2482201
Description
Flashcards by Andrea Smith, updated more than 1 year ago
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Created by Andrea Smith
over 9 years ago
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| Question | Answer |
| 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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