Physical Pharmacy

Question 1

Attraction between SIMILAR molecules

Answer 1

Cohesive Forces

Question 2

Attraction between DIFFERENT molecules

Answer 2

ADhesive Forces

Question 3

Intramolecular Forces of Attraction (2)

Answer 3

1.Covalent Bond
2. Ionic Bond

Question 4

Involves SHARING ‘‘mutual’’ of electrons

Answer 4

Covalent Bond

Question 5

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

Answer 5

Ionic Bond

Question 6

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

Answer 6

1. Polar covalent
2. Non-Polar covalent

Question 7

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

Answer 7

Coordinate covalent bond

Question 8

Intermolecular Forces (IMF) of Attraction (5)

Answer 8

1. Dipole-Dipole interaction
2. Dipole-Induced Dipole
3. Ion-dipole
4. Ion-induced dipole
5. Induced dipole-induced dipole

Question 9

• Aka KEESOM force
• Attractive forces among polar molecules
• Ex: H2O-H2O

Answer 9

Dipole-Dipole interaction

Question 10

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

Answer 10

Dipole-Induced Dipole

Question 11

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

Answer 11

Ion-dipole

Question 12

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

Answer 12

Ion-induced dipole

Question 13

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

Answer 13

Induced dipole-induced dipole

Question 14

VAN DER WAALS FORCES

molecular orientation/alignment

Answer 14

Keesom

Question 15

VAN DER WAALS FORCES

Dispersion effect

Answer 15

LonDon Force

Question 16

VAN DER WAALS FORCES

Induction effect

Answer 16

Debye

Question 17

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

Answer 17

First Law

Question 18

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

Answer 18

Second Law

Question 19

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

Answer 19

Third Law ***

Question 20

Temperature Equilibrium/ Thermal Equilibrium

Answer 20

0th Law

Question 21

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

Answer 21

Gibbs Free Energy

Question 22

The stronger the IMF = _____ boiling point

Answer 22

Increase

Question 23

What Formula is this
∆G=∆H-T∆S

Answer 23

Gibbs Free Energy

Question 24

In Gibb’s Free Energy

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

Answer 24

1. Exothermic (spontaneous)
2. Endothermic (non-spontaneous)
3. Equilbrium

Question 25

* Fluids that follow Newton’s Law * F=nG * Examples: water, oil, alcohol, SOLUTION

Answer 25

Newtonian fluids

Question 26

* Fluids that don’t follow Newton’s Law * Examples: suspension, emulsion, ointment

Answer 26

Non-Newtonian

Question 27

F=nG

Answer 27

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

Question 28

Linear when yield value (f) is exceeded

Answer 28

Plastic

Question 29

* Shear-THINNING * MORE viscous -> less viscous * Inc. G = Dec. n

Answer 29

Pseudoplastic

Question 30

* Shear-THICKENING * LESS viscous -> more viscous * Inc. G =Inc. n

Answer 30

Dilatant

Question 31

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

Answer 31

Thixotropic

Question 32

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

Answer 32

Rheopectic

Question 33

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

Answer 33

Both Newtonian & Non-Newtonian

Question 34

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

Answer 34

Osmosis

Question 35

What governs BUFFER system?

Answer 35

Henderson-Hasselbalch Equation/ Buffer Equation

Question 36

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

Answer 36

Nernst potential

Question 37

Resistance of the surface to an EXPANSION in AREA

Answer 37

Surface Tension

Question 38

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

Answer 38

HLB

Question 39

Molecules or ions that are ADSORBED at INTERFACES

Answer 39

Surfactant

Question 40

The difference between work of ADHESION and work of COHESION

Answer 40

Spreading coefficient

Question 41

1. Solid to Liquid 2. Liquid to Solid

Answer 41

1. Melting 2. Freezing

Question 42

1. Liquid to Gas 2. Gas to Liquid

Answer 42

1. Evaporation 2. Condensation

Question 43

1. Solid to Gas 2. Gas to Solid

Answer 43

1. Sublimation (moth, naphthalene balls) 2. Deposition (dry ice)

Question 44

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

Answer 44

1. VaporiZation curve 2. Sublimation curve 3. Fusion curve

Question 45

TWO-COMPONENT SYSTEM PARTS OF A GRAPH LINE from which a system separates into phases of constant composition

Answer 45

Tie line

Question 46

TWO-COMPONENT SYSTEM PARTS OF A GRAPH TEMP beyond which every proportion exists as 1 phase

Answer 46

Upper consolute temperature

Question 47

TWO-COMPONENT SYSTEM PARTS OF A GRAPH Determines the PROPORTION of each component

Answer 47

Tie line

Question 48

2 Laws that Inversely Proportional are:

Answer 48

1. Boyles Law 2. Graham's Law

Question 49

Ideal Gas Law

Answer 49

PV = nRT

Question 50

Factors Affecting Solubility (5)

Answer 50

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