MOD 2 Flashcards
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Molecules PACKED close together closely, vibrating in FIXED POSITION
SOLID
Molecules are close but RANDOMLY ARRANGED
Flows and ASSUMES SHAPE of container
LIQUID
Molecules are FAR APART
Fills any container completely
GAS
In order for molecules to exist in aggregates in gases, liquids, and solids, __________ must exist
INTERMOLECULAR FORCES
responsible for the behavior of molecules in solid, liquid, and gas
INTERMOLECULAR FORCES
Solid → liquid → gas
BREAKING OF BONDS
Gas → liquid → solid
FORMATION OF BONDS
factors that would make bonds either broken or established
TEMPERATURE & PRESSURE
Transition of a substance directly from SOLID state TO a GAS state
SUBLIMATION
A process in which a GAS does DIRECTLY to a SOLID, BYPASSING THE LIQUID PHASE
DEPOSITION
for VASODILATION, volatile, formulated in closed glass tube
AMYL NITRITE (liquid state)
Described as molecules that have HIGHER KINETIC ENERGY (energy in movement) that produces RAPID MOTION
GASEOUS STATE
ENERGY IN MOTION
KINETIC ENERGY
A FORCE per unit area (dynes/cm2) as they COLLIDE to ONE ANOTHER and to WALLS OF THE CONTAINER to which they are confined.
PRESSURE (gas)
Normal atmospheric level within sea level
1 atm or 760 mmHg
PROPERTIES OF GAS
pressure
volume
temperature
- perfectly ELASTIC collision
- NO intermolecular forces of attraction
IDEAL GAS LAW
PRESSURE and VOLUME of gases are INVERSELY PROPORTIONAL
- the lower the volume, the higher the pressure
BOYLE’S LAW
BOYLE’S LAW
pressure & volume are inversely proportional at constant temperature
states that the PRESSURE (p) of a given quantity of gas varies INVERSELY with its VOLUME (v) at CONSTANT TEMPERATURE
ROBERT BOYLE
Volume - Temperature relationship at constant Pressure
- the higher the volume, the higher the temperature
CHARLES’ LAW
CHARLES’ LAW
volume & temperature are directly proportional
what is constant in boyle’s law
TEMPERATURE
what is constant in charles’ law
PRESSURE
what is constant in gay lussac’s law
VOLUME
Pressure - Temperature relationship at constant Volume
- the higher the pressure, the higher the temperature
GAY-LUSSAC’S LAW
States that the PRESSURE of a given amount of gas held at CONSTANT VOLUME is DIRECTLY PROPORTIONAL to the Kelvin TEMPERATURE.
GAY-LUSSAC
States that the VOLUME of an ideal gas is DIRECTLY PROPORTIONAL to the absolute TEMPERATURE at CONSTANT PRESSURE.
CHARLES
IDEAL GAS LAW equation
PV = nRT
unit for volume
L
unit for Temperature
K
unit for Pressure
atm
unit for n
mol
formula if molwt hinahanap
PV = nRT/molwt
molwt = nRT/PV
Describes how gases consist of tiny particles in constant motion, with their behavior influenced by factors like temperature and pressure.
KINETIC MOLECULAR THEORY
The theory that was developed to EXPLAIN THE BEHAVIOR OF GASES and to lend additional support to the VALIDITY OF THE GAS LAWS.
KINETIC MOLECULAR THEORY
The volume of gas is (kinetic mol theo)
NEGLIGIBLE
Who showed that a LIGHTER GAS DIFFUSES MORE RAPIDLY through a porous membrane than does a heavier one
GRAHAM’S LAW
NOT composed of infinitely small and perfectly elastic non-attracting spheres
REAL GASES
▪ Have finite volume
▪ Tend to attract one another
* There is an intermolecular binding force.
REAL GASES
formula for REAL GAS
[P + an2/v2] (V - nb) = nRT
ATTRACTION BETWEEN THE GAS PARTICLES, brought about by intermolecular binding forces that may exist
INTERNAL PRESSURE [an2/v2)
VOLUME OCCUPIED BY THE GAS PARTICLES; volume lost when molecules are held closely together
EXCLUDED VOLUME (nb)
incompressability of molecules
nb - excluded volume
The TEMPERATURE to LIQUEFY THE GAS and establish intermolecular binding forces is
LOW ↓
The PRESSURE to LIQUEFY THE GAS and establish intermolecular binding forces is
HIGH ↑
↓ temperature
↑ pressure
LIQUEFACTION OF GASES
GAS → LIQUID
- Possess LESS kinetic energy than gases
- Occupy a DEFINITE VOLUME denser than gas
- Take the shape of the container
- INCOMPRESSIBLE
LIQUID STATE
Gas molecules LOSE their kinetic energy in the form of
HEAT
- Temperature above which LIQUID NO LONGER EXISTS
CRITICAL TEMPERATURE
- Pressure required to liquefy a gas at Tcrit
CRITICAL PRESSURE
critical temperature of water
374 °C
critical pressure of water
218atm
volume is approx 0
NEGLIGIBLE VOLUME
the particles of GAS DO NOT ATTARCT ONE ANOTHER at ___ pressures
LOW PRESSURES
one of the most obvious ways to liquefy a gas is to subject it to
INTENSE COLD using FREEZING MIXTURES
a rapid EXPANSION of ideal gas to which no heat could enter the system (gas)
ADIABATIC EXPANSION
Adiabatic expansion can be carried out by using ______ which effectively INSULATES the contents of the flask from the external environment
DEWAR or VACUUM FLASK
A ____ is observed when a HIGHLY COMPRESSED NONIDEAL GAS EXPANDS into a region of low pressure
COOLING EFFECT
the COOLING EFFECT that is observed when a HIGHLY COMPRESSED NONIDEAL GAS EXPANDS into a region of low pressure and differs from the cooling produced in adiabatic expansion
JOULE-THOMSON EFFECT
to bring about liquefaction by the Joule-Thomson effect, it may be necessary to __________ before allowing it to expand
PRECOOL THE GAS
a material that is LIQUID under the pressure conditions existing inside the container but that forms a GAS under normal atmospheric conditions
PROPELLANT
traditionally been utilized as propellants but is now BANNED
CHLOROFLUOROCARBONS & HYDROFLUOROCARBONS
Inside the aerosol
REAL GAS
outside the aerosol
IDEAL GAS
Subjecting the propellant into an EXTREME COLD TEMPERATURE and EXTREME HIGH PRESSURE
ADIABATIC EXPANSION
expanding the volume of gas using ideal gas
ADIABATIC EXPANSION
COMPRESSED real gas into an area with LOW PRESSURE
JOULE-THOMSON EFFECT
REMOVING ENERGY FROM THE SYSTEM will provide extreme cold temperature, wherein movement of gaseous molecule will become extremely slow and compress high pressure until intermolecular will exist and gas will be converted to liquid state
JOULE-THOMSON EFFECT
when the rate of condensation EQUALS the rate of vaporization at a definite temperature, the vapor becomes ________ and a dynamic _______ is established
SATURATED, EQUILIBRIUM
the PRESSURE OF SATURATED VAPOR above the liquid
EQUILIBRIUM VAPOR PRESSURE
Absorb heat energy → translated to kinetic energy → gas molecules move and oscillate → bonds are broken → molecules evaporate and converted to gaseous state (water vapor)
OPEN SYSTEM
high pressure (compressed system) → molecules of water vapor are held closed → vapor pressure returns to liquid state
CLOSED SYSTEM
equal evaporation and condensation
EQUILIBRIUM VAPOR PRESSURE
water is lost, all liquid will be converted to GASEOUS STATE
TEMP INCREASES, PRESSURE CONSTANT
NO more liquid state, ONLY VAPOR PRESSURE will exist
PRESSURE INCREASES, TEMP IS CONSTANT
the relationship between the VAPOR PRESSURE and the ABSOLUTE TEMPERATURE of a liquid is expressed by
CLAUSIUS-CLAPEYRON EQUATION
____________ by MOLECULES OF LIQUID so that it will be converted to the GASEOUS STATE
HEAT ABSORBED
_________ by the WATER VAPOR so that it will be converted to LIQUID STATE
HEAT LIBERATED
compute the CHANGE IN TEMPERATURE such as boiling point WHEN THERE IS A CHANGE IN PRESSURE
CLAUSIUS-CLAPEYRON EQUATION
heat absorbed by 1 mole of liquid when it passes to gas
MOLAR HEAT OF VAPORIZATION
the boiling point of water at 1 atm
100C
vapor pressure = atmospheric pressure
BOILING POINT
Drug substances in liquid state
problematic, volatile
Most of the drug substances exists in
CRYSTALLINE OR AMORPHOUS FORM
- They are MOST FAVORABLE drug substance since they are stable.
- Easiest to manipulate and to handle
SOLID
VASODILATOR (liquid) but can formulate as SUBLINGUAL TABLET (under the tongue), VOLATILE IF NOT SEALED PROPERLY
NITROGLYCERIN
They have a definite shape and GEOMETRICAL FORM
CRYSTALLINE
Crystalline solids have a _____ melting point
SHARP
a SOFT solid
GRAPHITE
crystalline solids have ____ cleavage
CLEAN
They have a DEFINITE HEAT OF INFUSION.
CRYSTALLINE SOLIDS
crystalline solids are _____
ANISTROPIC
amorphous solids are ______
ISOTROPIC
different arrangements of lattices/crystalline
HABIT
- Arranged in LATTICES – fixed geometric pattern
- Definite melting points
- Rate and stability
- Habit
CRYSTALLINE SOLIDS
6 CRYSTAL SYSTEMS
CUBIC
TETRAGONAL
HEXAGONAL
RHOMBIC
MONOCLINIC
TRICLINIC
IDENTIFY THE CRYSTAL SYSTEM:
sodium chloride
CUBIC
IDENTIFY THE CRYSTAL SYSTEM:
urea
TETRAGONAL
IDENTIFY THE CRYSTAL SYSTEM:
iodoform
HEXAGONAL
IDENTIFY THE CRYSTAL SYSTEM:
iodine
RHOMBIC
IDENTIFY THE CRYSTAL SYSTEM:
sucrose
MONOCLINIC
IDENTIFY THE CRYSTAL SYSTEM:
boric acid
TRICLINIC
morphology of a crystalline form
HABIT
Same elemental substances, but different crystalline forms
POLYMORPHISM
the ability for a compound to exist in MORE THAN ONE CRYSTAL FORM with different unit cell parameters
POLYMORPHISM
the existence of a chemical element in two or more forms
ALLOTROPY
examples of polymorphs
CARBON & SULFUR
a special case of polymorphism
ALLOTROPIC
a polymorphous natural fat
- consists mainly of a single glyceride
THEOBROMA OIL OR CACAO BUTTER
Theobroma oil is capable of existing in how many polymorphic forms
4
Melting point:
UNSTABLE GAMMA FORM
18C
Melting point:
ALPHA FORM
22C
Melting point:
BETA PRIME FORM
28C
Melting point:
STABLE BETA FORM
34.5C
- Crystalline structure containing WATER MOLECULE
- Hydrous form
- Anhydrous form
HYDRATES
- Crystalline structure containing solvent molecules
SOLVATES
Another term for amorphous solid
SUPERCOOLED LIQUIDS
- Has a YIELD VALUE and no definite melting point
- Difference in rate of dissolution of antibiotic novobiocin
AMORPHOUS SOLIDS
faster rate of dissolution
AMORPHOUS FORM OF NOVOBIOCIN
slower rate of dissolution
CRYSTALLINE FORM OF NOVOBIOCIN
heat absorbed so that solid can be converted to liquid state; heat liberated so that liquid is converted to solid state
LATENT HEAT OF FUSION
- For solids and liquids
- Compute for change in FREZZING and MELTING POINT
CLAPEYRON EQUATION
- The position of equilibrium will move in such a way as to COUNTERACT THE CHANGE
- The system in equilibrium will adjust to REDUCE STRESS.
- Volume of solid > Volume of liquid
LA CHATELIER’S PRINCIPLE
exhibit SIMILAR PROPERTIES in ALL DIRECTIONS
ISOTROPIC
showing DIFFERENT CHARACTERISTICS in VARIOUS DIRECTIONS along the crystal
ANISTROPIC
- Molecules are immobile and no rotations
CRYSTAL
- One of the mesophases or intermediate states
- Intermediate state between solid and liquid
LIQUID CRYSTAL
Two types of liquid crystals
SMECTIC
NEMATIC
mobile in 2 directions and rotate about 1 axis
SMECTIC
mobile in 3 directions and rotate about 1 axis
NEMATIC
special type of NEMATIC
CHOLESTERIC
Molecules are mobile in 3 directions and rotate about 3 axes
LIQUID
the temperature at which a liquid passes into the solid state
FREEZING POINT
a system at equilibrium READJUSTS to REDUCE THE EFFECT of an external stress
LE CHATELIER’S PRINCIPLE
ability of drug to be ABSORBED
BIOAVAILABILITY
antibacterial
SULFAMETER
antiviral na nagprecipitate
RITONAVIR
mas maganda from 2 pero most products that are available in the market is in form 3
SULFAMETER
solid + liquid properties
LIQUID CRYSTALLINE STATE
4th state of matter
LIQUID CRYSTALLINE STATE / MESOPHASE
solid compounds but MOLECULES ARE MOVING
LIQUID CRYSTALS
SOAP LIKE OR GREASE LIKE
SMECTIC
THREAD LIKE
NEMATIC
gas + liquid properties
SUPERCRITICIAL FLUID STATE
supercritical fluid state movement
LIKE GAS
a supercritical fluid is a _______ formed from the gaseous state where the gas is held under a combination of temperature and pressures that EXCEED THE CRITICAL POINT
MESOPHASE
LCD meaning
LIQUID CRYSTALLINE DISPLAY
for EMULSION STABILITY as well as increase in SOLUBILIZATION
SMECTIC
for LCD displays
NEMATIC
- Solubilization and dissolution of cholesterol found in GALLSTONES
- Used as BIOPHYSICAL model for the structure and functionality of cell membranes
LIQUID CRYSTALS
- Gas-like since it can go through spaces
- Liquid-like since it is dense
- BEYOND CRITICAL TEMPERATURE and when you keep applying pressure, this will increase in density and since it cannot be converted to liquid state, the VISCOSITY REMAINS AS A GAS.
- It has the DENSITY OF LIQUID, but the VISCOSITY IS GASEOUS.
SUPERCRITICAL FLUIDS
supercritical fluid density
liquid
supercritical fluid viscosity
gaseous
a point where it can exist as solid, liquid, gas
TRIPLE POINT
TEMP:
solid & gas
LOW TEMP
TEMP:
liquid & gas
MIDDLE TEMP
- Extraction
- Crystallization
- Preparation of formulations (for micro and nanoparticles)
- Decaffeination of coffee (has replaced methylene chloride)
SUPERCRITICAL FLUID
defined by a series of independent variables
PHASES OF MATTER
- Different phases are coexisting, such as coexistence of water and gas, coexistence of solid and gas, or coexistence of 3 states of matter AT THE SAME TIME
PHASE EQUILIBRIA & PHASE RULE
who formulated the PHASE RULE
J. WILLARD GIBS
a relationship for determining the LEAST NUMBER OF INTENSIVE VARIABLES that CAN BE CHANGED without changing the equilibrium state of the system, or, alternatively, the LEAST NUMBER required to define the state of the system
PHASE RULE
PHASE RULE EQUATION
F = C - P + 2
number of degrees of freedom
F
no of components
C
no of phases
P
the SMALLEST NUMBER OF CONSTITUENTS by which the composition of each phase in the system at equilibrium
NUMBER OF COMPONENTS
a HOMOGENOUS portion of a system that is SEPARATED from other portions of the system by bounding surfaces
PHASE
the LEAST NUMBER of INTENSIVE VARIABELS that must be FIXED/KNOWN to describe the system completely
NUMBER OF DEGREES OF FREEDOM
TWO variables (temp
and pressure) must be fixed to define the system
BIVARIANT
ONE variable (temp or
pressure) must be fixed to define the system
UNIVARIANT
temp and pressure are
already fixed and defined
INVARIANT (0)
hexane + water (phase)
2 PHASES
Two-Component System is also known as
CONDENSED SYSTEM
- System in which VAPOR PHASE IS IGNORED and only the SOLID and/or LIQUID phases are CONSIDERED
TWO-COMPONENT SYSTEM / CONDENSED SYSTEM
Containing Solid-Liquid Phases
EUTECTIC MIXTURES
area within the curve represents a two-phase system; Any point beyond it is a single phase
BINODAL CURVE
temperature beyond which every proportion of A & B will exist as 1-phase; maximum temperature to obtain a one phase system
CRITICAL SOLUTION TEMPERATER (UPPER CONSOLUTE TEMPERATURE)
line from which a system separates into phases of constant composition; used to approximate the proportions of components A & B existing at a particular temperature
TIE LINE
phases of constant composition that separate when a mixture is prepared within the boundary of the 2-phase system
CONJUGATE PHASE
the COMPOSITION OF TWO OR MORE COMPOUNDS that exhibits a melting temperature lower than that of any other mixture of the compounds.
o MPA+B < MPA or MPA+B < MPB
EUTECTIC MIXTURE
the point at which the liquid and solid phases have the SAME COMPOSITION, CO-EXISTING
EUTECTIC POINT
phenomenon of LOWERING THE MELTING POINT due to COMBINATION OF COMPONENTS (thymol-salol; camphor-menthol)
EUTEXIA
a system consisting 3 components existing in phase equilibrium.
THREE COMPONENT SYSTEM / TERNARY SYSTEM
In a three component system, Temperature and pressure are both made ______
CONSTANT
Consists of two liquids that are PARTIALLY MISCIBLE TO EACH OTHER and the third component acts as co-solvent which has the affinity to both immiscible layers
THREE COMPONENT SYSTEM
