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Physical Pharmacy > STATES OF MATTER > Flashcards

STATES OF MATTER Flashcards

1
Q

Three Primary States of Matter

A
  1. Solid
  2. Liquid
  3. Gas
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2
Q

Mesophases

A
  1. Liquid crystalline state
  2. Supercritical fluids
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3
Q
  • IM Forces is enough, but weaker than gasses
  • has definite volume and shape
  • dependent on the shape of the container
A

LIQUID

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4
Q
  • greater kinetic energy than any molecules
  • has no definite shape and volume
A

GAS

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5
Q
  • impact and definite shape and size
  • not dependent on the shape of the container
  • molecules are locked in position
A

SOLID

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6
Q

Temperature – 0 degrees C or 273.13 K

A

Temperature

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7
Q

Addition of energy

A

heat

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8
Q

Gas molecules travel in random paths

A

THE GASEOUS STATE

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9
Q

Liquid to gas

A

evaporation

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10
Q

Solid to liquid

A

melting

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11
Q

force per unit area; recorded in atmospheres or in mm of mercury (mmHg)

A

Pressure

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12
Q

Gas to liquid

A

condensation

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13
Q

NH3 Critical temperature

A

132

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14
Q

Solid to gas

A

sublimation

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15
Q

Liquid to solid

A

freezing

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16
Q

A lot os space between the particles compared to the size of the particles themselves

A

Kinetic Molecular Theory

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17
Q

Gas to solid

A

deposition

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18
Q

Pressure is inversely proportional to volume

A

Boyle’s Law (PiV)

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19
Q

expressed in L or cubic centimeters
(1 cm3 = 1 mL)

A

Volume

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20
Q

The speed that the particles move increases with increasing temperature

A

Kinetic Molecular Theory

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21
Q

Ideal Gas Equation

A

PV = nRT

n = number of moles
R = Gas constant (0.0821 L. atm / mole K)

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22
Q

Pressure is directly proportional to Temperature

A

Gay-Lussac’s Law (PdT)

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23
Q

Gas constant

A

(0.0821 L. atm / mole K)

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24
Q

When there is a cooling or compression of gasses it will turn into liquid and vice versa.

A

Liquefaction of Gases

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25
Q

Volume is directly proportional to Temperature

A

Charle’s Law (VdT)

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26
Q

Collection of particles in constant motion

A

Kinetic Molecular Theory

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27
Q

the pressure required to liquify a gas at its critical temperature; highest vapor pressure that liquid can have;

Water’s CP = 218 atm

A

Critical Pressure

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28
Q

No attraction or repulsions between particles; collisions like billiard ball collisions

A

Kinetic Molecular Theory

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29
Q

CO2 Critical temperature

A

31.2

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30
Q

CO Critical temperature

A

-141

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31
Q

point where liquid does not exist

A

Critical point

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32
Q

NH3 Critical temperature

A

132

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33
Q

the temperature which a liquid can longer exist;

Water’s CT = 374 degrees C or 647 K

A

Critical Temperature

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34
Q

C2H6O (Ethanol) Critical temperature

A

216

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35
Q

C3H8 (Propane) Critical temperature

A

97

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36
Q

CH4 (Methane) Critical temperature

A

-82

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37
Q

H2O (Water) Critical temperature

A

37

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38
Q

SO2 (Sulfur dioxide) Critical temperature

A

157

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39
Q

CO Critical Pressure

A

35.9

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40
Q

C2H6O Critical Pressure

A

65

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41
Q

CH4 Critical Pressure

A

45.8

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42
Q

NH3 Critical Pressure

A

115

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43
Q

CO2 Critical Pressure

A

77

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44
Q

C3H8 Critical Pressure

A

42

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45
Q

SO2 Critical Pressure

A

77.8

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46
Q

H20 Critical Pressure

A

217.8

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47
Q

 Depends on the cooling effect produced as gas expands using a Dewar or vacuum flask

 Ideal gas expand rapidly and no heat enters system

A

Adiabatic expansion

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48
Q

Propellants

A

CFC, HFC, N, CO2

49
Q

 Highly compressed non-ideal gas expands into a region of low pressure

 Leading to a drop in temperature resulting from energy used to bread the bonds between molecules

 Necessary to pre cool the gas before expansion – gas does external work

A

Joule-Thompson Effect

49
Q

A material that is liquid under the pressure conditions existing inside the container but that forms a gas under normal atmospheric condition

A

AEROSOLS

50
Q

 Gases can be liquefied under high pressures in a closed chamber as long as the chamber is maintained below the critical temperature.

 When the pressure is reduced, the molecules expand and the liquid reverts to a gas

A

AEROSOLS

51
Q

The temperature at which the vapor pressure of the liquid is equal to the external or atmospheric pressure.

A

BOILING POINT

51
Q

When the rate of condensation is equal to the rates of vaporization at a definite temperature, the vapor becomes saturated and dynamic __________ is established.

A

equilibrium

51
Q
  • The presence of air above the liquid decreases the rate of evaporation (but EQ is not affected)
  • As the temperature of liquid is elevated, more molecules approach the velocity necessary for escape and pass into the gaseous state = VP increases with increasing temperature
A

EQUILIBRIUM VAPOR PRESSURE

52
Q

Expresses the relationship between the vapor pressure and the absolute temperature

A

Clausius-Clapeyron Equation:
Heat of Vaporization

53
Q

All the heat absorbed is used to change the liquid to vapor, and the temperature does not rise until the liquid is completely vaporized

A

BOILING POINT

53
Q

the heat absorbed by 1 mole of liquid when it passes into the vapor state.

A

Molar Heat of Vaporization

53
Q

Water boils
760 mmHg =

A

100 degrees C (sea level)

53
Q

BOILING POINT
Decreased by:

A
  1. Branching of chain
53
Q

Water boils
700 mmHg =

A

97.7 degrees C

54
Q

Water boils
17.5 mmHg =

A

20 degrees C

54
Q

BOILING POINT
Increased with:

A
  1. Stronger intermolecular binding forces
  2. Increasing number of atoms
54
Q

Mol. Wt. 88.1

A

Butyric acid

54
Q

Mol. Wt. 111.1

A

Sodium butanoate

55
Q

At higher elevations, the atmospheric pressure ________ and the boiling point is lowered

A

decreases

55
Q

Mol. Wt. 88.1

A

Methyl propionate

55
Q

Boiling point 163 degrees C

A

Butyric acid

56
Q

Boiling point 80 degrees C

A

Methyl propionate

56
Q

Boiling point >260 degrees C

A

Sodium butanoate

57
Q

Strongest IMF Dipole - Dipole

A

Methyl propionate

58
Q

Strongest IMF Ionic

A

Sodium butanoate

58
Q

Strongest IMF Hydrogen Bonding

A

Butyric acid

59
Q

IMF in order

A

Ionic > Hydrogen Bonding > Dipole - Dipole > Van der Waals dispersion forces (London Forces)

59
Q

constructed from repeating units called “unit cells” – same size and contain the same number of molecules/ ions arranged in the same way.

A

Crystalline Solids

59
Q

the quantities of heat absorbed when the liquid is vaporized and liberated when the vapors condensed to liquids.

A

Latent Heat of Vaporization

60
Q

changes of the freezing/ melting point in pressure

A

Clapeyron equation

60
Q

ability of the compound to exist in more than one crystal form with different cell parameters

A

Polymorphism

60
Q

Its appearance is described by its overall shape or habit – where it affects:

  • ability to inject a suspension containing a drug in a crystal form
  • flow properties of the drug in the solid state
A

CRYSTALLINE SOLIDS

61
Q

depend on the conditions of crystallization such as:

  • solvents used
  • temperature
  • concentration & presence of impurities
A

Crystal habits

61
Q

Drugs that exhibit polymorphism

A
  • Tristearin (Triglyceride)
  • Chloramphenicol palmitate
  • Unstable liquid ritonavir
  • Cortisone acetate
  • Spiperone
  • Tamoxifen citrate
  • Carbamazepine
62
Q

has the ff. pharmaceutical implications/ formulation problems:

  • May be difficult to inject in suspension form or to formulate as tablets,
  • Transformation during storage can cause changes in crystal size in suspension and eventual caking,
  • Crystal growth in creams as a result of phase transformation can cause the cream become gritty.
  • Changes in polymorphic forms of vehicles used to make suppositories could cause products with different/ unacceptable melting characteristics.
A

Polymorphism

63
Q

When polymorphism occurs, the molecules arrange themselves in two/ more different ways in the crystal.

A

Polymorphism

64
Q

susceptible to polymorphism

A

Sulfonamides & Barbiturates

64
Q

crystallized by polar solvents (alcohols)

A

Beta polymorphs

65
Q

a special case of polymorphism where substances exist in more than one crystalline form. (ex. carbon, sulfur)

A

Allotropic

65
Q

when the change from one form to another is reversible.

A

Enantiotropic

66
Q

crystallized by non polar solvents such (carbon tetrachloride and cyclohexane)

A

Alpha polymorphs

66
Q

Types of Liquid Crystals

A
  1. Smectic
  2. Nematic
66
Q

is a less stable (metastable) crystalline form of carbon. High pressure and temperature lead to the formation of a diamond from elemental carbon

A

Diamond

67
Q

when the transition takes place in one direction only (ex. metastable to stable)

A

Monotropic

67
Q

crystals that contain solvent of crystallization that arise from the entrapped solvent in the crystal.

A

Solvates

67
Q

states that a system at equilibrium readjust so as to reduce the effect an external stress

A

Le Chatelier’s principle

68
Q

CRYSTALLINE SOLIDS

A

Solvates
Hydrates
Anhydrates

69
Q

when water is the solvent/ incorporated in the crystallization

A

Hydrates

70
Q

crystals that have no water of crystallization

A

Anhydrates

71
Q

“supercooled liquids” in which molecules are arranged in random manner as in the liquid state.
(ex. glass, polymers, gels,
beeswax, petrolatum)

A

Amorphous Solids

72
Q

Amorphous solids differs from Crystalline solids in that they tend to flow when subjected to sufficient pressure over a period of time, and they do not have definite melting points.

A

Amorphous solids differs from Crystalline solids

73
Q

the temperature at which a liquid passed in the solid state; also the Melting point of a pure crystalline compound

A

Freezing

73
Q

exhibit similar properties in all directions

A

Isotropic

74
Q

shows different characteristics in various directions along the crystals:

  • Electrical conductance
  • Refractive index
  • Crystal growth
  • Rate of solubility
A

Anisotropic

75
Q

This is the temperature at which the pure liquid and solid exist in equilibrium at an external pressure of one atm

A

Freezing

76
Q

heat absorbed when 1 g of solid melts; the heat liberated when it freezes.

A

Latent Heat of Fusion

77
Q

considered as the heat required to increase the interatomic/ intermolecular distances in crystals (allowing melting to occur)

A

Heat of fusion

77
Q

soap/ grease-like; molecules are mobile in two directions and can rotate about one axis

A

Smectic

77
Q

A crystal that is bound together by weak forces has a low heat of fusion and a low melting point; strong forces – both high

A

Melting point and Intermolecular Forces

77
Q

thread-like; molecules rotate only about one axis but are mobile in three dimensions

A

Nematic

78
Q
  1. Mobile, have the flow properties of liquids
  2. Birefringent, the light passing through a material is divided into different velocities and refractive indices
A

Liquid Crystals

79
Q

formed from the gaseous state where the gas is held under a combination of temperatures and pressures that exceed the critical point of a substance

A

mesophase

80
Q

Applications of Superficial Fluid:

A
  • Extraction
  • Crystallization
  • Preparation of formulation
  • Decaffeination of coffee
81
Q

Formulated by J. Williard Gibbs; a relationship for determining the least number of intensive variable that can be changed without changing the equilibrium state of the system.

A

PHASE RULE

82
Q

a homogenous, physically distinct portion of a system separated from otherportions of the system by bounding surfaces

A

Phase

83
Q

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/ equation

A

Number of components

84
Q

CaCO3 = _______ + ________
combination of any 2 of the chemical species present

A

CaCO3 = Calcium Oxide + Carbon dioxide

85
Q

maximum temperature at which two-phase region exists

Ex. Water and Phenol

A

Critical Solution

86
Q

solid-liquid mixtures in which two components are completely miscible in the liquid state and completely immiscible as solids

Ex. salol-thymol, salol-camphor, & acetaminophen-propyphenazone

A

Eutectic Mixtures

87
Q

the point at which the liquid and solid phases have the same composition/ eutectic composition

A

Eutectic Point

88
Q

composition of two or more compounds that exhibit a melting temperature lower than that of any other mixture of the compounds

A

Eutectic Composition

89
Q

On a phase diagram, the intersection of the eutectic temperature and the eutectic composition gives the ________

A

eutectic point

90
Q

Two-component systems containing Liquid Phases

A

Systems containing one component
Condensed systems

Physical Pharmacy (3 decks)

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