Molecular Orbital Theory through Physical Properties of Solutions
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| Result from the interaction of the atomic orbitals of the bonding atoms and are associated with the entire molecule | Molecular Orbitals
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| Lower energy and greater stability than the atomic orbitals from which it was formed | Bonding Molecular Orbitals
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| Higher energy and lower stablility than the atomic orbitals from which it was formed | Antibonding Molecular Orbitals
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| Electron density is concentrated symmetrically around a line between the 2 nuclei of the bonding atoms | Sigma Molecular Orbital
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| Electron density is conentrated above and below a line joining the 2 nuclei of the bonding atoms | Pi Molecular Orbital
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| Method of evaluating stablility-indicates the strength of a bond | Bond Order
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| Diatomic molecules containing atoms of the same elements | Homonuclear Diatomic Molecules
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| Hold atoms together in a molecule | Intramolecular forces
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| Dipole-Dipole, Dipole-induced dipole, and dispersion forces | Van der Waals forces
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| Attractive forces that pass between polar molecules, that is, between molecules that possess dipole moments | Dipole-Dipole Forces
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| Attract an ion (either a cation or anion and a polar molecule to each other | Ion-dipole forces
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| 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
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| Ease with which the elecron distribution in the atom or molecule can be distorted | polarizability
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| Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules | Dispersion Forces
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| 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
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| amount of energy required to stretch or increase the surface of a liquid by a unit area | surface tension
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| intermolecular attraction between like molecules | cohesion
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| an attraction between unlike molecules | adhesion
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| A measure of a fluid's resistance to flowgreater viscosity slower the liquid flows | Viscosity
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| Possesses rigid and long-range order; its atoms, molecules, or ions occupy specific positions | Crystalline solid
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| basic repeating structural unit of a crystalline solid | unit cell
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| Each sphere represents an atom, ion, or a molecule | lattice point
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| the number of atoms or ions surrounding an atom or ion in a crystal lattice | coordination number
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| Ex. glass-lack a regular 3-dimensional arrangement of atoms | Amorphous solids
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| Homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary | Phase
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| transformations from one phase to another | Phase Changes
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| At any given temperature, a certain number of the molecules in a liquid possess sufficient Kinetic Energy to escape from the surface | Evaporation
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| As the concentration of molecules in the vapor phase increases, some molecules return to the liquid phase | Condensation
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| 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
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| Vapor pressure measured under dynamic equilibrium of condensation and evaporation | Equilibrium vapor pressure
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| Energy required to vaporize one mole of a liquid | Molar Heat of Vaporization
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| Temperature at which the vapor pressure of a liquid is equal to the external pressure | Boiling Point
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| 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
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| Minimum pressure that must be applied to bring about liquefaction at the critical temperature | Critical Pressure
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| Temperature at which solid and liquid phases coexist in equilibrium | Melting Point
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| Energy required to melt 1 mole of a solid | Molar Heat of Fusion
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| Process in which molecules go directly fromm the solid into the vapor phase | Sublimation
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| Reverse Process that is vapor directly to solid | Deposition
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| Energy required to sublime one mole of a solid | Molar Heat of Sublimation
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| Conditions under which a substance exists as a solid, liquid, or gas | Phase Diagram
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| Only temperature and pressure at which all three phases can be in equilibrium with one another | Triple Point
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| Attractive forces between molecules | Intermolecular Forces
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| a solution that contains the maximum amount of a solute in a given solvent at a specific temperature | Saturated Solution
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| Contains less solute than it has the ability to dissolve | Unsaturated Solution
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| Contains more solute than is present in a saturated solution | Supersaturated Solution
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| Process in which dissolved solute comes out of solution and forms crystals | Crystallization
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| When two liquids are completely soluble in each other in all proportions | Miscible
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| the process in which an ion or a molecule is surrounded by solvent molecules arranged in a specific manner | Solvation
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| Percent by weight or the weight percent | Percent by mass
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| Number of moles of solute in one liter of solution | Molarity
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| Number of moles of solute in one kilogram | Molality
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| Continue with Section 13.4
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