanced Photon Sources (APS). Data were processed with APEX2 suite software [98] for cell refinement and reduction. The structure was solved by the direct method and refined on F2 (SHELXTL) [99]. Non-hydrogen atoms were refined with anisotropic displacement parameters, and hydrogen atoms on carbons were placed in idealized positions (C-H = 0.95 Å).

3.3. Sorption Experiments

Gravimetric gas adsorption measurements for the Ni-BpyMe sample were conducted on a Hiden IGA microbalance (Hiden Isochema, Warrington, United Kingdom). The crystalline sample was first extracted by soaking in methanol at room temperature overnight. The methanol-exchanged sample (≈25 mg) was activated by heating under vacuum at 70 °C until the sample weight stabilized. Isotherms were then measured under flowing gas regulated by a mass flow controller and back pressure regulator. Equilibrium was determined at each pressure step using an internal fitting algorithm in the instrument control software. Buoyancy corrections were then applied to the final equilibrium weights using known densities of all components in the sample and counterweight chambers from gas densities calculated using REFPROP software [100].
Sample integrity of the Ni-BpyMe sample after solvent exchange with methanol and evacuation was verified by comparing the powder X-ray diffraction pattern of the activated sample to one calculated from the solvated Ni-BpyMe crystal structure using Mercury software [101]. The pattern was also compared to one from a previously reported synthesis of the polycrystalline Ni-BpyMe sample [61]. Taking into consideration that slight variations in the evacuated and solvated patterns are expected due to changes in symmetry upon guest removal, the two patterns give satisfactory agreement. The powder pattern reported for the evacuated polycrystalline material in [61] also agrees well with the current sample. The powder diffraction results are included as supporting information (Figure S6).

3.4. Thermogravimetric Analyses

Thermogravimetric analyses were performed using a Mettler STARe TGA/DSC thermogravimetric analyzer (Mettler Toledo, Columbus, Ohio, USA). Samples (typically 5 mg to 10 mg) were run in a Pt pan under a dry air purge at temperatures >550 °C. Sample purity was determined from the ratio of the residual weight of NiO in the sample pan to the guest-free weight of the material at the appropriate place in the TGA scan. This experimental ratio was then compared to the NiO ratio expected from the guest-free formula weight of the material as determined from the crystal structure. A TGA scan in air will then allow the guest-free framework mass to be determined, which upon combustion in air will yield NiO. Since only one composition of NiO is possible, the method works well for these compounds, as opposed to other materials which contain variable oxidation state metals such as iron, cobalt, copper, manganese, etc. which could form mixed oxidation state oxides during the combustion. With nickel compounds, the TGA technique works according to the simple decomposition reaction: guest-free framework Ni(L)Ni(CN)4 → 2NiO. As such, the ratio of the mass of residual NiO to the mass of the guest-free framework in the TGA scan is the same as the ratio of the formula weight of NiO to the formula weight of the guest-free framework. Using the data in Figure 22 for the Ni(Bpy-Me)Ni(CN)4 compound as an example: Expected formula weight of Ni(Bpy-Me)Ni(CN)4 is 391.67 g/mol and the formula weight of 2NiO is 149.39 g/mol. The ratio of the formula weight of NiO to Ni(Bpy-Me)Ni(CN)4 = 149.39/391.67 = 0.3814. This same ratio should be observed in TGA scan when using the residual mass of NiO to the dry framework mass. From the TGA data, the residual mass of NiO is 1.26 mg and the mass of the guest-free framework is 3.25 mg. The ratio is 1.26/3.25 = 0.3877. This is within 98% of the expected value, thus confirming the crystal composition. The actual and expected values for the NiO to framework ratios for the other samples gave similar agreements. The values for each sample are shown on the TGA plots in the respective figures in the manuscript.
A TGA scan in air for a sample of neat crystals of Ni-BpyNH2 harvested from the stir bar is shown in Figure 23. The ratio of residual NiO to the guest-free framework (plateau region 250–300 °C after loss of guest DMSO) agrees well with that expected based on the guest-free Ni-BpyNH2 formula weight of 392.65 g/mol determined from the crystal structure. The TGA scan in air for crystals of neat Ni-Bpy is shown in Figure 24. The ratio of residual NiO to the crystal framework (plateau region 100–150 °C after loss of surface water) agrees well with that expected based on the Ni-Bpy formula weight of 411.70 g/mol determined from the crystal structure. The loss of the two coordinated NH3 ligands per Ni(Bpy)(NH3)2[Ni(CN)4] unit are shown by the step at ~200 °C. The relative weight loss for the release of the coordinated ammonia also agrees well with that expected from the crystal structure. The TGA scan in air for crystals of neat Ni-Naph are shown in Figure 25. The ratio of residual NiO to the crystal framework agrees well with that expected based on the Ni-Naph formula weight of 419.73 g/mol determined from the crystal structure if the initial starting mass in the TGA scan is used; however, the results are not as clear as with the other three samples. The sample does show a small initial mass loss below 100 °C which transitions into a larger step indicating that the loss of coordinated NH3 ligands is complete by ≈250°C. The low-temperature weight loss may indicate that the bulk sample has some small fraction of material in which coordinated NH3 ligands are partially replaced with coordinated water ligands or that the bulk material is not 100% phase pure. A likely impurity in the bulk material would be the result of incomplete removal of an insoluble green powder phase that precipitates with the crystalline sample, similar to that noted for the NiBpy-NH2 sample above.

4. Conclusions

Structure data for the PICNIC series of compounds increases our understanding of coordination chemistry and interactions of guest-host phenomena in these versatile materials. In particular, it’s interesting to compare the structures and guest adsorption behaviors of the 3-D structures when the ligands are Bpene, BpyMe and BpyNH2. All three materials adopt a similar pillared layer motif; however, the Bpene compound shows structurally dynamic behavior which transitions between a low-porosity and high-porosity state during the adsorption and desorption of guests, such as CO2, whereas the BpyMe and BpyNH2 compounds retain a rigid structure with no variation in pore structure between the guest-loaded and guest-free states. One possible explanation for the variation in structural rigidity in the series of materials may lie in the Ni-N-C bond angles associated with the octahedral Ni sites in the structures. These bonds result from the bridging interaction of the cyanide ligand between the square planar NiA(CN)4 complexes and the octahedral NiB sites. The Ni-Bpene material shows the greatest deviation from linearity with both Ni2-N3-C3 and Ni1-N4-C4 having bond angles of 171.4°. This bridging interaction corresponds to the Ni-N-C-Ni linkage running along the bc face diagonal. In contrast, the highest deflection in the Ni-BpyMe compound occurs in Ni1-N2-C8 with an angle of 174.3°. In Ni-BpyNH2, the bond is even more linear with a bond angle between Ni2-N1-C1 of 176.4°. (See supporting information Figures S1–S3) From this observation, there appears to be a stronger driving force to form a more corrugated Ni[Ni(CN)4]n network in the Bpene material which results in a more significant tilt in the Bpene pillar ligands relative to the Ni[Ni(CN)4]n plane. A flexible, hinge-like bond corresponding to the Ni-N-C linkage would provide a means for the relative tilt of the pillars to change, which in turn, would directly affect the inter-pillar distance and available pore volume.
The relative rates of NH3 outgassing and Ni-(L)-Ni chain propagation are important for the final structures of the single crystals. When the ligands were Bpene, BpyMe and BpyNH2, the relative rates are favorable for the formation of extended 3-D structures. In these materials, the pillar ligands and the Ni[Ni(CN)4] layers encase empty voids of parallelepiped shapes which are created by the absence of ligand coordination to the two Ni sites of the square plane [Ni(CN)4] building units. These void spaces provide pockets for the encapsulation of guest molecules. When these reaction rates vary significantly, structures with a lower dimensionality are obtained including a 2-D layered structure when Bpy is a bridging ligand and a 1-D structure when the bridging ligand is Naph.
In the 2-D and 1-D structures, the octahedral Ni sites contain coordinated –NH3 ligands which effectively block chain propagation in all three dimensions. In the 2-D structure, the two axial sites of the octahedral Ni complex are blocked by –NH3, allowing chain propagation through Bpy and Ni(CN)4 bridging interactions to occur in the xy plane only. Furthermore, when the ligand is Naph, a 1-D structure resulted. In the 1-D chain, the six-fold coordinated Ni is surrounded by four –NH3 groups while the chain is propagated along the –Naph-Ni-Naph-Ni– direction (c-direction). The chains are further interleaved with discrete isolated Ni(CN)4 units. Future challenges will be to refine the synthesis process in order to convert these low-dimensional structures into 3-D ones.
Results of more single-crystal data with a greater variety of ligands with different lengths and functional groups will further enhance our understanding of these materials. Continuing research is ongoing in our laboratories to prepare and characterize other novel 3-D PICNICs, and to explore their adsorption properties.

Supplementary Materials

The supplementary materials are available online at https://www.mdpi.com/2073-4352/6/9/108/s1.

Acknowledgments

This technical effort was performed in support of the National Energy Technology’s ongoing research in CO2 capture under the Research Contract DE-FE0004000. The authors gratefully acknowledge ChemMatCARS Sector 15 which is principally supported by the National Science Foundation/Department of Energy under grant number NSF/CHE-1346572. Use of the Advanced Photon Source was supported by the U.S. Department of Energy, Office of Science, Office of Basic Energy Sciences, under Contract No. DE-AC02-06CH11357.

Author Contributions

Winnie Wong-Ng performed single-crystal structure determination and wrote the paper. Jeff T. Culp was responsible for design and synthesis of materials, performing sorption experiments, and co-writing the paper. Yu-Sheng Chen performed data collection and structural studies and co-wrote the paper.

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Schematic drawing demonstrating the opening/collapsing (decreasing/increasing the angle between the basal plane and the ligand) of the unit cells of Ni(L)[Ni(CN)4] in the presence of CO2.
Figure 1. Schematic drawing demonstrating the opening/collapsing (decreasing/increasing the angle between the basal plane and the ligand) of the unit cells of Ni(L)[Ni(CN)4] in the presence of CO2.
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Figure 2. Tetracyano-nickelate square planar complex showing two different types of Nis (different coordination environment).
Figure 2. Tetracyano-nickelate square planar complex showing two different types of Nis (different coordination environment).
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Figure 3. Schematics of the pillar ligands with different lengths.
Figure 3. Schematics of the pillar ligands with different lengths.
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Figure 4. Comparing typical gas adsorption (blue)-desorption (red) cycles for a rigid porous material (top) and a flexible MOF (bottom). Adsorption in flexible sorbents is associated with a gate-opening effect at a specific threshold condition of temperature and pressure. Desorption is hysteretic.
Figure 4. Comparing typical gas adsorption (blue)-desorption (red) cycles for a rigid porous material (top) and a flexible MOF (bottom). Adsorption in flexible sorbents is associated with a gate-opening effect at a specific threshold condition of temperature and pressure. Desorption is hysteretic.
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Figure 5. Schematic drawing of the chemical formulas for the five pillar ligands: Naph, C8N2H6; Bpy, C10N2H8; BpyNH2, C10N3H9; BpyMe, C11N2H10; and Bpene, C12N2H10.
Figure 5. Schematic drawing of the chemical formulas for the five pillar ligands: Naph, C8N2H6; Bpy, C10N2H8; BpyNH2, C10N3H9; BpyMe, C11N2H10; and Bpene, C12N2H10.
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Figure 6. The basic motif of Ni-Bpene (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
Figure 6. The basic motif of Ni-Bpene (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
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Figure 7. The 2-D tetracyanonickelate square grid network in Ni-Bpene (C-grey, N-blue, Ni-green).
Figure 7. The 2-D tetracyanonickelate square grid network in Ni-Bpene (C-grey, N-blue, Ni-green).
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Figure 8. The Bpene ligands bridge the 2-D Ni[Ni(CN)4] sheets to form the 3-D pillared-layered structure (C-grey, N-blue, Ni-green).
Figure 8. The Bpene ligands bridge the 2-D Ni[Ni(CN)4] sheets to form the 3-D pillared-layered structure (C-grey, N-blue, Ni-green).
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Figure 9. The basic motif of the Ni(BpyMe)[Ni(CN)4] molecules (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
Figure 9. The basic motif of the Ni(BpyMe)[Ni(CN)4] molecules (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
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Figure 10. Structure of Ni-BpyMe with disordered DMSO solvent inside the rectangular cage (view along the b-axis; C-grey, N-blue, Ni-green, S-yellow, O-red).
Figure 10. Structure of Ni-BpyMe with disordered DMSO solvent inside the rectangular cage (view along the b-axis; C-grey, N-blue, Ni-green, S-yellow, O-red).
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Figure 11. Comparing CO2 adsorption data at 30 °C for Ni-BpyMe powder (black) and single-crystal (red) samples. Plot (b) is shown to contrast the adsorption (solid)–desorption (open) behavior for CO2 at 30 °C on the flexible PICNIC Ni-Bpene to that of the rigid Ni-BpyMe sample, plot (a).
Figure 11. Comparing CO2 adsorption data at 30 °C for Ni-BpyMe powder (black) and single-crystal (red) samples. Plot (b) is shown to contrast the adsorption (solid)–desorption (open) behavior for CO2 at 30 °C on the flexible PICNIC Ni-Bpene to that of the rigid Ni-BpyMe sample, plot (a).
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Figure 12. Adsorption data for CO2 (diamonds), CH4 (circles) and N2 (triangles) at 40 °C (a) and at 20 °C on a crystalline sample of Ni-BpyMe (b).
Figure 12. Adsorption data for CO2 (diamonds), CH4 (circles) and N2 (triangles) at 40 °C (a) and at 20 °C on a crystalline sample of Ni-BpyMe (b).
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Figure 13. The basic motif of the Ni(BpyNH2)[Ni(CN)4] molecules (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
Figure 13. The basic motif of the Ni(BpyNH2)[Ni(CN)4] molecules (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
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Figure 14. 2-D Ni(CN)4 wavy net connecting to each other via the Ni-BPyNH2 ligands to form a 3-D structure (C-grey, N-blue, Ni-green), viewing along a-axis.
Figure 14. 2-D Ni(CN)4 wavy net connecting to each other via the Ni-BPyNH2 ligands to form a 3-D structure (C-grey, N-blue, Ni-green), viewing along a-axis.
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Figure 15. Ni-BPyNH2 square net view down the b-axis of the molecule (C-grey, N-blue, Ni-green).
Figure 15. Ni-BPyNH2 square net view down the b-axis of the molecule (C-grey, N-blue, Ni-green).
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Figure 16. The basic motif of the Ni(Bpy)[Ni(CN)4] molecules (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
Figure 16. The basic motif of the Ni(Bpy)[Ni(CN)4] molecules (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
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Figure 17. 2-D structure of Ni-Bpy along a-axis, with sheet-like structure spreading in the bc direction (C-grey, N-blue, Ni-green).
Figure 17. 2-D structure of Ni-Bpy along a-axis, with sheet-like structure spreading in the bc direction (C-grey, N-blue, Ni-green).
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Figure 18. 2-D sheets in Ni-Bpy are connected to each other via van der Waal’s forces and hydrogen bonding (view along b-axis; C-grey, N-blue, Ni-green).
Figure 18. 2-D sheets in Ni-Bpy are connected to each other via van der Waal’s forces and hydrogen bonding (view along b-axis; C-grey, N-blue, Ni-green).
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Figure 19. Terminal C≡N groups of the neighboring Ni-C-N-Ni-N-C-Ni chains in the Ni-Bpy structure forming a zigzag fashion (view along c-axis; C-grey, N-blue, Ni-green). The red broken lines indicate H-bonding.
Figure 19. Terminal C≡N groups of the neighboring Ni-C-N-Ni-N-C-Ni chains in the Ni-Bpy structure forming a zigzag fashion (view along c-axis; C-grey, N-blue, Ni-green). The red broken lines indicate H-bonding.
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Figure 20. The basic motif of the Ni(Naph)[Ni(CN)4] molecules (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
Figure 20. The basic motif of the Ni(Naph)[Ni(CN)4] molecules (C-grey, N-blue, Ni-green; probability ellipsoids drawn at 50%).
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Crystals 06 00108 g021 1024
Figure 21. The Ni-Naph structure showing 1-D chains of Ni(Naph)(NH3)4 and individual units of planar [Ni(CN)4] groups (view along b-axis; C-grey, N-blue, Ni-green).
Figure 21. The Ni-Naph structure showing 1-D chains of Ni(Naph)(NH3)4 and individual units of planar [Ni(CN)4] groups (view along b-axis; C-grey, N-blue, Ni-green).
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Crystals 06 00108 g022 1024
Figure 22. TGA scan in air for crystals of Ni-BpyMe after extracting DMSO guests with methanol. All methanol guests are lost below 100 °C with no further weight loss prior to decomposition. The “expected” value on the plot is the expected ratio of the mass of residual NiO to mass of the guest-free framework as determined from the structure determined by single-crystal X-ray diffraction, whereas the “actual” ratio is the experimentally determined value taken at the indicated points in the scan. See Experimental Section for an explanation of how the ratio is calculated.
Figure 22. TGA scan in air for crystals of Ni-BpyMe after extracting DMSO guests with methanol. All methanol guests are lost below 100 °C with no further weight loss prior to decomposition. The “expected” value on the plot is the expected ratio of the mass of residual NiO to mass of the guest-free framework as determined from the structure determined by single-crystal X-ray diffraction, whereas the “actual” ratio is the experimentally determined value taken at the indicated points in the scan. See Experimental Section for an explanation of how the ratio is calculated.
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Figure 23. TGA scan in air for neat clean crystals of Ni-BpyNH2. Loss of guest DMSO is complete by 250 °C yielding the guest-free framework. The “expected” value on the plot is the expected ratio of the mass of residual NiO to the mass of the guest-free framework as determined from the structure determined by single-crystal X-ray diffraction, whereas the “actual” ratio is the experimentally determined value taken at the indicated points in the scan. See Experimental Section for an explanation of how the ratio is calculated.
Figure 23. TGA scan in air for neat clean crystals of Ni-BpyNH2. Loss of guest DMSO is complete by 250 °C yielding the guest-free framework. The “expected” value on the plot is the expected ratio of the mass of residual NiO to the mass of the guest-free framework as determined from the structure determined by single-crystal X-ray diffraction, whereas the “actual” ratio is the experimentally determined value taken at the indicated points in the scan. See Experimental Section for an explanation of how the ratio is calculated.
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Crystals 06 00108 g024 1024
Figure 24. TGA scan in air for neat crystals of Ni-Bpy. Loss of coordinated NH3 occurs over the temperature range of 200 °C to 300 °C. The “expected” value on the plot is the expected ratio of the mass of residual NiO to the mass of the framework as determined from the structure determined by single-crystal X-ray diffraction, whereas the “actual” ratio is the experimentally determined value taken at the indicated points in the scan. See Experimental Section for an explanation of how the ratio is calculated.
Figure 24. TGA scan in air for neat crystals of Ni-Bpy. Loss of coordinated NH3 occurs over the temperature range of 200 °C to 300 °C. The “expected” value on the plot is the expected ratio of the mass of residual NiO to the mass of the framework as determined from the structure determined by single-crystal X-ray diffraction, whereas the “actual” ratio is the experimentally determined value taken at the indicated points in the scan. See Experimental Section for an explanation of how the ratio is calculated.
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Figure 25. TGA scan in air for neat crystals of Ni-Naph. Loss of NH3 occurs in two steps out to 300 °C followed by immediate decomposition of the material. (The initial small weight loss at low temperature may also indicate some impurity in the bulk sample as discussed in the main text.) The “expected” value on the plot is the expected ratio of the mass of residual NiO to the mass of the framework as determined from the structure determined by single-crystal X-ray diffraction, whereas the “actual” ratio is the experimentally determined value taken at the indicated points in the scan. See Experimental Section for an explanation of how the ratio is calculated.
Figure 25. TGA scan in air for neat crystals of Ni-Naph. Loss of NH3 occurs in two steps out to 300 °C followed by immediate decomposition of the material. (The initial small weight loss at low temperature may also indicate some impurity in the bulk sample as discussed in the main text.) The “expected” value on the plot is the expected ratio of the mass of residual NiO to the mass of the framework as determined from the structure determined by single-crystal X-ray diffraction, whereas the “actual” ratio is the experimentally determined value taken at the indicated points in the scan. See Experimental Section for an explanation of how the ratio is calculated.
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Table
Table 1. Crystal Data and Structure Refinement for Four Cyanonickelate Compounds.
Table 1. Crystal Data and Structure Refinement for Four Cyanonickelate Compounds.
Ni-BPyMeNi-BPyNH2Ni-BPyNi-Naph
Formula (Expected)C15H10N6Ni2C14H9N9Ni2C14H8N6Ni2C12H6N6Ni2
Formula (Determined)C19H22N6Ni2O2S2C18H21N7Ni2O2S2C7H7N4NiC12H18N10Ni2
Formula weight546.96543.92205.88419.78
Temperature (K)100(2)100(2)100(2)100(2)
Wavelength (Å)0.413280.44280.413280.41328
Crystal systemMonoclinicOrthorhombicOrthorhombicTriclinic
Space groupP2/nCmcaPnnmP-1
Unit cell dimension
a (Å)13.3483(14)14.7000(5)7.2641(9)7.0315(3)
b (Å)7.1002(7)22.6879(7)9.9285(12)7.9219(3)
c (Å)13.5625(14)13.8028(4)11.4008(14)8.6103(3)
α (°)67.8160(10)
β (°)114.834(2)72.2820(10)
γ (°)73.6980(10)
V (Å3)1166.5(2)4603.4(2)822.2(2)415.51(3)
Z2841
Dcal, mg/m31.5571.5701.6631.678
µ (mm−1)0.4120.4620.4750.517
F(000)5622216420216
θ range (°)1.044 to 14.3491.379 to 23.4561.581 to 14.3511.524 to 23.837
Index ranges−16 ≤ h ≤ 1−24 ≤ h ≤ 20−8 ≤ h ≤ 8−13 ≤ h ≤ 13
−8 ≤ k ≤ 8−40 ≤ k ≤ 39−11 ≤ k ≤ 9−15 ≤ k ≤ 14
−16 ≤ l ≤ 16−17 ≤ l ≤ 22−13 ≤ l ≤ 12−10 ≤ l ≤ 15
No. reflections1410133326641012740
R(intensity)0.08660.08620.1120.0435
Completeness, θ(%)14.357(99.9)15.407(97.1)14.357(94.3)14.357(96.9)
Refinement methodFull matrix LSQ on F2Full matrix LSQ on F2Full matrix LSQ on F2Full matrix LSQ on F2
Data/restraints/parameters2116/6/1695839/48/159740/0/815162/0/148
Goodness-of-fit on F21.1521.0541.0861.030
R indices [I>2sigma(I)]
R10.05860.09230.03930.0300
wR20.14630.25820.10720.0750
R indices (all data)
R10.09910.15870.04110.0424
wR20.17540.30220.11030.0801
Extinction coefficient0.18(3)
Largest diff. peak (e.Å−3)0.9022.9521.0080.751
Largest diff. hole (e.Å−3)−0.523−2.676−0.65−0.729

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MDPI and ACS Style

Wong-Ng, W.; Culp, J.T.; Chen, Y.-S. Crystallography of Representative MOFs Based on Pillared Cyanonickelate (PICNIC) Architecture. Crystals 2016, 6, 108. https://doi.org/10.3390/cryst6090108

AMA Style

Wong-Ng W, Culp JT, Chen Y-S. Crystallography of Representative MOFs Based on Pillared Cyanonickelate (PICNIC) Architecture. Crystals. 2016; 6(9):108. https://doi.org/10.3390/cryst6090108

Chicago/Turabian Style

Wong-Ng, Winnie, Jeffrey T. Culp, and Yu-Sheng Chen. 2016. "Crystallography of Representative MOFs Based on Pillared Cyanonickelate (PICNIC) Architecture" Crystals 6, no. 9: 108. https://doi.org/10.3390/cryst6090108

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