Flashcards
Chem 1006 Key Terms
Cards in this deck (65)
- 1Intermolecular ForcesForces between molecules
- 2Intramolecular ForcesForces within molecules
- 3Strength of AttractionCompare intermolecular forces between molecules that dictates phases at particular temperatures
- 4Phase ChangesThe change of state of a molecule or solution
- 5Boiling PointWhen the kinetic energy between molecules is high enough to overcome the attractive forces and change from liquid to gas
- 6VaporizationLiquid to gas phase change
- 7CondensationGas to liquid phase change
- 8Melting PointWhen kinetic energy between molecules is high enough to overcome the attractive forces and change from solid to liquid phase
- 9MeltingSolid to liquid phase change
- 10FreezingLiquid to solid phase change
- 11SublimationSolid to gas phase change
- 12De-sublimationGas to solid phase change
- 13Ion-Dipole AttractionExists between an ion and a permanent dipole
- 14Hydrogen BondSlightly polar hydrogen is attached to a lone pair
- 15Dipole-Dipole ForcesMutual attraction between two dipoles
- 16Ion-Induced DipoleIon induces a dipole in another molecule
- 17Dipole-Induced DipoleDipole induces a dipole in another molecule
- 18Dispersion ForcesShifts in electron cloud density to induce momentary attractions between molecules
- 19Molecular SolidsSolids held together by intermolecular forces
- 20Network SolidsSolids held together by covalent bonds between atoms
- 21Metallic SolidsSolids held together by delocalized electrons shared between valence orbitals
- 22Ionic SolidsSolids held together by electrical forces
- 23SoluteWhat gets dissolved in the solution
- 24SolventThe solution that the solute gets dissolved into
- 25Homogenous MixtureSolute is evenly and uniformly distributed throughout the solvent so as they can not be separately identified
- 26Heterogenous MixtureSolute is not evenly dissolved in the solvent so you can identify the two separate species
- 27Colloidal SuspensionMolecules of different phase uniformly dispersed throughout the medium
- 28MiscibilityIf something will dissolve in a solution
- 29SolubilityHow much a solute will dissolve in a solvent
- 30Saturation PointReached when the maximum amount of solute has been dissolved in the solvent
- 31SurfactantsA substance that tends to reduce the surface tension of a liquid in which it is dispersed
- 32Colligative PropertiesProperties that change based on the amount of solute present in solution
- 33OsmosisMovement of solvent molecules through a semipermeable membrane
- 34KineticsHow fast reactions occur under various conditions
- 35Unimolecular ReactionsSingle molecule reactant changes to form different molecules
- 36Bimolecular ReactionsTwo molecules collide and react to form one or more different molecules
- 37Termolecular ReactionsThree molecules collide and react to form two or more different molecules
- 38Rate (of a Reaction)How fast a reactant is disappearing or how fast a product is appearing
- 39Exothermic ReactionReaction that releases heat
- 40Endothermic ReactionReaction that absorbs heat
- 41CatalystReactant that changes the mechanism of the overall reaction to lower the required activation energy
- 42Bronsted-Lowry AcidAny species that donates a proton
- 43Bronsted-Lowry BaseAny species that accepts a proton
- 44Amphiprotic SpeciesSpecies that can accept or donate protons
- 45Strong AcidSpecies fully dissociates to donate all protons
- 46Strong BaseSpecies that fully dissociates to form hydroxide ions
- 47Polyprotic AcidsAcidic species that can donate more than one proton
- 48Buffer SolutionSolution that contains a weak species and its conjugate to protect the solution from major pH changes
- 49Buffer CapacityAmount of hydroxide and hydronium ions that a solution can tolerate without exceeding a specific pH range
- 50Common Ion EffectOccurs when a solid salt is added to a solution that contains one of the dissociated ions and so the solubility decreases
- 51pH EffectSalt dissociates to form the conjugate base of a weak acid and the base will combine with water to from an acid species
- 52ThermodynamicsStudy of energy transfers and transformations
- 53SystemProcess being described or studied
- 54SurroundingsEverything that is not involved in the system
- 55First Law of ThermodynamicsEnergy cannot be created nor destroyed only transferred (from one body to another) or transformed (from one form to another)
- 56Molar Heat CapacityAmount of heat needed to raise the temperature of 1 mole by 1 degree
- 57WorkEnergy used to move an object against an opposing force
- 58State FunctionsThe conditions before and after a transformation takes place
- 59Path FunctionsHow a transformation occurs
- 60Path IndependenceAny combination of steps that will result in the same overall change
- 61Reaction EnergyNet change of all steps to complete a mechanism for an overall reaction
- 62EnthalpyTotal heat content or flow contained within a system
- 63Second Law of ThermodynamicsIn a spontaneous process the total entropy of the system increases
- 64EntropyThe amount of disorder of a system
- 65Third Law of ThermodynamicsThe entropy of a system approaches a constant value as the temperature reaches zero kelvin
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- Undergraduate Chem 1006 Flashcards on Chem 1006 Key Terms, created by Andrea Smith on 12/04/2015.
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- Andrea Smith
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