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31 Cards in this Set
- Front
- Back
Viscosity
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A measure of the resistance of a liquid to a flow
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Surface Tension
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The energy required to increase the surface area of a liquid by a given amount
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Surfactants
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Compounds that lower the surface tension of water are called active agents or this
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Crystalline Solid
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A solid whose atoms
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Unit Cell
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The smallest arrangement of connected points that can be repeated in three directions to form the lattice
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Amorphous Solid
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A solid in which the particles are not arranged in a regular
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Melting Point
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The temperature at which the forces holding a crystalline solids crystal lattice together are broken and it becomes a liquid
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Vaporization
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The process by which a liquid changes the a gas or vapor
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Evaporation
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When vaporization occurs only at the surface of a liquid
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Vapor Pressure
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The pressure exerted by a vapor over a liquid
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Boiling Point
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The temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure
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Sublimation
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The process by which a solid changes directly to a gas without first becoming a liquid
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Condensation
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The process by which a gas or a vapor becomes a liquid
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Deposition
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The process by which a substance changes from a gas or vapor to a solid without first becoming a liquid
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Freezing Point
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The temperature at which a liquid is converted into a crystalline solid
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Phase Diagram
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A graph of pressure versus temperature that shows in which phase a substance exists under different conditions of temperature and pressure
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Triple Point
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The point on a phase diagram that represents the temperature and pressure at which three phases of a substance can coexist
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Concentration
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A measure of how much solute is dissolved in a specific amount of solvent or solution
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Molarity (M)
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The number of moles of solute dissolved per liter of solution
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Molality
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The ration of the number of moles of solute dissolved in one kilogram of solvent
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Mole Fraction
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The ratio of the number of moles of solute in solution to the total number of moles of solute and solvent
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Colligative Properties
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Physical properties of solutions that are affected by the number of particles but not the identity of dissolved solute particles
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Vapor Pressure Lowering
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Due to the number of solute particles in solution and is a colligative property of solutions
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Boiling Point Elevation
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The temperature difference between a solution's boiling point a pure solvent's boiling point
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Freezing Point Depression
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The difference in temperature between its freezing point and the freezing point of its pure solvent
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Osmosis
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The diffusion of solvent particles across a semipermeable membrane from an area of higher solvent concentration to an area of lower solvent concentration
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Osmotic Pressure
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The amount of additional pressure caused by the water molecules that move into a solution
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Suspension
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A mixture containing particles that settle out if left undisturbed
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Colloid
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A heterogenous mixture of intermediate size particles (between the size of solution particles and suspension particles)
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Brownian Motion
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The erratic movement of colloid particles
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Tyndall Effect
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The phenomenon when dispersed colloid particles are large enough to scatter light
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