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Physical pharmacy > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

attraction like molecules

A

cohesion

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2
Q

attraction of unlike molecules

A

adhesion

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3
Q

reaction between two molecules that forces them apart.

A

repulsion

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4
Q

direction of decrease in attraction

A

moving away from one another

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5
Q

direction of increase in attraction

A

moving toward one another

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6
Q

to cohere

A

attractive forces

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7
Q

to prevent from interpenetrating and annihilating each other

A

repulsive forces

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8
Q

is due to the interpenetration of the electronic clouds of molecules and increases exponentially with a decrease in distance between molecules

A

repulsion

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9
Q

Measure of the strength of the bonds

A

bond energies

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10
Q

Hydrogen bonds

A

2-8kcal/mole

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11
Q

Covalent

A

50-100 kcal/mole

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12
Q

Ionic

A

over 100 kcal/mole

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13
Q

solid to liquid

A

melting

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14
Q

solid to gas

A

sublimation

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15
Q

reverse of sublimation; condensation into the solid state

A

deposition

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16
Q

4th phase; in between crystalline and liquid states; “liquid crystalline state”

A

mesophase

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17
Q

exists under high pressure and temperature and has properties intermediate between those of liquids and gases.

A

supercritical fluid

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18
Q

the pressure, temperature, and volume of gas are related to each other

A

Ideal Gas Law

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19
Q

The volume and pressure of a given mass of gas at constant temperature

A

Boyle’s law

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20
Q

the volume and absolute temperature of a given mass of gas at constants pressure are directly proportional

A

Gay-Lussac’s- Charles

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21
Q

The approximate molecular weight of a gas can be determined by use of what law

A

ideal gas law

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22
Q

most common way to determine the molecular weight of easily vaporized liquids such as alcohol and chloroform.

A

Regnault and Victor Meyer Methods

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23
Q

The theory that was developed to explain the behavior of gases and to lend additional support to the validity of the gas laws

A

Kinetic molecular theory

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24
Q

composed of molecules of a finite volume that tend to attract one another.

A

real gases

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25
Q

accounts for the internal pressure per mole resulting from the intermolecular forces of attraction between the molecules

A

a/V2

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26
Q

accounts for the incompressibility of the molecules, that is the excluded volume

A

b

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27
Q

have high internal pressures and serve as solvents only for substances of similar internal pressures

A

polar liquids

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28
Q

have low internal pressures and are not able to overcome the powerful cohesive forces of the polar solvent molecules

A

non-polar solvents

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29
Q

if the temperature is elevated sufficiently, a value is reached above which it is impossible to liquefy a gas irrespective of the pressure applied; the temperature above which a liquid can no longer exist

A

critical temperature

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30
Q

liquids are denser than gases and occupy a definite volume

A

True

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31
Q

an ideal gas is allowed to expand so rapidly that no heat enters the system

A

adiabatic expansion

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32
Q

an ideal gas is allowed to expand so rapidly that no heat enters the system

A

Joule-Thomson Effect

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33
Q

when the rate of condensation equals the rate if vaporization at a definite temperature, the vapor becomes saturated

A

equilibrium

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34
Q

the pressure of the saturated vapor pressure above the liquid

A

Equilibrium vapor pressure

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35
Q

occurs by the precipitation of the compound out of solution and into an ordered array

A

crystallization

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36
Q

show definite melting point, passing sharply from solid to liquid state

A

crystalline solids

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37
Q

6 distinct crystal systems (symmetry)

A 
▪ Cubic- sodium chloride
▪ Tetragonal- urea 
▪ Hexagonal- iodoform 
 Rhombic- iodine 
▪ Monoclinic- sucrose 
▪ Triclinic- boric acid
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38
Q

the morphology of a crystalline form

A

habit

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39
Q

crystallize with their chains lying in a parallel arrangement

A

Aliphatic hydrocarbons

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40
Q

crystallize in layers of dimers with the chains lying parallel or tilted at an angle with respect to the base plane

A

fatty acids

41
Q

hard and brittle; high melting points

A

Ionic and atomic crystals

42
Q

soft; low melting points

A

molecular crystals

43
Q

elemental substances like carbon and sulfur existing in more than one crystalline form

A

allotropic

44
Q

residual solvents can be trapped in the crystalline lattice

A

solvates

45
Q

supercooled liquids in which the molecules are arranged in a somewhat random manner as in the liquid state

A

amorphous solids

46
Q

the temperature at which a liquid passes into the solid state

A

freezing points

47
Q

a system at equilibrium readjusts so as to reduce the effect of an external stress.

A

chatelier’s principle

48
Q

molecules are mobile in two directions and can rotate about one axis

A

SMECTIC

49
Q

Smectic

A

SOAPLIKE OR GREASELIKE

50
Q

the molecules rotate only about one axis but are mobile in three dimensions

A

Surfactants nematic

51
Q

threadlike

A

Surfactants nematic

52
Q

have flow properties of liquids

A

mobile

53
Q

behaves as a gas irrespective of the applied P

A

Critical T

54
Q

is the minimum P required to liquefy a gas at a given temperature

A

Critical P

55
Q

on a DSC arises from desolvations, melting, glass transitions and decompositions.

A

endothermic reaction

56
Q

measured by DSC is usually indicative of a decomposition

A

exothermic reaction

57
Q

determines whether the desolvation may be attributed to water or residual solvents from chemical processing

A

Karl Fischer

58
Q

the ability of a solid to continuously absorb water until it goes into solution

A

Delinquescence

59
Q

weight loss measured under low relative humidity controlled with different salts

A

desorption

60
Q

formulated by J. Willard Gibbs

A

Phase Rule

61
Q

determines the least number of intensive variables that can be changed without changing the equilibrium state of the system

A

Phase Rule

62
Q

as a homogeneous physically distinct portion of a system that is separated from other portions of the system bounding surfaces

A

Phase

63
Q
  • is the smallest number of constituents by which the composition of each phase in the system at equilibrium can be expressed in the form of a chemical formula or equation
A

Number of components

64
Q

Systems in which the vapor phase is ignored and only solid and/or liquid phases are considered

A

Condensed system

65
Q

the composition of two or more compounds that exhibits a melting temperature lower than that of any other mixtures of the compounds

A

Eutectic mixture/composition

66
Q

is the component ratio that exhibits the lowest observed melting point -provides information on solutes interacting in solution

A

Eutectic point

67
Q

the solid phase is an intimate mixture of fine crystals of 2 compounds -results to lowest temperature over a composition range

A

Contact melting

68
Q

are examples of solid dispersions

A

Eutectic systems

69
Q

each solid phase contains both components, that is, a solid solute is dissolved in a solid solvent to give a mixed crystal

A

Solid solutions

70
Q

each solid phase contains both components, that is, a solid solute is dissolved in a solid solvent to give a mixed crystal

A

Solid solutions

71
Q

molecular dispersion of one component in another where the overall solid is amorphous

A

Amorphous or glass solutions

72
Q

pointed to the analogy between human behaviour and molecular phenomena

A

Moelwyn-Hughes

73
Q

refers to the different arrangement of atoms resulting from rotations about single bonds

A

Conformation

74
Q

are weak forces that involve the dispersion of charge across a molecule called a dipole

A

Vander Waals forces

75
Q

dipole-dipole (orientation effect)

A

Keesom forces

76
Q

dipole-induced dipole (conduction effect)

A

Debye force

77
Q

induced- dipole induced-dipole (dispersion effect)

A

London force

78
Q

positive pole

A

cationic

79
Q

negative pole

A

anionic

80
Q

Three primary states of matter

A

o Gases
o Liquids
o Crystalline solids

81
Q

also recorded in atmosphere or in millilitres of mercury because of the use of barometer in pressure movement

A

Pressure

82
Q

mass per unit volume

A

density

83
Q

showed that a lighter gas diffuses more rapidly through a porous membrane than does the heavier one

A

graham

84
Q

special case of polymorphism

A

allotropic

85
Q

is a polymorphous natural fat

A

Theobroma oil, or cacao butter

86
Q

pointed out the relationship between polymorphism and the preparation of cacao butter suppositories

A

Riegelman

87
Q

can also be a factor in suspension technology.

A

Polymorphism

88
Q

Factors that affect the interconversion of the different cortisone acetate forms

A
  1. Heating
  2. Grinding under the water
  3. Suspension in water
89
Q

studied the crystalline forms of tamoxifen citrate, an antiestrogenic and antineoplastic drug used in the treatment of breast cancer and postmenopausal symptoms

A

Goldberg and Becker

90
Q

are sometimes called pseudopolymorphs

A

Solvates

91
Q

change from one form to another is reversible

A

Enantiotrophic

92
Q

transition takes place in one direction only

A

Monotropic

93
Q

glass, pitch and many synthetic plastics

A

Amorphous Solids

94
Q
  • first recorded observation of a thermotropic liquid crystal in 1888 when he heated cholesteryl benzoate.
A

Reinitzer

95
Q

is the most commonly used method and is generally a more useful technique

A

Differential scanning calorimetry

96
Q

the least number of intensive variables that must be fixed/known to describe the system completely

A

Number of degrees of freedom

97
Q

shows the limit of temperature and concentration within which two liquid phases exist in equilibrium

A

Curve gbhci

98
Q

is the point at which the liquid and solid phases have the same composition

A

Eutectic point

Physical pharmacy (1 decks)

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