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M5: Pharmaceutics > Physical Pharmacy > Flashcards

Physical Pharmacy Flashcards

1
Q

Attraction between SIMILAR molecules

A

Cohesive Forces

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2
Q

Attraction between DIFFERENT molecules

A

ADhesive Forces

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3
Q

Intramolecular Forces of Attraction (2)

A

1.Covalent Bond
2. Ionic Bond

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4
Q

Involves SHARING ‘‘mutual’’ of electrons

A

Covalent Bond

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5
Q
  • Aka ELECTROVALENT bond
  • Electrostatic interaction between oppositely charged particles
  • Involves TRANSFER of electrons
A

Ionic Bond

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6
Q

under the Covalent Bond
1. UNEQUAL sharing of electrons
2. EQUAL sharing of electrons

A
  1. Polar covalent
  2. Non-Polar covalent
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7
Q

A covalent bond in which both electrons COME from the SAME ATOM

A

Coordinate covalent bond

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8
Q

Intermolecular Forces (IMF) of Attraction (5)

A
  1. Dipole-Dipole interaction
  2. Dipole-Induced Dipole
  3. Ion-dipole
  4. Ion-induced dipole
  5. Induced dipole-induced dipole
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9
Q
  • Aka KEESOM force
  • Attractive forces among polar molecules
  • Ex: H2O-H2O
A

Dipole-Dipole interaction

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10
Q
  • Aka Debye force
  • Attractive forces between polar and non-polar molecules
  • Example: H2O+oil
A

Dipole-Induced Dipole

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11
Q
  • Attraction between ion and polar molecules
  • Example: NaCl-H2O
A

Ion-dipole

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12
Q
  • a non-polar molecule is polarized by an ion placed near it
  • Example: I2 (non-polar) if added in KI (salt) matutunaw si Iodine
A

Ion-induced dipole

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13
Q
  • Aka London force
  • The only intermolecular force that occur between nonpolar molecules
  • Example: I2-I2
A

Induced dipole-induced dipole

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14
Q

VAN DER WAALS FORCES

molecular orientation/alignment

A

Keesom

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15
Q

VAN DER WAALS FORCES

Dispersion effect

A

LonDon Force

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16
Q

VAN DER WAALS FORCES

Induction effect

A

Debye

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17
Q

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

A

First Law

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18
Q

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

A

Second Law

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19
Q

LAW OF THERMODYNAMICS
*The entropy of a pure substance is 0 when that substance is in a physical state
*Numerical definition of Entropy (S)

A

Third Law ***

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20
Q

Temperature Equilibrium/ Thermal Equilibrium

A

0th Law

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21
Q
  • A measure of CHEMICAL ENERGY
  • Represents the combined contribution of enthalpy and entropy
A

Gibbs Free Energy

22
Q

The stronger the IMF = _____ boiling point

A

Increase

23
Q

What Formula is this
∆G=∆H-T∆S

A

Gibbs Free Energy

24
Q

In Gibb’s Free Energy

1.G<0 (-)
2.G>0 (+)
3.G=0

A
  1. Exothermic (spontaneous)
  2. Endothermic (non-spontaneous)
  3. Equilbrium
25
Q
  • Fluids that follow Newton’s Law
  • F=nG
  • Examples: water, oil, alcohol, SOLUTION
A

Newtonian fluids

26
Q
  • Fluids that don’t follow Newton’s Law
  • Examples: suspension, emulsion, ointment
A

Non-Newtonian

27
Q

F=nG

A

Newtonian fluids
F=shear stress
G=shear rate
n=viscosity

28
Q

Linear when yield value (f) is exceeded

A

Plastic

29
Q
  • Shear-THINNING
  • MORE viscous -> less viscous
  • Inc. G = Dec. n
A

Pseudoplastic

30
Q
  • Shear-THICKENING
  • LESS viscous -> more viscous
  • Inc. G =Inc. n
A

Dilatant

31
Q

*Aka Gel-Sol
Alone (undisturbed): Solid
When Shaken: Liquid

A

Thixotropic

32
Q

*Aka Sol-Gel
Alone (undisturbed): Liquid
When Shaken: Solid

A

Rheopectic

33
Q

Multipoint
Application: (can be use on?)
*Cup and Bob
*Cone and Plate

A

Both Newtonian & Non-Newtonian

34
Q

Transfer solvent for LOW to HIGH solute concentration via semipermeable membrane (barrier)

A

Osmosis

35
Q

What governs BUFFER system?

A

Henderson-Hasselbalch Equation/ Buffer Equation

36
Q

The difference in potential between the ACTUAL SURFACE and the ELECTRONEUTRAL region

A

Nernst potential

37
Q

Resistance of the surface to an EXPANSION in AREA

A

Surface Tension

38
Q

SCALE OF VALUES by means of which it is possible to establish a range of optimum efficiency for each class of surfactants

A

HLB

39
Q

Molecules or ions that are ADSORBED at INTERFACES

A

Surfactant

40
Q

The difference between work of ADHESION and work of COHESION

A

Spreading coefficient

41
Q
  1. Solid to Liquid
  2. Liquid to Solid
A
  1. Melting
  2. Freezing
42
Q
  1. Liquid to Gas
  2. Gas to Liquid
A
  1. Evaporation
  2. Condensation
43
Q
  1. Solid to Gas
  2. Gas to Solid
A
  1. Sublimation (moth, naphthalene balls)
  2. Deposition (dry ice)
44
Q

In Phase Diagram/ Phase Transition
1. ZO
2. XO
3. YO

A
  1. VaporiZation curve
  2. Sublimation curve
  3. Fusion curve
45
Q

TWO-COMPONENT SYSTEM PARTS OF A GRAPH

LINE from which a system separates into phases of constant composition

A

Tie line

46
Q

TWO-COMPONENT SYSTEM PARTS OF A GRAPH

TEMP beyond which every proportion exists as 1 phase

A

Upper consolute temperature

47
Q

TWO-COMPONENT SYSTEM PARTS OF A GRAPH

Determines the PROPORTION of each component

A

Tie line

48
Q

2 Laws that Inversely Proportional are:

A
  1. Boyles Law
  2. Graham’s Law
49
Q

Ideal Gas Law

A

PV = nRT

50
Q

Factors Affecting Solubility (5)

A
  1. Temperature (ENDO & EXOthermic)
  2. Salt (Salting in-Salting out)
  3. pH (Acid & Base)
  4. Particle size
  5. Polar & Non-Polar

M5: Pharmaceutics (12 decks)

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