IPS/CA2 Physical Pharmacy

Physical Pharmacy

Quantitative principles applied in pharmacy practice.

Intensive Properties

Independent of the amount of matter present.

Extensive Properties

Dependent on the quantity of matter present.

Additive Property

Depends on the sum of individual properties.

Constitutive Property

Depends on type and arrangement of components.

Colligative Property

Depends on the number of components present.

Molecular Weight

Sum of atomic weights in a chemical formula.

Molar Volume

Volume occupied by one mole of a substance.

Molar Refraction

Measure of how light bends in a substance.

Molar Parachor

Measure of molecular volume related to surface tension.

Solubility

Ability of a substance to dissolve in a solvent.

Optical Activity

Rotation of plane-polarized light by a substance.

Vapor Pressure Lowering

Decrease in vapor pressure due to solute addition.

Boiling Point Elevation

Increase in boiling point due to solute presence.

Freezing Point Depression

Decrease in freezing point due to solute presence.

Osmotic Pressure

Pressure required to stop osmosis in a solution.

Fundamental Dimensions

Basic measurable quantities like length, mass, time.

Derived Dimensions

Quantities derived from fundamental dimensions.

Surface Tension

Force per unit length at the surface of a liquid.

Energy

Capacity to do work, measured in Joules.

Determinate errors

Consistent errors affecting all observations similarly.

Indeterminate errors

Random errors varying between measurements.

Precision

Agreement of repeated measurements.

Accuracy

Agreement with the true value.

Range

Difference between highest and lowest values.

Mean deviation

Average of absolute deviations from the mean.

Standard deviation

Measure of data dispersion around the mean.

Variance

Square of the standard deviation.

Absolute error

Difference between measured and true value.

Relative error

Absolute error divided by true value.

Atom

Basic unit defining a chemical element.

Electron

Subatomic particle with negative charge.

Proton

Subatomic particle with positive charge.

Neutron

Neutral subatomic particle in the nucleus.

Nucleons

Collective term for protons and neutrons.

Ionic bond

Bond formed by electron transfer.

Covalent bond

Bond formed by electron sharing.

Non-polar bond

Equal sharing of electrons in a bond.

Polar bond

Unequal sharing of electrons in a bond.

Electronegativity

Tendency of an atom to attract electrons.

Cohesion

Attraction between similar molecules.

Adhesion

Attraction between different molecules.

Van der Waals Forces

Attractive forces between covalent molecules.

Hydrogen bond

Attraction involving hydrogen and electronegative atoms.

Water-Ethanol

A mixture of water and ethanol.

Water and Benzene

A mixture of water and benzene.

Benzene and Hexane

A mixture of benzene and hexane.

NaCl and Water

Dissolution of sodium chloride in water.

Debye Forces

Attraction from induced dipoles in non-polar molecules.

London Forces

Dispersion forces inducing polarity in non-polar molecules.

Keesom Forces

Attraction between permanent dipoles of polar molecules.

Hydrogen Bond

Attraction between hydrogen and electronegative atoms.

Ion-Dipole Forces

Attraction between ions and polar molecules.

Ion-Induced Dipole Interaction

Induction of polarity in non-polar molecules by ions.

Miscibility of HCl

Mixing of hydrochloric acid with other substances.

Formation of Carbonic Acid

Reaction of carbon dioxide with water.

Liquefaction of Gases

Process of converting gases into liquid form.

Preparation of NaCl

Formation of sodium chloride from sodium and chlorine.

Alpha Helix Stability

Stability of protein structure due to hydrogen bonds.

Kinetic Molecular Theory

Explains properties of matter based on particle motion.

Solid State

Matter with fixed shape and volume.

Liquid State

Matter with definite volume but no fixed shape.

Gas State

Matter with no fixed shape or volume.

Plasma State

Ionized gas with free-moving charged particles.

Bose-Einstein Condensate

State of matter at near absolute zero temperature.

Perfectly Elastic Collisions

Collisions where no energy is lost.

Crystalline Solid

Solid with a regular, repeating particle arrangement.

Amorphous Solid

Solid without a defined geometric structure.

Kinetic Energy

Energy enabling particle movement relative to each other.

Diffusion

Intermingling of molecules due to motion.

Kinetic Molecular Theory

Describes gas behavior based on particle motion.

Elastic Collisions

Collisions where total kinetic energy is conserved.

Volume of Gas

Gas occupies 10³ times liquid or solid volume.

Boyle's Law

P1V1 = P2V2 at constant temperature.

Charles's Law

V1/T1 = V2/T2 at constant pressure.

Gay-Lussac's Law

P1/T1 = P2/T2 at constant volume.

Combined Gas Law

P1V1/T1 = P2V2/T2 for all variables.

Avogadro's Law

Volume proportional to number of moles at STP.

Ideal Gas Law

PV = nRT relates pressure, volume, temperature.

Graham's Law

Effusion rate inversely proportional to molecular weight.

Dalton's Law

Total pressure equals sum of partial pressures.

Van der Waals Equation

Describes behavior of real gases considering interactions.

Van der Waals Constant a

Accounts for intermolecular forces in gases.

Van der Waals Constant b

Accounts for molecular volume and incompressibility.

Raoult's Law

Describes vapor pressure lowering in solutions.

Henry's Law

Gas solubility increases with pressure.

STP Conditions

Standard Temperature and Pressure: 0°C and 1 atm.

Molecular Weight

Mass of one mole of a substance.

Gas Volume at STP

1 mole occupies 22.4 L at STP.

Ideal Gas Behavior

Assumes no interactions between gas particles.

Real Gases

Do not behave ideally due to interactions.

Volume of gas

Negligible compared to confined space volume.

Continuous random motion

Particles move randomly due to kinetic energy.

Collision speed loss

Particles lose speed during collisions.

Real gas equation

Accounts for molecular interactions affecting pressure.

Van der Waals equation

Corrects ideal gas law for real gases.

Internal pressure per mole

Result of intermolecular forces between molecules.

Liquefaction of gases

Achieved by lowering temperature and increasing pressure.

Critical temperature

Above this, a liquid cannot exist.

Critical pressure

Pressure needed to liquefy gas at critical temperature.