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Chem Exam I
Molecular Orbital Theory through Physical Properties of Solutions
| Question | Answer |
|---|---|
| Result from the interaction of the atomic orbitals of the bonding atoms and are associated with the entire molecule | Molecular Orbitals |
| Lower energy and greater stability than the atomic orbitals from which it was formed | Bonding Molecular Orbitals |
| Higher energy and lower stablility than the atomic orbitals from which it was formed | Antibonding Molecular Orbitals |
| Electron density is concentrated symmetrically around a line between the 2 nuclei of the bonding atoms | Sigma Molecular Orbital |
| Electron density is conentrated above and below a line joining the 2 nuclei of the bonding atoms | Pi Molecular Orbital |
| Method of evaluating stablility-indicates the strength of a bond | Bond Order |
| Diatomic molecules containing atoms of the same elements | Homonuclear Diatomic Molecules |
| Hold atoms together in a molecule | Intramolecular forces |
| Dipole-Dipole, Dipole-induced dipole, and dispersion forces | Van der Waals forces |
| Attractive forces that pass between polar molecules, that is, between molecules that possess dipole moments | Dipole-Dipole Forces |
| Attract an ion (either a cation or anion and a polar molecule to each other | Ion-dipole forces |
| Separation of positive and negative charges in the atom or nonpolar molecule is due to the poximity of of an ion or a polar molecule | induced dipole |
| Ease with which the elecron distribution in the atom or molecule can be distorted | polarizability |
| Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules | Dispersion Forces |
| Special type of dipole-dipole interaction between the hydrogen atom in a polar bond such as N-H, O-H, or F-H and an electronegative O, N, or F atom | hydrogen bond |
| amount of energy required to stretch or increase the surface of a liquid by a unit area | surface tension |
| intermolecular attraction between like molecules | cohesion |
| an attraction between unlike molecules | adhesion |
| A measure of a fluid's resistance to flowgreater viscosity slower the liquid flows | Viscosity |
| Possesses rigid and long-range order; its atoms, molecules, or ions occupy specific positions | Crystalline solid |
| basic repeating structural unit of a crystalline solid | unit cell |
| Each sphere represents an atom, ion, or a molecule | lattice point |
| the number of atoms or ions surrounding an atom or ion in a crystal lattice | coordination number |
| Ex. glass-lack a regular 3-dimensional arrangement of atoms | Amorphous solids |
| Homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary | Phase |
| transformations from one phase to another | Phase Changes |
| At any given temperature, a certain number of the molecules in a liquid possess sufficient Kinetic Energy to escape from the surface | Evaporation |
| As the concentration of molecules in the vapor phase increases, some molecules return to the liquid phase | Condensation |
| Rate of a forward process is exactly balanced by the rate of the reverse process is reached when the rates of condenstation and evaporation are equal | Dynamic Equilibrium |
| Vapor pressure measured under dynamic equilibrium of condensation and evaporation | Equilibrium vapor pressure |
| Energy required to vaporize one mole of a liquid | Molar Heat of Vaporization |
| Temperature at which the vapor pressure of a liquid is equal to the external pressure | Boiling Point |
| Every substance has this above which its gas form cannot be made to liquefy, no matter how great the applied pressure --highest temperature at which a substance can exist as a liquid | Critical Temperature |
| Minimum pressure that must be applied to bring about liquefaction at the critical temperature | Critical Pressure |
| Temperature at which solid and liquid phases coexist in equilibrium | Melting Point |
| Energy required to melt 1 mole of a solid | Molar Heat of Fusion |
| Process in which molecules go directly fromm the solid into the vapor phase | Sublimation |
| Reverse Process that is vapor directly to solid | Deposition |
| Energy required to sublime one mole of a solid | Molar Heat of Sublimation |
| Conditions under which a substance exists as a solid, liquid, or gas | Phase Diagram |
| Only temperature and pressure at which all three phases can be in equilibrium with one another | Triple Point |
| Attractive forces between molecules | Intermolecular Forces |
| a solution that contains the maximum amount of a solute in a given solvent at a specific temperature | Saturated Solution |
| Contains less solute than it has the ability to dissolve | Unsaturated Solution |
| Contains more solute than is present in a saturated solution | Supersaturated Solution |
| Process in which dissolved solute comes out of solution and forms crystals | Crystallization |
| When two liquids are completely soluble in each other in all proportions | Miscible |
| the process in which an ion or a molecule is surrounded by solvent molecules arranged in a specific manner | Solvation |
| Percent by weight or the weight percent | Percent by mass |
| Number of moles of solute in one liter of solution | Molarity |
| Number of moles of solute in one kilogram | Molality |
| Continue with Section 13.4 |
Created by:
larryc166
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