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64 Cards in this Set
- Front
- Back
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Standard Atmosphere (atm)
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The pressure needed to support a column of mercury 760 mm high measured at 0 degrees C
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Boyle's Law
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The pressure-volume law
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Ideal Gas
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A gas that would obey the gas laws exactly over all temperatures and pressures
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Charle's Law
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Temperature-volume law
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Gay-Lussac's Law
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Pressure-temperature law
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Combined Gas Law
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The ratio PV/T is a constant for a fixed amount of gas
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Law of Combining Volumes
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When gases react at the same temperature and pressure, their combining volumes are in ratios of simple whole numbers
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Ideal Gas Law (Equation of State for an Ideal Gas)
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PV=nRT
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R (Universal Gas Constant)
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0.0821
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Dalton's Law of Partial Pressures
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The total pressure of a mixture of gases is the sum of their individual partial pressures
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Mole Fraction
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The ratio of the number of moles of a given component to the total number of moles of all components
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Diffusion
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The spontaneous mixing of the molecules of one gas with the molecules of another gas
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Effusion
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The gradual movement of gas molecules through a very tiny hole into a vacuum
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Graham's Law
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When comparing different gases at the same temperature and pressure, the rates of effusion are inversely proportional to the square roots of their densities
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Kinetic Theory of Gases
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1. A gas consists of an extremely large number of very tiny particles that are in constant, random motion
2. The gas particles themselves occupy a net volume so small in relation to the volume of their container that their contribution to the total volume can be ignored. 3. The particles often collide in perfectly elastic collisions with themselves and with the walls of the container, and they move in straight lines between collisions neither attracting nor repelling each other |
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Intermolecular Forces
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The attractions between molecules
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Intramolecular Forces
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The chemical bonds that hold molecules together
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Instantaneous Dipole (Momentary Dipole)
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When at any given moment the electron density of a particle can be unsymmetrical
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Induced Dipole
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A dipole created when the electron cloud of an atom or a molecule is distorted by a neighboring dipole or by an ion
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London Dispersion Forces
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Weak attractive forces caused by instantaneous dipole-induced dipole attractions
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Polarizability
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A term that describes the ease with which the electron cloud of a molecule or ion is distorted
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Ion-dipole Attractions
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The attraction between an ion and the charged end of a polar molecule
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Ion-induced Dipole
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Attraction between an ion and a dipole induced in a neighboring molecule
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Compressibility
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A measure of a substance's ability to be forced into a smaller volume
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Incompressible
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When it is very difficult to compress liquids or solids to a smaller volume by applying pressure
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Surface Tension
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The surface tension of a liquid is proportional to the energy needed to expand its surface area
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Wetting
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The spreading of a liquid across a surface to from a thin film
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Surfactants
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Chemicals that drastically lower the surface tension of water
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Viscosity
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A liquid's resistance to a change in form
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Evaporation
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When a liquid turns into a gas
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Sublimation
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When a solid goes directly to a gas without giong through the liquid state
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Condensation
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Vapor molecules changing to the liquid state
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Melting Point
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When a solid begins to change to a liquid as heat is added
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Vapor Pressure
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The pressure that is exerted by molecules that enter a vapor when a liquid evaporates
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Equilibrium Vapor Pressure of a Liquid
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When the rates of evaporation and concentration become equal, and the concentration of molecuoles in the vapor remains constant and the vapor exerts a constant pressure
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Equilibrium Vapor Pressure of a Solid
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The pressure of the vapor that is in equilibrium with a solid
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Boiling Point
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The temperature at which the vapor pressure of the liquid is equal to the prevailing atmospheric pressure
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Normal Boiling Point
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The boiling point of a liquid at 1 atm
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Superheated Liquid
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The condition of a substance in its liquid state above its boiling point
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Amorphous Solids
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Do not have the kinds of long-range repetitive internal structures that are found in crystals
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Glass
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Often used as a general term that refers to any amorphous solid
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Supercooled Liquid
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A term that is sometimes used to describe amorphous solids
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Ionic Crystals
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Have ions at the lattice sites and the bonding between them is mainly electrostatic, which is essentially nondirectional
*metal & nonmetal (ions) *high melting point *brittle *only conduct electricity in a solution or when molten |
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Molecular Crystals
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Solids in which the lattice sites are occupied either by atoms or molecules
*molecules in solid state *low melting point *weak forces holding together *don't conduct electricity |
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Covalent Crystals
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Solids in which lattice positions are occupied by atoms that are covalently bonded to other atoms at neighboring lattice sites
*bonded *high melting point *don't conduct electricity |
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Metallic Crystals
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*metals
*shiny *malleable *high melting point *conduct electricity (unique to type) |
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Triple Point
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The temperature and pressure at which there is an equilibrium between the solid, liquid, and gas phases
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Phase Diagram
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A graphical representation of the pressure-temperature relationships that apply to the equilibria between the phases of the substance
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Supercritical Fluid
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A substance that has a temperature above its critical temperature and a density near its liquid density
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Immiscible
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When two solutions are mutually insoluble
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Miscible
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When two solutions are mutually soluble
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"Like Dissolves Like" Rule
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When solute and solvent have molecules "like" each other in polarity, they tend to form a solution
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Hydration
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When ions become completely surrounded by water molecules
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Solvation
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The surrounding of a solute particle by solvent molecules
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Molar Enthalpy
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The total energy absorbed or released when a solute dissolves in a solvent at constant pressure to make a solution
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Colligative Properties
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Properties that depend mostly on the relative populations of particles in mixtures
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Nonvolatile Solutes
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Solutes that have no tendency to evaporate
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Freezing Point Depression
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The amount by which the freezing point is lowered
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Boiling Point Elevation
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The amount by which the boiling point is raised
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Dialysis
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The process in which a membrane is able to let both water and small solute particles through
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Osmotic Membrane
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A semipermeable membrane that will let only solvent molecules get through (the process of osmosis)
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Osmosis
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A net shift of solvent across the membrane from themore dilute solution (or pure solvent) into the more concentrated solution
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Osmotic Pressure
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The exact opposing pressure needed to prevent any osmotic flow when one of the liquids is pure solvent
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Ion Pairs
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Closely associated pairs
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