Area of pharmacy that deals with the quantitative and theoretic principles of science as they apply to the practice of pharmacy.

Biomedical aspects of the practice of pharmacy

Entity that is administered to the patients so that they receive an effective dose of a drug

is the fundamental unit of the metric system

Three fundamental dimensions: except

The larger the mass of the body and the greater the required acceleration, the greater the force that one must exert.

The lower the mass the higher the acceleration and force

Atmospheric pressure is measured through a

vapor pressure is measured through a

defined as the condition of a body that gives it the capacity to do work.

energy in action/motion

energy at rest

is the ratio of the mass of an object, determined in or referred to a vacuum, at a specified temperature, to the volume of the object at the same temperature.

mass under vacuum

differs from absolute density only in that the mass of the object is determined in air;

if the object and masses are made of the same material, or have the same density, there will be no difference in the buoyant effect, and the apparent density will be identical with the absolute density.

is an expression sometimes employed to indicate the mass of 1 mL (not cc, which is very slightly different) of a standard substance, such as water, at a specified temperature, relative to water at 4°C taken as unity.

relative density has a unit of joules

may be defined as the ratio of the mass of a substance to the mass of an equal volume of another substance taken as the standard

For gases, the standard may be hydrogen or air; for liquids and solids, it is water.

specific gravity is unitless

standard for solid and liquid

standard for gas except

“Unless otherwise stated, the specific gravity basis is 25°/25° , ie, the ratio of the weight of a substance in air at 25° to that of an equal volume of water at the same temperature.”

concrete number

is an abstract number

an unequal-arm designed for determining the density of liquids and solids by hydrostatic weighing.

A measure of the agreement among the values in a group of data

The agreement between the data and the true value

- the lowest and highest value

the average deviation from the mean

the attraction between molecules

attraction inside or within the molecule.

Electrostatic force of attraction between ions of opposite charge.

Transfer of electrons

Formed between atoms with a small difference in electronegativity

Sharing of electrons

Positive ions surrounded by a sea of mobile (delocalized) electrons. Strong electrostatic force of attraction binds the system together

the attraction of like molecules

the attraction of unlike molecules

When molecules interact, both repulsive and attractive forces operate.

Relate to nonionic interactions between molecules; yet involve charge to charge interactions

Weakest of all the intermolecular forces

Strongest van der waals force

also known as Orientation Effect

Dipolar molecules frequently tend to align themselves with their neighbors, so that the negative pole of one molecule points toward the positive pole of the next

Ex: water, HCl, alcohol, acetone, phenol

Permanent dipoles are capable of inducing an electric dipole in nonpolar molecules (which are easily polarizable) in order to produce dipole-induced dipole

Ex: methylene chloride, ether, ethyl acetate

Weakest vader waals force

Nonpolar molecules can induce polarity in one another by induced dipole-induced dipole because of the small size of a hydrogen atom and its electrostatic field, it can move in close to the electronegative atom and form an electrostatic type of union known as a hydrogen bond or hydrogen bridge.

Ex: organic solvents, organix compounds, hexane, carbon disulfite

Polar molecules are attracted to either positive charge (cations) or negative charge ion (anions)

Force of attraction is due to close proximity of charged ion to non polar element

Ex: potassium iodide

Strongest intermolecular force

The interaction between a molecule containing a hydrogen atom and a strongly electronegative atom such as fluorine, oxygen, or nitrogen is of particular interest.

Forces of attraction between non polar atoms and molecules in water

is a gaseous super-fluid phase formed by particles cooled to very low temperatures very near to absolute zero.

Cold liquid helium

increase or decrease in temperature, change in the state of matter

solid to liquid

liquid to solid

gas to liquid

liquid to gas

gas to plasma

plasma to gas

gas to solid

gas to liquid

assumes the shape and volume of its container particles can move past one another

compressible lots of free space between particles

flows easily particles can move past one another

assumes the shape of the part of the container which it occupies particles can move/slide past one another

not easily compressible little free space between particles

flows easily particles can move/slide past one another

retains a fixed volume and shape rigid - particles locked into place

not easily compressible little free space between particles

does not flow easily rigid - particles cannot move/slide past one another

IODINE GAS

Chlorine gas

Bromine gas

Inverse relationship pressure and volume at constant temperature

Direct relationship volume and temperature at constant pressure

Direct relationship pressure and temp at constant volume

INCREASE IN VOLUME, INCREASE IN TEMPERATURE

”At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.“

increase pressure, decrease solubility of gas

amount of gas dissolve in plasma is proportional to the partial pressure of the gas in equilibrium with the plasma

the total pressure exerted is equal to the sum of the partial pressures of the individual gases.

States that the total pressure in a mixture of gases is equal to the sum of the partial pressure of each gas

Speed of diffusion of gas

Relationship between the vapor pressure and the absolute temperature of a liquid

Heat taken up when the liquids vaporize and are lost or liberated when vapors condense to liquids

- ∆Hv is the heat absorbed by 1 mole of liquid when it passes into the vapor state

SOLID STATE 3 MAIN TYPES except

The structural units of crystalline solids, such as ice, sodium chloride, and menthol, are arranged in fixed geometric patterns or lattices.

Crystalline solids show definite melting points, passing rather sharply from the solid to the liquid state.

sodium chloride

urea

iodoform

sucrose

boric acid

the heat required to increase interatomic or intermolecular distances in crystals, thus allowing melting point to occur.

A crystal that is bound together by weak forces generally has a low heat of fusion and a low melting point, whereas one bound together by strong forces has a high heat of fusion and a high melting point.

Heat absorbed when 1 g of solid melts or the heat liberated when it freezes

Molar heat of fusion: amount of heat absorbed when 1 mole of solid changes to 1 mole of liquid

dictate the hardness and strength of metals

melts at 18 deg C

melts at 22 deg C

melts at 28 deg C

melts at 34.5 deg C

Polymorphism involves a change in one direction and is usually from a metastable to stable form

Examples: long-chain organics eg, fatty acids, glycerides and fats

Polymorphism involves a change in various direction and is usually associated with changes in temperature or solvent

Examples: Sulfur, water, aspirin

Also called as solvates

Crystals containing solvent molecules

Are those showing different characteristics in various directions along crystal

These crystals have unlike light properties in different sites

Crystals that exhibit similar properties and characteristics in all directions

These are amorphous solids and cubic crystals

may be considered as super cooled liquids in which the molecules are arranged in a random manner somewhat as in the liquid state.

These are carbon-based formed by the hybrodized carbon atom with S and P orbitals to give four valency bonds at fairly well defined angles.

fourth state of matter

The property of crystals and mesophase to divide passing light into two components with different velocities and refractive index

known as the Soap-like or Grease-like crystals

it is the phase that usually forms a ternary (complex) mixtures with other additives.

Known as the nematic form of liquid crystals

Crystals derived from the action of certain solvents on solids.

Crystals obtained by heating solids to obtain mesophase

The first thermotropic liquid crystal that was recorded studied by Reinitzer in 1888

- Is a mesophase formed from the gaseous state where the gas is held under a combination of temperature and pressure that exceed critical points

is device used for relating the effect of the least number of independent variables upon the various phases that can exist in an equilibrium system containing a given number of components.

is defined as bound space or a definite quantity of substance that is under observation and experimentation

- is a chemical and physical homogenous mixture of two are more substances

Depends on the sum of the individual properties of the components present in the system

Example: molecular weight

Depends on the type and arrangement of components in a system

levorotatory, dextrorotatory (the instrument used is a polarimeter)

Measures using a refractometer

Property that depends on the number of components in the system

Also known as Extrinsic property

Depends on the size and the amount of the materials in the system

Example: mass, length, volume, enthalpy, entropy, electrical resistance

Also known as Intrinsic property

Does not depend on the amount and size of material

Example: viscosity, density, temperature, velocity, specific gravity

consists of at least two phases with one or more dispersed (internal or solute) phases contained in a single continuous (external or solvent) phase.

- true solution

- particle size is less than 1 nanometer

greater than 0.5 micrometer

1 nanometer to 0.5 micrometer

a distinct homogenous part of a system separated by a definite boundaries from other parts of a system.

defined as a mixture of two or more components that form a homogenous molecular dispersion.

is a mixture of 2 or more substances in a single phase.

the part of a solution that is being dissolved (usually the lesser amount)

dissolving substance

the part of a solution that dissolves the solute (usually the greater amount)

dissolving medium

simplest solution

contains the maximum quantity of solute that dissolves at that temperature

Solute is usually at equilibrium of solvent

contains less than the maximum amount of solute that can dissolve at a particular temperature.

Solvent is greater than solute

contains more than the maximum amount of solute that a solvent can dissolve at a given temperature.

Solute is greater than solvent

are substances that do not ionize when dissolved in water and therefore do not conduct an electric current through the solution

are substances that form ions in solution, conduct electric current, and show apparent “anomalous” colligative properties.

strong electrolytes except

Examples include: sugar, glycerin, naphthalene, urea

Substances that do not yield ions when dissolved in water

proton loving or proton acceptor

examples: basic solvents like acetone, ether, liquid ammonia

- acidic solvent

- proton donor

example: formic acid, acetic acid, sulfuric acid, liquid hydrogen chloride and liquid hydrogen fluoride

Both acceptor and donor

Example: water and alcohol

Doesn’t accept, doesn’t donate

Example: hydrocarbon

moles of solute in 1 Liter of solution

gram equivalent weight in 1 liter of solution

moles of solute in 1000g of solvent

a ratio of the mole of one constituent to the total moles of all constituents

moles of one constituent in 100 moles of the solution;

grams of solute in 100 g of solution

milliliters of solute in 100mL of solution

grams of solute in 100mL of solution

it is the mass of one equivalent, that is the mass of a given substance which will:

• supply or react with one mole of hydrogen cations H+ in an acid–base reaction; or • supply or react with one mole of electrons e − in a redox reaction.

A stable phase structure with lowest free energy (internal energy) of a system, and also randomness or disorder of the atoms or molecules

Any changes in temperature, composition and pressure cause an increase in free energy and away from equilibrium thus forcing a move to another state

Is defined as any homogenous and physically distinct part of a system which is separated from other parts of the system by interphases

The number of components of a system at equilibrium is the smallest number of independently varying chemical constituents using which the composition of each and every phase in the system can be expressed.

Smallest number of constituent by which the composition of each phase in the system at equilibrium can be expressed in form of chemical formula or equation

Summarizes the conditions at which a substance exists as a solid, liquid or gas.

It is a “map” of the information about the control of phase structure of a particular material system

is a general relation between the variance, F, the number oc component, C, and the number of phases, P, at equilibrium, for a system of any composition

Independent variable that do not depend on the volume or the size, eg, temp, pressure

the line at which the system at equilibrium will separate into phases of constant composition, termed ‘conjugate phases’

a way to calculate the proportions of each phase present on a phase diagram in a two phase field (at a given temperature and composition)