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29 Cards in this Set
- Front
- Back
Valence Shell Electron Pair Repulsion Theory (VSEPR)
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the geometric arrangement of atoms about a central atom in a covalent compound is determined solely by the repulsions between electron pairs present in the valence shell of the central atom
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Unique Properties of Water
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polar; forms hydrogen bonds; bent; high boiling point;
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Boiling Point
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the temperature at which bonds the molecules of a liquid begin to separate and enter the gas state
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Vapor Pressure
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relates to the tendency of particles to escape from the liquid
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Freezing Point
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characteristic temperature at which a liquid turn into a solid
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Surface Tension
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property of the surface of a liquid that allows it to resist an external force
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Capillary Action
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the ability of liquid to flow against gravity where liquid spontaneously rises in a narrow space such as a thin tube
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Adhesion
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any attraction process between dissimilar molecular species that can potentially bring them in "direct contact"
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Cohesion
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property of like molecules sticking together, being mutually attractive
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Density of Solid
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something's mass per unit volume
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Polar Covalent Bonds
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the electrons shared by the atoms spend a greater amount of time, on the average, closer to the Oxygen nucleus than the Hydrogen nucleus. This is because of the geometry of the molecule and the great electronegativity difference between the Hydrogen atom and the Oxygen atom
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Hydrogen Bond
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the attractive interaction of a hydrogen atom with an electronegative atom; The hydrogen must be covalently bonded to another electronegative atom to create the bond
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Electronegativity
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chemical property that describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself and thus the tendency to form negative ions.
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Moving Left --> Right
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- Atomic Radius Decreases
- Ionization Energy Increases - Electronegativity Increases |
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Moving Top --> Bottom
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- Atomic Radius Increases
- Ionization Energy Decreases - Electronegativity Decreases |
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Polar Molecule
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A polar molecule is a bit like a magnet: the two ends of magnet are different
Read more: http://wiki.answers.com/Q/What_is_a_polar_molecule#ixzz1IcGOjSjv |
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Non-Polar Molecule
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Molecule which has no separation of charge, so no positive or negative poles are formed
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Dipole
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has two oppositely charged sides
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Intermolecular Forces
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(forces between two molecules) are weak compared to the intramolecular forces (forces keeping a molecule together)
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Solvation of Ionic Solids
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the process of attraction and association of molecules of a solvent with molecules or ions of a solute. As ions dissolve in a solvent they spread out and become surrounded by solvent molecules.
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Solution
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a homogeneous mixture composed of two or more substances
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Solute
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substance dissolved in solvent, forming a solution
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Solvent
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a liquid, solid, or gas that dissolves another solid, liquid, or gaseous solute, resulting in a solution
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Hydration Shell
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When a solute is being dissolved in an aqueous (water) solution the partially positive H atoms surround the solute (forming a shell) and attach to make bonds with the atoms of the solute, breaking them apart and making them part of the solution.
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Molarity
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mols per liter of solution
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Method for making solutions of a given molarity
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M1 x V1 = M2 x V2
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Dilution
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the process of reducing the concentration of a substance
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Colligative Properties
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properties of solutions that depend on the number of molecules in a given volume of solvent and not on the properties/identity (e.g. size or mass) of the molecules.
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London Dispersion Forces
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a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. (happens with non-polar compounds)
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