Phy Pharm Flashcards
(190 cards)
1
Q
- It is the science of the delivery of APIs to the target site to achieve the pharmacological effect
- The study of the ___________ and ___________ properties of drugs and their dosage
forms - It is the application of physics and chemistry in the study of drugs.
A
Physical Pharmacy
physical and chmical
2
Q
The basic and indivisible unit of matter
A
atom
3
Q
Combination of atoms (it may be the same OR different)
A
molecules
4
Q
A charged atom
* It may be a cation or anion
A
Ions
5
Q
A charged molecule
A
Dipole
6
Q
- Bond between Atoms within a molecule
A
Intramolecular
7
Q
Bond between Molecules
A
Intermolecular
8
Q
Non-Metal + Metal
A
Ionic
9
Q
Electronegativity of Ionic
A
> 1.7
10
Q
Crystal Lattice of Salts
A
Ionic
11
Q
Non-Metal + Non-Metal
A
Covalent
12
Q
two types of covalent
A
polar and non polar
13
Q
unequal sharing of electrons
EN :
A
POLAR COVALENT
0.5-1.7
14
Q
equal sharing of electrons
EN:
A
Non polar covalent
<0.5
15
Q
organic compounds
A
covalent
16
Q
metal + metal
A
metallic
17
Q
alloy formation
A
metallic
18
Q
amalgams (Hg)
Brass ( Cu + Zn)
Bronze (Cu + Sn)
A
metallic
19
Q
Weak forces that involve the dispersion of charge across a molecule called a dipole
A
Van der Waals
20
Q
Result from the tendency of molecules to align themselves with the oppositely charged
end of their neighbor
A
Keesom
21
Q
Polar molecules can produce a temporary electric dipole in a non-polar molecule
A
Debye
22
Q
- Responsible for the liquefaction of gases in an aerosolized dosage form.
- Brings about _____________ of non-polar gas molecules
A
London
condensation
23
Q
Solubility of ionic crystals in water
A
ion-dipole
24
Q
Formation of __________ ______, which accounts for solubility of iodine in KI test solution
A
ion-induced dipole
iodide complex
25
Forces necessary to cohere and forces necessary to prevent molecular interpenetration
Repulsive Attractive Forces
26
Uniquely strong Hydrogen + FONS
Hydrogen Bonding
27
Accounts for the unusual properties of water:
* High dielectric constant
* High boiling point
* Low vapor pressure
Hydrogen Bonding
28
* Important in biological structures
* Examples: Micelles and lipid bilayer membranes
Hydrophobic Interactions
29
from strongest to weakest
ionic
covalent
ion dipole
hydrogen bodning
dipole dipole
keesom
debye
london
30
Motion of
Solid _______
Liquid _________
gas ___________
Vibration
Gliding
Random Constant Motion
31
Intermolecular Forces of Attraction
solid __________
liquid __________
gas ____________
strongest
strong
weakest
32
phase between solid and liquid
mesophase
33
gas to plasma ________
plasma to gas ________
ionization
recombination
34
AKA: _______ ___________ _____, “Plasma”
* Exhibit properties intermediate between solids & liquids
* This is partly solid and partly liquid
Mesophase
Liquid Crystalline State
35
tends to flow like liquid under extreme conditions
Exhibits flow like properties
36
divide the passing light into two components with different velocities and refractive index
Birefringent
37
May lead to reorientation of the molecules
Sensitive to Electric Field
38
MOLECULES THAT FORM MESOPHASES
"ROPE"
Rigid
Organic
Polarizable, possess strong dipole
Elongated and Redilinear in Shape
39
* Soap-like or grease-like
* Rotate in _____ AXIS
* Mobile in _____ directions
* “Most pharmaceutical
significance”
Smectic
1 axis
2 directions
40
* Thread-like
* Rotate in ___ axis
* Mobile in ___ directions
Nematic
1 axis
3 directions
41
* Special case
* Chiral nematic
* Highest opacity
Cholesteric
42
have kinetic energy that produces rapid motion
held together by weak intermolecular forces (WEAKEST IFA)
Fills all available space
are compressible
Gas
43
All gases are invisible, except ____ → brownish red, pungent odor
NO2 (Nitrogen dioxide)
44
total volume of gas molecules is negligible as compared to the volume of space in which they are confined
gas particles do not attract one another but rather move independently from each other
particles exhibit continuous random movement due to their kinetic energy &
gas molecules exhibit perfect elasticity
Kinetic Molecular Theory of Gases
45
BOYLE’S LAW
Mariotte's Law
Constant Temperature
Isothermic
Non-linear
46
Gay Lussac's Law
Amonton's Law
Constant Volume
Isochoric
Linear
47
Charles Law
Constant Pressure
Isobaric
Linear
48
Avogadro's Law
Constant Pressure and Temperature
Isobaric
Linear
49
States that solubility of any gas increases as the external pressure is increased
Henry's Law
50
Concerned with the solute
Henry"s Law
51
The partial vapor pressure of the pure constituent multiplied by its mole fraction in the solution.
RAOULT’S LAW
52
Concerned with the solvent
Raoult's Law
53
In Raoult's Law, __________ vapor pressure = _________ solvent
increase, decrease
54
States that the total pressure in a mixture of gases is equal to the sum of the partial pressure of each gas.
Dalton's Law of Partial Pressure
55
This law states that the rate of diffusion of the gas and the speed of the gas molecules are inversely proportional to the square root of molar mass
GRAHAM’S LAW
56
* Diffusion:
* Effusion:
high to low concentration
low to high concentration
57
Classification of Dispersed Systems
True Solution/Molecular Dispersion
Colloidal Dispersion
Coarse Dispersion
58
Particle Size
True Solution _________
Colloidal Dispersion _________
Coarse Dispersion _________
< 0.1 nm
0.1 nm to 0.5 mcm
> 0.5 mcm
59
Visibility
True Solution _________
Colloidal Dispersion _________
Coarse Dispersion _________
invisible
only in electron microscope
ordinary and electron microscope
60
pass thru??
True Solution _________
Colloidal Dispersion _________
Coarse Dispersion _________
filter paper and semi-permeable membrane
filter paper
does not pass thru
61
cheese and butter
colloidal dispersion
62
emulsions and suspensions
coarse dispersions
63
Pressure of the saturated vapor above a liquid resulting from the escape of surface liquid molecules
Vapor Pressure
64
Describes the relationship between vapor pressure and the absolute
temperature of a liquid
Clausius- Clapeyron Equation
65
Heat absorbed by 1 mole of liquid when it passes into vapor state
Molar Heat of Vaporization
66
Molecules or ions dispersed throughout the solvent
solute
67
Do NOT yield ions in solution
NO electric current
Non electrolytes
68
Forms ions in solution
Conductor of electricity
electrolytes
69
Partial ionization, 80% dissociation
weak electrolytes
70
Complete ionization, 100% dissociation
strong electrolytes
71
2 ions _______
3 ions ________
4 ions _______
5 ions ________
1.8
2.6
3.4
4.2
72
* Phase of the solution
* Usually constitutes the largest proportion of the system in which the solute is dissolved
Solvent
73
When a non volatile solute is added to a volatile solvent, the solute reduces the escaping tendency of the solvent.
Vapor pressure lowering
74
Boiling point is when VP = Atmospheric pressure
Boiling point elevation
75
Freezing point is the temperature in which solid and liquid are in equilibrium under a pressure of 1 atm.
Freezing Point Depression
76
the movement of solvent (water) from a higher to lower concentration
osmosis
77
Equal w/ the other solution
0.9% NaCl
D5W
LRS, RS
Isotonic
78
less solute
D2.5W
swelling, bursting, lysis
hypotonic
79
more solute
D10W
crenation, shrinkage
hypertonic
80
METHODS OF DETERMINING TONICITY
Based on the effect on red blood cells suspended in solution
hemolytic method
81
METHODS OF DETERMINING TONICITY
Based on their colligative property, especially freezing point depression
cryoscopic method
82
are solutions that have the property of resisting changes in pH when acids or bases are added to them
buffers
83
this property results from the presence of a buffer pair which consists of either:
1. weak acid + some salt of a weak acid / its conjugate base
2. weak base + some salt of a weak base / its conjugate acid
84
Capacity of the substance to resist change in pH
Buffer capacity
85
most important buffer of blood
Bicarbonate
86
Biological Buffer System:
Phosphates
Oxyhemoglobin
Carbonates
87
Can be used to estimate the pH of a buffered solution by approximating the actual concentration ratio.
Henderson-Hasselbalch Equation
88
> -0.52 deg c
hypotonic
89
< -0.52 deg c
hypertonic
90
attributed to the effect of the properties of molecules located or close to the boundary between immiscible phases
INTERFACIAL PHENOMENA
91
boundary between 2 distinct phases
interphase
92
* force that pulls molecules of the interface together & contracts the surface
* (S-L, L-G)
Surface Tension
93
* force per unit length existing at the interface; between 2 immiscible liquids
* (L-L)
Interfacial Tension
94
Attraction on the surface
Adsorption
95
Permeation into capillary spaces
“Soaking up something”
Absorption
96
Binding force between similar molecules
- Manifests as convex meniscus
Cohesion
97
Binding force between different molecules
- Manifests as concave meniscus
Adhesion
98
Rise of a liquid on a narrow tube
capillarity
99
Surface active agents
They lower the interfacial/surface tension.
Surfactants
100
Aid in attaining intimate contact between solid particles and liquids
Wetting agents
101
Reduces interfacial tension between oil and water, minimizing surface energy through the
formation of globules
Emulsifying agents
102
Reduces surface tension and aid in wetting the surface and the dirt. The soil is emulsified and foaming generally occurs and washing away of the dirt.
Detergents
103
contact angle that a droplet of the liquid makes with the solid
Wetting phenomenon
104
Dependent on the surface and interfacial tension
Represented by the letter __
Spreading coefficient
S
105
Good spreading → ________
Adhesive > Cohesive
Positive S
formation of thin film
106
Bad spreading → ________
Cohesive > Adhesive
Negative S
liquid lens
107
The “degree of wetting”
_____ contact angle → better wetting
contact angle
smaller
108
A system having a particle size (____________) intermediate between that of a true solution and a coarse dispersion.
colloidal dispersion
0.1 nm - 0.5 mcm
109
* Ability to scatter or to disperse light
* Determines the ___________ of the colloid
Faraday-Tyndall Effect
molecular weight
110
Random collision of particles resulting from irregular zigzag motion (erratic movement)
Brownian motion
111
spontaneous movement of the particles from a region of higher concentration to one lower
concentration until the concentration of the
system is uniform throughout.
diffusion
112
Difference in potential between the actual surface of the particle and the electroneutral region of the dispersion
NERNST POTENTIAL /
ELECTROTHERMODYNAMIC
POTENTIAL
113
Difference in potential between the surface of the tightly bound layers and the electroneutral region of the dispersion
ZETA POTENTIAL /
ELECTROKINETIC POTENTIAL
for emulsions
114
* Spontaneous
* Thermodynamically stable
* Organic molecules
ex ___________
LYOPHILIC / HYDROPHILIC
* NaCl, LRS
* Proteins
115
* NON-spontaneous
* Thermodynamically unstable
* Inorganic molecules
ex ______________
LYOPHOBIC / HYDROPHOBIC
* Milk
* IV lipid emulsions
116
Involves surfactants which can accumulate and form micelles, which are colloidal in size
ex _____________
ASSOCIATION / AMPHIPHILIC
* Surfactant micelles
* Liposomes
117
Brownian Motion
increase tempt = ________
Increase particle size = ______
increase viscosity = __________
increase
decrease
decrease
118
Stokes equation
sedimentation rate
119
The number of intensive variables that must be defined to determine the state of the system
Gibb's Phase Rule
120
The least number of variables that can be changed without affecting the equilibrium of the system.
GIBB’S PHASE RULE
121
Formula of Gibb's Phase rule
F= C-P+2
122
F = ___________
degrees of freedom
123
124
The point of a phase diagram at which the three phases of matter coexist
Triple Point
125
The point of a phase diagram at which the substance is indistinguishable between
liquid and gas (supercritical fluid)
critical point
126
From the words, ______ which means “to flow,” and logos which means “science”
rheology
"rheo"
127
Reciprocal of viscosity
fluidity
128
Resistance to flow
viscosity
129
Colloidal property which is affected by the shape of particles of the dispersed phase
viscosity
130
LOW viscosity, LOW solvation
spherocolloids
131
HIGH viscosity, HIGH solvation
linearcolloids
132
Ability to bend without breaking
rheology
133
The application of horizontal force (F) over a unit area (A)
aka ______________
unit ______________
applied force
"shear stress"
dynes/cm2
134
The change in velocity over distance
aka ____________
unit ______________
rate of shear
"shear rate"
1/s
135
Example of Newtonian
alcohol, water
136
Types of Non newtonian
Shear dependent
Time dependent
137
Examples of Shear Dependent
Plastic
Pseudoplastic
Dilatant
138
Examples of Plastic
gels, flocculated, milk, toothpaste
139
Examples of pseudoplastic
PEG, gum, ketchup
140
Example of Dilatant
paint, deflocculated
141
Examples of time dependent
thixotropy
rheopexy
142
example of thixotropy
aqueous bentonite magma
143
example of rheopexy
serum albumin
144
Viscosity stays constant as the applied force changes.
newtonian
145
absolute viscosity _________
kinematic viscosity ________
poise
stoke
146
Does not flow until a shearing stress exceeds a yield value
aka __________
plastic
bingham plastic
147
Substances begin to flow when a shearing stress is applied with no yield value
aka _______________
pseudoplastic
"shear thinning system"
148
Substances deform instantaneously
aka _____________
dilatant
"shear thickening system"
149
* REVERSIBLE GEL-SOL
* Decreased viscosity with time
Thixotropic
150
* IRREVERSIBLE SOL-GEL
* Increased viscosity with time
Rheopexy
151
Regular arrangement
Repetitive 3D units
Crystalline
152
Irregular shape
No definite order
Amorphous
153
x ray diffraction
crystalline ___________
amorphous ___________
definite peaks
noise
154
Application of Crystalline
Long-acting insulin:
* Glargine
* Detemir
* Degludec
155
Application of Amorphous
Rapid-acting insulin:
* Lispro
* Aspart
* Glulisine
156
cubic _______
tetragonal _________
hexagonal _________
triclinic _________
monoclinic __________
rhombic ________
sodium chloride
urea
iodoform
boric acid
sucrose
iodine
157
Polymorphism
Change is reversible
Enantiotropic
158
Polymorphism
Change is irreversible
Monotropic
159
Polymorphism
Properties are similar in all directions
isotropic
160
Polymorphism
Properties are different in all directions
anisotropic
161
Methods of Determining Particle Size
* Most accurate method
* The use of a microscope to measure individual particles
Optical Microscopy
162
Length of a line that bisects the particle image
Martin's diameter
163
Distance between two tangents on opposite sides
Feret's Diameter
164
Diameter of a circle with the same area
Projected Area Diameter
165
Methods of Determining Particle Size
* USP Method
* _____________ = number of square openings per linear inch
Sieve Analysis
sieve or mesh #
166
Methods of Determining Particle Size
Based on the sedimentation rate or free fall velocity of particles
principle: ______
apparatus: _________
Sedimentation method
stoke's law
Andreasen Apparatus / Pipet
167
AUTOMATIC PARTICLE COUNTERS
Electrical resistance
Coulter Counter
168
AUTOMATIC PARTICLE COUNTERS
Light blockage
HIAC / ROYCO INSTRUMENT
169
AUTOMATIC PARTICLE COUNTERS
Faraday-Tyndall Effect
Gelman Counter
170
AUTOMATIC PARTICLE COUNTERS
Photon Correlation Spectroscopy
BECKMAN COUNTER
171
Energy can be transformed from one form to another but cannot be lost, destroyed, or created
1st Law of Thermodynamics
172
Concerned about the entropy (degree of disorderliness or randomness) and spontaneity of a system
2nd law of Thermodynamics
173
The entropy of perfectly crystalline substance is zero
3rd law of Thermodynamics
174
If two systems are in thermal equilibrium respectively with a third system, they must be in thermal equilibrium with each other
Zeroth Law of Thermodynamics
175
METAL-ION
COMPLEXES/
COORDINATION
COMPLEXES
Inorganic
Chelates
Olefin
Aromatic
176
ORGANIC
MOLECULAR
COMPLEXES
Quinhydrone
Picric Acid
Caffeine
Polymer
177
INCLUSION/
OCCLUSION
COMPOUNDS
Channel Lattice
Layer
Clathrates
Monomolecular
Macromolecular
178
One binding Site
Inorganic
179
“Claw”, 2 or more
Donating Group
EDTA
Chelates
180
Alkenes
Olefin
181
Sigma, pi, sandwich
Aromatic
182
Hydroquinone + Benzoquinone
Quinhydrone
183
Acid-base reaction
Butesin picrate
Picric acid
184
+ acidic drugs
To mask bitter taste
caffeine + gentisic acid
Caffeine
185
Nucleophilic oxygen
Hydrophobic interaction
PEG, CMC, PVP,
Polystyrenes, Tetracyclines
Polymer
186
Has a tubular channel
Deoxycholic acid, urea,
amylose, iodine and starch
Channel Lattice
187
Layer of carbon atoms
Graphite, montmorillonite
Layer
188
Cage-like structures
Hydroquinone + warfarin
Clathrates
189
Entrapment in a cavity
Cyclodextrins
Monomolecular
190
Molecular sieves
Zeolites, dextrins, silica gel
Macromolecular
