Solid state
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The document discusses different types of solids including crystalline solids, amorphous solids, and their properties. Crystalline solids have a defined structure and melting point while amorphous solids lack a defined structure. The melting point of a solid is the temperature at which it transitions to a liquid and is dependent on the strength of intermolecular forces, with stronger forces leading to higher melting points. Thermal analysis techniques can be used to characterize materials based on physical and chemical changes like melting point. Polymorphism, which is the ability to exist in multiple crystal structures, is important for pharmaceuticals as different polymorphs can have different properties.
Solid state
- 1. The Solids State General properties Crystalline Solids Amorphous Solids Melting point
- 2. General properties Solids are much denser than both gases and liquids due to the presence of very strong intermolecular forces. Solids are essentially incompressible (small empty spaces) Solids have definite volume and shape (rigid, not fluid) Solids have no translational motion (only vibration)
- 3. Crystalline Solids Crystalline solids, such as sodium chloride, and menthol, are composed of structural units arranged in fixed geometric patterns or lattices. Menthol Sodium Chloride
- 4. Crystalline Solids Crystalline solids show definite melting points, passing rather sharply from the solid to the liquid state. The morphology of a crystalline form is often referred to as its habit, where the crystal habit is defined as having the same structure but different outward appearance.
- 5. Crystalline Solids Types of crystalline solids The units that constitute the crystal structure can be atoms, molecules, or ions . Ionic Solid Lattice units consist of ions held together by ionic bonds e.g. NaCl Atomic Solid Lattice units consist of atoms held together by covalent bonds e.g. diamond Molecular Solid Lattice units consists of molecules held together by van der Waals forces e.g. Solid CO2 Ionic and atomic crystals in general are hard and brittle and have high melting points, while molecular crystals are soft and have relatively low melting points.
- 6. Crystalline Solids Types of crystalline solids Metallic crystals are composed of positively charged ions in a field of freely moving electrons. The atoms are held together by metallic bonding. Metals are good conductors of electricity because of the free movement of the electrons in the lattice. Metals may be soft or hard and have low or high melting points.
- 7. Amorphous Solids Amorphous solids may be considered as supercooled liquids in which the molecules are arranged in a somewhat random manner as in the liquid state. Amorphous Crystalline They differ from crystalline solids in that they tend to flow when subjected to sufficient pressure over a period of time, and they do not have definite melting points.
- 8. Amorphous Solids The amorphous state is unstable compared to the crystalline solid (it has higher energy than crystalline solid). The pharmaceutical advantages of amorphous solid is its higher solubility and bioavailability. Its pharmaceutical disadvantages is its low stability (over time, amorphous solid may transform to the more stable crystalline state).
- 9. Melting point Heat of fusion The temperature at which a solid passes into liquid state is known as the melting point. It is also the freezing point of the liquid state of that solid. The melting point of a pure crystalline solid (or freezing point of a liquid) is the temperature at which the pure liquid and solid exist in equilibrium. Normal melting or freezing point is the temperature of the equilibrium mixture at an external pressure of 1 atm. Unlike the boiling point, the melting point is relatively insensitive to pressure because the solid/liquid transition represents only a small change in volume.
- 10. Melting point Heat of fusion The heat (energy) absorbed when 1 g of a solid melts or the heat liberated when it freezes is known as the latent heat of fusion. ∆𝑻 𝑽𝒍 − 𝑽 𝒔 = 𝑻 ∆𝑷 ∆𝑯 𝒇 Vl and Vs: the molar volumes (cm3/mole) of the liquid and solid, respectively (Molar volume is computed by dividing the gram molecular weight by the density of the compound). ΔHf : the molar heat of fusion (the amount of heat absorbed when 1 mole of the solid changes into liquid) ΔT: the change of melting point brought about by a pressure change of ΔP.
- 11. Melting point Intermolecular forces • The heat of fusion may be considered as the heat required to increase the interatomic or intermolecular distances in crystals, thus allowing melting (increased molecular motion) to occur. • A crystal that is bound together by weak forces generally has a low heat of fusion and a low melting point, whereas one bound together by strong forces has a high heat of fusion and a high melting point.
- 12. Thermal analysis Applications Thermal analysis has many applications in pharmaceutical industry and quality control such as: Melting points for organic and inorganic compounds are often used for thermal analysis for- Characterization and identification of compounds. Determination of purity, polymorphism, and stability. Investigation of drug compatibility with excipient(s).
- 13. Thermal analysis Definition Thermal analysis is a number of methods for observing physical and chemical changes (e.g melting point) of a material upon heating or cooling. The most common types of thermal analysis are: Differntail scanning calorimetry (DSC) Differential thermal analysis (DTA), Thermogravimetric analysis (TGA) Thermomechanical analysis (TMA).
- 14. Polymorphism • Some elements like carbon (Dimond, graphite) and sulphur exist in more than one crystalline form which is known as polymorphism • Diamond is metastable (less stable) form of carbon • Polymorphs exhibit different- • Melting points • Solubility • Formation of different polymorphs depend upon crystallization conditions (Level of supersaturation, temperature)
- 15. Pharmaceutical significance of polymorphs • Nearly all long chain organic compounds exhibit polymorphism • Eg: Triglyceride tristearin shows • Low melting point metastable (α) • Beta prime (β’) • High melting point Stable beta (β) • Theobroma (coca butter) shows 4 forms γ, α, β’ and β. For making suppositories Theobroma should be melted at lowest possible temperature (33C) so that stable polymorph (β MP 34.5C)) should not destroy. • Because of difference in solubilities of polymorphs, one may be more active therapeutically than other. E.g. Sulfameter antimicrobial form II is more active than Form III. • Cortisone acetate suspension … out of 5 forms only one is stable in presence of water. During preparation of suspension stable form should be available to avoid caking.
- 16. References Sinko, P. J. Martin's physical pharmacy and pharmaceutical sciences: physical chemical and biopharmaceutical principles in the pharmaceutical sciences, Philadelphia, Lippincott Williams & Wilkins.