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Creado por Andrea Smith
hace más de 9 años
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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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