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Coordination polymers are inorganic structures containing metal cation centers linked by ligands, extending in an array. They can also be described as polymers whose repeat units are coordination complexes. Similar supramolecular archatectures are also called Metal-organic frameworks (MOFs), and coordination networks, with some inconsistancy in the distinctions between the terms.[1] Coordination polymers span scientific fields such as organic and inorganic chemistry, biology, materials science, electrochemistry, and pharmachology, having many potential applications.[2] This interdisciplinary nature has lead to extensive study in the past few decades.[3]
Coordination polymers can be classified in a number of different ways due to particular aspects of structure and composition. One important classification is referred to as dimensionality. A structure can be determined to be one, two or three dimensional, depending on the number of directions in space the array extends in. A one dimensional structure extends in a straight line (along the x axis); a two dimensional structure extends in a plane (two directions, x and y axes); and a three dimensional structure extends in all three directions (x, y, and z axes).[4] This is depicted in Figure 1.
History
[edit]Even though coordination polymers have experienced a research boom in the past decade or so, research in this field has been around for a long time. Alfred Werner, sometimes called the father of coordination chemistry, won the Nobel Prize for Chemistry in 1913 for "for his work on the linkage of atoms in molecules, by which he has thrown new light on earlier investigations and opened up new fields of research especially in inorganic chemistry."[5] This work laid a lot of the ground work for the future study of coordination polymers. Terms ubiquitous in the field, such as coordination number, were coined by Werner. He also determined that even neutral, stable molecules in their own right (such as ammonia or water) can behave like ligands, and enter into coordination bonds with metals.
In the past few decades, research in this field has boomed, partially because of the potential applications for metal-organic frameworks (MOF's) in areas such as hydrogen storage.
Synthesis and Propagation
[edit]Much of the mechanism for growth croordination polymers is based on self-assembly, involving crystallization of a metal salt with a ligand. This can be achieved by known crystallization and crystal engineering techniques, the details which are the subject of on-going research. The mechanisms of Molecular self-assembly processes on a molecular level are also currently being investigated, however it is accepted that coordination generally emerges due to the interaction of lone pairs of electrons on the ligand with the regions of low electron density on the cationic metal ion. [2] Crystals of coordination polymers are nucleated when an aggregate of coordinated ligand/metal complexes reaches a size where lowered energy of the bulk is more significant than the added surface energy, meaning that the grain will be driven to grow and unlikely to de-aggregate. This phanomonon is known as nucleation, and the nucleus is a localized, thermodynamic site for crystal growth to occur. More molecules (metals and ligands) can self-assemble onto the growing crystal in a periodic array.
The forces that lead to spontaneous arrangement of molecules (metal-ligand complexes in this case) are thought to be van der Waals forces, pi-pi interactions, hydrogen bonding, and stabilization of pi bonds by polarized bonds in addition to the coordination bond formed between the metal and the ligand. These intermolecular forces tend to be weak, with a long equilibrium distance (bond length) compared to covalent bonds. The pi-pi interactions between benzene rings, for example, have energy roughly 5-10 kJ/mol and optimum spacing 3.4-3.8 angstroms between parallel faces of the rings.
One of the main goals of the field of crystal engineering is the ability to predict the crystal structure of a coordination polymer based on the properties of the metal cations and ligands used. Additionally, because of the number of different variables that can be changed when synthesizing a coordination polymers, it is impossible right now to draw any all encompassing correlations between particular structural aspects and applications.
The synthesis methods utilized to produce coordination polymers are generally the same methods used to grow any crystal. These generally include solvent layering (slow diffusion), slow evaporation, and slow cooling. (Because the main method of characterization of coordination polymers is X-ray crystallography, growing a crystal of sufficient size and quality is important.)
Ligands
[edit]In most coordination polymers, a ligand (or group of atoms) will formally donate a lone pair of electrons to a metal cation and form a coordination complex via a Lewis acid/ base relationship (lewis acids and bases). Coordination polymers are formed when a ligand has the ability to form multiple coordination bonds and act as a bridge bridge between multiple metal centers. Ligands that can form one coordination bond are referred to as monodentate, but those which form multiple coordination bonds, which could lead to coordination polymers are called polydentate. Polydentate ligands are particularly important because it is through ligands that connect multiple metal centers together that an infinite array is formed. Polydentate ligands can also form multiple bonds to the same metal (which is called chelation). Monodentate ligands are also referred to as terminal because they do not offer a place for the network to continue. Often, coordination polymers will consist of a combination of poly- and monodentate, bridging, chelating, and terminal ligands.
Chemical Composition
[edit]Almost any type of atom with a lone pair of electrons can be incorporated into a ligand. Ligands that are commonly found in coordination polymers include polypyridines, pehnanthrolines, hydroxyquinolines and polycarboxylates. Oxygen and nitrogen atoms are commonly encountered as binding sites, but other atoms, such as sulfur[6] and phosphorus,[7][8] have been observed.
Ligands and metal cations tend to follow hard soft acid base theory (HSAB) trends. This means that larger, more polarizable soft metals will coordinate more readily with larger more polarizable soft ligands, and small, non-polarizable, hard metals coordinate to small, non-polarizable, hard ligands.
Structural Orientation
[edit]Ligands can be flexible or rigid. A rigid ligand is one that has no freedom to rotate around bonds or reorient within a structure. Flexible ligands can bend, rotate around bonds, and reorient themselves. This creates more variety in the structure. There are examples of coordination polymers that include two configurations of the same ligand within one structure,[9] as well as two separate structures where the only difference between them is ligand orientation.
Metal Centers
[edit]Also called nodes or hubs, each metal center bonds to a specific number of linkers at well defined angles. The number of linkers bound to a node is known as the coordination number, which, along with the angles they are held at, determines the dimensionality of the structure. The coordination number and coordination geometry of a metal center is determined by the nonuniform distribution of electron density around it, and in general the coordination number increases with cation size. Several models, most notibly hybridization model and molecular orbital theory, use the Schrodinger equation to predict and explain coordination gormetry, however this is difficult in part because of the commplex effect of environment on electron density distrobution.[10]
Transition Metals
[edit]Transition metals are commonly used as nodes. Partially filled d orbitals, either in the atom or ion, can hybridize differently depending on environment. This electronic structure causes some of them to exhibit multiple coordination geometrys, particularly Cu and Ag ions which, full d10 layers as neutral atoms.
Lanthanides
[edit]Lanthanides are large atoms with coordination numbers varying from 7 to 10 due to filling of f orbitals. They are strongly effected by their environment and difficult to pridict, makeing them challangeing to use as nodes. This challange may be worth it however, because the bonds formed by multiplexing(attaching to multiple linkers) have characteristic luminescent wavelengths.
Alkali/Alkaline Earth Metals
[edit]Alkali metals and alkaline earth metals exist as stable cations. Alkali metals readily form cations with stable valence shells, giving them different coordination behavior than lanthanides and transition metals. They are strongly effected by the counter ion they came with, which is hard to avoid.
Other Factors
[edit]
Counter Ion
[edit]Besides metal and ligand choice, there are many other factors that effect the structure of the coordination polymer. For example, most metal centers are positively charged ions which exist as salts. The counter ion in the salt can effect the overall structure. For example, silver salts such as AgNO3, AgBF4, AgClO4, AgPF6, AgAsF6 and AgSbF are all crystallized with the same ligand, the structures vary in terms of the coordination environment of the metal, as well as the dimensionality of the entire coordination polymer. [11]
Crystallization Environment
[edit]Additionally, variations in the crystallization environment can also change the structure. Changes in pH[12], exposure to light, or changes in temperature[13] can all change the resulting structure. Influences on the structure based on changes in crystallization environment are determined on a case by case basis.
Guest Molecules
[edit]The structure of coordination polymers often times incorporates empty space in the form of pores or channels. This empty space is thermodynamically unfavorable. In order to stabilize the structure and prevent collapse, the pores or channels are often occupied by guest molecules. Guest molecules do not form bonds with the surrounding lattice, but sometimes interact via intermolecular forces, such as hydrogen bonding or pi stacking. Most often, the guest molecule will be the solvent that the coordination polymer was crystallized in, but can really be anything (other salts present, atmospheric gases such as oxygen, nitrogen, carbon dioxide, etc.) The presence of the guest molecule can sometimes influence the structure by supporting a pore or channel, where otherwise none would exist.
Applications
[edit]Molecular Storage
[edit]Thanks to coordination polymerization in three dimensions, pores within the structure can be made. The size and shapes of the pore can be controlled by the linker size and the connecting ligands’ length and functional groups. To modify the pore size in order to achieve effective adsorption, nonvolatile guests (host-guest chemistry) are intercalated in the porous coordination polymer space to decrease the pore size. Active surface guests can also be used contribute to adsorption. For example, the large-pore MOF-177, 11.8 Å in diameter, can be doped by C60 molecules (6.83 Å in diameter) or polymers with a highly conjugated system in order to increase the surface area for H2 adsorption. Flexible porous coordination polymers are also convenient for molecular storage, since their pore sizes can be easily altered by physical changes. And example of this might be seen in a polymer that contains gas molecules in its normal state, but upon compression the polymer collapses and releases the stored molecules. Depending on the crystal structure of the polymer, it is possible that the structure be flexible enough that collapsing the pores is reversible and the polymer can be reused to uptake the gas molecules again.[14]
Luminescence
[edit]Luminescence arises from electronic transitions from an excited state, caused by photoexcitation, to the ground state, resulting in the emission of light. Most luminescent compounds require organic chromophoric ligands, which absorb light and then pass the excitation energy to the metal ion, which is referred to as a ligand-to-metal charge-transfer process (LMCT). Coordination polymers are potentially the most versatile luminescent species due to their emission properties being coupled with guest exchange. Coordination polymers also tend to have higher thermal stability than organic species alone, broadening their applications.[15]
Magnetism
[edit]Magnetism in coordination polymers is of interest, however, achieving long-range magnetic order throughout a polymer by coupling the spins of the paramagnetic centers. Since intramolecular interactions (such as bonding) are much more efficient than intermolecular interactions (i.e. through space), 3D coordination polymers are of interest because they connect their magnetic centers through direct coordinative links, and have the possibility for displaying high critical temperatures.[15]
Sensor Capability
[edit]Coordination polymers can also show color changes upon the change of solvent molecules incorporated into the structure. An example of this would be the two Co coordination polymers of the [Re6S8(CN)6]4- cluster that contains water ligands that coordinate to the cobalt atoms. This originally orange solution turns either purple or green with the replacement of water with tetrahydrofuran, and blue upon the addition of diethyl ether. The polymer can thusly act as a solvent sensor that physically changes color in the presence of certain solvents. The color changes are attributed to the incoming solvent displacing the water ligands on the cobalt atoms, resulting in a change of their geometry from octahedral to tetrahedral.[15]
See Also
[edit]References
[edit]- ^ Carlucci, Lucia (1999). "Coordination polymers and supramolecular architectures". Retrieved 26 March 2010.
{{cite web}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ a b Fromm, K. (2007). "Coordination polymer networks with s-block metal ions". Coord. Chem. Rev. 252 (8–9): 856–885. doi:10.1016/j.ccr.2007.10.032.
- ^ You, X. (2006). "Synthesis, structures and properties of alkaline earth metal benzene-1,4-dioxylacetates with three-dimensional hybrid networks". Coord. Chem. Rev. 359. Elsevier: 3257–3263.
- ^ Chen, X (2005). "Metal-organic molecular architectures with 2,2′-bipyridyl-like and carboxylate ligands". Coord. Chem. Rev. 249 (5–6). Elsevier: 545–565. doi:10.1016/j.ccr.2004.07.006.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ "Nobel Prize in Chemistry 1913: Presentation Speech". Amsterdam: Elsevier Publishing Company. 1996. Retrieved 29 March 2010.
- ^ Yan, S. (2001). "Silver(I) coordination polymers of cyclic sulfur ligand, 2,2′,3,3′-tetrahydro-4,4′-dithia-1,1′-binaphthylidene". Inorg. Chim. Acta. 322 (1–2): 133–137. doi:10.1016/S0020-1693(01)00556-4.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Hung-Low, F (2009). "Effect of anion and ligand ratio in self-assembled silver(I) complexes of 4-(diphenylphosphinomethyl)pyridine and their derivatives with bipyridine ligands". Inorg. Chim. Acta. 20 (2): 426–436. doi:10.1016/j.ica.2008.04.032.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Leone, G (2009). "Well-defined transition metal complexes with phosphorus and nitrogen ligands for 1,3-dienes polymerization". Coord. Chem. Rev. 254: 661–676.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Keller, S. (2002). "A Mixed-Ligand Coordination Polymer from the in Situ, Cu(I)-Mediated Isomerization of Bis(4-pyridyl)ethylene". Inorg. 41 (22). ACS: 5650–5652. doi:10.1021/ic025836c. PMID 12401066.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Bernstein, Jeremy (April 3, 2000). Modern Physics. Prentice-Hall. p. 624. ISBN 978-0139553110.
{{cite book}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Rizzato, Silvia (2002). "New polymeric networks from the self-assembly of silver(I) salts and the flexible ligand 1,3-bis(4-pyridyl)propane (bpp). A systematic investigation of the effects of the counterions and a survey of the coordination polymers based on bpp". CrystEngComm. 4 (22). RCS: 121–129. doi:10.1039/b201288j.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Zhou, Z. (2009). "pH- and mol-ratio dependent formation of zinc(II) coordination polymers with iminodiacetic acid: Synthesis, spectroscopic, crystal structure and thermal studies". J. Of Sol. Stat. Chem. 182 (10): 2698–2706. doi:10.1016/j.jssc.2009.06.042. PMC 2778864. PMID 20161370.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Ng, S. (2005). "Supramolecular Isomerism in Cadmium Hydroxide Phases. Temperature-Dependent Synthesis and Structure of Photoluminescent Coordination Polymers of α- and β-Cd2(OH)2(2,4-pyda)". Cryst. Grow. & Des. 5 (3): 837–839. doi:10.1021/cg049610r.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Bureekaew, Sareeya (2007). "Chemistry and Application of Flexible Porous Coordination Polymers". Sci. Technol. Adv. Mater. 9: 2–4.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ a b c Stuart R. Batten (2008). Coordination Polymers: Design, Analysis and Application. RSC Publishing. p. 297-307, 396-407.