| Term | Definition |
|---|
| kinetic molecular theory | 1) a gas is a collection of particles in constant straight-line motion 2) gas particles do not attract or repel eachother 3) there is a lot of space between gas particles 4) average kinetic energy of gas particles is proportional to temperature in kelvins |
| pressure | the result of the constant collisions between the atoms or molecules in a gas and the surface around them |
| 1 atm | = 760 mm Hg, = 760 torr |
| absolute zero | 0 K or 273.15 C |
| R | = .0821 (L*atm/ mol*K) |
| partial pressure component | the pressure due to any individual component in a gas mixture (= fractional composition of component x total pressure) |
| Dalton's law of partial pressure | P(tot)= P(a)+P(b)+P(c)+... |
| hypoxia | oxygen starvation caused by low oxygen levels |
| vapor pressure | the pressure of water in the mixture which depends on the temperature |
| standard temperature and pressure (STP) | 1 mol of gas at 273 K and 1 atm |
| intermolecular forces | attractive forces that exist between molecules (without them all matter would exist as gas) |
| surface tension | the tendancy of liquids to minimize their surface area |
| viscosity | the resistance of a liquid to flow |
| evaporation or vaporization | substance is converted from its liquid to gaseous form |
| condensation | substance is converted from its gaseous to liquid form |
| volatile | evaporate easily |
| dynamic equilibrium | point when the rates of condensation and evaporation become equal |
| vapor pressure | the partial pressure of a gas in dynamic equilibrium with its liquid |
| boiling point | temperature at which the vapor pressure of a liquid is equal to the pressure above it |
| evaporation | is endothermic |
| condensation | is exothermic |
| melting point | atoms and molecules have enough thermal energy to overcome the intermolecular forces that hold them at their stationary points |
| heat of fusion | amount of heat required to melt 1 mol of a solid |
| heat of vaporization | amount of heat required to vaporize 1 mol of liquid |
| sublimation | physical change in which a substance is converted directly from its solid to gaseous form |
| dispersion force | the default intermolecular force present in al molecules and atoms caused by fluctuations in the electron distribution within molecules or atoms |
| dipole-dipole force | exists within all polar molecules |
| miscibility | ability to mix without seperating into two phases of liquids |
| hydrogen bond | an additional intermolecular force of molecules of hydrogen bonded to fluorine, oxygen, or nitrogen; "super" dipole-dipole force |
| molecular solids | solids whose composite units are molecules |
| ionic solids | solids whose composite units are formula units |
| atomic solids | solids whose composite units are individual atoms |
| covalent solids | held together by covalent bonds; high melting point |
| nonbonding solids | held together by dispersion forces; low melting point |
| metallic solids | held together by metallic bonds; variable melting point |
| solution | a homogeneous mixture of two or more substances |
| solvent | the majority component of a solution |
| solute | the minority component of a solution |
| water | the most common solvent |
| solubility | the amount of the compound that will dissolve in a certain amount of liquid |
| saturated solution | a solution that holds the maximum amount of solute under the solution conditions |
| unsaturated solution | a solution holding less than the maximum amount of solute |
| supersaturated solution | a solution holding more than the the normal maximum amount of solute |
| electrolyte solution | a solution containing a solute that dissociates into ions |
| non electrolyte solution | a solution containing a solute that doesn't dissociate into ions and cannot conduct electricity |
| dilute solution | a solution containing small amounts of solute relative to solvent |
| concentrated solution | a solution containing large amounts of solute relative to solvent |
| mass percent | the number of grams of solute per 100 g of solution |
| molarity | the number of moles of solute per liter of solution |
| stock solution | solutions in concentrated forms |
| semipermeable membrane | a membrane that selectively allows some substances to pass through but not others |
| osmotic pressure | the pressure required to stop osmotic flow |
| osmosis | the flow of solvent from a less concentrated solution to a more concentrated solution |
| acids | produces H+ in an aqueous solution; have a sour taste; dissolve many metals; turn litmus paper red; pH <7 |
| bases | produces OH- in an aqueous solution; have a bitter taste; have a slippery feel; turn litmus paper blue; pH >7 |
| hydronium ion | H3O+ |
| Bronstead-Lowry definition | acid- donor; base- acceptor |
| Arrhenius base | acid- produces H+; base- produces OH- |
| amphoteric | substances that can act as an acid or base |
| conjugate acid-base pair | two substances related to each other by the transfer of a proton (example NH4+ and NH3) |
| neutralization reaction | acid-base reaction |
| salt | an ionic compound that usually remains dissolved in the solution |
| titration | when a substance in a solution of known concentration is reacted with another substance of unknown concentration |
| equivalence point | the point in the titration when the number of moles of OH- added equals the number of H+ originally in solution; when reached the titration is complete |
| indicator | dye whose color depends on the acidity of the solution |
| strong acid | one that completely ionizes in solution |
| strong electrolyte | a substance whose aqueous solutions are good conductors of electricity |
| monoprotic acids | acids containing only one ionizable patron |
| diprotic acids | acids containing two ionizable patrons |
| weak electrolyte | substance whose aqueous solutions are poor conductors of electricity |
| strong base | a base that completely dissociates in solution |
| ion product constant for water (Kw) | =[H3O+][OH-] |
| neutral solution | [H3O+][OH-] |
| acidic solution | [H3O+]>[OH-] |
| basic solution | [H3O+]<[OH-] |
| rate of chemical reaction | the amount of reactant that changes to product in a given period of time |
| collision theory | states that chemical reactions occur through collisions between molecules or atoms |
| reversible reaction | a reaction that can proceed in both the forward and reverse directions |
| dynamic equilibrium | in a chemical reaction, the condition in which the rate of the forward reaction equals the rate of the reverse reaction |
| equilibrium constant | the ratio, at equilibrium, of the concentrations of the products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients |
| Keq<1 | reverse reaction is favored; reactants are greater |
| Keq>1 | forward reaction is favored; products are greater |
| Le Chatelier's principle | when a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance |
| Exothermic chemical reaction | heat is a product |
| Endothermic chemical reaction | heat is a reactant |
| Solubility-product constant (Ksp) | the equilibrium expression for a chemical equation that represents the dissolving of an ionic compound |
| Molar solubility | the solubility units of moles per liter |
| Catalyst | a substance that increases the rate of a chemical reaction but is not consumed by the reaction |
Combine with other sets
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