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110 Cards in this Set
- Front
- Back
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compressible fluids, molecules widely separated
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gases
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relatively incompressible fluids, molecules more tightly compact
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liquids
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nearly incompressible and rigid, very close contact of molecules
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solid
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change of a substance from one state to another
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change of state or phase transition
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phase tranistion:L to S
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freezing
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phase tranistion:: S to L
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melting
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phase tranistion: G to L
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condensation
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phase tranistion: L to G
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boiling
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phase tranistion: G to S
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condensation or deposition
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phase tranistion: S to G
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sublimation
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the partial pressure of the vapor over a liquid, measured at equilibrium at a given temperature
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vapor pressure
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vapor pressure is dependent upon what other physical property
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temperature
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T up: VP: ?
& called what kind of relationship |
up
direct proportional |
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liquids and solids with relatively high vapor pressures at normal temperatures
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volatile
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temperature at which vapor pressure of a liquid equals the pressure exerted on the liquid
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boiling point
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boiling point at 1atm
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normal boiling point
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temperature at which pure liquid changes to crystalline soli
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freezing point
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identical numerically to freezing point, temperature at which a solid becomes a liquid
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melting point
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to melt a pure substance at its melting point requires an extra boost of energy to vercome these
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lattice energies
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the heat required to melt 1 mol of a pure substance
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heat of fusion
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heat of fusion units
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kJ/mol
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to boil a pure substance at its melting point requires an extra boost of energy to overcome these
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intermolecular forces
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heat required to boil 1 mol pure substance
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heat of vaporization
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heat of vaporization units
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kJ/mol
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It has been demonstrated that the logarithm of the vapor pressure of a liquid varies linearly with ...
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absolute temperature
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Clausius-Clapeyron Equation
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P2/P1 = DELTA-H-VAP/R(1/T1-1/T2), where R is 8.31 J/mol*K; must take antiln!
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antiln(a)=
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e^(a)=b
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graphical way to summarize the conditions under which the different states of a substance are stable
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phase diagram
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In a phase diagram, the 3 areas represent ____ where the curves represent ___.
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states
phase changes |
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dividing the solid region from the liquid region, represents the conditions under which the solid and liquid are in equilibrium
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Curve AB
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melting point curve
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Curve AB
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If a liquid is more dense than its solid, the curve leans slightly to the ___, left, causing the melting point to ___with pressure.
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left
decrease |
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If a liquid is ____ than its solid, the curve leans slightly to the right, causing the melting point to ____ with pressure
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less dense
increase |
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divides the liquid region from the gaseous region, represents the boiling points of the liquid for various pressures
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Curve AC
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divides the solid region from the gaseous region, represents the vapor pressures of the solid at various temperatures
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Curve AD
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triple point
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A
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The temperature above which the liquid state of a substance no longer exists regardless of pressure
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critical temperature
Tcrit |
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The vapor pressure at the critical temperature
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critical pressure
Pcrit |
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C
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critical point
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molecular structure of substance defines __ forces holding it together
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intermolecular
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physical properties attributed to intermolecular forces (4)
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vapor pressure
boiling point surface tension viscosity |
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energy required to increase surface area of a liquid by uit amount
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surface tension
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as IF's increase surface tension ___
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increase
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the resistance to flow exhibited by all liquids and gases
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viscosity
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as IF's increase viscosity ___
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increase
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2 types of intermolecular forces
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dipole-dipole
London (dispersion) forces hydrogen bonding |
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general term including dipole-dipole and London forces
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van der Waals forces
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van der Waals forces are considered to be relatively common and ___
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weak
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occurs in substances containing h atoms bonded to certain very electronegative atoms
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h ydrogen bonding
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IF where polar molecules attract one another
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dipole-dipole forces
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weak attractive forces resulting from instantaneous dipoles that occr due to the distortion of the electron cloud surrounding the molecule
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London forces
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London forces ___ with molecular weight
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increase
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all covalent molecules exhibit some ___ force
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London
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when IF are strong expect VP to be ___
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low
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when IF's are weak expect boiling points to be ___
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low
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surface tension ___ with increasig IF's
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increases
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viscosity increases with ___ IF's
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increasing
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a force that exists b/w a h atom covalently bonded to a very electronegative atom with a lone pair
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hydrogen bonding
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to exhibit h-bonding the electronegative atom must be one of these three
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N,O,F
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h-bonding molecules have abnormally high ___ ___ comparatively to van der Waals
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boiling points
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solids are characterized by the type of ___ holding the structural units together
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forces
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2 types of forces for olid structures
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intermolecular forces
chemical bonds |
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4 types of solids
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molecular
mettallic ionic covalent |
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a solid that consists of atoms held by intermolecular forces
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molecular solid
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solid of positive cores of atoms held by surrounding sea of electrons
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mettalic solid
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in mettallic bonding, postively charged atomic cores are surrounded by ___ electrons
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delocalized
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solid consists of cations and anions held by electrical attraction of opposite charges
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ionic solid
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solid consists atoms held in large networks or chains by covalent bonds
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covalent network solid
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physical properties of solids are attribbuted to __
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structure
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molecular solids tend to ahve __ melting points
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low
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ionic and covalent network solids tend to have ___ melting points
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high
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for mettallic solids there is considerable ___ in melting points
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variation
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mettallic in the middle of the ___ metals have the highest melting points
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transition
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depends on how easily structural units can be moved relative to eachother
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hardness
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molecular solids are relatively (hardness)
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soft
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ionic solids tend to (hardness) than mettallic solids
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harder
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covalent network solids are even (hardness) than ionic solids
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harder
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molecular and ionc srystals are said to be generally ___ due to the fact they tend to fracture along crystal planes
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brittle
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mettallic solids are describes to be
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malleable
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molecular and ionic solids are said to be __ electrical conductors
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non
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ionic solids only electrically conduct in their __ state
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molten
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molecular and ionic solids are said to be __ electrical conductors
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non
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mettallic solids are considered to be __ conductors
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good
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of covalent solids only __ conducts electricity
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graphite
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ionic solids only electrically conduct in their __ state
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molten
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2 types of solids
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crystalline
amorphous |
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mettallic solids are considered to be __ conductors
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good
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composed of one or more crystals
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crstalline solid
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of covalent solids only __ conducts electricity
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graphite
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each ___ has a well defined ordered structure in __-D
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crystal
3 |
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2 types of solids
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crystalline
amorphous |
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has a disordered structure
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amorphous solid
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composed of one or more crystals
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crstalline solid
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geometric arrangement of lattice points in a crystal
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crystal lattice
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each ___ has a well defined ordered structure in __-D
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crystal
3 |
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the smallest boxlike unit from which you can construct by stacking the units in 3d
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unit cell
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has a disordered structure
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amorphous solid
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geometric arrangement of lattice points in a crystal
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crystal lattice
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the smallest boxlike unit from which you can construct by stacking the units in 3d
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unit cell
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7 basic shapes lead to 7 basic crystal __
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systems
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7 basic crystal systems
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cubic
tetragonal orthohombic monoclinic hexagonal rhombohedral triclinic |
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a "primitive" lattice has points only at the __ of each cell
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corners
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a cubic unit cell in which lattice points are situated only at the corners
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simple
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cubic unit cell where there is a lattice point in the center of the cell as well as in the corners
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body-centered
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cubic unit cell where lattice points are at the center of each each face as well as corners
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face-centered
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2 kinds of crystalline defects
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chemical impurities
lattice formation |
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method for deter structure and dimensions of unit cell in crystalline compound
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x-ray diffraction
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normal bp for h2o
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100C
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normal fp for h2o
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0C
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name of the state of a substance beyong the critcal points of T and P
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supercritical fluid
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