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In materials science, polymorphism describes the existence of a solid material in more than one form or crystal structure. Polymorphism is a form of isomerism. Any crystalline material can exhibit the phenomenon. Allotropy refers to polymorphism for chemical elements. Polymorphism is of practical relevance to pharmaceuticals, agrochemicals, pigments, dyestuffs, foods, and explosives. According to IUPAC, a polymorphic transition is "A reversible transition of a solid crystalline phase at a certain temperature and pressure (the inversion point) to another phase of the same chemical composition with a different crystal structure."[1] According to McCrone, polymorphs are "different in crystal structure but identical in the liquid or vapor states."[2][3] Materials with two polymorphs are called dimorphic, with three polymorphs, trimorphic, etc.[4]

In some cases, polymorphism was "discovered" on a computer by crystal structure prediction first, before chemists actually synthesize the crystal in the lab.[5]


Many compounds exhibit polymorphism. It has been claimed that "every compound has different polymorphic forms, and that, in general, the number of forms known for a given compound is proportional to the time and money spent in research on that compound."[6][2][7]

Organic compounds

Calcite (on left) and Aragonite (on right), two forms of calcium carbonate. Note: the colors are from impurities.


The phenomenon was discovered in 1832 by Friedrich Wöhler and Justus von Liebig. They observed that the silky needles of freshly crystallized benzamide slowly converted to rhombic crystals.[8] Present-day analysis[9] identifies three polymorphs for benzamide: the least stable one, formed by flash cooling is the orthorhombic form II. This type is followed by the monoclinic form III (observed by Wöhler/Liebig). The most stable form is monoclinic form I. The hydrogen bonding mechanisms are the same for all three phases; however, they differ strongly in their pi-pi interactions.

Maleic acid

In 2006 a new polymorph of maleic acid was discovered, 124 years after the first crystal form was studied.[10] Maleic acid is manufactured on an industrial scale in the chemical industry. It forms salt found in medicine. The new crystal type is produced when a co-crystal of caffeine and maleic acid (2:1) is dissolved in chloroform and when the solvent is allowed to evaporate slowly. Whereas form I has monoclinic space group P21/c, the new form has space group Pc. Both polymorphs consist of sheets of molecules connected through hydrogen bonding of the carboxylic acid groups: in form I, the sheets alternate with respect of the net dipole moment, while in form II, the sheets are oriented in the same direction.


After 125 years of study, 1,3,5-trinitrobenzene yielded a second polymorph. The usual form has the space group Pbca, but in 2004, a second polymorph was obtained in the space group Pca21 when the compound was crystallised in the presence of an additive, trisindane. This experiment shows that additives can induce the appearance of polymorphic forms.[11]

Other organic compounds

Acridine has been obtained as eight polymorphs[12] and aripiprazole has nine.[13] The record for the largest number of well-characterised polymorphs is held by a compound known as ROY.[14][15] Glycine crystallizes as both monoclinic and hexagonal crystals. Polymorphism in organic compounds is often the result of conformational polymorphism.[16]

Inorganic compounds

Binary metal oxides

Polymorphism in binary metal oxides has attracted much attention because these materials are of significant economic value. One set of famous examples have the composition SiO2, which form many polymorphs. Important ones include: α-quartz, β-quartz, tridymite, cristobalite, moganite, coesite, and stishovite.[17] [18]

Metal oxides Phase Conditions of P and T Structure/Space Group
CrO2 α phase Ambient conditionsCl2-type Orthorhombic
RT and 12±3 GPa
Cr2O3 Corundum phase Ambient conditions Corundum-type Rhombohedral (R3c)
High pressure phase RT and 35 GPa Rh2O3-II type
Fe2O3 α phase Ambient conditions Corundum-type Rhombohedral (R3c)
β phase Below 773 K Body-centered cubic (Ia3)
γ phase Up to 933 K Cubic spinel structure (Fd3m)
ε phase -- Rhombic (Pna21)
Bi2O3 α phase Ambient conditions Monoclinic (P21/c)
β phase 603-923 K and 1 atm Tetragonal
γ phase 773-912 K or RT and 1 atm Body-centered cubic
δ phase 912-1097 K and 1 atm FCC (Fm3m)
In2O3 Bixbyite-type phase Ambient conditions Cubic (Ia3)
Corundum-type 15-25 GPa at 1273 K Corundum-type Hexagonal (R3c)
Rh2O3(II)-type 100 GPa and 1000 K Orthorhombic
Al2O3 α phase Ambient conditions Corundum-type Trigonal (R3c)
γ phase 773 K and 1 atm Cubic (Fd3m)
SnO2 α phase Ambient conditions Rutile-type Tetragonal (P42/mnm)
CaCl2-type phase 15 KBar at 1073 K Orthorhombic, CaCl2-type (Pnnm)
α-PbO2-type Above 18 KBar α-PbO2-type (Pbcn)
TiO2 Rutile Equilibrium phase Rutile-type Tetragonal
Anatase Metastable phase (Not stable)[19] Tetragonal (I41/amd)
Brookite Metastable phase (Not stable)[19] Orthorhombic (Pcab)
ZrO2 Monoclinic phase Ambient conditions Monoclinic (P21/c)
Tetragonal phase Above 1443 K Tetragonal (P42/nmc)
Fluorite-type phase Above 2643 K Cubic (Fm3m)
MoO3 α phase 553-673 K & 1 atm Orthorhombic (Pbnm)
β phase 553-673 K & 1 atm Monoclinic
h phase High-pressure and high-temperature phase Hexagonal (P6a/m or P6a)
MoO3-II 60 kbar and 973 K Monoclinic
WO3 ε phase Up to 220 K Monoclinic (Pc)
δ phase 220-300 K Triclinic (P1)
γ phase 300-623 K Monoclinic (P21/n)
β phase 623-900 K Orthorhombic (Pnma)
α phase Above 900 K Tetragonal (P4/ncc)

Other inorganic materials

Classical examples of polymorphism are the pair of minerals calcite and aragonite, both forms of calcium carbonate. Perhaps the most famous example is that of the polymorphs of carbon: graphite and diamond.

β-HgS precipitates as a black solid when Hg(II) salts are treated with H2S. With gentle heating of the slurry, the black polymorph converts to the red form.[20]

Factors affecting polymorphism

According to Ostwald's rule, usually less stable polymorphs crystallize before the stable form. The concept hinges on the idea that unstable polymorphs more closely resemble the state in solution, and thus are kinetically advantaged. The founding case of fibrous vs rhombic benzamide illustrates the case. Another example is provided by two polymorphs of titanium dioxide.[19] Nevertheless, there are known systems, such as metacetamol, where only narrow cooling rate favors obtaining metastable form II.[21]

Polymorphs have disparate stabilities. Some convert rapidly at room (or any) temperature. Most polymorphs of organic molecules only differ by a few kJ/mol in lattice energy. Approximately 50% of known polymorph pairs differ by less than 2 kJ/mol and stability differences of more than 10 kJ/mol are rare.[22] Valuable to mention that polymorph stability may change upon temperature[23][24][25] or pressure.[26][27] Important to note that structural and thermodybnamic stability are different. Thermodynamic stability may be studied using experimental or computational methods.[28][29]

Polymorphism is affected by the details of crystallisation. The solvent in all respects affects the nature of the polymorph, including concentration, other components of the solvent, i.e., species that inhibiting or promote certain growth patterns.[30] A decisive factor is often the temperature of the solvent from which crystallisation is carried out.[31]

Metastable polymorphs are not always reproducibly obtained, leading to cases of "disappearing polymorphs", with usually negative implications on law and business.[6][5][32]

In pharmaceuticals

Main article: Disappearing polymorphs

Legal aspects

Drugs receive regulatory approval and are granted patents for only a single polymorph.

In a classic patent dispute, the GlaxoSmithKline defended its patent for the Type II polymorph of the active ingredient in Zantac against competitors while that of the Type I polymorph had already expired.[33]

Polymorphism in drugs can also have direct medical implications since dissolution rates depend on the polymorph. Polymorphic purity of drug samples can be checked using techniques such as powder X-ray diffraction, IR/Raman spectroscopy, and utilizing the differences in their optical properties in some cases.[34]

Case studies

The known cases up to 2015 are discussed in a review article by Bučar, Lancaster, and Bernstein.[5]


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Multidisciplinary studies involving experimental and computational approaches were applied to pharmaceutical molecules to facilitate the comparison of their solid-state structures. Specifically, this study has focused on exploring how changes in molecular structure affect the molecular conformation, packing motifs, interactions in the resultant crystal lattices and the extent of solid-state diversity of these compounds. The results highlight the value of crystal structure prediction studies and PIXEL calculations in the interpretation of the observed solid-state behaviour and quantifying the intermolecular interactions in the packed structures and identifying the key stabilising interactions. An experimental screen yielded 4 physical forms for clozapine as compared to 60 distinct physical forms for olanzapine. The experimental screening results of clozapine are consistent with its crystal energy landscape which confirms that no alternate packing arrangement is thermodynamically competitive to the experimentally obtained structure. Whilst in case of olanzapine, crystal energy landscape highlights that the extensive experimental screening has probably not found all possible polymorphs of olanzapine, and further solid form diversity could be targeted with a better understanding of the role of kinetics in its crystallisation. CSP studies were able to offer an explanation for the absence of the centrosymmetric dimer in anhydrous clozapine. PIXEL calculations on all the crystal structures of clozapine revealed that similar to olanzapine, the intermolecular interaction energy in each structure is also dominated by the Ed. Despite the molecular structure similarity between amoxapine and loxapine (molecules in group 2), the crystal packing observed in polymorphs of loxa differs significantly from the amoxapine. A combined experimental and computational study demonstrated that the methyl group in loxapine has a significant influence in increasing the range of accessible solid forms and favouring various alternate packing arrangements. CSP studies have again helped in explaining the observed solid-state diversity of loxapine and amoxapine. PIXEL calculations showed that in absence of strong H-bonds, weak H-bonds such as C–H...O, C–H...N and dispersion interactions play a key role in stabilising the crystal lattice of both the molecules. Efficient crystal packing of amoxapine seems to be contributing towards its monomorphic behaviour as compared to the comparatively less efficient packing of loxapine molecules in both polymorphs. The combination of experimental and computational approaches has provided a deeper understanding of the factors influencing the solid-state structure and diversity in these compounds. Hirshfeld surfaces using Crystal Explorer represent another way of exploring packing modes and intermolecular interactions in molecular crystals. The influence of changes in the small substituents on shape and electron distribution can also be investigated by mapping the total electron density on the electrostatic potential for molecules in the gas phase. This allows straightforward visualisation and comparison of overall shape, electron-rich and electron-deficient regions within molecules. The shape of these molecules can be further investigated to study its influence on diverse solid-state diversity.[35]


The original formulations of posaconazole on the market licensed as Noxafil(R) were formulated utilising form I of posaconazole. The discovery of polymorphs of posaconazole increased rapidly and resulted in much research in crystallography of posaconazole. A methanol solvate and a 1,4-dioxane co-crystal were added to the Cambridge Structural Database (CSD).[36]


The antiviral drug ritonavir exists as two polymorphs, which differ greatly in efficacy. Such issues were solved by reformulating the medicine into gelcaps and tablets, rather than the original capsules.[37]


There was only one proven polymorph Form I of aspirin, though the existence of another polymorph was debated since the 1960s, and one report from 1981 reported that when crystallized in the presence of aspirin anhydride, the diffractogram of aspirin has weak additional peaks. Though at the time it was dismissed as mere impurity, it was, in retrospect, Form II aspirin.[5]

Form II was reported in 2005,[38][39] found after attempted co-crystallization of aspirin and levetiracetam from hot acetonitrile.

In form I, pairs of aspirin molecules form centrosymmetric dimers through the acetyl groups with the (acidic) methyl proton to carbonyl hydrogen bonds. In form II, each aspirin molecule forms the same hydrogen bonds, but with two neighbouring molecules instead of one. With respect to the hydrogen bonds formed by the carboxylic acid groups, both polymorphs form identical dimer structures. The aspirin polymorphs contain identical 2-dimensional sections and are therefore more precisely described as polytypes.[40]

Pure Form II aspirin could be prepared by seeding the batch with aspirin anhydrate in 15% weight.[5]


Paracetamol powder has poor compression properties, which poses difficulty in making tablets. A second polymorph was found with more suitable compressive properties.[41]

Cortisone acetate

Cortisone acetate exists in at least five different polymorphs, four of which are unstable in water and change to a stable form.


Carbamazepine, estrogen, paroxetine,[42] and chloramphenicol also show polymorphism.


Pyrazinamide has at least 4 polymorphs.[43] All of them transforms to stable α form at room temperature upon storage or mechanical treatment.[44] Recent studies prove that α form is thermodynamically stable at room temperature.[23][25]


Polytypes are a special case of polymorphs, where multiple close-packed crystal structures differ in one dimension only. Polytypes have identical close-packed planes, but differ in the stacking sequence in the third dimension perpendicular to these planes. Silicon carbide (SiC) has more than 170 known polytypes, although most are rare. All the polytypes of SiC have virtually the same density and Gibbs free energy. The most common SiC polytypes are shown in Table 1.

Table 1: Some polytypes of SiC.[45]

Phase Structure Ramsdell notation Stacking sequence Comment
α-SiC hexagonal 2H AB wurtzite form
α-SiC hexagonal 4H ABCB
α-SiC hexagonal 6H ABCACB the most stable and common form
α-SiC rhombohedral 15R ABCACBCABACABCB
β-SiC face-centered cubic 3C ABC sphalerite or zinc blende form

A second group of materials with different polytypes are the transition metal dichalcogenides, layered materials such as molybdenum disulfide (MoS2). For these materials the polytypes have more distinct effects on material properties, e.g. for MoS2, the 1T polytype is metallic in character, while the 2H form is more semiconducting.[46] Another example is tantalum disulfide, where the common 1T as well as 2H polytypes occur, but also more complex 'mixed coordination' types such as 4Hb and 6R, where the trigonal prismatic and the octahedral geometry layers are mixed.[47] Here, the 1T polytype exhibits a charge density wave, with distinct influence on the conductivity as a function of temperature, while the 2H polytype exhibits superconductivity.

ZnS and CdI2 are also polytypical.[48] It has been suggested that this type of polymorphism is due to kinetics where screw dislocations rapidly reproduce partly disordered sequences in a periodic fashion.


Solid phase transitions which transform reversibly without passing through the liquid or gaseous phases are called enantiotropic. In contrast, if the modifications are not convertible under these conditions, the system is monotropic. Experimental data are used to differentiate between enantiotropic and monotropic transitions and energy/temperature semi-quantitative diagrams can be drawn by applying several rules, principally the heat-of-transition rule, the heat-of-fusion rule and the density rule. These rules enable the deduction of the relative positions of the H and Gisobars in the E/T diagram. [1]

In terms of thermodynamics, two types of polymorphic behaviour are recognized. For a monotropic system, plots of the free energies of the various polymorphs against temperature do not cross before all polymorphs melt. As a result, any transition from one polymorph to another below the melting point will be irreversible. For an enantiotropic system, a plot of the free energy against temperature shows a crossing point before the various melting points.[49] It may also be possible to convert interchangeably between the two polymorphs by heating or cooling, or through physical contact with a lower energy polymorph.

A simple model of polymorphism is to model the Gibbs free energy of a ball-shaped crystal as . Here, the first term is the surface energy, and the second term is the volume energy. Both parameters . The function rises to a maximum before dropping, crossing zero at . In order to crystallize, a ball of crystal much overcome the energetic barrier to the part of the energy landscape.[50]

Figure 2

Now, suppose there are two kinds of crystals, with different energies and , and if they have the same shape as in Figure 2, then the two curves intersect at some . Then the system has three phases:

If the crystal is grown slowly, it could be kinetically stuck in form 1.

See also


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