Chem 1006 Key Terms

Pregunta	Respuesta
Intermolecular Forces	Forces between molecules
Intramolecular Forces	Forces within molecules
Strength of Attraction	Compare intermolecular forces between molecules that dictates phases at particular temperatures
Phase Changes	The change of state of a molecule or solution
Boiling Point	When the kinetic energy between molecules is high enough to overcome the attractive forces and change from liquid to gas
Vaporization	Liquid to gas phase change
Condensation	Gas to liquid phase change
Melting Point	When kinetic energy between molecules is high enough to overcome the attractive forces and change from solid to liquid phase
Melting	Solid to liquid phase change
Freezing	Liquid to solid phase change
Sublimation	Solid to gas phase change
De-sublimation	Gas to solid phase change
Ion-Dipole Attraction	Exists between an ion and a permanent dipole
Hydrogen Bond	Slightly polar hydrogen is attached to a lone pair
Dipole-Dipole Forces	Mutual attraction between two dipoles
Ion-Induced Dipole	Ion induces a dipole in another molecule
Dipole-Induced Dipole	Dipole induces a dipole in another molecule
Dispersion Forces	Shifts in electron cloud density to induce momentary attractions between molecules
Molecular Solids	Solids held together by intermolecular forces
Network Solids	Solids held together by covalent bonds between atoms
Metallic Solids	Solids held together by delocalized electrons shared between valence orbitals
Ionic Solids	Solids held together by electrical forces
Solute	What gets dissolved in the solution
Solvent	The solution that the solute gets dissolved into
Homogenous Mixture	Solute is evenly and uniformly distributed throughout the solvent so as they can not be separately identified
Heterogenous Mixture	Solute is not evenly dissolved in the solvent so you can identify the two separate species
Colloidal Suspension	Molecules of different phase uniformly dispersed throughout the medium
Miscibility	If something will dissolve in a solution
Solubility	How much a solute will dissolve in a solvent
Saturation Point	Reached when the maximum amount of solute has been dissolved in the solvent
Surfactants	A substance that tends to reduce the surface tension of a liquid in which it is dispersed
Colligative Properties	Properties that change based on the amount of solute present in solution
Osmosis	Movement of solvent molecules through a semipermeable membrane
Kinetics	How fast reactions occur under various conditions
Unimolecular Reactions	Single molecule reactant changes to form different molecules
Bimolecular Reactions	Two molecules collide and react to form one or more different molecules
Termolecular Reactions	Three molecules collide and react to form two or more different molecules
Rate (of a Reaction)	How fast a reactant is disappearing or how fast a product is appearing
Exothermic Reaction	Reaction that releases heat
Endothermic Reaction	Reaction that absorbs heat
Catalyst	Reactant that changes the mechanism of the overall reaction to lower the required activation energy
Bronsted-Lowry Acid	Any species that donates a proton
Bronsted-Lowry Base	Any species that accepts a proton
Amphiprotic Species	Species that can accept or donate protons
Strong Acid	Species fully dissociates to donate all protons
Strong Base	Species that fully dissociates to form hydroxide ions
Polyprotic Acids	Acidic species that can donate more than one proton
Buffer Solution	Solution that contains a weak species and its conjugate to protect the solution from major pH changes
Buffer Capacity	Amount of hydroxide and hydronium ions that a solution can tolerate without exceeding a specific pH range
Common Ion Effect	Occurs when a solid salt is added to a solution that contains one of the dissociated ions and so the solubility decreases
pH Effect	Salt dissociates to form the conjugate base of a weak acid and the base will combine with water to from an acid species
Thermodynamics	Study of energy transfers and transformations
System	Process being described or studied
Surroundings	Everything that is not involved in the system
First Law of Thermodynamics	Energy cannot be created nor destroyed only transferred (from one body to another) or transformed (from one form to another)
Molar Heat Capacity	Amount of heat needed to raise the temperature of 1 mole by 1 degree
Work	Energy used to move an object against an opposing force
State Functions	The conditions before and after a transformation takes place
Path Functions	How a transformation occurs
Path Independence	Any combination of steps that will result in the same overall change
Reaction Energy	Net change of all steps to complete a mechanism for an overall reaction
Enthalpy	Total heat content or flow contained within a system
Second Law of Thermodynamics	In a spontaneous process the total entropy of the system increases
Entropy	The amount of disorder of a system
Third Law of Thermodynamics	The entropy of a system approaches a constant value as the temperature reaches zero kelvin

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