Term
| Intermolecular Forces General Characteristics |
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Definition
| Weak, Temperature dependent, concentration dependent, intermolecular, reversible |
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| Intermolecular Forces Active Role In Drug Physical Chemistry |
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Definition
| distribution between immiscible phases, heat of fusion, heat of vaporization, melting point, boiling point, polymorphism, solubility, interfacial phenomena |
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Definition
| Definite, exact melting points, locked together by imf |
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Definition
Hard and brittle with high melting points
ionic bonds |
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Definition
vanderwaals forces and H-bonds
Soft, with low melting points |
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Definition
| different crystalline forms of the same substance. organic or inorganic. May have different MP, solubility, and therapeutic responses |
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| Amorphous forms (solid-state) |
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Definition
| non-crystalline powders, do not have sharp melting points. amorphous form sometimes preferred over crystalline form of the drug |
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Definition
occur during crystallization when some chemicals trap a fixed ratio of solvent molecules in the crystalline (solid state)
*If the solvent is water, it is a hydrate |
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Definition
| large molecules made of repeating units connected by covalent bonds PEGS can be solids or liquids |
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Definition
| inversely proportional to MW |
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Definition
| freeze-drying apparatus, sucks all the air out of the chamber with a vacuum |
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Definition
F=C-P+2
F= number of independent variables
C = # components
P = Number of Phases |
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Definition
| when two different substances, crystals, amorphous solids, together and you get the sweet spot where everything starts |
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Definition
| Transfer of energy to change the surrounding |
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Definition
| Proportional to amount, mass, volume, enthalpy, gibbs free enrgy, entropy etc |
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Definition
| independent of amount: density, temperature, surface tension, mp, bp |
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Definition
| Energy cannot be created or destroyed, it can only be transformed |
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Term
| Second Law Thermodynamics |
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Definition
| Systems have the tendency of increasing entropy, maximizing probabilites |
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Definition
| The entropy of a pure perfect crystal substance is zero at absolute zero (0k) |
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Definition
| Homogeneous Molecular dispersions with particle size <10A they are a mixture of two or more components that form a single phase |
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Definition
| Homogeneous or heterogeneous dispersions with particles size ranging from 10 to 5000 A heterogeneous colloids may undergo phase seperation |
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Definition
| hetergoenous dispersion with particle size >5000A eg supsensions and emulsions |
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Term
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Definition
| In chemistry, colligative properties are properties of solutions that depend upon the ratio of the number of solute particles to the number of solvent molecules in a solution, and not on the type of chemical species present. |
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Definition
| When a nonvolatile solid is dissolved in a liquid the vapor pressure of the solvent is lowered |
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Definition
| pressure difference btwn a pure solvent and a solution separated by a semipermeable membrane that allows the passage of the solvent |
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Definition
pi = R x T x m
\ pi is osmotic pressure in atm
R = 0.082
T = Absolute temperature in degrees Kelvin
m = solute molality |
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Definition
| Independent of size or identity of the solute |
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| Melting and freezing point depression, Osmotic PRessure, etc with "i's" (vant hoff factors) |
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Definition
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Definition
| Solutions with the same osmotic pressure are called isosmotic solutions. Implies physical chemical stability |
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Definition
| A solution that has the same tone (biological compatibility) of body fluids.Same colligative properties magnitudes of body fluids, i.e., same vapor pressure etc. implies biolgical compatability |
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| Hypertonic Or Hypotonic Effect on RBC |
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Definition
Hypotonic: RBC will cause cell swelling and lysis.
Hypertonic: will cause RBC shrinkage |
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Definition
| the weight of NaCl that produces the same osmotic effect as 1g of the drug |
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Definition
| depend on the number of dissociated ions; NaCl = 2 mOsmol. CaCl2 = 3mOsmol |
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