Physical Pharmacy Flashcards
Attraction between SIMILAR molecules
Cohesive Forces
Attraction between DIFFERENT molecules
ADhesive Forces
Intramolecular Forces of Attraction (2)
1.Covalent Bond
2. Ionic Bond
Involves SHARING ‘‘mutual’’ of electrons
Covalent Bond
- Aka ELECTROVALENT bond
- Electrostatic interaction between oppositely charged particles
- Involves TRANSFER of electrons
Ionic Bond
under the Covalent Bond
1. UNEQUAL sharing of electrons
2. EQUAL sharing of electrons
- Polar covalent
- Non-Polar covalent
A covalent bond in which both electrons COME from the SAME ATOM
Coordinate covalent bond
Intermolecular Forces (IMF) of Attraction (5)
- Dipole-Dipole interaction
- Dipole-Induced Dipole
- Ion-dipole
- Ion-induced dipole
- Induced dipole-induced dipole
- Aka KEESOM force
- Attractive forces among polar molecules
- Ex: H2O-H2O
Dipole-Dipole interaction
- Aka Debye force
- Attractive forces between polar and non-polar molecules
- Example: H2O+oil
Dipole-Induced Dipole
- Attraction between ion and polar molecules
- Example: NaCl-H2O
Ion-dipole
- a non-polar molecule is polarized by an ion placed near it
- Example: I2 (non-polar) if added in KI (salt) matutunaw si Iodine
Ion-induced dipole
- Aka London force
- The only intermolecular force that occur between nonpolar molecules
- Example: I2-I2
Induced dipole-induced dipole
VAN DER WAALS FORCES
molecular orientation/alignment
Keesom
VAN DER WAALS FORCES
Dispersion effect
LonDon Force
VAN DER WAALS FORCES
Induction effect
Debye
LAW OF THERMODYNAMICS
* Defines the law of CONSERVATION of energy
* Energy can be INTERCONVERTED, but the sum of energy must remain constant
* Closed system: ∆E = EB - EA
* ∆E is equal to 0 for a cyclic process in a closed system
First Law
LAW OF THERMODYNAMICS
* Defines Entropy (S)
* The entropy of the system plus that of the surroundings must INCREASE in an IRREVERSIBLE process and remains constant in a reversible process
* ∆Ssystem + ∆Ssurr ≥ 0
Second Law
LAW OF THERMODYNAMICS
*The entropy of a pure substance is 0 when that substance is in a physical state
*Numerical definition of Entropy (S)
Third Law ***
Temperature Equilibrium/ Thermal Equilibrium
0th Law
- A measure of CHEMICAL ENERGY
- Represents the combined contribution of enthalpy and entropy
Gibbs Free Energy
The stronger the IMF = _____ boiling point
Increase
What Formula is this
∆G=∆H-T∆S
Gibbs Free Energy
In Gibb’s Free Energy
1.G<0 (-)
2.G>0 (+)
3.G=0
- Exothermic (spontaneous)
- Endothermic (non-spontaneous)
- Equilbrium
- Fluids that follow Newton’s Law
- F=nG
- Examples: water, oil, alcohol, SOLUTION
Newtonian fluids
- Fluids that don’t follow Newton’s Law
- Examples: suspension, emulsion, ointment
Non-Newtonian
F=nG
Newtonian fluids
F=shear stress
G=shear rate
n=viscosity
Linear when yield value (f) is exceeded
Plastic
- Shear-THINNING
- MORE viscous -> less viscous
- Inc. G = Dec. n
Pseudoplastic
- Shear-THICKENING
- LESS viscous -> more viscous
- Inc. G =Inc. n
Dilatant
*Aka Gel-Sol
Alone (undisturbed): Solid
When Shaken: Liquid
Thixotropic
*Aka Sol-Gel
Alone (undisturbed): Liquid
When Shaken: Solid
Rheopectic
Multipoint
Application: (can be use on?)
*Cup and Bob
*Cone and Plate
Both Newtonian & Non-Newtonian
Transfer solvent for LOW to HIGH solute concentration via semipermeable membrane (barrier)
Osmosis
What governs BUFFER system?
Henderson-Hasselbalch Equation/ Buffer Equation
The difference in potential between the ACTUAL SURFACE and the ELECTRONEUTRAL region
Nernst potential
Resistance of the surface to an EXPANSION in AREA
Surface Tension
SCALE OF VALUES by means of which it is possible to establish a range of optimum efficiency for each class of surfactants
HLB
Molecules or ions that are ADSORBED at INTERFACES
Surfactant
The difference between work of ADHESION and work of COHESION
Spreading coefficient
- Solid to Liquid
- Liquid to Solid
- Melting
- Freezing
- Liquid to Gas
- Gas to Liquid
- Evaporation
- Condensation
- Solid to Gas
- Gas to Solid
- Sublimation (moth, naphthalene balls)
- Deposition (dry ice)
In Phase Diagram/ Phase Transition
1. ZO
2. XO
3. YO
- VaporiZation curve
- Sublimation curve
- Fusion curve
TWO-COMPONENT SYSTEM PARTS OF A GRAPH
LINE from which a system separates into phases of constant composition
Tie line
TWO-COMPONENT SYSTEM PARTS OF A GRAPH
TEMP beyond which every proportion exists as 1 phase
Upper consolute temperature
TWO-COMPONENT SYSTEM PARTS OF A GRAPH
Determines the PROPORTION of each component
Tie line
2 Laws that Inversely Proportional are:
- Boyles Law
- Graham’s Law
Ideal Gas Law
PV = nRT
Factors Affecting Solubility (5)
- Temperature (ENDO & EXOthermic)
- Salt (Salting in-Salting out)
- pH (Acid & Base)
- Particle size
- Polar & Non-Polar
