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57 Cards in this Set
- Front
- Back
phase
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a physically distinct portion of a system.
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intermolecular forces
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the attractive and repulsive forces among the particles-molecules, atoms, or ions-in a sample of matter.
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phase changes
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a physical change from one phase to another, usually refering to a change in physical state
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condensation
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the process of a gas changing into a liquid
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vaporization
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the process of changing from a liquid to a gas.
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melting (fusion)
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the change of a substance from a solid to a liquid.
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freezing
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the process of cooling a liquid until it solidifies.
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heat of vaporization
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the enthalpy change occurring when 1 mol of a liquid substance vaporizes.
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heat of fusion
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the enthalpy change occurring when 1 mol of a solid substance melts
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sublimation
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the process by which a solid changes directly into a gas.
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deposition
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the process of changing directly from gas to solid
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heat of sublimation
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the enthalpy change occurring when 1 mol of a solid substance changes directly to a gas. the sum of the heats of fusion and vaporization
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heating-cooling curve
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a plot of temperature vs. time for a substance when heat is absorbed or released by the system at a constant rate.
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vapor pressure
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the pressure exerted by a vapor at equilibriumwith its liquid in a closed system.
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clausius-clapeyron equation
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an equation that expresses the relationship between vapor pressure of a liquid and temperature
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boiling point
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the temperature at which the vapor pressure of a gas equals the external (atmospheric) pressure.
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melting point
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the temperature at which the solid and liquid forms of a substance are at equilibrium.
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critical point
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the point on a phase diagram above which teh vapor cannot be condensed to a liquid; the end of the liquid-gas curve.
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phase diagram
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a diagram used to describe the stable phases and phase changes of a substance as a function of temperature and pressure.
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van der waals radius
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one-half of the closest distance between teh nuclei of identical nonbonded atoms
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dipole-dipole forces
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the intermolecular between oppositely charged poles of nearby polar molecules.
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hydrogen bond (H bond)
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a type of dipole-dipole force that arises between molecules that have an H atom bonded to a small, highly electronegative atom with lone pairs, usually N, O, or F
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polarizability
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the ease with which a particle's electron cloud can be distorted.
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dipersion force (London force)
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the intermolecular attraction between oppositely charged poles of nearby polar molecules.
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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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capillarity
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a property that results in a liquid rising through a narrow space against the pull of gravity
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unit cell
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the smallest portion of a crystal that, if repeated in all three directions, gives the crystal.
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coordination number
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in a crystal, the number of nearest neighbors surrounding a particle.
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simple cubic unit cell
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a unit cell in which a particle occurs at each corner of a cube
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body-centered cuic unit cell
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a unit cell in which a particule lies at each corner and in the center of a cube.
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face-centered cubic unit cell
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a unit cell in which a particle occurs at each corner and in the center of each face of a cube.
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packing efficiency
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the percentage of the available voume occupied by atoms, ions, or molecules in a unit cell.
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hexagonal closest packing
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a crystal structure based on the hexagonal unit cell in which teh layers have an abab... pattern.
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cubic closest packing
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a crystal structure based on the face-centered cubic unit cell in which the layers have an abcabc... pattern.
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atomic solid
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a solid consisting of individual atom sheld together by dispersion foces; the frozen noble gases are the only example.
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molecular solid
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a solid held together by intermolecular forces between individual molecules.
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ionic solid
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a solid whose unit cell contains cations and anions.
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metallic solid
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a solid whose individual atoms are held together by metallic bonding
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network covalent solid
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a solid in which all the atoms are bonded covalently.
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band theory
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an extension of molecular orbital theory that explains many properties of metals, in particular, the differences in electrical conductivity of conductors, semiconductors, and insulators.
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valence band
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in band theory, the lowerenergy portion of the band of molecular orbitals, which is filled with valence electrons.
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conduction band
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In band theory, the empty, higher energy portion of the band of molecular orbitals into which electrons move when condcuting heat and electricity.
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conductor
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a substance (usually a metal) that conducts an electric current well.
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semiconductor
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a substance whose electrical conductivity is poor at room temperature but increases significantly with rising temperature.
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insulator
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a substance (usually a nonmetal) that does not conduct an electric current
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superconductivity
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the ability to conduct a current with no loss of energy to resistive heating.
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crystal defects
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any of a variety of disruptions in teh regularity of a crystal structure.
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doping
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adding small amounts of other elements into the crystal structure of a semiconductor to enhance a specific property, usually conductivity.
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liquid crystals
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a substance taht flows like a liquid but packs like a crystalline solid at the molecular level.
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ceramic
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a nonmetallic, nonpolymeric solid that is hardened by heating it to high temperatures and, in most cases, consists of silicatemicrocrystals suspended in a glassy cementing medium.
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degree of polymerization
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the number of monomer repeat units in a polymer chain.
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random coil
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teh shape adopted by most polymer chains adn causec by random rotation about the bodns joining the repeat units.
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radius of gyration
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a measure of the size of a coiled polymer chain as teh averae distance from the cnter of mass of the chain to its outside edge.
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branch
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a side chain appended to a polymer backbone.
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crosslinks
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a branch that covalently joins one polymer chain to another
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elastomers
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a polymeric material that can be stretched and springs back to its original shape when released.
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nanotechnology
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the science and engineering of nanoscale (1-100 nm)systems.
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